Solutions – Ch14 Test Bank | Full Version – 15e

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Package Title: Hein Test Bank

Course Title: Hein 15e

Chapter Number: 14

Question Type: Multiple Choice

1) Which liquid is miscible with water?

a) carbon tetrachloride

b) ethyl alcohol

c) bromine

d) oil

Difficulty: easy

Learning Objective 1: Define solubility and the factors that affect it.

Section Reference 1: Section: 14.2

2) Which liquid is miscible with hexane?

a) pentane

b) methyl alcohol

c) water

d) acetic acid

Difficulty: easy

Learning Objective 1: Define solubility and the factors that affect it.

Section Reference 1: Section: 14.2

3) The solubility of ammonium chloride at 70. ^°C is 60. g of solute per 100. g of water. Which solution would be saturated at 70. ^°C?

a) 90. g of solute in 180. g of water

b) 90 .g of solute in 200. g of water

c) 30. g of solute in 50. g of water

d) 35 g of solute in 50. g of water

Difficulty: medium

Learning Objective 1: Define solubility and the factors that affect it.

Section Reference 1: Section: 14.2

4) The solubility of ammonium chloride at 70. ^°C is 60. g of solute per 100. g of water. Which solution would be unsaturated at 70. ^° C?

a) 110. g of solute per 200. g of water

b) 120. g of solute per 200. g of water

c) 30. g of solute per 50. g of water

d) 35 g of solute per 50. g of water

Difficulty: medium

Learning Objective 1: Define solubility and the factors that affect it.

Section Reference 1: Section: 14.2

5) At which temperature would CO₂ gas be most soluble?

a) 10. ^°C

b) 20. ^°C

c) 30. ^°C

d) 40. ^°C

Difficulty: easy

Learning Objective 1: Define solubility and the factors that affect it.

Section Reference 1: Section: 14.2

6) Use the figure below to determine the mass of potassium chloride required to prepare a saturated solution in 50.0 mL of water at 40°C.

a) 40 g

b) 20 g

c) 10 g

d) 45 g

Difficulty: medium

Learning Objective 1: Define solubility and the factors that affect it.

Section Reference 1: Section: 14.2

7) At which temperature would KCl solid be most soluble?

a) 10. ^°C

b) 20. ^°C

c) 30. ^°C

d) 40. ^°C

Difficulty: medium

Learning Objective 1: Define solubility and the factors that affect it.

Section Reference 1: Section: 14.2

8) At which temperature would KNO₃ solid be most soluble?

a) 283 K

b) 293 K

c) 303 K

d) 313 K

Difficulty: medium

Learning Objective 1: Define solubility and the factors that affect it.

Section Reference 1: Section: 14.2

9) At which temperature would NH₃ gas be most soluble?

a) 283 K

b) 293 K

c) 303 K

d) 313 K

Difficulty: easy

Learning Objective 1: Define solubility and the factors that affect it.

Section Reference 1: Section: 14.2

10) At which pressure would carbon dioxide gas be most soluble?

a) 600 torr

b) 700 torr

c) 800 torr

d) 900 torr

Difficulty: easy

Learning Objective 1: Define solubility and the factors that affect it.

Section Reference 1: Section: 14.2

11) What kind of solute dissolves best under high pressure conditions?

a) solid

b) liquid

c) gas

d) All of the above

Difficulty: easy

Learning Objective 1: Define solubility and the factors that affect it.

Section Reference 1: Section: 14.2

12) At which pressure would nitrogen gas be most soluble?

a) 1.0 atm

b) 1.5 atm

c) 2.0 atm

d) 2.5 atm

Difficulty: easy

Learning Objective 1: Define solubility and the factors that affect it.

Section Reference 1: Section: 14.2

13) A solution containing 50.0 g of ammonium chloride in 100.0 mL of water at 60°C is

a) saturated.

b) unsaturated.

c) supersaturated.

Difficulty: medium

Learning Objective 1: Define solubility and the factors that affect it.

Section Reference 1: Section: 14.2

14) Which phase of matter can act as a solvent?

a) solid

b) liquid

c) gas

d) all of these choices

Difficulty: easy

Learning Objective 1: List the properties of a true solution.

Section Reference 1: Section: 14.1

15) Which phase of matter can act as a solute?

a) solid

b) liquid

c) gas

d) all of these choices

Difficulty: easy

Learning Objective 1: List the properties of a true solution.

Section Reference 1: Section: 14.1

16) A solution is a

a) homogeneous compound.

b) heterogeneous compound.

c) homogeneous mixture.

d) heterogeneous mixture.

Difficulty: easy

Learning Objective 1: List the properties of a true solution.

