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Question

When an aqueous solution of AgNO3 is electrolysed between platinum electrodes, which of the following is true?

A
Silver is deposited at cathode and O2 is liberated at anode
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B
Silver is deposited at cathode and dissolved at anode
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C
H2 is liberated at cathode and O2 is liberated at anode
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D
Silver is deposited at cathode and H2 is liberated at anode
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Solution

The correct option is A Silver is deposited at cathode and O2 is liberated at anode

Electrolysis of aqueous AgNO3:
Platinum electrode is an inert electrode.
This metal electrode doesn’t involve in the redox reaction of the cell.
Hence, this electrode can conduct electrons into or out of the cell but cannot take part in the half-reactions.

At cathode:
Ag+(aq)+eAg(s);E0Ag+/Ag=0.80 V

2H2O(l)+2eH2(g)+2OH(aq)
E0H2O/H2=0.83 V

The reaction with a higher reduction value of E0 takes place at the cathode. Therefore, deposition of silver will take place at the cathode.

At anode:
Since, Pt electrode are inert, it does not involve in redox reaction of cell.
Therefore, OH or NO3 ions can be oxidized at anode.
But OH ions having higher oxidation potential, therefore they get oxidised to O2
NO3 can't be further oxidised because already nitrogen attains its highest oxidation state (+5).
Anode reaction:
2H2O(l)4H+(aq)+O2(g)+4e

Hence, option (a) is correct.




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