impact of elevated dissolved co john david pugh rona …
TRANSCRIPT
IMPACT OF ELEVATED DISSOLVED CO2
ON AQUIFER WATER QUALITY
by
JOHN DAVID PUGH
RONA J. DONAHOE, COMMITTEE CHAIR
CHUNMIAO ZHENG
FRED ANDRUS
GEOFF TICK
JAMES REDWINE
A DISSERTATION
Submitted in partial fulfillment of the requirements
for the degree of Doctor of Philosophy
in the Department of Geological Sciences
in the Graduate School of
The University of Alabama
TUSCALOOSA, ALABAMA
2015
Copyright John David Pugh 2015
ALL RIGHTS RESERVED
1
ABSTRACT
The focus of the current study was to thoroughly characterize the properties of a typical
Gulf Coast potable aquifer for purposes of performing a controlled CO2 release experiment and
to construct coupled geochemical and transport models capable of predicting impacts from CO2
migration into a drinking water aquifer. The aquifer is a methanogenic environment composed
primarily of quartz and feldspars, with minor or trace amounts of pyrite, mica, illite, smectite,
and kaolinite. The formation water is dominantly Na-HCO3, consistent with the theory and
PHREEQC modeling results that suggest aquifer freshening and ion exchange have played
dominant roles in determining the present-day dissolved major ion composition.
This study also presents the design and implementation of a closed loop pumping and
injection system designed to simulate CO2 leakage into a test site aquifer. Process monitoring
results indicated that the test was performed with minimal variation in key process parameters,
including temperature, pressure and injectate pH. In situ instrumentation deployed in monitoring
wells allowed continuous readings of groundwater pH and conductivity, which were critical
parameters for evaluating the aquifer response to carbonation and acidification. Successful
modeling simulation of the pH response using results from the aquifer testing program suggested
that the test was implemented and monitored appropriately and that that future data
interpretations and modeling of the field experiment were not compromised by test design.
Test results showed that no constituent was mobilized in excess of US EPA maximum
contaminant levels, but that many constituents (primarily major and minor cations) were released
in a pulse-like response at levels above their baseline concentrations. Dissolution of trace
iii
carbonate and pyrite in the aquifer are hypothesized to have triggered cation exchange reactions,
a dominant geochemical process affecting major and minor cation behavior in the aquifer. The
test has shown that migration of carbon dioxide into a drinking water aquifer can mobilize ions
into solution, but at levels that may not exceed EPA MCLs under the field conditions tested for
this specific system. Data presented here are potentially applicable to assessments across the
Gulf Coast, where the potential for deep geologic carbon sequestration is high.
iv
DEDICATION
I dedicate this dissertation Graham David Pugh, in hopes that he will never stop pursuing his
dreams.
v
LIST OF ABBREVIATIONS AND SYMBOLS
CCS carbon capture and storage
CEC cation exchange capacity
cm centimeter
cu uniformity coefficient
d10 effective grain size (cm)
d50 mean grain size (mm)
DOE Department of Energy
e-
electron
Eh Reduction potential
EPA Environmental Protection Agency
EPRI Electric Power Research Institute
ft feet
gpm gallons per minute
GS geologic sequestration
hr hour
j exponent
Kh hydraulic conductivity
L liter
LC-MS liquid chromatography – mass spectrometry
M meter
vi
MCL maximum contaminant level
MDEQ Mississippi Department of Environmental Quality
mg milligram
min minutes
mm millimeter
MSL mean sea level
mV millivolts
µg microgram
µmhos micromhos
NC not calculated
n.t.u. nephelometric turbidity units
NWIS U.S. National Water Information System
pH acidity
PVC poly-vinyl chloride
r2 correlation coefficient
sec second
SECARB Southeast Regional Carbon Sequestration Partnership
SEM scanning electron microscope
S.I. saturation index
s.u. standard units
TOC total/dissolved organic crabon
US United States
USGS United States Geological Survey
vii
X ion exchange surface
XRD X-ray diffraction
viii
ACKNOWLEDGEMENTS
I thank my advisor Dr. Rona Donahoe for making this happen. My wife, Sarah, and son,
Graham David, are the ultimate inspiration for following through. My families in South Carolina
and Ohio have encouraged me greatly. The people at Southern Company have been more than
generous letting me squeeze this into a busy work schedule, and the Department of Geological
Sciences has been very accommodating. Thanks to Plant Daniel, James Douglas, Kheushla
Powe, Dan Patel and Rick Hagendorfer for supporting the project design and implementation.
Thanks to Rob Trautz and the Electric Power Research Institute (EPRI) for project direction and
funding.
ix
CONTENTS
ABSTRACT .................................................................................................................................... ii
DEDICATION ............................................................................................................................... iv
ACKNOWLEDGEMENTS ......................................................................................................... viii
LIST OF TABLES .......................................................................................................................... x
LIST OF FIGURES ....................................................................................................................... xi
INTRODUCTION .......................................................................................................................... 1
GEOCHEMICAL CHARACTERIZATION OF THE GRAHAM FERRY AQUIFER IN
COASTAL MISSISSIPPI ............................................................................................................... 9
DESIGN AND IMPLEMENTATION OF A FIELD EXPERIMENT EVALUATING
IMPACTS OF CO2 LEAKAGE INTO A CONFINED AQUIFER ............................................. 53
GEOCHEMICAL IMPACT OF A CONTROLLED CO2 RELEASE FIELD TEST ON A
SHALLOW POTABLE COASTAL PLAIN AQUIFER ............................................................. 80
SUMMARY ................................................................................................................................ 115
APPENDICES ............................................................................................................................ 119
x
LIST OF TABLES
Table 2.1 Sediment characteristics ............................................................................................... 21
Table 2.2. Well slug test results. ................................................................................................... 23
Table 2.3 Summary of field parameter data during baseline sampling ........................................ 25
Table 2.4 Summary of baseline major and minor cation and anion concentrations. .................... 26
Table 2.5 Summary of trace element data during baseline sampling ........................................... 30
Table 2.6. Groundwater major ion concentrations measured in the current study and
previously reported for the Miocene aquifer system in Mississippi (MDEQ 2013). .................... 39
Table 2.7. Typical CO2-generating reactions in groundwater systems. ........................................ 44
Table 3.1. Well spacing distances and injection rates. ................................................................. 56
Table 3.2. Aquifer properties and water column pressures. ......................................................... 59
Table 4.1 Summary of cation and anion concentrations compared to US EPA MCLs ................ 85
Table 4.2 Summary of trace element concentrations compared to US EPA MCLs ..................... 86
Table 4.3 Summary of stationary and non-stationary chemical parameters during the
baseline sampling period............................................................................................................... 87
Table 4.4 Summary of statistical exceedances above background in each well for each cation . 88
Table 4.5 Summary of test period durations and sampling schedule ........................................... 89
Table 4.6 Response to CO2 behavioral categories ...................................................................... 103
xi
LIST OF FIGURES
Figure 2.1 Site location and regional geologic cross section ........................................................ 11
Figure 2.2 Well locations .............................................................................................................. 12
Figure 2.3 Photo of well-field (well BG-1 not shown) ................................................................. 13
Figure 2.4 Typical well construction detail (showing BG-1) ....................................................... 15
Figure 2.5 Sands and gravels from the Citronelle (a and b) and fine,silty sand from the
Graham Ferry (c)........................................................................................................................... 19
Figure 2.6. Study site cross-section, illustrating sequence of clay and sand units beneath
the test site..................................................................................................................................... 20
Figure 2.7 Scanning electron photomicrograph showing (a) quartz and pyrite, (b) pyrite
framboid (magnified from (a)), (c) quartz gypsum and pyrite and (d) gypsum and pyrite
(magnified from square area in (c)). ............................................................................................. 22
Figure 2.8. Pumping test results showing displacement versus time curves for PW-1,
MW-1, and IW-1. .......................................................................................................................... 24
Figure 2.9 Spatial variability of Ca, Mg, Na and K during baseline sampling ............................. 27
Figure 2.10 Spatial variability of Fe, Ba, Mn and Sr during baseline sampling ........................... 28
Figure 2.11 Spatial variability of SO4 during baseline sampling.................................................. 29
Figure 2.12 Groundwater sulfate, carbonate, and sulfide saturation indices box-and-whisker
plots (triangle indicates the average and vertical bars represent maximum and minimum values).
....................................................................................................................................................... 32
Figure 2.13. Histograms of groundwater carbonate mineral saturation indices. ......................... 33
Figure 2.14. Groundwater aluminum, iron, and manganese oxyhydroxide mineral saturation
indices box-and-whisker plots. ..................................................................................................... 34
Figure 2.15. Groundwater silicate mineral saturation indices box-and-whisker plots. ............... 35
xii
Figure 2.17. Hydraulic conductivity measurements of the current study, for the Graham
Ferry aquifer and other Gulf Coast aquifers, and values estimated for typical sediment grain
size classifications. ........................................................................................................................ 37
Figure 2.17. Conceptual model illustrating aquifer freshening of saline groundwater (X
represents the exchangeable mole fraction). ................................................................................. 40
Figure 2.18. Results of a simple PHREEQC rainwater-saline water mixing model showing
trends in groundwater major ion concentrations over time during aquifer freshening. ................ 41
Figure 2.19. Aquifer freshening trends of groundwater major ion concentrations modeled
using PHREEQC and incorporating ion exhange (Exchangeable mole fraction (X) = 0.03;
Ca-montmorillonite, calcite, and K-feldspar allowed to dissolve and illite allowed to
precipitate). ................................................................................................................................... 42
Figure 2.20 Plot illustrating relationship between excess sodium and depletions in Ca+Mg
in the Miocene aquifer in Mississippi and similarity to the Texas Gulf Coast. ............................ 43
Figure 2.21. Relationship between pH and degree of CO2 supersaturation in groundwater,
showing a higher degree of supersaturation at lower pH. ............................................................. 45
Figure 2.22. Histogram of groundwater pH measurements during the baseline study period. .... 45
Figure 2.23. Relationship between measured Eh values and Eh calculated using measured
concentrations of redox pairs. ....................................................................................................... 47
Figure 2.25. Possible stages of geochemical evolution of the study site aquifer over
geologic time (FeS(m) = mackinawite). ....................................................................................... 49
Figure 3.1. Well field layout. ........................................................................................................ 56
Figure 3.2 Site cross-section illustrating the injectate fluid delivery system. .............................. 58
Figure 3.3. Carbonation and injection system photograph. .......................................................... 59
Figure 3.4 Picture showing dedicated bladder pump and well completion. ................................. 61
Figure 3.5 Schematic showing the pressurized monitoring well sampling system. ..................... 62
Figure 3.6. Injectate water pH during the test period, showing pre- and postcarbonation pH. .... 63
Figure 3.7. Inlet and outlet water temperature during the test period. .......................................... 63
Figure 3.8. Inlet and outlet water pressure during the test period. ................................................ 64
Figure 3.9. Injectate water flow rate measured during the test period. ......................................... 65
xiii
Figure 3.10. Potentiometric groundwater elevations in all monitoring wells during the test
period. ........................................................................................................................................... 65
Figure 3.11. Approximate hydraulic gradient and injectate flow rate during the test period. ...... 66
Figure 3.12. Downhole groundwater pH measurements during the test period. .......................... 67
Figure 3.13. Downhole groundwater conductivity measurements during the test period. ........... 68
Figure 3.14. Downhole and surface pH measurements for well MW-1 groundwater. ................. 69
Figure 3.15. Downhole and surface pH measurements for well MW-2 groundwater. ................. 69
Figure 3.16. Downhole and surface pH measurements for well MW-3 groundwater. ................. 70
Figure 3.17. Downhole and surface pH measurements for well MW-4 groundwater. ................. 70
Figure 3.18. Relationship between pH and dissolved CO2 to PCO2. .............................................. 72
Figure 3.19. Representation of the PHREEQC 1-D column transport model. ............................. 74
Figure 3.20. Measured and modeled groundwater pH in down-gradient well MW-3.
Groundwater pH was modeled using a PHREEQC 1-D transport model without buffering
reactions. ....................................................................................................................................... 75
Figure 4.1 Box-and-whisker plots illustrating stationary and non-stationary baseline datasets ... 87
Figure 4.2 pH trends during baseline, injection and post-injection time periods. ........................ 90
Figure 4.3 Eh trends during baseline, injection and post-injection time periods. ......................... 91
Figure 4.4 Conductivity trends during baseline, injection and post-injection time periods. ........ 91
Figure 4.5 Alkalinity trends during baseline, injection and post-injection time periods. ............. 92
Figure 4.6 Calcium trends during baseline, injection and post-injection time periods................. 93
Figure 4.7 Trends of ferrous and ferric iron, showing markedly different responses during
the CO2 injection but similar post-injection behavior................................................................... 94
Figure 4.8 Silicon trends during baseline, injection and post-injection time................................ 94
Figure 4.9 Trends of potassium and lithium, showing responses to CO2 injection against
highly variable baseline concentrations. ....................................................................................... 95
Figure 4.10 Sodium trends during baseline, injection and post-injection time. ........................... 96
xiv
Figure 4.11 Trends of Al, Cu, Pb, Hg, Zn and Sb, showing sporadic nature of detection
throughout all test periods. ............................................................................................................ 97
Figure 4.12 Molybdenum concentrations over time, showing decreases in concentration
following CO2 injection ................................................................................................................ 98
Figure 4.13 Trends of Ni, Co, Cr and Be, showing increasing trends during the CO2
injection phase. Relationship of Co and Ni trends to CO2 injection are suspect due to
timing of response in multiple wells. ............................................................................................ 99
Figure 4.14 Trends of chloride concentrations, showing mostly stable concentrations
during the test period. ................................................................................................................. 100
Figure 4.15 Trends of sulfate concentrations, showing an increase during the active
injection period. .......................................................................................................................... 101
Figure 4.16 Trends of fluoride concentrations, showing decreases during the injection
period. ......................................................................................................................................... 101
Figure 4.17 Trends of dissolved organic carbon, showing increases during the injection
period. ......................................................................................................................................... 102
Figure 4.18 Nickel and cobalt trends, showing possible impact from downhole probes. .......... 105
Figure 4.19 Saturation indices of siderite, calcite, dolomite and rhodochrosite, suggesting
the possibility of carbonate dissolution and release of Ca, Mg, Mn and Fe. .............................. 107
Figure 4.20 Eh-pH diagram illustrating stability fields of ferrous iron, Fe(OH)3am, and
pyrite. .......................................................................................................................................... 108
Figure 4.21 Relationship between molybdenum and pH during the experiment. ...................... 109
Figure 4.22 Cross-well resistivity monitoring results (Wu et al., 2012), illustrating
progression of high-conductivity plume past MW-3 over time. ................................................. 110
1
Chapter 1
INTRODUCTION
Carbon capture and storage (CCS), specifically by means of geologic sequestration (GS),
is a developing technology to reduce CO2 emissions to the atmosphere. This technology
involves separating CO2 from flue gas and transporting the CO2 to underground storage locations
that are isolated from the atmosphere. These storage locations are typically permeable and
porous geologic formations that are not useful for any other purpose, such as drinking water.
NETL (2012) estimated that between 1,610 and 20,155 gigatons of CO2 may be stored by
means of GS in the United States, mostly in saline formations. The Department of Energy
(DOE) created Regional Carbon Sequestration Partnerships to gather data regarding the
effectiveness and safety of GS in different regions of the United States. Various geologic
settings are being evaluated, including depleted oil and gas fields, un-mineable coal seams, saline
formations, and shale and basalt formations. Studies have since indicated that the Southeastern
United States Coastal Plain region is home to large potential CO2 sinks. In this region, deep
saline formations, coal seams, and oil and gas reservoirs will be opportunistic storage formations
for CO2 sequestration.
The large capacity for CO2 storage in the Southeastern U.S. Coastal Plain, however, has
created the need to evaluate the risk of contamination to potable water supplies resting above
target storage formations (Apps et al., 2008). Celia and Nordbotten (2009) reviewed three
scenarios in which CO2 may leak out of the target formation: 1) diffusive leakage through
caprock, 2) leakage through faults and fractures, and 3) leakage through abandoned oil or gas
2
wells in the area. Leakage under any of these three scenarios may result in secondary plumes
forming in permeable layers above the target formation, a portion of which may enter a potable
water supply. Gas-phase CO2 will continue to migrate vertically, whereas dissolved CO2 will
migrate in the direction of regional groundwater flow (Celia and Nordbotten, 2009).
The primary risk to potable water supplies due to CO2 leakage into the aquifer will result
from the reactions between dissolved CO2 and the host aquifer mineral assemblage (Apps et al.,
2008; Harvey et al., 2012). One such reaction is the dissolution of carbonate minerals such as
calcite (Langmuir, 1997):
(1) CaCO3 + CO2(g) + H2O = Ca2+
+ 2HCO3-
Carbonate mineral dissolution can release elements such as calcium, magnesium, iron,
and manganese to solution, in addition to other carbonate-forming minor and trace elements. In
the absence of significant acid buffering capacity, the dissociation of carbonic acid can produce
pronounced acidity in the form of H+. In these systems, other important reactions may include
the pH-dependent surface complexation of trace elements onto iron oxyhydroxides or other
sorbent surfaces, as represented by the following surface complexation reaction between arsenate
and iron oxyhydroxide:
(2) ≡FeOH-1/2
+ 2 H+ + AsO4
-3 = ≡FeOAsO3H
-3/2 + H2O
where ≡FeOH-1/2
represents a surface functional group on iron oxyhydroxide, and ≡FeOAsO3H-
3/2 represents a monodentate inner-sphere surface species wherein arsenic is bound to the iron
oxyhydroxide surface (EPRI, 2009). In reducing environments, iron sulfide mineral
solubilization may result in release of dissolved iron and sulfur, and possibly to other trace
element impurities, by a reaction such as that for mackinawite dissolution:
3
(3) FeS + H+ = Fe
2+ + HS
-
The specific reactions that take place will depend entirely on the aquifer initial conditions,
including pH, redox state, mineral assemblage, temperature, and pressure.
Screening-level studies have simulated the interactions of injected CO2 with formation
fluids and minerals, providing guidance regarding what factors may be most important with
respect to sequestration mechanisms such as mineralization (Bachu and Adams, 2003; Xu et al.,
2004; Xu et al., 2007; Zerai et al., 2006; Wigand et al., 2008). These studies have focused
primarily on estimating the carbon sequestration capacity of deep, non-potable aquifer systems.
In most cases, a limited range of scenarios are evaluated, based upon “typical” characteristics of
potential receiving formations. For example, Xu et al. (2004) analyzed the impact of CO2
immobilization through carbonate mineral precipitation in the following aquifer settings: a
glauconitic sandstone representative of the Alberta Sedimentary Basin, Gulf Coast Mesozoic and
Tertiary sandstones representative of saline aquifers in offshore Texas, and a dunite reservoir.
The authors evaluated the mass of CO2 that could be immobilized by alteration of these mineral
assemblages at elevated temperatures and pressures.
Many studies have focused simulation efforts on assessing risks posed to potable water
supplies by intrusion of CO from deep storage reservoirs (Apps et al., 2008; Zheng et al., 2008;
Zheng et al., 2009). Apps et al. (2008) conducted a nationwide assessment of aquifer
equilibrium conditions, based on water quality data from the U.S. National Water Information
System (NWIS). The study involved calculating mineral saturation indices for the nation’s water
supply aquifers in an effort to establish initial equilibrium conditions which may be perturbed if
CO2 migrated into the aquifer. Minerals known to host trace elements in coal and ore deposits
were evaluated, and those found to exhibit near-saturation in the representative aquifer were
4
assumed to be present in the aquifer. In this fashion, theoretical aquifer mineral assemblages
were constructed using data derived from multiple sources.
In a companion study, Zheng et al. (2008) subjected the constructed equilibrium
conditions established by Apps et al. (2008) to a simulated intrusion of CO2. An important
conclusion of the study was that arsenic may be mobilized to concentrations exceeding the
United States Evironmental Protection Agency’s (US EPA) maximum contaminant level (MCL)
of 10 µg/L in certain aquifer settings, particularly those containing arsenopyrite and appreciable
sorption capacity. In one scenario, the total arsenic present was quantified as the sum of three
reservoirs: 1) dissolved arsenic; 2) arsenic in arsenopyrite, and 3) arsenic adsorbed to clay
minerals such as illite. Perturbation to the system resulted in an initial mobilization of sorbed
arsenic to levels exceeding the MCL, followed by increased sorption and long-term
immobilization of the released arsenic as pH decreased. The relative magnitudes of arsenic
release and long-term attenuation were found to be most sensitive to the sorption capacity of the
aquifer system. Low sorption capacity resulted in lower initial dissolved concentrations, but also
produced less capacity for long-term attenuation of mobilized arsenic. On the other hand, higher
sorption capacity created the risk of mobilizing more arsenic initially, but provided the advantage
of greater long-term attenuation capacity. A general conclusion of the study was that several
scenarios are possible, and that site-specific characteristics will govern the extent of reactions
that may pose risk to the water supply.
Confidence in modeled results is greatly enhanced if they are shown to be comparable to
field observations (Xu et al., 2004). Kharaka et al. (2009) and EPRI (2008) provided evidence
that primary geochemical effects resulting from CO2 intrusion into an aquifer system are
carbonate and oxide mineral dissolution. Kharaka et al. (2009) reported geochemical changes in
5
a 1500 m deep sandstone aquifer, following injection of CO2 into the Frio Sandstone in Texas.
A drop in pH to approximately 3 standard units (s.u.) due to CO2 dissolution was interpreted to
have mobilized significant calcium, iron, and manganese from carbonates and metal oxides.
Likewise, EPRI (2008) injected CO2 into a shallow, unconfined aquifer system and observed a
decrease in pH – from pH 7 to 6 – and increased dissolved bicarbonate, calcium, and
magnesium. The test results were ultimately difficult to model and interpret due to the
occurrence of gas exsolution from the aquifer into the vadose zone, and subsequent redissolution
of CO2 into the water table farther downgradient. More recently, field push-pull tests have been
conducted at two sites, one in a shallow Gulf Coast aquifer in Cranfield, Missisippi (Yang et al.,
2013) and another in southern France (Rillard et al., 2014). Yang et al. (2013) reported a low
risk of trace element mobilization, with dominant reactions being silicate dissolution, ion
exchange, desorption and dissolution of trace amounts of carbonates. Rillard et al. (2014)
reported significant mobilization of Ca and Mg, and limited mobilization of Fe, Mn, Zn and As.
Karamalidis et al. (2013) suggested that Cr, Pb, Mn, and Fe could exceed EPA MCLs in
sandstone reservoirs reacting with CO2. In laboratory studies, Lu et al. (2010) proposed a
behavior-based categorization of element response to CO2: Type 1 and Type 2. In their
laboratory experiments, Type 1 elements (Ca, Mg, Si, K, Sr, Mn, B, Zn) were observed to
increase and remain elevated after exposure to CO2;Type 2 elements (Fe, Al, Mo, U, V, As, Cr,
Cs, Rb, Ni, Cu) were observed to increase rapidly and then decrease to baseline concentrations.
Proper assessment of risk will require development of models capable of predicting
impacts to drinking water sources, and the testing of models against field observations. The
objectives of this study are to:
6
1. Investigate whether sequestered CO2 released from a geologic storage reservoir will have
an adverse impact on underground sources of drinking water from a dominantly quartz-
rich aquifer, and
2. Identify geochemical mechanisms responsible for releasing elements under carbonated
conditions.
In order to achieve these objectives, a thorough geochemical and physical characterization of a
test aquifer was conducted, dissolved CO2 was injected into the test aquifer, and the groundwater
monitored for metals mobilization.
This dissertation consists of three main chapters. In Chapter 2, the baseline geochemical
and physical characterization of the test site is documented and compared to other sites in the
Southeastern United States. This effort is critical to understanding future impacts to the test site.
In Chapter 3, an innovative field test design is described in detail so that the test results can be
interpreted with confidence. The design and approach are critical to enable valid interpretation
of the results. Finally, Chapter 4 focuses on the results of the test, evaluating monitoring well
data from a statistical and regulatory perspective, in addition to interpreting the geochemical
data. Preliminary results from the study and companion laboratory and field studies from the
subject test site have been previously published (Dafflon et al., 2012; Trautz et al., 2012;
Varadharajan et al., 2013). All of the material in this dissertation represents original work.
7
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Zheng, L., J.A. Apps, Y. Zhang, T. Xu, and J.T. Birkholzer, 2009. On mobilization of lead and
arsenic in groundwater in response to CO2 leakage from deep geological storage.
Chemical Geology, Vol. 268, No. 3-4, pp. 281-297.
9
Chapter 2
GEOCHEMICAL CHARACTERIZATION OF THE GRAHAM FERRY AQUIFER IN
COASTAL MISSISSIPPI
Abstract
The focus of the current study was to thoroughly characterize the properties of a typical
Gulf Coast potable aquifer for purposes of performing a controlled CO2 release experiment and
to construct coupled geochemical and transport models capable of predicting impacts from CO2
migration into a drinking water aquifer. The aquifer is a methanogenic environment composed
primarily of quartz and feldspars, with minor or trace amounts of pyrite, mica, illite, smectite,
and kaolinite. Chemical disequilibrium is suggested by comparing aquifer mineralogy to
calculated mineral saturation indices and by the presence of dissolved ferric iron under
methanogenic conditions. The formation water is dominantly Na-HCO3, consistent with the
theory and PHREEQC modeling results that suggest aquifer freshening and ion exchange have
played dominant roles in determining the present-day dissolved major ion composition.
Ultimately, data from this study were used to design and implement a controlled CO2 release
field test at the site evaluating real-world impacts to an aquifer due to elevated CO2. Data
presented here are potentially applicable to assessments across the Gulf Coast, where both the
potential for deep geologic carbon sequestration and continued reliance upon groundwater
resources are high.
10
1. Introduction
In order to successfully permit geologic CO2 sequestration projects, the potential
impacts from CO2 leakage into drinking water aquifers must be addressed, either through
predictive modeling or direct experimentation. In 2009, a controlled release field test was
initiated to evaluate potential impacts of carbon dioxide leakage into a shallow aquifer in the
Gulf Coast region of the United States (Trautz et al., 2013). The test was designed so that
thorough aquifer characterization prior to implementing the test would foster the production of
coupled geochemical and transport models capable of reproducing experimental results. If
successful, predictive modeling efforts can be used to help evaluate impacts without the need for
further extensive field testing at every potential sequestration site.
The purpose of Chapter 2 is to describe the baseline physical and geochemical
characteristics of the test site aquifer. Slug testing, pumping tests and grain size analyses were
used to define the flow characteristics of the test aquifer. Major, minor, and trace element data
were collected, in addition to dissolved gases, redox indicators, and other field parameters such
as pH, temperature, and conductivity. Physical and geochemical characteristics of the aquifer are
used to evaluate the broader applicability of the study to other Gulf Coast settings.
2. Site Location and Regional Hydrogeologic Setting
The Plant Daniel power plant site, located just north of Pascagoula Mississippi (Figure
2.1), was chosen due to a variety of factors. First, the site was host to a previous deep geologic
CO2 injection test implemented by the Southeast Regional Carbon Sequestration Partnership
(SECARB) Program and sponsored by the U.S. Department of Energy (DOE) (SECARB, 2008).
The fact that the site overlies favorable geology for purposes of CO2 sequestration makes it ideal
11
for assessing the potential water quality impacts to overlying potable aquifers. Also, due to the
aquifer’s confinement and location beneath a large controlled-access property, the study area
posed minimal risk to surrounding property owners and water supplies.
Figure 2.1 Site location and regional geologic cross section
.
Hancock
Harrison
Jackson
A
A’
WestA
EastA’
0
-1,000
-2,000
-3,000
-4,000
-5,000
Base of Freshwater (1,000 mg/L TDS)
Depth(feet)
10 miles
Key:
Site Location
Gulf of Mexico
AL
LA
N
12
The Pliocene-Miocene Aquifer System underlying Jackson County is comprised of the
Catahoula, Hattiesburg, Pascagoula, Graham Ferry, and Citronelle formations. Sand beds in the
Graham Ferry and Pascagoula formations provide the primary water supply along the coast. The
formations consist of alternating beds of sands and clays which were deposited in a deltaic or
near-shore marine environment. The Graham Ferry Formation is most widely used in the
vicinity of Pascagoula, MS. Sands thin toward eastern Jackson County, and generally dip and
thicken toward the coast (MDEQ, 2000).
3. Methods
3.1. Drilling and well installation
Site drilling investigations proceeded in two stages. Wells PW-1, MW-1, and MW-2
were installed during January and February of 2010. These wells were used to perform a
preliminary pumping test so that additional wells could be properly located for the experiment.
Wells IW-1, MW-3, MW-4, and BG-1 were installed in August 2010 (Figure 2.2), after
preliminary flow modeling indicated proper well spacing across the test field (Trautz et al.,
2013). The well field is shown in Figure 2.3.
Figure 2.2 Well locations
BG-1
IW-1MW-3
MW-4
PW-1
MW-1
MW-2
Background
Monitoring Well
Pumping Well
Injection
Well
Downgradient
Monitoring Wells
15 ftN
13
Figure 2.3 Photo of well-field (well BG-1 not shown)
All boreholes were drilled using the rotosonic drilling technique, and core samples were
collected from selected horizons within, above, and below the target test interval using 1.52 m
Lexan® (polycarbonate) tubes inside of a stainless steel core barrel. When extracted from the
steel outer core barrel, the Lexan® tubes were immediately capped on both ends to prevent
fallout of recovered sediment and to reduce exposure to the atmosphere. The tube was then cut
using a stainless steel blade handsaw into sections of desired length, capping each end
immediately after cutting. All sections were placed on frozen blue ice beneath dry ice and
cooled in the field. Samples were kept frozen using dry ice until shipped overnight to Lawrence
Berkeley National Laboratory.
MW-2
PW-1
MW-4
IW-1
MW-3 MW-1
14
Monitoring wells consisted of 4-inch PVC riser pipe with 4.57 meter screened intervals.
Screened intervals consisted of 0.01-inch machine-slotted openings; clean, quartz sand filter
packs were emplaced to achieve adequate holdback of formation sediments. Filter sand was
extended to 0.6 m above the screened interval, and 0.6 to 0.9 m of bentonite pellets were
emplaced immediately above the filter pack sand. After allowing the bentonite time to hydrate
and swell, a bentonite-cement grout mixture was poured between the riser pipe and borehole
walls to seal the well from leakage and provide structural integrity. Wells were completed with
0.6 m x 0.6 m concrete pads for surface protection. A typical well construction detail is shown
in Figure 2.4.
Wells were initially developed using a submersible pump, drawing at a rate of 56.7 liters
per minute (L/m). Each well was pumped for 4 hours, until the water was visually clear. Wells
were developed further on 9/1/10 and 9/2/10, using a submersible pump drawing at a rate of 15.1
L/m. Wells were pumped until turbidity levels dropped below 10 nephelometric turbidity units
(NTU) and other parameters [pH, temperature, conductivity, dissolved oxygen, turbidity, and
oxidation-reduction potential (ORP)] stabilized.
3.2. Slug testing and pump testing
Slug tests were conducted by lowering a PVC cylinder, or “slug”, of known volume into
the well and recording changes in water levels using downhole pressure transducers. Baseline
water level data were first recorded prior to lowering the slug into the well. After lowering the
slug into the well, water exited the well into the formation and water levels were allowed to
return to baseline conditions before raising the slug from the well. After raising the slug from
the well, water was allowed to enter the well from the formation.
15
The changes in water levels over time were used to compute values for horizontal hydraulic
conductivity, using both the Hvorslev (1951) and the Bouwer and Rice (1976) methods.
Figure 2.4 Typical well construction detail (showing BG-1)
BG-1
Hole diameter: 8”
Well casing diameter: 4”
Bottom of hole: 182’
Bentonite: 182-178’
20/30 Filter sand: 178-177.5’
Screened: 177.5-162.5’
20/30 Filter sand: 162.5-160’
30/65 Filter sand: 160-159.5’
Bentonite: 159.5-157.2’
Bentonite/cement: 157.2-0’
Brown sandy clay with organics (0-15’)
Tan and white fine sand with silt (15-19’)
Light green and gray clayey silt (19-23’)
Gray/tan/orange silty fine-coarse sand
w/gravel and wood fragments (23-63’)
Olive-gray clay (63-76’)
Light brown/tan/orange/gray silty fine-coarse
Sand w/gravel (76-108’)
Green clay (108-151’)
Gray/green clayey fine sand (151-156’)
Gray silty fine sand (156-178’)
Green clayey sand (178-182’)
10
20
30
40
50
60
70
80
90
100
110
120
130
140
150
160
170
180
Dep
th (
ft)
16
3.3. Slug testing and pump testing
Two pumping tests were also performed: an 18-hr test and a 39-hr test. The 18-hr
constant rate pumping test was performed using MW-2 as the pumping well, and MW-1 and
BW-1 as observation wells. The well was pumped at a rate of 18.9 L/m, and water level
observations were recorded at 2 second intervals throughout the test, using downhole pressure
transducers. A 39-hr pumping test was run beginning 9/23/10. Well PW-1 was pumped at a
constant rate of 18.9 L/m for the majority of the test. However, the initial pumping rate until 42
minutes into the test was documented as 22.7 L/m. Water level drawdown were measured and
recorded over time in wells MW-1 and IW-1. Data were analyzed using AQTESOLV™ aquifer
test data analysis software (HydroSOLVE, Inc., 2006).
3.4. Groundwater sampling and analysis
Wells were sampled using dedicated QED™ bladder pumps and following EPA-
recommended low-flow sampling procedures (US EPA, 1996). During purging at 0.76 L/m,
water from the well was expelled from a bladder to the surface and into a sampling tube. The
tubing was connected to an in-line flow-through cell where measurements of pH, dissolved
oxygen, conductivity, temperature, and oxidation-reduction-potential were made. When these
parameters stabilized, samples were collected upstream of the flow-through cell into appropriate
containers with preservatives. Samples were placed on ice (if necessary) and immediately
delivered, or shipped overnight, to the laboratory for analysis.
Field measurements were conducted for alkalinity, ferrous iron and total sulfide.
Alkalinity titrations were performed on non-filtered samples using a HACH® digital titrator
following an EPA-compliant HACH® method 8203. Ferrous iron measurements were made
17
using a 1,10 phenantholine iron reagent colorimetric method HACH® test kit with a range of
0.0-10.0 mg/L. Field sulfide was measured using a HACH® model HS-WR colorimetric kit.
Laboratory analyses were performed by TestAmerica, Inc. in Pensacola, FL. Major,
minor and trace cations were analyzed using either inductively coupled plasma (ICP) (Li, Fe, Si)
or inductively coupled plasma-mass spectrometry (ICP-MS) (Al, Ba, Ca, K Mg, Mg, Na, Sr, Ag,
As, Be, Co, Cd, Cr, Cu, Mo, Ni, Pb, Sb, Se, Tl, Zn) following US EPA (1994). Mercury (Hg)
was determined using cold vapor atomic absorption (CVAA) following US EPA (1994).
Dissolved phosphorous (P) was analyzed according to colorimetric method EPA 365.4 (US EPA,
1974). Anions Br, Cl, F, and SO4 were determined using ion chromatography (IC) following
MCAWW (1983). Total and bicarbonate alkalinity were analyzed following titration method
SM2320B (APHA, 2012). Nitrate (NO3), nitrite (NO2) and ammonia (NH3) were analyzed using
ion selective electrodes following SM4500. Dissolved gases methane (CH4), ethane (C2H6),
ethylene (C2H4), carbon dioxide (CO2), carbon monoxide (CO), oxygen (O2) and nitrogen (N2)
were analyzed in the laboratory using gas chromatography (GC) following RSK 175 (US EPA,
2004). Dissolved sulfide was measured in the laboratory by titrimetry following US EPA
(1978). Acetic acid, propionic acid, pyruvic acid, n-butyric acid, and lactic acid were analyzed
using direct aqueous injection into gas chromatograph (TestAmerica, 2014). Dissolved organic
carbon was measured following EPA method 415.1 (MCAWW, 1983).
3.5. Sediment characterization (X-ray diffraction, scanning electron microscopy, cation
exchange capacity)
Select sediment samples were delivered to the University of Alabama, Department of
Geological Sciences, who performed semi-quantitative X-ray diffraction (XRD) analysis to
determine sample mineralogy. Scanning electron microscope (SEM) images were performed by
18
the Southern Company Services, Inc. metallurgy department. The samples were examined in a
Hitachi S-3700N Scanning Electron Microscope after being placed on a carbon backing. Oxford
Instruments INCA X-ACT model number 51-ADD0030 Electron Dispersive Spectroscopy
apparatus was used to identify the elemental composition of the individual samples. All images
and elemental spectra were taken in variable pressure mode at 20 Pa. at 30.0kV. All images
were recorded with the backscatter electron detector, with quadrants biased to enhanced
topographic contrast. Cation exchange capacity (CEC) measurements were performed by Charu
Varadharajan at Lawrence Berkeley National Laboratory, as described in Varadharajan et al.
(2013). Grain size distributions were measured at the Alabama Power Company soils laboratory
in Varnons, Alabama following ASTM method D422 (ASTM, 2007).
4. Results
4.1. Hydrostratigraphy, grain size and mineralogy
The first two sand units encountered consisted of orange and gray, gravel-rich sands,
while the third and lowermost aquifer unit was characterized as gray, well-sorted, fine-grained
sand with trace amounts of silt and clay (Figure 2.5). The lowermost aquifer was bound above
and below by olive green silt- and clay-rich confining to semi-confining units (Figure 2.6). The
Citronelle Formation contained more coarse sand and fine gravel than the target Graham Ferry
Formation. The Graham Ferry, bound above and below by silt- and clay-rich layers, was
composed primarily of well-sorted fine-grained sand, with minor silt and clay.
19
Figure 2.5 Sands and gravels from the Citronelle (a and b) and fine,silty sand from the Graham
Ferry (c)
(a) (b) (c)
20
Figure 2.6. Study site cross-section, illustrating sequence of clay and sand units beneath the test
site.
