Answer to Question #195439 in Inorganic Chemistry for Lovely Mae Zolina

Question

Silver chloride, AgCl(s), is an “insoluble” strong electrolyte. (a) Write the equation for the dissolution

of AgCl(s) in H2O(l). (b) Write the expression for Kc for the reaction in part (a). (c) The equilibrium

constant for the dissolution of AgCl in water is 1.6x10-10 at 25°C. In addition, Ag+

(aq) can react with

Cl-(aq) according to the reaction Ag+(aq) + 2 Cl-(aq) -> AgCl2(aq) where Kc=1.8x10-5

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.”)

Answer 1

The answer to your question is provided in the image: