Solubility Equilibria of Sparingly Soluble Salts

On decreasing the $\mathrm{pH}$ from $7$ to $2$, the solubility of a sparingly soluble salt $\left(\mathrm{MX}\right)$ of a weak acid $\left(\mathrm{HX}\right)$ increased from ${10}^{-4} \mathrm{mol} {\mathrm{L}}^{-1}$ to ${10}^{-3} \mathrm{mol} {\mathrm{L}}^{-1}$. The ${\mathrm{pK}}_{\mathrm{a}}$ of $\mathrm{HX}$ is

Select the correct statements regarding the following process.

The values of ${\mathrm{K}}_{\mathrm{sp}}$ of ${\mathrm{CaCO}}_3$ and ${\mathrm{CaC}}_2{\mathrm{O}}_4$ are $4.7\times {10}^{-9}$ and $1.3\times {10}^{-9}$ respectively at $25°\mathrm{C}$. If the mixture of these two is washed with water, what is the concentration of ${\mathrm{Ca}}^{2+}$ ions in water?

Calculate the oxalate concentration necessary to precipitate ${\mathrm{CaC}}_2{\mathrm{O}}_4$ in a saturated solution of calcium carbonate.

${\mathrm{K}}_{\mathrm{sp}}\left({\mathrm{CaC}}_2{\mathrm{O}}_4\right)=2.6\times {10}^{-9}; {\mathrm{K}}_{\mathrm{sp}}\left({\mathrm{CaCO}}_3\right)=8.7\times {10}^{-9}$

The lowering of vapour pressure in a saturated aq. solution of salt $\mathrm{A} \mathrm{B}$ is found to be $0.108$ torr. If vapour pressure of pure solvent at the same temperatuare is $300$ torr, find the solubility product of salt $\mathrm{AB}$:

The $\mathrm{p}\mathrm{H}$ at which $\mathrm{M}\mathrm{g}{\left(\mathrm{O}\mathrm{H}\right)}_2$ begins to precipitate from a solution containing $0.1\mathrm{M}\mathrm{ }\mathrm{M}{\mathrm{g}}^{2+}$ ion is ______.
$[{\mathrm{K}}_{\mathrm{s}\mathrm{p}}\mathrm{ }\mathrm{f}\mathrm{o}\mathrm{r}\mathrm{ }\mathrm{M}\mathrm{g}{\left(\mathrm{O}\mathrm{H}\right)}_2=1.0\times {10}^{-11}]$

Give the nearest integer as the answer.

Solubility products of $\mathrm{CuI}$ and ${\mathrm{Ag}}_2{\mathrm{CrO}}_4$ have almost the same value $\left(~4\times {10}^{-12}\right)$. The ratio of solubilities of the two salts $\left(\mathrm{CuI}:{\mathrm{Ag}}_2{\mathrm{CrO}}_4\right)$ is closest to 

The solubility of $\text{B}\text{a}\text{S}{\text{O}}_4$ in pure water (in $\text{g}{\text{L}}^{-1}$ ) is closest to
$\left[\right.$Given; ${\text{K}}_{\text{sp}}$ for $\text{B}\text{a}\text{S}{\text{O}}_4$ is $1.0\times {10}^{-10}$ at $25°\text{C}.$ Molecular weight of $\text{B}\text{a}\text{S}{\text{O}}_4$ is $233 \text{g} \text{m}\text{o}{\text{l}}^{-1}$ ]

If the solubility of a ${\mathrm{M}}_2\mathrm{S}$ salt is $3.6\times {10}^{-5}$, find its solubility product.

Name the process be which common salt is obtained from sea-water.

By which of the following processes can the common salt be purified?

Which acid is used in the purification of common salt?

A saturated solution of ${\mathrm{CaSO}}_4$ is prepared at $25°\mathrm{C}$. When $200 \mathrm{mL}$ of this solution is allowed to complete evaporation of water, $0.34 \mathrm{g}$ of residue obtained. The ${\mathrm{K}}_{\mathrm{sp}}$ of ${\mathrm{CaSO}}_4$ at $25°\mathrm{C}$ will be:

$\mathrm{pH}$ of a saturated solution of $\mathrm{Ba}{\left(\mathrm{OH}\right)}_2$ is $12$. Hence, ${\mathrm{K}}_{\mathrm{sp}}$ of $\mathrm{Ba}{\left(\mathrm{OH}\right)}_2$

Solubility of thorium phosphate (molar mass $=\mathrm{m}$) is $\mathrm{wg}/100 \mathrm{mL}$ at $25°\mathrm{C}$. The ${\mathrm{K}}_{\mathrm{sp}}$ of thorium phosphate is :

The ${\mathrm{K}}_{\mathrm{sp}}$ of ${\mathrm{Ag}}_2{\mathrm{CrO}}_4$ is $1.1\times {10}^{-12}$ at $298 \mathrm{K}$. The solubility (in $\mathrm{mol} {\mathrm{L}}^{-1}$) of ${\mathrm{Ag}}_2{\mathrm{CrO}}_4$ in a $0.1 \mathrm{M} {\mathrm{AgNO}}_3$ solution is :

The solubility of $\mathrm{AgCl}\left(\mathrm{s}\right)$ with solubility product $1.6\times {10}^{-10}$ in $0.1 \mathrm{M} \mathrm{NaCl}$ solution would be :

Calculate the molar solubility of $\mathrm{AgCl}$ at $25°\mathrm{C}$ in $3.0{\mathrm{MNH}}_3$

$\left({\mathrm{K}}_{\mathrm{sp}}\right.$ of $\mathrm{AgCl}=2.0\times {10}^{-10}, {\mathrm{K}}_{\mathrm{f}}$ of ${\left[\mathrm{Ag}{\left({\mathrm{NH}}_3\right)}_2\right]}^{+}=1.25\times {10}^7)$
 

If solubility of sparingly soluble compound $\mathrm{M}{\left(\mathrm{OH}\right)}_3$ in a solution of $\mathrm{pH}=12$ is $\mathrm{x}\times {10}^{-\left(\mathrm{y}\right)}$ then calculate $\mathrm{y}$. Solubility of $\mathrm{M}{\left(\mathrm{OH}\right)}_3$ in pure water is $2\times {10}^{-7}$.