the barbiturates in forensic chemistry
TRANSCRIPT
THE BARBITURATES IN FORENSIC CHEMISTRY
DISSERTATIONPresented in Partial Fulfillment of the Requirements
for the Degree Doctor of Philosophy- in the Graduate School of The Ohio State
University
EQr
GWENDOLYN BERTHA CARSON, B« S., M* A* The Ohio State University
195U
Approved by*
Department of Physiological Chemistry ___________
i
TABLE OP CONTENTSpage
A« Introduction 1B» Historical
1. The Barbiturates - - - - - - - - - - - - - - - - 22* Barbiturate Poisoning - - -------------------- U
a) Deaths due to Barbiturates in Pour Countiesand the United States - - ------ -----11
b) Doses of Barbiturates in Grains - - -- - - 163* Barbiturate Regulations-------------------- 21
C. Isolation of the Barbiturates----- ---- ----- 2h
D» Qualitative Tests for Barbiturates ----- — - ---- 26E. Quantitative Methods for Barbiturates - - - - - - - - 28F* Examination of Tissues --- — 30
1# Degradation Products of Barbiturates - - - - - - 312a Percent Recovery of Unchanged Barbiturates - - - 3
G. Experimental Procedures - - - - - - - - - - - - - - - 351* Effect of 5$ Potassium Hydroxide on Barbiturates- 362 . Effect of 20$ Acetic Acid on Barbiturates - - - - 383. Effect of Water on Salts of Barbituric Acids - - 38 k» Barbiturates Extracted from Liver with 5$ Potassium
Hydroxide - — _ _ _ ip.5. Barbiturates Extracted from Liver with 20$ Acetic
A c i d ------------------------------- Hi6. Barbiturates Extracted from Liver at pH 1 0 HU7. Refractive Indices of Barbiturates - ------- H68. Barbiturate-Cyanide Reaction---------------- 509» Effect of Atmospheric Conditions on Barbiturates- £2
H* Discussion --- 53I* Summary - - - - - - — — ----— ------------ 63J. Conclusion — --------- — ------- 6HK. Bibliography----------------------------------- 66Iw Autobiography--------------- 73
ii
LIST OF TABLESpage
Table I Formulae of Barbituric Acids - ----- 6Table II Names and Synonyms of Barbituric Acids - - - - 9Table III Patent Data for Barbituric Acids - - ---- 10Table IV Deaths due to Barbiturates in New York City - - - - 11Table V Deaths due to Barbiturates in Franklin County, Ohio 12Table VI Deaths due to Barbiturates in Cuyahoga County, Ohio 13Table VII Deaths due to Barbiturates in Los Angeles County,
California - -- -- -- -- -- -- -- -- -- - lit
Table VIII Deaths due to Barbiturates in 1+8 States -------- 15Table IX Doses of Barbituric Acid Derivatives in Grains - - 16Table X Minimum Quantity of Barbiturate found in Tissues in
Poison Cases - - - - - - - - - - - - - - - - - - - 20Table XI Degradation Products Reported for some Barbiturates 31Table XII Percent Recovery of Unchanged Barbiturates from Urine 3k
Table XIII Melting Points of Barbituric Acids Recovered after2k Hour Treatment with 5$ Potassium Hydroxide - - - 37
Table XIV Melting Points of Barbituric Acids Recovered after2k Hour Treatment with 20% Acetic Acid - 39
Table XV Melting Points of Barbituric Acids Recovered from their Salts after 2k Hour Treatment with Distilled W a t e r --- UO
Table XVI Melting Points of Barbituric Acids Recovered fromBarbiturate-Liver Mixtures after 2k Hour Treatment with 5$ Potassium Hydroxide - ----- k2
Table XVII Melting Points of Barbituric Acids Recovered fromBarbiturate-Liver Mixtures after 2k Hour Treatmentwith 2C$ Acetic A cid---------- - 1+3
Table XVIII Melting Points of Barbituric Acids Recovered fromBarbiturate-Liver Mixtures after 2i+ Hour Treatment at pH 10 - - - -------- 1+5
illLIST OF TABLES (continued)
pageTable XTX Melting Points of Pure Barbituric Acids - - - - - I46Table XX(a) Refractive Indices of Barbituric Acids - --- U7Table XX(b) Refractive Indices of Barbituric Acids - - --- H8Table XX(c) Temperatures at which Refractive Indices were
Measured --- k9
Table XXI Melting Points of Materials Recovered from theBarbituric Acid-Cyanide Reaction Mixtures - - - - $1
Table XXII Melting Points of Barbituric Acids after Exposureto Atmospheric Conditions at Room Temperature - - $2
iv
ACKNOWLEDGEMENT
The author wishes to acknowledge the assistance of Dr* Clayton S* Sbiith, her preceptor and Chairman of the Department of Physiological Chemistry and the helpful suggestions of Dr* Helen L* Wikoff, Associate Professor of Physiological Chemistry, in carrying out this investigation
She also wishes to acknowledge receipt of statistical data on deaths due to barbiturates from the Coroner's Office in New York City; Cuyahoga County, Ohio and Los Angeles County, California.
The author also wishes to acknowledge gifts of the following barbituric acid derivatives used in making the determinations investigated in this dissertation;
Allyl-n-butyl barbituric acid; Butethal; Ethyl allyl barbituric acid; Mosidal; Pentobarbital; Phenobarbital and Pentothal from Abbott Laboratories.
Nostal; Pemoston and Sigmodal from Ames Company, Inc*Dial from Ciba Pharmaceuticals, Inc*Alurate from Hofftaan-La Roche, Inc*Amobarbital and Secobarbital from Eli Lilly and Company*Rutonal from May and Baker, Ltd., Dagenham, England*Butisol from McNeil Laboratories, Inc*Ortal from Parke, Davis and Company,Sandoptal from Sandoz Pharmaceuticals*Delvinal froip Sharp and Dohme, Inc*Ipral from E. R. Squibb and Sons andCyclobarbital; Evipal and Mephobarbital from Winthrop-Steams, Inc*
THE BARBITUATES IN FORENSIC CHEM ISTRY
A.’ INTRODUCTION
Forensic chemistry may he defined as chemistry applied to the solution of legal problems which may arise in connection with the administration of justice* This field covers the application of chemistry to both criminal and civil investigations*1
The forensic chemist may be called upon to examine blood stains; clothing; counterfeit coins; documents; dusts; various types of fibers; strings and ropes; hairs and textiles, in addition to making chemical analyses of drugs, medicines and vital organs#
Of the numerous drugs and medicines which might be involved in forensic chemistry, the sedatives are by far the most important* The most widely used present day sedatives are the barbiturates# With the advent of the barbiturates, the older hypnotics such as chloroform, chloral hydrate, paraldehydes and urethanes have only a limited use«'
A study of accidental and suicidal deaths occurring in Los Angeles County during the fiscal year 19£3-195>U reveals more then 2h% increase in deaths due to barbiturates since 19k9-19$0*
It is obvious that with barbiturates involved in so many medicolegal cases, accurate methods for th9 detection of these compounds in tissue, blood and urine should be developed*1
While some of the barbiturates are readily detected by the older methods, others defy detection due principally to the fact that they are metabolized in the body and methods for the detection of the metabolites have not yet been developed in all cases#4
This being the fact, the present investigation was undertaken to
-2-
iraprove old methods or to develop new ones for the detection of thevarious barbiturates*B. HISTORICAL
1* The BarbituratesMalonylurea, prepared by Conrad and Gutzeit in 1882, was
supposedly naned after a 'Miss Barbara".* Other theories as to thename are (1) that Baeyer called the compound barbituric acid becausehe considered it to be a "key" to a series of such compounds and (2)that the name was selected because the compound was prepared on
aSt* Barbara's Feast Day *Barbituric acid, which is a combination of urea and malonic acid,
forms the basic structure for this series of compounds*The two hydrogen atoms at position $ in barbituric acid are quite
reactive and may be replaced by various radicals (R and R*). The barbiturates may be named according to the substituent groups in position
5. _________ HYPNOPHORE GROUPHN - C = 0 H !HN -_C « 0 B?
^ \ / S ~ X /HO - C C HO - C C ’x ^ \ xN - C - 0 H - C = 0 i_ JRJ,Barbituric Acid Disubstituted Barbituric Acid
The first disubstituted barbituric acid derivative to be preparedwas the diethyl compound made by Snil Fischer and J* von Mering in1903 and later patented under the name "VERONAL"* The compound wasVERONAL from the Latin word "vera" because Fischer believed it to be
2 3the true hypnotic and introduced it as a hypnotic In 1903 • Thiscompound has been officially known as BARBITAL since 1926 *
Further investigations established the fact that substitution of
dissimilar hydrocarbon groups on the side chain produced compounds which had clinical advantages over BARBITAL*1
The next barbiturate to appear was phenylettyl barbituric acid, prepared by Horlein in 1911* This compound, also known as PHENOBARBITAL, was introduced therapeutically several years after BARBITAL Tinder the trade name of WLtMINALH but became official at the same time as barbitalin 19264**
HN - C - 0 C,HS / \ /HO - Cn N - C^* O f ij
PHENOBARBITAL6In 191o , the parent compound was modified by having one of the
radicals, an ethyl group and the other a methyl butyl group*1 This product known as PENTOBARBITAL or NMBUTAL was developed by the Abbott Laboratories*'
AMYTAL developed by the Eli Lilly Company in 1921 was shovm in 19306 vby Shonle, et al and Volwiler, et al to be an isomer of PENTOBARBITAL•'
These compounds had the same empirical formula but the methyl group inthe alkyl side chain of AMYTAL was linked to the/carbon atom whereas,the methyl group was attached to the a carbon in PENTOBARBITAL^
HN - C » 0 C2HB HN • C - 0 C2HB/ 2 s ^ \ / 36- HO ~ C'
X / \ (a) w \ / V«>, sN - C^" 0 CH2«CH2-CH"CH3 - C^- 0 ch-(c h2)CH2«CH2**CH"CH3 'N • C'« 0 ch-(c h2)2-ch3I tch3 ch3
AMYTAL PENTOBARBITALIn later years several other barbiturates were synthesized and
marketed for clinical use* Table I shows some of these compounds, their
trade names and structural formulae* Table II lists names and synonyms of barbituric acids.
Table III based on the dates when the patents were issued shows the approximate time of the commercial appearance of the individual barbiturates*
2* Barbiturate Poisoning*'Poisoning both suicidal and homocidal has undergone many stages from
Socrates and his hemlock through the Borgias with their arsenic in the Middle Ages to bichloride of mercury, phenol and cresols (lysol) of recent years* At present, the barbiturates far outnumber other preparations for the sinister purpose of suicide* The significance of this last statement is clearly shown in tables IV to VIII* Tables DC and X show the wide variation in therapeutic, toxic and fatal doses of barbiturates*1
It should be apparent from the data presented that there should be some regulation of the traffic in barbiturates*
In 192*>, Leake and Ware discussed 6l cases of BARBITAL poisoning which they observed in a Los Angeles Hospital* Nineteen (19) of the cases were of suicidal intent* At that time there was no restriction on the sales of the drug in California^ however, since 1931* the sale of barbituric acid derivatives has been forbidden in California except on a physician*s prescription*1
9Achard in 1929 reported his observations on the extensive use of barbituric acid derivatives and the great increase in cases of voluntary poisonings*
10Haubrich in 1934* advocated the restriction of the indiscriminate sale and use of the barbituric acid preparations because they were habit
forming^ He also recommended that preparations which were available onlyon a physician* s prescription not be issued more than once on theoriginal prescription#
IXIn 1939, Tatum discussed the barbiturate problem primarily from the pharmacologist* s point of view, listing substances which were synergistic with or potentiated the action of this group of drugs.
