Ramendra C Mukerjee Solutions for Chapter: Electromotive Force, Exercise 2: Objective Problems

The half-cell potential of a hydrogen electrode at $\mathrm{pH}=10$ will be:

How much will the potential of a hydrogen electrode change when its solution initially at $\mathrm{pH}=0$ is neutralised to $\mathrm{pH}=7?$

A dilute aqueous solution of ${\mathrm{Na}}_2{\mathrm{SO}}_4$ is electrolysed using platinum electrodes. The products at the anode and cathode are:

The standard reduction potential of ${\mathrm{Cu}}^{2+}/\mathrm{Cu}$ and ${\mathrm{Cu}}^{2+}/{\mathrm{Cu}}^{+}$ are $0·337$ and $0·153$, respectively. The standard electrode potential of ${\mathrm{Cu}}^{+}/\mathrm{Cu}$ half-cell is:

Which of the following facts about the chemical cell and concentration cell is correct?

The temperature coefficient of a galvanic cell is $+5·0\times {10}^{-5 }{\mathrm{VK}}^{-1}$. During the discharge of the cell, the cell temperature

Standard electrode potential data are useful for understanding the suitability of an oxidant in a redox titration. Some half-cell reactions and their standard potentials are given below:

$\begin{array}{ll}{\mathrm{MnO}}_4^{- }\left(\mathrm{aq}\right)+8{\mathrm{H}}^{+}\left(\mathrm{aq}\right)+5{\mathrm{e}}^{-}\to {\mathrm{Mn}}^{2+}\left(\mathrm{aq}\right)+4{\mathrm{H}}_{2 }\mathrm{O}\left(l\right);& {\mathrm{E}}^0=1.51 \mathrm{V}\end{array}$

$\begin{array}{ll}{\mathrm{Cr}}_2{\mathrm{O}}_7^{2-}\left(\mathrm{aq}\right)+14{\mathrm{H}}^{+}\left(\mathrm{aq}\right)+6{\mathrm{e}}^{-}\to 2{\mathrm{Cr}}^{3+}\left(\mathrm{aq}\right)+7{\mathrm{H}}_2\mathrm{O}\left(l\right);& {\mathrm{E}}^0=1.38 \mathrm{V}\end{array}$

$\begin{array}{ll}{\mathrm{Fe}}^{3+}\left(\mathrm{aq}\right)+{\mathrm{e}}^{-}\to {\mathrm{Fe}}^{2+}\left(\mathrm{aq}\right);& {\mathrm{E}}^0=0.77 \mathrm{V}\end{array}$

$\begin{array}{ll}{\mathrm{Cl}}_2\left(\mathrm{g}\right)+2{\mathrm{e}}^{-}\to 2{\mathrm{Cl}}^{-}\left(\mathrm{aq}\right);& {\mathrm{E}}^0=1.40 \mathrm{V}\end{array}$

Identify the only incorrect statement regarding the quantitative estimation of aqueous $\mathrm{Fe}{\left({\mathrm{NO}}_3\right)}_2$.

Using the following Latimer diagram for bromine,

$$\begin{gathered} \mathrm{pH}=0 \\ {{\mathrm{BrO}}^{-}}_4\stackrel{1.82 \mathrm{V}}{⟶}{\mathrm{BrO}}_3^{-}\stackrel{1.50 \mathrm{V}}{⟶}\mathrm{HBrO}\stackrel{1.595 \mathrm{V}}{⟶}{\mathrm{Br}}_2\stackrel{1.0652 \mathrm{V}}{⟶}{\mathrm{Br}}^{-} \end{gathered}$$

the species undergoing disproportionation is: