NBS

PUBLICATIONS

AlllDE tlbbS3

NBS SPECIAL PUBLICATION 718

U.S. DEPARTMENT OF COMMERCE/National Bureau of Standards

Bibliographies of Industrial Interest:

Thermodynamic Measurements

on the Systems C02 -H20,

CuCI2 -H20, H2S04 -H20,

NH3 -H20, H2S-H20,

ZnCI2 -H20, and H3 P04-H20

B.R. Staples, D. Garvin, D. Smith-Magowan, T.L. Jobe, Jr.,

QC . J. Crenca, C.R. Jackson, T.F. Wobbeking, R. Joseph,

100 A. Brier, R.H. Schumm, and R.N. Goldberg

• U57

No .718

1986

NATL INST OF STANDARDS & TECH R.I.C.

A1 1102616653

Staples, B. R/Blbllographles of Industrl QC100 .U57 NO.718 1986 V1986 C.1 NBS-PUB
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ries ai Gaithershurg, MI), unless otherwise noted: mailing addro

ilhin ihc center arc located ai Boulder, CO 80303.

Icr, CO, vvii H some elements ai Gaithersburg, Ml).
NBS

RESEARCH

INFORMATION CENTER Bibliographies of Industrial Interest:

&uoo

Thermodynamic Measurements on the

Systems C02 -H2 0, CuCI2 -H2 0, H2S04 -H2 0, m

NH3 -H20, H2S-H20, ZnCI2 -H20,

*"y

and H3 P04 -H2 0

By:

B.R. Staples, D. Garvin, D. Smith-Magowan, T.L Jobe, Jr., J. Crenca, C.R. Jackson,

T.F. Wobbeking, R. Joseph, A. Brier, R.H. Schumm, and R.N. Goldberg

Chemical Thermodynamics Division

Center for Chemical Physics

National Measurement Laboratory

National Bureau of Standards

Gaithersburg, MD 20899

Sponsored by:

The Design Institute for Physical Property Data (Project 811)

American Institute of Chemical Engineers

New York, NY

U.S. DEPARTMENT OF COMMERCE, Malcolm Baldrige, Secretary

NATIONAL BUREAU OF STANDARDS, Ernest Ambler, Director

Issued September 1986
Library of Congress Catalog Number: 86-600544

National Bureau of Standards Special Publication 718

Natl. Bur. Stand. (U.S.), Spec. Publ. 718 146 pages (Sept. 1986)

CODEN: XNBSAV

U.S. GOVERNMENT PRINTING OFFICE

WASHINGTON: 1986

For sale by the Superintendent of Documents. U.S. Government Printing Office, Washington, DC 20402
ABSTRACT

Contained herein are bibliographies of sources of experimental

and correlated thermodynamic data for seven binary aqueous

mixtures of industrial importance, namely, mixtures of CO2 , H2S,

NH3 , H2SO4 , H3PO4 , CuCl 2 , and ZnCl2 with water. The categories

of equilibrium data included in the bibliographies are activity

and osmotic coefficients, equilibria in solution, enthalpies

and heat capacity data, vapor- liquid equilbria, and phase

equilbrium data.

KEY WORDS: ammonia; bibliography; carbon dioxide; copper

chloride; enthalpy; equilibrium constants;

heat capacity; hydrogen sulfide; phosphoric

acid; sulfuric acid; thermodynamics; water;

zinc chloride.

i i i

INTRODUCTION

This report is comprised of bibliographies on seven binary aqueous

mixtures of great industrial importance, mixtures of C0 2 , NH3, H2SO4,

H3PO14, H2S, CuCl2> and ZnCl2 with water. The bibliographies identify

sources of measurements or treatments of the equilibria that exist in

these systems and the effects of temperature and pressure upon these

equilibria. Treatments concerning more complex admixtures were not

explicitly sought but those that were found that also addressed a fundamental aspect, such as the effect of ionic strength, were retained in the

list. Three of the systems, C0 2 , NH3, and H2 S involve both vapor/liquid

equilibria and acid/base dissociations under most typical conditions.

Concerns regarding mixtures of H

2 S0 H and H3PO4 are limited for the most

part to acid/base dissociation. The two salt systems, CuCl 2 and ZnCl2

involve multiple association equilibria between cation and anion as well

as hydrolysis of the cation. Annotations have been provided to describe

the type of data reported in a particular publication and the environmental

conditions under which measurements were made or for which the treatment

is valid.

This report has been prepared for the Design Institute for Physical

Property Data (DIPPR) of the American Institute of Chemical Engineers as

part of the Project 811. Their support is gratefully acknowledged.

1
i

I

Table of Contents

System Authors Page

C0 2 -H 2 0 B. R. Staples, J. Crenca, C. R. Jackson and

D. Garvin* 3

CuCl 2-H 2

0 B. R. Staples, T. L. Jobe , Jr. and D. Garvin* 34

H

2 S0 i| -H 2 0 B. R. Staples, T. F. Wobbeking, R. Joseph,

A. Brier, and D. Garvin* • 45

NH-^-H-pO R. Joseph, D. Garvin, C. R. Jackson and

B. R. Staples* 71

H

2 S-H2

0 D. Garvin, A. Brier and R. H. Schumm* 92

ZnCl

2 -H 2 0 T. L. Jobe, Jr. and R. N. Goldberg 107

H

3 P0n-H 2 0 T. L. Jobe, Jr. and R. N. Goldberg 120

*prepared for publication by D. Smith-Magowan

2
C0 2 -H 2 0

Bert R. Staples, Jacqueline Crenca, Cynthia R.

Jackson, and David Garvin

INTRODUCTION

Listed in this bibliography are publications that

contain information on the vapor-liquid equilibrium between

CO2 gas and its solutions in water or data on the

ionization equilibria among C02(aq), H2C03(aq),

HC03"(aq) and C032"(aq). To a lesser extent

are publications on equilibria of CO2 with and in mixture

of water and organic compounds, on the enthalpies of

solution, dilution and ionization, on activity coefficients

and on the thermochemistry of the species listed above.

References reporting measurements or presenting correlations

or evaluations of data are included. Publications that

consider only applications of existing data to specific

systems but provide no new data have been avoided.

A subset of the papers is about the neutral molecule

H2CO3 , carbonic acid, as distinguished from dissolved

CO2 . The study of the formation and ionization is a problem in both kinetics and thermodynamics. See [75KER] for

a good introduction to this topic. Papers that refer to the

"true" ionization constant of carbonic acid are about

H2CO3 = H

+ + HCO3". Papers about the "apparent"

ionization constant of carbonic acid or of carbon dioxide

consider the overall process C02(aq) + H2O = H+ HCO3". There is confusion in the nomenclature but not

the numbers, the "true" K is approximately 10"^ and the

apparent K is about 10" ^ (because of the appreciable

solubility of CO2)

3
The references are listed alphabetically by first

author. Each citation is preceeded by a brief identification

code composed of the year of publication and three letters

from the last names of the first two authors. The citations

list the names of authors; the title of the article, chapter

or report as appropriate, and the source information, i.e.

journal or book title, volume, year of publication . The

structure of these citations does not conform to the

specifications established by the American National Standards

Institute but is the information necessary to direct the

reader to a particular reference. In a few instances only an abstract or secondary reference was available. In these

cases either the citation to Chemical Abstracts or source of

the secondary citation is given.

Some titles have been translated, e.g. those in

Russian. These translations come, by preference, from

abstracts in the papers themselves or from Chemical Abstracts

(The titles from the latter may be condesations

of the original)

Each paper has been annotated to show the class of data,

the temperature range and, if appropriate, pressure, solution

composition and pH. The data class designations are taken

from the Bulletin of Chemical Thermodynamics. They are two

letter codes with some mnemonic or physical chemical

associations. A list is appended. No attempt has been made

to assess the quality of the data, however, an annotation of

"Ze" indicates that a particular reference constitutes or includes an evaluation of experimental data from several

sources

The bibliography has been prepared by searching the

files of the NBS Chemical Thermodynamics Data Center, the

Bulletin of Chemical Thermodynamics and references in the

papers retrieved from those sources. It covers a time period

from the 19th century to 1982. Additions and corrections

will be welcomed.

4
22AD0/HEN: Adolph, E.F.; Henderson, L.J.; "The heat of reaction of oxygen with hemoglobin"; J. Biol. Chem. ; 50, 463-490

(1922); [CA 16-1254]

Hm, Hr, 22°C,

p? , solution and reaction with NaOH and KOH(aq)

7 7 AND: Anderson, G.R. ; "The Raman spectra of carbon dioxide in liquid H

20 and D20" ; J. Phys . Chem.; 81, 273-276

(1977) (negative results)

Md, 10°C, 45 atm, B^COj , Raman spec.

16ANT: Anthony; Bonfort's Wine and Spirit Circular; (1916) Pv, see 58LIN for table of data.

21APP: Appell, P.; "Resultats experimentaux sur l'absorption

de 1' anhydride carbonique par l'eau pure et salle"; Chaleur et Industrie; 2, 345-347, (1921)

Pv, t = ?, in H

20 and NaCl(aq),

cited in passing in 58LIN.

11AUE/PIC: Auerbach, F.; Pick, H . ; Arb . Kaiser Gesundh.; 38, 1243,

(1911) .#

Kk, 18°C, 2d ioniz. (from 64SIL/MAR)

63AUS/LAC: Austin, W.H.; LaCombe, E. ; Rand, P.W.; Chatterjee, M.

"Solubility of carbon dioxide in serum from 15 to 38°"

J. Appl. Physiol.; 18, 301-304, (1963); [CA 59:7969f]

Pv, 15-38°C, in H20 and blood serum.

56BAR/FRI: Bartholome, E.; Friz, H.; "Loslichkeit von Kohlendioxyd in Wasser bei hoheren Drucken"; Chemie - Ing . Tech.; 28, 706-708, (1956)

Pv, 10-30°C, 1-20 atm.

83BAR/HEP: Barbero, J. A.; Hepler, L.G.; McCurdy, K.G.; Tremaine, P. "Thermodynamics of aqueous carbon dioxide and sulfur

dioxide: heat capacities, volumes, and the temperature

dependence of ionization"; Can. J. Chem.; 61, 2509-2519,

(1983)

Dx, t = 25°C,

m(CO, ) = 0.01 - 0.1 mol/kg

66BAT/CLE: Battino, R.; Clever, H.L.; "The solubility of gases in liquids"; Chem. Rev.; 66, 395-463, (1966)

Zr , Ze, Pv, methods,

thermodynamic formulae,

bibliography, data quality but no data.

06BAU: Bauer, E.; "Uber die Dissociationskonstanten schwacher

Sauren"; Z. Phys. Chem.; 56, 212-222, (1906)

Pv, 25°C, 730 mmHg.

5
74BAU/GAS:

41BEL/SHP:

Bauer, K.; Gaspar, M.; "Solubility of Nagylengyel reservoir

rock in carbon dioxide-saturated formation water" ; Koolaj

Foldgaz; 7, 140-144, (1974)

Belopolsky; Shpunt; Palkina;

Ref. Zh. Khim. ; 4(6), 82-83, (1941)

Pv, 120°C, 10-70 kPa, in MgCOg and CaCOj sat. sol.

Pv, in aq. NH A C1-(NH 4

) 2S0

4

.

53BER/PAT: Berg, D.; Patterson, A., Jr.; "The high field conductance

of aqueous solutions of carbon dioxide at 25°C. The true ionization constant of carbonic acid"; J. Am. Chem. Soc.;

75, 5197-5200, (1953)

Kk, 25°C, H

2C0 3

.

78BER/VAN: Berg, R.L.; Vanderzee, C.E.; "Thermodynamics of carbon Hm, 25°C, C02 , NaHC03

, dioxide and carbonic acid- (a) the standard enthalpies Na2C0 3 in NaOH(dilute)

of solution of Na 2 C03 (s), NaHC03 (s), and C02 (g) in

in water 298.15 K, (b) the standard enthalpies of formation standard gibbs energies of formation, and standard entropies of C02 (aq), HC03 ~(aq), C03 2 ~(aq)

NaHC03 (s), Na2C0

3 (s), Na2C03

.

20( s )

, and

Na 2C0

3

. 10H2O(s )" ; J. Chem. Thermodyn . ; 10, 1113-1136, (1978)

78BER/VAN2: Berg, R.L.; Vanderzee, C.E.; "Enthalpies of dilution of Hm, Kk , 25°C, in sodium carbonate and sodium hydrogen carbonate solutions, carbonate sol. and the standard enthalpies of ionization of aqueous

carbonic acid, at 298. 15K"; J. Chem. Thermodyn.; 10, 1049-1075, (1978)

29BHA/DHA: Bhagwat, W.V.; Dhar, N.R.; "Dissociation constants of Pv, 20-30°C in aq. sol. KF and

some inorganic acids from solubility measurements"; salts of oxyacids, of P, Cr

J. Indian Chem. Soc; 6, 807-822, (1929) Mo, V, Ti , B, Sb , and I.

23BJE: Bjerrum, N.; "Dissoziationskonstanten von mehrbasischen Zr , Kk, 18°C, citing Sauren und ihre Anwendung zur Berechnung molekularer earlier data. Dimensionen" ; Z. Phys . Chem.; 106, 219-242, (1923)

1899BOH: Bohr, C; "Definition und Methode zur Bestimmung der Fv, 0-60°C, 1 atm.?, in H

20 Invasions- und Evasionscoef f icenten bei der Auflosung von and NaCl(aq). Gasen in Flussigkeiten . Werthe der Genannten Constanten

sowie der Absorptionscoef f icienten der Kohlensaure bei Auflosung in Wasser und in Chlornatr iumlosungen"

Ann. Phys.; 68, 500-525, (1899)

6
76BOU: Bourrie, G. ; "Relations between pH, alkalinity, buffer

intensity, and carbon dioxide equilibrium in natural

waters"; Bull. Assoc. Fr . Etude Sol; No. 3, 141-159,

(1976)

Pv, t ca . ambient , CO2 in natural water, analysis

of speciation.

69B0X/EMI: Boxkes, W. ; Emig, G. ; "Bestimmung von CC^-Loslichkeiten

in Wasser"; Chem.- Ing . - Tech.; 41, 1273-1276, (1969)

Pv, 15-80°C, pH 3.9-6,

[C02

] vs. pH (at 21°C)

33BRI/MAR: Brinkman, R. ; Margaria, R. ; Roughton, F.J.W.; "III. The kinetics of the carbon dioxide-carbonic acid reaction"

Phil Trans; A232, 65-97, (1933)

Kk, 15-18°C?, pH = 1-13,

f^COg (kinetics).

76BRU/BRU: Bruice, P.Y.; Bruice, T.C.; Yagi , H.; Jerina, D.M.; "Nucleophilic displacement on the arene oxides of phenanthrene" ; J. Am. Chem. Soc . ; 98(10), 2973-2981,

(1976)

Kk, 30°C, 2d ioniz. new data?

61BRU/NEL: Bruckenstein , S.; Nelson, D.C.; "Acid-base dissociation

constants in 1 . OM sodium chloride"; J. Chem. Eng. Data;

6(4), 605-606, (1961)

Kk, 25°C, in NaCl(aq)

38BUC: Buch, K.; "New determination of the second dissociation

constant of carbonic acid in sea water"; Acta Acad. Aboensis Math Physica; 11(5), 5-16, (1938)

Kk, Za, 20°C,

1 atm ., 2d ioniz

39BUC

Buch, K. ; "Kohlensaure in Atmosphare und Meer an der Grenze

Zum Arktikum" ; Acta Acad. Aboensis Math Physica; 11(12),

5-31, (1939)

Pv, ca.20°C, ca.10 4 atm, in seawater.

4 5BUC

Buch, K.; "Kolsyrej amuikten i Baltiksa Havet"; Fennia;

68(5), (1945)

Pv, in sea water,

cited in 770ST

1855BUN: Bunsen, R. ; "Memoires sur la loi de 1' absorption des gaz par les liquides"; Ann. Chim. Phys . ; 43, 496-508, (1855)

Pv, 0-20°C, 1 atm.

1855BUN2: Bunsen, R.; Justus Liebigs Ann. Chem.; 93, 1, (1855) Pv, 0-20°C, 1 atm, same data as 1855BUN.

1855BUN3

Buns en , M.R.j Phil . Mag . ( 4 th series ) ; "On the absorption

of gases"; 9, 116-130; 181-201, (1855)

Pv, 0-20°C, 1 atm, same data as 1855BUN.

7
27BUY/BRI:

05CHR:

Buytendyk, F.J.J. ; Brinkman, R. ; Mook, H.W.; "A study of

the system carbonic acid, carbon dioxide and water I. Determination of the true dissociation constant of carbonic

acid"; Biochem. J.; 21, 576-584, (1927)

Christoff , A. ; "Untersuchungen uber die Absorption des

CC>2 in wasserigen Salzlosungen und binaren

Flussigkeitsgemengen" ; Z. Phys . Chem. ; 53, 321-340, (1905)

Kk, 14-18°C, dil. sol., H2CO2 (kinetics

Pv, 15°C, in dil. aq. salt and acid sol.

06CHR: Christoff, A. ; "Uber die Abhangigkeit der Absorption von

der Oberflachenspannung" ; Z. Phys. Chem.; 55, 622-634,

(1906)

Pv, 20°C, in cone.

H

2SOA

.

71COA/KIN: Coan, C.R.; King, A.D., Jr.; "Solubility of water in Pv, t compressed carbon dioxide, nitrous oxide, and ethane. p = 1 Evidene for hydration of carbon dioxide and nitrous oxide in the Gas Phase"; J. Am. Chem. Soc; 93, 1857-1862, (1971)25 - 100°C,

60 atm.

82COB/MUR: Cobble, J.W.; Murray, R.C., Jr.; Turner, P.J.; Chen, K.; 'High-temperature thermodynamic data for species in aqueous solution'; EPRI NP-2400, Electric Power Research

Institute, Palo Alto, CA (1982)

Ze, Kk, Pv, 0-300°C, thermal functions, 2d ioniz.

79COL: Collins, P.L.F.; "Gas hydrates in CC^-bearing fluid

inclusions and the use of freezing data for estimation

of salinity"; Economic Geology; 74, 1435-1444 (1979)

Px, -30 to 30°C.

17C0S: Coste, J.H.; "The absorption of atmospheric gases by

water"; J. Soc. Chem. Ind.; 36, 846-853, (1917)

Pv, Zr, review of early meas .

62COX/HEA: Cox, J.D.; Head, A.J.; "Solubility of carbon dixoide in hydrofluoric acid solutions"; Trans. Faraday Soc.; 58, 1839-1845, (1962)

Pv, Hm, 20-30°C, 1 atm.

in H

20 and HF(aq)

67CUL/KES: Culberson, C; Kester, D.R.; Pytkowicz, R.M.; "High-pressure dissociation of carbonic and boric acids in seawater"; Science; 157, 59-61, (1967)

Kk, 22°C, 1-654 atm.

1st and 2d ioniz. in seawater

68CUL/PYT: Culberson, C.j Pytkowicz, R.M. ; "Effect of pressure on carbonic acid, boric acid, and the pH in seawater";

Limnol. Oceanog. 13(3), 403-417, (1968)

Kk, 2-22°C, 1-1000 atm, 1st and 2d ioniz. in seawater
38CUR/HAZ: Curry, J.; Hazelton, C.L.; "The solubility of carbon dioxide in deuterium oxide at 25°"; J. Am. Chem. Soc .

;

60, 2771-2773, (1938)

Pv, 25°C, in D 20.

38CUR/HAZ2: Curry, J.; Hazelton, C.J.; "The first thermodynamic

ionization constant of deuterio-carbonic acid at 25°"; J.

Am. Chem. Soc; 60, 2773-2776, (1938)

Kk, 25°C, 1 atm, 1st ioniz.

54CUT/STR:

65DIS/DIS:

67DIS/DIS:

56DOD/STU:

73DYR/HAN

:

70EDM/GIE:

Cuta, F.; Strafelda, F.; "The second dissociation constant

of carbonic acid between 60 and 90°C"; Chem. Listy; 48, 1308-1313, (1954)

Disteche, A.; Disteche, S.; "The effect of pressure on pH

and dissociation constants from measurements with buffered

and unbuffered glass electrode cells"; J. Electrochem. Soc; 112, 350-354, (1965)

Disteche, A.; Disteche, S.; "The effect of pressure on the dissociation of carbonic acid from measurements with

buffered glass electrode cells"; J. Electrochem. Soc.;

114, 330-340, (1967)

Dodds , W.S.; Stutzman, L.F.; Sollami , B.J.; "Carbon dioxide

solubility in water"; Ind . Eng. Chem.; 92-95, (1956)

Dyrssen, D.; Hansson, I.; "Ionic medium effects in sea

water. Comparison of acidity constants of carbonic acid in sodium chloride and synthetic sea water"; Marine Chem.;

1(2), 137-149, (1973); [CA 79:70056c]

Edmond, J.M.; Gieskes, J.M.T.M.; "On the calculation of the degree of saturation of sea water with respect to calcium

carbonate under in situ conditions"; Geochim. Cosmochim.

Acta; 34, 1261-1291, (1970)

Kk, 60-90°C, 2d ioniz. in dil. NaHC03 /Na2C0 3 sol.

Kk, Dm, 22°C p = 1000 kg

-9 cm ?, 1st and 2d ioniz.,

in KCl(aq)

.

Kk, Dm, 22°C, 1-1000 bar

pH 5.1-9.6

1=0-1.0 1st and 2d ioniz.

Zc, Pv, 0-120 C, 1-700 atm

.

Zr, Kk, 1st. and 2d ioniz.

in seawater.

Kk, Za, 5-35°C, 1-1000 atm. in seawater.

78EDW/MAU: Edwards, T.J.; Maurer, G.; Newman, J.; Prausnitz, J.M.; "Vapor-liquid equilibria in multicomponent aqueous solutions of volatile weak electrolytes"; AIChE J.; 24(6),

966, (1978)

Zc, Pv, Kk, 0-170°C, I to 6m, 1st ioniz.

9
7 5EDW/NEW: Edwards, T.J.; Newman, J.; Prausnitz, J.M.; "Thermodynamics

of aqueous solutions containing volatile weak

Electrolytes"; AIChE J.; 21(2), 248-259, (1975)

Zc, Pv, Kk, 0-100°C,

m(salt) to 2, 1st ioniz.

59ELL: Ellis, A.J.; "The effect of pressure on the first

dissociation constant of 'carbonic acid'"; J. Chem. Soc

3689-3699, (1959)

Kk, 25-65°C, P(total) to 3000 atm, 1st ioniz.

59ELL2: Ellis, A.J.; "The system Na2C0

3 -NaHC03 -C02 at temperatures up to 200°"; Am. J. Sci . ; 257,

287-296, (1959)

Pv, 120-200°C,

Na2C03 /NaHC03 sol.

59ELL3:

59ELL4 :

Ellis, A.J.; "The solubility of carbon dioxide in water at high temperatures"; Am. J. Sci.; 257, 217-234, (1959)

Ellis, A.J.; "The solubility of calcite in carbon dioxide

solutions"; Am. J. Sci.; 257, 354-365, (1959)

Pv, 115-350°C,

P(C02

) < 5 atm.

Pv, 100-300"C,

P(C02

) = 1-4 atm. , sat. CaC03 (aq)

57ELL/FYF: Ellis, A.J.; Fyfe, W.S.; "Hydrothermal chemistry"; Rev. Pure Appl. Chem.; 7, 261-316, (1957)

Zr, Pv, 25-370°C,

Kk, 0-300°, (graph)

63ELL/GOL: Ellis, A. J.; Golding, R. M.; "The solubility of carbon dioxide above 100°C in water and in sodium chloride

solutions"; Amer . J. Sci.; 261, 47-60, (1963)

Pv, 150-300°C,

m(NaCl) = 0-2.

56END/KLE

Enders, C; Kleber, W. ; Paukner, E.; "The solubility of carbon dioxide, oxygen, and nitrogen in beer and water"; Brauwissenschaft; 2-8, 50-59, (1956)

4% EtOH and beer.

57ERE:

59ERE

Eremenko, V.Ya.; "The value of the ionization constants of carbonic acid"; Gidrokhim. Materialy; 27, 122-134, (1957);

[CA 52: 13379c]

Eremenko, V.Ya.; Gidrokhim. Materialy;

28, 233, (1959)

Zr, Kk , literature review.

Zr, Kk, 0-38°C, 2d ioniz. (from 64SIL/MAR)

75ESP: Espinoza Gala, 0.; "Diagram for calculation of molar heats

of solution of carbon dioxide in water"; Bol. Soc. Quim.

Peru; 41, No. 2, 91-93, (1975)

Hm, Zc, -20 to +20°C,

graphical correlation,

data source not given.

10
75ESP2: Espinoza Gala, 0.; "Generalized nomogram for calculation of equilibrium data in the carbon dioxide-water system"; Bol.

Soc. Quim. Peru; 41, No. 2, 94-100, (1975)

Zc , Pv, graphical

correlation, data

source not given.

52ESS/GAN: Essery, R.E.; Gane , R. ; "Effect of storage on beers Pv, -20 and -5°C, in ice. concentrated by freezing, and on beers kept in the frozen

state- solubility of carbon dioxide in ice"; J. Inst. Brewing; 58, 129-133, (1952); [CA 46:9775a]

76EVE/MOO: Evelein, K.A.; Moore, R.G.; Heidemann, R.A.; "Correlation Zc , Pv, Px, t = 290-520°C,

of the phase behavior in the systems hydrogen sulf ide-water p to 2000 atm, 2 and 3 and carbon dioxide-water"; Ind. Eng. Chem. ; 15(3), 423-428 phase equilibrium.

(1976)

24FAU: Faurholt, C.; "Etudes sur les solutions aqueuses d'anyhydride carbonique et d'acide carbonique";

J. Chim. Phys.; 21, 400-455, (1924)

Kk, 0-18°C, H

2C03

.

21FAU: Fauholt, C .

(NH

A

) 2C03

" und "C02 + H20 =

H2C03

"; Z. Anorg. Allgem. Chem.;

120, 85-102, (1921)

Kk, 0°C, H

2C03 (kinetics

and thermo )

08FIN: Findlay, A. ; "Einfluss von Kolloiden auf die Absorption von

gasen, insbesondere von Kohlendioxyd , in Wasser"; Kolloid with added colloids.

Z.; 3, 169-170, (1908)

10FIN/CRE: Findlay, A.; Creighton, H.J.M.; "The influence of colloids

and fine suspensions on the solubility of gases in water. Part I. Solubility of carbon dioxide and nitrous oxide";

J. Chern. Soc; 97, 536-561, (1910)

Pv, 25°C, in H

20 and aq. suspensions of Fe(0H) 3

, dextrin, As 2

S

3

, and nat. macro-molecules

15FIN/H0W: Findlay, A.; Howell, O.R.; "The solubility of carbon Pv, 25°C, in aq. starch dioxide in water in the presence of starch"; J. Chem. Soc.; sol.

107, 282-284, (1915)

11FIN/SHE: Findlay, A.; Shen, B.; "The solubility of carbon dioxide Pv, 25°C, in H

20, in beer"; J. Chem. Soc; 1313-1320, (1911) alcohol-water sol., and

in beer.

11
12FIN/SHE: Findlay, A.; Shen, B.; "The influence of colloids and fine Pv, 25°C, 760- 1350mmHg

,

suspensions on the solubility of gases in water. Part II. also salt sol. and solubility of carbon dioxide and of hydrogen"; J. Chem. colloids.

Soc; 101, 1459-1468, (1912)

13FIN/WIL: Findlay, A.; Williams, T. ; "The influence of colloids and fine suspensions on the solubility of gases in water. Part

III. Solubility of carbon dioxide at pressures lower than atmospheric"; J. Chem. Soc; 103, 636-645, (1913)

Pv, 25°C, in H

2

0, and

aq. suspensions of Fe(0H) 3

, dextrin,

starch, etc.

59FOK: Fokeev, V.M.; "Determination of the saturation pressure of Pv, t = ?, carbon dioxide in water"; Izvst. Vysshikh Ucheb . Zavedenii, x(C02) = 0.5-0.95.

Geol. i Razvedka; (6), 87-92, (1959); [CA54:6280i]

29FRE/J0H: Frear, G.L.; Johnston, J.; "The solubility of calcium Pv, 25°C, 0.003-1 atm. carbonate (calcite) in certain aqueous solutions at 25°"; in sat. CaCO-^aq).

J. Am. Chem. Soc; 51, 2082-2093, (1929)

58FRY/NIL: Frydman, M. ; Nilsson, G.; Rengemo, T . ; Sillen, L.G.; "Some Kk , 25°C, 1st and 2d ioniz., in solution equilibria involving calcium sulfite and carbonate NaHCO^/NaCOj/NaClO^ sol.

III. The acidity constants of B^COg and ^SOg , and CaCOg CaSO-j equilibria in NaClO^ Medium at 25°C"; Acta Chem. Scand.; 12, 378-884, (1958)

26GAT: Gatterer, A.; "The absorption of gases by colloidal

solutions"; J. Chem. Soc; 299-316, (1926)

Pv, 5-25 C, in colloidal

sol

.

04GEF: Geffcken, G. ; "Beitrage zur Kenntnis der Loslichkeitsbeeinflussung" ; Z. Phys . Chem.; 49, 257-302,

(1904) alkali metal salts.

Pv, 15 and 25°C, in aq.

sol. of acids and of

79GEH/LEN: Gehrig, M. ; Lentz, H.; Franck, E.U.; "Thermodynamic Pv, Px, t<500°C,

properties of water-carbon dioxide-sodium chloride mixtures p<3kbar.

at high temperatures and pressures"; High-Pressure Sci. Technol., AIRAPT Conf . , 6th; 1, 539-542 (1979)

71GER/BIT: Gerecke, J.; Bittrich, H.J.; Wiss. Tech. Rochsch. Chem. Pv, 25"C, (from 77WIL/BAT) Carl Schorlemmer Leuna - Mersebur; 13, 115, (1971)

I,'
80GIG: Giggenbach, W.F.; "Geothermal gas equilibria"; Geochim. Pv, 100-300°C,

Cosmochim. Acta; 44, 2021-2032, (1980) application of previously published

data to geochemical

equilibria

82GIL/WIL: Gillespie, P.C.; Wilson, G.M. ; 'Vapor-liquid and liquid- Pv, t = 60 - 600°F,

liquid equilibria: water-methane, water-carbon dioxide, p = 17 - 3000 psi

water-hydrogen sulfide, water-npentane

water-methane-npentane' ; Research Report 48, Gas Processors Association; Tulsa, Okla. , (1982)

53GJA: Gjaldbaek, J. Chr . ; "The solubility of carbon dioxide in Pv, 25°C,

perfluoro-n-heptane , normal heptane, cyclo-hexane , carbon CCl^, CgE

tetrachloride, benzene, carbon disulphide and aqueous '-'7^16 solution of aerosol"; Acta Chem. Scand.; 7, 537-544,

(1953)

60GLA/LON: Glasoe, P.K.; Long, F.A.; "Use of glass electrodes to Kk , 25°C, 1st ioniz., measure acidities in deuterium oxide"; J. Phys . Chem.;

64, 188-190, (1960)

58GOL/MAL: Golutvin, Yu . , M. ; Malysheva, T.V.; Skorobogatova , V.I.-; Pv, 20°C. "Solubility of hydrogen sulfide and carbon dioxide in water

and aqueous solutions of ammonia and phenol"; Izvest.

Sibir. Otdel. Akad. Nauk SSSR; (8), 83-87, (1958); [CA

53:9787i]

74GOR/BAS: Gordienko, V.I.; Bashirova, L.Kh.; Leibert, B.M.; Kk, 25°C? 2d ioniz.,

"Hydrolysis constants for carbonate and bicarbonate ions in NaOH/NaHCO^ /NaCl( aq)

highly concentrated sodium chloride aqueous solutions";

Izv. Vyssh. Ucheb. Zaved . Khim. Khim. Tekhnol. ; 17, 1127-1131, (1974); [CA 82-22381]

73GRE: Greenwood, H.J.; "Thermodynamic properties of gaseous Da, 450-800°C,

mixtures of H

20 and C02 between 450° and in gaseous C02 + H20 mixtures.

800°C and 0 to 500 bars"; Am. J. Sci.; 273, 561-571 (1973)

20HAE: Haenel, 0.; "The strength of carbonic acid at higher Pv, Kk , 0°C, 1-50 atm. pressures"; Centr . Min. Geol.; 25-32, (1920); [CA 15:620]

13
1885HAM:

73HAN

73HAN2:

58HAN/BER:

01HAN/VAG:

45HAR/BON:

4 3HAR/DAV:

41HAR/SCH:

Hamberg, A.; "Beitrage zur Chemie des Meerwassers II. Ein Apparat zur Bestimmung des Stickstoffgases und der Kohlensaure im Meerwasser" ; J. Prakt. Chem. ; [2] 33, 433-463, (1885)

Pv, 0-20°C, in full-strength

and diluted seawater.

Hansson, I.; "The determination of dissociation constants

of carbonic acid in synthetic sea water in the salinity

range of 20-40 ppt . and temperature range of 5-30°C"; Acta Chem. Scand.; 27, 931-944, (1973)

Hansson, I.; "A new set of acidity constants for carbonic

acid and boric acid in sea water"; Deep-Sea Research; 20, 461-478, (1973)

Kk, Za, 5-30°C,

1 atm, 1st and 2d

ioniz. in seawater.

Kk, Zc, 10-35°C,

1 atm, in seawater.

Han, S.T.; Bernardin, L.J.; "Ionic activity coefficients of Kk , Dm, Da, Zc , 20-65°C,

sodium bicarbonate" ; Tappi ; 41, 540-544, (1958) 1 atm, I to 1.1

Hantzsch, A.; Vagt, A.; "Uber den Zustand Geloster Stoffe

auf Grund von Verteilungsversuchen" ; Z. Phys . Chem.; 38, 705-42, (1901)

Harned, H.S.; Bonner, F.T.; "The first ionization of carbonic acid in aqueous solutions of sodium chloride"; J. Am. Chem. Soc . ; 67, 1026-1031, (1945)

Harned, H.S.; Davis, R. Jr.; "The ionization constant of carbonic acid in water and the solubility of carbon dioxide

and in water and aqueous salt solutions from 0 to 50°";

J. Am Chem. Soc; 65, 2030-2037, (1943)

Harned, H.S.; Scholes , S.R., Jr.; "The ionization constant

of HC0

3

" from 0 to 50°"; J. Am. Chem. Soc; 63, 1706-1709, (1941)

Pv, 0-90°C,

P(C02

) = 0.3-0.7 atm.

Kk, 0-50°C, 1st ioniz. m(NaCl) = 0-1.

Pv, Kk, 0-50°C, 1st ioniz.

in and Na2C03(aq).

Kk, Hr, Ql, 2d ioniz. 0-50°C, in Na 2C0

3 (aq)

16HASHasselbalch, K.A. ; "Die Berechnung der Wasserstoff zahl des Blutes aus der freien und gebundenen Kohlensaure desselben, und die Sauerstof fbindung des Blutes als Funktion der Wasserstoff zahl"; Biochem. Z. ; 78, 112-144, (1916)

Kk, 18 and 38°C, in NaHC03 (aq) and blood.

14
25HAS/SEN: Hastings, A.B.; Sendroy, J., Jr.; "The effect of variation

in ionic strength on the apparent first and second dissociation constants of carbonic acid"; J. Biol. Chem.

