Embibe Experts Solutions for Chapter: Equilibrium, Exercise 1: Level 1

The aqueous solution of ${\mathrm{AlCl}}_3$ is acidic due to the hydrolysis of

The $\mathrm{pH}$ values of

(i) $0.1 \mathrm{M} \mathrm{HCl}$ aq

(ii) $0.1 \mathrm{M} \mathrm{KOH}$

(iii) tomato juice and

(iv) pure water

Follow the order:

Among ${\mathrm{CO}}_3^{2-}, {\mathrm{OH}}^{-}, {\mathrm{NH}}_3$ and ${\mathrm{HCO}}_3^{-}$, the species that acts as a Bronsted acid as well as a Bronsted base is:

The conjugate bases for ${\mathrm{HCO}}_3^{–}$ and ${\mathrm{NH}}_3,$ respectively, are

An aqueous solution of $\mathrm{HCl}$ has a $\mathrm{pH}$ of $2.0$. When water is added to increase the $\mathrm{pH}$ to $5.0$, the hydrogen ion concentration is:

The correct relationship between free energy change in a reaction and the corresponding equilibrium constant $\mathrm{K}$ is:

The effect of temperature on the equilibrium constant is expressed as, $\left({\mathrm{T}}_2>{\mathrm{T}}_1\right) \log \left(\frac{{\mathrm{K}}_2}{{\mathrm{K}}_1}\right)=\frac{-\mathrm{\Delta H}}{2.303\mathrm{R}}\left[\frac{1}{ {\mathrm{T}}_2}-\frac{1}{ {\mathrm{T}}_1}\right]$. For endothermic reactions, false statement is:

A reaction in equilibrium is represented by the following equation, $2{\mathrm{A}}_{\left(\mathrm{s}\right)}+3{\mathrm{B}}_{\left(\mathrm{g}\right)}\rightleftharpoons 3{\mathrm{C}}_{\left(\mathrm{g}\right)}+\mathrm{D}\left(\mathrm{g}\right)+{\mathrm{O}}_2$. If the pressure on the system is reduced to half of its original value: