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R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 04), P. 1 / 69 Chemistry 12 Provincial Exam Workbook Unit 04: Acid Base Equilibria Multiple Choice Questions 1. Calculate the volume of 0.300 M 3 HNO needed to completely neutralize 25.0 mL of 0.250 M 2 Sr OH . A. 10.4 mL B. 15.0 mL C. 20.8 mL D. 41.7 mL 2. Equal moles of which of the following chemicals could be used to make a basic buffer solution? A. HF and NaOH B. HCl and NaCl C. 3 KBr and NaNO D. 3 4 NH and NH Cl 3. Which reaction occurs when calcium oxide is added to water? A. 2 2 2CaO(s) Ca O (aq) B. 2 2CaO(s) 2Ca(aq) O (aq) C. 2 2 CaO(s) H O(l) Ca OH (aq) D. 2 2 CaO(s) H O(l) CaOH(aq) O (aq) 4. In which of the following is 3 HSO acting as a Brönsted-Lowry acid? A. 3 2 2 3 HSO HO H SO OH B. 2 3 3 4 3 NH HSO NH SO C. 2 3 3 4 2 3 4 HSO HPO H SO PO D. 2 2 4 3 2 4 2 3 HCO HSO HC O H SO

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Chemistry 12 Provincial Exam Workbook

Unit 04: Acid Base Equilibria

Multiple Choice Questions

1. Calculate the volume of 0.300 M 3HNO needed to completely neutralize 25.0 mL of

0.250 M 2

Sr OH .

A. 10.4 mL B. 15.0 mL C. 20.8 mL D. 41.7 mL 2. Equal moles of which of the following chemicals could be used to make a basic buffer

solution? A. HF and NaOH

B. HCl and NaCl

C. 3KBr and NaNO

D. 3 4NH and NH Cl

3. Which reaction occurs when calcium oxide is added to water?

A. 2 22CaO(s) Ca O (aq)

B. 22CaO(s) 2Ca(aq) O (aq)

C. 2 2CaO(s) H O(l) Ca OH (aq)

D. 2 2CaO(s) H O(l) CaOH(aq) O (aq)

4. In which of the following is 3HSO acting as a Brönsted-Lowry acid?

A. 3 2 2 3HSO H O H SO OH

B. 2

3 3 4 3NH HSO NH SO

C. 2 3

3 4 2 3 4HSO HPO H SO PO

D. 2 2 4 3 2 4 2 3H C O HSO HC O H SO

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5. What is the conjugate base of 2 4H PO ?

A. OH

B. 3

4PO

C. 2

4HPO

D. 3 4H PO

6. Which of the following is correct if the four solutions listed are compared to one

another?

7. Which of the following is the strongest acid that can exist in an aqueous solution?

A. 2O

B. 2NH

C. 3H O

D. 4HClO

8. Which of the following household products could have a pH = 12.0? A. soda pop B. tap water C. lemon juice D. oven cleaner 9. What is the pH of a 0.050 M KOH solution?

A. 0.30 B. 1.30 C. 12.70 D. 13.70

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10. What is the value of bK for 2 4H PO ?

A. 121.3x10

B. 86.2x10

C. 71.6x10

D. 37.5x10

11. Which of the following describes the net ionic reaction for the hydrolysis of 4NH Cl(s) ?

A. 4 4NH (aq) Cl (aq) NH Cl(s)

B. 4 4NH Cl(s) NH (aq) Cl (aq)

C. 2

Cl (aq) H O(l) HCl(aq) OH (aq)

D. 4 2 3 3NH (aq) H O(l) NH (aq) H O (aq)

12. Which of the following salts will produce a solution with the highest pH?

A. 1.0 M 3NaNO

B. 1.0 M 4NaHSO

C. 1.0 M 3NaHCO

D. 1.0 M 2 4NaH PO

13. What is true about the transition point of all indicators described by the following

equilibrium…

2 3HIn H O H O In

A. apH K

B. HIn In

C. 7

3H O 1.0x10 M

D. moles of 3H O equals moles of OH

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14. A chemical indicator has a 6

aK 4.0x10 . What is the pH at the transition point and

the identity of the indicator?

15. A 20.0 mL sample of HCl is titrated with 25.0 mL of 0.20 M 2

Sr OH . What is the

concentration of the acid? A. 0.13 M B. 0.20 M C. 0.25 M D. 0.50 M

16. Which of the following is the net ionic equation for the neutralization of 3HNO (aq) with

2

Sr OH (aq) ?

