Annotated Bibliography of 

Studies on the Density and other 

Volumetric Properties for 

Major Components in 

Geothermal Waters 1928-74

GEOLOGICAL SURVEY BULLETIN 1417

Annotated Bibliography of 

Studies on the Density and other 

Volumetric Properties for 

Major Components in 

Geothermal Waters 1928-74

By R. W. POTTER, II, D. R. SHAW, and J. L. HAAS, JR. 

GEOLOGICAL SURVEY BULLETIN 1417

UNITED STATES GOVERNMENT PRINTING OFFICE, WASHINGTON : 1975

i a ti I CQ» \j f\ A o o ' i o * * _, _ ' , . rt B"4r I I E-^S -s *» IQ /.iOlCOS I *4vJ vA UUOw
UNITED STATES DEPARTMENT OF THE INTERIOR

GEOLOGICAL SURVEY 

V. E. McKelvey, Director

Library of Congress Cataloging in Publication Data

Potter, Robert W.

Annotated bibliography of studies on the density and other volumetric properties for

major components in geothermal waters, 1928-74.

(Geological Survey Bulletin 1417)

Bibliography: p.

Supt. of Docs. No.: 119.3:1417

1. Geothermal resources-Testing-Bibliography. 2. Mineral waters-Testing-Bibliography. 

I. Shaw, Donnie R., joint author. II. Haas, John L., joint author. HI. Title: Annotated 

bibliography of studies on the density... IV. Series: United States. Geological Survey 

Bulletin 1417.

QE75.B9No.l417[Z7935] [GB1199.5] 557.3'08s[016.551.4'9] 75-619354

For sale by the Superintendent of Documents, U. S. Government Printing Office 

Washington, D. C. 20402

Stock Number 024-001-02747-0
Contents

Page

Introduction 1

Experimental methods 2

Nomenclature . . n

Breakdown of bibliography by chemical species 5

References cited 17

Bibliography 18

111

ANNOTATED BIBLIOGRAPHY 

OF STUDIES ON THE DENSITY

AND OTHER VOLUMETRIC

PROPERTIES FOR MAJOR COMPONENTS

IN GEOTHERMAL WATERS, 1928-74

BY R. W. POTTER, II, D. R. SHAW, and J. L. HAAS, JR.

Introduction

This bibliography supplies an annotated list of references 

pertaining to the density of solutions of importance in 

geothermal exploration and energy production. The list has been 

restricted to those references containing data on aqueous 

solutions of the following salts:

HC1

NaCl

KC1

CaCl 2

FeCl 2

H 2 S04

NaHS04

Na2 S04

KHSO*

K 2 SOA

FeS0 4 

H2 C0 3 

NaHC03 

Na 2 co3

KHC0 3

K 2C03

NaOH

KOH

Si02 [aq]

"sea water"

Other components in the geothermal waters are almost always 

minor. Examples are aluminum compounds* fluorides, and 

bisulfides. Densities of these solutions have been neglected 

because 1) data for these components at temperatures above 100°C 

are uniformly nonexistent, and 2) the salts are present in such 

minor quantities that they will have only a negligible effect on 

the overall physical properties of the geothermal water. The 

volumetric properties of "sea water" and its concentrates were 

included in the literature search. Sea water is similar to 

subsurface brines in that it is dominantly a NaCl brine. 

However, sea water contains significant concentrations of 

magnesium and only traces of calcium, whereas subsurface brines

(contain significant concentrations of calcium and only traces of 

magnesium. The difference in the composition will have a 

significant effect on the chemical properties of the brine, but

(only a minor effect on the physical properties such as density.

The period covered by this report is from 1928 to the 

[present. Data available prior to 1928 were evaluated and the 

jresults are given in volume 3 of the International Critical 

ITables (National Research Council, 1928). The list contained 

lere is as complete as a diligent search of literature and 

>ibliographies would permit. With few noted exceptions, copies 

)f all articles were used to prepare the annotation. The units
of measurement cited in the annotation are those used in the 

reference. No conversion to the International System of Units 

(Page and Vigoureux, 1972) has been made because that work would 

reguire a substantial effort, delay publication* and impair the 

timeliness of this bibliography.

An evaluation of the guality of the data given in the cited 

references is beyond the scope of this report. The report is 

intended to supply the national geothermal effort with an 

immediate location of unevaluated data for use in preliminary 

calculations. The report will also serve as a basis for 

preparing tables of the densities of brines and for planning a 

future research effort on the physical and thermochemical 

properties of brines. In the section, Breakdown of bibliography 

by chemical species, however, we have noted those studies that 

contain data for temperatures at and greater than 100°C. Those 

studies containing data for pressures greater than ambient (that 

is for the vapor-absent pressure-temperature region) are also 

flagged separately.

The bibliography is a first step toward satisfying the needs 

of scientists and engineers as were expressed at the Conference 

on Thermodynamics and National Energy Problems (National Academy 

of Sciences, 1974) and as further amplified by the Ad Hoc 

Committee on Geothermal Chemistry (197<t) convened by the 0. S. 

Atomic Energy Commission. Support for this work has come 

exclusively from the U. S. Geological Survey's geothermal 

research program.

Experimental methods

The diverse types of experimental methods and techniques 

utilized to measure the density of a brine are discribed briefly 

below. This description is not intended to be a detailed or 

exhaustive treatise on how to measure density and specific 

volume, but rather generally to inform the reader of the meaning 

of various phrases that are used in the text of the annotations 

to describe how the particular set of experimental data was 

collected. Because the precision of the individual experimental 

technique varies widely, depending largely on the experimental 

configuration and the investigator, no attempt was made in this 

bibliography to specify the precision or accuracy of the sundry 

methods and techniques given below.

The pycnometer is perhaps the simplest and most commonly 

used method for directly measuring the density of a brine below 

100°C. The basic principle of the method is to weigh a precisely 

known volume of brine at constant temperature. Knowing the 

volume and weight of that volume, the density or specific volume
can be readily calculated. Examples in the bibliography of 

studies employing this technique are: Akerlof and Teare (1938), 

Taskoprulu (1956), and Choi and Bonner (1973).

Another commonly used series of methods to determine the 

density of brines is to immerse an object in the brine and 

measure either its loss of weight or the weight required to make 

the object just sink or float. This has been accomplished in 

numerous and ingeniously different ways. The most 

straightforward method is to take a sinker of precisely known 

density and weigh it while suspended in the brine. Another 

method is to place a float in the brine and add weights until the 

float sinks. An interesting and very useful variation of this 

method is to measure the amount of current required by an 

electromagnet to allow a magnetic float to remain suspended in 

the liquid and neither float to the surface nor sink to the 

bottom. Another method is to attach two identical floats to a 

differential balance and to immerse one in pure water and the 

other in the brine. By measuring the resulting difference in 

weight, the difference in the densities of the brine and the pure 

water can be calculated. The following studies in the 

bibliography have employed various float techniques: Bremner, 

Thompson, and Dtterback (1938), Klotz and Eckart (1912), and 

Millero (1967).

Changes in the volume (density) of a brine with respect to a 

corresponding change in temperature or pressure or both are 

generally measured with a class of devices referred to as 

dilatometers. Basically, the change in volume is measured 

through the displacement of some medium such as a piston, or 

mercury from a constant temperature reference cell, or the brine 

itself by measuring the change in height of the brine in a tube. 

Examples of studies in the bibliography employing dilatometers 

are: Adams (1931), Wright (1940), and Ellis (1966).

At high temperature and pressure, the most common technique 

for obtaining densities of brines is by determining the filling 

temperature of an autoclave. This is accomplished by partially 

filling an autoclave at a reference temperature and ambient 

pressure. The autoclave is then heated while the pressure is 

monitored. There will be a sharp break in the p-t curve when the 

autoclave is filled with liquid. From this filling temperature, 

from the initial degree of filling and from the density of the 

brine at the reference temperature, the density of the solution 

at elevated pressure and temperature can be readily calculated. 

Examples of studies in the bibliography that used this method 

are: Lemmlein and Klevtsov (1961), and Hashovets and others 

(1973).

All objects vibrate at a natural resonance frequency that is
dependant on the density of the object. By measuring the 

resonance frequency of a hollow metallic tube filled with a 

brine, the density of the brine can be readily determined. A 

study in the bibliography that employed this technique is by 

Fortier, Philip, and Desnoyers (1974).

The adiabatic compressibility is related to the velocity of 

sound in the brine, and thus the adiabatic compressibility of a 

brine is frequently determined by measuring the velocity of sound 

in the brine. Examples in the bibliography of such studies are: 

Baranowski and others (1957), and Auslander and Onitiu (1970).

The attenuation of gamma rays is related to the density of 

the medium through which they pass. Khaibullin and Borisov 

(1963) used this relation to measure the density of NaCl 

solutions at high pressure and temperature.

Nomenclature

Ambient pressure is the saturated vapor pressure of the 

solution at the specified temperature(s).

Apparent molal volume is equal to the total volume of the 

solution minus the volume of the solvent divided by the number of 

moles of the solute.

Compressibility is the change in volume per unit change in 

pressure.

Density is the mass per unit volume of a substance.

Limiting apparent molal volume is the apparent molal volume 

at infinite dilution.

Molal refers to the number of moles of the solute per 1000 

grams of solvent.

Molar refers to the number of moles of the solute per liter 

of solution.

Normal'refers to one equivalent weight of the solute per 

liter of solution.

Partial molal volume is the change in volume of a solution 

which would be brought about by the addition of one mole of 

solute to such a large amount of solution that the composition of 

the solution remains essentially unchanged.

Relative density is the ratio of the mass of a given volume
of a substance to that of an equal volume of some arbitrary 

standard.

Relative volume is the ratio of the volume of a given mass 

of a substance to that of an equal mass of some arbitrary 

standard.

Specific gravity is the ratio of the mass of a given volume 

of a substance to that of an equal volume of water.

Specific volume is the volume per unit mass of a substance.

Breakdown of bibliography by chemical species

The following list gives a breakdown of the studies cited in 

the text by chemical species. The order of list is the same as 

given in the Introduction.

As an aid in identifying the maximum temperature considered 

in each of the studies, the following flags have been added in 

front of the reference:

Temperature Flag

99°C or less no flag

199°C or less *

299°C or less **

300°C or more ***

Those studies at pressures greater than ambient pressure 

(that is in the vapor-absent pressure-temperature region) are 

flagged with a plus sign (« ).

Binary systems containing one salute are listed first. 

Three component systems are listed next.

1. Hydrochloric acid (HCl):

1. Accascina and Schaifo, 1962

5. Akerlof and Teare, 1938

18. Berecz, 1971

20. Bhinasenachar and Subrahmanyam, 1957b

29. Chapman and Newman, 1968

42. Dunn, 1966

**+ 50. Ellis and McFadden, 1968b

64. Garrett and Woodruff, 1951

66. Geffcken, 1931

81. Gucker, 1933b
82. Clicker, 1934a

94. Ingham, 1928

96. Isono and Tamamushi, 1967

116. Klochko and Kurbanov, 1954

+ 132. Lanman and Hair, 1934

136. Lengyel, 1963a

142. Lunden, 1943

*** 148. Maksimova, 1965

153. Hathieson and Conway, 1974

* 155. Mikhailov and Shutilov, 1956

164. Millero, Hoff, and Kahn, 1972b

**+ 165. Millero, 1972c

171. Owen and Brinkley, 1941

173. Owen and Erinkley, 1949

***+ 187. Rau and Narayanan Kutty, 1970

192. Redlich and Bigeleisen, 1942a

193. Redlich and Bigeleisen, 1942b

**+ 200. Samoilovich, 1970

219. Taskoprulu, 1956

240. Zen, 1957

2. Sodium chloride (Bad):

+ 2. Adams, 1931

4. Adams, Yank, Christie, and Kruus, 1974

+ 8. Allan and Lee, 1966

13. Batuecus, 1946

15. Batuecas and Meijon, 1967b

**** 17. Benson, Copeland, and Pearson, 1953

18. Berecz, 1971

+ 24. Brander, 1936

26. Bremer, Thompson and Otterback, 1938

29. Chapman and Newman, 1968

30. Choi and Bcnner, 1973

31. Cholian, 1966

*+ 32. Chou, 1968

* 33. Cornec and Krombach, 1932

36. Desnoyers, Arel, Perron, and Jolicoeur, 1969

37. Devdariani, Kolobov, and Marenina, 1973

40. Duedall and Weyl, 1965

41. Duedall and Weyl, 1967

43. Dunn, 1968

***+ 45. Egorov and Ikornikova, 1973

*** 46. Ellis and Golding, 1963

**+ 47. Ellis, 1966

52. Epifanova and others, 1973

* 55. Fabus, Korosi, and Hug, 1966

* 56. Fabus and Korosi, 1967

* 57. Fabuss and Korosi, 1968
58. Fajans and Johnson, 1942

59. Falkenhagen and Bachem, 1935

60. Fortier, Philip and Desnoyers, 1974

61. Franks and Smith, 1967

62. Freyer, 1931

66. Geffcken, 1931

67. Geffcken, 1933a

68. Geffcken, Beckmann, and Kruis, 1933b

72. Gibson, 1934

* 74. Gibson and Loeffler, 1941

80. Gucker, 1933a

81. Gucker, 1933b

82. Gucker, 1934a

84. Gucker, Chernik, and Eoy-chowdhury, 1966

*** 85. Haas, 1970

*** 86. Haas, 1971

87. Halasey, 1941

89. Helmy, Assaad, Naguib Hassan, and Sadek, 1968

***+ 93. Ikornikova and Egorov, 1968

94. Ingham, 1928

96. Isono and Tamamushi, 1967

98. Jain and Lark, 1970

101. Jones and Christian, 1937a

106. Kaulgud, 1965a

107. Kaulgud, 1965b

***< 109. Khaibullin and Borisov, 1963

*** 110. Khaibullin and Borisov, 1966

*** 111. Khaibullin and Novikov, 1973

* 123. Korosi and Fabuss, 1968a

* 124. Korosi and Fabuss, 1968b

126. Kruis, 1936

129. Kuppers, 1974

130. Lamb and Lee, 1913

131. LaMer and Gronwall, 1927

+ 132. Lanman and Mair, 1934

133. Lee, 1966

***+ 135. Lemmlein and Klevtsov, 1961

136. Lengyel, 1963a

141. Lunden, 1941

146. Mahapatra and Ray, 1958

*** 148. Maksimova, 1965

149. Maksimova and Foterov, 1973

+ 150. Manucharov, Mikhailov, and Shutilov, 1964

153. Mathieson and Conway, 1974

154. Merkel, 1939

156. Mikhailov, Savina, and Feofanov, 1957

157. Mikhailov and Syrnikov, 1959

159. Mikhailov and Shutilov, 1964

160. Millero, 1967

161. Millero and Drost-Hansen, 1968
162. Hillero, 1970

+ 163. Hillero, Knox, and Emmet, 1972a

164. Millero, Hoff, and Kahn, 1972b

**+ 165. Millero, 1972c

170. Onitiu and Auslander, 1972

171. Owen and Erinkley, 1941

172. Owen, 1944

173. Owen and Brinkley, 1949

174. Owen and Kronick, 1961

175. Passynski, 1935

176. Passynski, 1938

***+ 182. Polyakov, 1965

183. Postnikov, 1970

184. Prang, 1938

186. Raqib, 1970

190. Redlich and Rosenfeld, 1931

191. Redlich, 1940

194. Redlich and Meyer, 1964

196. Rosen, 1959

*+ 197. Rowe and Chou, 1970

198. Salceanu, 1963

***+ 199. Samoilovich and Khetchikov, 1968

201. Satyavati, Jayarama Reddy, and Subrahmanyam,

* 203. Scott, 1931

+ 204. Scott, Obenhaus, and Wilson, 1934a

* 205. Scott and Wilson, 1934b

+ 206. Seifer and others, 1971

209. Shakhov, 1972

212. Simmons and Owen, 1957

214. Stankhanova and Vasilev, 1963

216. Szalay, 1934

219. Taskoprulu, 1956

222. Tikhomirova, 1957

* 223. Tribus and others, 1959

224. Tsujioka, 1957

* 226. Onterberg, 1964

***+ 227. Orusova, 1974

229. Vaslow, 1966

230. Vaslow, 1969

237. Wirth and LoSurdo, 1968

238. Wirth and Bangret, 1972

239. Wright, 1940

240. Zen, 1957

1962

Potassium chloride (KC1):

