Ch13_Testbank

13.1 Multiple Choice and Bimodal Questions

1) The process of solute particles being surrounded by solvent particles is known as __________.

A) salutation

B) agglomeration

C) solvation

D) agglutination

E) dehydration

Answer: C

Diff: 1

Page Ref: Sec. 13.1

2) Pairs of liquids that will mix in all proportions are called __________ liquids.

A) miscible

B) unsaturated

C) polar liquids

D) saturated

E) supersaturated

Answer: A

Diff: 1

Page Ref: Sec. 13.3

3) The solubility of oxygen gas in water at 25 °C and 1.0 atm pressure of oxygen is

0.041 g/L. The solubility of oxygen in water at 3.0 atm and 25 °C is __________ g/L.

A) 0.041

B) 0.014

C) 0.31

D) 0.12

E) 3.0

Answer: D

Diff: 2

Page Ref: Sec. 13.3

4) The solubility of nitrogen gas in water at 25 °C and a nitrogen pressure of 1.0 atm

is6.9?10-4 M. The solubility of nitrogen in water at a nitrogen pressure of 0.80 atm is

__________ M.

A) 5.5?10-4

B) 8.6?10-4

C) 1.2?103

D) 3.7?10-3

E) 0.80

Answer: A

Diff: 2

Page Ref: Sec. 13.3

5) The solubility of Ar in water at 25 °C is 1.6?10-3 M when the pressure of the Ar above the solution is 1.0 atm. The solubility of Ar at a pressure of 2.5 atm is __________ M.

A) 1.6?103

B) 6.4?10-4

C) 4.0?10-3

D) 7.5?10-2

E) 1.6?10-3

Answer: C

Diff: 2

Page Ref: Sec. 13.3

6) On a clear day at sea level, with a temperature of 25 °C, the partial pressure of N

in air

2

is 0.78 atm and the concentration of nitrogen in water is5.3?10-4 M. When the partial is __________ atm, the concentration in water is1.1?10-3 M.

pressure of N

2

A) 0.63 atm

B) 0.78 atm

C) 1.0 atm

D) 2.1 atm

E) 1.6 atm

Answer: E

Diff: 2

Page Ref: Sec. 13.3

7) Which one of the following vitamins is water soluble?

A) A

B) B

C) K

D) D

E) E

Answer: B

Diff: 3

Page Ref: Sec. 13.3

8) A sample of potassium nitrate (49.0 g) is dissolved in 101 g of water at 100 °C, with precautions taken to avoid evaporation of any water. The solution is cooled to 30.0 °C and no precipitate is observed. This solution is __________.

A) hydrated

B) placated

C) saturated

D) unsaturated

E) supersaturated

Answer: E

Diff: 2

Page Ref: Sec. 13.3

9) A sample of potassium chlorate (15.0 g) is dissolved in 201 g of water at 70 °C with precautions taken to avoid evaporation of any water. The solution is cooled to 30.0 °C and no precipitate is observed. This solution is __________.

A) hydrated

B) miscible

C) saturated

D) unsaturated

E) supersaturated

Answer: D

Diff: 2

Page Ref: Sec. 13.3

10) A sample of potassium nitrate (49.0 g) is dissolved in 101 g of water at 100 °C with precautions taken to avoid evaporation of any water. The solution is cooled to 30.0 °C and a small amount of precipitate is observed. This solution is __________.

A) hydrated

B) placated

C) saturated

D) unsaturated

E) supersaturated

Answer: C

Diff: 2

Page Ref: Sec. 13.3

monohydrate in water at 20 °C is 70.0 g per 100.0 mL of 11) The solubility of MnSO

4

water. A solution at 20 °C that is 4.22 M in MnSO

monohydrate is best described as a(n)

4

monohydrate is 168.97 g/mol.

__________ solution. The formula weight of MnSO

4

A) hydrated

B) solvated

C) saturated

D) unsaturated

E) supersaturated

Answer: E

Diff: 3

Page Ref: Sec. 13.3

in 375 g of water. The density of 12) A solution is prepared by dissolving 23.7 g of CaCl

2

is __________% by mass. the resulting solution is 1.05 g/mL. The concentration of CaCl

2

A) 5.94

B) 6.32

C) 0.0632

D) 0.0594

E) 6.24

Answer: A

Diff: 3

Page Ref: Sec. 13.4

13) The concentration of urea in a solution prepared by dissolving 16 g of urea in 39 g of

O is __________% by mass. The molar mass of urea is 60.0 g/mol.

H

2

A) 29

B) 41

C) 0.29

D) 0.41

E) 0.48

Answer: A

Diff: 3

Page Ref: Sec. 13.4

14) The concentration of nitrate ion in a solution that contains 0.900 M aluminum nitrate is __________ M.