Section Reference 1: Section: 14.1

17) As temperature decreases, the solubility of most solids in water

a) increases.

b) decreases.

c) remains the same.

Difficulty: easy

Learning Objective 1: Define solubility and the factors that affect it.

Section Reference 1: Section: 14.2

18) As temperature decreases, the solubility of a gas in water

a) increases.

b) decreases.

c) remains the same.

Difficulty: easy

Learning Objective 1: Define solubility and the factors that affect it.

Section Reference 1: Section: 14.2

19) O₂ gas is most soluble at

a) top of a lake.

b) bottom of a lake.

c) all levels since solubility is unaffected by the depth level.

Difficulty: medium

Learning Objective 1: Define solubility and the factors that affect it.

Section Reference 1: Section 14.2

20) Which of the following is correct?

a) Concentration of a solid in a solution is directly proportional to its pressure.

b) Concentration of a gas in a solution is directly proportional to its temperature.

c) Concentration of a solid in a solution is directly proportional to its temperature.

d) Concentration of a gas in a solution is directly proportional to its pressure.

Difficulty: easy

Learning Objective 1: Define solubility and the factors that affect it.

Section Reference 1: Section 14.2

21) In a ___ solution, the dissolved solute is in equilibrium with the undissolved solute.

a) saturated

b) unsaturated

c) supersaturated

Difficulty: easy

Learning Objective 1: Define solubility and the factors that affect it.

Section Reference 1: Section 14.2

22) As solute particle size increases, the rate of dissolving

a) increases.

b) decreases.

c) remains the same.

Difficulty: easy

Learning Objective 1: Describe the factors that affect the rate at which a solid dissolves.

Section Reference 1: Section: 14.3

23) As solute surface area increases, the rate of dissolving

a) increases.

b) decreases.

c) remains the same.

Difficulty: easy

Learning Objective 1: Describe the factors that affect the rate at which a solid dissolves.

Section Reference 1: Section: 14.3

24) Which of the following solutions will have the lowest freezing point?

a) 2.5 g of KCl in 100 g of water

b) 2.5 g of NH₄Cl in 100 g of water

c) 2.5 g of NaOH in 100 g of water

d) All the solutions will have the same freezing point.

Difficulty: medium

Learning Objective 1: Use the concept of colligative properties to calculate molality, freezing point, boiling point, freezing point depression, and boiling point elevation of various solutions.

Section Reference 1: Section: 14.5

25) For which of the following solutes would dissolving 40 g in 100 g of water result in an unsaturated solution at 30°C?

a) KNO₃

b) NH₄Cl

c) KCl

d) KClO₃

Difficulty: hard

Learning Objective 1: Define solubility and the factors that affect it.

Section Reference 1: Section: 14.2

26) The freezing point of pure water is 273 K. As a solute dissolves in water, the freezing point of the solution will

a) increase.

b) decrease.

c) remains the same.

Difficulty: easy

Learning Objective 1: Use the concept of colligative properties to calculate molality, freezing point, boiling point, freezing point depression, and boiling point elevation of various solutions.

Section Reference 1: Section: 14.5

27) The normal boiling point of pure water is 373 K. As a solute dissolves in water, the boiling point of the solution will

a) increase.

b) decrease.

c) remains the same.

Difficulty: easy

Learning Objective 1: Use the concept of colligative properties to calculate molality, freezing point, boiling point, freezing point depression, and boiling point elevation of various solutions.

Section Reference 1: Section: 14.5

28) Which of the following solutions will have the highest boiling point?

a) 1.0 g of NaCl in 100 g of water

b) 1.0 g of KNO₃ in 100 g of water

c) 1.0 g of NaC₂H₃O₂ in 100 g of water

d) All the solutions will have the same boiling point.

Difficulty: hard

Learning Objective 1: Use the concept of colligative properties to calculate molality, freezing point, boiling point, freezing point depression, and boiling point elevation of various solutions.

Section Reference 1: Section: 14.5

29) Which of the following aqueous solutions will have the lowest boiling point?

a) 1.0 g of NaCl in 100 g of water

b) 1.0 g of KNO₃ in 100 g of water

c) 1.0 g of NaC₂H₃O₂ in 100 g of water

d) All the solutions will have the same boiling point.

Difficulty: medium

Learning Objective 1: Use the concept of colligative properties to calculate molality, freezing point, boiling point, freezing point depression, and boiling point elevation of various solutions.

Section Reference 1: Section: 14.5

30) The addition of a crystal of sodium chlorate to a sodium chlorate solution causes additional crystals of sodium chlorate to precipitate. The original solution was

a) saturated.

b) supersaturated.

c) unsaturated.

