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5. 100 200 300 400 500 Misc.Acid misc.Base misc.Acid base definitions Titration pH/pOH

6. Acids produce ____ ions in water A 100

7. Hydronium; H 3 O + A 100

8. K w = ___x___=___ A 200

9. [H + ]; [OH - ]; 1.00x10 -14 A 200

10. Organic acids have a _____ backbone and a ______ group A 300

11. Carbon; carboxyl (COOH) A 300

12. What are dyes with pH- sensitive colors used for in Chemistry? A 400

13. Acid/base indicators A 400

14. Give two examples of compounds that could be produced by a neutralization reaction A 500

15. H 2 O; NaCl; NH 4 Cl; KCl; KNO 3 ; Ba(NO 3 ) 2 ; must have an ionic compound (salt) and water A 500

16. Acids make (blue) litmus paper turn this color B 100

17. Red B 100

18. Strong acids react with ____ to produce _____ and _____ B 200

19. Bases; salt; water B 200

20. Give an example of an oxyacid B 300

21. H 2 SO 4 ; H 3 PO 4 ; HNO 3 B 300

22. Which acid is produced in your stomach? B 400

23. Hydrochloric acid (HCl) B 400

24. List 4 strong acid names with their formulas B 500

25. Hydrochloric acid HCl, hydrobromic acid HBr, hydroiodic acid HI, nitric acid HNO 3, sulfuric acid H 2 SO 4 ; perchloric acid HClO 4 B 500

26. Bases either contain or react with water to form which ion C 100

27. OH - C 100

28. A strong base _______ completely and conducts _______ in water C 200

29. Dissociates; electricity C 200

30. Where on the periodic table can you find metals that will form strong bases (with hydroxide)? Are all those bases strong? C 300

31. Group 1; yes C 300

32. DAILY DOUBLE C 400 DAILY DOUBLE Place A Wager

33. Write a chemical equation that shows how ammonia reacts with water C 400

34. NH 3 + H 2 O => NH 4 + + OH - C 400

35. Calculate the hydroxide ion concentration in a solution with a hydrogen ion concentration of 1.00x10 -4 C 500

36. 1.00x10 -10 C 500

37. Arrhenius acids and bases form ___ in water D 100

38. Ions D 100

39. Arrhenius bases would increase the concentration of which ion in aqueous solutions? D 200

40. Hydroxide D 200

41. Bronsted-Lowry acids and bases donate or accept _____ D 300

42. Protons D 300

43. Tell whether these acids would form weak or strong conjugate bases: acetic acid, hydrochloric acid, sulfurous acid D 400

44. Strong, weak, strong D 400

45. A Lewis acid ____ electron pairs, while a Lewis base ____ electron pairs D 500

46. Accepts; donates D 500

47. What quantities must be known before beginning a titration? E 100

48. Concentration of either the acid or the base and the volume of the substance with the unknown concentration E 100

49. What quantity or quantities are measured during a titration? E 200

50. Volume of base (or acid if that’s the substance in the buret) E 200

51. A 750 mL sample of 1 M HCl is titrated with 0.5 M NaOH. What volume of NaOH is required to reach the endpoint of the titration? E 300

52. 1.5 L E 300

53. If 15 mL of a 5 M NaOH solution is needed to titrate 20 mL of HCl, what is the molarity of the HCl? E 400

54. 3.75 M E 400

55. Calculate the volume of 2.0 M Ba(OH) 2 that is required to titrate 10 mL of 0.05 M nitric acid. E 500

56. 0.125 mL Nitric acid reacts with barium hydroxide as expressed in the following reaction: 2HNO 3 + Ba(OH) 2 => Ba(NO 3 ) 2 + 2H 2 O The reaction products are barium nitrate and water. The barium nitrate is a salt, and in the classic acid-base reaction, the products are a salt and water. E 500

57. Acids have pH under __; neutral solutions have a pH of __; basic solutions have a pH over __ F 100

58. 7

59. pH=?; fill in the formula F 200

60. -log[H + ] F 200

61. pH + pOH= ___ F 300

62. 14 F 300

63. A solution with a high pH has a ___ pOH F 400

64. Low F 400

65. What is the hydronium ion concentration of a solution whose pH is 2.3? F 500

66. 5.0x10 -3 F 500

67. The Final Jeopardy Category is: Acid/base definitions Please record your wager. Click on screen to begin

68. What is the main assumption that the Arrhenius theory makes? Click on screen to continue

69. Acids and bases must produce ions in solution because they conduct electricity Click on screen to continue

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