PW-1 MW-4 MW-3 IW-1 BG-1
Sand and Gravel
Clay
Clay
Sand and Gravel
Silty Fine Sand
Clay
Clayey Sand
Fine Sand
Silt
Clay
0 M
-10 M
-20 M
-30 M
-40 M
-50 M
10 M .
0 M 10 M 20 M 30 M 40 M 50 M 60 M 70 M 80 M 90 M
Test Zone
NW SE
Ele
vation
(Mete
rs M
SL)
Distance (Meters)
A
A’
BG-1
IW-1MW-3
MW-4
PW-1
MW-1
MW-2
N
21
Bulk sample X-ray diffraction (XRD) revealed a mineral assemblage consisting of quartz,
albite, sanidine, pyrite, and illite (Table 2.1). Sandy samples exhibited the lowest cation
exchange capacities, and those containing illite and pyrite exhibited higher cation exchange
capacities. Pyrite was identified in organic-rich and clayey sediments. Scanning electron
microprobe images showed that pyrite framboids were present. Also present were needle-like
growths of what appeared to be gypsum on quartz, although gypsum was not detected with XRD
analysis (Figure 2.7).
Table 2.1 Sediment characteristics
Well Depth (m) CEC
(meq/100g)
Minerals Identified by XRD Notes
PW-1 48.7 1.34 Quartz, Sanidine Sand
MW-4 51.8 1.36 Quartz, Sanidine, Albite, Illite Sand
IW-1 52.1 1.48 Quartz, Sanidine, Albite Sand
MW-2 50.9 5.3 Quartz, Sanidine, Albite, Illite,
Pyrite Organics present
IW-1 46.9 2.13 Albite, Sanidine, Illite Clay above target
zone
MW-3 45.7 17.88 Quartz, Sanidine, Albite, Illite,
Pyrite
Clay above target
zone
BG-1 55.5 5.01 Quartz, Sanidine, Albite, Illite,
Pyrite
Clay below target
zone
MW-2 55.1 3.88 Quartz, Sanidine, Albite, Illite,
Pyrite
Clay below target
zone
22
Figure 2.7 Scanning electron photomicrograph showing (a) quartz and pyrite, (b) pyrite framboid
(magnified from (a)), (c) quartz gypsum and pyrite and (d) gypsum and pyrite (magnified from
square area in (c)).
4.2. Slug testing and pump testing
Slug tests were performed in wells PW-1, MW-1 and MW-2 (Table 2.2).
Using the slug withdrawal data (i.e., water flow from the aquifer toward the well), the average
calculated horizontal hydraulic conductivities were 0.015 and 0.011 cm/sec (42.5 and 31.2
ft/day) using the Hvorslev and Bouwer-Rice solutions, respectively.
Displacement versus time data for both observation wells in the first pumping test agree
with the Theis solution for confined aquifer conditions (Figure 2.8). Well MW-1 data after 2
minutes and all of well PW-1 data fit the Theis solution curve well. Hydraulic conductivity
calculated using the Theis solution for wells PW-1 and MW-1 during the first test were 44.4 and
150x 3,000x
350x 3,000x
(a) (b)
(c) (d)
Pyrite
Quartz
Gypsum
Gypsum
Pyrite
framboid
Quartz
Quartz
Pyrite
23
44.6 ft/day, respectively. Horizontal hydraulic conductivity calculated using the Theis solution
for wells MW-1 and IW-1 during the second test were 40.8 and 41.2 ft/day, respectively (Figure
2.8).
Table 2.2. Well slug test results.
Well Test
Hvorslev (1951)
solution
(cm/sec)/(ft/day)
Bouwer-Rice (1976)
solution
(cm/sec)/(ft/day)
PW-1 Slug in 0.026/73.7 0.018/51.0
Slug out 0.014/39.1 0.009/25.5
MW-1 Slug in 0.005/14.2 0.004/11.3
Slug out 0.015/42.5 0.012/34
MW-2 Slug in 0.007/19.8 0.006/17
Slug out 0.015/39.7 0.011/31.2
Slug in average 0.012/34.0 0.009/25.5
Slug out average 0.015/42.5 0.011/31.2
Displacement versus time data for both observation wells in the first pumping test agree
with the Theis solution for confined aquifer conditions (Figure 2.8). Well MW-1 data after 2
minutes and all of well PW-1 data fit the Theis solution curve well. Hydraulic conductivity
calculated using the Theis solution for wells PW-1 and MW-1 during the first test were 44.4 and
44.6 ft/day, respectively. Horizontal hydraulic conductivity calculated using the Theis solution
for wells MW-1 and IW-1 during the second test were 40.8 and 41.2 ft/day, respectively (Figure
2.8).
24
Figure 2.8. Pumping test results showing displacement versus time curves for PW-1, MW-1, and
IW-1.
4.3. Groundwater chemistry
All chemical data are tabulated in Appendix A, including field measurements (Table A-
1), major and minor cations (Table A-2), anions and alkalinity (Table A-3), trace elements
(Table A-4), dissolved organics (Table A-5) and dissolved gases (Table A-6). This section
summarizes data collected during the baseline sampling period from 2/12/10 to 10/18/11.
0.1 1. 10. 100. 1000. 1.0E+40.001
0.01
0.1
1.
Time (min)
Dis
pla
cem
ent (f
t)
Obs. Wells
TW-1
Aquifer Model
Confined
Solution
Theis
Parameters
T = 816.1 ft2/dayS = 0.0001694Kz/Kr = 0.1b = 20. ft
MW-1
Test 2
Theis solution
T = 816.1 f t2/d
S = 0.0001694
Kh = 40.8 f t/d
0.1 1. 10. 100. 1000. 1.0E+40.001
0.01
0.1
1.
Time (min)
Dis
pla
cem
ent (f
t)Obs. Wells
IW-1
Aquifer Model
Confined
Solution
Theis
Parameters
T = 832.3 ft2/dayS = 0.0001735Kz/Kr = 0.1b = 20. ft
IW-1Test 2
Theis solution
T = 823.3 ft2/d
S = 0.0001735
Kh = 41.2 ft/d
BW-1 Constant Rate
0.01 0.1 1. 10. 100. 1000. 1.0E+40.01
0.1
1.
Time (min)
Dis
pla
cem
ent (f
t)
Obs. Wells
BW-1
Aquifer Model
Confined
Solution
Theis
Parameters
T = 887.2 ft2/dayS = 0.000247Kz/Kr = 0.1b = 20. ft
0.01 0.1 1. 10. 100. 1000. 1.0E+40.01
0.1
1.
Time (min)
Dis
pla
cem
ent (f
t)
Obs. Wells
TW-1
Aquifer Model
Confined
Solution
Theis
Parameters
T = 891.8 ft2/dayS = 0.0002915Kz/Kr = 0.1b = 20. ft
PW-1
Test 1
Theis solution
T = 887.2 f t2/d
S = 0.000247
Kh = 44.4 f t/d
MW-1
Test 1
Theis solution
T = 891.8 f t2/d
S = 0.0002915
Kh = 44.6 f t/d
Dis
pla
ce
me
nt (
ft)
Dis
pla
ce
me
nt (
ft)
Dis
pla
ce
me
nt (
ft)
Dis
pla
ce
me
nt (
ft)
Time (min) Time (min)
Time (min)Time (min)
25
4.3.1. Field parameters
Baseline field parameter data are summarized in Table 2.3. pH was neutral to slightly
alkaline during the baseline test period. Measurements of oxidation-reduction potential (ORP)
and dissolved oxygen suggest that the aquifer was anaerobic. Reducing conditions were
indicated by the persistence of measurable dissolved ferrous iron, ranging from 0.01 to 0.64
mg/L. Conductivity and alkalinity were relatively constant during the study period.
Table 2.3 Summary of field parameter data during baseline sampling
Parameter Unit Minimum Maximum Mean
Temperature °C 22 26 23
El. Conductivity uS/cm 617 692 654
pH s.u. 7.36 8.69 7.89
ORP mV -276 10 -136
Ferrous iron mg/L 0.05 0.64 0.30
Alkalinity mg/L as CaCO3 239 327 297
Dissolved Oxygen mg/L 0.01 0.64 0.21
4.3.2. Major and minor cations and anions
Sodium and bicarbonate ions dominated the relative abundances of cations and anions,
respectively (Table 2.4). Calcium, magnesium, and potassium concentrations were less than 10
mg/L, and mean concentrations were less than 5 mg/L. Barium, strontium, lithium, and
manganese concentrations were all less than 0.1 mg/L. The degree of variability between wells
for major and minor cations is illustrated in Figure 2.9 and Figure 2.10. In general,
concentrations of Mg, K, Fe, Mn and Ba showed greater spatial variability than Ca, Na and Sr.
Nitrate and nitrite were not detected for the majority of sample events, with non-detect rates of
78% and 98%, respectively. Chloride concentrations were relatively stable, averaging 26 mg/L.
26
Sulfate concentrations averaged less than 1 mg/L, and were higher in BG-1 than in other wells
(Figure 2.11).
Table 2.4 Summary of baseline major and minor cation and anion concentrations.
Parameter Unit Minimum Maximum Mean
Ca mg/l 2.0 4.2 2.8
Mg mg/l 0.81 1.90 1.26
Na mg/l 140 190 157
K mg/l 1.80 7.60 3.10
Si mg/l 8.4 13 11.7
Total Fe mg/l 0.05 0.89 0.53
Fe2+
mg/l 0.05 0.64 0.30
Fe3+
mg/l 0* 0.67 0.23
Al ug/l <0.023 0.047 <0.023
Ba mg/l 0.027 0.076 0.056
Sr mg/l 0.075 0.14 0.098
Mn mg/l 0.025 0.10 0.064
Li mg/l 0.008 0.047 0.022
Cl mg/l 21 30 26
HCO3
mg/l 239 326 297
SO4
mg/l <0.015 3.4 0.577
Br mg/l <0.0041 0.5 0.11
F mg/l 0.30 0.60 0.45
NO3 mg/l <0.013 0.034 <0.013
NO2 mg/l <0.013 0.013 <0.013
*Calculated as difference between total Fe and Fe2+
27
Figure 2.9 Spatial variability of Ca, Mg, Na and K during baseline sampling
4.3.3. Trace elements
Table 2.5 summarizes baseline concentrations of trace elements. Silver, As, Be, Co, Cr,
Cu, Hg, Pb, and Tl were not present above method detection limits during the baseline study
period. Molybdenum was the only trace element detected at each sampling event, with a
concentration range of 0.002 to 0.013 mg/L and minor variability between wells (Table A-4).
MW-1 MW-3 MW-2 MW-4 BG-1
Stations
0
1
2
3
4
5
6
7C
a (
mg
/l)
H
H
H
H
H
H
H
H
H
H
75th Percentile
Median
25th Percentile
95th Percentile
5th Percentile
H
H
Max.
Min.
75th Percentile
Median
25th Percentile
95th Percentile
5th Percentile
H
H
Max.
Min.
MW-1 MW-3 MW-2 MW-4 BG-1
Stations
0.0
0.4
0.8
1.2
1.6
2.0
Mg
(m
g/l) H
H
H
H
H
H
H
H
H
H
75th Percentile
Median
25th Percentile
95th Percentile
5th Percentile
H
H
Max.
Min.
75th Percentile
Median
25th Percentile
95th Percentile
5th Percentile
H
H
Max.
Min.
MW-1 MW-3 MW-2 MW-4 BG-1
Stations
0
1
2
3
4
5
6
7
8K
(m
g/l)
H
H
H
H
H
H
H
H
H
H
75th Percentile
Median
25th Percentile
95th Percentile
5th Percentile
H
H
Max.
Min.
75th Percentile
Median
25th Percentile
95th Percentile
5th Percentile
H
H
Max.
Min.
MW-1 MW-3 MW-2 MW-4 BG-1
Stations
120
130
140
150
160
170
180
190
200
Na
(m
g/l)
H
H
H
H
H
H
H
H
H
H
75th Percentile
Median
25th Percentile
95th Percentile
5th Percentile
H
H
Max.
Min.
75th Percentile
Median
25th Percentile
95th Percentile
5th Percentile
H
H
Max.
Min.
28
Figure 2.10 Spatial variability of Fe, Ba, Mn and Sr during baseline sampling
4.3.4. Dissolved gases (oxidation-reduction potential, ammonia, ferrous iron, sulfate,
hydrogen sulfide, methane, carbon dioxide)
Methane was detected during each sampling event for all wells at levels ranging from
0.01 to 1.9 mg/L. Ammonia concentrations were consistently detected at values ranging from
0.16 to 0.5 mg/L, averaging 0.34 mg/L. Hydrogen sulfide was detected at concentrations up to
4.8 mg/L, but was generally not present above the method detection limit of 1.1 mg/L.
Laboratory-measured dissolved CO2 concentrations ranged from 9 to 120 mg/L, averaging 72
mg/L. Well MW-1 typically exhibited higher dissolved CO2 concentrations than the other wells,
while wells BG-1 and MW-3 exhibited the lowest dissolved CO2 concentrations
MW-1 MW-3 MW-2 MW-4 BG-1
Stations
0.0
0.1
0.2
0.3
0.4
0.5
0.6
0.7
0.8
0.9F
e (
mg
/l)
H
H
H
H
H
H
H
H
H
H
75th Percentile
Median
25th Percentile
95th Percentile
5th Percentile
H
H
Max.
Min.
75th Percentile
Median
25th Percentile
95th Percentile
5th Percentile
H
H
Max.
Min.
MW-1 MW-3 MW-2 MW-4 BG-1
Stations
0.00
0.02
0.05
0.07
0.10
0.12
Mn
(m
g/l)
H
H
H
H
H
H
H
H
H
H
75th Percentile
Median
25th Percentile
95th Percentile
5th Percentile
H
H
Max.
Min.
75th Percentile
Median
25th Percentile
95th Percentile
5th Percentile
H
H
Max.
Min.
MW-1 MW-3 MW-2 MW-4 BG-1
Stations
0.00
0.02
0.05
0.07
0.10
0.12
Ba
(m
g/l)
H
H
H
H
H
H
H
H
H
H
75th Percentile
Median
25th Percentile
95th Percentile
5th Percentile
H
H
Max.
Min.
75th Percentile
Median
25th Percentile
95th Percentile
5th Percentile
H
H
Max.
Min.
MW-1 MW-3 MW-2 MW-4 BG-1
Stations
0.0
0.1
0.2
0.3
0.4S
r (m
g/l)
H
HH
H
H
H
H
H
HH
75th Percentile
Median
25th Percentile
95th Percentile
5th Percentile
H
H
Max.
Min.
75th Percentile
Median
25th Percentile
95th Percentile
5th Percentile
H
H
Max.
Min.
29
Figure 2.11 Spatial variability of SO4 during baseline sampling
4.3.4. Data correlations
Correlation coefficients (r2) were calculated for data pairs spanning field parameters,
major ions, minor ions and trace elements from all wells. The highest positive correlation was
observed for lithium and potassium (r2 = 0.87). Other data pairs exhibiting positive correlation
(r2 > 0.5) included Ca vs Mg (r
2 = 0.67), Mg vs Mn (r
2 = 0.67), Mn vs Fe (r
2 = 0.71), Ba vs Ca (r
2
= 0.504), Ba vs Mg (r2 = 0.675), Ba vs Mn (r
2 = 0.669), Sr vs Ba (r
2 = 0.594), and Sr vs Ca (r
2 =
0.717). Negatively correlated data pairs (r2 < -0.5) included Fe vs K (r
2 = -0.543), pH vs CO2 (r
2
= -0.636), Li vs CO2 (r2 = -0.607), and K vs CO2 (r
2 = -0.584).
MW-1 MW-3 MW-2 MW-4 BG-1
Stations
0
1
2
3
4S
O4
(m
g/l)
H
H
H
H
H
H
H
H
H
H
75th Percentile
Median
25th Percentile
95th Percentile
5th Percentile
H
H
Max.
Min.
75th Percentile
Median
25th Percentile
95th Percentile
5th Percentile
H
H
Max.
Min.
30
Table 2.5 Summary of trace element data during baseline sampling
Chapter 3 Parameter Units
Chapter 4 Baseline
Range
Chapter 5 Mean
Ag mg/L <0.00025 <0.00025
As mg/L <0.0013 <0.0013
Be mg/L <0.00025 <0.00025
Cd mg/L <0.000095 <0.000095
Co mg/L <0.00015 <0.00015
Cr mg/L <0.0025-0.007 <0.0025
Cu mg/L <0.0011 <0.0011
Hg mg/L <0.00007 <0.00007
Mo mg/L 0.002-0.013 0.005
Ni mg/L <0.002-0.037 0.002
Pb mg/L <0.0002-0.0009 <0.0002
Sb mg/L <0.0023-0.003 <0.0023
Se mg/L <0.001-0.001 <0.001
Tl mg/L <0.0005 <0.0005
Zn mg/L <0.0083-0.028 <0.0083
4.3.5. Data correlations
Data were also investigated for pH-dependence using correlation coefficients.
Potassium and lithium concentrations each exhibited pH-dependence, particularly above pH of
approximately 7.9, with correlation coefficients of 0.61 and 0.62, respectively. No other
parameters exhibited significant pH-dependence (-0.5 > r2 > 0.5).
31
Noticeable differences in the pH, and K and Li concentrations in wells BG-1 and MW-3,
compared to the other wells, created concern that non-representative samples from these two
wells may have resulted from well construction or sampling. After eliminating well MW-3 and
well BG-1 data, no correlations with pH or dissolved CO2 were observed for any parameter, and
the r2 value for the data pair Li vs K decreased from 0.87 to 0.46. The highest correlation from
the edited data pool was between Ca and Sr, with r2 = 0.87. Potassium showed a strengthened
correlation with Ca, Mg, Mn, Ba, and Sr, with r2 > 0.65 for all pairs. In general, the correlations
between major and minor cation data pairs Ca, Mg, K, Na, Sr, Ba, Fe, and Mn were strengthened
in the edited data pool.
4.3.6. Mineral saturation indices
Groundwater saturation indices were calculated for carbonates, sulfate, sulfides,
oxides/oxyhydroxides and silicates using PHREEQC (wateq4f.dat thermodynamic database).
Groundwater saturation indices for sulfates, carbonates and sulfides are illustrated in Figure 2.12.
Groundwater samples were undersaturated with respect to all sulfate minerals, but highly
supersaturated with respect to pyrite and greigite (Fe3S4), and near saturation or slightly
supersaturated with respect to amorphous FeS(am) and mackinawite (FeStet). While the average
saturation index (S.I.) values for all carbonate minerals, except siderite (FeCO3), indicate
undersaturation, the maximum calculated saturation indices for these phases (except strontianite
and witherite) suggest that carbonate equilibrium or precipitation is theoretically possible.
However, with the exceptions of siderite and rhodochrosite, the majority of samples collected
during the baseline period indicate a tendency toward carbonate dissolution (Figure 2.13).
32
Figure 2.12 Groundwater sulfate, carbonate, and sulfide saturation indices box-and-whisker
plots (triangle indicates the average and vertical bars represent maximum and minimum values).
-1.2
-4.1
-7.0
-4.3
-6.7
-5.3
-7.2
-3.5
-6.5
-9.3
-6.8
-14.8
-11.8
-13.7
-2.3
-5.2
-8.0
-5.5
-11.3
-8.6
-10.6
-16.0
-14.0
-12.0
-10.0
-8.0
-6.0
-4.0
-2.0
0.0
Barite Celestite Epsomite Gypsum Alunite Jarosite-K Jarosite-Na
Satu
rati
on
In
de
x
0.20.1
0.4
-0.4
0.2
0.9
-0.7
-1.9
-1.1-1.2
-2.2
-1.7
-0.5
-0.9
-2.1
-3.2
-0.6-0.8
-1.3 -1.2
-0.1
0.4
-1.6
-2.7
-3.5
-3.0
-2.5
-2.0
-1.5
-1.0
-0.5
0.0
0.5
1.0
1.5
Calcite Aragonite Dolomite Magnesite Rhodochrosite Siderite Strontianite Witherite
Satu
rati
on
In
de
x
Sulfates
Carbonates
10.52
1.73
20.65
2.46
8.21
0.03
15.85
0.76
9.89
1.30
19.20
2.03
-2.0
0.0
2.0
4.0
6.0
8.0
10.0
12.0
14.0
16.0
18.0
20.0
22.0
Pyrite FeS(ppt) Greigite Mackinawite
Satu
rati
on
In
de
x
Sulfides
33
Figure 2.13. Histograms of groundwater carbonate mineral saturation indices.
Of the metal oxides and oxyhydroxides, groundwater samples were undersaturated with
respect to Mn-bearing phases, and supersaturated with respect to Fe-bearing phases. Fe(OH)3(am)
was the closest to equilibrium of the Fe-bearing oxides/oxyhydroxides. Samples were near
equilibrium with boehmite and gibbsite, undersaturated with respect to Al(OH)3(am) and
0%
10%
20%
30%
40%
50%
60%
70%
80%
90%
100%
0
5
10
15
20
25
30
-1 -0.75 -0.5 -0.25 0 0.25 More
Fre
qu
en
cy
Bin
Frequency
Cumulative %
0%
10%
20%
30%
40%
50%
60%
70%
80%
90%
100%
0
5
10
15
20
25
-2 -1.5 -1 -0.5 0 0.5 More
Fre
qu
en
cy
Bin
Frequency
Cumulative %
0%
10%
20%
30%
40%
50%
60%
70%
80%
90%
100%
0
5
10
15
20
25
30
Fre
qu
en
cy
Bin
Frequency
Cumulative %
0%
10%
20%
30%
40%
50%
60%
70%
80%
90%
100%
0
5
10
15
20
25
30
35
40
45
Fre
qu
en
cy
Bin
Frequency
Cumulative %
CaCO3 CaMg(CO3)2
FeCO3MnCO3
0%
10%
20%
30%
40%
50%
60%
70%
80%
90%
100%
0
5
10
15
20
25
Fre
qu
en
cy
Bin
Frequency
Cumulative %
SrCO3
0%
10%
20%
30%
40%
50%
60%
70%
80%
90%
100%
0
5
10
15
20
25
30
35
Fre
qu
en
cy
Bin
Frequency
Cumulative %
BaCO3
34
supersaturated with respect to diaspore. Silicate mineral saturation indices are shown in Figure
2.14. Of the silicates identified in aquifer sediments by XRD, S.I. values indicate that
groundwater is near chemical equilibrium to slightly supersaturated with respect to illite, while
potassium feldspar and sodium feldspar show a thermodynamic tendency to dissolve (Figure
2.15).
Figure 2.14. Groundwater aluminum, iron, and manganese oxyhydroxide mineral saturation
indices box-and-whisker plots.
-1.5
0.7
2.4
1.2
-2.6
-0.4
1.3
0.1
-2.0
0.2
1.9
0.7
-3.0
-2.0
-1.0
0.0
1.0
2.0
3.0
Al(OH)3(am) Boehmite Diaspore Gibbsite
Satu
rati
on
In
de
x
2.8
19.2
9.0
21.6
1.8
17.1
6.9
19.0
2.3
18.3
8.1
20.4
0.0
5.0
10.0
15.0
20.0
25.0
Fe(OH)3(am) Hematite Maghemite Magnetite
Satu
rati
on
In
de
x
-8.2
-5.6
-2.6
-5.1-6.0
-15.5 -15.2
-6.5 -6.8
-13.6-13.4 -12.9
-5.6 -5.9
-11.6
-18.0
-16.0
-14.0
-12.0
-10.0
-8.0
-6.0
-4.0
-2.0
0.0
Birnessite Hausmannite Manganite Pyrochroite Pyrolusite
Satu
rati
on
In
de
x
Al-oxyhydroxides
Fe-oxyhydroxides
Mn-oxyhydroxides
35
Figure 2.15. Groundwater silicate mineral saturation indices box-and-whisker plots.
-0.2-1.1
-2.7
-6.7
-3.7
2.31.2
-1.0
-2.2-1.5
-6.3
5.7
-1.2
1.3
-1.1-1.6
-3.1
-14.8
-4.4
-0.4
-9.8-8.9
-4.8
-6.8
-11.6
-1.9
-3.7
-0.2-0.6
-1.3
-2.9
-11.3
-4.2
1.1
-6.1 -6.0
-3.9-4.8
-9.7
1.8
-2.3
0.5
-20.0
-15.0
-10.0
-5.0
0.0
5.0
10.0Sa
tura
tio
n I
nd
ex
3.9
7.6
0.2
8.3
2.2
4.1
-0.2
-2.9 -2.5
6.6
-4.2
2.2
3.9
1.4
5.4
-0.7
6.5
-0.4
3.4
-1.0
-11.0
-5.6
4.3
-9.1
-5.5
-14.4
2.8
6.4
-0.2
7.5
1.1
3.7
-0.6
-8.1
-4.5
5.5
-7.2
-2.7
-7.5
-20.0
-15.0
-10.0
-5.0
0.0
5.0
10.0
Satu
rati
on
In
de
x
Silicates (a)
Silicates (b)
36
5. Discussion
5.1. Hydraulic conductivity regional comparison
The range of hydraulic conductivity (Kh) estimates (40-45 ft/day) produced for the study
site are similar to reported median values for the Graham Ferry Formation in Jackson County,
Mississippi, of 50 ft/day. Sumner et al. (1987), in a study simulating effects of groundwater
withdrawals on the Miocene aquifer system in Mississippi, reported model-derived Kh values for
the Graham Ferry aquifer of 30 ft/day, in close agreement with measured values at the study site.
Higher median Kh values in the Graham Ferry aquifer of 102 and 110 ft/day were reported for
Hancock and Harrison Counties, respectively, immediately west of Jackson County. Hydraulic
conductivity measurements reported statewide for the Graham Ferry aquifer range widely from
26 to 350 ft/day (Harvey et al., 1965).
Hydraulic conductivity values for unconsolidated sediments can be estimated based on
grain size distribution (Vukovic and Soro, 1992). When viewed in context of the aquifer
sediment grain size, the measured hydraulic conductivity at the test site falls within the range of
values reported for predominantly medium-grained sand aquifers or mixed sand-and-gravel
aquifers, but above the range expected for fine-grained sands (Figure 2.16), suggesting that a
simplistic estimation of aquifer hydraulic conductivity based on sediment grain size
classification alone is inadequate for this setting.
37
Figure 2.16. Hydraulic conductivity measurements of the current study, for the Graham Ferry
aquifer and other Gulf Coast aquifers, and values estimated for typical sediment grain size
classifications.
In fact, Hazen’s approximation, where K is approximated based on the effective grain
size (d10), significantly underestimates hydraulic conductivity at the test site. Using Hazen’s
approximation:
K = C(d10)2
where K is the hydraulic conductivity (cm/s), C is a coefficient based on grain size and sorting
characteristics, and d10 is the effective grain size (cm), the average hydraulic conductivity for the
site equates to 0.006 cm/s, or 18.1 ft/day (using a C value of 100 for well-sorted medium sand).
One possible explanation for the disagreement between effective grain size and estimated
hydraulic conductivity is the impact of textural maturity, as described by Shepherd (1989).
Shepherd (1989) derived the relationship:
0.01
0.1
1
10
100
1000
Sand and Gravel
Mixes
Coarse Sand Medium Sand Fine Sand Gulf Coast Aquifer
Systems
Graham Ferry
Aquifer Mississippi
Ho
rizo
nta
l Hyd
rau
lic C
on
du
ctiv
ity
(ft/
day
)
Current Study
38
K = Cd50j
where K is estimated hydraulic conductivity, C is a shape factor, d50 is the mean grain size (mm),
and j is an exponent. Values measured at the current study are in closer agreement with
Shepherd’s relationship derived for channel deposits (31.5 ft/day using K = 450*d501.65
), as
opposed to beach deposits (95.3 ft/day using K=1,600*d501.75
). However, the range of hydraulic
conductivity estimates derived using the method of Shepherd (1989), using assumptions of beach
deposits and channel deposits, produces the range of observed measured values in the Graham
Ferry across Mississippi (approximately 30 to 100 ft/day). In fact, Harvey et al. (1965) attributed
major spatial differences in measured transmissibility in the Graham Ferry in Mississippi to
textural variability.
5.2. Regional groundwater quality comparison and historical evolution
MDEQ (2013) reviewed groundwater quality for various potable aquifers in Mississippi,
including thirty measurements of major cation and anion concentrations for the Miocene aquifer
system (summarized in Table 2.6). Minor and trace element data were not reported. The
Miocene aquifer groundwater is characterized by highly variable conductivity measurements,
ranging from 22 to 1,650 mhos/cm. Overall, the major ion concentrations measured for
groundwater at the test site are within the range of values previously reported for the Miocene
aquifer system (MDEQ 2013). Mean values reported for the datasets are not similar, with the
exception of pH and silicon concentration. This similarity is reasonable given that the aquifers
are generally composed of silica sand with minor carbonates, which act to provide solubility
control (silica) or buffer acidity (pH) in the aquifer.
39
Table 2.6. Groundwater major ion concentrations measured in the current study and previously
reported for the Miocene aquifer system in Mississippi (MDEQ 2013).
Parameter Unit Current Study Miocene,
MDEQ (2013)
Range Mean Range Mean
Conductivity mhos/cm 617-692 654 22-1,650 353
pH s.u. 7.36-8.69 7.89 5.6-9.0 7.26
Ca mg/l 2.0-4.2 2.8 0.5-94 10.98
Mg mg/l 0.81-1.9 1.26 0.1-46 4.19
Na mg/l 140-190 157 1.7-380 65
K mg/l 1.8-7.6 3.1 0.5-5.2 1.55
Si mg/l 8.4-13 11.7 4.4-29 11.7
Fe mg/l 0.05-0.89 0.53 0.01-0.35 0.05
Cl mg/l 21-30 26 0.4-380 5.1
HCO3 mg/l 239-326 297 6-564 115
SO4 mg/l <0.008-3.4 0.577 0.2-63 9.6
F mg/l 0.3-0.6 0.45 0.1-1.4 0.2
NO3 mg/l <0.0065-0.034 0.011 0.1-4.2 0.15
At least 5 major geochemical processes are believed to affect water chemistry along the
United States Gulf coast: 1) leaching of soluble salts from the unsaturated zone, 2) alteration of
albite, 3) cation exchange, 4) mixing of water by the vertical flow of water from underlying units
and 5) the dissolution of halite from salt diapirs (Pettijohn, 1996). A viable approach to
interpreting present-day groundwater quality at the test site and in the region is to view the data
in the context of aquifer freshening (Appelo, 1994). As illustrated in Figure 2.17, rainwater is
simulated to infiltrate a biologically active, calcite-containing soil zone and percolate into the
phreatic zone. The originally saline groundwater is freshened by the infiltrating rainwater,
creating a front of freshwater advancement toward the ocean. Major ion concentrations are
modified by simple mixing and chemical reactions. Compositional deviations from simple
mixing must be accounted for by chemical reactions such as cation exchange.
40
Figure 2.17. Conceptual model illustrating aquifer freshening of saline groundwater (X
represents the exchangeable mole fraction).
In order to illustrate that a geochemical process which is thought to be regionally
dominant in determining major ion chemistry is also active at the test site, two modeling
scenarios were simulated. In the simplest case, PHREEQC mixing of rainwater and seawater
results in a much lower predicted groundwater sodium concentration than exists in the present-
day aquifer (Figure 2.18). At the time when the present-day chloride concentration (28 mg/L) is
achieved by simple mixing, the sodium concentration is predicted to be approximately 10 times
lower than the present-day concentration of 150 mg/L. The simple mixing model results in a
deficit of sodium and a surplus of calcium when compared to present-day chemical composition.
Therefore, chemical reactions must play a role in determining both groundwater sodium and
bicarbonate concentrations over time.
Recharge
Rainwater modified by the vadose zoneenvironment
Seawater in equilibrium with theaquifer matrix
WellOcean
2Na-X + Ca2+ = 2Na+ + Ca-X2
41
Figure 2.18. Results of a simple PHREEQC rainwater-saline water mixing model showing
trends in groundwater major ion concentrations over time during aquifer freshening.
PHREEQC simulations were run to evaluate the effects of aquifer freshening (rainwater
equilibrated with vadose zone calcite and atmospheric PCO2) on an aquifer medium with cation
exchange sites originally saturated with seawater. Because it is unlikely that illite was originally
present in the aquifer sediments, the simulation included Ca-montmorillonite, calcite, and
potassium feldspar as present initially, with illite allowed to precipitate as it exceeded saturation.
Under these conditions, both Na+ and HCO3
- concentrations are predicted more accurately using
the cation exchange model than through simple mixing (Figure 2.19). The disagreement
between measured and predicted SO42-
concentrations (i.e., more predicted SO42-
than is actually
present) could be due to microbial sulfate reduction in the aquifer, producing the sulfides
observed through XRD and SEM analyses.
0.1
1
10
100
1000
10000
100000
0 5 10 15 20 25 30 35 40
Dis
solv
ed C
on
cen
trat
ion
(m
g/L
)
Step
Cl
Na
Ca
Mg
HCO3
K
SO4
Cl = 26 mg/L
Present-Day Based on Chloride Concentration
Measured Modeledmg/L mg/L
Na 157 15K 1.5 0.5Ca 1.6 118
Mg 1.2 2HCO3 297 361
SO4 <1 5Cl (fixed) 26 26
42
Figure 2.19. Aquifer freshening trends of groundwater major ion concentrations modeled using
PHREEQC and incorporating ion exhange (Exchangeable mole fraction (X) = 0.03; Ca-
montmorillonite, calcite, and K-feldspar allowed to dissolve and illite allowed to precipitate).
Chowdhury et al. (2006) report supporting evidence that aquifer freshening and cation
exchange play a dominant role in determining major ion composition of the Texas Gulf Coast
Aquifer system. In particular, plots of excess sodium from sources other than halite and excess
calcium and magnesium from sources other than gypsum and carbonate showed nearly perfect
correlations (R2>0.95 for all Texas Gulf Coast Aquifers), and molar ratios of excess sodium
relative to depletions of calcium and magnesium of approximately 2 (Figure 2.20). This ratio is
indicative of an ion exchange reaction where calcium and magnesium are displacing sodium into
solution.
0.1
1
10
100
1000
10000
100000
0 5 10 15 20 25 30 35 40
Dis
solv
ed C
on
cen
trat
ion
(m
g/L
)
Step
Cl
Na
Ca
Mg
HCO3
K
SO4
Cl = 26 mg/L
Present-Day Based on Chloride Concentration
Measured Modeledmg/L mg/L
Na 157 160K 1.5 3.1Ca 1.6 2.8
Mg 1.2 1.2HCO3 297 340
SO4 <1 5Cl (fixed) 26 26
43
Nearly the exact same relationship is observed data reported for the Miocene aquifer system in
Mississippi (MDEQ, 2013), suggesting that aquifer freshening and cation exchange could be
dominant processes affecting major ion water quality not only at the study site, but in sandy
aquifers of the Gulf Coast region.
Figure 2.20 Plot illustrating relationship between excess sodium and depletions in Ca+Mg in the
Miocene aquifer in Mississippi and similarity to the Texas Gulf Coast.
5.3. Groundwater pH and PCO2
Biological processes often produce CO2 as a reaction by-product (Langmuir, 1997)
(Table 2.7). The degree of CO2 supersaturation relative to atmospheric values, or PCO2 groundwater /
PCO2 atmosphere, is a useful indicator parameter to quantify the degree of biological activity
occurring in an aquifer. A ratio of 1 indicates atmospheric equilibrium and values >1 indicate
Miocene in Mississippi:y = -2.111x + 0.1834
R² = 0.8364
-2
0
2
4
6
8
10
12
-5 -4 -3 -2 -1 0 1
Na -
Cl (m
mo
l/L
)
Ca + Mg - SO4 - 0.5*HCO3 (mmol/L)
Chowdhury et al. (2006):y = -1.842x - 0.16 R2 = 0.98
44
CO2 overpressures. It is generally accepted that groundwater and, to a lesser extent, surface
water are potential net sources of CO2 to the atmosphere (Langmuir, 1997).
Table 2.7. Typical CO2-generating reactions in groundwater systems.
Process Reaction
Aerobic respiration and decay 1/6C6H12O6 + O2 CO2 + H2O
Nitrate uptake and reduction NO3- + 2H
+ + 2CH2O NH4
+ + 2CO2 + H2O
Denitrification 5CH2O + 4NO3- + 4H
+ 5CO2 + 2N2 + 7H2O
Sulfate reduction 2CH2O + SO42-
+ H+ 2CO2 + HS
- + 2H2O
Methane fermentation C6H12O6 3CH4 + H2O + CO2
*After Langmuir (1997)
At the test site, the lowest pH values are indicative of aquifer CO2 supersaturation states
of up to 28 times the atmospheric value (Figure 2.21), suggesting that biological activity makes
the aquifer a potential net source of CO2 to the atmosphere. If true, then degassing of CO2
during groundwater sampling (which involves depressurization and possible gas exchange) is a
concern for proper design of an experiment intended to monitor the purposeful introduction of
CO2 to the aquifer. Figure 2.22 illustrates the statistical distribution of pH measurements taken
during the baseline study period. The presence of the tail on the right side of the statistical
distribution of pH measurements may indicate the relative ease of CO2 degassing and subsequent
pH rise (producing a right tail). In contrast, a mechanism to produce lower pH results than in situ
conditions is lacking, explaining the absence of a left-side tail.
45
Figure 2.21. Relationship between pH and degree of CO2 supersaturation in groundwater,
showing a higher degree of supersaturation at lower pH.
Figure 2.22. Histogram of groundwater pH measurements during the baseline study period.
7.2
7.4
7.6
7.8
8.0
8.2
8.4
8.6
8.8
0 5 10 15 20 25 30
pH
PCO2 groundwater / PCO2 atmosphere
0%
10%
20%
30%
40%
50%
60%
70%
80%
90%
100%
0
5
10
15
20
25
30
7 7.25 7.5 7.75 8 8.25 8.5 8.75 9 More
Fre
qu
en
cy
Bin
Frequency
Cumulative %
46
5.4. Groundwater redox conditions and Eh
The persistent detection of measureable methane and ammonia, and the occasional
detection of hydrogen sulfide in groundwater samples, suggest a chemically reducing
environment in the aquifer. Under equilibrium conditions, methanogenesis occurs after a
sequence of biologically-driven redox reactions. When an organic carbon source is present in
groundwater, aerobic decay will proceed until all dissolved oxygen is depleted. After available
oxygen is consumed, anaerobic processes (reduction of MnO2 to Mn2+
, NO3- reduction to NO2,
reduction of Fe3+
to Fe2+
, reduction of SO42-
to HS-, and reduction of HCO3
- to CH4) dominate.
