Lecture2 - Lecture 2 1/7/09 Background reading: Garrett and...

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Lecture 2 1/7/09 Weak acids and bases Henderson-Hasselbalch equation Buffers Polyprotic acids Outline: Background reading: Garrett and Grisham: Chapter 2: Pages 46-49 Assignment: Segel: Page 92: problems 25 (parts a-d) and 38 (parts a-d) Page 93: problems 40, 41 and 44 (Note: For your information, the Tris buffer that is used in Problem 41 is an amine. The two components of this buffer can be considered as RNH 3 + and RNH 2 .)
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The ionization constants considered in Lecture 1 are useful in calculations of [H + ] of solutions of weak acids and bases. Example: If have a 0.1 M solution of a weak acid, HA, can use the K a to calculate the [H+] of the solution. K a = [H+] [A - ] Consider the concentrations of the various components that will be present at: [HA] [HA] [H+] [A - ] Start 0.1 M 0 0 Equilibrium 0.1-x x x If x = [H+] [A - ] also = x K a = [x] [x] [0.1 – x] Thus, to solve for [H+], solve for x. If the amount that ionizes is less than 10% of the original concentration,
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This note was uploaded on 02/21/2009 for the course BIS BIS102 taught by Professor Hilt during the Winter '08 term at UC Davis.

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Lecture2 - Lecture 2 1/7/09 Background reading: Garrett and...

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