Table IFORMULAE OF BARBITURIC ACIDS
vCHg-CB«CH2R^ CHgf-CHgEthyl aUjrl barbituric acid
R,CH “CHbCH2CH -CH-CHa
Dial
,ch2-ch«ch2Rn CH (C%)2 Aprobarbital
^CH2-GH»CH2 .ch2-ch-ch2R Rn CH2-CH2-CH2-CH3 ^ ch2-ch (ch3)2Allyl^-butyl barbituric acid
Allyl barbital
ch2-ch»ch2R ‘S CH (CH3)2
Narconuraal
isomers
,CH2-GBr-CH2RNCH (ch3)2
Propallylonal
CH2-CBr“CH2R*^CH (CH3)2
Eunarcorx
R *• barbituric acid radical R*« N^nethyl barbituric acid
radical
^CH2-CBr-CH2S*R
X CH (CH3)2 Thionareon
ANALOGUES
_
N-methylN-methyl
Bromine Bromine
Siilfur Barbiturate
Derivative Derivative
Derivative Derivative
Table
I (Continued)
FORMULAE OF
BARBITURIC ACIDS
ANALOGUES___________________Bromine Sulfur
Barbiturate Derivative Derivative
mYtoP4
M
J O° /\ '
04M9M «
? ?K « p in« Y « 8
6 8 - e AN. /Oh
i
Ci
1ft)V0?O\ /Oh
a?Ya?*•33
Vg BO
(4
SISI
«st OrituYcrtfl\ /fri
t
j?VN M« w
V VWY«ixjo \ ✓I
■a
A
Surital
Kemithal
R/'CgHs' 0 *
Barbital
R*N>C2H6
Metharbital
R/ C2H5'ch-ch2-ch3tgh3
Butabarbital
Table I (Continued)FORMULAE OF BARBITURIC ACIDS
/GgHg /CgHs vCgHgR R R^ch2-ch2-ch2-ch3 n ch-ch2-ch2-ch3 ^ ch2-ch2-ch (ch3)2I
Butethalch3Pentobarbital
iscsners Lsome:
S-R S-RCH-CH2-CH3-CH3 ^ CH2-CH2-CH (ch3)2t
CH,Thiopental
isSSJThioethaayl
ers
wIH*d*%o
13.1I IH* H<3
S'S?
d £
R/CgHgC»CH-CH2-CH3 V CH,3Vinbarbital
.ch3
'OR.
Rutonal
R/CH2-CH2-CH3'ch2-ch2-ch3
Proponal -CH,
:0R»,
Hexobarbital
/ c2h5CH (CH3)2
ProbarbitalCjjHg
R* «
RCeHg
S-R'ch2-(ch2)4 ch3 n ch2-c - ch3
QHexethal ^C2H5
Phenobarbital OR«
ProminaL
ch3Methallatal
Cyclobarbital
ANALOGUES
MISCELLANEOUS COMPOUNDS
Table II________ NAMES AMD SYNONYMS OF THE BARB IT URIC ACIDS STUDIED____________ALLYLBARBITAL - allylbarbituric acid; sandoptal ALLYL-n-BUTYL BARBITURIC ACID - idobutalAMYTAL - amobarbital; amylobarbitone; 5-ethyl-5-isoaroyl barbituric acid APROBARBITAL - ^-allyl-^-isopropyl barbituric acid; alurate; isonal BARBITAL - barbitone; deba; diethyl barbituric acid; doraonal; hypogene;
malonalj xnedinalj sedeval; uronal; veronal; yesperal 5-(2-BRCMAXLIL) -5-(1-METHYLBUTYL) BARBITURIC ACID - p-bromallyl sec-amyl
barbituric acid; rectidon; sigmodal BUTABARBITAL - butabarbitone; butisol; 5-ethyl-5-methylpropyl barbituric
acid; 5-ethyl-5-secbutyl barbituric acid BUTALLYLONAL - p-bromallyl-secbutyl barbituric acid; 5-(2-bromallyl)-5-
secbutyl barbituric acid; pernoeton; pernoston BUTETHAL - 5-butyl-5-sthyl barbituric acid; etoval; neonal; saneiyl CYCLOBARBITAL - cyclobarbitone; ethyl cyclohexenyl barbituric acid;
namuron; palinum; phanodoni; phanodom; tetrahydrophenobarbital DIAL - diallyl barbituric acid; allobarbital; allobarbitone; allyl allyl
barbituric acid; curral; 5j5-diallyl barbituric acid ETHYL ALLYL BARBITURIC ACID - dcwminHEXETHAL - 5-ethyl-5-hexyl barbituric acid; hebaral; ortal HEXOBARBITAL - cyclonal; (cyclohexen-l-yl)-l,5-dimethyl barbituric acid;
dorico; evipal; evipan; hexanostab; methenexyl; N-methyl cyclohexenyl methyl barbituric acid
METHALLATAL - 5-ethyl-5-JJiethylallyl-2-thiobarbituric acid; mosidal PENTOBARBITAL - embutal; 5-9thyl-5-methylbutyl barbituric acid; nembutal;
pentobarbitone; pentone; pentyl; 8I4I1 PHENOBARBITAL - barbenyl; barbiphenyl; dorrairal; 5-ethyl-5-phenyl barbi
turic acid; euneiyl; gardenal; luminal; neurobarbital; nunol; phenobarbitone; phenonyl; phenylethylmalonylurea; somonal
PROBARBITAL - 5-ethyl-5-isopropyl barbituric acid; ipral PROMINAL - mebaral; mephobarbital; N-methylethyl phenyl barbituric acid;
phemitonePROPALLYLONAL -5-(2-bromallyl)-5-isopropyl barbituric acid; noctal;
nostalRUTONAL - 5-®ethyl-5-phenyl barbituric acidSECONAL — 5-allyl-5-methylbutyl barbituric acid; quinalbarbitone; seco-
barbitalTHIOPENTAL - 5-ethyl-5*<nethylbutyl thiobarbituric acid; itraval; neao-
donal; pentothal; thiopentone; thiothal VINBARBiCTAL - delvinal; 5-ethyl-5-methylbutenyl barbituric acid
Table HIBARBITURIC ACID PATENT DATA
Year Patent Number Compound
1903 German Ib6>k9& Barbital19121912
German 21*7,952 U. S. 1,025,872
PhenobarbitalPhenobarbital
1912 U. S. 1,01*2,265 Dial1916 German 293,163 Pentobarbital1918 U. S. 1,2#,951 Probarbital (2 Ca*3H20)1923 Uo S* 1,W*U,802 Aprobarbital1921* U. S. l,5li*,573 Amytal1926 U. S. 1,576,0114. Probarbital1926 U* S. 1,609,520 Butethal1927 u. s* 1,622,129 Propallylonal* u* s. l,62l*,51*6 Hexethal Sodium
1929 C. s. 1,739,662 Butallylonal# U. S. 1,91*7,91*1* Evipal (Hexobarbital)
1930 German 589,9k7 British 3U9,il55 French 38,680
CyclopalCyclopalCyclopal
1930 German 595,175 French 753,178
Evipal (Hexobarbital) Evipal (Hexobarbital)
193U U. S. 1,9514,1*29 Seconal Sodium* U. S. 2,090,591* Barbituric Acid
1939 U. S. 2,153,729 U* S. 2,153,731
Thiopehtal Sodium Thiopental Sodium
1939 U. S. 2,153,729 (?) Mosidal# According to the numerical order of the patents, the preparations should be placed in this position*
Table IVACCIDENTAL AND SUICIDAL DEATHS DDE TO BARBITURATES IN NEW YORK CITY*8
BARBITURATE 19hl 191*2 191*3 19hh 19h6 l?t*7 19i*8 19U9 1950 1951
XI•H.3
$■P
Jj•c•HOo«J
3.•ri•S8
+•pc$XI•HO -n
tg
CXI © •H Xl O *rl ri O
3 £•o <3•H T3 O *ri O
H(4
Xl•ri
3■P
■IO >H •ri o
rri(4Xf•ri
•ri8
3"g•§•Ho%
$3
* I•ri XJ O ’H •H O8 %
XJ•H•ri8
•p
IXI•HO
i—1(4
XI•ri
3IsXJ
O -H •H O8 3
AlLonal - - mm 1 mm - mb 2 - ae- - - •» «• -ALurate & Neonal m mm - mm - - • 1 m
Amytal 1 1 - 1 1* 1* 1* 1* 3 1* 6 2 3 1 1Amytal & Seconal 1* - - - •ft - - - - «*• - - 1 6 1Barbital •» mm - 1 1 2 mm 2 - 1 - - - 1 1Butisol - m mm- - - m- m- 1Ipral - - 1 m - mb - •*Nembutal (Pentobarbital) 3 mm 1 13 8 19 6 19 12 22 8 15 6 15 5Nembutal & Phenobarbital - - «• - - •» - 1Nembutal & Seconal - •a - - - - - 1Neonal - - 1 - m - - -
Neopental - - - - - - 1Phanodorn - m - •• •• - - -
Phenobarbital 1 1* 3 6 5 10 5 7 - 10 6 13 2 13 3Phenobarbital & Seconal - - - •• - - - - - - - - 1 1 —
Seconal - - - 5 13 9 8 9 1* 15 5 11 8 16 2Sodium Alurate - - - 1 «*• - - 1 - 1 - - - - 1Tuinsl «■ - - - - - - «•• •• - 1 1 1* 1Unknown 29 17 27 32 37 31 21 20 76 55 1*3 38 60 35 83 31* 76 63Total 38 22 31 32 37 31 50 1*2 119 78 O
0—•
J 58 113 60 127 56 136 79Total suicides & accidents/ year 60 i i _68___ 92_ 197 ll*5 173 183 215
+/-Nsi 3XI
•ri
8
*13•§•HO•§
186# figures for 191*5 not yet compiled; + Not broken down into types of barbiturates
Table V33DEATHS DUE TO BARBITURATES IN FRANKLIN COMFY, OHIO
BARBITURATE 19U8
Amytal 3Barbital 1Pentobarbital 1Pentothal -Phenobarbital £Seconal 1Unknown 1Total for year 12
19k9 1950 1951
2 3 1
2 11
23 8 122 3
J L X
37 20 16
1952 1553 195U(throughNovember)
lU •23 ** t»
21 2 25 - -Jt _= _aU? 2 ll
Table VI14ACCIDENTAL AND SUICIDAL DEATHS DUE TO BARBITURATES IN CUYAHOGA COUNTY, OHIO
SEX
MaleFemale
19li3 19k$ 19h6 19k7
*1
!aoa
•ri•ri
£
4"c■s•HO
h 8
*3•riO
3it
■3•p-ix>•HO*35
■3"d•rlO
3■§•riO
3ao•ri
U 2 8 2
•pI*U•rlO
It
H9z£
3 §i © 3 §3© _XJ *H O
a ^ si u l
22kL
•p S3<BXJ •ri O O *ri3 <g
0 S3
17 3 1
1950 1951 19523-P H S3 « © ■©XJ »ri
It 10 - 7 5 -
tQ2 5 5 U
3"£■§•ri©■§
Ha•S£
$S3•8•riO•§
2 2
3a a £
3 2- 2
Total U 8 6 7 2 8 6 12 U 9 11 £ U; 1 1U 8 1 7 9 2 2 3 ItTotal accidents, suicides & undetermined deaths for the year 12 15 Ut 16 20 20 23 16
H\jGI
INCIDENCE OF BARBITURATE POISONING AMISSIONS IN CLEVELAND, OHIO HOSPITALS 19U2 19U3 19UU 19U5 19U6 19lt7 19U8
14
19h9 1950 Total(# of totalpoisonings)
77 75 87 9k 129 161 136 123 112 99k 36ol
Table VII 1 5ACCIDENTAL AND SUICIDAL DEATHS DUE TO BARBITURATES, IN LOS ANGELES COUNTYa CALIFORNIA FOR FISCAL YEARS
BARBITURATE1910.- 191*2- 191*3-
19l|ii191*1*- 1915- 191*6-
191*6 191*7191*7- 19U8- 191*8 191*9
191*9-1950
1950- 1951-2 2 S L . 2 2 2 L .
1952- 19531951)
Allonal(Alurate)(Aprobarbital)
1 mm- mm- • * 1 1 1 2 1
Amytal(Amobarbital)
- 3 3 8 - 1 6 8 5 3 - 5 3
Barbital(Veronal)
1* mm 1 12 5 11* 1 1 1 - - - -
Barbiturate(Unclassified)
13 22 20 37 61* 78 66 70 1*9 88 103 123 Ill
Delvinal «• - 1 - - mm - - - - 1 - -Dial 1 mm
Ipral - - - - - mm mm 1 - 1 mm - -Luminal (Phenobarbital)
8 2 16 10 21* 23 31 27 16 20 10 11 17
Mebaral - mm - - mm «•> - 1 - 2 - -
Nembutal (Pentobarbital) 1* 5 6 19 8 20 15 1*1 39 1*0 26 25 ; 39
Secobarbital(Seconal)
m 9 1 10 12 18 19 26 28 19 16 19 13
Tuinal - - 1 1 2 2 _ 5 3 JLTOTAL 31 1*1 U8 96 113 151* 139 175 ll*2 171* 161* 188 189
-15-Table VIII Xe
SUICIDAL AMD ACCIDENTAL HEATHS DDE TO BARBITURATES IN U8 STATESSTATE 1??6 1221 I22i 1222 19itP !L2ki 1^2 19it3 19U£Alabama 3 10 it it 3 2 2 » it •ftArizona m 2 6 it It 3 3 1 3 «»Arkansas 2 1 1 l 2 3 2 2 1 mCalifornia 21 31 29 32 56 63 52 93 108 193Colorado •m 3 2 it 2 7 8 2 it -
Connecticut 6 9 9 10 9 8 8 6 10 •ftDelaware 1 -» - - - - •ft- •*- » —
Florida 8 10 13 10 12 lit 5 8 10 ■ftGeorgia 5 8 3 3 3 6 - it 2 9Idaho 2 it 2 l 3 1 l — 1 -
Illinois 33 63 56 51 70 70 2it 31 33 6oIndiana 11 18 12 16 27 17 12 9 lit -Iowa k 9 15 9 8 lit 5 5 8 9Kansas 3 h 3 9 11 3 3 3 1 9Kentucky 1 it 6 5 3 it it 2 3 6Louisiana it 1 it 9 2 it 5 1 2 •Maine h 3 1 it 3 5 it - 3 •Maryland it 1 1 1 5 3 5 7 7 9Massachusetts 22 20 20 22 2it 35 26 28 22 it2Michigan 11 lit 16 26 28 31 13 lit 11 -Minnesota 8 lit 11 9 9 12 12 13 lit 11Mississippi •* 3 -- — 9 12 lit 6 3 itMissouri 6 13 16 12 32 7 it 10 n mMontana 2 •• - 1 2 1 1 1 it m-Nebraska ft* 2 1 it 6 3 3 2 i -Nevada 3 - 1 2 1 •• 1 1 ■». —
New Hampshire 1 1 it 2 1 9 3 1 - -New Jersey 7 it 7 7 17 13 9 12 11 -New Mexico 1 3 1 2 3 it - 3 2 ■»New York 57 h9 62 58 6o 65 73 87 98 mNorth Carolina it 2 1 1 5 2 it it it -
North Dakota 1 - - — 3 1 2 •»<Ohio 28 21 16 32 55 71 it2 38 38 72Oklahoma 5 6 6 3 l 2 3 it 5Oregon 5 6 5 it 2 6 5 1 h 10Pennsylvania 12 15 10 15 18 20 18 21 18 -
Ehode Island 1 1 2 l 1 1 1 1 2South Carolina 3 3 3 3 1 2 - •ft 3 •
South Dakota - 1 •a- m- •» 1 1 -
Tennessee k 5 2 it 2 2 3 1 5 ■»
Texas 7 6 5 8 12 16 7 13 11 a*
Utah 2 6 5 3 1 1 1 — 3 m
Vermont m 1 2 - 3 1 3 - 1Virginia l ■a- - 2 2 3 1 it 7 it'Washington 16 17 10 5 8 9 7 12 n 15West Virginia 5 3 5 l 5 7 9 it 7Wisconsin 7 12 19 lit 15 17 13 9 6Wyoming - 1 ••- - - 2 - - 1 •
Table HDOSES OF BARBITURIC ACID DERIVATIVES IN GRAINS
NAME OF DRUG
Alphenal Alurate Alurate Elixir Amytal
Amytal Sodium Barbital
Butisol
THERAPEUTIC POSE* TCKIC DOSE* FATAL DOSE*_________Oral Intravenous Minimum Median Maximum Minimum Median Maximum
i.S-5171-217,18,19
, .17675
x 206 ounces_ 17,21-23 33 23 23 30 _,23 201.5-5 3 25 108 2U 25 io5
18 22 • 22 0.33-12 22.5-30 304*524 , 2 5 H
7.5-22.5^ 1*8 <?289027230
. 287.5-917.18-21,29 23 .2 3 23 20-23 20.23 . 235-io * * • 5 5o 5oo 30 * 90 360
24.29 31 22.24.26.30 207.5-15 * 1*27.5 75-300 1*9522 27l*5-i5o 552
, 270.5-1.5 11*9
Table IX (continued)DOSES OF BARBITURIC ACID DERIVATIVES IN GRAINS
NAME OF DRUG
Qyclopal
DelvinalDial
Evipal
Ipral
HosidalNeonal
NoctalOrtal
THERAPEUTIC DOSE* TOXIC DOSE* _______FATAL DOSE*___________Oral Intravenous Minimum Median Maximum Minimum Median Maximum.170.83-2.5
,212-1*
-1 7 ,2 10.5-5
.17,18,21,22 .22 220.5-5 *■ 9 30-37.5 above 37.5
.24 - , 21 24 24 32 ,20>7.5 1.5-H 30 72 36
.24 24 H1.5-5 7.5-15 t, ,21 ,17U-6 3-6
« .170.83-7.5o i*8 2-1*
,172.5
.17,21 270.83-1.5 * 230« ✓ 18 0.83-6.7_ .17 ,180.83-5. 17.18,213-6.7 ' *
Table IX (continued)1DSES OF BARBITURIC ACID DERIVATIVES IN GRAINS
NME OF 33RIX?
Pentobarbital
PentothalPernoston
Phanodom
Phenobarbital
THERAPEUTIC BOSE* TOXIC BOSE*_______________ FATAL POSE*_________Oral Intravenous Minimum Median Maximum Minimum Median Maximum
. 17*18,21,22,24 23 ,.23 23 23 260.5-3 12 Ui 15 15 30
24 , ^ 265-15 U8.7
, 20 k9. 27
2Ul17 17
0.83-1 .3 0 .83-1 .218,21
3 9.22 „ . 22
3-7 .5 7.5-1521 17 33 27 34
1.5-3 1 .5 -6 It50 276 30018,22 221.5-6 5 1817.18 . ,22 20.23
0 .2 -3 * 60-75 25-26 921,22,24 22,260.5-5 75-i5o
IHCOI
Table IX (continued)DOSES OF BARBITURIC ACID DERIVATIVES IN GRAINS
NAME OF DRUG_______THERAPEUTIC DOSE*____________ TOXIC DOSE*________________ FATAL DOSE*___________Oral Intravenous Minimum Median Maximum Minimum Median Maximum
Prominal 0*5-1021Rutonal 1-2.36 3?
1-15 12017.18.21Sandoptal 3-13 * *
. 17.21 ,38 23 25Seconal 1*5-3 28.5 15 3018 26
1.5-5 U8.7. 21Sigmodal 1*5-3
*The discrepancies in the various doses of barbituric acids illustrate that a definite quantity can not be
set as the toxic or fatal dose* A dose is considered toxic when sedation lasts longer than anticipated from39the quantity of drug administered* Wagner states that the therapeutic dose of the barbiturates can not be
definitely standardised and suggests starting with the dose ire commended by the manufacturer and varying the dosage, if necessary, to obtain the desired results*
Table XMIN3MUN QUANTITY OF BARBITURATE FOUND/lOO GRAMS OF TISSUE ERCM POISON CASES.
QUANTITY OF TISSUE ESTIMATEDANALYZED BARBITURATE FOUND QUANTITY FOUND FATAL DOSE*Grams Milligrams Grains100 Amytal 2.5 10
100 Dial 10,0 Uo
100 Evipal (Hexobarbital) 2.5 10
100 Luminal (Phenobarbital) 10.0 Uo
100 Nembutal (Pentobarbital) U.o 16100 Neonal (Butethal) U.o 16
100 Proponal 10 .0 Uo
100 Ortal (Hexethal) U.o 16
100 Seconal U.o 16100 Veronal (Barbital) 18.0 72
If the quantity of barbiturate isolated from 100 grams of tissue is multiplied by 21*0, the total amount of drug in the entire body of a 60 kilo person (exclusive of the gastrointestinal tract and urine) may be estimated40*
-21-3# Barbiturate Regulations.
41In 19U6, Robert A# Fischelis reviewed the status of the barbiturate regulation# A summary of his article follows:
As of October 1, 19 k$ , thirty-two states, Alaska, Puerto Rico and the District of Columbia had lews in force which either directly or indirectly controlled the distribution of barbiturates or of mixtures with other drugs#
The first law dealing solely with barbiturates was enacted by California in 1929#
Wide variations were found in the provisions of the laws regulating the refilling of prescriptions# Since no reference was made to the renewal of prescriptions in fifteen states, it was assumed that refills were permitted.*'
An analysis of the labeling requirements which must be observed by the pharmacist showed a marked lack of uniformity in these requirements#' This lack of uniformity was attributed to the difference of coverage by the various laws#
Illegal possession was made a violation in Arkansas, California, Georgia, Michigan, Minnesota, Mississippi, South Carolina and Puerto Rico#1 The conditions Tinder which possession was declared illegal were:
1# Possession other than as authorized by law2#* If not in the original container in which it was dispensed ty
the pharmacist or physician 3# Unless the label showed the name and address of the prescriber
and the name and address of the dispenserU# Unless furnished on the prescription of a physician, dentist,
chiropodist or veterinarian and
-22-5* Unless prescribed ty a practitioner possessing a valid U* S*
Narcotic license*Minnesota described a violation as a gross misdemeanor, while the
District of Columbia, Puerto Rico and twenty-two states designated theviolation as a misdemeanor* Violations in other states were not classified*
16Goldstein in bis review of the barbiturate situation drew the following conclusions in 191*7:
1*' Deaths caused by barbiturates were increasing especially inthose states with large urban population and in instances where 191*5 figures were available, a sharp increase was indicated in many states*
2*' The state laws as of October 1, 191*5 affecting the distribution of barbiturates appeared to have little effect on the increase in mortalities due to barbiturates*^
3* The ratio of barbiturate poisonings to the total number of cases admitted to the same hospitals for the periods of 1928-1937 and 191*0*191*5 showed an increase of 86$ in the frequency of occurrence of barbiturate poisonings in the 191*0-191*5 period*
1**‘ The ratio of barbiturate poisonings to all types of drug poisonings, with the exception of carbon monoxide and alcohol, showed a 193$ increase in the frequency of barbiturate poisonings in the 191*0-191*5 period over the 1928-1937 period for the same hospitals*
5*' A total of 1,01*9,785 cases were admitted as poisonings during the period from 1928-1937* One-seventh (l/7) of these cases was due to barbiturates*1 During the 191*0-191*5 period a total of 1,060,275 cases were admitted as poisonings* One-fifth (l/5)
-23-of these cases was due to barbiturates* In other words, the barbiturate poisonings increased from lk»3% to 20% from the 1928-193^ period to the 19UO-19U5 period for the same hospitals*
6, United States statistics indicated that fatal poisonings by all solid and liquid poisons were decreasing while the yearly fatal barbiturate poisonings were increasing*
This review showed that suicides from barbiturates were still increasing in 19U7 and as a result a corrective uniform state legislation was stressed*
In 19U7 an attempt was made by the Ohio State Pharmaceutical Association to secure the enactment of a barbiturate law; however, the bill failed to be enacted* Another attempt was made in the 19li9-1950 session of the legislature and with the cooperation of the Ohio State Medical Association, this bill was passed by the legislature and signed by the Governor on May 12, 19k9» The law which became effective in August, 19h9 was modelled after the Uniform Barbiturate Control as suggested by the American Pharmaceutical Association and is known as the Uniform Barbiturate Act of 19i+9«
The act essentially made refills illegal on all existing prescriptions filed prior to August 12, 19h9» Thereafter an original written prescription was required each time that any barbiturate or preparation of barbiturate was dispensed. Prescriptions and all invoices of receipts of barbiturates had to be kept on file for two years and to be available for inspection by authorities at any time0
- 211-
ISOLATION OF THE BARBITURATES
Methods for the detection of barbiturates usually involve preliminary treatment of the tissue with acid or base, with or without removal of the proteins, followed by extraction with an immiscible solvent**
A* (a) Chloroform was the solvent selected by several investiga-42tors* Koppanyi used chloroform to extract protein free
filtrates prepared from tissues digested by 5 percent KOH*'43Adrian! mentioned the extraction of tissues which had
been frozen, pulverized and acidulated* In the Stas-Otto procedure, the finely divided tissue acidified with tartaric acid is extracted several times with absolute alcohol which is then evaporated to diyness and the residue dissolved in acidulated water from which the barbiturates are extracted by chloroform*- The Haines* modification of the Dragendorf process is similar to the Stas-Otto procedure and differs principally in the longer time required because acidulated $0 percent alcohol followed by increasing concentrations of alcohol is used in place of the initial treatment with absolute alcohol*
(b) Several investigators used ether for extracting barbitur- 44ates* Valov digested his specimens with alkali before
preparing the protein free extracts for ether treatment**46Kozelka extracted a protein free filtrate prepared from
46an acid digestion mixture, Klingefuss and Reinert extracted urine with ether to remove Impurities, then obtained the barbiturates from the urine by further ether
extraction after acidulation.' Gould and Hine obtained barbiturates from serum by a continuous ether extraction
48without previous removal of proteins. Stainer reversed the order of procedure in separating barbiturates and salicylates occurring together in tablets. Both were dissolved in ether from which the salicylates were extracted by aqueous sodium bicarbonate solutions. A chloroform-
49ether mixture was used by Warren for extractingbarbiturates from a solution prepared from tabletsdissolved in aqueous sodium hydroxide and then acidifiedwith HCl.
so(c) Brundage used petroleum ether to extract barbituratesfrom mixtures of aqueous tissue extracts* activated charcoal and Planter of Parish Preliminary extraction with petroleum
51ether was used by Pucher to remove impurities from urinewhile further extraction of the urine with diethyl etherafter acidulation removed the barbiturate.
