Dissociation constat of weak acid $HA$ is $1.8 \times {10^{ - 4}}$ calculate Dissociation constant of its conjugate base ${A^ - }$

The ionization constant of phenol is $1.0 \times 10^{-10} .$ What the concentration of phenolate ion in $0.05$ $M$ solution of phenol? What will be its degree of ionization if the solution is a lso $0.01$ $M$ in sodium phenolate?

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

$K _{ a_1,}, K _{ a_2 }$ 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

$p{K_a}$ of a weak acid is defined as

$p{K_a}$ value for acetic acid at the experimental temperature is $5$. The percentage hydrolysis of $0.1\,\,M$ sodium acetate solution will be