Why doesn't water undergo electrolysis?

Why does Na2SO4 undergo electrolysis?

Water does indeed undergo electrolysis. Electrolysis is a chemical process that uses an electric current to drive a non-spontaneous reaction. In the case of water, electrolysis can separate it into its component elements, hydrogen and oxygen gas.

When an electric current is passed through water, it breaks down into its positive and negative ions. The positive ions (H+) are attracted to the negative electrode (cathode) while the negative ions (OH-) are attracted to the positive electrode (anode). At the cathode, hydrogen gas (H2) is produced, and at the anode, oxygen gas (O2) is produced. This happens because the electric current provides the energy required to overcome the energy barrier for the reaction to occur.

On the other hand, Na2SO4 (sodium sulfate) does undergo electrolysis because it dissociates into its component ions, sodium (Na+) and sulfate (SO4^2-) ions, in an aqueous solution. These ions are mobile and can move towards their respective electrodes during electrolysis. At the cathode, sodium ions are reduced to produce sodium metal, while at the anode, sulfate ions are oxidized to produce oxygen gas. The specific products of electrolysis depend on factors such as the type of electrodes used and the concentration of the solution.

In summary, water and Na2SO4 both undergo electrolysis, but the specific products formed depend on the nature of the substances and the conditions of the electrolysis process.