PHYSICAL CHEMISTRY LAB II

Paper Code: 
CHY 227
Credits: 
3
Contact Hours: 
90.00
Max. Marks: 
100.00
Objective: 

Course Objective(s) :
This course will enable the students to –
develop experimental skills of various instruments (spectrophotometer, pH meter, polarimeter etc.) and gain knowledge of basic terms regarding phase equilibrium, thermochemistry, optical measurement and Lambert-Beer law.

 

Course Outcomes (COs):

Course Outcomes

Teaching Learning Strategies

Assessment Strategies

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

CO70:calibrate and operate a variety of scientific instrument to perform observations related to the experiment.

CO71:explain the principles behind the experiments performed in the lab and calculate these values (stability constant, pKa value, partial molar volume)

CO72:perform experiments based on pH-metry, polarimetry, thermochemistry, phase equilibria and spectrophotometry.

CO73:perform scientific experiments as well as accurately record experimental data with proper significant figure and analyze the results of such experiments.
  • Laboratory instructions and Demonstrations

 
  • Conduction of Experiments
  • Lab Records
  • Viva voce

 

 

 
 


 

Unit I: 

A list of experiments under different headings is given below. Students are required to perform 10-12 experiments (minimum two from each category).

Thermochemistry
  1. To determine the solubility of benzoic acid at two temperatures in water-DMSO mixture (4:1)  and to calculate the enthalpy change of the dissolution process.
  2. To determine the lattice energy of calcium chloride from its heat of solution using Born-Haber cycle. Provided the enthalpy changes for Ca+2 (g) → Ca(g), 2Cl- (g) → 2Cl (g), Ca (g) → Ca (s), 2Cl (g) → Cl2 (g) and Ca (s) + 2Cl (g) → CaCl2 (s) are -451.1, 174.3, -38.8, -58.0 and -190.0 Kcal/mole respectively.
  3. To determine the partial molal volume of solute (KCl or NaCl) and solvent in a binary mixture at normal temperature and pressure.
  4. To determine the partial molar volume of methanol/ethanol-water system at normal temperature and pressure.
Phase Equilibrium
  1. To determine the solubility diagram for a three component liquid system chloroform, acetic acid and water / toluene, acetic acid and water / benzene ethanol and water. To discuss the diagram in a light of phase, component and degree of freedom.
  2. Nernst Distribution Law: To determine the formula of a complex ion formed between cupric ion and ammonia by distribution method.
  3. To study the freezing point curve of two components simple eutectic system (acetamide-benzoic acid/naphthalene-benzoic acid)
Polarimeter
  1. To determine the rate constant of the inversion of cane sugar in presence of hydrochloric acid and sulphuric acid by using polarimeter and evaluate the relative strength of the two acids.

pH Metry

  1. To titrate the given mixture of CO3-2 and HCO3- ions against a given strong acid   and to determine their strength.
  2. To determine pKa values of tribasic acid (H3PO4) against a strong base (NaOH).
  3. To determine the acidic and basic dissociation constant of an amino acid and hence its isoelectric point.
  4. To determine of pKa values of maleic/malonic acid by potentiometric titration with NaOH using glass electrode.
Spectrophotometry
  1. To determine the acid dissociation constant (pKa value) of methyl red.
  2. To determine the stability constant and composition of FeSCN+2 complex/ Fe(III)-salicylic acid/iron-phenanthroline complex/ zirconium alizarin red-S complex by jobs method of continuous variation and mole ratio method.

 

Essential Readings: 
  • Advanced Practical Physical Chemistry, Thirtieth Edition; J. B. Yadav; Krishna Prakashan Media Pvt. Ltd., Meerut, 2015.
  • Experimental Physical Chemistry, First Edition; V. D. Athawale and P. Mathur; New age International (P) Ltd. Publishers, New Delhi, 2011.

 

References: 

SUGGESTED READINGS:

  • Experiments in Physical Chemistry, Fifth Edition; D. P. Shoemaker, C. W. Garland and J. W. Nibler, Mc Graw-Hill, New York, 1998.
  • Introductory Practical Physical Chemistry, D. T. Burns and E. M. Rattenbury, Pergamon Press, 1966.

e-RESOURCES:

Scheme of Examination

The duration of examination will be 6 hrs.
The following exercise will be set in the examination
Physical Chemistry Experiment (two)                            
Experiment I      27 marks
Experiment II     28 marks
Viva                  15 marks
Total                 70 marks

1.Physical Chemistry Experiment

The exercise carries 27 marks / 28 marks. The exercises in Physical chemistry can be modified by the examiners and the same will be explained to the candidates. However, such modifications will not involve any departure from the basic principles over which experiments are prescribed in the syllabus.

Candidates shall be given one exercise out of the exercises prescribed in the syllabus. The distribution of marks will be as follows:

  1. Theory and procedure                                          3 marks
  2. Correct observation                                              5 marks
  3. Use of correct formula                                          5 marks
  4. Calculation                                                          7 marks
  5. Result                                                           7 marks / 8 marks

No marks for calculation will be awarded to a candidate for not calculating result.

The permissible error will depend on the nature of the experiment. Generally + 10% error may be taken as permissible error for experiments involving potentiometric and conductometric measurements. The constancy in values or rate constants may be taken into consideration while awarding mark in experiments on chemical kinetics. One mark shall be deducted for each + 2% error over permissible limit.

2.Viva

Oral questions shall generally be asked over the work assigned to the candidate. The purpose is to find out as to what extent the candidate has understanding the basic principles of chemistry.

 

 

Academic Year: 
2023-2024
  • Printer-friendly version
  • PDF version