The hydrogen ion concentration of a $0.006\,M$ benzoic acid solution is $({K_a} = 6 \times {10^{ - 5}})$
$0.6 \times {10^{ - 4}}$
$6 \times {10^{ - 4}}$
$6 \times {10^{ - 5}}$
$3.6 \times {10^{ - 4}}$
A weak monoprotic acid of $0.1\, M,$ ionizes to $1\% $ in solution. What will be the $pH $ of solution
The ionisation constant of acetic acid is $1.8 \times 10^{-5}$. The concentration at which it will be dissociated to $2\%$, 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.
$5.0$ $pH$ containing solution is dilute $100$ times. Calculate $pH$ of dilute solution.
Dissociation constat of weak acid $HA$ is $1.8 \times {10^{ - 4}}$ calculate Dissociation constant of its conjugate base ${A^ - }$