1. Acid and Base Review Game Chemistry

2. Name the Acid  HBr

3. Name the Acid  HBr  Hydrobromic Acid

4. Write the Formula  Lithium hydroxide

5. Write the Formula  Lithium hydroxide  LiOH

6. Name the Base  Mg(OH) 2

7. Name the Base  Mg(OH) 2  Magnesium Hydroxide

8. Arrhenius  What is the “technical” definition of an acid in regards to ?

9. Arrhenius  A substance which produces H + when put in water

10. Write the Formula  Hydroiodidic Acid

11. Write the Formula  Hydroiodidic Acid  HI

12. Arrhenius  What is the “technical” definition of a base

13. Arrhenius  What is the “technical” definition of a base?  A substance which produces OH - when put in water

14. Name the Base  KOH

15. Name the Base  KOH  Potassium Hydroxide

16.  If a soap has a hydrogen ion concentration of 2.0 x 10 -6 M, what is the pH of the solution? Is it an acid or a base?

17.  [H + ] = 2 x 10 -6 M pH = -log(2 x 10 -6 ) = 5.7  Acid because pH < 7

18.  What is the hydroxide ion concentration of a solution with a pH of 2.3? Is the substance an acid or base?

19.  pOH = 14 – 2.3 = 11.7  [OH - ] = 10 -11.7 = 2 x 10 -12 M  Acid because pH < 7

20. Name the Acid  H 2 SO 4

21. Name the Acid  H 2 SO 4  Sulfuric Acid

22.  What is the hydrogen ion concentration of a sample of phosphoric acid that has a pH of 4.9?

23.  [H + ] = 10 -4.9 = 1.3 x 10 -5 M

24. Neutralization Reaction  Write the balanced neutralization reaction for nitrous acid reacting with potassium hydroxide?

25. Neutralization Reaction  Write the balanced neutralization reaction for nitrous acid reacting with potassium hydroxide?  HNO 2 + KOH  KNO 2 + H 2 O

26. Name the Base  Ca(OH) 2

27. Name the Base  Ca(OH) 2  Calcium Hydroxide

28. Neutralization Reaction  Write the complete balanced equation for the neutralization of phosphoric acid with calcium hydroxide

29. Neutralization Reaction  Write the complete balanced equation for the neutralization of phosphoric acid with calcium hydroxide  2H 3 PO 4 + 3Ca(OH) 2  Ca 3 (PO 4 ) 2 + 6H 2 O

30.  How many grams of copper (II) sulfate pentahydrate will be needed to make 75 mL of a 0.250 M solution? (The molar mass of copper (II) sulfate pentahydrate is 249.5 g/mole)

31.  C M = n/V .25 = n/0.075  n = 0.01875 mol x 249.5 = 4.7 g

32. Name the Acid  HNO 2

33. Name the Acid  HNO 2  Nitrous Acid

34.  How many kilograms of sucrose, C 12 H 22 O 11,will be needed to make 3.50 L of a 1.15 M solution?

35.  C M = n/v  1.15 = n/3.5  n = 4.025 mol x 342 = 1376.55 g / 1000 = 1.38 kg

36.  What is the pH of a solution made with 0.15 grams of sodium hydroxide in 4500 mL of water?

37.  0.15 g / 40 = 0.00375 moles  M = 0.00375/4.5 = 8.33X10-4 [OH-]  pOH = -log (8.33x10-4)  pOH = 3.08  pH = 14-3.08 = 10.92

38. Write the Formula  Phosphoric Acid

39. Write the Formula  Phosphoric Acid  H 3 PO 4

40.  What is the molarity of a solution that contains 0.0750 moles of NaHCO 3 in a volume of 115 mL

41.  C M = n/v  C M = 0.075/.115 = 0.65 M

42. Write the Formula  Nitric Acid

43. Write the Formula  Nitric Acid  HNO 3

44.  A solution has 3.00 moles of solute in 2.00 L of solution, what is its molar concentration? How many moles would there be in 350 mL of solution?

