At $27^{\circ} C$,the degree of dissociation of $HA$ (weak acid) in $0.5 \ M$ of its solution is $1 \%$. The concentrations of $H_3O^{+}$,$A^{-}$,and $HA$ at equilibrium (in $mol \ L^{-1}$) are respectively

$0.1 \, M$ acetic acid is $1\%$ ionized. If its ionization increases to $10\%$,what will be its new concentration (in $, M$)?

Which of the following statement$(s)$ is/are correct.
$A$. The $pH$ of $1 \times 10^{-8} \ M$ aqueous solution of $HCl$ is $8$
$B$. The conjugate base of $H_2PO_4^{\ominus}$ is $HPO_4^{2-}$
$C$. $K_w$ increases with increase in temperature
$D$. When a solution of a weak monoprotic acid is titrated against a strong base,then at the half-neutralization point,$pH = pK_a$.

In a solution,$0.02 \ M$ acetic acid is $4 \%$ dissociated. The $[OH^{-}]$ in the solution is

Which one of the following statements is correct?

The incorrect relation for isohydric solutions is $:-$