Page 90 - CatalogNEP-LS

Thermochemistry: Standard state, standard enthalpy of formation- Hess‘s Law of heat summation
and its applications. Heat of reaction at constant pressure and at constant volume. Enthalpy of
neutralization. Bond dissociation energy and its calculation from thermo-chemical data,
temperature dependence of enthalpy. Kirchhoff‘s equation.
Thermodynamics-II: Second law of thermodynamics: Need for the law, different statements of the
law. Carnot cycle and its efficiency. Carnot theorem. Thermodynamic scale of temperature.
Statement of Third Law of thermodynamics and calculation of absolute entropies of substances.

UNIT-II: (8 Hours)
Chemical Equilibrium: Equilibrium constant and free energy. Thermodynamic derivation of law
of mass action. Le Chatelier‘s principle Reaction isotherm and reaction isochore- Clapeyron
equation and Clausius – Clapeyron equation, applications.
UNIT-III: (12Hours)

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. Salt hydrolysis-calculation of hydrolysis constant, degree of
hydrolysis and pH for different salts. Buffer solutions. Solubility and solubility product of
sparingly soluble salts, applications of solubility product principle.
UNIT-IV: (6 Hours)

Conductance: Conductivity, equivalent and molar conductivity, and their variation with dilution
for weak and strong electrolytes. Kohlrausch law of independent migration of ions.
Transference number and its experimental determination using Hittorf and Moving boundary
methods. Ionic mobility. Applications of conductance measurements: determination of degree of
ionization of weak electrolyte, solubility and solubility products of sparingly soluble salts, ionic
product of water, hydrolysis constant of a salt. Conductometric titrations (only acid-base).

UNIT-V: (9 Hours)
Electrochemistry: Reversible and irreversible cells. Concept of EMF of a cell. Measurement of
EMF of a cell. Nernst equation and its importance. Types of electrodes. Standard electrode
potential. Electrochemical series. Thermodynamics of a reversible cell, calculation of
thermodynamic properties: ΔG, ΔH and ΔS from EMF data. Calculation of equilibrium constant
from EMF data. Concentration cells with transference and without transference. Liquid junction
potential and salt bridge. pH determination using hydrogen electrode and quinhydrone electrode.
Potentiometric titrations -qualitative treatment (acid-base and oxidation-reduction only).

PRACTICAL (30 Hours)

1. Thermochemistry
i) Determination of Water Equivalent of a thermos flask.
ii) Determination of heat of solution of KNO3 and KCl.
iii) Determine the enthalpy of neutralization between strong acid and strong base.
iv) Determine the enthalpy of neutralization between strong acid and weak base.
v) Determine the enthalpy of hydration of CuSO4.
vi) Determine the enthalpy of neutralization of a weak acid/weak base versus strong
base/strong acid
2. pH measurements
Preparation of buffer solutions:
i) Sodium acetate-acetic acid
ii) Ammonium Chloride and Ammonium Hydroxide

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