62B. (a) Stolman and Stewart absorbed the barbiturates on synthetic magnesium silicate from which they were eluted with methyl alcohol.
63(b) Franchini and Repetto absorbed the barbiturates on activated charcoal and then eluted them with alkali.1
(c) Successful paper chromatography of barbiturates in urine54has been reported by Algeri and McBay and Algeri and
65 56 50 57Walker while MohrschulK 9 Brundage and Raventos wereunable to obtain satisfactory results.
Purification of the barbiturates obtained in the above procedures is
frequently necessary and several methods have been attempted# Sach59and Hanson report the destruction of impurities by oxidation of the
crude extract with potassium dichromate and potassium permanganatejrespectively. Other investigators attempted to remove proteins from
60crude extracts* Fleury and Guinnebault used mercuric sulfate for this61 62 purposej Zwikker , copper-pyridine# Bachem removed colored impur
ities from the crude extracts by absorbing them on charcoal# Sublimation of the crude extract is a successful method of purification according
63 64 65to Shonle, et al , Herwick and (Settler •
QUALITATIVE TESTS FOR BARBITURATES
Many of the qualitative tests for the detection of barbiturates include colorimetric procedures# Both the murexide test and Millon's
43test serve this purpose although Stainer found that MEBARAL and EVTPALdid not give the Millon's test.
Colors produced by the reaction between a cobalt ion and an imidegroup of the barbituric acid molecule on the addition of alkali havebeen extensively used# A pinkish violet or blue color develops whenbarbiturates are treated with a solution of cobaltous chloride inabsolute methyl alcohol followed by barium methylate (Zwikker test)#The thiobarbiturates produce a green color with the cobalt reagent#
66Bodendorf used cobaltous nitrate in anhydrous ethyl alcohol followed by potassium hydroxide in absolute ethyl alcohol and got a blue color
67as did Kozelka and Tatum who used sodium ethylate in alcohol as the63base. Gettler employed cobaltous acetate in absolute methyl alcohol
with isopropylamine as the base to produce a violet color while Selwyn
-27-6dand Bark used a more concentrated solution of cobalt acetate and
dilute isopropylamine.Other color tests for the detection of some of the barbiturates
include Ekkert’s test in which the identification of DIAL, LUMINAL and PHANODOHN is based on the production of colors following treatment with formaldehyde and concentrated sulfuric acid. Application of heat to the mixture produces a fluorescent solution if DIAL is present; a red solution if LUMINAL is present and a reddish-brown solution if EHANODORN
70is present. Dehusses applied heat to a mixture of m-nitrobenzaldehyde and concentrated sulfuric acid and got a red color with barbiturates containing the cyelohexenyl radical. Ekkert also used a mixture of selenous acid and sulfuric acid with which he distinguished BARBITAL and PHENOBARBITAL by emerald green and wine colors, respectively.
71Rhodes produced an intense brown color when he heated the phenyl derivative of the barbiturates on a slide with dilute sulfuric acid alone.
The odor of ammonia produced when barbiturates are heated alone or with alkali has been used as the basis for an additional qualitative test. Rhodes71 identified VERONAL, NEONAL, RUTONAL, LUMINAL, DIAL and APROBARBITAL by crystal formations on a slide when the respective compounds were dissolved in ammonia and acidified with sulfuric acid.
The iron-calcium chloride-iodide reagent of Ludy-Tenger and a copper-calcium chloride-iodide reagent have also been used to produce crystalline compounds with some of the barbiturates. Colorless to black crystals result from the formation of a copper complex and brownto black crystals from the formation of an iron complex. Kaiser,
72et al used these reagents and took melting points of the complexes
-28-to identify EVIPAL, LUMINAL, NOSTAL, PHANODORN, PERNOSTON,and VERONAL*
59,73,74Other investigators identified the barbiturates by determining the melting point of a derivative that had been prepared
59 74(frequently the di-p-nitrobenzyl derivative ).48Stainer employed various precipitation reactions and the Parra,
test to identify the barbiturates*
QUANTITATIVE METHODS FOR THE DETERMINATION OF BARBITURATES*
Many of the color reactions used in testing qualitatively for barbiturates have not been satisfactorily adapted for the quantitative
59,75estimation of barbiturates * The oolors developed by the cobalt42reactions fade or are not constant* However, Koppanyi , using cobalt
acetate, anhydrous methyl alcohol and isopropylamine as the base,76developed a color which he measured colorimetrically* Krause and Riley
varied the reagent concentrations used by Koppanyi and also obtained a77color suitable for colorimetric determinations* Bacila and Alcaide ,
using a 5hO filter in an Evelyn photoelectric colorimeter, made a quantitative estimation of' .barbiturates following their reaction with cobalt nitrate, ammonia and glycerol all dissolved in 96% ethyl alcohol* Unfortunately, the cobalt reaction is not specific for barbiturates but may be produced by any of the following compounds which frequently occur as impurities* These interferring substances includes acetic acid, aldehydes, biuret, creatine, creatinine, guanidine, hippuric acid, phospholipids, oxamide, substituted acetamides, substituted acetylureas,
50theobromine, theophylline and uric acid* Brundage and Gruber found that PENTOBARBITAL and ORTAL yielded metabolic products which were
measured as barbiturates by the cobalt test even though these products had no pharmacological action.
Spectrophotometric measurements of ultraviolet regions have been employed by several investigators using barbiturates dissolved in
78 47,79,80,81,82 81,83 83,84acid 5 in alkali 3 in chloroform and in ether •82However, one group of investigators reported salicylates and sulfon
amides as interferring substances.49Warren weighed the extracted material and determined the melting
points.85 86Both Bartilucci and Discher and Mattocks and Voshall employed
titrations for estimating barbiturates. The former investigators titrated potentiome trie ally with 0.1 N NaOH in an aqueous solution of the barbiturate. The latter pair used a silver, silver-silver chloride electrode system for titrating with silver nitrate*
'30'
BMHNATIQBT OF TISSUES
In the examination of tissues one must bear in mind that the drug originally administered may be present unchanged or may be in the form of a metabolite or degradation product.
Therapeutic doses of some barbiturates are believed to be destroyed in the liver. Most canpounds not destroyed in the liver are excreted by the kidneys. The ultra short acting compounds are destroyed in the
87gut • For convenience the barbiturates are classified as short acting, long acting and intermediate depending upon the length of time of the sedation which they produce.
Short acting compounds: are inactivated chemically by the tissues,principally the liver.
Intermediate acting compounds: are partially destroyed in the bodyand the unchanged portion excreted by the kidneys.
Long acting compounds: are eliminated practically unchanged in theurine.
Table XI showing the degradation products found in tissues after the administration of some of the barbiturates and Table JfJT showing the percent recovery of unchanged barbiturate from urine specimens follow:
DEGRADATION PRODUCTS-31 -Table XI
-BEgflKTED EQiL-SfflB-JARSITBSATES-
Drug Administered
( S 8 ) ( M )
VCH3 - N - C » 0
/0 * c c
\ /H - N - C - 0.0PRCMINAL
Compound, Pound in Tissue
H - N - C/ \ /CsH5
G 0 - c
N /H - N - C » 0FHENOBARBITAL
o(88)(89)
CH3 - N - C » O/ \ ^CaHe
0 - C C\ / x c3h5
H - N - C - 0 METHARBITAL
H - N - C » 0 / \ JJaHs
0 ■ c c V / x c2h5H - N - C - 0 BARBITAL
(88)
CH3 - N - B - 0 H - N -/ V /CaHg /0 - c c 0 - c
\ / \CH3 - N - C - 0 H - N -
N-ETHILBARBITAL(?3)(oo)CH3 - N - C - 0
/ \ .CH(CH3)a0 - C C
\ / VCHaCH*CHaH - N - C - 0
3 - 0
S X CaH5
N,N»-DHMETHYLBARBITAL BARBITAL(89)
CaHs - N - C - 0 H - N - C - 0/ > ^CaHs / N ^CaHs0 » c c 0 » c cN / N CaH6 \ ✓ V C 2HB
H - N - C - 0 H - N - C “ 0
BARBITAL
H - N - C => 0/ \ CH(CH3)a
0 - C C\ / X CHaCH«CHa
H - N - C « 0NARCGNUMAL ALURATE
-32-Table XI (continued)
DEGRADATION PRODUCTS REPORTED FOR SCME BARBITURATESDrug Administered
(91)H - N - C - 0
/ \ . CH,0 = c c-
\ /CHa - N - C - 0
EVTPAL
(aa)(93)(94)H -fi-C «0 / \
0 » c c,
\ ✓'H - N - C - 0&
Compound Found in Tissue
H - N - C - 0/ ' ^ ch30 - c c%, \ /
H - N - C - 0O ' 0DEALKYLATED CYCLOHEXENQNE
METABOLITE
H - N « c - 0/0 — C\
H - N - C - 0
PHANODORM CYCLOHEXENONE METABOLITE
(96)H - N - C - 0
0 - c c\ / N CH (CH3) CHaCH2CH3
H - N - C « 0PENTOBARBITAL
(ae)
\ X C4H9H - N - C - 0
/0 - c c
\ / N CH2 CBr-CH2H - N - C - 0
FEENOSTCN (BUTALLYLONAL)(91)(97)(9S)
H - N - C - 0/ \ .CH (CH3)20 » C c'\ / n ch2 cb« o h2H - N - C - 0 2
H - N - C - 0 / \ ^C2H5
0 » c c\ / X CH CH2CHQHCH3
H - N - C - 0 ^CH3HYDROXY DERIVATIVE
H - N - C - 0 / \ ^C4H9
0 » C c\ / X CH2 CO ch3
H - N - C - 0ACETONYL DERIVATIVE
H — N - C - 0/ ^ ,CH (CH3)20 - C\ / V CHa CO CH3H - N - C - 0
NOSTAL (PROPALLYLONAL) ACETGNYL ISOPROPYL DERIVATIVE
-33-Table XI (continued)
______DEGRADATION PRODUCTS REPORTED FOR SCME BARBITURATES_______Drug Administered Compound Found in Tissue
(99)H - N - C - 0/ \ OjHa
HS - C C^ / V CH (CH3) CH2CH2CH3N - C = 0
H - N - C - 0/ \ ^ ch8ch3
HS - C C r */ N CH CH2CH2CH3W
N-C - O
THIOPENTAL CARBOXYLIC ACID DERIVATIVE
The carboxyl group is believed to be in one of these three positions*
Some of the barbituric acid derivatives are not degraded in the tissues* These compounds, of which BARBITAL is an example, are excreted unchanged*
Table XIIPERCENT RECOVER! OF UNCHANGED BARBITURATES
fSHR OF BRUIj ft01 TISSUE QUANTITY FOUNDRECOVERED AHIINISTRATION EXAMINED IN PERCENT REFERENCEAmytal intravenous urine 0 100
intravenous urine 1*0-50# in 21* hours 101Aprobarbital intravenous urine 7% 102
oral urine l*,5-2l*# in 3 days 103Barbital oral urine 8% in 12 hours id*
oral urine 50# in 13-35 hours 105oral urine ll*-2Q# in 2k hours 60, 101*, 106oral urine 66-7$% in 21* hours 105oral urine - 36-90$ in 1*8 hours 10l*, 105, 107oral urine 50-90% in l*-8 days 75, 103, 3d*, ,
107*131oral urine 90-95% in 5 days after 4-1
theobromine therapy 310ButallyIonal oral urine 5-17* 93Cyelobarbital oral urine 2.5-7% 93, 91*Dial oral urine 1*0-$<$> in 3-1* hours -165Hexobarbital urine 30-1*0# 88Pentobarbital intravenous urine 0 312
oral urine 0 113-115oral urine 60# in 21* hours 116
Fhenobarbital oral urine 35-75# in 19 hours 105oral urine 20# in 9-10 days 103
Prominal oral urine 0 89Rutonal oral urine 25# in 11* days 317Seconal oral urine 0 313
-3 $ -EXPERIMENTAL PROCEDURES
