Abstract:This chapter begins with a very fundamental treatment of oxidation–reduction reactions and moves to its application to titrations and finally to ion-selective electrodes. Oxidation–reduction reactions...This chapter begins with a very fundamental treatment of oxidation–reduction reactions and moves to its application to titrations and finally to ion-selective electrodes. Oxidation–reduction reactions (sometimes shortened to redox reactions) are taking place in solution where there are no free electrons; thus, one must take place with the other. An electrochemical cell is an example of a galvanic cell that is composed of a two-electrode system where oxidation is taking place at one electrode and reduction is taking place at the second electrode. The Nernst equation describes the relationship between the potential of a galvanic cell and the activities of the redox species. There are two primary ways of determining a redox titration endpoint in the analytical laboratory by the analyst that include the use of a potentiometer where the data gathered are plotted and using a visual indicator.Read More
Publication Year: 2024
Publication Date: 2024-03-01
Language: en
Type: other
Indexed In: ['crossref']
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