47
R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 1 / 47 Chemistry 12 Provincial Exam Workbook Unit 03: Solubility Equilibrium Multiple Choice Questions 1. Which of the following would be true when equal volumes of 0.2 M NaBr and 0.2 M 3 AgNO are combined? A. No precipitate forms B. A precipitate of AgBr forms C. A precipitate of 3 NaNO forms D. Precipitates of both 3 NaNO and AgBr form 2. Using the solubility table, determine which of the following ions could not be used to separate 2 S from 2 4 SO by precipitation? A. 2 Be B. 2 Ca C. 2 Ba D. 2 Sr 3. Which of the following is true when solid 2 Na S is added to a saturated solution of CuS and equilibrium is re-established? A. 2 S increases B. 2 Cu increases C. 2 S does not change D. 2 Cu does not change

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R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 1 / 47

Chemistry 12 Provincial Exam Workbook

Unit 03: Solubility Equilibrium

Multiple Choice Questions 1. Which of the following would be true when equal volumes of 0.2 M NaBr and 0.2 M

3AgNO are combined?

A. No precipitate forms B. A precipitate of AgBr forms

C. A precipitate of 3NaNO forms

D. Precipitates of both 3NaNO and AgBr form

2. Using the solubility table, determine which of the following ions could not be used to

separate 2S from 2

4SO by precipitation?

A. 2Be

B. 2Ca

C. 2Ba

D. 2Sr

3. Which of the following is true when solid 2Na S is added to a saturated solution of

CuS and equilibrium is re-established?

A. 2S increases

B. 2Cu increases

C. 2S does not change

D. 2Cu does not change

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4. Which of the following describes the relationship between the solubility product

constant spK and the solubility s of 2PbI ?

A. 2

spK =s

B. 3

spK =4s

C. 3

spKs=

4

D. sps= K

5. Which of the following saturated solutions will have the lowest 2S ?

A. BaS

B. CaS

C. CuS

D. ZnS

6. What is the solubility of 2SrF ?

A. 253.2x10 M

B. 171.8x10 M

C. 94.3x10 M

D. 31.0x10 M

7. Which of the following is a suitable term for representing solubility? A. grams B. moles C. molarity D. millilitres per second

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8. A saturated solution is prepared by dissolving a salt in water. Which of the following graphs could represent the ion concentrations as the temperature is changed?

9. What is the concentration of OH ions in 250 mL of 0.20 M 2

Sr OH ?

A. 0.050 M B. 0.10 M C. 0.20 M D. 0.40 M

10. What happens when 10.0 mL of 0.2 M KOH is added to 10.0 mL of 0.2 M 4

CuSO ?

A. No precipitate forms

B. A precipitate of 2 4K SO forms

C. A precipitate of 2

Cu OH forms

D. Precipitates of 2 4K SO and 2

Cu OH form

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11. Consider the following equilibrium…

2 2

4 4CaSO (s) Ca (aq) SO (aq)

Which of the following would shift the above equilibrium to the left?

A. adding 4CaSO (s)

B. adding 4MgSO (s)

C. removing some 2Ca (aq)

D. removing some 2

4SO (aq)

12. Calculate the solubility of 2 4CaC O .

A. 92.3x10 M

B. 51.2x10 M

C. 54.8x10 M

D. 48.3x10 M

13. How many moles of dissolved solute are present in 100.0 mL of a saturated 3SrCO

solution?

A. 115.6x10 mol

B. 62.4x10 mol

C. 52.4x10 mol

D. 42.4x10 mol

14. What happens when equal volumes of 0.2 M 3AgNO and 0.2 M NaCl are combined?

A. A precipitate forms because the trial ion product > spK

B. A precipitate forms because the trial ion product < spK

C. No precipitate forms because the trial ion product > spK

D. No precipitate forms because the trial ion product < spK

15. Determine the maximum 2 3Na CO that can exist in 1.0 L of 0.0010M 3 2Ba NO

without forming a precipitate.

A. 122.6x10 M

B. 92.6x10 M

C. 62.6x10 M

D. 52.6x10 M

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16. Solid 2

Ba OH is added to water to prepare a saturated solution. Which of the

following is true for this equilibrium system?

A. anion cation

B. trial spK is less than

spK

C. blue litmus paper would turn red D. the rate of dissolving = the rate of crystallization

17. A saturated solution of 2PbI was subjected to a stress and the following graph was

obtained.