A. 2H (aq) OH (aq) H O(l)

B. 2

3 3 22Sr (aq) 2NO (aq) Sr NO (aq) 2H O(l)

C. 3 3 22 22HNO (aq) Sr OH (aq) Sr NO (aq) 2H O(l)

D. 2 2

3 3 22H (aq) 2NO (aq) Sr (aq) 2OH (aq) Sr (aq) 2NO (aq) 2H O(l)

17. When a strong acid is titrated with a strong base, what will the pH value be at the

equivalence point? A. 0.0 B. 6.8 C. 7.0 D. 8.6 18. Which of the following acids could not be present in a buffer solution? A. HF

B. 2HNO

C. 2 3H SO

D. 4HClO

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19. Which net ionic equation best describes the reaction between NaOH and 2H S ?

A. 2OH (aq) H (aq) H O(l)

B. 2

2 22OH (aq) H S(aq) 2H O(l) S (aq)

C. 2 2 22NaOH(aq) H S(aq) 2H O(l) Na S(aq)

D. 2 2

22Na (aq) 2OH (aq) 2H (aq) S (aq) 2H O(l) 2Na (aq) S (aq)

20. Which of the following is a general characteristic of Arrhenius acids?

A. They produce H in solution

B. They accept an H from water C. They turn bromthymol blue a blue colour

D. They react with 3H O ions to produce 2H

21. Identify a conjugate pair from the equilibrium provided…

3 2 2

4 3 4 3PO HCO HPO CO

A. 2 3

3 4CO and PO

B. 3

4 3PO and HCO

C. 3-

4PO and 2-

4HPO

D. 2

3 4HCO and HPO

22. Which of the following best describes a weak acid? A. Its 0.10 M solution will have pH of 1.00 B. It may be very soluble, but only partly ionized C. It must be very soluble and completely ionized D. It must be of low solubility and completely ionized

23. What is the pH at the transition point for an indicator with a aK of 42.5x10 ?

A. 42.5x10

B. 3.60 C. 7.00 D. 10.40

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24. What volume of 0.100 M NaOH is required to completely neutralize 15.00 mL of

0.100 M 3 4H PO ?

A. 5.00 mL B. 15.0 mL C. 30.0 mL D. 45.0 mL 25. What is the pH of the solution formed when 0.060 moles NaOH is added to 1.00 L of

0.050 M HCl ?

A. 2.00 B. 7.00 C. 12.00 D. 12.78 26. Which of the following graphs describes the relationship between the pH of a buffer

and the volume of NaOH added to the buffer?

27. A gas which is produced by internal combustion engines and contributes to the

formation of acid rain is…

A. 2H

B. 3O

C. 4CH

D. 2NO

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28. Consider the following reaction…

3 3 2 3 2H BO (aq) HS (aq) H BO (aq) H S(aq)

The order of Brönsted-Lowry acids and bases in this equation is…

A. acid, base, base, acid B. acid, base, acid, base C. base, acid, acid, base D. base, acid, base, acid 29. The conjugate base of an acid is produced by… A. adding a proton to the acid B. adding an electron to the acid C. removing a proton from the acid D. removing an electron from the acid

30. Which of the following represents the predominant reaction between 3HCO and

water?

A. 3 2 22HCO H O 2CO

B. 3 2 2 3HCO H O H CO OH

C. 2

3 2 3 3HCO H O H O CO

D. 2

3 2 3 3 22HCO H O H O CO OH CO

31. Water acts as an acid when it reacts with which of the following?

A. I and IV only B. II and III only C. I, II and IV only D. II, III and IV only

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32. A 41.0x10 M solution has a pH of 10.00. The solute is a…

A. weak acid B. weak base C. strong acid D. strong base 33. Consider the following Brönsted-Lowry equilibrium system…

2

3 2 4 3 3 4HSO H PO SO H PO

What are the two Brönsted-Lowry bases in the equilibrium above?

A. 2

3 3HSO and SO

B. 2

2 4 3H PO and SO

C. 3 3 4HSO and H PO

D. 2 4 3 4H PO and H PO

34. Which of the following will have the lowest electrical conductivity? A. 1.00M HCl

B. 1.00M 3HNO

C. 1.00M 2 4H SO

D. 1.00M 3 4H PO

35. Which of the following represents the ionization of water?

A. 2 2 2H O H 0.5O

B. 2 32H O H O OH

C. 2 2 2 22H O O 2H O

D. 2 2H O 0.5O 2H 2e

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36. Which of the following are amphiprotic?

