Lecture_2-Weak_Acids

Lecture_2-Weak_Acids - PART I: THE BASICS THE CHEMICAL...

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PART I: THE BASICS Water, Weak Acids and Bases THE CHEMICAL NATURE OF WATER H 2 O H + OH - + H 2 O + H 2 O H 3 O + OH - + hydronium hydroxide WATER IONIZES Water partially dissociates at 25°C, 2 out of every 10 9 water molecules ionizes K eq = H + [ ] OH [ ] H 2 O [ ] = 1.8 × 10 16 M H 2 O = 55.5 M K w = 55.5 M ( ) K eq ( ) = H + [ ] OH [ ] = 55.5 M × 1.8 × 10 16 M ( ) = 1.0 × 10 14 M 2 H + [ ] = OH [ ] = K w = 1.0 × 10 14 M 2 H + In pure water (at 25°C), the [H + ] is 0.0000001M = 1 × 10 7 M H 2 O H + OH - + this is the ionization constant of water THE pH SCALE pH = log 1 H + [ ] = log H + [ ] 1 H + = 1 1 × 10 7 = 10,000,000 [ H + ] = 0.0000001 M log10,000,000 = 7 log10 7 = 7 log10 7 = 7
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p ” denotes “negative logarithm of” pH = log 1 H + [ ] = log H + [ ] pH [OH - ] and [H + ] relationship Solution Classifcation 7 [OH-] = [H+] Neutral > 7 [OH-] > [H+] Basic < 7 [OH-] < [H+] Acidic
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This note was uploaded on 11/28/2011 for the course CHEM 340 taught by Professor T.baird during the Fall '11 term at S.F. State.

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Lecture_2-Weak_Acids - PART I: THE BASICS THE CHEMICAL...

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