+ 8. Allam and Lee, 1966

**+ 9. Androsov and Bagdasaryan, 1972

14. Batuecas and Varela, 1967a
*** 16. Bell, Helton, and Rogers, 1970

23. Branca and Carrelli, 1950

26. Bremer, Thompson and Otterback, 1938

28. Cantelo and Phifer, 1933

29. Chapman and Newman, 1968

30. Choi and Eonner, 1973

36. Desnoyers, Arel, Perron, and Jolicoeur, 1969

37. Devdariani, Kolobov, and Narenina, 1973

U1. Duedall and Heyl, 1967

U3. Dunn, 1968

*** HI. Ellis, 1966

52. Epifanova and others, 1973

* 56. Fabus and Korosi, 1967

* 57. Fabuss and Korosi, 1968

58. Fajans and Johnson, 1942

61. Franks and Smith, 1967

62. Freyer, 1931

** 63. Galinker, Rodnyansky, Korobkov, and Lekakh, 1964

* 66. Geffcken, 1931

67. Geffcken, 1933a

69. Geffcken and Price, 1934

72. Gibson, 1934

+ 73. Gibson, 1935

80. Gucker, 1933a

81. Gucker, 1933b

82. Gucker, 1934a

84. Gucker, Chernik, and Roy-Chowdhury, 1966

87. Halasey, 1941

***+ 93. Ikornikova and Egorov, 1968

94. Ingham, 1928

96. Isono and Tamamushi, 1967

99. Jones and Talley, 1933a

100. Jones and Talley, 1933b

102. Jones and Ray, 1937b

104. Kaminsky, 1957

105. Kaputstinskii, Stakhanova, and Vasilev, 1960

106. Kaulgud, 1965a

107. Kaulgud, 1965b

*** 110. Khaibullin and Borisov, 1966

120. Kolosov, Novik, and Chuprakova, 1971

* 123. Korosi and Fabuss, 1968a

* 124. Korosi and Fabuss, 1968b

126. Kruis, 1936

129. Kuppers, 1974

130. Lamb and Lee, 1913

131. LaHer and Gronwall, 1927

+ 132. Lanman and Hair, 1934

134. Legrand and Paris, 1966

136. Lengyel, 1963a

140. Longsworth, 1935
141. Lunden, 1941

144. Maclnnes, Dayhoff, and Ray, 1951

145. Maclnnes and Dayhoff, 1952

*** 148. Maksimova, 1965

+ 150. Manucharov, Mikhailov, and Shutilov, 1964

153. Mathieson and Conway, 1974

154. Merkel, 1939

156. Mikhailov, Savina, and Feofanov, 1957

157. Mikhailov and Syrnikov, 1959

+ 159. Mikhailov and Shutilov, 1964

161. Millero and Drost-Hansen, 1968

**+ 165. Millero, 1972c

167. Millero and Knox, 1973b

170. Onitiu and Auslander, 1972

171. Owen and Brinkley, 1941

172. Owen, 1944

173. Owen and Erinkley, 1949

174. Owen and Kronick, 1961

176. Passynski, 1938

* 178. Perman and Drry, 1929

***+ 182. Polyakov, 1965

183. Postnikov, 1970

184. Prang, 1938

186. Raqib, 1970

190. Redlich and Rosenfeld, 1931

191. Redlich, 1940

194. Redlich and Meyer, 1964

198. Salceanu, 1963

***+ 199. Samoilovich and Khetchikov, 1968

201. Satyavati, Jayarama Reddy, and Subrahmanyam, 1962

* 203. Scott, 1931

+ 204. Scott, Obenhaus, and Wilson, 1934a

+ 205. Scott and Wilson, 1934b

+ 206. Seifer and others, 1971

209. Shakhov, 1972

212. Simmons and Owen, 1957

213. Spedding, Pikal, and Ayers, 1966

216. Szalay, 1934

221. Thomas and Perman, 1934

222. Tikhomirova, 1957

224. Tsujioka, 1957

229. Vaslow, 1966

234. Wirth, 1937

239. Wright, 1940

240. Zen, 1957

4. Calcium chloride (CaCl 2 ):

11. Auslander and Onitiu, 1970

10
12. Baranowski, Jacob and Sarnowski, 1957

18. Berecz, 1971

* 22. Bogatykh and Evnovich, 1965

29. Chapman and Newman, 1968

39. Drucker, 1941

42. Dunn, 1966

'**+ 48. Ellis, 1967

53. Ezrokhi, 1967a

** 63. Galinker, Rodnyansky, Korobkov, and Lekakh, 1964

67. Geffcken, 1933a

80. Gucker, 1933a

81. Gucker, 1933b

83. Gucker, 1934b

90. Hepburn, 1932

92. Hurtado, Mateo, Serna, and Vidal-Abarca, 1973

96. Isono and Tamamushi, 1967

117. Klochko, Taukesheva, and Bezhaev, 1959

122. Kononemko and Sashevskaya, 1974

133. Lee, 1966

140. Longsworth, 1935

143. Lyons and Riley, 1954

*** 148. Maksimova, 1965

+ 150. Manucharov, Hikhailov, and Shutilov, 1964

157. Mikhailov and Syrnikov, 1959

* 159. Mikhailov and Shutilov, 1964

**+ 165. Millero, 1972c

+ 178. Perman and Orry, 1929

179. Perron, Desnoyers, and Millero, 1974

180. Pesce, 1932

***+ 182. Polyakov, 1965

198. Salceanu, 1963

* 203. Scott, 1931

210. Shedlovsky and Brown, 1934

228. Vasilev, Fedyainov, Karapet*yants, and Karpachev, 1973

* 232. Voitko, Kcvaleva, and Tspalin, 1972

240. Zen, 1957

5. Ferrous chloride (FeCl 2 ):

120. Kolosov, Novik, and Chuprakova, 1971

134. Legrand and Paris, 1966

*** 148. Maksimova, 1965

6. Sulfuric acid (H 2 S0 4 ):

18. Berecz, 1971

20. Bhimasenachar and Subrahmanyam, 1957b

29. Chapman and Newnan, 1968

11
64. Garrett and Woodruff, 1951

71. Gibson, 1931

113. Khare, 1962b

118. Klotz and Eckert, 1942

139. Lindstrom and Wirth 1969

* 155. Mikhailov and Shutilov, 1956

165. Millero, 1972c

240. Zen, 1957

7. Sodium hydrogen sulfate (NaHSO*):

139. Lindstrom and Wirth 1969

165. Millero, 1972c

171. Owen and Erinkley, 1941

8. Sodium sulfate (Na 2 S04 ):

23. Branca and Carrelli, 1950

29. Chapman and Newman, 1968

42. Dunn, 1966

**+ 49. Ellis, 1968a

52. Epifanova and others, 1973

* 55. Fabus, Korosi, and Hug, 1966

* 56. Fabus and Korosi, 1967

* 57. Fabuss and Korosi, 1968

69. Geffcken and Price, 1934

70. Gibson, 1927

72. Gibson, 1934

78. Glass and Madgin, 1934

82. Gucker, 1934a

106. Kaulgud, 1965a

*** 111. Khaibullin and Novikov, 1973

* 123. Korosi and Fabuss, 1968a

* 124. Korosi and Fabuss, 1968b

133. Lee, 1966

140. Longsworth, 1935

*** 148. Maksimova, 1965

* 150. Manucharov, Hikhailov, and Shutilov, 1964

156. Mikhailov, Savina, and Feofanov, 1957

159. Mikhailov and Shutilov, 1964

**+ 165. Millero, 1972c

167. Millero and Knox, 1973b

171. Owen and Erinkley, 1941

171. Owen and Erinkley, 1941

177. Pearce and Eckstrom, 1937

***+ 182. Polyakov, 1965

183. Postnikov, 1970

184. Prang, 1938

12
209. Shakhov, 1972

211. Shilovskaya and Lenkova, 1974

237. Wirth and LoSurdo, 1968

240. Zen, 1957

9. Potassium hydrogen sulfate (KHS04 ):

165. Millero, 1972c

10. Potassium sulfate (K2 S04 ):

+ 3. Adams, 1932

23. Branca and Carrelli, 1950

29. Chapman and Newman, 1968

41. Duedall and Weyl, 1967

42. Dunn, 1966

**+ US. Ellis, 1968a

* 77. Ginzburg, 1965

87. Halasey, 1911

102. Jones and Ray, 1937b

103. Jones and Colvin, 1940

104. Kaminsky, 1957

134. Legrand and Paris, 1966

138. Likhoded, Zapol'skii, and Sazhin, 1973

*** 148. Maksimova, 1965

**+ 165. Hillero, 1972c

167. Millero and Knox, 1973b

177. Pearce and Gckstrom, 1937

***+ 188. Ravich and Borovaya, 1971a

  189. Ravich and Borovaya, 1971b

196. Rosen, 1959

209. Shakhov, 1972

222. Tikhomirova, 1957

234. Wirth, 1937

240. Zen, 1957

11. Ferrous sulfate (FeS04 ):

134. Legrand and Paris, 1966

12. Carbonic acid and dissolved carbon dioxide 

(C0 2[ag]):

165. Millero, 1972c

13
13. Sodium hydrogen carbonate (NaHC03 ):

165. Millero, 1972c

** ** 182. Polyakov, 1965

183. Postnikov, 1970

211. Shilovskaya and Lenkova, 1974

14. Sodium carbonate (Na2 C03 ):

25. Brannland, 1958

59. Falkenhagen and Bachem, 1935

68. Gef£cken, Beckmann, and Kruis, 1933b

69. Geffcken and Price, 1934

+ 73. Gibson, 1935

* 76. Ginzburg, Pikulina, and Litvin, 1964b

* 77. Ginzburg, 1965

130. Lamb and Lee, 1913

156. Hikhailov, Savina, and Feofanov, 1957

165. Millero, 1972c

180. Pesce, 1932

183. Postnikov, 1970

184. Prang, 1938

211. Shilovskaya and Lenkova, 1974

240. Zen, 1957

15. Potassium hydrogen carbonate (KHC03 ):

41. Duedall and Heyl, 1967 

165. Billero, 1972c

16. Potassium carbonate (K 2C03 ):

**

*

* 

***

63. Galinker, Rodnyansky, Korobkov, and Lekakh, 1964

75. Ginzburg, Pikulina, and Litvin, 1964a

77. Ginzburg, 1965

148. Kaksimova, 1965

165. Millero, 1972c

184. Prang, 1938

203. Scott, 1931

240. Zen, 1957

17. Sodium hydroxide (NaOH):

6. Akerlof and Kegeles, 1939

19. Bhimasenachar and Subrahmanyam, 1957a

21. Bodanszky and Kauzmann, 1962

14
29. Chapman and Newman, 1968

***+ 38. Dibrov, Hashovets, and Matveeva, 1964

81. Gucker, 1933b

91. Hepler, Stokes, and Stokes, 1965

119. Kobus, 1955

*** 125. Krey, 1972

*** 127. Krumgal'z and Mashovets, 1964

+ 132. Lanman and Hair, 1934

136. Lengyel, 1963a

*** 147. Maksimova and Yushkevich, 1963

* 158. Mikhailov and Fenjou, 1960

164. Millero, Hoff, and Kahn, 1972b

165. Millero, 1972c

169. Nicolai, Ernst, and Wegkamp, 1951

171. Owen and Brinkley, 1941

183. Postnikov, 1970

195. Fiedl, 1972

215. Subrahmanyam, 1960

217. Tamas, 1963

218. Tamas, 1964

219. Taskoprulu, 1956

224. Tsujioka, 1957

240. Zen, 1957

18. Potassium hydroxide (KOH):

7. Akerlof and Bender, 1941

19. Bhimasenachar and Subrahmanyam, 1957a

29. Chapman and Newman, 1968

81. Gucker, 1933b

108. Kelley, Borza, and Harringer, 1965

+ 132. Lanman and Mair, 1934

136. Lengyel, 1963a

*** 151. Mashovets, Dibrov, Krumgal'z, and Natveeva, 1965

* 158. Mikhailov and Fenjou, 1960

165. Millero, 1972c

171. Owen and Brinkley, 1941

215. Subrahmanyam, 1960

217. Tamas, 1963

218. Tamas, 1964

* 220. Than, Gubbins, and Walker, 1967

** 231. Vogel, Boutsis, Kehrer, Landsman, and Tschinkel, 1967

240. Zen, 1957

19. "Silicic acid" (Si02 [ag]): 

No entries.

15
20. Sea water and sea water concentrates:

+ 11. Eckart, 1958

51. Ener and Taskoprulu, 1951

* 57. Fabuss and Korosi, 1968

* 65. Gastaldo, 1962

* 88. Hara, Nakamura, and Higashi, 1932

* 95. Isdale and Morris, 1972

* 121. Korosi and Fabuss, 1968b

***+ 152. Mashovets, Puchkov, Smaev, Federov, and Federov, 1973

21. Sodium chloride - potassium chloride (NaCl - KC1):

* 57. Fabuss and Korosi, 1968

97. Ivanova, 1972

** 115. Klevtsov, 1959

* 121. Korosi and Fabuss, 1968b

128. Kulkarni, 1969

137. Lengyel and Fezler, 1963b

166. Millero, 1973a

201. Satyavati, Jayarama Beddy, and Subrahmanyam, 1962

222. Tikhomirova, 1957

229. Vaslow, 1966

22. Sodium chloride - calcium chloride (NaCl - CaCl2 ):

* 51. Ezrokhi, 1967b

97. Ivanova, 1972

133. Lee, 1966

23. Potassium chloride - calcium chloride (KC1 - CaCl 2 ): 

* 51. Ezrokhi, 1967b

21. Sodium chloride - potassium chloride - calcium chloride 

(NaCl - KC1 - CaCl 2 ):

* 5U. Ezrokhi, 1967b

25. Other studies in complex solutions:

10. Anosov and Bysova, 1917

27. Bysova, 1963

3* 39. Drucker, 1911

'; * 51. Ezrokhi, 1967b

16
* 57. Fabuss and Korosi, 1968

71. Gibson, 1931

112. Khare, 1962a

120. Kolosov, Novik, and Chuprakova, 1971

122. Kononemko and Sashevskaya, 1974

* 124. Korosi and Fabuss, 1968b

133. Lee, 1966

134. Legrand and Paris, 1966

168. Nickels and Allmand, 1937

169. Nicolai, Ernst, and Wegkamp, 1951

171. Owen and Erinkley, 1941

185. Ramanathan and Raman, 1969

202. Satyavati, 1968

208. Sevzov, 1937

222. Tikhomirova, 1957

225. Dkinashi, 1959

233. Volz-Fladrich, 1962

234. Wirth, 1937

236. Wirth, 1940b

237. Wirth and LoSurdo, 1968

References cited

Ad Hoc Committee on Geothermal Chemistry, 1974, A recommended 

research program in geothermal chemistry: Wash., D. C., 

U.S. Atomic Energy Comm., Publ. WASH- 1344, 48 p.

National Academy of Sciences, 1974, Conference on thermodynamics 

and national energy problems: Wash. D. C., Natl. Acad. 

Sci., 424 p.

National Research Council, 1928, International critical tables of 

numerical data, physics, chemistry and technology: New 

York, McGraw-Hill, v. 3, 444 p.

Page, C. H. and Vigoureux, Paul, eds., 1972, The international 

system of units (SI): U.S. Natl. Bur. Stand. Spec. Publ. 

330, 42 p.

17
Bibliography

1. Accascina, Filippo, and Schaivo, Silvia, 1962,

Dltrasonic behaviour of liquid systems. Ultrasonic 

velocity and adiabatic compressibility of aqueous 

solutions of mineral acids at different temperatures, in 

Symposium on Electrolytes, Trieste, 1959. Published in 

Electrolytes, Proceedings of an International Symposium, 

p. 301 - 308 (printed in 1962).

Experimental study on the adiabatic compressibility of 

HCl from 0 to 9 molar at ambient pressure from 15° to 

60°C. Compressibility data were derived from the 

velocity cf sound in solutions. Adiabatic 

compressibility of the solutions and the partial molal 

compressibility and partial molal volume of H 2 0 in the 

solutions are given on a graph.

2. Adams, L. H., 1931, Equilibrium in binary systems under

pressure. I. Experimental and thermodynamic 

investigations of the system, NaCl-H 2O, at 25°C: Am. 

Chem. Soc. Jour., v. 53, p. 3769 - 3813.

Experimental study of the compressibility of NaCl 

solutions (0 to 25 wt percent) at 25°C and 0 to 12 kb of 

pressure. Compressibility was measured by the 

piston-displacement method. Data are presented as 

tables of experimental and smoothed numbers.

3. Adams, L. H., 1932, Equilibrium in binary systems under

pressure. II. The system K 2 S0 4 - H 20 at 25°C: Am. 

Chem. Soc. Jour., v. 54, p. 2229 - 2243.

An experimental study of the compressibility and density 

of K 2 S04 solutions (0 to 10 wt percent) at 25°C and from 

0 to 10 kb. Density was measured only at ambient 

pressure. The compressibility was measured by the 

piston-displacement method and the density was measured 

with a pycnometer. Data are presented in tables as both 

experimental and smoothed numbers and graphically.

4. Adams* W. A., Yank, R., Christie, R. 0., and Kruus,

J. , 1974, An automated apparatus for precision density 

measurements of liquids: Canadian Jour. Chem. Eng., v. 

52, p. 121 - 124.

18
The densities of NaCl solutions, 0.026 to 0.502 molar, 

were measured at 25° and ambient pressure using a 

vibrating density meter. Data are presented in a table 

and are represented by the Redlich-Meyer equation. The 

appropriate constants are also given in a table. [Note: 

The authors have used 0.997075 g/cm 3 as the density of 

water at 25° and 1 atm. This value is correct for the 

density of water in g/ml. The correct density is 

0.9970U7

5. Akerlof, Gosta, and Teare, J. W., 1938, A note on the

density of aqueous solutions of hydrochloric acid: Am. 

Chem. Soc. Jour., v. 60, p. 1226 - 1228.

Experimental study on the apparent molal volume and 

density of HC1 solutions (0.56 to 16.81 molal) at 

ambient pressure and in the temperature range 0° to 

80°C. Density data were derived from pycnometry. 

Experimental data are presented in tables, on graphs, 

and as empirical equations.

6. Akerlof, Gosta, and Kegeles, Gerson, 1939, The density

of aqueous solutions of sodium hydroxide: Am. Chem. 

Soc. Jour., v. 61, p. 1027 - 1032.

Experimental study on the density and apparent molal 

volume of NaOH solutions (0.51 to 27.08 molal) at 

ambient pressure and in the temperature range 0° to 

70°C. Density data were derived from pycnometry. 

Experimental data are contained in tables, on graphs, 

and represented as expirical equations.

7. Akerlof, Gosta, and Bender, Paul, 1941, The density of

aqueous solutions of potassium hydroxide: Am. Chem. 

Soc. Jour., v. 63, p. 1085 - 1088.

Experimental study on the density and apparent molal 

volume of KOH solutions (0.36 to 17.82 molal) at the 

ambient pressure and in the temperature range 0° to 

70°C. Density data were derived from pycnometry. 

Experimental data are given in tables, on a graph, and 

as empirical equations.

8. Allam, D. S. and Lee, W. H., 1966, Ultrasonic studies

of electrolyte solutions. II. Compressibilities of 

electrolytes: Chem. Soc. (London) Jour., v. 1966A, p.

19
5-9.

Experimental and calculated study on the compressibility 

of KC1 and NaCl solutions (2.0 to U.2 molar) at 1 kb and 

25°C. Compressibility data were derived from 

measurements of the velocity of sound. Experimental and 

smoothed data are given in tables, on graphs, and as 

expirical eguations.

9. Androsov, V. I., and Bagdasaryan, V. S., 1972,

[Densities of aqueous solutions of potassium chloride at 

high temperatures]: Tr. Gos. Nauch-Issled. Inst. 

Automat. Proizvod. Protsessov Khim. Prom. Tsvet Met., 

v. 1972, p. 35 - 38. In Russian.

The density of agueous KC1 solutions from 0.001. to 0.5 

molal were measured at 75 atm from 40° to 280°C. The 

data fits the empirical eguation: density = 1.058 + 

0.0386 m - 5.3/(10» m ) - (9.98 - 0.605 m)/(10* t) where 

m is the molality and t is the temperature in °C. 

[Original text unavailable to the authors. Data were 

taken from Chem. Abs., 79:U595Um, 1973.]

10. Anosov, V. Ya., and Bysova, E. A., 1947, [Equilibrium

in the system KC1 - K 2 S0 4 - H 20]: Akad. Nauk SSSR., 

Inst. Obshchei Neorg. Khim., Sektor Fiz.-Khim. Anal., v. 

15, p. 118 - 12U. In Russian.

Experimental study of the composition and density of 

saturated aqueous solutions in the system KCl - K 2 SO« - 

H 2 0 at ambient pressure between 0° and 70°C. Densities 

were derived from pycnometry. Experimental data are 

given in a table.

11. Auslander, D. and Onitiu, Lia, 1970, [Compressibility

of aqueous solutions of some halogens III.

Alkaline-earth chlorides]: Jour. Chim. Physics

Physiochim. Eiol., v. 67, p. 1557 - 1562. In French.

Experimental study on the adiabatic compressibility of 

CaCl 2 solutions (0.2 to 3 molal) at ambient pressure in 

the temperature range 15° to 50°C. Compressibility data 

were derived from measurements of the velocity of sound. 

Experimental data are presented graphically.

12. Baranowski, B., Jacob, H. P. and Sarnowski, M., 1957,

20
[Study of selective solutions by sound velocity and 

compressibility measurements]: Naturwissenschaften, v. 

44, p. 30 - 31. In German.

Experimental study on the compressibility and density of 

CaCl 2 solutions (2.1, 4.2, and 4.9 molar) at ambient 

pressure and 25°C. Compressibility data were derived 

from velocity of sound measurements and densities from 

pycnometry. Experimental data are presented in 

graphical form.

13. Batuecus, T., 1946, [Partial molecular volumes at 0°,

of water, sodium chloride, and potassium chloride in 

solutions of those halogens]: Anales de Fisica Quimica 

(Madrid), v. 42, p. 713 - 722. In Spanish.

Theoretical study on the apparent molal volume of NaCl 

and KCl solutions at 0°C and ambient pressure. Data 

were derived from earlier literature and given as 

smoothed values in tables.

14. Batuecas, T., and Varela, Concepcion, 1967a,

[Experimental investigation on aqueous solutions of 

strong electrolytes. II. Densities, apparent molal 

volumes, and partial molal volumes of KCl, NaCl, and KBr 

at 25°C and concentrations in the interval 0.5 to 0.6V 2 

H]: Real Acad. Ciencias (Madrid) Rev., v. 61, p. 1 89 - 

211. In Spanish.

Experimental study of the density of 0.02 to 0.5 molar 

KCl solutions at ambient pressure and 25°C. Densities 

were obtained from pycnometry. Experimental densities 

and the apparent and partial molal volumes are given in 

tables and by empirical equations.

15. Batuecas, T., and Meijon, Carmen, 1967b, [Experimental

investigation on aqueous solutions of strong 

electrolytes. III. Densities, apparent molal volumes, 

and partial molal volumes at 25°C and concentrations in 

the interval 0.5 to 0.1 M of NaCl]: Real Acad. Ciencias 

(Madrid) Rev., v. 61, p. 563 - 571. In Spanish.

