Chemistry: The Central Science, 13e (Brown et al.)
Chapter 13 Properties of Solutions
13.1 Multiple-Choice Questions
1) 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
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
3) Hydration is a specific example of the phenomenon known generally as ________.
A) salutation
B) disordering
C) solvation
D) condensation
E) dilution
4) 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
5) 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
6) 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
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
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
9) A solution with a concentration higher than the solubility is ________.
A) not possible
B) unsaturated
C) supercritical
D) saturated
E) supersaturated
10) 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
11) 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
12) Which one of the following vitamins is water soluble?
A) A
B) B
C) K
D) D
E) E
13) 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
14) 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
15) Which of the following substances is more likely to dissolve in CH3OH?
A) CCl4
B) Kr
C) N2
D) CH3CH2OH
E) H2
16) Which one of the following substances is more likely to dissolve in CCl4?
A) CBr4
B) HBr
C) HCl
D) CH3CH2OH
E) NaCl
17) Which one of the following substances is more likely to dissolve in benzene (C6H6)?
A) CH3CH2OH
B) NH3
C) NaCl
D) CCl4
E) HBr
18) Which one of the following is most soluble in water?
A) CH3OH
B) CH3CH2CH2OH
C) CH3CH2OH
D) CH3CH2CH2CH2OH
E) CH3CH2CH2CH2CH2OH
19) Which one of the following is least soluble in water?
A) CH3OH
B) CH3CH2CH2OH
C) CH3CH2OH
D) CH3CH2CH2CH2OH
E) CH3CH2CH2CH2CH2OH
20) Which one of the following is most soluble in hexane (C6H14)?
A) CH3OH
B) CH3CH2CH2OH
C) CH3CH2OH
D) CH3CH2CH2CH2OH
E) CH3CH2CH2CH2CH2OH
21) 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
22) 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.
7
23) 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.
24) Pressure has an appreciable effect on the solubility of ________ in liquids.
A) gases
B) solids
C) liquids
D) salts
E) solids and liquids
25) 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.
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
27) 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
28) 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.
29) 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.
30) 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.
31) 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
32) 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)
33) 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
34) Of the concentration units below, only ________ uses kg of solvent in its calculation.
A) mass %
B) ppm
C) ppb
D) molarity
E) molality
35) 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
36) 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
37) 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
38) 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
39) The magnitudes of Kf and of Kb depend on the identity of the ________.
A) solute
B) solvent
C) solution
D) solvent and on temperature
E) solute and solvent
40) 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
41) 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)
42) 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)
43) 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)
44) 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)
45) 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
46) 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
47) 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
48) 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
49) 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
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
51) 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
52) 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
53) 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
54) The process of a substance sticking to the surface of another is called
A) absorption
B) diffusion
C) effusion
D) adsorption
E) coagulation
55) 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.
56) 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
13.2 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
2) Pairs of liquids that will mix in all proportions are called ________ liquids.
A) miscible
B) unsaturated
C) polar liquids
D) saturated
E) supersaturated
3) 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
4) 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
5) 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
6) 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
7) 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
8) 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
9) 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
10) 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
11) 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
12) 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
13) 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
14) 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
15) 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
16) 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
17) 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