chapter 11: properties of liquids
DESCRIPTION
Chapter 11: Properties of Liquids. Dr. Aimée Tomlinson. Chem 1212. Section 11.1. Solutions. What is a solution?. Solutions are formed from the addition of two species. Solution. Solute: dilute species. Solvent: abundant species. +. =. thegldc.com/blog/tag/water/. - PowerPoint PPT PresentationTRANSCRIPT
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CHAPTER 11: PROPERTIES OF LIQUIDS
Dr. Aimée TomlinsonChem1212
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Solutions
Section 11.1
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gusville.com/index/LIS753/images/
What is a solution?Solutions are formed from the addition of two species
Solute: dilute species
www.webmd.com/diet/slideshow-salt-shockers
Solvent: abundant species Solution
+ =
thegldc.com/blog/tag/water/
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Energy Changes & Solution Processes
Section 11.2
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Universal Solution Rule
Like dissolves LikePolar/ionic species require polar solvent
Nonpolar compounds require nonpolar solvents
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Energy Steps in Solution FormationStep 1: solute is separated into its individual components – endothernic, ΔH1 Step 2: IF between solvent molecules are broken – endothermic, ΔH2 Step 3: IF are generated between solute and solvent – exothermic, -ΔH3
On the left we have ΔHsolution < 0 Solute is completely solubleE.g. NaCl in water
1 2 3solutionH H H H
On the right we have ΔHsolution > 0 Solute is only partially solubleE.g. CaSO4 in water
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Units of Concentration
Section 11.3
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Measuring Solute to Solvent
moles of soluteML of solvent
Molarity
100%mass of soluteMass percentmass of solution
Mass Percent/Percent by weight
A AA
A B tot
n nn n n
Mole Fraction
moles of solutemkg of solvent
Molality
6 or 10mg of solute g of soluteppmkg of solvent g of solvent
Parts per Million, ppm
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Factors that Affect Solubility
Section 11.4
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Chemical StructureMiscibility
How well two substances mix togetherwww.bridalwave.tv/alternative_hen/
ImmiscibilityWhen two substances do not mix together
Partial MiscibilityHydrophilic component will mix in water while hydrophobic part won’tThe longer he hydrophobic chain the less miscible it will be in water
novocreamseparators.com/blog/clean-separation/
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Which one is more soluble in H2O?
CHCl3 CCl4
C6H11OH CH3OH
NaF MgO
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Pressure
Primarily important for gases dissolved in solvent
Henry’s Law: gas solubility is directly proportional to gas pressureMathematically: Cgas = kHPgas
where Cgas is concentration of the gas in solution kH is Henry's constant for this gas in a particular solution
As we increase the pressure we increase the number of gaseous moles we can push into solutionThe opposite is also true, reduce P we reduce concentration
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Example CalculationCalculate the solubility of oxygen in water at 20C and an atmospheric pressure of 0.35 atm. The mole fraction of O2 in the air is 0.209 and kO2 = 1.3 x 10-3 mol/L*atm. (Answer: 9.5 x 10-5 M)
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Temperature
we have already mentioned that we can increase T to force mixing between compounds
I should point out that if we are trying to mix polar and nonpolar species no amount of heat increase will ever cause miscibility
previously, I eluded to the idea that the sign ΔHsoln of is a predictor as to the solubility of two species
whille it is true to some extent there are many other factor which must also be consideredto be technically correct we must perform experiments to truly determine the extent of miscibility or immiscibility of two species
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Physical Behavior of Solutions: Colligative Properties
Section 11.5
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Here they are …
Vapor Pressure/Boiling Point Elevation
http://cirellio.files.wordpress.com/2008/06/boiling-water.jpg
Freezing Point Depression
www.blog.thesietch.org/.../
Osmotic Pressure
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Vapor Pressures of Solutions
Section 11.6
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Vapor Pressure & Temperature
VP increases as T increasesWhen T increases so do the molecular motions & kinetic E eventually allowing molecules to escape from l to g
RULE: to go from l → g, VP must equal atmospheric P
