B.Pharmacy 1st Semester Pharmaceutical Analysis Notes Download Pdf

1st Semester

Complete B.Pharm 1st Semester Pharmaceutical Analysis Notes Unit 1 to 5 explained with syllabus, titrations, limit tests, errors, and pharmaceutical applications for exam preparation.

B.pharmacy 1st sem Pharmaceutical Analysis Notes

Unit 1

1. Definition & Scope

  • Pharmaceutical Analysis is defined as the branch of chemistry that deals with the process of determining the identity, quality, and quantity of pharmaceutical substances and formulations.
  • Scope includes:
    • Checking purity of drugs.
    • Determining active pharmaceutical ingredients (APIs).
    • Ensuring safety by testing for impurities.
    • Standardizing raw materials.

2. Types of Analysis

  • Qualitative Analysis – determines the presence of a substance (e.g., chloride test in sodium chloride).
  • Quantitative Analysis – determines the amount of a substance (e.g., % purity of aspirin tablet).

3. Techniques of Analysis

  1. Chemical Methods –
    • Titrimetric analysis (volumetric analysis).
    • Gravimetric analysis.
  2. Instrumental Methods –
    • UV-Visible spectroscopy, chromatography, potentiometry, etc.

4. Errors in Pharmaceutical Analysis

  • Determinate (Systematic) Errors: reproducible errors like wrong standard solution preparation.
  • Indeterminate (Random) Errors: occur by chance, e.g., reading fluctuation in burette.
  • Personal Errors: due to observer, e.g., parallax error.
  • Instrumental Errors: due to faulty instruments.

5. Minimization of Errors

  • Calibration of instruments.
  • Careful handling of reagents.
  • Use of blank determinations.
  • Repetition of experiments.

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Unit 1 Notes

Unit 2

1. Theories of Acids and Bases

  • Arrhenius Theory: Acid produces H⁺, base produces OH⁻.
  • Bronsted-Lowry Theory: Acid = proton donor, Base = proton acceptor.
  • Lewis Theory: Acid = electron pair acceptor, Base = electron pair donor.

2. Neutralization Reactions

  • Example: HCl + NaOH → NaCl + H₂O.
  • Used to assay strong and weak acids/bases.

3. Buffers

  • Solutions that resist pH changes.
  • Example: Acetate buffer (CH₃COOH + CH₃COONa).
  • Role in pharmacy: maintains stability of drugs, used in biological systems.

4. Indicators

  • Substances that show endpoint by color change.
  • Examples:
    • Phenolphthalein (colorless → pink).
    • Methyl orange (red → yellow).

5. Non-Aqueous Titrations

  • Carried out in solvents other than water.
  • Useful for weak acids/bases insoluble in water.
  • Example: Assay of sodium benzoate using non-aqueous titration.

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Unit 2 Notes

Unit 3

1. Principle

  • Based on oxidation and reduction reactions.
  • Oxidizing agent → accepts electrons.
  • Reducing agent → donates electrons.

2. Common Redox Reagents

  • Potassium permanganate (KMnO₄) – strong oxidizing agent.
  • Potassium dichromate (K₂Cr₂O₇) – oxidizing agent.
  • Iodine (I₂) – used in iodometry and iodimetry.
  • Cerium salts (Ce⁴⁺) – oxidizing agents.

3. Indicators in Redox Titrations

  • Self-indicator: KMnO₄ acts as its own indicator.
  • Starch solution: used in iodine titrations (blue complex).
  • Diphenylamine: used with dichromate titrations.

4. Examples of Redox Titrations

  • Permanganometry: Assay of ferrous sulfate using KMnO₄.
  • Iodimetry/Iodometry: Determination of ascorbic acid, copper salts.
  • Cerimetry: Assay of ferrous ammonium sulfate.

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Unit 3 Notes

Unit 4

1. Precipitation Titrations

  • Based on the formation of insoluble precipitates.
  • Common methods:
    • Mohr’s Method: Uses chromate indicator. Example: Estimation of chloride using AgNO₃.
    • Volhard’s Method: Back titration using thiocyanate.
    • Fajans’ Method: Uses adsorption indicators like fluorescein.

2. Complexometric Titrations

Assay of calcium gluconate, magnesium salts, zinc oxide.

Based on complex formation between metal ions and ligands.

Common ligand: EDTA (Ethylenediaminetetraacetic acid).

Metal indicators: Eriochrome Black T (EBT), Murexide.

Applications:

Determination of hardness of water.

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Unit 4 Notes

Unit 5

1. Gravimetric Analysis

  • Based on measurement of mass of a substance.
  • Steps:
    1. Precipitation of analyte.
    2. Filtration.
    3. Washing.
    4. Drying/Ignition.
    5. Weighing.
  • Example: Estimation of barium as barium sulfate.

2. Limit Tests

  • Used to detect small quantities of impurities in pharmaceuticals.
  • Limit Test for Chlorides: Precipitation with silver nitrate.
  • Limit Test for Sulphates: Precipitation with barium chloride.
  • Limit Test for Iron: Color comparison with thioglycolic acid.
  • Limit Test for Arsenic: Reduction to arsine gas (Gutzeit test).
  • Limit Test for Heavy Metals: Formation of colored sulfide precipitate.

3. Pharmaceutical Applications

  • Ensures drugs are free from toxic impurities like arsenic, lead, and mercury.
  • Maintains Indian Pharmacopoeia (IP) and USP standards.

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Unit 5 Notes

Pharmaceutical Analysis Notes Overview

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