The solubility product constant ${K_{sp}} $ of $Mg{(OH)_2}$ is $9.0 \times {10^{ – 12}}.$ If a solution is $0.010\,\,M$ with respect to $M{g^{2 + }}$ ion, what is the maximum hydroxide ion concentration which could be present without causing the precipitation of $Mg\,{(OH)_2}$

The solubility product of $PbC{l_2}$ at ${20\,^o}C$ is $1.5 \times {10^{ – 4}}.$ Calculate the solubility

Assertion : $KOH$ is more soluble in water than $NaOH$.
Reason : $NaOH$ is a stronger base than $KOH.$

The solubility of $[Ag^+]$ and $[Cl^-]$ solution is $1.43\times 10^{-3}\,gL^{-1}$ then what is the value of $K_{sp}$ at $25\,^oC$ of $AgCl$ .

If this is passed in solution of $0.1$ $M$ $Zn^{2+}$ and $0.01$ $M$ $Cu^{+}$ and concentration of ${S^{2 – }}$ made $8.1 \times {10^{ – 31}}$ $M$. Precipitation of $ZnS$ and $CuS$ will take place ? ${K_{sp}}$ of $\left( {ZnS} \right) = 3.0 \times {10^{ – 23}}$ and ${K_{sp}}$ of $\left( {CuS} \right) = 8.0 \times {10^{ – 34}}$