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

Consider the cell `Ag|AgBr(s)Br^(-)||AgCl(s)Cl^(-)|Ag` at 298 K the solubility product of AgCl and AgBr are `1xx10^(-10)` and `5xx10^(-13)` respectively. What should be the ratio of concentration of `Br^(-)` and `Cl^(-)` by which emf of the cell becomes zero?

A

150/1

B

1/150

C

1/180

D

1/200

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