At $25^{\circ} C$,the solubility product of $MCl$ is $1 \times 10^{-10}$. What is its molar solubility in $0.1 \ M \ NaCl$ solution at the same temperature?

The solubility of $AgBr$ is $7.1 \times 10^{-7} \ mol \ dm^{-3}$. Calculate its solubility product at the same temperature.

$A$ solution is saturated with $SrCO_3$ and $SrF_2$. The $[CO_3^{2-}]$ is found to be $1.2 \times 10^{-3} \ M$. The concentration of $F^{-}$ in the solution would be:
Given: $K_{sp}(SrCO_3) = 7.0 \times 10^{-10}$, $K_{sp}(SrF_2) = 7.9 \times 10^{-10}$

The solubility products of $Al(OH)_3$ and $Zn(OH)_2$ are $8.5 \times 10^{-23}$ and $1.8 \times 10^{-14}$ at room temperature. If the solution contains $Al^{3+}$ and $Zn^{2+}$ ions,the ion first precipitated by adding $NH_4OH$ is

Solubility products of $CuI$ and $Ag_{2}CrO_{4}$ have almost the same value $(\sim 4 \times 10^{-12})$. The ratio of solubilities of the two salts $(CuI : Ag_{2}CrO_{4})$ is closest to $....$

If the solubility product of $AB_2$ is $4 \times 10^{-12}$,then its solubility is .......?