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Consider the following electrode process...

Consider the following electrode processes of a cell,
`Cl^- rightarrow 1/2 Cl_2 +e^-.
[MCl +e^- rightarrow M +Cl^-]`.
If EMF of the cell is -1.140 V and `E^@` value of the cell is -0.55V at 298K, the value of the equilibrium constant of the sparingly soluble salt MCl is in the order of

A

`10^-10`

B

`10^-8`

C

`10^-7`

D

`10^-11`

Text Solution

Verified by Experts

The correct Answer is:
A
Answer(1) `MCl rightarrow M + 1/2 Cl_2`
Nernst equation, `E_cell = E^@_cell - 0.059/n log K_c` .
-1.140 = -0.55 -0.059/1 `log K_c` .
-0.59 = -0.059 log `K_c` .
`Rightarrow log K_c =10`.
`therefore K_c = 10^10` .
solubility product (K_sp) for `M + 1/2 Cl_2 rightarrow MCl rigtharrow M^+ Cl^-` .
`therefore K_sp = 1/K_c = 1/10^10 = 10^-10`.
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