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The electrochemical cell shown below is a concentration cell.
$$M \mid M^{2+}$$ (saturated solution of a sparingly soluble salt, $$MX_2$$) $$\parallel M^{2+}$$ (0.001 mol $$dm^{-3}$$) $$\mid M$$
The emf of the cell depends on the difference in concetration of $$M^{2+}$$ ions at the two electrodes. The emf of the cell at 298 is 0.059 V
Question 29
The solubility product ($$K_{sp};mol^3 dm^{-9}$$) of $$MX_2$$ at 298 based on the information available the given concentration cell is (take $$2.303 \times R \times \frac{298}{F} = 0.059 V$$)
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