If degree of ionisation is $0.01$ of decimolar solution of weak acid $HA$ then $pKa$ of acid is
$5$
$7$
$2$
$3$
${K_a} = C{ \propto ^2} = 0.1 \times {(0.01)^2} = {10^{ – 5}}$
$pKa = 5$
Ionisation constant of $CH_3COOH$ is $1.7 \times 10^{-5}$ and concentration of $H^+$ ions is $3.4 \times 10^{-4}$. Then find out initial concentration of $CH_3COOH$ Molecules
Derive ${K_a} \times {K_b} = {K_w}$ equation.
The $pH$ of $ 0.1 \,M$ solution of a weak monoprotic acid $1\%$ ionized is
Given the two concentration of $HCN (K_a = 10^{-9})$ are $0.1\,M$ and $0.001\,M$ respectively. What will be the ratio of degree of dissociation ?
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