Deck 13: Properties of Solutions

Question 1

Hydration is a specific example of the phenomenon known generally as ________.

A)salutation
B)disordering
C)solvation
D)condensation
E)dilution

Answer 1

solvation

Question 2

Which one of the following is most soluble in hexane (C₆H₁₄)?

A)CH₃OH
B)CH₃CH₂CH₂OH
C)CH₃CH₂OH
D)CH₃CH₂CH₂CH₂OH
E)CH₃CH₂CH₂CH₂CH₂OH

Answer 2

CH₃CH₂CH₂CH₂CH₂OH

Question 3

Which one of the following substances is more likely to dissolve in benzene (C₆H₆)?

A)CH₃CH₂OH
B)NH₃
C)NaCl
D)CCl₄
E)HBr

Answer 3

CCl₄

Question 4

Which of the following substances is more likely to dissolve in water?

A)HOCH₂CH₂OH
B)CHCl₃
C) O CH₃(CH₂)₉CH
D)CH₃(CH₂)₈CH₂OH
E)CCl₄

Question 5

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

Question 6

The principal reason for the extremely low solubility of NaCl in benzene (C₆H₆)is the ________.

A)strong solvent-solvent interactions
B)hydrogen bonding in C₆H₆
C)strength of the covalent bond in NaCl
D)weak solvation of Na⁺ and Cl^- by C₆H₆
E)increased disorder due to mixing of solute and solvent

Question 7

Compounds composed of a salt and water combined in definite proportions are known as ________.

A)clathrates
B)homogenates
C)ionic solids
D)molecular solids
E)hydrates

Question 8

A supersaturated solution ________.

A)is one with more than one solute
B)is one that has been heated
C)is one with a higher concentration than the solubility
D)must be in contact with undissolved solid
E)exists only in theory and cannot actually be prepared

Question 9

A solution with a concentration higher than the solubility is ________.

A)not possible
B)unsaturated
C)supercritical
D)saturated
E)supersaturated

Question 10

In a saturated solution of a salt in water, ________.

A)the rate of crystallization > the rate of dissolution
B)the rate of dissolution > the rate of crystallization
C)seed crystal addition may cause massive crystallization
D)the rate of crystallization = the rate of dissolution
E)addition of more water causes massive crystallization

Question 11

Which one of the following vitamins is water soluble?

A)A
B)B
C)K
D)D
E)E

Question 12

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

Question 13

Which one of the following is least soluble in water?

A)CH₃OH
B)CH₃CH₂CH₂OH
C)CH₃CH₂OH
D)CH₃CH₂CH₂CH₂OH
E)CH₃CH₂CH₂CH₂CH₂OH

Question 14

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

Question 15

An unsaturated solution is one that ________.

A)has no double bonds
B)contains the maximum concentration of solute possible, and is in equilibrium with undissolved solute
C)has a concentration lower than the solubility
D)contains more dissolved solute than the solubility allows
E)contains no solute

Question 16

Which one of the following substances is more likely to dissolve in CCl₄?

A)CBr₄
B)HBr
C)HCl
D)CH₃CH₂OH
E)NaCl

Question 17

Which of the following substances is more likely to dissolve in CH₃OH?

A)CCl₄
B)Kr
C)N₂
D)CH₃CH₂OH
E)H₂

Question 18

The dissolution of water in octane (C₈H₁₈)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

Question 19

Which one of the following is most soluble in water?

A)CH₃OH
B)CH₃CH₂CH₂OH
C)CH₃CH₂OH
D)CH₃CH₂CH₂CH₂OH
E)CH₃CH₂CH₂CH₂CH₂OH

Question 20

Which of the following substances is least likely to dissolve in water?

A)HOCH₂CH₂OH
B)CHCl₃
C) O CH₃(CH₂)₉CH
D)CH₃(CH₂)₈CH₂OH
E)CCl₄

Question 21

If the partial pressure of oxygen in the air a diver breathes is too great, ________.

A)respiratory tissue is damaged by oxidation
B)hyperventilation results
C)the urge to breathe is increased and excessive CO₂ is removed from the body
D)the urge to breathe is reduced and not enough CO₂ is removed from the body
E)No problems result from this situation.

Question 22

The concentration of CO₂ in a soft drink bottled with a partial pressure of CO₂ of 6.5 atm over the liquid at 29 °C is 2.2 × 10^-1 M. The Henry's law constant for CO₂ at this temperature is ________.