65, 445-455, (1925)

Kk, 38°C, 1st and 2d ioniz. NaHC03 /Na2C0

3 /NaCl/NaOH

sol

73HAW/PYT: Hawley, J.E.; Pytkowicz, R.M. ; "Interpretation of pH Kk , 25°C, 1 atm, measurements in concentrated electrolyte solutions"; Marine in NaCl. Chemistry; 1, 245-250, (1973)

71HAY/MAL: Hayduk, W. ; Malik, V.K. ; "Density, Viscosity, and carbon Pv, 25°C, 1 atm., in dioxide solubility and diffusivity in aqueous ethylene r^O-glycol mixt, x=0 to 1 glycol solutions"; J. Chem. Eng. Data; 16, 143-146,

(1971)

15HEA: Heath, W.P.; Privately Printed, Atlanta, GA. ; (1915) Pv, see 58LIN for data.

67HEL: Helgeson, H.C.; "Thermodynamics of complex dissociation in aqueous solution at elevated temperatures"; J. Phys . Chem.; 71(10), 3121-3126, (1967)

Ze, Kk, Pv, 0-200°C

76HEL/KIR: Helgeson, H.C.; Kirkham, D.H.; "Theoretical prediction of Kk , Zc , Ze

,

the thermodynamic properties of aqueous electrolytes at 25-3000 °C, high pressures and temperatures. III. Equation of state 1-1000 atm. for aqueous species at infinite dilution"; Am. J. Sci.;

276, 97-240, (1976)

81HEL/KIR: Helgeson, H.C.; Kirkham, D.H.; Flowers, G.C.; "Theoretical Ze, Kk , Da, Dm, prediction of the thermodynamic behavior of aqueous 0-600 °C, 0-5kB electrolytes at high pressures and temperatures: IV. Calculation of activity coefficients, osmotic coefficients,

and apparent molal and standard and relative partial molal

properties to 600°C and 5kB"; Am. J. Sci.; 281,

1249-1516, (1981)

7 0HER/GOD: Hertz, M.B.; Godbold, T.M.; "Sodium carbonate equilibrium

with monoethanolamine additive"; Roth, J. A.; 15(1),

137-139, (1970)

Pv, Kk, 30°C, in NaHC03 /Na2C03 sol. and with added monoethanolamine

75HOR: Horrath, A.L.; "Reference literature to the critical Zr, Vc properties of aqueous electrolyte solutions"; J. Chem. Infor. Comp. Sci.; 15, 245-247 (1975)

15
57HOU/MCL: Houghton, G. ; McLean, A. M. ; Ritchie, P. D.; Pv, Vg, 0-100"C, p = 0-36 "Compressibility, fugacity, and water-solubility of carbon atm. , xCCC^) = 0.6 to 10, dioxide in the region 0-36 Atm. and 0-100°C"; Chem. Eng. reanalysis, new eq. of state.

Sci. ; No. 6, pg. 132, (1957)

72HU/SIN: Hu, A.T.; Sinke, G.C.; Mansson, M. ; Ringner, B.; "Test Ze , Pv, Hm, 25°C. Substances for Bomb Combustion Calorimetry. p-chlorobenzoic

acid"; J. Chem. Thermodyn.; 4, 283-299, (1972)

78JHO/NEA: Jho, C; Nealon, D.; Shogbola, S.; King, A. D., Jr.; "Effect of pressure on the surface tension of water adsorption of hydrocarbon gases and carbon dioxide on water

at temperatures between 0 and 50°C"; J. Colloid Interface

Sci.; 65, 141-154, (1978)

Hs, 25°C, effect of C02 on surface tension of

01JUS: Just, G. ; "Loslichkeit von gasen in Organischen 25°C, 1 atm.?, also in Losungsmitteln" ; Z. Phys . Chem.; 37, 342-367, (1901) 43 organic liq. at 15,

20, and 25°C.

73KAL/DUB: Kalinin, Yu. Ya.; Dubinin, A. B.; "Specific heats of a Ql, Qh, Qg, 0-320°C,

boiling liquid and dry saturated water vapor, Freon 21, and sat. process, carbon dioxide along the left and right branches of a boundary curve"; Izv. Vyssh. Ucheb. Zaved., Energ . ; 16, No. 6, 142-147, (1973)

34KAU: Kauko, Y.; "The first dissociation constant of the carbonic Zr , Kk , 1st ioniz., 0-25°C. acid equilibrium"; Ann. Acad. Sci. Fennicae; A39(3), 88, (1934); [CA 29:3218 7]

35KAU: Kauko, Y.; "The value of the first dissociation constant of Ze , 18°C, 1st ioniz. carbonic acid"; Ann. Acad. Sci. Fennicae; No. 9, 8 pp. (1935) ; [CA 30-2828 4]

37KAU/AIR: Kauko, Y.; Airola, A.; "Die Zweite Dissoziationskonstante

der Kohlensaure"; Z. Phys. Chem.; A179, 307-313, (1937)

Zr, Kk, 0-38°C, dilute

Na 2C03 /NaHC0

3 sol.

35KAU/CAR: Kauko, Y.; Carlberg, J.; "Zur Kenntnis der Ersten Dissoziationskonstante der Kohlensaure"; Z. Phys. Chem. A173, 141-149, (1935)

Kk, 18°C, 1st ioniz.

39KAU/ELO: Kauko, Y.; Elo, H.; "Die erste Dissoziation der Ze, Kk, 1st ioniz., Kohlensaure"; Z. Phys. Chem.; A184, 211-230, (1939) 0-25"C.

16
16KEN: Kendall, J.; "The specific conductivity of pure water in equilibrium with atmospheric carbon dioxide"; J. Am. Chem. Soc; 38, 1480-1497, (1916)

Pv, Kk, 1st ioniz. 0-25°C.

60KER: Kern, D.M.; "The hydration of carbon dioxide"; J. Chem. Education; 37, 14-23, (1960)

Zr, Kk, 25°C, H

2C0 3 (kinetics and thermo)

73KHI/KAD: Khitarov, N. I.; Kadik, A. A.; "Water and carbon dioxide in magmatic melts and peculiarities of the melting process";

Contrib. Mineral. Petrology; 41, 205-215, (1973)

Pv, above 1000°C, p

lOkb.

37KIS/LAJ: Kiss, A.V. ; Lajtai, I.; Thury, G. ; "Uber die Loslichkeit

von gasen in Wasser-Nichtelektroltgemischen" ; Z. Anorg.

Allgem. Chem.; 233, 346-352, (1937)

Pv, 0-25°C, in and its mixtures

with org. compounds.

26KLE/HER: Klemenc , A.; Herzog, M. ; "Zur Kenntnis der Dissoziationskonstante der Kohlensaure" ; Montsh. ; 47, 405-413, (1926)

Kk, 0, 12.5°C, 1st ioniz. very dil. solutions.

35KOB/WIL: Kobe, K.A.; Williams, J.S.; "Confining liquids for gas analysis"; Ind . Eng. Chem.; 7(1), 37-38, (1935)

Pv, 25°C, 1 atm. , in H2O, acid and salt sol.

61KOE/ENG:

28KOL/BOS:

Koefoed, J. ; Engel, K. ; "Kinetics of the carbon dioxide

hydration under conditions of enforced stationarity" ; Acta

Chem. Scand.; 15, 1319-1326, (1961)

Kolthoff, I.M.; Bosch, W. ; "The influence of neutral

saltson acid-salt equilibria III. The second dissociation constant of carbonic acid and the influence of salts on the activity of the hydrogen ions in a bicarbonate

carbonate mixture"; Rec . Trav. Chim. ; 47, 819-825, (1928)

Kk, 0°C, H2C03 (kinetics),

Kk, 25°C, 2d ioniz., in B* 20 and alkali metal salt sol.

80KOR/KAR: Korbutova, Z. V.; Karpova, Yu . G. ; Leites , I. L .

"Solubility of carbon dioxide in aqueous solutions of potassium carbonate"; Khim. Prom-st.; No. 12, 721-725,

(1980); Tr. The Soviet Chemical Industry, 1401-1404,

(1980)

Pv, 40-70°C?, 20-40 wt%

17
70KRA/SOB: Kratochvil, J.; Sobr, J.; Matous , J.; Pick, J.; "Solubility Pv, 25°C, p to 40 of carbon dioxide in heavy water at pressures up to 40 atm. , sol. in D2O. Atm."; Collect. Czech. Chem. Commun . ; 35, 3761-3764,

(1970)

35KRI/SHA: Kritschewsky , I.R.; Shaworonkof f , N.M.; Aepelbaum, V.A.; Pv, 20-30°C, 5-30 bar. "Gemeinsame Loslichkeit der gase in Flussigkeiten unter

Druck. I. Loslichkeit des Kohlendioxyds in Wasser aus seinen Gemischen mit Wasserstoff bei 20 und 30°C und

9 Gesamtdruck bis 30 kg/cm "; Z. Phys . Chem.; A175,

232-238, (1935)

82KRU/FRA : Kruse, R. ; Franck, E.U.; "Raman spectra of hydrothermal

solutions of CC>2 and KHCOg at high temperatures

and pressures"; Ber . Bunsenges. Phys. Chem.; 86, 1036-1038 (1982)

Kk, 22-300 C, 1st ioniz., p to 2000 bar.

71KRY/STA: Kryukov, P. A.; Starostina, L.I.; Tarasenko, S.Ya.; Pavlyuk, Kk , 25-100°C, 1st and

L.A.; Smolyakov, B.S.; "Ionization constants of carbonic 2d ioniz.

acid, hydrogen sulfide, boric acid, and sulfuric acid at high temperatures"; Larionov, E.G.; Mezhdunar. Geokhim.

Kongr., [Dokl.], 2, 186-198, (1971); [CA 81-69193]

22KUN: Kunerth, W.; "Solubility of CO2 and ^0 in certain solvents"; Phys. Rev.; 19, 512-524 (1922)

Pv, 18-34°C, approx. 1 atm. and 2d ioniz.

69LAR/HEP: Larson, J.W. ; Hepler, L.G. ; "Heats and entropies of Zr.Kk, Hr , 25°C, Of ionization"; 'Solute-Solvent Interactions', 1st and 2d ioniz. Coetzee, J.F. and Ritchie, C.D.(eds);

Marcel Dekker, NY and London, (1969)

71LI/TSU: Li, Y.-H.; Tsui, T.-F.; "Solubility of Pv, t = 0-30°C, [salt] carbon dioxide in water and sea water"; = 0-2.9%, CI and

J. Geophys. Res. ; 76,4203-4207, (1971) 0.64m NaCl.

58LIN: Linke, W.F. ; 'Solubilities' , 4th ed.; D. Van Nostrand, Ze, Pv, 0-10000, compiled

Princeton, (1958) [originated by A. Seidel] solubility data for CO2 in water salt solutions

and mixed solvents.

18
Lindberg, A.; Borno, C; "Calculation of calcium

carbonate-carbon dioxide equilibrium in water and mixtures

of water"; Verh.-Int. Ver. Theor. Angew. Limnol.; No. 19,

Pt. 2, 1511-1517, (1975)

Za, Kk, 0-100°C,

selected ionization

constants (from

Schmitt(1955) )

Ljunggren, S.; Lamm, 0.; "A determination of moderately

chemical equilibrium"; Acta

(1958)

relaxation method for the rapid reaction rates near

Chem. Scand.; 12, 1834-1850,

Kk, 4°C, H

2C0 3 (kinetics

and thermo )

Loprest, F.I.; "A method for the rapid determination of Pv, Px , 2--60°C. the solubility of gases in liquids at various temperatures";

J. Phys. Chem.; 61, 1128-1130 (1957)

Maclnnes, D.A.; Belcher, D.; "The thermodynamic ionization Kk , 25°C, constants of carbonic acid"; J. Am. Chem. Soc; 55, 1st and 2d ioniz. 2630-2646, (1933)

Maclnnes, D.A.; Belcher, D.; "The thermodynamic ionization Kk , 38°C, constants of carbonic acid at 38° from electromotive 1st and 2d ioniz. force measurements"; J. Am. Chem. Soc.; 57, 1683-1685,

(1935)

Mackenzie, J.J.; "Uber die Absorption der gase durch Salzlosungen" ; Ann. Phys.; 237, 438, (1877)Pv 8-30°C, 1 atm?

aq NaCl, KC1, NH^Cl,

and BaCl--

Mai, K.L.; Babb, A.L.; "Vapor-liquid equilibria by Pv, 20-65°C, in radioactive tracer techniques. System carbon dioxide Na^O^/NaHCOj sol. hydrogen sulfide-sodium carbonate-sodium bicarbonate sodium

sulfide-water" ; Ind. Eng. Chem.; 47, 1749-1757, (1955)

Makarov, A. V.; Kapyrina, Yu . D . ; Fokeev, V. M. ; Pv, 290-370 K, "Solubility of carbon dioxide in aqueous-saline solutions in 0 . 1M NaCl. under pressure"; Izv. Vyssh. Ucheb. Zaved., Geol. Razved.;

17, No. 4, 90-92, (1974)

Malinin, S.D.; "The system H

20-C02 at high

temperatures pressures"; Geokhimiya; No. 3, 235-245,

(1959); [CA 53:18612f] Tr . Geochemistry No. 3 292,

(1959)

and Pv, t = 200-330°C,

p = 100-500kg/cm2

, [salt] = 0, 10% CaCl2

.

19
74MAL

Malinin, S.D.; "Questions concerning the thermodynamics of

the - CO2 system"; Geokhimiya; No. 10, 1523-1549, (1974)

Zr, V, 100-600°C.

78MAL: Malinin, S.D.; "CO2 solubility in aqueous solutions of electrolytes"; Geokhimiya; No. 10, 1452-1465, (1978)

Zc, Pv, 25-300"C, in

75MAL/KUR: Malinin, S. D.; Kurovskaya, N. A.; "Solubility of carbon dioxide in chloride solutions at elevated temperatures and carbon dioxide pressures"; Geochem. Intern.; 12, 199-201,

(1975)

Pv, t = 25-100°C, p to

50kg/crrf 2

, [salt] = 0 to

7 molal, solubility in NaCl and CaCl2

solutions

72MAL/SAV: Malinin, S.D.; Savelyeva, N.I.; "The solubility of C02 in NaCl and CaC^ solutions at 25, 50 and 75° under elevated CO2 pressures"; Geochem. Int.; 9, 410-418 (1972)

Pv, 25-75°,

in NaCl and CaCl- solutions

41MAR/KOB: Markham, A.E.; Kobe, K.A. ; "The solubility of gases in liquids"; Chem. Rev.; 41, 519-588, (1941)

Zr, Pv, methods,

thermodynamic formulae,

bibliography, data quality but no values

for solubilities.

41MAR/KOB2: Markham, A.E.; Kobe, K.A.; "The solubility of carbon Pv, 25°C, in H

2 S0 4 (aq) and dioxide in aqueous solutions of sulfuric and perchloric in HC10/) (aq), 0-100%. acids at 25°"; J. Am. Chem. Soc; 63, 1165-1166, (1941)

41MAR/KOB3: Markham, A.E.; Kobe, K.A.; "The solubility of carbon Pv, 0.2-40°C,

dioxide and nitrous oxide in aqueous salt solutions"; J. in various salt solutions.

Am. Chem. Soc; 63, 449-454 (1941)

58MAR/LOP: Marshall, W.L.; Loprest, F.J.; Secoy, C.H.; "The Pv, 200-290°C, P to 200 atm., equilibrium Li 2C03 (s) + CO2 + H20 = 2 Li +

+ at high in sat. I^CO-j sol. 2HCO2 temperature and pressure"; J. Am. Chem. Soc; 80, 5646-5651, (1958)

74MAS/KIN: Massoudi, R . ; King, A. D . , Jr.; "Effect of pressure on the Ps , 25 V C. surface tension of water. Adsorption of low molecular

weight gases on water at 25°C"; J. Phys . Chem.; 78 , 2262-2266, (1974)

20
Matous, J.; Sobr, J.; Novak, J. P.; Pick, J.; "Solubility

of carbon dioxide in water at pressures up to AO atm"

Collect. Czech. Chem. Commun.; 34, 3982-3985, (1969)

Pv, 30-80°C,

P(CO,) = 10.38 atm.

McCoy, H.N.; "Equilibrium in the system composed of sodium Kk, near 25°C, 2d ioniz.,

carbonate, sodium bicarbonate, carbon dioxide, and water"; in NaHC03 /Na2C03 sol. Amer. Chem. J.; 29, 437-462, (1903)

Mehrbach, C; Culberson, C.H.; Hawley, J.E.; Pytkowicz, Kk, 2-35°C, 1 atm., in R.M. ; "Measurement of the apparent dissociation constants seawater.

of carbonic acid in sea water at atmospheric pressure";

Limnol. Oceanogr.; 18(6), 897-907, (1973); [CA

80: 112427c]

Meier, J.; Schwarzenbach , G. ; "Eine mit Glaselecktroden Kk, 20°C, formation of ausgerustete Stromungsapparatur (Uber die I^COg (kinetics and aciditatskonstante der wahren Kohlensaure und deren thermo).

Dehydratationsgeschwindigkeit" ; Helv. Chem. Acta; 40, 907-917, (1957)

Meissner, H.P.; Peppas , N.A.; "Activity coefficients,

aqueous solutions of polybasic acids and their salts" AIChEJ.; 19, 806-809, (1973)

Zc, Da, Pv, 25°C,

generalized activity

coefficient correlation

(to high ionic strengths).

Menzel, H.; "Uber Dissoziations- und Kk , 18°C, 1st ioniz.,

Hydrolysengleichgewichte in Losungen kohlensaurer und in dil. NaHC03 (aq).

borsaurer Salze"; Z. Phys . Chem.; 100, 276-315, (1922)

Metschl, J.; "The supersaturation of gases in water and Pv, 25°C?,

certain organic liquids"; J. Phys. Chem.; 28, 417-437, supersaturation.

(1924)

Michaelis, L.; Mizutani, M.; "Die Dissoziation der Kk, 20°C, 2d ioniz. Schwachen Elektrolyte in Wasserig-alkoholischen Losungen";

Z. Phys. Chem.; 116, 135-139, (1925) with EtOH

Michaelis, L.; Rona, P.; "Die Dissoziationskonstante der Kohlensaure"; Biochem. Z.; 67, 182-192, (1914)Kk, 16-37°C,

1st and 2d ioniz., in NaHC03 /Na2C03 /NaCl sol.
72MIL/BER: Millero, F.J.; Berner, R.A. ; "Effect of pressure on carbonate equilibria in seawater" ; Geochim. Cosmochim.

Acta; 36, 92-98, (1972)

Kk, Dm, 25°C, 1000 atm. calc. of partial molar volume from pressure

dependence

.

4 0MIL/URE : Mills, G.A. ; Urey, H.C.; "The kinetics of isotopic exchange Kk , 0 and 25°C, H

2

CC>

3

?, 18r between carbon dioxide, bicarbonate ion, carbonate ion and water"; J. Am. Chem. Soc . ; 62, 1019-1026, (1940)

0 exchange.

31MOR/MAA: Morgan, O.M.; Maass, 0.; "An investigation of the equilibria existing in gas-water systems forming

electrolytes"; Can. J. Res.; 5, 162-199, (1931)

Pv, Kk, 0-25°C, 5-80 mmHg, 1st ioniz.

30MOR/PYN : Morgan, J.L.R.; Pyne, H.R.; "Solubility relations in gas-liquid systems. I. A new apparatus for determining gas solubilities"; J. Phys . Chem.; 34, 1578-1582, (1930)Pv, 25°C, 1 atm?.

52MOR/BIL: Morrison, T.J.; Billett, F.; "The salting-out of non-electrolytes. Part II. The effect of variation in non-electrolyte"; J. Chem. Soc; 3819-3822, (1952)

Pv, 13-75°C, 1 atm.

67MUN: Munjal, P. K. ; "Solubility of carbon dioxide in sea water

and its concentrates"; Diss. Abstr. B; 27, 3952-3953,

(1967) sea water

Pv, 5-25°C, p = 10-45 atm. p = 10-45 atm

and concentrates.

7 1MUN/STE : Munjal, P.; Stewart, P.B.; "Correlation equation for solubility of carbon dioxide in water, seawater, and seawater concentrates"; J. Chem. Eng. Data; 16(2),

170-172, (1971)

Zc, Pv, -5 to 25°C, 1-45

atm., in H^O, seawater

and its concentrates.

71MUR/RIL: Murray, C. N . ; Riley, J. P.; "Solubility of gases in distilled water and sea water. IV. carbon dioxide";

Deep-Sea Res . ; 18, 533-541, (1971)

acidified seawater, and brines to 3.8% CI .

7 1MUX

Muxart, T.S.; "Solubility of calcite in water in the presence of carbon dioxide"; Mezhdunar. Geokhim. Kongr

.

(Dokl] 1st; 4(Part 1), 326-337 (1971); [CA 80-100687]

Kk, 20 and 30°C, 2d ioniz., in sat. CaCOj(aq),

7 7MYS: Mysen, B.O.; "The solubility of water and carbon dioxide

under predicted magma genesis conditions and some petrological and geophysical implications"; Rev. Geophys

.

Space Phys.; 15, 351-361, (1977)

Zr, Pv, t to 1600°C, p to 40 kbar, solubility

in silicate melts.

22
70NAK: Nakayama, F.S.; "Sodium bicarbonate and carbonate ion pairs

and their relation to the estimation of the first and second dissociation constants of carbonic acid"; J. Phys

Chem. ; 74(13), 2726-2728, (1970)

Zc, Kk, 25 °C, C02 and ion pairs in NaHC03 (aq) and Na2CO-3 ( aq) .

7 1NAK

Nakayama F.S.; "Thermodynamic functions for the dissociation of NaHC03

°, NaC03 ~, HCO3"";

H2C0 3 and HC03 ~"; J. Inorg. Nucl. Chem.;

33, 1287-1291, (1971)

Kk, 0-50°C, ion pairing

in Na2C03 (aq) and NaHC03 (aq)

4 6NAS

Nasanen, R.; "Die zweite Dissoziationskonstante der Kohlensaure in NaCl- und KCl-Losungen" ; Suomen Kemistilehti; 19B, 90-93, (1946)

Kk, 25°C, I<2m, 2d ioniz., in NaCl(aq)

4 7NAS:

61NAS/MER:

74NAU/KHA

68NEZ

58NIL/REN

Nasanen, R. ; "Potentiometric study on the first ionization

of carbonic acid in aqueous solutions of sodium chloride"; Acta Chem. Scand.; 1, 204-209, (1947)

Nasanen, R.; Merilainen, P.; Leppanen, K. ; "Potentiometric

Determination of the solubility product of lead carbonate"; Acta Chem. Scand.; 15, 913-918, (1961)

Naumov, V. B.; Khakimov, A. Kh.; Khodakovsky, I.L.; "On the solubility of carbon dioxide in concentrated chloride

solutions at high temperatures and pressures"; Geokhimiya;

No. 1, 45-55, (1974)

Nezdoiminoga, N. A.; "On the question of the solubility of carbon dioxide in water"; Izv. Akad. Nauk Arm. SSR; Ser. Tekh. Nauk., 21, No. 3, 11-17, (1968)

Nilsson, G.; Rengemo, T.; Sillen, L.G.; "Some solution

equilibria involving calcium sulfite and carbonate I. Simple solublity equilibria of CO2 , SO2

Acta Chem. Scand.; 12, 868-872,

Kk, 5-45°C, 1st ioniz. m(NaCl) = 0-3.

Kk, 25°C, 2d ioniz.

in 2m KNO3-

Zr, Pv, Kk, 100-500', C, 600-2500 bar.

Pv, 24°C, 0. 1-5 atm.

carbonate solutions.

Pv, 25, 35 and 75°C, in NaC104 (aq)

(1958)

61NOV/FRINovak, J.; Fried, V.; Pick, J.; "Loslichkeit des Kohlendioxyds in Wasser bei verschiedenen Drucken und temperaturen" ; Collection Czech. Chem. Communs . ; 26, 2266-2270, (1961)Pv, 10-80°C, 100-760 mmHg

23
70OND/SAD : Onda, K.; Sada, E.; Kobayashi ,' T .

; Kito, S.; Ito, K. ; Pv, 25°C, 1 atm. , in aq "Salting-out parameters of gas solubility in aqueous salt salt sol. solutions"; J. Chem. Jap.; 3(1), 18-24, (1970); [CA 73:39198c]

360RC/SEE: Orcutt, F.S.; Seevers, M.H.; "A method for determining the Pv, 25°C, 1 atm., in H

20 solubility of gases in pure liquids or solutions by the Van and org. solv. Slyke-Neill Manometric Apparatus"; J. Biol. Chem.; 117, 501-507, (1936)

770ST: Ostrom, B.; "Solubility of carbon dioxide total carbon dioxide content and primary production is sea water. Relations and formulas for calculations"; Botanica Marina;

20(2), 69-74, (1977)

Pv, -2 to 30°C,

reanalysis of data of 45BUC for solubility of C0o in seawater.

680SU/SAT: Osugi , J.; Sato, M. ; Fujii, T .

; "Pressure- jump study on the Kk , 25°C, H

2CO kinetics of reactions in ionic solutions"; Nippon Kagaku

Zasshi; 89(6), 562-565, (1968)

69PAR/KEV: Parkinson, W.J.; deNevers, N .

; "Partial molal volume of carbon dioxide in water solutions"; Ind. Eng. Chem. Fund.

8, 709-713, (1969)

V, 0-40, P(C02

) = 15-500 psia

.

31 PAS

:

Passauer, H.; "Neue gasanalytische Sperrflussigkeiten"

;

Feuerungsteck; 19, 142, (1931)

Pv, 20°C, in water and

sat. salt sol.

82PAT/SLO: Patterson, C.S.; Slocum, G.H.; Busey, R.H.; Mesmer, R.E.; Kk, t = 50 - 300°C, "Carbonate equilibria in hydrothermal systems: first p = psat to psat + 70 bar ionization of carbonic acid in NaCl media to 300°C"; Geochim. Cosmochim. Acta 46, 1653-1663, (1982)

74PER/SAN: Perez, J. F.; Sandall, 0. C; "Carbon dioxide solubility in aqueous carbopol solutions at 24°, 30°, and 35°C";

J. Chem. Eng. Data; 19(1), 51-53, (1974)

Pv,24-350C, in H

20

and carboxy polymethylene

56PIN/PEA: Pinsent, B.R.W.; Pearson, L.j Roughton, F.J.W.; "The Kk, 0-40°C, H 2C03 Kinetics of combination of carbon dioxide with hydroxide (kinetics),

ions"; Trans. Faraday Soc; 52, 1512-1520, (1956)

24
49PIN/ROU: Pinsent, B.R.W.; Roughton, F.J.W.; Abs . 1st Internal Congr. Kk , 0-38°C, 2d ioniz. Biochem. , Cambridge, England; (1949). # (from 64SIL/MAR)

.

37PIT:

82PLU/BUS:

Pitzer, K.S.; "The heats of ionization of water, ammonium

hydroxide, carbonic, phosphoric, and sulfuric acids. The variation of ionization constants with temperature and the entropy change with ionization"; J. Am. Chem. Soc . ; 59, 2365-2371, (1937)

PLummer, L.N.; Busenberg, E.; "The solubilities of calcite,

aragonite, and vaterite in C02 -H20 solutions

between 0 and 90 °C, and an evaluation of the aqueous model for the system CaC0g-C02 -H20" ; Geochim.

Cosmochim. Acta; 46, 1011-1040, (1982)

Zc, Kk, Hr, 1st ioniz . , 0-60°C

.

Zr, Pv, Kk, 0-250°C,

1st and 2d ioniz., 1 atm. to 100°C, p(H2

0, sat) above 100 °C, evaluation of data.

77POC/BJO: Pocker, Y . ; Bjorkquist, D.W.; "Stoped-flow studies of carbon dioxide hydration and bicarbonate dehydration in

and D2O. Acid-base and metal ion catalysis";

J. Am. Chem. Soc; 99(20), 6537-6543, (1977)

Kk, 25°C, 1st ioniz.

in H20 and D 20, from kinetic data.

67PON: Ponnamperuma , F. N.; "A theoretical study of aqueous carbonate equilibria"; Soil Sci.; 103, 90-110, (1967)

Zc , Px, 25 C, influence of p(C02

) on pH and solubilities of carbonates and hydroxides

.

78POS/PED: Postigo, M. A.; Pedrosa, G. ; Katz, M. ; "New experimental

method for determining gas solubility in liquids"; Ann. Asoc. Quim. Argent.; 66, No. 1, 25-30, (1978)

Pv, Hm, 15-55°C, 25°C, Bunsen coefficients in

10 to 60 wt% sucrose.

45PRU/SAV: Prutton, C.F.; Savage, R.L.; "The solubility of carbon dioxide in calcium chloride-water solutions at 75, 100, 120° and high pressures"; J. Am. Chem. Soc.; 67, 1550-1554, (1945)

Pv, 75-120°C, 16-694

1895PRY/HOL: Prytz, K. ; Hoist, H. ; "Die Absorptionscoeff icienten der Kohlensaure und des Schwefelwasserstoffs in Wasser bei

dessen Gefrierpunkt" ; Ann. der Phys . ; 290, 130-138, (1895)

Pv, 0°C, 1 atm.

16PUS

:

Pusch, L.; "Uber die Zeitreaktion bei der Neutralisation

der Kohlensaure und die wahre Dissoziationskonstante der Kohlensaure"; Zeit. Elektrochemie ; 22, 206-212, (1916)

Kk, t = ?, H

2C03 (kinetics and thermo).

25
16PUS2:

74PYT/HAW:

7 5REA:

Pusch, L.; "Nachtrag zu meiner Arbeit: Uber die

Zeitreaktion bei der Neutralisation der Kohlensaure und die wahre Dissoziationskonstante de Kohlensaure"; Zeit. Elektrochemie; 22, 293, (1916)

Kk,

Pytkowicz, R.M.; Hawley, J.E.; "Bicarbonate and carbonate

ion-pairs and a model of seawater at 25°C"; Limnol.

Oceanog.; 19(2), 223-234, (1974)

Read, A.J.; "The first ionization constant of carbonic acid from 25 to 250°C and to 2000 bar"; J. Solution Chem.;

4(1), 53-70, (1975)

Kk, 25°C,

1 atm. in seawater.

V, Kk, 25-250°C, 1st ioniz.

H2C0 3

, 1-2000 bar.

11RIL: Riley, 0.; J. Inst. Brewing; 17, 124, (1911). # Pv, see 58LIN for table of data.

59ROB/STO: Robinson, R.A.; Stokes, R.H.; Butterworths , London; 'Electrolyte solutions'; second edition (1959)

Ze, Kk , Da, summary

of useful data.

68ROB/ZIM:

4 1ROU

63RYZ:

28SAA

Robb, R.A. ; Zimmer, M.F.; "Solubility and heat of solution

of carbon dioxide in aqueous solutions of arsenous oxide,

arsenic pentoxide, and hydrochloric acid. Standard state correction for the combustion calorimetry of organochlorine

compounds"; J. Chem. Eng. Data; 13, 200-203, (1968)

Roughton, F.J.W.; "The kinetics and rapid thermochemistry

of carbonic acid"; J. Am. Chem. Soc . ; 63, 2930-2934,

(1941)

Ryzhenko, B.N.; "Determination of dissociation constants of carbonic acid and calculation of degree of hydrolysis of

the C0

3 2- and HCq3

" ions in solutions of carbonate and bicarbonate at elevated temperatures";

Geokhimiya; 137-148, (1963); [CA 58 : 10785g

Pv, 20-30°C, 1 atm. , in water, HCl(aq), arsenite

and arsenate solutions.

Kk, 100-300 C, 1st and 2d ioniz.

Saal, R.N.J. ; "The velocity of ionic reactions"; Rec . Trav. Kk , 14°C, H2CO3

Chim. Pays Bas . ; 47, 264-285, (1928) (kinetics and thermo),

74SAD/KIT: Sada, E . ; Kito, S.; Ito, Y. ; "Solubilities of gases in aqueous solutions of weak acids"; J. Chem. Eng. Jap.; 7,

No. 1, 57-59, (1974)

Pv, 25°C, [acid] to 5 molar, solubility in phosphoric and five organic acids.

26
69SAL/HAK:

69SAL/VES

Salomaa, P.; Hakala, R.; Vesala, S.; Aalto, T.; "Solvent

deuterium isotope effects on acid-base reactions III. Relative acidity constants of inorganic oxyacids in light

and heavy water. Kinetic applications"; Acta Chem. Scand.;

23, 2116-2126, (1969)

Salomaa, P.; Vesala, A.; Vesala, S.; "Solvent deuterium

isotope effects on acid-base reactions. Part II. Variation

of the first and second acidity constants of carbonic and sulfurous acids in mixtures of light and heavy water"; Acta

Chem. Scand.; 23, 2107-2115, (1969)

Kk, 25°C, 2d ioniz.

Pv, Kk, 25°C, 1st and 2d ioniz., in B^O mixt.

58SCH/BRO: Scheurer, P.G.; Brownell, R.M.; DuValle, J.E.; "An apparatus for the investigation of rapid reactions . The kinetics of the carbonic acid dehydration"; J.Phys. Chem.

62, 809-812, (1958)

Kk, 17-37°C, H

2C03 (kinetics and thermo).

55SCH: Schmitt, C.j "Contribution a 1' etude du system chaux- carbonate et de calcium bicarbonate de calcium-acid

carbonic-eau ' ; These Renne; Ser. B; 12 (1955)

Kk, 0-100°C, literature

review ( from75LIN/BOR)

73SCH: Schroder, W. ; "Untersuchungen uber die

temperaturabhangigkeit der Gasloslichkeit in Wasser" Chemie- Ing. Tech.; 45, 603-608, (1973)

Zc, Pv, 50-300°C, 120-2000 atm.

28SCH/BER: Schwab, G.-M.; Berninger, E.; "Invasion und Solvatation von

gasen in Wasser"; Z. Phys . Chem.; A138, 55-74, (1928)

Pv, 20- °C? .

62SEG/H0L: Segnit, E.R.; Holland, H.D.; Biscardi, C.J.; "The solubility of calcite in aqueous solutions - I The solubility of calcite in water between 75 and 200 at CO2 pressures up to 60 atm"; Geochim. Cosmochim. Acta;

26, 1301-1331, (1962)

Pv, 75-200°C, 2-60 atm. in sat. CaCOj(aq).

17SEY/LLO: Seyler, C.A.; Lloyd, P.V.; "Studies of the carbonates. Kk , 25°C, 1st and 2d ioniz. Part II. Hydrolysis of sodium carbonate and bicarbonate and Na2C0g/NaHC0g sol. the ionisation constants of carbonic acid"; J. Chem. Soc .

111, 138-158, (1917)

17SEY/LL02: Seyler, C.A.; Lloyd, P.V.; "Studies of the carbonates.

Part III. Lithium, calcium, and magnesium carbonates"; J. Chem. Soc; 111, 994-1001, (1917)

Pv, 25°C, in LiHC03 sol.

