The solubility product of $Mg(OH)_2$ is $1 \times 10^{-12}$. At what $pH$ will precipitation occur in a $0.01 \ M$ $MgCl_2$ solution?

If the solubility product of $BaSO_4$ is $1.44 \times 10^{-12}$,then the solubility of $SO_4^{2-}$ is .....

Why only $As^{3+}$ gets precipitated as $As_2S_3$ and not $Zn^{2+}$ as $ZnS$ when $H_2S$ is passed through an acidic solution containing $As^{3+}$ and $Zn^{2+}$?

$A$ precipitate of calcium oxalate will not dissolve in

Determine the solubilities of silver chromate,barium chromate,ferric hydroxide,lead chloride,and mercurous iodide at $298 \, K$ from their solubility product constants. Determine also the molarities of individual ions. (Given $K_{sp}$ values: $Ag_{2}CrO_{4} = 1.1 \times 10^{-12}$,$BaCrO_{4} = 1.2 \times 10^{-10}$,$Fe(OH)_{3} = 1.0 \times 10^{-38}$,$PbCl_{2} = 1.6 \times 10^{-5}$,$Hg_{2}I_{2} = 4.5 \times 10^{-29}$)

An excess of $Ag_{2}CrO_{4(s)}$ is added to a $5 \times 10^{-3} \ M$ $K_{2}CrO_{4}$ solution. The concentration of $Ag^{+}$ in the solution is closest to
[ Solubility product for $Ag_{2}CrO_{4} = 1.1 \times 10^{-12}$ ]