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.
$\mathrm{K}_{a}=1 \times 10^{-1}$ | $1 \times 10^{-2}$ | $1 \times 10^{-3}$ |
$\mathrm{pK}_{a}=1$ | $2$ | $3$ |
Calculate the $pH$ of a $0.10 \,M$ ammonia solution. Calculate the pH after $50.0 \,mL$ of this solution is treated with $25.0 \,mL$ of $0.10 \,M$ $HCl$. The dissociation constant of ammonia, $K_{b}=1.77 \times 10^{-5}$
Derive the equation of ionization constant $({K_b})$ of weak base.
In aqueous solution the ionization constants for carbonic acid are
$K_1 = 4.2 \times 10^{-7}$ and $K_2 = 4.8 \times 10^{-11}$
Select the correct statement for a saturated $0.034\, M$ solution of the carbonic acid.
The ionisation constant of acetic acid is $1.8 \times 10^{-5}$. The concentration at which it will be dissociated to $2\%$, is
${K_a} = 1.4 \times {10^{ - 5}}$ of propanoic acid. Calculate its $pH$ of $0.1$ $M$ solution.