The $K_{sp}$ of $Ag_2CrO_4$ is $1.1 \times 10^{-12}$ at $298 \ K$. The solubility (in $mol/L$) of $Ag_2CrO_4$ in a $0.1 \ M \ AgNO_3$ solution is

Select the ion exchange reaction,which proceeds in the forward direction in an aqueous medium.

Which of the following pairs of ions,when their solutions are mixed,will result in precipitation?

$A$ solution is $0.1 \ M$ in $Cl^{-}$ and $0.001 \ M$ in $CrO_{4}^{2-}$. Solid $AgNO_{3}$ is gradually added to it. Assuming that the addition does not change in volume and $K_{sp}(AgCl) = 1.7 \times 10^{-10} \ M^{2}$ and $K_{sp}(Ag_{2}CrO_{4}) = 1.9 \times 10^{-12} \ M^{3}$. Select the correct statement from the following:

Assertion : Addition of silver ions to a mixture of aqueous sodium chloride and sodium bromide solution will first precipitate $AgBr$ rather than $AgCl$.
Reason : $K_{sp}$ of $AgCl < K_{sp}$ of $AgBr$.

The solubility product of $PbCl_2$ at $298 \ K$ is $1 \times 10^{-6}$. Its solubility in $mol/L$ is: