Chemistry - Electrochemistry Question with Solution | TestHub

The electrochemical cell shown below is a concentration cell. $\mathrm{M}\mid {\mathrm{M}}^{2+}$ (saturated solution of a sparingly soluble salt, ${\mathrm{MX}}_2)\Vert {\mathrm{M}}^{2\perp }\left(0.001\mathrm{mol}{\mathrm{dm}}^{-3}\right)\mid \mathrm{M}$. The emf of the cell depends on the difference in concentrations of ${\mathrm{M}}^{2+}$ ions at the two electrodes. The emf of the cell at $298\mathrm{K}$ is $0.059\mathrm{V}$. Question:The solubility product $\left({\mathrm{K}}_{sp};{\mathrm{mol}}^3{\mathrm{dm}}^{-9}\right)$ of ${\mathrm{MX}}_2$ at $298\mathrm{K}$ based on the information available for the given concentration cell is (take $2.303\times \mathrm{R}\times 298/\mathrm{F}=0.059\mathrm{V}$ )