A) 0.900

B) 0.450

C) 0.300

D) 2.70

E) 1.80

Answer: D

Diff: 3

Page Ref: Sec. 13.4

15) The concentration of KBr in a solution prepared by dissolving 2.21 g of KBr in 897 g of water is __________ molal.

A) 2.46

B) 0.0167

C) 0.0207

D) 2.07?10-5

E) 0.0186

Answer: C

Diff: 3

Page Ref: Sec. 13.4

16) The concentration of lead nitrate (Pb(NO

3)

2

) in a 0.726 M solution is __________

molal. The density of the solution is 1.202 g/mL.

A) 0.476

B) 1.928

C) 0.755

D) 0.819

E) 0.650

Answer: C

Diff: 5

Page Ref: Sec. 13.4

17) The concentration of a benzene solution prepared by mixing 12.0 g C

6H

6

with 38.0 g

CCl

4

is __________ molal.

A) 4.04

B) 0.240

C) 0.622

D) 0.316

E) 0.508

Answer: A

Diff: 4

Page Ref: Sec. 13.4

18) A solution is prepared by dissolving 15.0 g of NH

in 250.0 g of water. The density of

3

in the solution is

the resulting solution is 0.974 g/mL. The mole fraction of NH

3

__________.

A) 0.0640

B) 0.0597

C) 0.940

D) 0.922

E) 16.8

Answer: B

Diff: 4

Page Ref: Sec. 13.4

19) A solution is prepared by dissolving 15.0 g of NH

in 250.0 g of water. The density of

3

in the solution is __________. the resulting solution is 0.974 g/mL. The molarity of NH

3

A) 0.00353

B) 0.882

C) 60.0

D) 3.24

E) 3.53

Answer: D

Diff: 4

Page Ref: Sec. 13.4

20) A solution is prepared by dissolving 23.7 g of CaCl

2

in 375 g of water. The density of the resulting solution is 1.05 g/mL. The concentration of Cl- in this solution is

__________ M.

A) 0.214

B) 0.562

C) 1.12

D) 1.20

E) 6.64?10-2

Answer: C

Diff: 4

Page Ref: Sec. 13.4

21) A solution is prepared by dissolving 23.7 g of CaCl

2

in 375 g of water. The density of

the resulting solution is 1.05 g/mL. The concentration of CaCl

2

in this solution is

__________ molal.

A) 0.214

B) 0.569

C) 5.70

D) 63.2

E) 1.76

Answer: B

Diff: 4

Page Ref: Sec. 13.4

22) The concentration of HCl in a solution that is prepared by dissolving 5.5 g of HCl in

200 g of C

2H

6

O is __________ molal.

A) 27.5

B) 7.5?10-4

C) 3.3?10-2

D) 0.75

E) 1.3 Answer: D Diff: 3

Page Ref: Sec. 13.4

23) The concentration (M) of HCl in a solution prepared by dissolving 5.5 g of HCl in 200

g of C

2H

6

O is __________ M. The density of the solution is 0.79 g/mL.

A) 21

B) 0.93

C) 0.58

D) 6.0?10-4

E) 1.72

Answer: C

Diff: 3

Page Ref: Sec. 13.4

24) The mole fraction of He in a gaseous solution prepared from 4.0 g of He, 6.5 g of Ar, and 10.0 g of Ne is __________.

A) 0.60

B) 1.5

C) 0.20

D) 0.11

E) 0.86

Answer: A

Diff: 3

Page Ref: Sec. 13.4

25) The mole fraction of urea (MW = 60.0 g/mol) in a solution prepared by dissolving 16 g of urea in 39 g of H

2

O is __________.

A) 0.58

B) 0.37

C) 0.13

D) 0.11

E) 9.1

Answer: D

Diff: 3

Page Ref: Sec. 13.4

26) The concentration of urea (MW = 60.0 g/mol) in a solution prepared by dissolving 16 g of urea in 39 g of H

O is __________ molal.

2

A) 96

B) 6.8

C) 0.68

D) 6.3

E) 0.11

Answer: B

Diff: 3

Page Ref: Sec. 13.4

27) The molarity of urea in a solution prepared by dissolving 16 g of urea (MW = 60.0

g/mol) in 39 g of H

O is __________ M. The density of the solution is 1.3 g/mL.

2

A) 0.11

B) 3.7

C) 6.8

D) 6.3

E) 0.16

Answer: D

Diff: 3

Page Ref: Sec. 13.4

28) What is the molarity of sodium chloride in solution that is 13.0% by mass sodium chloride and that has a density of 1.10 g/mL?

A) 143

B) 2.45

C) 2.56

D) 2.23

E) 1.43?10-2

Answer: B

Diff: 4

Page Ref: Sec. 13.4

29) The concentration of sodium chloride in an aqueous solution that is 2.23 M and that has

a density of 1.01 g/mL is __________% by mass.

