For a weak acid $HA,$ Ostwald's dilution law is represented by the equation
${K_a} = \frac{{\alpha c}}{{1 - {\alpha ^2}}}$
${K_a} = \frac{{{\alpha ^2}c}}{{1 - \alpha }}$
$\alpha = \frac{{{K_a}c}}{{1 - c}}$
${K_a} = \frac{{{\alpha ^2}c}}{{1 - {\alpha ^2}}}$
Calculate the $pH$ of a $0.10 \,M$ ammonia solution. Calculate the pH after $50.0 \,mL$ of this solution is treated with $25.0 \,mL$ of $0.10 \,M$ $HCl$. The dissociation constant of ammonia, $K_{b}=1.77 \times 10^{-5}$
The ionisation constant of acetic acid is $1.8 \times 10^{-5}$. The concentration at which it will be dissociated to $2\%$, is
The dissociation constants of two acids $HA_1$ and $HA_2$ are $3.0 \times 10^{-4}$ and $1.8 \times 10^{-5}$ respectively. The relative strengths of the acids will be
Find $pH$ of $5 \times 10^{-3}\, M$ $H_2CO_3$ solution having $10\%$ dissociation
$pH$ of an aqueous solution $H_2CO_3$ is $3.3$. If ${K_{{a_1}}} = {10^{ - 3}}$and ${K_{{a_2}}} = {10^{ - 13}}$ then $[HCO_3^-]$ is