The solubility of $BaS{O_4}$ in water is $2.33 \times {10^{ – 3}}\,gm/litre.$ Its solubility product will be (molecular weight of $BaS{O_4} = 233)$

A salt $MX$ has $K_{sp}$ = $4 × 10^{-10}$ . What value of $K_{sp}$ must another salt $MX_3$ have if the molar solubility of the two salts is to be identical

Solid $Ba(NO_3)_2$ is gradually dissolved in $1.0 \times 10^{-4} \,M \,Na_2CO_3$  solution. At which concentration of $Ba^{2+}$ the precipition will begin? ( $K_{sp}$ $BaCO_3 = 5.1 \times 10^{-9}$)

The concentration of $KI $ and $KCl$  in certain solution containing both is $0.001\,M $ each. If $20 \,ml$  of this solution is added to $20 \,ml $ of a saturated solution of $AgI $ in water? What will happen

A mixture of $100\, m\, mol$ of $Ca(OH)_2$ and $2\, g$ of sodium sulphate was dissolved in water and the volume was made upto $100\, mL$. The mass of calcium sulphate formed and the concentration of $OH^-$ in resulting solution, respectively are 

(Molar mass of $Ca(OH)_2, Na_2SO_4$ and $CaSO_4$ are $74, 143$ and $136\, g\, mol^{-1}$ respectively; $K_{sp}$ of $Ca(OH)_2$ is $5.5 \times 10^{-6}$)