27
57SHC/DEV: Shchennikova , M.K. ; Devyatykh, G.G. ; Korshunov, I. A.; Pv, 20-75°C, in "Determination of the solubility of carbon dioxide in R^SO^taq). aqueous solutions of sulfuric acid by the isotopic dilution

method"; J. Appl . Chem. USSR; 30, 881-886, (1957); Tr. of Zh. Prikl. Khim. , 30, 833-838, (1957)

35SHE/MAC: Shedlovsky, T.; Maclnnes, D.A.; constant of carbonic acid, 0 to measurements"; J. Am. Chem. Soc

"The first ionization Kk , Hr, 0-38°C,

38, from conductance 1st ioniz.

; 57, 1705-1710, (1935)

36SHO/FER: Showalter, H.A.; Ferguson, J.B.; "The solubility of carbon Pv, 15°C, P < 1 atm. dioxide in aqueous solutions containing alcohols and sugars"; Can. J. Res.; B14, 120-126, (1936)

62SIE: Siesjo, B.K.; "Solubility of carbon dioxide in cerebral cortical tissues of cats. With a note on the solubility of carbon dioxide in water, 0 . 16M NaCl, and cerebrospinal

fluid"; Acta Physiol. Scand.; 55, 325-341, (1962) [CA

58: 11750f

solutions, acid, spinal

fluid, tissue.

64SIL/MAR: Sillen, L.G.; Martell, A.E.; 'Stability constants of metal-ion complexes. Section I. Inorganic ligands', The Chemical Society (London); 215-216, (1964); Special

Publication No. 17#

Ze, Kk, 0-200°C, 1st and 2d ioniz. compiled data, see for early references.

71SIL/MAR: Sillen, L.G.; Martell, A.E.; 'Stability constants of metal-ion complexes. Supplement No 1', The Chemical

Society (London); (1971); Special Publication No. 25#

Kk, 20-350"C,

compiled data.

58SIR: Sirs, J. A.; "Electrometr ic stopped flow measurements of rapid reactions in solution Part 2. Glass electrode pH Measurements"; Trans. Faraday Soc; 54, 207-212, (1958)

Kk, 0-30°C, H 2C0 3 (kinetics )

76SMI/MAR: Smith, R.M.; Martell, A.E.; 'Critical stability constants'; Ze , Kk ,

r H , A r S 25°C,

4, 37, (1976) 1=0, 0.5 and 1.0, 2d ioniz., evaluated data.

84SON/KOB: Song, K.Y.; Kobayashi , R. ; Marsh, W. ; "The water content Pv, Px, 0-77"?, of CC^Tich fluids in equilibrium with liquid water p to 2000 psia.

or hydrate"; 'Research Report RR-80'; Gas Producers

Assoc., Tulsa, OK, (1984)

28
28STA/HAW

70STE/MUN

Stadie, W.C.; Hawes, E.R.; "Studies on the oxygen-, acid-, and base-combining properties of blood III. The validity of hydrogen ion activity determinations by the hydrogen

electrode in systems containing carbonic acid, carbonates,

hemoglobin, carbon monoxide hemoglobin, and methemoglobin"

J. Biol. Chem.; 77, 2*1-301, (1928)

Stewart, P. B.; Munjal, P.; "solubility of carbon dioxide

in pure water, synthetic sea water, and synthetic sea water

concentrates at -5° to 25°C. and 10- to 45-atm. pressure"; J. Chem. Eng. Data; 15(1), 67-71, (1970)

Kk, 38°C, 1st ioniz. very dil. solutions.

Pv, -5 to 25°C, 10-45 atm, in H

2

0, sea water and its concentrates

16STR: Strohecker, E.R.; "Contributions to the knowledge of aqueous solutions of carbon dioxide"; Z. Nahr . -Genus sm .

31, 121-160, (1916); [CA 10:1826]

Kk, 4°C (and 18 C?),

H

2C03

.

75SZE/ADA: Sze, Y.K.; Adams, W.A.; Davis, A.R.; "A laser Raman study

of clathrate and aqueous solutions of carbon dioxide";

'Chemistry and Physics of Aqueous Gas Solutions',

Adams, W.A. (editor); The Electrochemical Society,

Princeton, (1975)

Kk, hydrate formation

from Raman spectra,

12-18°C, 0.04-1.76 kbar.

64TAK/KEN: Takesonchi, S.; Kennedy, G.C.; "The binary system

H2O-CO2 at high temperatures and pressures";

Am. J. Sci.; 262, 1055-1074 (1964)

Pv, Px, 110-350°C, p to 3000 bars

62TAN: Tans, A.M. P.; "Solubility of carbon dioxide in water"; Ind. Chemist; 38, 411 (1962); [CA -14485 d]

Pv, t=? , nomogram

55TAY: Taylor, C.E.; "Thermodynamics of sodium carbonate in solution"; J. Phys . Chem.; 59, 653-657, (1955)

Kk, Pv, Da, 15-95"C,

0. 1-2. 5m in Na 2C03

14THI/STR: Thiel, A.; Strohecker, E.R.; "Dynamics of the time

reactions between carbonic acid and bases"; Ber.; 47, 1061-1068, (1914); [CA 8:2293]

Kk, 4°C, H

2C03 (kinetics )

82TOD: Todheide, K. ; "Hydrothermal solutions"; Ber. Bunsenges.

Phys. Chem.; 86, 1005-1016 (1982)

Zr: Pv, Px, Kk, Da, 0-1000°C, p to 800 bar,

in water and in NaCl solutions.

solutions

29
63TOD/FRA:

7 5TOK:

Todheide, K. ; Franck, E. V.; "Das Zweiphasengebiet und die

kritische Kurve in system Kohlendioxid-wasser bis zu Drucken von 3500 bar"; Z. Phys . Chem. ; 37, 387-401,

(1963)

Tokunaga, J.; "Solubilities of oxygen, nitrogen, and carbon dioxide in aqueous alcohol solutions"; J. Chem. Eng. Data; 20(1), 41-46, (1975)

Pv, Px, 50-350°C, p to 3500 bar, critical

phenomena

Pv, 10 and 20 °C, in H

20 and aq. EtOH.

10USH:

81VAN/HAA:

Usher, F.L.; "The influence of non-electrolytes on the solubility of carbon dioxide in water"; J. Chem. Soc . ; 97, 66-78, (1910)

Vanderzee, C.E.; Haas, N.C.; "Second cross virial

coefficients B-j^ for the gas mixture (carbon dioxide + water) from 300 to 1000 K"

J. Chem. Thermodyn.; 13, 203-211 ,(1981)

Pv, 20°C, in H

20 and aq. sol. of sugars, amides

and acids.

Ze, Da, t = 300 - 1000 K

p < 30MPa.

28VAN/SEN: Van Slyke, D.D.; Sendroy, J. Jr.; Hastings, A.B.; Neill,

J.M.; "Studies of gas and electrolyte equilibria in blood.

X. Solubility of carbon dioxide at 38° in water, salt solution, serum, and blood cells"; J. Biol. Chem.; 78, 765-799, (1928)

Pv, 38"C, approx. 2 atm., in H2O, various

salts and acids and in blood

77VES/SAL: Vesala, A.; Saloma, E.; "Determination of basicity

constants by potentiostatic titration"; Finn. Chem. Lett.

(6), 160-163, (1977)

Kk, 25°C, 2d ioniz.

in K2C03 (aq)

82WAG/EVA: Wagman, D.D.; Evans, W.H.; Parker, V.B.; Schumm, R.H.; Halow, I.; Bailey, S.M.; Churney, K.L.; Nuttall, R.L.; "The NBS Tables of chemical thermodynamic properties"; J. Phys. Chem. Ref. Data; 11, Supplement No 2 (1982)

Pv, Kk, 25°C. A

f

H, A£G, S, compiled

thermochemical data.

27WAL/BRA: Walker, A.C.; Bray, U.B.; Johnston, J.; "Equilibrium in solutions of alkali carbonates"; J. Am. Chem. Soc.; 49, 1235-1256, (1927)

Pv, Da, Kk, 25 and 37°C, 1st ioniz., in bicarbonate

and chloride sol.

00WAL/COR: Walker, J.; Cormack , W.; "The dissociation constants of very weak acids"; J. Chem. Soc; 77, 5-21, (1900)

Kk, 18°C, 1st. ioniz. const

22WAR: Warburg, E.J.; "Studies on carbonic acid compounds and hydrogen ion activities in blood and salt solutions";

Biochem. J.; 16, 153, (1922)

Kk, 16-20°C, in NaCl

sol

30
80WAS/BUL: Wasmund, R. ; Bultmann, H.; "Carbon dioxide adsorption in Pv, 0-60°C, 1-9 bar. pure water and its dependence on pressure and temperature"; Monatsschr. Brau.; 33, pgs . 356, 358-360, (1980)

35WEI: Weider, 0.; "Determination of the second dissociation

constant of carbonic acid"; Ber.; 68B , 1423-1430, (1935);

Kk, 0, 18°C, 0.01-0. lm, 2d ioniz.

in NaCl/NaHC03 /Na 2CO3 sol.

74WEI: Weiss, R. F.; "Carbon dioxide in water and sea water- solubility of a nonideal gas"; Mar. Chem.; 2, 203-215,

(1974)

Pv, Zc, 6 to 20°C, -1 to

40 °C, [salt] = 0, 4%.

78WEN/RUP: Wenzel, H.; Rupp, W. ; "Calculation of phase equilibria in systems containing water and supercritical components";

Chem. Eng. Sci.; 33, 683-687, (1978)

Zc, Pv, Px, 298-573K,

p to 500 bar.

41WIE: Wiebe, R. ; "The Binary system carbon dioxide-water under

pressure"; Chem. Rev.; 29, 475-481, (1941)

Pv, 12-100°C, 1-700 atm.

39WIE/GAD: Wiebe, R. ; Gaddy, V.L.; "The solubility in water of Pv, 50-100°C,

carbon dioxide at 50, 75, and 100°, at pressures to 25-700 atm. 700 atmospheres"; J. Am. Chem. Soc . ; 61, 313-318 (1939)

40WIE/GAD: Wiebe, R. ; Gaddy, V. L .

; "The solubility of C02 in water at various temperatures from 12 to 40° and at pressures to 500 atmospheres"; J. Am. Chem. Soc.; 62, 815-817, (1940)

Pv, 12-40°C, 25-500 atm

41WIK/GAD: Wikbe, R. ; Gaddy, V.L.; "Vapor phase composition of carbon dioxide-water mixtures at various temperatures and

at pressures to 700 atmospheres"; J. Am. Chem. Soc; 63, 475-477 (1940)

Pv, 25-75°C,

1 to 700 atm.

21WIL: Wilke, E . ; "Zur Kenntnis wassriger Kohlensaurelosungen"

Anorg. Chem.; 119, 365-379, (1921)

Kk, 18-40°C, 1st ioniz., in water and alkali

metal chloride sol.

77WIL/BAT: Wilhelm, E.; Battino, R. ; Wilcock, R.J.; "Low-pressure

solubility of gases in liquid water"; Chem. Rev.; 77, 219-262, (1977)

Ze, Pv, 0-100°C, P=l

atm, methods, tables,

thermodynamic properties,

correlations and theory.

31
83WIL/BRA: Wilson, G.M.; Brady, C.J.; "Heats of mixing of steam with Hm, 780-1180 °F

,

N

2 , C02 , H2 , CH

A

, and CO at high 500-2500 psia,

temperatures and pressures using a new high temperature C02

(g) + H

20(g).

calorimeter"; 'Research Report RR-73'; Gas Producers Assoc.,

Tulsa, OK, (1983)

06WIN: Winkler, L.W.; "Gesetzmassigkeit bei der Absorption der Zr , Pv, 0-60°C, analysis Gase in Flussigkeiten" ; Z. Phys . Chem.; 55, 344, (1906) # of early meas. Data in 58LIN p. 1153.

54WIS/FRE: Wissbrun, K.F.; French, D.M.; Patterson, A. Jr.; "The true Kk , Hr , 5-45°C, H

2CO; ionization constant of carbonic acid in aqueous solution

from 5 to 45°C"; J. Phys. Chem.; 58, 693-695, (1954)

27WOL/KRA: Wolf, 0.; Krause; "Sperrflussigkeiten fur technisch

gasuntersuchen" ; Arch. Warmewirt; 8, 216-218, (1927) aq. acids and salts,

(data in 58LIN)

81WON/CHU: Won, Y.S.; Chung, D.K.; Mills, A.F.; "Density, viscosity, Pv, 25°C, in H

20, EtOH surface tension, and carbon dioxide solubility and and PrOH aq. sol. diffusivity of methanol, ethanol, aqueous propanol, and aqueous ethylene glycol at 25°C"; J. Chem. Eng. Data;

26, 140-141, (1981)

1882WRO: Wroblewksi, S.; "Sur les lois carbonique dans l'eau sous de Rend.; 94, 1355-1357, (1882)

de solubilite de l'acide Pv, 0-12°C, 1-30 atm. hautes pressions"; Compt

79YAS/TSU: Yasunishi, A.; Tsuji, M. ; Sada, E . ; "Solubility of carbon dioxide in aqueous mixed-salt solutions"; Adv. Chem. Ser.;

177, 189-203, (1979)

Pv, 25°C, p(C02

) = 1 atm. [salt] = 0.3 to 4 molar,

solubility in aqueous mixtures (binary and ternary) containing

halides and sulfates

79YAS/YOS: Yasunishi, A.; Yoshida, F.; "Solubility of carbon dioxide

in aqueous electrolyte solutions"; J. Chem. Eng. Data; 24(1), 11-14, (1979)

Pv, 15-35°C, 1 atm, sol. as fn . of salt cone,

in aq. chlorides,

nitrates and sulfates.

64YEH/PET: Yeh, S.-Y.; Peterson, R.E.; "Solubility of carbon dioxide,

krypton, and xenon in aqueous solution"; J. Pharm. Sci.;

53, 822-824, (1964)

Pv, 25-45°C, 1 atm. , in water, NaCl(aq) and phosphate buffer.

32
40ZAA: Zaalishvili , ; "Solubility of CO2 in mixtures with other

gases at 20, 30, 35 and 50°C"; Zhur. Fiz. Khim. ; 14, 413-417 (1940)

qPv, 20-50°C, in mixt.

with H£ and other gases.

81ZAW/MAL: Zawisza, A.; Malesinska, B.; "Solubility of carbon dioxide

in liquid water and of water in gaseous carbon dioxide in the range 0.2-5 MPa and at temperatures up to 473K"; J. Chem. Eng. Data; 26, 388-391, (1981)

Pv, 50-200°C, 0.2-5MPa.

39ZEL: Zelvenskii; Zh. Prikl. Khim.; 12, 1311-1329, (1939) Pv, 0-100°C, p<100 atm, (data in 58LIN)

.

39ZHA: Zhavoronkov, N.M.; "The partial pressure of ammonia, carbon dioxide and water over copper ammonium solutions"; J. Chem.

Ind.; 16(10), 36-37, (1939); [CA 34:2233 9]

Pv, 20-80°C, in copper- ammoni a ( aq) and formate solutions.

33
CuCl 2-H 2 0

Bert R. Staples, Thomas L. Jobe , Jr. , and David Garvin

INTRODUCTION

Listed in this bibliography are publications that

contain information on the equilibria that exist in aqueous

solutions of cupric chloride. The species present are Cu2+ (aq), CuCl+ (aq), CuCl 2 (aq) and CuCl 3

" (aq)

The position of the equilibrium is dependent upon the

CI" concentration and to a lesser extent the acidity and

total salt concentration.

The references listed here treat the stability

constants, solubilities, activity coefficients, enthalpies of

solution and dilution, heat capacities and thermochemistry of

the solids. The only vapor species of any importance above

the solutions is water; the measurement of its pressure is

considered in papers treating activity coefficients.

Publications reporting measurements or presenting

correlations/evaluations are included but publications that

consider only applications of existing data to specific

problems without providing new data have been avoided.

The references are listed alphabetically by first

author. Each citation is preceeded by a brief identification

code composed of the year of publication and three letters

from the last names of the first two authors. The citations

list the names of authors; the title of the article , chapter

or report as appropriate, and the source information, i.e.

journal or book title , volume , and year of publication. The

structure of these citations does not conform to the

specifications established by the American National Standards

Institute but is the information necessary to direct the

reader to a particular reference. In a few instances only an abstract or secondary reference was available. In these cases either the citation to Chemical Abstracts or source of

the secondary citation is given.

34
Some titles have been translated, e.g. those in

Russian. These translations come, by preference, from

abstracts in the papers themselves or from Chemical Abstracts.

(The titles from the latter may be condensations of the original)

Each paper has been annotated to show the class of data,

the temperature range and, if appropriate, pressure, solution

composition and pH. The data class designations are taken

from the Bulletin of Chemical Thermodynamics . They are two

letter codes with some mnemonic or physical chemical

associations. A list is appended. No attempt has been made

to assess the quality of the data, however, an annotation of

"Ze" indicates that a particular reference constitutes or includes an evaluation of experimental data from several

sources

The bibliography has been prepared by searching the

files of the NBS Chemical Thermodynamics Data Center, the

Bulletin of Chemical Thermodynamics and references in the

papers retrieved from those sources. It covers a time period

from the 19th century to 1982. Additions and corrections

will be welcomed.

35
75ADE/NWA: Adeosun, S.O.; Nwanze, V.O.; "Thermochemistry of dialkylamine complexes of Cu(II) halides"; J. Inorg. Nucl.

Chem. ; 37, 2091-2093 (1975)

Ql, dialkyamine

complexes of CuCl2 and other halides

28AGO: Agostini, P.; "Heats of formation of the double chlorides Hm, temp, given, 600 of copper and potassium"; Atti . Acad. Lincei.; 7, ^2^' 1030-1032 (1928)

71AND/CHA: Andreev, S.N.; Chaiko, A.I.; "Effect of the dielectric Kk , alcohol complexes, constant of the solvent on the stability of complexes"; me thru n-butyl.

Zh. Neorg. Khim.; 16, 1965-1967 (1971)

7 1AST/KRA : Astakhova, R.K. ; Krasikov, B.S.; "Electrochemical behavior Kk

of copper in chloride electrolytes"; Zh . Prikl. Khim.; 44, 363-371 (1971); [CA 74:150198]

60BAR/BET:

73BAR/PAN

Barton, P.B., Jr.; Bethke, P.M.; "Thermodynamic properties of Px, Kk, 25 to 75°C, some synthetic zinc and copper minerals"; Am. J. Sci.; Cu(OH) 2Cl2 in KC1

258A, 21-34 (1960) and HC1.

Barvinok, M.S.; Panin, A.V. ; Obozova, L.A.; "Compounds of pyridine with cobalt (II), copper (II), and zinc (II) chlorides"; Zh. Neorg. Khim.; 18, 1572-1575 (1973)

Kd, Hm, 25°C,

pyridine complexes.

73BEL/KON: Belousov, E.A.; Konstantinova, K.K.; Bocharov, V.V.; Kk , 25°C in tributyl

Alovyainikov , A. A.; Mironov, V.E.; "The composition and phosphate - HC1 mixt

stability of copper(II) and cobalt(II) chloride complexes

in hydrochloric acid solutions in tributyl phosphate";

Zh. Fiz. Khim.; 47, 1869-1871 (1973)

1873BER: Berthelot, M. ; "Recherches sur les sels metalliques et sur Hm, 18°C, 100-300

les ferriques en particulier " ; Ann. Chim. Phys . ; [4], 30, H

20. 145-204 (1873)

1879BER: Berthelot, M. ; "Sur le protochlorure de cuivre" ; Compt

rend. ; 89, 967-971 (1879)

Hr, 16.5°C, react. Ba02 + CuCl + HCl(aq)

BaCl 2 + CuCl2 (aq)

1880BER: Berthelot, M. ; "Recherches sur les sels basiques et sur

1' atakamite" ; Compt. rend.; 91, 450-453 (1880)

Hr, 15

0 C, with KOH

36
77BJE/SKI

:

Bjerrum, J.; Skibsted, L.H.; "A contribution to our knowledge of weak chloro complex formation by copper (II) in aqueous chloride solutions"; Acta Chem. Scand.; 31, 673-677 (1977)

Kk, 25°C, meas.

,

discussion of earlier

work

.

74BLO/RAZ: Blokhin, V.V. ; Razmyslova, L.I.; Shalaevskaya , M.I.; Makashev, Yu.A.; Mironov, V.E.; "Thermodynamics of copper (II) monochloride complexes in aqueous alcoholic

solutions"; Zh. Fiz. Khim. ; 48, 469-471 (1974)

Hr, Kk, 25°C, 0-80% ethanol or methanol, 1=3 NaClO.

50BOB/LAR: Bobtelsky, M. ; Larisch, R.D.; "The heat of solution of halides, sulphuric acid, oxalic acid, sodium hydroxide, and urea in ethyl alcohol-water mixtures"; J. Chem. Soc .

;

3612-3615 (1950)

Hm, 22.5°C, 307 H2

0, dihydrate

.

76CAR/WET: Carlsson, B.; Wettermark, G.; "Determination of the equilibrium constants and uv-absorption spectra for Cu2+-Cl"complexes in 1 M HC104 "; J. Inorg

.

Nucl. Chem.; 38, 1525-1527 (1976)

Kk, 25"C, 1 M perchloric acid, CI complexes

.

76CAR/WOO:

62D'A/CAL:

16DER/YNG:

1892DEV/STA:

Cartwright, M; Woolf, A. A. ; "Heats of formation of tin and titanium iodides"; J. Chem. Soc, Dalton Trans.; 829-833

(1976)

D'Amore, G. ; Calabro, G.; Curro, P.; "A study of solution

complexity by ion exchangers. I. Copper ( II ) -chloride

system"; Atti Soc. Peloritana Sci. Fis. Mat. Nat.; 8, 265-281 (1962)

Derby, I.H.; Yngve, V.; "The dissociation tensions of certain

hydrated chlorides and the vapor pressures of their

saturated solutions"; J. Am. Chem. Soc.; 38, 1439-1451

(1916)

van Deventer, CM.; van de Stadt, H.J.; "Over the relation

between solubility and heats of solution of salts"; Maandblad Natuurwetenschappen ; 17, 1-9 (1892)

Hr, 25°C.

Kk, 30°C, fctn of molality, Cu(II)

complexes

.

Pv, 26.6-64.5°C

and 17.9-64.2°C.

Hm, 18°C, 8

H 9 0.

40

76DOW/PIT: Downes , C.J.; Pitzer, K.S.; "Thermodynamics of electrolytes. Binary mixtures formed from aqueous NaCl, Na 2S04 , CuCl2 and CuSO^ at 25°C"; J. Solution Chem.;

5, 389-398 (1976)

Da, 25°C, osmotic

coef s . and activ. coefs

.

37
62FAU/CRE: Faucherre, J.; Crego, A.; "Determination cryoscopique de constantes de dissociation de complexes peu stables"; Bull.

Soc. Chim. Fr.; 1820-1824 (1962)

Kd, Kd for CuCl+

in KNO3

eutectic

.

1853FAV/SIL: Favre, P. -A.; Silbermann, J.-T.; "Recherches sur les quantites de chaleur degagees dans les actions chimiques et moleculaires" ; Ann. Chim. Phys . ; [3], 37, 406-508 (1853)

Hm, t = 11-13°C?,

sol. in acid.

37FED/SIL: Fedorov, A.S.; Sil'chenko, G.F.; "Heats of formation and solution of saturated aqueous solutions of some salts";

Ukr. Khem. Zh. ; 12, 53-60 (1937)

52FRI: Friedberg, S.A.; "The specific heat of CuCl2 .2H20 between 1.5 and 20°K"; Physica (Utrecht); 18, 714-722 (1952)Ql, 1.5 - 20°K, Cp.

70GED/PEA: Gedansky, L.M.; Pearce, P.J.; Hepler, L.G.; "Thermochemistry of copper compounds; Cu(OH)2, CuCl2

, Cu(I03

) 2

.H20 and Cu(I02

) 2

"; Can. J. Chem. ; 48, 1770-1773 (1970)

Hm, 25°C, 5 m.

79GOL:

72GRI/PHI:

58GUG/STO:

Goldberg, R.N.; "Evaluated activity and osmotic

coefficients for aqueous solutions: Bi-univalent compounds

of lead, copper, manganese, and uranium"; J. Phys. Chem.

Ref. Data; 8, 1005-1050 (1979)

Gritzner, G. ; Phillips, R.F.; "Densities, viscosities, and vapor pressures of copper(II) chloride solutions in hydrochloric acid"; J. Chem. Eng. Data.; 17, 425-428

(1972)

Guggenheim, E.A.; Stokes, R.H.; "Activity coefficients of

2:1 and 1:2 electrolytes in aqueous solution from isopiestic data"; Trans. Faraday Soc; 54, 1646-1649

(1958)

Ze, Da, 25°C.

Xd, Xv, 30-90°C, 4-7M HC1.

Da, 25°C, revision

of activ. coeffics.

4 9GUI: Guiter, H.; "The hydrolysis of the chloride nitrate, and Kk , t = ??, sulfate of copper"; Compt . rend.; 228, 569-570 (1949) CuClgOH2 "

( aq)

,

64HAM/GRE: Hammer, R.R.; Gregory, N.W.; "Vaporization reactions in the copper chloride-chlorine system"; J. Phys. Chem.; 68, 3229-3233 (1964)

Pp, 285 and 440°C, H and

S calculated, at 298"K.

38
46HER: Herrera, C.G.; "Fisico-quimica de las soluciones de cloruro cuprico"; An. Fis. Quim.

;

42, 165 (1946)

Kg, Kk, Xr, conductivity, room temp.

38HIE/FED: Hieber, W. ; Feder, E.E.; "Heats of formation of cupric and Hm, Kr, 20°C,

mercuric halogen compounds with amines"; Z. Elektrochem. ; sol in HCl(aq).

44, 881-887 (1938)

66HUA/PAN: Huang, J.-T.; Pan, K. ; "Osmotic and activity coefficients Da, Px, 0°C, of copper (II) chloride and cadmium chloride from freezing m < 0.1. point measurements"; J. Chin. Chem. Soc . (Taipei); 13, 64 (1966)

1891ISA: Isaachsen, D.; "Die Farbenanderung von Salzlosungen" ; Px, Pv, 0 and 100°C,

Z. Phys. Chem.; 8, 145 (1891) freezing and boiling

points , m < 0.4.

75KAK/GIE: Kakolowicz, W. ; Giera, E. ; "Heat of formation of chelate Hm, 25°C, 4.36M HC1,

complexes of some d-electron elements and metal-oxygen bond sol. energy"; Conf. Intern. Thermodyn. Chim. Quat.; 1, 73-79

(1975)

66KEN/LIS: Kennedy, M.B.; Lister, M.W. ; "Heats of association of Hr, 25 and 40°C, I = 2m aqueous copper, nickel, and cobalt ions with halide ions"; CuClO^(aq) +

Can. J. Chem.; 44, 1709-1716 (1966) NaCKaq).

59KEN: Kenttamaa, J. ; "A cryoscopic study of the dissociation of Px, Kk, 0°C, some bivalent metal chlorides in aqueous solutions complexation

.

saturated with electrolyte"; Suom. Kemistil. B.; 32B, 68-70 (1959)

76KHA/SCH: Khan, M.A. ; Schwing-Weill, M.J.; "Stability and electronic Kk, Md, t=? , I=5M,

spectra of the copper (II) chloro complexes in aqueous CI complexes,

solutions"; Inorg. Chem.; 15, 2202-2205 (1976)

72KIR/TRU: Kirintsev, A.N. ; Trushnikova, L.N.; Lavrent'eva, V.Q. ; Px, -40 to 120°C, 'Handbook of phase diagrams of inorganic substances in x=0 to .60, pg. 23. water'; Khimiya, Leningrad; (1972)

39
71KLY/GLE: Klygin, A.E. ; Glebov, V.A.; Lekae, V.A.; Kolyada, N.S.; Kk , 25°C?, complexes in Smirnova, I.D.; Nikol'skaya, N.A.; Zavrazhnova, D.M.; M(HC1) = 0-10 solns. "Complex formation by the ions of metals of the first

transition series in hydrochloric acid solutions"; Zh. Neorg. Khim. ; 16, 1590-1595 (1971)

69KOL: Kolonin, G.R. ; "Chloride complexes of ore-forming metals at Kk, 25 and 200°C,

high temperatures (calculated data)"; Eksp. Issled. complexation

.

Mineral.; 105-117 (1969-1970); [CA 77 ; 118904

]

76KON/FED: Koneva, T.N.; Fedorov, V.A.; "Influence of the ionic Kk , 25°C, in strength of the solution on the stabili

Zh. Neorg. Khim.; 21, 1132 -1135 (1976)

strength of the solution on the stability of CuCl (aq)"; 0.05 - 8M CIO. (aq)

72LEB/NIK: Lebedeva, A. P.; Nikolaev, V.P.; Frolov, Yu.G.; Vlasenko, Hm, Dx, mixing of CuCl2 (aq) K.K. ; Karapet'yants , M-. Kh. ; "Change in excess thermodynamic with LiCl(aq).

functions during mixing of the isopiestic solutions sodium

chloride-water + cobalt(II) chloride-water, rubidium

chloride-water + cobalt(II) chloride-water, and lithium

chloride-water + copper(II) chloride-water"; Tr. Mosk

.

Khim.-Tekhnol. Inst.; 71, 105-106 (1972); [CA

80: 100769}

73LIB: Libus, Z.; "Nature and stability of the CuCl+ complex Kk, 25°C, CI

in aqueous solution"; Inorg. Chem. ; 12, 2972-2977 (1973) complexes in perchlorate

media

.

58LIN: Linke, W.F.; 'Solubilities'; D. Van Nostrand, N.Y. ; 1, Px, 0-360°C, in H

20, Fourth Edition (1958) sol. of acids and aq. salts

.

60LIS/ROS: Lister, M.W. ; Rosenblum, P.; "Some equilibrium constants of Kk , 12,25,40°C, I = transition metal halides"; Can. J. Chem.; 38, 1827-1836 2.0m NaClO^ , Kl and K2

.

(1960)

7 1MAK/KUL : Makashev, Yu.A.; Kul'ba, F.Ya.; Agaf, M.I.; Volokhov, Kk, 15-50°C, NaCIO

Yu.A.; Mironov, V.E.; "Effect of ionic strength and media,

solution temperature on the formation of inner-sphere and outer-sphere copper(II) complexes"; Zh. Fiz. Khim.; 45, 734-735 (1971)

40
65MAN/IWA: Manahan, S.E.; Iwamoto, R.T.; "Chloro complexes of copper (II) and copper (I) in acetonitrile" ; Inorg. Chem.

4, 1409-1413 (1965)

Kk, 25°C,

complexation

.

1876MAR:

69MAV/MIR:

Marignac, C; "Sur les chaleurs specifiques des solutions

salines"; Ann. Chim. Phys . ; 8, 410-430 (1876)

Mavrina, I.V.; Mironov, V.E. ; Makashev, Yu.A.; "Inner sphere and outer sphere complexes of copper (II)"; Uch. Zap., Leningrad Gos . Pedagog. Inst. im. A. I. Gertsena;

385, 153-157 (1969);- [CA 75:122861]

Ql, 19-51°C, 10-200

H2O, specific heats.

Kk, 25°C, aq solns. of LiX mixtures

.

50MCC/DAV: McConnell, H. ; Davidson, N. ; "Optical interaction between

the chloro-complexes of copper (I) and copper (II) in solutions of unit ionic strength"; J. Am. Chem. Soc . ; 72, 3168-3173 (1950)

Kk, 25 and 47°C,

complexation K's.

74MIH: Mihailov, M.H.; "A correlation between the overall stability Kk, theory, stepwise constants of metal complexes.- I. Calculation of the complex formation,

stability constants using the formation function n" ; J. Inorg. Nucl. Chem.; 36, 107-113 (1974)

68MIR/MAK: Mironov, V.E.; Makashev, Yu.A.; Mavrina, I.Ya.; Kk, 25°C, in Markhaeva, D.M.; "Determination of stability constants 3 . 0M LiClO^ and LiCl. of inner-sphere and outer-sphere complex compounds";

Zh. Fiz. Khim. ; 42, 2987-2989 (1968)

69MIR/MAK: Mironov, V.E.; Makashev, Yu.A.; Mavrina, I.Ya.; Kk, 25°C, in 3 . 0M "Inner-sphere and outer-sphere complexes of copper (II)";

Zh. Nerog. Khim.; 14, 1424-1425 (1969)

70MIR/MAK : Mironov, V.E. ; Makashev, Yu.A.; Mavrina, I.Ya.; Kk, 25°C,

Kryzhanovskii , M.M. ; "Outer-sphere and inner-sphere I = 3m, complexation.

complexes of cobalt(II), and nickel(II), and copper(II)";

Zh. Neorg. Khim.; 15, 1301-1304 (1970)

51M0N: Monk, C.B.; "Electrolytes in solutions of amino acids. Kk, 25°C, Part II. The cupric complexes of glycine, alanine, and CuCl+

. glycyl-glycine" ; Trans. Faraday Soc; 47, 285-291 (1951)

41
62MOR/SHO: Morris, D.F.C.; Short, E.L.; "Stability Constants of Kk , 20°C, I = 0.691m Copper(II) Complexes"; J. Chem. Soc . ; 2672-2675 (1962) HCIO^, stability

constants of CI complexes

50NAS: Nasanen, R.; "Complex formation in dilute aqueous solutions Kk, 25°C, in of cupric chloride, spectrophotometric determination of HCl(aq).

equilibrium involving slight complex for formation in electrolytic solution"; Acta Chem. Scand.; 4, 140-145

(1950)

51NAS/LUM: Nasanen, R. ; Lumme , P.; "Potentiometric studies on the Kk , 25°C, NaClO^ and equilibria of some copper ( II ) -hydroxysalts in aqueous salt NaCl solns

solutions, and involved complex formation"; Acta Chem. Scand.; 5, 13-22 (1951)

49NAS/TAM: Nasanen, R. ; Tamminen, V.; "The equilibria of cupric Px, Kk , 25°C,

hydroxysalts in mixed aqueous solutions of cupric alkali CuCOHJoCl in KC1. salts at 25°C"; J. Am. Chem. Soc; 71, 1994-1998 (1949)

770IK/GEO: Oikova, T.; Georgiev, G. ; "The CuCl2 -MnCl2 -H20 system at 25°C"; Zh. Neorg. Khim. ; 22, 3147-3151 (c/aq).

(1977)

29PAR/SOP: Partington, J.R.; Soper, W.E.; "The heats of solution Hm, 25"C, 0-10. 049m, of some salts in water and ethyl alcohol solutions"; Philos. H soln and diln. Mag. ; 7, 209-247 (1929)

1890REI/DEV: Reicher, L. T.j Van Deventer, C. M. ; "Uber einige Hm, 11°C, heat of eigentumlichkeiten von kupferchloridlosungen in thermischer soln etc. hinsicht"; Z. phys . Chem. (Leipzig); 5, 559-565 (1890)

74RIC/BRO: Richardson, D.W.; Brown, R.R. ; "Enthalpy of formation of Hm, 25°C, formation

malachite [Cu2 (C0 3

) (OH

)

2

] " ; U.S. Bur. Mines. and soln for malachite

Rept. Invest.; 7851, 5pp. (1974) (Cu 2 (C03

) (0H) 2

.

40ROB/STO: Robinson, R.A.; Stokes, R.H.; "Part VI . The activity Da, Pv , 25°C, 0.1 to coefficients of manganese, cobalt, nickel and copper 2.769m, isopiestic meas

chloride in aqueous solution at 25°"; Trans. Faraday

Soc. ; 36, 1137-1138 (1940)

59ROB/STO: Robinson, R.A.; Stokes, R.H.; 'Electrolyte Solutions'; Ze , Pv, Da, 25°C,

Butterworths , London; Second Edition, (1959) 0.1-6.0m.