Difficulty: easy

Learning Objective 1: Define solubility and the factors that affect it.

Section Reference 1: Section: 14.2

31) Which anion will not precipitate silver ion?

a) chloride

b) nitrate

c) bromide

d) carbonate

Difficulty: easy

Learning Objective 1: Define solubility and the factors that affect it.

Section Reference 1: Section: 14.2

32) One liter of 2.0 M KCl solution and two liters of 1.0 M KCl solution have the same

a) density.

b) concentration.

c) volume.

d) number of moles of solute.

Difficulty: easy

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4

33) Which of the following substances would be the most soluble in water?

a) AgCl

b) NaCl

c) PbCl₂

d) Hg₂Cl₂

Difficulty: easy

Learning Objective 1: Define solubility and the factors that affect it.

Section Reference 1: 14.2

34) Which of the following would most likely increase the solubility of a solid in water?

a) stirring

b) increase the surface area of the solid

c) increase the pressure

d) increase the temperature

Difficulty: easy

Learning Objective 1: Define solubility and the factors that affect it.

Section Reference 1: Section: 14.2

35) Which of the following salts is most soluble in water?

a) chromium(III) nitrate

b) calcium carbonate

c) silver iodide

d) barium phosphate

Difficulty: medium

Learning Objective 1: Define solubility and the factors that affect it.

Section Reference 1: Section: 14.2

36) Which of the following salts is least soluble in water?

a) Sodium chloride

b) Iron(II) sulfide

c) Copper(II) bromide

d) Ammonium sulfide

Difficulty: medium

Learning Objective 1: Define solubility and the factors that affect it.

Section Reference 1: Section: 14.2

37) Liquids which are capable of mixing and forming a solution are

a) unsaturated.

b) dilute.

c) miscible.

d) immiscible.

Difficulty: easy

Learning Objective 1: Define solubility and the factors that affect it.

Section Reference 1: Section: 14.2

38) Which of the following solution would have the highest freezing point?

a) 0.01 m CH₃OH

b) 0.005 m CH₃OH

c) 0.05 m CH₃OH

d) 0.001 m CH₃OH

Difficulty: medium

Learning Objective 1: Use the concept of colligative properties to calculate molality, freezing point, boiling point, freezing point depression, and boiling point elevation of various solutions.

Section Reference 1: Section: 14.5

39) Which of the following molar solution would have the highest boiling point?

a) 0.01 m CH₃OH

b) 0.001 m CH₃OH

c) 0.005 m CH₃OH

d) 0.05 m CH₃OH

Difficulty: easy

Learning Objective 1: Use the concept of colligative properties to calculate molality, freezing point, boiling point, freezing point depression, and boiling point elevation of various solutions.

Section Reference 1: Section: 14.5

40) What is the percent by mass of the solution formed when 5.0 g of solute is dissolved in 40. g of water?

a) 8.0 %

b) 11 %

c) 13 %

d) 14 %

Difficulty: easy

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4

41) What is the percent by mass of a solution formed by dissolving 50.0 g of glucose in 1000. g of water?

a) 4.76 %

b) 5.00 %

c) 5.26 %

d) 50.0 %

Difficulty: medium

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4

42) What masses of KBr and water are needed to produce 300. g of a solution that is 3.00 % by mass?

a) 9.00 g of KBr and 300. g of water

b) 9.00 g of KBr and 291 g of water

c) 300. g of KBr and 9.00 g of water

d) 291 g of KBr and 9.00 g of water

Difficulty: medium

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4

43) What mass of NaOH is needed to produce 400. g of a solution that is 12.0 % by mass?

a) 4.80 g

b) 48.0 g

c) 352 g

d) 4800 g

Difficulty: medium

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4

44) How many parts per million of solute is present in a solution that is 0.300 % by mass?

a) 0.300 ppm

b) 30.0 ppm

c) 300. ppm

d) 3.00 × 10³ ppm

Difficulty: easy

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4

45) A solution is prepared by dissolving 0.400 g of solute in 1000. g of water. How many parts per million of solute are in this solution?

a) 0.400 ppm

b) 4.00 ppm

c) 400. ppm

d) 4.00 × 10³ ppm

Difficulty: easy

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4

46) A sample of a 20.0 % solution of KCl in water has a mass of 400. g. What mass of KCl is contained in this solution?

a) 20.0 g

b) 80.0 g

c) 320. g

d) 400. g

Difficulty: easy

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4

47) What mass of glucose is dissolved in 1000. g of a solution that is 5.00 % by mass?

a) 5.00 g

b) 50.0 g

c) 5.00 g

d) 5.0010³ g

Difficulty: easy

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4

48) How many mL of a 4.50 (m/v)% solution would contain 23.0 g of solute?

