Lecture 6 (10am) Chapter 4 et al (Acid-Base) September 18 2009

Lecture 6 (10am) Chapter 4 et al (Acid-Base) September 18 2009

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Acids and Bases continued (Chapters 4.4, 18.1-18.3 and 19.2) Lecture 6 September 18, 2009
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Equilibrium constants for weak acids and weak bases: K a and K b Weak Acids: HA (aq) + H 2 O (l) ↔ H 3 O + (aq) + A - (aq) K a = acid dissociation constant (equilibrium constant for “reaction” of weak acid and water)
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Weak Bases: B (aq) + H 2 O (l) ↔ BH + (aq) + OH - (aq) K b = base ionization constant (equilibrium constant for “reaction” of weak base and water)
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The auto-ionization of water – water reacts with itself
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The weakest of the bases listed is Acid Conjugate Base K a (Ionization Constant of Acid) HI I 100% ionized H 2 SO 3 HSO 3 1.4 x 10 –2 HNO 2 NO 2 - 7.1 x 10 –4 HSO 3 SO 3 2– 6.5 x 10 –8 (A) I (B) HSO 3 (C) NO 2 - (D) SO 3 2–
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The relationship between K a , K b and K W
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The pH scale pH 0 pH 1 pH 2 pH 3 pH 4 pH 5 pH 8 pH 9 pH 10 pH 11 pH 12 pH 13 pH 14 pH 6 pH 7 “Pure” Water Battery Acid HCl Secreted by stomach lining Lemon Juice Orange Juice Acid Rain Black Coffee Saliva Sea water Baking Soda Milk of Magnesia Ammonia Soapy Water Bleach Liquid Drain Cleaner
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Example: What is the pOH of a 0.264 M HCl solution at 25 o C?
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The pH of a 1.65 x 10 -2 M Ba(OH) 2 solution at 25 °C is (A) 1.48 (B) 1.78 (C) 12.22 (D) 12.52
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