42
34ROT/BUC: Roth, W.A. ; Biichner, A.; "The heats of ionization of

some metals"; Z. Elektrochem. ; 40, 87-89 (1934)

Hm, 20°C, 999-3640

76RUD/YAG: Rud'ko, P.K.; Yaglova, V.N.; Novikova, G.I.; "Thermal

dehydration of copper (II) chloride dihydrate"; Zh. Fiz. Khim. ; 50, 2988 (1976)

Hr, 20-300°C, vap

press, measured also.

1889SAB: Sabatier, P. ; "Sur les chlorures metalliques hydrates'

Bull. Soc. Chim. Fr. ; [3], 1, 88-91 (1889)

Hm, 20°C, sol. in

73SCH: Schwing-Weill, M.J.; "Copper(II) chloride complexes in aqueous solutions"; Bull. Soc. Chim. Fr.; [3], 1, 823-830 (1973); [CA 79:58291]

Kk, 25°C, CI = .005

- 4.9 M, I NaCl, pH = 2, succesive

form, of mononucl. complexes

.

54SHC/ORA: Shchukarev, S.A.; Oranskaya, M.A. ; "Thermal stability of copper halides"; Zh. Obshch. Khim.; 24, 1926-1935

(1954)

Kd, 219-495°C, meas. pressure C^Cg), mp +436°C.

27SIE/GOT: Sieverts, A.; Gotta, A.; "Heat of formation of copper hydride"; Justus Liebigs Ann. Chem. ; 453, 289-297 (1927)

Hr, 23.5°C, reduction

of cupric to cuprous.

64SIL/MAR:

76SMI/MAR:

56SMI/TIK:

Sillen, L.G.; Martell, A.E.; 'Stability constants of metalion complexes'; Chemical Soc, London; Special Publ.

No. 17, (1964)

Smith, R.M.; Martell, A.E.; 'Critical Stability Constants.

Vol. 4: Inorganic complexes'; Plenum Press, N.Y. ; (1976)

Smirnov, V.I.; Tikhonov, A.I.; "Concerning the equilibrium

reactions of chlorides of cobalt, nickel and copper with

oxygen"; Izvest. Akad. Nauk SSSR, Otdel. Tekh. Nauk; 9, 48-54 (1956)

Kk, -3 to 75°C,

compiled data.

Kk, 25°C, I = 0-1 m, crit. evaluation.

Kk, 300-450°C,

CuCl2 /CuO,Cu2Cl2 /CuO.

48STO: Stokes, R.H.; "A thermodynamic study of bivalent metal

halides in aqueous solution. Part XVII - Revision of data

for all 2:1 and 1:2 electrolytes at 25°, and discussion

of results"; Trans. Faraday Soc; 44, 295-307 (1948)

Da, 0.1 - 6m, activ. coef f

.

43
70SZA/PAL: Szabo, Z.G. ; Palfalvi-Rozsahegyl, M. ; Burger, K.

;

"Hydration of metal ions"; Proc . Symp. Coord. Chem. 3rd.

1, 99-110 (1970)

Hm, t=?, CuCl2 (aq) +

(HC1 + LiCl2 (aq) )

.

74VAS/KAR: Vasilev, V.A.; Karapet'yants , M.Kh. ; Sanaev, E.S.; Novikov, Ql, 25°C, Cp solns

.

S.N.; "Heat capacities of copper(II) chloride solutions at 25°C"; Zh. Fiz. Khim. ; 48, 2360-2362 (1974)

76VAS/SAN: Vasilev, V.A.; Sanaev, E.S.; Karapet'yants, M.Kh.; "The Ql, 25°C, mixtures

heat capacities of mixed aqueous solutions containing of CuCl2 with

chlorides of d transition metals in the fourth period";

Zh. Fiz. Khim.; 50, 1128-1131 (1976)

66VDO/KOL: Vdovenko , V.M. ; Kolokol' tsov, V.B.; Stebunov, O.B.; Kk, 25°C?, complexation

.

"Resonance processes in complex formation"; Radiokhimiya;

8, 286-290 (1966)

76VIL/DEM: Vilcu, R.; De Madrinan, E.C.; I-Lnei, F.; "Thermodynamic Da, activ. coeff. in properties of electrolyte solutions. V. Differential mixtures with NaCl or KC1. cryoscopy in sodium chloride + copper (II) chloride

+ water and potassium chloride + copper (II) chloride + water ternary systems and in associated

binaries"; Rev. Roum. Chim. ; 21, 333-341 (1976); [CA

85: 131441]

71VLA/KAR: Vlasenko, K.K. ; Karapet'yants, M.Kh.; "Thermodynamic

properties of mixed electrolyte solutions. IX. Temperature variation of the heats of mixing of aqueous

lithium, sodium, and cesium chlorides with copper(II)

chloride solutions"; Zh. Fiz. Khim.; 45, 2460-2463

(1971)

Hm, 0, 25, 40°C, heat

of mixing with isomolal Cs

,

Li or Na chloride solns.

30WAR/WER: von Wartenberg, H.; Werth, H.; "The heats of formation of Hr , temp, not given, cuprous and cupric chloride"; Z. Physik. Chem.; 151A; formation of CuCLo from 109-112 (1930) elements.

53YAT/KHA: Yatsimirskii , K.B.; Kharitonov, V.V. ; "On the Hm, 25°C, in 6.24m thermochemistry of anthranylates" ; Zh. Fiz. Khim.; 27, HC1. 799-804 (1953)

44
H

2 S0 4 -H 2 0

Bert R. Staples, Theresa F. Wobbeking, Rebecca Joseph,

Abby Brier and David Garvin

INTRODUCTION

Listed in this bibliography are publications that report

data on equlibria in mixtures of sulfuric acid and water and

on the associated vapor- liquid equilibria and solubilities

(at low temperature) as shown in phase diagrams. To a lesser

extent there are data on enthalpies of mixing, on activity

coefficients and on the thermochemistry of the system.

Sulfuric acid is a dibasic acid in solutions below 0.01

dissociating into 2H+ and SO^ -. Above 1 molal it

is a monobasic strong acid, forming H+ and HSO4". At

the sulfuric acid rich side of the phase diagram, molecular

species predominate. Several crystaline hydrates have been

studied at low temperatures.

References reporting measurements or presenting the

results of correlations and evaluations have been included.

Publications that consider only applications of existing data

to specific problems without providing new data have been

avoided. References concerning mixtures with organic

substances have also been excluded.

The citations are listed alphabetically according to

first author. Each is prceeded by a brief identification

code composed of the year of publication and three letters

from the last names of the first two authors. The citations

list, in order, the names of authors; the title of the

article, chapter or report as appropriate; and the source

information, i.e. journal or book title .volume , and year of

publication. The structure of these citations does not

conform to the specifications established by the American

National Standards Institute but the information given is

that necessary to direct the reader to a particular

reference. In a few instances only an abstract or secondary

reference was available. In these cases either the citation

to Chemical Abstracts or to the secondary reference is given.

45
Some titles have been translated, e.g. those in

Russian. These translations come, by preference, from

abstracts in the papers themselves or from Chemical

Abstracts. ( The titles from the latter may be condensations

of the originals.)

Each publication has been annotated to show the class of

data, the temperature range and, if appropriate, pressure,

solution composition and pH. The data class designations are taken from the Bulletin of Chemical Thermodynamics. They are

two letter codes with some mnemonic or physical chemical

associations. A list is appended. No attempt has been

made to assess the quality of the data, however, an annotation

of "Ze" indicates that a particular reference constitutes or includes an evaluation of experimental data from several sources

.

The bibliography has been prepared by searching the

files of the NBS Chemical Thermodynamics Data Center, the Bulletin

of Chemical Thermodynamics, and references in the papers

retrieved from those sources. It covers a time period from

the 19th century to 1982. Additions and corrections will be

welcomed.

46
46ABE: Abel, E.; "The Vapor Phase Above the System Sulfuric

Acid-Water"; J. Phys . Chem. ; 50, 260 (1946)

Zr, Pv, vapor pressures, m = 2.5 to 90.

26AGD/HOL: Agde, G. ; Holtmann, H. ; "Die Spezifischen Warmen der Ql, 25-45°C. Systeme Schwefelsaure-Wasser , Eisenvitrol-Wasser

,

Schwefelsaure-Eisenvitrol-Wasser" ; Z. Anorg. Allgem.

Chem. ; 158, 317 (1926)

69ADH/GAN: Adhikari, M. ; Ganguli , D.; Biswas, G. ; Ghosh, D . ; Ke, 25 and 30°C,

"Determination of the Second Dissocation Constant of H2SO4 m = .001-. 005, clay

from Measurements of E.M.F. Across Cation Exchange membranes.

Membrane"; J. Ind. Chem. Soc . ; 46, 1131 (1969)

26AKE : Akerlof, G. ; "Investigations of Sulfate Solutions. Ke, t = ?, m = .01-3.6. Experimental Methods and Results on Cells Without Liquid

Junction"; J. Am. Chem. Soc; 48, 1160 (1926)

62AUS/MAI: Austin, J.M.; Mair, R.D.; "The Standard Enthalpy of Hm, m = .007. Formation of Complex Sulfate Ions in Water. I., HS0^~,

LiSOi", NaS04 ~"; J. Phys. Chem.; 66, 519 (1962)

60BAS/GIL: Bass, S.J.; Gillespie, R.J.; Oubridge, J.V. ; "Solutions in Da, Pt, t = 0, MHSO^ and Sulphuric Acid. Part XXVIII. Osmotic Coefficients of Some org. bases. Electrolyte Solutions"; J. Chem. Soc; 837 (1960)

60BEC/DOB : Beck, W.H. ; Dobson, J.V. ; Wynne-Jones, W.F.K. ; "The Ke, 5-55°C, m= 0.1-8. Potentials of the Mercurous Sulphate/Mercury Electrode";

Trans Faraday Soc; 56, 1172 (1960)

59BEC/SIN: Beck, W.H. ; Singh, K.P.; Wynne- Jones, W.F.K. ; "The Ke, 5-55°C, m= 0.1-8. Behaviour of the Lead Dioxide Electrode. Part 6. The Potentials of the Lead Dioxide/Lead Sulphate Electrode";

Trans Faraday Soc; 55, 331 (1959)

34BEC/ROT: Becker, G. ; Roth, W.A. ; "Zur Bestimming der Zr, Hm, 20°C, 10000 H

2

0. Verbrennungswarme von Organischen Schwefelverbundungen"

Z. Phys. Chem.; A169, 287 (1934)

09BED: Bedford, T.G.; "The Depression of Freezing Point in very Pt, t = 0, m = 0.0005-001. Dilute Aqueous Solutions"; Proc . Roy. Soc. London; 83A, 454 (1909)

47
19BER/HAR: Berkeley, R . [8th earl]; Hartley, E.G.J. ; Burton, C.V. "On Osmotic Pressures Derived from Vapour-Pressure

Measurements: Aqueous Solutions of Cane Sugar and

and Methyl Glucoside"; Philos. Trans. Royal Soc

London; 218, 295 (1919)

Po, Pv, 0 and 30°C.

1873BER: Berthelot, M. ; "Parallels between the Formation of Solid Hr, 18°C?, Salts [of] Picric, Hydrochloric, Nitric, Sulfuric, Acetic neutralization,

and Benzoic Acids"; Ann. Chim. Phys . ; *(4)29, 328 (1873)

1873BER2: Berthelot, M. ; "On Anhydrous Potassium Bisulfate and

on the Heat of Solution of Anhydrous Sulfuric Acid"; Ann. Chim. Phys.; *(4)30, 433 (1873)

Hm, 18°C?

1874BER: Berthelot, M. ; "On the Crystalline Hydrates of Sulfuric

Acid"; Compt. Rend.; 78, 716 (1874)

Hm, 12°C, sol of hydrates

1875BER: Berthelot, M. ; "Refrigeration Mixtures"; Ann. Chim.

Phys. ; *(5)4, 47 (1875)

Hm, t < 0°C, H

20(cr) and hydrates of ^SO^ .

1875BER2: Berthelot, M. ; "On the Heat of Combination as Carried to the Solid State. New Expressions of the Reactions"; Ann. Chim. Phys.; *(5)4, 74-104 (1875)

Hm, 10-15'C, in 50 to

sulfates

1875BER3: Berthelot, M. ; "On the Crystalline Hydrates of Sulfuric

Acid"; Ann. Chim. Phys.; *(5)4, 154 (1875)

Hm, 12°C, sol of hydrates, same as 1874BER.

1875BER4

Berthelot, M. ; "Solution of Acids and Bases"; Ann. Chim.

Phys. ; *(5)4, 445 (1875)

Hm, 18°C?, dilution.

1878BER: Berthelot, M. ; "Some of the Fundamental Laws of Thermochemistry"; Ann. Chim. Phys.; 13, 5 (1878)

He, t = ?

1878BER2: Berthelot, M. ; "New Remarks on the Heat Release by the Reaction of Water with Sulfuric Acid in Great Excess";

Ann. Chim. Phys.; *(5)14, 443 (1878)

Hm, 20°C, in 70 H

2

0.

1898BER: Berthelot, M.; "On the Heat Released by the Reaction of Small Quantities of Water with Sulfuric Acid Used in Considerable Excess"; Ann. Chim. Phys.; '"(7)13, 77 (1898)

Hm, 22°C, 1-4 H

20.

48
60BEW: Bewley, D.K. ; "Heat of Reaction Between Ferrous Ammonium

Sulphate and Hydrogen Peroxide in Aqueous Solution" ; Trans

.

Faraday Soc; 56, 1629-1632 (1960)

Hm, Ql(?),

25°C(?), dilution.

22BIC: Bichowsky, F.R.; "Equilibrium in the Reaction Between

Sulfur Dioxide and Water"; J. Am. Chem. Soc; 44, 116 (1922)

Kk, t = 530-615K,

S(1)+H2S04.

1899BIN: Binon, E.; "Heat Capacities of Water Solutions of Sulfuric

Acid"; Russkue-Fiziko Khim. Obsh., Petr . ; 31, 171 (1899)

Ql, m = 0-400 waters

.

1889BOD: Bode, F. ; "Specific Heat of Sulfuric Acid"; Z. Angew.

Chem.; 2, 244 (1889)

Ql, 15°C, 5-400 waters.

05BOS:

52BRA/RUT

:

03BRI:

10BRO:

4 5BRO:

04BUR:

Bose, E.; "Observations on Julius Thomsen's Measurements of

the Heat of Mixing of Acids"; Phys . Z. ; 6, 550 (1905)

Brand, J. CD.; Rutherford, A.; "The Vapour Pressure of the System Sulphuric Acid-Disulphuric Acid"; J. Chem. Soc;

3916 (1952)

Briggs, E.; "The Vapour Pressures of Concentrated Solutions

of Sulphuric Acid at High Temperatures"; J. Soc. Chem.

Ind. ; 22, 1275 (1903)

Bronsted, J.N. ; "Studies on Chemical Affinity III. Mixing Affinity of Binary Systems. The Sulfuric Acid-Water

System"; Z. Phys. Chem. (Leipzig); 68, 693 (1910)

Broughton, D.B.; Chem.; "Sulphuric Acid and Oleum Enthalpy

Chart"; Chem. Met. Eng.; 52(4), 123 (1945)

Burt, B.C.; "The Vapour Pressure of Sulphuric Acid

Solutions and the Molecular Condition of Sulphuric Acid in Concentrated Solution"; J. Chem. Soc; 85, 1339 (1904)

Hm, t = 18°C, 1-1600 waters

.

Pv, 20-80°C, 50-63 mol%

S03 or SO^

.

Pv, t = 100-200°C.

Hm, Vx, t = 18°C?

Hm, 17°C, 0-100/2 H

2S0^

.

Pv, 55-105°C, vp of sol 55-235°C and for cone. 24.92-95.94% H2S0A

.

72CAB/GIA: Cabani , S.; Gianni, P.; "Analysis of Some Calorimetric Data Kk, review of Concerning the Formation of Bisulfate Ion in Aqueous equilibria.

Solution"; Anal. Chem.; 44, 253 (1972)

49
1889CAT: Cattaneo, C . ; "Sulla Caloricita Specifica delle Soluzioni

Acquose dell'acido Solforico"; Nuovo Cimento; 26, 50 (1889)

Ql, 5-22°C.

33COL: Collins, E.M.; "The Partial Pressures of Water in Equilibrium with Aqueous Solutions of Sulfuric Acid";

J. Phys. Chem.; 37, 1191 (1933)

65COV/DOB: Covington, A.K.; Dobson; J.V.; Wynne- Jones, W.F.K.; Ke, Da, m = 0.007-0.1. "Stoichiometric Activity Coefficients of Sulphuric Acid and t = 25°C. the Standard Potentials of the Lead Dioxide/Lead Sulphate

and Mercury/Mercurous Sulphate Electrodes at 25°C"; Trans. Faraday Soc . ; 61, 2050 (1965)

34COW/SHR: Cowperthwaite , I. A.; Shrawder, J. Jr.; "The Partial Molal Ke, 0-50°C. Heat of Dilution of Sulphuric Acid from Electromotive Force Measurements"; J. Am. Chem. Soc; 56, 2345 (1934)

40CRA/VIN: Craig, D.N.; Vinal, G.W. ; "Thermodynamic Properties of Ze , Ql, Hm, Ke, 20 and Sulphuric-Acid Solutions and their Relation to the 25°C. Electromotive Force and Heat of Reaction of the Lead

Storage Battery"; J. Res. Nat. Bur. Stand.; A24, 475

(1940)

62D ' A/FRE : D'Ans, J.; Freund, W.E.; Woelk, N.H.; Px, -60 to 40°C,

"Losungsgleichgewichte von festen und flussigen x(H2S0^) =0 to 1. Stoffen in Flussikeiten" ; ' Landolt-Bornstein Tabellen'

Auflage 6, Band II, Teil 2b, p. 3-11 (1962)

23DAU : Daudt, W. ; "Eine Differentialmethode zur Messung Pv, -40 to -10°C, vp for kleiner Drucke mittels der Warmeleitung" ; Z. phys. Chem.; 20-60 mol/kg.

106, 255 (1923)

52DAV/J0N: Davies C.W.; Jones, H.W.; Monk C.B.; "E.M.F. Studies of Ke, 0-50°C. Electrolytic Dissociation. I. Sulphuric Acid in Water"; Trans Faraday Soc; 48, 921 (1952)

33DAW: Dawson, H.M.; "The Ionisation of Sulphuric Acid";

Proc. Leeds Phil. Lit. Soc; 2, 359 (1933)

Kk, 25°C, m = 0.001-0.1,

k determined from rates

of hydrolysis of ethyl acetate

50
54DEN/TAF: Deno, N.C.; Taft, R.W. , Jr.; "Concentrated Sulfuric

Acid-Water"; J. Am. Chem. Soc . ; 76, 244 (1954)

Da, 25"C, 83-99.8%

H

2

SC>4 , act . of H

20 and acidity function.

1893DIE: Dieterici, C. ; "Uber die Dampfdrucke wasseriger Losungen

bei 0

o C"; Ann. Phys . ; 286, 47 (1893)

Pv, 0°C, m(H2S04

) to 11.

1897DIE:

1899DIE:

11DRU:

20DRU:

34DRU:

68DUI/GIA:

Dieterici, C; "Uber die Dampfdrucke verdunnter wasseriger

Losungen bei 0°C"; Ann. Phys.; 298, 616 (1897)

Dieterici, C. ; "Uber die Dampfdrucke verdunnter wasseriger

Losungen bei 0°C"; Ann. Phys.; 303, 859 (1899)

Drucker, K. ; "Das Dissoziationsschema der Schwefelsaure und

die Beweglichkeit des Hydrosulfations" ; Z. Electrochem.

17, 398 (1911)

Drucker, C; "Weitere Untersuchungen uber die Dissoziation

ternarer Elektrolyte" ; Z. Phys. Chem.; 96, 381-427 (1920)

Drucker, C; "Salzeffecte in concentrirten Losungen. Die

Veranderung der LOsungswarme von Kaliumchlorid durch andere Elektrolyte"; Ark. Kemi, Mineral. Geol. ; 11A, 1-27 (1934)

Duisman, J. A. ; Giauque W.F.; "Thermodynamics of the Lead

Storage Cell. The Heat Capacity and Entropy of Lead Dioxide

from 15 to 318K"; J. Phys. Chem.; 72, 562 (1968)

Pv, 0°C, m(H2S0

4

) to

0.4.

Pv, 0°C, m(H2S0

4

) to

0.5.

Kk, Da, 0-25°C, m = (H2S04

) < 0.1.

Ke, 18°C, ioniz. from emf data.

Ql, 18°C, but

mostly about Cp

for KC1 in H2S0A (aq).

Ke, 0-60 °C, EMF' s from Third Law.

64DUN/NAN: Dunsmore, H.S.; Nancollas, G.H. ; "Dissociation of the Bisulfate Ion"; J. Phys. Chem.; 68, 1579 (1964)

Zr, Kk, 25°C.

65EDW/WAN: Edward, J.T. ; Wang, I.C.; "Ultraviolet Study of the Ionization of Bisulfate Ion"; Can. J. Chem.; 43, 2867

(1965)

Mm, m = 0 .010 to 0.30.

55EIC/RAB: Eichler, E.; Rabideau, S.; "The Determination of the Bisulfate Dissociation Quotient from Potentiometric

Measurements"; J. Am. Chem. Soc.; 77, 5501 (1955)

Ke, Zr, t = ? bisulfate

dissociation in aq. perchlorate, m = 0.01-1.

51
7 1EVA/M0N

Evans, C.E.; Monk, C.B.; "E.M.F. Studies of Electrolytic

Dissociation"; Trans Faraday Soc . ; 67, 2652 (1971)

Ke, 25 C, I = 0.006 to 0.06.

1853FAV/SIL: Favre, P. A. ; Silbermann, J.T.; "Recherches sur les Quantites de Chaleur Degagees dans les Actions

Chimiques et Moleculaires Troisieme Partie";

Ann. Chim. Phys . ; (3), 37, 4 (1853)

Hm,

74FEI/FUC: Feilchenfeld , H . ; Fuchs, J.; "Hydration Numbers of Some Acids and Salts"; Israel J. Chem.; 12, 899 (1974)

Kk, hydration at 25°C.

21FER/FRA:

61FLI

Ferguson, A.L.; France, G.F.; "The Transference Numbers of Sulfuric Acid by the Concentration Cell Method"; J. Am. Chem.

Soc. ; A3, 2150-2160 (1921)

Flis, I.E.; "Energies of the Process of Formation of Ions

9_ _ SO^ and HSO^ in Aqueous Solutions at Various

Temperatures"; Zh. Prikl. Khim. ; 34, 1744 (1961)

Ke, 25°C.

Ke, 10-15°C, enthalpy of bisulfate ion.

58FLI/MIS: Flis, I.E.; Mishchenko, K.P.; Pakhomova, N.V. ; "The Thermochemistry of Dissociation of Sulphuric and Hypochlorous Acids in Aqueous Solution"; Russ. J. Inorg. Chem. ; 3, 1772 (1958)

Hr, 10-15°C,

neutralization

1884FOR:

50GAB/BET:

69GAR/JEK:

de Forcrand, R. ; "Sur les Sulfites et Bisulfites de Soude' Ann. Chim. Phys.; (6), 3, 242 (1884)

Gable, CM.; Betz , H.F.; Maron, S.H.; "Phase Equilibria of the System Sulfur Trioxide-Water" ; J. Am. Chem. Soc; 72, 1445 (1950)

Gardner, W.L.; Jekel, E.C.; Cobble, J. W. ; "The Thermodynamic Properties of High-Temperature Aqueous

Solutions. IX. The Standard Partial Molal Heat Capacities

of Sodium Sulfate and Sulphuric Acid from 0 to 100°"; J. Phys. Chem.; 73, 2017 (1969)

Hm, 10°C.

Pt, 1.5-93.7% S02

, freezing points from -35

to +35°C.

Dm, Cp by integral heat

method.

69GAR/MIT

Gardner, W.L.; Mitchell, R.E.; Cobble, J.W.; "The Thermodynamic Properties of High-Temperature Aqueous

Solutions. X. The Electrode Potentials of Sulphate Ion Electrodes from 0 to 100. Activity Coefficients and the Entropy of Aqueous Sulfuric Acid"; J. Phys. Chem.; 73, 2021 (1969)

Da, 0-100"C, third law method to calculate act

and cone (0.1 to 4.0 mol/kg)

52
60GIA/HOR: Giauque, W.F.; Hornung, E.W.; Kunzler, J. E.; Rubin, T.R.; Hm, 15-300K.

"The Thermodynamic Properties of Aqueous Sulfuric Acid

Solutions and Hydrates from 15 to 300K"; J. Am. Chem. Soc; 82, 62 (1960)

56GIA/KUN: Giauque, W.F.; Kunzler, J.E.; Hornung, E.W.; "The Freezing Px, 0-2 H

2

0, Point Method of Determining Free Energies in a 2-Component freezing points = 0.2 to System Forming Compounds. Concentrated Aqueous Sulphuric -80°C. Acid"; J. Am. Chem. Soc; 78, 5482 (1956)

81GIA/WUS: Giazitzoglou, Z. ; Wuster, G. ; "Das binare System H2S0 A Pv, 450 - 823 K, H

2

0; p,v,T-Daten und Dampfdruckkurven in weiten 1-50 bar, cone. = 20-98 Konzentrationsbereichen bei erhohtem Druck"; Ber . Bun. Phys . mole percent H2SO4

Chem.; 85, 127-132 (1981)

50GIL: Gillespie, R.J.; "Cryoscopic Measurements in Sulphuric Px, aq. ammonium

Acid. Part IV. Reactions of Ionised Sulphates in Sulphuric sulfate and bisulfate in Oleum. Self-ionisation Equilibria in Sulphuric Acid, and sulfuric acid. Ionic Equilibria in Oleum. The Polysulphuric Acids"; J. Chem. Soc. ; 2516 (1950)

50GIL/HUG: Gillespie, R. J. ; Hughes, E.D.; IngoldC.K.; "Cryoscopic Hp, Px. Measurements in Sulphuric Acid. Part I. Principles and Methods. The Cryoscopic Constant and Some Other Constants

of Sulphuric Acid"; J. Chem. Soc; 2473 (1950)

56GLU/KIT: Glueckauf, E.; Kitt, G.P. ; "Thermodynamic Data on Da, bithermal isopiestic

Concentrated Sulphuric Acid Solutions"; Trans Faraday Soc; method, m = 20-65.

52, 1074 (1956)

7 7GOL/STA: Goldberg, R.N.; Staples, B.R.; Nuttall, R.L.; Arbuckle, R.; Zr , bibliog. of activity

Nat. Bur. Stand. (U.S.) Spec. Pub.; 'A Bibliography of data for sulfuric acid Sources of Experimental Data Leading to Activity or Osmotic and other aq. systems.

Coefficients for Polyvalent Electrolytes in Aqueous

Solution'; No. 485, 49 pp. (1977)

60GOO/LAC: Good, W.D.; Lacina, J.L.; McCullough, J. P.; "Sulfuric Acid He, heat of formation of Heat of Formation of Aqueous Solutions by Rotating-bomb

Calorimetry" ; J. Am. Chem. Soc; 82, 5589 (1960)

73GOP/RAO: Gopinath C .R. ; Rao, K.S.R.; "Thermodynamic Properties of Md, Zr , 100-1000K, set Some Molecules of XO7Y2 an(* X02YZ Types"; Curr. Sci.; 42, of thermo. properties.

164 (1973)

53
1843GRA: Graham, T.; "Experiments on the Heat Disengaged in Combinations"; Philos. Mag.; 22, 329 (1843)

Hm, t = ?

25GRE: Greenewalt, C. H.; "Partial Pressure of Water Out of Aqueous Solutions of Sulfuric Acid"; Ind. End. Chem. ; 17, 522 (1925)Zr, Zc, 0-100°C, vp of water over 0-95% sulfuric acid.

3 1GR0

Groenier, W.L.; "The Heats of Dilution of Sulphuric Acid

Solutions"; Thesis, Univ. Chicago; (1931)

Hm, about 25°C, m = 0.003

to 4.0.

25GRO/FRA:

58GUG/STO:

Grollman, A.; Frazer, J.C.W.; "The Vapor-Pressure Lowering

of Aqueous Sulfuric Acid Solutions at 25°C"; J. Am. Chem.

Soc. ; 47, 712 (1925)

Guggenheim, E.A. ; Stokes, R.H. ; "Activity Coefficients of 2:1 and 1:2 Electrolytes in Aqueous Solution from Isopiestic Data"; Trans Faraday Soc; 54, 1646 (1958)

Pv, 25°C, m = 0.1 to 3.

Zc, Da, 25°C, m = 0.1.

65GUN: Gunn, S.R.; "Comparison Standards for Solution

Calorimetry"; J. Phys . Chem.; 69, 2902 (1965)

Hr, 25°C, reaction with

NaOH.

12HAC:

63HAL:

Hacker, C; "Uber die Anderung der Dampfspannung von wasserigen Schwefelsaurelosungen mit der Temperatur"; Ann. Phys . ; 275, 1342 (1912)

Hala, E. ; "Liquid-Vapour Equilibrium in Systems of Electrolytic Components. I. Excess Free-Energy of Dilution

and the Mean Rational Activity Coefficients of Ions"; Coll. Czech. Chem. Communications; 28, 1780 (1963)

Pv, 0-100°C, m = 2.9 to

9.2.

Zc, 308-330°C, S03 +H2 0.

35HAM: Hamer, W. J.; "The Potential of the Lead Dioxide-Lead

Sulfate Electrode at Various Temperatures"; J. Am. Chem.

Soc. ; 57, 9 (1935)

Px, 0-60°C, m = 0.005 to

7 .

3 5HAM2

Hamer, W.J.; "Temperature Variation in Transference Numbers

of Concentrated Solutions of Sulfuric Acid as Determined by

the Galvanic Cell Method"; J. Am. Chem. Soc; 57, 662

(1935)

Ke, 0-60°C, m = 0.05 to

17 .

33HAM/DEY: Hammett, L.P.; Deyrup, A.J.; "Some Properties of Electrolytes in the Solvent Sulfuric Acid"; J. Am. Chem.

Soc. ; 55, 1900 (1933)

Pt, fp of sulfuric acid, m - 0.1 to 0.4.

54
35HAR/HAM: Harned, H. S.; Hamer, W. J.; "The Thermodynamics of Aqueous

Sulfuric Acid Solutions from Electromotive Force Measurements"; J. Am. Chem. Soc . ; 57, 27 (1935)

Ke, 0-60°C, m = 0.05 to

17.5.

25HAR/STU: Harned, H.S.; Sturgis, R.D.; "The Free Energy of Sulfuric Ke, 25°C, m = 0.01 and Acid in Aqueous Sulfate Solutions"; J. Am. Chem. Soc.; 47, 0.1. 945 (1925)

15HAR: Hartung, E. J.; "A New Method for Determining the Specific

Heats of Liquids"; Trans. Faraday Soc; 11, 64 (1915)

Ql, Q, 17 to 20°C.

02HAU: Hausrath, H. ; "Eine Differentialmethode zur Bestimmung

kleiner Gefrierpunktsdepressionen" ; Ann. Phys .

;

314, 522 (1902)

Kk, Hp, t < 0°C, m = 0.0001 to 0.02.

76HEL/KIR: Helgeson, H.C.; Kirkham, D.H.; "Theoretical prediction of Kk, Zc , Ze, the thermodynamic properties of aqueous electrolytes at 25-300 °C, high pressures and temperatures. III. Equation of state 1-1000 atm. for aqueous species at infinite dilution"; Am. J. Sci.;

276, 97-240 (1976)

81HEL/KIR: Helgeson, H.C.; Kirkham, D.H.; Flowers, G.C.; "Theoretical Ze, Kk, Da, Dm, prediction of the thermodynamic behavior of aqueous 0-600 °C, 0-5kB. electrolytes at high pressures and temperatures : IV. Calculation of activity coefficients, osmotic coefficients,

and apparent molal and standard and relative partial molal

properties to 600°C and 5kB" ; Am. J. Sci.; 281, 1249-1516

(1981)

1886HEL: Helmholtz, R. ; "Untersuchungen uber Dampfe und Nebel, Pv, 0-50°C, in 10, 17, besonders uber solche von Losungen" ; Ann. Phys.;

263, 508 (1886)

41HER: Herrmann, C.V.; "Heat of Formation of Oleums from Sulfur

Trioxide and Water"; Ind. Eng. Chem.; 33, 898 (1941)

Zc, Hm, 18°C, diln. and soln

.

28HEP: Hepburn, J. R. I.; "The Vapour Pressure of Water over Sulphuric Acid-Water Mixtures at 25°C, and its Measurements by an Improved Dew-Point Apparatus"; Proc

.

Phys. Soc. London; 40, 24 9 (1928)

Hv, m = 7 to 12.5, dew

point method.

55
62HOG: Hogfeldt, E.; "On the Dissociation of Strong Acids. Comments on the Paper: ' Konzentrierte wassrige

Losungen, II'"; Z. Phys . Chem. ; 35, 260 (1962)

Kk, 25°C?, cone, sol, comment on 62KAN.

56HOR/BRA: Hornung, E. W. ; Brackett, I.E.; Giauque, W.F.; "The Low Ql, 15-320K,

Temperature Heat Capacity and Entropy of Sulfuric Acid f^SO^ : 6 . 5H2O

.

Hemihexahydrate . Some Observations on Sulfuric Acid

Octahydrate" ; J. Am. Chem. Soc . ; 78, 5747 (1956)

55HOR/GIA: Hornung, E.W.; Giauque, W. F.; "The Vapour Pressure of Hv, 23 to 70°C, m = 14-28. Water over Aqueous Sulfuric Acid at 25 " ; J. Am. Chem.

Soc . ; 77, 2744 (1955)

55HOR/GIA2: Hornung, E.W.; Giauque, W.F.; "The Heat Capacities and Ql,,Hp, 15-300K, props. Entropies of Sulfuric Acid Tri- and Tetrahydrates" ; J. Am. of hydrates.

Chem. Soc; 77, 2983 (1955)

69IZA/EAT: Izatt, R. M. ; Eatough, D.; Christensen, J. J.; Bartholomew, Kk, Ke, thermo . prop.

C. H.; "Calorimetrically Determined Log K, H, and S Values from titrations at 25° C. for the Interaction of Sulphate Ion with H+, Na+, and K+

in the Presence of Tetra-n-alkyl-ammonium Ions"; J. Chem. Soc; 1, 45 (1969)

63 JOH/SUN : Johnson, W. H.; Sunner, S.; "The Heats of Solution and Hm, 25°C, in 2500 H

2

0. Oxidation of Sulfur Dioxide"; Acta Chem. Scand. ; 17, 1917

(1963)

1893JON: Jones, H.C. ; "Uber die Bestimmung des Gefrierpunktes von Px, m = 0.001 to 0.1. verdunnten Losungen einiger Sauren, Alkalien, Salz und organischen Verbindungen" ; Z. Phys. Chem. (Leipzig); 12, 623 (1893)

51J0N: Jones, F.R.; "An Accurate Method for the Determination of Pv, absorption method to Aqueous Vapour Pressure: The Equilibrium Humidities of calc . vp, m = 0.5 to 55. Solutions of Sulphuric Acid"; J. Appl. Chem.; 1, S144

(1951)

02JON/GET: Jones, H.C. ; Getman, F.H.; "The Lowering of the Freezing- Px, m = 0.1 to 2.8. point of Water Produced by Concentrated Solutions of Certain Electrolytes, and the Conductivity of Such Solutions"; Am. Chem. J.; 27, 433 (1902)

56
04 JON/GET: Jones, H.C.; Getman, F.H.; "On the Nature of Concentrated

Solutions of Electrolytes-Hydrates in Solution"; Am. Chem.

