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

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