Which stress was applied at time 1t ?

A. the addition of 2PbI

B. a temperature change C. an increase in volume D. the evaporation of water

18. A solution is prepared containing both 0.2 M OH and 0.2 M 3

4PO ions. An equal

volume of a second solution is added in order to precipitate only one of these two anions. The second solution must contain which of the following?

A. 0.2 M Cs

B. 0.2 M 2Zn

C. 0.2 M 2Pb

D. 0.2 M 2Sr

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19. Consider the following equilibrium…

2 2CaS(s) Ca (aq) S (aq)

When 3 2Ca NO (aq) is added to this solution, the equilibrium shifts to the…

A. left and 2S increases

B. left and 2S decreases

C. right and 2S increases

D. right and 2S decreases

20. How many moles of 2Pb are there in 500.0 mL of a saturated solution of 4PbSO ?

A. 163.2x10

B. 99.0x10

C. 56.7x10

D. 41.3x10

21. Which of the following compounds is least soluble in water? A. CuI

B. BeS

C. CsOH

D. 3AgBrO

22. Which of the following will dissolve to form a molecular solution?

A. 2 4H SO

B. 3AgNO

C. 2

Ca OH

D. 6 12 6C H O

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R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 7 / 47

23. Consider the following equilibrium…

energy AgCl(s) Ag (aq) Cl (aq)

Addition of which of the following will increase the solubility of AgCl ?

A. heat B. HCl

C. 3AgNO

D. a catalyst

24. What is the Cl when 15.0 g of NaCl is dissolved in enough water to make 100.0

mL of solution? A. 0.150 M B. 0.390 M C. 2.56 M D. 3.90 M

25. An equal number of moles of 2 3Na CO is added to four different 10.0 mL samples.

A precipitate forms in only one of the samples. Identify the cation which is present in the precipitate.

A. 2Ba

B. 2Ca

C. 2Mg

D. 2Sr

26. What is the net ionic equation for the reaction between BaS(aq) and 2

Sr OH (aq) ?

A. 2 2Sr (aq) S (aq) SrS(s)

B. 2

2Ba (aq) 2OH (aq) Ba OH (s)

C. 2 2 2

2Ba (aq) S (aq) Sr (aq) 2OH (aq) Ba OH (s) SrS(s)

D. 2 2 2 2 2-

2Ba (aq) S (aq) Sr (aq) 2OH (aq) Ba OH (s) Sr (aq) S (aq)

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27. In which of the following would 2PbCl (s) be least soluble?

A. 1 M HCl

B. 1 M 2BaCl

C. 1 M 2 4K SO

D. 1 M 3 2Pb NO

28. The solubility of 3ZnCO is 96.4x10 M . What is the value of spK for 3ZnCO ?

A. 174.1x10

B. 96.4x10

C. 81.3x10

D. 58.0x10

29. What is the spK for the salt 3 2Pb IO if its solubility is -55.0x10 M?

A. -135.0x10

B. -131.3x10

C. -92.5x10

D. -55.0x10

30. What is the maximum -

3IO that can exist in a -26.9x10 M 2+Cu solution?

A. -62.0x10 M

B. -61.0x10 M

C. -31.0x10 M

D. -26.9x10 M

31. Which of the following will form a saturated solution?

A. 0.10 mol 4CaSO added to 1.0 L of water

B. 0.10 mol 2 4Cs SO added to 1.0 L of water

C. 0.20 mol 4MgSO added to 2.0 L of water

D. 0.50 mol 3 2Pb NO added to 2.0 L of water

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32. Which of the following would be an appropriate measure of solubility? A. moles of solute per volume of solute B. mass of solute per volume of solution C. volume of solvent per mass of solvent D. moles of solute at a specific temperature 33. What is the complete ionic equation for the precipitation reaction between MgS(aq)

and 2

Sr OH (aq) ?

A. 2+

2Mg (aq)+2OH(aq) Mg OH (s)

B. 2 2

MgS(aq)+Sr OH (aq) SrS(aq)+Mg OH (s)

C. 2+ 2- 2+ 2+ -Mg (aq)+S (aq)+Sr (aq)+2OH (aq) SrS(s)+Mg (aq)+2OH (aq)

D. 2+ 2- 2+ 2+ 2-

2Mg (aq)+S (aq)+Sr (aq)+2OH (aq) Sr (aq)+S (aq)+Mg OH (s)

34. What is the spK expression for the low solubility salt formed when 2 3K SO (aq) and

3AlCl (aq) are mixed?

