Seema Saini Solutions for Chapter: Ionic Equilibrium, Exercise 4: DPP 7.4

The solubility of ${\mathrm{CaF}}_{2 }\left({\mathrm{K}}_{\mathrm{sp}}=3.4\times {10}^{-11}\right)$ in $0.1 \mathrm{M}$ solution of $\mathrm{NaF}$ would be

When equal volumes of the following solutions are mixed precipitation of $AgCl\left({\mathrm{K}}_{\mathrm{sp}}^{\mathrm{o}}=1.8\times {10}^{-10}\right)$ will occur only with

If ${\mathrm{s}}_0,{\mathrm{s}}_1,{\mathrm{s}}_2$ and ${\mathrm{s}}_3$ are the solubilities of $\mathrm{AgCl}$ in water $0.01 \mathrm{M} {\mathrm{CaCl}}_2.0.01 \mathrm{M} \mathrm{NaCl}$ and $0.05 \mathrm{M} {\mathrm{AgNO}}_3$ solutions respectively, then:

Equal volumes of $0.2 \mathrm{M} {\mathrm{AgNO}}_3$ and $0.1 \mathrm{M} \mathrm{NaCl}$ solutions are mixed at $25°\mathrm{C}$. If ${\mathrm{K}}_{\mathrm{sp}}\left(\mathrm{AgCl}\right)=1.8\times {10}^{-10}{\mathrm{M}}^2$,  what will be the concentration of ${\mathrm{Cl}}^{-}$ ions in the solution?

The solubility product of ${\mathrm{BaCrO}}_4$ is $2.4\times {10}^{-10}{\mathrm{M}}^2$. The maximum concentration of $\mathrm{Ba}{\left({\mathrm{NO}}_3\right)}_2$ possible without precipitation in a $6\times {10}^{-4}\mathrm{M} {\mathrm{K}}_2{\mathrm{CrO}}_4$ solution is

What is the solubility of $\mathrm{Al}(\mathrm{OH}{)}_3,\left({\mathrm{K}}_{\mathrm{sp}}=1\times {10}^{-33}\right)$ in a buffer solution $\mathrm{pH}=4$?

Arrange in increasing order of solubility of $\mathrm{AgBr}$ in the given solutions.

$\text{ (i) }0.1 \mathrm{M} {\mathrm{NH}}_3$

$\text{ (ii) }0.1 \mathrm{M} {\mathrm{AgNO}}_3$

$\left(\mathrm{iii}\right) 0.2 \mathrm{M} \mathrm{NaBr}$

$\left(\mathrm{iv}\right)$ Pure water

If $\mathrm{pH}$ of saturated solution of $\mathrm{Ba}(\mathrm{OH}{)}_2$ is $12$, the value of ${\mathrm{K}}_{\mathrm{sp}}$ is not: