For the calomel half-cell, `Hg, Hg_(2)Cl_(2)|Cl^(-)(aq)` values of electrode potentials are plotted at different log `[Cl^(-)]`. Variation is represented by

Options

A.
B.
C.
D.

Answer

D

Explanation

Half-cell reaction is :
`2Hg(l)+2Cl^(-)(aq)rarr Hg_(2)Cl_(2)(s)+2e^(-)`
`therefore K (1)/([Cl^(-)]^(2))`
`E=E^(@)-(0.0591)/(2)"log"(1)/([Cl^(-)]^(2))`
`E=E^(@)+0.0591 log [Al^(-)]`
Thus, E increase as `[Cl^(-)]` increases.