Aquatic Chemistry 367 Civil and Environmental Engineering Meeting
- Slides: 11
Aquatic Chemistry 367 Civil and Environmental Engineering Meeting time: MWF 11: 00 -11: 50 am Meeting room: Abbott Auditorium in Pancoe Pavillion Instructor: Jean-Francois Gaillard, jfgaillard@northwestern. edu Grader: Amy Dahl, a-dahl@northwestern. edu
Logistics • Introductions • http: //www. civil. northwestern. edu/ehe/cour ses/ce-367. htm • Keep on top of the homework!
Why study Aquatic Chemistry?
Why study Aquatic Chemistry? • Required for life • Pollution transport almost always requires water • Many environmentally relevant reactions occur in water • Critical for controlling cycling of many elements – Nutrients – Toxins – Oxygen, nitrogen, carbon dioxide – atmosphere control
Applications of aquatic chemistry: • • • Arsenic Chromium Mercury Acid mine drainage Global warming
What is water? • • • Universal Solvent Required for life Molecular structure Hydrogen bonding: water clustering Anomalous behavior compared to other liquids
What is in water? Soluble Species Suspended Particles Small Complexes e. g. , Inorganic Metal Complex Me(CO 3 )ny. Hydrated Ion Particles • Colloidal, aggregates • Oxides (Al, Fe, Mn, Si) • Adsorption: surface complexation • Co-entrainment Men+ (H 2 O)n Complexes with Macromolecules e. g. , Fulvic Acid Sediments! Sediments Living Organisms • Intra/extra-cellular • Oligoelements • Toxicity • Defense Mechanisms e. g. , amorphous ore. g. , crystalline solidsor(precipitates and mineral formation) amorphous crystalline solids
What is in water? • Dissolved ions: – – – Major Cations (Ca, Na, Mg, K, Fe) Trace elements (Zn, Cr, Cu, Cd) Anions (F, Cl, nitrate, sulfate) Complexes (non-charged) Organic molecules (humic substances) • http: //www. ar. wroc. pl/~weber/kwasy 2. htm • Particulate – Organic matter – Clays – Oxides
Chemical Reactions • • Acid-base chemistry Coordination chemistry Precipitation and dissolution Redox reactions
Kinetic approach • Does not assume equilibrium has been reached • Use a rate constant, k, to describe the rate of formation of products or consumption of reactants
Thermodynamic explanation • Assumes equilibrium of a reaction is reached • Simplifies solving mathematical expressions of chemical systems • Use an equilibrium constant, K, to describe ratio of products to reactants
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