A. I and II only. B. I and III only. C. II and III only. D. I, II and III. 37. Consider the following equilibrium:

2 32H O(l) energy H O (aq) OH (aq)

The temperature is increased and a new equilibrium is established. The new equilibrium can

be described by…

A. 14

WpH pOH and K 1.0x10

B. 14

WpH pOH and K 1.0x10

C. 14

WpH pOH and K 1.0x10

D. 14

WpH pOH and K 1.0x10

38. What is the 3H O at the equivalence point for the titration between HBr and KOH?

A. 91.0x10 M

B. 71.0x10 M

C. 51.0x10 M

D. 0.0 M 39. Which of the following would form a buffer solution when equal moles are mixed

together? A. HCl and NaCl

B. HCN and NaCN

C. 3KNO and KOH

D. 2 4Na SO and NaOH

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40. Which of the following oxides dissolves to form a solution with a pH greater than 7?

A. 2SO

B. 2CO

C. 2N O

D. 2K O

41. The pH of acid rain could be… A. 5.0 B. 7.0 C. 9.0 D. 11.0 42. A hydronium ion has the formula…

A. 2H

B. OH

C. 2H O

D. 3H O

43. The conjugate acid of 6 5 2C H NH is…

A. 6 5C H NH

B. 6 5 3C H NH

C. 6 5 2C H NH

D. 6 5 3C H NH

44. Which of the following is a property of 1.0 M HCl but not a property of 1.0 M

3CH COOH?

A. turns litmus red B. ionizes completely C. has a pH less then 7.0

D. produces 3H O in solution

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45. In a 1.0 M HF solution, the concentration of HF , F , and OH , from highest to lowest

is…

A.

B. F HF OH

C. OH HF F

D. OH F HF

46. In which of the following reactions is water behaving as a Brönsted-Lowry acid?

A. 2 2 22H O 2H O

B. 2 3HCl H O H O Cl

C. 3 2 4NH H O NH OH

D. 4 2 3 3NH H O H O NH

47. What is the OH of a solution with 2

3H O 9.3x10 M ?

A. 169.3x10 M

B. 138.6x10 M

C. 131.1x10 M

D. 29.3x10 M

48. The pH of 0.10 M 3HNO is…

A. 0.79 B. 1.00 C. 1.26 D. 13.00 49. What term is used to describe the point at which a chemical indicator changes

colour? A. titration point B. transition point C. equivalence point D. stoichiometric point

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50. When 25.0 mL samples of the strong acid 2 4H SO were titrated with 0.25 M NaOH

the following results were obtained…

What is the concentration of the 2 4H SO sample?

A. 0.20 M B. 0.21 M C. 0.40 M D. 0.42 M 51. Which of the following equations describes the predominant reaction that occurs at

the equivalence point of a titration between 3CH COOH(aq) and NaOH(aq) ?

A. 2H (aq) OH (aq) H O(l)

B. 3 2 3CH COO (aq) H O(l) CH COOH(aq) OH (aq)

C. 3 3 2CH COOH(aq) NaOH(aq) NaCH COO(aq) H O(l)

D. 3 3 2H (aq) CH COO (aq) Na (aq) OH (aq) Na (aq) CH COO (aq) H O(l)

52. Why is the solution below not considered to be a true buffer solution?

32 5 7

HCN(aq) H O (aq) CN (aq)H O(l)

1.0M 2.2x10 M 2.2x10 M

A. excessive HCN

B. excessive 3H O

C. insufficient CN

D. insufficient HCN

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53. What could be added to 1.0 L of the solution below in order for it to behave as a true buffer?

32 5 7

HCN(aq) H O (aq) CN (aq)H O(l)

1.0M 2.2x10 M 2.2x10 M

A. 1.0 mol HCl

B. 1.0 mol HCN

C. 1.0 mol 3H O

D. 1.0 mol NaCN

54. Which of the following equations correctly represents the reaction of a metallic oxide

with water?

