Embibe Experts Solutions for Chapter: Equilibrium, Exercise 2: Level 2

The extent of dissociation of ${\mathrm{PCl}}_5$ at a certain temperature and one atm pressure, is $20\%$. Calculate the pressure at which this substance is half dissociated at the same temperature.

Consider the reactions:

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

(ii) ${\mathrm{N}}_2{\mathrm{O}}_4 \left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{NO}}_2 \left(\mathrm{g}\right)$

The addition of an inert gas at a constant volume:

At $248°\mathrm{C}$, the ${\mathrm{K}}_{\mathrm{p}}$ for the reaction, ${\mathrm{SbCl}}_5 \left(\mathrm{g}\right)\rightleftharpoons {\mathrm{SbCl}}_3 \left(\mathrm{g}\right)+{\mathrm{Cl}}_2 \left(\mathrm{g}\right)$ is $1.07$ atm at a total pressure of $1$ atm. Calculate the degree of dissociation of ${\mathrm{SbCl}}_5$.

What is the solubility of $\mathrm{Al}{\left(\mathrm{OH}\right)}_3, \left({\mathrm{K}}_{\mathrm{sp}}=1\times {10}^{-33}\right)$ in a buffer solution $\mathrm{pH}=4?$

Which of the following statements is correct for a solution saturated with $\mathrm{AgCl}$ and $\mathrm{AgBr}$ if their solubilities in moles per litre in separate solutions are $\mathrm{x}$ and $\mathrm{y}$ respectively?

A saturated solution of ${\mathrm{BaSO}}_4$ is heated from $25°\mathrm{C}$ to $35°\mathrm{C}$ and the conductance of the solution and the solubility of ${\mathrm{BaSO}}_4$ are measured. It is found that:

In a container equilibrium
${\mathrm{N}}_2{\mathrm{O}}_4 \left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{NO}}_2 \left(\mathrm{g}\right)$
is attained at $25°\mathrm{C}$. The total equilibrium pressure in container is $380$ $\mathrm{torr}$. If equilibrium constant of above equilibrium is $0.667$ $\mathrm{atm}$, then degree of dissociation of ${\mathrm{N}}_2{\mathrm{O}}_4$ at this temperature will be:

The volume of $0.1 \mathrm{M}$ acetic acid $\left({\mathrm{pK}}_{\mathrm{a}}=4.76\right)$ that should be added to $10 \mathrm{ml}$ of $0.2 \mathrm{M}$ sodium acetate solution to prepare a buffer solution of $\mathrm{pH} 4.91$ is-