Embibe Experts Solutions for Chapter: Equilibrium, Exercise 3: Exercise-3

The incorrect expression among the following is

The thermal dissociation equilibrium of ${\mathrm{CaCO}}_3\left(\mathrm{s}\right)$ is studied under different conditions. ${\mathrm{CaCO}}_3\left(\mathrm{s}\right)\rightleftharpoons \mathrm{CaO}\left(\mathrm{s}\right)+{\mathrm{CO}}_2\left(\mathrm{g}\right)$ For this equilibrium, the correct statement(s) is (are) :

For the reaction in equilibrium,

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

the concentrations, of ${\mathrm{N}}_2{\mathrm{O}}_4$ and ${\mathrm{NO}}_2$ at equilibrium are $4.8\times {10}^{-2}$ and $1.2\times {10}^{-2} \mathrm{mol} {\mathrm{L}}^{-1}$ respectively. The value of ${\mathrm{K}}_{\mathrm{c}}$ for this reaction is:

Aniline behaves as a weak base. When $0.1 \mathrm{M}, 50 \mathrm{mL}$ solution sample of aniline was mixed with $0.2 \mathrm{M},$ $12.5 \mathrm{mL}$ solution of $\mathrm{HCl},$ the $\mathrm{pH}$ of the resulting solution was $8.$ Then:

Which of the following mixtures will act as buffer?

In a solution containing equal concentrations of ${\mathrm{X}}^{-}, {\mathrm{Y}}^{-}$ and ${\mathrm{Z}}^{-}, \mathrm{MCl}$ ($\mathrm{s}$) (a readily soluble salt) is gradually added. If ${\mathrm{K}}_{\mathrm{sp}}\left(\mathrm{MX}\right)>{\mathrm{K}}_{\mathrm{sp}}\left(\mathrm{MY}\right)>{\mathrm{K}}_{\mathrm{sp}}\left(\mathrm{MZ}\right),$ then: (Assume no hydrolysis of any ion).

In a solution containing equal concentrations of ${\mathrm{X}}^{-}, {\mathrm{Y}}^{-}$ and ${\mathrm{Z}}^{-}, \mathrm{MCl}$ ($\mathrm{s}$) (a readily soluble salt) is gradually added. If ${\mathrm{K}}_{\mathrm{sp}}\left(\mathrm{MX}\right)>{\mathrm{K}}_{\mathrm{sp}}\left(\mathrm{MY}\right)>{\mathrm{K}}_{\mathrm{sp}}\left(\mathrm{MZ}\right),$ then : (Assume no hydrolysis of any ion).

In above question, If $[\mathrm{X}{]}_{\mathrm{i}} : [\mathrm{Y}{]}_{\mathrm{i} }: [\mathrm{Z}{]}_{\mathrm{i}}=100:10:1 \& {\mathrm{K}}_{\mathrm{sp}}[\mathrm{MX}] : {\mathrm{K}}_{\mathrm{sp}}[\mathrm{MY}] : {\mathrm{K}}_{\mathrm{sp}}[\mathrm{MZ}]=10:0.1:1,$ order of precipitation will be:

A solution contains $\left[\mathrm{NaCl}\right]=\left[{\mathrm{Na}}_2{\mathrm{CO}}_3\right]=\mathrm{C} \mathrm{M}$. Upon gradually adding ${\mathrm{AgNO}}_3$$\left(\mathrm{s}\right):$(Assume no hydrolysis of any ion.)