Deck 13: Properties of Solutions

Question 1

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 1

hydration

Question 2

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

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

Answer 2

solvation

Question 3

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

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

Answer 3

supersaturated

Question 4

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 limit
D)contains more dissolved solute than the solubility allows
E)contains no solute

Question 5

Which one of the following is most soluble in water?

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

Question 6

Which one of the following is least soluble in water?

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

Question 7

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 8

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

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

Question 9

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

A)CCl₄
B)Kr
C)N₂
D)CH₃CH₂OH
E)H₂

Question 10

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 11

The dissolution of water in octane (C₈H₁₈)is principally 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 12

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 13

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 14

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

A)CBr₄
B)HBr
C)HCl
D)CH₃CH₂OH
E)NaCl

Question 15

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

A)CH₃CH₂OH
B)NH₃
C)NaCl
D)CCl₄
E)HBr

Question 16

Which one of the following vitamins is water soluble?

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

Question 17

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 limit
D)must be in contact with undissolved solid
E)exists only in theory and cannot actually be prepared

Question 18

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 19

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

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

Question 20

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 21

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 22

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 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

What is the concentration in ppm of a solution which is prepared by dissolving 15 mg of NaCl in 200 mL water?

A)1.5 × 10^-5
B)75
C)0.075
D)15
E)7.5 × 10^-5

Question 25

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 26

A 0.200 m solution of which one of the following solutes will have the lowest vapor pressure?

A)LiCl
B)AlCl₃
C)CaCl₂
D)glucose
E)KCl

Question 27

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 28

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 29

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 30

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 31

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

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

Question 32

A solution contains 15 ppm of benzene.The density of the solution is 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 33

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 34

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 35

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 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 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 38

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 39

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 40

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

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

Question 41

A 81.5 g sample of calcium chloride is dissolved in 102 g of water at 45 °C.The solution is cooled to 20.0 °C and no precipitate is observed.This solution is ________.

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

Question 42

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 is .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 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

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

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

Question 45

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 46

All of the following are considered to be colloids except ________.

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

Question 47

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 48

A 2.05 m aqueous solution of some unknown had a boiling point of 102.1 °C.Which one of the following could be the unknown compound? The boiling point elevation constant for water is

A)NaCl
B)CH₃OH
C)C₆H₁₂O₆
D)Na₂CO₃
E)CaBr₂

Question 49

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

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

Question 50

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 51

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 52

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 53

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

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

Question 54

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 55

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 56

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 57

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 58

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 59

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 60

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 61

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 62

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 63

A 17.2 g sample of potassium chlorate is dissolved in 250 g of water at 65 °C.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 64

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

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

Question 65

What is the mole fraction of LiCl in solution that is 9.0% by mass LiCl and has a density of 1.00 g/mL?

A)0.960
B)2.33
C)0.0403
D)2.12
E)9.00

Question 66

A solution is prepared by dissolving 23.7 g of CaCl₂ in 375 g of water.The density of the resulting solution is 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 67

The molarity of urea (MW = 60.0 g/mol)in a solution prepared by dissolving 11 g of urea in of H₂O is ________ M.Assume the volume of the solution does not change when dissolving the urea.

A)0.314
B)5.24
C)314
D)0.00524
E)0.00642

Question 68

A solution at that is 3.75 M in MnSO₄ monohydrate is considered a(n)________ solution.The solubility of MnSO₄ monohydrate in water at 20 °C is 70.0 g per 100.0 mL of water.

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

Question 69

A solution is prepared by dissolving 24.7 g of KBr in 375 g water at 20.0 °C.What is the molarity (M)of KBr in this solution? Density of the solution at 20.0 °C is 0.998 g/mL.

A)0.552
B)0.0659
C)0.000552
D)552
E)65.9

Question 70

A 30.0 g sample of potassium nitrate is dissolved in 100 g of water at 60 °C.The solution is cooled to 20.0 °C and a small amount of precipitate is observed.This solution is ________.

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

Question 71

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 72

What is the concentration (M)of HCl in a solution that is prepared by dissolving 25.5 g of HCl in of water? (Assume volume does not change after adding HCl.)

A)1.28
B)0.0350
C)35.0
D)3.50 × 10^-5
E)14.0

Question 73

A solution is prepared by dissolving 15.8 g of MgCl₂ in 255 g of water.What is the mole fraction of Cl^- in this solution?

A)0.977
B)0.0116
C)0.0232
D)0.988
E)0.00583

Question 74

The solubility of MnSO₄ monohydrate in water at 20 °C is 70.0 g per 100.0 mL of water.A solution at 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 75

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 76

What is the mole fraction of HCl in a solution that is prepared by dissolving 25.5 g of HCl in of water? The density of the solution is 1.0 g/mL.

A)0.0155
B)0.0319
C)0.984
D)0.874
E)32.0

Question 77

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 78

A solution is prepared by dissolving 23.7 g of CaCl₂ in 375 g of water.The density of the resulting solution is .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 79

What is the molality of LiCl in solution that is 9.0% by mass LiCl and has a density of 1.00 g/mL?

A)9.00
B)2.12
C)2.33
D)90.0
E)0.0900

Question 80

A solution is prepared by dissolving 25.0 g of NaCl in 500.0 g of water.What is the molality (m)of NaCl in the solution? The density of the solution is 1.0 g/mL.

A)0.000856
B)0.0500
C)50.0
D)8.56
E)0.856