Degree of dissociation is $10\%$ for $10^{-3}\, M$ solution of $H_2CO_3$ then $pH$ of solution is
$4$
$2.7$
$3.7$
$3.3$
Write characteristic and uses of weak base equilibrium constant ${K_b}$.
A solution of weak acid $HA$ containing $0.01$ moles of acid per litre of solutions has $pH = 4$. The percentage degree of ionisation of the acid and the ionisation constant of acid are respectively.
The $ pH$ of $ 0.1$ $M$ acetic acid is $3$, the dissociation constant of acid will be
The solution of $N{a_2}C{O_3}$ has $pH$
$HClO$ is a weak acid. The concentration of ${H^ + }$ ions in $0.1\,M$ solution of $HClO\,({K_a} = 5 \times {10^{ - 8}})$ will be equal to