The concentration of $[{H^ + }]$ and concentration of $[O{H^ - }]$ of a $ 0.1$ aqueous solution of $2\%$ ionised weak acid is [Ionic product of water $ = 1 \times {10^{ - 14}}]$
$2 \times {10^{ - 3}}$ $M$ and $5 \times {10^{ - 12}}$ $M$
$1 \times {10^3}\;M\;{\rm{and}}\;3 \times {10^{ - 11}}M$
$0.02 \times {10^{ - 3}}\;M\;{\rm{and}}\;5 \times {10^{ - 11}}M$
$3 \times {10^{ - 2}}\;M\;{\rm{and}}\;4 \times {10^{ - 13}}M$
Which solution contains maximum number of ${H^ + }$ ion
If the dissociation constant of an acid $HA$ is $1 \times {10^{ - 5}},$ the $pH$ of a $ 0.1$ molar solution of the acid will be approximately
Derive the equation of ionization constants ${K_a}$ of weak acids $HX$.
Heat of neutralisation of weak acid and strong base is less than the heat of neutralisation of strong acid and strong base due to
The ${K_b}$ of ammonia is $1.8 \times {10^{ - 5}}$ at $298$ $K$ temperature. Calculate the $pH$ of $0.1$ $M$ solution.