Practical: Investigate the electrolysis of aqueous solutions
Aim:
To electrolyse aqueous solutions of sodium chloride, sulfuric acid and copper(II)sulfate, and to collect and identify the products at each electrode
Diagram:
Electrolysis cell for collecting gaseous products from aqueous solutions
Method:
- Add the aqueous solution to a beaker and cover the electrodes with the solution
- Invert two small test tubes to collect any gaseous products
- Connect the electrodes to a power pack or battery
- Turn on the power pack or battery and allow electrolysis to take place
- Observations at each electrode are made
- Gases collected in the test tube can be tested and identified
Testing the products
- If the gas produced at the cathode burns with a ‘pop’ when a sample is lit with a lighted splint, the gas is hydrogen
- If the gas produced at the anode relights a glowing splint dipped into a sample of the gas, the gas is oxygen
- If the anode gas bleaches of a piece of litmus paper, chlorine has been produced
- If a solid forms around the electrode, the metal have been formed
- The colour can indicate the metal formed
Results:
Solution | Cathode observation | Anode observation |
Sodium chloride | Colourless gas evolved which goes 'pop' with a lighted splint | Gas evolved which bleaches litmus paper |
Dilute sulfuric acid | Colourless gas evolved which goes 'pop' with a lighted splint | Colourless gas evolved which relights a glowing splint |
Copper(II) sulfate | Pink-brown deposit seen on the electrode | Colourless gas evolved which relights a glowing splint |
Conclusions:
- Sodium chloride solutions produces hydrogen at the cathode and chlorine at the anode
- Dilute sulfuric acid produces hydrogen at the cathode and oxygen at the anode
- Copper(II)sulfate solution produces copper at the cathode and oxygen at the anode