The validity of some of the existing qualitative and quantitative methods for the detection of barbiturates has been questioned by previous investigators© Extraction procedures for the isolation of barbiturates from the tissues give rise to two possible sources of error (a) destruction of some of the barbiturate through contact with the solvent (acids or alkalies) and (b) failure of the solvent to dissolve all of the barbiturate© This situation might arise if the barbiturate were incompletely soluble in the solvent or if it had been occluded by impurities (such as precipitated proteins) and thus was not exposed to the action of the solvent©
Extraction of the crude aqueous solution with immiscible solvents, particularly ether, might remove other substances which would be weighed along with the barbiturate. The use of dichramate or permanganate for the destruction of contaminating substances in the crude barbiturate extracts may also be questioned, since some of the barbiturates are unsaturated and may be oxidized by such treatment. Separation of the barbiturates by adsorption on solids (charcoal, Plaster of Paris) has bean criticized on the grounds that later removal of the barbiturates from the adsorbent may be incomplete©
The several satisfactory methods developed for the extraction and determination of barbiturates in pure aqueous solutions or medicaments such as tablets have not yet been satisfactorily extended to the determination of barbiturates in tissues for two possible reasons, (a) Macromethods used in the former instances are unsuited for the detection of the small quantity of drug present in the tissues; (b) No provision has
-36-been made for removing contaminants arising from the presence of tissue*
Many of the investigators who weighed residues and reported them as barbiturates failed to ascertain the purity of the substances by determining the melting points. No identification should be based on a color test alone since there are other substances besides the barbiturates (particularly proteins) which give the same color tests* However, because of the limited amounts of barbiturates isolated from tissues, it is seldom possible to prepare chemical derivatives as some investi-
45,59*71,74,118gators have proposed •In the present investigation we studied many of these points to
determine which of the previous methods might be safely employed for extracting barbiturates from tissues* The next step involved the purification of the barbiturates and the final problem was the identification of the material*
The stability of the various barbiturates in water, 20$ acetic acid and 5$ potassium hydroxide for 2b hour periods was first determined since these were the reagents most commonly used for extracting tissues*
(a) Determination of the effect of 5$ potassium hydroxide on barbiturates* Solutions of the 2b barbiturates under investigation were prepared
by dissolving respectively 25 mg. of each In 25 cc. portions of $%
potassium hydroxide. These solutions, each containing 1 mg* of barbiturate per cc, alkali stood for 2b hours at room temperature and then were transferred to separatory funnels and acidified with 10$ hydrochloric acid, an excess of 2 cc* acid being added to each* Four extractions with chloroform (15 cc. portions) were then made to remove the barbiturates from the acidified solutions. After evaporating the
-37-
chloroform from, the combined extracts for each solution, melting points of the recovered barbiturates were determined and compared with those of the starting materials* The percentage of each barbiturate recovered was estimated by weighing* These results are included in Table XIII*
Table XIIIMELTING POINTS OF BARBITURATES RECOVERED AFTER 2l+ HOUR TREATMENT WITH
5# POTASSIUM HYDROXIDEMelting Point Melting Point
Percent of Recovered of Original Pure Compound___________________ Recovery Material (°C) Barbiturate (°C)
Allylbarbital 62.8 136..5-137 138..5-139Allyl-n-butyl barbituric acid 1+6.7 •» 123..5-121+Amytal 50.2 m -11+8.5 1U8 -11+8,Aprobarbital l+o.o 135 -138 li+2Barbital 8.1+ 182 1865-( 2-Bromallyl)-5- (1-methyl
butyl barbituric acid ioi+.5 157..5 157Butabarbital 59.8 162 161+Butallylonal 63.6 131 -132 131 -132Butethal 21.5 117 -118 123 -121+Cyclobarbit al 33.3 158 -159 ll+9 -150Dial 56.0 charred 161+ -165Ethyl allyl barbituric acid 35.1 155 157Hexethal 56.6 111 -112 122 -123Hexobarbital 25.0 charred 139 -ll+OMethallatal 6.8 152 156 -157Pentobarbital 31. h 121 -122 121 -122Phenobarbital 17.6 170 -171 171 -172Probarbital 39.0 198 198Prominal 1+.8 179 - 172Propallylonal 31+.3 170 -171 178 -179Rutonal 8.6 * 215Seconal 1+5.5 65 81+ -85Thiopental 77.3 153 153
-151+Vinbarbital 63.8 152 152
#Material recovered was not crystalline
I
-38-(b) Determination of the effect of 20$ acetic acid on barbiturates*
Solutions of the 2I4. barbiturates under investigation were prepared by dissolving respectively 25 mg* of each in 25 cc* portions of 20$ acetic acid* These solutions, each containing 1 mg* of barbiturate per cc* acid stood for 2U hours at room temperature. The ten (10). compounds marked * in Table XIV were not completely soluble in 20$ acetic acid. The preparations were transferred to separatory funnels and 10 cc, of concentrated hydrochloric acid added to each* Four extractions with chloroform (15 cc* portions) were made to remove the barbiturates from the acidified solutions* After evaporating the chloroform from the combined extracts of each solution, melting points of the recovered barbiturates were determined and compared with those of the starting materials* The percentage of each barbiturate recovered was estimated by weighing. The results are included In Table XIV*
(c) Determination of the effect of water on salts of barbituric acids*
Solutions of salts of the 2k barbiturates under investigation were prepared by dissolving respectively 25 mg* of each in 25 cc* portions of distilled water* These solutions, each containing 1 mg* of barbiturate per cc. water stood for 2k hours at room temperature. Ten (10) cc* of each solution were used to determine the percent of salt present^ the remaining 15 cc* of each were transferred to separatory funnels and acidified with 10$ hydrochloric acid, an excess of 2 cc* acid being added* Four extractions with chloroform (15 cc. portions) were then made to remove the barbiturates from the acidified solutions* After evaporating the chloroform from the combined extracts for each solution,
Table XIVMELTING POIHTS OF BARBITURATES RECOVERED AFTER 2li HOUR TREATMENT WITH
ZQ$ ACETIC ACIDMelting Point Melting Point
Percent of Recovered of Original Pore Compound___________________ Recovery Material (°C) Barbiturate (°C)
Allylbarbital 73.5 138.5-139 138.5-139Allyl-n-butyl barbituric acid 55.7 125.5-126 123..5-12U.Amytal 87.0 . 1U8 -1U8.5 1U8 -1U8.Aprobarbital 70.2 1U2 1U2Barbital 72.lt 186 186*5- (2-Bromal3yl)-5-(1-methyl
butyl barbituric acid 100.0 155 -156 157Butabarbital 70.8 163 16UButallylonal ioU.i 128 -129 131 -132Butethal 75.6 123 -12U 123 -121+Cyclobarbital 7U-7 157 Ht9 -150*Dial 77.U 163 16U -16$Ethyl allyl barbituric acid 38.0 157 157■aHexethal 75.3 123 122 -123■ifHexobarbital 7U.5 1U2 -143 139 -1J4.0■HMethallatal 71.2 155 -156 156 -157Pentobarbital 80.6 121 -122 121 -122Phenob arbital 95.6 171 171 -172*Probarbital 7 8.5 198 198ttProminal 97.7 172 172*Pr op al lylonal 92.0 170 -171 178 -179Rutonal 95.1 215 215Seconal 86.2 65 Bb -85^Thiopental 86.7 153 153Winbarbital 102.3 152 152 -15U*These compounds were not completely soluble in 20$ acetic acid, therefore this method is not applicable for their isolation.
melting points of the recovered barbiturates were determined and compared with those of the free acids. The percent of salts present at the end of the 2it hour period and the melting points of the recovered barbituric acids together with those of pure barbituric acids are recorded in Table XV.
V
-Uo-
Table XVMELTING POINTS OF BARBITURATES RECOVERED FRCM THEIR SALTS AFTER 2h HOUR
TREATMENT WITH DISTILLED WATER
CompoundPercent Melting Point Melting Point Recovery of Extracted of Barbituric of Salt Acid (°C) Acid (°C)
Allylbarbital Sodium 55 136 -138.5 138.5-■139Allyl-n-butyl barbituric acid 85 121 -123 123.5--121;Amytal Sodium salt 100 llj.8 -11*9 11*8 -ll*8.,Aprobarbital Sodium 76 1U2 -H*3 1U2Barbital Sodium 97 185 1865-( 2-Bromallyl)-5-(l-methyl
157butyl barbituric acid salt 7k 152Butabarbital Sodium 100 153..5-151* l6 kButallylonal Sodium U5 12? -130 131 -132Butethal Sodium 35 119 -120 123 -121;Cyclobarbital Calcium 100 l5ii -155 H*9 -150Dial Sodium 70 163 l6i| -165Ethyl allyl barbituric acid salt 75 153 -15U 157Hexethal Sodium 100 m -119 122 -123Hexobarbital Sodium 100 lUo 139 -HiOMethallatal Sodium 81 155 -156 156 -157Pentobarbital Sodium 100 120 -121 121 -122Phenobarbital Sodium 100 165 -169 171 -172Probarbital Calcium 100 197 -198 198Prominal Sodium 100 173 -1 7 k 172Propallylonal Sodium U5 176 -179 178 -179Rutonal Sodium 73 211; -215 215Seconal Sodium 93 no crystals 81* -85Thiopental. Sodium 97 152 -153 153Vinbarbital Sodium 9k 152 -153 152 -151*
After determining the effect of $% potassium hydroxide, 20$ acetic acid and distilled water on barbiturates for 2k hour periods at room temperature, the same concentrations of acid and alkali and also distilled water were employed to extract tissues known to contain definite quantities of barbiturates*
-1*1-LIVER TISSUE EXPERIMENTS
(a) Digestion of barbiturate-llver mixtures with 5% potassium hydroxide.
Mixtures containing 15 grams of liver and 30 milligrams respectively of each of the barbiturates prepared by using the Waring Blendor were allowed to remain at room temperature for 1* hours to permit absorption of the barbiturates by the tissue. At the end of this period, 30 cc. aliquots prepared by adding 5$ potassium hydroxide to the liver specimens containing the various barbiturates were kept at room temperature for 21* hours. The protein material was then precipitated with £$ copper sulfate and filtered. The protein free filtrates, placed in separatory funnels, were acidified with 10$ hydrochloric acid and each solution extracted with chloroform. Four chloroform extracts obtained from each specimen were combined and evaporated on a steam bath. The residues obtained after evaporation of the chloroform extracts, were dried at 100°C for 1 hour, cooled, weighed and the melting points determined.These results as well as the melting points of the original compounds are shown in Table XVI.
(b) Digestion of barbiturate-liver mixtures with 20$ acetic acid.
Mixtures of liver and barbiturates were prepared the same as in (a) above. At the end of the 1* hour period, 30 cc. aliquots prepared by adding 20$ acetic acid to the liver specimens containing the various barbiturates were kept at room temperature for 21+ hours. The protein material was precipitated with 10$ sodium tungstate. The protein free filtrates, placed in separatory funnels, were acidified with 10% hydro-
-1*2- Table XVI
MELTING POIHTS OF BARBITURATES RSCQ7ERED FRQM BARBITPRATE-LIVER MIXTURES AFTER 21* HOUR TREATMENT WITH 5% POTASSIIM HYDROXIDE.
