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?

Consider the cell Ag| AgBr Br^(-) ||CI|AgCl Ag at 25^(@) C the solubility product of AgCl and AgBr are 1xx10^(@) and 5xx10^(-13) respectively. At which ratio of concentration of Br and Clions would the emf of cell be zero?

Consider the cell AG|AgBr(s)|Br^(-)||AgCI(s)|CI^(-)|Ag at 25^(@)C . The solubility product constants of AgBr & AgCI are respectively 5 xx 10^(-13) & 1 xx 10^(-10) . For what ratio of the concentration of Br^(-) & CI^(-) ions would the emf of the cell be zero?

Consider the cell AG|AgBr(s)|Br^(-)||AgCI(s)|CI^(-)|Ag at 25^(@)C . The solubility product constants of AgBr & AgCI are respectively 5 xx 10^(-13) & 1 xx 10^(-10) . For what ratio of the concentration of Br^(-) & CI^(-) ions would the emf of the cell be zero?

Consider the cell AG|AgBr(s)|Br^(-)||AgCI(s)|CI^(-)|Ag at 25^(@)C . The solubility product constants of AgBr & AgCI are respectively 5 xx 10^(-13) & 1 xx 10^(-10) . For what ratio of the concentration of Br^(-) & CI^(-) ions would the emf of the cell be zero?

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

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