A. 2 2K O H O 2KOH

B. 3 2 2 4SO H O H SO

C. 2 2 2 2 2Na O H O Na O H

D. 2 2NaOH H O Na 2H O

55. A definition for a Brönsted-Lowry acid should contain which of the following phrases?

A. the donation of H

B. the donation of OH

C. the acceptance of H

D. the acceptance of OH

56. Which equation represents the reaction of a Brönsted-Lowry base with water?

A. 2 22Na 2H O 2NaOH H

B. 2 4 2 2 5N H H O N H OH

C. 2 3

4 2 3 4HPO H O H O PO

D. 2 2 4 2 3 2 4H C O H O H O HC O

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57. Given the equilibrium…

2

2 3 2 4 3 3 4H BO H PO H BO HPO

Which is the strongest acid?

A. 2

4HPO

B. 3 3H BO

C. 2 4H PO

D. 2 3H BO

58. Which species will result in a solution with the greatest 3

H O ?

A. NaCN

B. 3 4Na PO

C. 2 3Na CO

D. 2 2 4Na C O

59. Which species is not amphiprotic?

A. 2H O

B. 3 3H BO

C. 2 4H PO

D. 2 6 5 7H C H O

60. At a given temperature a sample of pure water has a pH = 7.10. Which of the

following is true?

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61. Which of the following is a definition of pH?

A. 3pH log H O

B. pH pOH 14

C. 3pH log H O

D. wpH pOH pK

62. What is the mass of NaOH required to prepare 100.0 mL of NaOH(aq) that has a pH

of 13.62? A. 0.38 g B. 0.42 g C. 1.67 g

D. 142.40x10 g

63. Which of the following hypothetical acids would have the lowest conductivity?

64. What is the net ionic equation for the hydrolysis of 4NH Cl ?

A. 4 4NH Cl(aq) NH (aq) Cl (aq)

B. 2Cl (aq) H O(l) HCl(aq) OH (aq)

C. 4 2 3 3NH (aq) H O(l) H O (aq) NH (aq)

D. 2

4 2 4NH (aq) H O(l) HNH (aq) OH (aq)

65. What is the approximate pH of a 0.1 M solution of the salt 4NH Cl ?

A. 1.0 B. 5.0 C. 7.0 D. 9.0

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66. Consider the following indicator equilibrium…

2 3

HIn(aq) In (aq)H O H O (aq)

colourless blue

What is the effect of adding HCl to a blue sample of this indicator?

67. An indicator has a 6

aK 4x10 . Which of the following is true for this indicator?

68. Oxalic acid dihydrate is a pure, stable, crystalline substance. Which of the following

describes one of its uses in acid-base titrations? A. buffer B. primary standard C. chemical indicator D. stoichiometric indicator 69. What is the net ionic equation that describes the reaction of HCl(aq) with

2

Pb OH (s)?

A. 2H (aq) OH (aq) H O(l)

B. 2 222HCl(aq) Pb OH (s) PbCl (s) 2H O(l)

C. 2 222H (aq) 2Cl (aq) Pb OH (s) PbCl (s) 2H O(l)

D. 2 2 -

22H (aq) 2Cl (aq) Pb (aq) OH (aq) Pb (aq) 2Cl (aq) 2H O(l)

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70. Which of the following would be used to prepare an acidic buffer solution?

A. 3HF and H O

B. 2H S and NaHS

C. 3 4NH and NH Cl

D. 3 3HNO and NaNO

71. Four samples of rain are collected from different geographic regions and the pH is

measured for each sample.

Which of the above samples would be classified as acid rain? A. 1 only B. 1 and 2 C. 1, 2 and 3 D. 1, 2, 3 and 4 72. Which of the following is a characteristic that is common to bases?

A. They react with metals to produce -OH .

B. They produce a yellow colour in bromthymol blue solution.

C. They produce solutions with -OH smaller than -71x10 .

D. They produce solutions with +

3H O smaller than -71x10 .

73. What is a common substance found in solid drain cleaner? A. Na B. HCl C. NaCl D. NaOH

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74. Which equation contains a Brönsted-Lowry acid-base pair?

A. 2 2 22H (g)+O (g) 2H O(g)

B. + -NaOH(aq) Na (aq)+OH (aq)

C. 2 2Zn(s)+2HCl(aq) H (g)+ZnCl (aq)

D. + -

2 3H O(l)+HCN(aq) H O (aq)+CN (aq)

75. Which solution would have the greatest electrical conductivity? A. 0.1 M HCl

B. 0.1 M 3NH

C. 0.1 M 3 3H BO

D. 0.1 M 3CH OH

76. Which acid has the strongest conjugate base?

A. 2 2H O

B. 2 3H CO

C. 3HCO

D. 2 4HC O

77. What is the equilibrium expression for the water ionization constant?

A. w a bK K K

B. -14

wK =1.0x10

C. wK =pH+pOH

D. + -

w 3K = H O OH

78. What is the +

3H O in 100.0 mL of 0.0050 M NaOH?

