(B) The reduction of $H^+$ ions at a $Hg$ cathode requires a higher overpotential (voltage) compared to a $Pt$ cathode. Due to this high overpotential

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More voltage is required to reduce $H^+$ ions at a $Hg$ cathode than at a $Pt$ cathode.

(B) The reduction of $H^+$ ions at a $Hg$ cathode requires a higher overpotential (voltage) compared to a $Pt$ cathode. Due to this high overpotential,the reduction of $Na^+$ ions to $Na$ metal becomes more favorable at the $Hg$ cathode,which then reacts with $Hg$ to form sodium amalgam $(Na-Hg)$.

Class 12 Chemistry Electrochemistry Electrolytes and Electrolysis

Medium

During the electrolysis of $NaCl$ solution,$H_2$ gas is liberated at the cathode when a $Pt$ electrode is used,whereas sodium amalgam is formed when a $Hg$ cathode is used. What is the reason for this?

A
$Hg$ is more inert than $Pt$.
B
More voltage is required to reduce $H^+$ ions at a $Hg$ cathode than at a $Pt$ cathode.
C
$Na$ dissolves in $Hg$ while it does not dissolve in $Pt$.
D
The concentration of $H^+$ is higher when a $Pt$ electrode is used.

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Electrochemistry

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Electrolytes and Electrolysis

Predict the products of electrolysis in each of the following:
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$ii$. An aqueous solution of $AgNO_3$ with platinum electrodes
$iii$. $A$ dilute solution of $H_2SO_4$ with platinum electrodes
$iv$. An aqueous solution of $CuCl_2$ with platinum electrodes.

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During the electrolysis of aqueous $NaCl$,if $3 \ mole$ of $H_2O$ are electrolysed,then how much charge (in $F$) is required if the current efficiency is $75 \ \%$?

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$A$ solution of sodium sulphate in water is electrolysed using inert electrodes. The products at the cathode and anode are respectively:

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Explain: Oxidation of $Cl^{-}$ ion is carried out near the anode when electrolysis of aqueous (concentrated) $NaCl$ solution is carried out using an inert electrode.

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Which of the following is $NOT$ produced during the electrolysis of brine solution?

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During the electrolysis of $NaCl$ solution,$H_2$ gas is liberated at the cathode when a $Pt$ electrode is used,whereas sodium amalgam is formed when a $Hg$ cathode is used. What is the reason for this?

Similar Questions

During the electrolysis of aqueous $NaCl$,if $3 \ mole$ of $H_2O$ are electrolysed,then how much charge (in $F$) is required if the current efficiency is $75 \ \%$?

$A$ solution of sodium sulphate in water is electrolysed using inert electrodes. The products at the cathode and anode are respectively:

Explain: Oxidation of $Cl^{-}$ ion is carried out near the anode when electrolysis of aqueous (concentrated) $NaCl$ solution is carried out using an inert electrode.

Which of the following is $NOT$ produced during the electrolysis of brine solution?

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