After successful completion of course student will able to

1. Pharmaceutical Analysis
(BP102T) Subject Orientation

2. Teaching Scheme
 Evaluation scheme
 Syllabus
 Course Objectives
 Course Outcomes
 Previous Question Paper
Overview

3. Teaching & Evaluation Scheme
Course
Code
Course Name Lectures Assigned
Theory Practical Tutorial Total
BP102T Pharmacy 03 Hrs. per
week
04 Hrs. per
week
01 Hrs. per
week
04 Hrs. per
week
Course
Code
Course
Name
Evaluation Scheme
BP102T Pharmacy Theory Practical Total
Credit
4
Internal
25
External
75
Total
100
Internal
15
External
35
Total
50

4. Evaluation Guidelines
 End Semester Examination [ 75 Marks]:
Paper pattern and marks distribution for End Semester Exam: As per
university guideline.
Internal Examination [ 25 Marks]:
Sessional exam shall be conducted for 30 marks for theory and shall be
computed for 15 marks. Similarly Sessional exam for practical shall
be conducted for 40 marks and shall be computed for 10 marks.
Sr. no Question type Marks
1 Objective Types Questions (Answer 5 out of 7) 5x3=15
2 Long Answers (Answer 2 out of 4) 2x10=20
3 Short Answers (Answer 8 out of 10) 8x5=40
Total = 75M

6. Course Outcomes (COs):
After successful completion of course student will able to
 CO1
 After successful completion of course student will able to Explain volumetric
analysis method for estimation of selected compound officially
pharmacopeia.
 CO2
 After successful completion of course student will able to Explain
electrochemical analysis method for estimation of selected compound
officially pharmacopeia.
 CO3
 After successful completion of course student will able to Explain
gravimetric analysis method for estimation of selected compound officially
pharmacopeia.
 CO4
 After successful completion of course student will able to Explain various
method of expressing conc. & uses of primary and secondary std. for
chemical analysis.
 CO5
 After successful completion of course student will able to Explain error in
measurement.

7. UNIT-I
 Pharmaceutical analysis-
 Definition and scope
 Different techniques of analysis
 Methods of expressing concentration
 Primary and secondary standards.
 Preparation and standardization of various molar and normal
solutionsOxalic acid, sodium hydroxide, hydrochloric acid, sodium
thiosulphate, sulphuric acid, potassium permanganate and ceric
ammonium sulphate
 Errors :Sources of errors, types of errors, methods of minimizing errors,
accuracy, precision and significant figures

8. UNIT-II
 Acid base titration:
 Theories of acid base indicators, classification of acid base titrations
and theory involved in titrations of strong, weak, and very weak
acids and bases, neutralization curves.
 Non aqueous titration:
 Solvents, acidimetry and alkalimetry titration and estimation of
Sodium benzoate and Ephedrine HCl

9. UNIT-III
 Precipitation titrations:
 Mohr’s method, Volhard’s, Modified Volhard’s, Fajans method,
estimation of sodium chloride.
 Complexometric titration:
 Classification, metal ion indicators, maskingand demasking reagents,
estimation of Magnesium sulphate, and calcium gluconate.
 Gravimetry:
 Principle and steps involved in gravimetric analysis. Purity of the
precipitate: co-precipitation and post precipitation, Estimation of barium
sulphate.

10. UNIT-IV
 Redox titrations
 (a) Concepts of oxidation and reduction
 (b) Types of redox titrations (Principles and applications)
Cerimetry, Iodimetry, Iodometry, Bromatometry, Dichrometry,Titration
with potassium iodate

11. UNIT-V
 Electrochemical methods of analysis
 Conductometry-
 Introduction, Conductivity cell, Conductometric titrations, applications.
 Potentiometry –
 Electrochemical cell, construction and working of reference (Standard
hydrogen, silver chloride electrode and calomel electrode) and indicator
electrodes (metal electrodes and glass electrode), methods to determine end
pointt of potentiometric titration and applications.
 Polarography –
 Principle, Ilkovic equation, construction and working of dropping mercury
electrode and rotating platinum electrode, applications
 Refractometry –
 Introduction, refractive index, specific and molar refraction, measurement
of RI, Abbe’s refractometer and applications

12. Previous Question Paper
 Q1) Answer the following [10 × 2 = 20]
 a) How will you calculate equivalent weight of acid and base? Explain
with example.
 b) Starch indicator give blue color with iodine, justify it.
 c) Define the term normality and molality
 d) Explain accuracy and precision.
 e) Give the preparation of 0. 1N potassium permanganate with reaction.
 f) Give applications of polarography.
 g) Define oxidation and reduction with examples.
 h) How will you standardize 0.05 M disodium EDTA solution?
 i) What is half wave potential? j) How will you prepare and standardize
0.1 N Silver nitrate solution?

13. Previous Question Paper
 Q2) Answer of the following (any two) [2 × 10 = 20]
 a) What is volumetric analysis. Classify them with example. Write
principle, reaction of assay for Boric acid and Aspirin.
 b) Explain methods to determine end point of potentiometric titrations
and its application.
 c) What is complex metric titration? Classify them with example. Write
detailed about types of complexometric titrations.

14. Previous Question Paper
 Q3) Answer the following (any seven) : [7 × 5 = 35]
 a) Explain assay sodium benzoate by non aqueous titration.
 b) Write a note on accuracy and precision.
 c) Give an account on solvents used in non aqueous titration.
 d) Write about limit test of lead.
 e) Write principle and application of Diazotization titrations.
 f) Explain construction and working of dropping mercury electrode.
 g) Write a note on K Fajan’s method?
 h) Explain principle, reaction of calcium gluconate injection.
 i) Explain mechanism of co precipitatio