The solubility product of a sulphide $MS$ is $3 \times 10^{-25}$ and that of another sulphide $NS$ is $4 \times 10^{-40}$. In an ammoniacal solution,which of the following occurs?

The solubility of $AgCl$ at $20\,^oC$ is $1.435 \times 10^{-3} \, g/L$. The solubility product of $AgCl$ is .......

What is the molarity of $F^{-}$ in a saturated solution of $InF_3$? $(K_{sp} = 7.9 \times 10^{-10})$

The solubility product constants $(K_{sp})$ of $CuS$,$Ag_2S$,and $HgS$ are $10^{-37}$,$10^{-44}$,and $10^{-54}$ respectively. The order of their solubility is:

Calculate the minimum concentration of sulphate ion required to precipitate $BaSO_4$ in a solution containing $10^{-4} \ mol/L$ of $Ba^{2+}$. $(K_{sp} \ BaSO_4 = 4 \times 10^{-10})$

$A$ $1.0 \ L$ of aqueous solution contains $1 \times 10^{-8} \ M \ NaBr$,$1 \times 10^{-8} \ M \ NaCl$ and $1 \times 10^{-8} \ M \ NaI$. To this solution,$1 \times 10^{-10} \ M$ aqueous $AgNO_3$ solution is added dropwise. The order of precipitation of $AgX$ $(X = Cl, Br, I)$ is:
$(K_{sp}(AgCl) = 1.8 \times 10^{-10}; K_{sp}(AgBr) = 5 \times 10^{-13}; K_{sp}(AgI) = 8.3 \times 10^{-17})$