A student prepares a saturated solution of lead(II) iodide by adding solid \(\text{PbI}_2\) to distilled water at \(25^\circ\text{C}\) until excess solid remains at the bottom of the beaker:

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

The value of \(K_{sp}\) for \(\text{PbI}_2\) at \(25^\circ\text{C}\) is \(3.2 \times 10^{-8}\). Assuming no other equilibria occur, what is the concentration of \(\text{I}^-(aq)\) in the saturated solution at \(25^\circ\text{C}\)?