Hydrogen peroxide is largely manufactured by the electrolysis of 50% Sulphuric acid at between platinum anode and lead cathode separated by a porous diaphragm.
50% Sulphuric acid solution is taken in a stoneware vessel. A platinum rod is dipped in the solution which acts as anode. A lead wire acts as the cathode. These two electrodes are separated of a porous diaphragm.
The vessel is placed in a trough of ice to maintain the temperature at .
On passing current the following reactions takes place.
Oxidizing properties :
decomposes as [O]. Because of this tendency, it acts as powerful oxidant.
It oxidizes black lead sulphide to white lead sulphate.
It oxidizes potassium iodide to iodine in presence of sulphuric acid.
It oxidizes ferrous sulphate to ferric sulphate in presence of sulphuric acid.
Reducing Properties :
acts as a reducing agent because of the ease with which it accepts nascent oxygen from other oxidising agent.
It reduces moist silver oxide to metallic silver.
It reduces ozone to oxygen.
It decolourises acidified potassium permanganate solution.