A student prepares a saturated solution by adding an excess of a sparingly soluble metal hydroxide, \(\text{M(OH)}_2\text{(s)}\), to an aqueous buffer solution maintained at a constant \(\text{pH}\) of \(11.00\) at \(25^\circ\text{C}\). The dissolution equilibrium and solubility product constant are shown below:

\[ \text{M(OH)}_2\text{(s)} \rightleftharpoons \text{M}^{2+}\text{(aq)} + 2\,\text{OH}^-\text{(aq)} \quad\quad K_{sp} = 4.0 \times 10^{-12} \text{ at } 25^\circ\text{C} \]

Assuming the buffer capacity is sufficient to maintain the \(\text{pH}\) at \(11.00\), what is the molar solubility of \(\text{M(OH)}_2\text{(s)}\) in this buffer solution?