J. ; 31, 303 (1904)

Px, m = 0.1-2.5, K(diss) at

0°C.

04JON/GET2: Jones, H.C. ; Getman, F.H. ; "A Study of the Molecular Px, m = 0.5-2.5. Lowering of the Freezing-point of Water Produced by

Concentrated Solutions of Electrolytes"; Phys . Rev.; 18, 146 (1904)

07 JON/GET : Jones, H.C. ; Getman, F.H.; Basset, H.P.; McMaster, L.; Px, m = 0.1 to 6.4,

Uhler, H.S.; "Hydrates in Aqueous Solutions. Evidence freezing point lowering

for the Existence of Hydrates in Solution, their and conductivity.

Approximate Composition, and Certain Spectroscopic

Investigations Bearing Upon the Hydrate Problem"; Carnegie Institution of Washington, Publication No. 60, (1907)

07 JON/PEA: Jones, H.C; Pearce, J.N.; "Dissociation as Measured by Kk, Px, fp, m = 0.01-2.0. Freezing Point Lowering and by Conductivity-Bearing on the Hydrate Theory. The Approximate Composition of the Hydrate

Formed by a Number of Electrolytes"; Am. Chem. J.; 38, 683 (1907)

62KAN: Kangro, W. ; "Konzentrierte wassrige Losungen. II"; Z. Phys. Chem.; 32, 273 (1962)

Kk, 25°C, interp. of part, press . , see 62HOG.

24KAR: Karve, D.D.; "Thermo-chemical Investigations on the Constitution of Acids in Solution"; J. Indian Chem. Soc.

1-2, 247 (1924-25)

Hm, 0-40°C.

57KEN: Kenttamaa, J.; "The Solubility of Silver Sulphate and the Kk, 25°C, from Dissociation of the Bisulphate Ion"; Suomen Kemi . ; 30B, 9 solubility of Ag2S0^ in (1957) acid.

57KER: Kerker, M. ; "The Ionization of Sulfuric Acid"; J. Am. Chem. Kk, m = 0-1.80. Soc; 79, 3664 (1957)

58KIR/WYA: Kirkbride, B. J.; Wyatt, P.A.H.; "The Partial Molar Heat Hm, 25°C. Contents of Solutes in Sulphuric Acid at 25°C. An

Investigation of the Self-Dissociation of Sulphuric Acid"; Trans Faraday Soc; 54, 4 (1958)

57
72KIR/TRU: Kirintsev, A.N. ; Trushnikova, L.N. ; Lavrent'eva, V.G. ; Px, -62 to 8°C, 'Handbook of Phase Diagrams of Inorganic Substances in water'; x = 0 to 1

Khimiya, Leningrad, 105-106 (1972)

42KLO/ECK

01KNI:

Klotz, I.M.; Eckert, C.F.; "The Apparent Molal Volumes of Aqueous Solutions of Sulfuric Acid at 25°C"; J. Am. Chem.

Soc. ; 64, 1878 (1942)

Knietsch, R. ; "Ueber die Schwefelsaure und ihre Fabrication

nach dem Contactverfahren" ; Ber. Deutsch. Chem. Gesellsch.

34, 4069 (1901)

Dm, Xd, 25°C, m = .014-3.19.

Ql, Hm, 20 and 30°C.

1898KOH/HOL: Kohlrausch, F.; Holborn, L.; 'Das Levitvermogen der Elektrolyte' ; Leipzig, B.G. Teubner, (1898)Kk, Zc,

18, 25°C.

16KOH HOL: Kohlrausch, F.; Holborn, L.; 'Ds Levitvermogen der Kk, Zc

Elektrolyte'; Second Edition, Leipzig, B.G. Teubner, (1916) 18, 25°C.

52KUN/GIA:

52KUN/GIA2:

52KUN/GIA3

50LAN/CRO:

33LAN/MON:

Kunzler, J. E.; Giauque, W. F.; "The Heat Capacity and Entropy of Sulfuric Acid Trihydrate Glass and Cystals from

15 to 300K"; J. Am. Chem. Soc; 74, 797 (1952)

Kunzler, J. E. ; Giauque, W. F.; "Aqueous Sulfuric Acid. Heat Capacity. Partial Specific Heat Content of Water at 25 and -20"; J. Am. Chem. Soc; 74, 3472 (1952)

Kunzler, J.E.; Giauque, W.F.; "The Freezing Point Curves

of Concentrated Aqueous Sulfuric Acid"; J. Am. Chem. Soc;

74, 5271 (1952)

Land, J.E.; Crockford, H.D.; "The Activity Coefficients of Sulfuric Acid in Aqueous 2-Propanol Solutions at 25"; J.

Am. Chem. Soc; 72, 1895 (1950)

Lange, E.; Monheim, J.; Robinson, A.L.; "The Heats of Dilution of Aqueous Solutions of Zinc, Cadmium and Copper

Sulfates and Sulfuric Acid at 25"; J. Am. Chem. Soc.; 55, 4733 (1933)

Ql, 15-300K, liq, vit. and crystal trihydrate.

Ql, 25°C.

Px, m > 30.

Da, 25°C, m < 1, in water

and aq. propanol.

Hm, 25°C, m < 1.

76LAR/HEP

Larson, J.W.; Hepler, L.G. ; "Heats and entropies of Zr , Hr, Kk,

ionziation"; 'Solute-Solvent Interactions', Coetzee, J.F. and 25°C 2d ioniz. Ritchie, C.D.(eds); Marcel Dekker, NY and London, (1969)

58
37LAU/ODA:

37LAU/ODA2:

80LEN/RAF:

14LEW/LAC:

19LEW/LIN:

Lauer, K. ; Oda, R; "Der einfluss des Losungsmittels auf den Ablauf chemischer Reaktionen, XII. Mitteil. : Losungswarme

und Aktivierungsenergie bei der Sulfurierung des Anthrachinons" ; Ber. Bunsenges. Phys . Chem. ; 70B, 333 (1937)

Lauer, K. ; Oda, R. ; "Der Einfluss des Losungsmittels auf

den Ablauf chemischer Reaktionen, XIII. Mitteil.:

Losungswarme und Aktivierungsenergie bei Umsetzungen, deren

einer Teilnehmer als Losungsmittel dient" ; Ber. Bunsenges.

Phys. Chem.; 70B, 1707 (1937)

Lennartz, H.; Rafflenbenl, L.; Hartmann, H. ; "Verdampfungsgleichgeurchte des Systems I^O/H^SO^";

'Hydrogen as an energy vector', Strub, A. A. and Imarisio, G. (eds); D. Reidel Publish. Co., Dordrecht, Holland, (1980)

Lewis, G.N.; Lacey, W.N. ; "The Potential of the Copper

Electrode and the Activity of Bivalent Ions"; J. Am. Chem. Soc; 36, 804 (1914)

Lewis, G. N.; Linhart, G. A.; "The Degree of Ionization of Very Dilute Electrolytes"; J. Am. Chem. Soc; 41, 1951

(1919)

Hm, t = ? sol. of H

20 in

cone. H

2S0^

Hm, t = ? sol. of H20 in cone. H2SO4

Pv, Px, 200 to 500°C,

0 o 100% H2S04

,

1 to 15 bar.

Ke, 25°C, m = 0.005 and

0.05.

Kk, 0°C, interp. of freezing point lowering.

21LEW/RAN: Lewis, G. N. ; Randall, M. ; "The Activity Coefficient of Strong Electrolytes"; J. Am. Chem. Soc; 43, 1112 (1921)

Zr, Da, 25°C, review of early work.

61LIE/ST0: Lietzke, M.H.; Stoughton, R.W. ; Young, T.F.; "The Bisulfate

Acid Constant from 25 to 225" as Computed from Solubility

Data"; J. Phys. Chem.; 65, 2247-2249 (1961)

Kk, 25-225°C, Psat, 2d ioniz., from solb. of Ag2SOA

75LIL/BRI: Lilley, T. H.; Briggs, C.C.; "Stoichiometric Activity

Coefficients of Aqueous H2S0^ Solution at 298. 15K"; Electrochim. Acta; 20, 257 (1975)

Zr, Da, 25°C, m < 0.02.

58LIN: Linke, W.F.; "Solubilities"; D. Van Nostrand, Princeton,

4th ed.; 1, 1153-1156 (1958); [originated by A. Seidel]

Ze, Pv, compiled and correlated solubilities.

69LIN/WIR: Lindstrom, R.E.; Wirth, H.E.; "Estimation of the Bisulfate

Ion Dissociation in Solutions of Sulfuric Acid and Sodium

Bisulfate"; J. Phys. Chem.; 73, 218 (1969)

Zc, Kk, V, 25°C?, m < 0.01.

59
57LLO/WYA: Lloyd, L . ; Wyatt, P.A.H.; "The Partial Molar Heats of Solution of Water in Dinitrogen Pentoxide Solutions and of Potassium Nitrate and Sulphuric Acid in Nirtic Acid at 0°";

J. Chem. Soc. ; 4262 (1957)

Ql, Hm, 0"C, in cone, aq HNO3.

1893LOO: Loomis, E.H.; "Ueber ein exacteres Verfahren bei der Bestimmung von Gefrierpunktserniedrigungen" ; Ber. Bunsenges. Phys . Chem.; 26, 797 (1893)Px, 0°C, m < 0.2, freezing

point lowering, same data in 1894L00.

1894L00: Loomis, E. H. ; "On the Freezing-Points of Dilute

Solutions. II."; Phys. Rev.; 1, 274 (1894)

Px, 0°C, m < 0.2, freezing

point lowering.

1894L002: Loomis, E.H.; "Ueber Ein Exacteres Verfahren bei der Bestimmung von Gefrierpunktserniedrigungen" ; Ann. Physik.;

51, 500 (1894)

Kk, 0°C, m < 0.2, freezing

point lowering, same data in 1894LCO.

56LUC: Luchinskii, G.P.; "Vapor-liquid Equilibrium in System

fi^O-SOg . I. Physico-chemical Observations on the System

H

20-S03

"; Zh. Fiz. Khim. ; 30, 1207 (1956)

Pv, 20-200°C.

59LUC:

33MAC/BLU:

67MAK:

Luchinskii, G.P.; "Physico-chemical Investigation of the System H

20-S03

. II. The Heats of Interaction of the Components in the System H2O-SO3 with the Liquid Phase of Varying Composition"; Zh. Fiz. Khim.; 33, 1275 (1959)

Hm, 25°C?

MacDougall, F. H. ; Blumer, D.R.; "The Activity of Each

Component in Aqueous Solutions of Sulfuric Acid and Acetic

Acid"; J. Am. Chem. Soc; 55, 2236 (1933)

Maksimova, I.N.; "Free Energy, Entropy, and Enthalpy of Ionic Equilibria in Aqueous Solution at High Temperatures";

Russ. J. Phys. Chem.; 41, 27 (1967)

Ke, V, 25°C,

[H2S04

] = 0.05 to 2.2.

Kk, 20-300°C, few exper. data

.

63MAN/SUN: Mansson, M. ; Sunner, S.; "The Heat of Formation of Sulphuric Acid"; Typescript, Thermochemistry Lab, Univ. of Lund; (1963)He, 25°C, combustion of sulfur

.

1876MAR: Marignac, M.C.; "Specific Heat of Saline Solutions"; Arch.

Sci. Phys. Nat.; 55, 113 (1876)

Ql, 16-18°C, 20-50 H

20.

1876MAR2: Marignac, M.C.; "Sur les Chaleurs Specifiques des Solutions

Salines"; Ann. Chim. Phys.; *(5)8, 410 (1876)

Ql, 16-18"C, same data

as in 1876MAR.

60
66MAR/JON: Marshall, W. L.; Jones, E.V.; "Second Dissociation Constant

of Sulfuric Acid from 25 to 350 Evaluated from Solubilities of Calcium Sulfate in Sulfuric Acid

Solutions"; J. Phys . Chem. ; 70, 4028 (1966)

Kk, 25-350°C, in CaSO^Caq, sat).

1890MAT: Mathias, M.E.; "Sur la Chaleur de Vaporisation des Gaz Liquefies"; Ann. Chim. Phys.; *(6)21, 69 (1890)

Hm, 16°C, into cone. H2S04

.

42MCC/MCK: McCurdy, J.L.; McKinley C; "The System Nitric AcidSulfuric Acid-Water"; Ind. Eng. Chem.; 34, 1002 (1942)

Zc, Qh, Hm, 32-500°F?,

nomograph for mixt of

H

2S0A /HN03 /H2

0.

27MCH: McHaffie, I. R. ; "The Vapour Pressure of Water over Sulphuric Acid-Water Mixture at 25"; J. Chem. Soc . ; 112

(1927)

Pv, 25°C, 66-84% H2S0A.

32MEY: von Meyeren, W. ; "Eine einfache Methode zur Messung kleiner

Dampfdrucke" ; Z. Phys. Chem. (Leipzig); A160, 272 (1932)

Pv, 0-40°C, 60-70 wt%

H

2SCv

42MOR: Morgen, R. A.; "Heats of Solution of the System Sulfur

Trioxide-Water" ; Ind. Eng Chem.; 34, 571 (1942)

Zc, Dm, 18°C,

enthalpies

43MOR/BEN:

13MUL:

Morgan, J.J.; Bender, D.A. ; Capell, R.G. ; "Specific Heats

of Mixed Acids at Higher Temperatures"; Chem. Met. Eng.;

50, 122 (1943)

Muller, J. A.; "Sur les Chaleurs de Dilution a l'infini des Solutions Aqueuses Moleculaires d'Acide Chlorhydrique et d'Acide Sulfur i que " ; Bull. Soc. Chim. France; 13, 1053 (1913)

Zc, Qh, 0-100°C, in H20 and mixt. with HNO3-

Rm, 14-38°C, at inf. dil.

28NAU: Naude, S.M.; "Uber die Verdunnungswarme schwach konzentrierter Losungen" ; Z. Phys. Chem. (Leipzig); 135, 209 (1928)

Hm, 18°C, [H2 S0A

] = 0.001-0.5.

60NEC: Neckel, A.; "Gefrierpunktsniedrigung" ; ' Landolt-Bornstein

Tabellen'; Auflage 6, Band II Teil 2a, p. 862 (1960)

Ze, Hm, 0°C, freezing

point lowering.

07NOY: Noyes, A. A. ; 'The Electrical Conductivity of Aqueous

Solutions'; Publ. 63, Carnegie Institution of Washington,

153-234, (1907)

Kk, 25-306°C.

61
10NOY/FAL:

56PAP/CAN

Noyes, A. A. ; FaLk, K.G. ; "The Properties of Salt Solutions

in Relation to the Ionic Theory. I. Mol-Numbers Derived

from the Freezing-Point Lowering"; J. Am. Chem. Soc .

32,1017 (1910)

Papee, H.M. ; Canady, W.J.; Laidler, K.J.; "The Heat of Neutralization of Strong Acids and Bases in Highly Dilute

Aqueous Solutions"; Can. J. Chem.; 34, 1677 (1956)

Zr, Kk, 0°C, freezing

point lowering.

Hr, 25°C, m < 3x10-2,

neutralization.

20PAS/GAR: Pascal, P.; Gamier, M. ; "Chaleur Specifique des Acides

Sulfuriques, des Acides Nitriques et de Leurs Melanges

(1)"; Bull. Soc. Chim. France; 27, 8 (1920)

Ql, 20°C, x(H 2SO^) = .10 to 1.0.

1890PIC:

1890PIC2:

Pickering, S.U.; "The Nature of Solutions, as Elucidated by

the Freezing Points of Sulphuric Acid Solutions"; J. Chem.

Soc. ; 57, 331 (1890)

Pickering, S.U.; "The Nature of Solutions, as Elucidated by

a Study of the Density, Electric Conductivity, Heat Capacity, Heat of Dissolution and Expansion by Heat of Sulphuric Acid Solutions"; J. Chem. Soc; 57, 64 (1890)

Px, t < 20°C, solidus,

x(H2SOA

) = 0 to 0.94.

V, Vm, Q, Hr, 8-38°C, but diff for various

props

1891PIC: Pickering, S.U.; Verhandlungen uber die Theorie der Losungen"; Z. Phys . Chem. (Leipzig); 7, 378 (1891)

Kk, t < 0°C, freezing

point lowering, comment

by J. Walker, pg 396.

1892PIC: Pickering, S.U.; "Das kryoskopische Verhalten schwacher

Losungen"; Ber. Deutsch. Chem. Ges . ; 25, 1099 (1892)

Kk, t < 0°C, to 2 wt 1, freezing point lowering.

76PIT:

77PIT/ROY:

Pitzer, K.S.; "Thermodynamic Properties of Dilute Sulfuric

Acid and the Potential of the Lead Sulfate-Lead Electrode";

J. Phys. Chem.; 80, 2863 (1976)

Pitzer, K.S.; Roy, R.N.; Silvester, L.F.; "Thermodynamics

of Electrolytes. 7. Sulfuric Acid"; J. Am. Chem. Soc; 99 4930 (1977)

Da, 25°C.

Ze, Da, Kk, 25°C, 0-6 m.

73PLA; Platford, R.F.; "Osmotic Coefficients of Aqueous Solutions

of Seven Compounds at 0°C"; J. Chem. Eng. Data; 18, 215

(1973)

Da, 0°C, 1-11 m.

62
Porter, A. W. ; "The Thermal Properties of Sulphuric Acid

and Oleum"; Trans Faraday Soc . ; 13, 373 (1918)

Zr, Q, Hp, Hm, various

t . , dil . and cone

sol.

Pretat, M. ; "Determination des Chaleurs de Dilutions des Hm, 20-25°C, cone. Melanges Sulfonitriques" ; Mem. Poudres ; 24 , 119 (1930) H

2S04 and H

2S0 4 /HN0

3 mixt

Quist, A.S.; Marshall, W.L.; Jolley, H.R. ; "Electrical Kk, 0-800°C, p to 4000 Conductances of Aqueous Solutions at High Temperatures and bar, Kl and K2 (ioniz.), Pressure. II. The Conductances and Ionization Constants of AH (ioniz) rrKH^O^)

Sulfuric Acid-Water Solutions from 0 to 800 °C and at < 0.01. Pressures up to 4000 Bars"; J. Phys . Chem. ; 69, 2726

(1965)

Radulescu, D . ; Jula, 0.; "Beitrage zur Bestimmung der Ql, 15-18°C, [H2SO^] = 2 Abstufung der Polaritat des Aminstickstoff es in den organischen Verbindungen" ; Z. Phys. Chem. (Leipzig); B26, 390 (1934)

Randall, M. ; Cushman, O.E.; "The Free Energy of Dilution of Ke, 25°C,

Sulfuric Acid"; J. Am. Chem. Soc; 40, 393 (1918) x(H2S0A

) = 0.0001-0.128.

Randall, M. ; Langford, C.T.; "The Activity Coefficient of Ke, Da, 25°C,

Sulfuric Acid in Aqueous Solutions with Sodium Sulfate at M(S0^") = 0.2 to 2, 25"; J. Am. Chem. Soc; 49, 1445 (1927) a(H2S04

) from EMF

Randall, M. ; Scott, G.N. ; "The Freezing Point and Activity Px, Da, 0°C,

Coefficient of Aqueous Barium Nitrate, Sodium Sulfate and M(H2S0Z( ) < 0.1, a(H2 S0

A

) Sulfuric Acid"; J. Am. Chem. Soc; 49, 647 (1927) a(H20) .

Randall, M. ; Taylor, M. D.; "Heat Capacity and Density of Ql, Vx, 25°C,

Aqueous Solutions of Potasssium Iodate, Potassium Acid m(H2S0^) = 0.04 to 2.2. Sulfate, Iodic Acid, and Sulfuric Acid at 25°C"; J. Phys. Chem. ; 45, 959 (1941)

Rard, J. A.; "Isopiestic Determination of the Osmotic Pv, Da, 25°C,

Coefficients of Aqueous H

2SO^ at 25°C"; J. Chem. Eng. Data; m(H2SOA

) = 0.14 to

28, 384-387 (1983) 3.1, isopiestic studies.

Rard, J. A.; Habenschuss, A.; Spedding, F.H.; "A Review of Ze, Da, Pv, 25°C, the Osmotic Coefficients of Aqueous H

2 SO^ at 25 °C"; J. m(H2SO^) = 0.1 to 28, Chem. Eng. Data; 21, 374-379 (1976) a(H20)
77RAR/SPE:

69REA/COB

Rard, J. A.; Spedding, E.H.; "Isopiestic Determination of the Osmotic Coefficients of Aqueous CaCl2 Solutions at 25°C"; J. Chem. Eng. Data; 22, 56 (1977)

Readnour, J.M. ; Cobble, J.W. ; "Thermodynamics Properties

for the Dissociation of Bisulfate Ion and the Partial Molal

Heat Capacities of Bisulfuric Acid and Sodium Bisulfate

over an Extended Temperature Range"; Inorg. Chem.; 8, 2174

(1969)

Da, Pv, 25°C, m = 2.6 to

8.8.

Hm, Q, Kk, 0-lOCTC,

K2(ioniz.), enthalpy of solution of Na^O^ in

1845REG: Regnault, M.V. ; "Etudes sur l'Hygrometrie" ; Ann. Chem. Phys . ; 15(3) , 129 (1845)

Pv, 8-52°C, H2SO i( (H20) to H

2SO^(18H20)

38RHO/NELRhodes, F. H. ; Nelson, C.C.; "Heats of Dilution of 'Mixed Acids'"; Ind. Eng. Chem.; 30, 648 (1938)Hm, 18°C,

H

20/acid = 0-3.5, AH (sol): H

2S0 A , HN03 and their mixtures into

H,0.

39ROB: Robinson, R.A. ; "The Activity Coefficients of Sulphuric

Acid and Lanthanum Chloride in Aqueous Solution at 25"; Trans Faraday Soc . ; 35, 1229 (1939)

Pv, Da, 25°C,

m(H2S04) = 0.2-3,

isopiestic method vs. KC1.

4 5ROB: Robinson, R.A. ; "The Vapour Pressure of Solutions of Potassium Chloride and Sodium Chloride"; Trans. R. Soc. N.Z.; 75, 203 (1945)

Pv, 25°C,

m(H2S0A

) = 1.3-4.3,

isopiestic method vs. NaCl, a(H20).

30ROT/GRA: Roth, W.A. ; Grau, R. ; Meichsner, A.; "Beitrage zur Thermochemie des Schwefels. Ill"; Z. Anorg. Allgem. Chem.

193, 161 (1930)

Hm, 18-20°C, m(H2S04) <

0.033, AH(sol),

AH(dil)

3 1ROT

Roth, W.A. ; "Losungs-und Verdunnungswarme von Sauren und Basen" ; ' Landolt-Bornstein Physikalisch-Chemsche Tabellen'

Auf. 5, Erg 2, 1547-50 (1931)

Ze, Hm, 8-18*C.

52RUB/GIA: Rubin, T.R.; Giauque, W.F.; "The Heat Capacities and Entropies of Sulfuric Acid and its Mono- and Dihydrates

from 15 to 300K" ; J. Am. Chem. Soc; 74, 800 (1952)

Ql, 15-300K, includes

data on solutions above melting points of the hydrates

64
07RUM: Rumelin, G.; "Uber die Verdunnungswarme konzentrierter

Losungen"; Z. Phys . Cpm. (Leipzig); 58, 449 (1907)

Hm, Pv, 10-16°C,

H

20/H2SOZ( = 2-200.

64RYZ: Ryzhenko, B.N.; "Determination of the Second Dissociation Constant of Sulfuric Acid and the Precipitation of Salts in the Reciprocal System Ca2+ Ba 2+

SO,. CO. under Hydrothermal Conditions"; Geokhimiya; 1, 8 (1964)

Kk, 100-218°C, K2

and (ioniz) from conductance of KHSO^(aq)

74SAN: San'ko, Yu. P. ; "Heat Capacity of Aqueous Solutions of Sulfuric Acid at Low Temperatures (to -196°C)"; Inzh-fiz.

Zh.; 27, 78 (1974)

Ql, -190 to 20°C, 40-953

H

2S04

.

73SAU/SAW: Saunders, A.; Sawistowski, H. ; "Correlation of Activity

Coefficients of Water in Solutions of Sulphuric Acid and Toluene Sulphonic Acid"; J. Appl. Chem. Biotechnol. ; 23, 111 (1973)

Pv, t~100°C, vapor

pressures, activity

coefficients of ternary

mixture

38SCA/HAM:

09SCH:

Scatchard, G. ; Hamer, W.J.; Wood, S.E.; "Isotonic

Solutions. I. The Chemical Potential of Water in Aqueous

Solutions of Sodium Chloride, Potassium Chloride, Sulfuric

Acid, Sucrose, Urea and Glycerol at 25°"; J. Am. Chem.

Soc. ; 60, 3061 (1938)

Schlesinger, H. ; "Die spezifischen Warmen von Losungen. I' Phys. Z. ; 10, 210 (1909)

Pv, Da, 25°C, m = 0.1-4.4

a(H20), isopiestic

method

Ql, 0-70°C, 5 and 857= H

2SCv

65SCH/FER: Schwabe, K. ; Ferse, E.; "Untersuchungen an den Ketten:

(Pt), H

2 /H2

0, HC1, Hg2Cl2 (S)/Hg und (Pt), H

2 /H2

0, H2S0 4

, Hg 2S0

A (S)/Hg"; Ber. Bunsenges . Phys. Chem.; 69(5), 383 (1965)

Ke, 25°C, m(H2S0 4

) <

0.01, EMF in the presence of Na2 SO^ and

Li 2SO^

39SHA/GOR

Shankman, S.; Gordon, A.R. ; "The Vapor Pressure of Aqueous

Solutions of Sulfuric Acid"; J. Am. Chem. Soc; 61, 2370

(1939)

Pv, 25°C, m(H2 S0^) = 2-23 isopiestic method,

a(H20)

70SHA/PRA: Sharma, L.; Prasad, B.; "Standard E.M.F. of the Cell: Pt

Q.H. H2S0^/H2S0A /H2S0A , Hg 2SOA /Hg and the Standard

Electrode Potential of Hg/Hg2S0A , S04 2_ at 5, 15, 25, and 35°C"; J. Ind . Chem. Soc; 47, 379 (1970)

Ke, Da, 5-35°C,

[H2SOZ( ]=0. 008-0. 32 a(H2SO^)

65
39SHE/JAN:

81SHE/VAL

Sheffer, H . ; Janis, A. A. ; Ferguson, J.B.; "The Activity of Water in Sulphuric Acid Solutions at 25°C by the Isopiestic

Method"; Can. J. Res.; B17, 336 (1939)

Da, 25°C,

m(H2 SOA

) = 0.02-4.3,

a(H2 0), isopiestic

method

Shenfel'd, B.E.; Valeev, R.R. ; Vasil'ev, B.T.; Sushcher, V.S.; Zc : Kk, 700-1200 K.

Z. Prikl. Khim.; 56, 1142-1144 (1983)

34SHR/COW: Shrawder, J. Jr.; Cowperthwaite , I. A.; "The Activity

Coefficients of Sulfuric Acid at Temperatures from 0 to

50"; J. Am. Chem. Soc . ; 56, 2340 (1934)

Ke, Da, Dm, 0-50°C,

[H2SO^] = 0.001-0.02,

a(H2S0^), AH(dil).

64SIL/MAR: Sillen, L.G.; Martell, A.E.; "Stability Constants of Metal-ion Complexes, Section I, Inorganic Ligands";

Special Publication No. 17, Chemical Society (London); 215-216 (1964)

Ze, Kk, compiled

solution equilibria.

71SIL/MAR: Sillen, L.G.; Martell, A.E.; 'Stability Constants of Metal- Kk, 20-350°C,

Ion Complexes. Supplement No., 1'; The Chemical Soc, London; compiled data. Spec. Publ. 25 (1971)

75SIN/PUR: Sinha, O.P.; Puri, O.P.; "Specific Heat Anomaly of Sulphuric Acid with Dilution"; Chem. Phys . Letters; 32, 495 (1975)

Q, Vx, theoretical

interpretation

79SMI/GOL:

76SMI/MAR:

Smith-Magowan, D.; Goldberg, R.N. ; "A Bibliography of Experimental Data Leading to Thermal Properties of Binary

Aqueous Electrolyte Solutions"; Nat. Bur. Stand. (U.S.)

Spec. Pub. ; No. 537 (1979)

Smith, R.M.; Martell, A.E.; 'Critical Stability Constants'

4 (1976)

Hm, Ql, Vx, annotated bibliography

Ze, Kk, H, Q, evaluated solution equilibria.

24SMI/MAY: Smith, D.F.; Mayer, J.E.; "The Free Energy of Aqueous

Sulfuric Acid"; J. Am. Chem. Soc; 46, 75 (1924)

Ke, 80°C, H

2S04 + 6HI

32SOC: Socolik, A. S. ; "Warmekapazitaten der wasserigen Losungen

von Schwefelsaure" ; Z. Angew. Chem.; 158, 305 (1932)

Q, 60 and 80°C, 5-100%

32SOC2: Socolik, A.; "Heat Capacity of Solutions of Sulfuric

Acid"; Zh. Obshchei Khim.; 2, 311 (1932)

Q, 60 and 80°C, 5-100%

66
1890SOR: Sorel, E.; "The Manufacture of Sulphuric Acid"; J. Soc

Chem. Ind. ; 9, 175 (1890)

Zr, Pv, 10-95'C, 44-82% K^SO^ , review.

81STA: Staples, B.R.; "Activity and Osmotic Coefficients of Aqueous Sulfuric Acid"; J. Phys . Chem. Ref. Data; 10, 779

(1981) of data.

Ze, Da, Dx, 25°C, m(H2S0 4) = 0 to 28, critical review

81STA/WOB: Staples, B.R.; Wobbeking, T.F.; 'A Compilation of Thermodynamic and Transport Properties of Aqueous

Sulfuric Acid', Nat. Bur. Stand., NBSIR; 81-2276

(1981)

Zr, bibliography.

4 5STO: Stokes, R.H. ; "The Derivation of Water Activities from Electromotive Force Data"; J. Am. Chem. Soc.; 67, 1686

(1945)

Zc, Da, 25°C.

47STO:

4 8STO:

Stokes, R.H.; "The Measurement of Vapour Pressures of Aqueous Solutions by Bi-thermal Equilibration through the Vapor Phase"; J. Am. Chem. Soc; 69, 1291 (1947)

Stokes, R.H. ; "A Thermodynamic Study of Bivalent Metal

Halides in Aqueous Solutions. Part XVII. Revision of Data

for all 2:1 and 1:2 Electrolytes at 25, and Discussion of Results"; Trans Faraday Soc; 44, 295 (1948)

Pv, Da, 25°C,

m(H2SO

A

) = 3-11.5, two temperature isopiestic

method.

Zr, Da, 25°C,

m(H2S04

) = 0.1-22, review,

a(H20)

63STU/SEC: Stuckey, J.E.; Secoy, C.H.; J. Chem. Eng. Data; 8, 386-389 (1963)

Pt, Vc, 218-670°C.

41TAR/NEW: Tartar, H.V. ; Newschwander , W.W. ; Ness, A.T.; "A Thermodynamic Study of the System Zinc Sulfate-Sulfuric

Acid-Water at 25°"; J. Am. Chem. Soc; 63, 28 (1941)

Ke, Pv, 25°C,

m(H2S0

4

) = 0.1 to 4.

13THI: Thibaut, R. ; "Die Elektromotorische Kraft des Bleiakkumulators in Abhangigkeit von Temperatur und

Sauredichte" ; Z. Electrochem. ; 19, 881 (1913)

Ke, 15-45°C,

m(H2S04

) = 0.4-5.2, EMF of lead accumulator.

1882THO: Thomsen, J.; ' Thermochemische Untersuchungen '

, J. A. Barth

Verlag, Leipzig; 1, 36 (1882)

Ql, 18°C, 5-200 H

20.

1883THO: Thomsen, J.; 'Thermochemische Untersuchungen', J. A. Barth

Verlag, Leipzig; 3, 39 (1883)

Hm, 20°C, H

2SO i( /H2

0 = 1 to

800, dilution heats.

67
33TRI/EBE: Trimble, H.M.; Ebert, P.F.; "The Effect of Ethylene Glycol

upon the Activity of Sulfuric Acid in Aqueous Solutions";

J. Am. Chem. Soc . ; 55, 958 (1933)

Ke, Dm, 25°C,

m(H2 SO^) = 0.005-1,

in and aq. ethylene glycol.

74TUR: Turner, D.J.; "Dissociation of the Bisulphate Ion at Moderate Concentrations"; J. Chem. Soc. Faraday Trans. I;

70, 1346 (1974)

Kk, 25°C,

m[S0A 2 "] = 0.02-4, K2 (ioniz), ion pairing.

67VDO/LAZ:

29VOS/CRA:

Vdovenko, V.M. ; Lazarev, L.N. ; Khvorostin, Ya. S.; "Determination of the Dissociation Constants of Hydrogen

Sulphate Ions in Solutions at Different Ionic Strengths and Temperatures"; Russ. J. Inorg . Chem.; 12, 610 (1967)

Vosburgh, W.C.; Craig, D.N.; "The Lead Dioxide-Lead Sulfate

Electrode"; J. Am. Chem. Soc; 51, 2009 (1929)

Kk, 20-35°C, I = 0 to 2m, K2 in presence of Na salts

Ke, 20-40°C,

m(H2 SO^) =0.1, EMF of Lead Sulfate-Sulfuric

acid cell.

27VRE: Vrevskii, M.S.; "Latent Heat of Vaporization of Pure Liquids and of Solutions"; Zh. Fiz. Khim. Obs . ; 59, 69

(1927)

Hp, 96.5°C, 53% H2S04

, vaporization

27VRE/NIK: Vrevskii, M.S.; Nikol'skii; "Determination of the Latent

Heat of Vaporization of H

20 from Solutions of Sulphuric

Acid for 79.3 and the Comparison of the Thermal Effect

and of Work of Dilution of these Aqueous Solutions";

Zh. Russ. Fiz. Khim. Obs.; 59, 77-78 (1927)

Hp, 80°C, 17-60 wt%,

vaporiz

82WAG/EVA: Wagman, D.D.; Evans, W.H.; Parker, V.B.; Schumm, R.H.; Halow, I.; Bailey, S.M. ; Churney, K.L.; Nuttall, R.L.;

J. Phys. Chem. Ref. Data; 11, Supplement No 2 (1982); "The NBS Tables of Chemical Thermodynamic Properties"

Ze, H, K, Q, evaluated thermochemical data.

