1. Acids and Bases

2. Arrhenius Acid and Base Bronsted-Lowry Acid and Base Lewis Acid and Base Conjugate Acid and Base

3. Swedish Chemist: Svante Arrhenius Arrhenius Acid = compound that ionizes to yield hydrogen-ions (H+) in solution

4. Swedish Chemist: Svante Arrhenius Arrhenius Base = compound that ionizes to yield Hydroxide ions (OH-) in solution

5. Problem with Arrheinius Broad Definition Ex: Sodium carbonate and ammonia are not hydroxide compounds but are still basic

6. English Chemist: Thomas Lowry Bronsted-Lowry Acid: is a hydrogen ion (H+) donor

7. English Chemist: Thomas Lowry Bronsted-Lowry Base: is a hydrogen ion (H+) acceptor

8. Sample?

9. What do we call the products of these Bronsted-Lowry Reactions? Conjugates Conjugate Acid = base gains a hydrogen ion Conjugate Base = acid donated a hydrogen ion

10. Simplify this Identify the acid and base in beginning, find the opposite product in the end (acid/base)

11. Chemist: Gilbert Lewis Lewis Acid – accepts a pair of electrons Lewis Base – donates a pair of electrons

13. pH Scale

14. Apply the Numbers

15. NOTE [ BRACKETS ] = CONCENTRATION (MOLARITY)

16. Determining Strength Dissociation: compound breaking into ions HCl  H + Cl -

17. Determining Strength [H+] or [H 3 O+] = Acidic Strength [OH-] = Basic Strength

18. Using Water to Determine Strength K w = [H+] x [OH-] = 1.0x10 -14 Reference table!!!!!!!!!

19. Determining Strength We use the concentrations to determine if a solution is acidic or basic. Careful, since we are using a negative coefficient. The larger the coefficient = the smaller number. (this’ll make sense shortly)

21. Cokes are slightly acidic, if the [H+] in a solution is 1x10^5 M, is the solution acidic, basic, neutral? What is the [OH-] of the solution?

22. Is a [H+] = 6.0x10^-10 M solution acidic, basic, or neutral? (think logically, not # crunching)

23. Crunching Molarity and Kw can be complicated. pH

24. [H+] pH = -log [H+ ] Ref table

25. [OH-] pOH = -log[OH-] Ref table

26. What iF I gave you a hydroxide concentration and asked for pH pH + pOH = 14 Ref table

27. What is the [OH-] from a solution with a pH of 4.5?

28. What is the pH of a solution with a pOH of 3.2?

29. What is the pOH of a solution with [H+] = 3.5x10^-8 M

31. Acid Dissociation HCl --> H + and Cl -1-

32. Sour Taste React with metals Turn litmus paper RED http://www.cybered.net/library/Teaching_Resources/Chemistry/Properties_of_Acids/Image_Gallery/Properties-HydrogenHydroniu.jpg 3 Properties of Acids

33. Acid Examples

34. Bases

35. Bases end in “OH” (hydroxide)  NaOH  KOH  Mg(OH) 2

36. BASES Break into (OH) - ions

37. Base Dissociation Mg(OH) 2 --> Mg +2 and (OH) -

38. Properties of Bases Bitter taste Slippery feel (like soap) Turn litmus paper BLUE http://www.cybered.net/library/Teaching_Resources/Chemistry/Properties_of_Acids/Image_Gallery/Properties-HydrogenHydroniu.jpg

39. Acid + Base Acid + Base --> Water + Salt

40. pHpH

41. What is pH pH measures how ACIDIC (H) + a solution is

42. Every solution has both acidic (H) + and basic (OH) - ions in it, whichever ions have more will tell us the type of solution

44. The pH scale 0 --> 14 Color your pH scale according to the following slide

46. Neutral pH 7.0 Pure Water

47. Base pH Level pH greater than 7.0

48. Base pH Strength (common sense) Higher = Stronger

49. pH 12 stronger base than pH 9

50. Acids pH Levels pH below 7.0

51. Acid pH Strength (Reverse of common sense) Lower Number = Stronger

52. pH 1 is stronger acid than pH 5

53. How much does strength increase or decrease? Moving up/down on pH scale is by a factor of 10x

54. Compare pH of 4 to a pH of 5 Acidic pH of 4 is 10x more acidic than pH of 5 Basic pH of 5 is 10x more basic than pH of 4

55. Compare pH 9 to pH 12 Acidic pH 9 is 1000x more acidic (10x10x10) than pH 12 Basic pH 12 is 1000x more basic than pH 9

56. http://www.cybered.net/library/Teaching_Resources/Chemistry/Properties_of_Acids/Image_Gallery/Properties-PHconcept.jpg pH=0 Strongly Acidic pH=7 neutral pH=14 Strongly basic

57. What substance would you use to neutralize an acid with a pH of 1.5? A. Milk C. Ammonia B. Vinegar D. Water

58. Neutralization To neutralize a solution ADD Opposite! Add base to neutralize an acid Add acid to neutralize a base

59. Easy step Neutralizing pH calculation find neutralizing pH 14 – pH given = pH needed to neutralize

60. What pH would neutralize a stomach acid (ph of 2)

61. Pepto Bismol vs Milk of Magnesia pH ~6.0 pH ~10.0 Which would be better? Think about it!

62. Give dissociation of calcium hydroxide

63. pOH is 11.64, and you have 2.55L of solution, how many grams of Calcium hydroxide are in solution?

64. 1.5L of solution containing 5.6 g of hydroiodic acid, what is the pH