The electrochemical cell shown below is a concentration cell
`M|M^(2+)` (saturated solution of a sparingly soluble salt, `MX_(2))||M^(2+)(0.001mol dm^(-3))|M`
The emf of the cell depends on the difference in concentration of `M^(2+)` ions at the electrodes. The emf of the cell at `298K` is `0.059V`
The solubility product `(K_(sp), mol^(3) dm^(-9))` of `MX_(2)` at `298K` based on the information available for the given concentration cell is (take `2.303 xx R xx 298//F = 0.059V)`

Options

A. `-5.7`
B. `5.7`
C. `11.4`
D. `-11.4`

Answer

D

Explanation

`triangleG=-nFE_(cell)=-2xx96500xx0.059xx10^(-3)kJ//"Mole"`
`=-11.4kJ//"mole"`