Ramendra C Mukerjee Solutions for Chapter: Electrolysis and Electrolytic Conductance, Exercise 1: PROBLEMS

For the electrolytic production of ${\mathrm{NaClO}}_4$ from ${\mathrm{NaClO}}_3$ as per reactions:

${\mathrm{ClO}}_3^{-}+{\mathrm{H}}_2\mathrm{O}\to {\mathrm{ClO}}_4^{-}+2{\mathrm{H}}^{+}+2e^{-}$

Electric current is passed through two cells$\text{'}\mathrm{A}\text{'}$and $\text{'}\mathrm{B}\text{'}$ in series. Cell $\text{'}\mathrm{A}\text{'}$ contains an aqueous solution of ${\mathrm{Ag}}_2{\mathrm{SO}}_4$ and platinum electrodes. The cell ' ${\mathrm{B}}^{\text{'}}$ contains aqueous solution of ${\mathrm{CuSO}}_4$ and $\mathrm{Cu}$ electrodes. The current is passed till $1.6 \mathrm{g}$ of oxygen is liberated at the anode of cell $\text{'}\mathrm{A}\text{'}$.

Give equations for the reaction taking place at each electrode.

Electric current is passed through two cells $\text{'}\mathrm{A}\text{'}$ $\text{'}\mathrm{B}\text{'}$ in series. Cell$\text{'}\mathrm{A}\text{'}$ contains an aqueous solution of ${\mathrm{Ag}}_2{\mathrm{SO}}_4$ and platinum electrodes. The cell  $\text{'}\mathrm{B}\text{'}$ contains an aqueous solution of ${\mathrm{CuSO}}_4$ and $\mathrm{Cu}$ electrodes. The current is passed till $1.6 \mathrm{g}$ of oxygen is liberated at the anode of cell $\text{'}\mathrm{A}\text{'}.$

Calculate the quantities of substances deposited at the cathodes of the two cells.$(\mathrm{Ag}=108, \mathrm{Cu}=63.5)$

$40 \mathrm{mL}$ of $0.125 \mathrm{M}$ of ${\mathrm{NiSO}}_4$ solution is electrolysed by a current of $0.05 \mathrm{amp}$ for $40 \mathrm{minutes}.$

$\left(\mathrm{i}\right)$ Write the equation for the reactions occurring at each electrode.

Given the equivalent conductance of sodium butyrate, sodium chloride and hydrogen chloride as $83,127$ and $426 \mathrm{mho} {\mathrm{cm}}^2$ at $25°\mathrm{C}$, respectively. Calculate the equivalent conductance of butyric acid (in unit of $\mathrm{mho} {\mathrm{cm}}^2$) at infinite dilution. 

A dilute solution of $\mathrm{KCl}$ was placed between two platinum electrodes $10 \mathrm{cm}$ apart, across which a potential of $6 \mathrm{volts}$was applied. How far would the ${\mathrm{K}}^{+}$ ion move in $2 \mathrm{hours}$ at $25°\mathrm{C}?$ Ionic conductance of ${\mathrm{K}}^{+}$ ion at infinite dilution at $25°\mathrm{C}$ is $73.52$ $\mathrm{mho}$${\mathrm{cm}}^2 {\mathrm{mol}}^{-1}$.

For $0.0128 \mathrm{N}$ solution of acetic acid at $25°\mathrm{C}$, equivalent conductance of the solution is $1.4$ $\mathrm{mho} {\mathrm{cm}}^2{\mathrm{eq}}^{-1}$ and ${\text{Λ}}_0=391 \mathrm{mho} {\mathrm{cm}}^2{\mathrm{eq}}^{-1}$. Calculate the dissociation constant $\left({\mathrm{K}}_{\mathrm{a}}\right)$ of acetic acid.  Give answer as $({\mathrm{K}}_{\mathrm{a}} \times {10}^7)$.

The specific conductance at $25°\mathrm{C}$ of a saturated solution of $\mathrm{AgCl}$ in water is $1.826\times {10}^{-6} \mathrm{mho} {\mathrm{cm}}^{-1}.$ If ${\mathrm{\Lambda }}_{\mathrm{AgCl}}°$ is equal to$138.26 \mathrm{mho} {\mathrm{cm}}^2 {\mathrm{mol}}^{-1},$ find out the solubility of $\mathrm{AgCl}$ in water in $\mathrm{milligrams} \mathrm{per} \mathrm{litre}.$