A. 2-

sp 3K = SO

B. + -

spK = K Cl

C. 2 3

3+ 2-

sp 3K = Al SO

D. 3 2

3+ 2-

sp 3K = Al SO

35. Which compound has the lowest solubility? A. ZnS

B. CuS

C. AgCl

D. 4SrSO

36. What is the solubility of the salt 2PbCl ?

A. -21.4x10 M

B. -32.4x10 M

C. -33.5x10 M

D. -51.2x10 M

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37. A solution is found to contain a 2+Pb of 0.10 M. What is the maximum 2-

4SO that

can exist in this solution before a precipitate forms?

A. 2- -9

4SO =1.8x10 M

B. 2- -8

4SO =1.8x10 M

C. 2- -7

4SO =1.8x10 M

D. 2- -4

4SO =1.3x10 M

38. Which solute will result in a molecular solution? A. HCN

B. 2

Ba OH

C. 3CH COOH

D. 3 2CH CH OH

39. Which best describes the equilibrium in a saturated solution? A. The rate of crystallization determines the solubility. B. The rate of crystallization equals the rate of dissolving. C. There is no solid solute on the bottom of the container. D. The solute is completely dissolved and the equilibrium favours the products. 40. Which compound will have a solubility greater than 0.1 M at 25°C? A. SrS

B. CoS

C. 4BaSO

D. 2 4Ag SO

41. What is the net ionic equation for the reaction between 0.10 M 2Na S and 0.10 M

3 2Zn NO ?

A. 2= 2-Zn (aq)+S (aq) ZnS(s)

B. + -

3 3Na (aq)+NO (aq) NaNO (s)

C. 2 3 32Na S(aq)+Zn NO (aq) ZnS(s)+2NaNO (aq)

D. + 2- 2+ - + -

3 32Na (aq)+S (aq)+Zn (aq)+2NO (aq) ZnS(s)+2Na (aq)+2NO (aq)

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42. When equal volumes of 0.20 M NaOH and 0.20 M CaS are mixed together…

A. a precipitate forms and the trial spK would be less than

spK

B. no precipitate forms and the trial spK would be less than

spK

C. a precipitate forms and the trial spK would be greater than

spK

D. no precipitate forms and the trial spK would be greater than spK

43. Which of the following solutes will produce a molecular solution? A. HCl

B. 3 3Fe S

C. 3HNO

D. 3CH OH

44. Which of the following would best describe the solubility of a solute? A. litres per gram B. moles per litre C. grams per mole D. moles per second 45. Which compound will have the lowest solubility? A. FeS

B. 4CaSO

C. 3AgBrO

D. 3 3Fe NO

46. Which of the following precipitates may form when equal volumes of 0.3 M 3AgNO ,

0.3 M 2SrCl and 0.3 M 2 3Na CO are mixed together?

A. 3SrCO and AgCl

B. 2 3Ag CO and AgCl

C. 3SrCO and 2 3Ag CO

D. 3SrCO , 2 3Ag CO and AgCl

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47. An experiment is conducted to identify an unknown cation that is present in each of four beakers.

Which of the following could be the unknown cation?

A. Ag

B. 3Fe

C. 2Ba

D. 2Be

48. Given the equilibrium reaction…

3 2 3 22NaNO (aq) Ag S(s) 2AgNO (aq) Na S(aq)

Which spK expression best describes the net ionic reaction?

A. 2

2

spK Ag S

B. sp 22

1K

Ag S

C.

22

sp

2

Ag SK

Ag S

D.

2

3 2

sp 2

3

AgNO Na SK

NaNO

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49. Two salt solutions were mixed and a trial spK was calculated to be 92.0x10 . The

spK

value is 101.0x10 . From this information, which of the following is a true statement?

50. A saturated solution of 4SrSO has an 2

4SO of 41.0x10 M . What is the 2Sr

?

A. 33.4x10 M

B. 45.8x10 M

C. 41.0x10 M

D. 73.4x10 M

51. Which of the following would form a saturated solution when 0.010 mol of the solid

solute is added to 100 mL of water?

A. 3BaCO

B. 4FeSO

C. NaCN

D. 3 2Pb NO

52. Which net ionic equation best describes the reaction that exists in a solution prepared

by mixing equal volumes of 0.20 M 3 2Ca NO and 0.20 M 2 3Na CO ?

