The degree of dissociation $(\alpha )$ of $PCl_5$ obeying the equilibrium;  is $PC{l_5}\, \rightleftharpoons \,PC{l_3}\, + \,C{l_2}$ related to the pressure at equlibrium by

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?

Values of dissociation constant, $K_a$ are given as follows

Correct order of increasing base strength of the base $CN^-,F^-$ and $NO_2^-$ will be

Dimethyl amine ${\left( {C{H_3}} \right)_2}NH$ is weak base and its ionization constant $ 5.4 \times {10^{ – 5}}$. Calculate $\left[ {O{H^ – }} \right],\left[ {{H_3}O} \right]$, $pOH$ and $pH$ of its $0.2$ $M$ solution at equilibrium.