A. -175.0x10 M

B. -132.0x10 M

C. -122.0x10 M

D. -112.0x10 M

79. What is the pH of a 2.5 M KOH solution?

A. -0.40 B. 0.40 C. 13.60 D. 14.40

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80. What is the value of bK for -

2 4H PO ?

A. -121.3x10

B. -86.2x10

C. -71.6x10

D. -37.5x10

81. One of the products of the reaction between HCl(aq) and 4

NH OH(aq) undergoes

hydrolysis. What is the net ionic equation for this hydrolysis reaction?

A. + -

4 4NH Cl(aq) NH (aq)+Cl (aq)

B. - -

2Cl (aq)+H O(l) HCl(aq)+OH (aq)

C. + +

4 2 3 3NH (aq)+H O(l) H O (aq)+NH (aq)

D. 4 4 2HCl(aq)+NH OH(aq) NH Cl(aq)+H O(l)

82. One of the species in the chemical indicator HIn exhibits a yellow colour. If acid is added, the indicator turns red. Which of the following is correct?

83. An indicator changes colour in the pHpH range of 6.40 to 7.20. What is the aK for

this indicator?

A. -74.0x10

B. -71.6x10

C. 0.80 D. 6.80

84. A 25.0 mL sample of the weak acid 2H S is titrated with 31.8 mL of 0.30 M NaOH (a

strong base). What is the concentration of the acid? A. 0.19 M B. 0.24 M C. 0.38 M D. 0.76 M

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85. Which of the following is the net ionic equation for the titration reaction of 3NH (aq)

with HCl(aq)?

A. + -

2H (aq)+OH (aq) H O(l)

B. + +

3 4NH (aq)+H (aq) NH (aq)

C. 3 4NH (aq)+HCl(aq) NH Cl(aq)

D. + +

3 4NH (aq)+H (aq)+Cl (aq) NH (aq)+Cl (aq)

86. What is the main function of a buffer solution? A. to neutralize acids B. to resist changes in pH C. to maintain solution neutrality D. to prevent acids from mixing with bases 87. Which of the following would commonly be used to prepare a buffer solution? A. HCl and KCl

B. 3NH and 4

NH Cl

C. 2H S and 2 4Na SO

D. 2 3Na CO and NaOH

88. Which of the following represents a reaction that can occur between a non-metallic

oxide and water?

A. 2 2 2 3SO +H O H SO

B. 2 2Na O+H O 2NaOH

C. 2 2CaO+H O Ca OH

D. 2 2 2 2NO +H O H NO+O

89. Which of the following represents the results of tests on an acidic solution?

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90. Which of the following represents a protonated water molecule?

A. 2H O

B. 3H O

C. +

2H O

D. +

3H O

91. Which of the following best describes a weak base?

92. Which species will produce the greatest hydroxide ion concentration in solution?

A. +

4NH

B. 3-

4PO

C. -

3HCO

D. 2 3H CO

93. Water will react most completely as an acid with...

A. 2-

3SO

B. -

2 3H BO

C. -

6 5C H O

D. -

3CH COO

94. What does this equation represent?

A. wK

B. the ionization of water C. the ion product of water D. the equilibrium expression for water

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95. Which of the following is correct for water?

96. What is the pH of 0.50 M LiOH?

A. -142.0x10

B. -0.30 C. 0.30 D. 13.70 97. What is the equilibrium constant expression for the predominant equilibrium in

3NaHSO (aq)?

A.

+ 2-

3 3

-

3

H O SO

HSO

B. -

2 3

-

3

OH H SO

HSO

C. + -

3 3NaHSO (aq) Na (aq)+HSO

D. - + 2-

3 2 3 3HSO (aq)+H O(l) H O (aq)+SO

98. Which of the following 0.10 M solutions would have the lowest pH? A. HF

B. 3NH

C. 3HNO

D. 2 3H CO

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99. Which of the following describes a solution of 4LiClO (aq) with respect to hydrolysis?

