The introductory electrolysis of CuSO4 (copper sulfate) involves the use of an electrochemical cell to carry out a redox reaction, resulting in the deposition of copper metal onto the cathode and the evolution of oxygen gas at the anode.
Here is the process of the introductory electrolysis of CuSO4:
Setup: Prepare an electrolytic cell with a suitable container, such as a beaker. Place a copper sulfate solution in the cell, ensuring that it covers both the cathode and the anode. The cathode is typically a metal electrode, such as a copper electrode, while the anode can be made of inert material like platinum or carbon.
Electrolyte: The copper sulfate solution acts as the electrolyte, providing copper ions (Cu2+) and sulfate ions (SO42-) necessary for the electrochemical reaction. Initially, the solution is blue due to the presence of copper ions.
Cathode: Connect the cathode to the negative terminal of a power supply or battery. When the power supply is turned on, electrons flow from the cathode to the cathode compartment of the electrolytic cell.
Anode: Connect the anode to the positive terminal of the power supply. The anode compartment is where oxidation occurs. At the anode, water molecules undergo electrolysis, resulting in the liberation of oxygen gas (O2) and the generation of hydrogen ions (H+). The oxygen gas is typically seen as bubbles.
Reduction at Cathode: Copper ions (Cu2+) from the copper sulfate solution are attracted to the cathode, where they gain electrons from the cathode and get reduced to copper metal (Cu). As a result, a layer of copper metal gradually builds up on the surface of the cathode. This leads to a decrease in the concentration of copper ions in the solution.
Oxidation at Anode: In the anode compartment, the oxidation of water molecules occurs. Water molecules (H2O) lose electrons and are converted into oxygen gas (O2) and hydrogen ions (H+). The hydrogen ions typically remain in the solution, contributing to the acidity.
Overall, the introductory electrolysis of CuSO4 leads to the deposition of copper metal onto the cathode while oxygen gas evolves at the anode. This process can be used for various applications, including electroplating, purification of copper, and studying redox reactions.