Experimental study of the densities of 0.1 to 0.5 molar 

NaCl solutions at 25°C and ambient pressure. Data were 

derived from pycnometry. Experimental data for 

densities apparent and partial molal volumes are given 

in tables and by empirical equations.

21
16. Bell, J. T., Helton, D. M. and Rogers, T. G. , 1970,

Densities of aqueous KCl and D02 S0 4 from 25° to 371°: 

Jour. Chem. Eng. Data, v. 15, p. 44 - 46.

Experimental study on the density of aqueous KCl (0.1 to 

1.0 molar) at ambient pressure from 25° to 370°C. 

Density data were obtained from dilatometry using X-ray 

absorption to measure fluid level. Experimental data 

are given in tabular and graphical form.

17. Benson, S. W., Copeland, C. S. and Pearson, D., 1953,

Molal volumes and compressibilities of the system sodium 

chloride - water above the critical temperature of 

water: Jour. Chem. Phys., v. 21, p. 2208 - 2212.

Experimental study on the compressibility and on the 

apparent and partial molal volumes of the system NaCl - 

H 2 0 (0.2 to 6.74 wt percent NaCl) in the pressure range 

232 to 300 bars and in the temperature range 380 to 

400°C. Experimental data are given in tables, on 

graphs, and as empirical equations.

18. Berecz, E., 1971, [Structure of molal chloride -

hydrochloric acid - water and metal sulfate - sulfuric 

acid - water type systems]: Teor. Rastvorov. v. 1971, 

p. 77 - 85. In Russian.

An experimental study of the viscosity of H2 S04 , HC1, 

CaCl 2 , and NaCl solutions from 10° to 50°c at ambient 

pressure. (Original unavialable. Data taken from Chem. 

Abs., 78:48058p, 1973.)

19. Bhimasenachar, J. and Subrahmanyam, S. V., 1957a,

Compressibilities of sodium and potassium hydroxides: 

Nature, v. 179, p. 627 - 628.

Experimental study on the compressibility of NaOH and 

KOH solutions (0 to 8.0 molar) at ambient pressure and 

25°C. Compressibility data were derived from optical 

diffraction. The data are presented graphically and as 

empirical equations.

20. Bhimasenachar, J., and Subrahmanyam, S. V., 1957b,

Compressibilities of mineral acids: Acoustical Soc. 

Am. Jour., v. 29, p. 899-901.

22
Experimental study on the apparent molal compressibility 

of HC1 from 0 to 5 molar and H 2 S0 4 from 0 to 9 molar at 

ambient pressure and 27°c. Data are derived from the 

velocity of sound in the solutions. Results are given 

on a graph and as empirical equations.

21. Bodanszky, Agnes and Kauzmann, Walter, 1962, The

apparent molal volume of sodium hydroxide at infinite 

dilution and the volume change accompanying the 

ionization of water: Jour. Phys. Chem., v. 66, p. 177 

- 179.

Experimental and calculated study on the apparent molal 

volume of NaOH solutions (0.06 to 1.0 molar) at ambient 

pressure and 30°C. Apparent molal volume data were 

derived from dilatometry. Experimental data of the 

authors on NaOH and from other sources on KCl, NaCl, and 

HCl are given on a graph. An empirical equation was 

also used.

22. Bogatykh, S. A. and Evnovich, I. D., 1965, [Density of

aqueous solutions of lithium chloride, lithium bromide, 

and calcium chloride]: Zh. Prikl. Khim., v. 38, p. 945 

- 946. In Russian. English translation in Russian 

Jour. Applied Chem., v. 38, p. 932 - 933.

Experimental study on the density of CaCl 2 solutions in 

the concentration range 30 to 45 wt percent at ambient 

pressure and from 10° to 100°C. Density data were 

derived from areometry. Experimental data are presented 

in tables.

23. Branca, G., and Carrelli, A., 1950, [The

compressibility of electrolyte solutions]: II Nuovo 

Cimento, v. 7, p. 190 - 195. In Itallian.

Experimental study of the apparent molar compressibility 

of solutions of KCl at 3.60 and 1.80 mol/1, of Na 2 S04 at 

0.87 and 0.43 mol/1 and of K 2 S04 at 0.57 and 0.28 mol/1 

at ambient pressure and temperature. Data were derived 

from the measurement of the velocity of sound. 

Experimental results are given in a table and on a 

graph.

24. Brander, Einar, 1936, [Compressibility of aqueous

solutions]: Fennica Sci. Soc. Commentationes

23
Phys.-Hath., v. 9, p. 1 - 8. In German.

Calculated study on the compressibility of NaCl 

solutions in the pressure range 157 to 472 kg/cm* and in 

the temperature range 0° to 12°C. Smoothed data are 

presented in tables and as empirical equations.

25. Brannland, R., 1958, [Density and viscosity of sodium

carbonate and sodium sulfide solutions]: Ost. Chem.

Zeit., v. 59, p. 104 - 106. In German.

Experimental study of the density of Na 2C0 3 solutions 

from 0 to 2.5 molar at 20° and 50°C and ambient 

pressure. Data derived from pycnometry. Densities are 

presented in tables and on graphs.

26. Bremner, R. W. , Thompson, T. G. and Otterback, C. L.,

1938, Specific gravities of pure and mixed salt 

solutions in the temperature range of 0° to 25°: Am. 

Chem. Soc. Jour., v. 60, p. 2616 - 2618.

Experimental and calculated study on the specific 

gravity of NaCl, KC1, and MgS0 4 solutions and their 

mixtures at ambient pressure between 0° and 25°C. 

Specific gravity measurements were derived from weighing 

an immersed glass bulb. Although not all of the data 

are presented, some experimental data are given in 

tables and as empirical equations.

27. Bysova, E. A., 1963, [Agueous solutions in the System

K 2C0 3-K 2 S0 4 -KC1-H 2 0 at 0, 30, 50, and 70°]: zh. Neorg. 

Khim., v. 8, p. 1950 - 1954. In Russian. English 

translation in Russian Jour. Inorg. Chem., v. 8, p. 

1014 - 1017.

Specific gravity of saturated solutions in the system 

K 2 C03 -K2 S04 -KC1-H 2 0 at 0°, 30°, 50°, and 70°C and 

ambient pressure. Data used are from previous studies 

of the same author. Experimental results are given in 

tables and on figures.

28. Cantelo, R. C. and Phifer, H. E. , 1933, Partial molal

volumes of cobalt sulfate and cadmium iodide: Am. 

Chem. Soc. Jour., v. 55, p. 1333 - 1338.

Calculated study on the partial molal volume of

24
solutions of KC1 from 0.27 to 2.30 molal at ambient 

pressure and 25°C. Calculated data are given as a 

smoothed table, as graphs, and as empirical eguations.

29. Chapman* T. H., and Newman, John, 1968, A compilation

of selected thermodynamic and transport properties of 

binary electrolytes in aqueous solutions: Univ. 

California (Berkeley), Lawrence Radiation Lab., Rept. 

No. OCRL-17767, 297 p.

A compilation of observed densities and other properties 

at ambient pressure between 0° and 70°C for the 

following sclutes: CaCl2 , HC1, H 2 so 4 , KCI, KOH, K 2 so 4 , 

NaCl, NaOH, and Na 2 S04 . Data are given in tables. 

Densities are taken without annotation from the 

literature.

30. Choi, Y. S. and Bonner, 0. D., 1973, The partial molal

volumes of some representative solutes in H 2 0 and D2 0: 

Zeit. Phys. Chem., Neue Folge, v. 87, p. 188 - 197.

Experimental study of apparent molal volumes based on 

density measurements of NaCl and KCI solutions from 

"0.0" to 1.0 molal at ambient pressure over the 

temperature range 0.19° to 76.68°C. Densities were 

measured by pycnometry. Data are presented as tables of 

apparent molal volumes.

31. Cholian, P. P., 1966, [Adiabatic compressubility of

aqueous solutions of electrolytes]: Akust. Zhur., v. 

12, p. 93 - 97. In Russian.

Experimental study on the adiabatic compressibility of 

NaCl and KCI solutions, 0 to 9 mol percent at ambient 

pressure and 20°C. Compressibilities were derived from 

measurements of the velocity of sound in the solutions. 

Experimental data are given graphically and in a table.

32. Chou., J. C.-S., 1968, Thermodynamic properties of

aqueous sodium chloride solutions from 32° to 350°F: 

Okla. State Univ., Ph. D. Dissertation, 121 p.

Experimentally measured compressibilities of NaCl 

solutions from 0 to 25 wt percent between 250 and 5000 

psig from 72° to 350°F. Compressibilities were derived 

from displacement of a calibrated piston. Experimental 

data are given in a table as a function of wt percent

25
Nad, Celcius temperatures and pressures at 10, 100, 

200, and 300 atm. An empirical function in temperature, 

pressure, and composition is derived from experimental 

data and the data of Fabuss (1965), and those in the 

International Critical Tables, v. 3, 1928. Some results 

are also given graphically.

33. Cornec, E. and Krombach, H., 1932, [Equilibrium between

potassium chloride, sodium chloride, and water from -23

to 190°C]: Annales Chim., v. 18, p. 5 - 31. In French.

Experimental study on the volume of NaCl (0.75 to 3.56 

molal) and KCl (0.26 to 2.43 molal) solutions at ambient 

pressure in the temperature range -23° to 190°C. Volume 

data were derived by filling an autoclave. Experimental 

data are given in tables and on graphs.

34. Couture, A. M., and Laidler, K. J., 1956, The partial

molal volumes of ions in agueous solutions. I. 

Dependence on charge and radius: Canadian Jour. Chem., 

v. 3U, p. 1209 - 1216.

A theoretical discussion on the relation between molal 

volumes of ions to the Goldschmidt crystal radius and 

the ionic charge. Partial molal volumes and effective 

radii of monatomic cations and anions are derived for 

ambient pressure and 25°C. The source data are 

contained in the International Critical Tables, vol 3, 

of 1928 and in earlier compilations. The results are 

given on tables, graphs, and by empirical equations.

35. Couture, A. M., and Laidler, K. J. , 1967, The partial

molal volumes of ions in aqueous solutions. II. An 

empirical equation for oxy-anions: Canadian Jour. 

Chem., v. 35, p. 207 - 210.

A theoretical discussion on the relation of partial 

molal volumes of oxyanions to the Goldschmidt crystal 

radium and ionic charge. Partial molal volumes and 

effective radii of oxyanions are derived from density 

data given in the International Critical Tables, vol. 

3, of 1928 at ambient pressure and 25°C. Data are given 

in a table, on a figure and by empirical equations.

36. Desnoyers, J. E., Arel, M., Perron, G., and Jolicoeur,

C., 1969, Apparent molal volumes of alkali halide in

26
water at 25°. Influence of concentration dependence: 

Jour. Phys. Chem., v. 73, p. 3346 - 3351.

Experimental and calculated study on the apparent molal 

volume and density of 0.03 to 0.5 molar solutions of 

NaCl, NaF, KF and KC1 at ambient pressure and 25°C. 

Density and apparent molal volume data were derived from 

the weight of a sinker in solution. Experimental and 

calculated data are presented in tables, on graphs, and 

as empirical equations.

37. Devdariani, A. K., Kolobov, N. P., and Marenina, K. N.,

1973, [Ultrasonic study of the volumetric properties of 

aqueous solutions of some electrolytes]: Zhur. Fiz. 

Khim. , v. 47, p. 3006 - 3009. In Russian.

Experimental study in which the partial molal volume of 

NaCl and KC1 in aqueous solution was determined by sound 

velocity measurements. [Original text unavailable to 

authors. Data taken from Chem. Abs. 80:112984g, 1973.]

38. Dibrov, I. A., Hashovets, V. P, and Hatveeva, R. R.,

1964, [Density and compressibility of aqueous solutions 

of sodium hydroxide at high temperatures]: Zh. Prikl. 

Khim., v. 37, p. 29 - 36. In Russian. English 

translation in Russian Jour. Applied Chem., v. 37, p. 

38 - 44.

Experimental study on the density and compressibility of 

3 to 18 wt percent NaOH solution at pressures up to 1450 

bars and from 0° to 350°C. Density data were calculated 

from electromagnetic float measurements. Experimental 

and smoothed data are given in tables, on graphs, and as 

empirical equations.

39. Drucker, Carl, 1941, [Study on partial specific volumes

in binary and ternary solutions]: Arkiv Kemi, Mineral. 

Geol., v. 14A, p. 1-48. In German.

Experimental and calculated study on the partial 

specific volume of CaCl 2 - Na 2 S0 4 solutions from 0.001 

to 0.02 g CaCl 2 per g of 6.094 wt percent Na2 S0 4 and of 

CaCl2 solutions from 0.002 to 0.02 g CaCl 2 per g of 

solution at ambient pressure and 25°C. Volume data were 

derived from pycnometry. Data were corrected for 

barometric pressure. Experimental data are presented in 

tables, on graphs, and as empirical equations.

27
40. Duedall, I. W., and Weyl, P. K., 1965, Apparatus for

determining the partial equivalent volumes of salts in 

aqueous solutions: Rev. Sci. Instrum., v. 36, p. 528 - 

531.

Experimental study on the partial molal volume of NaCl 

at ambient pressure and 0.8°C. Data were obtained from 

dilatometry. The equipment and procedure are described 

in detail. The limiting apparent molal volume of NaCl 

is 12.78 ml/mol. The partial molal volumes of some 

major salts in artificial sea water (3.013 wt percent 

solids) at 0.8°C are also given in a table.

41. Duedall, I. H. and Weyl, P. K., 1967, The partial

equivalent volumes of salts in seawater: Limnol.

Oceanog., v. 12, p. 52 - 59.

Experimental study on the partial molal volume of NaCl, 

KC1, Na2 S04 , K 2 S0 4 , and KHC0 3 solutions of 30 to 40 per 

mill salinity at ambient pressure and from 0° to 25°C. 

Volume data were derived from dilatometry. Experimental 

data are presented in tables, on graphs, and as 

empirical equations.

42. Dunn, L. A., 1966, Apparent molal volumes of

electrolytes. Part I. Some 1-1, 1-2, 2-1, 3-1 

electrolytes in aqueous solutions at 25°C: Faraday Soc. 

Trans., v. 62, p. 2348 - 2354.

Experimental study on the density and apparent molal 

volumes of 0.001 to 1.0 molar solutions of Na 2 S04 , 

K 2 S0 4 , CaCl 2 , and HCl at ambient pressure and 25°C. 

Limiting apparent molar volumes of the dissolved salts 

and of ionic species were calculated, using the volume 

of the aqueous chloride ion equal to 22.32 ml/mole. 

Density data were obtained from pycnometry and 

dilatometry. Experimental data are presented in 

graphical and tabular form.

43. Dunn, L. A., 1968, Apparent molal volumes of

electrolytes, Part II. Some 1-1 electrolytes in aqueous 

solution at 25°c: Faraday Soc. Trans., v. 64, p. 1898 - 

1903.

Experimental study on the apparent molal volume and 

density of 0.001 to 1.0 molal solutions of KC1 and NaCl 

at ambient pressure and 25°C. Limiting apparent molar

28
volumes of the dissolved salts and of ionic species were 

calculated. Density data were calculated from 

pycnometry and apparent molal volumes from dilatooetry. 

Experimental data are given in tables, on graphs, and as 

empirical equations.

44. Eckart, C., 1958, Properties of water. II. The

equation of state of water and sea water at low 

temperatures and pressures: Am. Jour. Sci., v. 256, p. 

225 - 240.

Calculated study on the p-v-t properties of seawater (0 

to 40 g/kg salinity ) from 0 to 1000 atm of pressure and 

in a temperature range from 0° to 40°C. Smoothed data 

are given in tables, on graphs, and as empirical 

equations.

45. Egorov, V. M., and Ikornikova, N. Yu., 1973, [Partial

molar volumes of aqueous chloride solutions at high 

temperatures and pressures]: Zap. Vses. Mineral. 

Obshchestva (Lenningrad), v. 102, p. 272 - 282. In 

Russian.

Theoretical study on the apparent molal volume of NaCl 

solutions from 1 to 6 molal at 500, 1000, and 1500 

kg/cm2 from 200° to 700°C. Data were taken from 

Ikornikova and Egorov (1968). Results are given in a 

table and on a graph.

46. Ellis, A. J. and Golding, R. H., 1963, The solubility

of carbon dioxide above 100°C in water and sodium 

chloride solutions: Am. Jour. Sci., v. 261, p. 47 - 60.

An experimental and calculated study on the density of 

NaCl solutions from 0.5 to 3.0 molal in the pressure 

range 0 to 101.3 bars and at temperatures from 0° to 

350°C. Data were obtained by a modified filling 

technique using a stainless steel vessel. Density data 

are presented in tabular and graphical form.

47. Ellis, A. J., 1966, Partial molal volumes of alkali

chlorides in aqueous solutions to 200°C: Chem. Soc. 

(London) Jour., v. 1966A, p. 1579 - 1584.

Experimental study on the partial molal volume and 

density of NaCl and KCl solutions from 0.1 to 1.0 molal

29
at 20 atm between 0° and 200°C. Partial mplal volume 

and density data vere calculated from a mercury 

displacement technique. Experimental data are given 

graphically, in tables* and as empirical equations.

48. Ellis, A. J., 1967, Partial molal volumes of MgCl2 ,

CaCl 2 , SrCl 2 , and BaCl 2 in aqueous solutions to 200°C: 

Chem. Soc. (London) Jour., v. 1967A, p. 660-664.

Experimental and calculated study on the density and 

partial molal volume of CaCl2 solutions from 0.1 to 1.0 

molal at 20 atm and from 25° to 200°C. Data were 

derived from a mercury displacement technique. 

Experimental data are presented in tables, on graphs, 

and as empirical equations.

49. Ellis, A. J., 1968a, Partial molal volumes in high

temperature water. Part III. Halide and oxyanion 

salts: Chem. Soc. (London) Jour., v. 1968A, p. 1138 - 

1143.

Experimental study on the density of K 2 S0 4 (0.05 to 0.5 

molal) and Na 2 S04 solutions (0.05 to 1.0 molal) at a 

pressure of 20 atm and from 25° to 200°C. Limiting 

partial molar volumes of the dissolved salts and of the 

alkali and alkaline earth cations and of the sulfate ion 

were obtained by assuming a value for the chloride ion. 

Density data were derived from a mercury displacement 

technique. Experimental data are given in tables, 

graphically, and as empirical equations.

50. Ellis, A. J. and HcFadden, I. M., 1968b, The partial

molal volume of hydrochloric acid in high-temperature 

water: Chem. Communications., v. 287, p. 516 - 517.

Experimental study on the partial molal volume of HC1 

from 0.2 to 2.0 molal at 20 atm and at 25° to 200°C. 

Limiting partial molar volumes of the dissolved acid and 

of the hydrated protron were calculated from these 

results and those of previous studies. Volume data were 

derived by mercury displacement from a 25°C reference 

cell. The experimental data are presented in tabular 

and graphical form.

51. Ener, C. and Taskoprulu, N. S., 1954, Measurements of

the velocity of ultrasound in sea water (Black Sea and

30
Sea of Marmara): Istanbul Dniv. Fac. Sci. Rev., Ser. 

C. t v. 19, p. 105 - 1-9.

Experimental study on the compressibility of sea salt 

solutions at ambient pressure and 20°C. Compressibility 

data were obtained from measurements of the velocity of 

sound. Experimental data are given in tables, on 

graphs, and as empirical eguations.

52. Epifanova, S. S., Kaprina, Yu. D., Kaptsova, T. M.,

Korcheoskaya, K. M., Krasilnikova, 6. G., Likhacheva, 0. 

A., Hakarov, A. V., Makareva, T. S., Maksimova, M. P., 

and Fokeev, V. M., 1973, [Viscosity of salt solutions 

simulating natural solutions]: Izv. Vysch. Ocheb. 

