Deck 13: Properties of Solutions

Question 1

Which one of the following substances would be the least soluble in CCl₄?

A)CH₃CH₂OH
B)H₂O
C)NH₃
D)C₁₀H₂₂
E)NaCl

Answer 1

NaCl

Question 2

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

Answer 2

HOCH₂CH₂OH

Question 3

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

Answer 3

weak solvation of Na⁺ and Cl^- by C₆H₆

Question 4

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

Question 5

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 6

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

Question 7

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 8

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 9

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

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

Question 10

Which one of the following substances would be the most soluble in CCl₄?

A)CH₃CH₂OH
B)H₂O
C)NH₃
D)C₁₀H₂₂
E)NaCl

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

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 14

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 15

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

Question 16

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

Question 18

A saturated solution __________.

A)contains as much solvent as it can hold
B)contains no double bonds
C)contains dissolved solute in equilibrium with undissolved solute
D)will rapidly precipitate if a seed crystal is added
E)cannot be attained

Question 19

Ammonium nitrate (NH₄NO₃)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

Question 20

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

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

Question 21

Calculate the molarity of a 25.4% (by mass)aqueous solution of phosphoric acid (H₃PO₄).

A)2.59 m
B)3.47 m
C)4.45 m
D)25.4 m
E)The density of the solution is needed to solve the problem.

Question 22

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

A)CCl₄
B)Kr
C)N₂
D)CH₃CH₂OH
E)H₂

Question 23

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

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

Question 24

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 25

Calculate the molality of a 25.4% (by mass)aqueous solution of phosphoric acid (H₃PO₄).

A)2.59 m
B)3.47 m
C)4.45 m
D)25.4 m
E)The density of the solution is needed to solve the problem.

Question 26

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 27

The largest value of the Henry's Law constant for the liquid solvent H₂O will be obtained with __________ gas as the solute and a temperature of __________°C.

A)C₂H₄, 45
B)Ar, 11
C)HCl, 49
D)CO₂, 32
E)N₂, 15

Question 28

Which one of the following is most soluble in water?

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

Question 29

The Procter & Gamble Company product called olestra^tm is formed by combining a sugar molecule with __________.

A)alcohols
B)vitamin A
C)fatty acids
D)protein
E)cholesterol

Question 30

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

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

Question 31

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 32

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 33

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 34

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 35

A solution contains 28% phosphoric acid by mass. This means that __________.

A)1 mL of this solution contains 28 g of phosphoric acid
B)1 L of this solution has a mass of 28 g
C)100 g of this solution contains 28 g of phosphoric acid
D)1 L of this solution contains 28 mL of phosphoric acid
E)the density of this solution is 2.8 g/mL

Question 36

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

A)CBr₄
B)HBr
C)HCl
D)CH₃CH₂OH
E)NaCl

Question 37

Which one of the following is least soluble in water?

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

Question 38

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 39

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 40

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 41

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 42

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 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

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 45

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

A)0.0607
B)0.0572
C)0.278
D)3.37
E)1.75

Question 46

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 L of this solution
B)100 g of the solution contains 15 g of benzene
C)100 g of the solution contains 15 mg of benzene
D)the solution is 15% by mass of benzene
E)the molarity of the solution is 15

Question 47

Calculate the mole fraction of HCl in a 10.0% (by mass)aqueous solution.

A)0.00111
B)0.0344
C)0.0520
D)0.0548
E)0.122

Question 48

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

A)3.37
B)0.278
C)2.78
D)0.212
E)The density of the solution is needed to solve the problem.

Question 49

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 50

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 51

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 52

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 53

Of the concentration units below, only __________ is temperature dependent.

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

Question 54

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 55

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 56

Calculate the mole fraction of phosphoric acid (H₃PO₄)in a 25.4% (by mass)aqueous solution.

A)0.0589
B)0.0626
C)0.259
D)1.00
E)4.14

Question 57

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 58

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 59

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

A)0.274 m
B)2.74 m
C)3.05 m
D)4.33 m
E)The density of the solution is needed to solve the problem.

Question 60

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 61

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 62

Which of the following cannot be a colloid?

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

Question 63

Of the following, a 0.2 M aqueous solution of __________ will have the highest freezing point.

A)(NH₄)₃PO₄
B)Pb(NO₃)₂
C)Na₃PO₄
D)Mg(NO₃)₂
E)NaCl

Question 64

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 65

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

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

Question 66

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 67

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 68

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 69

The ideal value of i (van't Hoff factor)for (NH₄)₃PO₄.

A)1
B)2
C)3
D)4
E)5

Question 70

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 71

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 72

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 73

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 74

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

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

Question 75

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

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

Question 76

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 77

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 78

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 79

Which produces the greatest number of ions when one mole dissolves in water?

A)NaCl
B)NH₄NO₃
C)NH₄Cl
D)Na₂SO₄
E)sucrose

Question 80

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)