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 $233 \text{g} \text{m}\text{o}{\text{l}}^{-1}$ ]

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?

What is the minimum mass of $\mathrm{NaBr}$ which should be added in $200 \mathrm{ml}$ of $0.0004\mathrm{M} {\mathrm{AgNO}}_3$ solution just to start the precipitation of $\mathrm{AgBr}$ ? The value of ${\mathrm{K}}_{\mathrm{sp}}$ of $\mathrm{AgBr}=4\times {10}^{-13}$ $\left(\mathrm{Br}=80\right)$

Salting out action of soap is based on:

Salting out relies on the principle that most proteins are less soluble in solutions of high salt concentrations.

Why is salting out necessary in soap production?

Calculate the molar solubility of $\mathrm{Ni}(\mathrm{OH}{)}_2$ in 0.10 M $\mathrm{NaOH}$. The ionic product of $\mathrm{Ni}(\mathrm{OH}{)}_2$ is $2.0\times {10}^{–15}$ .

Using Gibb’s free energy change,$∆{\mathrm{G}}^0 = 57.34 \mathrm{kJ} {\mathrm{mol}}^{-1}$, for the reaction ${\mathrm{X}}_2\mathrm{Y}\left(\mathrm{s}\right)\to 2{\mathrm{X}}^{+}\left(\mathrm{aq}\right) + {\mathrm{Y}}^{2-}\left(\mathrm{aq}\right)$. Calculate the solubility product of ${\mathrm{X}}_2\mathrm{Y}$ in water at $300\mathrm{K} \left(\mathrm{R}= 8.3 {\mathrm{JK}}^{-1 }{\mathrm{mol}}^{-1}\right)$.

The expression for the solubility product of ${\text{Ca}}_3{\left({\text{PO}}_4\right)}_2$ will be ${\text{K}}_{\mathrm{sp}}=$_____.

$\left(\mathrm{A}\right) {\left[{\mathrm{Ca}}^{2+}\right]}^2{\left[{\mathrm{PO}}_4^{3-}\right]}^2; \left(\mathrm{B}\right) {\left[{\mathrm{Ca}}^{2+}\right]}^3{\left[{\mathrm{PO}}_4^{3-}\right]}^2; \left(\mathrm{C}\right) {\left[{\mathrm{Ca}}^{2+}\right]}^2{\left[{\mathrm{PO}}_4^{3-}\right]}^3$

Enter your correct answer as A, B or C.

Find the solubility product in ${\mathrm{mol}}^5 {\mathrm{L}}^{-5}$ of ${\mathrm{Ca}}_3({\mathrm{PO}}_4{)}_2$, whose solubility in water is $\mathrm{X} \mathrm{mol} {\mathrm{L}}^{-1}$?