Ionic Strength Function in Anhydrous Acetic Acid. III. Solubility of Potassium Bromide and Potassium Perchlorate

Abstract

The application of the Debye-Huckel theory to the treatment of ionic strength effects on dilute solutions of electrolytes in anhydrous acetic acid has been discussed in the two preceding notes in this series (2, 3). By using the simple assumption that the calculated ionic strength should include only the contribution from the unassociated ions of the diverse electrolyte, it was possible to identify an electrolytic influence upon two types of equilibria: (a) the solubility of a slightly soluble strong electrolyte; and (b) the molnomer-dimer association for a weak electrolyte. In the latter instance an ionic strength influence on the system was evident even though the constants used for dimerization and ion pair dissociation were not obtained at identical temperatures. The adequacy of the model for the analysis of these two equilibria prompted a re-examination of published data on the solubilities of inorganic solutes in anhydrous acetic acid within the temperature interval from 20 to 30°C. Nearly all of the ion pair dissociation constants that have been determined in acetic acid fall within this temperature range. Two additional solubility equilibria have been found for which the tffect exerted by the diverse 1-1 electrolyte in the solution phase is described by equation 1.