AP Chemistry
7.12 Common-Ion Effect
7.11 Introduction to Solubility Equilibria
A student prepares a saturated solution of \(\text{BaSO}_4\) by adding solid \(\text{BaSO}_4\) to a \(0.10\text{ M }\text{Na}_2\text{SO}_4\text{(aq)}\) solution at \(25^\circ\text{C}\). The dissolution equilibrium and its solubility product constant at this temperature are represented below.
\[ \text{BaSO}_4\text{(s)} \rightleftharpoons \text{Ba}^{2+}\text{(aq)} + \text{SO}_4^{2-}\text{(aq)} \quad K_{sp} = 1.0 \times 10^{-10} \]
Assuming that the volume of the solution does not change and that the dissolution of \(\text{BaSO}_4\text{(s)}\) contributes a negligible amount of \(\text{SO}_4^{2-}\text{(aq)}\), what is the molar solubility of \(\text{BaSO}_4\text{(s)}\) in this solution?
\[ \text{BaSO}_4\text{(s)} \rightleftharpoons \text{Ba}^{2+}\text{(aq)} + \text{SO}_4^{2-}\text{(aq)} \quad K_{sp} = 1.0 \times 10^{-10} \]
Assuming that the volume of the solution does not change and that the dissolution of \(\text{BaSO}_4\text{(s)}\) contributes a negligible amount of \(\text{SO}_4^{2-}\text{(aq)}\), what is the molar solubility of \(\text{BaSO}_4\text{(s)}\) in this solution?
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