Ionic theory

Electrolysis

Electrolysis is the decomposition of electrolytes by the passage of an electric current through them.

Electrolyte

An electrolyte is a substance that, either in solution or in molten state, conducts electric current and undergoes decomposition due to its passage. Examples of electrolytes include:

1. H₂SO₄ – Sulphuric acid
2. HNO₃ – Nitric acid
3. NaCl – Sodium chloride

Non-electrolyte

A non-electrolyte is a substance that, in either solution or molten state, does not conduct an electric current. Examples of non-electrolytes include:

1. Sugar
2. Ethanol
3. Urea

Types of electrolytes

i. Strong electrolytes

Strong electrolytes are substances that ionize completely in solution. Some examples are:

1. H₂SO₄ – Sulphuric acid
2. HCl – Hydrochloric acid
3. NaCl – Sodium chloride
4. NaOH – Sodium hydroxide

ii. Weak electrolytes

Weak electrolytes are substances that ionize partially in solution. Some examples include:

1. Weak acids such as CH₃COOH (acetic acid), H₂CO₃ (carbonic acid)
2. Water
3. Weak bases such as NH₃ (ammonia solution) or NH₄OH (ammonium hydroxide)