S C Kheterpal, S N Dhawan and, P N Kapil Solutions for Chapter: Ionic Equilibrium in Solution, Exercise 36: PROBLEMS FOR PRACTICE

The $\mathrm{pH}$ of $0.1 \mathrm{M}$ monobasic acid is $4.50$. Calculate the concentration of the species ${\mathrm{H}}^{+}, {\mathrm{A}}^{-}$ and $\mathrm{HA}$ at equilibrium. Also determine the value of ${\mathrm{K}}_{\mathrm{a}}$ and ${\mathrm{pK}}_{\mathrm{a}}$ of the monobasic acid.

Calculate the $\mathrm{pH}$ of $0.08 \mathrm{M}$ solution of hypochlorous acid, $\mathrm{HOCl}$. The ionization constant of the acid is $2.5\times {10}^{-5}$. Determine the percent dissociation of $\mathrm{HOCl}$.

The $\mathrm{pH}$ of $0.04 \mathrm{M}$ hydrazine solution is $9.7$. Calculate its ionization constant ${\mathrm{K}}_{\mathrm{b}}$ and ${\mathrm{pK}}_{\mathrm{b}}$.