Understanding Acid-Base Chemistry

📋 Course Outline

1. Acid-Base Definitions
2. pH Scale and Calculation
3. Strong vs. Weak Acids/Bases
4. Acid-Base Theories
5. Neutralization Reactions
6. Titration Methods
7. pH Indicators
8. Buffer Solutions and Capacity
9. Biological Buffer Systems
10. Environmental Acid-Base Impact
11. Salt Properties in Solution

📖 1. Acid-Base Definitions

🔑 Key Concepts & Definitions

• Acid (Arrhenius Definition): A substance that increases the concentration of H⁺ ions (protons) in aqueous solution.
  Example: HCl dissociates to produce H⁺ and Cl⁻.

• Base (Arrhenius Definition): A substance that increases the concentration of OH⁻ ions in aqueous solution.
  Example: NaOH dissociates to produce Na⁺ and OH⁻.

• Proton (H⁺) Donor (Brønsted-Lowry Definition): An acid is a substance that donates a proton to another species.
  Example: H₂SO₄ donates H⁺ ions in solution.

• Proton (H⁺) Acceptor (Brønsted-Lowry Definition): A base is a substance that accepts a proton from another species.
  Example: NH₃ accepts H⁺ to form NH₄⁺.

• Electron Pair Acceptor (Lewis Definition): An acid is a substance that can accept a pair of electrons to form a covalent bond.
  Example: BF₃ accepts an electron pair from NH₃.

• pH: A logarithmic scale measuring the acidity or alkalinity of a solution, calculated as (\text{pH} = -\log[H^+]).
  Range: 0 (most acidic) to 14 (most basic), with 7 being neutral.

📝 Essential Points