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Ch14 z5e acid base
- 4. Figure 14.1 The Reaction of HCI and H 2 O
- 9. B. Definitions H 2 O + HNO 3 H 3 O + + NO 3 – CB CA A B
- 17. Figure 14.5 Acid Strength Versus Conjugate Base Strength z5e 661
- 29. Figure 14.7 Two Water Molecules React to Form H 3 O + and OH -
- 33. Figure 14.8 The pH Scale and pH Values of Some Common Substances
- 34. Basic Acidic Neutral 10 0 10 -1 10 -3 10 -5 10 -7 10 -9 10 -11 10 -13 10 -14 [H + ] 0 1 3 5 7 9 11 13 14 pH Basic 10 0 10 -1 10 -3 10 -5 10 -7 10 -9 10 -11 10 -13 10 -14 [OH - ] 0 1 3 5 7 9 11 13 14 pOH
- 40. Z5e p637 Solving Weak Acid Equilibrium Problems pp
- 47. Figure 14.10 p. 643. The Effect of Dilution on the Percent Dissociation and (H+) of a Weak Acid Solution
- 73. Acid-base Properties of Aqueous Ions
- 76. Strength of oxyacids Electron Density Cl O H
- 77. Strength of oxyacids Electron Density O Cl O H
- 78. Strength of oxyacids O O Electron Density Cl O H
- 79. Strength of oxyacids O O O Electron Density Cl O H
- 81. Metal Ion Surrounded by Water Molecules
- 87. Lewis Acids and Bases Al +3 ( H H O Al ( H H O + 6 +3 ) ) 6
- 89. Z5e Solving Acid-Base Problems p. 667 pp
Editor's Notes
- Z5e 14.1 658 The Nature of Acids and Bases Alternative link if can’t get through to YouTube: http://dailycackle.com/2007/01/20/science-experiment-gone-wrong/
- Z53 Fig. 14.1 659: reaction of HCl and H20
- Z5e 660 SE 14.1 a, c, e
- Z5e fig. 14.5 p. 661
- Z5e 661 14.2 Acid Strength; see Table 14.1
- For SE 14.2 -- you need to “remember” that HCl is a strong acid, so Cl - is a weak base (since id does not easily accept a proton (or a H + ). That is, acid strength is inversely proportional to its conjugate base strength.
- Z5e 663 SE 14.2
- Z5e 663 SE 14.2
- Z5e 663 SE 14.2
- Rf. Z5e 664 Note: in =m expression, H 2 O (l) is a pure liquid, so constant and drops out of the expression. K w called the ion-product constant (or the dissociation constant)
- Rf. Z5e 664 Note: in =m expression, H 2 O (l) is a pure liquid, so constant and drops out of the expression. K w called the ion-product constant (or the dissociation constant)
- Z5e 666 SE 14.4
- Z5e 664 Fig. 14.7
- Z5e 14.3 The pH Scale
- Z5e Fig. 14.8 667
- Z5e 668. SE 14.6
- Z5e 669 Section 14.4: Calculating the pH of Strong Acid Solutions
- Z5e 670 SE 14.7b
- Z5e 671 Section 14.5: Calculating the pH of Weak Acid Solutions
- [H + ] = .0060, so pH = 2.22 pOH = 11.78; [OH - ] = 1.7 x 10 -12 & [H + ] = 6.0 x 10 -3
- Z5e 675 Major species: HF, HOC 6 H 5 , H 2 O Since HF is dominant producer of H + , use its Ka Set up “RICE” table, use approximations and 5% rule [H + ] = .030 & pH = 1.53
- Z5e 675 Major species: HF, HOC 6 H 5 , H 2 O Since HF is dominant producer of H + , use its Ka Set up “RICE” table, use approximations and 5% rule [H + ] = .030 & pH = 1.53
- Rf. Z5e 675 SE 14.9
- Z5e 677 [H] = 4.24 x 10 -3 vs. 1.34 x 10 -4 So % dissociation (aka % ionization) = 0.42% vs. 1.3%
- Rf. Z5e 680 SE 14.11 Since (X/0.100)(100%) = 8.1%, x = 8.1 x 10 -3 = [H + ] = [A - ], then plug into =m to solve for Ka. Ans. = 6.6 x 10 -4
- Z5e 680 fig. 14.10
- Z5e 681 Section 14.6 Bases
- See next slide for explanation
- [hydroxide] = 1.2 x 10 -10
- Z5e 688 Section 14.7 Polyprotic Acids
- [H + ] = 7.1 x 10 -2 [H 2 AsO 4 2- ] = 7.1 x 10 -2 also [HAsO 4 3- ] = 8.0 x 10 -8 = Ka 2 [AsO 4 3- ] = 6.8 x 10 -16 Remember: Must consider [H + ] from all sources
- [H + ] = 7.1 x 10 -2 [H 2 AsO 4 2- ] = 7.1 x 10 -2 also [HAsO 4 3- ] = 8.0 x 10 -8 = Ka 2 [AsO 4 3- ] = 6.8 x 10 -16 Remember: Must consider [H + ] from all sources
- [H + ] = 7.1 x 10 -2 [H 2 AsO 4 2- ] = 7.1 x 10 -2 also [HAsO 4 3- ] = 8.0 x 10 -8 = Ka 2 [AsO 4 3- ] = 6.8 x 10 -16 Remember: Must consider [H + ] from all sources
- [H + ] = 7.1 x 10 -2 [H 2 AsO 4 2- ] = 7.1 x 10 -2 also [HAsO 4 3- ] = 8.0 x 10 -8 = Ka 2 [AsO 4 3- ] = 6.8 x 10 -16 Remember: Must consider [H + ] from all sources
- [H + ] = 7.1 x 10 -2 [H 2 AsO 4 2- ] = 7.1 x 10 -2 also [HAsO 4 3- ] = 8.0 x 10 -8 = Ka 2 [AsO 4 3- ] = 6.8 x 10 -16 Remember: Must consider [H + ] from all sources
- Both [H + ] and [HSO4 - ] are 2 M , since completely dissociated.
- Both [H + ] and [HSO4 - ] are 2 M , since completely dissociated.
- Z5e 694 Section 14.8 Acid-Base properties of Salts
- Z5e 695 Write major species Set up =m between anion and water Since product includes hydroxide ion, must use K b so need to convert from K a Calculate hydroxide concentration, convert to pOH, subtract from 14 to get pH
- Z5e 695 Write major species Set up =m between anion and water Since product includes hydroxide ion, must use K b so need to convert from K a Calculate hydroxide concentration, convert to pOH, subtract from 14 to get pH
- Z5e 697
- Z5e 697
- Z5e 699 Table 14.5
- Z5e 701 Section 14.9 The Effect of Structure on Acid-Base Properties
- Z5e 702 Figure 14.11
- Z5e Section 14.10 Acid-Base Properties of Oxides
- Z5e 704 Section 14.11 The Lewis Acid-Base Model
- Al ion is Lewis acid and water is Lewis base
- Z5e 707 Section 14.12 Strategy for Solving Acid-Base Problems: A Summary
- Z5e 708; Tr 160.