$HClO$ is a weak acid. The concentration of ${H^ + }$ ions in $0.1\,M$ solution of $HClO\,({K_a} = 5 \times {10^{ - 8}})$ will be equal to
$7.07 \times {10^{ - 5}}\,m$
$5 \times 10^{-9}\,\,m$
$5 \times {10^{ - 7}}\,m$
$7 \times {10^{ - 4}}\,m$
Degree of dissociation is $10\%$ for $10^{-3}\, M$ solution of $H_2CO_3$ then $pH$ of solution is
$25$ $mL$ $0.1$ $M$ $HCl$ solution is diluted till $500$ $mL$. Calculate $pH$ of dilute solution.
The ionisation constant of acetic acid is $1.8 \times 10^{-5}$. The concentration at which it will be dissociated to $2\%$, is
For a weak acid, the incorrect statement is
$0.01\, M \,HA(aq.)$ is $2\%$ ionized, $[OH^-]$ of solution is :-