States
of Matter and Phase Equilibria
Gaseous
state: Ideal Gas law, Molecular
Weight determination, Kinetic Molecular Theory and Vander-waals Equation for
Real Gases;
Liquid
state: Liquefaction of Gase, Methods
of Achieving Liquefaction, Vapor pressure of Liquids, Boiling Point and Heat of
Vaporization including Clausus – Claypeyron equation;
Solids
and Crystalline state: Crystalline
Solids --- X-ray diffraction, melting point and heat of fusion, Intermolecular
forces, Polymorphism. Amorphous solids and Liquid crystalline state.
Phase
equilibria: The phase rule; Systems
containing one, two and three components, Rules relating to Triangular
Diagrams; Solid dispersions;
Thermal
Analysis: Differential scanning
Calorimetry; Diffrential thermal analysis and Thermogravimetric and Thermochemical
Analysis;
Physical
properties of drug molecules:
Refractive index & Molar refraction
Thermodynamics
Defintion
of Thermodynamic Terms: Specific
Heat, Sensible Heat, Latent Heat and Heats of Transition; Laws of Conservation
of Energy; Meaning of Energy Balance and its importance and Inputs of Energy
balance; Concept of Heat and Work;
First
Law of Thermodynamics: Statement,
Definition of Internal Energy, Enthalpy and Heat Capacity; Heat Capacities at
constant Volume and Pressure and their relationship; Thermochemistry:
Standard State Heats of Formation and Combustion; Standard Enthalpy of
Formation – Hess’s Law of Heat summation and its application; Heat of reaction
at constant pressure and at constant volume; Enthalpy of neutralization; Bond
dissociation energy and its calculations from thermochemical data;
The
second and third laws of thermodynamics: Statements, Definiton of Entropy, Free
energy and Gibbs Free Energy; Free Energy functions and applications.
Solutions
of electrolytes: Arrhenius theory of
electrolytic dissociation; Modern theory of strong electrolytes; Debye- Huckel
theory; Coefficients for expressing colligativce properties – L value, Osmotic
Coefficient and Osmolality.
Ionic
equilibria: Acid-base equilibria –
Ionisation of weak acids, weak bases, water and ampholytes, Sorensen’s pH
scale. Acidity constants – effect of ionic strength upon acidity constants,
effect of temperature on ionic equilibria. Determination of Acidity constants.
Buffered
and Isotonic solutions: The Buffer
equation – Common ion effect and the buffer equation for weak acid and its salt
and a weak base and its salt; pH indicators; Factors influencing pH of buffer
solutions; Measurement and calculating tonicity and methods of adjusting
tonicity and pH; Buffer capacity and its calculations; Van Slyke equation;
Influence of concentration on buffer capacity and maximum buffer capacity;
Buffers
in Pharmaceutical and biological systems – in vivo biologic buffer systems
Drugs
as buffers: Pharmaceutical buffers
and their preparation, influence of buffer capacity and pH on tissue
irritation, stability vs optium therapeutic response, pH and solubility.
Electro
Motive Force and Oxidation-Reduction:
Electrochemical cells, Types of Electrodes, measuring the EMF of cells,
reference electrodes and standard potentials, electrometric determination of pH
and specific ions; Hydrogen and glass electrodes, operation of pH meter, ion
elective electrodes, Applications of Oxdn – Redn Potentials (Redox potentials)
in pharmacy.
Catalysis: Defeinition of Catalysis and Catalyst; Types of
Catalyst; Promoters and Inhibitors; Mechnism of Simple Catalytic Reactions;
Factors affecting the catalyst and Catalysis;