The $ pH$ of $ 0.1$ $M$ acetic acid is $3$, the dissociation constant of acid will be
$1.0 \times {10^{ - 4}}$
$1.0 \times {10^{ - 5}}$
$1.0 \times {10^{ - 3}}$
$1.0 \times {10^{ - 8}}$
The ionisation constant of acetic acid is $1.8 \times 10^{-5}$. The concentration at which it will be dissociated to $2\%$, is
The degree of dissociation of $0.1\,M\,HCN$ solution is $0.01\%$ . Its ionisation constant would be
Write characteristic and uses of weak base equilibrium constant ${K_b}$.
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
Write examples of weak acids and weak bases and give ionic equilibrium in its aqueous solution.