These reactions will generally proceed in the order as listed above, as the redox potential
becomes more negative, but will only occur in the presence of solute sources to the groundwater,
such as minerals, gases or anthropogenic inputs. For example, methanogenesis may occur in the
absence of SO42-
reduction, if there is no source of dissolved SO42-
to the groundwater (Appelo
and Postma, 1999).
The presence of dissolved ferric iron in a methanogenic environment, in addition to other
measurements, suggests a condition of redox disequilibrium. To be at equilibrium, a system
producing methane gas would have progressed through complete reduction of ferric to ferrous
iron, either in dissolved or mineralized form. Comparing all measured Eh values to those
calculated using redox pairs for Fe, S, and C suggests that the higher measured Eh values may be
reflective of the Fe2+
/Fe(OH)3 redox couple while the lower measured values may be reflective
of the SO42-
/FeS2 redox couple (Figure 2.23).
47
Figure 2.23. Relationship between measured Eh values and Eh calculated using measured
concentrations of redox pairs.
This redox disequilibrium could be an artifact of sampling and analytical procedures,
including the measurement of Eh itself. Field measurements can represent mixed potentials of
various active redox couples (Langmuir, 1997; US EPA, 2002), which may result when a species
is present in too low a concentration to create a significant current flow at the measuring
electrode. Langmuir (1997) asserts that thermodynamically-meaningful Eh measurements may
be possible in groundwater containing elevated concentrations of dissolved Fe, Mn, and H2S, but
are often not possible in groundwater where C, N, O, H, and oxidized S are the dominant redox-
sensitive elements.
A sequence of chemical reactions through time may explain the current state of redox
disequilibrium (Figure 2.24). The sequence assumes that the Graham Ferry sediments were
-400
-350
-300
-250
-200
-150
-100
-50
0
50
-400 -350 -300 -250 -200 -150 -100 -50 0 50
Cal
cula
ted
Eh
(m
V)
Measured Eh (mV)
HCO3-/CH4(aq) SO42-/FeS2 Fe(OH)3/Fe2
48
originally deposited in a marine or nearshore environment (Stage 1), and were primarily
composed of organic material, quartz, feldspars, clays, and calcite. Extended periods of burial
and atmospheric isolation (Stage 2) led to anoxic conditions, reduction of dissolved iron and
sulfate, and subsequent precipitation of FeS(m). A period of atmospheric exposure (Stage 3),
possibly related to sea level fall, led to sulfide oxidation, iron oxyhydroxide precipitation,
gypsum precipitation, and calcite dissolution. Incomplete oxidation of ferrous iron could have
resulted in the precipitation of siderite during this stage. Resubmergence of the sediments (Stage
4), potentially due to sea level rise, isolated this mineral assemblage under anoxic conditions,
leading to another phase of sulfide (possibly pyrite) precipitation. The net reaction for the
process during exposure and oxidation is:
(4) FeS2(cry) + 3.5O2 + CaCO3 + Fe2+
+ 3H2O = FeCO3 +
CaSO4:2H2O + Fe(OH)3(s) + SO42-
+ 5H+ + e
-
Groundwater saturation indices suggest thermodynamic equilibrium with FeS, rather than
crystalline FeS2, although pyrite was detected with XRD. Groundwater is highly supersaturated
with respect to pyrite, suggesting that pyrite may be currently forming from amorphous sulfides.
In summary, the groundwater does not appear to be in redox equilibrium with the aquifer
mineralogy, suggesting a dynamic chemical system. The interpretation provided, however,
allows for a phased progression toward present-day conditions which relies on the assumption
that sediments were deposited, exposed to the atmosphere, and then reburied and isolated from
the atmosphere. This type of sequence can occur in a transgressive-regressive sedimentation
cycle which would be typical of coastal environments during the Miocene-Pliocene.
49
Figure 2.24. Possible stages of geochemical evolution of the study site aquifer over geologic
time (FeS(m) = mackinawite).
6. Conclusions
This chapter reviewed the results of a baseline aquifer testing program conducted at the
Plant Daniel study site in Pascagoula, MS. The purpose of the testing program was to produce
physical and chemical data necessary to design, implement and interpret a controlled-release
field test evaluating impacts of elevated PCO2 on aquifer water quality at the Plant Daniel site.
Stage 1 –Deposition Stage 2 – Burial/Anoxic
Stage 3 – Exposure/Oxidation Stage 4 – Reburial/Anoxic
Calcite
Quartz/Feldspars/Clays
FeS
Calcite
Quartz/Feldspars/Clays
CaCO3 + H+ = Ca2+ + HCO3-
FeS(m) + 3.5 O2 + H2O = Fe2+ + SO42- + 2 H+
Quartz/Feldspars/Clays Quartz/Feldspars/Clays
Ca2+ + SO42- + 2H2O = CaSO4:2H2O
Gypsum
Calcite?
FeS FeS
FeS2
Calcite?
Deposits primarily calcite,quartz, feldspars, clays
Fe2+ + HS- = FeS(m) + H+
Fe2+ + CO32-= FeCO3
Siderite
Gypsum
Siderite
Fe2+ + 2HS- = FeS2 + 2H+
50
Aquifer testing revealed hydraulic conductivity values that are typical for the Mississippi Gulf
Coast and provide the necessary data for flow modeling at the site. PHREEQC simulations
indicate that ion exchange reactions are important for understanding the evolution of dissolved
major ion composition of the site groundwater over geologic time and the possible anthropogenic
impacts from intrusion of CO2. The aquifer is chemically reducing, but due to stages of exposure
and reburial over time, measurements of dissolved redox indicators and aquifer mineralogy most
likely represent a state of redox disequilibrium. The aquifer media contains pyrite and clay
minerals, which are known to be susceptible to dissolution under acidic conditions. These
dissolution reactions are likely to promote ion exchange reactions in the event of acidification
due to elevated CO2. Due to similarities in the evolution of Gulf Coast aquifers over time, the
results of this particular study are believed to be relevant to other sites in the United States Gulf
Coast where opportunities exist for geologic sequestration of CO2.
51
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Publishers, Rotterdam, Netherlands. 536 p.
Appelo, C.A.J., 1994. Cation and proton exchange, pH variations, and carbonate reactions in a
freshening aquifer. Water Resources Research, Vol. 30. No. 10, pp. 2793-2805.
American Public Heath Association (APHA), 2012. Standard methods for the examination of
water and wastewater, 22nd
Edition. 724 p. ISBN 0875530133.
ASTM, 2007. ASTM D422-63. Standard Test Method for Particle-Size Analysis of Soils, ASTM
International, West Conshohocken, PA.
Bouwer, H. and Rice, R.C., 1976. A slug test method for determining hydraulic conductivity of
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Chowdhury. A.H, Boghici, R., and Hopkins, J., 2006. Hydrogeochemistry, Salinity Distribution,
and Trace Constituents: Implications for Salinity Sources, Geochemical Evolution, and Flow
Systems Characterization, Gulf Coast Aquifer, Texas. In Aquifers of the Gulf Coast of Texas.
Texas Water Development Board 365. February, 2006.
Harvey, E.J., H.G. Golden and H.G. Jeffery, 1965. Water Resources of the Pascagoula Area
Mississippi. United States Geological Survey Water-Supply Paper 1763. 144 p.
Hvorslev, M.J., 1951. Time Lag and Soil Permeability in Ground-Water Observations, Bull. No.
36, Waterways Experimental. Station Corps of Engineers, U.S. Army, Vicksburg,
Mississippi, pp. 1-50.
HydroSOLVE, Inc., 2006. AQTESOLV Version 4.0 Professional. HydroSOLVE, Inc. Reston,
Virginia.
Langmuir, D., 1997. Aqueous Environmental Geochemistry. Prentice-Hall, NJ. 600 p.
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MDEQ, 2000. Ground-water study of historical water-level and water-quality data in Jackson
County, Mississippi. Open-file report 99-102. May 1999. Revised February 2000.
MDEQ, 2013. State of Mississippi Groundwater Quality Assessment. Available online at
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b2013/$FILE/305b_2013.pdf?OpenElement.
52
Pettijohn, R.A., 1996. Geochemistry of ground-water in the Gulf Coast aquifer systems, south-
central United States: U.S. Geological Survey Water-Resources Investigations Report 96-
4107,158 p.
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November 18, 2013. http://www.secarbon.org/files/2008-11-newsletter.pdf
Shepard, R.G.,1989. Correlations of permeability and grain size. Ground Water, Vol. 27, No. 5,
pp. 633-638.
Sumner, D.M., B. E. Wasson, and S.J. Kalkhoff, 1987. Geohydrology and simulated effects of
withdrawals on the Miocene aquifer system in the Mississippi Gulf Coast area. United
States Geological Survey Water Resources Investigations Report 87-4172.
Trautz, R.C., J.D. Pugh, C. Varadharajan, L. Zheng, M. Bianchi, P. S. Nico, N. F. Spycher, D. L.
Newell, R. A. Esposito, Y. Wu, B. Dafflon, S. S. Hubbard, and J. T. Birkholzer, 2013.
Effect of Dissolved CO2 on a Shallow Groundwater System: A Controlled Release Field
Experiment. Environmental Science and Technology. 47, 298−30
TestAmerica, 2014. TestAmerica, Inc. Standard Operating Procedure, VFA.
UA EPA, 2004. EPA RSKSOP-175 Sample Prep And Calculations For Dissolved Gas Analysis
In Water Samples Using A GC Headspace Equilibration Technique, rev 2, pp. 14.
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Digester AA II), pp. 5.
US EPA, 1994. Methods for the determination of metals in environmental samples. Supplement
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US EPA, 1994. EPA Method 7470A. Mercury in liquid waste (manual cold-vapor technique). 6
pp.
US EPA, 1996. Low stress (low flow) purging and sampling procedure for the collection of
groundwater samples from monitoring wells. EQASOP-GW 001. Revised 2010.
US EPA, 2002. Workshop on monitoring oxidation-reduction processes for ground-water
restoration. EPA/600/R-02/002. January 2002.
Varadharajan, C., Tinnacher, R. M., Pugh, J. D., Trautz, R. C., Zheng, L., Spycher, N. F.,
Birkholzer, J. T., Castillo-Michel, H., Bianchi, M., Esposito, R. A., and Nico, P. S. 2013.
A laboratory study of the initial effects of dissolved carbon dioxide (CO2) on metal
release from shallow sediments. International Journal of Greenhouse Gas Control., Vol.
19. pp. 183-211.
Vukovic, M. and A. Soro, 1992. Determination of hydraulic conductivity of porous media from
grain-size composition. Water Resources Publications, Littleton, Colorado, 83 p.
53
Chapter 3
DESIGN AND IMPLEMENTATION OF A FIELD EXPERIMENT EVALUATING IMPACTS
OF CO2 LEAKAGE INTO A CONFINED AQUIFER
Abstract
Geologic carbon sequestration operated at full-scale will require extensive performance
monitoring, including potable groundwater monitoring. However, researchers and regulators do
not fully understand what impact elevated CO2 levels would have on groundwater quality in the
event that CO2 should leak into an overlying aquifer. One way to understand the impacts of CO2
leakage is to perform a field simulation of the leakage scenario and measure the impacts. The
critical aspects of the design and implementation are the ability to control experimental
conditions in the field (e.g., pressure, temperature, redox) and be able to detect responses to the
disturbance (e.g., hydraulic control, downhole pH, conductivity) with enough confidence to
support conclusions and modeled predictions related to CO2-induced groundwater quality
impacts (e.g., trace element mobilization). This study presents the design and implementation of
a closed loop pumping and injection system designed to simulate CO2 leakage into a test site
aquifer. Process monitoring results indicated that the test was performed with minimal variation
in key process parameters, including temperature, pressure and injectate pH. In situ
instrumentation deployed in monitoring wells allowed continuous readings of groundwater pH
and conductivity, which were critical parameters for evaluating the aquifer response to
carbonation and acidification. Successful modeling simulation of the pH response using results
from the aquifer testing program suggested that the test was implemented and monitored
54
appropriately and that that future data interpretations and modeling of the field experiment were
not compromised by test design.
1. Introduction
Geologic carbon sequestration operated at full-scale will require extensive performance
monitoring, including potable groundwater monitoring (EPA, 2010). However, researchers and
regulators currently do not fully understand what impact elevated CO2 levels would have on
groundwater quality in the event that CO2 should leak into an overlying aquifer. Furthermore,
coupled geochemical and transport models which have been verified by field data are limited,
making predictive modeling of CO2 impacts highly uncertain. This knowledge gap ultimately
makes it difficult to develop a truly effective aquifer monitoring plan.
To address this knowledge gap, the Electric Power Research Institute (EPRI) funded two
field experiments evaluating the impacts of PCO2 on aquifer water quality. EPRI (2008) injected
CO2 into a shallow, unconfined aquifer system in Montana and observed a decrease in
groundwater pH – from pH 7 to 6 – and increased bicarbonate, calcium, and magnesium
concentrations. The study was ultimately difficult to model with coupled flow and transport
codes, due to the occurrence of gas exsolution from the aquifer into the vadose zone and
subsequent redissolution of CO2 into the water table further down-gradient. Recognizing these
limitations, a second field experiment, the subject of this chapter, was conducted in a more
controlled hydrogeologic setting, in an effort to simulate a leak of CO2 into a shallow aquifer and
observe the effects on water quality. To accomplish this, thorough aquifer characterization and
planning were conducted to ensure that test results and interpretive modeling efforts were highly
defensible.
55
The purpose of this chapter is to describe the design and implementation process for
simulating a leakage of CO2 into the second EPRI test site aquifer in Pascagoula, MS. The
critical aspects of the design and implementation are the ability to control experimental
conditions in the field (e.g., pressure, temperature, redox) and detect responses to the disturbance
(e.g., hydraulic control, downhole pH, conductivity) with enough confidence to support
conclusions and modeled predictions related to CO2-induced groundwater quality impacts (e.g.,
trace element mobilization). Data from the above-ground process monitoring instrumentation
and monitoring wells are provided as a means to assess the project design success. It is expected
that the methodology described will be useful to other researchers planning to implement similar
evaluations at potential CO2 sequestration sites.
2. Methods
2.1. Well layout
Results of the 2010 hydrogeologic investigation (Chapter 2) were used to develop a
conceptual model of the test site, upon which relatively simple flow and transport models were
based (Trautz et al., 2013). These preliminary models described in Trautz et al. (2013) were used
to design the final well field (Figure 3.1), including the distance between wells and the final
injection and pumping rates (Table 3.1). A submersible pump was installed in well PW-1, and
designed to produce a continuous pumping rate of 22.7 liters per minutes (L/m). This was the
pumping rate determined that would produce a small hydraulic gradient between the injection
and observation wells, allowing and balance between timely execution of the test and minimizing
the velocity of the injected water so that mineral reactions could occur. The hydraulic gradient
56
between the two wells was increased slightly by pumping 22.7 L/m from well PW-1, discarding
17 L/m of groundwater to surface runoff, and supplying 5.7 L/m to the carbonation unit.
Figure 3.1. Well field layout.
Table 3.1. Well spacing distances and injection rates.
Description Well Designation Distance from
Well IW-1 (m)
Average Injection (+),
Withdrawal (-) Rates
(L/min)
Injection Well IW-1 0 +5.7
Monitoring Wells
MW-1 16.3 --
MW-2 12.8 --
MW-3 4.6 --
MW-4 20.0 --
Background Well BG-1 21.2 --
Pumping Well PW-1 63.4 -22.7
BG-1
IW-1MW-3
MW-4
PW-1
MW-1
MW-2
Background
Monitoring Well
Pumping Well
Injection
Well
Downgradient
Monitoring Wells
15 ftN
57
2.2. Pumping, piping, and carbonation system
The fluid delivery system was a critical component of the experiment that allowed
carbonated groundwater to be injected under pressure into the test interval at a depth of 46.9 to
54.6 m. The piping, pumping, and carbonation system was designed to ensure that line
pressurization and temperature would be maintained as close to aquifer conditions as feasible
during the test (Figure 3.2). A submersible Grundfos™ pump was installed in PW-1, and a
booster pump was installed at the ground surface at well PW-1. Groundwater was pumped from
the aquifer at the rate of 18.9 to 22.7 L/min from well PW-1. Approximately two-thirds of the
clean groundwater (17 L/m) was discharged to a surface water drain and the remaining one-third,
or 5.7 L/min, was pumped to the carbonation unit. The forced gradient between wells PW-1 and
IW-1 was used to control the shape and direction of the dissolved CO2 plume, allowing
carbonated groundwater to be drawn across the intervening monitoring wells where groundwater
samples were collected for further analysis. The temperature of the groundwater withdrawn
from the confined aquifer was maintained by using thermal insulation around all process piping.
The thermal insulation was wrapped in reflective tape so that heating from solar radiation was
minimized. A cartridge filter was installed between the supply pump and the carbonation unit to
remove any sediment from the groundwater before it entered the carbonation unit (Figure 3.3).
58
Figure 3.2 Site cross-section illustrating the injectate fluid delivery system.
The carbonation unit consisted of a contact membrane with food-grade CO2 gas
contacting one side of the membrane and untreated groundwater flowing past the other side. The
CO2 gas was sourced from a liquid CO2 storage tank equipped with an evaporator (Figure 3.3).
The desired amount of CO2 to be dissolved into the aquifer is that which would occur if a bubble
of CO2 were to exist at the aquifer depth and pressure, as represented by the height of the water
column above the top of the aquifer in the monitoring wells (Table 3.2).
PW-1 MW-4 MW-3 IW-1 BG-1
Sand and Gravel
Clay
Clay
Sand and Gravel
Clay
Clayey Sand
Fine Sand
Silt
Clay
0 M
-10 M
-20 M
-30 M
-40 M
-50 M
10 M .
0 M 10 M 20 M 30 M 40 M 50 M 60 M 70 M 80 M 90 M
Test Zone
Ele
vation
(Mete
rs M
SL)
Distance (Meters)
Inflatable
packer
Submersible
Pump (22.7 L/m)
Non-carbonated H2O
Insulated piping
17 L/m
5.7 L/m
Carbonated
H2O at 5.7 L/m
Carbonation
unit
59
Figure 3.3. Carbonation and injection system photograph.
Table 3.2. Aquifer properties and water column pressures.
Well
Aquifer
Bottom
(m)
Aquifer
Top (m)
Aquifer
Thickness
(m)
Depth to
Water
(m)
Water Column
above Aquifer
Bottom (m)
Water Column
above Aquifer
Top (m)
IW-1 54.6 47.5 7.0 9.2 45.4 38.3
PW-1 52.7 47.2 5.5 9.4 43.4 37.9
MW-1 52.7 46.9 5.8 9.2 43.5 37.7
MW-2 54.3 47.9 6.4 9.1 45.1 38.7
MW-3 54.0 47.2 6.7 9.2 44.7 38.0
MW-4 54.0 47.9 6.1 9.3 44.6 38.6
BG-1 54.3 47.5 6.7 9.0 45.2 38.5
Average 53.6 47.5 6.1 9.2 44.6 38.2
psi 63.3 54.33
bar 4.36 3.74
Depths reported in meters below ground surface; 1.42 psi per meter of water; 1 bar = 14.5038
psi; T = 22 ºC
60
The on-demand gas delivery system supplied CO2 to the carbonation unit at 3.3 to 4 bars
pressure, while a slightly lower groundwater pressure was maintained on the “wet” side of the
membrane. This allowed gas to diffuse across the membrane and saturate the groundwater with a
corresponding CO2 concentration around 0.15 molal (~6,600 mg/L as CO2). The process was
expected to reduce the pH of the pumped groundwater from 7.5 to 5.0 units, producing a strong
input and detection signal for the injection experiment.
An additional vent valve after the membrane module was used to ensure that there was no
excess CO2 in the groundwater. Water pressure, temperature, pH, and flow rate were monitored
continuously both upstream and downstream of the carbonation unit (Figure 3.3). Meters and
transmitters were used to communicate data in real-time, accessible from a local internetwork
connection. The meters were designed for process applications and to be removable for
calibration purposes. Interruptions to flow or carbonation effectiveness were diagnosed from a
remote location.
2.3. Downhole pH and conductivity monitoring
Submersible probes with onboard memory were deployed in the monitoring wells to
measure groundwater temperature, pH, electrical conductivity, and oxidation reduction potential
(ORP). These data provide a long-term record of groundwater quality spanning nearly a year,
with a sampling frequency of one measurement every 2-3 hours. The nearly continuous
electronic data set compliments the individual data points for pH, electrical conductance, and
ORP collected manually during the test period.
The monitoring wells were sealed to prevent cross-contamination by atmospheric transfer
and groundwater was sampled using dedicated bladder pumps installed in each well (Figure 3.4).
61
Figure 3.4 Picture showing dedicated bladder pump and well completion.
Following low-flow sampling procedures (US EPA, 1996), groundwater was purged at a low rate
of 0.6 L/min before samples were collected using a technique that reduced outgassing of CO2
from the samples. The water was pumped from the well to the surface through a sampling tube
connected to an in-line flow-through cell where measurements of pH, dissolved oxygen,
conductivity, temperature, and oxidation-reduction-potential were recorded using a
multiparameter probe. When these parameters stabilized, samples were collected upstream of the
flow-through cell into appropriate preserved sample containers. The downstream end of the
flow-through cell was connected to a pressure regulator such that the groundwater samples could
be collected against a back-pressure of 1-2 bars to minimize exsolution of dissolved gases
(Figure 3.5).
62
Figure 3.5 Schematic showing the pressurized monitoring well sampling system.
3. Results
3.1. Process temperature, pressure, and pH
Groundwater pumped from well PW-1 exhibited pH values ranging from 7.21 to 7.83,
averaging 7.52 prior to carbonation (August 12, 2011 to October 18, 2011) (Figure 3.6). Inlet
water temperature during the entire test period fluctuated between 18.4 to 28.6 ºC, and averaged
21.8 ºC. Outlet temperature was slightly higher than inlet temperature during the test period,
ranging from 18.5 to 29.5 ºC, and averaging 22.6 ºC (Figure 3.7). Inlet and outlet pressure
remained fairly steady throughout the test, predominantly ranging between 46 and 50 psi. A
growing differential between inlet and outlet pressure appeared to occur as the study progressed
(Figure 3.8).
63
Figure 3.6. Injectate water pH during the test period, showing pre- and postcarbonation pH.
Figure 3.7. Inlet and outlet water temperature during the test period.
3.00
3.50
4.00
4.50
5.00
5.50
6.00
6.50
7.00
7.50
8.00
7/26/11 9/14/11 11/3/11 12/23/11 2/11/12 4/1/12 5/21/12
Inje
ctat
e p
H (
s.u
.)
Date
15
17
19
21
23
25
27
29
7/26/11 9/14/11 11/3/11 12/23/11 2/11/12 4/1/12 5/21/12
Tem
per
atu
re (
celc
ius)
Date
Outlet temperature Inlet temperature
64
Figure 3.8. Inlet and outlet water pressure during the test period.
3.2. Groundwater levels and hydraulic control
Injectate flow remained fairly consistent throughout the test period, averaging
approximately 1.5 gpm (Figure 3.9). Water levels responded rapidly to the beginning of
pumping (dynamic baseline period) and to the end of pumping (end CO2) (Figure 3.10). During
the test period, groundwater elevations were consistently highest at well MW-3 and lowest at
well MW-4, indicating flow toward well MW-4 from the injection well. Overall, the test was not
disturbed by any significant fluctuations in water levels, with the exception of a spike in water
levels in February 2012. The calculated hydraulic gradient between wells MW-3 and MW-4 also
remained fairly consistent throughout the test period, with the exception of during the period of
increased injectate flow (Figure 3.11).
45
46
47
48
49
50
51
52
53
7/26/11 9/14/11 11/3/11 12/23/11 2/11/12 4/1/12 5/21/12
Pre
ssu
re (
PSI
)
Date
Outlet pressure Inlet pressure
65
Figure 3.9. Injectate water flow rate measured during the test period.
Figure 3.10. Potentiometric groundwater elevations in all monitoring wells during the test period.
0.00
0.50
1.00
1.50
2.00
2.50
3.00
7/26/11 9/14/11 11/3/11 12/23/11 2/11/12 4/1/12 5/21/12
Inje
ctat
e fl
ow
rat
e (g
pm
)
Date
-2.00
-1.80
-1.60
-1.40
-1.20
-1.00
-0.80
-0.60
-0.40
-0.20
0.00
8/10/10 11/18/10 2/26/11 6/6/11 9/14/11 12/23/11 4/1/12 7/10/12 10/18/12 1/26/13
Wat
er
Leve
ls (
m M
SL)
Date
MW-1 MW-2 MW-3 MW-4 BG-1 Dynamic Baseline Start CO2 End CO2
66
Figure 3.11. Approximate hydraulic gradient and injectate flow rate during the test period.
3.3. Groundwater pH and conductivity
Groundwater pH values in down-gradient wells showed sharp declines to levels similar to
the upper range of injectate pH over time, approximately 5.25 s.u. (Figure 3.12). The apparent
arrival of CO2 at well MW-3 occurred 10 days after initiation of injectate carbonation, and
similar downward pH trends followed in wells MW-2, MW-1, and MW-4. The lowest pH values
measured in wells MW-1 and MW-4 after CO2 breakthrough were higher than the injectate pH.
These wells were located furthest down-gradient from well IW-1 and the experiment was
terminated upon indication that the front had arrived at well MW-4 (157 days after injection).
0.0
0.5
1.0
1.5
2.0
2.5
3.0
-0.004
-0.003
-0.002
-0.001
0.000
0.001
0.002
0.003
0.004
7/26/11 9/14/11 11/3/11 12/23/11 2/11/12 4/1/12
Inje
ctat
e F
low
(gp
m)
Hyd
rau
lic G
rad
ien
t (m
/m)
Date
Hydraulic Gradient Dynamic Baseline Start CO2 End CO2 Flow
67
Figure 3.12. Downhole groundwater pH measurements during the test period.
After initiating carbonation, groundwater conductivity levels rose sharply to a peak
nearly twice the baseline level in well MW-3, but then decreased to near-baseline levels (Figure
3.13). Wells MW-2, MW-1, and MW-4 also exhibited conductivity increases, followed by
declines, until the experiment was terminated. After CO2 injection ceased, groundwater
conductivity levels began to rise again in wells MW-2 and MW-3.
4.0
4.5
5.0
5.5
6.0
6.5
7.0
7.5
8.0
8.5
9.0
6/6/11 7/26/11 9/14/11 11/3/11 12/23/11 2/11/12 4/1/12 5/21/12 7/10/12 8/29/12
pH
Date
IW-1 MW-1 MW-2 MW-3 MW-4
Start Injection 10/18/11
Baseline pHrange
Injectate pHrange
Stop Injection 3/23/12
10 days 71 days 108 days 157 daysCO2 arri val times:
68
Figure 3.13. Downhole groundwater conductivity measurements during the test period.
3.4. Downhole versus surface groundwater pH measurements
Groundwater pH measurements conducted at the surface using the backpressure sampling
system were comparable to those made in downhole measurements (Figure 3.14 to Figure 3.17).
0.50
0.60
0.70
0.80
0.90
1.00
1.10
1.20
1.30
1.40
6/6/11 7/26/11 9/14/11 11/3/11 12/23/11 2/11/12 4/1/12 5/21/12 7/10/12 8/29/12
Spe
cifi
c C
on
du
ctan
ce (m
s/cm
)
Date
MW-1 MW-2 MW-3 MW-4
Start Injection 10/18/11
Stop Injection 3/23/12
69
Figure 3.14. Downhole and surface pH measurements for well MW-1 groundwater.
Figure 3.15. Downhole and surface pH measurements for well MW-2 groundwater.
5.00
5.50
6.00
6.50
7.00
7.50
8.00
8.50
7/6/2009 1/22/2010 8/10/2010 2/26/2011 9/14/2011 4/1/2012 10/18/2012 5/6/2013 11/22/2013
pH
Date
MW-1 surface pH MW-1 downhole pH
4.50
5.00
5.50
6.00
6.50
7.00
7.50
8.00
8.50
7/6/2009 1/22/2010 8/10/2010 2/26/2011 9/14/2011 4/1/2012 10/18/2012 5/6/2013 11/22/2013
pH
Date
MW-2 surface pH MW-2 downhole pH
70
Figure 3.16. Downhole and surface pH measurements for well MW-3 groundwater.
Figure 3.17. Downhole and surface pH measurements for well MW-4 groundwater.
4.00
5.00
6.00
7.00
8.00
9.00
10.00
11.00
1/22/2010 8/10/2010 2/26/2011 9/14/2011 4/1/2012 10/18/2012 5/6/2013 11/22/2013
pH
Date
MW-3 surface pH MW-3 downhole pH
6.00
6.50
7.00
7.50
8.00
8.50
9.00
1/22/2010 8/10/2010 2/26/2011 9/14/2011 4/1/2012 10/18/2012 5/6/2013 11/22/2013
pH
Date
MW-4 surface pH MW-4 downhole pH
71
4. Discussion
4.1. Leakage simulation
The critical factors affecting the successful simulation of a CO2 leakage scenario are: 1)
ability to simulate a CO2 gas bubble in equilibrium with aquifer water at the appropriate
temperature and pressure, and 2) ability to detect a response to the disturbance with confidence.
The pH measurements of the injectate indicated that adequate carbonation was achieved
during the test. Dissolution of CO2(g) in water is described as:
(5) CO2(g) + H2O = H2CO3o
where H2CO3o is the combination of true dissolved H2CO3
* and CO2(aq), and the contribution of
H2CO3* to H2CO3
o is less than 0.3%. Under ideal conditions the dissolution of CO2(g) in water is
governed by Henry’s Law, which states that at a given temperature, the solubility of a gas in
water is proportional to the partial pressure of the gas. For CO2, the Henry’s Law equation is
described as:
(6) KCO2 (M/bar) = [CO2(aq)]/PCO2
and the value of KCO2 can vary with temperature. H2CO3o will undergo two dissociation steps,
written as:
(7) H2CO3o = H
+ + HCO3
-
where the equilibrium expression is:
(8) K1 = [H+][ HCO3
-]/[ H2CO3
o] = 10
-6.35
and:
(9) HCO3- = H
+ + CO3
2-
where the equilibrium expression is:
(10) K2 = [H+][CO3
2-]/[ HCO3
-] = 10
-10.33.
72
The pH of the water in equilibrium with CO2(g) can be derived from the above equations as:
(11) [H+] = (KCO2*K1*P CO2)/[ HCO3
-]
A titration model simulating incremental additions of CO2(g) to the average aquifer water
composition (reported in Chapter 2) was conducted using PHREEQC (Parkhurst and Appello,
2013). The model results showed that saturating the solution with CO2 at a PCO2 of 4 bars,
resulted in a pH drop from 7.7 to 4.97, and a total dissolved CO2 concentration of 6,050 mg/kg
(Figure 3.18).
Figure 3.18. Relationship between pH and dissolved CO2 to PCO2.
The average surface injection pressure was 3.3 bar (slightly below the calculated aquifer pressure
of 3.74 bar), which should have produced an injectate pH of approximately 5 s.u. The average
injectate pH during the test period was 4.99 s.u., indicating that the injectate contained a strong
pH signal for detecting impacts in downgradient monitoring wells. Results suggest that the CO2
leakage scenario was adequately simulated.
0
2000
4000
6000
8000
10000
12000
14000
16000
4.00
4.50
5.00
5.50
6.00
6.50
7.00
7.50
8.00
0 1 2 3 4 5 6
mg
CO
2/
kg
H2O
pH
PCO2 (bar)
pH mg CO2 / kg H2O
73
4.2. Injectate plume detection (pH and conductivity)
The second critical factor for successful field demonstration was the ability to detect the
disturbance created by the injection. Due to the volatility of gas phases and resulting difficulty
obtaining accurate sampling results, it was important to test the applicability of a backpressured
sampling system and compare results to downhole measurements. Results of the field test
showed that pH measurements conducted at the surface under a backpressure were successful
and compared well to downhole measurements, with few exceptions. There are advantages and
disadvantages to both approaches. Downhole probes provide high-resolution data at relatively
low cost, compared to using field labor on a very frequent basis. Multiple measurements can be
made simultaneously and data can be transmitted to remote access locations for project
monitoring. A disadvantage to downhole measurements is that they most often rely on batteries
and can drift out of calibration range or stop working, if left unattended. The advantage of
surface sampling, if conducted properly, is that the equipment is always calibrated and accurate
and can be linked directly to measured concentrations of other analytes in the sample at the time
of collection. The best way to plan a monitoring program will be based on site-specific
considerations and budgetary constraints. It is suggested that a combination of downhole and
pressurized surface measurements, such as was used in this study, be used to determine changes
in groundwater pH over time. Groundwater pH measurements taken under ambient pressure
conditions should be avoided.
4.3. Modeled downhole pH response
74
The pH response in well MW-3 was modeled using PHREEQC 1-D transport modeling.
Conceptually, the model was a 1-D column consisting of 10 cells, each 0.46 meters in length
between wells IW-1 and MW-3 (Figure 3.19).
Figure 3.19. Representation of the PHREEQC 1-D column transport model.
Dispersivity was set to 0.1 m (as determined by Trautz et al., 2013) and an average velocity was
computed as 0.46 m/d, based upon a previously conducted argon tracer test (Trautz et al., 2013).
Only the aqueous dissolution of CO2(g) and carbonate speciation were considered in the
geochemical reactions. No solid phases, exchange sites, or surface sorption sites were included.
As shown in Figure 3.20, the actual pH response of groundwater in well MW-3 was very
similar to that modeled with PHREEQC using no solid phase buffering reactions such as ion
exchange, indicating a very limited aquifer buffering capacity. A lack of buffering capacity is
also supported by the conclusions of Trautz et al. (2013), and by detailed sediment
characterization performed by Varadharajan et al. (2013). This model results provides
IW-1 MW-3
10 cells
Cell length: 0.46 m
Dispersivity: 0.1 m
Time step: 86400 s
v = 0.46 m/d
Porosity: 0.35
4.6 m
IW-1 MW-3IW-1 MW-3
10 cells
Cell length: 0.46 m
Dispersivity: 0.1 m
Time step: 86400 s
v = 0.46 m/d
Porosity: 0.35
4.6 m
75
confidence that the aquifer characterization data (Chapter 2) and the test design provided a sound
basis for interpreting and modeling the chemical data collected during the test period.
Figure 3.20. Measured and modeled groundwater pH in down-gradient well MW-3.
Groundwater pH was modeled using a PHREEQC 1-D transport model without buffering
reactions.
4.4. Comparison to Similar Studies
A growing number of studies have been conducted attempting to simulate a leak of CO2 into
an aquifer (EPRI, 2008; Trautz et al., 2013; Yang et al., 2013; Humez et al., 2014). EPRI
(2008) was the first known field attempt to assess impacts of CO2 intrusion to shallow
groundwater, but was ultimately difficult to model with coupled flow and transport due to the
occurrence of gas exsolution from the aquifer into the vadose zone, and subsequent redissolution
of CO2 into the water table further downgradient. This study attempted to inject CO2 into an
unconfined system, which promoted exsolution of CO2 into the vadose zone. While the study
4.0
4.5
5.0
5.5
6.0
6.5
7.0
7.5
8.0
8.5
9.0
6/6/11 7/26/11 9/14/11 11/3/11 12/23/11 2/11/12 4/1/12 5/21/12 7/10/12 8/29/12
pH
Date
Measured MW-3 No reactions Downhole pH data
76
concluded that various major, minor and trace elements could be released to groundwater due to
CO2 intrusion, the uncertainty regarding possible CO2 exsolution from the test aquifer introduced
questions regarding the strength of these conclusions of strength of the conclusions. Yang et al.
(2013) conducted a push-pull test on a very similar hydrogeologic setting to the current test in
Cranfield, Mississippi. The test consisted of extracting water from the target aquifer, saturating
the water with CO2 and reinjecting the water into the extraction well. After a period of residence
time, the water from the well was sampled for changes in chemistry that would have been
attributable to the presence of CO2 (a tracer was added to correct for wellbore effects and
impacts of physical heterogeneity). Similarly, Humez et al. (2014) conducted a push-pull test in
an aquifer in southern France, using techniques and with comparable results as to that of Yang et
al. (2013).
While push-pull tests are generally economic and informative at a screening level, the test
results are subject to numerous corrections and calculations, based primarily on tracer recovery.
Similarly, the test results are specific to the chosen test well and the near-borehole area, which
can often be disturbed by well drilling and installation. The current study is unique for at least
three reasons. First, a confined aquifer was purposely chosen to limit possible gas exsolution
pathways. Second, a thorough aquifer characterization was conducted in order to understand
and predict the physical and chemical responses to an injection of dissolved CO2. This
characterization included a lengthy baseline monitoring period so that pre-injection conditions
could be well-established. Third, the test was designed such that extracted water was passively
carbonated and allowed to pass through the entire aquifer thickness prior to monitoring at
downgradient wells. Above-ground and downhole measurements of pH, temperature and
pressure were collected throughout the experiment in order to maintain and troubleshoot the
77
injection loop. Excursions in flow rate or pH could be corrected quickly by modifications to the
flow control valves or outlet CO2 pressure, respectively. Downhole pH measurements were
compared to above-ground measurements to evaluate the success of a back-pressured well
purging technique. Ultimately, the extensive site characterization and attention to monitoring
techniques in this study facilitate subsequent data interpretations and modeling.
