SOLUTIONS AND PHASE RULE

Paper Code: 
CHY 313
Credits: 
3
Contact Hours: 
45.00
Max. Marks: 
100.00
Objective: 

Course Objective(s):

This course will enable the students to -

  • understand phase, co-existence of phases, phase diagram, CST and distribution law
  • study the concept of ionization in aqueous solution, pH, buffers and various applications of ionization.

Course Outcomes (COs):

Course Outcomes

 

Teaching Learning Strategies

Assessment

Strategies

On completion of this course, the students will be able to;

CO73: apply the concept of ionic equilibrium to discuss  ionization of an electrolyte, salt hydrolysis, buffer solutions, solubility, solubility product, acid-base indicators.

CO74: discuss the concepts of colligative properties and their application to calculate molecular weight of solute.

 CO75: describe the dissociation of ionic compounds in solution and the effects on colligative properties (van’t Hoff factor, i ).

CO76: compute the concentration of solutions

CO77: analyse the behaviour of azeotropes and partially miscible liquids.

CO78: outline different regions, lines, points in phase diagrams and identify normal boiling point, melting point, critical point and triple point.
  • Interactive lectures
  • Explicit teaching discussion
  • Didactic questions
  • Tutorials
  • Multimedia presentations,
  • Demonstration
  • Self-learning assignments,
  • Peer assessment,
  • Concept mapping,
  • Think/Pair/Share,
  • Problem solving exercise,
  • PowerPoint presentation,
  • Handouts

 
  • Oral and written examinations (scheduled and surprise tests)
  • Closed book and open book tests
  • Quiz
  • Assignments
  • Presentations

 

 

9.00
Unit I: 
Ionic Equilibria

Strong, moderate and weak electrolytes, degree of ionization, factors affecting degree of ionization, ionization constant and ionic product of water, ionization of weak acids and bases, pH scale, common ion effect; dissociation constants of mono-, di- and tri- protic acids (exact treatment), salt hydrolysis-calculation of hydrolysis constant, degree of hydrolysis and pH for different salts.
Buffer solutions, derivation of Henderson equation and its applications, buffer capacity, buffer range, buffer action and applications of buffers in analytical chemistry and biochemical processes in the human body, solubility product of sparingly soluble salts and its applications, qualitative treatment of acid – base titration curves (calculation of pH at various stages), theory of acid – base indicators, selection of indicators and their limitations.

 

9.00
Unit II: 
Ideal and Non-ideal Solutions

Ideal solutions, Henry.s law and Raoult's law, deviations from Raoult's law- nonideal solutions, vapour pressure-composition and temperature-composition curves of ideal and non-ideal solutions,distillation of solutions, lever rule, azeotropes- (ethanol-water system), partial miscible liquids: phenol-water, trimethylamine-water and nicotine-water systems, critical solution temperature, effect of impurity on partial miscibility of liquids, immiscibility of liquids, principle of steam distillation, Nernst distribution law and its applications, solvent extraction.

 

9.00
Unit III: 
Dilute Solutions– Colligative Properties

Dilute solutions- methods of expressing concentrations of solutions, colligative properties, Raoult’s law, relative lowering of vapour pressure and its measurement, osmosis, osmotic pressure and its measurement, elevation of boiling point and its measurement, depression of freezing point and its measurement, thermodynamic basis of the colligative properties and derivation of expressions for these using chemical potential, use of colligative properties in molecular weight determination, non-ideal behaviour and van’t Hoff’s factor ‘i’.

 

9.00
Unit IV: 
Heterogeneous Equilibria I

Introduction to phase, component and degree of freedom, Gibbs phase rule and its thermodynamic derivation, derivation of Clausius- Clapeyron equation and its importance in phase equilibria,
Phase equilibria of one component system-water, CO2 and sulphur system, liquid helium.
Phase equilibria of two component system-solid-liquid equilibria, simple eutectic – Bi-Cd, KI-H2O, Pb-Ag systems, desilverisation of lead.

 

9.00
Unit V: 
Heterogeneous Equilibria II

Solid solutions: compound formation with congruent melting point (Mg-Zn) and incongruent melting point (NaCl-H2O), (FeCl3 – H2O), (CuSO4 – H2O)and (Na2SO4–H2O) system, freezing mixtures (acetone – dry ice).
Phase diagrams for three component systems: Acetic acid –chloroform-water

 

Essential Readings: 
  • A Textbook of Physical Chemistry; A.S. Negi, S.C. Anand; New Age International (P) Limited, New Delhi, 2007.
  • Principles of Physical Chemistry, B. R. Puri, L. R. Sharma, M. S. Pathania, Vishal Publishing Co. 2011.

 

References: 

SUGGESTED READINGS:

  • Atkin’s Physical Chemistry, Eighth Edition; P.W. Atkins, J. Paula; Oxford University Press, International Student Edition, 2017.
  • Physical Chemistry Through Problems, Second Edition; S.K. Dogra and S. Dogra; New Age International Pvt. Ltd, New Delhi, 2001.
  • A text book of Physical Chemistry, Applications of Thermodynamics, Volume III, Fourth Edition, K. L. Kapoor; McGraw Hill Education Private Limited, 2015.

e-RESOURCES:

 

Academic Year: 
2022-2023
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