At `25^(@)`, the solubility product values of AgCl and AgCNS are `1.8xx10^(-10)` and `1.6xx10^(-11)` respectively. When a solution is saturated with both solids, calculate the ratio `([Cl^(-)])/([CNS^(-)])` and also `[Ag^(+)]` in the solution.

The solubility product constant of Ag_(2)CrO_(4) and AgBr are 1.1xx10^(-12) and 5.0xx10^(-13) respectively. Calculate the ratio of the molarities of their saturated solutions.

The solubility product constant of Ag_(2)CrO_(4) and AgBr are 1.1xx10^(-12) and 5.0xx10^(-13) respectively. Calculate the ratio of the molarities of their saturated solutions.

The solubility product constant of Ag_(2)CrO_(4) and AgBr are 1.1xx10^(-12) and 5.0xx10^(-13) respectively. Calculate the ratio of the molarities of their saturated solutions.

The solubility product constant of Ag_(2)CrO_(4) and AgBr are 1.1xx10^(-12) and 5.0xx10^(-13) respectively. Calculate the ratio of the molarities of their saturated solutions.

Solubility products of Ag_2 CrO_4 and AgCl are 9 xx 10^(-12) and 1 xx 10^(-10) respectively at 298. Concentration of Ag^(+) is more in the saturated solution of which salt?

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?

The solubility product of AgCl is 1.8xx10^(-10) at 18^(@)C . The solubility of AgCl in 0.1 M solution of sodium chloride would be