In an aqueous solution,$SCN^-$,$Br^-$,$I^-$,and $Cl^-$ are present. Which will get precipitated first when $AgNO_3$ is added to the solution? Given that:
$K_{sp}(AgCl) = 1.2 \times 10^{-10}$,
$K_{sp}(AgI) = 1.7 \times 10^{-16}$,
$K_{sp}(AgSCN) = 7.1 \times 10^{-7}$,
$K_{sp}(AgBr) = 3.5 \times 10^{-13}$

If the solubility of lithium sodium hexafluoroaluminate $Li_3Na_3(AlF_6)_2$ is $S \ mol/L$,then its solubility product $K_{sp}$ is equal to?

The solubility product of a sparingly soluble salt $AB$ at room temperature is $1.21 \times 10^{-6}$. Its molar solubility is

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

Solubility products $(K_{sp})$ of the salts of types $MX, MX_2$ and $M_3X$ at temperature $T$ are $4.0 \times 10^{-8}, 3.2 \times 10^{-14}$ and $2.7 \times 10^{-15}$ respectively. Solubilities (in $mol \text{ dm}^{-3}$) of the salts at temperature $T$ are in the order:

Consider two Group $IV$ metal ions $X^{2+}$ and $Y^{2+}$. $A$ solution containing $0.01 \ M$ $X^{2+}$ and $0.01 \ M$ $Y^{2+}$ is saturated with $H_2S$. The pH at which the metal sulphide $YS$ will form as a precipitate is . . . . . . (Nearest integer). (Given: $K_{sp}(XS)=1 \times 10^{-22}$ at $25^{\circ} C$,$K_{sp}(YS)=4 \times 10^{-16}$ at $25^{\circ} C$,$[H_2S]=0.1 \ M$ in solution,$K_{a1} \times K_{a2}(H_2S)=1.0 \times 10^{-21}$,$\log 2=0.30, \log 3=0.48, \log 5=0.70$)