A. 2 2

3 3Ca (aq) CO (aq) CaCO (s)

B. 3 3Na (aq) NO (aq) NaNO (s)

C. 3 2 3 3 32Ca NO (aq) Na CO (aq) 2NaNO (s) CaCO (s)

D. 3 2 3 3 32Ca NO (aq) Na CO (aq) 2NaNO (aq) CaCO (s)

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53. Which compound will have the greatest solubility in water? A. CuCl

B. 3FeCO

C. 4MgSO

D. 3 4 2Cu PO

54. Which cation below can be used to separate 2

4SO from 2S ions by precipitation?

A. 2Sr

B. 2Pb

C. Cs

D. 2Be

55. What will be the effect of adding some solid 3AgNO to a saturated solution of AgCl ?

A. The 3AgNO will not dissolve

B. More solid AgCl will dissolve

C. More solid AgCl will be produced

D. The 3AgNO will not affect the AgCl equilibrium

56. For a saturated solution, the spK expression does not contain any solid solute term.

What is the reason for this? A. The solid solute is a product B. The solid solute is a reactant C. The solid solute continues to change in amount D. The solid solute does not change in concentration

57. Which of the statements below describes the spK expression for the salt barium

phosphate?

A. 2 3

sp 4K Ba PO

B. 3 2

2 3

sp 4K Ba PO

C. 2 3

sp 4K 3Ba 2PO

D. 2 2

2 3

sp 4K 3Ba 2PO

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58. What is the solubility of 2

Fe OH ?

A. 174.9x10 M

B. 171.2x10 M

C. 63.7x10 M

D. 62.3x10 M

59. Which of the following ions would have the highest concentration in 0.1 M 2

3CO ?

A. 2Ba

B. 2Ca

C. 2Sr

D. 2Mg

60. Which of the solutes below can form an ionic solution with the highest conductivity? A. PbS

B. 3CH Cl

C. 3NaNO

D. 3CH COOH

61. The following data was collected to determine the solubility of a substance…

Mass of solute dissolved 5.00 g Volume of solvent 250.0 mL

Molar mass of solute 100.0 g/mol Molar mass of solvent 20.0 g/mol

Which of the following best describes its solubility?

A. 22.00x10 g/mL

B. 25.00x10 mol

C. 0.250 mol

D. 1.00 mol/L

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62. Which value best represents the total ion concentration when 0.10 moles of 3 4K PO is

present in 0.5 L of solution? A. 0.1 M B. 0.2 M C. 0.4 M D. 0.8 M

63. What will happen when equal volumes of 0.20 M 4 2NH S and 0.20 M

2Sr OH are

mixed? A. SrS precipitates

B. 4

NH OH precipitates

C. Both 4

NH OHand SrS precipitate

D. No precipitate forms 64. Which anion would be most effective in removing the cations responsible for hard

water?

A. 2S

B. Cl

C. 3

4PO

D. 2

4SO

65. Which of the following is the spK expression for barium phosphate?

A. 2 3

sp 4K Ba PO

B. 3 2

2 3

sp 4K Ba PO

C. 2 3

sp 4K 3Ba 2PO

D. 3 2

2 3

sp 4K 3Ba 2PO

66. The solubility of 2

Mg OH is found to be 41.2x10 M . What is its spK ?

A. 126.9x10

B. 121.7x10

C. 81.4x10

D. 41.2x10

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67. Which of the following is true for the salt 2SrF at 25 C?

A. It has a high solubility B. It will not dissolve at all

C. Its solubility is 31.6x10 M

D. Its solubility is 31.0x10 M

68. Which of the following ions could be used in the lowest concentration to remove Ag

ions from a polluted water sample?

A. I

B. Br

C. 3BrO

D. 2

3CO

69. Which of the solutes below is both ionic and most soluble? A. RbOH

B. 3

CH OH

C. 2

Ca OH

D. 3

Fe OH

70. Which of the following is commonly used to describe the solubility of a solute? A. mass of solute moles of solute B. moles of solution mass of solute C. mass of solute volume of solution D. mass of solution volume of solute

71. Given a saturated solution of 2

Ca OH which of the following statements is always

true?

