1. Acids and Bases

2. pH Scale

3. Apply the Numbers

4. NOTE [ BRACKETS ] = CONCENTRATION (MOLARITY)

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

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

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

8. 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)

10. Always get to this if confused

11. 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?

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

13. Crunching Molarity and Kw can be complicated. pH

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

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

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

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

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

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

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

22. 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

23. Acid Examples

24. Bases

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

26. BASES Break into (OH) - ions

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

28. 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

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

30. pHpH

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

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

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

36. Neutral pH 7.0 Pure Water

37. Base pH Level pH greater than 7.0

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

39. pH 12 stronger base than pH 9

40. Acids pH Levels pH below 7.0

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

42. pH 1 is stronger acid than pH 5

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

44. 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

45. 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

46. 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

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

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

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

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

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

52. Give dissociation of calcium hydroxide

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

54. 1.5L of solution containing 5.6 g of hydroiodic acid, what is the pH