1. Acids and Bases Chapter 19

2. I. Describing Acids & Bases

3. A. Taste

4. I. Describing Acids & Bases A. Taste B. Touch

5. I. Describing Acids & Bases A. Taste B. Touch C. Reactions with Metals

6. I. Describing Acids & Bases A. Taste B. Touch C. Reactions with Metals D. Electrical Conductivity

7. I. Describing Acids & Bases A. Taste B. Touch C. Reactions with Metals D. Electrical Conductivity E. Indicator

8. Indicator Substance that is one color in an acidic solution and another color in a basic solution

9. I. Describing Acids & Bases A. Taste B. Touch C. Reactions with Metals D. Electrical Conductivity E. Indicator 1. litmus

10. I. Describing Acids & Bases A. Taste B. Touch C. Reactions with Metals D. Electrical Conductivity E. Indicator 1. litmus 2. phenolphthalein

11. I. Describing Acids & Bases A. Taste B. Touch C. Reactions with Metals D. Electrical Conductivity E. Indicator 1. litmus 2. phenolphthalein 3. bromothymol blue

12. II. Defining Acids & Bases

13. A. Arrhenius Definition

14. II. Defining Acids & Bases A. Arrhenius Definition 1. Acid

15. Arrhenius Acid A substance that dissociates in water to produce H + ion

16. A. Arrhenius Definition 1. Acid 2. Base II. Defining Acids & Bases

17. Arrhenius Base A substance that dissociates in water to form OH - ions

18. B. Bronsted-Lowry Definition II. Defining Acids & Bases

19. B. Bronsted-Lowry Definition 1. Acid II. Defining Acids & Bases

20. Bronsted-Lowry Acid A substance that can donate a proton

21. B. Bronsted-Lowry Definition 1. Acid 2. Base II. Defining Acids & Bases

22. Bronsted-Lowry Base A substance that can accept a proton

23. B. Bronsted-Lowry Definition C. Polyprotic Acids II. Defining Acids & Bases

24. Polyprotic Acids Those acids that donate more than one proton

25. III. Reactions

26. A. What does an acid do in water?

27. III. Reactions A. What does an acid do in water? 1. Arrhenius Acid

28. III. Reactions A. What does an acid do in water? 1. Arrhenius Acid 2. Bronsted-Lowry Acid

29. III. Reactions A. What does an acid do in water? 1. Arrhenius Acid 2. Bronsted-Lowry Acid B. What does a base do in water?

30. III. Reactions A. What does an acid do in water? 1. Arrhenius Acid 2. Bronsted-Lowry Acid B. What does a base do in water? 1. Arrhenius Base

31. III. Reactions A. What does an acid do in water? 1. Arrhenius Acid 2. Bronsted-Lowry Acid B. What does a base do in water? 1. Arrhenius Base 2. Bronsted-Lowry Base

32. III. Reactions A. What does an acid do in water? 1. Arrhenius Acid 2. Bronsted-Lowry Acid B. What does a base do in water? 1. Arrhenius Base 2. Bronsted-Lowry Base C. Conjugate Acid-Base Pairs

33. IV. Water

34. A.Water is amphoteric

35. IV. Water A.Water is amphoteric B.Water experiences self- ionization

36. IV. Water A.Water is amphoteric B.Water experiences self- ionization C.If there’s water, there’s H 3 O + and OH -

37. V. pH Scale

38. pH Scale A way to describe how much acid (H 3 O + ) is in a solution.

39. A.[H 3 O + ] can vary greatly V. pH Scale

40. A.[H 3 O + ] can vary greatly B.A neutral solution contains 0.0000001 mol/L H 3 O + V. pH Scale K eq = 1.0 x 10 -14

41. A.[H 3 O + ] can vary greatly B.A neutral solution contains 0.0000001 mol/L H 3 O + C.The pH scale is a logarithmic scale V. pH Scale pH = - log [H 3 O + ]

42. A.[H 3 O + ] can vary greatly B.A neutral solution contains 0.0000001 mol/L H 3 O + C.The pH scale is a logarithmic scale D.Finding [OH - ] V. pH Scale

43. A.[H 3 O + ] can vary greatly B.A neutral solution contains 0.0000001 mol/L H 3 O + C.The pH scale is a logarithmic scale D.Finding [OH - ] E.Calculating pOH V. pH Scale

44. VI. Strong Acids & Weak Acids

45. A. Strong Acids

46. VI. Strong Acids & Weak Acids A. Strong Acids 1. Completely dissociate

47. VI. Strong Acids & Weak Acids A. Strong Acids 1. Completely dissociate 2. Are good electrolytes

48. VI. Strong Acids & Weak Acids A. Strong Acids 1. Completely dissociate 2. Are good electrolytes 3. Equation notation:

49. HClHBrHI The 7 Strong Acids HNO 3 H 2 SO 4 HClO 3 HClO 4

50. Self Check – Ex. 1 What is the concentration of H 3 O + ions in a 0.25 M solution of HBr. What is the pH of this solution?

51. VI. Strong Acids & Weak Acids A. Strong Acids B. Weak Acids

52. 1. Partially dissociate before... VI. Strong Acids & Weak Acids A. Strong Acids B. Weak Acids

53. 1. Partially dissociate before... 2. Poor electrolyte VI. Strong Acids & Weak Acids A. Strong Acids B. Weak Acids

54. 1. Partially dissociate before... 2. Poor electrolyte 3. Described by: VI. Strong Acids & Weak Acids A. Strong Acids B. Weak Acids

55. 1. Partially dissociate before... 2. Poor electrolyte 3. Described by: 4. Finding H 3 O + for weak acids VI. Strong Acids & Weak Acids A. Strong Acids B. Weak Acids

56. Self Check – Ex. 2 What is the concentration of H 3 O + ions in a 1.0 M solution of HC 2 H 3 O 2 (K a = 1.8 x 10 -5 )

57. Solving weak acid problems

58. 1.Write equilibrium equation

59. Solving weak acid problems 1.Write equilibrium equation 2.Write equilibrium expression

60. Solving weak acid problems 1.Write equilibrium equation 2.Write equilibrium expression 3.Make a table of concentrations (before, change, & equilibrium)

61. Solving weak acid problems 1.Write equilibrium equation 2.Write equilibrium expression 3.Make a table of concentrations (before, change, & equilibrium) 4.Substitute equilibrium values into equilibrium expression.

62. Solving weak acid problems 1.Write equilibrium equation 2.Write equilibrium expression 3.Make a table of concentrations (before, change, & equilibrium) 4.Substitute equilibrium values into equilibrium expression. 5.Solve

63. Self Check – Ex. 2 What is the concentration of H 3 O + ions in a 1.0 M solution of HC 2 H 3 O 2 (K a = 1.8 x 10 -5 )

64. Self Check – Ex. 3 The pH of a 0.100 M solution of formic acid is 2.38. What is the K a for HCOOH?