a) 19.6 mL

b) 511 mL

c) 1.04 × 10³ mL

d) 10.35 mL

Difficulty: easy

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4

49) What mass of KCl is dissolved in 250. mL of a solution that is 4.00 % by mass/volume?

a) 4.00 g

b) 10.0 g

c) 40.0 g

d) 100. g

Difficulty: easy

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4

50) A solution is prepared by mixing 50.0 mL of ethanol with 300.0 mL of water. What is the volume percent of ethanol in this solution? Assume volumes are additive.

a) 14.3 %

b) 16.7 %

c) 25.0 %

d) 50.0 %

Difficulty: medium

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4

51) A solution is prepared by mixing 20.0 mL of methanol with enough water to produce 400.0 mL of solution. What is the volume percent of methanol in this solution?

a) 0.500 %

b) 4.76 %

c) 5.00 %

d) 5.26 %

Difficulty: easy

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4

52) What is the molality of a solution prepared by dissolving 40.0 g of glucose (C₆H₁₂O₆) in 4.00 kg of water?

a) 0.0555 m

b) 10.0 m

c) 0.0100 m

d) 0.222 m

Difficulty: easy

Learning Objective 1: Use the concept of colligative properties to calculate molality, freezing point, boiling point, freezing point depression, and boiling point elevation of various solutions.

Section Reference 1: Section: 14.5

53) What is the molality of a solution in which 0.300 moles of solute is dissolved in 1500. g of solvent?

a) 0.000200 m

b) 0.00200 m

c) 0.0200 m

d) 0.200 m

Difficulty: easy

Learning Objective 1: Use the concept of colligative properties to calculate molality, freezing point, boiling point, freezing point depression, and boiling point elevation of various solutions.

Section Reference 1: Section: 14.5

54) How many moles of solute are dissolved in 400. mL of a 0.200 M solution?

a) 0.0800 mol

b) 0.800 mol

c) 8.00 mol

d) 80.0 mol

Difficulty: easy

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4

55) Molarity is expressed as

1. g/L
2. moles/L
3. L/moles
4. Moles/1kg

Difficulty: easy

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4

56) The molarity of 10% (mass/volume) acetic acid (CH₃COOH, density =1.05 g/mL) is

1. 1M
2. 10 M
3. 2M
4. 0.83 M

Difficulty: easy

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4

57) The mass of H₂SO₄ (molar mass 98 g/mol) in 400. mL of 0.100 M solution is

1. 2.45 g
2. 3.92 g
3. 4.90 g
4. 9.80 g

Difficulty: easy

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4

58) The molarity of pure water is _________. (Hint: Density of water is 1.00 g/mL)

1. 55.6 M
2. 50.0 M
3. 100. M
4. 18.0 M

Difficulty: easy

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4

59) 9.8 g of H₂SO₄ is present in 2.0 L of a solution. The molarity of the solution is

1. 0.10 M
2. 0.050 M
3. 0.20 M
4. 0.010 M

Difficulty: easy

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4

60) What is the molarity of the resulting solution when 300. mL of a 0.400 M solution is diluted to 800. mL?

a) 0.109 M

b) 0.150 M

c) 1.07 M

d) 1.47 M

Difficulty: easy

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4

61) What is the molarity of the resulting solution when 400. mL of a 0.400 M solution is diluted to 800. mL?

a) 1.20 M

b) 0.800 M

c) 0.200 M

d) 0.133 M

Difficulty: easy

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4

62) If 250. mL of 0.250 M NaCl solution is diluted with water to a volume of 500. mL, the new concentration of the solution is__________.

a) 0.167 M

b) 0.125 M

c) 0.0833 M

d) 0.0167 M

Difficulty: easy

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4

63) What is the molarity of the resulting solution when 300. mL of a 0.600 M aqueous solution is diluted by the addition of 400. mL of water? Assume volumes are additive.

a) 0.257 M

b) 0.450 M

c) 0.800 M

d) 1.40 M

Difficulty: medium

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4

64) Concentrated laboratory ammonia, NH₃, is 14.8 M and density of 0.898 g/mL. What is the molality of the solution of ammonia? (Hint: Assume 1.00 L of the solution.)

a) 14.8 m

b) 22.8 m

c) 5.76 m

d) 1.45 m

Difficulty: hard

Learning Objective 1: Use the concept of colligative properties to calculate molality, freezing point, boiling point, freezing point depression, and boiling point elevation of various solutions.

