What is the $pH$ of the resulting solution when equal volumes of $0.1\, M\, NaOH$ and $0.01\, M\, HCl$ are mixed?
$2$
$7$
$1.04$
$12.65$
A solution of weak acid $HA$ containing $0.01$ moles of acid per litre of solutions has $pH = 4$. The percentage degree of ionisation of the acid and the ionisation constant of acid are respectively.
$0.01\, M \,HA(aq.)$ is $2\%$ ionized, $[OH^-]$ of solution is :-
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
For a weak acid $HA,$ Ostwald's dilution law is represented by the equation
$5.0$ $pH$ containing solution is dilute $100$ times. Calculate $pH$ of dilute solution.