Hydrolysis of Salts and pH of their Solutions

The $\mathrm{pH}$ of $1\times {10}^{-3} \mathrm{M} {\mathrm{H}}_2{\mathrm{O}}_2$ solution $\left({\mathrm{K}}_{\mathrm{a}}=2.2\times {10}^{-12}\right)$ is:

Calculate the $\mathrm{pH}$ of $0.1 \mathrm{M}$ solution of sodium acetate $\left({\mathrm{K}}_{\mathrm{a}}=1.0\times {10}^{-5}\right)$.

(Assume degree of hydrolysis <<<1)

The $\mathrm{pH}$ of a $0.1 \mathrm{M}$ solution of ${\mathrm{NH}}_4\mathrm{Cl}$ is $5.13$ and if the dissociation constant of ${\mathrm{NH}}_4\mathrm{OH}$ is $\mathrm{A} \mathrm{X} {10}^{-5}$, Report the value of $\mathrm{A}$ in the nearest integer.

Which of the following salts will give a basic solution on hydrolysis? 

Which of the following salts with a concentration $0.1\mathrm{M}$ will give a basic solution?

An aqueous solution of ammonium carbonate is

A weak acid is titrated with a weak base. Consider the following statements regarding the $\mathrm{pH}$ of the solution at the equivalence point:
(i) $\mathrm{pH}$ depends on the concentration of acid and base.
(ii) $\mathrm{pH}$ is independent of the concentration of acid and base
(iii) $\mathrm{pH}$ depends on the ${\mathrm{pK}}_{\mathrm{a}}$ of acid and ${\mathrm{pK}}_{\mathrm{b}}$ of base.
(iv) $\mathrm{pH}$ is independent of the ${\mathrm{pK}}_{\mathrm{a}}$ of acid and ${\mathrm{pK}}_{\mathrm{b}}$ of base.
The correct statements are:-

Solution A and B contains respectively $1$ and $2$ moles of ${\mathrm{CH}}_3{\mathrm{COONH}}_4$ in one litre. Then hydrolysis will be;

If the ${\mathrm{pK}}_{\mathrm{a}}$ of acetic acid and ${\mathrm{pK}}_{\mathrm{b}}$ of dimethylamine are $4.76$ and $3.26$ respectively, the $\mathrm{pH}$ of dimethyl ammonium acetate solution is

Which among the following produces a basic aqueous solution?

$2.5 \mathrm{mL}$ 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  $25°\mathrm{C}$.  The concentration of $\left[{\mathrm{H}}^{+}\right]$ at equivalence point is $({\mathrm{K}}_{\mathrm{w}} =1\times {10}^{-14}$ at ${25}^{\circ }\mathrm{C})$.

The degree of hydrolysis is dependent on concentration for:

What will be the degree of hydrolysis of 0.1 M solution of NaX? When a weak acid HX forms a salt NaX on reacting with NaOH and the dissociation constant of HX is 10^-5

Out of which of the following salt , the degree of hydrolysis is independent of the concentration of salt solution - 

If the blood contains ${\mathrm{C}\mathrm{O}}_2$ and ${\mathrm{H}\mathrm{C}\mathrm{O}}_3^{-}$, what is the ratio of conjugate base $\left(HC{O_3}^{-}\right)$ to acid $\left({\mathrm{H}}_2{\mathrm{C}\mathrm{O}}_3\right)$ to maintain the $\mathrm{p}\mathrm{H}$ of the blood equal to 7.4 ?

[Given: $\mathrm{p}{\mathrm{K}}_{{\mathrm{a}}_1\mathrm{ }}$of ${\mathrm{H}}_2{\mathrm{C}\mathrm{O}}_3=\mathrm{6.4]}$

Which of the following pair cannot exist together in solution?

Among the following ions, the ion(s) responsible for the acidic nature of potash alum, due to hydrolysis is/are:

How to calculate the $\mathrm{pH}$ of aqueous solution of Borax?

What will happen to the $\mathrm{pH}$ of $\frac{\mathrm{M}}{10}$ ${\mathrm{NH}}_4\mathrm{CN}$ solution on dilution?