A. + +

2Li (aq)+H O(l) LiOH(aq)+H (aq)

B. 4 2 4LiClO (aq)+H O(l) LiOH(aq)+HClO (aq)

C. - -

4 2 4ClO (aq)+H O(l) OH (aq)+HClO (aq)

D. No hydrolysis reaction occurs. 100. Which of the following is a basic salt solution?

A. 3NH (aq)

B. 4NH I(aq)

C. 3KNO (aq)

D. 2 3Na CO (aq)

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Written Questions

1. Calculate the pH of a 1.5 M 2H S solution. (4 marks)

2. Consider the following reaction…

2 222HCl(aq) Ba OH (s) BaCl (aq) 2H O(l)

When 3.16 g samples of 2

Ba OH were titrated to the equivalence point with an HCl solution,

the following data were recorded…

Using the data above, calculate the original HCl . (4 marks)

3. In aqueous solutions 3H O is the strongest acid present. This phenomenon is called

the leveling effect. Explain why this occurs. (2 marks)

4. A 1.00 M OCl solution has an OH of 45.75x10 M .

A. Calculate bK for OCl . (3 marks)

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B. Calculate aK for HOCl . (1 mark)

5. Calculate the mass of 2 4

H PO needed to prepare 2.0 L of a solution with a pH of

12.00. (3 marks)

6. Consider a Brönsted-Lowry acid-base equation, where 2HNO is a reactant and

2 4H PO is a product.

A. Complete the following equation: 2 2 4HNO ? ? H PO (1 mark)

B. Identify the weaker base in the equilibrium in part a). (1 mark)

7. A 0.0200 M solution of methylamine, 3 2CH NH , has a pH of 11.40.

Calculate the bK for methylamine. (4 marks)

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8. A titration was performed by adding 0.115 M NaOH to a 25.00 mL sample of 2 4H SO .

Calculate the 2 4H SO from the following data. (3 marks)

9. A sample of a weak acid was found to conduct an electric current better than a

sample of a strong acid. Explain these results in terms of ion concentration. (2 marks)

10. Calculate the OH of 0.10 M 3NH . (4 marks)

11. A titration was performed by adding 0.175 M 2 2 4H C O to a 25.00 mL sample of

NaOH . The following data was collected…

Calculate the NaOH . (3 marks)

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B. Explain why the pH at the equivalence point is greater than 7.0. (1 mark)

12. A 0.100 M solution of an unknown weak acid, HX , has a pH of 1.414.

What is the aK for HX ? (4 marks)

13. Consider the salt ammonium acetate, 4 3NH CH COO .

A. Write the equation for the dissociation of 4 3NH CH COO . (1 mark)

B. Write equations for the hydrolysis reactions which occur. (2 marks)

C. Explain why a solution of 4 3NH CH COO has a pH of 7.00. Support your answer with

calculations. (2 marks)

14.

A. Define the term Brönsted-Lowry conjugate acid-base pair. (1 mark)

B. Give an example of a conjugate acid-base pair. (1 mark)

Acid:

Base:

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15. Consider the acids HCl and HF …

A. Only one of the following reactions occurs. Complete the equation for the reaction which does occur. (1 mark)

HCl F ?

HF Cl ?

B. For the reaction that occurs, are reactants or products favoured? Explain. (1 mark)

C. Explain why the other reaction will not occur. (1 mark)

16. Calculate the 3H O of 0.10 M 2HNO . (3 marks)

17. Write the formula equation and the net ionic equation for the reaction between 0.10 M

2 4H SO and 0.10 M 2

Sr OH . (3 marks)

Formula equation:

Net ionic equation:

18. Consider the following Brönsted-Lowry equilibrium:

2

2 3 4 2 4 3H SO (aq) HPO (aq) H PO (aq) HSO (aq)

A. Identify the two Brönsted-Lowry acids in the above equilibrium. (1 mark)

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B. Define the term conjugate acid. (1 mark)

19. A 250.0 mL sample of HCl with a pH of 2.000 is completely neutralized with 0.200 M

NaOH .

