The solubility of ammonium chloride in acetonitrile, dioxane, and 2-propanol in the range 298.153338.15 K was determined using 36 Cl tracer. The influence of properties of nonaqueous solvents on the solubility of ammonium, potassium, and sodium chlorides was subjected to thermodynamic and correlation analysis. The low solubility of ammonium chloride in dioxane and acetonitrile is due to the endothermic effect, and its high solubility in 2-propanol, to the exothermic effect of the salt solution. The entropy of solution affects the solubility of ammonium chloride in acetonitrile only slightly, in contrast to dioxane and 2-propanol in which the entropies of solution are significant and have opposite signs. The solubility of ammonium and potassium chlorides depends on the electron-acceptor power of the solvents and electrostatic interactions in solution, whereas the solubility of sodium chloride in organic solvents is determined by the combined influence of the donor3acceptor and dielectric properties of the solvents.The standard thermodynamic characteristics of solution and solvation of electrolytes reflect the total effect from the ion3solvent and solvent3solvent interactions. The ion3solvent interactions involve the following effects [1]: polarization of the medium; changes in the solvent structure; creation of a cavity in the solvent for accommodation of the dissolved ion; specific interactions of ions with solvent molecules (hydrogen bonding, donor3acceptor interactions).Our goal was to study the thermodynamics of solution of ammonium chloride in dioxane, acetonitrile, and 2-propanol and to examine the solvent effects on the solubility of ammonium, sodium, and potassium chlorides in nonaqueous solvents by methods of correlation and regression analysis, based on the experimental results obtained and on the published data. The solubility of ammonium chloride in dioxane, acetonitrile, and 2-propanol in the range 298.153 338.15 K was determined using 36 Cl tracer. The labeled salt NH 4 36 Cl was prepared by ion exchange of ammonium chloride with H 36 Cl. The total error of the radiometric measurement results was evaluated according to GOST (State Standard) 8-207376 [2]. The solubilities L in nonaqueous solvents at 298.153338.15 K, calculated as arithmetic mean values of separate determinations at a confidence level of 0.95, are listed in Table 1. The confidence interval [D a = +t a sn 31/2 , where t a is Student's coefficient; s, rms deviation of the solubility; n, number of samples taken (no less than 18)] for theH 4 Cl solubility is +(6 0 10 36 3 0.001) M depending on the solvent and temperature. The values by which the solubility in the examined solvents varies with temperature (DL T ) exceed the error of L determination: dL T is 21.5 0 10 35 in dioxane, 3.2 0 10 34 in acetonitrile, and 4.0 0 10 33 M in 2-propanol (Table 1).With increasing temperature, the salt solubility in nonaqueous solvents increases. The coefficients of the temperature dependence of the NH 4 Cl solubility in nonaqueous solvents, ln L = a + b...