NCERT Class XII Chemistry
Chapter - Electrochemistry
Questions with Solutions
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Question : 18
Total: 32
Predict the product of electrolysis in each of the following:
(i) An aqueous solution ofA g N O 3 with silver electrodes.
(ii) an aqueous solution ofA g N O 3 with platinum electrodes.
(iii) A dilute solution ofH 2 S O 4 with platinum electrodes.
(iv) An aqueous solution ofC u C l 2 with platinum electrodes.
(i) An aqueous solution of
(ii) an aqueous solution of
(iii) A dilute solution of
(iv) An aqueous solution of
Solution:
(i) Electrolysis of aqueous solution of A g N O 3 with silverelectrodes,
A g N O 3 ( s ) + a q – – – – – ▶ A g + ( a q ) + N O – 3 ( a q )
H 2 O ⇌ H + + O H −
At cathode: Ag+ ions have lower discharge potential than H+ ions. Hence,Ag+ ions will be deposited as Ag in preference to H+ ions.
At anode: As Ag anode is attacked by NO– 3 ions, Ag of the anode willdissolve to form Ag+ ions in the solution.
A g – – – – – ▶ A g + + e –
(ii) Electrolysis of aqueous solution ofA g N O 3 using platinum electrodes,
At cathode: Ag will be deposited.
At anode: As anode is not attacked, out of OH– and NO– 3 ions, OH– ionshave lower discharge potential. Hence, OH– ions will be discharged inpreference to NO– 3 ions, and OH– will then decompose to give out O2 .
O H – ( a q ) – – – – – ▶ O H + e – ,
4 O H – – – – – ▶ 2 H 2 O ( l ) + O 2 ( g )
(iii) Electrolysis of diluteH 2 S O 4 with platinum electrodes,
H 2 S O 4 ( a q ) 2 H + ( a q ) + S O 2 – 4 ( a q )
H 2 O ⇌ H + + O H –
At cathode:H + + e – – – – – – ▶ H ,
H + H – – – – – ▶ H 2 ( g )
At anode:O H – – – – – – ▶ O H + e – ,
4 O H – – – – – ▶ 2 H 2 O + O 2 ( g )
Thus,H 2 is liberated at the cathode and O 2 at the anode.
(iv) Electrolysis of aqueous solution ofC u C l 2 with platinum electrodes,
C u C l 2 ( s ) + a q – – – – – ▶ C u 2 + ( a q ) + 2 C l – ( a q )
H 2 O ⇌ H + + O H –
At cathode:C u 2 + ions will be reduced in preference to H + ions.
C u 2 + + 2 e – – – – – – ▶ C u
At anode: Cl– ions will be oxidized in preference to OH– ions.
C l – – – – – – ▶ C l + e – ,
C l + C l – – – – – ▶ C l 2 ( g )
Thus, Cu will be deposited on the cathode andC l 2 will be liberated at theanode.
At cathode: Ag
At anode: As Ag anode is attacked by NO
(ii) Electrolysis of aqueous solution of
At cathode: Ag will be deposited.
At anode: As anode is not attacked, out of OH
(iii) Electrolysis of dilute
At cathode:
At anode:
Thus,
(iv) Electrolysis of aqueous solution of
At cathode:
At anode: Cl
Thus, Cu will be deposited on the cathode and
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