A. The 2Ca is twice that of OH

B. The OH precipitates half as fast as the 2Ca

C. The rate of crystallization equals the rate of dissolving D. The rate of dissolving is greater than the rate of crystallization

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72. Solid NaCl is added to a saturated AgCl solution. How have the Ag and Cl

changed when equilibrium has been re-established?

73. Which of the following expressions represents 3Fe in a saturated

3Fe OH

solution?

A. spK

3 OH

B. sp

3

K

OH

C. sp

3

K

OH

D. 3

spK OH

74. What is the value of spK for 2

Zn OH if the solubility of 2

Zn OH is equal to

64.2x10 M ?

A. 21.0x10

B. 34.0x10

C. 111.8x10

D. 163.0x10

75. What is the maximum number of moles of Cl that can exist in 500.0 mL of 2.0 M

3AgNO ?

A. 114.5x10

B. 119.0x10

C. 101.8x10

D. 91.8x10

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76. What is the concentration of the ions in 3.0 L of 0.50 M 2 4 3Al SO ?

77. Consider the following equilibrium…

2 2

3 3MgCO (s) Mg (aq) CO (aq)

Adding which of the following would cause the solid to dissolve?

A. HCl

B. 2 3K CO

C. 3MgCO

D. 3 2Mg NO

78. Which of the following compounds could be used to prepare a solution with a 2S

greater than 0.1 M? A. ZnS

B. PbS

C. 2

Ag S

D. 2

Rb S

79. Which of the following will not form a precipitate when mixed with an equal volume of

0.2 M 3

AgNO ?

A. 0.2 M NaBr

B. 0.2 M 3

NaIO

C. 0.2 M 3

NaNO

D. 0.2 M 3

NaBrO

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80. How many moles of solute are dissolved in 200.0 mL of a saturated solution of FeS?

A. 191.2x10

B. 196.0x10

C. 101.5x10

D. 107.7x10

81. Consider the following 10.0 mL solutions…

Equal moles of 3AgNO are added to each solution. It is observed that a precipitate forms in

all but one solution. Which solution does not form a precipitate?

A. Cl

B. Br

C. 3IO

D. 3BrO

82. Which of the following could dissolve a precipitate of 2 4CaC O in a saturated solution

of 2 4CaC O ?

A. NaOH

B. 2 4CaC O

C. 2 2 4H C O

D. 3 2Ca NO

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83. Which of the following will dissolve in water to produce a molecular solution?

A. 2CaCl

B. NaOH

C. 3CH OH

D. 2

Sr OH

84. In a solubility equilibrium, the… A. rate of dissolving equals the rate of crystallization B. neither dissolving nor crystallization are occurring C. concentration of solute and solvent are always equal D. mass of dissolved solute is greater than the mass of the solution

85. Which of the following solutions would have 3Fe 0.020M ?

A. 0.40 L of 0.050 M 3 3Fe NO

B. 0.80 L of 0.020 M 4 3Fe SO

C. 0.50 L of 0.040 M 6 5 7FeC H O

D. 0.50 L of 0.010 M 2 2 4 3Fe C O

86. Which of the following substances has the lowest solubility? A. BaS

B. CuS

C. FeS

D. ZnS

87. The complete ionic equation for the reaction between MgS and 2

Sr OH is…

A. 2 2MgS(aq) Sr(OH) (aq) Mg(OH) (s) SrS(s)

B. 2 2MgS(aq) Sr(OH) (aq) Mg(OH) (s) SrS(aq)

C. 2 2 2 2Mg (aq) S (aq) Sr (aq) 2OH Mg (aq) 2OH (aq) SrS(s)

D. 2 2 2 2 2-

2Mg (aq) S (aq) Sr (aq) 2OH Mg OH (s) Sr (aq) S (aq)

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88. Consider the following equilibrium…

2

2Fe OH (s) Fe (aq) 2OH (aq)

Which of the following will cause the equilibrium to shift to the right?