45.  C M = n/V  C M = 3/2 = 1.5M  1.5 = n/0.35  n = 0.53 mol

46. Write the Formula  Sodium carbonate

47. Write the Formula  Sodium carbonate  Na 2 CO 3

48.  Describe how you would prepare 1.00L of a 0.85 M solution of formic acid HCO 2 H?

49.  C M = n/v  0.85 = n/1  n = 0.85 mol x 46 = 39.1 g  Take 39.1 grams of formic acid and dissolve in a little bit of water. Put into a 1.00 L volumetric flask and fill to the line with water

50.  What is the molarity of a sulfuric acid solution which contains 5.4 grams of sulfuric acid in 250 mL of water?

51.  5.4g/98 = 0.055 mol  C M = 0.055/0.25 = 0.22 M

52.  What is the molarity of a potassium hydroxide solution which contains 0.94 moles of potassium hydroxide in 450 mL of water?

53.  C M = 0.94/0.45 = 2.1 M

54. Write the Formula  Barium hydroxide

55. Write the Formula  Barium hydroxide  Ba(OH) 2

56.  In the titration of 35 mL of liquid drain cleaner containing NaOH, 50 mL of 0.4M HCl must be added to reach the equivalence point. What is the molarity of the base in the cleaner?

57.  M a V a = M b V b  (0.4)(50) = M b (35) 0.57 M 0.57 M

58.  Calculate how many milliliters of 0.50M NaOH must be added to titrate 46 mL of 0.40 M HClO 4

59.  M a V a = M b V b  0.4(46) = 0.5V b  V b = 36.8 mL

60. Name the Base  NaOH

61. Name the Base  NaOH  Sodium Hydroxide

62.  A 15.5 mL sample of 0.215 M KOH was titrated with an acetic acid solution, It took 21.2 mL of the acid to reach the equivalence point. What is the molarity of the acetic acid?

63.  (0.215)(15.5) = M a (21.2)  0.157 M

64.  What is the molarity of a solution of acetic acid with a pH of 2.65?

65.  10 -2.65 = 0.0022M

66.  A 20 mL sample of an HCl solution was titrated with 27.4 mL of a standard solution of NaOH. The concentration of the standard is 0.0154 M. What is the molarity of the HCl?

67.  (0.0154)(27.4) = M a (20)  = 0.021 M

68.  I want to dilute 20 mL of a 6M solution of acetic acid to a 3.8M solution of acetic acid. How much water should I add to the 6M acetic acid to achieve this?

69.  6(20) = 3.8V  V = 31.6 mL  ADD 11.6 mL of water

70.  I mix 20 mL of 4.5M NaCl with 40 mL of water. What is the new concentration of the NaCl?

71.  4.5(20) = M(60) Note: final volume is 20+40 mL water added  M = 1.5 M

72.  A 450 mL solution of 1.5 M HCl is sat out over night. 150 mL of the water evaporated. What is the new concentration of the HCl?

73.  1.5 (450) = M (300) NOTE: final vol is 450 – 150 evaporated = 300  2.25 M

74.  What does the term “strong acid” mean?

75.  Strong acid means that the acid dissociates completely in water

76.  I used 50 grams of potassium chromate to make a 1.4M solution. What is the volume of the solution?

77.  50 g K 2 CrO 4 / 194 = 0.26 mol  1.4 =.26/v  V = 0.184 L

78. Write the Formula  Acetic Acid

79. Write the Formula  Acetic Acid  HC 2 H 3 O 2

80.  What is the pH of a solution made by putting 6.0 grams of phosphoric acid in 250 L of water?

81.  6 g H 3 PO 4 / 98 = 0.0612 mol  [H 3 PO 4 ] = 0.0612 / 250 = 2.45 x 10 -4  [H + ] = 3(2.45 x 10 -4 ) = 7.35 x 10 -4  pH = -log(7.35 x 10 -4 ) = 3.13

82. Name the Acid  HCl

83. Name the Acid  HCl  Hydrochloric Acid

84.  What is the pH of a solution made by putting 3.25 grams of strontium hydroxide in 5000 L of water?

85.  3.25 g Sr(OH) 2 / 121.6 = 0.0267 mol  [Sr(OH) 2 ] = 0.0267/ 5000 = 5.34 x 10 -6 M  [OH - ] = 2(5.34 x 10 -6 ) = 1.07 x 10 -5 M  pOH = -log(1.07 x 10 -5 ) = 4.97  pH = 14 – 4.97 = 9.03