The solubility of salt $BA_2$ is $4 \times 10^{-4} \ mol \ dm^{-3}$. What is the solubility product of the salt?

Arrange the following in increasing order of solubility product $(K_{sp})$: $Ca(OH)_2, AgBr, PbS, HgS$

How many grams of $CaC_2O_4$ (molecular weight $= 128$) on dissolving in $1 \ L$ of distilled water will give a saturated solution? $[K_{sp}(CaC_2O_4) = 2.5 \times 10^{-9} \ mol^2 L^{-2}]$

An aqueous solution contains $SCN^{-}$,$Br^{-}$,$I^{-}$,and $Cl^{-}$ ions. When $AgNO_3$ is added to the solution,which of these will precipitate first? Given: $K_{sp}(AgCl) = 1.2 \times 10^{-10}$,$K_{sp}(AgI) = 1.7 \times 10^{-16}$,$K_{sp}(AgSCN) = 7.1 \times 10^{-7}$,$K_{sp}(AgBr) = 3.5 \times 10^{-13}$.

$A_{3}B_{2}$ is a sparingly soluble salt of molar mass $M \ g \ mol^{-1}$ and solubility $x \ g \ L^{-1}$. The solubility product satisfies $K_{sp} = a(\frac{x}{M})^{5}$. The value of $a$ is ...... . (Integer answer)

The $K_{sp}$ of $CaF_2$ is $1.7 \times 10^{-10}$. What is the volume in $mL$ of a saturated solution containing $10 \ mg$ of $CaF_2$? (Molecular mass of $Ca = 40, F = 19$).