Two electrolytic cells for solutions in a (i) and (ii) respectively were connected in series. A current of 1.5 A was passed for 600 seconds. The first cell contained aqueous copper (II) sulphate and had copper electrodes. The anode showed a loss in mass of 0.296 g but there was no change in the appearance of the electrolyte. The sodium chloride with little sodium hydroxide had copper electrodes and a reddish brown precipitate formed.

(i) Why was there no change in the appearance of the electrolyte in the first cell

(ii) Why was a small amount of sodium hydroxide added to aqueous sodium chloride in the second cell?

(iii) Name the reddish- brown precipitate formed (1 mk)

(iv) Write an ionic equation for the formation of substance in (iii)

(v) Calculate the value of Faraday constant (1 mk)

Answer rating: 100% (QA)

i There was no change in the appearance of the electrolyte in the first cell because the reaction ta... View the full answer