At $25\,^o C$, the dissociation constant of a base $BOH$ is $1.0 \times {10^{ - 12}}$. The concentration of Hydroxyl ions in $0.01\, M$ aqueous solution of the base would be
$2.0 \times {10^{ - 6}}\,mol\,{L^{ - 1}}$
$1.0 \times {10^{ - 5}}\,mol\;{L^{ - 1}}$
$1.0 \times {10^{ - 6}}\,mol\,{L^{ - 1}}$
$1.0 \times {10^{ - 7}}\,mol\;{L^{ - 1}}$
Dissociation constant for a monobasic acid is $10^{-4}$ . What is the $pH$ of the monobasic acid ? (If $\%$ dissociation $= 2\,\%$ )
The $pH $ of a $0.01\,M$ solution of acetic acid having degree of dissociation $12.5\%$ is
$5.0$ $pH$ containing solution is dilute $100$ times. Calculate $pH$ of dilute solution.
Calculate the ${H^ + }$ ion concentration in a $1.00\,(M)$ $\,HCN\,$ litre solution $({K_a} = 4 \times {10^{ - 10}})$
Which solution contains maximum number of ${H^ + }$ ion