5. Conclusions
This study evaluated the design and implementation of a controlled CO2 release field
experiment that was performed in a well-confined, well-characterized aquifer. A field test was
performed instead of a laboratory evaluation so that the impacts of CO2 to a groundwater aquifer
could be evaluated in situ. The critical aspects of the design and implementation were the ability
to control experimental conditions in the field (e.g., pressure, temperature, redox) and detect
responses to the disturbance (e.g., hydraulic control, downhole pH, conductivity) with enough
confidence to support conclusions and modeled predictions related to CO2-induced groundwater
quality impacts (e.g., trace element mobilization). The selection of a confined aquifer as
opposed to an unconfined system allowed for minimal, if any, degassing of CO2 from the test
aquifer during the experiment. A closed loop pumping and injection system, and in-line passive
carbonation technology were used to achieve the objective of simulating CO2 leakage into the
aquifer at near aquifer temperature and pressure conditions. Process monitoring results indicated
that the test was performed with minimal variation in key process parameters, including
temperature, pressure and injectate pH. In situ instrumentation deployed in monitoring wells
allowed continuous readings of groundwater pH and conductivity, which were critical
parameters for evaluating the aquifer response to carbonation and acidification. Successful
78
modeling simulation of the pH response using results from the aquifer testing program suggested
that the test was implemented and monitored appropriately. Ultimately, the results presented in
this study provide confidence that future data interpretations and modeling of the field
experiment were not compromised by test design. Future studies seeking to assess impacts of
CO2 on shallow groundwater aquifers can utilize methods employed here to ensure meaningful
test results.
79
REFERENCES
Electric Power Research Institute (EPRI), 2008. Preliminary evaluation of CO2 impacts on
shallow groundwater. EPRI, Palo Alto, CA: 2008. Technical Report 1015848.
Trautz, R.C., Pugh, J.D., Varadharajan, C., Zheng, L., Bianchi, M., Nico, P.S., Spycher, N.F.,
Newell, D.L., Esposito, R.A., Wu, Y., Dafflon, B., Hubbard, S.S., and Birkholzer, J.T.,
2013. Effect of Dissolved CO2 on a Shallow Groundwater System: A Controlled Release
Field Experiment. Environmental Science and Technology., Vol. 47, pp. 298−330.
US EPA, 1996. Low stress (low flow) purging and sampling procedure for the collection of
groundwater samples from monitoring wells. EQASOP-GW 001. Revised 2010.
Parkhurst, D.L. and Appelo, C.A.J., 2013, Description of input and examples for PHREEQC
version 3--A computer program for speciation, batch-reaction, one-dimensional transport,
and inverse geochemical calculations: U.S. Geological Survey Techniques and Methods,
book 6, chap. A43, 497 p.
Varadharajan, C. R. M. Tinnacher, J. D. Pugh, R. C. Trautz, L. Zheng N. F. Spycher, J. T.
Birkholzer, H. Castillo-Michel, M. Bianchi, R. A. Esposito, and P. S. Nico. A laboratory
study of the initial effects of dissolved carbon dioxide (CO2) on metal release from
shallow sediments. International Journal of Greenhouse Gas Control. Vol. 19. pp. 183-
211.
Yang, C., Mickler, P.J., Reedy, R., Scanlon, B.R., Romanak, K.D., Nicot, J.-P., Hovorka,S.D.,
Trevino, R.H., Larson, T., 2013. Single-well push–pull test for assessing potential
impacts of CO2 leakage on groundwater quality in a shallow Gulf Coast aquifer in
Cranfield, Mississippi. International Journal of Greenhouse Gas Control,
http://dx.doi.org/10.1016/j.ijggc.2012.12.030.
Humez, P., Negrel, P., Lagneau, V., Lions, J., Kloppmann, W., Gal, F., Millot, R., Guerrot, C.,
Flehoc, C., Widory, D., Girard, J.-F., 2014. CO2-water-mineral reactions during CO2
leakage: Geochemical and isotopic monitoring of a CO2 injection field test. Chemical
Geology, Vol. 368, pp. 11-30.
80
Chapter 4
GEOCHEMICAL IMPACT OF A CONTROLLED CO2 RELEASE FIELD TEST ON A
SHALLOW POTABLE COASTAL PLAIN AQUIFER
Abstract
Geologic sequestration of carbon dioxide has the potential to mitigate concerns over
emissions of greenhouse gas to the atmosphere. The technology involves injected carbon
dioxide into deep geologic reservoirs that are sufficiently protected from drinking water sources,
such as shallow freshwater aquifers. However, the potential for gas migration from deep
reservoirs into potable water sources exists due to geologic features such as faults and fractures
and man-made conduits such as well boreholes. Therefore, it is necessary to assess the impact
that a leak of carbon dioxide would have to a potable aquifer. In this study, carbon dioxide was
introduced into a shallow aquifer in the United States Gulf Coast, a region well-suited for
geologic sequestration, in a controlled release field test. The test was designed to mimic the
migration of a carbon dioxide gas bubble and dissolution into a shallow aquifer, and to monitor
the geochemical impacts to the aquifer resulting from the release. Results at the test site showed
that no constituent was mobilized in excess of US EPA maximum contaminant levels, but that
many constituents (major and minor cations) were released in a pulse-like response at levels
above their baseline concentrations. Dissolution of trace carbonate and pyrite in the aquifer are
hypothesized to have triggered cation exchange reactions, a dominant geochemical process
affecting major and minor cation behavior in the aquifer. Overall, the test has shown that the
migration of carbon dioxide into a drinking water can mobilize ions into solution, but at levels
that are not likely to be of concern to human health.
81
1. Introduction
Potential gas leakage into potable aquifer systems, although a low probability event, is a
major concern for those planning to utilize geologic sequestration for purposes of mitigating CO2
releases to the atmosphere. According to Harvey et al. (2012), the most concerning release
scenario may be that of slow, diffusive leakage from a wellbore or geologic conduit due to its
difficulty to detect for long periods of time. Under this scenario, the fate of CO2 is primarily
governed by the structure and reactivity of the overlying geologic formations. Assuming
structural pathways exist for gas migration, the fate of CO2 depends upon chemical composition
of the aquifer matrix and porewater and their potential interactions with CO2 under specific
temperature and pressure conditions.
In the aqueous phase, the most important reaction will involve dissolution of CO2,
formation of carbonic acid, and subsequent dissociation of carbonic acid (Harvey et al., 2012).
During the dissociation process, protons are released to solution and pH decreases. These
reactions in isolation may or may not be deleterious to water quality, depending upon the extent
of acidification. In fact, the primary risk to potable water supplies due to CO2 leakage into the
aquifer will result from the reactions between dissolved CO2 and the host aquifer mineral
assemblage (Apps et al., 2008). One such reaction is the dissolution of carbonate minerals such
as calcite (Langmuir, 1997):
(1) CaCO3 + CO2(g) + H2O = Ca2+
+ 2HCO3-
Carbonate mineral dissolution can release elements such as calcium, magnesium, iron
and manganese to solution, in addition to other carbonate-forming minor and trace elements.
Other important reactions may include the pH-dependent surface complexation of trace elements
82
onto iron oxyhydroxides or other sorbing surfaces, as represented by the following surface
complexation reaction between arsenate and iron oxyhydroxide:
(12) ≡FeOH-1/2
+ 2 H+ + AsO4
-3 = ≡FeOAsO3H
-3/2 + H2O
where ≡FeOH-1/2
represents a surface functional group on iron oxyhydroxide, and ≡FeOAsO3H-
3/2 represents a monodentate inner sphere surface species wherein arsenic is bound to the iron
oxyhydroxide surface (EPRI, 2009). In reducing environments, sulfide solubilization may result
in release of iron and sulfur, in addition to other common sulfides by a reaction such as that for
mackinawite:
(13) FeS + H+ = Fe
2+ + HS
-
The specific reactions that take place will depend upon the aquifer initial conditions, including
pH, redox state, mineral assemblage, temperature and pressure.
Proper assessment of risk will require development of models capable of predicting
impacts to drinking water sources, and the testing of models against field observations.
Confidence in modeled results is greatly enhanced if comparable to field observations (Xu et al.,
2004). Kharaka et al. (2009) and EPRI (2008) provide evidence that primary geochemical
effects resulting from CO2 intrusion into an aquifer system are carbonate and oxide mineral
dissolution as well as ion exchange. Kharaka et al. (2009) reported geochemical changes in a
1500 m deep sandstone aquifer following injection of CO2 into the Frio Sandstone in Texas. A
drop in pH to approximately 3 s.u. was interpreted to have mobilized significant calcium, iron
and manganese from carbonates and metal oxides. Likewise, EPRI (2008) injected CO2 into a
shallow, unconfined aquifer system and observed a decrease in pH – from pH 7 to 6 – and
increased bicarbonate, calcium and magnesium. The study was ultimately difficult to model
83
with coupled flow and transport due to the occurrence of gas exsolution from the aquifer into the
vadose zone, and subsequent redissolution of CO2 into the water table further downgradient.
To strengthen the current understanding of water quality impacts resulting from potential
CO2 leakage, the Electric Power Research Institute (EPRI) funded a field experiment to test the
effects of elevated CO2 on water quality in a shallow aquifer. The goal of the experiment was to
simulate a leak of CO2 into a shallow aquifer and observe the effects on water quality as it
dissolved into the aquifer. Described in greater detail in Chapter 3 and in Trautz et al. (2012),
the test was designed based upon thorough aquifer characterization and planning.
Chapter 4 presents the results of the experiment and a discussion of the possible
mechanisms underlying field observations. Results are assessed based on their statistical and
regulatory significance and interpretations are provided as to possible geochemical mechanisms
at work. The results of this effort can be used to inform the assessment of risk from geologic
storage projects and the development of models capable of predicting major changes in water
quality resulting from CO2 leakage.
2. Site Location and Regional Hydrogeologic Setting
Site location and regional hydrogeologic setting are described in Chapter 2.
3. Methods
3.1. Site characterization
Methods pertaining to site drilling, well installations and aquifer testing are described in
detail in Chapter 2.
84
3.2. Groundwater sampling and analysis
Groundwater sampling and analytical methods are described in detail in Chapter 2.
3.3. Well layout and test design
The well layout and test design are described in detail in Chapters 2 and 3, respectively.
4. Results
4.1. Intrawell statistics and comparison to regulatory levels
Summaries of pre- and post-CO2 injection concentration ranges for major, minor and
trace constituents are provided in Table 4.1 and. There were no exceedances of US EPA
maximum contaminant levels (MCLs) for any constituent during the test period. All constituents
were evaluated for baseline monitoring period stationarity using box-and-whisker plots (Figure
4.1) in order to determine whether interwell or intrawell comparisons were appropriate.
Although some parameters did appear to reflect stationarity, as required for an interwell
comparison, enough parameters were found to be non-stationary to suggest that an intrawell
comparison was the most appropriate statistical method for the test site (Table 4.3). Therefore,
intrawell analyses were performed on all parameters for this data set. MANAGES, EPRI's data
management and statistical analysis software, was used to automatically perform the statistical
comparison using the following procedure: Outlier Test > Determine Detection Frequency >
Normality Test > Limit Calculation >Comparison to Compliance Data.
85
Table 4.1 Summary of cation and anion concentrations compared to US EPA MCLs
Parameter Units Baseline Range Baseline
Mean
Post-Injection
Range
US EPA
MCL
Calcium mg/L 1.9-6.2 2.9 1.7-15
Magnesium mg/L 0.83-1.9 1.33 0.73-7.8
Sodium mg/L 140-190 157 130-280
Potassium mg/L 1.8-7.6 2.94 1.8-6.1
Silicon mg/L 8.4-13 11.6 11-56
Barium mg/L 0.04-0.11 0.06 0.04-0.48 2
Strontium mg/L 0.07-0.37 0.10 0.06-0.55
Ferric Iron mg/L 0-0.67 0.23 0.01-31.7
Ferrous Iron mg/L 0.05-0.64 0.33 0.04-7.6
Manganese mg/L 0.03-0.11 0.07 0.04-0.65
Lithium mg/L 0.01-0.23 0.02 0.02-0.06
Aluminum mg/L <0.023-0.047 <0.023 <0.023-0.24
Chloride mg/L 13-32 25 20-29 250
Sulfate mg/L <0.015-2.5 0.34 0.034-27 250
Fluoride mg/L 0.18-0.60 0.45 0.05-0.67 4
86
Table 4.2 Summary of trace element concentrations compared to US EPA MCLs
Parameter Units Baseline Range Baseline
Mean
Post-Injection
Range
US EPA
MCL
Silver mg/L <0.00025 <0.00025 <0.00025-0.0007
Arsenic mg/L <0.0013 <0.0013 <0.0013 0.01
Beryllium mg/L <0.00025 <0.00025 <0.00025-0.0007 0.004
Cadmium mg/L <0.000095 <0.000095 <0.000095-0.00024 0.005
Cobalt mg/L <0.00015 <0.00015 <0.00015-0.012
Chromium mg/L <0.0025-0.007 <0.0025 <0.0025-0.013 0.1
Copper mg/L <0.0011 <0.0011 <0.0011-0.002 1.3
Mercury mg/L <0.00007 <0.00007 <0.00007-0.00023 0.002
Molybdenum mg/L 0.002-0.013 0.005 <0.0015-0.012
Nickel mg/L <0.002-0.037 0.002 <0.002-0.1
Lead mg/L <0.0002-0.0009 <0.0002 <0.0002-0.0009 0.015
Antimony mg/L <0.0023-0.003 <0.0023 <0.0023-0.003 0.006
Selenium mg/L <0.001-0.001 <0.001 <0.001-0.0021 0.05
Thallium mg/L <0.0005 <0.0005 <0.0005 0.002
Zinc mg/L <0.0083-0.028 <0.0083 <0.0083-0.036 5
87
Figure 4.1 Box-and-whisker plots illustrating stationary and non-stationary baseline datasets
Table 4.3 Summary of stationary and non-stationary chemical parameters during the baseline
sampling period
Analyte Category Stationary Non-Stationary
Major/Minor Cations Ca, Sr, Na, Si Mg, Fe, Mn, Ba, K, Li
Anions HCO3, Cl SO4
Trace Elements* Mo
Field Parameters Temperature Conductivity, pH
Redox Indicators/Other Ammonia, Methane, Ethane, Fe(2),
Fe(3), CO2, ORP
*Most trace element data were non-detect during the baseline study period, preventing creation
of meaningful box-and-whisker plots. Data were assumed non-stationary.
Although no regulatory levels were exceeded, a large percentage of the post-injection
data exceeded background levels and a majority of these metals exhibited an increasing trend in
concentrations above background, indicative of CO2-induced mobilization. Parameters
exhibiting statistical exceedances in the most wells were typically major or minor cations (Table
88
4.4). With the exception of Cr and Ni, less frequent exceedances were observed for trace
elements (Table 4.4).
Table 4.4 Summary of statistical exceedances above background in each well for each cation
MW-1 MW-2 MW-3 MW-4
Element # Events Element # Events Element # Events Element # Events
Ba 22 Ba 35 Fe 23 Fe 4
Si 22 Ca 35 Mn 23 Ba 3
Fe 21 Fe 35 Si 22 Pb 3
Li 21 K 35 Ba 20 Ca 2
Sr 21 Li 35 Mg 20 Co 2
Ca 20 Mg 35 Be 14 K 2
Mg 20 Mn 35 Ca 13 Li 2
Mn 20 Si 35 Ni 12 Mg 2
Na 20 Sr 35 Cr 9 Mn 2
K 19 Cr 31 Na 8 Na 2
Cr 11 Ni 19 Co 6 Si 2
Hg 2 Na 15 Sr 5 Sr 2
Al 1 Co 8 Zn 2 Cu 1
Co 1 Zn 1 Ag 1 Ag 0
Cu 1 Ag 0 Cd 1 Al 0
Ni 1 Al 0 Hg 1 As 0
Pb 1 As 0 Sb 1 Be 0
Ag 0 Be 0 Al 0 Cd 0
As 0 Cd 0 As 0 Cr 0
Be 0 Cu 0 Cu 0 Hg 0
Cd 0 Hg 0 K 0 Mo 0
Mo 0 Mo 0 Li 0 Ni 0
Sb 0 Pb 0 Mo 0 Sb 0
Se 0 Sb 0 Pb 0 Se 0
Tl 0 Se
Tl
0 Se 0 Tl 0
Zn 0 0 Tl 0 Zn 0
Exceeded in All Wells: Fe>Si>Ba=Mn>Mg>Ca>Sr>Li>K>Na>Co
Exceeded in 3 Wells: Cr>Ni
Exceeded in 2 Wells: Pb>Hg=Zn>Cu
Exceeded in 1 Well: Be>>Cd=Sb=Ag=Al
Exceeded in 0 Wells: Cd=As=Mo=Se=Tl
89
4.2. Temporal trends
Temporal trends for inorganic constituents are discussed below, and illustrated in the
context of four major test periods (Table 4.5): A, B, C, and D. Test period A represents a period
of static baseline testing, where ambient groundwater was sampled under natural flow
conditions. Test period B is a period of induced gradient by pumping from PW-1 and injecting
non-carbonated water into IW-1. Test period C represents no change in pumping or injection
rates, but the dissolution of CO2 into the injectate stream. Test period D represents a return to
non-pumping conditions.
Table 4.5 Summary of test period durations and sampling schedule
Test Period Start Date End Date Approx.
Duration (mos)
Wells
Sampled
Pre-CO2 injection baseline 2-Sep-2010 18-Oct-
2011 13
All wells
Pre-pumping (static baseline) 2-Sep-2010 12-Aug-
2011 11
All wells
Pumping (dynamic baseline) 12-Aug-
2011
18-Oct-
2011 2
MW, BG
wells
CO2 injection (pumping
continues)
18-Oct-
2011
23-Mar-
2012 5
MW, BG
wells
Post-CO2 injection 23-Mar-
2012 15-Jan-2013 10
MW, BG
wells
4.2.1. Dissolved CO2 plume indicators (pH, conductivity, alkalinity, Eh)
Arrival of the dissolved CO2 plume was indicated by sharp decreases in pH at all wells,
reaching a minimum pH reflecting that of the injectate (Figure 4.2). The arrival of dissolved
CO2 at MW-3 was indicated 7 days after start of CO2 injection by sharp decreases in pH and
increases in Eh, conductivity and alkalinity. Considering data from all downgradient wells, pH
decreased to as low as 4.66 from a baseline range of 7.36-8, and increased slightly after pumping
90
and injection ended (Figure 4.2). Eh increased sharply up to sustained positive values during the
injection phase, and decreased slightly after the active pumping and injection phase ended
(Figure 4.3). Conductivity exhibited a pulse-like post-injection response reaching a short-term
peak of nearly double the baseline values (Figure 4.4). Field alkalinity concentrations also
exhibited a pulse-like response, reaching peaks at approximately double the baseline
concentration range in downgradient wells (Figure 4.5).
Figure 4.2 pH trends during baseline, injection and post-injection time periods.
91
Figure 4.3 Eh trends during baseline, injection and post-injection time periods.
Figure 4.4 Conductivity trends during baseline, injection and post-injection time periods.
92
Figure 4.5 Alkalinity trends during baseline, injection and post-injection time periods.
4.2.2. Major and minor cations (Ca, Mg, Ba, Sr, Mn, Si, Fe, Si, K, Li, Na)
The temporal trends of Ca, Mg, Ba, Sr, Mn, total Fe, Na and Si were all very similar to one
another, and to the trends of both alkalinity and electrical conductivity. In most cases,
concentrations gradually declined to near baseline values and increased again to new stable
levels after pumping and injection ceased. In most cases, the stable post-injection concentrations
were less than the peak concentrations observed during active injection, with the exception of Ca
which rebounded temporarily to the maximum injection phase concentration. Calcium responses
in all wells are shown in Figure 4.6 as an example of typical responses for Ca, Mg, Ba, Sr, and
Mn.
93
Figure 4.6 Calcium trends during baseline, injection and post-injection time periods.
Dissolved ferrous and ferric iron displayed different responses from one another during the
active injection phase (Figure 4.7). Baseline and post-injection concentrations for each were
similar, but the increase in ferric iron was much more pronounced and pulse-like than for ferrous
iron. In this respect, ferric iron behaved more similarly to other divalent cations.
Dissolved silicon responded similarly to ferric iron and other divalent cations, characterized
by a sharp increase after injection and subsequent decline toward baseline concentrations as
injection continued (Figure 4.8). Concentrations rebounded gradually to a nearly stable
concentration after the injection phase ended.
94
Figure 4.7 Trends of ferrous and ferric iron, showing markedly different responses during the
CO2 injection but similar post-injection behavior.
Figure 4.8 Silicon trends during baseline, injection and post-injection time.
10
100
-400 -350 -300 -250 -200 -150 -100 -50 0 50 100 150 200 250 300 350 400 450 500
Silic
on
(m
g/L
)
Days after Start of CO2 Injection
MW-1 MW-2 MW-3 MW-4 BG-1 Begin Pumping Start CO2 End CO2
Baseline Post-CO2
C DBA
Inject CO2
95
Monovalent cations potassium and lithium were similar in that sharp concentrations increases
occurred after injection, although at a lower peak concentration than the maximum baseline
concentration and a more gradual decline in concentration after the initial increase (Figure 4.9).
Sodium concentrations increased in a pulse-like response relative to baseline concentrations and
returned to baseline concentrations, even after the active pumping and injection phase (Figure
4.10).
Figure 4.9 Trends of potassium and lithium, showing responses to CO2 injection against highly
variable baseline concentrations.
4.2.3. Trace elements (Ag, Al, As, Be, Co, Cd, Cr, Cu, Hg, Mo, Ni, Pb, Sb, Se, Tl, Zn)
Arsenic and Tl exhibited no detectable response to the active injection phase, and were not
detected throughout the experiment. Selenium was only detected during baseline and post-
injection periods, exhibiting no evidence of CO2-induced release. Silver and Cd were only
detected once during the active CO2 injection phase at MW-3, 15 days after injection began.
Cadmium was also detected on one event in the post-injection monitoring phase.
96
Figure 4.10 Sodium trends during baseline, injection and post-injection time.
Aluminum, Cu, Pb, Hg, Zn, and Sb all exhibited detections throughout the experiment, with
no clear increasing trends related to CO2 injection (Figure 4.114). Molybdenum was unique
among detectable trace elements, exhibiting decreasing concentrations during the active injection
and post-injection phase of the project (Figure 4.12).
100
1000
-400 -350 -300 -250 -200 -150 -100 -50 0 50 100 150 200 250 300 350 400 450 500
Sod
ium
(m
g/L
)
Days after Start of CO2 Injection
MW-1 MW-2 MW-3 MW-4 BG-1 Begin Pumping Start CO2 End CO2
Baseline Post-CO2
C DBA
Inject CO2
97
Figure 4.11 Trends of Al, Cu, Pb, Hg, Zn and Sb, showing sporadic nature of
detection throughout all test periods.
98
Figure 4.12 Molybdenum concentrations over time, showing decreases in concentration
following CO2 injection
Beryllium, Co, Cr and Ni all exhibited noticeable increasing trends during the injection
and/or post-injection monitoring periods (Figure 4.13). Beryllium exhibited an increasing trend
only in MW-3 beginning 29 days after the injection began and persisting into the post-injection
phase. Cobalt increased during the test period, with the highest increases occurring in the most
downgradient well MW-4. Nickel increases were most notable in wells MW-1 and MW-2. Both
Co and Ni exhibited elevated concentrations immediately prior to the baseline pumping phase
immediately after installation of ERT probes used for cross-well resistivity monitoring,
suggesting that stainless steel components could be an alternate source of at least Co and Ni, if
not other metals (Sb, Zn and Mo also increased on this sample event). The elevations observed
during the CO2 injection phase did not necessarily coincide with anticipated plume arrival times
0.001
0.01
0.1
-450 -400 -350 -300 -250 -200 -150 -100 -50 0 50 100 150 200 250 300 350 400 450 500
Mo
lyb
den
um
(m
g/L
)
Days after Start of CO2 Injection
MW-1
MW-2
MW-3
MW-4
BG-1
CO2Baseline Post-CO2
C DBA
Inject CO2
99
as indicated by changes in pH and conductivity. Chromium increased notably in wells MW-3
and MW-2, with a lesser response in MW-1, and no increase in MW-4. Chromium behavior
resembled that of other major and minor cations.
4.2.4. Inorganic anions (Cl, SO4, F, NO3, NO2) and dissolved organic carbon
Chloride concentrations remained stable throughout the test, with the exception of a sharp
decrease immediately prior to CO2 injection (Figure 4.14). Dissolved sulfate concentrations
remained low until seven months after the test ended, when concentrations rose as high as 27
mg/L (Figure 4.15). Fluoride concentrations decreased during the test, sharply at MW-3, and did
not recover to baseline concentrations after the test (Figure 4.16). Dissolved organic carbon
Figure 4.13 Trends of Ni, Co, Cr and Be, showing increasing trends during the CO2
injection phase. Relationship of Co and Ni trends to CO2 injection are suspect due to
timing of response in multiple wells.
100
appeared relatively stable during the test, although concentrations did appear to increase
immediately after the active phase (Figure 4.17).
Figure 4.14 Trends of chloride concentrations, showing mostly stable concentrations during the
test period.
5. Discussion
5.1. Response to CO2 behavioral categories
Based on the observed temporal trends and statistical evaluation, the responses of various
constituents to CO2 can be grouped into four major behavioral categories (Table 4.6): Types I, II,
III and IV. Type I constituents were either not detected throughout the duration of the
experiment, or they did not show significant or sustained deviations from background conditions.
1
10
100
-450 -400 -350 -300 -250 -200 -150 -100 -50 0 50 100 150 200 250 300 350 400 450 500
Ch
lori
de
(m
g/L
)
Days after Start of CO2 Injection
MW-1 MW-2 MW-3 MW-4 BG-1 Begin Pumping Start CO2 End CO2
Baseline Post-CO2
C DBA
Inject CO2
101
Figure 4.15 Trends of sulfate concentrations, showing an increase during the active injection
period.
Figure 4.16 Trends of fluoride concentrations, showing decreases during the injection period.
0.01
0.1
1
10
100
-450 -400 -350 -300 -250 -200 -150 -100 -50 0 50 100 150 200 250 300 350 400 450 500
Sulf
ate
(m
g/L
)
Days after Start of CO2 Injection
MW-1 MW-2 MW-3 MW-4 BG-1 Begin Pumping Start CO2 End CO2
Baseline Post-CO2
C DBA
Inject CO2
0.01
0.1
1
10
-450 -400 -350 -300 -250 -200 -150 -100 -50 0 50 100 150 200 250 300 350 400 450 500
Flu
ori
de
(m
g/L
)
Days after Start of CO2 Injection
MW-1
MW-2
MW-3
MW-4
BG-1
Baseline Post-CO2
C DBA
Inject CO2
102
Figure 4.17 Trends of dissolved organic carbon, showing increases during the injection period.
Type II constituents did exhibit some apparent response to CO2, but are known to or are highly
likely to have been sourced from stainless steel components of ERT probes installed for purposes
of resistivity monitoring during the test. Type III constituents are those which consistently
exceeded baseline concentrations during the test at all wells, and displayed very similar temporal
trends throughout the test. Type IV constituents exhibited an overall decreasing trend in
response to CO2.
5.1.1. Type I: No significant detectable response
A significant result of the study is that both As and Pb are Type I constituents, in contrast
to modeled predictions of Wang and Jaffe (2004) and Zheng et al (2009) or results from a field
experiment at the ZERT site (Kharaka et al. 2010).
0.1
1
10
100
-450 -400 -350 -300 -250 -200 -150 -100 -50 0 50 100 150 200 250 300 350 400 450 500
Dis
solv
ed
Org
anic
Car
bo
n (
mg
/L)
Days after Start of CO2 Injection
MW-1 MW-2 MW-3 MW-4 BG-1 Begin Pumping Start CO2 End CO2
Baseline Post-CO2
C DBA
Inject CO2
103
Table 4.6 Behavioral categories
Trend Description Trend
Category
Constituents Comments
Concentrations are at or
below method detection
and/or reporting levels
(with or without a minor
random detection) or do
not deviate significantly
from background
I Cations: Al, Sb,
As, Be, Cd, Cu,
Pb, Hg, P, Se,
Ag, Tl
Anions/other:
Br, Cl, NO3-,
NO2-, SO4
2-,
H2S
Beryllium was non-
detect for all wells
except MW-3,
which showed a
delayed Type III
trend
Concentrations become
elevated after ERT probes
are installed and active
II Co, Ni, Zn Type III trend for
Co observed in
MW-4 only after
CO2 arrives
Pulse response and/or
increasing concentrations
observed in response to
CO2 breakthrough
III Ca, Mg, Ba, Sr,
Fe, Mn, Na, Si,
alkalinity, K,
Li, Cr electrical
cond.
K and Li elevated in
baseline period for
MW-3 and BG-1
Concentrations decrease in
response to CO2
breakthrough
IV NH3, Methane,
Acetic acid,
Mo, F
Likewise, Karmalidis et al (2013) suggested that Cr, Pb, Mn and Fe could exceed EPA maximum
contaminant levels in sandstone aquifers reacting with CO2. The aquifer studied in this
experiment is most similar in geologic setting and composition to that studied by Yang et al
(2013) in a Gulf Coastal Plain aquifer in Natchez, Mississippi. A push-pull test into a very
similar aquifer revealed As and Pb concentrations at approximately 3% and 1%, respectively, of
their EPA maximum contaminant levels (Yang et al., 2013). Other constituents exhibiting Type
I behavior included many oxyanions, which are either likely to be non-reactive (Cl, Br) or whose
mobilization may have been suppressed by a low-pH and favorable adsorption environment (Sb,
104
As, Se, P). Redox-sensitive oxyanions NO3, NO2, and SO4 did not respond significantly,
suggesting that introduction of oxygen during the experiment was not a complicating issue.
Beryllium is also classified as a Type I constituent, although its behavior at MW-3
suggests a delayed Type III trend. In the cases of Al, Cd, Cu, Hg, and Ag, the detections
throughout the experiment were sporadic and temporally isolated enough so that a direct link to
mobilization by CO2 could not be established with confidence. In a companion laboratory study,
Varadharajan et al. (2013) examined sediments from the current test site and found that Ag, Be,
Cd, Cr, Cu and Pb all exhibited low release potential under acidified conditions.
5.1.2. Type II: Alternate source
Although Type II constituents exhibited increasing trends in multiple wells throughout
the test, the direct linkage of these constituents to CO2 cannot be established with confidence.
Several constituents (Zn, Sb, Co, Ni, Mo) exhibited a short-term increase in concentration when
ERT probes with stainless steel components were installed in monitoring wells approximately 90
days prior to CO2 injection. LANL (2007) performed an exhaustive review of the reliability of
chemical data from wells with variable construction methods, and found that wells with stainless
steel components as part of the screened intervals could produce false positives for Fe, Cr, Ni,
Mn, Si, Mo, P and S. Iron, Cr and Ni were reported as the most likely to leach from the well
screens, but the specific metals would be a function of the type of steel. For Co and Ni, elevated
concentrations were observed in multiple wells simultaneously prior to the time of CO2 arrival,
and concentrations appeared to decrease when the probes were removed.
105
Figure 4.18 Nickel and cobalt trends, showing possible impact from downhole probes.
Although the downhole equipment was a possible source of metals during the
experiment, there are geologic sources that must be considered. Varadharajan et al. (2013)
examined sediments from the current test site, and found that Co, Ni and Zn were all subject to
mobilization under acidified conditions, and that Ni and Zn were only sourced from an organic-
rich sand that was not found widespread in the aquifer. Cobalt has been found to be mobilized
106
by CO2 in multiple laboratory studies (Lu et al., 2010; Smyth et al., 2009; Little and Jackson,
2010) and exceeded baseline concentrations in all four monitoring wells during the current field
test. Additionally, Co levels remained elevated in MW-4 after the ERT probes were removed,
suggesting a possible geologic source in the aquifer.
The detections of Zn and Sb in MW-3 could also be attributed to the stainless steel, but
they were not significant enough to be a concern. Similarly, a slight increase in Mo was
observed upon ERT probe installation, but the presence of Mo in baseline monitoring and
decreasing concentrations during the experiment suggest that the probes were not a significant
influence on Mo response.
Type III: Significant response to CO2
There is a growing amount of evidence that Type III constituents will be the most likely to be
mobilized in the event of CO2 leakage into a freshwater aquifer. They are ubiquitous in geologic
materials, commonly associated with ion exchange sites, bound within readily soluble carbonate
minerals, or exist as components of soluble oxides or sulfides. The susceptibility of these same
constituents to release from carbonated conditions is reported by laboratory studies (Lu et al.,
2010; Smyth et al., 2009; Little and Jackson, 2010) and a field test at a very similar geologic
setting (Yang et al., 2013). Varadharajan et al. (2013) performed carbonated water leaching tests
on sediments from the current test aquifer and concluded that fast-acting processes such as cation
exchange and carbonate dissolution could be largely responsible for increased concentrations of
many ions. Selective extractions showed that Ca, Mg, Na, K, Si, Al, Ba, Sr and Mn could be
mobilized by all sediment types through fast-acting mechanisms such as cation exchange or
107
carbonate dissolution. A sample of organic-rich sand from the aquifer leached these elements as
much as an order of magnitude higher in concentration than the sandy bulk aquifer sediments.
Assuming cation exchange is an important mechanism, there are multiple possibilities for a
cation exchange trigger, including calcium from dissolution of carbonate minerals, iron from
pyrite dissolution or simply protonation of exchange surfaces. Varadharajan et al. (2013)
reported evidence of calcite in the bulk sandy aquifer sediments identified using micro X-ray
spectroscopy. Based upon saturation indices alone, carbonates may have been a source of Ca,
Mg, Mn and Fe (Figure 4.19).
Figure 4.19 Saturation indices of siderite, calcite, dolomite and rhodochrosite, suggesting the
possibility of carbonate dissolution and release of Ca, Mg, Mn and Fe.
-2.0
-1.5
-1.0
-0.5
0.0
0.5
1.0
1.5
8/10/10 2/26/11 9/14/11 4/1/12 10/18/12
Sid
eri
te S
I
Date
-4.0
-3.5
-3.0
-2.5
-2.0
-1.5
-1.0
-0.5
0.0
0.5
8/10/10 2/26/11 9/14/11 4/1/12 10/18/12
Cal
cite
SI
Date
-3.0
-2.5
-2.0
-1.5
-1.0
-0.5
0.0
0.5
1.0
8/10/10 2/26/11 9/14/11 4/1/12 10/18/12
Rh
od
och
rosi
teSI
Date
-8.0
-7.0
-6.0
-5.0
-4.0
-3.0
-2.0
-1.0
0.0
1.0
8/10/10 2/26/11 9/14/11 4/1/12 10/18/12
Do
lom
ite
SI
Date
108
Another possible cation exchange trigger is Fe released from pyrite dissolution. The rise in
Eh values as the CO2 plume migrated through the aquifer may be attributable to equilibrium with
pyrite (Figure 4.20), which was found in both euhedral and framboidal form in the organic-rich
sediments and detected by x-ray diffraction in the sandy and clay-rich sediments. Field-
measured pH and Eh values during the test period agree well with the theoretical redox couple
for FeS2/SO42-
, suggesting that pyrite dissolution may be an important factor for ion exchange
reactions.
Figure 4.20 Eh-pH diagram illustrating stability fields of ferrous iron, Fe(OH)3am, and pyrite.
5.1.3. Type IV: Decreasing response to CO2
Some constituents decreased in concentration during the CO2 injection test. For NH3,
methane and acetic acid, the decrease could have been in response to changes in redox conditions
or disruption of the dissolved gas phase equilibrium. Molybdenum and F, as oxyanions, may
have been immobilized through adsorption under acidified conditions. The relationship between
109
Mo and pH is indicative of oxyanion sorption behavior (Figure 4.21), and is very similar in both
concentrations and relationship to pH to that reported by Smedley et al. (2014) for streamwaters
in England and Wales.
Figure 4.21 Relationship between molybdenum and pH during the experiment.
5.1.4. Impacts of site heterogeneity on data interpretations
The groundwater chemical data interpretations presented here must also be considered in the
context of companion studies, including cross-well resistivity monitoring (Wu et al., 2012) and
laboratory sediment characterization studies (Varadharajan et al., 2013). Cross-well resistivity
monitoring coupled with downhole gamma ray logs provided clear evidence that vertical
physical heterogeneity in the aquifer created discrete flow paths for the injected dissolved CO2
and resulting high-conductivity plumes (Figure 4.22). Resistivity inversions of near-borehole
data for MW-3 revealed that the initial decreases in resistivity occurred near the top of the well
110
(interval 1) at approximately 10 days, followed by appearance of two discrete low resistivity
plumes arriving simultaneously at 21 days in the middle-upper and lower portions of the aquifer
(intervals 2 and 3). These portions of the aquifer are characterized by relatively low gamma-ray
emissions, typical of coarser-grained sand intervals with relatively higher permeability than silt-
and clay-bearing zones. At 23 days, a low-resistivity signature was observed in the middle
portion of the aquifer (interval 4), peaking at nearly 31 days and passing through MW-3
sometime after 44 days.
Figure 4.22 Cross-well resistivity monitoring results (Wu et al., 2012), illustrating progression of
high-conductivity plume past MW-3 over time.
Laboratory sediment characterizations of these discrete flow paths are available, and provide
a unique opportunity to identify depth-discrete impacts in an otherwise depth-integrated
111
monitoring system. All intervals are composed primarily of quartz sand, with varying amounts
of clay minerals, feldspars and sulfides. The bulk sand (intervals 2 and 3) contains very small
amounts of calcite and exhibited the lowest measured cation exchange capacity. The organic-
rich interval (4) contained more abundant pyrite (with some framboidal pyrite identified through
SEM), higher clay (illite) content, and exhibited nearly 4 times higher cation exchange capacity
than the bulk sediment.
Interpretations of the data through coupled geochemical reaction and transport modeling
must consider not only the presence of physical and geochemical heterogeneity, but also the
averaging effect of a typical monitoring well in a heterogeneous aquifer. It is reasonable to
conclude based on the resistivity monitoring and companion laboratory study results that the
dissolved CO2 plume progressed through the aquifer impacting different geochemical
environments at variable flow rates. While this heterogeneity was obvious using geophysical
methods and detailed laboratory experiments, it must be considered that the monitoring well
measurement is an averaged concentration of all contributions from the target aquifer,
dampening the potential impact of the thinner and less permeable organic-rich layer.
