Write characteristics and uses of ${K_a}$ value.
The characteristics and uses of $\mathrm{K}_{a}$ value as under :
$(i)$ The value of $\mathrm{K}_{a}$ is larger, the stronger is the acid.
$(ii)$ $\mathrm{K}_{a}$ is a dimensionless quantity.
$(iii)$ $\left[\mathrm{H}^{+}\right]$of weak acid and $\mathrm{pH}$ calculate using of value of $\mathrm{K}_{a}$.
$(iv)$ Calculate the ionization degree $\alpha$ with the help of $K_{a}$ value.
$(v)$ $\mathrm{pK}_{a}$ is calculated by using the value of $\mathrm{K}_{a}$. $\mathrm{pK}_{a}=-\log \left(\mathrm{K}_{a}\right)$
If the $\mathrm{pK}_{a}$ value is more than the acid become less strong.
$\mathrm{K}_{a}=1 \times 10^{-1}$ | $1 \times 10^{-2}$ | $1 \times 10^{-3}$ |
$\mathrm{pK}_{a}=1$ | $2$ | $3$ |
For a weak acid, the incorrect statement is
A weak monoprotic acid of $0.1\, M,$ ionizes to $1\% $ in solution. What will be the $pH $ of solution
What concentration of $Ac^-$ ions will reduce $H_3O^+$ ion to $2 × 10^{-4}\ M$ in $0.40\ M$ solution of $HAc$ ? $K_a (HAc) = 1.8 × 10^{-5}$ ?
Concentration $C{N^ - }$ in $0.1\,M\,HCN$ is $[{K_a} = 4 \times {10^{ - 10}}]$
$0.1$ $mol$ of $H_2S(g)$ is kept in a $0.4$ litre vessel at $1000\,K$. For the reaction -
$2{H_2}S(g)\,\rightleftharpoons\,2{H_2}(g)\, + \,{S_2}(g)\,;\,{K_c} = {10^{ - 6}}\% $ dissociation of $H_2S$ is.......$\%$