66WAL: Wallace, R.M.; "Determination of the Second Dissociation Constant of Sulfuric Acid by Donnan Membrane Equilibrium"

J. Phys. Chem.; 70, 3922 (1966)

Kk, 25-50°C, K2 (ioniz)

and H

2 (ioniz)

69WAN/ZWI: Wanders, A. CM.; Zwietering, Th.N.; "Calculation of AH

and K Values from Thermometric Titration Curves"; J. Phys. Chem. ; 73, 2076 (1969)

Kk , calculation method

for K2 (ioniz) and H2

.

68
OOWHE: Whetham, CD.; "The Ionization of Dilute Solutions at the Freezing Point"; Phil. Trans A; 194, 321-360 (1900)

Kk, 0-70°C, 1st ioniz. m = .00005 - 0.02.

53WHI/LAN:

21WIL:

71WIR:

29WRE:

Whitten, W.N.; Land, J.E.; "The Thermodynamics of Aqueous

2-Propanol-Sulfuric Acid Solutions from Electromotive Force Measurements"; J. Am. Chem. Soc . ; 75, 2202 (1953)

Wilson, R.E.; "Humidity Control by Means of Sulfuric Acid

Solutions, with Critical Compilation of Vapor Pressure

Data"; Ind. Eng. Chem.; 13, 326 (1921)

Wirth, H.E.; "Activity Coefficients in Sulphuric Acid and Sulphuric Acid-Sodium-Sulphate Mixtures"; Electrochim.

Acta; 16, 1345 (1971)

Wrewsky, M. S.; "Theoretische und experimentelle

Untersuchung uber Verdampfung binarer Gemische. I. Methode

der Bestimmung von Verdampfungswarmen reiner Flussigkeiten

und Losungen"; Z. Phys . Chem.; A144, 244 (1929)

[Vrevskii, M.S.]

Ke, Da, Dm, 5-25°C,

[H2SOA

] = 0.05-1, mixed

solvent system.

Pv, Zc, 0-50°C,

x(H2S04

) = 0-1.

Zc, Dm, 25°C,

reevaluation and calculational method.

Pv, Hp, JQ.Z'C, 53.66% H2SO4 , transpiration

method for H(uap)

.

57WU: Wu, Y. C; "Part I. Thermal Effects of the Interactions Between Univalent Ions. Part II. Heat of Dilution of Sulfuric Acid in Aqueous Solution"; Thesis, Univ. of Chicago (1957)

Hm, 25 C, m(H2S0A

) = 0.001-6.5, also data on LiCl and HC1.

80WU/YOU: Wu, Y.C.; Young, T.F. ; "Enthalpies of Dilution of Aqueous Electrolytes: Sulfuric Acid, Hydrochloric Acid, and Lithium Chloride"; J. Res. Nat. Bur. Stand.; 85,

11 (1980)

Hm, 25°C,

m(H2S04) = 0.001-6.5, also data on LiCl and HC1, see 57WU.

60WYA: Wyatt, P.H.A.; "The Constitution of 80-100% Aqueous

Sulphuric Acid: A Case of Overlapping Equilibria";

Trans. Faraday Soc; 56, 490 (1960)

Kk, 83-97% H

2S0

4

, ionization constants, reassessment

.

62Y0U/IRI: Young, T. F.; Irish, D. E.; "Solutions of Electrolytes'

Ann. Review Phys. Chem.; 13, 435 (1962)

Zr, Kk, Px, Hm, review

of solution equilib. to

1961.

59YOU/MAR: Young, T.F.; Maranville, L.F.; Smith, H.M. ; "Raman Spectral

Investigations of Ionic Equilibria in Solutions of Strong

Electrolytes"; 'The Structure of Electrolytic Solutions',

Hamer, W.J.(ed); John Wiley and Sons, Inc., New York, (1959)

Kk, Mm, 0-50°C, 0.05 - 18m.

69
63ZAR/VIN : Zarakhani, N.G.; Vinnik, M.I.; Russ. J. Phys . Chem. ; 37, Kk, 25°C. 260-263 (1963)

70
NH

3

-H 2

0

Rebecca Joseph, David Garvin, Cynthia R. Jackson, and

Bert R. Staples

INTRODUCTION

Publications are listed in this bibliography that have

data on equilibria in mixtures of ammonia and water and on

the associated vapor- liquid equilibrium and solubilities (at

low temperatures) as shown in phase diagrams. To a lesser

extent, there are data on enthalpies of mixing, on activity

coefficients and on the thermochemistry of the system.

References reporting measurements or presenting

correlations or evaluations of data are included.

Publications that consider only applications of existing data

to specific systems but provide no new data have been

avoided.

Ammonia is completely miscible with water but relatively

volatile. It is a monoprotic base , abstracting a proton from

water to form the ammonium cation. Ammonium salts have a wide

variety of commercial applications and solutions of these

have been studied extensively in association with the study

of equilibria involving ammonia. Ammonia also complexes with

many metal cations in solution .

The references are listed alphabetically by first

author. Each citation is preceeded by a brief identification

code composed of the year of publication and three letters

from the last names of the first two authors. The citations

list the names of authors; the title of the article , chapter

or report as appropriate, and the source information, i.e.

journal or book title , volume , year of publication. The

structure of these citations does not conform to the

specifications established by the American National Standards

Institute but is the information necessary to direct the

reader to a particular reference. In a few instances only an abstract or secondary reference was available. In these cases either the citation to Chemical Abstracts or source of

the secondary citation is given.

71
Some titles have been translated, e.g. those in

Russian. These translations come, by preference, from

abstracts in the papers themselves or from Chemical

Abstracts. ( The titles from the latter may be condensations

of the originals.)

Each publication has been annotated to show the class of

data, the temperature range and, if appropriate, pressure,

solution composition and pH. The data class designations are taken from the Bulletin of Chemical Thermodynamics. They are

two letter codes with some mnemonic or physical chemical

associations. A list is appended. No attempt has been

made to assess the quality of the data, however, an annotation

of "Ze" indicates that a particular reference constitutes or includes an evaluation of experimental data from several sources

The bibliography has been prepared by searching the

files of the NBS Chemical Thermodynamics Data Center, the Bulletin

of Chemical Thermodynamics, and references in the papers

retrieved from those sources. It covers a time period from

the 19th century to 1982. Additions and corrections will be

welcomed.

72
02ABE/RIE: Abegg, R. ; Riesenfeld, H.; "Uber das losungsverraogen von

salzlosungen fur ammoniak nach messungen seines

partialdrucks . I."; Z. Phys . Chem. ; 40, 84-108 (1902)

Pv, 25,35°C, and in the presence of alkai

and alkaline earth

salts

.

65ABL/BUR: Ablov, A.V. ; Burnasheva, Z.P.; Konunova, Ts.B.; "Heats of addition of amines to zinc halides"; Zh. Neorg. Khim.

;

10, 2286-2292 (1965)

Hm, 25°C, in 2N HC1.

81ALL/W00: Allred, G.C. ; Woolley, E.M.; "Heat capacities of aqueous acetic acid, sodium acetate, ammonia, and ammonium

chloride at 283.15, 298.15, and 313.15 K: AC°p for ionization of acetic acid and for dissociation of ammonium ion"; J. Chem. Thermodyn.; 13, 155-164

(1981)

Ql, Vx, 10-30°C,

dil. solns

.

1842AND:

1870AND:

59ARN/FRE:

78ART/KOC

Andrews, T.; "Sur la chaleur developpee pendant la combinaison des acides avec les bases"; Ann. Chim. Phys.;

[3], 4, 316-329 (1842)

Andrews, T.; "On the heat developed in the combination of

acids and bases"; J. Chem. Soc . ; 23, 432-441 (1870)

Arnold, E.; Freitag, H.; Patterson, A., Jr.; "Ionization

equilibria in ammonia-water solutions from 5° to 55°C. as obtained from high field conductance measurements";

'The structure of electrolytic solutions ' ,W . J. Hamer.ed.; John Wiley and Sons, Inc., New York, 281-290 (1959)

Artyukhov, A. P.; Kochetkov, V.N.; Vitkov, V.S.; Mikhailov, G.V. ; "Equations for calculating heat capacity

and enthalpy in the ammonia-phosphorus pentoxide-water

systems"; Khim. Prom-st. (Moscow); *(8), 625-627 (1978);

[CA 89:205121z]

Hr, 11-15°C(?),

reaction with acid.

Hr, 11-15°C(?),

reaction with HCl(aq),

HNOg(aq) and acetic

acid

.

Kk, Za, 5-55°C

Zc , Px, t=? , in phosphate

sol . , theoret

.

71BAL/SPE: Baldi, G. ; Specchia, V.; "Solubilitia dell * ammoniaca in acqua"; Chim. Ind . (Milan); 53(10), 929-933 (1971)

Pv, 25°C, 0.65 atm.

,

Solubility in solutions

of alkali halides

nitrates and sulfates.

73
7 1BAL/SPE2 : Baldi , G. ; Specchia, V.; "Solubilita dell ' ammoniaca in soluzioni saline"; Chim. Ind. (Milan); 53(11), 1022-1027

(1971)

Pv, 25°C, 0.65 atm.

Solubility in solutions

of alkali halides

nitrates and sulfates.

66BAT/CLE: Battino, R. ; Clever, H.L.; "The solubility of gases in liquids"; Chem. Rev.; 66, 395-463 (1966)Ze.Zr, Pv, methods,

thermodynamic formulae,

bibliography

but no data.

49BAT/PIN: Bates, R.G. ; Pinching, G.D.; "Dissociation constant of ammonium ion 0° to 50 °C, and the base strength of

ammonia"; J. Res. Nat. Bureau Standards; 42, 419-430

(1949)

Kk, Da, Hr, Q, 0-50°C,

m(NH3

) to 0.1, in NH4Cl(aq).

50BAT/PIN: Bates, R.G. ; Pinching G.D.; "Dissociation constant of aqueous ammonia at 0° to 50° from E. M. f . studies of the ammonium salt of a weak acid"; J. Am. Chem. Soc .

72, 1393-1396 (1950)

Kk, 0-50°C, m(NH3

) to 0.1 in NHF^CKaq)

09BAU/GAY: Baud, E.; Gay, L.; "Determination des hydrates, en solution, par la methode thermique. Application au systeme eau ammoniac liquide"; Ann. Chim. Phys .

[8]17, 398-418 (1909)

Hm, 12°C 1 . atm.

17-63% NH3 by weight.

14BAU/TYK: Baume, G. ; Tykociner, A. ; "Recherches quantitatives sur

les systemes volatils. Courbe de fusibilite du system

anhydride sulfureux-eau" ; J. Chim. Phys.; 12, 270-275

(1914)

Px, -90 to 13°C,

liquidus

34BEC/ROT: Becker, G.; Roth, W.A. ; "Die Bildungswarme von Ammoniak

und Salpetersaure" ; Z. Elektrochem. ; 40, 836 (1934)

Ze, Hr, 20°C,

reaction with HN0 3 (aq).

76BEG: Beggerow, G. ; "Mixing and solution heats"; 'Landolt -

Bornstein Zahlenwerte und functionen aus Naturwissenschaften und Technik'; A Gruppe IV, Neue Serie, Band 2, 79-80 (1976)

Hm, 3-61'C, 1-150

53BER/PAT: Berg, D.; Patterson, A., Jr.; "The high field conductance

of aqueous solutions of ammonia at 25

75, 5731-5733 (1953)

'C" ; J. Am. Chem. Soc.

Kk, 25°C.

74
1873BER: Bertbelot, M. ; "Recherches calorimetriques sur l'etat des corps dans les dissolutions. Recherches sur les acides

forts et les acides faibles et sur les sels qu'ils

forment avec la potasse, la soude et 1' ammoniaque"

Ann. Chim. Phys . ; [4], 29, 433-514 (1873)

Hr, 18°C, reaction

with HN03 (aq) and HCl(aq)

1873BER2: Berthelot, M. ; "Parallele entre la formation des sels solides engendes par les acides picrique, chlorhydrique

azotique, sulfurique, acetique et benzoique" ; Ann. Chim. Phys.; [4], 29, 328-351 (1873)

Hr, 18°C, reaction

with HN03 (aq) and HCl(aq)

1875BER: Berthelot, M. ; "Dissolution des acides et des alcalis,

Septieme memoire. Sur la chaleur degagee dans la reaction

entre l'eau et 1' amrnonique . " ; Ann. Chim. Phys.; [5], 4, 526-531 (1875)

Hm, 10°C, solution

in 250-370 H

20, als dilution data at 14°C.

1875BER2: Berthelot, M. ; "Recherches sur les acides gras et leurs

sels alcalins"; Ann. Chim. Phys.; 80, 592-598 (1875)

Hr, 18°C, reaction

with acetic acid.

1875BER3: Berthelot, M. ; "Recherches sur les acides gras et leurs

sels alcalins"; Ann. Chim. Phys.; [5], 6, 325-334 (1875)

Hr, 18°C, reaction

with acetic acid.

1881BER: Berthelot, M. ; "Recherches sur l'acide perchlorique"

Compt. Rend.; 93, 240-246 (1881)

Hr, 18°C, reaction

with HC10A

.

1882BER: Berthelot, M. ; "Recherches sur l'acide perchlorique"

Ann. Chim. Phys.; [5], 27, 214-222 (1882)

Hr, 18°C, reaction

with HC104

.

25BIL/MES: Biltz, W. ; Messerknecht, C; "Beitrage zur systematischen

Verwandtschaftslehre XXXIII. Uber die Ammoniakate der Berylliumhalogenide" ; Z. Anorg. Allgem. Chem. ; 148, 157-169 (1925)

Hr, t = ?, reaction with

HC1.

41BJE: Bjerrum, J.; 'Metal ammine formation in aqueous solution.

Theory of reversible step reactions', P. Haase and Son, Copenhagen; (1941)

Kk, 22 and 30 C, in

03BOU: Bouzat, M. ; "Composes cuproammoniques" ; Ann. Chim. Phys.

[7], 29, 305-383 (1903)

Hr, Hm, 13°C,

reaction with HC1.

75
11BRI:

17BRU/LEV

Brichaux, A. ; "Loi relative a la solubilite de Pammoniague

a differentes temperatures et sou differentes pressions";

Bull. Soc. Chem. Beige; 25, 145-153 (1911)

Bruni , G. ; Levi, G. ; "Gli ammoniacati dei sali d'argento. Nota III."; Gazz. Chim. Ital. ; 47, 259-272 (1917)

Zc, Pv, 15-120°C, 3-50% NH- reinterp. of

03 PER and 08MOL.

Hr, 12°C(?),

HCIO^

33CAL: Calvet, E.; "Measures thermochimiques directes en chimie

organique. Vitesses et chaleurs de saponification des amides, II."; J. Chim. Phys . ; 30, 140-149 (1933)

Hm, 17°C, dil. from

70 to 200 H,0.

65CHA: Chan, J.P.C.; "The heat capacity and entropy of ammonia

di-hydrate"; Ph.D. Thesis, Univ of California, Berkeley;

Diss Abstr. 652957, 25, 6250 (1965)

Ql, 15-298 K

, NH3 -2H20 (cr and 1)

71CHEChernen'kaya, E.I.; "Experimental determination of the specific heats of aqueous solutions of NH^HCOg

Na2CO.j, and of liquors of the sot a industry at 25°C"; J. Appl. Chem. (USSR); 44, 1562-1566 (1971)

Ql, 25°C,

m(NH3

) = 1-13.

71CHE2:

75CHE/BRA:

Chernen'kaya, E.I.; "Determination of the heat capacities

of liquids of the soda industry at 25°C by calculation.

Communication II"; J. Appl. Chem. (USSR); 44, 1744-1747

(1971)

Chernen'kaya, E.I.; Bratash, E.G.; "Calculation of specific heats of aqueous salts systems over a wide temperature

range"; J. Appl. Chem. (USSR); 48, 1910-1912 (1975)

Zc, Ql, 25°C, in mixt. of CI

SO,, 2 ".

CO, and

Zc, Ql, 25-60°C,

NH^Cl(aq) and

NH<,HC03 (aq) .

33CLI/HUN: Clifford, I.L.; Hunter, E.; "The system ammonia-water at the temperatures up to 150 °C and at pressures up to twenty atmospheres"; J. Phys. Chem.; 37, 101 (1933)Pv, Zc, 60-100°C to

1 . 5 atm. , 0 . 02-10 atm.

NH 3 to 25%, correlation

to 10 atm.

82COB/MUR: Cobble, J.W. ; Murray, R.C., Jr.; Turner, P.J.; Chen, K.

"High temperature thermodynamic data for species in aqueous

solution"; EPRI NP-2400 Research Project 1167-1; (1982)

Zr, 0-200°C, thermal functions.

76
73COU/PET: Couturier, Y. ; Petitfaux, C; "Composition and stability

of cupric and cuprous complexes of aminopyridines . II. complexes of 3-amino-pyridine in aqueous solution"; Bull.

Soc. Chim. Fr . ; *(2)(Pt.l), 445-451 (1973);

[CA 78:128998j]

Kk, 20°C, Cited in 76SMI/MAR.

77D'A/SUR: D'Ans, J.; Surawslio, H.; Synowietz, C; "Specific heat

of solutions"; 'Landolt - Bornstein Zahkerwerte und functionen aus Naturwissenschaften und Technik';

*Gruppe IV, Neue Serie, Band I, Teil b, 274-275 (1977)

Ql, 2-61°C, 1-25

wt%.

1898DEL: Delepine, M. ; "Amines et amides derives des aldehydes";

Ann. Chim. Phys.; [7], 15, 469-574 (1898)

Hr, T = ?, reaction with

HC1.

66DUR/SCH:

63DVO/BOU:

78EDW/MAU:

75EDW/NEW:

78EDW/NEW:

Durst, R.A. ; Schmidt, P.G.; Feldman, I.; "Mass spectrometric

method for the determination of the activity coefficient

of ammonia in aqueous salt solutions"; J. Phys. Chem.

70, 2058 (1966)

Dvorak, K. ; Boubkik, T.; "Liquid-vapour equilibria. XXIX. Measurement of equilibrium data in systems with high

equilibrium ratio of the components"; Coll. Czech. Chem. Commun.; 28, 1249-1255 (1963)

Edwards, T.J.; Maurer, G. ; Newman, J.; Prausnitz, J.M.

"Vapor-liquid equilibria in multicomponent aqueous solutions of volatile weak electrolytes"; AIChE J.; 24(6),

966-976, (1978)

Edwards, T.J.; Newman, J.; Prausnitz, J.M. ; "Thermodynamics

of aqueous solutions containing volatile weak

electrolytes"; AIChE J.; 21(2), 248-259, (1959)

Edwards, T.J.; Newman, J.; Prausnitz, J.M.; "Thermodynamics

of vapor-liquid equilibria for the ammonia-water system";

Ind. Eng. Chem. Fundam. ; 17(4), 264-269 (1978)

Px, Pv, Da, and

22°C, m(NH3 )=0-4 in salt solns.

Pv, 90°C, 0.3 - 2.3 wt% NH3 in sol.

Zc, Pv, Kk, 0-170°C,

I to 6m.

Zc, Pv, 0-100°C,

Zc, Da, Pv, 60-170° F, X(NH3

) = 0-1

64EFR/PRY: Efremova, G.D.; Pryanikova, R.O. ; "Phase and volume

relations in the adipodinitrile-ammonia system"; Zh.

Fiz. Khim.; 38, 686 (1964)

Pv, Hm, 25-125°C.

77
24ELL: Elliott, L.D.; "The freezing point curve of the system

water-ammonia"; J. Phys . Chem. ; 28, 887-888 (1924)

Px, -97 to -77°C,

liquidus

75EME/RUS: Emerson, K. ; Russo, C; Lund, R.E.; Thurston, R.V. ; Kk, 0-30°C, pH 6-10. "Aqueous ammonia equilibrium calcualtions . Effect of pH and temperature"; J. Fish. Res. Board Can.; 32, 2379-2383 (1975)

79ERO/BAB: Eroshchenkov, S.A.; Babichenko, A.K.; "Calculation of Pv? (not seen),

compositions of equilibrium phases of water-ammonia

solutions"; Vestn. Khar'kov. Politekhn, In-ta; 78(145), 54-56 (1979) [CA 91:28082]

62ESV/TYR: Esval, O.E.; Tyree, S.Y. Jr.,; "The activity coefficients Da 25°C, nUNH^ClO^)

of ammonium perchlorate in water at 25°" ; J - Phys chem -

i = 0.1-2.1.

66, 940-942 (1962)

54EVE/LAN: Everett, D.H.; Landsman, D.A.; "A redetermination of the Kk , Hr , 25-45°C,

dissociation constant of the ammonium ion and the base [NH^+

]<0 . 04m, in strength of ammonia in water"; Trans. Faraday Soc . ; 50, HCl(aq).

1221-1229, (1954)

38EVE/WYN: Everett, D.H.; Wynne-Jones, W.F.K.; "The dissociation of Kk, 5-45°C, I to the ammonium ion and the basic strength of ammonia in 0.2m, in NH^Cl(aq).

water"; Proc . Roy. Soc; A169, 190-204 (1938)

52EVE/WYN : Everett, D.H.; Wynne-Jones, W.F.K.; "The dissociation Kk, Hr , Q, 0-40°C, constants of the ammonium and methyl ammonium ions in 60% I<0.2m, NH3/NH4CI in aq. aqueous methanol"; Trans. Faraday Soc.; 48, 531-536 MeOH.

(1952)

1853FAV/SIL: Favre, P. A. ; Silbermann, J.T.; "Recherches sur les Hm, 15°C, dil. sol. quantities de chaleur degages dans les actions chemiques

et moleculaires"; Ann. Chim. Phys.; * (3)37, 406-508

(1853)

00GAU: Gaus , W. ; "liber den Einfluss von Neutralsalzen auf die Pv, 25°C,

Tension des Ammoniaks aus wasseriger Losung"; Z. Anorg. m(NH3)<1.0.

Allgem. Chem.; 25, 236-264 (1900)

78
80GIG:

1884GUN:

75HAK:

77HAK/EDW

79HAL/DRE

30HAR/OWE

58HAR/OWE

28HAR/R0B

67HEL:

Giggenbach, W.F.; "Geothermal gas equilibria"; Geochim.

Cosmochim. Acta; 44, 2021-2032 (1980)

Pv, 100-300°C,

application of previously published

data to geocheroical

equilibria

.

Guntz, A.; "Recherches thermiques sur les combinaisons du Hr, 13°C, reaction

fluor avec les metaux"; Ann. Chim. Phys . ; [6], 3, 5-66 with HF(aq), quoting

(1884) earlier work.

Hakuta, T.; "Vapor-liquid equilibrium of polluting Pv, 80-100°C, NH 3 = materials in sea water. 1. Vapor-liquid equilibrium of 1.2-10.6 ppm. , pH 6~t ammonia-water system"; Nippon Kaisui Gakkai-Shi in borate buffer.

28, 353-359 (1975)

Hakuta, T.; Edwards, T.J.; Prausnitz, J.M.; "Vapor-liquid Pv Zc , Kk, 273-400 K

equilibria pf some pollutants in aqueous and saline Speciated model for weak

solutions. Part II. Correlation for dilute weak electrolytes in water. electrolytes in aqueous buffered solutions"; Desalination;

21, 23-33 (1977)

Hales, J. M. ; Drewes, D. R. ; "Solubility of ammonia in Pv, 280-300 K ' water at low concentrations"; Atmos . Environ.; 13, m(NH.j= 3x10"'' in H£0 and 1133-47 (1979) in very dilute H2SOA

Harned, H.S.; Owen, B.B.; "The thermodynamic properties of Ze, Kk, 25°C. weak acids and bases in salt solutions, and an exact method of determining their dissociation constants";

J. Am. Chem. Soc . ; 52, 5079-5091 (1930)

Harned, H.S.; Owen, B.B.; 'The Physical Chemistry of Kk, 25°C. Electrolyte Solutions' Reinhold Publ. Corp., New York, 3d

ed.; (1958)

Harned, H.S.; Robinson, R.A. ; "The ionic concentrations Kk, 25°C, I<1.5. and activity coefficients of weak electrolytes in certain

salt solutions"; J. Am. Chem. Soc; 50, 3157 (1928)

Helgeson, H.C.; "Thermodynamics of complex dissociation Ze, Kk, 0-306°C.

in aqueous solution at elevated temperatures"; J. Phys. Chem.; 71, 3121-3136, (1967)

79
76HEL/KIR: Helgeson, H.C.; Kirkham, D.H.; "Theoretical prediction of Kk, Zc , Ze, the thermodynamic properties of aqueous electrolytes at 25-3000°C,

high pressures and temperatures. III. Equation of state 1-1000 atm. for aqueous species at infinite dilution"; Am. J. Sci .

276, 97-240 (1976)

81HEL/KIR: Helgeson, H.C.; Kirkham, D.H. ; Flowers, G.C.; "Theoretical Ze, Kk, Da, Dm, prediction of the thermodynamic behavior of aqueous 0-600 °C, 0-5kB. electrolytes at high pressures and tempeatures: IV. Calculation of activity coefficients, osmotic coefficients,

and apparent molal and standard and relative partial molal

properties to 600°C and 5kB"; Am. J. Sci.; 281, 1249-1516

(1981)

11HER: Herzen, E.; "Abaque des tensions de vapeur d'une solution Zc , Pv, 0-150°C, aqueuse ammonicale"; Bull. Soc . Chem. Beige; 25, 154-157

(1911)

53HIL/GIA: Hildenbrand, D.L.; Giauque, W.F.; "Ammonium oxide and ammonium hydroxide. Heat capacities and thermodynamic

properties from 15 to 300 K" ; J. Am. Chem. Soc; 75 2811-2818 (1953)

Ql, 25°C, on

NH

3 (H20), and from -73

to -18°C, on more

cone. sol.

76HIT/MES: Hitch, B. F. ; Mesmer, R. E. ; "The ionization of aqueous Kk , 50-300°C, p to 100 ammonia to 300°C in KC1 media"; J. Solution Chem.; 5, bar, in KC1. 667-79 (1976)

75HOS/NAG: Hoshino, D.; Nagahama, K. ; Hirata, M. ; "A new apparatus

for measuring vapor-liquid equilibria of gas-solvent

systems at constant pressure"; Bull. Jap. Petrol. Inst.;

17, 9-13 (1975)

Pv, x=0-l, 1 atm, E=-40-100 3 C.

25H0U: Hougen, O.A. ; " Absorption of ammonia "; Chem. Met. Eng.

32(14), 704-705 (1925)

Zc, Pv, 15-25°C, p(NH 3

) meas ,

78IKE/SAS: Ikemizu, K. ; Sasaki, K. ; Morooka, S.; Kato, Y . ; Shinohara,

H.; "Dif fusivities and solubilities of NH 3 gas in aqueous solutions of ammonium salts"; Kagaku Kogaku

Rombunshu; 4(3), 273-276 (1978)

Pv, 35-65°C, NH 3 = 3-12 m, solubility in water and aq. mixt. of

80
71JAI/GAB : Jain, P.C.; Gable, G.K. ; "Equilibrium property data equations for aqua-ammonia mixtures"; Amer . Soc . Heat., Refrig. Air-Cond. Eng., Trans.; 77 (pt.l), 149-151

(1971)

Zc, Pv, 22-132°F,

50-350 psia, equation

for data in 64MAC/EAK.

65JEN:

63 JON:

07KAN:

Jennings, B.H.; "Ammonia-water properties (Experimentallydetermined P,V,T,x liquid-phase data)"; ASHRE Trans.; 711, 21-29 (1965)

Jones, M.E.; "Ammonia equilibrium between vapor and liquid

aqueous phases at elevated temperatures"; J. Phys . Chem.

67, 1113-1115 (1963)

Kanolt, C.W.; "Ionization of water at 0° 18°and25° derived from conductivity measurements of the hydrolysis

of the ammonium salt of diketotetrahydrothiazole" ; J. Am. Chem. Soc; 29, 1402-1416 (1907)

Pt, Xd, 10-100Zwg NH 3

, t=75-312°C, 7-540 psi

Pv, 147-318°C,

2,20,200 ppm.

Kk, 0-25°C.

71KAR: Karov, E.G.; "Isothermal invariant points"; Zh. Neorg.

Khim. ; 16(11), 3110-14 (1971)

Pv, 25°C, 720 mmHg.

57KAU/DOG: Kauko, Y. ; Doger, S. ; "Bestimmung kleiner Mengen von

Ammoniak in Gasmischungen" ; Acta Chem. Scand. ; 11, 804-810 (1957)

Pv, Kk, 25 and 40°C.

30KIN/HAL: King, H.H. ; Hall, J.L.; Ware, G.C. ; "A study of the density, surface tension and adsorption in the water-ammonia system at 20°": J - Chem - Soc - 52 ' 5128-5135 (1930)

Vx, 20°C, x(NH3 )= .20-1.00, density data.

72KIR/TRU: Kirintsev, A.; Trushnikova, L.N.; Lavrent'eva, V.G.

'Handbook of phase diagrams of inorganic substances

in water'; Khimiya, Leningrad, 95-96 (1972)

Px, -100 to 0°C, x=0 to 1.

62KIS: Kiseleva, E.V.; "About the state of ammonia in aqueous

solutions"; Tr. Mosk . Khim. -Tekhnol . Inst.; *(38), 71 (1962)

Pv, 20 and 30°C,

p(NH

3

) and p(H20) meas

24KLA: Klarmann, E.; "Das Henrysche Gesetz bei wassrigen

Ammoniaklosungen und die Hydrolyse der Ammonsalze"; Z. Anorg. Chem.; 132, 289-300 (1924)

Pv, Kk, 0-25°C, NH 3 (aq) and NH^Ac

81
67KOM/SUN: Komar ' , N.P.; Sung, N. T . S.; "Protonation of weak bases: The NH3 + H

30

+

= NH^ +

+ H20 system";

Russ. J. Inorg. Chem. ; 12 (5), 669-675 (1967)

Kk, 25°C, I<3,

73KON/LAN: Koneczny, H. ; Lango, D.; Lango, M. ; "System potassium

chloride-ammonia-water"; Chem. Stosow. ; 17, 115-125

(1973); [CA 80-41382w]

Px, 20-6CTC,

in sat . KC1( aq)

75KON/LAN: Koneczny, H. ; Lango, D.; Lango, M. ; "Potassium sulfate- ammonia-water system"; Chem. Stostow. ; 19, 27-36 (1975);

[CA 83-33493e]

Px, 20-60°C, 0-25% NH3

, in

sat. K2SO^(aq).

74KON/SAS: Kononenko, A.F.; Sashevskaya, Z.G.; "Relation of density

and viscosity to temperature for some salt solutions";

Zh. Priklad. Khim. ; 47, 211-212 (1974)

Pv, Vx, -20 to 20°C, cone . NaCl(aq)

25KOW/HOU: Kowalke, O.L.; Houge, O.A. ; Watson, K.M. ; "Absorption of ammonia in towers"; Chem. Met. Eng.; 32, 443-446 (1925)

Zc, Pv, 0-7% NH-.

28KRA: Kracek, F.C. ; "P-T-X relations for systems of two or more Ze, Pv, Px, components and containing two or more phases (L-V, -89 to 170 °C, L 1~ L2~V and S_L_V systems)"; 'International 5-100% NH3

. Critical Tables' , Washburn, E.W. , ed; 3, 351-385, (1928);

p. 362 for NH3

.

30KRA: Kracek, F.C; "Vapor pressures of solutions and the Ramsay-Young rule. Application to the complete system

water-ammonia"; J. Phys . Chem.; 34, 499-521 (1930)

Ze, Pv, Px, -89 to 170°C,

24LAR: Larsson, E.; Diss Lund.; (1924) Kk, 25°C, in H

20-EtOH,

cited in 64SIL/MAR.

34LEW/SCH: Lewis, G.N.; Schutz, P.W.; "The ionization of some weak electrolytes in heavy water"; J. Am. Chem. Soc . ; 56, 1913-1915 (1934)

Kk, 25°C, ND3 in

65LIN: Linke, W.F.; 'Solubilities'; American Cyanamid Co., Stamford, Conn., 4th ed . ; 2, 590-603 (1965); originated

by Atherton Seidell, Ph.D.

Zr, Pv, in H

2

0, salt solns., organic

solvents and mixed systems,

major compilation.

82
04LOC/FOR:

07LUN:

Locke, J. ; ForssalL, J. ; "The action of ammonia upon copper sulphate solutions"; Am. Chem. J.; 31, 268-302 (1904)

Lunden, H. ; "Hydrolyse des sels des acides faibles et des bases faibles et sa variation avec la temperature"; J. Chim. Phys.; 5, 574-608 (1907)

Pv, 25"C, [NHg] to 1, [Cu-2

] to 0.11.

Kk, 10-50 °C, NH3 and

08LUN: Lunden, H.; "Influence de la temperature sur l'energie

interne et l'energie libre des dissociations

electrolytiques des acides et bases faibles"; J. Chim. Phys.; 6, 681-698 (1908)

Kk, Hr, 10-50°C,

reaction with acid.

64MAC/EAK: Macriss, R.A. ; Eakin, B.E.; Ellington, R.T.; Huebler, J. "Physical and thermodynamic properties of ammonia-water

mixtures"; Research Bulletin, No. 34, American Gas Assn.

(1964)

Pv, 140-200°F, 96-100% NH3

, 200-500 psia, Ql, Qg

106-441°F, 50-500 psia,

Vt, Zc, -50 to 400°F, 0-450 psia.

71MAC/R0R: MacKellar, W.J.; Rorabacher, D.B.; "Solvent effects in coordination kinetics. I. Inner-sphere effects in the reaction of solvated nickel(II) ion with ammonia in methanol-water mixtures"; J. Am. Chem. Soc . ; 93, 4379-

4387 (1971)

Kk, 25°C, citing

71R0R/MAC and unpub.

work

79MAE/ARN: Maeda, M. ; Arnek, R. ; Biedermann, G. ; "A potentiometric

and calorimetric study of the system Ag+ -NH3 in 3M NaClO^, 3M LiClC^ and 3M NaN03 media";

J. Inorg. Chem.; 41, 343-346 (1979)

Kk, Hr, 25°C, in C10^~(aq) and N03 ~(aq

from data on Ag+-NH 3 complexes

1897MAL: Mallet, J.W. ; "On the solubility of ammonia in water at temperatures below 0°C"; Am. Chem. J.; 19, 804-809 (1897)

Pv, -40 to -10°C,

74mmHg

4 1MAR/K0B : Markham, A.E.; Kobe, K.A. ; "The solubility of gases in liquids"; Chem. Rev.; 41, 519-588 (1941)

Zr, Pv, methods,

thermodynamic formulae,

bibliography, data quality but no values

for solubilities.

67MAR/KAT: Martynova, O.I.; Katkovskaya, K. Ya. ; Vaineikis, A.; Dubrovskii, I. Ya. ; Feodoseichuk , T. A.; "The effect of solution ionic composition on the distribution of ammonia

between water and saturated vapor"; Teploenergetika

14(12), 39-42 (1967)

Pv, 25 and 230-300°C, pH = 3 to

8, in nitrate sol.

83
02MAS: Massol, G. ; "Chaleurs de dissolution de 1 ' ammoniaque solide

et liquids prise vers -75° et chaleur latent de fusn de

1 ' ammoniaque solide"; Compt. Rend.; 134, 653 (1902)

Hm, NH 3(at. -75°C)

into water (at

10°C)

25MIC/MIZ: Michaelis, L.; Mizutani, M. ; "Die Dissoziation der schwachen Elektrolyte in wasserig-alkoholischen Losungen"

Z. Phys. Chem. ; 116, 135-139 (1925)

Kk, 18°C.

