The $pH$ of two equimolar weak acids are $3.0$ and $5.0$ respectively. Their relative strength is

The ionization constant of $HF$ is $3.2 \times 10^{-4}$. Calculate the degree of dissociation of $HF$ in its $0.02 \ M$ solution. Calculate the concentration of all species present ($H_{3}O^{+}$,$F^{-}$ and $HF$) in the solution and its $pH$.

$A$ 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.

It has been found that the $pH$ of a $0.01 \ M$ solution of an organic acid is $4.15$. Calculate the concentration of the anion,the ionization constant of the acid and its $pK_a$.

For a weak acid $HA$ with dissociation constant $10^{-9}$,the $pOH$ of its $0.1 \ M$ solution is:

What is the percent dissociation of acetic acid in its $0.01 \ M$ solution if the dissociation constant of the acid is $1.34 \times 10^{-6}$ (in $\%$)?