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.
$1\% ,\,{10^{ - 6}}$
$0.01\% ,\,{10^{ - 4}}$
$1\% ,\,{10^{ - 4}}$
$0.01\% ,\,{10^{ - 6}}$
Write characteristics and uses of ${K_a}$ value.
The dissociation constant of an acid $HA$ is $1 \times {10^{ - 5}}$. The $pH$ of $0.1$ molar solution of the acid will be
What is the $pH$ of the resulting solution when equal volumes of $0.1\, M\, NaOH$ and $0.01\, M\, HCl$ are mixed?
${K_a}$ of $C{H_3}COOH$ is $1.76 \times {10^{ - 5}}$ at $298$ $K$ temperature. Calculate dissociation constant of its conjugate base.
$5.0$ $pH$ containing solution is dilute $100$ times. Calculate $pH$ of dilute solution.