Lecture Notes: Acid and Base Reactions

Introduction

• Presenter: Robert Smith
• Institution: New River Community College's Academic Assistance
• Topic: Classifying species as Bronsted acids or bases

Key Concepts

• Bronsted Acid: A substance that donates a proton (hydrogen ion) in a solution.
• Bronsted Base: A substance that accepts a proton in a solution.

Examples and Explanations

1. Hydrochloric Acid (HCl)

• Dissociation Equation: HCl (aq) → H⁺ (aq) + Cl⁻ (aq)
  • HCl splits into a hydrogen ion (proton) and a chlorine ion in aqueous solution.
• Classification:
  • Bronsted Acid
  • Reason: It donates a proton (H⁺) in solution.

2. Phosphate Ion (PO₄³⁻)

• Proton Accepting Reaction: PO₄³⁻ (aq) + 3H⁺ (aq) → H₃PO₄ (aq)
  • Phosphate ion accepts three hydrogen ions to form H₃PO₄.
• Classification:
  • Bronsted Base
  • Reason: It accepts protons in solution.

3. Sulfuric Acid (H₂SO₄)

• Proton Donating Reaction:
  • H₂SO₄ in an aqueous solution separates to release two protons.
• Ion Charge:
  • Sulfate ion (SO₄²⁻) is identified as having a 2- charge after the release of two protons.
• Classification:
  • Bronsted Acid
  • Reason: It donates protons in solution.

Conclusion

• Understanding whether a species is a Bronsted acid or base helps in predicting chemical behavior in reactions.
• The process involves observing whether a compound donates or accepts protons in a solution.
• Key takeaway: Bronsted acids donate protons, while Bronsted bases accept protons.