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 concentration of $CO_3^{2-}$ is $0.034\, M.$
The concentration of $CO_3^{2-}$ is greater than that of $HCO_3^-.$
The concentrations of $H^+$ and $HCO_3^-$ are approximately equal.
The concentration of $H^+$ is double that of $CO_3^{2-}.$
Concentration $C{N^ - }$ in $0.1\,M\,HCN$ is $[{K_a} = 4 \times {10^{ - 10}}]$
Which of the following base is weakest
A monoprotic acid in a $0.1\,\,M$ solution ionizes to $0.001\%$. Its ionisation constant is
The ionization constant of dimethylamine is $5.4 \times 10^{-4}$. Calculate its degree of ionization in its $0.02$ $M$ solution. What percentage of dimethylamine is ionized if the solution is also $0.1 \,M$ in $NaOH ?$
For a weak acid $HA,$ Ostwald's dilution law is represented by the equation