The solubility product of a sparingly soluble salt AX$_2$ is 4 x 10$^{-12}$. If the concentration of A$^{2+}$ ions in a saturated solution is 2 x 10$^{-4}$ M, the concentration of X$^-$ ions is:

The value of the ionic product of water depends

If the salts ${M_2}X,\;Q{Y_2}$ and $P{Z_3}$ have the same solubilities, ${K_{sp}}$ values are related as:

For a salt $A_2B$, the expression for the solubility product ($K_{sp}$) is:

The expression for the solubility product of ${\rm{A}}{{\rm{g}}_2}{\rm{C}}{{\rm{O}}_3}$ will be

The solubility of $\rm{Ag_2CrO_4}$ in water is $1.32 imes 10^{-4} \, mol \, L^{-1}$ at $\rm{298 \, K}$. What is the value of its solubility product (Ksp)?

The solubility of ${\rm{AgCl}}\left( {{K_{sp}} = 1.2 imes {{10}^{ - 10}}} \right)$ in a $0.10\;M\,{\rm{NaCl}}$ solution is:

Solubility of Agl in presence of 0.2 M Nal solution will be $\left( {{K_{sp}}\,of\,Agl = 8.3 imes {{10}^{ - 17}}} \right)$

The metallic sulphide not precipitated if ${{\rm{H}}_2}{\rm{S}}$ gas is passed through an aqueous solution containing cuprous chloride, bismuth chloride, mercuric chloride and sodium chloride is:

The volume of water needed to dissolve $1\,{\rm{g}}$ of ${\rm{BaS}}{{\rm{O}}_4}\left( {{K_{sp}} = 1.1 imes {{10}^{ - 10}}} \right)$ at 25\,^\circ C is:

A litre of solution is saturated with ${\rm{AgCl}}$. To this solution if $1.0 imes {10^{ - 4}}$ mole of solid ${\rm{NaCl}}$ is added, what will be the $\left[ {{\rm{A}}{{\rm{g}}^ + }} \right]$, assuming no volume change?