US EPA

8152519 

Journal Article 

Equilibria in silver acetate solutions 

Macdougall, FH; Peterson, S 

1947 

1 

Journal of Physical Chemistry
ISSN: 0022-3654 

51 

6 

1346-1361 

English 

10.1021/j150456a009 

1. We have measured the E.M.F. at 25°C. and at 34.7°C. of cells in which one of the solutions contained sodium acetate and either silver acetate or silver nitrate. 2. We have determined the solubility of silver acetate at 25°C. in 2.95 M sodium perchlorate. 3. In the discussion and interpretation of our results we have made use of previous studies on the solubility of silver acetate in water in the presence of added electrolytes. We have also availed ourselves of a recent investigation of Leden on the E.M.F. of certain cells. 4. The most important result of our work is the determination of the ionization constant, Ki, of silver acetate. For example, in 0.06 molal silver acetate in aqueous solution the degree of ionization is about 85 per cent. 5. We confirmed the existence of the complex ion, AgA2-, and determined its dissociation constant, K2. 6. Our results enabled us to correct previous estimates of the true activity product, K1, of Ag+ and A- in saturated aqueous solutions. 7. We give here a list of equilibrium constants expressed in terms of molal activities and the result obtained in a determination of solubility: (a) For the reaction AgA = Ag+ + A-, Ki = 0.186 at 25°C.; Ki = 0.179 at 34.7°C. (b) For the reaction AgA2- = Ag+ + 2A-, K2 = 0.230 at 25°C.; K2 = 0.217 at 34.7°C. (c) For the equilibria AgA(s) = AgA = Ag+ + A-, K1 = aAg+aA- = 0.00195 at 25°C. (d) For the molality, m, and molarity, c, of silver acetate at 25°C. in 2.95 molar sodium perchlorate, saturated with silver acetate, m = 0.06160 and c = 0.05304.