A student adds excess solid \(\text{PbCl}_2\) to a \(0.10\text{ M }\text{NaCl}\) solution at \(25^\circ\text{C}\). The dissolution equilibrium is represented below.

\[ \text{PbCl}_2(s) \rightleftharpoons \text{Pb}^{2+}(aq) + 2\,\text{Cl}^-(aq) \]

At \(25^\circ\text{C}\), the solubility product constant, \(K_{sp}\), for \(\text{PbCl}_2\) is \(1.6 \times 10^{-5}\). Assuming that the contribution of \(\text{Cl}^-\) from the dissolution of \(\text{PbCl}_2\) is negligible, what is the molar solubility of \(\text{PbCl}_2\) in this solution?