If the solubility of $MX_2$ in water is $0.0002 \ mol/L$,then its $K_{sp}$ is:

Zirconium phosphate $[Zr_3(PO_4)_4]$ dissociates into three zirconium cations of charge $+4$ and four phosphate anions of charge $-3$. If molar solubility of zirconium phosphate is denoted by $S$ and its solubility product by $K_{sp}$,then which of the following relationships between $S$ and $K_{sp}$ is correct?

Assign $A, B, C, D$ from the given type of reaction.
$CaC_2O_4 \downarrow + CH_3COOH \longrightarrow$ No reaction

If the concentration of $CrO_4^{2-}$ ions in a saturated solution of silver chromate is $2 \times 10^{-4} \ M$,the solubility product of silver chromate will be:

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

Up to what $pH$ must a solution containing a precipitate of $Cr(OH)_3$ be adjusted so that the precipitate just dissolves? (Given: $[Cr^{3+}] = 0.1 \ mol/L$,$K_{sp} = 6 \times 10^{-31}$)