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Electrolysis of dilute sulfuric acid The products of electrolysing water acidified with sulfuric acid are hydrogen gas and oxygen gas Two experimental setups are described, the Hofmann voltameter demonstration (left diagram) and a simple cell (right diagram) for use in schools and colleges for pupils to use. Dilute sulfuric acid is used as the electrolyte in this investigation. The Hofmann voltameter is filled with the electrolyte (sulphuric acid) by opening the taps at the top of the outer tubes to allow any gas to escape. The gases formed on the electrolysis of the dilute sulfuric acid can be collected via the same taps. The platinum or carbon electrodes are inert. You need inert (non–reactive) electrodes like platinum (left) and much cheaper carbon (graphite, right). In the simple electrolysis cell, the graphite (carbon) electrodes are, through a large rubber bung, 'upwardly' dipped into an solution of acidified water. In this cheap and simple apparatus the gaseous products (hydrogen and oxygen) are collected in small test tubes inverted over the carbon electrodes. You have to fill the little test tubes with the electrolyte (dil. sulfuric acid), hold the liquid in with your finger and carefully invert them over the nearly full electrolysis cell. The gases can be collected and tested. Students should note that the electrolysis will only take place when electricity is passed through the dilute sulfuric acid solution. Both gasses can be collected with a small plastic test tube and ignited with a lit splint, giving a satisfying pop. The electrolyte is dilute sulphuric acid (= acidified water) which, during electrolysis is split into hydrogen and oxygen gases. Theoretically into a 2 : 1 ratio by gas volume. This is one experimental method of showing water is a compound composed of the elements hydrogen and oxygen atoms i.e. by splitting liquid water into two gaseous element molecules of hydrogen (H2) and oxygen (O2). Water only ionises to a tiny extent giving minute concentrations of hydrogen ions and hydroxide ions, so the presence of high concentrations of hydrogen ions (H+ or H3O+) and sulfate ions (SO42–) from the acid, makes water a much better electrical conductor (a much better electrolyte solution). These small extra ion concentrations of hydrogen ions (H+) and hydroxide ions (OH–) are from the self-ionisation of water itself.PDF Image | ELECTROLYSIS OF SALT WATER
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