Zaved. Geol. Razved., v. 16, p. 154 - 156. In Russian.

The densities of concentrated solutions of Nad, KC1, 

and Na 2 S04 were measured at various temperatures. 

(Original unavailable. Data taken from Chem. Abs., 

79:108303w, 1973.)

53. Ezrokhi, L. L., 1967a, [Viscosity of solutions of

calcium chloride]: Leningrad Vsesoiuznyi 

Nauchno-Issledovatel'skii Inst. Galurgii, Trudy, v. 52, 

p. 3-9. In Russian.

Experimental study of the viscosity and density of CaCl 2 

solutions, 10 to 40 wt percent at ambient pressure and 

25°, 40°, and 60°C. Densities were obtained from 

pycnometry. Experimental data are given in a table.

54. Ezrokhi, L. L., 1967b, [Density of complex solutions

containing calcium chloride]: Leningrad Vsesoiuznyi 

Nauchno-Issledovatel'skii Inst. Galurgii, Trudy, v. 52, 

p. 10-19. In Russian.

Empirical study giving coefficients in an expression for 

the density of solutions in the system CaCl2 - NaCl - 

Na 2 S04 - KC1 - K2 SO* - MgCl 2 - MgS0 4 at ambient pressure 

between 0° and 100°C. Constants are given in tabular 

form. Examples for the application are also given.

55. Fabuss, B. H., Korosi, Alexander, and Hug, Shamsul,

1966, Densities of binary and ternary aqueous solutions 

of NaCl, Na2 S04 , and MgS04 , of sea water and sea water 

concentrates: Jour. Chem. Eng. Data, v. 11, p. 324 - 

331.

31
Experimental and calculated study on the density of NaCl 

(0.02 to 2.5 molal) and Na 2 S0 4 (0.01 to 0.15 molal) 

solutions at ambient pressure in the temperature range 

25° to 175°C. Experimental density data were derived 

from pycnometry and dilatometry. Experimental data are 

given in tables, on graphs, and as empirical equations.

56. Fabuss, B. M., and Korosi, Alexander, 1967,

Thermodynamic properties of sea water and its 

concentrates: Desalination, v. 2, p. 271 - 278.

Calculated study on the density of NaCl, Na 2 S0 4 , and KC1 

solutions at ambient pressure and in the temperature 

range 25° to 175°C. Densities were obtained from 

pycnometry. Calculated data for sea water are presented 

as graphs and as empirical equations.

57. Fabuss, B. H., and Korosi, Alexander, 1968, Properties

of sea water and solutions containing sodium chloride, 

potassium chloride, sodium sulfate, and magnesium 

sulfate: O.S. Off. Saline Water, Res. Develop. 

Progress Kept. No. 38U, 133p.

A collection of tables giving the smoothed densities, 

vapor pressure, boiling point elevations, and other 

quantities at ambient pressure from 20° to 150°C and 

from 60° to 300°F for the following solutions from 0 

molal up to the concentrations indicated: NaCl to 3.5 

molal, KC1 to 3.5 molal, Na 2 S04 to 1.2 molal, KaCl-KCl 

to 3.5 total molality, NaCl-Na 2 S0 4 to 3.4 total 

molality, and sea water to 13 wt percent solids. The 

tables are based on published, experimental research by 

the authors. Values are given in tables and on graphs. 

The empirical functions and their coefficients, which 

were used to generate the tables and graphs, are given.

58. Fajans, Kasimir and Johnson, Oliver, 1942, Apparent

volumes of individual ions in aqueous solutions: Am. 

Chem. Soc. Jour., v. 64, p. 668 - 678.

Theoretical study on the apparent volume of NaCl and KC1 

from infinite dilution up at ambient pressure and at 25° 

to 55°C. Apparent volumes of common ions are given at 

15° to 20°, at 25°, and at 35°C. The apparent volume 

was used to calculate the volume of ions. Smoothed data 

are given in tables and graphically.

32
59. Falkenhagen, H., and Bachem, Ch., 1935, [On the

compressibility of strong electrolytes]: Zeit. 

Elektrochem., v. 41, p. 570 - 575. In German.

Experimental study on the apparent molal compressibility 

of NaCl and Ma 2 C0 3 solutions at ambient pressure and 

25°C. Data were derived from the optical measurement of 

the wavelength of high frequency sound in solutions 

using a stroboscope and progressive waves. The 

dependence of the apparent molal compressibility with 

the sguare root of concentration is given in a table.

60. Fortier, Jean-Iuc, Philip, P. R. and Desnoyers, J. E.,

1974, Thermodynamic properties of alkali halides. III. 

Volumes and heat capacities of transfer from H 2 0 to D 2 0 

at 25°C: Jour. Sol. Chem., v. 3, p. 523 - 538.

Experimental study on the density of NaCl, NaF, and KF 

solutions from 0.07 to 0.82 molal at ambient pressure 

and 25°C. Density data were derived from a vibrating 

densimeter. Experimental data are presented in tables 

and on graphs.

61. Franks, F. and Smith, H. T., 1967, Apparent molal

volumes and expansibilities of electrolytes in dilute 

aqueous solutions: Faraday Soc. Trans., v. 63, p. 2586 

- 2598.

Experimental study on the apparent molal volume of 0.002 

to 1.0 molal solutions of NaCl and KC1 at ambient 

pressure and at 5° and 25°C. Volume data were derived 

from magnetic float measurements. Limiting apparent 

molal volume data are 14.15 and 16.65 cm 3 /mole for NaCl 

and 24.65 and 26.90 cm 3 /mole at 5° and 25°, 

respectively. Experimental data are given in tables, on 

graphs, and as empirical equations.

62. Freyer, E. B., 1931, Sonic studies of the physical

properties cf liquids. II. The velocity of sound in 

solutions of certain alkali halides and their 

compressibilities: Am. Chem. Soc. Jour., v. 53, p. 

1313 - 1320.

Experimental compressibilities of NaCl and KC1 from 1 to 

24 wt per cent at ambient pressure from 15° to 55°C. 

Compressibilities were derived from measurements of the 

velocity of sound. Data are presented as smoothed

33
tables, graphs, and in empirical equations.

63. Galinker, I. S., Rodnyansky, I. H., Korobkov, V. I.,

and Lekakh, N. B., 1964, [Difference in the 

thermodynamic properties of water and electrolyte 

solutions depending on the temperature]: Ukrainf skyi 

Fizichnyi Zhur., v. 9, p. 401 - 405. In Russian.

Experimental study on the compressibility and 

expansivity of KCl (1 to 3 n), K 2C0 3 (1 to 6 n) and 

CaCl 2 (1 to 6 n) at ambient pressure and 25° and 230°C 

(n is the number of gram equivalents per 1000 g of H 2 0). 

Experimental data are given in a table.

64. Garrett, A. B., and Woodruff, S. A., 1951, A study of

several physical properties of electrolytes over the 

temperature range of 25°C to -73<>C: Jour. Phys. 

Colloid Chem., v. 55, p. 477 - 490.

Experimental densities, viscosities, and specific 

conductivities for HC1 (23.3, 21.8, and 27.6 wt percent) 

and H 2 S0 4 (36 wt percent) at ambient pressure between 

25° and -73°C. Densities were measured by pycnometry. 

Experimental data are given graphically. The listing of 

the experimental data is deposited in the Microfilm 

Library, Ohio State University, Columbus, Ohio.

65. Gastaldo, Charles, 1962, Determination of coefficients

for thermodynamic equations for determining the 

properties of sea water, particularly vapor pressure: 

Univ. California (Los Angeles), Dept. Eng., Rept. 

61-80, 149 p.

Empirical fitting of equations to experimental data for 

sea water concentrates given by Hara, Nakamura, and 

Higashi (1932) between 0 and 28 wt percent solids from 

0° to 175°C at ambient pressure. Smoothed data for 

densities and partial molal volumes of H 2 0 for the sea 

water concentrates are given in tables and on graphs. 

The constants for the empirical equations are given in a 

table.

66. Geffcken, W., 1931, [On the apparent molal volumes of

dissolved electrolytes]: Zeit. Phys. Chem., v. A 155, 

p. 1 - 28, In German.

34
Theoretical discussion where the validity of Masson's 

Rule is tested using published data for the alkali 

halides at ambient pressure and at the concentration and 

temperature ranges indicated: KF, 1.79 to 10.7 molar, 

25°c KC1, 0.16 to 4.1 molar, 0° to 100°C NaCl, 0.25 to 

5.3 molar, 25° to 45°C and HCl, 0.58 to 10.7 molar, 

25°C. Densities and apparent molal volumes are given in 

tables and on graphs.

67. Geffcken, W., 1933a, [The apparent molal volume of

dissolved electrolytes II. The pressure coefficient of 

apparent molal volumes]: Zeit. phys. Chem., v. A 167, 

p. 240 - 244. In German.

. A theoretical discussion of the pressure coefficient of 

the apparent molal volumes. Constants for KC1, NaCl, 

and CaCl 2 at 25°C and ambient pressure are given in the 

text. They are derived from published data.

68. Geffcken, W., Beckmann, Ch., and Kruis, A., 1933b,

[Molar refraction in dilute solutions. I. A 

differential method for precision measurement of the 

density]: Zeit. Phys. Chem., v. B20, p. 398 - 419. In 

German.

Theoretical study of the apparent molal volumes of NaCl 

and Na 2 C0 3 at 25°C and ambient pressure. Apparent molal 

volume data are given in a table, on graphs, and by an 

empirical equation.

69. Geffcken, W., and Price, D., 1934, [Dependence of the

apparent molal volume and apparent molal refraction in 

dilute solutions on concentration]: Zeit. phys. Chem., 

v. B 26, p. 81 - 99. In German.

Densities and apparent molal volumes of KCl (0 to 0.8 

normal), Na 2 S04 (0 to 1.8 normal), and Na 2C0 3 (0 to 2.6 

normal) solutions at ambient pressure and 25°C. Data 

were derived from pycnometry. Results are given in 

tables and on graphs.

70. Gibson, R. E., 1927, The system sodium sulfate-water.

I. The densities and specific volumes of agueous 

solutions of sodium sulfate between 25 and 40° and the 

fictive volumes of sodium sulfate in solution. Jour. 

Phys. Chem., v. 31, p. 496 - 510.

35
Experimental and calculated study on the specific volume 

and density of 0 to 28 wt percent Na 2 S0 4 solutions at 

ambient pressure and in the temperature range 25° to 

UO°C. Specific volume measurements were derived from 

dilatometry and densities from pycnometry. Experimental 

and smoothed data are given on tables, graphs, and by 

empirical equations.

71. Gibson, R. E., 1931, The fictive volumes of sodium

sulfate in aqueous solutions of sulfuric acid and of 

iodine in aqueous solutions of potassium iodide: Jour. 

Phys. Chem., v. 35, p. 690-699.

Experimental and calculated study on the partial molal 

and specific volumes of Na 2 S0 4 ranging in concentration 

from 0 to 30 wt percent in 5 and 10 wt percent H 2 S04 at 

ambient pressure and 25°C. Volume data were derived 

from pycnometry. Experimental data are presented in 

tables, on graphs, and as empirical equations.

72. Gibson, R. E., 193U, A note on the computation of the

partial volumes of the components of aqueous solutions: 

Jour. Phys. Chem., v. 38, p. 319 - 326.

Calculated study on the partial molal volumes of NaCl (0 

to 25 wt per cent), KC1 (0 to 0.29 g KCl per cm 3 of 

solution), and Na 2 S0 4 (0 to 28 wt per cent) solutions at 

ambient pressure and 25°C. Partial molal volumes were 

calculated from data taken from other sources. 

Calculated values are presented as smoothed tables, 

graphs, and as empirical equations.

73. Gibson, R. E., 1935, The influence of the concentration

and nature of the solute on the compressions of certain 

aqueous salts: Am. Chem. Soc. Jour., v. 57, p. 284 - 

293.

Experimental and calculated study on the compressibility 

of KCl (5.9 to 25.5 wt per cent) and Na 2 C0 3 (3.9 to 20.3 

wt per cent) solutions in the pressure range of 1 to 

1000 bars at 25°C. Compressibility data were derived 

from piezometer and pycnometer measurements. Data are 

presented as experimental and smoothed tables, graphs, 

and as empirical equations. Smoothed data for NaCl are 

also given.

36
71. Gibson, R. E., and Loeffler f 0. H., 1911, Pressure

volume relations in solutions. IV. The apparent volumes 

and thermal expansibilities of sodium chloride and 

sodium bromide in aqueous solutions between 25° and 

95°C: Am. Chem. Soc. Jour., v. 63, p. 113 - 119.

Experimental and calculated study on the apparent 

volumes of NaCl solutions from 5 to 25 wt percent at 

pressures from 1 to 1000 bars between 25° and 95°C. 

Apparent racial volume data were derived from 

dilatooetry. Experimental and smoothed data are 

presented in tables, on graphs, and as empirical 

equations.

75. Ginzburg, D. H., Pikulina, N. S. , and Litvin, V. P.,

1961a, [Density of potassium carbonate solutions]: Zh. 

Prikl. Khim., v. 37, p. 2353 - 2357. In Russian. 

English translation in Russian Jour. Applied Chem., v. 

37, p. 2327 - 2330.

Experimental and calculated study on the density and 

vapor pressure of K 2 C0 3 solutions, 16 to 62 wt percent, 

at ambient pressure and from 25° to 130°C. Density data 

dere derived from pycnometry and vapor pressure data 

from the two-bulb method. Experimental data are 

presented in tables. Empirical equations are also 

given.

76. Ginzburg, D. H., Pikulina, N. S., and Litvin, V. P.,

1961b, [Density of sodium carbonate solutions]: Zh. 

Prikl. Khim., v. 37, p. 2719 - 2750. In Russian. 

English translation in Russian Jour. Applied Chem., v. 

37, p. 2710 - 2711.

Experimental and calculated study on the density of 16 

to 30 wt percent Na 2 C0 3 solutions at ambient pressure in 

the temperature range 35" to 110°C. Density data were 

derived from the two-bulb method. Experimental data are 

contained in tables and an empirical equation is given.

77. Ginzburg, D. M., 1965, [The density and vapor pressure

of sodium and potassium carbonate solutions]: Zh. 

Prikl. Khim., v. 38, p. 55 - 58. In Russian. English 

translation in Russian Jour. Applied Chem., v. 38, p. 

50 - 53.

Experimental and calculated study on the density of

37
mixed solutions of K 2 C0 3 (0.53 to 61.16 wt percent), 

Na 2 C0 3 (0.37 to 25,9 wt percent) and K 2 S0 4 (0.09 to 5.0 

wt percent) at ambient pressure from 20° to 120°C. 

Density data were derived from the two-bulb weighing 

method. Experimental and calculated data are contained 

on tables and graphs. An empirical equation is also 

given.

78. Glass, H. H., and Madgin, W. H., 1934, Viscosities of

aqueous solutions of electrolytes. Part I. Sodium 

sulfate solutions over the temperature range 25-40°: 

Chem. Soc. (London) Jour., v. 1934, p. 1124 - 1128.

An experimental study on the density of Na 2 S04 solutions 

from 0.0005 to 0.072 molar at ambient pressure and 25°C. 

Densities were measured by pycnometry. Experimental 

data are given in tables.

79. Gleukauf, E., 1965, Molar volumes of ions: Faraday 

Soc. Trans., v. 61, p. 914 - 921.

Theoretical discussion of the molal volumes of solvated 

ions and the structure of water at 25°C and ambient 

pressure. Internally consistent limiting partial molal 

volumes of ions are calculated from cited experimental 

studies. Results are given in tables and on graphs.

80. Gucker, F. T., 1933a, The compressibility of solutions.

I. The apparent molal compressibility of strong 

electrolytes: Am. Chem. Soc. Jour., v. 55, p. 2709 - 

2118.

A calculated study on the apparent molal compressibility 

of 0 to 8.0 molal solutions of KC1, NaCl, and CaCl2 at 

ambient pressure in the temperature range 0° to 80°C. 

Smoothed data are given in tables, on graphs, and as 

empirical equations.

81. Gucker, F. T., 1933b, The apparent molal heat capacity,

volume, and compressibility of electrolytes: Chem.

Rev., v. 13, p. 111 - 130.

Calculated study on the compressibility and apparent 

molal volume of HC1, KC1, NaCl, CaCl 2 , KOH, and SaOH 

solutions at ambient pressure and 25°C. Data are given 

as constants, as empirical equations, in tables, and on

38
graphs.

82. Gucker, F. T., 193<la, The apparent molal expansibility

of electrolytes and the coefficient of expansibility 

(thermal expansion) as a function of concentration: Am. 

Chem. Soc. Jour., v. 56, p. 1017 - 1021.

Calculated study on the apparent molal volume of KC1, 

NaCl, Na 2 S0 4 , and HC1 solutions at ambient pressure and 

in the temperature range 0° to 70°C. Smoothed data are 

given in tables, on graphs, and as empirical equations.

83. Gucker, F. T. Jr., 1934b, The calculated partial molal

solute quantities as functions of volume concentration, 

with special reference to the apparent molal volume: 

Jour. Phys. Chem., v. 38, p. 307 - 317,

Calculated study on the apparent molal volume of CaCl2

solutions at ambient pressure and 25°C. Data are

treated by means of graphs and empirical equations.

8U. Gucker, F. T. Jr., Chernik, C. L., and Roy-Chowdhury,

Phanibusan, 1966, A frequency-modulated ultrasonic 

interferometer: Adiabatic compressibility of aqueous 

solutions of NaCl and KC1 at 25°C: U. S. Natl. Acad. 

Sci. Proc., v. 55, p. 12 - 19.

Experimental study on the compressibility and density of 

NaCl (0.16 to a.5 molar) and KC1 (0.26 to 3.6 molar) 

solutions at ambient pressure and 25°C. Limiting 

partial molal volumes are obtained. Compressibility 

data were derived from measurements of the velocity of 

sound (equipment described) and density data from 

pycnometry. Experimental data are given in tabular and 

graphical form.

85. Haas, J. L. Jr., 1970, Equation for the density of

vapor-saturated NaCl - H 20 solutions from 75° to 325°C: 

Am. Jour. Sci., v. 269, p. U90 -U94.

Calculated study on the density of NaCl solutions from 0 

to 8.0 molal at ambient pressure from 75° to 325°C. 

Smoothed data are presented as tables, on a graph, and 

as an empirical equation.

39
86. Haas, J. L. Jr., 1971, The effect of salinity on the

maximum thermal gradient of a hydrothermal system at 

hydrostatic pressure: Econ. Geol., v. 66, p. 940 - 946.

An empirical expression for the density of Had 

solutions from 0 vt percent to saturation at ambient 

pressure between 75° and 325°C. Smoothed data are given 

in tables.

87. Halasey, Sr. M. Eva, 1941, Partial molal volumes of

potassium salts of the Hofmeister Series: Jour. Phys. 

Chem., v. 45, p. 1252 - 1263.

Experimental study on the partial molal volume and 

density of 0.005 to 0.5 molal KC1, NaCl, and K 2 SO« 

solutions at ambient pressure and in the temperature 

range 5° to 30°C. Partial molal volume data were 

derived from dilatometry. Experimental data are given 

in tables, on graphs, and as empirical equations.

88. Hara, Ryosaburo Nakamura, Kazumoto and Higashi,

Katsumi 1932, The specific gravity and the vapor 

pressure of concentrated sea water at 0° - 175°C: 

Tohoku Imperial Oniv. Tech. Rept., v. 10, p. 433 - 452.

Experimental study on the specific gravity and vapor 

pressure of normal sea water and its concentrates up to 

halite (NaCl solid) saturation at ambient pressure from 

0° to 175°C. Specific gravity was measured with a 

pycnometry at temperatures at and below 75°C and with a 

dilatometer above 75°C. Smoothed specific gravities are 

given on a table as a function of temperature and 

chloride concentration.