A. adding KOH

B. adding 2Na S

C. adding 2

Fe OH

D. adding 3 2Fe NO

89. Consider the following experiment…

The unknown solution could contain…

A. 0.20 M OH

B. 0.20 M 3NO

C. 0.20 M 3

4PO

D. 0.20 M 2

4SO

90. A compound has a solubility of 57.1x10 M at o25 C . The compound is…

A. CuS

B. AgBr

C. 3CaCO

D. 4CaSO

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91. A saturated solution of NaCl contains 36.5 g of solute in 0.100 L of solution. The

solubility of the compound is… A. 0.062 M B. 1.60 M C. 3.65 M D. 6.24 M

92. Calculate the Li in 200.0 mL of 1.5 M 4LiSO …

A. 0.30 M B. 0.60 M C. 1.5 M D. 3.0 M 93. When equal volumes of 0.20 M RbCl and 0.20 M SrS are combined…

A. no precipitate forms

B. a precipitate of 2Rb S only forms

C. a precipitate of 2SrCl only forms

D. precipitates of both 2Rb S and 2SrCl form

94. A solution contains both Ag and 2Mg ions. During selective precipitation, these ions

are removed one at a time by adding…

A. I followed by OH

B. OH followed by 2S

C. 2

4SO followed by Cl

D. 3NO followed by 3

4PO

95. The spK expression for a saturated solution of 2

Mg OH is…

A.

22

sp

2

Mg OHK

Mg OH

B. 2

2

spK Mg OH

C. 2

spK Mg OH

D. 2

2

spK Mg 2OH

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96. Consider the following saturated solutions: 4CuSO , 4BaSO , 4CaSO . The order of

cation concentration, from highest to lowest, is…

A. 2 2 2Ba Ca Cu

B. 2 2 2Ca Cu Ba

C. 2 2 2Cu Ca Ba

D. 2 2 2Cu Ba Ca

97. When 31.0x10 moles of 2CuCl (s) are added to 1.0 L of 3

31.0x10 M IO , the…

A. Trial spK spK and a precipitate forms

B. Trial spK spK and a precipitate forms

C. Trial spK spK and no precipitate forms

D. Trial spK spK and no precipitate forms

98. Which of the following forms a molecular solution in water?

A. 4SrSO

B. 3 4Na PO

C. 6 12 6C H O

D. 4 3NH CH COO

99. Which of the following is necessary to form a saturated solution at equilibrium? A. excess solute B. an ionic solute C. solute of low solubility

D. trial ion product is less than spK

100. Which of the following will produce a solution with the highest OH ?

A. AgOH

B. 2

Sr OH

C. 3

Fe OH

D. 2

Mg OH

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Written Questions

1. A 30.00 mL sample of a saturated solution of 2 4Ag SO was heated in an evaporating

dish until all the water was evaporated. The following data were recorded...

Calculate the spK value for 2 4Ag SO . (5 marks)

2. Consider the following equilibrium and accompanying graph...

2+ -

3 32Zn IO (s) Zn (aq)+2IO (aq)

A. Identify the stress applied at 1t . (1 mark)

Complete the above graph from 1t to 3t for the -

3IO . (2 marks)

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3. Calculate the solubility of 4SrSO in grams per litre. (3 marks)

4. A 100.0 mL saturated solution of 2FeF contains 0.0787 g of solute. Determine the

2+Fe and the -F

in the solution. (3 marks)

5. Consider the following information and the accompanying diagram. In a titration

experiment, 3AgNO (aq) was used to determine the -Cl in a water sample and the

following data were recorded...

+ -Ag (aq)+Cl (aq) AgCl(s)

3AgNO 0.125 M

Volume of water sample containing -Cl 20.00 mL

Initial buret reading of 3AgNO 5.15 mL

Final buret reading of 3AgNO 37.15 mL

Using the above data, determine the -Cl in the water sample. (3 marks)

6. Calculate the mass of NaI necessary to begin precipitation of +Cu from a 250.0 mL

sample of 0.010 M 3CuNO . (4 marks)

7.

A. Write the net ionic equation for the reaction between 3 2Pb NO and NaCl . (2 marks)

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B. Determine, with calculations, whether a precipitate will form when 15.0 mL of 0.050 M

3 2Pb NO is added to 35.0 mL of 0.085 M NaCl . (4 marks)

8. After a 50.0 mL sample of a saturated solution of 2 4Ag SO was heated to dryness, -47.2x10 g of solid 2 4Ag SO remained. What is the value of spK for 2 4Ag SO ? (5

marks)

9. Calculate the maximum mass of 2BaCl (s) that can be added to 250 mL of 0.50 M

3 2Pb NO (aq) without forming a precipitate of 2PbCl (s) . (6 marks)

10. Sufficient 2 4Na SO is added to 0.10 M 3 2Ba NO to cause a precipitate to form.

A. Write the net ionic equation for the precipitate formation. (1 mark)

B. Calculate the 2-

4SO at the moment the precipitate starts to form. (2 marks)

11. Calculate the mass of solid 3AgNO that can be added to 2.0 L of a 0.10 M 2 4K CrO

solution in order to just start precipitation. (4 marks)

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12.