6. Conclusions
The test showed that the primary constituents of concern due to CO2 intrusion into a
sandy aquifer system are major and minor cations. These cations were likely released due to
cation exchange triggered by dissolution of trace carbonate or pyrite in the aquifer. No
constituent exceeded a level of regulatory concern in this test, although some trace elements did
show statistically significant exceedances above baseline concentrations. These elements were
most likely sourced from a thin organic-rich layer and associated with pyrite dissolution or
112
exchange sites on organic matter or clay minerals. Cobalt and Ni were likely elevated during the
experiment, at least in part, due to leaching of stainless steel components of downhole
geophysical monitoring equipment. Certain oxyanions appeared to be immobilized by the CO2
plume, providing useful insight regarding a potential remedial technique for oxyanions in
groundwater.
The study showed that downhole pH and conductivity measurements provided adequate,
low-cost methods for detecting the arrival of a dissolved CO2 plume in an aquifer. Constituents
such as alkalinity or major cations do not provide useful indicator parameters due to their “pulse-
like” response to the advancing CO2 plume. More complex methods such as cross-well
resistivity provided the most informative information regarding the nature of plume movement in
the aquifer, but is less likely to be practical in a detection monitoring application. Companion
laboratory experiments provided insight as to the important geochemical mechanisms to
consider, and informed the interpretation of temporal trends observed in site monitoring wells.
Overall, this study represents a well-designed and implemented controlled CO2 release
field test that provides valuable information to the regulatory community and public regarding
the risk of CO2 leakage into drinking water aquifers. At the current site, the impact of CO2
leakage to the aquifer was primarily limited to mobilization of major and minor cations. The site
is considered representative of a sandy, coastal plain aquifer, located in a region of the United
States that contains vast deep geologic sequestration opportunities. Continued research into the
risks associated with geologic sequestration of CO2 should facilitate decision-making and
permitting efforts related to full-scale CO2 mitigation efforts.
113
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CO2 leakage from geologic CO2 sequestration. Environmental Science and Technology.
Vol. 44, No. 23, pp. 9213−9218.
Yang, C., Mickler, P.J., Reedy, R., Scanlon, B.R., Romanak, K.D., Nicot, J.-P., Hovorka,S.D.,
Trevino, R.H., Larson, T., 2013. Single-well push–pull test for assessing potential
impacts of CO2 leakage on groundwater quality in a shallow Gulf Coast aquifer in
Cranfield, Mississippi. International Journal of Greenhouse Gas Control,
http://dx.doi.org/10.1016/j.ijggc.2012.12.030.
Yang, C., Mickler, P.J., Reedy, R., Scanlon, B.R., Romanak, K.D., Nicot, J.-P., Hovorka,S.D.,
Trevino, R.H., Larson, T., 2013. Single-well push–pull test for assessing potential
impacts of CO2 leakage on groundwater quality in a shallow Gulf Coast aquifer in
Cranfield, Mississippi. International Journal of Greenhouse Gas Control,
http://dx.doi.org/10.1016/j.ijggc.2012.12.030.
Zheng, L., J.A. Apps, Y. Zhang, T. Xu, and J.T. Birkholzer, 2009. On mobilization of lead and
arsenic in groundwater in response to CO2 leakage from deep geological storage.
Chemical Geology, Vol. 268, No. 3-4, pp. 281-297.
115
Chapter 5
SUMMARY
Carbon capture and storage (CCS), specifically by means of geologic sequestration (GS),
is a developing technology to reduce CO2 emissions to the atmosphere. This technology
involves separating CO2 from flue gas and transporting the CO2 to underground storage locations
that are isolated from the atmosphere. These storage locations are typically permeable and
porous geologic formations that are not useful for any other purpose, such as drinking water.
The objectives of this study were to:
1. Investigate whether sequestered CO2 released from a geologic storage reservoir will
have an adverse impact on underground sources of drinking water from a dominantly
quartz-rich aquifer, and
2. Identify geochemical mechanisms responsible for releasing elements under
carbonated conditions.
In order to achieve these objectives, a thorough geochemical and physical characterization of a
test aquifer was conducted, dissolved CO2 was injected into the test aquifer, and the groundwater
monitored for metals mobilization.
In Chapter 2, the baseline geochemical and physical characterization of the test site were
documented and compared to other sites in the Southeastern United States. The site was found
to be a well-confined aquifer with physical and chemical characteristics that are similar to other
United States gulf coastal plain aquifers. A geochemical model based upon the concept of
aquifer freshening showed that ion exchange is a dominant factor affecting major ion
116
composition of the aquifer. Sediment analysis revealed that clay and sulfide minerals likely play
an important role in affecting the trace element composition of the aquifer.
Chapter 3 documented the design and implementation of the field test so that test results
could be properly interpreted and modeled. Site selection was a key part of the study. Due to
the potential volatility of injected dissolved carbon dioxide, it was critical that the aquifer was
well-confined and that the fluid delivery system operated in a closed loop. This concept has not
been duplicated in similar field efforts. Process monitoring during the test proved that injection
test was conducted with minimal disturbance to temperature and pressure, key factors affecting
gas solubility. Injectate maintained a consistently low pH of approximately 5, so that response in
downgradient monitoring wells was obvious. Downhole monitoring of pH and conductivity
provided high-resolution data that were used to interpret and substantiate aquifer chemical and
physical characteristics that were the subject of Chapter 2. Additionally, a backpressure
sampling system was developed and proved necessary to obtain surface pH measurements
similar to downhole pH measurements.
Chapter 4 focused on interpreting the dissolved chemical data during the test, comparing
the post-injection data to pre-injection conditions. There were no exceedances of US EPA
maximum contaminant levels during the test, although statistically significant increases above
background values were documented for a variety of constituents. Based on the observed
temporal trends and statistical evaluation, the responses of various constituents to CO2 can be
grouped into four major behavioral categories: Types I, II, III and IV. Type I constituents (Al,
Sb, As, Be, Cd, Cu, Pb, Hg, P, Se, Ag, Tl, Br, Cl, NO3, NO2, SO4, H2S) were either not detected
throughout the duration of the experiment, or they did not show significant or sustained
deviations from background conditions. Type II constituents (Co, Ni, Zn) did exhibit some
117
apparent response to CO2, but are known to or are highly likely to have been sourced from
stainless steel components of ERT probes installed for purposes of resistivity monitoring during
the test. Type III constituents (Ca, Mg, Ba, Sr, Fe, Mn, Na, Si, alkalinity, K, Li, Cr) are those
which consistently exceeded baseline concentrations during the test at all wells, and displayed
very similar temporal trends throughout the test. Type IV constituents (NH3, CH4, acetic acid,
Mo, F) exhibited an overall decreasing trend in response to CO2.
The key results of the study include:
1. The impact of elevated dissolved CO2 on a Gulf coastal plain aquifer system can be
simulated in the field with careful control over the site selection, fluid delivery system
design and monitoring techniques.
2. pH and conductivity are valuable indicator parameters for detecting impacts
groundwater resulting from elevated dissolved CO2. Accurate pH measurements are
critical, and a backpressure sampling system proved valuable in obtaining accurate
surface pH measurements.
3. No constituent exceeded a US EPA maximum contaminant level in response to
elevated CO2, although statistically significant exceedances over background were
shown for many constituents.
4. Intrawell statistical methods are preferred over interwell statistical methods, and pre-
disturbance chemical data is critical to understanding impacts.
5. The major impact of elevated dissolved CO2 at the study site was an increase in major
and minor cations, most likely due to ion exchange reactions. Dissolution of pyrite or
carbonates are likely associated with triggering ion exchange reactions.
118
6. Many constituents either showed no response or decreased in concentration as a result
of elevated CO2. This may be attributable to increased adsorption tendency of
oxyanions such as arsenic and fluoride at lower pH.
If geologic sequestration occurs at full-scale projects in the United States Gulf Coast
region, the results of this study suggest that impacts at sites similar to the Plant Daniel site in
Mississippi are limited in increases in major and minor cations at levels below established
drinking water standards.
For constituents such as molybdenum and fluoride, dissolved CO2 may act to remove the
element from the dissolved phase. This observation provides a possible research path forward
for site remediation development where the constituents of concern may include oxyanions.
Additional research could be conducted to further understand the effect of site heterogeneity on
dissolved groundwater chemistry. Chapter 4 and other studies are finding substantial evidence
that data interpretations can be complicated by the presence of vertical and horizontal chemical
and physical heterogeneity in aquifers. Baseline chemical data from relatively closely spaced
monitoring wells show significant non-stationarity, precluding the use of interwell statistical
methods even for a relatively homogeneous site. Given the degree of non-stationarity observed
at this relatively homogeneous coastal plain aquifer, the adequacy of interwell statistical methods
at any site should be questioned.
119
APPENDICES
120
Table A-1. Field parameter data
Well Date Temp DO Eh pH Conductivity Ferrous
Fe
Field
H2S
Field Alkalinity
Celcius mg/L mV S.U. umhos/cm mg/L mg/L mg/L as CaCO3
BG-1 9/2/2010 23.60 0.08 -253 8.25 669
BG-1 10/6/2010 21.90 0.10 -61 7.86 682 0.07 319
BG-1 10/29/2010 21.70 0.14 -95 8.41 637 0.29 0.00 275
BG-1 12/3/2010 22.70 0.58 -204 8.59 706 0.31 0.00 321
BG-1 12/27/2010 21.60 0.41 -181 7.85 685 0.09 0.00 300
BG-1 1/25/2011 22.80 0.01 -225 7.84 690 0.28 0.00 310
BG-1 2/23/2011 21.80 0.15 -27 7.67 648 0.43 0.00 290
BG-1 5/18/2011 22.20 0.07 -260 8.24 670 0.07 0.24 264
BG-1 6/22/2011 23.90 0.04 -184 8.08 657 0.27 0.00 300
BG-1 7/18/2011 23.30 0.02 -175 8.57 677 0.12 0.00 280
BG-1 9/7/2011 22.20 0.28 -30 8.39 668 0.07 0.16 326
BG-1 9/14/2011 22.40 0.25 -27 8.34 676 0.01 0.16 319
BG-1 9/21/2011 22.00 0.26 -119 8.21 668 0.14 0.16 322
BG-1 9/28/2011 21.70 0.25 -123 8.19 671 0.21 0.16 326
BG-1 10/19/2011 21.80 0.12 -238 7.78 673 0.02 0.16 326
BG-1 11/10/2011 21.80 0.20 -230 8.36 683 0.05 0.16 336
BG-1 12/1/2011 21.50 0.18 -231 8.30 637 0.02 0.11 325
BG-1 3/15/2012 21.90 0.16 -218 8.23 662 0.02 0.00 339
BG-1 4/11/2012 22.40 0.21 -175 8.11 663 0.04 0.00 276
BG-1 10/4/2012 23.70 -216 8.24 681 0.16 297
BG-1 1/14/2013 21.20 0.09 -230 8.11 661 0.16 0.00 277
IW-1 9/2/2010 23.50 0.08 -319 8.18 656
IW-1 12/3/2010 23.10 0.14 -121 8.52 713 0.30 0.00 302
IW-1 12/28/2010 22.30 0.04 -231 7.81 692 0.47 0.00 310
IW-1 1/26/2011 22.30 0.02 -188 7.84 682 0.38 0.00 290
IW-1 2/22/2011 21.80 1.53 -10 7.99 656 0.01 0.00 308
IW-1 10/5/2012 23.40 19 5.44 607 0.24 245
MW-1 2/12/2010 22.30 0.24 -210 7.08 657
121
Well Date Temp DO Eh pH Conductivity Ferrous
Fe
Field
H2S
Field Alkalinity
Celcius mg/L mV S.U. umhos/cm mg/L mg/L mg/L as CaCO3
MW-1 6/28/2010 23.00 0.47 -82 7.46 644
MW-1 8/25/2010 24.00 0.22 -101 7.75 621 0.44
MW-1 10/5/2010 22.10 0.24 -171 7.36 645 0.42 0.00 305
MW-1 10/28/2010 21.90 0.24 -26 7.56 623 0.55 0.00 287
MW-1 12/3/2010 22.10 0.11 -163 8.32 670 0.38 0.00 308
MW-1 12/29/2010 22.50 0.16 -180 7.64 685 0.64 0.00 312
MW-1 1/26/2011 22.70 0.02 -156 7.58 664 0.36 0.00 310
MW-1 2/23/2011 21.90 0.34 -16 7.56 639 0.58 0.00 290
MW-1 5/19/2011 22.20 0.14 -217 7.78 639 0.55 0.00 265
MW-1 6/21/2011 25.20 0.27 -137 7.77 645 0.32 0.00 300
MW-1 7/19/2011 23.30 0.12 -17 7.71 643 0.21 0.00 290
MW-1 9/8/2011 22.00 0.39 -13 7.62 631 0.49 0.00 309
MW-1 9/16/2011 22.00 0.40 -103 7.80 640 0.58 0.00 312
MW-1 9/22/2011 22.20 0.21 -114 7.71 641 0.27 0.00 316
MW-1 9/28/2011 22.20 0.30 -119 7.85 646 0.62 0.00 315
MW-1 10/19/2011 21.90 0.30 -194 7.70 641 0.31 0.00 319
MW-1 11/10/2011 21.90 0.23 -190 7.75 659 0.54 0.00 320
MW-1 12/1/2011 22.00 0.18 -187 7.75 611 0.56 0.00 314
MW-1 1/6/2012 21.90 0.37 -194 7.78 631 0.06 0.00 310
MW-1 1/9/2012 22.00 0.70 -180 7.75 579 0.04 0.00
MW-1 1/11/2012 21.30 0.56 -182 7.91 593 0.05 0.00 320
MW-1 1/13/2012 21.50 0.24 -189 8.25 577 0.16 0.00 300
MW-1 1/16/2012 22.00 0.53 -180 7.73 623 0.47 0.00 313
MW-1 1/18/2012 21.80 0.62 -179 7.76 623 0.48 0.00 311
MW-1 1/20/2012 21.90 0.44 -174 7.69 627 0.35 0.00 309
MW-1 1/23/2012 21.90 0.45 -184 7.72 640 0.40 0.00 313
MW-1 1/30/2012 21.80 0.37 -185 7.71 648 0.52 0.00 310
MW-1 2/1/2012 21.70 0.10 -184 7.70 644 0.48 0.00 310
MW-1 2/3/2012 21.70 0.22 -175 7.61 631 0.56 0.00 300
MW-1 2/6/2012 21.60 0.15 -168 7.54 656 0.48 0.00 295
122
Well Date Temp DO Eh pH Conductivity Ferrous
Fe
Field
H2S
Field Alkalinity
Celcius mg/L mV S.U. umhos/cm mg/L mg/L mg/L as CaCO3
MW-1 2/8/2012 21.80 0.17 -166 7.43 684 0.66 0.00 295
MW-1 2/10/2012 21.60 0.13 -146 7.34 723 0.48 0.00 290
MW-1 2/13/2012 21.80 0.15 -127 7.28 814 1.66 0.00 256
MW-1 2/15/2012 21.80 0.30 -110 7.04 879 2.34 0.00 437
MW-1 2/17/2012 21.80 0.18 -96 6.79 942 2.80 0.00 488
MW-1 2/29/2012 21.90 0.35 -43 6.05 1226 3.22 0.00 641
MW-1 3/2/2012 21.90 0.27 -125 6.01 1208 5.80 0.00 649
MW-1 3/5/2012 22.00 0.28 -38 5.94 1229 4.40 0.11 643
MW-1 3/7/2012 21.90 0.20 -89 5.83 1187 5.20 0.05 647
MW-1 3/9/2012 21.80 0.27 -27 5.75 1199 5.40 0.05 648
MW-1 3/12/2012 21.80 0.20 13 5.67 1166 6.00 0.11 643
MW-1 3/14/2012 22.10 0.13 -36 5.50 1133 6.00 0.05 616
MW-1 3/19/2012 22.00 0.23 -86 5.63 1110 6.00 0.11 589
MW-1 3/21/2012 21.90 0.40 -42 5.61 1165 6.00 0.11 575
MW-1 3/23/2012 22.00 0.26 -6 5.53 1083 6.40 0.00 585
MW-1 3/26/2012 21.80 0.81 8 5.66 1142 2.12 0.00 574
MW-1 4/2/2012 22.00 0.54 31 5.10 1114 6.60 0.00 561
MW-1 4/9/2012 22.00 0.30 15 5.68 881 1.90 0.00
MW-1 4/12/2012 21.60 0.20 31 5.57 1091 5.00 0.00 450
MW-1 4/16/2012 22.00 0.57 41 5.65 1154 3.04 536
MW-1 10/5/2012 22.00 -19 6.01 1045 2.76 448
MW-1 1/15/2013 21.70 0.14 -11 6.04 982 2.70 444
MW-2 2/12/2010 22.10 0.13 -270 7.14 659
MW-2 6/28/2010 23.40 0.23 -31 7.50 628
MW-2 8/25/2010 23.20 0.15 -49 7.93 614 0.14
MW-2 10/5/2010 21.80 0.14 -173 7.61 641 0.21 307
MW-2 10/28/2010 21.80 0.18 -95 7.83 623 0.46 285
MW-2 12/2/2010 22.60 0.14 -183 8.31 673 0.23 0.00 302
MW-2 12/28/2010 22.40 0.33 -186 7.61 684 0.00 290
MW-2 1/26/2011 22.30 0.02 -214 7.72 674 0.26 0.00 275
123
Well Date Temp DO Eh pH Conductivity Ferrous
Fe
Field
H2S
Field Alkalinity
Celcius mg/L mV S.U. umhos/cm mg/L mg/L mg/L as CaCO3
MW-2 2/22/2011 21.70 0.15 -23 7.57 637 0.55 0.00 292
MW-2 5/20/2011 22.40 0.12 -234 7.93 644 0.45 0.00 243
MW-2 6/21/2011 24.50 0.33 -151 7.95 649 0.31 0.00 284
MW-2 7/19/2011 25.00 0.13 -116 7.81 650 0.18 0.00 270
MW-2 9/7/2011 22.00 0.39 -49 7.90 635 0.42 0.00 314
MW-2 9/15/2011 22.00 0.29 -69 7.70 643 0.42 0.00 308
MW-2 9/21/2011 22.00 0.25 -139 7.82 642 0.58 0.00 305
MW-2 9/28/2011 21.80 0.24 -118 7.88 646 0.60 0.00 318
MW-2 10/19/2011 21.70 0.14 -209 7.39 643 0.38 0.00 314
MW-2 11/10/2011 21.80 0.23 -207 7.96 658 0.09 0.00 322
MW-2 11/16/2011 21.90 0.25 -200 7.73 652 0.05 0.00 308
MW-2 12/1/2011 21.80 0.21 -193 7.83 607 0.42 0.00 320
MW-2 12/7/2011 21.70 0.16 -188 7.85 639 0.34 0.00 319
MW-2 12/14/2011 21.80 0.21 -188 7.77 656 0.35 0.00 316
MW-2 1/6/2012 21.90 0.25 -49 6.35 897 5.00 0.00 378
MW-2 1/9/2012 21.90 0.46 -36 6.26 942 6.40 0.00
MW-2 1/11/2012 21.30 0.48 -56 6.41 942 5.50 0.00 350
MW-2 1/13/2012 21.40 0.40 -45 6.39 975 6.00 0.00 360
MW-2 1/16/2012 21.90 0.36 1 5.78 1079 4.40 0.00 557
MW-2 1/18/2012 21.70 0.31 10 5.81 1046 4.60 0.00 541
MW-2 1/20/2012 21.90 0.30 11 5.64 1014 6.00 0.00 551
MW-2 1/23/2012 21.80 0.25 17 5.70 1030 5.40 0.00 535
MW-2 1/27/2012 21.70 0.17 2 5.65 989 5.20 0.00 260
MW-2 1/30/2012 21.70 0.39 -3 5.69 958 5.60 0.00 310
MW-2 2/1/2012 21.80 0.22 -10 5.71 952 6.00 0.00 330
MW-2 2/3/2012 21.70 0.26 4 5.58 913 6.60 0.00 348
MW-2 2/6/2012 21.50 0.26 -4 5.62 898 6.40 0.00 335
MW-2 2/8/2012 21.70 0.20 -11 5.59 878 6.40 0.00 320
MW-2 2/10/2012 21.60 0.19 8 5.62 870 6.40 0.00 340
MW-2 2/13/2012 21.80 0.17 25 5.64 877 6.00 0.00 432
124
Well Date Temp DO Eh pH Conductivity Ferrous
Fe
Field
H2S
Field Alkalinity
Celcius mg/L mV S.U. umhos/cm mg/L mg/L mg/L as CaCO3
MW-2 2/15/2012 21.70 0.39 32 5.42 872 7.40 0.00 423
MW-2 2/17/2012 21.80 0.23 41 5.29 860 2.90 0.00 425
MW-2 2/29/2012 21.70 0.39 -4 5.41 796 2.69 0.00 387
MW-2 3/2/2012 21.80 0.23 -71 5.09 788 7.20 0.00 440
MW-2 3/5/2012 21.90 0.51 16 5.35 769 6.20 0.00 377
MW-2 3/7/2012 21.70 0.18 -45 5.23 761 5.60 0.00 379
MW-2 3/9/2012 21.70 0.26 -9 5.40 763 6.40 0.00 380
MW-2 3/12/2012 21.70 0.15 32 5.33 749 6.40 0.00 375
MW-2 3/14/2012 21.80 0.24 -13 5.40 746 6.80 0.00 366
MW-2 3/19/2012 21.70 0.25 -45 4.74 751 6.60 0.00 366
MW-2 3/21/2012 21.80 0.33 -10 5.05 753 6.60 0.00 355
MW-2 3/23/2012 21.70 0.30 3 5.30 750 7.00 0.00 373
MW-2 3/26/2012 21.80 0.42 34 4.67 787 2.10 0.00 377
MW-2 4/2/2012 21.90 0.24 37 5.10 793 7.60 0.00 404
MW-2 4/9/2012 21.90 0.35 14 5.44 636 5.80 0.00
MW-2 4/11/2012 21.90 0.27 39 5.29 798 6.10 0.00 265
MW-2 4/16/2012 21.80 0.21 34 5.28 850 6.00 0.00 384
MW-2 10/4/2012 23.90 -19 5.56 856 4.24 350
MW-2 1/14/2013 21.50 0.21 42 5.61 864 4.51 315
MW-3 9/2/2010 26.80 0.08 -285 8.24 663
MW-3 10/5/2010 22.10 0.16 -138 7.47 641 0.11 0.00 313
MW-3 10/28/2010 22.10 0.45 -122 8.03 633 0.15 0.00 305
MW-3 12/2/2010 21.70 0.15 -188 8.41 679 0.22 0.00 291
MW-3 12/28/2010 22.70 0.04 -227 7.81 690 0.51 0.00 304
MW-3 1/24/2011 22.10 0.03 -191 7.88 675 0.13 0.00 285
MW-3 2/22/2011 21.80 0.52 -27 7.77 649 0.34 0.00 292
MW-3 5/19/2011 22.30 0.06 -276 8.48 653 0.05 0.00 258
MW-3 6/21/2011 23.50 0.02 -91 7.97 676 0.20 0.00 290
MW-3 7/19/2011 24.70 0.64 -75 8.69 664 0.26 0.00 300
MW-3 7/20/2011 24.20 0.09 -175 8.40 657
125
Well Date Temp DO Eh pH Conductivity Ferrous
Fe
Field
H2S
Field Alkalinity
Celcius mg/L mV S.U. umhos/cm mg/L mg/L mg/L as CaCO3
MW-3 7/21/2011 23.70 0.06 -202 8.37 646
MW-3 8/21/2011 22.10 0.14 -260 8.14 666 0.22 0.00 275
MW-3 9/1/2011 22.00 0.24 -236 8.14 635 0.42 0.00 317
MW-3 9/8/2011 22.10 0.13 -200 8.31 637 0.21 0.00 309
MW-3 9/15/2011 22.00 0.20 -219 8.15 640 0.30 0.00 311
MW-3 9/22/2011 22.10 0.16 -227 8.30 643 0.24 0.00 324
MW-3 9/28/2011 22.20 0.32 -243 8.34 651 0.27 0.00 303
MW-3 10/5/2011 22.30 0.17 -160 8.19 638 0.00
MW-3 10/12/2011 22.10 0.18 -261 8.21 641 0.21 0.00 306
MW-3 10/17/2011 22.30 0.20 -254 8.22 641 0.18 0.00 299
MW-3 10/19/2011 22.10 0.19 -253 8.15 640 0.25 0.00 300
MW-3 10/21/2011 22.10 0.12 -242 8.29 639 0.23 0.00 311
MW-3 10/24/2011 22.30 0.14 -239 8.24 624 0.29 0.00 313
MW-3 10/26/2011 22.20 0.10 -234 8.00 626 0.26 0.00 301
MW-3 10/28/2011 22.20 0.15 -176 7.41 658 2.15 0.00 327
MW-3 10/31/2011 22.20 0.20 -80 6.43 779 1.98 0.00 359
MW-3 11/2/2011 22.10 0.21 -67 6.18 888 2.33 0.00 434
MW-3 11/4/2011 21.90 0.38 -52 5.98 1043 1.40 0.00 527
MW-3 11/9/2011 22.20 0.35 -45 5.75 1105 2.89 0.00 556
MW-3 11/10/2011 22.00 0.32 -11 5.54 1082 3.38 0.00 562
MW-3 11/11/2011 21.90 0.41 -10 5.70 1075 3.30 0.00 564
MW-3 11/14/2011 21.80 0.29 -19 5.64 975 3.30 0.00 510
MW-3 11/16/2011 21.90 0.26 5 5.53 950 3.30 0.00 487
MW-3 11/18/2011 21.80 0.23 9 5.62 901 3.14 0.00 467
MW-3 11/21/2011 22.00 0.33 9 5.38 781 3.14 0.12 412
MW-3 11/23/2011 21.90 0.30 16 5.32 762 5.50 0.00 382
MW-3 11/25/2011 21.80 0.29 8 5.52 722 6.50 0.00 370
MW-3 11/28/2011 21.60 0.28 28 5.58 664 6.00 0.11 345
MW-3 11/30/2011 21.70 0.36 36 5.48 679 4.50 0.11 333
MW-3 12/2/2011 21.80 0.22 29 5.53 674 5.00 0.05 323
126
Well Date Temp DO Eh pH Conductivity Ferrous
Fe
Field
H2S
Field Alkalinity
Celcius mg/L mV S.U. umhos/cm mg/L mg/L mg/L as CaCO3
MW-3 12/5/2011 21.80 0.33 38 5.38 691 5.00 0.05 323
MW-3 12/7/2011 21.50 0.29 23 5.40 685 4.50 0.11 311
MW-3 12/14/2011 21.80 0.27 42 5.40 700 6.00 0.00 316
MW-3 1/4/2012 21.60 0.35 65 5.64 650 6.00 0.00 303
MW-3 3/15/2012 22.00 0.11 50 4.66 628 2.29 0.00 266
MW-3 4/12/2012 21.70 0.30 32 5.29 622 4.00 0.00 220
MW-3 10/5/2012 22.30 30 5.51 695 2.54 276
MW-3 1/15/2013 21.20 0.16 74 5.51 627 2.45 270
MW-4 9/2/2010 24.00 0.01 -189 8.18 670 0.24
MW-4 10/5/2010 22.20 0.16 -156 7.64 648 0.09 0.00 309
MW-4 10/28/2010 21.80 0.16 -77 7.79 623 0.30 0.00 310
MW-4 12/3/2010 21.90 0.48 -184 8.47 681 0.14 0.00 300
MW-4 12/29/2010 22.10 0.21 -175 7.75 685 0.58 0.00 297
MW-4 1/25/2011 22.60 0.02 -202 7.76 674 0.23 0.00 290
MW-4 2/23/2011 22.10 0.15 -8 7.63 642 0.30 0.00 296
MW-4 5/20/2011 22.50 0.15 -214 7.86 649 0.32 0.00 239
MW-4 6/21/2011 25.50 0.19 -154 7.84 648 0.27 0.00 290
MW-4 7/19/2011 24.40 0.09 -144 7.90 617 0.24 0.00 310
MW-4 9/7/2011 22.00 0.31 10 7.80 631 0.38 0.00 307
MW-4 9/16/2011 22.20 0.26 -127 7.90 639 0.37 0.00 309
MW-4 9/22/2011 22.10 0.31 -88 7.76 642 0.32 0.00 311
MW-4 9/28/2011 22.20 0.27 -105 7.90 645 0.32 0.00 327
MW-4 10/19/2011 22.00 0.22 -198 7.80 639 0.34
MW-4 11/10/2011 21.70 0.19 -195 7.84 656 0.07 0.00 313
MW-4 12/1/2011 21.90 0.34 -183 7.84 607 0.28 0.00 314
MW-4 3/14/2012 22.00 0.11 -143 6.85 630 0.27 0.00 299
MW-4 3/19/2012 22.00 0.19 -162 7.55 643 0.22 0.00 314
MW-4 3/21/2012 22.00 0.36 -174 7.58 638 0.32 0.11 318
MW-4 3/23/2012 21.80 0.38 -148 7.53 638 0.26 0.05 321
MW-4 3/26/2012 22.00 0.34 -144 7.59 675 0.14 0.00 332
127
Well Date Temp DO Eh pH Conductivity Ferrous
Fe
Field
H2S
Field Alkalinity
Celcius mg/L mV S.U. umhos/cm mg/L mg/L mg/L as CaCO3
MW-4 4/2/2012 22.00 0.24 -115 7.02 667 0.35 0.00 328
MW-4 4/9/2012 21.90 0.21 -107 7.44 558 0.54 0.00
MW-4 4/11/2012 22.00 0.18 -78 7.22 710 0.48 0.00 290
MW-4 4/16/2012 21.90 0.26 -52 7.09 772 0.86 0.00 367
MW-4 10/4/2012 24.20 -42 6.16 1164 2.18 0.00 425
MW-4 1/15/2013 21.50 0.16 -7 6.06 1112 2.10 0.00 415
PW-1 2/12/2010 22.50 0.06 -318 7.56 663
PW-1 6/28/2010 23.30 0.33 -45 8.38 666
PW-1 8/25/2010 24.20 0.18 -102 8.56 656 0.02
PW-1 12/4/2010 21.70 0.08 -180 8.39 673 0.38 0.00 299
PW-1 12/27/2010 22.60 0.10 -216 7.74 679 0.15 0.00 295
PW-1 1/25/2011 23.30 0.02 -222 7.72 673 0.36 305
PW-1 2/24/2011 22.20 0.35 3 7.70 639 0.31 308
128
Table A-2. Major and minor cation concentrations.