At higher elevations there is less atmospheric P so less heat is needed to boil (why water will boil below 100⁰C in Denver
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Experiment – DI water vs Seawater
Over time, DI water is reduced as seawater increases
Water escapes from DI beaker faster
DI water liquifies back into the salt water beakerThe driving force is water wants to solvate salt Recall ion-dipole forces are stronger (more stable) than HbondingThis is why we use desicator packets to protect leather goods
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TAKEHOME MESSAGE
The presence of a nonvolatile solute lowers the VP of a solvent
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Calculating Vapor PressureWe use Raoult’s Law: solution solvent solventP P
Example problem: What is the vapor pressure of water in a 50:50 mixture of glycerol (DC3H8O3 = 1.261 g/mL) and water at 25C (PH2O = 23.8 torr)? (Answer: Psoln = 19.1 torr)
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Vapor Pressure for Volatile MixturesPetroleum Industry
Oil is composed of a number of different hydrocarbonsThese all have similar but different boiling pointsThey can be separated through fractional distillation (see Section 11.10)
Raoult’s Law for a Volatile Mixture: All ideal solutions obey this Law
Example for Ideal Solution: Octane & Heptane
solution i ii
P P
They possess the following similarities:SizeBoiling pointIntermolecular forces (solute-solute,
solvent-solvent, and solute-solvent
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Deviations from Raoult’s Law
Negative deviations: Solute-solvent interactions are stronger than solute-solute or solvent-solvent one
Positive deviations: Solute-solvent interactions are weaker than solute-solute or solvent-solvent one
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Example of Volatile MixtureAt 20C, the VP of ethanol is 45 torr and the VP. of methanol is 92 torr. What is the VP at 20C of a solution prepared by mixing 75g of methanol and 25g of ethanol? (Answer: Psoln = 83 torr)
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Boiling Pt Elevation & Freezing Pt Depression
of Solutions
Section 11.7
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Reminder: VP & Bpt Relationship
At boiling VP = Patm
Recall Seawater ExperimentThe salt lowered VP of water
This makes a larger energy gap to reach Patm
A larger gap means more heat required to boil
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TAKEHOME MESSAGE II
The presence of a nonvolatile solute raises the boiling point of a solution
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Boiling Point ElevationBoiling point line is shifted when nonvolatile solute is added
Mathematically: where ΔTb is the change in boiling point, Kb is a
constant, and msolute is the molality of the solute in solution
b b soluteT K m
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Example Bpt Elevation ProblemIf the boiling point of a sample is 2.3 Celcius above the boiling point of pure water, what is the molality of NaCl in the sample?(Answer: 4.4 m NaCl)
, 0.52 /ob waterK C kg mol
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Freezing Point Depression
Similar to Boiling PointSalt melts ice by lowering the VP
This makes the freezing point lower
Lowering freezing point ends up allowing water to melt above its normal freezing point T
Mathematically: f f soluteT K m www.uniongas.com/images/meltingIcetechnology.jpg
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Osmosis & Osmotic Pressure
Section 11.8
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Osmosis
When solvent passes through a semipermeable membrane to balance the solute concentrations on each side of the membrane
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Osmotic Pressureamount of pressure needed to stop the solvent from flowing to the more concentrated side of a semipermeable membrane
http://nanotech.sc.mahidol.ac.th/genchem/liquid1/osmo.jpg
0.0821 L atmmol KMRT R
M molarity T in K
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Easy Example ProblemCalculate the osmotic pressure across a semipermeable membrane separating seawater (1.14 M) from a solution of normal saline (0.31 M) at a T = 20C. (Answer: 20 atm)
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Difficult Example ProblemA solution was made by dissolving 5.00 mg of hemoglobin in water to give a final volume of 1.00 mL. The osmotic pressure of this solution was 1.91 x 10-3 atm at 25 oC. Calculate the molar mass of hemoglobin. (Answer: 6.41 x 104 g/mol)
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Reverse Osmosissolvent is pumped through semi-impermeable membrane at a pressure greater than leaving behind solute particles
www.goodhousekeeping.com/cm/goodhousekeeping/...
