When a sparingly soluble salt such as is introduced into an aqueous solution that…
CHEMISTRY · Single correct · AP · Chemistry · Equilibrium · Equilibrium
Problem
When a sparingly soluble salt such as AgCl is introduced into an aqueous solution that already contains a large concentration of Cl− from dissolved NaCl, which of the following statements best describes the effect on the solubility of AgCl?
(a) Its solubility increases because the added Cl− drives the dissolution equilibrium to the right.
(b) Its solubility decreases because the added Cl− shifts the dissolution equilibrium toward the solid phase.
(c) Its solubility remains unchanged because the solubility product constant Ksp is fixed at the given temperature.
(d) Its solubility first increases and then decreases as the ionic strength of the solution rises.