Introduction to Solubility Equilibria Practice Test

A student adds excess solid silver chloride, $\text{AgCl}(s)$, to $1.00,\text{L}$ of pure water at $25^\circ\text{C}$ and stirs until equilibrium is established. The $K_{sp}$ of $\text{AgCl}$ at $25^\circ\text{C}$ is $1.6\times10^{-10}$.

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

Assuming the initial ion concentrations are zero, what is the equilibrium concentration of $\text{Ag}^+(aq)$?

ICE table (in M):

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.)