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Consider the cell Ag(s)|AgBr(s)|Br^(-)(a...

Consider the cell `Ag(s)|AgBr(s)|Br^(-)(aq)||AgCl(s)|Cl^(-)(aq)|Ag(s)` at `25^(@)C`. The solubility product constants of `AgBr` & `AgCl` are respectively `5xx10^(-13)&1xx10^(-10)` for what ratio of the concentrations of `Br^(-)` & `Cl^(-)` ionns would the emf of the cell be zero?
(A). `1:200`
(B). `1:100`
(C). `1:500`
(D). `200:1`

A

Cell cannot function as anode and cathode are of the same material

B

`E_("cell")=0.0591V`

C

`E_("cell")=0.80V`

D

`E_("cell")=0.0296V`

Text Solution

Verified by Experts

The correct Answer is:
B
It is a concentration cell
`E_("cell")=(0.0591)/(n)"log" (C_(2)(RHS))/(C_(1)(LHS))`
`=(0.0591)/(1)"log"(0.1)/(0.01)=0.0591V`
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