89. Helmy, A. K., Assaad, F. P., Naguib Hassan, H., and

Sadek, H., 1968, Apparent and partial molal volumes of 

Na-Kaolin and NaCl in kaolin suspensions: Jour. Phys. 

Chem., v. 71, p. 2358 - 2361.

Experimental study on the density of NaCl solutions from 

0.1 to 1.0 molal at ambient pressure and 30°C. 

Densities were derived from pycnometry. Experimental 

data are given in tables.

90. Hepburn, J. R. I., 1932, The vapor pressure of water

over aqueous solutions of chlorides of the alkaline

40
earth metals. III. Correlation with other physical 

properties of the solutions: Chem. Soc. (London), v. 

1932A, p. 575 - 582.

Calculated study attempting to correlate vapor pressure 

of CaCl2 solutions to the specific gravity of the same 

from 0.1 to 1 molar at ambient pressure from 0° to 25°C. 

Results are negative.

91. Hepler, L. G., Stokes. J. B., and Stokes, E. H., 1965,

Dilatometric measurements of apparent racial volumes of 

dilute aqueous electrolytes: Faraday Soc. Trans., v. 

61, p. 20 - 29.

Experimental study on the density and apparent molal 

volumes of 0.001573 to 0.02U45, 0.2735, and 0.8U51 molar 

NaOH solutions at ambient pressure and 25°C. Density 

data were derived from pycnometry and apparent molal 

volume data from dilatometry. Experimental data are 

given in tabular and graphical form.

92. Hurtado, G. G., Hateo, P. L., Serna, A., and

Vidal-Abarca, J. B., 1973, [Diffusion and viscosity in 

agueous media. Behavior of calcium(II) and cerium(III) 

ions and their complexes with EDTA and DCTA 

(1,2-diaminocyclohexanetetraacetic acid)]: An. Quim., 

v. 69, p. 295 - 303. In Spanish.

The densities of CaCl 2 solutions from 10° to 35<>C at 

ambient pressure were measured. (Original text 

unavailable. Data taken from Chem. Abs., 79:35259z, 

1973. )

93. Ikornikova, N. Yu., and Egorov, V. M., 1968,

[Experimental PTFC diagrams of aqueous solutions of 

lithium, sodium, potassium, and cesium chlorides]: in 

Lobachev, A. N., Editor, 1968, Gidrotermalni Sintez 

Krystallov: Moskow, Nauka Press. In Russian. English 

translation in Lobachev, A. N., editor, 1971, 

Hydrothermal synthesis of crystals: New York, 

Consultants Bureau, p. 3U - 51.

Experimental study of the specific volume of LiCl, NaCl, 

KC1, and CsCl solutions from 1.0 to 7.0 molal in the 

pressure range 200 to 2500 kgf/cm 2 from 150° to 700°C. 

The specific volumes were derived from recording the
pressure at temperature for various percentages of 

filling of the steel pressure vessel at 20°C. 

Experimental data are presented in tables, on graphs, 

and as empirical equations.

94. Ingham, J. W., 1928, The apparent hydration of ions.

Part I. The densities and viscosities of saturated 

solutions of sodium and potassium chlorides in 

hydrochloric acid: Am. Chem. Soc. Jour., v. 50, p. 

1917 - 1930.

Experimental and calculated study on the density of NaCl 

(0.017 to 5.43 molar) and KCl (0.20 to 4.17 molar) 

solutions in HC1 (13.41 to 0.46 molar) at ambient 

pressure and 25°C. Density measurements were derived 

from pycnometry. Experimental data are presented 

graphically and in tables. Empirical equations are also 

given.

95. Isdale, J. D. and Morris, R., 1972, Physical properties

of sea water solutions: Density: Desalination, v. 10, 

p. 329 - 339.

The density of "synthetic" sea waters of the following 

salinities 63.12, 92.66, 121.04, and 148.45 g/kg were 

measured at ambient pressure between 70° and 180°C using 

a glass dilatometer. Experimental and smoothed data are 

given in tables, on figures, and by an empirical 

equation.

96. Isono, T., and Tamamushi, R., 1967, Relation between

the viscosity B-coefficient and the molal volume of 

electrolytes in aqueous solutions: Electrochim. Acta, 

v. 12, p. 1479 - 1482.

Experimental study on the viscosity and density of HC1, 

NaCl, KCl, and CaCl 2 solutions at 5° and 25°C and 

ambient pressure. Densities were obtained from 

pycnometry. Limiting partial molal volumes for the 

unhydrated and hydrated solutes are given in a table.

97. Ivanova, F. I., 1972, [Regular variations in viscosity

as a result of mixing of ideal liquids]: Sb. 

Aspirantsk. Rabot, Kazansk. Univ. Estetsv Nauk Kazan., 

v. 1962, p. 3 - 12. In Russian.

42
The densities of aqueous solutions of NaCl - KC1 and 

NaCl - CaCl 2 were studied. [Original text unavailable 

to authors. Data taken from Chem. Abs. 60:13906e, 

1964. ]

98. Jain, D. V. S., and Lark, B. S., 1970, Apparent molal

volume and expansibility of electrolytes: Indian Jour. 

Chem., v. 8, p. 1133 - 1134.

Density of NaCl solutions at 0.002 to 0.2 molar at 

ambient pressure and 25°, 30°, and 40°C with an accuracy 

of 1 ppm. [Original text unavailable to authors. Data 

taken from Chem. Abs., 74:91851, 1971.]

99. Jones, Ginnell, and Talley, S. K., 1933a, The viscosity

of aqueous solutions as a function of the concentration: 

Am. Chem. Soc. Jour., v. 55, p. 624 - 642.

Experimental study on the density of 0.002 to 0.2 molar 

solutions of KC1 at ambient pressure and 25°C. Density 

data were derived from pycnometry. Experimental data 

are given in tables.

100. Jones, Grinnell, and Talley, S. K., 1933b, The

viscosity of aqueous solutions as a function of the 

concentration. II. Potassium brimide and potassium 

chloride: Amer. Chem. Soc. Jour., v. 55, p. 4124 - 

4125.

An experimental study of the density of KCl solutions 

from 0.5 to 3 normal at ambient pressure and 25°C. Data 

were derived from pycnometry. Experimental data are 

reported as specific gravities in tables.

101. Jones, Grinnell, and Christian, S. M., 1937a, The

viscosity of aqueous solutions of electrolytes as a 

function of concentration. V. Sodium chloride: Am. 

Chem. Soc. Jour., v. 59, p. 484 - 486.

Experimental study on the density and viscosity of 0.002 

to 0.2 normal solutions of NaCl at ambient pressure and 

0° and 25°C. Density data were derived from pycnometry. 

Experimental data are given in tables and as an 

empirical equation.

43
102. Jones, Grinnell, and Bay, W. A., 1937b, The surface

tension of solutions of electrolytes as a function of 

the concentration. I. A differential method for 

measuring relative surface tension: Amer. Chem. Soc. 

Jour., v. 59, p. 187 - 198.

An experimental study in which the density of KC1 

(0.0001 to 3 normal) and K 2 S04 (0.0002 to 1 normal) 

solutions were measured by pycnometry at 25°C and 

ambient pressure. Experimental data are listed in 

tables and are represented by empirical equations.

103. Jones, Grinnell, and Colvin, J. H., 1910, The viscosity

of solutions of electrolytes as a function of the 

concentration. VII. Silver nitrate, potassium sulfate, 

and potassium chromate: Am. Chem. Soc. Jour., v. 62, 

p. 338 - 340.

Experimental study on the density and viscosity of 

0.0005 to 0.5 molar solutions of K 2 S04 at ambient 

pressure and 25°C. Density data were derived from 

pycnometry. Experimental and smoothed data are given in 

tables and as an empirical equations.

104. Kaminsky, Manfred, 1957, [Experimental investigation of

the effect of concentration and temperature on the 

viscosity of strong electrolyte solutions. Part III. 

KC1, K 2 SO«, MgCl 2 , BeS04 , and MgS04 solutions]: Zeit. 

Phys. Chem., N.F., v. 12, p. 206 - 231. In German.

An experimental study on the density of KCl (0.001 to 

0.5 molar) and K 2 S04 (0.002 to 0.09 molar) solution at 

ambient pressure and at 12.5° and 42.5°C. Data were 

derived from pycnometry. Experimental data are given in 

tables.

105. Kaputstinskii, A. F., Stakhanova, M. S., and Vasilev,

V. A., 1960, [Density and heat capacity for mixed 

aqueous solutions of the chlorides of lithium and 

potassium at 25°C]: Izv. Akad. Nauk SSSR., Otd. Khim. 

Nauk, v. 1960, p. 2082 - 2089. In Russian.

Experimental study on the density and partial molal 

volume of solutions of 0.49 to 4.5 molal KCl, 0.50 to 

4.5 molal LiCl, and their 1:1 mixtures over a similar 

concentration range at ambient pressure and 25°C. 

Density data were derived from densimeter measurements.

44
Experimental data are given in tables, on graphs, and as 

empirical equations.

106. Kaulgud, M. V., 1965a, Velocity of sound in dilute

electrolyte solutions: Z. Phys. Chem., N.F., v. U7, p. 

2H - <M.

Experimental and calculated study on the compressibility 

of 0.0 to 0.0625 molar solutions of KC1, NaCl, and 

Na 2 S0 4 at ambient pressure and 25°C. Compressibility 

data were derived from velocity of sound measurements. 

Experimental data are given in tables, on graphs, and as 

empirical equations.

107. Kaulgud, M. V., 1965b, [The measurement with a

phase-comparison interferometer of very small changes of 

sound velocity in electrolyte solutions]: Acustica, v. 

15, p. 377 - 382. In German.

Experimental study of the velocity of sound in NaCl and 

KC1 solutions from 0 to 0.6 molar at ambient pressure 

and 25°C. The experimental method is described in 

detail. Velocities are given on a graph.

108. Kelley, H. R., Eorza, P. F., and Harringer, R. D.,

1965, Densities and viscosities of potassium hydroxide 

solutions at low temperatures: Jour. Chem. Eng. Data, 

v. 10, p. 233 - 23U.

Experimental study on the density of KOH solutions from 

1.99 to 17.11 molal at ambient pressure between -53.8° 

and 0°C. Density data were derived from pycnometry. 

Experimental data are given in tables.

109. Khaibullin, I. Kh., and Borisov, N. M., 1963,

[Investigation of the density of a liguid phase system 

by the gamma radiation transmission method]: 

Teploenergetika, v. 10, p. 78 - 82. In Russian.

Density of 0.2 wt percent NaCl solution at 150 to 240 

kg/cm* and 340° to 378°C, and of 6 wt percent NaCl 

solution at 1 to 400 kg/cm* and 101° to 437°C. Data are 

derived from gamma ray attenuation in the brine. 

Densities are given in tables and on figures.
110. Khaibullin, I. Kh., and Borisov, N. N., 1966,

[Experimental investigations of the thermal properties 

of aqueous and gaseous solutions of sodium and potassium 

chloride in the presence of a vapor phase]: Akad. Nauk 

SSSR, Teplofiz. Vysokikh Temperatur, v. U, p. 518 - 523. 

In Russian.

Experimental study on the density of 1 to 25 wt percent 

NaCl and of 1 to 20 vt percent KC1 solutions at ambient 

pressure (given) between 100° and 440°C. Data were 

obtained from gamma ray transmissivity. Densities for 

the vapor and the liguid are given in tables along with 

the ambient pressure and the salt content of the vapor.

111. Khaibullin, I. Kh., and Novikov, B. E., 1973,

[Thermodynamic study of aqueous and vapor solutions of 

sodium sulfate at high temperatures]: Akad. Nauk SSSR, 

Teplofiz. Vysokikh Temperatur, v. 11, p. 320 - 327. In 

Russian.

Experimental study on the density of Na 2 S04 solutions 

from 0.5 to 30 wt percent and of NaCl solutions from 1 

to 5 wt percent at ambient pressure (given) from 100° to 

417°C. Data were obtained from gamma ray 

transmissivity. Densities of the gas and liquid phases 

are given in tables along with the ambient pressures.

112. Khare, P. L., 1962, Compressibilities of mixtures of

electrolytes: Jour. Sci. Industr. Res. (New Delhi), v. 

21B, p. 61 - 64.

Experimental study on the compressibility of Na 2 so 4 in 1 

molar NaCl solution and of K 2 S04 in 0.5 molar Na 2 S04 

solution at ambient pressure and 30°C. Densities were 

measured with a pycnometer and compressibilities were 

calculated from the velocity of sound in the solutions. 

Compressibilities are given on graphs and as constants.

113. Khare, P. L., 1962, Compressibility of dilute solutions

of sulfuric acid: Faraday Soc. Trans., v. 58, p. 363 

- 367.

Experimental study on the compressibility and apparent 

molal volume of 0.3 to 28.3 wt percent H 2 S0 4 solutions 

at ambient pressure and 30°C. Compressibility data were 

derived from measurements of the velocity of sound and 

apparent molal volume data from pycnometry.
Experimental data are presented in tables, on graphs, 

and as an empirical equation.

Klarmann, Bodo, 1950, [Determination of the density of 

aqueous salt solutions]: Zeit. anal. Chem. , v. 130, 

p. 186 - 192. In German.

The apparent consistency of the ratio of the density of 

two salt solutions taken at constant pressure 

temperature, and wt percent solute is discussed. Data 

used are from other sources at ambient pressure between 

15° and 20QC.

115. Klevtsov, P. V., 1959, [Concerning the density of

solutions in the system H2 0-NaCl-KCl]: Zapiski 

Vsesoyuz. Mineral. Obshchestva, v. 88, p. 93 - 96. In 

Russian.

Calculated densities of NaCl-KCl solutions of varying 

ratios and total weight percentages at ambient pressure 

between 50° and 200°C. Results are derived from data 

for NaCl and KC1 at 80° and 150°C by using a described 

principle of additivity in the calculations of the 

specific volume of electrolyte solutions. Data are 

given in a table and on a figure.

116. Klochko, M. A., and Kurbanov, H. Sh., 1954, [Study of

aqueous solutions of hydrogen chloride and perchloric 

acid by methods of physicochemical analysis]: Akad. 

Nauk SSSR, Sektor Fiz.-Khim. Anal. Izv., v. 24, p. 237 

- 251. In Russian.

Densities of 5.9 to 44.9 wt percent (or 2.61 to 28.68 

mole percent) HC1 at ambient pressures between -30° and 

25°c. Densities were derived from pycnometry. 

Experimental results are given in tables and on graphs 

along with experimentally measured conductances and 

viscosities.

117. Klochko, N. A., Taukesheva, S. M., and Bezhaev, M. S. ,

1959, [An investigation of the calcium chloride - water 

system by physicochemical analysis]: Ochenya Zapiski 

Dagestansk Gosudarst -Univ., v. 5, p. 103 - 116. In 

Russian.

The density of CaCl2 solutions from 2 wt percent to

47
saturation was measured at ambient pressure from 25° to 

35OC. [Original text unavailable to authors. Data 

taken from Chem. Abs. 56:10990, 1962.]

118. Klotz, I. M., and Eckert, C. F., 1942, The apparent

molal volumes of aqueous solutions of sulfuric acid at 

25°C: Am. Chem. Soc. Jour., v. 64, p. 1878 - 1880.

Experimental study on the density and apparent molal 

volumes of H 2 S04 solutions from 0.014 to 3.2 molar at 

ambient pressure and 25°C. The densities were obtained 

from the weight of a sinker in the solution. Molal 

volumes of (H+ + HS0 4 -) and (2H+ * S04 2-) are derived 

from these data. Experimental data are presented in 

tabular form.

119. Kobus, G. I., 1955, [Electrical conductivity,

viscosity, and density of highly concentrated solutions 

of sodium hydroxide]: Tr. Odessk. Gidrometeorol Inst., 

v. 1955, p. 113 - 127. In Russian.

The density of aqueous NaOH solutions from 1.0 to 28.7 

normal were measured by pycnometry and dilatometry at 

ambient pressure from 25° to 80°C. [Original text 

unavailable to authors. Data taken from Chem. Abs. 

52:17908b, 1958.]

120. Kolosov, A. S., Novik, V. Ph., and Chuprakova, T. V.,

1971, [The system KC1 - FeCl2 - H 2 0 at 0°C]: Akad. 

Nauk SSSR, Sib. Otd., Ser. Khim. Nauk, Izv., v. 1971, p. 

24 - 28. In Russian.

Experimental study of saturated solutions in the ternary 

system KCl - FeCl 2 - H 2 0 at 0°C and ambient pressure. 

Specific gravity of saturated solutions taken at 0°C 

were measured at 25°C and are given in a table.

121. Kondrat'ev, V. P., and Androsov, V. I., 1973,

[Approximate equation of the temperature dependence of 

density of liquids]: Zhur. Fiz. Khim., v. 47, p. 2768 - 

2770. In Russian.

An equation for the temperature dependence of the 

density of aqueous solutions is derived. Calculated 

results agree with experimental data. [Original test 

unavailable to authors. Data taken from Chem. Abs.

48
80:52447x, 1973.]

122. Kononemko, A. F., and Sashevskaya, Z. G., 1974,

[Influence of temperature on density and viscosity of 

certain salt solutions]: Zhur. Prikl. Khim., v. 47, p. 

211 - 212. In Russian. English translation is given in 

Jour. Applied Chetn., v. 47, p. 208 - 209.

Experimental study of the density of a 28 wt percent 

CaCl2 solution and of a 20 wt percent NaCl plus 0.5 wt 

percent Na 2 C03 solution at ambient pressure between -20° 

and +20°C. Results were obtained from pycnometry. 

Experimental data are given in a table.

123. Korosi, Alexander, and Fabuss, B. M., 1968a,

Viscosities of binary aqueous solutions of NaCl, KC1, 

Na 2 S04 , and MgS04 at concentrations and temperatures of 

interest in desalination processes: Jour. Chem. Eng. 

Data, v. 13, p. 548 - 552.

Experimental and calculated study on the density of KC1 

(0.1 to 3.5 molal), NaCl (0.1 to 3.5 molal), Na 2 S04 

(0.033 to 1.2 molal), and MgS0 4 (0.025 to 0.9 molal) 

solutions at pressure ranges from 1 to 200 psig and in 

the temperature range from 25° to 150°C. Densities were 

derived from pycnometry. Experimental data are 

presented in tables. An empirical equation is given.

124. Korosi, Alexander, and Fabuss, B. M., 1968b,

Thermophysical properties of saline water: U.S. Off. 

Saline Hater, Res. Develop. Progress Rept. No. 363, 53 

PExperimental study on the density and viscosity of NaCl 

and KCl solutions between 0.1 and 3.5 molal, of Na 2 S04 

solutions between 0.03 and 1.2 molal, of NaCl-KCl 

solutions at ionic strengths between 0.7 and 3.6 molal, 

and of NaCl-Na 2 S0 4 solutions at ionic strengths between 

0.7 and 3.5 molal at ambient pressure from 25° to 

150°C. The study also includes synthetic sea water at 

ionic strengths between 0.7 and 2.1 molal. Densities 

were obtained from pycnometry. Experimental data are 

given on tables. Constants for empirical functions are 

given on graphs and tables.

125. Krey, J., 1972, [Vapor pressure and density of the

49
system H 2 0 - NaOH ]: Z. Phys. Chem. N.F., v. 81, p. 

252 - 273. In German.

Experimental study on the density of 0.1 to 1.0 molal 

solutions of NaOH at ambient pressure and in the 

temperature range 0° to 350°C. Densities were derived 

from pressure vessel-filling measurements. Data are 

given in smoothed tables, graphically, as constants, and 

as empirical equations.

126. Kruis, A., 1936, [The depencence on concentration of

the apparent molal volumes of a strong electrolyte]: 

Zeit. phys. Chem., v. B 34, p. 1 - 12. In German

Experimental determination of the density of NaCl 

(0.0026 to 0.74 molar) and KCl (0.040 to 3.72 molar) 

solutions at ambient pressure and 25°C. Data for NaCl 

were calculated from the weight of a sinker for KCl 

from dilatometry. Densities are given in tables. 

