Chem 287_Chapter 14

Chem 287_Chapter 14 - Lectures: Classical Methods of...

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Lectures: Classical Methods of Chemical Analysis 1 Electrode Potentials Chapter 14 To be covered: 1) Oxidation/reduction 2) Electrochemical Cells 3) Potentiometry 4) Standard Potentials Problems: 6,8,10,12,14,23 5) Nernst equation Additional Information: http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch20/electro.php Oxidation and Reduction Oxidation is the loss of electrons to give a more positive oxidation state. Reduction is the gain of electrons to give a more negative oxidation state. Oxidizing Oxidizing agents get reduced: M a+ + ne - ֕ M (a-n)+ Reducing Reducing agents get oxidized: M a+ ֕ M (a+n)+ +ne - Reducing agents get oxidized: M + ne Redox reaction: Ox1 + Red2 ֕ Red1 + Ox2
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Lectures: Classical Methods of Chemical Analysis 2 Electrochemical Cell Galvanic Cell (Voltaic Cell) uses a spontaneous redox chemical reaction to generate electricity Electrolytic Cell uses electricity to cause a redox chemical reaction. e- Voltage or Current Anode Cathode Oxidation Reduction SaltBridge To prevent direct redox reactions from occuring in the solution and not through the electrodes, two half cells can be constructed with an adjoining ion bridge e- Voltage or Current Cl- K+ Anode Cathode Ox+ Red-
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Lectures: Classical Methods of Chemical Analysis 3 Cell Convention To express a given redox coupled cell, a notation has been developed to identify the cell arrangement. been developed to identify the cell arrangement.
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This note was uploaded on 07/15/2011 for the course CHEM 287 taught by Professor Burns during the Fall '08 term at McGill.

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Chem 287_Chapter 14 - Lectures: Classical Methods of...

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