If $K_{sp}$ is the solubility product of $Al(OH)_3$,its solubility is expressed by the formula:

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

The $K_{sp}$ of $M(OH)_2$ is $3.2 \times 10^{-11}$. The $pH$ of its saturated solution in water is:

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 solution?

Calculate the solubility of sparingly soluble salt $BA$ in $mol \ dm^{-3}$ at $300 \ K$ if its solubility product is $4.9 \times 10^{-9}$ at same temperature.

$A$ very dilute acidic solution of $Cd^{2+}$ and $Ni^{2+}$ gives only yellow precipitate of $CdS$ on passing $H_2S$ gas. This is due to: