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Predict the products of electrolysis in each of the following: (i) An aqueous solution of AgNO_(3) with silver electrodes. (ii) An aqueous solution of AgNO_(3) with platinum electrodes. |
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Answer» Solution :(i) Electrolysis of aqueous solution of `AgNO_(3)` using silver electrodes : `AgNO_(3)(s)overset("water")toAg^(+)(aq)+NO_(3)^(-)(aq)` `H_(2)OhArrH^(+)OH^(-)` cathode. `Ag^(+)` ions have lower discharge potential than `H^(+)` ions. Hence `Ag^(+)` ions will be deposited as silver (in preference to `H^(+)` ions) At ANODE. Since silver electrode is attacked by `NO_(3)^(-)` ions, Ag anode will DISSOLVE to form `Ag^(+)` ions in the solution. `Ag""toAg^(+)+e^(-)` (ii) Electrolysis of aqueous solution of `AgNO_(3)` using platinum electrodes : At cathode. Same as above. At anode. Since silver is not attacked, out of `OH^(-)` and `NO_(3)^(-)` ions, `OH^(-)` ions have lower discharge potential and hence `OH^(-)` ions will be discharged in preference to `NO_(3)^(-)`. The `OH^(-)` will decompose to give `O_(2)`. `OH^(-)(aq)toOH+e^(-)` `4OHto2H_(2)O(l)+O_(2)(g)` |
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