A)2.2 × 10^-1 mol/L-atm
B)7.6 × 10^-3 mol/L-atm
C)5.6 × 10^-3 mol/L-atm
D)3.4 × 10^-2 mol/L-atm
E)More information is needed to solve the problem.

Question 23

A 0.100 m solution of which one of the following solutes will have the highest vapor pressure?

A)KClO₄
B)Ca(ClO₄)₂
C)Al(ClO₄)₃
D)sucrose
E)NaCl

Question 24

Which of the following statements is false?

A)Nonpolar liquids tend to be insoluble in polar liquids.
B)The weaker the attraction between the solute and solvent molecules, the greater the solubility.
C)Substances with similar intermolecular attractive forces tend to be soluble in one another.
D)The solubility of a gas increases in direct proportion to its partial pressure above the solution.
E)The solubility of gases in water decreases with increasing temperature.

Question 25

Calculate the molarity of a 17.5% (by mass)aqueous solution of nitric acid.

A)0.274 m
B)2.74 m
C)3.04 m
D)4.33 m
E)The density of the solution is needed to solve the problem.

Question 26

Pressure has an appreciable effect on the solubility of ________ in liquids.

A)gases
B)solids
C)liquids
D)salts
E)solids and liquids

Question 27

A solution contains 11% by mass of sodium chloride. This means that ________.

A)there are 11 g of sodium chloride in in 1.0 mL of this solution
B)100 g of the solution contains 11 g of sodium chloride
C)100 mL of the solution contains 11 g of sodium chloride
D)the density of the solution is 11 g/mL
E)the molality of the solution is 11

Question 28

A solution is prepared by dissolving calcium chloride in water and diluting to 500.0 mL. If this solution contains 44 ppm chloride ions, the concentration of calcium ions is ________ ppm.

A)44
B)88
C)22
D)11
E)500

Question 29

As the concentration of a solute in a solution increases, the freezing point of the solution ________ and the vapor pressure of the solution ________.

A)increases, increases
B)increases, decreases
C)decreases, increases
D)decreases, decreases
E)decreases, is unaffected

Question 30

The magnitudes of K_f and of K_b depend on the identity of the ________.

A)solute
B)solvent
C)solution
D)solvent and on temperature
E)solute and solvent

Question 31

Of the concentration units below, only ________ uses kg of solvent in its calculation.

A)mass %
B)ppm
C)ppb
D)molarity
E)molality

Question 32

A 0.100 m solution of which one of the following solutes will have the lowest vapor pressure?

A)KClO₄
B)Ca(ClO₄)₂
C)Al(ClO₄)₃
D)sucrose
E)NaCl

Question 33

The concentration of CO₂ in a soft drink bottled with a partial pressure of CO₂ of 4.0 atm over the liquid at 25 °C is 1.2 × 10^-1 M. The Henry's law constant for CO₂ at this temperature is ________.

A)3.0 × 10^-2 mol/L-atm
B)4.5 × 10^-3 mol/L-atm
C)5.6 × 10^-3 mol/L-atm
D)2.3 × 10^-2 mol/L-atm
E)More information is needed to solve the problem.

Question 34

Calculate the molarity of a 10.0% (by mass)aqueous solution of hydrochloric acid.

A)0.274 m
B)2.74 m
C)3.04 m
D)4.33 m
E)The density of the solution is needed to solve the problem.

Question 35

Molality is defined as the ________.

A)moles solute/moles solvent
B)moles solute/liters solution
C)moles solute/kg solution
D)moles solute/kg solvent
E)none (dimensionless)

Question 36

Which of the following choices has the compounds correctly arranged in order of increasing solubility in water? (least soluble to most soluble)

A)CCl₄ < CHCl₃ < NaNO₃
B)CH₃OH < CH₄ < LiF
C)CH₄ < NaNO₃ < CHCl₃
D)LiF < NaNO₃ < CHCl₃
E)CH₃OH < Cl₄ < CHCl₃

Question 37

Which one of the following concentration units varies with temperature?

A)molarity
B)mass percent
C)mole fraction
D)molality
E)all of the above

Question 38

A solution contains 15 ppm of benzene. The density of the solution is 1.00 g/mL. This means that ________.

A)there are 15 mg of benzene in 1.0 g of this solution
B)100 g of the solution contains 15 g of benzene
C)1.0 g of the solution contains 15 × 10^-6 g of benzene
D)1.0 L of the solution contains 15 g of benzene
E)the solution is 15% by mass of benzene

Question 39

Which component of air is the primary problem in a condition known as "the bends"?

A)O₂
B)CO₂
C)He
D)N₂
E)CO

Question 40

The solubility of nitrogen gas at 25 °C and 1 atm is 6.8 × 10^-4 mol/L. If the partial pressure of nitrogen gas in air is 0.76 atm, what is the concentration (molarity)of dissolved nitrogen?

A)6.8 × 10^-4 M
B)5.2 × 10^-4 M
C)4.9 × 10^-4 M
D)3.8 × 10^-4 M
E)1.1 × 10^-5 M

Question 41

The most likely van't Hoff factor for an 0.01 m CaI₂ solution is ________.

A)1.00
B)3.00
C)1.27
D)2.69
E)3.29

Question 42

Pairs of liquids that will mix in all proportions are called ________ liquids.

A)miscible
B)unsaturated
C)polar liquids
D)saturated
E)supersaturated

Question 43

Which of the following liquids will have the lowest freezing point?

A)pure H₂O
B)aqueous glucose (0.60 m)
C)aqueous sucrose (0.60 m)
D)aqueous FeI₃ (0.24 m)
E)aqueous KF (0.50 m)

Question 44

Which of the following aqueous solutions will have the highest boiling point?

A)0.10 m Na₂SO₄
B)0.20 m glucose
C)0.25 m sucrose
D)0.10 m NaCl
E)0.10 m SrSO₄

Question 45

Colligative properties of solutions include all of the following except ________.

A)depression of vapor pressure upon addition of a solute to a solvent
B)elevation of the boiling point of a solution upon addition of a solute to a solvent
C)depression of the freezing point of a solution upon addition of a solute to a solvent
D)an increase in the osmotic pressure of a solution upon the addition of more solute
E)the increase of reaction rates with increase in temperature

Question 46

Hydrophobic colloids ________.

A)are those that contain water
B)can be stabilized by adsorption of ions
C)are those that do not contain water
D)can be stabilized by coagulation
E)will separate into two phases if they are stabilized

Question 47

Calculate the vapor pressure of a solution made by dissolving 109 grams of glucose (molar mass = 180.2 g/mol)in 920.0 ml of water at 25 °C. The vapor pressure of pure water at 25 °C is 23.76 mm Hg. Assume the density of the solution is 1.00 g/ml.

A)0.278 mm Hg
B)0.605 mm Hg
C)22.98 mm Hg
D)23.48 mm Hg
E)23.76 mm Hg

Question 48

A 1.35 m aqueous solution of compound X had a boiling point of 101.4 °C. Which one of the following could be compound X? The boiling point elevation constant for water is 0.52 °C/m.

A)CH₃CH₂OH
B)C₆H₁₂O₆
C)Na₃PO₄
D)KCl
E)CaCl₂

Question 49

Which of the following cannot be a colloid?

A)an emulsion
B)an aerosol
C)a homogeneous mixture
D)a foam
E)All of the above are colloids.

Question 50

Which one of the following solutes has a limiting van't Hoff factor (i)of 3 when dissolved in water?

A)KNO₃
B)CH₃OH
C)CCl₄
D)Na₂SO₄
E)sucrose

Question 51

The process of a substance sticking to the surface of another is called

A)absorption
B)diffusion
C)effusion
D)adsorption
E)coagulation

Question 52

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

Question 53

The ratio of the actual value of a colligative property to the value calculated, assuming the substance to be a nonelectrolyte, is referred to as ________.

A)Henry's law
B)vapor pressure lowering
C)the van't Hoff factor
D)freezing point depression
E)osmotic pressure

Question 54

Which of the following liquids will have the highest freezing point?

A)pure H₂O
B)aqueous glucose (0.60 m)
C)aqueous sucrose (0.60 m)
D)aqueous FeI₃ (0.24 m)
E)aqueous KF (0.50 m)

Question 55

Of the following, a 0.1 M aqueous solution of ________ will have the lowest freezing point.

A)NaCl
B)Al(NO₃)₃
C)K₂CrO₄
D)Na₂SO₄
E)sucrose

Question 56

The process of solute particles being surrounded by solvent particles is known as ________.

A)salutation
B)agglomeration
C)solvation
D)agglutination
E)dehydration

Question 57

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

Question 58

Which of the following liquids will have the lowest freezing point?

A)pure H₂O
B)aqueous glucose (0.050 m)
C)aqueous CoI₂ (0.030 m)
D)aqueous FeI₃ (0.030 m)
E)aqueous NaI (0.030 m)

Question 59

Which of the following liquids will have the highest freezing point?

