Level of study
BAC +4
ECTS
2 credits
Component
Faculty of Science
Description
This course of solution chemistry aims at introducing the different concepts necessary to the study of complex liquid mixtures used in separative chemistry. The proposed approach is mainly thermodynamic. We explain in particular the role of concentration effects, beyond the ideal laws valid only for dilute solutions.
CM : 12 H
TD : 8 H
Objectives
The aim is to provide the future Master's graduate with a solid knowledge to describe complex solutions and to interpret the scientific data and bibliography of separative chemistry.
Necessary pre-requisites
General chemistry undergraduate degree in chemistry and/or physics.
Bachelor's degree course in thermodynamics and structure of matter.
Knowledge control
Final exam with a possible second session.
Syllabus
I General thermodynamics applied to solutions
Donder's criterion - LAM - central role of the chemical potential - ideal solution - ideal mixture - quantity characterizing the composition of a mixture - effects of the activity coefficients - experimental measurement of the activity coefficients - Gibbs-Duhem equality -
Application: cmc measurement, practical example of activity measurement for lanthanide salts - comparison of equilibria in - micellisation models
II Acid-base equilibrium and the role of concentration
Interest of pH for speciation - experimental methods - Role of solvents - case of concentrated solutions - The case of water: pOH and preponderant role of hydroxides
Applications: Separation of actinides by acid extractant, solubility of metal ions
III Oxidation-reduction equilibria and speciation diagrams
Reminder of the redox course - Pourbaix diagrams - drawing and use
Applications: the relatively simple case of lanthanides, the much more difficult case of actinides
IV Complexation equilibria
Ligands and solvation - Successive equilibria - Classification of ligands - enthalpic and entropic factors - pC
Applications: transition elements - supramolecular and separative chemistry - generalized speciation diagrams
V Precipitation equilibria
Solubility - Competition between ionic species - solid solutions - kinetic factors
Application: Berthelot-Nernst and Doerner Hoskins coprecipitation.
Additional information
Administrative contact(s):
Secretariat Master Chemistry
https://master-chimie.edu.umontpellier.fr/