A. How would a saturated solution be prepared at room temperature? (1 mark)

B. Write a chemical equation to illustrate the equilibrium that exists in a saturated solution of

3 4 2Be PO . (2 marks)

13. Calculate the iodate ion concentration in a saturated copper (II) iodate solution at

25C. (3 marks)

14. A solution is prepared by mixing equal moles of 3 2Ba NO , 2 4K SO , and BaS and

precipitation occurs. Identify the precipitate(s) and write the net ionic equation

Precipitate (1 mark)

Net Ionic Equation (2 marks)

15. What is the maximum 2+Pb that can exist in a saturated solution of 4BaSO without

causing precipitate formation? (4 marks)

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16. Consider the equilibrium for a saturated solution of 3CaCO ...

2+ 2-

3 3CaCO (s) Ca +CO

What is the maximum 2+Mg that can exist in a saturated solution of 3CaCO without causing

a precipitate to form? (4 marks)

17. Consider the equilibrium for a saturated solution of 2PbI (s) ...

2+ -

2PbI (s) Pb (aq)+2I (aq)

What is the maximum +Ag that can exist in a saturated solution of 2PbI (s) without causing

a precipitate to form? (4 marks)

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18. Consider the following equilibrium...

2+ -

2Mg OH (s) Mg (aq)+2OH (aq)

A. What happens to the amount of solid 2

Mg OH (s) when some HCl(aq) is added? (1 mark)

B. On the graph below, sketch the effect of adding HCl(aq) at time 1t . (3 marks)

19. Will a precipitate form when 10.0 mL of 1.0 M 3 2Pb NO is mixed with 40.0 mL of

-22.0x10 M NaCl? Justify your answer. (4 marks)

20. At 25°C, will a precipitate form when 25.0 mL of 0.010 M 3 2Pb NO is combined with

75.0 mL of 0.010 M NaI? Support your answer with calculations. (3 marks)

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21. Write the complete ionic equation for the reaction between 3NaBrO and 3AgNO . (1

mark)

A. Complete Ionic Equation

B. What is the maximum 3NaBrO that can exist in equilibrium with 2.0 M 3AgNO ? (2 marks)

22. Write the balanced complete ionic equation for the reaction that occurs when 0.20 M

of 3 2Ba NO is added to an equal volume of 0.20 M 2 3Na CO . (2 marks)

Complete Ionic Equation

23. Calculate the minimum number of moles of 3 2Pb NO required to start precipitation in

50.0 mL of 0.15 M 2ZnI . (5 marks)

24. In a titration, 25.00 mL of NaCl(aq) reacts completely with 42.20 mL of 0.100 M

3AgNO .

What is the Cl in the original solution? (3 marks)

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25. The following data was obtained when 20.0 mL of a saturated solution of 2PbI was

evaporated to dryness.

Use this information to determine the spK of 2PbI . (4 marks)

26. Calculate the molar solubility of 2SrF . (4 marks)

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Multiple Choice Questions Answer Key

1 B 21 A 41 A 61 A 81 D

2 A 22 D 42 C 62 D 82 A

3 A 23 A 43 D 63 D 83 C

4 B 24 C 44 B 64 C 84 A

5 C 25 D 45 A 65 B 85 D

6 D 26 B 46 D 66 A 86 B

7 C 27 B 47 B 67 D 87 D

8 D 28 A 48 A 68 A 88 B

9 D 29 A 49 B 69 A 89 A

10 C 30 C 50 A 70 C 90 C

11 B 31 A 51 A 71 C 91 D

12 C 32 B 52 A 72 B 92 D

13 B 33 D 53 C 73 B 93 A

14 A 34 C 54 A 74 D 94 A

15 C 35 B 55 C 75 A 95 B

16 D 36 A 56 D 76 B 96 C

17 B 37 C 57 B 77 A 97 D

18 D 38 D 58 D 78 D 98 C

19 B 39 B 59 D 79 C 99 A

20 C 40 A 60 C 80 C 100 B

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Written Questions Answer Key 1.

2.

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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. (03062004)

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13.

14.

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15.

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16.

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17.

18.

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19.

20.

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21.

22.

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23.

24.

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25.

26.