Define ${\mathrm{P}}^{\mathrm{H}}$ ? What is buffer solution? Derive Henderson- Hasselbalch equation for calculating the ${\mathrm{P}}^{\mathrm{H}}$ of an acidic buffer solution

Explain the term Hydrolysis of salts with examples. Discuss the ${\mathrm{P}}^{\mathrm{H}}$ of the following salt solution.

a) salt of weak acid and strong base

Explain the term Hydrolysis of salts with examples. Discuss the ${\mathrm{P}}^{\mathrm{H}}$ of the following salt solution.

a) salts of strong acid and weak base.

Nitrogen dioxide forms dinitrogen tetroxide according to the equation $2{\mathrm{NO}}_2\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{N}}_2{\mathrm{O}}_4\left(\mathrm{g}\right)$ When $0.1 \mathrm{mole} \mathrm{of} {\mathrm{NO}}_2$ is added to a $1$litre flask at ${25}^{\circ }\mathrm{C}$, the concentration changes so that at equilibrium $\left[{\mathrm{NO}}_2\right]=0.016\mathrm{M} \mathrm{and} \left[{\mathrm{N}}_2{\mathrm{O}}_4\right]=0.042\mathrm{M}$

a) What is the value of the reaction Quotient before any reaction occurs.

Nitrogen dioxide forms dinitrogen tetroxide according to the equation $2{\mathrm{NO}}_2\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{N}}_2{\mathrm{O}}_4\left(\mathrm{g}\right)$ When $0.1 \mathrm{mole} \mathrm{of} {\mathrm{NO}}_2$ is added to a $1$litre flask at ${25}^{\circ }\mathrm{C}$, the concentration changes so that at equilibrium $\left[{\mathrm{NO}}_2\right]=0.016\mathrm{M} \mathrm{and} \left[{\mathrm{N}}_2{\mathrm{O}}_4\right]=0.042\mathrm{M}$

b) What is the value of equilibrium constant for the reaction.