Electrolysis of Water and Copper sulfate

Electrolysis Process of H₂O and CuSO₄ Solutions

Electrolysis of Water (H₂O)

Pure water does not conduct electricity well, so a small quantity of an acid, base, or salt is usually mixed in to enhance its electrical conductivity. When electric current passes through water during electrolysis, it breaks down into its basic elements, hydrogen and oxygen gases.

Chemical reaction:

2H₂O (l) → 2H₂ (g) + O₂ (g)

What happens at the electrodes:

• Cathode (negative electrode): Hydrogen ions (H⁺) gain electrons (reduction) to form hydrogen gas.
  Reaction: 2H⁺ + 2e⁻ → H₂ (gas)
• Anode (positive electrode): At the anode, hydroxide ions (OH⁻) undergo oxidation by releasing electrons, producing oxygen gas and water.
  Reaction: 4OH⁻ → O₂ (gas) + 2H₂O + 4e⁻

Thus, hydrogen gas is collected at the cathode, and oxygen gas is collected at the anode in the ratio of 2:1.

Electrolysis of Copper Sulfate (CuSO₄) Solution

Copper sulfate is frequently used as an electrolyte in electrolysis experiments. When its solution is subjected to electrolysis with copper electrodes, copper is deposited on the cathode, while oxygen gas is produced at the anode.

Chemical reactions:

• Cathode (negative electrode): At the cathode, copper ions (Cu²⁺) receive electrons and are reduced to form solid copper metal.
  Reaction: Cu²⁺ + 2e⁻ → Cu (metal)
• Anode (positive electrode): Water molecules lose electrons to form oxygen gas and hydrogen ions.
  Reaction: 2H₂O → O₂ (gas) + 4H⁺ + 4e⁻

The copper deposited on the cathode appears as a solid layer, and oxygen gas bubbles form at the anode. The sulfate ions (SO₄²⁻) remain in the solution and do not undergo any reaction.

In electrolysis, water breaks down into hydrogen and oxygen gases, while copper sulfate solution produces copper metal at the cathode and oxygen gas at the anode. These processes are widely used in industries for extraction and purification of metals and for producing gases.