55MIR: Mironov, K.E.; Zh. Obshch. Khim. ; 25, 1081-1086 (1955);

"Diagram of the phase transformations of the system h^O- NH3

"; J. Gen., Chem., USSR; 25, 1039 (1955)

Px, -123 to 0°C,

x(NH3

) = 0-1.0,

liquidus

08MOL: Mollier, H. ; "Dampfdruck von wassrigen Ammoniaklosugen"

Z. Ver. Dtch. Ing.; 52(3), 1315-1320 (1908)

Pv, 10-120°C, x(NH3

) = 0,1-0.5.

12MOO/WIN: Moore, T.S.; Winmill, T.F.; "The state of amines in aqueous Kk , 18-35°C(?),

solution"; J. Chem. Soc; 101, 1635-1676 (1912) calc.

31MOR/MAA: Morgan, O.M. ; Maass, 0.; "An investigation of the equilibria existing in gas-water systems forming

electrolytes"; Can. J. Res.; 5, 162-199 (1931)

Pv, Kk, 0-25°C, P <

1 atm

00NEW: Newth, G.S.; "Note on partially miscible aqueous inorganic

solutions"; J. Chem. Soc; 77, 776-788 (1900)

Px, 1-43°C, sol. in K

2C03 (aq)

21NEU/PAT: Neuhausen, B.S.; Patrick, W.A. ; "A study of the system

ammonia-water as a basis for a theory of the solution of gases in liquids"; J. Phys. Chem.; 25, 693-720 (1921)

Pv, Vx, 0, 20, A0°C,

1000-4000mmHg, p(NH3

) and p(H2

0).

07NOY: Noyes, A. A. ; 'The electrical conductivity of aqueous solutions'; Publication 63, Carnegie Institution of Washington, 153-234 (1907)Kk, 18-306°C,Psat

NH

3 (aq) and NH^Ac(aq).

08NOY: Noyes, A. A. ; "The conductivity and ionization of salts,

acids, and bases in aqueous solutions at high temperatures'

J. Am. Chem. Soc; 30, 335-352 (1908)

Kk, 18-306°C,Psat

10NOY/KAT: Noyes, A. A. ; Kato, Y . ; Sosman , R.B.; "The hydrolysis of ammonium acetate and the ionization of water at high

temperatures"; J. Am. Chem. Soc; 73, 159-178 (1910)

Kk, 18-306°C,Psat

NH 3 (aq) and NH^Ac(aq)

84
10NOY/KAT2: Noyes, A. A. ; Kato, Y . ; Sosman, R.B.; "Die Hydro lyse von

Ammoniumacetat und die Ionisation von Wasser bei hohen

temperaturen" ; Z. Phys . Chem. ; 73, 1-24 (1910);

Translation of 10NOY/KAT

Kk, 0-300°C,Psat

hydrolysis of NHg(aq)

750LO: Olofsson, G. ; "Thermodynamic quantities

for the dissociation of the ammonium ion and

for the ionization of aqueous ammonia over a wide

temperature range"

J. Chem. Thermodyn. ; 7, 507-14 (1975)

Kk, Hr, Qh, 278-418 K.

340WE: Owen, B.B.; "The determination of the dissociation

constants of weak bases by the silver iodide electrode'

J. Am. Chem. Soc . ; 56, 2785-2786, (1934)

Kk, 25°C.

65PAO/STE:

65PAR:

Paoletti, P.; Stern, J.H.; Vacca, A.; "Thermochemical

studies. XV. Thermodynamics of protonation of triethylenediamine , trimethylamine , and ammonia in aqueous solution at 25°C"; J. Phys. Chem.; 69, 3759-3762 (1965)

Parker, V.B.; "Thermal properties of aqueous uni-univalent

electrolytes"; NSRDS-NBS 2; 1-66, (1965)

Kk, Hr, 25°C, NH^Cl.

Ze, Ql, Hm, 25°C,

NH^taq) and ammonium

salts

37PEA/PUM: Pearce, J.N. ; Pumplin, G.G. ; "The vapor pressures and activity coefficients of aqueous solutions of ammonium

chloride at 25°C"; J. Amer. Chem. Soc; 59, 1219-1220

(1937)

Pv, Da, 25°C,

M(NH4 C1) to 7.3.

80PEN/ROB:

01PER:

Peng, D.-Y.; Robinson, D.B.; "Two- and three-phase

equilibrium calculations for coal gasification and related

processes"; ACS Symp. Ser.; No. 133, 393-414, (1980);

Thermodyn. Aqueous Syst. Ind. Appl.

Perman, E.P.; "Vapour pressure of aqueous ammonia solution. Part I"; J. Chem. Soc; 81, 718-725 (1901)

Zc, Pv, 100-300° F,

of VLE data,

Pv, 0-60°C,

01PER2: Perman, E.P.; "Influence of sodium sulfate on the vapour pressure of aqueous ammonia solution"; J. Chem. Soc.;

81, 725-729 (1901)

Pv, 26-47°C,

35
iX'O" '* '• ti J' t' Jf' I' *« I* !• f* I* i> v

\> 4

.

' :

k . > Of, f> ft, H.. |. J %i (, lv 1» (• | [, j, f/

* I *

02PER: Perman, E. P.; "The influence of salts and other substances on the vapour pressure of aqueous ammonia

solution"; J. Chem. Soc . ; 81, 480-89 (1902)

Pv, 20-60°C 150-1000 mmHg , sol. in aq. urea, manitol KC1, NH 4 C1, CuCl2

.

03PER: Perman, E.P.; "Vapour pressure of aqueous ammonia solution. Pv, 0-60°C, 0-305 Part II"; J. Chem. Soc; 83, 1168-1184 (1903) NH,

.

59PIE: Pierre, B.; "Total vapor pressure in bars over aqueous Pv, 175-650 psia, NH3 up ammonia-water solutions" Kyltek . Tidsk . ; Aug (1959), to AO wt.%, as cited in sheet 14. 64MAC/EAK.

37PIT: Pitzer, K.S.; "The heats of ionization of water, ammonium Hr, Ql, 25°C,

hydroxide, carbonic, phosphoric, and sulfuric acids. The ionization,

variation of ionization constants with temperature and the entropy change with ionization"; J. Am. Chem. Soc; 59, 2365-2371 (1937)

75POL/LU: Polak, J.; Lu, B.C.-Y.; "Vapor-liquid equilibria in system Pv, 90-100°C, 15,65

ammonia-water at 14.69 and 65 psia"; J. Chem. Eng. Data; psia, x(NHj) to 0.043.

20, 182-3 (1975)

20POS: Postma, S.; "Le systeme ammoniaque - eau" ; Rec. Trav. Chim.; 39, 515-536 (1920)

Pv, Px, +65°C.

-103 to

68QUI/MAR: Quist, A.S.; and Marshall, W.L.; "Ionization equilibria in ammonia-water solutions to 700 °C and to 4000 bars of pressure"; J. Phys . Chem.; 72(9), 3122-8 (1968)

Kk, 0-700°C, up to 4000 bar,

m(NH3 )=0.01-0.05.

74RAB/OZU : Rabenstein, D. L . ; Ozubko , R.; Libich, S.; Evans, C.A.; Kk , as cited in 76SMI/MAR.

Fairhurst, M.T.; Suvanprakorn , C; "Nuclear magnetic resonance studies of the solution chemistry of metal

complexes X. Determination of the formation constants of the methylmercury complexes of selected amines and aminocarboxylic acids"; J. Coord. Chem.; 3(4), 263-271

(1974) ; [CA 82:65120b]

31RAM/HAN: Ramstetter, H.; Hantke, G. ; "Eine neue Methode zur Hm, 20°C, m(NHj

)

Messung von Warmetonungen" ; Z. Phy . Chem. Bodenstein 0.15 - 2.6. Festband; 662-668 (1931)

86
1874RAO: Raoult, F.-M.; "Recherches sur 1' absorption de l'ammoniaque par les dissolutions salines"; Ann. Chim. France; *[5] 1, 262-274 (1874)

Pv, 0-28°C, in water

and salt solutions.

67RAS/CHE: Rashkovskaya , E.A.; Chernen ' kaya , E.I. NaHCOQ , NH.C1

'Densities of

and of ammonia in the 20-100° range"; Zh. Prikl. Khim.

40, 301-308 (1967); Russ. J. Appl. Chem. ; 40, 289-295 (1967)

Xd, 2-16% NH 3 20-100°C p=l atm.

03REI: Reisenfeld, H.; "Uber das Losungsvermogen von Salzlosungen

fur Ammoniak nach Messungen seines Partial drukes. II.";

Z. phys. Chem.; 45, 467 (1903)

Pv, 35"C, in aq. soln. of K and Na salts

77RIC/NED: Rice, N.M. ; Nedved, M. ; "Dissociation constant of ammonium ions at high ionic strength"; Chem. Ind.

July 2, 539-540 (1977)

Kk, 25°C,

59ROB/STO: Robinson, R.A. ; Stokes, R.H. ; 'Electrolyte solutions'

Butterworths , London, 2nd Ed.; (1959)

Ze, Kk, Da, various

temperatures

56ROL/VUI: Rollet, A. P.; Vuillard, G. ; "Sur un nouvel hydrate de l'ammoniac"; Compt. Rend.; 243, 383-386 (1956)

Px, -50 to -103°C,

liquidus

71R0R/MAC: Rorabacher, D.B.; MacKellar, W.J.; Shu, F.R.; Bonavita, M.

"Solvent effects on protonation constants. Ammonia, acetate,

polyamine, and polyaminocarboxylate ligands in methanol- water mixtures"; Anal. Chem.; 43, 561-572 (1971)

Kk, 25 °C, in H

20 and mixt . with MeOH.

10RUP: Rupert, F.F.; "The solid hydrates of ammonia. II.";

J. Am. Chem. Soc . ; 32, 748-749 (1910)

Px, -100 to 0°C,

liquidus

51SAN/Y0U: Sanders, B.H. ; Young, D.A.; "Graphical correlation of physical properties of a ternary system Vapor pressure and specific gravity for ammonia- ammonium nitrate-water"; Ind. Eng. Chem.; 43, 1430-1433 (1951)Vx, Pv, Zc, 30-120°F, binary and ternary systems

correlated, no new data

47SCA/EPS: Scatchard, G.; Epstein, L.F.; Warburton, J., Jr.; Cody,

P.J.; "Thermodynamic properties of NH3-H2O liquid

and vapor mixtures from -60°F to 370°F and from 0-100%

NH 3 in liquid"; J. Am. Soc. Refrig. Eng.; 413-419, 446,

450, 452 (1947)

Zc, Pv, Vg, -60-370°F, x(NH 3 )=

0-1, enthalpy and PvTx

87
25SCH/WIJ

:

Scheffer, F.E.C.; de Wijs, H.J.; "Sur des solutions

d'ammoniac"; Rec . Trav. Chim. ; 44, 655 (1925)

Pv, 25°C.

73SCH: Schulz, S.C.G.; "Equations of state for the system

ammonia-water for use with computers"; Progr . Refrig. Sci. Technol. , Proc . Int. Congr. Refrig.; 13th, 2, 431-6

(1973)

Zc, Vg, Vx, 200-450 K 0.01-25

bar, theory, data, sources not cited.

36SCH/EPP: Schwarzenbach , G.; Epprecht, A.; Erlenmeyer, H.; "Uber Dissoziationskonstanten in Wasser und Deuteriumoxyd.

Messungen mit der Deuter iumelektrode" ; Helv. Chim. Acta;

19, 1292-1304 (1936)

Kk, 20°C, m = 0.007,

NaOH(aq)

.

25SHE: Sherwood, T.K.; "Solubilities of sulfur dioxide and ammonia in water"; Ind. Eng. Chem. ; 17, 745-747 (1925)

Zc," Pv, 0-60°C, p 10-1000 mmHg.

62SHU/MAK: Shul'ts, M.M. ; Makarov, L.L.j Yu-jeng, S.; "Activity

coefficients of NH^Cl in binary and ternary solutions

at 25°"; Russ. J. Phys . Chem.; 36(10), 1181-1183 (1962)

Da, 25°C, m(NHA Cl)

2 to 7.

66SHU/SIM: Shul'ts, M.M. ; Simanova, S.A. ; "Activity coefficients of ammonium bromide in aqueous solutions at 25 •' ^uss - J- Phys. Chem.; 40(2), 247-248 (1966)

Da, 25°C, 1.1-7.9 m, activity of NH^Br(aq).

73SIN: Singh, N.M. ; "Transport and equilibrium properties of water-ammonia gaseous mixtures"; Progr. Refrig. Sci. Technol., Proc. Int. Congr. Refrig.; 13th, 2, 473-80

(1973)

Zc, Vg, 323-673 K, fugacity

.

72SLO/ORE: Slobodkina, G.L.; Orekhov, I.I. ; Sverdlova, V.P.; "Vapor pressures of water and ammonia over ammoniated phosphoric

acid solutions"; Tr . Sev.-Zap. Zaoch. Politekh. Inst.; *(21), 8-12 (1972); [CA 80:41154y]

Pv, Hp, Da, 30-90°C,

in 13-60% H 3 P04 (aq).

53SPI: Spike, C.G.; "Entropy factors in chelation"; Diss. Abstr.

Publ. No. 5098; U. Michigan, (1953)

Kk, Cited in 76SMI/MAR.

77SYN: Synowietz, C.j "Densities of binary aqueous systems"; 'Landolt - Bornstein Zahlenwerte und functionen aus Natuwissenschaften und Technik'; "Gruppe IV, Neue Serie, Band 1, Teil b, 69-70 (1977)

Vx, 0-100°C, 1-100

wtZ.

88
1882THO: Thomsen, J.; ' Thermochemische Untersuchungen' , Barth,

Leipzig; (1882-86)

Hm, 18°C, (vol. 2 pg 72), Hr, 18°C,

neutral, (vol. 1, pg

312)

80THU/RUS: Thurston, R.V. ; Russo, R.C.; Emerson, K.M. ; Gov. Rep. Announce. Index (U.S.); "Aqueous ammonia equilibrium - tabulation of percent un-ionized ammonia"; 80(1); 55 (1980)

65TSI/LIN: Tsiklis, D.S.; Linshits, L.R.; Goryunova, N.P.; "Phase equilibria in the system ammonia-water"; Russ . J. Phys

Chem.; 39, 1590-1592 (1965)

Kk, Zc, 0-40°C

pH=5-12, Tables of un-ionized NH3

,

Pv, 0-100%wg NH 3 t=97-320°C.

72VAN/KIN: Vanderzee, C.E.; King, D.L.; "The enthalpies of solution

and formation of ammonia"; J. Chem. Thermodynamics; 4, 675-683 (1972)

Ze, Hm, 25°C,

vfH(NH

3 ,g).

72VAN/KIN2: Vanderzee, C.E.; King, D.L., Wadso, I.; "The enthalpy of ionization of aqueous ammonia"; J. Chem. Thermodyn.;

4, 685-689 (1972)

Hr, 25°C, sol. of

68VAS/KOC: Vasil'ev, V.P.; Kochergina, L.A.; "Heat of ionisation of Hr, 18-40°C, I = ammonium hydroxide in sodium nitrate solutions at various 0.5-3m, in acidified aq. temperatures"; Russ. J. Physical Chemistry; 42(2), NaN03

. 199-202 (1968)

60VOR/PRI: Vorob'ev; A.F.; Privalova, N.M. ; Monaenkova, A.S.; Hr, 25°C,

Skuratov, S.M. ; "Standard enthalpy of formation of neutralization,

hydrochloric acid and some perchlorates" ; Dokl. Akad. Nauk

SSSR; 135(6), 1388-1390 (1960)

23VRE/KAI: Vrewskii, M.S.; Kaigorodov, A.N. ; "Heat capacity of aqueous Ql, Pv, 2.4°C -

solutions of HCL and NH 3 "; Zhur. Russ. Fiz-Khim. 60.9°C, 1.39% to Obschest, Chast Fiz ches . ; 54, 336-347 (1923)

03 PER

23VRE/ZAV: Vrewskii, M.S.; Zavaritskii, N.N.; "Measuring the heat of Hm, 199, 41°C,

solution of gas in water"; Zhur. Russ. Fiz. Khim. , m(=.3405 to 0.61). Obshch. Clast; 54, 348 (1923)

***VREWSKII , SEE ALSO WREWSKY*'"'

89
06WHE: Whetham, W.C.D.; "Die elektrische Leitfahigkeit verdunnter

Losungen von Schwefelsaure" ; Z. Phys . Chem. ; 55, 200-205

(1906)

Kk, 18°C, with

80WIL/OWE: Wilson, G.M. ; Owens, R.S.; Roe, M.W. ; "Sour water

equilibria. Ammonia volatility down to ppm levels. pH vs. composition and effect of electrolytes on ammonia

volatility"; ACS Symp; Ser. 133 (1980); (Thermodyn.

Aqueous Syst . Ind. Appl.)

Pv, 80-120°C,

NH3 =0. 09-10 wtZ, [NH3

] and p(NH3

) meas; includes effect of NaOH and Na-acetate (0-25%).

25WIL: Wilson, T.A.; "The total and partial vapor pressures of aqueous ammonia solutions"; Bull., Univ. 111. Eng. Expt.

Sta.; 146, (1925)

Pv, 32-190° F ' P t0

170 psia, as cited in 64MAC/EAK.

53WIS/STO:

54WIS/STO

:

Wishaw, B.F.; Stokes, R.H.; "The osmotic and activity

coefficients of aqueous solutions of ammonium chloride and ammonium nitrate at 25°": Trans Far aday Soc • i « 9 . 27 " 31 (1953)

Wishaw, B.F.; Stokes, R.H.; "Activities of aqueous ammonium sulphate solutions at 25°" ; Trans - Faraday Soc

50, 952-954 (1954)

Da, 25°C, m(NH^Cl)

to 7.4, m(NHA N0 3

) to 25.9.

Da, 25°C, m(NH^S04

) = 0.1 to 5.8.

80WON/SEL: Won, K.W. ; Selleck, F.T. ; Walker, C.K.; "Vapor-liquid

equilibria of the ammonia-water system"; EFCE Publ. Ser. 11 (Phase Equilib. Fluid Prop. Chem. Ind.); 45-9

(1980)

Zc.Vg, No new data. Reassessment of work of 64MAC/EAK and 32CLI/HUN.

74WOR/DUN: Worswick, R.D.; Dunn, A.G. ; Staveley, L.A.K.; J. Chem. Thermodyn.; "The enthalpy of solution of ammonia in water

and in aqueous solutions of ammonium chloride and ammonium

bromide"; 6(6); 565-70 (1974)

Hm, 298.15 K, m(NH3)=l-4 in H20, NHA Cl(aq) and NH^Br(aq).

24WRE: Wrewsky, M. ; "Uber das Gleichgewicht zwischen Dampf und Flussigkeit wasseriger Losungen des Ammoniaks"; Z. Phys. Chem. ; 112, 117-127 (1924)Hm, 3-60°C, m =

0.8-2.8.

24WRE/KAI: Wrewsky, M. ; Kaigorodoff, A.; "Warmekapazitat wasseriger

Losungen von Chlorwasserstof f und Ammoniak bei verschiedenen Temperaturen" ; Z. Physik. Chem.; 112, 83-89

(1924)

Ql, 3-60°C, m =

0.8-2.8.

90
24WRE/SAW: Wrewsky, M. ; Sawaritzky, N.; "Die Bildungswarmen

waseriger Losungen von HC1 und NHj bei verschiedenen

Temperaturen" ; Z. Phys . Chem. ; 112, 90-96 (1924)

Ql, Hm, 3-60°C, sol and dil.

***WREWSKY , SEE ALSO VREWSKII***

32WUC: Wucherer, J.; "Messung von Druck, Temperatur und Zc , -3 to 200°C, x Zusammensetzung der flussigen und dampfforraigen Phase von 0 to 1, summary and Ammoniak-Wassergemischen im Sattigungszustand. 6. tables. Beurteilung der Ergebnisse und Vergleich mit fruheren

Messungen"; Z. Gesamtes Kalte-Ind . ; 39, 97-104, 136-140

(1932)

78ZAT/DER: Zatorskii, A. A. ; Dergachev, A.G. ; "Determination of parameters of a Kholod. Tekh. Tekhnol.; 25, 67-71

Kokhanskii, A.I..; Zc, t=? , theoret. water-ammonia solution";

(1978); [CA 89:221886h]

39ZHA: Zhavoronkov, N.M. ; "The partial pressure of ammonia,

carbon dioxide and water over copper ammonium solutions";

J. Chem. Ind.; 16(10), 36-37 (1939)

Pv, 20-80°C, Copper

ammonium formate solutions

34ZIN: Zinner, K. ; "The heat content of mixtures of ammonia and Hm, 50°F, 0-100% water dependent upon the composition and temperature"; NHj, as cited in

Z. Gesamt. Kalte-Ind.; 41, 21-29 (1934) 64MAC/EAK.

91
H

2 S-H 2 0

INTRODUCTION

Listed in this bibliography are publications that have

data on the vapor- liquid equilibrium between H2S gas and

its solutions in water or that contain information on the

ionization equilibria in solution among H2S(aq), HS'(aq),

S

2 " (aq) and H

+ (aq)

To a lesser extent there are references on measurement

or calculation of the enthalpies of those processes, on activity coeffients, and on the thermochemistry of the

species mentioned above. Publications reporting measurements

and those presenting correlations or evaluations of data are included, however, references that concern only applications

of existing data to specific problems or models have been

avoided.

The citations are listed alphabetically by first author.

Each is preceeded by a brief identification code (composed

of the year of publication and the first three letters of the

first two authors' names) and contains the author names; the

title of the article, report, or chapter; the name of the source ( j ournal ,book, or issuing agency) and the year of

publication. The structure of these citaions does not

conform to the specifications established by the American

Standards Institute but the information given is sufficient

to direct the reader to the particular reference. In a few

instances only an abstract or secondary reference was available. In these cases either the citation to Chemical

Abstracts or the source of the secondary citation is given.

Some titles have been translated, e.g. those in

Russian. These translations come, preferably, from abstracts

in the papers themselves or from Chemical Abstracts. (The

titles from the latter may be condensations of the original)

92
Each reference is annotated to show the class of data,

the temperature range and, if appropriate, pressure, solution

composition, and pH. The data class designations are taken

from the Bulletin of Chemical Thermodynamics and are two-letter codes with some mnemonic or physical chemical

associations. A list is appended. No attempt has been made

to assess the quality of the data, however, an annotation of

"Ze" indicates that a particular reference constitutes or includes an evaluation of experimental data from several

sources

The bibliography was prepared by searching the files of

the NBS Chemical Thermodynamics Data Center, the Bulletin of

Chemical Thermodynamics and references in the publications

retrieved from those sources. It covers a time period from

the 19th century to 1982. Additions and corrections will be

appreciated

93
04AUE: Auerbach, F.; "Der Zustand des Schwefelwasserstoffs in Mineralquellen" ; Z. Phys . Chem. ; 49, 217-223 (1904)

K, 18°C conductivity

28AUM: Aumeras, M. ; "Sur l'etat d'ionisation des solutions

d'hydrogene sulfure" ; Compt. Rend.; 186, 1724-1726 (1928)

Kk, 16 or 25°C?,

2d, ioniz., from CdS solubility.

66BAT/CLE: Battino, R. ; Clever, H.L.; "The solubility of gases in liquids"; Chem. Rev.; 66, 395-463 (1966)

Pv, 0-60°C,

0-2000mmHg. , bibliography.

67BER:

49BON/RUS:

Berner, R. A.; "Thermodynamic stability of sedimentary iron

sulfides"; Am. J. Sci.; 265, 773-785 (1967)

Bond, D.C.; Russell, N.B.; "Effect of antifreeze agents

on the formation of hydrogen sulfide hydrate"; Trans. AIME;

179, 192-198 (1949)

Kk, 25°C, 1st. ioniz.

Px, 29.5°C.

82BRE: Brewer, L.; "Thermodynamic values for desulfurization

processes"; Am. Chem. Soc . Sytnp. Ser.; 188, 1-40 (1982)

Ze, H, Kk, Qh, 25°C and higher

thermochemical data.

69BUR/GER: Burgess, M. P.; Germann, R.P.; "Physical properties

of hydrogen sulfide-water mixtures"; AIChE J.; 15, 272-275 (1969)

Zc, Pv, 30-170"C,

P(total)=250-340 psia,

refit of tabulated data.

30BUT/MAA: Butler, K.H.; Maass, 0.; "Hydrogen disulfide"; J. Am. Chem. Soc; 43, 2539-2548 (1930)

Qg, 25°C, H

2

S

2

, Cp.

81CAD: Cady, G.H.; "Composition of chlathrate gas hydrates of CHC1F2 , CC13 F, Cl2 , CIO3F, H2

S, and SF 6

"; J. Phys. Chem.; 85, 3225-3230 (1981)

Kk, hydration data, 0°C.

7 1CLA/GLE : Clarke, E. C. W. ; Glew, D. N . ; "Aqueous nonelectrolyte

solutions, part VIII. Deuterium and hydrogen sulfides

solubilities in deuterium oxide and water"; Can. J. Chem.

49, 691-698 (1971)

Pv, 0-50°C, 0.5-1 atm.

64COB: Cobble, J. W. ; "The thermodynamic properties of high

temperature aqueous solutions. VI. Applications of entropy correspondence to thermodynamics and kinetics"; J.

Am. Chem. Soc; 86, 5394-5401 (1964)

Zc, Qh, Da, Pv, Kk

0-300°C, 1st and 2nd ioniz.

94
82C0B/MUR: Cobble, J. W. ; Murray, R. C. Jr.; Turner, P. J.; Chen, K.

'High-temperature thermodynamic data for species in aqueous

solution', EPRI Report NP-2400, Electric Power Research

Institute, Palo Alto, CA, (1982)

Ze, Kk, Pv, 0-350°C, 1st and 2d ioniz.

80COX: Cox, J. D.; "Tentative set of key values for thermodynamics, part VIII"; CODATA Special Report 8; (1980)Ze, 25°C, A

fH, A fG, S for S

2

"

78EDW/MAU: Edwards, T. J.; Maurer, G. ; Newman, J.; Prausnitz, J. M. "Vapor-liquid equilibria in multicomponent aqueous solutions of volatile weak electrolytes"; AIChE J.; 24, 966-975 (1978)

Zc, Pv, Kk, 0-170°C, I to 6m.

75EDW/NEW: Edwards, T. J.; Newman, J.; Prausnitz, J. M.

"Thermodynamics of aqueous solutions containing volatile

weak electrolytes"; AIChE J.; 21, 248-259 (1975)

Zc, Pv, Kk, 0-100°C, m

0 to 1, 1st ioniz.

61ELL/AND:

71ELL/GIG:

Ellis, A. J.; Anderson, D. W. ; "The first acid dissociation

constant of hydrogen sulphide at high pressures"; J. Chem.

Soc. ; 4678-4680 (1961)

Ellis, A. J.; Giggenbach, W. ; "Hydrogen sulphide ionization

and sulphur hydrolysis in high temperature solution";

Geochim. Cosmochim. Acta.; 35, 247-260 (1971)

Kk, 25°C, m to 0.4, 1-2000 atm. , 1st ioniz.

Kk, 25-270°C,

1st and 2d ioniz. in strong alkali.

59ELL/GOL: Ellis, A. J.; Golding, R. M. ; "Spectrophotometric

determination of the acid dissociation constants of hydrogen sulphide"; J. Chem. Soc; 127-130 (1959)

Kk, 25°C.

1st and 2d

67ELL/MIL: Ellis, A. J.; Milestone, N. B.; "The ionization constants Kk, 20-90"C,

of hydrogen sulfide from 20 to 90 °C"; Geochim. Cosmochim. 1st and 2d Acta.; 31, 615-620 (1967) ioniz.

38EPP: Epprecht, A. G. ; "Die Dissoziationskonstante der ersten Stufe des Schwefelswasserstoff

" ; Helv. Chim. Acta; 21, 205-211 (1938)

Kk, t = 20°C(? )

1st ioniz. , dil. H

2

S HS" sol

95
76EVE/MOO: Evelein, K. A.; Moore, R. G. ; Heidemann, R. A.; "Correlation of the phase behavior in the systems hydrogen

sulf ide-water and carbon dioxide-water"; Ind. Eng. Chem.

Process Des . Dev.; 15, 423-428 (1976)

Pv, 298-444 K,200 atm.

phase behavior predicted

using Redlich-Kwong

equation. No new data

47FEH/HEU: Feher, F.; Heuer, E.; "Zur thermochemie der polyschwefelwasserstoffe" ; Z. Anorg . Allgem. Chem.; 255,

185-194, (1947)

Hr, 25°C,

polysulfides . heat

of decomposition.

63FEH/SEY: Feher, F.; Seyfried, K. ; "Die spezifiechen Warmen der sulfane ion fussigen Zustand" ; Z. Anorg. Allgem. Chem.

322, 155-161 (1963)

Qh, 25°C,

polysulfides

57FEH/WIN: Feher, F.; Winkhaus , G.; "Zur thermochemie der sulfane Bildungsenthalpien und Bindungsenergien" ; Z. Anorg. Allgem.

Chem.; 292, 210-223 (1957)

He, 25°C,

polysulfides

heat of combustion.

1883FOR: de Fo; <.» - i, R. ; "Recherches sur les hydrates sulfhydres'

Ann. Chim. Phys.;[5], 28, 5-67 (1883)

Hr, Kd, 0.5 - 28.5"C

1888FOR/VIL: de Forcrand, R. ; Villard, P.; "Sur l'hydrate d'hydrogene

sulfure"; Compt . Rend.; 106, 939-941 (1888)

Kd, 20°C?,

72GAL/MIL : Galley, M.R. ; Miller, A.I.; Atherley, J.F.; Mohn, M. ; "GS (Girdler-sulf ide) process physical properties"; At. Energy

Can. Ltd.; *AECL-4255, 78pp (1972); [CA 77-146735e]

Zc, Pv, Qh, V, t?

67GAM/RAI: Gamsjaeger, H.; Rainer, W. ; Schindler, P.; "Loslichkeitskonstanten und freie Bildungsenthalpien von Metallsulfiden , 4. Mitt.: Die Loslichkeit von H2S in HClO^-NaClO^^O-Mischungen" ; Monatsh. Chem.;

98, 1793-1802 (1967)

Ze, Hm, Pv, 25°C, 1 atm.?,

I < 3m, solution in presence of electrolytes.

69GAM/SCH: Gamsjaeger, H . ; Schindler, P.; "Loslichkeiten und Aktivitatskoeff izienten von H2S in Elektrolytmischungen" ; Helv. Chim. Acta.; 52, 1395-1402

(1969)

Pv, Da, 25°C, 1 atm.?, solubility as function of

pH and salt concn.

72GER: Gerrard, W. ; "Solubility of hydrogen sulphide, dimethyl

ether, methyl chloride and sulfur dioxide in liquids.

Prediction of solubility of all gases"; J. Appl . Chem. Biotechnol.; 22(5), 623-650 (1972); [CA 80-31037y]

Pv, Zc, several temps, 1 bar.

96
71GIG:

80GIG:

Giggenbach, W. F.; "Optical Spectra of Highly Alkaline

Sulfide Solutions and the Second Dissociation Constant of Hydrogen Sulfide"; Inorg. Chem. ; 10, 1333-1338 (1971)

Giggenbach, W. F. ; "Geothermal gas equilibria"; Geochim.

Cosmochim. Acta; 44 2021-2032 (1980)

Kk, 25-250°C,

2d ioniz. in cone. NaOH(

Pv, 100-300°C,

application of previously published

data to geochemical

equilibria

80GIL/WIL: Gillespie, P.C.; Wilson, G.M. ; 'Vapor-liquid equilibrium

data on water-substitute gas components: N

2 ~H20, H2-H2 CO-H20, H

2 -CO-H2

0, and H

2S-H2

0' ; Research Report-41, Gas Processors Association; Tulsa, Okla.; 1-34 (1980)

Pr, t = 100 - 600°F,

p=50-2000 psi

52GOA/GOR: Goates, J. R. ; Gordon, M. B.; Faux, N. D.; "Calculated

values of the solubility product constants of the metallic

sulfides"; J. Am. Chem. Soc; 74, 835-836 (1952)

Kk, 25°C, 2d ioniz. based on 49KON/LEB.

75GOL/KAP: Goldhaber, M. B.; Kaplan, I. R. ; "Apparent dissociation

constants of hydrogen sulfide in chloride solutions";

Marine Chem.; 3, 83-104 (1975)

Kk, 7.5-25°C, 1st and 2d ioniz

10GOL/LAR: Goldschmidt, H. ; Larsen, H. ; "The reduction of the nitro

group by hydrogen sulphide. A study of catalysis"; Z. Phys. Chem.; 71, 437-512 (1910); (seep. 449-454)

Pv, 15-45°C, P = 1 atm Solubility in the presence of NaHS,

polysulfides

58GOL: Golovin, F. I.; "The thermodynamic dissociation constant of hydrogen sulfide and its application to analysis of water"; Trudy Molodykh Nauch Rabotnikov Akad. Nauk Kirgiz. SSR; 119-137 (1958); [CA 55-4130f]

Kk, Pv, 18-45°C.

61GOL/NEM: Golovin, F. I.; Nemirov, G. V.; "Hydrolysis of NaHS"

Gidrokhim. Materialy; 33, 160-165 (1961); [CA 57-9281d]

Kk, 18-45°C, in NaHS

solutions, 1st. ioniz.

70GOR: Gorbunov, L. V.; "Correlation between thermodynamic

parameters and the solubility of salts and gases in water

at increased temperatures"; Geokhimiya; A (l), 116 (1970);

[CA 72-82795m]

Px, Hm, 40-90°C, also S and chem. pot.

97
67HEL: Helgeson, H. C; "Thermodynamics of complex dissociation in aqueous solution at elevated temperatures"; J. Phys . Chem.

71, 3121-3136 (1967)

Ze, Kk, Hm, 25-300°C,

1st and 2d ioniz.

76HEL/KIR: Helgeson, H.C; Kirkham, D.H.; "Theoretical prediction Kk, Zc , Ze, of the thermodynamic properties of aqueous electrolytes 25-300°C,

at high pressures and temperatures. III. Equation of 1-1000 atm. state for aqueous species at infinite dilution"; Am. J. Sci.; 276, 97-240 (1976)

81HEL/KIR: Helgeson, H.C. ; Kirkham, D.H.; Flowers, G.C.; "Theoretical Ze, Kk, Da, Dm, prediction of the thermodynamic behavior of aqueous 0-600°C, 0-5kB. electrolytes at high pressures and temperatures: IV. Calculation of activity coefficients, osmotic coefficients

and apparent molal and standard and relative partial molal

properties to 600°C and 5kB"; Am. J. Sci.; 281, 1249-1516

(1981)

76HER/HEL: Herr, F. L. Jr.; Helz, G. R. ; "Measurement of the activity Da, 12-83°C, m(NaHS) < coefficient of aqueous NaHS to 80°C and 0.2m in the 0.2m, p(H2S) < 1 atm. system NaHS-H2S-H20" ; J. Solution Chem.; 5, 833-852 (1976)

80ISA/OTT: Isaacs, E. E. ; Otto, F. D.; Mather, A. E . ; "Solubility of Pv, 100°C, P < 3.4 kPa,

mixtures of H->S and C02 in a monoethanolamine in monoethanolamine

solution at low partial pressures"; J. Chem. Eng. Data;

25, 118-120 (1980)

33JEL: Jellinek, K. ; "Lehrbuch der physikalischen Chemie"; F. Enke, Kk, 25°C, data from 22JEL/CZE,

Stuttgart; *IV, 62 (1933) 1st and 2d ioniz.

