Previous investigations carried out in this laboratory have dealt with the solubility and the activity coefficient of silver acetate in the presence of an added strong electrolyte in aqueous solutions (3, 6), in water-alcohol mixtures (4), and in mixtures of water and acetone (5).When the added electrolyte was a nitrate of a univalent metal, the observed effect could be accounted for satisfactorily on the basis of the theoiy of Debye and Hückel. WTien the added salt was a nitrate of a bivalent metal, the theory seemed at first to be less successful. The assumption, however, that the second stage of ionization of acetates of bivalent metals is incomplete was found to be capable of explaining this apparent failure of the Debye theory; in fact, it was possible to calculate fairly consistent values for the second dissociation constants of acetates of calcium, strontium, and barium in water, in mixtures of water and ethyl alcohol, and in mixtures of water and acetone (5). SUMMARY 1. The solubility of silver acetate at 25°C. in aqueous solutions containing sodium acetate, potassium acetate, calcium acetate, or strontium acetate has been measured.2. The apparent solubility product in the presence of added acetates increases more rapidly with the ionic strength than when the added salt has no ion in common with silver acetate. 3. The apparent inapplicability of the theory of Debye can be accounted for by assuming the formation of the diacetato-argentate ion.4. The dissociation constant of AgA¡" is found to be equal to 0.28 ± 0.05. 5. Reference is made to the possible formation of acetatodisilver ion, Ag2A4'.
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