The ionization constant of $0.1$ $M$ weak acid is $1.74 \times {10^{ – 5}}$ at $298$ $K$ temperature. Calculate $pH$ of its $0.1$ $M$ solution.

The degree of ionization of a $0.1 \,M$ bromoacetic acid solution is $0.132$ Calculate the $pH$ of the solution and the $p K_{ a }$ of bromoacetic acid.

What is $[{H^ + }]$ of a solution that is $0.01\,M$ in $HCN$ and $0.02\,M$ in $NaCN$ $({K_a}$for $HCN = 6.2 \times {10^{ – 10}})$

Derive the equation of ionization constant $({K_b})$ of weak base.

$K _{ a_1,}, K _{ a_2 }$ and $K _{ a_3}$ are the respective ionization constants for the following reactions $(a), (b),$ and $(c)$.

$(a)$ $H _{2} C _{2} O _{4} \rightleftharpoons H ^{+}+ HC _{2} O _{4}^{-}$

$(b)$ $HC _{2} O _{4}^{-} \rightleftharpoons H ^{+}+ HC _{2} O _{4}^{2-}$

$(c)$ $H _{2} C _{2} O _{4} \rightleftharpoons 2 H ^{+}+ C _{2} O _{4}^{2-}$

The relationship between $K_{a_{1}}, K_{ a _{2}}$ and $K_{ a _{3}}$ is given as