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.
$\mathrm{K}_{b}$ | $1 \times 10^{-1}$ | $1 \times 10^{-2}$ | $1 \times 10^{-3}$ |
$\mathrm{pK}_{b}$ | $+1$ | $+2$ | $+3$ |
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 ? ......$\%$
The percentage of pyridine $(C_5H_5N)$ that forms pyridinium ion $(C_5H_5N^+H)$ in a $0.10\, M$ aqueous pyridine solution ($K_b$ for $C_5H_5N = 1.7 \times 10^{-9}$) is
A weak monoprotic acid of $0.1\, M,$ ionizes to $1\% $ in solution. What will be the $pH $ of solution
What is the $pH$ of solution of $7$ $gm$ $N{H_4}OH$ per $500$ $mL$ ? ( ${K_b}$ of $N{H_4}OH 1.8 \times {10^{ - 5}}$, Molecular moles of $N{H_4}OH$ is $35\,g\,mo{l^{ - 1}}$ )
Explain a general step-wise approach to evaluate the $pH$ of the weak electrolyte.