Introduction to Solubility Equilibria Practice Test

A student adds excess solid barium sulfate, $\text{BaSO}4(s)$, to pure water at $25^\circ\text{C}$. After equilibrium is established, the solubility product constant is $K{sp}(\text{BaSO}_4)=1.0\times10^{-10}$. What is the equilibrium concentration of $\text{Ba}^{2+}(aq)$? (Assume volume change is negligible.)

Excess solid copper(I) chloride, $\text{CuCl}(s)$, is placed in pure water at $25^\circ\text{C}$ until equilibrium is established. The $K_{sp}$ of $\text{CuCl}$ is $1.0\times10^{-6}$.

Dissolution: $\text{CuCl}(s)\rightleftharpoons \text{Cu}^+(aq)+\text{Cl}^-(aq)$

Starting with zero ion concentrations, what is the equilibrium concentration of $\text{Cl}^-(aq)$?

ICE table (in M):