What is the difference between a strong and weak electrolyte?

An electrolyte is a substance that produces ions when dissolved in water, allowing the solution to conduct electricity. The difference between strong and weak electrolytes lies in how completely they ionize (break into ions).

🔹 Strong Electrolyte

• Definition: Substances that completely dissociate (ionize) into ions in water.
• Ionization: Nearly 100% of solute molecules turn into ions.
• Conductivity: Very high, because there are lots of free ions to carry current.
• Examples:
  • Salts: Sodium chloride (NaCl), Potassium nitrate (KNO₃)
  • Strong acids: Hydrochloric acid (HCl), Sulfuric acid (H₂SO₄)
  • Strong bases: Sodium hydroxide (NaOH), Potassium hydroxide (KOH)

🔹 Weak Electrolyte

• Definition: Substances that only partially dissociate into ions in water.
• Ionization: Only a small fraction of molecules form ions; most remain as molecules.
• Conductivity: Low, because fewer free ions are present.
• Examples:
  • Weak acids: Acetic acid (CH₃COOH), Carbonic acid (H₂CO₃)
  • Weak bases: Ammonia (NH₃ in water)
  • Some salts: Mercury(II) chloride (HgCl₂)

Key Difference in One Line:

• Strong electrolytes ionize completely and conduct electricity well.
• Weak electrolytes ionize partially and conduct electricity poorly.