A) 2.21

B) 7.83

C) 45.3

D) 12.9

E) 10.1

Answer: D

Diff: 4

Page Ref: Sec. 13.4

30) The vapor pressure of pure ethanol at 60 °C is 0.459 atm. Raoult's Law predicts that a solution prepared by dissolving 10.0 mmol naphthalene (nonvolatile) in 90.0 mmol ethanol will have a vapor pressure of __________ atm.

A) 0.498

B) 0.413

C) 0.790

D) 0.367

E) 0.0918

Answer: B

Diff: 3

Page Ref: Sec. 13.5

31) The vapor pressure of pure water at 25 °C is 23.8 torr. What is the vapor pressure (torr) of water above a solution prepared by dissolving 18.0 g of glucose (a nonelectrolyte, MW = 180.0 g/mol) in 95.0 g of water?

A) 24.3

B) 23.4

C) 0.451

D) 0.443

E) 23.8

Answer: B

Diff: 4

Page Ref: Sec. 13.5

32) The vapor pressure of pure water at 25 °C is 23.8 torr. Determine the vapor pressure (torr) of water at 25 °C above a solution prepared by dissolving 35 g of urea

(a nonvolatile, non-electrolyte, MW = 60.0 g/mol)in 75 g of water.

A) 2.9

B) 3.3

C) 21

D) 27

E) 0.88

Answer: C

Diff: 4

Page Ref: Sec. 13.5

33) The freezing point of ethanol (C 2H 5OH) is -114.6 °C. The molal freezing point depression constant for ethanol is 2.00 °C/m. What is the freezing point (°C) of a solution prepared by dissolving 50.0 g of glycerin (C 3H 8O 3, a nonelectrolyte) in 200.0 g of ethanol?

A) -115

B) -5.42

C) -132.3

D) -120.0

E) -114.6

Answer: D

Diff: 4

Page Ref: Sec. 13.5

34) What is the freezing point (°C) of a solution prepared by dissolving 11.3 g of

Ca(NO

3)

2

(formula weight = 164 g/mol) in 115 g of water? The molal freezing point

depression constant for water is 1.86 °C/m.

A) -3.34

B) -1.11

C) 3.34

D) 1.11

E) 0.00

Answer: A

Diff: 4

Page Ref: Sec. 13.5

35) A solution containing 10.0 g of an unknown liquid and 90.0 g water has a freezing point of -3.33 °C. Given K f = 1.86 °C/m for water, the molar mass of the unknown liquid is __________ g/mol.

A) 69.0

B) 333

C) 619

D) 161

E) 62.1

Answer: E

Diff: 4

Page Ref: Sec. 13.5

36) A solution is prepared by dissolving 0.60 g of nicotine (a nonelectrolyte) in water to make 12 mL of solution. The osmotic pressure of the solution is 7.55 atm at 25 °C. The molecular weight of nicotine is __________ g/mol.

A) 28

B) 43

C) 50

D) 160

E) 0.60

Answer: D

Diff: 4

Page Ref: Sec. 13.5

37) A solution is prepared by dissolving 6.00 g of an unknown nonelectrolyte in enough water to make 1.00 L of solution. The osmotic pressure of this solution is 0.750 atm at

25.0 °C. What is the molecular weight (g/mol) of the unknown solute?

A) 16.4

B) 196

C) 110

D) 30.6

E) 5.12?10-3

Answer: B

Diff: 4

Page Ref: Sec. 13.5

38) Calculate the freezing point (0 °C) of a 0.05500 m aqueous solution of glucose. The molal freezing-point-depression constant of water is 1.86 °C/m.

A) 0.0286

B) 0.106

C) -0.0562

D) -0.102

E) -0.204

Answer: D

Diff: 2

Page Ref: Sec. 13.5

39) Calculate the freezing point (0 °C) of a 0.05500 m aqueous solution of NaNO

. The

3 molal freezing-point-depression constant of water is 1.86 °C/m.

A) 0.0286

B) -0.106

C) 0.102

D) -0.0562

E) -0.205

Answer: E

Diff: 4

Page Ref: Sec. 13.5

40) An aqueous solution of a soluble compound (a nonelectrolyte) is prepared by dissolving 33.2 g of the compound in sufficient water to form 250mL of solution. The solution has an osmotic pressure of 1.2 atm at 25 °C. What is the molar mass (g/mL) of the compound?

A) 1.0?103

B) 2.7?103

C) 2.3?102

D) 6.8?102

E) 28

Answer: B

Diff: 4

Page Ref: Sec. 13.5

. 41) Determine the freezing point (°C) of a 0.015 molal aqueous solution of MgSO

4 Assume i = 2.0 for MgSO

. The molal freezing-point-depression constant of water is

4

1.86 °C/m.