22JEL/CZE : Jellinek, K. ; Czerwinski, J.; "Uber die Dissoziation von Kk.Ke, Px, 25°C,

H

2

S, Na2S und NaHS in wasseriger Losung" ; Z. Phys. Na2S , NaSH. Chem.; 102, 438-479 (1922) 1st and 2d ioniz.

54 JUZ/LAU : Juza, R. ; Laurer, P.; "Zur Kenntnis des Hr , 25°C, LiOH(aq) + Lithiumhydrogensulfids" ; Z. Anorg . Allgem. Chem.; 275 H

2 S(aq). 79-93 (1954)

4 1KAP/ANV : Kapustinsky, A. F . ; Anvaer, B. I.; "Setschenoff' s rule and Pv, 25°C, 1 atm. the solubility of hydrogen sulfide in hydrochloric acid Aq. solutions of FeCl2 solutions"; Compt . Rend. Acad. Sci. URSS; 30, 625-628

(1941); [CA 37-2981]

98
58KAR/KAN

21KEN/AND

65KHO/ZHO

37KIS/LAJ

06KNO:

31K0L:

49KON/LEB

31K0R/SCH

64KOZ:

65KOZ:

Kapustinskii , A. F.; Kan'kovskii, R. T.; "Thermochemistry of He, 25°C, H2S(g)

Isotopes. I. Calorimetric determination of the heat of heat of condensation,

formation of hydrogen sulfide and deuterium sulfide"; Zh. Fiz. Khim.; 32, 2810-2816 (1958)

Kendall, J.; Andrews, J. C; "The solubilites of acids in Pv, 25°C, 1 atm, sol in aqueous solutions of other acids"; J. Am. Chem. Soc . ; A3, HCl(aq).

1545 (1921)

Khodakovskii, I. L.; Zhogina, V. V.; Ryzhenko, B. N. ; Ze, Kk, 0-50°C, 1st and "Dissociation constants of hydrogen sulfide at elevated 2d ioniz. temperatures"; Geokhimiya; 7, 827-833 (1965)

Kiss, A. v.; Lajtai, I.; Thury, G. ; "Uber die Loslichkeit Pv, 0-25°C, 1 atm., in aq. von Gasen in Wasser-Nichtelektrolytgemischen" ; Z. Anorg. sol. of alcohol, glycerine

Allgem. Chem.; 233, 346-352 (1937) and carbamide.

Knox, J.; "Zur Kentniss der Ionenbildung des Schwefels und Kk, 2d ioniz. der Komplexionen des Quecksilbers" ; Z. Elektrochem; 12, cited in 64SIL/MAR.

477 (1906)

Kolthoff, I. M. ; "The solubilities and solubility products Kk, 1st and 2d ioniz., of metallic sulfides in water"; J. Phys . Chem.; 35, cited in 64SIL/MAR, 2711-2721 (1931) Source of data not given.

Konopik, N.; Leberl, 0.; "Die zweite Dissoziationskonstante Kk, 20°C, 2d ioniz. von Schwefelwasserstoff

" ; Monatsh. Chem.; 80, 781-787 (1949) in Na2S sol.

Korvezee, A.E.; Scheffer, F.E.C.; "La composition de ' Px, Pv, -25 to -2°C,

l'hydrate de l'hydrogene sulfure"; Rec . Trav. Chim. Pays. H20-6H2

0, reinterp.

Bas.; 50, 256-260 (1931) of 19SCH/MEY

Kozintseva, T. N . ; "Solubility of hydrogen sulfide in water Pv, 160-330°C.

at elevated temperature"; Geokhimiya; 758-765 (1964); [CA

61-9292b]

Kozintseva, T. N. ; "The solubility of H

2

S in water and Pv, 150-330"C, 1 and 2 atm

the salt solutions at elevated temperatures"; Geokhim. in water, NaCl,

Issled. v Obi. Povyshennykh Davlenii i Temperatur., Akad. CaCl2 ,and Na 2 S0^ sol. Nauk SSSR, Inst. Geokhim. i Analit. Khim., Sb . Statei

121-134 (1965); [CA 64-10459b]

99
73KRY/STA : Kryukov, P. A.; Starostina, L. I.; Tarasenko, S. Ya.; Kk , 25-150°C, 1st and 2d Pavlyuk, L. A.; Smolyakov, B. S.; Larionov, E. G. ; ioniz. "Ionization constants of carbonic acid, hydrogen sulfide,

boric acid, and sulfuric acid at high temperatures"; Mezhdunar. Geokhim. Kongr. [Dokl.] 1st, (1971); 2, 186-198 (1973); [CA 81-69193]

74KRY/STA: Kryukov, P. A.; Starostina, L. I.; Tarasenko, S. Ya.; Kk , 25-150°C, 2d ioniz. Primanchuk, M. P. ; "Second ionization constant of hydrogen

sulfide at temperatures up to 150°C"; Geokhimiya; 1003-1013 (1974)

46KUB: Kubli, H.; "Die Dissoziation von Schwefelwasserstoff

" ; Kk, 20°C, m(Na2S) = 0.04 Helv. Chim. Acta.; 29, 1962-1973 (1946) - 0.08, 1st and 2d

53KUR/ZIE: Kury, J. W. ; Zielen, A. J.; Latimer, W. M. ; "Heats of Hr, 25°C,

formation and entropies of HS- and S~. Potential of 1st and 2d ioniz. sulfide-sulfur couple"; J. Electrochem. Soc . ; 100, 468-470 (1953)

05KUS/HEB: Kuster, F. W. ; Heberlein, E . ; "Beitrage Zur Kenntnis der Kk, hydrolysis of Na2

S, Polysulfide I."; Z. Anorg . Allgem. Chem. ; 43, 53-84 (1905) polysulfides . See 22JEL/CZE

69LAR/HEP: Larson, J.W. ; Hepler, L.G.; "Heats and Entropies of Zr , Kk, Hr, 25°C Ionization"; 'Solute-Solvent Interactions', Marcel- 1st and 2d ioniz. Dekker, New York and London, 1969 and 1976; 1, chapter 1 (1969)

76LAW/GAR: Lawson, J. D.; Garst, A. W. ; "Gas sweetening data: Pv, 80-300°F, p to Equilibrium solubility of hydrogen sulfide and carbon 27,800mmHg, in H2O/

dioxide in aqueous monoethanolamine and aqueous ethanolamines

diethanolamine solutions"; J. Chem. Eng. Data; 21, 20-30

(1976)

77LEE/MAT: Lee, J.I.; Mather, A. E.; "Solubility of hydrogen sulfide Pv, 10-180°C, P to 6.7

in water"; Ber. Bunsenges. Phys . Chem.; 81, 1020-1023 MPa. (1977)

100
73LEE/OTT: Lee, J. I.; Otto, F. D.; Mather, A. E . ; "Solubility of hydrogen sulfide in aqueous diethanolamine solutions at high pressures"; J. Chem. Eng. Data.; 18, 71-73 (1973)

Pv, 25-120°C, .02-20 atm.

in H

20/diethanolamine

solution

73LEE/OTT2:

74LEE/OTT:

Lee, J. I.; Otto, F. D.; Mather, A. E.; "Partial pressures

of hydrogen sulfide over aqueous diethanolamine

solutions."; J. Chem. Eng. Data; 18, 420 (1973)

Lee, J. I.; Otto, F. D.; Mather, A. E.; "Solubility of mixtures of carbon dioxide and hydrogen sulfide in aqueous diethanloamine solutions"; Can. J. Chem. Eng.; 52, 125-127 (1974); [CA 81-30275]

Pv, 25-120°C, .0007-20 atm.,

in H

20/diethanolamine

solution

Pv, 50 and 100°C, .01-840 psia, H2S/C02 = 0-67 in h^O-diethanolamine

mixt

76LEE/OTT: Lee, J. I.; Otto, F. D.; Mather, A. E. ; "Equilibrium in hydrogen sulfide-monoethanolamine-water system"; J. Chem.

Eng. Data; 21, 207-208 (1976)

Pv, 25-120°C, p(H2S) =

.15 to 2317 kPa,

ethanolamine-water mixt.

76LET/THO: Letoffe, J. M. ; Thouroy, J.; Perachon, G. ; Bousquet, J.; "Determination des enthalpies standards de formation des polysulfures de sodium et de lithium"; Bull. Soc . Chim. France; 424 (1976)Hm, 25°C, Na2S and polysulfides

58LIN: Linke, W. F.; D. Van Nostrand, Princeton; "Solubilities' 4th ed.; 1, 1153-1156 (1958); [originated by A. Seidel]

Ze, Pv, 0-100°C, 270-3500mmHg,

in water and salt solutions, data compiled.

28LOO: Loomis, A. G. ; in Washburn, E. W. ; "Solubilities of gases

in water"; ed., "International Critical Tables", McGraw

Hill, N.Y.; *III, 259 (1928)

Pv, 0-100°C, Winkler's

data (06WIN).

61L0Y/HIM: Loy, H. L.; Himmelblau, D. M. ; "The first ionization constant of hydrogen sulfide in water"; J. Phys . Chem.

65, 264-267 (1961)

Kk, 0-50°C, 1st ioniz.

41MAR/K0B: Markham, A. E . ; Kobe, K. A.; "The solubility of gases in liquids"; Chem. Rev.; 28, 519 588 (1941)Zr, Pv, methods,

bibliography, data

quality, no values for solubilities

59MAR: Maronny, G. ; "Constantes de dissociation de l'hydrogene

sulfure"; Electrochim. Acta; 1, 58-69 (1959)

Kk, 0-25°C.

2d ioniz. and polysulfides

101
59MAR2: Maronny, G.; "Fonctions thermodynamiques standards des ions Kk , 25 ' sulfurs et polysulfures en solution aqueuse II. polysulfides

.

Determination des tensions standards"; J. Chim. Phys . -Phys .

Chim. Biol.; 56, 202-213 (1959)

59MAR3: Maronny, G. ; "Fonctions thermodynamiques standards des ions Kk, Hr, 20-25°C, sulfures et polysulfures en solution aqueuse"; J. Chim. polysulfides . 2d ioniz.

Phys. Phys. -Chim. Biol.; 56, 214-221 (1959)

55MAR/VAL: Maronny, G. ; Valensi, G.; "Calorimetric determination of Kk , Hr, 25°C

n _ thermodynamic al functions of the ion"; Compt . polysulfides

.

Rend, de la Septieme Reunion, Lindau; 266-274 (1955)

03MCL: McLauchlan, W. H.; "Uber den Einfluss von Salzen auf die Pv, 25°C, 1 atm. , in Wasserloslichkeit von Schwefelwasserstoff , Jod und Brom" ; water and salt solutions.

Z. Phys. Chem.; 44, 600-633 (1903)

83MEY/WAR: Meyer, B , ; Ward, K. ; Koshlap, K. ; Peter, L.; "Second Kk, 25°C,

dissociation constant of hydrogen sulfide"; Inorg. Chem.; 2d ioniz.,

22, 2345-2346 (1983) in cone. NaOH.

75MIL/WIL: Miles, D.H.; Wilson, G.M. ; "Vapor-liquid equilibrium data Pv, as cited

for design of sour water strippers"; Annual Report to by 78EDW/MAU

American Petroleum Institute, 1974; (1975)

61MUH/SUN: Muhammad, S. S.; Sundaram, E. V.; "The spectrophotometric Kk, 30°C, 1st and 2d determination of the dissociation constants of hydrogen ioniz. sulfide"; J. Sci. Ind. Res. (Delhi); 20B, 16-18 (1961)

77NAS/MAT: Nasir, P.; Mather, A. E.; "The measurement and prediction Pv, 80-100°C, P to 9 of the solubility of acid gases in monoethanolamine kPa, I^S.CC^ and their

solutions at low partial pressures"; Can. J. Chem. Eng.; mixt . in f^O/ethanolamine

.

55, 715-717 (1977); [CA 88-42271]

77NOW/CHA: Nowak , E. S.; Chan, J. S.; "A mixture saturation theory and Qh, 300-400 K, 10-20 experimental measurements of the thermal properties of a bar, liq and gas mixt. two component-two phase system"; Proc . Symp. Thermophys

.

Prop. ; 7, 538-545 (1977)

1899PAU: Paul, T.; "Tuberinger Chemische Gesellschaft Sitzung, 2 Juni"; Kk , 1st ioniz., conductivity

Chem. Ztg.; 23, 535 (1899) cited in 77RAO/HEP

and 64SIL/MAR.

102
76PAV/KRY

80PEN/ROB:

49PES/VAL:

61P0H:

Pavlyuk, L. A.; Kryukov, P. A.; "Spectrophotometric

determination of the first ionization constant of hydrogen

sulfide at elevated temperatures"; Izv. Sib. Otdel. Akad. Nauk SSSR; *(6), 25 (1976)

Kk, 25-110°C.

1st ioniz.

Peng, D.-Y.; Robinson, D.B.; "Two-and three-phase equilibrium Zc , Pv, 100-340°F calculations for coal gasification and related processes"; 100-5000 psia, ACS Symp. Ser.; No. 133, 393-414 (1980) correlation of VLE data.

Peschanski, D.; Valensi, G. ; "Contribution a L ' electrochimie des solutions aqueuses de polysulfures" ; J. Chim. Phys.; 46, 602-619 (1949)

Pohl, H. A.; "Thermodynamics of the hydrogen sulf ide-water

system relevant to the dual temperature process for the production of heavy water"; J. Chem. Eng. Data; 6, 515

(1961)

Ke, 20°C, polysulfide.

Zc, Pv, Qh, 0-160°C, 0-400 psia.

62POH

Pohl, H. A.; "Solubility of iron sulfides"; J. Chem. Eng. Data; 7, 295 (1962)

Ze, Kk, 25°C, values

from 52LAT/KUR selected.

09POL: Pollitzer, F.; "Uber das Gleichgewicht der Reaktion

H2SI+ 2J I 2HJ + S und die Dissoziation des Schwefelwasserstoffs" ; Z. Anorg. Allgem. Chem.; 64, 121-14? (1909)

Pv, 40-60°C, from a study of reaction

equilibrium.

1895PRY/HOL: Prytz, K. ; Hoist, H. ; "Die Absorptionscoefficienten der Kohlensaure und des Schwefelwasserstoffs in Wasser bei

dessen Gefrierpunkt" ; Ann. Phys.; 290(54 3rd ser.), 130-138 (1895)

Pv, 0°C, 1 atm.

77RAO/HEP: Rao, S. R. ; Hepler, L. G. ; "Equilibrium constants and thermodynamics of ionization of aqueous hydrogen sulfide"

Hydrometallurgy; 2, 293 299 (1977)

Ze, Kk, Hr, 25-200°C,

1st and 2d ioniz.

1881SAB: Sabatier, P.; "Les sulfures"; Ann. Chim. et Phys.; 22[5] 5-98 (1881)

Hr, 15°C, NaOH(aq) + H2S(aq) polysulfides

13SCH: Scheffer, F.E.C.; "Das System Schwefelwasserstoff -Wasser

Z. Phys. Chem.; 84, 734-745 (1913)

Pv, Px, -25 to-2°C,

103
19SCH/MEY:

60SCH/FIS

52SEL/CAR:

64SIL/MAR:

Scheffer, F.E.C.; Meyer, G. ; "On an indirect analysis of gas-hydrates by a thermodynamic method and its application

to the hydrate of sulphuretted hydrogen"; Proceedings of the Section of Sciences; 21(6-10) Pt. 2, 1338-1348 (1919)

Schwarzenbach , G. ; Fischer, A.; "Die Aciditat der Sulfane und die Zusammensetzung wasseriger Polysulfidlosungen"

Helv. Chim. Acta; A3, 1365-1390 (1960)

Selleck, F. T.; Carmichael, L. T.; Sage, B. H. ; "Phase behavior in the hydrogen sulfide-water system"; Ind. Eng. Chem.; 44, 2219-2226 (1952)

Sillen, L. G. ; Martell, A. E.; "Stability constants of metal-ion complexes, Section I, Inorganic ligands"; Special

Publication No. 17, Chemical Society (London); 215-216

(1964) early references.

Pv, Px. -25 to -2°C,

vap . press

Kk, 20°C, 1=0. lm,

H2S, H2S

3 , H2S^,

Pv, Px, 100-340°F,

P to 5200 psia.

good summary.

Ze, Kk, 0-200°C, 1st and

2d ioniz. compiled data, see for

71SIL/MAR: Sillen, L.G.; Martell, A.E.; 'Stability constants of metal-ion complexes. Supplement No 1'; The Chemical

Soc, London; Spec. Pub. 25 (1971)

Kk, 20-350"C,

compiled data.

28SMI

76SMI/MAR:

Smith, D. F.; in Washburn, E. W. ; "The solubility of gases

in solution"; ed. , International Critical Tables, McGraw

Hill, N.Y.; *III, 274, (1928)

Smith, R. M. ; Martell, A.E.; 'Critical stability constants' Plenum Press, N.Y.; 4, 76 (1976)

Pv, 0-30°C, HC1, HI, NaCl, and NaHS

solutions

Ze, Kk, 20 and 25°C,

evaluated data.

50SOU/SCH: Souchay, P.; Schaal, R. ; "Determination cryoscopique des constantes de dissociation d'acides tres faibles"; Bull.

Soc. Chim. France; 819-824 (1950)

Kk, 32, 38°C, 2d ioniz.

inNa2SOA (10H2

O)

74SRE

Sretenskaya, N. G. ; "Electrical conductivity of hydrogen

sulfide aqueous solutions and the first constant of hydrogen sulfide acid dissociation at various

temperatures"; Geokhimiya; 996-1002 (1974)

Kk, 25-90°C.

1st ioniz.

7 1STE/COB : Stephens, H. P.; Cobble, J. W. ; "Thermodynamic properties

of the aqueous sulfide and bisulfide ions and the second ionization constant of hydrogen sulfide over extended

temperatures"; Inorg. Chem.; 10, 619-625 (1971)

Kk, Hr, Qh, Zc, 25"C,

95°C, from

K HS(cr) + KOH(aq)

104
64STE/T0R: Ste-Marie, J.; Torma, A. E . ; Gubeli, A. 0.; "The stability

of thiocomplexes and solubility products of metal

sulphides"; Can. J. Chem; 42, 662 (1964)

Kk, 25°C, 1st and 2d

ioniz

57SUN/WAD:

69SYR/KRA:

78TAG/POL:

71TED:

Sunner, S.; Wadso, I.; "The heat of hydrolysis of thiolacetic acid"; Trans. Faraday Soc . ; 53, 455-459

(1957)

Syrkina, I. G. ; Krasheninnikova, A. A.; Zaliopo, V. M.

"Solubility of sulfur dioxide, hydrogen sulfide, and chlorine in hydrochloric acid"; Zh. Neorg. Khim. ; 14(5), 1331-1334 (1969); [CA 71"33884k]

Tagieva, L. V.; Poltoratskii , G. M. ; Maksimov, V. F.; Tyutyunnik, L. F.; "Equilibrium between the liquid and the vapor in the water-sodium sulfide-sodium hydrogen sulfide

system"; Zh. Priklad. Khim.; 51, 49-52 (1978)

Teder, A. ; "The equilibrium between elementary sulfur and aqueous polysulfide solutions"; Acta Chem. Scand. ; 25, 1722-1728 (1971)

Hm, 25°C.

in acid sol.

Pv, 2.5-75°C, in HC1

solutions

Pv, Da, Dm, 298-343 K.

Kk, 25 and 80°C, S, polysulfide equilib.

1882THO:

76TSO/COU:

57TUM/MIS:

82WAG/EVA:

Thomsen, J.; "Thermochemische Untersuchen" ; Leipzig; 4, 188 (1882-86)

Tsonopoulos, C; Coulson, D. M. ; Inman, L. B.; "Ionization

constants of water pollutants"; J. Chem Eng. Data; 21, 190-193 (1976)

Tumanova, T. A.; Mishchenko, K. P.; Flis, I. E.; "The dissociation of hydrogen sulfide in aqueous solutions at various temperatures"; J. Inorg. Chem., USSR; 2, 1990 (1957)

Wagman, D. D.; Evans, W. H.; Parker, V. B.; Schumm, R. H. Halow, I.; Bailey, S. M. ; Churney, K. L.; Nuttall, R. L.; "The NBS tables of chemical thermodynamic properties"; J. Phys. Chem. Ref. Data; 11, Supplement No 2 (1982)

Hm, 18°C.

Kk, 25-150°C.

1st and 2d ioniz.

Kk, 10-15°C.

1st ioniz.

Kk, 25°C.

A fG, S, A f

H,

00WAL/COR: Walker, J.; Cormack, W. ; "The dissociation constants of very weak acids"; J. Chem. Soc; 77, 5 (1900)

Kk, cited in 77RAO/HEP and 64SIL/MAR, 1st ioniz., conduct.

105
23WAS

Wasastjerna, J. A.; "Hydrolysis of potassium hydrosulfide

in aqueous solution"; Soc. Sci. Fennica Com. Phys.-Mat.;

1(39), 1-15 (1923); [CA 18-1076]

Hr, 25°C, 2d ioniz.

23WAS2: Wasastjerna, J. A. ; "Hydrolysis of potassium monosulfide"

Soc. Sci. Fennica Com. Phys.-Mat.; 1(40), 1-24 (1923);

[CA 18-1076]

Kk, Hr, 0 and 25"

2d ioniz.

11WEN/RUP: Wenzel, H.; Rupp, W. ; "Calculation of phase equilibria in systems containing water and supercritical components";

Chem. Eng. Sci.; 33, 683 (1978)

Zc, Pv, Px, 410-444 K, p:to 350 bar, phase

equilibria calc. using

Redlich-Kwong equation.

77WIL/BAT: Wilhelm, E . ; Battino, R. ; Wilcock, R. J.; "Low-pressure

solubility of gases in liquid water"; Chem. Rev.; 77, 219-262, (1977)

Ze, Pv, 0-100°C, P=l

atm, methods, tables,

thermodynamic

properties

correlations and theory.

06WIN: Winkler, L. W. ; "Gesetzmassigkeit bei der Absorption der Gase in Flussigkeiten" ; Z. Phys . Chem.; 55, 344 (1906)

Zr, Pv, 0-60°C, analysis

of early meas . Data in 58LIN p. 1153.

32WRI/MAA: Wright, R. H. ; Maass, 0.; "The solubility of hydrogen

sulphide in water from the vapor pressures of the solutions"; Can. J. Research; 6, 94 (1932)

Pv, 25°C.

32WRI/MAA2:

51YUI;

60ZAV/KRY

Wright, R. H.; Maass, 0.; "Electrical conductivity of aqueous solutions of hydrogen sulfide and the state of the dissolved gas"; Can. J. Research; 6, 588 (1932)

Kk, 25°C, 1st ioniz.

Yui , N. ; "On the ionization constant of hydrogen sulfide";

Sci. Repts. Tohoku Imp. Univ.; 35[1], 53-61 (1951)

Zavodnov, S. S.; Kryukov, P. A.; "The magnitude of the second dissociation constant of hydrogen sulfide"; Izvest. Akad. Nauk SSSR, Otdel. Khim. Nauk; 1704-1706 (1960)

Kk, 25°C, 1st and 2d ioniz

Kk, 20-60°C. 2d ioniz.

34ZEU/ROT: Zeumer, H.; Roth, W. A.; "Die Bildungswarme und Losungswarme von Schwefelwasserstoff

" ; Z. Elektrochem.

40, 777-783 (1934)

Hm, 20°C.

106
ZnCl 2 ~H2

0

T. L. Jobe, Jr. and R. N. Goldberg

INTRODUCTION

Aqueous zinc chloride solutions are of both scientific and

industrial importance. The purpose of this bibliography is to identify

papers which contain either experimental thermodynamic data for these

systems or reviews or correlations of this data. The thermodynamic

properties of interest include most types of equilibrium data: activity

and osmotic coefficients, equilibrium constants in solution, enthalpies,

and heat capacities. Density and solubility data are not included in this

bibliography. The search of the literature was based upon a search of

the following sources: a computer aided search of Chemical Abstracts from

1967 to 1983, the Bulletin of Chemical Thermodynamics [1] from 1960 to

1981, the files of the Chemical Thermodynamics Data Center at the National

Bureau of Standards, and of the references found in the papers identified

in the search itself. The authors would appreciate learning of any papers

which may have been missed in the search.

The papers are listed alphabetically by first author. Each

bibliographic citation includes a brief reference citation (the year and

three letters from the names of the first two authors), the authors names,

the title of the article and the source. When only an abstract was

available only the Chemical Abstracts citation is given. The attempt was

made to adhere to the journal abbreviations used in the Chemical Abstracts

Source Index [2].

107
For each paper we have indicated the type of data, the temperature

range and, if appropriate, the pressure, solution composition, and pH.

The codes used for the properties are from the Bulletin of Chemical

Thermodynamics [1]; they are reproduced in Table I.

The Russian titles have been translated into English. These translations come, by preference, from the papers themselves or from Chemical

Abstracts. The titles from the latter source may be condensations of the

originals

This bibliography was sponsored by the Design Institute for Physical

Property Data (DIPPR) of the American Institute of Chemical Engineers.

[1] Bulletin of Chemical Thermodynamics, R. D. Freeman, editor,

Thermochemistry, Inc., Stillwater, OK, 1977 to 1981.

[2] Chemical Abstracts Service Source Index: 1907-1979 Cumulative, in

two volumes; American Chemical Society, Washington, DC, 1979.

108
TABLE I

Property Symbol

Category Subgroup

D DaDm

Dx

Description of Properties

Derived Quantities of Special Interest (not listed elsewhere)

Activity, fugacity

Partial molar quantities

Excess functions for mixtures

He

HrHm

Hp

Hs

KdKe

Kk

Md

Mi

Mg

MmMx

Mb

Pt

Pp

P-v Px

PoP3

Ql

Qh

Qg

Vg

VcVx

Vt

Enthalpy Changes for Processes, by Calorimetry

for combustion in 0

2 or F2 for other chemical reactions

for mixing: solution, dilution, etc. for phase transitions, fusion, vaporization

for surface processes: adsorption, desorption, etc.

Reaction Equilibria and Related Data Dissociation/decomposition pressures and derived enthalpy/entropy changes.

Electrochemical cell potentials, etc. and derived enthalpy/entropy changes.

Equilibrium constants for chemical reactions and derived enthalpy/entropy changes.

Thermodynamic Quantities Calculated from Molecular Parameters

Data (e.g., structural or spectroscopic) for molecular parameters;

atomic energy levels; ionization potentials.

Ideal gases: thermodynamic functions (e.g., tabulations).

Real.gases: intermolecular potentials, derived equations of state Mixtures

Crystal, solid and liquid states. Bond energies; non-bonded interactions.

Phase Equilibria

Temperatures: freezing point, boiling point, triple point, other phase transition

Vapor pressure and derived quantities for vaporization and/or sublimation,

pure substances

Vapor/liquid equilibria and related phase diagrams, mixtures

Condensed phase equilibria: solubility, freezing points, phase diagrams.

Osmotic pressure/membrane equilibria

Surface phenomena: surface tension, surface energy, adsorption, etc.

Thermal Properties for Non-Re acting Systems, by Calorimetry

Condensed phase, T S 400 K: heat capacity, enthalpy, entropy, etc. Condensed phase, T 1 400 K: heat capacity, enthalpy, entropy, etc. Gas phase: heat capacity, enthalpy, entropy etc. as f(T,P).

Volume as f(T,P); Empirical Equations of State

Gases: PVT, and related data

Critical state properties

Condensed phases: compressibility , thermal expsansivity

Tables and charts of data, e.g., Mollier diagrams.

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Physical Properties of a Single Phase

Dennity

Viscosity

Refractive index

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Evaluations and compilations

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T. L. Jobe, Jr. and R. N. Goldberg

INTRODUCTION

Aqueous phosphoric acid solutions are of both scientific and industrial importance. The purpose of this bibliography is to identify papers

which contain either experimental thermodynamic data for these systems or

reviews or correlations of this data. The thermodynamic properties of

interest include most types of equilibrium data: activity and osmotic

coefficients, equilibrium constants in solution, enthalpies,, and heat

capacities. Density and solubility data are not included in this bibliography. The search of the literature was based upon a search of the

following sources: a computer aided search of Chemical Abstracts from 1967

to 1983, the Bulletin of Chemical Thermodynamics [1] from 1960 to 1981,

the files of the Chemical Thermodynamics Data Center at the National

Bureau of Standards, and of the references found in the papers identified

in the search itself. The authors would appreciate learning of any papers

which may have been missed in the search.

The papers are listed alphabetically by first author. Each bibliographic citation includes a brief reference citation (the year and

three letters from the names of the first two authors), the authors names,

the title of the article and the source. When only an abstract was

available only the Chemical Abstracts citation is given. The attempt

was made to adhere to the journal abbreviations used in the Chemical

Abstracts Source Index [2].
For each paper we have indicated the type of data, the temperature range and, if appropriate, the pressure, solution composition and pH.

The codes used for the properties are from the Bulletin of Chemical

Thermodynamics [13; they are reproduced in Table I.

The Russian and Japanese titles have been translated into

English. These translations come, by preference, from the papers themselves or from Chemical Abstracts. The titles from the latter source may

be condensations of the originals.

This bibliography was sponsored by the Design Institute for

Physical Property Data (DIPPR) of the American Institute of Chemical

Engineers.

[1] Bulletin of Chemical Thermodynamics, R. D. Freeman, editor,

Thermochemistry, Inc., Stillwater, OK, 1977 to 1981.

[2] Chemical Abstracts Service Source Index: 1907-1979 Cumulative, in

two volumes; American Chemical Society, Washington, DC, 1979.

121
TABLE I

Property Symbol

Category Subgroup

D Da

DmDx

Description of Properties

Derived Quantities of Special Interest (not listed elsewhere)

Activity, fugacity

Partial molar quantities

Excess functions for mixtures

H Enthalpy Changes for Processes, by Calorimetry

He for combustion in 0

2 or Fo Hr for other chemical reactions Hm for mixing: solution, dilution, etc. Hp for phase transitions, fusion, vaporization

Ks for surface processes: adsorption, desorption, etc.

K Reaction Equilibria and Related Data

Kd Dissociation/decomposition pressures and derived enthalpy/entropy changes.

Ke Electrochemical cell potentials, etc. and derived enthalpy/entropy changes.

Kk Equilibrium constants for chemical reactions and derived enthalpy /entropy change

H Thermodynamic Quantities Calculated from Molecular Parameter s Md Data (e.g., structural or spectroscopic) for molecular parameters;

atomic energy levels: ionization potentials.

Mi Ideal gases: thermodynamic functions (e.g., tabulations).

Kg Real gases: intermolecular potentials, derived equations of state Mm Mixtures

Mx Crystal, solid and liquid states. Mb Bond energies; non-bonded interactions.

P Phase Equilibria

Pt Temperatures: freezing point, boiling point, triple point, other phase transiti

Pp Vapor pressure and derived quantities for vaporization and/or sublimation,

pure substances

Pv Vapor/liquid equilibria and related phase diagrams, mixtures

Px Condensed phase equilibria: solubility, freezing points, phase diagrams.

Po Osmotic pressure/membrane equilibria

Ps Surface phenomena: surface tension, surface energy, adsorption, etc.

Q Thermal Properties for K' on-Reacting Systems, by Calorimetry

Ql Condensed phase, T i ^OC K: heat capacity, enthalpy, entropy, etc. Qh Condensed phase, T i ^00 K: heat capacity, enthalpy, entropy, etc. Qg Gas phase: heat capacity, enthalpy, entropy etc. as f(T,P).

V Volume as f(T,P); Empirical Equations of State

Vg Gases: PVT, and related data

Vc Critical state properties

Vx Condensed phases: compressibility, thermal expsansivity

Vt Tables and charts of data, e.g.. Mollier diagrams.

Physical Properties of a Single Phase Xd Density

Xv Viscosity

Xr Refractive index

Compi

at ion s, Corre 1 a t i on s and Reviews

Za Analysis of experimental data and of errors

Zc Empirical Correlations

Ze Evaluation!- ana compilations

Zr Reviews

Physical States: (c)rystal, solid (aq)uoous

(amorp)hou3 (nonaq)uecus , includes fused salts, solid solutions

(Uq)uid

(g)as (Ads)orbcd

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NBS-H4A (REV. 2-8C) U.S. DEPT. OF COMM. BIBLIOGRAPHIC DATA

SHEET (See instructions)

PUBLICATION OR

REPORT NO.

NBS/SP-718

2. Performing Organ. Report No 3. Publication Date September 1986

4. TITLE AND SUBTITLE

Bibliographies of Industrial Interest: Thermodynamic Measurements on the Systems

C0

2+H2

0 : H

2 S02

+H

2 0, NH

3

+H

2 0, ^S+^O, ZnCl^^O, and H^C^+I^O

5. AUTHOR(S) B.R. Staples, D. Garvin, D. Smith-Magowan, T.L. Jobe, Jr., J. Crenca,

C.R. Jackson, T.F. Wobbeking, R. Joseph, A. Brier, R.H. Schumm, and R.N. Goldberg

6. PERFORMING ORGANIZATION (If joint or other than NBS, see instructions)

National Bureau of Standards

Department of Commerce

Gaithersburg, Maryland 20899

7. Contract/Grant No.

8. Type of Report & Period Covered

Fi nal

9. SPONSORING ORGANIZATION NAME AND COMPLETE ADDRESS (Street. City, State. ZIP)

The Design Institute for Physical Property Data (Project 811)

American Institute of Chemical Engineers

New York, NY

10. SUPPLEMENTARY NOTES

Library of Congress Catalog Card Number: 86-600544

J

Document describes a computer program; SF-185, FIPS Software Summary, is attached.

11. ABSTRACT (A 200-word or less factual summary of most significant information. If document includes a significant

bibliography or literature survey, mention it here) Contained herein are bibliographies of sources of experimental and correlated

thermodynamic data for seven binary aqueous mixtures of industrial importance,

namely mixtures of C0

2

, H

2 S, NH^ , H2

S °4> H

3

P°4> CuC1

2 and ZnC1

2 with water - The

categories of equilibrium data included in the bibliographies are activity and

osmotic coefficients, equilibria in solution, enthalpies and heat capacity data,

vapor-liquid equilibria, and phase equilibrium data.

12. KEY WORDS (Six to twelve entries; alphabetical order; capitalize only proper names; and separate key words by semicolons)

ammonia; bibliography; carbon dioxide; copper chloride; enthalpy; equilibrium

constants; heat capacity; hydrogen sulfide; phosphoric acid; sulfuric acid;

thermodynamics; water; zinc chloride..

13. AVAILABILITY

L~X] Unlimited For Official Distribution. Do Not Release to NTIS

Hv] Order From Superintendent of Documents, U.S. Government Printing Office, Washington, D.C

20402.

Order From National Technical Information Service (NTIS), Springfield, VA. 22161

14. NO. OF

PRINTED PAGES

146

15. Price

USCOMM-DC 6043-P80
U.S. Department of Commerce

National Bureau of Standards

Gaithersburg, MD 20899

Official Business

Penalty for Private Use $300