Section Reference 1: 14.5

65) What is the molarity of a solution in which 1.20 mol of solute is dissolved in 3.00 L of solution?

a) 0.400 M

b) 15.0 M

c) 3.60 M

d) 360. M

Difficulty: easy

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4

66) What is the molarity of a solution in which 4.00 mol of potassium chloride is dissolved in 3.00 L of solution?

a) 1.33 M

b) 6.00 M

c) 2.67 M

d) 4.00 M

Difficulty: easy

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4

67) What is the molarity of a solution in which 0.300 mol of glucose is dissolved in 500. mL of solution?

a) 1.67 M

b) 0.600 M

c) 0.0006 M

d) 150. M

Difficulty: easy

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4

68) What is the molarity of a solution in which 0.800 mol of sodium hydroxide is dissolved in 1500. mL of solution?

a) 0.0533 M

b) 53.3 M

c) 5.33 M

d) 0.533 M

Difficulty: easy

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4

69) What is the molarity of a solution in which 55.49 g of calcium chloride is dissolved in enough water to make 500. mL of solution?

a) 0.500 M

b) 1.00 M

c) 2.00 M

d) 4.00 M

Difficulty: medium

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4

70) What is the molarity of a solution in which 7.1 g of sodium sulfate is dissolved in enough water to make 100. mL of solution?

a) 2.0 M

b) 1.0 M

c) 0.50 M

d) 0.050 M

Difficulty: medium

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4

71) What is the molarity of a solution which contains 85.00 g of sodium nitrate dissolved in 2.00 L of an aqueous solution?

a) 0.500 M

b) 1.00 M

c) 2.00 M

d) 4.00 M

Difficulty: medium

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4

72) What is the molarity of a solution which contains 9.12 g of hydrogen chloride in 200. mL of solution?

a) 0.250 M

b) 0.500 M

c) 1.00 M

d) 1.25 M

Difficulty: medium

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4

73) How many moles of solute are present in 300. mL of a 0.240 M solution?

a) 0.0720 mol

b) 0.240 mol

c) 0.800 mol

d) 1.25 mol

Difficulty: easy

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4

74) How many total moles of ions are present when KCl is dissolved in 1.20 L of a 0.400 M KCl solution?

a) 0.333 mol

b) 0.400 mol

c) 0.480 mol

d) 0.960 moles

Difficulty: medium

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4

75) How many moles of KF are dissolved in 1400. mL of a 3.00 M KF aqueous solution?

a) 0.467 mol

b) 2.14 mol

c) 3.00 mol

d) 4.20

Difficulty: easy

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4

76) What mass of silver nitrate is dissolved in 40.0 mL of a 0.400 M aqueous solution of silver nitrate?

a) 0.272 g

b) 2.72 g

c) 27.2 g

d) 272 g

Difficulty: medium

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4

77) What mass of calcium chloride is dissolved in 100. mL of a 1.20 M solution of calcium chloride in water?

a) 0.120 g

b) 1.20 g

c) 13.3 g

d) 133 g

Difficulty: medium

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4

78) What mass of sodium hydroxide is dissolved in 250. mL of a 0.1 M solution of sodium hydroxide in water?

a) 4.0 g

b) 1.0 g

c) 2.0 g

d) 10. g

Difficulty: medium

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4

79) What mass of magnesium sulfate is dissolved in 400. mL of a 0.800 M solution of magnesium sulfate in water?

a) 0.320 g

b) 2.00 g

c) 38.5 g

d) 241 g

Difficulty: medium

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4

80) When table salt is dissolved in water

1. melting point of the solution increases
2. boiling point of the solution increases
3. boiling point of the solution decreases
4. both melting and boiling points decreases

Difficulty: easy

Learning Objective 1: Use the concept of colligative properties to calculate molality, freezing point, boiling point, freezing point depression, and boiling point elevation of various solutions.

Section Reference 1: Section: 14.5

81) The freezing point depression constant for water is 1.86°C kg solvent/mol solute. If 342 g of cane sugar (C₁₂H₂₂O₁₁) is dissolved in 1.00 kg of water, the solution will freeze at ________.

1. -1.86 °C
2. 1.86 °C
3. -3.92 °C
4. 2.42 °C

Difficulty: easy

Learning Objective 1: Use the concept of colligative properties to calculate molality, freezing point, boiling point, freezing point depression, and boiling point elevation of various solutions.

Section Reference 1: Section: 14.5

82) The freezing point depression constant for water is 1.86°C kg solvent/mol solute. The freezing point of a 0.05 molal solution of a non-electrolyte in water is _________.

1. -1.86 °C
2. -0.93 °C
3. -0.093 °C
4. 0.93 °C

Difficulty: easy

Learning Objective 1: Use the concept of colligative properties to calculate molality, freezing point, boiling point, freezing point depression, and boiling point elevation of various solutions.

