The ionization constant of dimethylamine is $5.4 \times 10^{-4}$. Calculate its degree of ionization in its $0.02$ $M$ solution. What percentage of dimethylamine is ionized if the solution is also $0.1 \,M$ in $NaOH ?$

The dissociation constant of an acid $HA$  is $1 \times {10^{ – 5}}$. The $pH$ of $0.1$ molar solution of the acid will be

Dimethyl amine ${\left( {C{H_3}} \right)_2}NH$ is weak base and its ionization constant $ 5.4 \times {10^{ – 5}}$. Calculate $\left[ {O{H^ – }} \right],\left[ {{H_3}O} \right]$, $pOH$ and $pH$ of its $0.2$ $M$ solution at equilibrium.

Values of dissociation constant, $K_a$ are given as follows

Correct order of increasing base strength of the base $CN^-,F^-$ and $NO_2^-$ will be

Which of the following will occur if a $0.1 \,M$  solution of a weak acid is diluted to $0.01\,M$ at constant temperature