A student investigates the solubility of calcium fluoride, \(\text{CaF}_2(s)\), in different aqueous environments at \(25^\circ\text{C}\). The relevant equilibrium processes and their equilibrium constants at this temperature are given below.

\[\text{CaF}_2(s) \rightleftharpoons \text{Ca}^{2+}(aq) + 2\,\text{F}^-(aq) \quad K_{sp} = 3.9 \times 10^{-11}\]
\[\text{HF}(aq) \rightleftharpoons \text{H}^+(aq) + \text{F}^-(aq) \quad K_a = 6.3 \times 10^{-4}\]

The student compares the molar solubility of \(\text{CaF}_2(s)\) in pure water at \(\text{pH} = 7.0\) to its molar solubility in a buffer solution maintained at \(\text{pH} = 3.0\). Which of the following correctly predicts and justifies the relative solubility of \(\text{CaF}_2(s)\) in the buffer solution at \(\text{pH} = 3.0\) compared to pure water?