S C Kheterpal, S N Dhawan and, P N Kapil Solutions for Chapter: Ionic Equilibrium in Solution, Exercise 25: PROBLEMS FOR PRACTICE

Calculate the degree of ionization and $\left[{\mathrm{H}}_3{\mathrm{O}}^{+}\right]$ of $0.01 \mathrm{M} {\mathrm{CH}}_3\mathrm{COOH}$ solution. The equilibrium constant of acetic acid is $1.8\times {10}^{-5}$.

A $0.01 \mathrm{M}$ solution of acetic acid is $1.34\%$ ionised (degree of dissociation$=0.0134$) at $298 \mathrm{K}$. What is the ionization constant of acetic acid?

What will be the percentage of dissociation in $1.0 \mathrm{M}$ ${\mathrm{CH}}_3\mathrm{COOH}$ at equilibrium having dissociation constant of $1.8\times {10}^{-5}$?

Nicotinic acid $({\mathrm{K}}_{\mathrm{a}}=1.4\times {10}^{-5})$ is represented by the formula $\mathrm{HNiC}$. Calculate its percentage dissociation in a solution which contains $0.10$ mole of nicotinic acid per $2.0$ litre of solution.

Calculate the concentration of ${\mathrm{H}}^{+}$ (aq) in $0·2 \mathrm{M}$ solution of $\mathrm{HCN}$. Given that the dissociation constant of $\mathrm{HCN}$ in water is $4.9\times {10}^{-10}$.