A sample of solid silver chloride, AgCl(s), is stirred with distilled water in a sealed container at constant temperature until equilibrium is reached between the undissolved solid and the aqueous ions.
After equilibrium is established, a small amount of solid sodium chloride, NaCl(s), is introduced into the container while all other conditions are kept the same.
(1) Describe qualitatively what will happen to the concentrations of Ag⁺(aq) and Cl⁻(aq) in the solution after the NaCl is added and the system once again reaches equilibrium.
(2) Predict the observable macroscopic change, if any, in the amount of AgCl(s) present in the container once the new equilibrium is attained. Give a chemical explanation for your prediction.
(3) Explain, in terms of the equilibrium that exists between AgCl(s) and its ions in solution, why the addition of NaCl(s) produces the changes you described in parts (a) and (b). Your explanation should explicitly reference the positions of reactants and products in the equilibrium expression.