Department of Pharmacy
24, Mirpur Road; Globe Centre Campus,
Opposite to Dhaka College, Dhaka-1205
Course Outline
Program
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Course Title
|
Course Code
|
Batch
|
Semester
|
Total Credits
|
Credit Hours
|
B. Pharm (Hons.)
|
Physical Pharmacy-I
|
PHARM
1205 | 2A & 2B | Fall-2017 |
For each section
| |
3.0
|
42
| |||||
Load of Credits and Credit Hours (For two sections)
|
3☓2=6
|
42☓2=84
| ||||
Course Teacher : Md. Imran Nur Manik
Designation : Lecturer, Department of Pharmacy
Contact No. : +8801521-540470
E-mail : imrannurmanik@nub.ac.bd
Course Synopsis
Physical Pharmacy is the application of physics and chemistry in the study of pharmaceutics.
This course involves an analysis and application of the principles of physics and chemistry in various important sectors of the pharmaceutical sciences today.
This course involves an analysis and application of the principles of physics and chemistry in various important sectors of the pharmaceutical sciences today.
Rationale
Physical Pharmacy provides the students with the integrated knowledge of the elements of mathematics, chemistry, and physics as they relate to drug dosage form design, development, preparation, sterilization, and evaluation.
Course Objectives
The course aims are:
- To enable the students to obtain fundamental knowledge, outlooks, and expertise related to the study of the physical and chemical properties of pharmaceutical dosage forms, applicable in the performance of future professional responsibilities.
- To make the students understand the chemical and physical phenomena that governs the in-vivo and in-vitro actions of pharmaceutical products, which he or she prepares and dispenses.
- To expertise the students to different types of methods used in the calculations of concentrations of solution, tonicity, predict stability and compatibility.
- To qualify the students to empirically mix the art and descriptive science for the quantitative application of fundamental physical and chemical scientific principles to pharmaceutical systems and dosage forms.
Teaching Learning Strategy
The teaching strategy would be as follows:
⦿ Class lecture
⦿ Home work
⦿ Home assignment
⦿ Demonstration
⦿ Question and answering session
⦿ Group discussion
⦿ Group assignment
⦿ Video tapes etc.
Lecture will mostly be presented in English. Technical terms will be simplified in easy English and can be explained in Bengali terms for better understanding.
Assessment Strategy
The process of collecting, analysing and interpreting information to determine the extent to which learning objectives have been achieved would be mostly as follows:
✰ Sudden test ✰ True/False
✰ Viva voce ✰ MCQ
✰ Short Answer ✰ Mock test
✰ Matching ✰ Assignment
✰ Matching ✰ Assignment
✰ Discussion ✰ Class test etc.
Recommended Books:
- M. M. Haque and M. A. Nawab : Principles of Physical Chemistry
- A. Martin and J. Swarbrick : Martin’s Physical Pharmacy and pharmaceutical Sciences
- P.W. Atkins : Physical Chemistry
- K.K. Sharma and L.K. Sharma : A Textbook of Physical Chemistry
- B.S. Bahl, D.G. Tuli and Arun Bahl : Essentials of Physical Chemistry
- N. Kundu and S.K. Jain : Physical Chemistry
- S. H. Maron and C.F. Prutton : Principles of Physical Chemistry
* Other Books will be indicated as per requirements
Marks Distribution and Evaluation:
Assessment Type
|
Marks Distribution
|
Total
|
Class Test-1
|
10
|
10
|
Class Test-2
|
10
| |
Class Test-3
|
10
| |
Class Test-4
|
10
| |
Presentation and Assignment
|
05
|
05
|
Attendance
|
05
|
05
|
Mid Term
|
30
|
30
|
Semester Final
|
50
|
50
|
Grand Total
|
100
| |
Class Schedule:
Lec. No.
|
Chapter
|
Topics
|
L-01
|
Properties of gases
|
Gas laws, ideal gas equation, Dalton’s law of partial pressure,
|
L-02
|
Diffusion of gases, kinetic theory of gases, mean free path,
| |
L-03
|
Deviation from ideal gas behaviour, Van der Waals equation, critical constants.
| |
L-04
|
Liquefaction of gases, determination of molecular weights, law of corresponding states and heat capacity.
| |
L-05
|
Solutions
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Types and properties of solutions. Units of concentration,
|
L-06
|
Ideal and real solutions. Partition coefficient, distribution of solids between two immiscible liquids and Distribution law
| |
L-07
|
Henry’s law, and solvent extraction.
| |
L-08
|
Class test and Review class.
| |
L-09
|
Ionic equilibria
|
pH, determination of pH of different acids and bases, salt solutions and buffers. Titration curves of acids and bases and indicators.
|
L-10
|
Buffer capacity
|
Preparation of buffers, buffers and isotonic systems.
