Silver chloride, AgCl(s), is an “insoluble” strong electrolyte.

(a) Write the equation for the dissolution of AgCl(s) in H₂O(I).

(b) Write the expression for Kc for the reaction in part (a).

(c) Based on the thermochemical data in Appendix C and Le Châtelier’s principle, predict whether the solubility of AgCl in H₂O increases or decreases with increasing temperature.

(d) The equilibrium constant for the dissolution of AgCl in water is 1.6 × 10^-10 at 25°C. In addition, Ag⁺(aq) can react with Cl^-(aq) according to the reaction Ag⁺(aq) + 2Cl^- (aq) ⇌ AgCl₂^-(aq) where K_c = 1.8 × 10⁵ at 25°C. Although AgCl is “not soluble” in water, the complex AgCl₂^- is soluble. At 25°C, is the solubility of AgCl in a 0.100 M NaCl solution greater than the solubility of AgCl in pure water, due to the formation of soluble AgCl₂^- ions? Or is the AgCl solubility in 0.100 M NaCl less than in pure water because of a Le Châtelier-type argument? Justify your answer with calculations. (Hint: Any form in which silver is in solution counts as “solubility.”)