Accumulation of lactic acid $(HC_3H_5O_3),$ a monobasic acid in tissues leads to pain and a feeling of fatigue. In a $0.10\, M$ aqueous solution, lactic acid is $3.7\%$ dissociates. The value of dissociation constant, $K_a,$ for this acid will be
$1.4 \times 10^{-5}$
$1.4 \times 10^{-4}$
$3.7 \times 10^{-4}$
$2.8 \times 10^{-4}$
Derive the equation of ionization constants ${K_a}$ of weak acids $HX$.
${K_a}$ of $C{H_3}COOH$ is $1.76 \times {10^{ - 5}}$ at $298$ $K$ temperature. Calculate dissociation constant of its conjugate base.
$0.01\, M \,HA(aq.)$ is $2\%$ ionized, $[OH^-]$ of solution is :-
The dissociation constants of two acids $HA_1$ and $HA_2$ are $3.0 \times 10^{-4}$ and $1.8 \times 10^{-5}$ respectively. The relative strengths of the acids will be
The ionization constant of $0.1$ $M$ weak acid is $1.74 \times {10^{ - 5}}$ at $298$ $K$ temperature. Calculate $pH$ of its $0.1$ $M$ solution.