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 $pH$ of $0.1\, M$ monobasic acid is $4.50$ Calculate the concentration of species $H ^{+},$ $A^{-}$ and $HA$ at equilibrium. Also, determine the value of $K_{a}$ and $pK _{a}$ of the monobasic acid.
For a weak acid $HA$ with dissociation constant ${10^{ - 9}},\,\,pOH$ of its $0.1 \,M$ solution is
If $pK_a =\, -\,log K_a=4$ for a weak acid $HX$ and $K_a= C\alpha ^2$ then Van't Haff factor when $C = 0.01\,M$ is
What is the dissociation constant for $NH_4OH$ if at a given temperature its $0.1\,N$ solution has $pH = 11.27$ and the ionic product of water is $7.1 \times 10^{-15}$ (antilog $0.73 = 5.37$ )
${K_a}$ of $C{H_3}COOH$ is $1.76 \times {10^{ - 5}}$ at $298$ $K$ temperature. Calculate dissociation constant of its conjugate base.