The dissociation constant of an acid $HA$  is $1 \times {10^{ - 5}}$. The $pH$ of $0.1$ molar solution of the acid will be

The solubility of a salt of weak acid $( A B )$ at $pH 3$ is $Y \times 10^{-3} mol L ^{-1}$. The value of $Y$ is

. . . . . (Given that the value of solubility product of $A B \left( K _{ sp }\right)=2 \times 10^{-10}$ and the value of ionization constant of $H B \left( K _{ a }\right)=1 \times 10^{-8}$ )

The ionization constant of phenol is $1.0 \times 10^{-10} .$ What the concentration of phenolate ion in $0.05$ $M$ solution of phenol? What will be its degree of ionization if the solution is a lso $0.01$ $M$ in sodium phenolate?

Concentration $C{N^ - }$ in $0.1\,M\,HCN$ is $[{K_a} = 4 \times {10^{ - 10}}]$

What is the $ pH$  of $0.01\, M$  glycine solution? For glycine, $K{a_1} = 4.5 \times {10^{ - 3}}$ and $K{a_2} = 1.7 \times {10^{ - 10}}$ at  $298 \,K$

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 ? ......$\%$