$K_{sp}$ for $AgBr$ at $25\,^oC$ is $4.9 × 10^{-13}$. How much $AgBr$ will dissolved in $20\  litres$ of its saturated solution if molecular weight of $AgBr =$  $188$

The solubility of salt of weak acid $MX$ (e.g. phosphoric) is increase at tower $pH$ explain with equation.

The solubility product of lead bromide is $8\times10^{-5}$. If the salt is $80\%$ dissociated in saturated solution, find the solubility of the salt

On decreasing the $p \mathrm{H}$ from $7$ to $2$ , the solubility of a sparingly soluble salt ($MX$) of a weak acid ($HX$) increased from $10^{-4} \mathrm{~mol} \mathrm{~L}^{-1}$ to $10^{-3} \mathrm{~mol} \mathrm{~L}^{-1}$. The $p \mathrm{~K}_{\mathrm{s}}$ of $\mathrm{HX}$ is:

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.