Abstract
Solubilities of alkali metal chlorides except lithium were determined in ammonia, EDA, methyl- and
ethylamines, DME, and THF at three different temperatures. From these data, standard thermodynam- ic functions of solution and solvation with respect to ion formation were calculated. The standard free energies of solvation increased linearly as a function of D_1. However, the requirements of the Bom equation were not satisfied because the slopes and intercepts of these plots were not equal. Values of the entropies of solvation are roughly accounted for on the basis of the freezing out of a fixed number of sol- vent molecules. The superiority of ammonia as an agent for solvating ions is attributed to its relatively low molecular entropy compared to other solvents. A criterion for salt-like behavior is introduced and used to suggest that saturated alkali metal solutions are salt like and are probably dominated by the
+· ~ ion pairs. On this basis solubilities of metals in ammonia are too large to be accounted for without introducing additional species.