M K Verma Solutions for Chapter: Electrochemistry, Exercise 1: TOPICWISE QUESTIONS

The conductivity of $0.002 \mathrm{M}$ acetic acid is $8\times {10}^{-5} \mathrm{S}$ ${\mathrm{cm}}^{-1}.$ If $\mathrm{\Lambda }°$ of acetic acid is $392 \mathrm{S} {\mathrm{cm}}^2 {\mathrm{mol}}^{-1}$, what is the $\mathrm{pH}$ of the solution?

A solution contains ${10}^{-40} \mathrm{M} {\mathrm{Cu}}^{2+}$ and $1 \mathrm{M} {\mathrm{Zn}}^{2+}$ as the only cations. On passing electric current, which of the ions will be reduced at the cathode first?

Given, ${\mathrm{E}}_{{\mathrm{Cu}}^{+2}/ \mathrm{Cu}}^0=0.34 \mathrm{V}$ and ${\mathrm{E}}_{{\mathrm{Zn}}^{2+}/\mathrm{Zn}}^{\mathrm{o}}=-0.76 \mathrm{V}$.

$\mathrm{M}\left|{\mathrm{M}}^{2+}\right(\mathrm{salt} \mathrm{solution} \mathrm{of} {\mathrm{MX}}_2)$ $\Vert {\mathrm{M}}^{2+}\left(0.001 \mathrm{mol} {\mathrm{dm}}^{-3}\right)|\mathrm{M}$.

The above electrochemical cell is a concentration cell with EMF $0.059 \mathrm{V}$. What is the solubility product of ${\mathrm{MX}}_2$ at $298 \mathrm{K}$?

The efficiency of a fuel cell is $80\%$ and standard enthalpy of the reaction is $-300 \mathrm{kJ} {\mathrm{mol}}^{-1}$. The reaction involves two electrons in the redox change. What is the value of ${\mathrm{E}}_{\text{cell }}^{\mathrm{o}}$?

$\mathrm{X}\to \mathrm{Y}, {\mathrm{\Delta }}_{\mathrm{r}}\mathrm{G}°=-193 \mathrm{kJ} {\mathrm{mol}}^{-1}$.

All the energy released from the above reaction is used for oxidizing ${\mathrm{M}}^{+}$ to ${\mathrm{M}}^{+3}+2{\mathrm{e}}^{-}$. $\mathrm{E}°$ is equal to $-0.25 \mathrm{V}$. Under standard conditions, the number of moles of ${\mathrm{M}}^{+}$ oxidized when one mole of $\mathrm{X}$ is converted to $\mathrm{Y}$ is

What is the reduction potential of ${\mathrm{Cu}}^{+2}/\mathrm{Cu}$ at $\mathrm{pH}=10$? $\left({\mathrm{K}}_{\mathrm{sp}} \mathrm{of} \mathrm{Cu}(\mathrm{OH}{)}_2=1\times {10}^{-18} \& {\mathrm{E}}_{{\mathrm{Cu}}^{+2}/\mathrm{Cu}}^{\mathrm{o}}=0.34 \mathrm{V}\right)$

Two electrolytic cells containing silver nitrate solution and dilute sulphuric acid solution were connected in series. A steady current of $2.5 \mathrm{A}$ was passed through them till $1.078 \mathrm{g}$ of silver was deposited. What is the total weight of oxygen gas liberated in the process?

$\left(\mathrm{Ag}=107.8 \mathrm{g} {\mathrm{mol}}^{-1}\right)$

Molar conductance of a $0.5 \mathrm{M} {\mathrm{NH}}_4\mathrm{OH}$ solution is $2.5\times {10}^{-3} \mathrm{S} {\mathrm{m}}^{2 }{\mathrm{mol}}^{-1}.$ Molar conductance of $\mathrm{Ba}(\mathrm{OH}{)}_2$, ${\mathrm{BaCl}}_2$ and ${\mathrm{NH}}_4\mathrm{Cl}$ at infinite dilutions are $525\times {10}^{-4},$ $280\times {10}^{-4}$ and $130\times {10}^{-4} \mathrm{S} {\mathrm{m}}^2 {\mathrm{mol}}^{-1}$, respectively. What is the $\mathrm{pH}$ of the solution?