A) -0.056

B) -0.028

C) -0.17

D) -0.084

E) 0.000

Answer: A

Diff: 3

Page Ref: Sec. 13.5

42) A solution is prepared by dissolving 2.60 g of a strong electrolyte (formula weight = 101 g/mol) in enough water to make 1.00 L of solution. The osmotic pressure of the solution is 1.25 atm at 25.0 °C. What is the van't Hoff factor (i) for the unknown solute?

A) 0

B) 0.99

C) 1.98

D) 2.98

E) 0.630

Answer: C

Diff: 4

Page Ref: Sec. 13.5

43) George is making spaghetti for dinner. He places 4.01 kg of water in a pan and brings it to a boil. Before adding the pasta, he adds 58 g of table salt (NaCl) to the water and again brings it to a boil. The temperature of the salty, boiling water is __________ °C. Assume a pressure of 1.00 atm and negligible evaporation of water. K b for water is

0.52 °C/m

A) 99.87

B) 100.26

C) 100.13

D) 99.74

E) 100.00

Answer: B

Diff: 3

Page Ref: Sec. 13.5

13.2 Multiple-Choice Questions

1) The dissolution of water in octane (C

8H

18

) is prevented by __________.

A) London dispersion forces between octane molecules

B) hydrogen bonding between water molecules

C) dipole-dipole attraction between octane molecules

D) ion-dipole attraction between water and octane molecules

E) repulsion between like-charged water and octane molecules

Answer: B

Diff: 2

Page Ref: Sec. 13.1

2) When argon is placed in a container of neon, the argon spontaneously disperses throughout the neon because __________.

A) of the large attractive forces between argon and neon atoms

B) of hydrogen bonding

C) a decrease in energy occurs when the two mix

D) the dispersion of argon atoms produces an increase in disorder

E) of solvent-solute interactions

Answer: D

Diff: 2

Page Ref: Sec. 13.1

3) Hydration is a specific example of the phenomenon known generally as __________.

A) salutation

B) disordering

C) solvation

D) condensation

E) dilution

Answer: C

Diff: 1

Page Ref: Sec. 13.1

4) The dissolution of gases in water is virtually always exothermic because __________.

A) one of the two endothermic steps (separation of solute particles) in the

solution-formation process is unnecessary

B) the exothermic step in the solution-formation process is unnecessary

C) gases react exothermically with water

D) neither of the two endothermic steps in the solution-formation process is necessary

E) all three steps in the solution-formation process are exothermic

Answer: A

Diff: 2

Page Ref: Sec. 13.1

5) Formation of solutions where the process is endothermic can be spontaneous provided that __________.

A) they are accompanied by another process that is exothermic

B) they are accompanied by an increase in order

C) they are accompanied by an increase in disorder

D) the solvent is a gas and the solute is a solid

E) the solvent is water and the solute is a gas

Answer: C

Diff: 2

Page Ref: Sec. 13.1

6) The phrase "like dissolves like" refers to the fact that __________.

A) gases can only dissolve other gases

B) polar solvents dissolve polar solutes and nonpolar solvents dissolve nonpolar solutes

C) solvents can only dissolve solutes of similar molar mass

D) condensed phases can only dissolve other condensed phases

E) polar solvents dissolve nonpolar solutes and vice versa

Answer: B

Diff: 1

Page Ref: Sec. 13.1

7) Ammonium nitrate (NH

4NO

3

) dissolves readily in water even though the dissolution is

endothermic by 26.4 kJ/mol. The solution process is spontaneous because __________.

A) the vapor pressure of the water decreases upon addition of the solute

B) osmotic properties predict this behavior

C) of the decrease in enthalpy upon addition of the solute

D) of the increase in enthalpy upon dissolution of this strong electrolyte

E) of the increase in disorder upon dissolution of this strong electrolyte

Answer: E

Diff: 2

Page Ref: Sec. 13.1

8) When solutions of strong electrolytes in water are formed, the ions are surrounded by water molecules. These interactions are described as a case of __________.

A) hydration

B) supersaturation

C) crystallization

D) dehydration

E) saturation

Answer: A

Diff: 2

Page Ref: Sec. 13.1

9) When two nonpolar organic liquids are mixed, a solution forms and the enthalpy of solution is quite small. Label the two organic liquids as A (solvent) and B (solute). The formation of solution is favored by __________.

A) hydration of the solute, B

B) the equal enthalpy of the solvent and solute

C) the highly negative enthalpy of the solution process

D) solvation of the solvent, A

E) an increase in disorder, since A-A, B-B, and A-B interactions are similar Answer: E

Diff: 2

Page Ref: Sec. 13.1