AP Chemistry
7.11 Introduction to Solubility Equilibria
A student measures the solubility of a sparingly soluble salt, \(\text{MX}_2\), in pure water at \(25^\circ\text{C}\) according to the dissolution equilibrium below.
\[ \text{MX}_2(s) \rightleftharpoons \text{M}^{2+}(aq) + 2\text{X}^-(aq) \]
The student finds that the solubility of \(\text{MX}_2\) is \(0.40\text{ g/L}\) at \(25^\circ\text{C}\). Given that the molar mass of \(\text{MX}_2\) is \(200\text{ g/mol}\), what is the value of the solubility product constant, \(K_{sp}\), for \(\text{MX}_2\) at this temperature?
\[ \text{MX}_2(s) \rightleftharpoons \text{M}^{2+}(aq) + 2\text{X}^-(aq) \]
The student finds that the solubility of \(\text{MX}_2\) is \(0.40\text{ g/L}\) at \(25^\circ\text{C}\). Given that the molar mass of \(\text{MX}_2\) is \(200\text{ g/mol}\), what is the value of the solubility product constant, \(K_{sp}\), for \(\text{MX}_2\) at this temperature?
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