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

For a $10^{-3} \ M \ H_2CO_3$ solution,if the degree of dissociation $\alpha = 10\%$,what will be the value of $pH$?

$A$ solution of weak acid $HA$ containing $0.01 \ mol/L$ of acid has $pH = 4$. The percentage degree of ionisation of the acid and the ionisation constant of acid are respectively.

What is the $pH$ of a weak dibasic acid,that is $2 \%$ dissociated in its $M/100$ solution at $298 \ K$?

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

$A$ weak acid,$HA,$ has a $K_a$ of $1.00 \times 10^{-5}.$ If $0.100 \ mol$ of this acid is dissolved in one litre of water,the percentage of acid dissociated at equilibrium is closest to $...\%$