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

Consider the cell Ag(s)[AgBr(s)|`Br^(-)(aq)`||AgCl(s)| Ag(s) at `25^(@)C`.The solubility product constants of AgBr & AgCl are `5xx10^(-13)` & `1xx10^(-10)` respectively.For what ratio of the concentrations of `Br^(-)` & `Cl^(-)` ions would the emf of the cell be zero ?

A

As `E_(Ag^(+)//Ag)^(@)` is not given so `E_("cell")` cannot be determined

B

`E_("cell")` is `0.0413` volt

C

`/_\Glt0`

D

`E^(@)=0`

Text Solution

Verified by Experts

The correct Answer is:
B, C
`E_(cl^(-)//AgCl//Ag)^(@)=E_(Ag^(+)//Ag)^(@)+(RT)/F IN K_(sp)`………..(i)
`E_(Br^(-))^(@)//AgBr//Ag=E_(Ag^(+)//Ag)^(@)+(RT)/F In K_(sp)`…..(ii)
as `E_(Ag^(+)//Ag)^(@)` will be cancelled onn subtractions (i) & (ii)
So `E_("cell")` can be determined
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