The hydrogen ion concentration in weak acid of dissociation constant ${K_a}$ and concentration $c$ is nearly equal to
$\sqrt {{K_a}c} $
$c/{K_a}$
${K_a}c$
$\sqrt {{K_a}/c} $
$2\, gm$ acetic acid and $3\, gm$ sodium acetate are present in $100\, ml$. aqueous solution then what will be the $pH$ of solution if ionisation constant of acetic acid is $1.8 \times 10^{-5}$
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
Which of the following base is weakest
$0.01\, M \,HA(aq.)$ is $2\%$ ionized, $[OH^-]$ of solution is :-
The ionization constant of $HF$, $HCOOH$ and $HCN$ at $298\, K$ are $6.8 \times 10^{-4}, 1.8 \times 10^{-4}$ and $4.8 \times 10^{-9}$ respectively. Calculate the ionization constants of the corresponding conjugate base.