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Electrochemistry

Question
CBSEENCH12005934
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Predict the products of electrolysis in each of the following:
(i) An aqueous solution of AgNO3 with silver electrodes.
(ii) An aqueous solution of AgNO3 with platinum electrodes.
(iii) A dilute solution of H2SO4 with platinum electrodes.
(iv) An aqueous solution of CuCl2 with platinum electrodes.

Solution
Answer:


At cathode: Ag+ are preferably discharged as compared to H+ as its reduction potential is higher

Ag++e- → Ag(s)

At anode: Silver electrode (being reactive) dissolves to produce Ag+



As the electrodes are inert, these do not take part in the reaction. At cathode, Ag+ ions are discharged in preference to H+ ions and OH– are discharged in preference to NO3– ions at anode

Here, only H+ are discharged at cathode as there is no other positive ion. Out of OH– and SO42– ions, OH– ions are discharged at anode preferably



The platinum electrodes are inert and do not take part in the reaction. The following reactions occur at platinum (inert) electrodes.

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