Apparent molal volumes are given in tables, on graphs, 

and as a function of the square root of molarity.

127. Krumgal'z, B. S. and Mashovets, V. P., 1964, [Density

of concentrated solutions above 45 percent of NaOH and 

temperatures up to 400°C]: Zh. Prikl. Khim., v. 37, p. 

2596 - 2600. In Russian. English translation in 

Russian Jour. Applied Chem., v. 37, p. 2563 - 2566.

Experimental study on the density of 46.16 to 90.73 wt 

percent solutions of NaOH at ambient pressure and from 

150° to 400°C. Densities were derived from dilatometry. 

Experimental and smoothed data are given in tables, on 

graphs, and as empirical equations.

128. Kulkarni, A. G., 1969, Compressibility studies in mixed

aqueous electrolytes: Indian Jour. Chem., v. 7, p. 

333 - 335.

Among other binary systems, the compressibility of 

NaCl-KCl mixtures at total molarity of 1 and 3.5 were 

measured at ambient pressure and 25°C. Data are 

calculated from the measurement of the velocity of 

sound. Breaks in the slope of compressibility versus 

composition are absent at 1 molar but five are found at 

3.5 molar. These are interpreted as changes in 

hydration. Only the ratios of KCl:NaCl for the breaks 

are given.

50
129. Kuppers, J. R. , 1974, Partial racial expansibilities

from the temperature of maximum density of aqueous 

solutions: Jour. Phys. Chem., v. 78, p. 1041 - 1042.

Calculated study on the expansivity of NaCl and KC1 

solutions at ambient pressure and 3.98°C. Tables of 

thermal coefficients are given and an empirical equation 

is used.

130. Lamb, A. B., and Lee, R. E., 1913, The density of

certain dilute aqueous solutions by a new and precise 

method: Am. Chem. Soc. Jour., v. 35, p. 1666 - 1693.

Experimental study on the density of Na 2 C0 3 , NaCl, and 

KC1 solutions at ambient pressure and 20°C. Density 

data were derived from magnetic float measurements. 

Experimental and smoothed data are presented on tables.

131. LaMer, V. K., and Cornwall, T. H., 1927, The partial

racial volumes of water and salt in solutions of alkali

halides: Jour. Phys. Chem., v. 31, p. 393 - 406.

Calculated study on the partial molal volume of NaCl and 

KC1 solutions at ambient pressure from 0° to 50°C. Data 

are given in tables of constants and graphically. An 

empirical equation is also used.

132. Lanman, E. H., and Hair, B. J., 1934, The

compressibility of aqueous solutions: Am. Chem. Soc. 

Jour., v. 56, p. 390 - 393.

Experimental study on the compressibility of NaCl, KC1, 

HC1, KOH, and NaOH solutions from 0.55 to 2.21 molal at 

pressures between 100 and 300 Mbars at 25°C. 

Compressibilities were derived from piezometry. 

Experimental data are given graphically and in tables.

133. Lee, Shiu, 1966, The apparent and partial molal volumes

of electrolytes in water and in aqueous sodium chloride 

solutions: Ph. D. Thesis, Yale Univ., 141 p Oniv. 

Microfilms, Ord. No. 66-4906 Abs. in Dissertation 

Abs., v. B27, p. 131.

Experimental and theoretical study of the density of 

solutions in binary, ternary, and higher order systems. 

The study includes experimental data at ambient pressure

51
and 25°C for solutions of NaCl (0.15 to 3.4 molal), and 

of CaCl2 (0.04 to 1.2 molal) and Na 2 S0 4 (0.016 to 1.3 

molal) in 0, 0.16, and 0.725 molal NaCl solutions. Data 

were obtained from pycnometry. Densities, apparent 

molal volumes and partial molal volumes are given in 

tables, on graphs, and as empirical equations.

134. Legrand, Michel, and Paris, R. A., 1966, [The systems:

water, ferrous sulfate, potassium sulfate water, 

ferrous chloride, ferrous sulfate water, ferrous 

chloride, potassium chloride water, potassium chloride, 

potassium sulfate at 20°]: Soc. Chim. France Bull., v. 

8, p. 2699 - 2701. In French.

Experimental study on the density of mixed solutions of 

FeS0 4 -K2 S0 4 , FeS04 -FeCl2 , FeCl 2 -KCl, and KC1-K 2 S0 4 near 

saturation at ambient pressure and 20°C. Density data 

were derived from pycnometry. Experimental data are 

given in tables.

135. Lemmlein, G. 6., and Klevstov, P. V., 1961, Relations

among the principal thermodynamic parameters in a part 

of the system H 2 0-NaCl: Geochemistry, v. 1961, p. 148 

- 158.

Experimental study on the volume of NaCl-H 2 0 solutions 

at 5, 10, 20, and 30 wt percent NaCl from 250 to 1750 

atm and from 150° to 500°C. Volume data are derived 

from pressure-temperature measurements for a given 

percent of fill of the pressure vessel at 20°C. 

Experimental data are given in tabular and graphical 

form.

136. Lengyel, Sandor, 1963a, [Studies on the sturcture of

aqueous ionic solutions by analysis of the density 

against molality curves]: Magyar Kern. Foly., v. 69, p. 

4 - 17. In Hungarian.

Theoretical study of the density of NaCl, KC1, HC1, 

NaOH, and KOH solutions from 2 to about 5 molar at 

ambient pressure and 0°, 25°, and 50°C. Constants for 

an empirical equation are given in tables.

137. Lengyel, Sandor, and Fezler, Gyula, 1963b, [Studies on

the structure of aqueous solutions containing two 

electrolytes by density determinations]: Magyar Kern.

52
Foly., v. 69, p. 128 - 131. In Hungarian. English 

translation in Acad. Sci. Hungary, Acta Chim., v. 37, p. 

319 - 327.

Experimental study on the density of NaCl solutions from 

0.8 to 2.5 mclar in 2.0 molar KC1 solutions at ambient 

pressure and 25°C. Densities were obtained from 

pycnometry. Relative densities are given in a table.

138. Likhoded, A. D., Zapol'skii, A. K., and Sazhin, V. S.,

1973, [Investigation of the density and viscosity of 

aluminum and potassium sulfate solutions]: 

Khimicheskaya Tekhnologiya (Kharkov), v. 1973, p. 55 - 

57. In Russian.

Experimental study of the density of K 2 S04 solutions 

from 33.9 to 67.8 g/liter at ambient pressure from 85° 

to 95°C. Density was measured with a hydrometer. 

Experimental data are given in a table.

139. Lindstrom, R. £., and Hirth, H. E., 1969, Extimation of

the bisulfate ion dissociation in solutions of sulfuric 

acid and sodium bisulfate: Jour. Phys. Chem., v. 73, 

p. 218 - 223.

Experimental study on the density of NaHS04 (0.001 to 

4.0 molal) and H 2 S04 (0.0012 to 2.33 molal) solutions at 

ambient pressure and 25°C. Experimental density 

measurements were derived from the weight of a sinker in 

solution. Experimental data are given in tabular form.

140. Longsworth, L. G., 1935, Transference numbers of

aqueous solutions of some electrolytes at 25° by the 

moving boundary method: Am. Chem. Soc. Jour., v. 57, p. 

1185 - 1191.

Smoothed partial molal volumes of CaCl 2 , KC1, and Na 2 SO« 

at ambient pressure and 25°C. Data for CaCl2 are taken 

from the author's unpublished research (method is not 

stated) data for KC1 and Na 2 S04 are derived from the 

tabulations in volume 3 of the International Critical 

Tables, 1928. Partial molal volumes are given by 

equation only.

141. Lunden, Bertil, 1941, [The compressibility of

mono-monovalent electrolyte solutions]: Svensk Kemisk

53
Tidshrift, v. 53, p. 86 - 96. In German.

Experimental study on the compressibility of NaCl and 

KC1 solutions from 0.02 to 1 molar at ambient pressure 

and 20°C. Data are derived from the velocity of sound 

using densities taken from the literature. Experimental 

compressibilities and the limiting apparent molal 

compressibility are given in tables.

112. Lunden, Bertil, 1943, [The compressibility of

electrolyte solutions]: Zeit. phys. Chem., v. 192, p. 

345 - 378. In German.

Experimental compressibilities of 0.07 to 0.6 molar HCl 

at ambient pressure and 20°C. Compressibilities were 

calculated from the velocity of sound in the solutions. 

Results are given in tables and on graphs.

143. Lyons, P. A., and Riley, J. F., 1954, Diffusion

coefficients for aqueous solutions of calcium chloride 

and cesium chloride at 25°: Amer. Chem. Soc. Jour., V. 

76, p. 5126 - 5220.

An experimental study in which the density of CaCl 2 

solutions from 0.095 to 2.0 molar were measured with a 

pycnometer at 25°C and ambient pressure. Experimental 

data are reported in a table.

144. Maclnnes, D. A., Dayhoff, M. 0., and Ray, B. R., 1951,

A magnetic float method for determining the densities of 

solutions: Rev. Sci. Instruments, v. 22, p. 642 * 646.

Experimental study on the density of 0.2 to 4.5 wt 

percent KC1 solutions at ambient pressure and 25°C. 

Densities were calculated from magnetic float 

measurements described in text. Experimental data are 

given graphically.

145. Maclnnes, D. A., and Dayhoff, M. 0., 1952, The partial

molal volumes of potassium chloride, potassium and 

sodium iodides and of iodine in aqueous solutions at 

25°: Am. Chem. Soc. Jour., v. 74, p. 1017 - 1020.

Experimental study on the partial molal volume of KC1 

(0.0086 to 0.60 molal) at ambient pressure and 25°C. 

Densities were derived from the measurements using the

54
magnetic float technique. Experimental data are given 

in tables and as empirical equations.

116. Nahapatra, P. K., and Ray, B. C., 1958, On the

variation of compressibility of water and electrolytic 

solutions with temperature: Indian Jour. Phys., v. 32, 

p. 439 - 442.

Experimental study on the compressibility of NaCl 

solutions (0.85, 1.7, and 3.4 normal) at ambient 

pressure and from 0° to 90°C. Compressibilities were 

calculated from velocity of sound measurements. 

Experimental data are given on graphs.

147. Maksimova, I. N., and Yushkevich, V. F., 1963,

[Electrical conductivity of solutions of NaOH at 

elevated temperatures]: Zhur. Fiz. Khim., v. 37, p. 

903 - 907. In Russian.

Calculated densities of NaOH solutions, 0.05 to 49 wt 

percent at ambient pressure from 20° to 300°C. 

Densities are given in a table and as an empirical 

expression.

148. Maksimova, I. N., 1965, [Density determinations of

solutions]: Zh. Fiz. Khim., v. 39, p. 551 - 554. In 

Russian.

Calculated study to derive a generalized equation for 

the density of common inorganic compounds from 1 wt 

percent solute to near saturation at ambient pressure 

and between 20° and 300°C. The derived equation has 

been applied to binary solutions containing NaCl, KC1, 

HC1, CaCl2 , FeCl2 , K2 SO*, Na 2 S04 , and K 2 C03 . Errors in 

calculation using given solute-dependent constants are 

about 0.1 to 0.3 percent between 20° and 140°C and about 

1 to 6 percent at 200° to 300°C.

149. Maksimova, I. N., and Foterov, N. V., 1973, [Density of

aqueous electrolyte solutions]: Okr. Khim. Zhur., v. 

39, p. 234 - 237. In Russian.

A theoretical study for calculating the volume of NaCl 

solutions based on the molecular volume of water and the 

molecular volume of the salt as calculated from the 

crystal radii. An empirical equation and tables of

55
smoothed numbers are given.

150. Manucharov, Tu. S., Mikhailov, I. 6., and Shutilov, V.

A., 1964, [The dependence of sound velocity and 

compressibility of electrolyte solutions on temperature 

and concentration at various hydrostatic pressures]: 

Leningrad Oniv. Vestnik, Ser. Fiz. Khim., v. 1964, no. 

3, p. 65 - 83. In Russian.

Experimental study of the compressibility and density 

between 20° and 80°C of the following solutions at the 

pressures indicated: CaCl 2 , 0.56 and 1.02 mol/kg at 0 

and 200 atm gauge Na 2 S04 , 0.07 to 0.71 mol/kg at 0 and 

250 atm gauge NaCl, 0.17 to 2.64 mol/kg at 0 and 250 

atm gauge and KCl, 0.13 to 2.36 mol/kg at 0, 200, and 

300 atm gauge. Data were derived from measurments of 

the velocity of sound in solution. Experimental 

densities and compressibilities are given in tables.

151. Mashovets, V. P., Dibrov, I. A., Krumgal'z, B. S., and

Matveeva, R. P., 1965, [Density of aqueous solutions of 

KOH at high temperatures in a wide range of 

concentrations]: Zh. Prikl. Khim., v. 38, p. 2344 - 

2317. In Russian. English translation in Russian Jour. 

Applied Chem., v. 38, p. 2297 - 2299.

Experimental study on the density of 4.5 to 92.4 wt 

percent KOH solutions at ambient pressure in the 

temperature range 0° to 4000C. Densities were obtained 

by electromagnetically weighing a float in an autoclave. 

Experimental data are given in graphical and tabular 

form.

152. Mashovets, V. P., Puchkov, L. V., Smaev, V. N.,

Federov, M. K., and Federov, N. V., 1973, [Density, 

viscosity and electrical conductivity of sea water at 

temperatures up to 300-350°C]: Zh. Prikl. Khim., v. 

46, p. 1865 - 1868. In Russian. English translation in 

Russian Jour. Applied Chem., v. 46, p. 1988 - 1990.

Experimental study on the density of 3.6 wt percent sea 

water solutions from ambient to 150 atm pressure in the 

temperature range 10° to 350°C. Densities were obtained 

from pycnometry up to 90°C and from pressure 

temperature - degree of filling measurements above 90°C. 

Experimental data are given in tables for temperatures 

up to 275°C and 150 atm, on graphs for temperatures up

56
to 350°C and as empirical equations.

153. Mathieson, J. G., and Conway, B. E., 1974, Partial

molal compressibilities of salts in aqueous solution and 

assignment of ionic contributions: Jour. Soln. Chem., 

v. 3, p. 455 - 477.

Experimental and calculated study on the compressibility 

of 0 to 1 molal solutions of NaCl, KCl, and HC1 at 

ambient pressure and 25°C. Compressibilities were 

derived from velocity of sound measurements. 

Experimental data are given in tables, on graphs, and as 

empirical equations.

154. Merkel, J. H. C., 1939, [The maximum density and

compressibility of salt solutions]: Rec. Trav. Chim., 

v. 58, p. 465 - 470. In German.

Theoretical discussion on the compressibility of NaCl 

and KCl solutions and the temperature of maximum 

density. Data are given in tables and equations for 1.5 

molal solutions.

155. Mikhailov, I. G., and Shutilov, V. A., 1956, [The

velocity of sound and the compressibility of aqeuous 

solutions of inorganic acids]: Leningrad Dniv. 

Vestnik, Ser. Fiz. Khim., v. 1956, no. 3, p. 16 - 28. 

In Russian.

Experimental study on the volumetric properties of H 2 S04 

(4.2 to 91.3 wt percent) and HCl (9.7 to 27 wt percent) 

at ambient pressure from 15° to 100°C. Data were 

derived from measurements of the velocity of sound in 

the solutions. Densities, coefficients of expansion and 

of compressibility are given in tables and on graphs.

156. Nikhailov, I. G., Savina, L. I., and Feofanov, G. N.,

1957, [The ultrasonic velocity and compressibility of 

strong electrolyte solutions]: Leningrad Univ. 

Vestkik, Ser. Fiz. Khim., v. 1957, no. 4, p. 25 - 42. 

In Russian.

Experimental study on the volumetric properties at 

ambient pressure between 0° and 90°C for the following 

solutions: KCl, 0.1 to 4 mol/kg NaCl, 0.1 to 6 mol/kg 

Na 2 C03 , 0.1 to 2 mol/kg and Na 2 S0 4 , 0.1 to 1.3 mol/kg.

57
Data were derived from measurements of the velocity of 

sound in the solutions. Experimental compressibilities 

and densities are given in tables.

157. Mikhailov, I. G., and Syrnikov, Yu. P., 1959,

[Temperature dependence of adiabatic compressibility of 

aqueous solutions of salts at low concentrations]: 

Stoenie i Fiz. Svoistva Veshchestva v Zhidkom 

Sostoyanii, Nin. Vysshego i Srednego Spets. Obrazov. 

Okr. SSR. Kievsk. Gos. Oniv., Materialy 4-go 

(Chetvertogo) Soveshch., Kiev, 1959 (publ. 1962), p. 74 

- 78. In Russian.

Experimental study of the adiabatic compressibility of 

0.5 to 3 wt percent NaCl, KC1, and CaCl2 solutions at 

ambient pressure between 58° and 74°C. Data were 

derived from the velocity of sound in solution. Results 

are given in the text and on graphs.

158. Mikhailov, I. G. f and Fenjou, 1960, [Sound velocity and

compressibility of aqueous solutions of LiOH, NaOH, and 

KOH]: Leningrad Univ. Vestnik, Ser. Fiz. Khim., v. 

1960, no. 3, p. 22 - 35. In Russian.

Experimental study on the volumetric properties of NaOH 

(0.24 to 24.4 mol/kg) and KOH (0.15 to 16.7 moI/kg ) at 

ambient pressure from 13° to 100°C. Data were obtained 

from measurments of the velocity of sound in solutions. 

Experimental compressibilities and densities are given 

in tables.

159. Mikhailov, I. G., and Shutilov, V. A., 1964, [Nonlinear

accustical behavior of aqueous solutions of 

electrolytes]: Akust. Zhur. , v. 10, p. U50 - 455. In 

Russian.

Experimental study on aqueous solutions of KC1 (2.5 and 

5 wt percent), CaCl2 (4.1 and 11 wt percent), NaCl (1, 

4, 10, and 14 wt percent), and Na 2 SO« (1, 2, 6, and 10 

wt percent). KCl and CaCl 2 solutions were studied at 

ambient and 200 atm above ambient pressure and at 30° 

and 80°C. NaCl and Na 2 S0 4 solutions were studied at 

ambient pressure only at 20° and 80°C. Experimental 

velocities of sound and densities are given in a table 

and on graphs.

58
160. Millero, F. J. , 1967, High precision magnetic float

densimeter: Bev. Sci. Instruments, v. 38, p. 1441 - 

1444.

An experimental study on the density of NaCl solutions 

from 0.02 to 0.31 molal at ambient pressure and 25°C. 

The densities were measured with a magnetic float 

densimeter which is described in detail. Partial molal 

volumes and the densities from which they were 

calculated are presented in tables.

161. Millero, F. J., and Drost-Hansen, W., 1968, Apparent

molal volumes of aqueous monavalent salt solutions at 

various temperatures: Jour. Chem. Eng. Data, v. 13, p. 

330 - 333.

An experimental study on the density and apparent molal 

volumes of NaCl (0.114 molal) and KC1 (0.115 molal) 

solutions at ambient pressure between 20° and 40°C. The 

densities were measured with a magnetic float 

densimeter. Partial molal volumes were calculated from 

the densities and are presented in tables. Included 

also are empirical equations.

162. Millero, F. J., 1970, The apparent and partial molal

volume of aqueous soldium chloride solutions at various 

temperatures: Jour. Phys. Chem., v. 74, p. 356 - 362.

Experimental study on the density of NaCl solutions from 

0.010 to 0.964 molal at ambient pressure between 0° and 

55°C. Density data were derived from a magnetic float 

densimeter. Experimental data are given in tables and 

on graphs.

163. Millero, F. J. , Knox, J. H., and Emmet, B. I., 1972a, A

high-precision, variable-pressure magnetic float

densimeter: Jour. Soln. Chem., v. 1, p. 173 - 186.