Well Date Al Ba Ca Fe Li Mg Mn K Si Na Sr
mg/L mg/L mg/L mg/L mg/L mg/L mg/L mg/L mg/L mg/L mg/L
BG-1 9/2/2010 0.1 0.04 2.5 0.24 0.024 0.94 0.04 2.7 12 150 0.084
BG-1 10/6/2010 0.032 0.027 2.5 0.18 0.021 0.81 0.025 2.4 11 160 0.091
BG-1 10/29/2010 0.03 0.044 2.8 0.58 0.02 0.98 0.061 2.4 11 160 0.1
BG-1 12/3/2010 0.028 0.044 2.5 0.58 0.021 1 0.055 2.8 11 150 0.095
BG-1 12/27/2010 0.03 0.046 2.6 0.6 0.02 0.93 0.054 2.3 12 160 0.086
BG-1 1/25/2011 <0.023 0.049 3.2 0.57 0.022 1.1 0.06 2.8 11 160 0.094
BG-1 2/23/2011 <0.023 0.056 2.9 0.59 0.022 1.2 0.078 2.6 13 140 0.089
BG-1 5/18/2011 0.027 0.045 2.9 0.3 0.029 1.2 0.04 5.1 12 190 0.087
BG-1 6/22/2011 <0.023 0.049 2.9 0.22 0.03 0.95 0.043 5.7 11 180 0.098
BG-1 7/18/2011 0.034 0.048 2.7 0.22 0.04 1.2 0.041 6.8 12 170 0.1
BG-1 9/7/2011 0.024 0.043 2.3 0.14 0.033 0.92 0.036 5.4 12 150 0.093
BG-1 9/14/2011 <0.023 0.048 2.4 0.19 0.033 1 0.046 5 12 160 0.099
BG-1 9/21/2011 <0.023 0.045 2.5 0.23 0.027 1 0.054 3.9 12 160 0.093
BG-1 9/28/2011 <0.023 0.051 3 0.027 1.2 0.067 4.5 12 180 0.1
BG-1 10/19/2011 <0.023 0.042 2.9 0.16 0.033 0.9 0.04 4.7 12 150 0.087
BG-1 11/10/2011 <0.023 0.045 2.2 0.24 0.029 0.86 0.048 3.9 12 140 0.084
BG-1 12/1/2011 <0.023 0.046 2.6 0.3 0.03 0.97 0.053 4.4 12 160 0.089
BG-1 3/15/2012 <0.023 0.043 2.3 0.21 0.034 0.91 0.048 4.8 12 150 0.088
BG-1 4/11/2012 0.054 0.059 2.5 0.42 0.025 0.98 0.067 3.6 12 150 0.094
BG-1 10/4/2012 <0.023 0.049 2.4 0.17 0.065 0.87 0.049 6.8 12 150 0.11
BG-1 1/14/2013 <0.023 0.053 2.9 0.32 0.06 1.1 0.059 7 12 180 0.1
IW-1 9/2/2010 <0.023 0.07 3.6 0.33 0.031 2.1 0.093 4.8 11 150 0.16
IW-1 12/3/2010 0.13 0.078 3.5 0.85 0.042 1.8 0.08 7.5 11 150 0.18
IW-1 12/28/2010 <0.023 0.059 2.9 0.89 0.021 1.5 0.07 2.8 12 140 0.11
IW-1 1/26/2011 <0.023 0.068 4.2 0.73 0.025 1.9 0.077 3.9 11 160 0.14
IW-1 2/22/2011 <0.023 0.044 3.3 0.27 0.019 1.3 0.055 2.9 11 150 0.11
IW-1 10/5/2012 0.035 0.051 2.2 0.92 0.02 1.1 0.045 2.4 13 140 0.078
MW-1 2/12/2010 <0.023 0.06 2.8 0.43 0.021 1.6 0.072 2.9 11 150 0.096
MW-1 6/28/2010 <0.023 0.064 3.3 0.66 0.018 1.7 0.095 2.9 10 160 0.098
MW-1 7/30/2010 <0.023 0.061 2.8 0.65 0.02 1.5 0.093 2.8 11 140 0.1
129
Well Date Al Ba Ca Fe Li Mg Mn K Si Na Sr
mg/L mg/L mg/L mg/L mg/L mg/L mg/L mg/L mg/L mg/L mg/L
MW-1 8/25/2010 <0.023 0.06 3.3 0.69 0.018 1.7 0.096 2.9 10 150 0.099
MW-1 10/5/2010 <0.023 0.063 3 0.72 0.019 1.7 0.1 2.5 11 150 0.11
MW-1 10/28/2010 <0.023 0.056 2.7 0.61 0.021 1.5 0.078 2.9 12 160 0.092
MW-1 12/3/2010 <0.023 0.06 2.5 0.62 0.021 1.6 0.073 3.5 12 160 0.094
MW-1 12/29/2010 <0.023 0.058 2.4 0.61 0.02 1.3 0.066 2.5 12 140 0.082
MW-1 1/26/2011 <0.023 0.06 3 0.59 0.02 1.5 0.075 3 12 160 0.095
MW-1 2/23/2011 <0.023 0.064 3 0.69 0.018 1.4 0.088 3.1 12 150 0.099
MW-1 5/19/2011 <0.023 0.064 3.4 0.8 0.018 1.9 0.092 3.3 12 180 0.093
MW-1 6/21/2011 <0.023 0.065 3.3 0.68 0.017 1.7 0.1 3.3 12 170 0.11
MW-1 7/19/2011 <0.023 0.068 3.1 0.4 0.019 1.8 0.091 3.5 12 150 0.11
MW-1 9/8/2011 <0.023 0.063 2.7 0.84 0.02 1.5 0.086 3.1 12 150 0.096
MW-1 9/16/2011 <0.023 0.059 2.5 0.8 0.021 1.4 0.08 2.8 12 140 0.091
MW-1 9/22/2011 <0.023 0.067 2.8 0.72 0.018 1.6 0.099 2.9 12 160 0.1
MW-1 9/28/2011 <0.023 0.067 3.2 0.31 0.018 1.8 0.096 3.4 12 180 0.11
MW-1 10/19/2011 <0.023 0.062 2.6 0.76 0.018 1.5 0.084 3 12 150 0.092
MW-1 11/10/2011 <0.023 0.059 2.5 0.77 0.019 1.4 0.073 2.6 12 140 0.083
MW-1 12/1/2011 <0.023 0.062 2.7 0.79 0.019 1.5 0.085 3 12 150 0.092
MW-1 1/6/2012 <0.023 0.059 2.8 0.73 0.018 1.5 0.073 2.9 12 150 0.089
MW-1 1/9/2012 0.24 0.057 2.4 0.71 0.018 1.3 0.071 2.9 12 140 0.084
MW-1 1/11/2012 <0.023 0.054 2.3 0.71 0.019 1.3 0.074 2.7 12 140 0.085
MW-1 1/13/2012 <0.023 0.057 2.6 0.72 0.019 1.5 0.072 3 12 150 0.09
MW-1 1/16/2012 <0.023 0.057 2.3 0.71 0.019 1.4 0.075 2.9 12 150 0.09
MW-1 1/18/2012 <0.023 0.055 2.2 0.68 0.019 1.3 0.069 2.8 12 140 0.083
MW-1 1/20/2012 <0.023 0.062 2.2 0.67 0.019 1.5 0.075 3 12 160 0.091
MW-1 1/23/2012 <0.023 0.061 2.5 0.68 0.019 1.7 0.074 3.1 12 160 0.089
MW-1 1/30/2012 <0.023 0.056 2.2 0.69 0.019 1.3 0.069 2.7 12 130 0.083
MW-1 2/1/2012 <0.023 0.059 2.4 0.72 0.019 1.4 0.073 2.9 12 150 0.087
MW-1 2/3/2012 <0.023 0.063 2.5 0.75 0.02 1.5 0.077 3 12 150 0.095
MW-1 2/6/2012 <0.023 0.07 2.9 0.85 0.021 1.7 0.098 3.1 12 170 0.1
MW-1 2/8/2012 <0.023 0.073 2.9 1 0.022 1.8 0.091 3 13 160 0.11
MW-1 2/10/2012 <0.023 0.087 3.4 1.3 0.023 2 0.11 3.6 13 160 0.12
130
Well Date Al Ba Ca Fe Li Mg Mn K Si Na Sr
mg/L mg/L mg/L mg/L mg/L mg/L mg/L mg/L mg/L mg/L mg/L
MW-1 2/13/2012 <0.023 0.25 7.8 1.9 0.025 3.7 0.32 4 14 200 0.28
MW-1 2/15/2012 <0.023 0.14 5 2.6 0.03 2.9 0.17 3.8 15 190 0.2
MW-1 2/17/2012 <0.023 0.15 5.8 3.2 0.033 3.5 0.17 4.5 17 220 0.22
MW-1 2/29/2012 <0.023 0.29 10 7.3 0.047 5.8 0.35 5.6 28 270 0.39
MW-1 3/2/2012 <0.023 0.28 9.7 6.5 0.047 5.6 0.33 5.5 29 270 0.38
MW-1 3/5/2012 <0.023 0.3 11 7.5 0.051 6 0.37 5.9 34 270 0.42
MW-1 3/7/2012 <0.023 0.27 9.1 6.2 0.052 5.2 0.32 5.2 37 240 0.37
MW-1 3/9/2012 <0.023 0.29 10 6.7 0.053 6.1 0.34 6 40 270 0.41
MW-1 3/12/2012 <0.023 0.31 10 7.2 0.057 5.8 0.35 5.8 45 260 0.41
MW-1 3/14/2012 <0.023 0.3 9.9 7 0.055 5.6 0.34 5.6 48 250 0.39
MW-1 3/19/2012 <0.023 0.29 9.7 7.2 0.058 5.6 0.35 5.4 53 250 0.38
MW-1 3/21/2012 <0.023 0.3 10 7.4 0.058 6 0.37 5.6 55 260 0.39
MW-1 3/23/2012 <0.023 0.28 9.5 7.2 0.059 5.5 0.34 5.4 54 240 0.36
MW-1 3/26/2012 <0.023 0.29 9.7 7.3 0.06 5.6 0.35 5.5 55 240 0.38
MW-1 4/2/2012 <0.023 0.3 9.9 7.6 0.063 5.8 0.36 5.8 56 250 0.41
MW-1 4/9/2012 <0.023 0.3 9.7 7.1 0.061 5.6 0.36 5.7 56 240 0.4
MW-1 4/12/2012 <0.023 0.29 9.6 6.3 0.058 5.6 0.36 5.8 50 250 0.39
MW-1 4/16/2012 <0.023 0.3 10 6.6 0.059 6 0.37 5.7 49 260 0.39
MW-1 10/5/2012 <0.023 0.41 12 12 0.049 7.8 0.49 6.1 35 220 0.52
MW-1 1/15/2013 <0.023 0.33 11 11 0.05 6.6 0.42 6.1 33 220 0.4
MW-2 2/12/2010 0.11 0.059 2.7 0.8 0.02 1.4 0.07 2.4 11 150 0.093
MW-2 6/28/2010 <0.023 0.066 2.9 0.63 0.014 1.3 0.065 2.4 9.6 150 0.095
MW-2 7/30/2010 0.024 0.065 2.8 0.54 0.014 1.4 0.066 2.4 10 140 0.1
MW-2 8/25/2010 0.038 0.06 2.9 0.43 0.013 1.3 0.063 2.3 10 150 0.09
MW-2 10/5/2010 0.023 0.069 3.2 0.51 0.015 1.5 0.075 2.3 11 180 0.11
MW-2 10/28/2010 <0.023 0.049 2.1 0.62 0.018 0.9 0.064 2.3 11 150 0.079
MW-2 12/2/2010 <0.023 0.044 1.9 0.58 0.019 0.94 0.05 2.6 12 150 0.073
MW-2 12/28/2010 <0.023 0.054 2.3 0.66 0.018 1.1 0.061 2.2 12 150 0.079
MW-2 1/26/2011 <0.023 0.066 3.2 0.79 0.019 1.4 0.077 2.9 12 170 0.097
MW-2 2/22/2011 <0.023 0.05 2.2 0.7 0.018 0.83 0.057 2.3 12 150 0.075
MW-2 5/20/2011 <0.023 0.06 2.8 0.73 0.015 1.4 0.069 2.6 11 160 0.087
131
Well Date Al Ba Ca Fe Li Mg Mn K Si Na Sr
mg/L mg/L mg/L mg/L mg/L mg/L mg/L mg/L mg/L mg/L mg/L
MW-2 6/21/2011 <0.023 0.076 3.4 0.46 0.013 1.4 0.083 3 10 180 0.12
MW-2 7/19/2011 <0.023 0.062 2.9 0.33 0.016 1.5 0.072 2.6 11 170 0.097
MW-2 9/7/2011 <0.023 0.056 2.3 0.69 0.018 0.96 0.062 2.2 12 150 0.081
MW-2 9/15/2011 <0.023 0.054 2.1 0.76 0.018 0.96 0.062 2.1 12 140 0.078
MW-2 9/21/2011 <0.023 0.059 2.5 0.73 0.018 1.1 0.076 2.2 12 160 0.087
MW-2 9/28/2011 <0.023 0.054 2.6 0.53 0.018 1.1 0.068 2.4 12 170 0.083
MW-2 10/19/2011 <0.023 0.053 2.3 0.7 0.019 0.98 0.061 2.1 11 150 0.075
MW-2 11/10/2011 <0.023 0.05 2.2 0.72 0.018 0.92 0.053 2.2 11 140 0.067
MW-2 11/16/2011 <0.023 0.052 2.3 0.7 0.018 0.98 0.058 2.2 11 160 0.072
MW-2 12/1/2011 <0.023 0.05 2.3 0.71 0.019 0.96 0.058 2.2 12 150 0.071
MW-2 12/7/2011 <0.023 0.053 2.2 0.66 0.017 0.96 0.059 2.2 11 150 0.076
MW-2 12/14/2011 <0.023 0.048 2.3 0.71 0.019 1 0.056 2.3 12 160 0.072
MW-2 1/6/2012 <0.023 0.18 6.2 5.2 0.029 3 0.19 3.4 18 210 0.24
MW-2 1/9/2012 0.22 8.4 8.6 0.034 3.8 0.27 3.8 22 230 0.29
MW-2 1/11/2012 0.27 9.6 13 0.037 4.3 0.38 4.1 23 230 0.38
MW-2 1/13/2012 <0.023 0.31 10 14 0.039 5.3 0.38 4.8 25 250 0.4
MW-2 1/16/2012 <0.023 0.29 8.9 16 0.041 4.5 0.34 4.1 33 230 0.36
MW-2 1/18/2012 <0.023 0.34 10 16 0.043 5.3 0.4 5.2 39 280 0.43
MW-2 1/20/2012 0.031 0.3 9.3 16 0.045 4.9 0.35 4.7 40 240 0.37
MW-2 1/23/2012 <0.023 0.31 9.6 17 0.047 4.7 0.36 4.8 42 230 0.36
MW-2 1/27/2012 <0.023 0.29 9.2 16 0.046 4.5 0.35 4.7 41 220 0.34
MW-2 1/30/2012 <0.023 0.29 8.6 17 0.045 4.2 0.36 4.4 42 210 0.34
MW-2 2/1/2012 <0.023 0.26 7.6 16 0.045 3.6 0.32 4 42 190 0.3
MW-2 2/3/2012 <0.023 0.27 7.7 16 0.048 3.7 0.32 4.2 45 200 0.3
MW-2 2/6/2012 0.027 0.26 8.2 15 0.046 3.9 0.35 4.1 41 210 0.3
MW-2 2/8/2012 <0.023 0.24 7.4 14 0.049 3.5 0.31 3.9 43 200 0.28
MW-2 2/10/2012 <0.023 0.24 7 14 0.049 3.4 0.31 3.9 43 180 0.28
MW-2 2/13/2012 <0.023 0.12 4.9 13 0.045 2.7 0.14 3.6 40 200 0.17
MW-2 2/15/2012 <0.023 0.23 6.6 13 0.052 3.1 0.28 3.7 42 190 0.26
MW-2 2/17/2012 0.031 0.29 9.1 13 0.053 4.5 0.27 5.2 41 230 0.33
MW-2 2/29/2012 0.029 0.2 5.8 10 0.048 2.8 0.26 3.6 35 170 0.22
132
Well Date Al Ba Ca Fe Li Mg Mn K Si Na Sr
mg/L mg/L mg/L mg/L mg/L mg/L mg/L mg/L mg/L mg/L mg/L
MW-2 3/2/2012 <0.023 0.18 5.3 9 0.05 2.6 0.23 3.6 34 170 0.2
MW-2 3/5/2012 0.023 0.17 5.2 8.9 0.048 2.4 0.24 3.3 33 150 0.2
MW-2 3/7/2012 0.023 0.16 5 8.5 0.053 2.3 0.22 3.6 34 170 0.19
MW-2 3/9/2012 0.023 0.18 5.4 8.9 0.05 2.7 0.23 3.9 32 170 0.2
MW-2 3/12/2012 <0.023 0.19 5.6 8.5 0.051 2.7 0.24 3.7 32 170 0.21
MW-2 3/14/2012 <0.023 0.18 5.3 8.7 0.052 2.5 0.23 3.6 32 160 0.2
MW-2 3/19/2012 0.028 0.17 5.3 7.6 0.053 2.5 0.23 3.5 32 170 0.19
MW-2 3/21/2012 0.024 0.19 5.9 8.2 0.054 2.8 0.25 3.9 32 180 0.2
MW-2 3/23/2012 <0.023 0.2 5.9 8.5 0.054 2.9 0.27 3.9 33 170 0.22
MW-2 3/26/2012 <0.023 0.21 6.1 9.1 0.054 3 0.28 3.9 33 170 0.23
MW-2 4/2/2012 <0.023 0.23 7.1 11 0.059 3.6 0.31 4.4 37 170 0.26
MW-2 4/9/2012 <0.023 0.29 8.6 14 0.055 4.3 0.38 5 37 180 0.33
MW-2 4/11/2012 0.025 0.23 7.1 12 0.053 3.4 0.32 4.4 34 170 0.27
MW-2 4/16/2012 <0.023 0.28 8.3 12 0.056 4.1 0.35 4.7 36 170 0.3
MW-2 10/4/2012 <0.023 0.29 8.2 8.5 0.06 4.9 0.32 5.2 39 180 0.34
MW-2 1/14/2013 <0.023 0.29 8.7 8.5 0.061 5.1 0.33 5.7 39 190 0.32
MW-3 9/2/2010 0.37 0.11 6.2 0.094 0.23 1 0.039 0 12 180 0.37
MW-3 10/5/2010 0.03 0.055 3.2 0.36 0.033 1.1 0.042 3 12 180 0.12
MW-3 10/28/2010 <0.023 0.055 3.1 0.35 0.023 1 0.049 2.8 12 160 0.11
MW-3 12/2/2010 <0.023 0.063 3.1 0.37 0.023 1.2 0.055 3.4 12 170 0.13
MW-3 12/28/2010 <0.023 0.06 2.6 0.78 0.021 1.2 0.067 2.2 13 140 0.092
MW-3 1/24/2011 <0.023 0.062 3.5 0.5 0.026 1.3 0.07 3.9 12 150 0.11
MW-3 2/22/2011 <0.023 0.058 3 0.58 0.023 1 0.065 2.6 12 150 0.1
MW-3 5/19/2011 <0.023 0.068 3.2 0.24 0.029 1.4 0.056 4.2 12 160 0.12
MW-3 6/21/2011 <0.023 0.062 2.5 0.1 0.047 0.96 0.029 7.6 10 160 0.12
MW-3 7/19/2011 0.047 0.061 3.2 0.051 0.042 1.3 0.026 6 11 160 0.12
MW-3 7/20/2011 <0.023 0.071 3.4 0.19 0.031 1.5 0.061 4.2 13 160 0.13
MW-3 7/21/2011 <0.023 0.071 3.5 0.31 0.026 1.4 0.082 3.9 12 160 0.12
MW-3 8/21/2011 <0.023 0.072 3.1 0.51 0.025 1.4 0.08 3.1 12 150 0.11
MW-3 8/23/2011 <0.023 0.077 3.6 0.46 0.026 1.7 0.085 3.6 12 170 0.13
MW-3 8/25/2011 0.084 0.064 2.8 0.48 0.024 1.2 0.089 3 12 140 0.11
133
Well Date Al Ba Ca Fe Li Mg Mn K Si Na Sr
mg/L mg/L mg/L mg/L mg/L mg/L mg/L mg/L mg/L mg/L mg/L
MW-3 8/27/2011 <0.023 0.076 3.2 0.75 0.024 1.5 0.11 3.4 13 160 0.12
MW-3 8/29/2011 <0.023 0.071 3 0.78 0.023 1.4 0.1 3.2 13 150 0.12
MW-3 9/1/2011 <0.023 0.068 2.7 0.69 0.025 1.3 0.073 3.2 13 140 0.11
MW-3 9/8/2011 <0.023 0.069 2.9 0.6 0.026 1.3 0.065 3.9 12 150 0.12
MW-3 9/15/2011 <0.023 0.066 2.7 0.61 0.025 1.2 0.066 3.5 12 140 0.11
MW-3 9/22/2011 <0.023 0.068 2.8 0.54 0.026 1.3 0.073 3.4 11 150 0.12
MW-3 9/28/2011 <0.023 0.064 2.9 0.75 0.024 1.3 0.068 3.8 12 160 0.11
MW-3 10/5/2011 0.12 0.069 3 0.63 0.023 1.3 0.068 3.4 12 150 0.11
MW-3 10/12/2011 <0.023 0.064 2.7 0.65 0.025 1.2 0.09 3.4 12 140 0.1
MW-3 10/17/2011 <0.023 0.061 2.5 0.69 0.024 1.2 0.067 3.1 12 140 0.097
MW-3 10/19/2011 <0.023 0.062 2.6 0.74 0.024 1.2 0.074 3.1 12 140 0.1
MW-3 10/21/2011 <0.023 0.07 3.3 0.84 0.022 1.6 0.086 3.2 12 180 0.11
MW-3 10/24/2011 <0.023 0.063 2.8 0.86 0.022 1.4 0.078 2.8 12 170 0.098
MW-3 10/26/2011 <0.023 0.068 3 0.88 0.021 1.5 0.085 3 12 180 0.11
MW-3 10/28/2011 <0.023 0.088 3.5 1.9 0.023 1.7 0.12 3.1 12 150 0.13
MW-3 10/31/2011 <0.023 0.19 6.5 8.4 0.027 3.3 0.25 3.4 16 160 0.26
MW-3 11/2/2011 <0.023 0.28 9.8 13 0.031 4.9 0.37 4.3 20 200 0.35
MW-3 11/4/2011 <0.023 0.42 14 26 0.038 6.4 0.54 4.5 29 190 0.5
MW-3 11/10/2011 0.034 0.48 15 33 0.047 6.6 0.61 4.8 40 200 0.55
MW-3 11/11/2011 <0.023 0.45 14 35 0.048 6.9 0.65 4.9 43 220 0.53
MW-3 11/14/2011 <0.023 0.41 12 34 0.048 6 0.58 4.4 43 200 0.44
MW-3 11/16/2011 <0.023 0.35 11 27 0.047 5.3 0.49 4.4 41 210 0.39
MW-3 11/18/2011 <0.023 0.32 9.5 22 0.045 4.8 0.45 4.3 38 210 0.35
MW-3 11/21/2011 <0.023 0.28 8.3 19 0.044 4 0.38 4.2 34 180 0.29
MW-3 11/23/2011 <0.023 0.24 7 17 0.044 3.5 0.33 4.1 33 180 0.23
MW-3 11/25/2011 <0.023 0.25 7.3 16 0.044 3.6 0.35 4.4 31 190 0.24
MW-3 11/28/2011 <0.023 0.21 6 14 0.043 3 0.3 4 30 180 0.2
MW-3 11/30/2011 <0.023 0.19 6.2 12 0.041 2.9 0.28 4.1 28 160 0.18
MW-3 12/2/2011 <0.023 0.18 5.1 12 0.04 2.5 0.25 3.7 28 160 0.16
MW-3 12/5/2011 <0.023 0.17 4.8 11 0.038 2.4 0.26 3.8 25 160 0.17
MW-3 12/7/2011 <0.023 0.18 5.6 11 0.038 2.5 0.28 4.1 24 160 0.18
134
Well Date Al Ba Ca Fe Li Mg Mn K Si Na Sr
mg/L mg/L mg/L mg/L mg/L mg/L mg/L mg/L mg/L mg/L mg/L
MW-3 12/14/2011 <0.023 0.19 6.2 11 0.038 2.7 0.31 4.1 22 160 0.18
MW-3 1/4/2012 <0.023 0.15 5.6 7.4 0.03 2 0.27 3.7 18 150 0.16
MW-3 3/15/2012 0.041 0.088 3.7 2.9 0.024 1.2 0.14 3.2 14 140 0.12
MW-3 4/12/2012 0.046 0.11 5.7 3.7 0.027 1.5 0.22 3.8 16 150 0.17
MW-3 10/5/2012 <0.023 0.17 9.5 6.9 0.041 1.9 0.34 3.8 18 140 0.26
MW-3 1/15/2013 <0.023 0.16 8.5 7 0.043 1.9 0.34 4 19 150 0.2
MW-4 9/2/2010 0.14 0.05 2.3 0.13 0.019 1.2 0.046 2.2 11 150 0.077
MW-4 10/5/2010 0.032 0.046 2.7 0.3 0.008 1.2 0.042 1.8 8.4 150 0.077
MW-4 10/28/2010 <0.023 0.045 2.4 0.41 0.018 1.1 0.047 2.2 11 160 0.079
MW-4 12/3/2010 <0.023 0.051 2.4 0.43 0.019 1.3 0.05 2.7 12 170 0.086
MW-4 12/29/2010 <0.023 0.053 2.5 0.49 0.018 1.3 0.052 2.1 12 150 0.085
MW-4 1/25/2011 <0.023 0.061 3.4 0.44 0.017 1.5 0.062 2.8 11 170 0.1
MW-4 2/23/2011 <0.023 0.054 3 0.45 0.013 1.2 0.055 2.4 11 150 0.089
MW-4 5/20/2011 0.031 0.053 2.8 0.49 0.012 1.4 0.056 2.3 11 160 0.086
MW-4 6/21/2011 <0.023 0.062 3.4 0.39 0.012 1.5 0.066 2.5 11 180 0.11
MW-4 7/19/2011 0.031 0.056 3 0.32 0.013 1.6 0.056 2.3 12 160 0.097
MW-4 9/7/2011 <0.023 0.049 2.2 0.62 0.018 1 0.05 2.1 13 150 0.081
MW-4 9/16/2011 <0.023 0.048 2 0.53 0.018 0.91 0.05 1.8 12 140 0.079
MW-4 9/22/2011 <0.023 0.057 2.8 0.49 0.017 1.2 0.068 2.3 12 190 0.093
MW-4 9/28/2011 <0.023 0.047 2.4 0.59 0.017 1 0.055 2.1 12 170 0.079
MW-4 10/19/2011 <0.023 0.047 2.3 0.49 0.018 0.98 0.052 2.1 12 170 0.076
MW-4 11/10/2011 <0.023 0.042 1.9 0.49 0.018 0.8 0.042 1.8 12 140 0.063
MW-4 12/1/2011 <0.023 0.041 1.9 0.45 0.018 0.79 0.045 1.9 12 150 0.065
MW-4 3/14/2012 <0.023 0.036 1.7 0.47 0.019 0.73 0.038 1.8 12 140 0.059
MW-4 3/19/2012 <0.023 0.038 1.7 0.48 0.019 0.73 0.039 1.8 12 150 0.06
MW-4 3/21/2012 <0.023 0.04 1.8 0.46 0.018 0.78 0.041 1.9 12 160 0.064
MW-4 3/23/2012 <0.023 0.041 1.8 0.47 0.019 0.77 0.041 1.9 12 160 0.063
MW-4 3/26/2012 <0.023 0.041 1.8 0.47 0.018 0.78 0.042 1.9 12 150 0.065
MW-4 4/2/2012 0.024 0.043 2 0.58 0.021 0.86 0.048 2.1 13 160 0.071
MW-4 4/9/2012 <0.023 0.054 2.4 0.77 0.021 1 0.06 2.2 13 160 0.09
135
Well Date Al Ba Ca Fe Li Mg Mn K Si Na Sr
mg/L mg/L mg/L mg/L mg/L mg/L mg/L mg/L mg/L mg/L mg/L
MW-4 4/11/2012 <0.023 0.059 2.5 0.83 0.021 1.1 0.065 2.3 13 170 0.094
MW-4 4/16/2012 <0.023 0.068 2.9 1.1 0.022 1.2 0.072 2.2 13 180 0.1
MW-4 10/4/2012 <0.023 0.28 9.8 7.5 0.048 4.1 0.29 3.9 26 260 0.37
MW-4 1/15/2013 <0.023 0.29 11 8.5 0.048 4.4 0.3 4.2 28 270 0.37
PW-1 2/12/2010 <0.023 0.057 3.7 0.43 0.019 1.5 0.067 2.7 9.4 150 0.11
PW-1 6/28/2010 0.027 0.044 3.4 <0.05 0.008 1.1 0.024 2.3 5.7 140 0.088
PW-1 7/30/2010 0.025 0.057 3.8 <0.05 0.01 1.3 0.03 2.5 5.8 140 0.11
PW-1 8/25/2010 0.038 0.057 4.2 <0.05 0.01 1.4 0.033 2.7 6.3 160 0.11
PW-1 12/4/2010 <0.023 0.055 2.6 0.71 0.02 1.3 0.07 3.2 12 160 0.088
PW-1 12/27/2010 <0.023 0.049 2.5 0.82 0.019 1.1 0.066 2.3 13 150 0.075
PW-1 1/25/2011 <0.023 0.063 3.3 0.78 0.019 1.4 0.086 2.9 11 150 0.1
PW-1 2/24/2011 <0.023 0.045 2.6 0.42 0.019 0.91 0.06 2.3 11 150 0.086
136
Table A-3. Measured concentrations of dissolved anions and alkalinity
Well Date HCO3 Alkalinity Total Alkalinity Cl Br F NO3 NO2 + NO3 NO2 SO4
mg/L mg/L mg/L mg/L mg/L mg/L mg/L mg/L mg/L
BG-1 9/2/2010 330 330 29 0.31 0.44 <0.018 <0.0087 <0.018 1.8
BG-1 10/6/2010 330 340 26 <1 0.48 <0.018 0.013 <0.018 <1.6
BG-1 10/29/2010 320 330 27 <1 0.57 <0.018 <0.0087 <0.018 <1.6
BG-1 12/3/2010 310 320 26 0.037 0.43 <0.013 <0.0087 <0.013 0.9
BG-1 12/27/2010 320 330 28 0.036 0.45 0.031 0.033 <0.013 0.22
BG-1 1/25/2011 330 330 27 0.032 0.45 <0.013 <0.0087 <0.013 3.4
BG-1 2/23/2011 310 320 27 0.19 0.46 <0.013 0.011 <0.013 0.79
BG-1 5/18/2011 330 340 24 0.041 0.46 <0.013 <0.0087 <0.013 2.6
BG-1 6/22/2011 330 340 28 0.046 0.52 <0.013 <0.013 <0.013 2.3
BG-1 7/18/2011 330 340 27 0.039 0.42 <0.013 <0.013 <0.013 3.4
BG-1 9/7/2011 340 340 26 0.033 0.32 <0.013 <0.013 <0.013 0.93
BG-1 9/14/2011 330 340 28 <0.0041 0.3 <0.013 <0.013 <0.013 1.1
BG-1 9/21/2011 330 340 27 <0.0041 0.41 <0.013 <0.013 <0.013 0.83
BG-1 9/28/2011 340 350 23 <0.0041 0.51 <0.013 <0.013 <0.018 0.89
BG-1 10/19/2011 320 330 29 0.039 0.66 <0.013 <0.013 <0.013 <1.4
BG-1 11/10/2011 330 330 25 0.04 0.59 <0.013 <0.013 <0.013 <1.4
BG-1 12/1/2011 320 320 24 0.035 0.54 <0.018 <0.012 <0.018 <1.4
BG-1 3/15/2012 330 340 27 <0.0041 0.57 <0.018 <0.012 <0.018 <1.4
BG-1 4/11/2012 330 330 27 <0.067 0.72 <0.018 <0.012 <0.018 <1.4
BG-1 10/4/2012 26 2.3
BG-1 1/14/2013 330 340 28 <0.067 0.61 <0.09 <0.09 <0.018 <1.4
IW-1 9/2/2010 330 330 28 0.31 0.49 <0.018 <0.0087 <0.018 1.1
IW-1 12/3/2010 330 340 27 0.037 0.5 <0.013 <0.0087 <0.013 0.17
IW-1 12/28/2010 320 320 30 0.036 0.49 0.034 0.035 <0.013 0.22
IW-1 1/26/2011 320 330 25 0.036 0.5 <0.013 <0.0087 <0.013 0.084
IW-1 2/22/2011 320 330 26 0.039 0.46 0.014 0.018 <0.013 0.21
IW-1 10/5/2012 27 13
MW-1 2/12/2010 310 310 27 0.04 0.44 <0.018 <0.01 <0.018 <1.6
MW-1 6/28/2010 320 330 26 0.044 0.55 <0.018 <0.01 <1.6
MW-1 7/30/2010 320 320 27 0.045 0.52 <0.018 <0.0087 2
137
Well Date HCO3 Alkalinity Total Alkalinity Cl Br F NO3 NO2 + NO3 NO2 SO4
mg/L mg/L mg/L mg/L mg/L mg/L mg/L mg/L mg/L
MW-1 8/25/2010 330 330 27 0.32 0.42 <0.018 <0.0087 <0.018 <1.6
MW-1 10/5/2010 330 340 26 <1 0.52 0.03 0.031 <0.018 <1.6
MW-1 10/28/2010 320 320 26 <1 0.6 <0.018 <0.0087 <0.018 <1.6
MW-1 12/3/2010 320 320 24 0.038 0.42 <0.013 <0.0087 <0.013 0.23
MW-1 12/29/2010 310 310 25 0.036 0.47 0.033 0.035 <0.013 0.32
MW-1 1/26/2011 320 320 26 0.032 0.47 <0.013 <0.0087 <0.013 0.28
MW-1 2/23/2011 320 320 26 0.04 0.45 0.013 0.018 <0.013 0.3
MW-1 5/19/2011 320 320 23 0.04 0.48 <0.013 <0.0087 <0.013 0.023
MW-1 6/21/2011 330 330 28 0.044 0.51 <0.013 <0.013 <0.013 0.076
MW-1 7/19/2011 310 310 27 0.04 0.51 <0.013 <0.013 <0.013 0.12
MW-1 9/8/2011 320 320 26 0.041 0.41 <0.013 <0.013 <0.013 0.11
MW-1 9/16/2011 320 320 26 <0.0041 0.3 <0.013 <0.013 <0.013 0.14
MW-1 9/22/2011 320 330 26 <0.0041 0.43 <0.013 <0.013 <0.013 <0.015
MW-1 9/28/2011 330 330 <0.0041 0.54 <0.013 <0.013 <0.018 <0.015
MW-1 10/19/2011 310 310 29 0.038 0.67 <0.013 <0.013 <0.013 0.11
MW-1 11/9/2011 0.016 0.6 <1.4
MW-1 11/10/2011 300 300 22 0.037 0.41 <0.013 <0.013 <0.013 0.12
MW-1 12/1/2011 310 310 24 0.034 0.58 <0.018 <0.012 <0.018 <1.4
MW-1 3/14/2012 650 650 27 <0.0041 0.11 <0.018 <0.012 <0.018 <1.4
MW-1 4/12/2012 560 580 26 <0.067 0.14 <0.018 <0.012 <0.018 <1.4
MW-1 10/5/2012 25 6
MW-1 1/15/2013 530 530 27 <0.067 0.11 <0.018 <0.018 <0.018 <1.4
MW-2 2/12/2010 310 310 27 0.038 0.47 <0.018 <0.01 <0.018 <1.6
MW-2 6/28/2010 320 320 25 0.045 0.55 <0.018 <0.01 <1.6
MW-2 7/30/2010 320 320 26 0.044 0.54 <0.018 0.012 <1.6
MW-2 8/25/2010 320 330 21 0.29 0.38 <0.018 <0.0087 0.025 <1.6
MW-2 10/5/2010 320 330 26 <1 0.52 <0.018 0.016 <0.018 <1.6
MW-2 10/28/2010 320 320 26 <1 0.59 <0.018 <0.0087 <0.018 <1.6
MW-2 12/2/2010 300 300 24 0.036 0.46 <0.013 <0.0087 <0.013 0.14
MW-2 12/28/2010 310 310 25 0.034 0.43 0.026 0.027 <0.013 0.3
MW-2 1/26/2011 320 320 25 0.032 0.46 <0.013 <0.0087 <0.013 0.028
138
Well Date HCO3 Alkalinity Total Alkalinity Cl Br F NO3 NO2 + NO3 NO2 SO4
mg/L mg/L mg/L mg/L mg/L mg/L mg/L mg/L mg/L
MW-2 2/22/2011 310 310 28 0.039 0.42 0.014 0.018 <0.013 0.24
MW-2 5/20/2011 320 320 24 0.043 0.47 <0.013 <0.0087 <0.013 0.077
MW-2 6/21/2011 320 330 28 0.043 0.45 <0.013 <0.013 <0.013 0.06
MW-2 7/19/2011 320 320 26 0.039 0.44 <0.013 <0.013 <0.013 0.025
MW-2 9/7/2011 320 320 26 0.04 0.43 <0.013 <0.013 <0.013 0.081
MW-2 9/15/2011 320 320 27 0.04 0.4 <0.013 <0.013 <0.013 0.13
MW-2 9/21/2011 320 330 26 <0.0041 0.45 <0.013 <0.013 <0.013 <0.015
MW-2 9/28/2011 310 320 18 <0.0041 0.53 <0.013 <0.013 <0.018 <0.015
MW-2 10/19/2011 310 310 23 0.037 0.42 <0.013 <0.013 <0.013 0.57
MW-2 11/10/2011 300 300 24 0.037 0.41 <0.013 <0.013 <0.013 0.12
MW-2 11/16/2011 300 300 23 0.04 0.4 <0.013 <0.013 <0.013 0.2
MW-2 12/1/2011 300 310 24 0.024 0.57 <0.018 <0.012 <0.018 <1.4
MW-2 3/14/2012 390 390 26 <0.0041 0.13 <0.018 <0.012 <0.018 1.5
MW-2 4/11/2012 420 420 27 <0.067 0.12 <0.018 <0.012 <0.018 <1.4
MW-2 1/14/2013 470 470 28 <0.067 0.048 <0.018 <0.018 <0.018 <1.4
MW-3 9/2/2010 260 440 13 0.29 0.18 <0.018 <0.0087 <0.018 2.5
MW-3 10/5/2010 320 330 26 <1 0.52 0.018 0.019 <0.018 <1.6
MW-3 10/28/2010 320 330 26 <1 0.58 <0.018 <0.0087 <0.018 <1.6
MW-3 12/2/2010 300 300 28 0.037 0.43 <0.013 <0.0087 <0.013 0.17
MW-3 12/28/2010 310 320 29 0.036 0.45 0.026 0.027 <0.013 0.25
MW-3 1/24/2011 320 330 25 0.035 0.46 <0.013 <0.0087 <0.013 0.22
MW-3 2/22/2011 310 320 26 0.041 0.43 <0.013 <0.0087 <0.013 0.28
MW-3 5/19/2011 320 330 21 0.046 0.47 <0.013 <0.0087 <0.013 0.35
MW-3 6/21/2011 220 250 27 0.051 0.42 <0.013 <0.013 <0.013 0.5
MW-3 7/19/2011 310 330 26 0.033 0.46 <0.013 <0.013 <0.013 0.55
MW-3 7/20/2011 320 320 27 0.041 0.46 <0.013 <0.013 <0.013 0.49
MW-3 7/21/2011 320 330 27 0.042 0.45 <0.013 <0.013 <0.013 0.57
MW-3 8/21/2011 320 320 26 0.042 0.42 <0.013 <0.013 0.013 0.75
MW-3 8/23/2011 320 330 26 0.039 0.4 <0.013 <0.013 <0.013 0.63
MW-3 8/25/2011 310 320 26 0.041 0.42 <0.013 <0.013 <0.013 0.41
MW-3 8/27/2011 320 320 27 0.038 0.4 <0.013 <0.013 <0.013 0.43
139
Well Date HCO3 Alkalinity Total Alkalinity Cl Br F NO3 NO2 + NO3 NO2 SO4
mg/L mg/L mg/L mg/L mg/L mg/L mg/L mg/L mg/L
MW-3 8/29/2011 310 390 26 0.041 0.33 <0.013 <0.013 <0.013 0.36
MW-3 9/1/2011 320 320 26 0.021 0.36 <0.013 <0.013 <0.013 0.32
MW-3 9/8/2011 320 320 25 0.04 0.34 <0.013 <0.013 <0.013 0.35
MW-3 9/15/2011 310 320 27 <0.0041 0.37 <0.013 <0.013 <0.013 0.3
MW-3 9/22/2011 320 330 26 <0.0041 0.33 <0.013 <0.013 <0.013 0.26
MW-3 9/28/2011 330 330 22 <0.0041 0.53 <0.013 <0.013 <0.018 0.28
MW-3 10/5/2011 330 330 15 <0.0041 0.53 <0.013 <0.013 <0.013 0.37
MW-3 10/12/2011 310 310 23 <0.0041 0.52 <0.013 <0.013 <0.013 <0.015
MW-3 10/19/2011 310 320 28 0.035 0.42 <0.013 <0.013 <0.013 0.19
MW-3 10/26/2011 300 310 22 0.004 0.43 <0.013 <0.013 <0.013 0.2
MW-3 11/2/2011 20 0.035 0.34 0.027 0.027 <0.013 0.34
MW-3 11/9/2011 24 0.035 0.18 1.7
MW-3 11/10/2011 590 590 24 0.022 0.054 <0.013 <0.013 <0.013 0.47
MW-3 11/16/2011 470 470 24 <0.0041 0.081 <0.013 <0.013 <0.013 0.46
MW-3 11/23/2011 390 390 24 <0.0041 0.064 <0.018 <0.012 0.018 <1.4
MW-3 11/30/2011 340 340 24 0.024 0.051 <0.018 <0.012 <0.018 <1.4
MW-3 3/15/2012 310 310 26 <0.0041 0.13 <0.018 <0.012 <0.018 <1.4
MW-3 4/12/2012 320 320 26 <0.067 0.14 <0.018 <0.012 <0.018 <1.4
MW-3 10/5/2012 27 27
MW-3 1/15/2013 350 350 28 <0.067 0.085 <0.018 <0.018 <0.018 <1.4
MW-4 9/2/2010 320 320 32 0.31 0.51 <0.018 <0.0087 <0.018 1.1
MW-4 10/5/2010 320 330 26 <1 0.52 0.024 0.025 <0.018 <1.6
MW-4 10/28/2010 320 320 26 <1 0.59 <0.018 <0.0087 <0.018 <1.6
MW-4 12/3/2010 320 320 29 0.039 0.41 <0.013 <0.0087 <0.013 0.16
MW-4 12/29/2010 310 320 27 0.036 0.47 0.029 0.031 <0.013 0.11
MW-4 1/25/2011 320 320 24 0.034 0.46 <0.013 <0.0087 <0.013 0.058
MW-4 2/23/2011 310 320 27 0.041 0.44 0.017 0.021 <0.013 0.16
MW-4 5/20/2011 320 320 22 0.041 0.46 <0.013 <0.0087 <0.013 <0.015
MW-4 6/21/2011 330 330 28 0.039 0.44 <0.013 <0.013 <0.013 0.086
MW-4 7/19/2011 250 260 26 0.04 0.45 <0.013 <0.013 <0.013 0.04
MW-4 9/7/2011 320 320 26 0.034 0.37 <0.013 <0.013 <0.013 0.052
140
Well Date HCO3 Alkalinity Total Alkalinity Cl Br F NO3 NO2 + NO3 NO2 SO4
mg/L mg/L mg/L mg/L mg/L mg/L mg/L mg/L mg/L
MW-4 9/16/2011 320 320 27 0.041 0.41 <0.013 <0.013 <0.013 0.055
MW-4 9/22/2011 330 330 26 <0.0041 0.3 <0.013 <0.013 <0.013 <0.015
MW-4 9/28/2011 320 320 18 0.044 0.52 <0.013 <0.013 <0.018 <0.015
MW-4 10/19/2011 310 310 22 0.042 0.41 <0.013 <0.013 <0.013 0.034
MW-4 11/9/2011 24 0.035 0.6 <1.4
MW-4 11/10/2011 310 310 22 0.04 0.42 <0.013 <0.013 <0.013 0.05
MW-4 12/1/2011 300 300 24 0.034 0.57 <0.018 <0.012 <0.018 <1.4
MW-4 3/14/2012 320 320 26 0.025 0.59 <0.018 <0.012 <0.018 <1.4
MW-4 4/11/2012 360 360 26 <0.067 0.6 <0.018 <0.012 <0.018 1.7
MW-4 10/4/2012 25 8.6
MW-4 1/15/2013 620 620 28 <0.067 0.25 <0.018 <0.018 <0.018 <1.4
PW-1 2/12/2010 310 310 27 0.03 0.48 <0.018 <0.01 <0.018 <1.6
PW-1 6/28/2010 310 330 25 0.045 0.45 <0.018 <0.01 3.7
PW-1 7/30/2010 320 330 26 0.044 0.5 <0.018 <0.0087 5.2
PW-1 8/25/2010 330 340 24 0.33 0.42 <0.018 <0.0087 <0.018 9.4
PW-1 12/4/2010 310 320 22 0.038 0.54 <0.013 <0.0087 <0.013 0.74
PW-1 12/27/2010 310 320 25 0.034 0.48 0.033 0.035 <0.013 0.55
PW-1 1/25/2011 310 320 24 0.036 0.5 <0.013 <0.0087 <0.013 1.8
PW-1 2/24/2011 310 320 25 0.19 0.52 <0.013 <0.0087 <0.013 3.3
141
Table A-4. Trace element data.
