Equal volumes of 0.002 M solutions of A$_2$B and CB$_2$ salts are mixed. If the K$_{sp}$ of AB is 4 x 10$^{-8}$ and that of CB is 9 x 10$^{-8}$, which salt will precipitate first?

Two sparingly soluble salts, AB and CD, have K$_{sp}$ values of 4 x 10$^{-10}$ and 1 x 10$^{-12}$ respectively. Which salt is more soluble?

The expression for the solubility product of ${\rm{A}}{{\rm{l}}_2}{\left( {{\rm{S}}{{\rm{O}}_4}} \right)_3}$ is

The solubility of $AgBr(s)$ with solubility product $5.0 imes {10^{-13}}$ in $0.05\,M\,NaBr$ solution would be

The solubility product of ${\rm{PbC}}{{\rm{l}}_2}\;{\rm{is}}\;2.3 imes {10^{ - 32}}$ Its solubility will be

Solubility product constant [${K_{sp}}$] of salts of types $MX,M{X_2}\;{\rm{and}}\;{M_3}X$ at temperature $'T'$ are $4.0 imes {10^{ - 8}},3.2 imes {10^{ - 14}}\;{\rm{and}}\;2.7 imes {10^{ - 15}}$ respectively. Solubilities (${\rm{mol}},\;{\rm{d}}{{\rm{m}}^{ - 3}}$) of the salts at temperature ${T'}$ are in the order

If the solubility of ${\rm{Ca}}{\left( {{\rm{OH}}} \right)_2}$ is $\sqrt 3$. The solubility product of ${\rm{Ca}}{\left( {{\rm{OH}}} \right)_2}$ is:

The solubility in water of a sparingly soluble salt ${{\rm{A}}_2}{\rm{B}}$ is $1.0 imes {10^{ - 3}}{\rm{mol}}\;{{\rm{L}}^{ - 1}}$. Its solubility product will be

If ${K_{sp}}\;{\rm{of}}\;{\rm{ A}}{{\rm{g}}_2}{\rm{S }}\;{\rm{is}}\;{10^{ - 17}}$, the solubility of ${\rm{A}}{{\rm{g}}_2}{\rm{S}}\;in\;0.1\;M$ solution of ${\rm{N}}{{\rm{a}}_2}{\rm{S}}$ will be

${K_{sp}}$ of ${\rm{AgCl}}$ at ${\rm{18}}^\circ {\rm{C}}$ is $1.8 imes {10^{ - 10}}$. If ${\rm{A}}{{\rm{g}}^ + }$ of sodium is $4 imes {10^{ - 3}}{\rm{mol}}/{\rm{litre}}$ the ${{\rm{C}}{{\rm{l}}^ - }}$ that must exceed before ${\rm{AgCl}}$ is precipitated would be:

In a saturated solution of the sparingly soluble strong electrolyte ${\rm{AgI}}{{\rm{O}}_3}$ (molecular mass=283) the equilibrium which sets in is

${\rm{AgI}}{{\rm{O}}_3}\left( s \right)\;\leftrightharpoons\;{\rm{A}}{{\rm{g}}^ + }\left( {aq} \right) + {\rm{IO}}_3^ - \left( {aq} \right)$

If the solubility product constant ${K_{sp}}\;{\rm{of }}\;{\rm{AgI}}{{\rm{O}}_3}\;{\rm{at}}\;{\rm{ a}}\;{\rm{ given}}\;{\rm{ temprature }}\;{\rm{is}}\;1.0 imes {10^{ - 8}}$, what is the mass of ${\rm{AgI}}{{\rm{O}}_3}$ contained in $100\;mL$ of its saturated solution?