Supplements in solution chemistry

This course on solution chemistry aims to introduce the various concepts necessary for studying complex liquid mixtures used in separation chemistry. The approach taken is mainly thermodynamic. In particular, we explain the role of concentration effects, beyond the ideal laws that apply only to dilute solutions.

CM: 12 H

Tutorial: 8 hours

The aim is to enable future master's graduates to acquire a solid knowledge base for describing complex solutions and interpreting scientific data and bibliography in the field of separation chemistry.

Undergraduate general chemistry in a Bachelor's degree in chemistry and/or physics.

Bachelor's degree in thermodynamics and structure of matter.

Final exam with a possible second session.

I General thermodynamics applied to solutions

De Donder criterion - LAM - central role of chemical potential - Ideal solution - Ideal mixture - Quantity characterizing the composition of a mixture - Effects of activity coefficients - Experimental measurement of activity coefficients - Gibbs-Duhem equality -

Application: CMC measurement, practical example of activity measurement for lanthanide salts - comparison of equilibria in - micellization models

II Acid-base balance and the role of concentration

Importance of pH for speciation - experimental methods - Role of solvents - case of concentrated solutions - The case of water: pOH and the predominant role of hydroxides

Applications: Separation of actinides by acid extractant, solubility of metal ions

III Redox equilibria and speciation diagrams

Review of redox reactions - Pourbaix diagrams - plotting 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 chemistry 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.

Administrative contact(s):

Master's Program in Chemistry Secretariat

https://master-chimie.edu.umontpellier.fr/