The solubility of $CaCl_2$ is $1.11 \times 10^{-8} \ g/100 \ mL$. If the molar mass of $CaCl_2$ is $111 \ g/mol$,find the $K_{sp}$.

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

The solubility of a sparingly soluble salt $AX_2$ is $1 \times 10^{-4} \ mol \ dm^{-3}$ at $298 \ K$. Calculate its solubility product $(K_{sp})$?

Which one of the following arrangements represents the correct order of solubilities of sparingly soluble salts $Hg_2Cl_2$,$Cr_2(SO_4)_3$,$BaSO_4$ and $CrCl_3$ respectively?

When solid $Pb(NO_3)_2$ is added to $1 \, L$ of $H_2SO_4$ $(1 \times 10^{-3} \, M)$ to make the concentration of $Pb(NO_3)_2$ equal to $0.002 \, M$,what will happen? $(K_{sp} \text{ of } PbSO_4 = 1.3 \times 10^{-8})$

In a saturated solution of an electrolyte,the product of the concentrations of its ions is constant at a constant temperature. This constant for the electrolyte is known as: