Practice Test 6

A student adds excess solid silver chloride, $\text{AgCl}(s)$, to $1.00,\text{L}$ of pure water at $25^\circ\text{C}$. The equilibrium expression is $K_{sp}=\text{Ag}^+\text{Cl}^-$, and $K_{sp}(\text{AgCl})=1.6\times10^{-10}$. What is the equilibrium concentration of $\text{Ag}^+$ in the solution? (Assume volume change is negligible.)

Excess solid iron(II) sulfide, $\text{FeS}(s)$, is placed in pure water at $25^\circ\text{C}$ until equilibrium is reached. For $\text{FeS}(s)\rightleftharpoons \text{Fe}^{2+}(aq)+\text{S}^{2-}(aq)$, $K_{sp}=6.4\times10^{-19}$. What is the equilibrium concentration of $\text{Fe}^{2+}$ in the saturated solution?