1. UNITS 9 & 10 Review Game
Chemistry

2. Write the Formula
Lithium hydroxide

3. Write the Formula
Lithium hydroxide
LiOH

4. Name the Acid
HBr

5. Name the Acid
HBr
Hydrobromic Acid

6. If a soap has a hydrogen ion concentration of 2
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?

7. If a soap has a hydrogen ion concentration of 2
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?
[H+] = 2 x 10-6M pH = -log(2 x 10-6) = 5.7
Acid because pH < 7

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

9. What is the hydroxide ion concentration of a solution with a pH of 2.3? Is the substance an acid or base?
pOH = 14 – 2.3 = 11.7
[OH-] = = 2 x M
Acid because pH < 7

10. Name the Base
Mg(OH)2

11. Name the Base
Mg(OH)2
Magnesium Hydroxide

12. Write the Formula
Hydroiodidic Acid

13. Write the Formula
Hydroiodidic Acid HI

14. I used 50 grams of potassium chromate to make a 1. 4M solution
I used 50 grams of potassium chromate to make a 1.4M solution. What is the volume of the solution?

15. I used 50 grams of potassium chromate to make a 1. 4M solution
I used 50 grams of potassium chromate to make a 1.4M solution. What is the volume of the solution?
50 g K2CrO4 / 194 = 0.26 mol
1.4 = .26/v
V = L

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

17. What is the molarity of a potassium hydroxide solution which contains 0.94 moles of potassium hydroxide in 450 mL of water?
CM = 0.94/0.45 = 2.1 M

18. Name the Acid
H2SO4

19. Name the Acid
H2SO4
Sulfuric Acid

20. Name the Base
KOH

21. Name the Base
KOH
Potassium Hydroxide

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

23. What is the hydrogen ion concentration of a sample of phosphoric acid that has a pH of 4.9?
[H+] = = 1.3 x 10-5M

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?
HNO2 + KOH  KNO2 + H2O

26. Name the Base
Ca(OH)2

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

28. Name the Acid
HNO2

29. Name the Acid
HNO2
Nitrous Acid

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

31. Neutralization Reaction
Write the complete balanced equation for the neutralization of phosphoric acid with calcium hydroxide
2H3PO4 + 3Ca(OH)2  Ca3(PO4)2 + 6H2O

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

33. How many grams of copper (II) sulfate pentahydrate will be needed to make 75 mL of a M solution? (The molar mass of copper (II) sulfate pentahydrate is g/mole)
CM = n/V
.25 = n/0.075
n = mol x = 4.7 g

34. How many kilograms of sucrose, C12H22O11 ,will be needed to make 3
How many kilograms of sucrose, C12H22O11 ,will be needed to make 3.50 L of a 1.15 M solution?

35. How many kilograms of sucrose, C12H22O11 ,will be needed to make 3
How many kilograms of sucrose, C12H22O11 ,will be needed to make 3.50 L of a 1.15 M solution?
CM = n/v
1.15 = n/3.5
n = mol x 342 = g / 1000 = 1.38 kg

36. What is the pH of a solution made with 0
What is the pH of a solution made with 0.15 grams of sodium hydroxide in 4500 mL of water?

37. What is the pH of a solution made with 0
What is the pH of a solution made with 0.15 grams of sodium hydroxide in 4500 mL of water?
0.15 g / 40 = moles
M = /4.5 = 8.33X10-4 [OH-]
pOH = -log (8.33x10-4)
pOH = 3.08
pH = = 10.92

38. Write the Formula
Phosphoric Acid

39. Write the Formula
Phosphoric Acid
H3PO4

40. Write the Formula
Nitric Acid

41. Write the Formula
Nitric Acid
HNO3

42. What is the molarity of a solution that contains 0
What is the molarity of a solution that contains moles of NaHCO3 in a volume of 115 mL

43. What is the molarity of a solution that contains 0
What is the molarity of a solution that contains moles of NaHCO3 in a volume of 115 mL
CM = n/v
CM = 0.075/.115 = 0.65 M

44. A solution has 3. 00 moles of solute in 2
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. A solution has 3. 00 moles of solute in 2
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?
CM = n/V
CM = 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
Na2CO3

48. Write the Formula
Barium hydroxide

49. Write the Formula
Barium hydroxide
Ba(OH)2

50. Describe how you would prepare 1. 00L of a 0
Describe how you would prepare 1.00L of a 0.85 M solution of formic acid HCO2H?

