AP Chemistry
7.12 Common-Ion Effect
7.11 Introduction to Solubility Equilibria
7.9 Introduction to Le Châtelier’s Principle
A student investigates the dissolution of calcium fluoride, \(\text{CaF}_2\text{(s)}\), at \(25\ ^\circ\text{C}\). The dissolution process is represented by the following equilibrium equation:
\[ \text{CaF}_2\text{(s)} \rightleftharpoons \text{Ca}^{2+}\text{(aq)} + 2\,\text{F}^-\text{(aq)} \]
The student compares the molar solubility of \(\text{CaF}_2\) in pure distilled water with its molar solubility in a \(0.10\text{ M }\text{NaF(aq)}\) solution at the same temperature. Which of the following statements best compares the molar solubility of \(\text{CaF}_2\) in \(0.10\text{ M }\text{NaF(aq)}\) with its molar solubility in pure water and provides the correct justification?
\[ \text{CaF}_2\text{(s)} \rightleftharpoons \text{Ca}^{2+}\text{(aq)} + 2\,\text{F}^-\text{(aq)} \]
The student compares the molar solubility of \(\text{CaF}_2\) in pure distilled water with its molar solubility in a \(0.10\text{ M }\text{NaF(aq)}\) solution at the same temperature. Which of the following statements best compares the molar solubility of \(\text{CaF}_2\) in \(0.10\text{ M }\text{NaF(aq)}\) with its molar solubility in pure water and provides the correct justification?
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