A. What volume of NaOH is required to reach the stoichiometric point? (4 marks)

B. Write the net ionic equation for the above neutralization reaction. (1 mark)

C. If the HCl were titrated with a 0.200 M 3NH (aq) instead of 0.200 M NaOH , how would the

volume of base required to reach the equivalence point compare with the volume calculated in part a) ? Explain your answer. (1 mark)

20. Consider the following equilibrium…

2 3energy 2H O H O OH

A. Explain how pure water can have a pH of 7.30. (2 marks)

B. Calculate the value of WK for the sample of water with a pH of 7.30. (2 marks)

21. Identify a gas which causes acid rain, and write an equation showing this gas reacting

with water. (2 marks)

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22. Consider the 0.10 M solutions of the following two acids:

A. What can you conclude about the acids that will explain these different pH values? (1 mark)

You can conclude that acid HA:

You can conclude that acid HB:

B. Compare the volume of 0.10 M NaOH needed to neutralize equal volumes of each of

these acid samples. (1 mark)

23. Consider a 1.0 M solution of 4NH F …

A. Write both hydrolysis reactions that occur when 4NH F is dissolved in water. (2 marks)

B. Will the above 4NH F solution be acidic, basic, or neutral? Support your answer with

calculations. (2 marks)

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24. An indicator is often used during acid-base titrations…

A. Define the term transition point for an indicator. (1 mark)

B. Calculate the aK value for methyl red. (1 mark)

C. A mixture of indicators is made by combining equal amounts of methyl orange and bromthymol blue. Complete the following table, showing the colour of each indicator and the

mixture at pH of 5 and pH of 9. (2 marks)

25. Will 2 4HC O act predominantly as an acid or as a base in solution? Support your

answer with calculations. (3 marks)

26. The two reactants in an acid-base reaction are 2HNO (aq) and -

3HCO (aq) .

A. Write the equation for the above reaction. (2 marks)

B. Define the term conjugate acid-base pair. (1 mark)

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C. Write the formulas for a conjugate acid-base pair for the above reaction. (1 mark)

27. At 10.0 C, -15

wK =2.95x10 for pure water.

A. Calculate the pH of water at 10.0 C. (3 marks)

B. A mixture of the indicators phenolphthalein and bromcresol green is added to the water. What is the resulting colour of the mixture? Explain. (2 marks)

28. At a particular temperature a 1.0 M 2H S solution has a pH of 3.75 . Calculate the

value of aK at this temperature. (4 marks)

29. What is the main function of a buffer solution? (1 mark)

30. The ion -

2 4H PO is an amphiprotic anion.

A. Define the term amphiprotic. (1 mark)

B. Write the balanced equation for the reaction when -

2 4H PO reacts with HF . (2 marks)

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31. Write an equation for a reaction in which 2H O acts only as a Brönsted-Lowry base. (2

marks)

32. Calculate the pH of 0.25 M 2

Sr OH . (2 marks)

33. Calculate the pH of 0.25 M 4NH Cl . (5 marks)

34. A 0.1 M unknown acid is titrated with 0.10 M NaOH and the following titration curve

results…

A. Choose a suitable indicator (other than phenolphthalein) and give a reason for your choice. (1 mark)

B. Is the unknown acid weak or strong? Explain. (2 marks)

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35. The cyanide ion, -CN , is a Brönsted-Lowry base.

A. Define Brönsted-Lowry base. (1 mark)

B. Write the equation representing the reaction of -CN with water. (2 marks)

C. Identify a conjugate pair in B. above. (1 mark)

36. Write an equation to show the ionization of water. (2 marks)

37. Calculate the pH of 1.50 M 3NH . (5 marks)

38. Consider the following buffer equilibrium...

+ -

32

HF(aq) H O F+H O(l) +

high concentration low concentration high concentration

Using Le Chatelier’s Principle, explain what happens to the pH of the buffer solution when a

small amount of NaOH is added.

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39. Consider the following equilibria…

A. In equation I above, the reactants are favoured. Identify the stronger acid. (1 mark)

B. In equation II above, the products are favoured. Identify the stronger acid. (1 mark)

C. Consider the following reaction… - -HOCN+ClO OCN +HClO . Does this reaction favour

reactants or products? Explain. (2 marks)

40. At 60 C, the pH for pure water is 6.51. Determine the value of wK at this temperature.

(3 marks)

41. Calculate the pH of 0.35 M 2 3H CO . (4 marks)

42. A strong acid strong base titration has a pH of 7.0 at the equivalence point. A weak

acid strong base titration has a pH greater than 7.0 at the equivalence point.

A. What causes the difference in these pH values? (2 marks)

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B. Select one indicator which could be used for both titrations. (1 mark)

43. Write a chemical reaction showing an amphiprotic anion reacting as a base in water.

(2 marks)

44. Calculate the pOH of 0.25 M 2

Sr OH . (2 marks)

45. A 2.00 M diprotic acid has a pH of 0.50. Calculate the aK value. (5 marks)

46. The following two experiments were conducted…

Titration A A strong acid was titrated with a strong base.

