Calculate the ${H^ + }$ ion concentration in a $1.00\,(M)$ $\,HCN\,$ litre solution $({K_a} = 4 \times {10^{ - 10}})$
$4 \times {10^{ - 14}}\,mole/litre$
$2 \times {10^{ - 5}}\,mole/litre$
$2.5 \times {10^{ - 5}}\,mole/litre$
None of these
The $pH $ of a $0.01\,M$ solution of acetic acid having degree of dissociation $12.5\%$ is
The $pH$ of two equimolar weak acids are $3.0$ and $5.0$ respectively. Their relative strength is
A weak base $MOH$ of $0.1\, N$ concentration shows a $pH$ value of $9$. What is the percentage degree of ionisation of the base ? ......$\%$
The $pH$ of $0.1$ $M$ solution of cyanic acid $(HCNO)$ is $2.34$. Calculate the ionization constant of the acid and its degree of ionization in the solution.
Dissociation constant for a monobasic acid is $10^{-4}$ . What is the $pH$ of the monobasic acid ? (If $\%$ dissociation $= 2\,\%$ )