Experimental study on the density and partial molal 

volume of NaCl solutions at 0.75 and 1.0 molal from 0 to 

1.2 kb applied pressure and 25°C. Density data were 

derived from magnetic float densimeter measurements. 

Experimental and smoothed data are presented in tables.

164. Millero, F. J., Hoff, E. V., and Kahn, Larry, 1972b,

The effect of pressure on the ionization of water at

59
various temperatures from molal volume data: Jour. 

Soln. Chem., v. 1, p. 309 - 327.

Experimental and calculated study on the apparent molal 

volume and density of HCl (0.002 to 1.0 molal) and NaOH 

(0.001 to 1 molal) solutions at 0°, 25°, and 50°C and, 

0.005 to 1 molal NaCl solutions at 50°C and ambient 

pressure. Density data were derived from the use of a 

magnetic float densimeter. Experimental data are 

presented in tables, on graphs, and as experimental 

equations.

165. Millero, F. J., 1972c, The partial molal volumes of

electrolytes in aqueous solutions: in Home, R. A., 

WATER AND AQUEOUS SOLUTIONS: New York, 

Wiley-Interscience, p. 519 - 595.

A review of available partial molal volumes of 

electrolytes. Included is an addendum giving partial 

molal volumes at infinite dilution, V°, and the apparent 

molal volume concentration dependence constants, S and 

b at various temperatures between 0° and 200°C.

166. Millero, F. J., 1973a, Seawater - A test of

multicomponent electrolyte solution theories. I. 

Apparent equivalent volume, expansibility, and 

compressibility of artificial seawater: Jour. Soln. 

Chem., v. 2, p. 1 - 22.

Experimental and calculated study on the 

compressibility, apparent equivalent volume and density 

of the system KCl-NaCl-H 20 (0.1 to 0.8 molal) at ambient 

pressure and in the temperature range 0 to UO°C. 

Density data were derived from magnetic float densimeter 

measurements and compressibilities were derived from 

piezometry. Experimental data are given in tables, on 

graphs, and as empirical equations.

167. Millero, F. J. , and Knox, J. H., 1973b, Apparent molal

volumes of aqueous NaF, Na2 S04 , KC1, K 2 S0 4 , MgCl, and 

HgSO* solutions at 0° and 50°C: Jour. Chem. Ehg. Data, 

v. 18, p. U07 - 411.

Experimental study on the density and apparent molal 

volume of Na 2 S04 (0.002 to 1.0 molal), KCl (0.028 to 1.0 

molal), and K 2 S04 (0.002 to 0.7 molal) solutions at 

ambient pressure in the temperature range 0° to 50°C.

60
Data are derived from magnetic float densimeter 

measurements. Experimental data are given in tabular 

and graphical form.

168. Nickels, L. and Allmand, A. J., 1937, The electrical

conductivities and viscosities at 25°c of solutions of 

potassium, sodium, and lithium chlorides in water and in 

one-tenth molar hydrochloric acid: Jour. Phys. Chem., 

v. 41, p. 861 - 872.

An experimental study in which the densities of KC1 and 

NaCl solutions from 0.1 to 5.5 molar in 0.1 molar HC1 

were measured by pycnometry at 25°C and ambient 

pressure. Experimental data are reported in tables.

169. Nicolai, H. H., Ernst, W., and Wegkamp, H., 1951,

[Viscosity as an analytical method for electrolyte 

solutions]: Chem. Weekblad, v. 17, p. 88 - 90. In 

Dutch.

An experimental study of the density of NaOH solutions 

from 23 to 52 wt percent and of NaCl - KC1 - Na 2 S0 4 

solutions at 25°C and ambient pressure. Experimental 

and smoothed data are given in tables.

170. Onitiu, Lia, and Auslander, D., 1972, [Compressibility

of aqueous solutions of certain halides. I. Alkali 

metal chlorides]: Acta Chim. (Budapest), v. 75, p. 15 

- 51. In French.

An experimental study on the compressibility of NaCl (.2 

to 4 molal) and KC1 (0.2 to 3 molal) solutions from 15° 

to 50°C at ambient pressure. Compressibility data were 

derived from the measurements of the velocity of sound 

in the solutions. Experimental data are given 

graphically.

171. Owen, B. B., and Brinkley, S. R. Jr., 1941, Calculation

of the effects of pressure upon ionic equilibrium in 

pure water and in salt solutions: Chem. Rev., v. 29, p. 

461 - 474.

Calculated study on the partial molal volume and 

compressibility of HC1, KOH, NaOH, KC1, NaCl, NaHS04 , 

Na 2 S04 , and Na 2 C0 3 at infinite dilution and at 0.725 

molal NaCl matrix solution, at ambient pressure and

61
25°C. Smoothed data are presented on tables, on graphs, 

and as empirical equations.

172. Owen, B. B., 1944. Some aspects of pressure upon the

properties of liquids and solutions of electrolytes. 

Jour. Chem. Education, v. 21, p. 59 - 63.

Calculated study on the partial molal volume, 

compressibility, and density of KC1 and NaCl solutions 

in the temperature ranqe 0° to 85°C. Smoothed data are 

presented in tables, on graphs, and as empirical 

equations.

173. Owen, B. B., and Brinkley, S. R. Jr., 19U9,

Extrapolation of apparent molal properties of strong 

electrolytes: New York Acad. Sci. Annals, v. 51, p. 

753 - 76U.

Theoretical and calculated study on the apparent molal 

volume of HC1, NaCl, and KC1 solutions at ambient 

pressure and 25°C. Data are presented as constants in 

tables, as empirical equations, and on graphs.

17U. Owen, B. B., and Kronick, P. L., 1961, Standard partial

molal compressibilities by ultrasonics. II. Sodium and 

potassium chlorides and bromides from 0° to 30°C: Jour. 

Phys. Chem., v. 65, p. 84 - 87.

Experimental and calculated study on the compressibility 

of 0 to 0.07 normal solutions of NaCl and KCl at ambient 

pressure from 0° to 30°C. The compressibilities were 

derived from measurements of the velocity of sound. 

Experimental data are presented in tables, on graphs, 

and as empirical equations.

175. Passynski, A., 1935, [The velocity of ultrasound in

colloidal solutions]: Acta Physicochim O.R.S.S., v. 3, 

p. 779 - 782. In German.

Experimental study on the velocity of sound and density 

of NaCl solutions from 2.6 to 21.3 wt percent at ambient 

pressure and 20°C. Densities were measured with a 

pycnometer. Experimental data are given in a table.

176. Passynski, A., 1938, Compressibility and solvation of

62
solutions of electrolytes: Acta Physicochim. O.R.S.S., 

v. 8, p. 385 - 418.

Experimental and theoretical study of the 

compressibility of KC1 (0.13 to 2.7 normal) and NaCl 

(0.17 to 3.6 normal) solutions at 20°C and ambient 

pressure. Compressibilities were obtained from the 

measurements of the velocity of sound in the solutions. 

Densities were obtained from pycnometry. Experimental 

data are given in tables.

177. Pearce, J. N., and Eckstrom, H. C., 1937, Vapor

pressures and partial molal volumes of aqueous solutions 

of the alkali sulfates at 25°: Am. Chem. Soc. Jour., 

v. 59, p. 2689 - 2691.

Experimental study on the apparent and partial molal 

volume of 0 molal to saturated solutions of K 2 S04 and 

Na 2 S0 4 at 25°C and ambient pressure. Volume and density 

data were derived from pycnometry. Experimental data 

are presented in tables, on graphs, and as empirical 

equations.

178. Perman, E. P., and Orry, H. D., 1929, The

compressibility of aqueous solutions: Royal Soc.

(London) Proc., v. A126, p. 4U - 78.

Experimental study on the compressibility of KC1 (2.5 to 

22.1 wt percent) and CaCl2 (7 to 50 wt percent) 

solutions at pressures from 1 to 200 atm and 

temperatures from 30° to 80°C. Experimental 

compressibilities were derived from pie2ometry. Data 

are presented in tables, on graphs, and as empirical 

equations.

179. Perron, Gerald, Desnoyers, J. E., and Millero, F. J.,

1974, Apparent molal volumes and heat capacities of 

alkaline earth chlorides in water at 25°C: Canadian 

Jour. Chem., v. 52, p. 3738 - 3741.

Experimental densities and heat capacities of CaCl 2 

solutions from 0.0125 to 0.33 molal at 25°C and ambient 

pressure. Densities were measured using a flowing 

densimeter. Experimental densities and apparent molal 

volumes are given in a table and on a figure. Constants 

for the Redlich-Meyer equation are also given in a 

table.

63
180. Pesce, G., 1932* [On the concentration dependence of

equivalent refraction of strong electrolytes in 

solution]: Zeit. phys. Chem., v. A 160, p. 295 - 300. 

In German.

Experimental study on the molar refraction of CaCl 2 

(2.57 to 13.1 equivalents per kg H 2 0) and Na 2 C03 (0.95 

to 4.91 equivalents per kg H 2 0) solutions at ambient 

pressure and 25°C as a function of normality and 

density. Densities were derived from pycnometry. 

Results are given on a brief table only.

181. Picker, Patrick Tremblay, Edmund and Jolicoeur,

Carmel, 1971, A high-precision digital readout flow 

densimeter of liquids: Jour. Solution Chem., v. 3, p. 

377 - 381.

A precision densimeter for liquids, based on the 

oscillating-tube principle is described. On 5 to 7 cm3 

of solution, density measurements of ppm precision are 

carried out routinely.

182. Polyakov, E. A., 1965, [Electric resistivity and

density of aqueous salt solutions under high pressure 

and temperature]: Prikl. Geofizika, Vses. 

Nauchno-Issled. Inst. Geofiz. Metodov Bazvedki Sb. 

Stadei, No. 11, p. 163 - 180. In Russian.

Experimental study of density and electrical resistivity 

of solutions of NaCl at 1, 10, and 26 wt percent, of 

MgS04 , Na 2 SC4 , CaCl2 , and KCl at 10 wt percent, and of 

NaHC0 3 at 8 wt percent. Data were measured at 20°, 

100°, 2000, and 30QOC and 1, 100, 500, 1000, and 1500 

atm. Data were derived from piezometry and pycnometry. 

Densities are given in tables and on figures. 

Coefficients of expansion and compressibility are 

derived and given in tables.

183. Postnikov, V. A., 1970, [Density and viscosity of

saturated aqueous solution of certain substances]: Zh. 

Prikl. Khim., v. 11, p. 236 - 238. In Russian.

Review of densities and viscosities at ambient pressure 

from 10° to 80°C for solutions saturated in inorganic 

salts. Data for KCl, Nad, NaOH, NaHC0 3 , Na 2 C03 , and 

Na2 S0 4 are given in a table.

6U
184. Prang, Willy, 1938, [The dependence of density and

refractive index on the concentration of very dilute 

aqueous solutions of strong electrolytes. A 

differential method for the determination of small 

differences in density]: Annal Phys., 5th Ser., v. 31, 

p. 681 - 713. In German.

Experimental study on the density of 0.1 to 0.0007 

normal solutions of NaCl, KC1, Na 2 S0 4 , Na 2C0 3 , and K 2C0 3 

at ambient pressure and 18°C. Experimental data are 

obtained by a differential float method. Experimental 

data are presented in tables, on graphs, and as 

empirical equations.

185. Ramanathan, VR., and Raman, N., 1969, Ultrasonic

velocity and compressibility index in acid - base 

solutions: Defense Science Jour., v. 19, p. 1U9 - 152.

Experimental study on the compressibility and density of 

solutions from 0.5 to 4 normal in the system HCl - NaCl 

NaOH - H 2 0 at 29°C and ambient pressure. Densities 

were measured by pycnometry and adiabatic 

compressibility data were calculated from the density 

data and measurements of the velocity of sound in the 

solutions. Experimental and smoothed data are given 

graphically.

186. Ragib, M. A., 1970, Apparent molar volumes of

electrolytes in aqueous solution at very low

concentrations: Sci. Ind. (Karachi), v. 7, p. U1 - HH.

Apparent molal volumes of NaCl and KC1 solutions down to 

10 6 molar. Measurements were made with a newly 

developed, highly sensitive densimeter. [Original text 

unavailable to authors. Data taken from Chem. Abs., 

74:16251, 1971.]

187. Rau, Hans, and Narayanan Kutty, T. R., 1970,

[PVT-measurements of concentrated hydrochloric acid to 

500°C and 1500 bars: Ber. Bunsen-Gesellschaft Phys. 

Chem., v. 76, p. 6U5 - 651. In German.

Experimental study on the apparent molal volume and 

density of 37 wt percent HCl soluticns at pressures from 

0 to 1500 bars and at temperatures from 0° to 500°C. 

Volume data were derived from dilatometry. Experimental 

data are presented in tabular and graphical form.

65
188. Ravich, M. I., and Borovaya, F. E., 1971a,

[Experimental methods and results of determining the 

densities of aqueous solutions of potassium sulfate at 

397°C in the 600 - 1500 kg/cm* pressure range]: Zhur. 

Neorg. Khim. , v. 16, p. 1776 - 1781. In Russian.

Experimental study of the density of 5 to 35 wt percent 

K 2 SO4 solutions at 397°C between 600 and 1500 kg/cm*. 

Data were obtained from dilatometry. Experimental 

specific volumes are given in a table. Specific 

volumes, compressibilities and the partial racial volumes 

of H 2 0 and K 2 S04 are given on graphs.

189. Ravich, M. I., and Borovaya, F. E., 1971b, [Volume

properties of potassium sulfate solutions at high 

pressures in the 3000 - 500°C range]: Zhur. Neorg. 

Khim., v. 16, p. 3135 - 31U1. In Russian.

Experimental study on the specific volume of K 2 S04 

solutions from 5 to 50 wt percent between 300 and 1500 

kg/cm* at 300°C, between 850 and 1500 kg/cm* at HH8°C, 

and between 1300 and 1500 kg/cm 2 at 500°C. Data are 

derived from dilatometry. Specific volumes are given in 

tables, on graphs, and as empirical equations. 

Compressibilities and the partial molal volumes of H 2 0 

and K 2 S04 are given on graphs.

190. Redlich, Otto, and Rosenfeld, P., 1931, [On the theory

of molal volumes of aqueous electrolytes II. ]: Zeit. 

Elektrochem., v. 37, p. 705 - 711. In German.

Theoretical discussion of the apparent and partial molal 

volumes of NaCl and KC1 solutions at ambient pressure 

and 0°, 25°, and 50°C. Results are given in a table and 

on graphs.

191. Redlich, Otto, 19UO, Molal volumes of solutes IV: 

Jour. Phys. Chem., v. 44, p. 619 - 629.

Calculated study on the apparent molal volume of 0 to 1 

molar solutions of KCl and NaCl at ambient pressure and 

at temperatures from 0° to 50°C. Smoothed data are 

presented in tables, on graphs, and as empirical 

equations.

192. Redlich, Otto, and Bigeleisen, J., 1942a, Molal volumes

66
of solutes. VI. Potassium chlorate and hydrochloric 

acid: Am. Chem. Soc. Jour. , v. 64, p. 758 - 760.

Experimental study on the molal volume and density of 

HC1 solutions from 0.0034 to 1.88 molar at ambient 

pressure and at 25°C. Experimental volume and density 

data were derived from the weight of a sinker in the 

solution. Experimental data are presented in tables and 

as an empirical equation.

193. Redlich, Otto, and Bigeleisen, J., 1942b, Thermodynamic

properties of electrolytes at infinite dilution: Chem. 

Rev., v. 30, p. 171 - 179.

Calculated and theoretical study on the apparent molal 

volume of 0.1 to 1.0 molal HC1 solutions at ambient 

pressure and 25°C. Smoothed data are presented in 

tables, on graphs, and as empirical equations.

194. Redlich, Otto, and Meyer, D. M., 1964, The molal

volumes of electrolytes: Chem. Rev., v. 64, p. 221 - 

227.

Review study on the molal volume and density of NaCl 

(0.05 to 0.881 molar) and KC1 (0.07 to 0.77 molar) 

solutions at ambient pressure in the temperature range 

0° to 70°C. Smoothed data are presented in tables, on 

graphs, and as empirical equations.

195. Riedl, Istvan, 1972, Analysis of physiochemical

characteristics and activation thermodynamical functions 

of the sodium hydroxide - water and sodium hydroxide - 

water - aluminum oxide systems: Nehezip Husz. Egyet, 

Miskolc, Idennyelva Kozlem, v. 32, p. 217 - 231.

An experimental study of the density of NaOH solutions 

as a function of temperature and composition at ambient 

pressure. (Original text unavailable. Data taken from 

Chem. Abs., 78:140501z, 1973.)

196. Rosen, J. S., 1959, Solutions under pressure: Jour. 

Chem. Phys., v. 30, p. 547 - 555.

Calculated study on the specific volume of NaCl and 

K 2 S04 solutions at pressures from 0 to 10.13 kb at 25°C. 

Specific volume data are given in smoothed tables and an

67
empirical equation is used.

197. Rowe, A. H. Jr., and Chou, J. C.-S., 1970,

Pressure-volume-temperature-concentration relation of 

aqueous NaCl solutions: Jour. Chem. Eng. Data, v. 15, 

p. 61 - 66.

Experimental and calculated study on the compressibility 

of NaCl (0 tc 2.5 molar) solutions at pressures from 1 

to 300 atm and at temperatures from 20° to 175°C. 

Compressibility data were derived from pvt measurements 

in stainless steel vessels. Smoothed data are given in 

tables, on graphs, and as empirical equations.

198. Salceanu, Constantin, 1963, [Speed of sound in

equimolar aqueous solutions and in some organic 

liquids]: Acad. Sci. (Paris) Comptes rendus, v. 257, p. 

1595 - 1598. In French.

Experimental compressibility of KC1, NaCl, and CaCl 2 

solutions from 0.2 to 0.6 molal at ambient pressure and 

in the temperature range 20° to 22°C. Compressibility 

data were calculated from the measurements of the 

velocity of sound in the solutions. Experimental data 

are given as tables and as an empirical equation.

199. Samoilovich, I. A., and Khetchikov, L. N., 1968,

[Relations among pressure, temperature, and density in 

aqueous solutions of sodium chloride and potassium 

chloride]: Akad. Nauk SSSR, Doklady, v. 180, p. 1450 - 

1452. In Russian.

Relative volumes [v( 20°C)/v(t) ] for 6 and 12 wt percent 

NaCl and for U and 8 wt percent KCl solutions at ambient 

pressure (given) from 185° to U14°c. Relative volumes 

are obtained from breaks in the slope of plots of 

pressure against temperature for various percentages of 

filling of an autoclave at 20°C. Experimental data are 

given on a table. Pressure-temperature isochores are 

given graphically between 180° and 550°C and to 1500 

kg/cm 2 for 6 wt percent NaCl and 8 wt percent KCl. The 

graph is contoured at 0.01 for relative volumes of 0.90 

to 0.65.

200. Samoilovich, L. A., 1970, [Interrelations of pressure,

temperature, filling factor, and concentration of

68
aqueous solutions of hydrochloric acid at high 

temperatures and pressures]: Tr. Vses. Nauch.-Issled. 

Inst. Sin. Miner. Syr'ya, v. 1970, p. 50 - 54. In 

Russian.

Relative volumes [v(20°C)/v(t)] for 3 and 6 normal HC1 

up to 300 atm and between 20° and 280°C. Relative 

volumes are obtained from breaks in the slope of plots 

of pressure against temperature for various percentages 

of filling of an autoclave at 20°C. [Original text 

unavailable to authors. Data taken from Chem. Abs., 

76-37645, 1972.]

201. Satyavati, T., Jayarama Reddy, P., and Subrahmanyam, S.

V., 1962, Ultrasonic studies in electrolytic 

mixtures-Complex ion formation: Japan Phys. Soc. 

Jour., v. 17, p. 1061 - 1064.

Experimental study on the adiabatic compressibility and 

density of 1.0 and 2.0 molar solutions of NaCl, KC1, and 

NaCl-KCl mixtures at ambient pressure and 25°C. 

Compressibility data were derived from velocity of sound 

measurements. Experimental data are given in graphical 

form.

202. Satyavati, A. V., 1968, Ultrasonic behaviour in simple

and complex ternary systems of electrolytes: Acustica, 

v. 19, p. 350 - 354.

Experimental study of the compressibility of K 2 S0 4 

Na 2 S0 4 solutions of constant 0.5 molarity at ambient 

pressure and 31.5°C. Compressibilities were obtained 

from the velocity of sound in the solution densities 

were obtained from pycnometry. Experimental data are 

given on a graph only.

203. Scott, A. F., 1931, The apparent volumes of salts in

solution. I. A test of the empirical rule of Masson: 

Jour. Phys. Chem., v. 35, p. 2315 - 2329.

Calculated study on the apparent volume of KC1 (2.25 to 

4.77 molar), NaCl (5.1 to 5.42 molar), K 2 C0 3 , and CaCl 2 

solutions at ambient pressure in the temperature range 

from 0° to 100°C. Smoothed apparent volume data are 

given in tables and on a graph.

69
204. Scott, A. F., Obenhaus, V. M., and Wilson, 6. H., 1934,

The compressibility coefficients of solutions of eight 

alkali halides: Jour. Phys. Chem., v. 38, p. 931 - 

940.

Experimental study on the compressibility and density of 

2.86 to 24.82 wt percent NaCl solutions and of 7.44 to 

26.52 wt percent KCl solutions at pressures from 100 to 

300 Mb at 35°C. Compressibilities were derived from 

piezometry. Experimental data are given in tabular and 

graphical form.

205. Scott, A. F., and Wilson, R. W., 1934b, The apparent

volumes of salts in solution and their 

compressibilities: Jour. Phys. Chem., v. 38, p. 951 - 

977.

Calculated study on the apparent volume and 

compressibility of NaCl (0.49 to 5.0 molar) and KCl 

(1.03 to 4.17 molar) solutions at 200 atm and 35°C. 

Smoothed data are given in tables, on graphs, and as 

empirical equations.

206. Seifer, A. L., Razumikhin, V. N., Sekoyan, S. S.,

Razynich, R. A., and Nevolina, M. A., 1971, [Sound 

velocity and adiabatic compressibility coefficients of 

strong electrolyte agueous solutions under 1200 bar 

pressure]: Teplofiz. Svoistva Veshchestv. Hater., v. 

1971, p. 171 - 177. In Russian.

The density and compressibility of NaCl and KCl 

solutions were measured at 1200 bars at 20° and 45°C. 

Compressibility was determined from velocity of sound 

measurements. [Original text unavailable to authors. 

Data taken from Chem. Abs. 77:39475y, 1971.]

207. Sergeevich, V. I., and Zhuze, T. P., 1960, [The

viscosity and density of formation waters and binary 

solutions of electrolytes at various temperatures and 

pressures]: Akad. Nauk SSSR, Inst. Geol. i. Razrabotki 

Goruckikh Iskopaemikh, Trudy, v. 2, p. 104 - 112. In 

Russian.

Experimental densities and viscosities of 

methane-saturated formation waters (analyses given) at 

40°C from 50 to 300 atm. Densities were derived from 

the weight of a sinker. Densities are given in a table.

70
208. Sevzov, A. I., 1937, [Determination of the viscosity

and density of caustic aqueous solutions]: Zh. Prikl. 

Khim., v. 10, p. 1500 - 1503. In Russian with abstract 

in French.

Experimental densities and viscosities of NaOH+Na 2 C03 

solutions (industrial solutions, approximate salt ratio 

6:1) from 5.3 to 28.4 wt percent at ambient pressure 

over the temperature range 15° to 95°C. Densities were 

measured with a hydrometer. Results are given on a 

table, a graph, and as an empirical equation.

209. Shakhov, Yu. A., 1972, [Calculation of the density of

aqueous salt solutions using digital computers]: Trudy 

Vses. Nauch.-Issled. Proekt. Inst. Galurgii, v. 1972, 

p. 227 - 234. In Russian.

A computer routine for calculating density as a function 

of composition based on a second degree polynomial 

equation is described. Calculated results for NaCl, 

KC1, Na 2 S0 4 , and K 2 S0 4 agree well with experimental 

data. (Original text unavailable. Data taken from 

Chem. Abs., 80:100332e, 1974.)

210. Shedlovsky, Theodore, and Brown, A. S. , 1934, The

electrolytic conductivity of alkaline earth chlorides in 

water at 25°: Amer. Chem. Soc. Jour., v. 56, p. 1066 - 

1071.

An experimental study in which the density of CaCl 2 

solutions from 0.08 to 0.26 normal were measured with a 

pycnometer at 25°C and ambient pressure. Experimental 

data and data calculated from an empirical equation are 

given in tables.

211. Shilovskaya, M. E., and Lenkova, V. I., 1974,

Determining the density and viscosity of concentrated 

solutions of certain salts in the 20 - 80°C temperature 

range: Teploenergetika, v. 21, no. 1, p. 93 - 94.

Experimental study on the density and viscosity of 

solutions of Na 2 C0 3 (0.1 to 2.4 molar), NaHC0 3 (0.1 to 

1.1 molar) and Na 2 S0 4 (0.1 to 1.1 molar) at ambient 

pressure from 20° to 80°C. Densities were obtained from 

pycnometry. Results are given on graphs and as 

empirical equations.

71
212. Simmons, H. L. , and Owen, B. B., 1957, Standard partial

molal compressibilities by ultrasonics. I. Sodium 

chloride and potassium chloride at 25°: Jour. Phys. 

Chem., v. 61, p. 479 - 482.

Calculated and experimental study on the compressibility 

of 0 to 0.07 normal solutions of KCl and NaCl at ambient 

pressure and 25°C. Compressibility data were calculated 

from measurements of the velocity of sound in the 

solutions. Experimental data are given in tables, on 

graphs, and as an empirical equation.

213. Spedding, F. H., Pikal, M. J., and Ayers, B. 0., 1966,

Apparent molal volumes of some aqueous rare earth 

chloride and nitrate solutions at 25°: Jour. Phys. 

Chem., v. 70, p. 2440 - 2449.

Experimental study on the specific gravity of 0.0073 to 

0.41 molal KCl solutions at ambient pressure and 25°C. 

Specific gravity data were derived from magnetic float 

densimeter measurements. Data are presented in tables 

and as an empirical equation.

214. Stankhanova, M. S. and Vasilev, V. A., 1963,

[Volumetric and heat capacity changes in aqueous salt 

solutions. I. The systems CsCl - LiCl - H2 0 and CsCl - 

NaCl - H 2 0]: Zhur. Fiz. Khim., v. 37, p. 1568 - 1573. 

In Russian.

Experimental study on the density of NaCl solutions from 

0.5 to 4.5 molal at ambient pressure and 25°C. Data 

were derived from pycnometry. Relative densities are 

given in a table.

215. Subrahmanyam, S. V., 1960, Adiabatic compressibilities

of electrolytic solutions: Jur. Sci. Industr. Res. 

(New Delhi), v. 19C, p. 333 - 336.

Experimental study on the compressibility of KOH and 

NaOH solutions from 0 to 5 molar at ambient pressure and 

30°C. Data were measured with a piezometer. 

Experimental results are given graphically.

216. Szalay, A., 1934, [The compressibility of dilute

electrolyte solutions]: Physik. Zeit., v. 35, p. 639 - 

643. In German.

72
Experimental study on the compressibility of NaCl and 

KC1 solutions from 0 to 0.2 molar at ambient pressure 

and at approximately 25° to 30°C. Compressibilities 

were derived from the velocity of sound. Results are 

given on a graph.

217. Tamas, Jozsef, 1963, [Density of aqueous solutions of

some strong electrolytes]: Magyar Kemiai Folyoirat 

(Budapest), v. 69, p. 497 - 499. In Hungarian.

Refer to Tamas (1964) for the English language version 

of this report.

218. Tamas, Jozsef, 1964, Density of some aqueous

electrolyte solutions: Hungary Acad. Sci., Acta Chim., 

v. 40, p. 117 .- 123.

Experimental study on the density of NaOH from 3.7 to 49 

wt percent and KOH from 4.0 to 43 wt percent at ambient 

pressure and 25°C. Densities were obtained by 

pycnometry. Experimental data are given in a table and 

on figures.

219. Taskoprulu, N. S., 1956, Volumes and compressibilities

of mixtrues of solutions of univalent electrolytes: 

Istanbul Univ. Fac. Sci. Rev., Ser. C, v. 21, p. 118 - 

125.

Experimental study on the compressibility of 

approximately 10.0 molar solutions of KC1, NaOH, and 

NaCl at ambient pressure and 26°C. Compressibilities 

were obtained from measurements of the velocity of sound 

and densities from pycnometry. Experimental data are 

given in tables and with empirical equations.

220. Tham, N. K., Gubbins, K. E., and Walker, R. D. Jr.,

1967, Densities of potassium hydroxide solutions: Jour. 

Chem. Eng. Data, v. 12, p. 525 - 526.

Experimental study on the density of KOH solutions from 

6.1 to 77.1 wt percent at ambient pressure and from 

59.9° to 161.4°C. Density data were derived from a 

hydrostatic weighing method. Experimental data are 

given in tables.

73
221. Thomas, W. G., and Perman, E. P., 1934, The

compressibility of aqueous solutions II. Royal Soc. 

(London) Proc., v. A146, p. 640 - 650.

Experimental study on the compressibility of 0.259 to 

2.21 molal solutions of KCl at 0 to 100 atm and 30°C. 

Compressibility data were obtained from piezometry. 

Experimental data are given in tables, on graphs, and as 

empirical equations.

222. Tikhomirova, N. N., 1957, [Application of methods o*

physical chemical analysis in analytical chemistry]: 

Sbornik Nauch. Rabot., Leningrad Inst. Sovet. Torgovli, 

v. 1957, no. 11, p. 134 - 142. In Russian.

Experimental study on the density at ambient pressure of 

Nad - KCl solutions at 25° and of KCl - KgSO* solutions 

at 20°C. Densities as a function of composition from 

about 1 wt percent to near saturation are given in 

tables and on graphs.

223. Tribus, Myron Asimow, Robert Richardson, Neal

Gastaldo, Charles Elliot, Keith Chambers, John and 

Evans, Robert 1959, Thermodynamic and economic 

considerations in the preparation of fresh water from 

the sea: Univ. California (Los Angeles), Oept. Eng., 

Rept. No. 59-34, 170 p.

Compilations of partial molal volumes of NaCl and H 2 0 in 

NaCl solutions from 0 to 26 wt percent between 32° and 

212°F at ambient pressure. Data are derived from a 

literature review. The references are not given. 

Volumes are given in tables and graphs with volumes in 

ftVlb-mol.

224. Tsujioka, Akira, 1957, Changes of volume on mixing

electrolytic solutions with water: Proc. Fujihara

Memorial Fac. Eng. Keio Univ., v. 10, p. 15 - 28.

A theoretical study on calculations of the density of a 

solution after diluting the solution with water. An 

empirical equation was derived from the data in the 

International Critical Tables (1928). Calculations are 

for solutions of NaCl, KCl, and NaOH at ambient pressure 

and 25°C. Smoothed data are presented in tables and on 

graphs.

74
225. Ukinashi, Hiroshi, 1959, [Physico-chemical properties

of sodium silicate solutions. Part 7, The dependency of 

density and viscosity on the composition of sodium 

silicate solutions, and its relation to the molecular 

behavior in solutions]: Asahi Garasu Kenkyu Hokoku, v. 

9, p. 137 - 161. In Japanese with English abstract.

Experimental study of the density of Na 2 0 - Si0 2 - H 2 0 

solutions, water glass, from 5° to 60°C at ambient 

pressure. The ratio of Si0 2 to Na2 0 in solution varied 

from 1 to 3.95. The concentration of Na 2 0 varied from 

0.5 to 20.74 mole percent. Experimental densities are 

given in a table and on graphs. The thermal expansivity 

is shown graphically. Coefficients for an empirical 

expression are given on a table as a function of the 

mole ratio of Si0 2 to Na 2 0 and the function is plotted 

on all graphs.

226. Unterberg, Walter, 1964, Thermophysical properties of

aqueous sodium chloride solutions: Dniv. California

(Los. Angeles), Dept. Eng., Kept. No. 64-21, 41 p.

Compilation of density and other thermophysical data for 

NaCl from 0 wt percent to saturation between 30° and 

300°F at ambient pressure. Data are derived indirectly 

from the International Critical Tables, v. 3 (1928). 

Smoothed densities are given in graphs in units of 

Ib/ft3.

227. Orusova, M. A., 1974, [Phase equilibria and

thermodynamic characteristics of solutions in the 

systems NaCl - H 2 0 and NaOH - H 2 0 at 350 - 550°C[: 

Geokhimiya, v. 1974, p. 1360 - 1366. In Russian.

Experimental study on the density of NaCl solutions from 

10 to 45 wt percent at pressures to 230 kg/cm 2 on the 

350°C isotherm and to 600 kg/cm 2 on the 400° and 450°C 

isotherms. Densities were obtained from dilatometry. 

Experimental data are given on a graph only.

228. Vasilev, V. A., Fedyainov, N. V., Karapet'yants, M, K.,

and Karpachev, A. I., 1973, [Use of equations relating 

the specific heat capacity or density of electrolyte 

solutions tc concentration]: Izv. Vyssh. Ucheb. 

Zaved., Khim. Khim. Tekhnol., v. 16, p. 689 - 693. In 

Russian.

75
An equation is presented for calculating the density of 

CaCl2 solutions as a function of composition at 25°C. 

The equation fits the experimental data with a precision 

of 0.0002 g/ml. (Original text unavailable. Data taken 

from Chem. Abs., 79: 8U062p, 1973.)

229. Vaslov, Fred, 1966, The apparent molal volumes of

alkali metal chlorides in aqueous solutions and evidence 

for salt-induced structure transitions: Jour. Phys. 

Chem., v. 76, p. 2286 - 229U.

Experimental study of the apparent molal volumes of NaCl 

and KC1 from 0 to 3.5 molal at ambient pressure and 

25°C. Volumes were measured using a differential 

hydrostatic balance. Apparent molal volumes are given 

in graphical and tabular form.

230. Vaslow, Fred, 1969, The apparent molal volumes of

lithium and sodium halides. Critical-type transitions 

in aqueous solution: Jour. Phys. Chem., v. 73, p. 3715 

- 3750.

Experimental study on the apparent molal volume of NaCl 

solutions from 0.05 to 3.5 molal at ambient pressure and 

5°C. Experimental apparent molal volumes were 

calculated from measurements using a differential 

density balance. Data are presented in tabular form.

231. Vogel, W. H., Routsis, K. J., Kehrer, V. J., Landsman,

D. A., and Tschinkel, J. G., 1967, Some physiochemical 

properties of the KOH-H 2 0 system: Jour. Chem. Eng. 

Data, v. 12, p. 465 - 472.

Calculated and experimental study on the density of 

KOH-H2 0 solutions from 55 to 85 wt percent KOH at 

ambient pressure and from 120° to 250°C. Density data 

were derived from the float technique. Experimental 

data are presented in tables, on graphs, and as 

empirical equations.

232. Voitko, A. N., Kovaleva, R. I., and Tspalin, R. A.,

1972, [Thermophysical characteristics of aqueous calcium 

chloride solutions]: Novye Metody Tekhnol. Kontr. 

Konserv. Vinodol Proizvod, v. 1972, p. 172 - 177. In 

Russian.

76
An experimental study of the density of CaCl2 solutions 

from 22 to H9 mol percent at ambient pressure from 50° 

to 130°C. (Original text unavailable. Data taken from 

Chem. Abs., 78:16U<»06g, 1973.)

233. Volz-Fladrich, H., 1962, [Physical-chemical

examinations on the systems MgCl 2 -HCl-H2 0, NaCl-HCl-H 2 0, 

and KC1-HC1-H 2 0]: Freiberger Forschungh. v. 13U, p. 1 - 

85. In German.

Experimental study on the density of 0 to nearly 

saturated solutions of NaCl-HCl-H 20 and KC1-HC1-H 2 0 at 

ambient pressure and the temperatures 0°, 25°, 35°, and 

45°C. Density data were derived from pycnometry. 

Experimental data are given in tables and on graphs.

234. Wirth, H. E., 1937, The partial molal volumes of

potassium chloride, potassium bromide, and potassium 

sulfate in sodium chloride solutions: Am. Chem. Soc. 

Jour., v. 59, p. 2549 - 2554.

Experimental and calculated study on the partial molal 

volume of KC1 (0 to 0.638 molar) and K 2 S0 4 (0 to 0.338 

molar) contained in 0 to 0.97 molar NaCl solutions at 

ambient pressure and 25°C. Partial molal volumes and 

densities were calculated from the weight of a sinker in 

the solution. Experimental data are presented in 

tables, on graphs, and as empirical eguations.

235. Wirth, H. E., 1940a, Apparent and partial molal volumes

of sodium chloride and hydrochloric acid in mixed 

solutions: Am. Chem. Soc. Jour., v. 62, p. 1128 - 113U.

Experimental study on the apparent and partial molal 

volumes of mixed solutions of HC1 and NaCl from 0.01 to 

3.0 normal at ambient pressure and 25°C. Volume data 

were calculated from the weight of a sinker in the 

solutions. Experimental data are given in tables, on 

graphs, and as empirical eguations.

236. Wirth, H. E., 1940b, The problem of the density of sea 

water: Jour. Marine Research, v. 3, p. 230 - 217.

Calculated study on the density of sea water, NaCl, KC1, 

K2 S04 , and CaCl 2 at ambient pressure and 25°C. Smoothed 

data are given in tables, graphically, and as empirical

77
equations.

237. Wirth, H. E., and LoSurdo, Antonio, 1968, Temperature

dependence of volume changes on mixing electrolyte

solutions: Jour. Chem. Eng. Data, v. 13, p. 226 - 231.

Experimental study on the volume and density of 4.0 

molal NaCl and 1.33molal Na 2 S04 solutions and their 

mixtures at ambient pressure between 5° and 45°C. 

Density and volume data were derived from dilatometry. 

Experimental data are presented in tables, on graphs, 

and as empirical equations.

238. Wirth, H. E., and Bangret, F. K., 1972, Apparent molal

volumes of sodium chloride and magnesium chloride in 

aqueous solution: Jour. Phys. Chem., v. 76, p. 3188 

3491.

Experimental study on the apparent molal volume of Nad 

from 0 to 4 molal at ambient pressure and 25°C. 

Apparent molal volume data were derived from dilatometry 

and the sinker method. Experimental data are given in 

tables, graphically, and as empirical equations.

239. Wright, Robert, 1940, The relation between the

coefficient of thermal expansion and structure of 

solutions: Chem. Soc. (London) Jour., v. 1940A, p. 870 

- 873.

Experimental study on the coefficient of thermal 

expansion of NaCl (1 to 6 molal) and KC1 (1 to 4 molal) 

at ambient pressure in the temperature range 25° to 

78°C. Thermal expansion data were derived from the 

height of solution in a silica tube. Experimental data 

are given in tabular form.

240. Zen, E-an, 1957, Partial molal volumes of some salts in

aqueous solutions: Geochim. Cosmochim. Acta, v. 12, 

p. 103 - 122.

Review paper on the partial molal volumes of KC1, NaCl, 

HC1, KOH, NaOH, CaCl2t K 2 C0 3 , Na 2 C0 3> K 2 S04 , Na 2 S04 , and 

H 2 S0 4 at ambient pressure and 0° and 25°C. Data are 

given in tables.

78

.S. GOVERNMENT PRINTING OFFICE: 1975-0-690-036/42