Consider the cell: Ag( {s}) \/ AgBr( {s}) \/ {Br}^{-}( {aq}) \| {Cl}^{-}( {aq}) \/ {AgCl}( {s}) \/ {Ag}( {s}) at 298 {K}. The solubility product of AgBr and {AgCl} are 8 \times 10^{-13} and 10^{-10} respectively. For what ratio of the concentrations of Br- and Cl ions would the emf of the cell be zero?

JEE Advanced 2020 Full Test 1 Paper 2

Question : 22 of 54

Marks: +1, -0

Consider the cell: Ag(s)∕AgBr(s)∕Br−(aq)|Cl−(aq)∕AgCl(s)∕Ag(s) at 298K. The solubility product of AgBr and AgCl are 8×10−13 and 10−10 respectively. For what ratio of the concentrations of Br- and Cl ions would the emf of the cell be zero?

7×10−3
8×10−3
8×10−3
None of these

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