lecture18 - 1-1Chapter 16Redox Titrations1-2Suggested Text...

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Unformatted text preview: 1-1Chapter 16Redox Titrations1-2Suggested Text Problems: Chapter 14: 4, 5, 9, 12, 14, 16, 17, 19, 24, 25, 26 Chapter 15: 2, 3, 5, 6, 8, 21, 24, 26, 30, 31, 33, 34(a&b), 35Chapter 16: 1, 2, 3, 5, 6, 7Chapter 17: 2, 3, 4, 10, 14, 15, 16, 21, 22, 26, 27, 28, 291-3Text CoverageChapter 14Sections 1, 2, 3, 4, 5Chapter 15Sections 1, 2, 3, 4, 5 (except pp. 308-310), 6, 7Chapter 16Sections 1, 2 are the important sections. [In sections 4, 5, 6, 7 just have some general awareness of these applications, i.e., how you could use permanganate, ceric, dichromate, and iodine}Chapter 17Just through Stripping Analysis (p 366-middle of 367) and not responsible for Box 17-3.1-4Blood Analysis1-51-61-7Typical Redox TitrationAt the Pt indicator electrode, tworeactions come to equilibriumboth equilibria established at the Pt electrode.1-8Regions of a Redox Titration Curve1. Before titrant added, cannot calc. (no Fe+3) 2. Titrant added, before equivalence point3. Equivalence point4. Past equivalence point1-91-10Region 1: Before the Equivalence PointOne special point is reached before the equivalence point. When the volume of titrantis one-half of the amount required to reach the equivalence point(V= ½Ve), [Fe3+] = [Fe2+]. In this case, the log term is 0, and E+= E° for the Fe3+| Fe2+couple. The point at which V = ½Veis analogous to the point at which pH= pKawhen V = ½Vein an acid-base titration.1-11Region 2: At the Equivalence PointAdding these two expressions:[Ce3+] = [Fe3+] and [Ce4+] = [Fe2+] at equiv. pt.1-12Region 2: At the Equivalence PointBecause [Ce3+] = [Fe3+] and [Ce4+] = [Fe2+] at the equivalence point, the ratio of concentrationsin the log term is unity. Therefore, the logarithmis 0 1-13Region 3: After the Equivalence Point1-14Theoretical curve for titrationof 100.0 mL of 0.010 0 M Tl+with 0.010 0 M in 1.00 M HCl.1-15Theoretical curve for titrationof 10.0 mL of 0.010 0 M Tl+with 0.010 0 M IO3-in 1.00 M HCl. The equivalence pointat 0.842 V is not at the center of the steep part of the curve. When the stoichiometryof the reaction Is not 1:1, the curve is not symmetric. 1-16Redox Indicators1-171-181-191-201-21Chapter 17Electroanalytical Techniques1-22Fundamental of ElectrolysisPlace Cu and Pt electrodesinto a solution of Cu2+and force electric currentthrough to deposit copper metal at the cathodeand to liberate O2at the anode1-23Electrolysis SchematicThe electrodeat which the reaction of interest occurs is called the working electrode. In Figure 17-1, we happen to be interested in reductionof Cu2+, so Cu is the working electrode...
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This note was uploaded on 07/23/2010 for the course CHM 3120 taught by Professor Harrison during the Fall '08 term at University of Florida.

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lecture18 - 1-1Chapter 16Redox Titrations1-2Suggested Text...

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