51. Describe how you would prepare 1. 00L of a 0
Describe how you would prepare 1.00L of a 0.85 M solution of formic acid HCO2H?
CM = 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

52. What is the molarity of a sulfuric acid solution which contains 5
What is the molarity of a sulfuric acid solution which contains 5.4 grams of sulfuric acid in 250 mL of water?

53. What is the molarity of a sulfuric acid solution which contains 5
What is the molarity of a sulfuric acid solution which contains 5.4 grams of sulfuric acid in 250 mL of water?
5.4g/98 = mol
CM = 0.055/0.25 = 0.22 M

54. 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?

55. 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?
MaVa = MbVb
(0.4)(50) = Mb(35)
0.57 M

56. Calculate how many milliliters of 0
Calculate how many milliliters of 0.50M NaOH must be added to titrate 46 mL of 0.40 M HClO4

57. Calculate how many milliliters of 0
Calculate how many milliliters of 0.50M NaOH must be added to titrate 46 mL of 0.40 M HClO4
MaVa = MbVb
0.4(46) = 0.5Vb
Vb = 36.8 mL

58. Name the Base
NaOH

59. Name the Base
NaOH
Sodium Hydroxide

60. Write the Formula
Acetic Acid

61. Write the Formula
Acetic Acid
HC2H3O2

62. A 15.5 mL sample of 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. A 15.5 mL sample of 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?
(0.215)(15.5) = Ma(21.2)
0.157 M

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

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

66. A 20 mL sample of an HCl solution was titrated with 27
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 M. What is the molarity of the HCl?

67. A 20 mL sample of an HCl solution was titrated with 27
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 M. What is the molarity of the HCl?
(0.0154)(27.4) = Ma(20)
= M

68. I want to dilute 20 mL of a 6M solution of acetic acid to a 3
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. I want to dilute 20 mL of a 6M solution of acetic acid to a 3
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?
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
I mix 20 mL of 4.5M NaCl with 40 mL of water. What is the new concentration of the NaCl?

71. I mix 20 mL of 4. 5M NaCl with 40 mL of water
I mix 20 mL of 4.5M NaCl with 40 mL of water. What is the new concentration of the NaCl?
4.5(20) = M(60) Note: final volume is mL water added
M = 1.5 M

72. A 450 mL solution of 1. 5 M HCl is sat out over night
A 450 mL solution of 1.5 M HCl is sat out over night mL of the water evaporated. What is the new concentration of the HCl?

73. A 450 mL solution of 1. 5 M HCl is sat out over night
A 450 mL solution of 1.5 M HCl is sat out over night mL of the water evaporated. What is the new concentration of the HCl?
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. What does the term “strong acid” mean?
Strong acid means that the acid dissociates completely in water

76. Name the Acid
HCl

77. Name the Acid
HCl
Hydrochloric Acid

78. What is the pH of a solution made by putting 6
What is the pH of a solution made by putting 6.0 grams of phosphoric acid in 250 L of water?

79. What is the pH of a solution made by putting 6
What is the pH of a solution made by putting 6.0 grams of phosphoric acid in 250 L of water?
6 g H3PO4 / 98 = mol
[H3PO4] = / 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

80. What is the pH of a solution made by putting 3
What is the pH of a solution made by putting 3.25 grams of strontium hydroxide in 5000 L of water?

81. What is the pH of a solution made by putting 3
What is the pH of a solution made by putting 3.25 grams of strontium hydroxide in 5000 L of water?
3.25 g Sr(OH)2 / = mol
[Sr(OH)2] = / 5000 = 5.34 x 10-6M
[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