Write characteristic and uses of weak base equilibrium constant ${K_b}$.
$(i)$ If the value of $K_{b}$ is more than base is more strong. $(ii)$ $K_{b}$ is a dimensionless quantity.
$(iii)$ With the help of $\mathrm{K}_{b}$, calculate $\left[\mathrm{OH}^{-}\right]$of weak base and then $pOH.$ $(iv)$ The ionization degree $(\alpha)$ of base can be calculated by value of $K_{b}$.
$(v)$ $\mathrm{pK}_{b}$ is calculate by using the value of $\mathrm{K}_{b^{*}}$
$\mathrm{pK}_{b}=-\log \left(\mathrm{K}_{b}\right)$
If $\mathrm{pK}_{b}$ value is more then base is less strong.
$\mathrm{K}_{b}$ | $1 \times 10^{-1}$ | $1 \times 10^{-2}$ | $1 \times 10^{-3}$ |
$\mathrm{pK}_{b}$ | $+1$ | $+2$ | $+3$ |
The ionization constant of propanoic acid is $1.32 \times 10^{-5}$. Calculate the degree of ionization of the acid in its $0.05\, M$ solution and also its $pH$. What will be its degree of ionization if the solution is $0.01$ $M$ in $HCl$ also?
Derive ${K_a} \times {K_b} = {K_w}$ equation.
$0.01\, M \,HA(aq.)$ is $2\%$ ionized, $[OH^-]$ of solution is :-
A weak base $MOH$ of $0.1\, N$ concentration shows a $pH$ value of $9$. What is the percentage degree of ionisation of the base ? ......$\%$
A $0.1\, M$ solution of $HF$ is $1\%$ ionized. What is the $K_a$