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

The solubility products of $NiS$,$ZnS$,$CdS$,and $HgS$ are $4.7 \times 10^{-5}$,$1.6 \times 10^{-24}$,$8 \times 10^{-27}$,and $4 \times 10^{-53}$ respectively. An aqueous solution contains $Ni^{2+}$,$Zn^{2+}$,$Cd^{2+}$,and $Hg^{2+}$ of equal concentration. $H_2S$ gas was passed into this solution very slowly. The first and the last ions that precipitate as sulphides are respectively.

$A$ white powder soluble in $NH_4OH$ but insoluble in water is:

Which of the following substances is insoluble in acetic acid?

The solubility product of a salt having the general formula $MX_2$ in water is $4 \times 10^{-12}$. What is the concentration of $M^{2+}$ ions in the saturated aqueous solution of the salt?

The $K_{sp}$ values of $Ag_2CrO_4, AgCl, AgBr,$ and $AgI$ are $1.1 \times 10^{-12}, 1.8 \times 10^{-10}, 5.0 \times 10^{-13},$ and $8.3 \times 10^{-17}$ respectively. If $AgNO_3$ solution is added to a solution containing equal moles of $NaCl, NaBr, NaI,$ and $Na_2CrO_4$,which will precipitate last?