If the solubility of $PbBr_2$ is $S \, mol/L$,and it undergoes $100\%$ ionization,then the solubility product constant $(K_{sp})$ is equal to:

Which of the following provides the best explanation for the solubility of $MnS$ in dilute $HCl$?

Assign $A$,$B$,$C$,$D$ from the given type of reaction.
$BaC_2O_4 \downarrow + 2AcOH \longrightarrow Ba(AcO)_2 + H_2C_2O_4$

When $150 \ mL$ of $0.0008 \ M$ ammonium sulfate solution is mixed with $50 \ mL$ of $0.04 \ M$ calcium nitrate solution,given $K_{sp} = 2.4 \times 10^{-5}$ for $CaSO_4$,what is the ionic product of $CaSO_4$?

For a sparingly soluble strong electrolyte $AgIO_3$ (molar mass = $283 \, g/mol$),the equilibrium in a saturated solution is given by $AgIO_3(s) \rightleftharpoons Ag^+(aq) + IO_3^-(aq)$. If the solubility product constant $K_{sp}$ of $AgIO_3$ at a given temperature is $1.0 \times 10^{-8}$,how many grams of $AgIO_3$ are contained in $100 \, mL$ of its saturated solution?

The $pH$ at which $Mg(OH)_2$ $[K_{sp} = 1 \times 10^{-11}]$ begins to precipitate from a solution containing $0.10 \ M$ $Mg^{2+}$ ions is . . . . . .