Solubility of $BaF_2$ in a solution of $Ba(NO_3)_2$ will be represented by the concentration term:

If the solubility product $(K_{sp})$ of $Ni(OH)_2$ is $1.9 \times 10^{-15}$, the molar solubility of $Ni(OH)_2$ in $1.0 \ M \ NaOH$ is:

Which of the following reagents can dissolve the precipitate of $HgS\,\downarrow$?

What is the molarity of $F^{-}$ ions in a saturated solution of $BaF_2$? $(K_{sp} = 1.0 \times 10^{-6})$

The solubility product of $BaCl_2$ is $4 \times 10^{-9}$. Its solubility in moles/litre would be:

Solid $Ba(NO_3)_2$ is gradually dissolved in a $1.0 \times 10^{-4} \ M \ Na_2CO_3$ solution. At which concentration of $Ba^{2+}$,precipitate of $BaCO_3$ begins to form? ($K_{sp}$ for $BaCO_3 = 5.1 \times 10^{-9}$)