Calculate the pH of a centimolar solution of a monoacidic weak base which is $10 \%$ dissociated in its aqueous solution.

What is the molar concentration of a weak monobasic acid if its dissociation constant is $5 \times 10^{-8}$ and it undergoes $0.5 \%$ dissociation (in $M$)?

Derive the equation for the ionization constant $K_a$ of a weak acid $HX$.

For a weak base $BOH$ at $25\,^oC$,the dissociation constant $K_b$ is $1.0 \times 10^{-12}$. The concentration of hydroxyl ions in its $0.01\,M$ aqueous solution will be:

The $pH$ of $0.01 \ M$ solution of acetic acid is $5.0$. What are the values of $[H^{+}]$ and $K_a$ respectively?

The $pH$ of $0.004 \, M$ hydrazine solution is $9.7$. Calculate its ionization constant $K_{b}$ and $pK_{b}$.