Section Reference 1: Section: 14.5

83) The elevation of boiling point of a solution is

1. directly proportional to molal concentration
2. inversely proportional to molal concentration
3. directly proportional to the molarity of the solution
4. inversely proportional to the molarity of the solution

Difficulty: easy

Learning Objective 1: Use the concept of colligative properties to calculate molality, freezing point, boiling point, freezing point depression, and boiling point elevation of various solutions.

Section Reference 1: Section: 14.5

84) What is the freezing point of a 1.40 m aqueous solution of a nonvolatile un-ionized solute? (The freezing point depression constant for water is 1.86°C kg solvent/mol solute.)

a) -2.60°C

b) 0.00°C

c) 2.60°C

d) 102.60°C

Difficulty: easy

Learning Objective 1: Use the concept of colligative properties to calculate molality, freezing point, boiling point, freezing point depression, and boiling point elevation of various solutions.

Section Reference 1: Section: 14.5

85) What is the freezing point of a 0.400 m aqueous solution of a nonvolatile un-ionized solute? (The freezing point depression constant for water is 1.86°C kg solvent/mol solute.)

a) 0.744^°C

b) 0.00^°C

c) -7.44^°C

d) -0.744^°C

Difficulty: easy

Learning Objective 1: Use the concept of colligative properties to calculate molality, freezing point, boiling point, freezing point depression, and boiling point elevation of various solutions.

Section Reference 1: Section: 14.5

86) What is the freezing point of a 3.00 m aqueous solution of a nonvolatile un-ionized solute? (The freezing point depression for water is 1.86°C kg solvent/mol solute.)

a) 3.00 ^oC

b) –5.58 ^oC

c) 3.00^oC

d) 5.58 ^oC

Difficulty: medium

Learning Objective 1: Use the concept of colligative properties to calculate molality, freezing point, boiling point, freezing point depression, and boiling point elevation of various solutions.

Section Reference 1: Section: 14.5

87) What is the boiling point of a 4.00 m aqueous solution of a nonvolatile un-ionized solute? (The boiling point elevation constant for water is 0.512°C kg solvent/mol solute.)

a) 100.^°C

b) 102^°C

c) 98.0^°C

d) 2.05^°C

Difficulty: easy

Learning Objective 1: Use the concept of colligative properties to calculate molality, freezing point, boiling point, freezing point depression, and boiling point elevation of various solutions.

Section Reference 1: Section: 14.5

88) What is the boiling point of a 3.40 m aqueous solution of a nonvolatile un-ionized solute? (The boiling point elevation constant for water is 0.512°C kg solvent/mol solute.)

a) 1.74^°C

b) 98.3^°C

c) 100.^°C

d) 102^°C

Difficulty: easy

Learning Objective 1: Use the concept of colligative properties to calculate molality, freezing point, boiling point, freezing point depression, and boiling point elevation of various solutions.

Section Reference 1: Section: 14.5

89) What is the boiling point of a 6.00 m aqueous solution of a nonvolatile un-ionized solute? (The boiling point elevation constant for water is 0.512°C kg solvent/mol solute.)

a) 100.^°C

b) 103.^°C

c) 3.07^°C

d) 96.9^°C

Difficulty: easy

Learning Objective 1: Use the concept of colligative properties to calculate molality, freezing point, boiling point, freezing point depression, and boiling point elevation of various solutions.

Section Reference 1: Section: 14.5

90) When compared to pure water, aqueous solutions always have

a) higher boiling point and higher freezing point.

b) lower boiling point and lower freezing point.

c) higher boiling point and lower freezing point.

d) lower boiling point and higher freezing point.

Difficulty: easy

Learning Objective 1: Use the concept of colligative properties to calculate molality, freezing point, boiling point, freezing point depression, and boiling point elevation of various solutions.

Section Reference 1: Section: 14.5

91) When salt is dissolved in water

a) melting point of the solution increases.

b) boiling point of the solution increases.

c) boiling point of the solution decreases.

d) both melting and boiling points increases.

Difficulty: easy

Learning Objective 1: Use the concept of colligative properties to calculate molality, freezing point, boiling point, freezing point depression, and boiling point elevation of various solutions.

Section Reference 1: Section: 14.5

92) What mass of water must be added to 30.5 g of KNO₃ to prepare a 45.0% by mass solution?

a) 13.7 g

b) 44.2 g

c) 37.3 g

d) 67.8 g

Difficulty: medium

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4

93) How would you prepare 150.0 mL of a 0.200 M aqueous solution of potassium chloride from a 0.500 M aqueous solution of potassium chloride?

a) Add 60.0 mL of water to the 0.500 M solution.

b) Take 60.0 mL of the 0.500 M solution and add enough water for a total volume of 150.0 mL of solution.

c) Add 90.0 mL of water to the 0.500 M solution.

d) Take 90.0 mL of the 0.500 M solution and add enough water for a total volume of 150.0 mL of solution.

Difficulty: medium

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4

94) How many liters of Cl₂ gas at a pressure of 0.950 atm and a temperature of 298 K will be collected from the reaction of 25.0 mL of a 0.100 M aqueous solution of KMnO₄ and an excess of HCl?

2 KMnO₄(aq) + 16 HCl(aq) 2 MnCl₂(aq) + 5 Cl₂(g) + 8 H₂O(l) + 2 KCl(aq)

a) 0.321 L

b) 0.0644 L

c) 0.145 L

d) 0.161 L

Difficulty: hard

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4

95) How many grams of Zn(s) will react completely with 100.0 mL of 0.0525 M HCl according to the following equation?

Zn(s) + 2 HCl(aq) ZnCl₂(aq) + H₂(g)

a) 0.172 g

b) 5.25 g

c) 0.343 g

d) 0.687 g

Difficulty: hard

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4

96) In order to decrease the freezing point of 500. g of water to 1.00°C, how many grams of ethylene glycol (C₂H₆O₂) must be added? (K_f = 1.86 °C kg solvent/mol solute.)

a) 5.37 g

b) 1.08 g

c) 16.7 g

d) 66.7 g

Difficulty: medium

Learning Objective 1: Use the concept of colligative properties to calculate molality, freezing point, boiling point, freezing point depression, and boiling point elevation of various solutions.

Section Reference 1: Section: 14.5

Question Type: True/False

97) Salt water has a higher freezing point than pure water.

Difficulty: easy

Learning Objective 1: Use the concept of colligative properties to calculate molality, freezing point, boiling point, freezing point depression, and boiling point elevation of various solutions.

Section Reference 1: Section: 14.5

98) Salt water has a higher boiling point than pure water.

Difficulty: easy

Learning Objective 1: Use the concept of colligative properties to calculate molality, freezing point, boiling point, freezing point depression, and boiling point elevation of various solutions.

Section Reference 1: Section: 14.5

99) As more solute is added to a saturated solution, the concentration of the solution increases.

Difficulty: easy

Learning Objective 1: Define solubility and the factors that affect it.

Section Reference 1: Section: 14.2

100) Freezing point depression, boiling point elevation, and osmotic pressure are all colligative properties.

Difficulty: easy

Learning Objective 1: Use the concept of colligative properties to calculate molality, freezing point, boiling point, freezing point depression, and boiling point elevation of various solutions.

Learning Objective 2: Discuss osmosis and osmotic pressure and their importance in living systems.

Section Reference 1: Section: 14.5 and 14.6

101) When a solution is diluted by adding more solvent, the number of moles of solute remains constant.

Difficulty: easy

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4

102) A solution has a lower vapor pressure than the pure solvent, therefore, it will have a lower boiling point.

Difficulty: easy

Learning Objective 1: Use the concept of colligative properties to calculate molality, freezing point, boiling point, freezing point depression, and boiling point elevation of various solutions.

Section Reference 1: Section: 14.5

103) The solvent is the most abundant component of a solution.

Difficulty: easy

Learning Objective 1: List the properties of a true solution.

Section Reference 1: Section: 14.1

104) A solution made by dissolving 20. g of NaCl in 100.0 mL of water has the same % by mass as a solution made by dissolving 10.0 g of NaCl in 50.0 mL of water.

Difficulty: medium

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4

105) Polar molecules tend to be insoluble in water.

Difficulty: easy

Learning Objective 1: Define solubility and the factors that affect it.

Section Reference 1: Section: 14.2

106) As particle size increases, surface area increases, and the rate of dissolving increases.

Difficulty: easy

Learning Objective 1: Define solubility and the factors that affect it.

Section Reference 1: Section: 14.2

107) Ammonium chloride is the most soluble salt at 20°C. Refer to the following figure.

Difficulty: easy

Learning Objective 1: Define solubility and the factors that affect it.

Section Reference 1: Section: 14.2

Question Type: Essay

108) A cup of coffee has a volume of 250. mL, a mass of 250. g, and contains 125 mg of caffeine, C₈H₁₀N₄O₂.

a) What is the molarity of the caffeine in the coffee?
b) What is the mass percent of the caffeine in the coffee?

Difficulty: medium

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4

109) A solution of 5.36 g of a molecular compound dissolved in 76.8 g of benzene has a boiling point of 81.48^° C. The boiling point of pure benzene is 80.10^° C and the boiling point elevation constant for benzene is 2.53°C kg solvent/mol solute. What is the molar mass of the solute?

