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:

In qualitative analysis,the metals of group $I$ can be separated from other ions by precipitating them as chloride salts. $A$ solution initially contains $Ag^{+}$ and $Pb^{2+}$ at a concentration of $0.10 \, M$. Aqueous $HCl$ is added to this solution until the $Cl^{-}$ concentration is $0.10 \, M$. What will the concentrations of $Ag^{+}$ and $Pb^{2+}$ be at equilibrium? ($K_{sp}$ for $AgCl = 1.8 \times 10^{-10}$,$K_{sp}$ for $PbCl_2 = 1.7 \times 10^{-5}$)

The minimum volume of water required to dissolve $0.1 \ g$ of lead $(II)$ chloride to get a saturated solution ($K_{sp}$ of $PbCl_2 = 3.2 \times 10^{-8}$; atomic mass of $Pb = 207 \ u$,$Cl = 35.5 \ u$) is......$L$

In a saturated solution of the sparingly soluble strong electrolyte $AgIO_3$ (molecular mass $= 283$),the equilibrium which sets in is $AgIO_{3(s)} \rightleftharpoons Ag^+_{(aq)} + IO^-_{3(aq)}$. If the solubility product constant $K_{sp}$ of $AgIO_3$ at a given temperature is $1.0 \times 10^{-8}$,what is the mass of $AgIO_3$ contained in $100 \ mL$ of its saturated solution?

Which of the following precipitates does not dissolve even in a large excess of $NH_4OH$?

$A$ solution of $0.01 \ M$ $MgCl_2$ will form a precipitate of $Mg(OH)_2$ at a limiting $pH$ of: (Given: $K_{sp}$ of $Mg(OH)_2 = 1 \times 10^{-12}$)