$A$ $0.1 \ M$ solution of $HF$ is $1 \%$ ionized. What is the $K_a$?

The hydrogen ion concentration in a weak acid of dissociation constant $K_a$ and concentration $c$ is nearly equal to:

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,$CO(NH_{2})_{2}$	$1.3 \times 10^{-14}$

What is the value of $pH$ of a $NaOH$ solution that dissociates $2 \%$ in its $0.01 \ M$ solution?

An organic monobasic acid has a dissociation constant of $2.25 \times 10^{-6}$. What is the percent dissociation in its $0.01 \ M$ solution (in $\%$)?

Find $pH$ of $5 \times 10^{-3} \ M$ $H_2CO_3$ solution having $10\%$ dissociation.