Aqueous Chemistry Semester 2 - 1CMCHI03

Goal(s)

This course provides solid basis in aqueous chemistry, in order to understand and simulate physicochemical evolutions in aqueous solution: general notions on equilibria; precipitation / dissolution; acid-base equilibria ; oxido-reduction reactions.

Content(s)

Aqueous Chemistry

• Aqueous Solutions
  • Microscopic interpretation of solutes dissolution
  • Concept of strong and weak electrolyte
  • Conductimetry and application to conductimetric measurements: interpretation of the slope change before and after equivalence point (theory and labwork)

• Chemical equilibrium
  • Solutes activities, reaction quotient, equilibrium constant (in relation with thermodynamics)
  • Chemical theoretical yield, equilibrium state of a system using a predominant reaction

• Acid-base equilibria
  • Brönsted and Lewis acids and bases
  • Acid-base reactions: water as an amphoteric solvent, leveling effect of solvents, strength of acids and bases
  • Predicting acid-base reactions in a solution, predominance diagrams
  • Theoretical calculation of pH using the predominant acid-base reaction in a mixing of acids and bases
  • Interpretation of a pHmetric titration curve : equivalent point, titration reactions, simultaneous and successive reactions of titration, buffer solutions

• Solubility and precipitation equilibria
  • Definitions, solubility product, equilibria displacement, competitive precipitations, influence of pH on solubility.
  • Saturated or unsaturated solutions with respect to solid ou gazeous species.
  • Use and construction of solubility versus pH or other physicochemical parameters curves.

• Oxydoreduction reactions

• • redox couples, electrode potential, Nernst law
  • definition and determination of oxydation numbers
  • Standard potential calculations for redox couples involving an insoluble salt or acid-base properties of one of the two species.
  • Electrochemical cells : electromotive force, reactions at the electrodes, calculation of the redox equilibrium constant with standard potentials.