Titration B A weak acid was titrated with a strong base.

A. How does the pH at the equivalence point of Titration B compare with the pH at the

equivalence point in titration A? (1 mark)

B. Explain your answer to A. (2 marks)

47. An acid-base reaction occurs between -

3HSO and -

3IO .

Write the equation for the equilibrium that results. (1 mark)

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B. Identify one conjugate acid base pair in the reaction. (1 mark)

C. State whether reactants or products are favoured and explain how you arrived at your answer. (2 marks)

48. At 10 C, -15

wK =2.95x10 .

A. Determine the pH of water at 10 C. (3 marks)

B. State whether water at this temperature is acidic, basic or neutral, and explain. (1 mark)

49. Calculate the pH of 0.50 M 2H S . (4 marks)

50. Outline a procedure to prepare a buffer solution. (3 marks)

51. Calculate the pH of a 0.60 M 4NH I . Start by writing the equation for the predominant

equilibrium reaction. (5 marks)

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52. Calculate the pH of a 0.35 M solution of the salt ammonium bromide. Begin by writing the equation for the predominant equilibrium. (5 marks)

53. The following three solutions are mixed in a fourth container, what pH results? (3

marks)

54. Complete the following equilibrium, then predict whether the reactants or products will

be favoured and explain why. (3 marks)

Equilibrium equation

- -3 4HSO +HSO _____ _____

Reactants or products favoured?

Explanation:

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55. Calculate the initial concentration of a KF salt solution that has a pH of 6.5. Begin by writing the equation for the predominant equilibrium reaction. (5 marks)

56. In three separate trials, 10.00 mL samples of 2 4H SO were titrated with 0.40 M NaOH

and the results are as below. Calculate the concentration of the 2 4H SO . (3 marks)

57. A Solution of 2

Sr OH (aq) is titrated with 2 4H SO . Explain what will happen to the

electrical conductivity during the titration. Begin by writing the balanced formula equation, including states, to support your answer. (3 marks)

Balanced formula equation

Explanation

58. Aniline 6 5 2C H NH is a weak base with a -10

bK =4.3x10 . Calculate the concentration

of an aniline solution that has a pH of 8.00. Begin by writing the equation for the predominant equilibrium. (5 marks)

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59. Calculate the OH that results when 800.0 mL of 0.010 M HCl is mixed with 1.216

g 2

Sr OH . Assume no volume change on mixing. (3 marks)

60. For the reactant pair 2 4KHC O and 2 4Na HPO , write the net ionic equation for the

predominant equilibrium reaction that will be established. Predict whether the equilibrium will favour reactants or products and explain why. (3 marks)

Equilibrium

Reactants or products favoured?

Explanation

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Multiple Choice Questions Answer Key

1 D 21 C 41 A 61 C 81 C

2 D 22 B 42 D 62 C 82 D

3 C 23 B 43 D 63 B 83 B

4 B 24 D 44 B 64 C 84 A

5 C 25 C 45 A 65 B 85 B

6 C 26 D 46 C 66 A 86 B

7 C 27 D 47 C 67 C 87 B

8 D 28 A 48 B 68 B 88 A

9 C 29 C 49 B 69 C 89 A

10 A 30 B 50 A 70 B 90 D

11 D 31 C 51 B 71 B 91 A

12 C 32 D 52 C 72 D 92 B

13 B 33 B 53 D 73 D 93 C

14 A 34 D 54 A 74 D 94 B

15 D 35 B 55 A 75 A 95 C

16 A 36 B 56 B 76 A 96 D

17 C 37 A 57 C 77 D 97 A

18 D 38 B 58 D 78 C 98 C

19 B 39 B 59 B 79 D 99 D

20 A 40 D 60 D 80 A 100 D

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Written Questions Answer Key 1.

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2.

3.

4.

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5.

6.

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7.

8.

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9.

10.

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11.

12.

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13.

14.

15.

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16.

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17.

18.

19.

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20.

21.

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22.

23.

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24.

25.

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26.

27.

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28.

29.

30.

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31.

32.

33.

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34.

35.

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36.

37.

38.

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39.

40.

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41.

42.

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43.

44.

45.

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46.

47.

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48.

49.

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50.

51.

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52.

53.

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54.

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55.

56.

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57.

58.

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59.

60.