If the ionization constant of hypochlorous acid $(HOCl)$ is $2.5 \times 10^{-5}$,the $pH$ of $1.0 \ M$ of its solution is $(\log 5=0.7)$.

Find the $pOH$ value of $10^{-3} \ M \ NH_4OH$. Given $K_b = 10^{-5}$.

Dissociation constant of $0.01 \ M$ weak acid is $10^{-4}$. What is percent dissociation of acid (in $\%$)?

The dissociation constants of monobasic acids $A$,$B$,$C$ and $D$ are $6 \times 10^{-4}$,$5 \times 10^{-5}$,$3.6 \times 10^{-6}$ and $7 \times 10^{-10}$ respectively. The $pH$ values of their $0.1 \ M$ aqueous solutions are in the order

$1.0 \ mol$ of $HCl$ and $1.0 \ mol$ of $CH_3COONa$ are dissolved in water to make a $1 \ L$ solution. What is the concentration of $H^+$ in the solution? ($K_a$ for $CH_3COOH = 1.6 \times 10^{-5}$)

The $pH$ of a monoacidic base is $10$. Calculate its percentage dissociation in $0.01 \ M$ solution at $298 \ K$. (in $\%$)