Compound Percent Melting Point Melting PointMixed with Recovery of Recovered of Original PureLiver_____________________ of Acid Material (°C) Barbiturate (°C)
Allylbarbital 60*3 136 -137 138.>5-139Allyl-n-butyl barbituric acid 1*1*. 0 no crystals 123.5-121*Amytal ^0.0 ll*8 *11*9 1U8 -11*8,Aprobarbital 37.3 135 -138 11*2Barbital 8.0 181 1865- ( 2-Bromallyl) -5-(1-methyl
157 157butyl barbituric acid 102.0Butabarbital 57.3 162 -163 161*Butallylonal 60,3 130 -131 131 -132Butethal 21.0 119 -120 123 -121*Cyclobarbital 30.0 158 -160 11*9 -i5oDial 52.0 charred 161* -165Ethyl al3yl barbituric acid 33.6 155.5-156.5 157Hexethal 52.3 110 -112 122 -123Hexobarbital 25.0 charred 139 -11*0Methallatal 5.0 152 156 -157Pentobarbital 30.3 120 -121 121 -122Phenobarbital 15.3 170 -171 171 -172Probarbital 32.0 192 -19U.5 198Prcminal 2.2 178 -180 172Propallylonal 30.3 171 -172 178 -179Rutonal 5.3 no crystals 215Seconal 1*0.3 65 - 66 81* - 85Thiopental 73.0 152 -153.5 153Vinbarbital 6l.o 152 -153 152 -151*
chloric acid and extracted with chloroform* After combining and evaporating the extracts on a steam bath, the residues were dried at 100°C for 1 hour, cooled and weighed* The melting points of these residues were compared with those of the original compounds and are included in Table XVII.
-U3- Table XVII
MELTING POINTS OF BARBITURATES RECOVERED FROM BARBITURATE-LIVER MIXTURESAFTER 2k HOUR TREATMENT -WITH 20# ACETIC ACID*
Compound Percent Melting Point Melting PointMixed with Recovery of Recovered of Original PureLiver of Acid Material (°C) Barbiturate (°C)
Allylbarbit al 7U.3 138.5-139 138.5-139Allyl-n-butyl barbituric acid 55.6 125.5-126 123.5-12UAmytal 88.3 114-7 -1U8 1U8 -1U8.5Aprobarbital 70.6 1U1.5-1H2 1U2Barbital 72.3 185 -186 186#5-( 2-Bromallyl)-5-( 1-methyl
155 -156butyl barbituric acid 1.0 157BufcEbarbital 72.0 163 -163.5 16UButallylonal 100.3 128 -129 131 -132Butethal 75.6 122 -12U.5 123 -12UCyclobarbital 7U.6 156 -157 1U9 -150*0131 32.6 163.5 16U -165Ethyl allyl barbituric acid 36.0 159 157aHexethal 51.0 123 -12h 122 -123■aHexobarbital U7.3 ll;3 -lUU 139 -lUoaMethallatal I4I.0 155 -156 156 -157Pentobarbital 80.1 121 -122 121 -122Phenobarbital 91.6 170 -171 171 -172■aprobarbital 70.0 198 198a-Prominal 2.0 170.5-172 172#Propallylon al 8.0 170 -172 178 -179Rutonal 90.6 21U -216 215Seconal 83.0 66 8U - 85a-Thiopental 12.0 153 -153.5 153Winbarbital 12.6 151 -152 152 -15U
Crystals of barbiturates were visible in the ground liver after removal of the extract, therefore, this method of extraction can not be used for the quantitative isolation of these compounds*
Since the salts of the barbiturates and in most cases not the free acids are water soluble, we used barbiturate salts in determining the effect of water on these compounds* However, we employed the free acids in our investigations of the effects of acid and base because these are forms in which most of the barbiturates are available to the public*
- k k -
In the experiment which follows immediately, the effects of wateron mixtures of tissue and barbiturates were studied* Here the salts
119were produced by adding sodium hydroxide till a pH of 10 , that ofaqueous solutions of most of the barbiturates, was reached*
(c) The extraction of barbiturate-liver mixtures at pH 10*
Twenty-four mixtures containing 1$ grams of ground liver and 30 milligrams of the respective barbiturates were prepared and allowed to stand at room temperature for k hours to permit absorption of the barbiturates by the tissue* Thirty (30) cc, of distilled water were then added to each mixture and the pH adjusted to 10 with sodium hydroxide* After standing for 2k hours at room temperature, the mixtures were filtered and the filtrates treated with $% copper sulfate to remove the protein material which was then filtered. The protein free filtrates were extracted twice with chloroform to remove some of the impurities, then acidified with 10% hydrochloric acid and extracted with U successive 1$ cc* portions of chloroform to obtain the barbiturates* Evaporation of the chloroform extracts from each specimen left residues in each case* Since some of the residues appeared amorphous, all of the residues were dissolved in 10 cc. of 0,1 N NaOH. The resulting solutions were filtered to remove impurities, acidified with 10% hydrochloric acid, and re-extracted with U successive V~> cc. portions of chloroform. The purified residues remaining after evaporation of the chloroform were dried at 100°G for 1 hour, cooled, weighed and the melting points determined* (With the exception of SECONAL, all of the purified barbiturates were crystalline. These values comprise Table XVIII)•
-It5-Table XVIII
MELTING POINTS OF BARBITURATES RECOVERED FRCM BARBITtlRATE-LIVER MIXTURESAFTER 2k HOUR TREATMENT AT pH 351
Compound Rercent Melting Point Melting PointMixed with Recovery of Recovered of Original PureLiver______________________of Acid______ Acid (°C)_Barbiturate (°C)Ally lb arbit al £.2 138 -139 138.,5-139Allyl-n-butyl barbituric acid 78.3 122 -123 123.-5-12UAmytal 83.3 1U7 -1U9 1U8 -lit8,Aprobarbital 77.0 lit2 -Ht3 lit 2Barbital 93.1 185 -186 1865-(2-Bromallyl)-5-(1-methyl
butyl barbituric acid 78.0 152 157Butabarbital 82.lt 152 -l51t l6itButallylonal U8.3 128 -129 131 -132Butethal 39.2 119 -120 123 -1 2 kCyclobarbital 86.1 153 -155 lit9 -150Dial 79.9 163 16U -165Ethyl allyl barbituric acid 77.2 153 -15U.5 157Hexethal 92.3 118 -120 122 -123Hexobarbital 93.7 139 -litO 139 -ll+OMethallatal 78.2 155 -156 156 -157Pentobarbital 91.3 120 -120.5 1ZL -122Phenobarbital 93.it 166 -169 171 -172Probarbital 90.6 196 -197 198Prominal 92.3 171 -173 172Propallylonal it6.1 176 -179 178 -179Ru tonal 70.2 213 -211; 215Seconal 90.1 liquid 8U - 85Thiopental 93.0 152 -153 153Viribarbital 90.2 151 -153 152 -15&
It has been noted earlier that color reactions of the barbiturates are not well defined and that melting points as well should be determined to establish the identity of the barbiturates# However, an inspection of Table XIX will show that the melting points of some of the barbiturates are so close together that the identity of the compounds may be difficult to establish by the melting point alone# For this
-US- Table XIX
MELTING POINTS OF BARBITURIC ACIDSMelting Point (*G) Name of Barbituric Acid
8H - 85 Seconal121 -122 Pentobarbital122 -123 Hexethal123 -12U Butethal123.S-12U Allyl-n-butyl barbituric acid131 -132 Butallylonal138.5-139 Allylbarbital139 -lUO Hexobarbital1U2 Aprobarbital1U8 -1U8.5 Anytal1U9 -150 Cyclobarbit al352 -15U Viribarbital153 Thiopental156 -157 Methallatal157 Ethyl allyl barbituric acid157 5-(2-Brom allyl)-5-(1-methyl
butyl barbituric acid16U Butabarbital16U -165 Dial171 -172 Phenobarbital172 Praminal178 -179 Propallylonal186 Barbital198 Probarbital215 Rutonal
reason, it was decided to see if other physical properties of the barbiturates could be used to identify them and the refractive indices were next investigated.
Determination'of the refractive indices of the 2k barbiturates under inve s tigation, ' 1 —
These determinations were made by using a Fisher Refractometer witha melting point heating head, A few crystals of a barbituric acid were placed- on the glass portion of the heating head and covered with a «m»n
glass prism* The temperature, controlled by means of a rheostat, was allowed to rise slowly until the compound had melted and the refractive index could be measured. It happened that the refractive index could not be measured at the melting point of the barbiturate, therefore, the temperature at which a definite reading could be observed on the optical scale of the refractometer was recorded. The refractive indices together with the temperatures at which the readings were taken are shown in the following Tables XX (a) through (c)*
Table & (a)REFRACTIVE INDICES OF BARBITURATES DETERMINED BI THE FISHER REFRACTCMBTBR
Refractive Temperature Melting PointIndex of at which of thethe Melted Refractive Original PureBarbituric Index was Barbituric
Compound Acid taken (°C) Acid (°C)Allylbarbital 1.1+75Allyl-n-butyl barbituric acid 1.1+80Amytal 1*1+55Aprobarbital 1.1+81+Barbital 1.5l65-( 2-Bromallyl)-5-(l-methyl
butyl barbituric acid 1.1+98Butab arbital 1.510Butallylonal 1.500Butethal 1*1+70Cyclobarbital 1.506Dial 1.500Ethyl allyl barbituric acid 1.1+81+Hexethal 1.516Hexob arbital 1. 1+50Methallatal 1.531+Pentobarbital 1.1+78Phenobarbital 1.530Probarbital 1*1+53Prominal 1.5o5Propallylonal 1.500Rutonal 1.520Seconal 1*1+93Thiopental 1.5o8Viribarbital__________ 1.520
11+3 138.5-139130 123.5-121+168-169 li+8 -21+8150 li+2202 186178 157167 161+135 131 -132128-129 123 -121+175 11+9 -150176 161+ -165161+ 157127 122 -12311+5 139 -H+o176 156 -157135 121 -122188 171 -172213 198193 172191+ 178 -17921+5 21595 81+ - 85171 153M ..... ... . -i5?_ -iLa,
-US-
Table XX (a) is arranged alphabetically according to the barbiturates investigated. The same material has been reassembled to produce Tables XX (b) and XX (c) by arranging respectively according to the increasing values for refractive indices and for temperatures at which the refractive indices were determined. These tables may be employed in the identification of unknown barbiturates when only small quantities of the compounds are’ available. The melting point can be determined while preparing to measure the refractive index of the same material.
Table XX (b)REFRACTIVE INDICES OF BARBITURATES DETERMINED BT THE FISHER REFRACTCMETERRefractive Index of the Melted Barbituric Acid
i.U5o±•1631.U551.U701.U751.U781.U801.U8U1*U8U1.U93I.U981.5001.5001.5001.5051.506 1.508 1.5101.5161.5161.5201.5201.5301.53U
Temperature at which Refractive Index was taken(°C)
iU5213168-169 128-1291U3 135 130 150 16U 55 17813517619U193175 171 167 127 202 165 216 188176
BarbituriclAcid
HexobarbitalProbarbitalJimytalButethalAllylbarbitalPentobarbitalAllyl-n-butyl barbituric acid AprobarbitalEthyl allyl barbituric acid Seconal5- (2-Bromallyl) -5- (1-methyl
butyl barbituric acid Butallylonal DialPropallylonalProminalCyclobarbitalThiopentalButabarbitalHexethalBarbitalViribarbitalRutonalPhenobarbitalMethallatal
-1+9** Table XX (c)
TEMISRATtKES AT WHICH REFRACTIVE IM33CES WERE 1MEMNED (FISHER REFRACTOMETER)Temperature at
which Refractive Index was taken (°C)
Refractive Index of the Melted Barbituric Acid Barbituric Acid
95 1*1+93 Seconal127 I.$l6 Hexethal128-129 1.1+70 Butethal130 1.1+80 Allyl-n-butyl barbituric acid135 l.i+78 Pentobarbital3-35 l.$00 ButallylonalH+3 1.1+75 Allylbarbituric acidU+5 1.1+50 HexobarbitalISO 1.1+81+ Aprobarbital161+ 1.1+81+ Ethyl allyl barbituric acid16$ l.$20 Viribarbital167 l.$10 Butabarbital168-169 1.1+55 Amytal171 1.508 Thiopental175 1.506 Qyclobarbital176 1.500 Dial176 1.53U Methallatal178 1.1+98 $- ( 2-Bromallyl)-$- (1-methyl
butyl barbituric acid188 1.530 Phenobarbital193 i.$o5 Prominal191+ 1.500 Propallylonal202 1.516 Barbital213 1.1+53 Probarbital21+$ 1.520 Ru tonalRecently it was found that the presence of sodium cyanide effected
a barbiturate determination • In our medicolegal work we have noticed that the presence of cyanide interfered with the identification of some of the barbiturates* Therefore, we decided.to investigate farther.the effect of the presence of cyanide in the detection of barbiturates.