Difficulty: hard

Learning Objective 1: Use the concept of colligative properties to calculate molality, freezing point, boiling point, freezing point depression, and boiling point elevation of various solutions.

Section Reference 1: Section: 14.5

110) Ethylene glycol is used as an antifreezing agent. Calculate the amount of ethylene glycol to be added to 4 kg of water to prevent it from freezing at –6.0^° C? (The freezing point depression constant for water is 1.86°C kg solvent/mol solute.)

Difficulty: medium

Learning Objective 1: Use the concept of colligative properties to calculate molality, freezing point, boiling point, freezing point depression, and boiling point elevation of various solutions.

Section Reference 1: Section: 14.5

111) Explain why the solubility of gases decreases with increasing temperature.

Difficulty: easy

Learning Objective 1: Define solubility and the factors that affect it.

Section Reference 1: Section: 14.2

112) What mass of ethanol, C₂H₅OH, is required to decrease the freezing point of 2.000 L of water to –10.00^° C? (The freezing point depression constant for water is 1.86°C kg solvent/mol solute.)

Difficulty: medium

Learning Objective 1: Use the concept of colligative properties to calculate molality, freezing point, boiling point, freezing point depression, and boiling point elevation of various solutions.

Section Reference 1: Section: 14.5

113) A solution made by dissolving 0.3200 g of a non electrolyte in 25.00 g of water has a freezing point of –0.021^° C. Calculate the molar mass of the non electrolyte. (The freezing point depression constant for water is 1.86°C kg solvent/mol solute.)

Difficulty: medium

Learning Objective 1: Use the concept of colligative properties to calculate molality, freezing point, boiling point, freezing point depression, and boiling point elevation of various solutions.

Section Reference 1: Section: 14.5

114) Calculate the volume (in mL) of a 0.300 M aqueous NaOH solution required to react completely with 32.5 mL of a 0.200 M aqueous solution of H₂SO₄.

H₂SO₄(aq) + 2 NaOH(aq) Na₂SO₄(aq) + 2 H₂O(l)

Difficulty: medium

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4

115) An ethylene glycol, C₂H₄(OH)₂, solution contains 500. g of ethylene glycol dissolved in 600. g of water. (The boiling point elevation constant for water is 0.512°C kg solvent/mol solute.)

a) What is the molality of the solution?
b) What is the boiling point of the solution?

Difficulty: medium

Learning Objective 1: Use the concept of colligative properties to calculate molality, freezing point, boiling point, freezing point depression, and boiling point elevation of various solutions.

Section Reference 1: Section: 14.5

116) What mass of ethylene glycol, C₂H₄(OH)₂, is required to raise the boiling point of 1.400 kg of water to 103.50^°C? (The boiling point elevation constant for water is 0.512°C kg solvent/mol solute.)

Difficulty: medium

Learning Objective 1: Use the concept of colligative properties to calculate molality, freezing point, boiling point, freezing point depression, and boiling point elevation of various solutions.

Section Reference 1: Section: 14.5

117) Calculate the boiling point of solution made by dissolving 6.000 g of urea (N2H4CO) in 200.0 g of water. (The boiling point elevation constant for water is 0.512°C kg solvent/mol solute.)

Difficulty: medium

Learning Objective 1: Use the concept of colligative properties to calculate molality, freezing point, boiling point, freezing point depression, and boiling point elevation of various solutions.

Section Reference 1: Section: 14.5

118) A sample of a compound with a mass of 90.10 g is dissolved in 250.0 g of water. The freezing point of the resulting solution is –3.72^° C. The freezing point depression constant for water is 1.86°C kg solvent/mol solute. Upon analysis the compound is found to consist of 39.99 % carbon, 6.727 % hydrogen, and 53.28 % oxygen. What is the molecular formula of this compound?

Difficulty: hard

Learning Objective 1: Use the concept of colligative properties to calculate molality, freezing point, boiling point, freezing point depression, and boiling point elevation of various solutions.

Section Reference 1: Section: 14.5

119) A sulfuric acid solution that is 34.0 % by mass has a density of 1.25 g/mL. What is the molarity of the solution?

Difficulty: hard

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4

120) Calculate the mass of the precipitate formed when 250. mL of a 0.100 M aqueous solution of silver nitrate reacts with 200. mL of a 0.150 M aqueous solution of sodium chloride.

AgNO₃(aq) + NaCl(aq) AgCl(s) + NaNO₃(aq)

Difficulty: hard

Learning Objective 1: Solve problems involving mass percent, volume percent, molarity, and dilution.

Section Reference 1: Section: 14.4