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Introduction to Acid-Base Reactions

Acid-base reactions involve the transfer of protons (H⁺ ions) between reactants. These reactions are central in chemistry, biology, and environmental processes.

Key Concepts​

  • Acid: Proton donor (Bronsted-Lowry definition)
  • Base: Proton acceptor (Bronsted-Lowry definition)
  • pH: Measure of hydrogen ion concentration; pH = −log[H⁺]
  • pOH: Measure of hydroxide ion concentration; pOH = −log[OH⁻]

Types of Acid-Base Reactions​

  1. Strong Acid + Strong Base

    • Complete dissociation in water
    • Example: HCl + NaOH → NaCl + H₂O

  2. Weak Acid + Strong Base

    • Partial dissociation of weak acid
    • Example: CH₃COOH + NaOH → CH₃COONa + H₂O

  3. Strong Acid + Weak Base

    • Example: HCl + NH₃ → NH₄Cl

  4. Neutralization Reactions

    • Formation of water and a salt from an acid and a base

Importance​

  • Understanding acid-base reactions is critical for:
    • Buffer solutions
    • Titration calculations
    • Biological systems (enzyme activity, blood pH)
    • Environmental chemistry (acid rain, water treatment)

Indicators​

  • Substances that change color depending on pH
  • Examples: Litmus paper, phenolphthalein, bromothymol blue

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