AP Chemistry
7.12 Common-Ion Effect
7.11 Introduction to Solubility Equilibria
A student prepares a saturated solution of silver chromate, \(\text{Ag}_2\text{CrO}_4(s)\), by adding excess solid to a \(0.050\text{ M }\text{K}_2\text{CrO}_4(aq)\) solution at \(298\text{ K}\). The dissolution equilibrium and solubility product constant, \(K_{sp}\), are represented below.
\[\text{Ag}_2\text{CrO}_4(s) \rightleftharpoons 2\,\text{Ag}^+(aq) + \text{CrO}_4^{2-}(aq) \quad K_{sp} = 2.0 \times 10^{-11}\text{ at }298\text{ K}\]
Assuming the change in volume upon adding the solid is negligible, what is the molar solubility of \(\text{Ag}_2\text{CrO}_4\) in the \(0.050\text{ M }\text{K}_2\text{CrO}_4(aq)\) solution at \(298\text{ K}\)?
\[\text{Ag}_2\text{CrO}_4(s) \rightleftharpoons 2\,\text{Ag}^+(aq) + \text{CrO}_4^{2-}(aq) \quad K_{sp} = 2.0 \times 10^{-11}\text{ at }298\text{ K}\]
Assuming the change in volume upon adding the solid is negligible, what is the molar solubility of \(\text{Ag}_2\text{CrO}_4\) in the \(0.050\text{ M }\text{K}_2\text{CrO}_4(aq)\) solution at \(298\text{ K}\)?
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