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M/M^2+ //M^2+(0.001)/M. The solubility p...

M/M^2+ //M^2+(0.001)/M. The solubility product `(K_Sp: mol^(3) dm^(-9))` of `MX^(2)` at 298 based on the information available the given concentration cell is ( taken `2.303xxRxx298//F= 0.059V`). The em of the cell given is 0.059.

A

`1xx10^(-15)`

B

`4xx10^(-15)`

C

1xx10^-12`

D

`4xx10^9

Text Solution

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To solve the problem, we need to find the solubility product (Ksp) of the sparingly soluble salt MX² at 298 K, using the given information about the concentration cell. ### Step-by-Step Solution: 1. **Identify the Cell Reaction:** The cell is represented as M/M²⁺ // M²⁺(0.001)/M. The half-reactions involved are: - At the anode: \( M \rightarrow M^{2+} + 2e^- \) (oxidation) - At the cathode: \( M^{2+} + 2e^- \rightarrow M \) (reduction) ...
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