Titration: Principles, Types & Indicators

Principle, Theory, and Types of Titration

Fundamentals of titration in analytical chemistry and role of indicators

1. Principle of Titration

Fundamentals and principles of titration processes.

2. Chemical Theory of Titration

Chemical theory underlying titration reactions and equilibria.

3. Types of Titration

Classification and examples of different titration methods.

4. Chemical Indicators

Role and selection of chemical indicators in titrations.

5. Applications and Conclusion

Practical applications and final summary of titration.

01

Principle of Titration

Determination of concentration through stoichiometric reaction with known solution

• Based on acid-base, redox, precipitation or complexation reactions
• Equivalence point: reactants in stoichiometric proportion
• Titration curve shows pH or potential changes

• Titration determines unknown concentration using known solution.
• Theory based on stoichiometric reaction equivalence point.
• Types: acid-base, redox, complexometric, precipitation.
• Indicators change color at endpoint, e.g., phenolphthalein pink in base.

• Equivalence point where moles of acid equal base.
• pH changes sharply around equivalence point.
• Indicator transitions color at endpoint.

• Acid-base indicators change color with pH (e.g., phenolphthalein pink at pH 8-10)
• pKa close to equivalence point for optimal change
• Detect end point approximate to equivalence point

• 3.7: Methyl Orange pKa

Red (3.1-4.4) to yellow

• 9.3: Phenolphthalein pKa

Colorless (8.2-10) to pink

• 4.4: Bromocresol Green pKa

Yellow (3.8-5.4) to blue

• 7.0: Bromothymol Blue pKa

Yellow (6.0-7.6) to blue

• ±1: Ideal pKa

Near equivalence pH

Precise titration: key in chemical analysis.

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