Pitzer and Brewer Tabulations

Pitzer and L. Brewer used equation (18.12) as the base for tabulating a summary of the thermodynamic properties of aqueous electrolyte solutions at 298.15 K. They wrote equation (18.12) in the form that involves base 10 logarithms 

They chose a reference system (KC1 for a 1 1 electrolyte and CaCI2 for a 2 1 electrolyte) for which they tabulated detailed values of f , (j)L, L2, 4 CP, and 

Values of AB are tabulated by Pitzer and Brewer4 for a number of 1 1, 2 1, and 1 2 electrolytes from which 7 can be calculated. 

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Chapter 18 describes electrolyte solutions that are too concentrated for the Debye-Hiickel theory to apply. Gugenheim s equations are presented and the Pitzer and Brewer tabulations, as a method for obtaining the thermodynamic properties of electrolyte solutions, are described. Next, the complete set of Pitzer s equations from which all the thermodynamic properties can be calculated, are presented. This discussion ends with an example of the extension of Pitzer s equations to high temperatures and high pressures. Three-dimensional figures show the change in the thermo-... 

The ideality of the solvent in aqueous electrolyte solutions is commonly tabulated in terms of the osmotic coefficient 0 (e.g., Pitzer and Brewer, 1961, p. 321 Denbigh, 1971, p. 288), which assumes a value of unity in an ideal dilute solution under standard conditions. By analogy to a solution of a single salt, the water activity can be determined from the osmotic coefficient and the stoichiometric ionic strength Is according to,... 

That is, an interaction term (related to the molality of the solution) is added to the Debye-Hiickel function. B values may be calculated from the tabulations in Pitzer and Brewer (1961). 

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