Well Date Sb As Be Cd Cr Co
mg/L mg/L mg/L mg/L mg/L mg/L
BG-1 9/2/2010 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 0.0002
BG-1 10/6/2010 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
BG-1 10/29/2010 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
BG-1 12/3/2010 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
BG-1 12/27/2010 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
BG-1 1/25/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
BG-1 2/23/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
BG-1 5/18/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
BG-1 6/22/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
BG-1 7/18/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
BG-1 9/7/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
BG-1 9/14/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
BG-1 9/21/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
BG-1 9/28/2011 0.002 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
BG-1 10/19/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
BG-1 11/10/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
BG-1 12/1/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
BG-1 3/15/2012 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
BG-1 4/11/2012 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
BG-1 10/4/2012 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
BG-1 1/14/2013 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
IW-1 9/2/2010 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
IW-1 12/3/2010 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
IW-1 12/28/2010 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
IW-1 1/26/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
IW-1 2/22/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
IW-1 10/5/2012 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-1 2/12/2010 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 0.0005
MW-1 6/28/2010 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 0.0002
MW-1 7/30/2010 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 0.0005
MW-1 8/25/2010 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
142
Well Date Sb As Be Cd Cr Co
mg/L mg/L mg/L mg/L mg/L mg/L
MW-1 10/5/2010 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-1 10/28/2010 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-1 12/3/2010 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-1 12/29/2010 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-1 1/26/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-1 2/23/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-1 5/19/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-1 6/21/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-1 7/19/2011 0.003 <0.0013 <0.00025 <0.000095 <0.0025 0.0005
MW-1 9/8/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-1 9/16/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-1 9/22/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-1 9/28/2011 0.002 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-1 10/19/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 0.0002
MW-1 11/10/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 0.0002
MW-1 12/1/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 0.0003
MW-1 1/6/2012 <0.0023 <0.0013 <0.000095 <0.0025 0.0003
MW-1 1/9/2012 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 0.0002
MW-1 1/11/2012 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-1 1/13/2012 0.002 <0.0013 <0.00025 <0.000095 <0.0025
MW-1 1/16/2012 0.002 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-1 1/18/2012 0.002 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-1 1/20/2012 0.002 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-1 1/23/2012 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-1 1/30/2012 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 0.0002
MW-1 2/1/2012 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-1 2/3/2012 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 0.0002
MW-1 2/6/2012 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 0.0002
MW-1 2/8/2012 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 0.0002
MW-1 2/10/2012 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 0.0002
MW-1 2/13/2012 <0.0023 <0.0013 <0.00025 <0.000095 0.007 0.0009
MW-1 2/15/2012 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-1 2/17/2012 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
143
Well Date Sb As Be Cd Cr Co
mg/L mg/L mg/L mg/L mg/L mg/L
MW-1 2/29/2012 <0.0023 <0.0013 <0.00025 <0.000095 0.003 0.0002
MW-1 3/2/2012 <0.0023 <0.0013 <0.00025 <0.000095 0.003 0.0002
MW-1 3/5/2012 <0.0023 <0.0013 <0.00025 <0.000095 0.004 0.0002
MW-1 3/7/2012 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-1 3/9/2012 0.002 <0.0013 <0.00025 <0.000095 0.003 <0.00015
MW-1 3/12/2012 <0.0023 <0.0013 <0.00025 <0.000095 0.003 <0.00015
MW-1 3/14/2012 <0.0023 <0.0013 <0.00025 <0.000095 0.003 <0.00015
MW-1 3/19/2012 <0.0023 <0.0013 <0.00025 <0.000095 0.003 <0.00015
MW-1 3/21/2012 <0.0023 <0.0013 <0.00025 <0.000095 0.004 <0.00015
MW-1 3/23/2012 <0.0023 <0.0013 <0.00025 <0.000095 0.003 <0.00015
MW-1 3/26/2012 <0.0023 <0.0013 <0.00025 <0.000095 0.003 <0.00015
MW-1 4/2/2012 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-1 4/9/2012 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-1 4/12/2012 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-1 4/16/2012 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-1 10/5/2012 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-1 1/15/2013 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-2 2/12/2010 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-2 6/28/2010 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 0.0003
MW-2 7/30/2010 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 0.0006
MW-2 8/25/2010 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-2 10/5/2010 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-2 10/28/2010 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-2 12/2/2010 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-2 12/28/2010 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-2 1/26/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-2 2/22/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-2 5/20/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-2 6/21/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-2 7/19/2011 0.002 <0.0013 <0.00025 <0.000095 <0.0025 0.0002
MW-2 9/7/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-2 9/15/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-2 9/21/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
144
Well Date Sb As Be Cd Cr Co
mg/L mg/L mg/L mg/L mg/L mg/L
MW-2 9/28/2011 0.002 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-2 10/19/2011 <0.0023 <0.0013 <0.00025 <0.000095 0.004 <0.00015
MW-2 11/10/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 0.0002
MW-2 11/16/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 0.0003
MW-2 12/1/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 0.0003
MW-2 12/7/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 0.0003
MW-2 12/14/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 0.0002
MW-2 1/6/2012 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 0.0004
MW-2 1/9/2012 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 0.0004
MW-2 1/11/2012 <0.0023 <0.0013 <0.00025 <0.000095 0.003 0.001
MW-2 1/13/2012 0.002 <0.0013 <0.00025 <0.000095 0.004 0.0014
MW-2 1/16/2012 0.002 <0.0013 <0.00025 <0.000095 0.005 0.0004
MW-2 1/18/2012 0.002 <0.0013 <0.00025 <0.000095 0.007 0.0003
MW-2 1/20/2012 0.002 <0.0013 <0.00025 <0.000095 0.006 0.0004
MW-2 1/23/2012 <0.0023 <0.0013 <0.00025 <0.000095 0.006 0.0005
MW-2 1/27/2012 <0.0023 <0.0013 <0.00025 <0.000095 0.007 0.0013
MW-2 1/30/2012 <0.0023 <0.0013 <0.00025 <0.000095 0.007 0.0012
MW-2 2/1/2012 <0.0023 <0.0013 <0.00025 <0.000095 0.007 0.001
MW-2 2/3/2012 <0.0023 <0.0013 <0.00025 <0.000095 0.007 0.0007
MW-2 2/6/2012 <0.0023 <0.0013 <0.00025 <0.000095 0.009 0.0013
MW-2 2/8/2012 <0.0023 <0.0013 <0.00025 <0.000095 0.008 0.001
MW-2 2/10/2012 <0.0023 <0.0013 <0.00025 <0.000095 0.007 0.0006
MW-2 2/13/2012 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 0.0002
MW-2 2/15/2012 <0.0023 <0.0013 <0.00025 <0.000095 0.006 0.0003
MW-2 2/17/2012 <0.0023 <0.0013 <0.00025 <0.000095 0.009 0.0006
MW-2 2/29/2012 <0.0023 <0.0013 <0.00025 <0.000095 0.007 0.0005
MW-2 3/2/2012 <0.0023 <0.0013 <0.00025 <0.000095 0.006 0.0003
MW-2 3/5/2012 <0.0023 <0.0013 <0.00025 <0.000095 0.008 0.0006
MW-2 3/7/2012 <0.0023 <0.0013 <0.00025 <0.000095 0.005 0.0002
MW-2 3/9/2012 0.002 <0.0013 <0.00025 <0.000095 0.005 0.0002
MW-2 3/12/2012 <0.0023 <0.0013 <0.00025 <0.000095 0.004 0.0002
MW-2 3/14/2012 <0.0023 <0.0013 <0.00025 <0.000095 0.004 0.0002
MW-2 3/19/2012 <0.0023 <0.0013 <0.00025 <0.000095 0.004 0.0002
145
Well Date Sb As Be Cd Cr Co
mg/L mg/L mg/L mg/L mg/L mg/L
MW-2 3/21/2012 <0.0023 <0.0013 <0.00025 <0.000095 0.004 0.0002
MW-2 3/23/2012 <0.0023 <0.0013 <0.00025 <0.000095 0.006 0.0002
MW-2 3/26/2012 <0.0023 <0.0013 <0.00025 <0.000095 0.005 0.0002
MW-2 4/2/2012 <0.0023 <0.0013 <0.00025 <0.000095 0.005 0.0002
MW-2 4/9/2012 <0.0023 <0.0013 <0.00025 <0.000095 0.005 0.0003
MW-2 4/11/2012 <0.0023 <0.0013 <0.00025 <0.000095 0.004 0.0002
MW-2 4/16/2012 <0.0023 <0.0013 <0.00025 <0.000095 0.005 0.0002
MW-2 10/4/2012 <0.0023 <0.0013 <0.00025 <0.000095 0.003 0.0002
MW-2 1/14/2013 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 0.0002
MW-3 9/2/2010 <0.0023 <0.0013 <0.00025 <0.000095 0.007 0.0004
MW-3 10/5/2010 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-3 10/28/2010 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-3 12/2/2010 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-3 12/28/2010 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-3 1/24/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-3 2/22/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-3 5/19/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-3 6/21/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-3 7/19/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-3 7/20/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-3 7/21/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-3 8/21/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-3 8/23/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-3 8/25/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-3 8/27/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-3 8/29/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-3 9/1/2011 0.002 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-3 9/8/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-3 9/15/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-3 9/22/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-3 9/28/2011 0.002 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-3 10/5/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-3 10/12/2011 <0.0023 <0.0013 <0.00025 <0.000095 0.007 0.0003
146
Well Date Sb As Be Cd Cr Co
mg/L mg/L mg/L mg/L mg/L mg/L
MW-3 10/17/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-3 10/19/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-3 10/21/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-3 10/24/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-3 10/26/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-3 10/28/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-3 10/31/2011 <0.0023 <0.0013 <0.00025 <0.000095 0.003 <0.00015
MW-3 11/2/2011 <0.0023 <0.0013 <0.00025 0.00024 0.004 <0.00015
MW-3 11/4/2011 <0.0023 <0.0013 <0.00025 <0.000095 0.005 <0.00015
MW-3 11/10/2011 <0.0023 <0.0013 <0.00025 <0.000095 0.01 0.0002
MW-3 11/11/2011 <0.0023 <0.0013 <0.00025 <0.000095 0.013 0.0002
MW-3 11/14/2011 <0.0023 <0.0013 <0.00025 <0.000095 0.013 0.0002
MW-3 11/16/2011 <0.0023 <0.0013 0.0003 <0.000095 0.013 0.0002
MW-3 11/18/2011 <0.0023 <0.0013 0.0003 <0.000095 0.012 0.0002
MW-3 11/21/2011 <0.0023 <0.0013 0.0003 <0.000095 0.009 0.0004
MW-3 11/23/2011 <0.0023 <0.0013 0.0003 <0.000095 0.009 0.0003
MW-3 11/25/2011 <0.0023 <0.0013 0.0003 <0.000095 0.009 0.0004
MW-3 11/28/2011 <0.0023 <0.0013 0.0003 <0.000095 0.007 0.0003
MW-3 11/30/2011 <0.0023 <0.0013 0.0003 <0.000095 0.006 0.0004
MW-3 12/2/2011 <0.0023 <0.0013 0.0003 <0.000095 0.006 0.0003
MW-3 12/5/2011 <0.0023 <0.0013 0.0003 <0.000095 0.006 0.0002
MW-3 12/7/2011 0.003 <0.0013 0.0003 <0.000095 0.006 0.0003
MW-3 12/14/2011 <0.0023 <0.0013 0.0004 <0.000095 0.004 0.0006
MW-3 1/4/2012 <0.0023 <0.0013 0.0003 <0.000095 0.004 0.0004
MW-3 3/15/2012 <0.0023 <0.0013 0.0007 <0.000095 0.004 0.0003
MW-3 4/12/2012 <0.0023 <0.0013 0.0007 <0.000095 0.005 0.0004
MW-3 10/5/2012 <0.0023 <0.0013 0.0004 <0.000095 0.005 0.0004
MW-3 1/15/2013 <0.0023 <0.0013 0.0005 <0.000095 0.004 0.0003
MW-4 9/2/2010 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-4 10/5/2010 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-4 10/28/2010 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-4 12/3/2010 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-4 12/29/2010 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
147
Well Date Sb As Be Cd Cr Co
mg/L mg/L mg/L mg/L mg/L mg/L
MW-4 1/25/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-4 2/23/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-4 5/20/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-4 6/21/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-4 7/19/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 0.0002
MW-4 9/7/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-4 9/16/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-4 9/22/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 0.0002
MW-4 9/28/2011 0.002 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-4 10/19/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-4 11/10/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-4 12/1/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-4 3/14/2012 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-4 3/19/2012 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-4 3/21/2012 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-4 3/23/2012 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-4 3/26/2012 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-4 4/2/2012 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-4 4/9/2012 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-4 4/11/2012 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-4 4/16/2012 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
MW-4 10/4/2012 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 0.0044
MW-4 1/15/2013 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 0.012
PW-1 2/12/2010 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
PW-1 6/28/2010 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
PW-1 7/30/2010 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
PW-1 8/25/2010 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
PW-1 12/4/2010 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
PW-1 12/27/2010 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
PW-1 1/25/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
PW-1 2/24/2011 <0.0023 <0.0013 <0.00025 <0.000095 <0.0025 <0.00015
148
Well Date Cu Pb Hg Mo Ni
mg/L mg/L mg/L mg/L mg/L
BG-1 9/2/2010 <0.0011 0.0005 <0.00007 0.007 <0.002
BG-1 10/6/2010 <0.0011 <0.0002 0.00013 0.005 <0.002
BG-1 10/29/2010 <0.0011 <0.0002 <0.00007 0.004 <0.002
BG-1 12/3/2010 <0.0011 <0.0002 <0.00007 0.004 <0.002
BG-1 12/27/2010 <0.0011 <0.0002 <0.00007 0.003 <0.002
BG-1 1/25/2011 <0.0011 <0.0002 <0.00007 0.005 <0.002
BG-1 2/23/2011 <0.0011 <0.0002 <0.00007 0.004 <0.002
BG-1 5/18/2011 <0.0011 <0.0002 <0.00007 0.007 <0.002
BG-1 6/22/2011 <0.0011 <0.0002 <0.00007 0.007 <0.002
BG-1 7/18/2011 <0.0011 <0.0002 <0.00007 0.008 <0.002
BG-1 9/7/2011 <0.0011 <0.0002 <0.00007 0.005 <0.002
BG-1 9/14/2011 <0.0011 <0.0002 <0.00007 0.005 <0.002
BG-1 9/21/2011 <0.0011 <0.0002 <0.00007 0.004 <0.002
BG-1 9/28/2011 <0.0011 <0.0002 <0.00007 0.005 <0.002
BG-1 10/19/2011 <0.0011 <0.0002 <0.00007 0.004 <0.002
BG-1 11/10/2011 <0.0011 <0.0002 0.00008 0.004 <0.002
BG-1 12/1/2011 <0.0011 0.0021 <0.00007 0.004 <0.002
BG-1 3/15/2012 <0.0011 <0.0002 <0.00007 0.003 <0.002
BG-1 4/11/2012 <0.0011 0.0008 <0.00007 0.003 <0.002
BG-1 10/4/2012 <0.0011 <0.0002 <0.00007 0.004 0.002
BG-1 1/14/2013 <0.0011 <0.0002 <0.00007 0.004 <0.002
IW-1 9/2/2010 <0.0011 <0.0002 <0.00007 0.008 <0.002
IW-1 12/3/2010 0.002 0.0003 <0.00007 0.007 <0.002
IW-1 12/28/2010 <0.0011 <0.0002 <0.00007 0.004 <0.002
IW-1 1/26/2011 <0.0011 <0.0002 <0.00007 0.005 <0.002
IW-1 2/22/2011 <0.0011 <0.0002 <0.00007 0.006 <0.002
IW-1 10/5/2012 <0.0011 <0.0002 <0.00007 0.002 0.003
MW-1 2/12/2010 <0.0011 0.0005 <0.00007 0.004 <0.002
MW-1 6/28/2010 <0.0011 <0.0002 <0.00007 0.011 <0.002
MW-1 7/30/2010 <0.0011 <0.0002 <0.00007 0.009 <0.002
MW-1 8/25/2010 <0.0011 0.0004 <0.00007 0.008 <0.002
149
Well Date Cu Pb Hg Mo Ni
mg/L mg/L mg/L mg/L mg/L
MW-1 10/5/2010 <0.0011 <0.0002 0.00015 0.007 <0.002
MW-1 10/28/2010 <0.0011 <0.0002 <0.00007 0.003 <0.002
MW-1 12/3/2010 <0.0011 <0.0002 <0.00007 0.003 <0.002
MW-1 12/29/2010 <0.0011 <0.0002 <0.00007 0.003 <0.002
MW-1 1/26/2011 <0.0011 <0.0002 <0.00007 0.003 <0.002
MW-1 2/23/2011 <0.0011 <0.0002 <0.00007 0.003 <0.002
MW-1 5/19/2011 <0.0011 <0.0002 <0.00007 0.004 <0.002
MW-1 6/21/2011 <0.0011 <0.0002 0.00013 0.004 <0.002
MW-1 7/19/2011 <0.0011 <0.0002 <0.00007 0.013 0.037
MW-1 9/8/2011 <0.0011 <0.0002 <0.00007 0.005 0.004
MW-1 9/16/2011 <0.0011 <0.0002 <0.00007 0.007 0.006
MW-1 9/22/2011 <0.0011 <0.0002 <0.00007 0.006 0.004
MW-1 9/28/2011 <0.0011 <0.0002 <0.00007 0.006 0.007
MW-1 10/19/2011 <0.0011 <0.0002 <0.00007 0.008 0.008
MW-1 11/10/2011 <0.0011 <0.0002 <0.00007 0.008 0.012
MW-1 12/1/2011 <0.0011 <0.0002 <0.00007 0.012 0.015
MW-1 1/6/2012 <0.0011 <0.0002 <0.00007 0.01 0.012
MW-1 1/9/2012 <0.0011 <0.0002 0.00008 0.008 0.009
MW-1 1/11/2012 <0.0011 <0.0002 <0.00007 0.005 0.006
MW-1 1/13/2012 <0.0011 0.0003 <0.00007 0.005 0.006
MW-1 1/16/2012 <0.0011 <0.0002 <0.00007 0.005 0.007
MW-1 1/18/2012 <0.0011 <0.0002 <0.00007 0.004 0.007
MW-1 1/20/2012 <0.0011 <0.0002 <0.00007 0.005 0.008
MW-1 1/23/2012 <0.0011 <0.0002 <0.00007 0.005 0.004
MW-1 1/30/2012 <0.0011 <0.0002 <0.00007 0.005 0.007
MW-1 2/1/2012 <0.0011 <0.0002 <0.00007 0.003 0.005
MW-1 2/3/2012 <0.0011 <0.0002 <0.00007 0.004 0.007
MW-1 2/6/2012 <0.0011 <0.0002 <0.00007 0.008 0.008
MW-1 2/8/2012 <0.0011 <0.0002 <0.00007 0.005 0.008
MW-1 2/10/2012 0.002 <0.0002 0.00023 0.005 0.008
MW-1 2/13/2012 <0.0011 <0.0002 <0.00007 0.003 0.061
MW-1 2/15/2012 <0.0011 <0.0002 <0.00007 0.002 0.004
MW-1 2/17/2012 <0.0011 <0.0002 <0.00007 0.002 0.006
150
Well Date Cu Pb Hg Mo Ni
mg/L mg/L mg/L mg/L mg/L
MW-1 2/29/2012 <0.0011 <0.0002 <0.00007 0.002 0.013
MW-1 3/2/2012 <0.0011 <0.0002 0.0001 0.002 0.009
MW-1 3/5/2012 <0.0011 <0.0002 0.00017 0.002 0.013
MW-1 3/7/2012 <0.0011 <0.0002 0.00014 <0.0015 0.005
MW-1 3/9/2012 <0.0011 <0.0002 <0.00007 <0.0015 0.006
MW-1 3/12/2012 <0.0011 <0.0002 <0.00007 <0.0015 0.006
MW-1 3/14/2012 <0.0011 <0.0002 <0.00007 <0.0015 0.007
MW-1 3/19/2012 <0.0011 <0.0002 <0.00007 <0.0015 0.006
MW-1 3/21/2012 <0.0011 <0.0002 <0.00007 <0.0015 0.008
MW-1 3/23/2012 <0.0011 <0.0002 <0.00007 <0.0015 0.007
MW-1 3/26/2012 <0.0011 0.0008 <0.00007 <0.0015 0.007
MW-1 4/2/2012 <0.0011 <0.0002 <0.00007 <0.0015 0.007
MW-1 4/9/2012 <0.0011 0.0002 <0.00007 <0.0015 0.006
MW-1 4/12/2012 <0.0011 <0.0002 <0.00007 <0.0015 0.005
MW-1 4/16/2012 <0.0011 <0.0002 <0.00007 <0.0015 0.006
MW-1 10/5/2012 <0.0011 <0.0002 <0.00007 <0.0015 0.005
MW-1 1/15/2013 <0.0011 <0.0002 <0.00007 <0.0015 0.002
MW-2 2/12/2010 <0.0011 <0.0002 <0.00007 0.004 <0.002
MW-2 6/28/2010 <0.0011 <0.0002 <0.00007 0.007 <0.002
MW-2 7/30/2010 <0.0011 <0.0002 <0.00007 0.007 <0.002
MW-2 8/25/2010 <0.0011 0.0009 <0.00007 0.008 <0.002
MW-2 10/5/2010 <0.0011 <0.0002 0.00017 0.008 <0.002
MW-2 10/28/2010 <0.0011 <0.0002 <0.00007 0.004 <0.002
MW-2 12/2/2010 <0.0011 <0.0002 <0.00007 0.003 <0.002
MW-2 12/28/2010 <0.0011 <0.0002 <0.00007 0.003 <0.002
MW-2 1/26/2011 <0.0011 <0.0002 <0.00007 0.003 <0.002
MW-2 2/22/2011 <0.0011 <0.0002 <0.00007 0.003 <0.002
MW-2 5/20/2011 <0.0011 <0.0002 <0.00007 0.004 <0.002
MW-2 6/21/2011 <0.0011 <0.0002 0.0001 0.005 <0.002
MW-2 7/19/2011 <0.0011 <0.0002 <0.00007 0.013 0.016
MW-2 9/7/2011 <0.0011 <0.0002 <0.00007 0.004 0.003
MW-2 9/15/2011 <0.0011 <0.0002 <0.00007 0.004 0.004
MW-2 9/21/2011 <0.0011 <0.0002 <0.00007 0.004 <0.002
151
Well Date Cu Pb Hg Mo Ni
mg/L mg/L mg/L mg/L mg/L
MW-2 9/28/2011 <0.0011 <0.0002 <0.00007 0.004 0.003
MW-2 10/19/2011 <0.0011 <0.0002 <0.00007 0.006 0.009
MW-2 11/10/2011 <0.0011 <0.0002 <0.00007 0.009 0.016
MW-2 11/16/2011 <0.0011 <0.0002 <0.00007 0.008 0.014
MW-2 12/1/2011 <0.0011 <0.0002 <0.00007 0.01 0.015
MW-2 12/7/2011 <0.0011 <0.0002 <0.00007 0.01 0.013
MW-2 12/14/2011 <0.0011 <0.0002 <0.00007 0.007 0.008
MW-2 1/6/2012 <0.0011 <0.0002 <0.00007 0.002 0.02
MW-2 1/9/2012 <0.0011 <0.0002 <0.00007 0.002 0.022
MW-2 1/11/2012 <0.0011 <0.0002 <0.00007 0.003 0.05
MW-2 1/13/2012 <0.0011 0.0002 <0.00007 0.005 0.078
MW-2 1/16/2012 <0.0011 <0.0002 <0.00007 0.002 0.018
MW-2 1/18/2012 <0.0011 <0.0002 <0.00007 0.002 0.017
MW-2 1/20/2012 <0.0011 <0.0002 <0.00007 0.002 0.022
MW-2 1/23/2012 <0.0011 <0.0002 <0.00007 0.003 0.029
MW-2 1/27/2012 <0.0011 <0.0002 <0.00007 0.006 0.09
MW-2 1/30/2012 <0.0011 <0.0002 <0.00007 0.005 0.092
MW-2 2/1/2012 <0.0011 <0.0002 <0.00007 0.004 0.079
MW-2 2/3/2012 <0.0011 <0.0002 <0.00007 0.002 0.047
MW-2 2/6/2012 <0.0011 <0.0002 <0.00007 0.005 0.1
MW-2 2/8/2012 <0.0011 <0.0002 <0.00007 0.004 0.078
MW-2 2/10/2012 <0.0011 <0.0002 <0.00007 0.003 0.041
MW-2 2/13/2012 <0.0011 <0.0002 <0.00007 0.004 0.007
MW-2 2/15/2012 <0.0011 <0.0002 <0.00007 <0.0015 0.02
MW-2 2/17/2012 <0.0011 <0.0002 <0.00007 0.002 0.039
MW-2 2/29/2012 <0.0011 <0.0002 0.00016 0.002 0.032
MW-2 3/2/2012 <0.0011 <0.0002 <0.00007 <0.0015 0.015
MW-2 3/5/2012 <0.0011 <0.0002 <0.00007 0.003 0.043
MW-2 3/7/2012 <0.0011 <0.0002 <0.00007 0.002 0.01
MW-2 3/9/2012 <0.0011 <0.0002 <0.00007 0.002 0.01
MW-2 3/12/2012 <0.0011 <0.0002 <0.00007 0.002 0.008
MW-2 3/14/2012 <0.0011 <0.0002 <0.00007 0.002 0.006
MW-2 3/19/2012 <0.0011 <0.0002 <0.00007 <0.0015 0.006
152
Well Date Cu Pb Hg Mo Ni
mg/L mg/L mg/L mg/L mg/L
MW-2 3/21/2012 <0.0011 <0.0002 <0.00007 <0.0015 0.006
MW-2 3/23/2012 <0.0011 <0.0002 <0.00007 <0.0015 0.007
MW-2 3/26/2012 <0.0011 0.0005 <0.00007 <0.0015 0.005
MW-2 4/2/2012 <0.0011 0.0002 <0.00007 <0.0015 0.004
MW-2 4/9/2012 <0.0011 <0.0002 <0.00007 <0.0015 0.009
MW-2 4/11/2012 <0.0011 0.0004 <0.00007 <0.0015 0.005
MW-2 4/16/2012 <0.0011 <0.0002 <0.00007 <0.0015 0.006
MW-2 10/4/2012 <0.0011 <0.0002 <0.0015 0.004
MW-2 1/14/2013 <0.0011 <0.0002 <0.00007 <0.0015 0.002
MW-3 9/2/2010 <0.0011 0.0009 <0.00007 0.011 <0.002
MW-3 10/5/2010 <0.0011 <0.0002 0.00012 0.002 <0.002
MW-3 10/28/2010 <0.0011 <0.0002 <0.00007 0.002 <0.002
MW-3 12/2/2010 <0.0011 <0.0002 <0.00007 0.002 <0.002
MW-3 12/28/2010 <0.0011 <0.0002 <0.00007 0.002 <0.002
MW-3 1/24/2011 <0.0011 <0.0002 <0.00007 0.003 <0.002
MW-3 2/22/2011 <0.0011 <0.0002 <0.00007 0.002 <0.002
MW-3 5/19/2011 <0.0011 <0.0002 <0.00007 0.004 <0.002
MW-3 6/21/2011 <0.0011 <0.0002 0.00017 0.004 <0.002
MW-3 7/19/2011 <0.0011 <0.0002 <0.00007 0.005 <0.002
MW-3 7/20/2011 <0.0011 <0.0002 <0.00007 0.004 <0.002
MW-3 7/21/2011 <0.0011 <0.0002 <0.00007 0.004 <0.002
MW-3 8/21/2011 <0.0011 <0.0002 <0.00007 0.003 <0.002
MW-3 8/23/2011 <0.0011 <0.0002 <0.00007 0.003 <0.002
MW-3 8/25/2011 <0.0011 <0.0002 <0.00007 0.002 <0.002
MW-3 8/27/2011 <0.0011 <0.0002 <0.00007 0.004 0.002
MW-3 8/29/2011 <0.0011 <0.0002 <0.00007 0.004 <0.002
MW-3 9/1/2011 <0.0011 <0.0002 <0.00007 0.005 <0.002
MW-3 9/8/2011 <0.0011 <0.0002 <0.00007 0.004 <0.002
MW-3 9/15/2011 <0.0011 <0.0002 <0.00007 0.004 <0.002
MW-3 9/22/2011 <0.0011 <0.0002 <0.00007 0.003 <0.002
MW-3 9/28/2011 <0.0011 <0.0002 <0.00007 0.003 <0.002
MW-3 10/5/2011 <0.0011 0.0007 <0.00007 0.003 0.003
MW-3 10/12/2011 0.002 <0.0002 <0.00007 0.004 0.006
153
Well Date Cu Pb Hg Mo Ni
mg/L mg/L mg/L mg/L mg/L
MW-3 10/17/2011 <0.0011 <0.0002 <0.00007 0.003 0.002
MW-3 10/19/2011 <0.0011 <0.0002 <0.00007 0.002 <0.002
MW-3 10/21/2011 <0.0011 <0.0002 <0.00007 0.002 <0.002
MW-3 10/24/2011 <0.0011 <0.0002 <0.00007 0.002 <0.002
MW-3 10/26/2011 <0.0011 <0.0002 0.00012 0.003 <0.002
MW-3 10/28/2011 0.001 <0.0002 <0.00007 0.002 0.002
MW-3 10/31/2011 <0.0011 <0.0002 <0.00007 0.003 0.004
MW-3 11/2/2011 <0.0011 <0.0002 <0.00007 0.002 0.003
MW-3 11/4/2011 <0.0011 <0.0002 <0.00007 <0.0015 0.003
MW-3 11/10/2011 <0.0011 <0.0002 <0.00007 <0.0015 0.005
MW-3 11/11/2011 <0.0011 <0.0002 <0.00007 <0.0015 0.003
MW-3 11/14/2011 <0.0011 <0.0002 <0.00007 <0.0015 <0.002
MW-3 11/16/2011 <0.0011 <0.0002 <0.00007 <0.0015 0.004
MW-3 11/18/2011 <0.0011 <0.0002 <0.00007 <0.0015 <0.002
MW-3 11/21/2011 <0.0011 <0.0002 <0.00007 <0.0015 0.013
MW-3 11/23/2011 <0.0011 <0.0002 <0.00007 <0.0015 0.009
MW-3 11/25/2011 <0.0011 <0.0002 0.00023 <0.0015 0.009
MW-3 11/28/2011 <0.0011 <0.0002 0.00007 <0.0015 0.009
MW-3 11/30/2011 <0.0011 <0.0002 <0.00007 <0.0015 0.018
MW-3 12/2/2011 <0.0011 <0.0002 <0.00007 <0.0015 0.004
MW-3 12/5/2011 <0.0011 <0.0002 <0.00007 <0.0015 0.005
MW-3 12/7/2011 <0.0011 <0.0002 <0.00007 <0.0015 0.009
MW-3 12/14/2011 <0.0011 <0.0002 <0.00007 <0.0015 0.026
MW-3 1/4/2012 <0.0011 <0.0002 <0.00007 <0.0015 0.016
MW-3 3/15/2012 <0.0011 <0.0002 <0.00007 <0.0015 0.007
MW-3 4/12/2012 <0.0011 <0.0002 <0.00007 <0.0015 0.012
MW-3 10/5/2012 <0.0011 <0.0002 <0.00007 <0.0015 0.014
MW-3 1/15/2013 <0.0011 <0.0002 <0.00007 <0.0015 0.009
MW-4 9/2/2010 <0.0011 0.0002 <0.00007 0.003 <0.002
MW-4 10/5/2010 <0.0011 <0.0002 0.00019 0.01 <0.002
MW-4 10/28/2010 <0.0011 <0.0002 <0.00007 0.003 <0.002
MW-4 12/3/2010 <0.0011 <0.0002 <0.00007 0.003 <0.002
MW-4 12/29/2010 <0.0011 <0.0002 <0.00007 0.004 <0.002
154
Well Date Cu Pb Hg Mo Ni
mg/L mg/L mg/L mg/L mg/L
MW-4 1/25/2011 <0.0011 <0.0002 <0.00007 0.005 <0.002
MW-4 2/23/2011 <0.0011 <0.0002 <0.00007 0.004 <0.002
MW-4 5/20/2011 <0.0011 <0.0002 <0.00007 0.006 <0.002
MW-4 6/21/2011 <0.0011 <0.0002 <0.00007 0.006 <0.002
MW-4 7/19/2011 <0.0011 <0.0002 <0.00007 0.01 0.008
MW-4 9/7/2011 <0.0011 <0.0002 <0.00007 0.003 0.002
MW-4 9/16/2011 <0.0011 <0.0002 <0.00007 0.005 0.006
MW-4 9/22/2011 <0.0011 <0.0002 <0.00007 0.006 0.003
MW-4 9/28/2011 <0.0011 <0.0002 <0.00007 0.004 0.003
MW-4 10/19/2011 <0.0011 <0.0002 <0.00007 0.005 0.007
