A $0.1\,N $ solution of an acid at room temperature has a degree of ionisation $ 0.1$ . The concentration of $O{H^ - }$ would be
${10^{ - 12}}\,M$
${10^{ - 11}}\,M$
${10^{ - 9}}\,M$
${10^{ - 2}}\,M$
The $pH$ of $0.1$ $M$ $HCN$ solution is $5.2$ calculate ${K_a}$ of this solution.
What is the percent ionization $(\alpha)$ of a $0.01\, M\, HA$ solution ? .......$\%$ $(K_a = 10^{-6})$
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
$0.2$ molar solution of formic acid is ionized $3.2\%$. Its ionization constant is
Calculate the $pH$ of the solution in which $0.2 \,M\, NH _{4} Cl$ and $0.1 \,M\, NH _{3}$ are present. The $pK _{ b }$ of ammonia solution is $4.75$