$p{K_a}$ of a weak acid is defined as
$log_{10}{K_a}$
$\frac{1}{{lo{g_{10}}{K_a}}}$
$log _{10}\frac{1}{{{K_a}}}$
$-log_{10}\frac{1}{{{K_a}}}$
Calculate the $pH$ of $0.08\, M$ solution of hypochlorous acid, $HOCl$. The ionization constant of the acid is $2.5 \times 10^{-5}$ Determine the percent dissociation of $HOCl.$
The $pH$ of two equimolar weak acids are $3.0$ and $5.0$ respectively. Their relative strength is
The $pH$ of $0.1\, M$ monobasic acid is $4.50$ Calculate the concentration of species $H ^{+},$ $A^{-}$ and $HA$ at equilibrium. Also, determine the value of $K_{a}$ and $pK _{a}$ of the monobasic acid.
$5.0$ $pH$ containing solution is dilute $100$ times. Calculate $pH$ of dilute solution.
Given the two concentration of $HCN (K_a = 10^{-9})$ are $0.1\,M$ and $0.001\,M$ respectively. What will be the ratio of degree of dissociation ?