The ${K_{sp}}$ of $Mg{\left( {OH} \right)_2}$, is $1.0 \times {10^{ – 12}}$. At which $pH$ the $0.01$ $M$ $Mg{\left( {OH} \right)_2}$ begins to precipitate ? Calculate solubility.

If $S$ and ${K_{sp}}$ are respectively solubility and solubility product of a sparingly soluble binary electrolyte, then

The ${K_{sp}}$ of $Ca{F_2}$ is $1.7 \times {10^{ – 10}}$. Then what is the volume in mililitre of saturated solution of $10$ miligram $Ca{F_2}$ ? ( Molecular mass of $Ca (40), F(19)$ ).

In a saturated solution of the sparingly soluble strong electrolyte $AgIO_3$ (molecular mass $= 283$) the equilibrium which sets in is

$AgIO_{3(s)} \rightleftharpoons  Ag^+_{(aq)} +IO^-_{3(aq)}.$ 

If the solubility product constant $K_{sp}$ of $AgIO_3$ at a given temperature is $1. 0 \times 10^{-8},$ what is the mass of $AgIO_3$ contained in $100\, ml$ of its saturated saolution ?

Which of the following would increase the solubility of $Pb(OH)_2$