Methods for adjustment of tonicity of solutions. Buffers in pharmaceutical and biological systems.
|
L-11
|
Class Test and Review Class (Before Mid Semester Exam)
| |
L-12
|
Presentation and Assignment.
| |
L-13
|
Chemical equilibrium
|
Law of mass action, determination of equilibrium constant,
|
L-14
|
Law of mass action,heterogeneous equilibrium and homogenous equilibrium,
| |
L-15
|
Le chateliar principle and Vant hoff equation.
| |
L-16
|
Colligative properties of dilute solutions
|
Lowering of vapor pressure, elevation of boiling point including necessary thermodynamic derivations.
|
L-17
|
Depression of freezing point and osmotic pressure including necessary thermodynamic derivations.
| |
L-18
|
Class Test and Review class
| |
L-19
|
Phase equilibria
|
Phase, components and degrees of freedom,
|
L-20
|
The phase rule and its thermodynamic derivation. The phase diagrams of water and sulphur systems,
| |
L-21
|
Partially miscible liquid pairs: the phenol and water and nicotine-water systems. Completely miscible liquid pairs and their separation by fractional distillation, Sulphur systems Freeze drying (lyophilization).
| |
L-22
|
Chemical thermodynamics
|
Introduction, the first law of thermodynamics, work, energy and heat. Work of expansion, internal energy, determination of internal energy,
|
L-23
|
Heat change at constant volume and constant pressure. Thermodynamic reversibility. Work in isothermal reversible expansion of gases, the maximum work under the isothermal expansion of a gas,
| |
L-24
|
Heat capacities, difference between molar heats. Adiabatic process. Joule-thomson experiment,
| |
L-25
|
Thermochemistry and thermochemical laws, hess’s law. Second law of thermodynamics,
| |
L-26
|
Carnot’s cycle and efficiency of a perfect engine, The concept of entropy and entropy changes for an ideal gas expansion. Entropy changes of materials under various conditions,
| |
L-27
|
Free energy and work functions. Gibbs-helmholtz equation, free energy changes under equilibrium. The clausius clapyeron equation.
| |
L-28
|
Class Test and Review Class (Before Semester Final Exam)
|
*Lecture plans may have revision in accordance with the needs & competence of the students.
Course Policies:
- Attendance: To have presence in class is mandatory. Only three absences are allowed with prior permission. More than three absences may result in reduction of grade and would be informed to respective guardians.
- Text Book: Students are required to have text books by the first week of the semester.
- Surprise test/Sudden test: On the completion of a chapter as well as a lecture, students have to face surprise test/sudden test.
N.B: There will be no make up for any surprise test/sudden test.
- Makeup Class: All makeup classes will be held as per the rescheduling suggested by the course teacher.
- Makeup Exam: There will be no makeup exam for any of the previously held exams.
- Academic honesty: Any academic misconduct will be dealt according to the provisions of the students’ code of conduct.
- Counseling hour: Students are most welcome to make appointment at the time convenient to both the teacher & students.
- E-Learning: All the course resources would be available in the NUB E-Learning Management System (http://182.160.97.196:8081/moodle). Students are asked to actively use the facilities to get help for the course.
Prepared by
Md. Imran Nur Manik
Lecturer
Department of Pharmacy
Northern University Bangladesh.
Northern University Bangladesh
Department of Pharmacy
Faculty of Health Science
Syllabus of Bachelor of Pharmacy
Physical Pharmacy-I (PHARM 1205)
1. Properties of gases: gas laws, ideal gas equation, Dalton’s law of partial pressure, diffusion of gases, kinetic theory of gases, mean free path, deviation from ideal gas behavior, Vander Waal’s equation, critical constants, liquefaction of gases, determination of molecular weights, law of corresponding states and heat capacity
2. Chemical equilibrium: law of mass action, determination of equilibrium constant, heterogeneous equilibrium and homogenous equilibrium, Le chateliar principle and Vant hoff equation
3. Chemical thermodynamics: introduction, the first law of thermodynamics, work, energy and heat. Work of expansion, internal energy, determination of internal energy, heat change at constant volume and constant pressure. Thermodynamic reversibility. Work in isothermal reversible expansion of gases, the maximum work under the isothermal expansion of a gas. Heat capacities, difference between molar heats. Adiabatic process. Joule-thomson experiment.
Thermochemistry and thermochemical laws, hess’s law. Second law of thermodynamics. Carnot’s cycle and efficiency of a perfect engine, the concept of entropy and entropy changes for an ideal gas expansion. Entropy changes of materials under various conditions. Free energy and work functions. Gibbs-helmholtz equation, free energy changes under equilibrium. The clausius clapyeron equation.
4. Phase equilibria: phase, components and degrees of freedom. The phase rule and its thermodynamic derivation. The phase diagrams of water and sulphur systems, partially miscible liquid pairs: the phenol and water and nicotine-water systems. Completely miscible liquid pairs and their separation by fractional distillation. Freeze drying (lyophilization).
5. Solutions: types and properties of solutions. Units of concentration, ideal and real solutions. Henry’s law, distribution of solids between two immiscible liquids, distribution law. Partition coefficient and solvent extraction.
6. Colligative properties of dilute solutions: lowering of vapour pressure, elevation of boiling point, depression of freezing point and osmotic pressure including necessary thermodynamic derivations.
7. Ionic equilibria: pH, determination of pH of different acids and bases, salt solutions and buffers. Titration curves of acids and bases and indicators.
- Buffer capacity: preparation of buffers, buffers and isotonic systems. Methods for adjustment of tonicity of solutions. Buffers in pharmaceutical and biological systems.
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