Lecture 9 - 1 Today Completing through Ch 7.7...

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1 Today: Completing through Ch. 7.7
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2 Strong Acid: e.g. HCl (completely ionized) Bronsted-Lowry Theory: An acid is a proton donor; a base is a proton acceptor. Base Acid What is the [H 3 O + ] for 0.25M HCl (aq)? [H 3 O + ] = 0.25M
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3 Weak Acid- CH 3 COOH (Acetic Acid)
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4 Weak Acid- CH 3 COOH (Acetic Acid) K a K a [ ] [ ] 5 10 x 8 . 1 2 O 3 H 2 HC O 3 H 2 O 3 H 2 C a K = + = Acid Ionization Constant, K a : What is the [H 3 O + ] for 0.100 M Acetic Acid? Calculation is the same as in previous eq’m problems.
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5 Weak Acid- CH 3 COOH (Acetic Acid) K a K a [ ] [ ] 5 10 x 8 . 1 2 O 3 H 2 HC O 3 H 2 O 3 H 2 C a K = + = Acid Ionization Constant, K a : Acid Conjugate acid/base pair Acid Base Base Conjugate acid/base pair Conjugate acid/base pairs differ by a proton (H + )
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6
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7 Weak Base- Ammonia [ ] [ ] 5 10 x 8 . 1 3 NH OH 4 NH b K = + = Base Ionization Constant, K b : K b K b Weak Base Rel. Strong Acid Weak Acid Strong Base What is the [OH - ] for a 0.250 M Ammonia Solution?
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8
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9 Strong acids have relatively weak conjugate bases.
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