Which of the following formulas can be used to calculate the solubility of $Ag_2CO_3$?

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 $PbCl_2 = 1.7 \times 10^{-5}$)

What mass of $AgI$ will dissolve in $1.0 \ L$ of its saturated solution? [Given $: K_{sp}(AgI) = 1.0 \times 10^{-16} ; (At. \ wt. \ Ag = 108; I = 127)$]

The sulphide ion concentration $[S^{2-}]$ in a saturated $H_2S$ solution is $1 \times 10^{-22} \ M$. Which of the following sulphides should be quantitatively precipitated by $H_2S$ in the presence of dilute $HCl$?

Product	Sulphide Solubility $(K_{sp})$
$I$	$1.74 \times 10^{-16}$
$II$	$1.2 \times 10^{-22}$
$III$	$8.2 \times 10^{-46}$
$IV$	$5.0 \times 10^{-34}$

Which of the following has the maximum solubility? ($K_{sp}$ values are given in parentheses.)

Assign $A$,$B$,$C$,$D$ from the given type of reaction.
$AgCl \downarrow + 2KCN \longrightarrow K[Ag(CN)_2] + KCl$