-5o-
Tbese experiments were set up to cover a period of three days since ordinarily at least three days elapse between the time the poison is ingested by the victim and the analysis is completed by the chemist*This three day interval allows time for the finding of the deceased by the police or other persons^ the post mortem examination and the actual chemical analysis*
The estimation of barbiturates in the presence of cyanide*
Twenty-five (25) cc. of solution of each of the 2i+ barbiturates (containing one milligram of a barbiturate and one milligram of sodium cyanide per cc* of distilled water) were prepared. These solutions were allowed to stand in the hood for three days at room temperature, and at the end of this time, and still in the hood were acidified with 10# hydrochloric acid, an excess of 2 cc. of hydrochloric acid being added in each case. In the case of pure barbiturates, this treatment frees the barbituric acid, crystals of which are usually preceptible with the naked eye* In six (6) of the barbiturate-cyanide mixtures only, could crystals be seen with the naked eye after the addition of hydrochloric acid. The acidulated solutions were then extracted with U successive 15 cc. portions of chloroform* The residues obtained after the evaporation of the combined chloroform extracts were dried at 100°C for 1 hour, cooled, weighed and the melting points were then determined* These results are given in Table XXI*
Table XXIMELTING POINTS OF MATERIALS RECOVERED FRCM BARBITURATE-CTAMIDE MIXTURES
Precipitate Visible after
Barbiturate HC1 AdditionMelting Point of Recovered Campound(°C)
Melting Point of Original Pure Barbiturate (°C)
Ally lb arbital 128-132 138.5-139Allyl-n-butyl barbituric -
acid . _ . 12U-12S 123.5-121*Amytal — ll*8 11*8 -11*8.5Aprdbarbital — ll*0-ll*l 11*2Barbital 182 1865-(2-Bromallyl) -5- (1-methyl
butyl barbituric acid + 157 157Butabarbital — 161* 161*Butallylonal — 132-133 131 -132Butethal — 121-122 123 -HSUCyclob arbital — 152-153 01§
Dial — 165-166 161* -165Ethyl allyl barbituric acid •m M 155 157Hexethal + 121-122 122 -123Hexobarbital — 137-138 139 -11*0Methallatal + 155-156 156 -157Pentobarbital + 120-121 121 -122Phenobarbital — 166-167 171 -172Probarbital - - 19U 198Prcminal + 171+ 172Propallylonal — n h 178 -179Rutonal •M m 215 215Seconal ----- 131-132 81* -85Thiopental + 155 153Vinbarbital 157 152 -151*
Our final investigations were made to determine the stability of the solid barbiturates to air and atmospheric moisture in the presenceof light and heat, since there appears to be some uncertainty on this point •
-52-
Determination of the stability of solid barbiturates*
The barbituric acids were exposed to the atmosphere at room temperature for 60 days* At the end of this time* the melting points of these barbituric acids were compared with those of the original pure barbituric acids* These results are given in Table XXII*
Table XXIIMELTING POINTS OF BARBITURIC ACIDS PRIOR AND AFTER EXPOSURE TO AMCSPHERIC
CONDITIONS AT RQCM TEMPERATUREMelting Point (°C) of Melting Point (°C)Barbituric Acid after of Original Pure
Barbituric Acid__________ 60 Day Exposure______ Barbituric AcidAllylbarbital 138,.5-139 138,.5-139Allyl-n-butyl barbituric acid 119 123..5-12UAmytal lii-7 —124.8 1U8 - mAprob arbital 139 -1U0 1U2Barbital 186 -187 1865-(2-Bromallyl)-5-(1-methyl
butyl barbituric acid -156 157Butabarbital 16 3 I6I4.Butallylonal 129 -130 131 -132Butethal 122 -123 123 -1 2 kCyclobarbital 151 -i£2 Hi9 -150Dial 16k -166 16k -165Ethyl allyl barbituric acid 160..5 157Hexethal 120 -121 122 -123Hexobarbital liiO —li|2 139 -litOMethallatal 155 -156 156 -157Pentobarbital 113 -119 121 -122Iftenobarbital 171 -173 171 -172Probarbital 199 -200 198Prominal 17U -175 172Propallylonal 178 -179 178 -179Rutonal 215 -216 215Seconal 83 - 8U 8U - 85Thiopental 152 153Vinbarbital 157
CO9
..... & -151*Several salts of the barbituric acids left exposed for the same
period of time were examined visually and all appeared unchanged with the exception of HEXOBAHBITAL SODIUM.
-53-DISCUSSION
The percent recovexy of barbiturates subjected to treatment with potassium hydroxide and recovered by extraction of the acidified salts with chloroform ranged from lu8 to I0lu5 as shown in Table XIII.: BAB** BITAL And RUTONAL, two of the long acting barbiturates, were among thecompounds which apparently decomposed during the alkali extraction process* The percent recovery of BARBITAL was 8*b while that of RUTONAL was 8*6* two other compounds which seemed to have been effected by the action of the alkali were METHALLATAL with 6*8 percent recovery and FROM INAL with a U*8 percent recovery* Three of these four compounds, BARBITAL, FROM INAL and METHALLATAL have ethyl groups as one of the side chains* There is no other similarity in the Structure of these compounds, therefore, it seems unlikely that the results are due to a particular structure*
Seventy-five percent of the acids recovered after the alkali treatment had melting points different from the original barbituric acids* With the exception of CYCLOBAR BITAL, DIAL, HEXOBARBITAL and PROW INAL, the melting points of the acids in this seventy-five percent were the same or lower than those of the corresponding original compounds* The melting points of six of the barbiturates (AMYTAL, 5-(2-BRCMALLSL)-5-(1-METHYLBUTYL) BARBITURIC-ACID, BUTALLYLONAL, PENTOBARBITAL, PROBARBITAL and THIOPENTAL) were unchanged by treatment with alkali* There is no correlation between the structure of the compounds the melting points of which were unchanged and the percent recovexy of these six compounds*'
Two compounds, ALLIL-n-BUTXL BARBITURIC ACID AND RUTONAL, after treatment with 5% potassium hydroxide and recovexy of the material from an acidified solution, yielded products which had no crystalline structures.'1 Here again, there seemed to be no correlation between the structure of the compound, the percent recovery of these two acids or
-A-thelr melting points*
The 10U.5 percent recovexy of 5>- (2-BRCMAlLXL)-£- (1-METHHBDTIL) BARBITURIC ACID may have been due to partial oxidationy the behavior did not correspond to that of the other bromallyl derivatives, BUTALLIL- CNAL and FRGPALLILONAL, when treated in ths same fashion*
It has now been established that all of the 2k barbiturates studied may be recovered in varying quantities after treatment with potassium hydroxide* Occasionally the recovered barbituric acid may not be in crystalline form*
The recovexy of barbituric acids after treatment with 20% acetic acid was better than after treatment with alkali* Table XIV shows that the percent recovexy ranged from 38*0 to 10U*l* Compounds marked (*) in Table XIV were visibly insoluble or only partially soluble in 2056 acetic acid*1 The recovery of such compounds ranged from 71*256 for METHALLATAL to 102.356 for VINBARBITAL*
It would seem that even if a barbiturate were insoluble in 2056 acetic acid, a chlorofonn extraction <f the mixture of insoluble barbiturate in acid might afford a recovery of 100 percent. This however, was not the case. Of the ten (10) barbiturates which were insoluble or not completely soluble in 2056 acetic acid, only two (2) of ihe derivatives,5-(2-BR(MALLTL)-5»(l«MEmrLBUTrL) BARBITURIC ACID and VINBARBHAL were completely recovered*" On the other hand, BUTABARBITAL, which was completely soluble in 2056 acetic acid, was among the compounds which yielded a high percent recovery (10U56). In this case, the k% increase in weight was probably due to some degree of oxidation**
It appears, therefore, that no correlation can be made between the
solubility of the barbituric acids in 20$ acetic acid and the extent to which they are recovered ty extraction with chloroform*!
All of the materials recovered after the 2h hour treatment of the barbiturates with 20% acetic acid had melting points which were somewhere within the range of those of the original barbituric acid, with three exceptions, CYCLOBARBITA1, FROPALLYLONAL and SECONAL, CXCLOBARBITAL had a melting point higher than the original acid while FROPALLYLONAL and SECONAL, had a melting points lower than the original barbituric acids*
It has now been established that all of the 2b barbituric acids studied can be recovered to some extent following 2h hour treatment with 20% acetic acid*
The behavior of the various barbituric acid salts allowed to stand for 2h hours in distilled water is shown in Table XV* At the end of the 2k hour period, 100$ of nine of the barbituric acid salts studied was re* covered*' The recovery of other barbiturates ranged from 35$ for BUTETHAL SQDUM to 97$ for BARBITAL SODIUM • There appeared to be no correlation between the percent recovery of the barbituric acid and its structure*1 In no case was the percent recovexy over 100$* SECONAL was the only barbituric acid which could not be recovered in crystalline form after treatment with distilled water for 2k hours at room temperature*'
These results indicate that salts of barbiturates are stable in water for at least 2b hours moreover, when thB acids are freed from the salts and extracted with chlorofoim, crystalline residues may be obtained after evaporation of the chloroform except in the case of SECONAL*)
SECONAL, CXCLOBARBITAL and BUTABARBITAL were three compounds which possessed melting points which did not compare favorably with the
original compounds (Table XV)* SECONAL crystals could not be obtained; BUTABARBITURIC ACID had a lew melting point while the melting point of CYCLOBARBITORIC ACID was too high*
It may then be concluded th^t aqueous solutions of the salts of barbituric acids are more stable over a 2k hour period than barbituric acids in $% potassium hydroxide or 20% acetic acid*
The quantity of barbiturates recovered from the tissue by a 2k hourextraction with $% potassium hydroxide ranged from 2,2% far FRCMINA1 to 1G2*0/6 far 5-(2-BR<HAim,)«$-(l-}!ETHS£LBDm) BARBITURIC ACID (Table XV ). Da one or two cases, the results were almost similar to those obtained when the pure compounds were treated with 5>j6 potassium hydroxide, but in the majority of cases the results were slightly less*
The quantity of barbiturates recovered from the tissue by a 2k hour extraction with 2056 acetic acid ranged from 1*056 for 5-(2*»BRCMALLYL)-5^1 -METHYLBUTTL) BARBITURIC ACID to 100.3/6 for BUTALLYLONAL (Table XVII). Barbiturates extracted from tissues by this method had a wider melting point range in some cases than the barbiturates treated in a similar manner in the absence of tissue (Table XIV)* With the exception of ETHIL ALLYL BARBITURIC ACID, the barbiturates which were not recovered in appreciable quantities were the compounds which were not completely soluble or were insoluble in 2056 acetic acid. Da some instances the extracted tissues still, contained visible crystalline material. Da all probability, the presence of these crystals in the extracted liver after extraction would account for the apparent loss of the barbiturate.'
