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?

The solubility products of AgCl and Ag_2CrO_4 are 1.5 xx 10^(-10) and 9 xx 10^(-12) respectively. Which of the following statement is correct ?

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?

Calculate the simultaneous solubility of AgSCN and AgBr. K_(sp) for AgSCN and AgBr are 1 xx 10 ^(-12) and 5 xx 10 ^(-13) respectively.

The solubility product of Ag_2CrO_4 is 1.9xx10^(-12) at 300 K. What is its solubility ?

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?