$A$ saturated solution of $Ag_2SO_4$ is $2.5 \times 10^{-2} \ M$. The value of its solubility product is:

The ionization constant of benzoic acid is $6.46 \times 10^{-5}$ and $K_{sp}$ for silver benzoate is $2.5 \times 10^{-13}$. How many times is silver benzoate more soluble in a buffer of $pH$ $3.19$ compared to its solubility in pure water?

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 of a sparingly soluble salt $AB_2$ is $18.78 \times 10^{-4} \text{ g/dm}^3$. What is its solubility product? (Molar mass of $AB_2 = 187.8 \text{ g mol}^{-1}$)

The concentration of $KI$ and $KCl$ in a solution containing both is $0.001 \ M$ each. If $20 \ mL$ of this solution is added to $20 \ mL$ of a saturated solution of $AgI$ in water,what will happen?

At $25\,^oC$,$K_{sp}$ for $PbBr_2$ is equal to $8 \times 10^{-5}$. If the salt is $80\%$ dissociated,what is the solubility of $PbBr_2$ in $mol/L$?