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Introduction to Titration

Titration is a laboratory technique used to determine the concentration of a solution by reacting it with a solution of known concentration.

Key Concepts​

  • Analyte: The solution whose concentration is unknown
  • Titrant: The solution of known concentration used to react with the analyte
  • Equivalence Point: Point where the amount of titrant exactly neutralizes the analyte
  • End Point: Point indicated by a color change of an indicator, close to the equivalence point

Types of Titrations​

  1. Acid-Base Titration

    • Determines concentration of an acid or base
    • Common indicators: phenolphthalein, bromothymol blue

  2. Redox Titration

    • Involves electron transfer reactions
    • Example: Titration of Fe²⁺ with KMnO₄

  3. Complexometric Titration

    • Forms complexes with metal ions
    • Example: EDTA titrations for hardness of water

  4. Precipitation Titration

    • Formation of a precipitate signals completion
    • Example: AgNO₃ titration for Cl⁻ ions

Importance​

  • Accurate determination of solution concentration
  • Used in industrial quality control, environmental testing, and laboratory research
  • Helps understand reaction stoichiometry and chemical equivalence

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