Since the pH of aqueous solutions of salts of the barbiturates isXX9believed to be between 9 and 10 , we carried out the extraction of the
barbiturates from tissues at this pH* The recovexy under these conditions (39*2-93.7/6) compared favorably with that obtained when pure salts were
allowed to stand in water, acidified and extracted with chloroform (35-lOOjC). The poorest recovexy (39.2J6) was greater than either with the acid or the alkali treatment*1 There was no apparent correlation between the percent recovery and the structure of the compound*1 With the exception of BUTABAEBITAL and SECONAL, the melting points of the compounds recovered after this treatment compared favorably with that of the pure barbituric acids* SECONAL* as usual, was a viscous liquid*1 The melting point of BUTAEARBITAL was about 10 degrees too low*1
Table XIX shows that PENTOBARBITAL (nwp* 121-122*C); HEXETHAL (m.p. 122-123°C)j BUTETHAL (nup. 123-12i*°C) and ALUL-n-BUTIL BARBITURIC ACID (m.p. 123.5-12R°C) melt within a very narrow range, however, it may be seen in Table XX (a) that the refractive indices of these four compounds are far enough apart so that these four barbiturates may easily be identified;
PENTOBARBITAL m.p. 121 -122*C R*I* UHftxsBHEXETHAL m.p. 122 -123°C R.I. l.£l6X87BUTETHAL uup* 123 •12U°C R.I. l*H70xae-129ALLTL-n-EUTTL BARBITURIC ACID m.p. 123.5-12R“C RalV l.U80X3OThe following compounds may be identified in a similar manner,
using melting points in conjunction with the refractive indices*ALLYL BARBITAL m.p*1 138;£-139°C R.I* l.U?SX43HEXOBARBITAL HUp*1 139 *Hl0*C R.I. 1*160X46APROBARBITAL m.p. ll*2°C R.I. 1.1*81 ,50BUTABARBITAL m.p. 16U*C R*I* l.£l0167DIAL m.p. 161; —165>*C R.I. l.J?00X7gPHEN0BARB1TAL m.p. 171 •172* C R.I. l.£30X88PR®INAL nup. 172 R.I. l.£0£x98There are also a number of barbiturates (7) which have melting
points between 11*8 and 15>7*C* These compounds likewise may be differentiated by means of tha refractive indices. They are*
-58-AMYTAL m.p. lU8-ll*8.5°C R.I. l.U5516Q l69CYCLOBARBIT AL m.p. lltf-l CTC R.I. 1.5o617sVINBARBITAL m.p. l52-l5U°C R.I. 1,520^5THIOPENTAL m.p.X53°C R.I. 1.5o8i7iMETHALLATAL m,p. 156-157 °C R.I. 1.53i|i7QETHYL ALLYL BARBITAL m.p. l57°C R.I. l.U8i|l845~( 2-BRCM ALLYL) -5~(l’*IETHYL
BUTYL BARBITURIC ACID m.p. l57°C R.I. l.U98lvaAlthough ETHYL ALLYL BARBITURIC ACID and 5-(2-BRCMALLYL)-5-(l-
METHYLBUTYL) BARBITURIC ACID have the same melting point, the temperatures at which the refractive indices are observed are different as indicated by the subscripts. ETHYL ALLYL BARBITURIC ACID (m.p.R.I. l.i4.8Ul84)j 5-(2-BRCMALLYL)-5-(1-METHILBUTYL) BARBITURIC ACID (m.p. 157 C$ R.I. I*l4-98 7g).
The remaining six compounds investigated had melting points which were far enough apart for their identification, nevertheless, the refractive indices of these barbiturates were determined and recorded in Tables XX (a) through (c).
Investigations of the effect of the presence of cyanide on the determination of barbiturates suggest the formation of some type of barbiturate-cyanide complex. Filter paper strips moistened with 0.2$ alcoholic guiaic solution and 0.1$ aqueous copper sulfate did not give any definite indication of the evolution of hydrocyanic acid when held over the neck of the flasks after the barbiturate-eyanide mixture was acidified. A positive reaction would have been indicated if the moistened filter paper strip had turned blue. After the barbiturate- eyanide solutions were acidified and an excess of 2 cc. of 10$ hydrochloric acid added to each, only six (6) of the mixtures yielded cloudy solutions as do pure barbiturate solutions. Pure barbiturate solutions
-59-yield cloudy* solutions upon acidification if their salts are present in a concentration of 1 mg* per cc* of water* Even though the free barbituric acid was not visible as a precipitate after the addition of 10% hydrochloric acid to the barbiturate-eyanide solutions, crystalline substances remained in every case after evaporation of the chloroform extract* Melting points run on these residues ranged from 10° below to 1|S*C above those of the original barbiturates (Table XXI)*
With the exception of THIOPENTAL, all of the compounds which exhibited an increase in melting point were unsaturated compounds* These barbiturates were: ALLIL-n-BDTXL BARBITURIC ACID} BUTALLYLONAL;CYCLOBARBITAL} HEXETHAL; FRCMINAL; SECONAL and VINBARBITAL* There were, however, some unsaturated barbituric acids which yielded compounds with lower melting points than the original respective barbiturate and still others in which the melting points did not change at all* SECONAL, which is usually viscous upon recovexy from chloroform, was crystalline in this instance* CYCLOBARBITAL; SECONAL and V INBAR BITAL were three compounds with increases of 3°C or more in the melting points* Among the recovered barbiturates with melting points little altered were: ALLYL-n-BUTIL BARBITURIC ACID; JMYTAL; APROBARBITAL; 5-(2-HRCMALLYL)-5- (1-METHYLBUTXL) BARBITURIC ACID; BUTALLYLONAL; BUTETHAL} DIAL; HEXOBARBITAL; PENTOBARBITAL; PROS!INAL and RUTONAL*'
Da the barbiturate procedure when the barbiturate-eyanide mixtures were acidified with lo£ hydrochloric acid to pemit the extraction by chloroform, all of the eleven (11) compounds just mentioned appeared to
-60-be physic ally changed since they did not form cloudy solutions as is usually the case when hydrochloric acid is added* If our theory that these barbiturates formed complexes with the cyanide in the eleven cases is correct, then we may possibly explain the fact that the melt* ing points remained unchanged by one or the other of the following assumptions, the first one of which seems to be more likelyt
1* The barbiturate-eyanide complex was destroyed during removal of the chloroform or the subsequent 1 hour drying at 100°C, or
2* The barbiturate-eyanide complex has the same melting point as the respective barbiturate*
None of the barbiturates used in the barbiturate-eyanide experiment which yielded a cloudy solution upon acidification with hydrochloric acid showed an appreciable increase in melting point* These six (6 ) barbiturates which yielded cloudy solutions when acidified were: 5*(2-BRCM ALLYL)-5-(l-KE'fflYL'BUiYL) BARBITURIC ACID} HEXETHAL} METHALLA- TALj PENTOBARBITAL; FRCMINAL and THIOPENTAL* The melting points of the six recorded barbiturates did not change appreciably over those of the respective pure compounds*
Since the guiaic*copper sulfate-filter paper test did not indicate the presence of free hydrocyanic acid in this instance, after acidification of the barbiturate-eyanide reaction mixtures, it can be said that six (6) of the barbiturate-eyanide reaction mixtures behaved as barbiturates under similar conditions* Li this group of six barbiturates, FRCMINAL and THIOPENTAL were the only two which yielded compounds with a melting point 2° or more above that of the original compound*
-&UA determination of the carbon content of these extracted compounds
might indicate whether or not the cyanide had remained in combination with the barbituric acid*
If the barbiturates deteriorate by long exposure to the atmosphere, this fact was not apparent by the melting point, with the possible exception of V IN BARBITAL (Table XXI}* It would seem that a reaction at the double bond in the unsaturated barbiturates or oxidation of the side c ha ink) at one of the terminal carbon atoms would be indicated by a noticeable change in the melting point. At the end of 60 days HEXOBARBITAL SODUM was the only barbituric acid salt, which upon a visual observation, appeared to have picked up moisture*
In order to cover the field of Forensic Chemistry 3s applied to barbiturates, representative products as they appear on the open market were used in these investigations*
We gratefully acknowledge gifts of thB following barbiturates which were used in this investigation:
ALLYL-n-BUTYL BARBITURIC ACID; BUTETHAL? ETHYL ALLYL BARBITURIC ACID; MOSIBAL* PENTOBARBITAL; PHENOBARBITAL and PENTOTRAL from Abbott Laboratories^
NOSTAL, PERNOSTON and S2EM0BAL from Ames Company, Inc*DIAL from Giba Pharmaceuticals, Inc*ALTJRATE from Hoffraan-La Roche, Inc*AMOBARBITAL and SECOBARBITAL from Eli Lilly and Company*RUTONAL from Hay and Baker Ltd, Dagenham, England BUTISOL from McNeil Laboratories, Ihc*ORTAL from Parka, Davis and Company
•62-
SANLOPTAL from Sandoz Pharmaceuticals DELVINAL from Sharp and Dohme, Inc*IPRAL from E. R* Squibb and Sons, andCYCLOBARBITAL5 EVTPAL and MEPH OB ARB IT AL from Winthrop-Stearnsi* Inc*
-63-SUMMABJ
Twenty-four barbiturates were tested for their stability in %%
potassium hydroxide (Table XIII) and in 20% acetic acid (Table XIV) for 2k hours at room temperature. The stability of the salts of this sane series of barbiturates in distilled water for 2h hours at room temperature was also investigated (Table XV).
Tissues containing known quantities of the various barbiturates were extracted by three methods:1. With potassium hydroxide for 2b hours at room temperature (Table
XVI).2. With 20% acetic acid for 2k hours at room temperature (Table XVII)3. At pH 10 (corresponding to that of salts of barbituric acids in
distilled water) for 2h hours at room temperature (Table XVIII).Refractive indices Tables XX(a) through (c) of the series of
barbiturates were determined by use of a Fisher Refractometer with a melting point heating head. The readings were taken at temperatures at which the refractive indices could best be observed and not at the transition points. The temperatures at which the readings were taken are recorded in Table XX(c).
A study of barbiturates in the presence of sodium cyanide was made. There was no apparent correlation between the type of reaction and the structure of the compound. The fact that none of the barbiturate- eyanide mixtures yielded hydrocyanic acid when acidified with hydrochloric acid (as indicated by the negative guiaic-copper sulfate-filter paper test) would seem to suggest that all of the barbiturates had reacted with sodium cyanide; however, the melting point of the reaction
product was not enough evidence that the product was a barbiturate- eyanide addition complex* In 75$ of the barbiturates investigated, physical evidence was indicated by the following observations: (1) the addition of hydrochloric acid to the barbiturate-eyanide mixtures did not produce cloudy solutions and (2) the negative guiaic-copper sulfate filter paper test.
Barbituric acids and their respective salts were exposed to the atmosphere for 60 days at room temperature* The melting point of VINBARBITAL increased. Melting points of the other barbituric acids remained the sane* that is, within the same range*
HEXOBARBITAL SODIIM was the only salt which, by visual observation, picked up moisture to any degree in 60 days*
CONCLUSIONS
The results of this investigation seem to justify the conclusion that the extraction of barbiturates' from tissues with aqueous solutions at pH 10 is the method of choice for Forensic Chemistry*
Comparison of the results obtained by extraction of barbiturates from tissues treated with 5$ potassium hydroxide or 20$ acetic acid for 2k hours with the results obtained by extraction of barbiturates from solutions of 5$ potassium hydroxide or 20$ acetic acid after standing 2h hours showed little differences*
Refractive indices of melted barbiturates may be used as an aid in the identification of the compounds*
Aqueous solutions of salts of barbituric acids do not deteriorate
-65-
appreciably during a 2k hour period*Sodium cyanide interferes with the identification of barbiturates
to some extent*With the exception of VINB ARBITAL and HEXOBARBITAL SODIUM, exposure
of barbiturates and their respective salts to atmospheric conditions apparently does not cause deterioration of the compounds*
-66-
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-73-autobiography
I, Gwendolyn Bertha Carson, was bom in Berkeley, California, October 25, 1918* I received my secondary school education at South High School in Columbus, Ohio* Both my undergraduate and graduate training to date have been received at The Ohio State University*The Bachelor of Science degree in Bacteriology was conferred in 19U3 and the Master of Arts degree with Physiological Chemistry as my field of specialization in 1?U5« While in residence, I acted in the capacity of part-time Technical Assistant in the Department of Physiological Chemistry* From 19ll5-1950, I held a full time appointment as Technical Assistant specializing in Toxicology under the supervision of Dr. Clayton S* Smith* In this capacity, I analyzed foods, medicaments and various biological specimens for doctors, hospitals, coroners and law enforcement officers throughout the State of Ohio* In 1?50, I received an appointment as Instructor at The Ohio State University, where I have continued my previous services in addition to teaching laboratory courses in Toxicology, Food Analysis and Blood Analysis* Since the language requirements and most of the course work had been completed before I became an Instructor, I was permitted to carry on my work on the dissertation while .holding this appointment*