Used to purify water
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Applications & Fractional Distillation
Section 11.9 & 11.10
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Fractional Distillation
Mixtures are separated by this method
Lower bpt components boil first & collected at the top (e.g. petrol)
Higher bpt special boil last and are collected at the bottom (e.g. crude oil)
http://gcsesciencealive.co.uk/images/Fractional%20distillation.gif
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Electrolytic Solutions
Section
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Reminder: What are Electrolytes?
They are solutions possessing ions
They allow water to conduct electricity
Strong electrolytes dissolve completely (e.g. NaCl)
Weak electrolytes only partially dissolve (e.g. CaSO4)
Non-electrolytes do not dissolve inwater at all and are not ionic (e.g. glycerol)
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van’t Hoff Factor, i
Used to indicated the strength of the electrolyte
moles of particles in solutionimoles of solutedissolved
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What is i for the following?
LiF
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What is i for the following?
MgO
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What is i for the following?
Calcium Phosphate
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True Colligative EquationsElectrolytes DO matter!!!
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Example ProblemThe van't Hoff factor for a 0.05 m solution of magnesium sulfate is 1.3. What is the freezing point of the solution?(Answer: ΔTf = -0.12⁰C)
f, 1.86 /owaterK C kg mol
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If the boiling point of a sample is 2.3 Celcius above the boiling point of pure water, what is the molality of NaCl in the sample? (Answer: 2.2 m NaCl)
Bpt Example with i
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Conceptual ProblemFor the list of compounds below rank them in order of increasing boiling point, freezing point, osmotic pressure and vapor pressure. Assume a 1.0M solution for each reagent and complete dissociation where applicable. C11H22O11, KBr, Li2SO4
First, we determine i for each compound.
C11H22O11 → i = 1
KBr → i =2
Li2SO4→ i = 3
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Conceptual ProblemFor the list of compounds below rank them in order of increasing boiling point, freezing point, osmotic pressure and vapor pressure. Assume a 1.0M solution for each reagent and complete dissociation where applicable. C11H22O11, KBr, Li2SO4
We use i,C11H22O11(i = 1), KBr(i =2), Li2SO4( i = 3), and the mathematical equation for each trend
Boiling Point Trend:
C11H22O11 < KBr < Li2SO4
b b soluteT iK m
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Conceptual ProblemFor the list of compounds below rank them in order of increasing boiling point, freezing point, osmotic pressure and vapor pressure. Assume a 1.0M solution for each reagent and complete dissociation where applicable. C11H22O11, KBr, Li2SO4
We use i,C11H22O11(i = 1), KBr(i =2), Li2SO4( i = 3), and the mathematical equation for each trend
Freezing Point Trend:
Li2SO4 < KBr < C11H22O11
f f soluteT iK m
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Conceptual ProblemFor the list of compounds below rank them in order of increasing boiling point, freezing point, osmotic pressure and vapor pressure. Assume a 1.0M solution for each reagent and complete dissociation where applicable. C11H22O11, KBr, Li2SO4
We use i,C11H22O11(i = 1), KBr(i =2), Li2SO4( i = 3), and the mathematical equation for each trend
Osmotic Pressure Trend:
C11H22O11 < KBr < Li2SO4
iMRT
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Conceptual ProblemFor the list of compounds below rank them in order of increasing boiling point, freezing point, osmotic pressure and vapor pressure. Assume a 1.0M solution for each reagent and complete dissociation where applicable. C11H22O11, KBr, Li2SO4
We use i,C11H22O11(i = 1), KBr(i =2), Li2SO4( i = 3), and the mathematical equation for each trend
Vapor Pressure Trend:
Li2SO4 < KBr < C11H22O11
lnso solvent solvent
solventsolvent
solute solvent
P Pn
i n n
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Example VP Problem with iWhat is the VP of a solution containing 1L of water and 500 g of NaCl? (at 25⁰C the VP of water is 23.8 torr) (Answer: 18.2 torr)