Solutions and Phase Rule

Paper Code: 
CHY-313
Credits: 
3
Contact Hours: 
45.00
Objective: 

Course Objectives:

This course will enable the students to -

1. understand the concepts of ionic equilibria, solutions and application of thermodynamics to heterogeneous equilibria.

Course Outcomes (COs):

Course

Learning outcomes

(at course level)

Learning and teaching strategies

Assessment

Strategies

Paper Code

Paper Title

 

 

 

 

 

CHY-313

Solutions and Phase Rule

 

 

 

 

 

The students will be able to –

 

CO75: apply the concept of ionic equilibrium to discuss  ionization of an electrolyte, salt hydrolysis, buffer solutions, solubility, solubility product, acid-base indicators.

CO76: discuss the concepts of the four colligative properties and calculate molecular weight of solute.

 CO77: describe the dissociation of ionic compounds in solution and the effects on colligative properties (van’t Hoff factor, i ).

CO78: compute the concentration of solutions in terms of molarity, mass percent, molality, and mole fraction.

 CO79: analyse the behaviour of azeotropes and partially miscible liquids.

CO80: outline different regions, lines, points in phase diagrams and identify normal boiling point, melting point, critical point and triple point.

Approach in teaching:

  • Interactive Lectures
  • Explicit Teaching  Discussion
  • Didactic questions  Tutorials
  • Multimedia Presentations,
  • Demonstration

Learning activities for the students:

  • Self-learning Assignments,
  • Peer Assessment,
  • Concept mapping,
  • Think/Pair/Shar e, Problem Solving, Power Point Presentation, Handouts

 

The oral and written examinations (Scheduled and surprise tests) Closed book and open book tests

  • Quiz
  • Problem solving exercises
  • Assignments
  • Presentation
  • Semester End Examinations

 

 

 

12.00
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 and solubility product of sparingly soluble salts – applications of solubility product principle. Qualitative treatment of acid – base titration curves (calculation of pH at various stages). Theory of acid – base indicators; selection of indicators and their limitations. Multistage equilibria in polyelectrolyte systems; hydrolysis and hydrolysis constants.

9.00
Unit II: 
Dilute Solutions– Colligative Properties

Introduction, colligative properties, Raoult’s law, relative lowering of vapour pressure; Osmosis, law of osmotic pressure and its measurement, Elevation of boiling point and its measurement, Depression of freezing point and its measurement, Use of colligative properties in molecular weight determination; Non-ideal behaviourandvan’t Hoff’s factor ‘i’.

8.00
Unit III: 
Solutions and Non-ideal Solutions

Solutions: Ideal and non-ideal solutions, methods of expressing concentrations of solutions, Solution of gases in liquid: Henry’s law, deviation from Henry’s law. Non ideal system: Azeotropes –ethanol-water systems. Partially miscible liquids: Phenol-water, trimethylamine-water, nicotine-water systems; lower and upper consolute temperature, effect of impurity on consolute temperature; Immiscible liquids.

9.00
Unit IV: 
Heterogeneous Equilibria I

Introduction to phase, component and degree of freedom, derivation of Gibbs phase rule; 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.

 

7.00
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.

 

References: 
  •  A Textbook of Physical Chemistry; A.S. Negi, S.C. Anand; New Age International (P) Limited, New Delhi, 2007.
  • Elements of Physical Chemistry; Seventh International Edition. P.W. Atkins, J. Paula; Oxford, India 2017.
  • Elements of Physical Chemistry; Seventh Edition. P.W. Atkins, J. Paula; Oxford University Press, New York, 2016.
  • Physical Chemistry; Fourth Edition; R.A. Alberty; Wiley Eastern Ltd., Singapore, 2004.
  • Physical Chemistry Through Problems; S.K. Dogra and S.Dogra; Second Edition;New Age International Pvt. Ltd, New Delhi, 2001.
Academic Year: 
2021-2022
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