Embibe Experts Solutions for Chapter: Equilibrium, Exercise 4: EXERCISE-III (Analytical Questions)

For the reaction,

${{\mathrm{PCl}}_5}_{\left(\mathrm{g}\right)}\rightleftharpoons {{\mathrm{PCl}}_3}_{\left(\mathrm{g}\right)}+{{\mathrm{Cl}}_2}_{\left(\mathrm{g}\right)}$

the forward reaction at constant temperature is favoured by :-

(a) Introducing an inert gas at constant volume

(b) Introducing chlorine gas at constant volume

(c) Introducing an inert gas at constant pressure

(d) Increasing volume of the container

(e) Introducing ${\mathrm{PCl}}_5$ at constant volume

A reaction mixture containing ${\mathrm{H}}_2, {\mathrm{N}}_2$ and ${\mathrm{NH}}_3$ has partial pressure $2$ $\mathrm{atm}$, $1$$\mathrm{atm}$ and $3$ $\mathrm{atm}$, respectively at $725 \mathrm{K}$. If the value of ${\mathrm{K}}_{\mathrm{p}}$ for the reaction, ${\mathrm{N}}_2+3{\mathrm{H}}_2\rightleftharpoons 2{\mathrm{NH}}_3$ is $4.28\times {10}^{-5} {\mathrm{atm}}^{-2}$ at $725 \mathrm{K}$, in which direction the net reaction will go?

At $25 °\mathrm{C}$, the dissociation constant of a base $\mathrm{BOH}$ is $1.0\times {10}^{-12}$. The concentration of hydroxyl ions in $0.01 \mathrm{M}$ aqueous solution of the base would be

The solubility product of ${\mathrm{BaSO}}_4$ at $25°\mathrm{C}$ is $1.0\times {10}^{-9}$. What would be the concentration of ${\mathrm{H}}_2{\mathrm{SO}}_4$ to precipitate ${\mathrm{BaSO}}_4$ from a solution of $0.01 \mathrm{M} {\mathrm{Ba}}^{2+}$ ions ?

The ${\mathrm{K}}_{\mathrm{sp}}$ for $\mathrm{Cr}(\mathrm{OH}{)}_3$ is $1.6\times {10}^{-30}$. The molar solubility of this compound in water is

The $\mathrm{pH}$of a $0.1$ molar solution of the acid $\mathrm{HQ}$ is $3$. The value of the ionization constant ${\mathrm{K}}_{\mathrm{a}}$ of the acid is: 

The first and second dissociation constants of an acid ${\mathrm{H}}_2\mathrm{A}$ are $1.0\times {10}^{-5}$ and $5.0\times {10}^{-10}$respectively. The overall dissociation constant of the acid will be: 

The incorrect expression among the following is