A)pure H₂O
B)aqueous glucose (0.050 m)
C)aqueous CoI₂ (0.030 m)
D)aqueous FeI₃ (0.030 m)
E)aqueous NaI (0.030 m)

Question 60

Of the following, a 0.1 M aqueous solution of ________ will have the highest freezing point.

A)NaCl
B)Al(NO₃)₃
C)K₂CrO₄
D)Na₂SO₄
E)sucrose

Question 61

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

Question 62

The concentration of urea (MW = 60.0 g/mol)in a solution prepared by dissolving 16 g of urea in 39 g of H₂O is ________ molal.

A)96
B)6.8
C)0.68
D)6.3
E)0.11

Question 63

A solution is prepared by dissolving 23.7 g of CaCl₂ 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

Question 64

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

Question 65

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

Question 66

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

A)2.23
B)1.30
C)2.56
D)2.03
E)1.10

Question 67

The mole fraction of HCl in a solution prepared by dissolving 5.5 g of HCl in 200 g of C₂H₆O is ________. The density of the solution is 0.79 g/mL.

A)0.027
B)0.034
C)0.028
D)0.035
E)0.151

Question 68

A solution is prepared by dissolving 23.7 g of CaCl₂ in 375 g of water. The density of the resulting solution is 1.05 g/mL. The concentration of CaCl₂ in this solution is ________ molal.

A)0.214
B)0.569
C)5.70
D)63.2
E)1.76

Question 69

A solution is prepared by dissolving 15.0 g of NH₃ in 250.0 g of water. The density of the resulting solution is 0.974 g/mL. The molality of NH₃ in the solution is ________ m.

A)0.00353
B)0.882
C)60.0
D)3.24
E)3.53

Question 70

A solution is prepared by dissolving 15.0 g of NH₃ in 250.0 g of water. The density of the resulting solution is 0.974 g/mL. The molarity of NH₃ in the solution is ________ M.

A)0.00353
B)0.882
C)60.0
D)3.24
E)3.53

Question 71

The concentration (M)of HCl in a solution prepared by dissolving 5.5 g of HCl in 200 g of C₂H₆O 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

Question 72

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

A)0.0442
B)0.0462
C)0.223
D)0.483
E)0.505

Question 73

The mole fraction of urea (MW = 60.0 g/mol)in a solution prepared by dissolving 16 g of urea in 39 g of H₂O is ________.

A)0.58
B)0.37
C)0.13
D)0.11
E)9.1

Question 74

A solution is prepared by dissolving 23.7 g of CaCl₂ in 375 g of water. The density of the resulting solution is 1.05 g/mL. The concentration of CaCl₂ in this solution is ________ molar.

A)0.564
B)0.571
C)0.569
D)0.537
E)0.214

Question 75

The molarity of urea in a solution prepared by dissolving 16 g of urea (MW = 60.0 g/mol)in 39 g of H₂O is ________ M. The density of the solution is 1.3 g/mL.

A)0.11
B)3.7
C)6.8
D)6.3
E)0.16

Question 76

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

Question 77

The solubility of MnSO₄ monohydrate in water at 20 °C is 70.0 g per 100.0 mL of water. A solution at 20 °C that is 0.401 M in MnSO₄ monohydrate is best described as a(n)________ solution. The formula weight of MnSO₄ monohydrate is 168.97 g/mol.

A)hydrated
B)solvated
C)saturated
D)unsaturated
E)supersaturated

Question 78

The solubility of MnSO₄ monohydrate in water at 20 °C is 70.0 g per 100.0 mL of water. A solution at 20 °C that is 4.22 M in MnSO₄ monohydrate is best described as a(n)________ solution. The formula weight of MnSO₄ monohydrate is 168.97 g/mol.

A)hydrated
B)solvated
C)saturated
D)unsaturated
E)supersaturated

Question 79

A solution is prepared by dissolving 23.7 g of CaCl₂ in 375 g of water. The density of the resulting solution is 1.05 g/mL. The mole fraction of Cl^- in this solution is ________.

A)0.0103
B)0.0200
C)0.0201
D)0.0632
E)0.0630

Question 80

The concentration of HCl in a solution that is prepared by dissolving 5.5 g of HCl in 200 g of C₂H₆O is ________ molal.

A)27.5
B)7.5 × 10^-4
C)3.3 × 10^-2
D)0.75
E)1.3