What are Electrolytes

 What are Electrolytes?

Definition

Electrolytes are substances that conduct electricity when dissolved in water or in a molten state by producing free-moving ions.

Explanation

When an electrolyte dissolves in water or melts, it splits into positive and negative ions. These ions move freely, allowing electric current to pass through. Electrolytes are essential in electrolysis because they supply the charged particles needed for chemical reactions at the electrodes.

They may be acids, bases, or salts, and their strength depends on how well they dissociate into ions.

Key Points

• Conduct electricity by producing mobile ions

• Needed for electrolysis to occur

• Can be solid (molten) or liquid (aqueous solution)

• Include strong and weak electrolytes

• Enable redox reactions at electrodes

Types of Electrolytes

 1. Strong Electrolytes – Completely dissociate (e.g., NaCl, HCl)

 2. Weak Electrolytes – Partially dissociate (e.g., CH₃COOH)

 3. Non-electrolytes – Do not conduct electricity (e.g., sugar solution)

Examples

• NaCl (salt water) → Na⁺ and Cl⁻ ions

• H₂SO₄ (sulfuric acid) → H⁺ and SO₄²⁻ ions

• CuSO₄ solution used in copper electrolysis

• Molten Al₂O₃ in aluminium extraction

Applications / Relevance

• ⚡ Electrolysis of compounds in industry

• 🔋 Function of batteries and electrochemical cells

• 💧 Biological systems (body electrolytes like Na⁺, K⁺, Cl⁻)

• ⚗️ Electroplating and purification of metals

• 🚰 Water treatment and testing conductivity

Question

Why can solid salt not conduct electricity but saltwater can?

Answer:

Because ions in solid salt are fixed in place, but in saltwater, they are free to move and carry electric cu