The $pH$ value of decinormal solution of $N{H_4}OH$ which is $20\%$ ionised, is
$13.3$
$14.7$
$12.3$
$12.95$
At $25\,^oC$, the dissociation constant of $CH_3COOH$ and $NH_4OH$ in aqueous solution are almost the same. The $pH$ of a solution $0.01\, N\, CH_3COOH$ is $4.0$ at $25\,^oC$. The $pH$ of $0.01\, N\, NH_4OH$ solution at the same temperature would be
In aqueous solution the ionization constants for carbonic acid are
$K_1 = 4.2 \times 10^{-7}$ and $K_2 = 4.8 \times 10^{-11}$
Select the correct statement for a saturated $0.034\, M$ solution of the carbonic acid.
A monoprotic acid in a $0.1\,\,M$ solution ionizes to $0.001\%$. Its ionisation constant is
$5\%$ ionization is occur in $0.01$ $M$ $C{H_3}COOH$ solution. Calculate its dissociation constant.
The ionization constant of $0.1$ $M$ weak acid is $1.74 \times {10^{ - 5}}$ at $298$ $K$ temperature. Calculate $pH$ of its $0.1$ $M$ solution.