MW-4 11/10/2011 <0.0011 <0.0002 <0.00007 0.006 0.003
MW-4 12/1/2011 <0.0011 <0.0002 <0.00007 0.006 0.003
MW-4 3/14/2012 <0.0011 <0.0002 <0.00007 0.004 <0.002
MW-4 3/19/2012 <0.0011 <0.0002 <0.00007 0.004 <0.002
MW-4 3/21/2012 <0.0011 <0.0002 <0.00007 0.004 <0.002
MW-4 3/23/2012 <0.0011 <0.0002 <0.00007 0.004 <0.002
MW-4 3/26/2012 <0.0011 <0.0002 <0.00007 0.004 <0.002
MW-4 4/2/2012 0.001 0.0006 <0.00007 0.004 <0.002
MW-4 4/9/2012 <0.0011 0.0008 <0.00007 0.003 <0.002
MW-4 4/11/2012 <0.0011 0.0009 <0.00007 0.004 0.002
MW-4 4/16/2012 <0.0011 <0.0002 <0.00007 0.004 0.004
MW-4 10/4/2012 <0.0011 <0.0002 <0.00007 0.002 0.006
MW-4 1/15/2013 <0.0011 <0.0002 <0.00007 0.002 0.004
PW-1 2/12/2010 <0.0011 <0.0002 <0.00007 0.003 <0.002
PW-1 6/28/2010 <0.0011 <0.0002 <0.00007 0.014 <0.002
PW-1 7/30/2010 <0.0011 <0.0002 <0.00007 0.013 <0.002
PW-1 8/25/2010 <0.0011 0.0003 <0.00007 0.011 <0.002
PW-1 12/4/2010 <0.0011 <0.0002 <0.00007 0.003 <0.002
PW-1 12/27/2010 <0.0011 <0.0002 <0.00007 0.003 <0.002
PW-1 1/25/2011 <0.0011 <0.0002 <0.00007 0.004 <0.002
PW-1 2/24/2011 <0.0011 <0.0002 <0.00007 0.004 <0.002
155
Well Date P Se Ag Tl Zn
mg/L mg/L mg/L mg/L mg/L
BG-1 9/2/2010 0.26 <0.001 <0.00025 <0.0005 <0.0083
BG-1 10/6/2010 0.29 <0.001 <0.00025 <0.0005 <0.0083
BG-1 10/29/2010 0.2 <0.001 <0.00025 <0.0005 <0.0083
BG-1 12/3/2010 0.24 <0.001 <0.00025 <0.0005 <0.0083
BG-1 12/27/2010 0.37 <0.001 <0.00025 <0.0005 <0.0083
BG-1 1/25/2011 0.3 0.001 <0.00025 <0.0005 <0.0083
BG-1 2/23/2011 0.27 <0.001 <0.00025 <0.0005 <0.0083
BG-1 5/18/2011 0.43 <0.001 <0.00025 <0.0005 <0.0083
BG-1 6/22/2011 0.33 <0.001 <0.00025 <0.0005 <0.0083
BG-1 7/18/2011 0.24 <0.001 <0.00025 <0.0005 <0.0083
BG-1 9/7/2011 0.3 <0.001 <0.00025 <0.0005 <0.0083
BG-1 9/14/2011 0.25 <0.001 <0.00025 <0.0005 <0.0083
BG-1 9/21/2011 0.35 <0.001 <0.00025 <0.0005 <0.0083
BG-1 9/28/2011 0.25 <0.001 <0.00025 <0.0005 <0.0083
BG-1 10/19/2011 0.32 <0.001 <0.00025 <0.0005 <0.0083
BG-1 11/10/2011 0.38 <0.001 <0.00025 <0.0005 <0.0083
BG-1 12/1/2011 0.28 <0.001 <0.00025 <0.0005 <0.0083
BG-1 3/15/2012 0.27 <0.001 <0.00025 <0.0005 <0.0083
BG-1 4/11/2012 0.24 <0.001 <0.00025 <0.0005 <0.0083
BG-1 10/4/2012 <0.001 <0.00025 <0.0005 <0.0083
BG-1 1/14/2013 0.17 <0.001 <0.00025 <0.0005 <0.0083
IW-1 9/2/2010 0.26 <0.001 <0.00025 <0.0005 <0.0083
IW-1 12/3/2010 0.27 <0.001 <0.00025 <0.0005 <0.0083
IW-1 12/28/2010 0.3 <0.001 <0.00025 <0.0005 <0.0083
IW-1 1/26/2011 0.31 <0.001 <0.00025 <0.0005 <0.0083
IW-1 2/22/2011 0.31 <0.001 <0.00025 <0.0005 <0.0083
IW-1 10/5/2012 <0.001 <0.00025 <0.0005 0.027
MW-1 2/12/2010 0.28 <0.001 <0.00025 <0.0005 0.013
MW-1 6/28/2010 0.44 <0.001 <0.00025 <0.0005 <0.0083
MW-1 7/30/2010 0.38 <0.001 <0.00025 <0.0005 <0.0083
MW-1 8/25/2010 0.46 <0.001 <0.00025 <0.0005 <0.0083
156
Well Date P Se Ag Tl Zn
mg/L mg/L mg/L mg/L mg/L
MW-1 10/5/2010 0.4 <0.001 <0.00025 <0.0005 <0.0083
MW-1 10/28/2010 0.19 <0.001 <0.00025 <0.0005 <0.0083
MW-1 12/3/2010 1.3 <0.001 <0.00025 <0.0005 <0.0083
MW-1 12/29/2010 0.27 <0.001 <0.00025 <0.0005 <0.0083
MW-1 1/26/2011 0.29 0.001 <0.00025 <0.0005 <0.0083
MW-1 2/23/2011 0.39 0.001 <0.00025 <0.0005 <0.0083
MW-1 5/19/2011 0.33 <0.001 <0.00025 <0.0005 <0.0083
MW-1 6/21/2011 0.32 <0.001 <0.00025 <0.0005 <0.0083
MW-1 7/19/2011 0.2 <0.001 <0.00025 <0.0005 0.028
MW-1 9/8/2011 0.21 <0.001 <0.00025 <0.0005 <0.0083
MW-1 9/16/2011 0.26 <0.001 <0.00025 <0.0005 <0.0083
MW-1 9/22/2011 0.28 <0.001 <0.00025 <0.0005 <0.0083
MW-1 9/28/2011 0.17 <0.001 <0.00025 <0.0005 <0.0083
MW-1 10/19/2011 0.26 <0.001 <0.00025 <0.0005 <0.0083
MW-1 11/10/2011 0.4 <0.001 <0.00025 <0.0005 <0.0083
MW-1 12/1/2011 0.26 <0.001 <0.00025 <0.0005 <0.0083
MW-1 1/6/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-1 1/9/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-1 1/11/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-1 1/13/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-1 1/16/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-1 1/18/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-1 1/20/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-1 1/23/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-1 1/30/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-1 2/1/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-1 2/3/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-1 2/6/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-1 2/8/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-1 2/10/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-1 2/13/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-1 2/15/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-1 2/17/2012 <0.001 <0.00025 <0.0005 <0.0083
157
Well Date P Se Ag Tl Zn
mg/L mg/L mg/L mg/L mg/L
MW-1 2/29/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-1 3/2/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-1 3/5/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-1 3/7/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-1 3/9/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-1 3/12/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-1 3/14/2012 0.29 <0.001 <0.00025 <0.0005 <0.0083
MW-1 3/19/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-1 3/21/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-1 3/23/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-1 3/26/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-1 4/2/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-1 4/9/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-1 4/12/2012 0.34 <0.001 <0.00025 <0.0005 <0.0083
MW-1 4/16/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-1 10/5/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-1 1/15/2013 0.21 <0.001 <0.00025 <0.0005 <0.0083
MW-2 2/12/2010 0.3 <0.001 <0.00025 <0.0005 0.013
MW-2 6/28/2010 0.36 <0.001 <0.00025 <0.0005 <0.0083
MW-2 7/30/2010 0.38 <0.001 <0.00025 <0.0005 <0.0083
MW-2 8/25/2010 0.45 <0.001 <0.00025 <0.0005 <0.0083
MW-2 10/5/2010 0.44 <0.001 <0.00025 <0.0005 <0.0083
MW-2 10/28/2010 0.22 <0.001 <0.00025 <0.0005 <0.0083
MW-2 12/2/2010 0.21 <0.001 <0.00025 <0.0005 <0.0083
MW-2 12/28/2010 0.31 <0.001 <0.00025 <0.0005 <0.0083
MW-2 1/26/2011 0.29 <0.001 <0.00025 <0.0005 <0.0083
MW-2 2/22/2011 0.3 <0.001 <0.00025 <0.0005 <0.0083
MW-2 5/20/2011 0.34 <0.001 <0.00025 <0.0005 <0.0083
MW-2 6/21/2011 0.39 <0.001 <0.00025 <0.0005 <0.0083
MW-2 7/19/2011 0.24 <0.001 <0.00025 <0.0005 <0.0083
MW-2 9/7/2011 0.29 <0.001 <0.00025 <0.0005 <0.0083
MW-2 9/15/2011 0.26 <0.001 <0.00025 <0.0005 <0.0083
MW-2 9/21/2011 0.31 <0.001 <0.00025 <0.0005 <0.0083
158
Well Date P Se Ag Tl Zn
mg/L mg/L mg/L mg/L mg/L
MW-2 9/28/2011 0.26 <0.001 <0.00025 <0.0005 <0.0083
MW-2 10/19/2011 0.25 <0.001 <0.00025 <0.0005 <0.0083
MW-2 11/10/2011 0.41 <0.001 <0.00025 <0.0005 <0.0083
MW-2 11/16/2011 0.26 <0.001 <0.00025 <0.0005 <0.0083
MW-2 12/1/2011 0.24 <0.001 <0.00025 <0.0005 <0.0083
MW-2 12/7/2011 <0.001 <0.00025 <0.0005 <0.0083
MW-2 12/14/2011 <0.001 <0.00025 <0.0005 <0.0083
MW-2 1/6/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-2 1/9/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-2 1/11/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-2 1/13/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-2 1/16/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-2 1/18/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-2 1/20/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-2 1/23/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-2 1/27/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-2 1/30/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-2 2/1/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-2 2/3/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-2 2/6/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-2 2/8/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-2 2/10/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-2 2/13/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-2 2/15/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-2 2/17/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-2 2/29/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-2 3/2/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-2 3/5/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-2 3/7/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-2 3/9/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-2 3/12/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-2 3/14/2012 0.24 <0.001 <0.00025 <0.0005 <0.0083
MW-2 3/19/2012 <0.001 <0.00025 <0.0005 <0.0083
159
Well Date P Se Ag Tl Zn
mg/L mg/L mg/L mg/L mg/L
MW-2 3/21/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-2 3/23/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-2 3/26/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-2 4/2/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-2 4/9/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-2 4/11/2012 0.27 <0.001 <0.00025 <0.0005 0.036
MW-2 4/16/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-2 10/4/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-2 1/14/2013 0.22 <0.001 <0.00025 <0.0005 <0.0083
MW-3 9/2/2010 0.27 <0.001 <0.00025 <0.0005 <0.0083
MW-3 10/5/2010 0.28 <0.001 <0.00025 <0.0005 <0.0083
MW-3 10/28/2010 0.18 <0.001 <0.00025 <0.0005 <0.0083
MW-3 12/2/2010 0.21 <0.001 <0.00025 <0.0005 <0.0083
MW-3 12/28/2010 0.28 <0.001 <0.00025 <0.0005 <0.0083
MW-3 1/24/2011 0.28 <0.001 <0.00025 <0.0005 <0.0083
MW-3 2/22/2011 0.27 <0.001 <0.00025 <0.0005 <0.0083
MW-3 5/19/2011 0.3 <0.001 <0.00025 <0.0005 0.008
MW-3 6/21/2011 0.3 <0.001 <0.00025 <0.0005 <0.0083
MW-3 7/19/2011 0.31 <0.001 <0.00025 <0.0005 <0.0083
MW-3 7/20/2011 0.31 <0.001 <0.00025 <0.0005 <0.0083
MW-3 7/21/2011 0.26 <0.001 <0.00025 <0.0005 <0.0083
MW-3 8/21/2011 0.27 <0.001 <0.00025 <0.0005 <0.0083
MW-3 8/23/2011 0.28 <0.001 <0.00025 <0.0005 <0.0083
MW-3 8/25/2011 <0.019 <0.001 <0.00025 <0.0005 <0.0083
MW-3 8/27/2011 0.34 <0.001 <0.00025 <0.0005 <0.0083
MW-3 8/29/2011 0.3 <0.001 <0.00025 <0.0005 <0.0083
MW-3 9/1/2011 0.32 <0.001 <0.00025 <0.0005 <0.0083
MW-3 9/8/2011 0.2 <0.001 <0.00025 <0.0005 <0.0083
MW-3 9/15/2011 0.29 <0.001 <0.00025 <0.0005 <0.0083
MW-3 9/22/2011 0.3 <0.001 <0.00025 <0.0005 <0.0083
MW-3 9/28/2011 0.26 <0.001 <0.00025 <0.0005 <0.0083
MW-3 10/5/2011 0.27 <0.001 <0.00025 <0.0005 <0.0083
MW-3 10/12/2011 0.29 <0.001 <0.00025 <0.0005 <0.0083
160
Well Date P Se Ag Tl Zn
mg/L mg/L mg/L mg/L mg/L
MW-3 10/17/2011 <0.001 <0.00025 <0.0005 <0.0083
MW-3 10/19/2011 0.27 <0.001 <0.00025 <0.0005 <0.0083
MW-3 10/21/2011 <0.001 <0.00025 <0.0005 <0.0083
MW-3 10/24/2011 <0.001 <0.00025 <0.0005 <0.0083
MW-3 10/26/2011 0.26 <0.001 0.0003 <0.0005 <0.0083
MW-3 10/28/2011 <0.001 <0.00025 <0.0005 <0.0083
MW-3 10/31/2011 <0.001 <0.00025 <0.0005 <0.0083
MW-3 11/2/2011 0.24 <0.001 0.0007 <0.0005 <0.0083
MW-3 11/4/2011 <0.001 <0.00025 <0.0005 <0.0083
MW-3 11/10/2011 0.36 <0.001 <0.00025 <0.0005 <0.0083
MW-3 11/11/2011 <0.001 <0.00025 <0.0005 <0.0083
MW-3 11/14/2011 <0.001 <0.00025 <0.0005 <0.0083
MW-3 11/16/2011 0.26 <0.001 <0.00025 <0.0005 <0.0083
MW-3 11/18/2011 <0.001 <0.00025 <0.0005 <0.0083
MW-3 11/21/2011 <0.001 <0.00025 <0.0005 <0.0083
MW-3 11/23/2011 0.23 <0.001 0.0003 <0.0005 0.009
MW-3 11/25/2011 <0.001 0.0003 <0.0005 <0.0083
MW-3 11/28/2011 <0.001 0.0003 <0.0005 <0.0083
MW-3 11/30/2011 0.25 <0.001 <0.00025 <0.0005 0.008
MW-3 12/2/2011 <0.001 <0.00025 <0.0005 <0.0083
MW-3 12/5/2011 <0.001 <0.00025 <0.0005 <0.0083
MW-3 12/7/2011 <0.001 <0.00025 <0.0005 <0.0083
MW-3 12/14/2011 <0.001 <0.00025 <0.0005 0.009
MW-3 1/4/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-3 3/15/2012 0.29 <0.001 <0.00025 <0.0005 <0.0083
MW-3 4/12/2012 0.28 <0.001 <0.00025 <0.0005 <0.0083
MW-3 10/5/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-3 1/15/2013 0.28 <0.001 <0.00025 <0.0005 <0.0083
MW-4 9/2/2010 0.26 <0.001 <0.00025 <0.0005 0.01
MW-4 10/5/2010 0.56 <0.001 <0.00025 <0.0005 <0.0083
MW-4 10/28/2010 0.2 <0.001 <0.00025 <0.0005 <0.0083
MW-4 12/3/2010 0.22 <0.001 <0.00025 <0.0005 <0.0083
MW-4 12/29/2010 0.31 <0.001 <0.00025 <0.0005 <0.0083
161
Well Date P Se Ag Tl Zn
mg/L mg/L mg/L mg/L mg/L
MW-4 1/25/2011 0.29 <0.001 <0.00025 <0.0005 <0.0083
MW-4 2/23/2011 0.34 <0.001 <0.00025 <0.0005 <0.0083
MW-4 5/20/2011 0.41 <0.001 <0.00025 <0.0005 <0.0083
MW-4 6/21/2011 0.39 <0.001 <0.00025 <0.0005 <0.0083
MW-4 7/19/2011 0.27 <0.001 <0.00025 <0.0005 <0.0083
MW-4 9/7/2011 0.2 <0.001 <0.00025 <0.0005 <0.0083
MW-4 9/16/2011 0.28 <0.001 <0.00025 <0.0005 <0.0083
MW-4 9/22/2011 0.31 <0.001 <0.00025 <0.0005 <0.0083
MW-4 9/28/2011 0.26 <0.001 <0.00025 <0.0005 <0.0083
MW-4 10/19/2011 0.24 <0.001 <0.00025 <0.0005 <0.0083
MW-4 11/10/2011 0.37 <0.001 <0.00025 <0.0005 <0.0083
MW-4 12/1/2011 0.24 <0.001 <0.00025 <0.0005 <0.0083
MW-4 3/14/2012 0.28 <0.001 <0.00025 <0.0005 <0.0083
MW-4 3/19/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-4 3/21/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-4 3/23/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-4 3/26/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-4 4/2/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-4 4/9/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-4 4/11/2012 0.25 <0.001 <0.00025 <0.0005 <0.0083
MW-4 4/16/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-4 10/4/2012 <0.001 <0.00025 <0.0005 <0.0083
MW-4 1/15/2013 0.21 <0.001 <0.00025 <0.0005 <0.0083
PW-1 2/12/2010 0.32 <0.001 <0.00025 <0.0005 0.014
PW-1 6/28/2010 0.56 <0.001 <0.00025 <0.0005 <0.0083
PW-1 7/30/2010 0.25 <0.001 <0.00025 <0.0005 <0.0083
PW-1 8/25/2010 0.49 <0.001 <0.00025 <0.0005 <0.0083
PW-1 12/4/2010 0.23 <0.001 <0.00025 <0.0005 <0.0083
PW-1 12/27/2010 0.31 <0.001 <0.00025 <0.0005 <0.0083
PW-1 1/25/2011 0.31 <0.001 <0.00025 <0.0005 <0.0083
PW-1 2/24/2011 0.27 <0.001 <0.00025 <0.0005 <0.0083
162
Table A-5. Dissolved organics.
Well Date
Acetic
Acid
Dissolved
Organic
Carbon
Lactic
Acid
Propionic
Acid Pyruvic Acid
mg/L mg/L mg/L mg/L mg/L
BG-1 9/2/2010 <0.24 0.74 <2.2 <0.093 <0.21
BG-1 10/6/2010 0.87 1.9 <2.2 <0.093 <0.21
BG-1 10/29/2010 0.72 2.1 <2.2 <0.093 <0.21
BG-1 12/3/2010 1.4 2 <2.2 <0.093 <0.21
BG-1 12/27/2010 <0.24 1.6 <2.2 <0.093 <0.21
BG-1 1/25/2011 0.37 1.9 <2.2 <0.093 <0.21
BG-1 2/23/2011 0.57 2.2 <2.2 0.093 0.21
BG-1 5/18/2011 2.4 3.1 <2.2 <0.093 <0.21
BG-1 6/22/2011 1.7 2.5 <2.2 <0.093 <0.21
BG-1 7/18/2011 2.4 2.6 <2.2 <0.093 <0.21
BG-1 9/7/2011 1.4 2.4 <2.2 <0.093 <0.21
BG-1 9/14/2011 0.38 2.2 <2.2 <0.093 <0.21
BG-1 9/21/2011 0.35 2 <2.2 <0.093 <0.21
BG-1 9/28/2011 0.24 2.2 <2.2 <0.093 <0.21
BG-1 10/19/2011 0.87 2.1 <2.2 0.097 <0.21
BG-1 11/10/2011 <0.24 1.3 <2.2 <0.093 <0.21
BG-1 12/1/2011 <0.24 1.8 <2.2 <0.093 <0.21
BG-1 3/15/2012 <0.24 1.3 <2.2 <0.093 <0.21
BG-1 4/11/2012 <0.24 2.7 <2.2 <0.093 <0.21
BG-1 1/14/2013 <0.24 6.2 <2.2 <0.093 <0.21
IW-1 9/2/2010 <0.24 0.8 <2.2 <0.093 <0.21
IW-1 12/3/2010 <0.24 2.6 <2.2 <0.093 <0.21
IW-1 12/28/2010 <0.24 1.7 <2.2 <0.093 <0.21
IW-1 1/26/2011 1.1 2.4 <2.2 <0.093 <0.21
IW-1 2/22/2011 0.61 2.8 <2.2 0.093 0.21
MW-1 2/12/2010
2
MW-1 6/28/2010 3.6 4.1
MW-1 7/30/2010 1.6 3.1
MW-1 8/25/2010 1.6 2.4
MW-1 10/5/2010 0.84 1.9 <2.2 <0.093 <0.21
MW-1 10/28/2010 <0.24 1.5 <2.2 <0.093 <0.21
MW-1 12/3/2010 <0.24 1.3 <2.2 <0.093 <0.21
MW-1 12/29/2010 <0.24 1.5 <2.2 <0.093 <0.21
MW-1 1/26/2011 <0.24 1.6 <2.2 <0.093 <0.21
MW-1 2/23/2011 <0.24 2 <2.2 0.093 0.21
MW-1 5/19/2011 <0.24 1.5 <2.2 <0.093 <0.21
MW-1 6/21/2011 0.24 1.4 <2.2 <0.093 <0.21
MW-1 7/19/2011 <0.24 3.2 <2.2 <0.093 <0.21
MW-1 9/8/2011 <0.24 2.1 6.1 <0.093 <0.21
MW-1 9/16/2011 <0.24 2.2 <2.2 <0.093 <0.21
MW-1 9/22/2011 <0.24 1.8 <2.2 <0.093 <0.21
163
Well Date
Acetic
Acid
Dissolved
Organic
Carbon
Lactic
Acid
Propionic
Acid Pyruvic Acid
mg/L mg/L mg/L mg/L mg/L
MW-1 9/28/2011 <0.24 1.9 <2.2 <0.093 <0.21
MW-1 10/19/2011 <0.24 2.5 <2.2 <0.093 <0.21
MW-1 11/10/2011 <0.24 1.5 <2.2 <0.093 <0.21
MW-1 12/1/2011 <0.24 1.9 <2.2 <0.093 <0.21
MW-1 3/14/2012 <0.24 4.4 <2.2 <0.093 <0.21
MW-1 4/12/2012 <0.24 11 <2.2 <0.093 <0.21
MW-1 1/15/2013 <0.24 9 2.4 <0.093 <0.21
MW-2 2/12/2010
2
MW-2 6/28/2010 2.7 2.9
MW-2 7/30/2010 0.24 2
MW-2 8/25/2010 0.3 2.3
MW-2 10/5/2010 <0.24 1.6 <2.2 <0.093 <0.21
MW-2 10/28/2010 <0.24 1.5 <2.2 <0.093 <0.21
MW-2 12/2/2010 <0.24 1.2 <2.2 <0.093 <0.21
MW-2 12/28/2010 <0.24 1.5 <2.2 <0.093 <0.21
MW-2 1/26/2011 <0.24 1.6 <2.2 <0.093 <0.21
MW-2 2/22/2011 <0.24 1.9 <2.2 0.093 0.21
MW-2 5/20/2011 <0.24 1.5 <2.2 <0.093 <0.21
MW-2 6/21/2011 0.24 1.5 <2.2 <0.093 <0.21
MW-2 7/19/2011 <0.24 4.6 <2.2 <0.093 <0.21
MW-2 9/7/2011 <0.24 2.2 <2.2 <0.093 <0.21
MW-2 9/15/2011 <0.24 2 <2.2 <0.093 <0.21
MW-2 9/21/2011 <0.24 1.9 <2.2 <0.093 <0.21
MW-2 9/28/2011 <0.24 1.9 <2.2 <0.093 <0.21
MW-2 10/19/2011 <0.24 2.2 <2.2 <0.093 <0.21
MW-2 11/10/2011 <0.24 1.3 <2.2 <0.093 <0.21
MW-2 11/16/2011 <0.24 <0.5 <2.2 <0.093 <0.21
MW-2 12/1/2011 <0.24 2.1 <2.2 <0.093 <0.21
MW-2 3/14/2012 <0.24 5.9 <2.2 <0.093 <0.21
MW-2 4/11/2012 <0.24 7.5 <2.2 <0.093 <0.21
MW-2 1/14/2013 <0.24 16 <2.2 <0.093 <0.21
MW-3 9/2/2010 0.42 1.4 <2.2 <0.093 <0.21
MW-3 10/5/2010 <0.24 1.3 <2.2 <0.093 <0.21
MW-3 10/28/2010 <0.24 1.5 <2.2 <0.093 <0.21
MW-3 12/2/2010 <0.24 1.2 <2.2 <0.093 <0.21
MW-3 12/28/2010 <0.24 1.6 <2.2 <0.093 <0.21
MW-3 1/24/2011 <0.24 1.8 <2.2 <0.093 <0.21
MW-3 2/22/2011 <0.24 1.9 <2.2 0.093 0.21
MW-3 5/19/2011 <0.24 2 <2.2 <0.093 <0.21
MW-3 6/21/2011 1.2 3 <2.2 <0.093 <0.21
MW-3 7/19/2011 1.3 2.6 <2.2 <0.093 <0.21
MW-3 7/20/2011 0.3 2.2 <2.2 <0.093 <0.21
164
Well Date
Acetic
Acid
Dissolved
Organic
Carbon
Lactic
Acid
Propionic
Acid Pyruvic Acid
mg/L mg/L mg/L mg/L mg/L
MW-3 7/21/2011 <0.24 2.1 <2.2 <0.093 <0.21
MW-3 8/21/2011 <0.24 1.8 <2.2 <0.093 <0.21
MW-3 8/23/2011 <0.24 2.1 <2.2 <0.093 <0.21
MW-3 8/25/2011 <0.24 2 <2.2 <0.093 <0.21
MW-3 8/27/2011 <0.24 2.1 <2.2 <0.093 <0.21
MW-3 8/29/2011 <0.24 1.9 <2.2 <0.093 <0.21
MW-3 9/1/2011 0.61 2 <2.2 <0.093 <0.21
MW-3 9/8/2011 0.42 2.4 <2.2 <0.093 <0.21
MW-3 9/15/2011 <0.24 2.1 <2.2 <0.093 <0.21
MW-3 9/22/2011 <0.24 2 <2.2 <0.093 <0.21
MW-3 9/28/2011 <0.24 2 <2.2 <0.093 <0.21
MW-3 10/5/2011 <0.24 2.3 <2.2 <0.093 <0.21
MW-3 10/12/2011 <0.24 2 <2.2 <0.093 <0.21
MW-3 10/19/2011 <0.24 2.4 <2.2 <0.093 <0.21
MW-3 10/26/2011 <0.24 2 <2.2 <0.093 <0.21
MW-3 11/2/2011
2.5
MW-3 11/10/2011 <0.24 3.4 <2.2 <0.093 <0.21
MW-3 11/16/2011 <0.24 1.4 <2.2 <0.093 <0.21
MW-3 11/23/2011 <0.24 2.1 <2.2 <0.093 <0.21
MW-3 11/30/2011 <0.24 3.2 <2.2 <0.093 <0.21
MW-3 3/15/2012 <0.24 5.7 <2.2 <0.093 <0.21
MW-3 4/12/2012 <0.24 9.8 <2.2 <0.093 <0.21
MW-3 1/15/2013 0.24 17 6.9 <0.093 <0.21
MW-4 9/2/2010 <0.24 1.3 <2.2 <0.093 <0.21
MW-4 10/5/2010 7.2 6.1 <2.2 <0.093 <0.21
MW-4 10/28/2010 <0.24 1.6 <2.2 <0.093 <0.21
MW-4 12/3/2010 <0.24 1.8 <2.2 <0.093 <0.21
MW-4 12/29/2010 <0.24 1.7 <2.2 <0.093 <0.21
MW-4 1/25/2011 0.39 2.2 <2.2 <0.093 <0.21
MW-4 2/23/2011 2.1 3 <2.2 0.093 0.21
MW-4 5/20/2011 <0.24 2 <2.2 <0.093 <0.21
MW-4 6/21/2011 0.24 1.7 <2.2 <0.093 <0.21
MW-4 7/19/2011 <0.24 3.7 <2.2 <0.093 <0.21
MW-4 9/7/2011 <0.24 2.1 <2.2 <0.093 <0.21
MW-4 9/16/2011 <0.24 2.1 <2.2 <0.093 <0.21
MW-4 9/22/2011 <0.24 2.1 <2.2 <0.093 <0.21
MW-4 9/28/2011 <0.24 21 <2.2 <0.093 <0.21
MW-4 10/19/2011 <0.24 2.3 <2.2 <0.093 <0.21
MW-4 11/10/2011 <0.24 1.5 5.2 <0.093 <0.21
MW-4 12/1/2011 <0.24 2.1 <2.2 <0.093 <0.21
MW-4 3/14/2012 <0.24 1.6 <2.2 <0.093 <0.21
MW-4 4/11/2012 <0.24 3 <2.2 <0.093 <0.21
165
Well Date
Acetic
Acid
Dissolved
Organic
Carbon
Lactic
Acid
Propionic
Acid Pyruvic Acid
mg/L mg/L mg/L mg/L mg/L
MW-4 1/15/2013 <0.24 11 <2.2 <0.093 <0.21
PW-1 2/12/2010
1.9
PW-1 6/28/2010 16 9.1
PW-1 7/30/2010 2.1 7.1
PW-1 8/25/2010 4.7 1.9
PW-1 12/4/2010 <0.24 1.6 <2.2 <0.093 <0.21
PW-1 12/27/2010 <0.24 1.7 <2.2 <0.093 <0.21
PW-1 1/25/2011 <0.24 1.9 <2.2 <0.093 <0.21
PW-1 2/24/2011 <0.24 2.1 <2.2 0.093 0.21
166
Table A-6. Dissolved gas measurements.
Well Date NH3 as N Carbon
Dioxide
Carbon
Monoxide
Oxygen Ethane Ethylene Methane Nitrogen Sulfide, Lab
mg/L ug/L ug/L ug/L ug/L ug/L ug/L ug/L mg/L
BG-1 9/2/2010 0.3 51 <1.1
BG-1 10/6/2010 0.35 39 <0.17 <0.11 11 <1.1
BG-1 10/29/2010 0.27 47 <0.17 <0.11 20 1.3
BG-1 12/3/2010 0.34 56 0.19 <0.11 50 <1.1
BG-1 12/27/2010 0.38 63 <0.17 <0.11 24 <1.1
BG-1 1/25/2011 0.25 57 0.2 <0.11 45 <1.1
BG-1 2/23/2011 0.28 68 <0.17 <0.11 38 <1.1
BG-1 5/18/2011 0.32 49 0.2 0.13 150 1.6
BG-1 6/22/2011 0.28 40 <0.17 <0.11 240 <1.1
BG-1 7/18/2011 0.41 36 0.32 <0.11 160 <1.1
BG-1 9/7/2011 0.43 35 <13 0.25 <0.11 140 4800 <1.1
BG-1 9/14/2011 0.32 55 <13 0.23 <0.11 130 4600 <1.1
BG-1 9/21/2011 0.31 52 <13 <0.17 <0.11 110 7000 <1.1
BG-1 9/28/2011 0.3 54 <13 1600 0.2 <0.11 120 4700 <1.1
BG-1 10/19/2011 0.33 38 <13 1900 0.28 <0.11 150 5700 <1.1
BG-1 11/10/2011 0.35 67 <13 1400 0.26 <0.11 170 4400 <1.1
BG-1 12/1/2011 0.35 170 <13 1300 0.25 <0.11 120 3900 <1.1
BG-1 3/15/2012 0.24 0.27 <0.11 96 <1.1
BG-1 4/11/2012 0.31 0.2 <0.11 77 <1.1
BG-1 1/14/2013 0.088 <0.75 <0.55 120
IW-1 9/2/2010 0.17 57 <1.1
IW-1 12/3/2010 0.35 25 0.34 0.45 210 <1.1
IW-1 12/28/2010 0.43 67 <0.17 <0.11 33 <1.1
IW-1 1/26/2011 0.28 57 <0.17 <0.11 160 <1.1
IW-1 2/22/2011 0.23 45 0.19 <0.11 190 1.3
MW-1 2/12/2010 0.29 100 3.8 <1.1
MW-1 6/28/2010 82 <1.1
MW-1 7/30/2010 94 <1.1
MW-1 8/25/2010 0.21 98 <1.1
167
Well Date NH3 as N Carbon
Dioxide
Carbon
Monoxide
Oxygen Ethane Ethylene Methane Nitrogen Sulfide, Lab
mg/L ug/L ug/L ug/L ug/L ug/L ug/L ug/L mg/L
MW-1 10/5/2010 0.32 83 1 0.29 640 <1.1
MW-1 10/28/2010 0.26 120 0.19 <0.11 45 1.3
MW-1 12/3/2010 0.33 96 <0.17 <0.11 28 <1.1
MW-1 12/29/2010 0.39 120 <0.17 <0.11 48 <1.1
MW-1 1/26/2011 0.27 100 0.18 <0.11 57 <1.1
MW-1 2/23/2011 0.24 95 0.56 <0.11 230 4.8
MW-1 5/19/2011 0.32 110 0.92 <0.11 260 1.2
MW-1 6/21/2011 0.33 91 1 <0.11 330 <1.1
MW-1 7/19/2011 0.38 110 2.5 <0.11 340 <1.1
MW-1 9/8/2011 0.42 120 <13 0.31 <0.11 63 4800 <1.1
MW-1 9/16/2011 0.34 120 <13 0.33 <0.11 110 6100 <1.1
MW-1 9/22/2011 0.32 120 <13 0.23 <0.11 81 5000 <1.1
MW-1 9/28/2011 0.35 100 <13 1700 0.23 <0.11 87 5200 <1.1
MW-1 10/19/2011 0.34 120 <13 1600 0.39 <0.11 110 4800 <1.1
MW-1 11/10/2011 0.34 330 <13 1500 0.35 <0.11 120 4700 <1.1
MW-1 12/1/2011 0.36 150 <13 1500 0.4 <0.11 140 4400 1.1
MW-1 3/14/2012 0.19 1.9 <0.11 6.8 1.6
MW-1 4/12/2012 0.083 1.9 <0.11 9 2.1
MW-1 1/15/2013 0.14 1.9 <0.55 130
MW-2 2/12/2010 0.28 74 11 <1.1
MW-2 6/28/2010 74 1.1
MW-2 7/30/2010 92 <1.1
MW-2 8/25/2010 0.24 62 <1.1
MW-2 10/5/2010 0.38 80 2.2 <0.55 1900 1.1
MW-2 10/28/2010 0.27 80 <0.17 <0.11 290 1.5
MW-2 12/2/2010 0.32 98 <0.17 <0.11 170 <1.1
MW-2 12/28/2010 0.36 110 <0.17 <0.11 180 <1.1
MW-2 1/26/2011 0.26 84 0.21 <0.11 190 <1.1
MW-2 2/22/2011 0.2 82 <0.17 <0.11 180 <1.1
MW-2 5/20/2011 0.38 93 1.3 <0.11 430 <1.1
168
Well Date NH3 as N Carbon
Dioxide
Carbon
Monoxide
Oxygen Ethane Ethylene Methane Nitrogen Sulfide, Lab
mg/L ug/L ug/L ug/L ug/L ug/L ug/L ug/L mg/L
MW-2 6/21/2011 0.32 58 2.1 <0.11 800 1.3
MW-2 7/19/2011 0.41 84 2.4 <0.11 620 <1.1
MW-2 9/7/2011 0.45 90 <13 0.33 <0.11 160 5300 <1.1
MW-2 9/15/2011 0.33 110 <13 0.26 <0.11 140 4400 <1.1
MW-2 9/21/2011 0.32 110 <13 <0.17 <0.11 120 4800 <1.1
MW-2 9/28/2011 0.3 110 <13 1600 0.2 <0.11 110 4900 <1.1
MW-2 10/19/2011 0.31 91 <13 1500 0.29 <0.11 170 5000 <1.1
MW-2 11/10/2011 0.32 180 <13 1800 0.3 <0.11 180 5200 <1.1
MW-2 11/16/2011 0.26 220 <13 1500 0.2 <0.11 98 4200 <1.1
MW-2 12/1/2011 0.36 140 <13 1500 0.19 <0.11 69 4200 <1.1
MW-2 3/14/2012 0.09 2.6 <0.11 20 1.6
MW-2 4/11/2012 0.079 2 <0.11 30 <1.1
MW-2 1/14/2013 0.032 <0.75 <0.55 9.3
MW-3 9/2/2010 0.44 7 <1.1
MW-3 10/5/2010 0.37 56 <0.17 <0.11 13 <1.1
MW-3 10/28/2010 0.29 56 <0.17 <0.11 10 <1.1
MW-3 12/2/2010 0.33 70 <0.17 <0.11 11 <1.1
MW-3 12/28/2010 0.45 68 <0.17 <0.11 13 <1.1
MW-3 1/24/2011 0.28 45 0.26 <0.11 20 <1.1
MW-3 2/22/2011 0.16 57 <0.17 <0.11 26 1.6
MW-3 5/19/2011 0.36 29 <0.17 <0.11 82 1.3
MW-3 6/21/2011 0.43 9 <0.17 <0.11 190 <1.1
MW-3 7/19/2011 0.5 18 <0.17 <0.11 120 <1.1
MW-3 7/20/2011 0.45 30 <0.17 <0.11 67 <1.1
MW-3 7/21/2011 0.46 46 <0.17 <0.11 37 <1.1
MW-3 8/21/2011 0.39 59 <13 <0.17 <0.11 20 5300 <1.1
MW-3 8/23/2011 0.4 46 <13 <0.17 <0.11 23 5100 <1.1
MW-3 8/25/2011 0.37 51 <13 <0.17 <0.11 22 5200 <1.1
MW-3 8/27/2011 0.36 59 <13 <0.17 <0.11 24 6000 <1.1
MW-3 8/29/2011 0.35 76 <13 <0.17 <0.11 43 4800 <1.1
169
Well Date NH3 as N Carbon
Dioxide
Carbon
Monoxide
Oxygen Ethane Ethylene Methane Nitrogen Sulfide, Lab
mg/L ug/L ug/L ug/L ug/L ug/L ug/L ug/L mg/L
MW-3 9/1/2011 0.45 56 <13 <0.17 <0.11 41 7100 <1.1
MW-3 9/8/2011 0.46 45 <13 0.17 <0.11 65 4000 <1.1
MW-3 9/15/2011 0.36 52 <13 <0.17 <0.11 64 5200 <1.1
MW-3 9/22/2011 0.39 47 <13 <0.17 <0.11 34 4900 <1.1
MW-3 9/28/2011 0.33 49 <13 1500 <0.17 <0.11 25 4300 <1.1
MW-3 10/5/2011 0.33 54 <13 1500 <0.17 <0.11 19 4400 <1.1
MW-3 10/12/2011 0.37 55 <13 1600 <0.17 <0.11 19 4800 <1.1
MW-3 10/19/2011 0.35 69 <13 1500 <0.17 <0.11 17 4400 <1.1
MW-3 10/26/2011 0.31 110 <13 1300 <0.17 <0.11 26 4000 <1.1
MW-3 11/2/2011 0.31 5400 <13 920 0.77 <0.11 23 3100 <1.1
MW-3 11/10/2011 0.16 17000 <13 150 1.9 <0.11 25 380 <1.1
MW-3 11/16/2011 0.067 19000 <13 190 1.3 <0.11 14 450 <1.1
MW-3 11/23/2011 0.065 9900 <13 100 0.33 <0.11 3.2 170 1.1
MW-3 11/30/2011 0.13 19000 <13 190 1.8 <0.11 14 360 <1.1
MW-3 3/15/2012 0.056 1.3 <0.11 3.7 <1.1
MW-3 4/12/2012 0.045 0.49 <0.11 2 1.6
MW-3 1/15/2013 0.16 <0.75 <0.55 8.2
MW-4 9/2/2010 0.35 80 <1.1
MW-4 10/5/2010 0.32 57 0.32 0.65 120 <1.1
MW-4 10/28/2010 0.28 80 <0.17 <0.11 17 <1.1
MW-4 12/3/2010 0.31 83 <0.17 <0.11 21 1.5
MW-4 12/29/2010 0.38 77 <0.17 <0.11 45 <1.1
MW-4 1/25/2011 0.26 68 <0.17 0.18 81 <1.1
MW-4 2/23/2011 0.21 65 1.1 <0.11 320 <1.1
MW-4 5/20/2011 0.35 84 1.8 <0.11 930 <1.1
MW-4 6/21/2011 0.3 73 <0.85 <0.55 1500 <1.1
MW-4 7/19/2011 0.39 74 1.8 <0.11 1000 1.7
MW-4 9/7/2011 0.41 99 <13 0.22 <0.11 130 4900 <1.1
MW-4 9/16/2011 0.33 110 <13 0.26 <0.11 200 5400 <1.1
MW-4 9/22/2011 0.36 110 <13 0.19 <0.11 150 4500 <1.1
170
Well Date NH3 as N Carbon
Dioxide
Carbon
Monoxide
Oxygen Ethane Ethylene Methane Nitrogen Sulfide, Lab
mg/L ug/L ug/L ug/L ug/L ug/L ug/L ug/L mg/L
MW-4 9/28/2011 0.27 92 <13 1800 0.22 <0.11 180 5400 <1.1
MW-4 10/19/2011 0.33 96 <13 1700 0.19 <0.11 120 4900 <1.1
MW-4 11/10/2011 0.33 150 <13 1500 0.3 <0.11 200 4600 <1.1
MW-4 12/1/2011 0.35 140 <13 1500 0.26 <0.11 170 4600 <1.1
MW-4 3/14/2012 0.24 0.27 <0.11 110 1.1
MW-4 4/11/2012 0.32 0.28 <0.11 100 <1.1
MW-4 4/16/2012
MW-4 1/15/2013 0.13 1.3 <0.55 310
PW-1 2/12/2010 0.3 41 3.8 <1.1
PW-1 6/28/2010 17 <1.1
PW-1 7/30/2010 51 <1.1
PW-1 8/25/2010 0.15 30 <1.1
PW-1 12/4/2010 0.32 75 <0.17 <0.11 170 1.2
PW-1 12/27/2010 0.43 69 <0.17 <0.11 87 <1.1
PW-1 1/25/2011 0.29 63 0.37 0.12 260 <1.1
PW-1 2/24/2011 0.33 60 0.58 0.47 520 <1.1