The electrochemical cell shown below is a concentration cell, M|M2+ (Saturated solution of a sparingly soluble salt, MX2)||M2+(0.001 mol dm−3)M. The emf of the cell depends on the difference in concentration of M2+ ions at the two electrodes. The emf of the cell at 298K is 0.059 The solubility product (Ksp:mol3dm−9) of MX2 at 298 K based on the information available the given concentration cell is (take 2.303×R×298/F=0.059V)

The electrochemical cell shown below is a concentration cell, M|M2+ (S

1.	The electrochemical cell shown below is a concentration cell, M\|M2+ (Saturated solution of a sparingly soluble salt, MX2)\|\|M2+(0.001 mol dm−3)M. The emf of the cell depends on the difference in concentration of M2+ ions at the two electrodes. The emf of the cell at 298K is 0.059 The solubility product (Ksp:mol3dm−9) of MX2 at 298 K based on the information available the given concentration cell is (take 2.303×R×298/F=0.059V)
Answer» The electrochemical cell shown below is a concentration cell, $M \| M^{2 +}$ (Saturated solution of a sparingly soluble salt, $M X_{2}) \| \| M^{2 +} (0.001 m o l d m^{- 3}) M .$ The emf of the cell depends on the difference in concentration of $M^{2 +}$ ions at the two electrodes. The emf of the cell at 298K is 0.059 The solubility product $(K_{s p} : m o l^{3} d m^{- 9})$ of $M X_{2}$ at 298 K based on the information available the given concentration cell is (take $2.303 \times R \times 298 / F = 0.059 V)$