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Question

The electrochemical cell shown below is a concentration cell, M|M2+ (Saturated solution of a sparingly soluble salt, MX2)||M2+(0.001 mol dm3)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:mol3dm9) of MX2 at 298 K based on the information available the given concentration cell is (take 2.303×R×298/F=0.059V)

A
1×1015
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B
4×1015
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C
1×1012
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D
4×1012
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Solution

The correct option is B 4×1015
The solubility equilibrium for MX2 is
MX2(s)M2+(aq)+2X(aq)
Solubility product, Ksp=][M2+][X]2
=105×2×105)2=4×1015
[ In saurated solution of MX2,[X]=2[M2+]]

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