$A$ weak base is $5 \%$ dissociated in its $0.01 \ M$ solution. Calculate the dissociation constant.

What is the $pH$ of $0.001 \,M$ aniline solution? The ionization constant of aniline can be taken from the table. Calculate the degree of ionization of aniline in the solution. Also,calculate the ionization constant of the conjugate acid of aniline.

Base	$K_{b}$
Dimethylamine,$(CH_{3})_{2}NH$	$5.4 \times 10^{-4}$
Triethylamine,$(C_{2}H_{5})_{3}N$	$6.45 \times 10^{-5}$
Ammonia,$NH_{3}$	$1.77 \times 10^{-5}$
Quinine	$1.10 \times 10^{-6}$
Pyridine,$C_{5}H_{5}N$	$1.77 \times 10^{-9}$
Aniline,$C_{6}H_{5}NH_{2}$	$4.27 \times 10^{-10}$
Urea,$CO(NH_{2})_{2}$	$1.3 \times 10^{-14}$

The $pH$ of a $0.1 \ M$ solution of the acid $HA$ is $3$. The value of the ionization constant,$K_a$ of this acid is

$HClO$ is a weak acid. The concentration of ${H^+}$ ions in $0.1 \ M$ solution of $HClO$ $(K_a = 5 \times 10^{-8})$ will be equal to:

Calculate the dissociation constant of a weak monobasic acid if it is $0.05 \%$ dissociated in a $0.02 \ M$ solution.

The $pH$ of a $0.1 \ M$ solution of a weak monoprotic acid that is $1\%$ ionized is: