Summary
The Brønsted–Lowry theory defines acids as proton donors and bases as proton acceptors. Acids increase the concentration of H+ ions in solution, while bases decrease it.
- Acid — A substance that donates protons (H+ ions) in a solution. Example: Hydrochloric acid (HCl) donates H+ ions in water.
- Base — A substance that accepts protons (H+ ions) in a solution. Example: Sodium hydroxide (NaOH) accepts H+ ions in water.
- Strong Acid — Completely dissociates in aqueous solution to release ions. Example: Sulfuric acid (H2SO4) fully dissociates in water.
- Weak Acid — Partially dissociates in aqueous solution to release ions. Example: Ethanoic acid (CH3COOH) partially dissociates in water.
- Strong Base — Fully dissociates in aqueous solution to release OH- ions. Example: Potassium hydroxide (KOH) fully dissociates in water.
- Weak Base — Partially dissociates in aqueous solution to release OH- ions. Example: Ammonia (NH3) partially dissociates in water.
- Neutralization Reaction — Reaction where H+ and OH- ions form water. Example: HCl reacting with NaOH to form water and salt.
Exam Tips
Key Definitions to Remember
- Acid: Proton donor
- Base: Proton acceptor
- Strong Acid: Completely dissociates in solution
- Weak Acid: Partially dissociates in solution
- Strong Base: Fully dissociates in solution
- Weak Base: Partially dissociates in solution
Common Confusions
- Strong vs. concentrated: Strong refers to dissociation, concentrated refers to amount
- Weak vs. dilute: Weak refers to partial dissociation, dilute refers to low concentration
Typical Exam Questions
- What is a Brønsted–Lowry acid? A substance that donates protons (H+ ions).
- How does a strong acid differ from a weak acid? A strong acid completely dissociates in solution, while a weak acid only partially dissociates.
- What happens during a neutralization reaction? H+ ions react with OH- ions to form water.
What Examiners Usually Test
- Understanding of acid and base definitions
- Differences between strong and weak acids/bases
- Ability to explain neutralization reactions