Lecture 22 - Final Exam Final Exam (10:00 am -12:00 pm)...

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inal Exam Final Exam Final Exam (10:00 am -12:00 pm) Thurs., Apr. 30th ocations: Locations: CLB 130 (Last Names: A to L) Flint 50 (Last Names: M to Z) (Chapters 0, 1, 2, 3, 5): ~10% nalytical Measurements Analytical Measurements Methods/Errors Statistics Calibrations (Chapters 6, 7, 8, 9, 10, 11): ~40% Equilibrium/Titrations Acid Base Equilibria Acid Base Titrations
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(Chapters 14, 15, 16, 17): ~30% Electrochemistry Potentiometry/Redox Titrations Electroanalytical Methods (Chapters 18, 19, 20): ~20% Spectrophotometry Spectrophotometers
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Chapters 6, 7, 8, 9, 10, and 11 Equilibrium/Titrations Acid Base Equilibria Acid Base Titrations The equilibrium constant 1. The equilibrium constant Le Chatelier’s principle:
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Solubility Product: In a complex equilibrium system, all equilibriaare ±satisfied simultaneously! herefore the concentration of a ion that satisfies any one Therefore, the concentration of a ion that satisfies any one equilibrium must Satisfy all equilibria, and then there is only one concentration of the ion in the solution. Lewis acid: Lewis base: Electron pair cceptors Electron pair onors acceptors donors Protic Acid: Bronsted-Lowry Acid: Lowis acid ronsted owry Base: Protic Base: Bronsted-Lowry Base: Lowis base:
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Conjugate Acids and Bases: Strong Acid and Base: Weak Acid and Base:
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Relation between K a and K b
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Titrant: is a substance used to react with analyate in a titration. Equivalence point: is the point when the quantity of added titrant is the exact amount to complete the stoichiometric action with nalyte theoretical result). End point reaction with analyte (a theoretical result). : is the actually point marked by a sudden change of a physical property of the solution. Indicator:
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Lecture 22 - Final Exam Final Exam (10:00 am -12:00 pm)...

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