Salt Hydrolysis

$2.5 \mathrm{mL}$ of $\frac{2}{5}\mathrm{M}$ weak monoacidic base $({\mathrm{K}}_{\mathrm{b}}=1\times {10}^{-12}$ at ${25}^{\circ }\mathrm{C})$ is titrated with $\frac{2}{15}\mathrm{M} \mathrm{HCl}$ in water at  ${25}^{\circ }\mathrm{C}$. The concentration of $\left[{\mathrm{H}}^{+}\right]$ at equivalence point is $({\mathrm{K}}_{\mathrm{w}} =1\times {10}^{-14}$ at ${25}^{\circ }\mathrm{C})$.

Which of the following salt is the most basic in aqueous solution?

${\mathrm{pK}}_{\mathrm{a}}$ of weak acid $\left(\mathrm{HA}\right)$ and ${\mathrm{pK}}_{\mathrm{b}}$ of weak base $\left(\mathrm{BOH}\right)$ are $3.2$ and $3.4$ respectively. The $\mathrm{pH}$ of their salt $\left(\mathrm{AB}\right)$ solution is.

Which of an aqueous solution of the following salts will have the lowest $\mathrm{pH}$?

Which of the following salts will have the highest $\mathrm{pH}$ in water?

Equimolar solutions of the following were prepared in water separately. Which one of the solutions will record the highest $\mathrm{pH}$ ?

The ${\mathrm{pK}}_{\mathrm{a}}$ of an acid $\mathrm{HA}$ is $4.77$ and ${\mathrm{pK}}_{\mathrm{b}}$ of a base $\mathrm{BOH}$ is $4.75$. The $\mathrm{pH}$ of $0.1 \mathrm{M}$ aqueous solution of the salt $\mathrm{AB}$ is

A weak acid $\mathrm{HX}$ has the dissociation constant $1\times {10}^{-5 }\mathrm{M}$. It forms a salt $\mathrm{NaX}$ on reaction with alkali. The degree of hydrolysis of $0.1\mathrm{M}$ solution of $\mathrm{NaX}$ is  

The $\mathrm{pH}$ of $0.1 \mathrm{M}$ solution of the following salts increases in the order :