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Mayer's Ionic Solution Theory Applied to Electrolyte Mixtures
1.J. E. Mayer, J. Chem. Phys. 18, 1426 (1950).
2.H. S. Frank and M. S. Tsao, Ann. Rev. Phys. Chem. 4, 43 (1953).
3.However, there are two important errors in their review. Their first equation, expressing the assumption that the potential of average force is the sum of pairwise contributions, is not, as stated, essential to the theory. This is shown by Friedman (reference 4). The other error is the statement that Poirier’s equations give exactly the thermodynamic properties of the primitive model. In fact Poirier neglected terms corresponding to , , , in the terminology of the present paper.
4.H. L. Friedman, Molecular Phys. 2, 23 (1959).
5.H. L. Friedman, J. Chem. Phys. (to be published).
6.In this paper, parentheses are used in mathematical expressions to indicate functional dependence, as d(x).
7.H. L. Friedman, Molecular Phys. 2, 190 (1959);
7.H. L. Friedman, 2, 436 (1959)., J. Mol. Spectrosc.
8.This divides Eq. (4.1) into two terms, each of which is singular for any K. By an alteration of this procedure it is possible to avoid these infinities but this would complicate the discussion and obscure the point of interest.
9.G. Placzek, National Research Council of Canada, Division of Atomic Energy, Document No. MT‐1 (NRC 1547), 1946.
10.J. Poirier, J. Chem. Phys. 21, 972 (1953).
11.A. Erdelyi, W. Magnus, F. Oberhettinger, and F. Tricomi, Higher Transcendental Functions (McGraw‐Hill Book Company, Inc., New York, 1953), Vol. 2, p. 134.
12.T. Hill, Statistical Mechanics (McGraw‐Hill Book Company, Inc., New York, 1956), p. 203.
13.R. A. Robinson, J. Am. Chem. Soc. 74, 6035 (1952).
13.R. A. Robinson, “Electrochemical Constants,” Nat. Bureau Standards Circ. 524, 191 (1953);
13.R. A. Robinson, Trans. Faraday Soc. 49, 1147 (1953).
13.Robinson and Lim, Trans. Faraday Soc. 49, 1144 (1953)., Trans. Faraday Soc.
14.T. F. Young and M. B. Smith, J. Phys. Chem. 58, 716 (1954).
15.L. Pauling, The Nature of the Chemical Bond (Cornell University Press, Ithaca, New York, 1945), p. 346.
16.H. S. Harned and B. B. Owen, (a) The Physical Chemistry of Electrolyte Solutions (Reinhold Publishing Corporation, New York, 1958), 3rd ed., Table 12–5–2, second column ; (b) ibid., Chap. 14.
17.H. S. Harned and M. A. Cook, J. Am. Chem. Soc. 59, 1890 (1937).
18.Calculated by using Eq. (6.9) of reference 5.
19.G. Scatchard and S. S. Prentiss, J. Am. Chem. Soc. 56, 2320 (1934).
20.T. F. Young, Y. C. Wu, and A. A. Krawetz, Discussions Faraday Soc. 24, 37 (1957).
21.E. Meeron, J. Chem. Phys. 27, 1238 (1957).
22.J. N. Bro/nsted, J. Am. Chem. Soc. 44, 877 (1922).
23.Bro/nsted’s theory as first formulated included a salting‐out interaction in addition to the specific ion interaction. The former has not been employed in the later theories referred to here.
24.E. A. Guggenheim, Rept. of Scandinavian Sci. Congr. (Copenhagen, 1929), p. 298;
24.Phil. Mag. 19, 588 (1935).
25.R. A. Robinson and R. H. Stokes, Electrolyte Solutions (Butterworths Scientific Publications, London, 1955).
26.Unpublished work by Tsao described in reference 2.
27.S. Levine and H. E. Wrigley, Discussions Faraday Soc. 24, 43 (1957).
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