The Chemistry of Acids and Bases

1. The Chemistry of Acids and Bases

2. Acids and Bases: CharacteristicsAt the conclusion of our time together, you should be able to: Give examples of acids and bases List some properties of acids and bases Compare and contrast the characteristics of acids and bases

3. Hopefully, when we get done, you won’t be in this much trouble!!

4. Acid and Bases

5. Acid and Bases

6. Acid and Bases

7. Acids Have a sour taste. Ex. Vinegar is a solution of acetic acid. Citrus fruits contain citric acid. React with certain metals to produce hydrogen gas. React with carbonates and bicarbonates to produce carbon dioxide gas Bases Have a bitter taste. Feel slippery. Many soaps contain bases.

8. Kid’s Letters to God:

9. Some Properties of Acids • Produce H+ (as H3O+) ions in water (the hydronium ion is a hydrogen ion attached to a water molecule) • Taste sour, Corrode metals, Electrolytes • React with bases to form a salt and water • pH is less than 7, Turns blue litmus paper to red “Blue to Red A-CID”

10. Some Properties of Bases • Produce OH- ions in water • Taste bitter, chalky, are electrolytes • Feel soapy, slippery • React with acids to form salts and water • pH greater than 7 • Turns red litmus paper to blue “Basic Blue”

11. How Are a Texas Tornado And a Tennessee Divorce The Same? Somebody's Gonna Lose A Trailer.

12. Acids and Bases: CharacteristicsLet’s see if you can: Give examples of acids and bases List some properties of acids and bases Compare and contrast the characteristics of acids and bases

13. Get Your Clicker!!!

14. Which of the following is not a characteristic of an acid? • Tastes sour • pH is lower than 7 • Reacts with a base to form salt and water • Turns litmus paper blue • Produces H+ ions in water • All answers are correct

15. Which of the following is not a characteristic of a base? • Tastes bitter • pH is higher than 7 • Reacts with an acid to form salt and water • Turns litmus paper blue • Produces OH- ions in water • All answers are correct

17. The Chemistry of Acids and Bases

18. Acids and Bases: TheoriesAt the conclusion of our time together, you should be able to: Explain the 3 different theories for an acid, Arrhenius, Bronsted-Lowry, Lewis Explain the 3 different theories for a base, Arrhenius, Bronsted-Lowry, Lewis Identify conjugate acids and bases

19. Oh, that smarts!!

20. Acid/Base Theories • Theory #1: Arrhenius (traditional) Acids – produce H+ ions (or hydronium ions H3O+) Bases – produce OH- ions Simple look for an H at the beginning or an OH at the end of a compound (problem: some bases don’t have hydroxide ions!)

21. Arrhenius acid is a substance that produces H+ (H3O+) in water. Notice the H on the left. Arrhenius base is a substance that produces OH- in water, but notice there is no OH- on the left!!

22. Acid

23. Base

24. Acid/Base Theories • Theory #1: Arrhenius (traditional) Try the practice on your handout. • A • S • A • B • S • B

25. Pinned!!!

26. Acid/Base Theories Theory #2: Brønsted – Lowry Acids – proton donor Bases – proton acceptor A “proton” is really just a hydrogen atom that has lost its electron!

27. A Brønsted-Lowry acid is a proton donor A Brønsted-Lowry base is a proton acceptor conjugate acid conjugate base base acid

28. Acid-Base Theories The Brønsted definition means NH3 is a BASE in water — and water is itself an ACID

29. Conjugate Pairs

30. Learning Check! CH3OH + NH2-   CH3O+ + NH3 conjugate base conjugate acid acid base Label the acid, base, conjugate acid, and conjugate base in each reaction:

31. Learning Check! HCN + SO4-2   HSO4- + CN- conjugate acid conjugate base acid base Label the acid, base, conjugate acid, and conjugate base in each reaction:

32. Acid/Base Theories Theory #2: Brønsted – Lowry Try Top Table 1b. OH- 2b. H2O 3a. HCO3- 4b. NO3- 5a. NH4+

33. Acid/Base Theories Theory #2: Brønsted – Lowry Try Bottom Table 1b. H3O+ 2b. HCO3- 3b. H2CO3 4a. SO42- 5b. H3PO4

34. Kid’s Letters to God:

35. Acids & Base Theories Lewis acid - a substance that accepts an electron pair Theory #3 – Lewis Lewis base - a substance that donates an electron pair

36. Lewis Acids & Bases • Electron pair of the new O-H bond originates on the Lewis base. Formation of hydronium ion is an excellent example of the Lewis definition.

37. Lewis Acid or Bases Do the Lewis Structures of Both!! • BH3 • Lewis Acid • PBr3 • Lewis Base

38. Acids and Bases: TheoriesLet’s see if you can: Explain the 3 different theories for an acid, Arrhenius, Bronsted-Lowry, Lewis Explain the 3 different theories for a base, Arrhenius, Bronsted-Lowry, Lewis Identify conjugate acids and bases

39. Pass the Clicker!!!

40. Which of the following definitions of an acid includes conjugate acids? • Arrhenius • Bronsted-Lowry • Lewis

41. Which of the following definitions of an acid defines an acid as a proton donor? • Arrhenius • Bronsted-Lowry • Lewis

42. Which of the following definitions of an acid defines an acid as accepting an electron pair? • Arrhenius • Bronsted-Lowry • Lewis

43. Oh my goodness!!!

44. Which of the following definitions of an acid defines an acid as producing hydrogen ions? • Arrhenius • Bronsted-Lowry • Lewis

45. Identify the conjugate base in the following equation. • NH3 • H2O • NH4+ • OH-

46. Red-Neck Innovations:

47. According to Arrhenius theory, Cu(OH)2 is a(n): • Acid • Base • Salt

48. According to Arrhenius theory,Na2SO4 is a(n): • Acid • Base • Salt

49. Using the Bronsted Lowry theory, the conjugate base of H2SO4 would be: • HSO4+ • H3SO4- • HSO4- • H3SO4+

50. H2O + CO32- OH- + HCO3According to Bronsted Lowry theory, in the above reaction, H2O is a(n) • Acid • Base • Conjugate acid • Conjugate base