The $pH$ at which $Mg(OH)_2$ $[K_{sp} = 1 \times 10^{-11}]$ begins to precipitate from a solution containing $0.10 \ M$ $Mg^{2+}$ ions is . . . . . .

$A$ $1.0 \ L$ of aqueous solution contains $1 \times 10^{-8} \ M \ NaBr$,$1 \times 10^{-8} \ M \ NaCl$ and $1 \times 10^{-8} \ M \ NaI$. To this solution,$1 \times 10^{-10} \ M$ aqueous $AgNO_3$ solution is added dropwise. The order of precipitation of $AgX$ $(X = Cl, Br, I)$ is:
$(K_{sp}(AgCl) = 1.8 \times 10^{-10}; K_{sp}(AgBr) = 5 \times 10^{-13}; K_{sp}(AgI) = 8.3 \times 10^{-17})$

The solubility product of $AgCl$ is $1.44 \times 10^{-4}$ at $100\,^{\circ}C$. The solubility of silver chloride in boiling water may be

Which of the following equations represents the relation between solubility and solubility product for salt $BA_3$?

The volume of the water needed to dissolve $1 \ g$ of $BaSO_4$ $(K_{sp} = 1.1 \times 10^{-10})$ at $25 \ ^oC$ is ..... $litre$.

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