What is $[{H^ + }]$ of a solution that is $0.01\,M$ in $HCN$ and $0.02\,M$ in $NaCN$ $({K_a}$for $HCN = 6.2 \times {10^{ - 10}})$
$3.1 \times {10^{10}}$
$6.2 \times {10^5}$
$6.2 \times {10^{ - 10}}$
$3.1 \times {10^{ - 10}}$
Which oxychloride has maximum $pH$
The solution of $N{a_2}C{O_3}$ has $pH$
$0.2$ molar solution of formic acid is ionized $3.2\%$. Its ionization constant is
When $CO_2$ dissolves in water, the following equilibrium is established
$C{O_2} + 2{H_2}O\, \rightleftharpoons {H_3}{O^ + } + HCO_3^ - $
for which the equilibrium constant is $3.8 \times 10^{-7}$ and $pH = 6.0$. The ratio of $[HCO_3^- ]$ to $[CO_2]$ would be :-
The hydrogen ion concentration of $0.1\,N$ solution of $C{H_3}COOH,$ which is $30\%$ dissociated, is