Chemistry: The Central Science, 12e (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 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
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
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
7) 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
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
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
10) 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
11) 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
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
13) 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
14) 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
15) 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
16) 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
17) Which one of the following vitamins is water soluble?
A) A
B) B
C) K
D) D
E) E
18) Which one of the following substances would be the most soluble in CCl4?
A) CH3CH2OH
B) H2O
C) NH3
D) C10H22
E) NaCl
19) Which one of the following substances would be the least soluble in CCl4?
A) CH3CH2OH
B) H2O
C) NH3
D) C10H22
E) NaCl
20) 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
21) 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
22) Which of the following substances is more likely to dissolve in CH3OH?
A) CCl4
B) Kr
C) N2
D) CH3CH2OH
E) H2
23) Which one of the following substances is more likely to dissolve in CCl4?
A) CBr4
B) HBr
C) HCl
D) CH3CH2OH
E) NaCl
24) Which one of the following substances is more likely to dissolve in benzene (C6H6)?
A) CH3CH2OH
B) NH3
C) NaCl
D) CCl4
E) HBr
25) Which one of the following is most soluble in water?
A) CH3OH
B) CH3CH2CH2OH
C) CH3CH2OH
D) CH3CH2CH2CH2OH
E) CH3CH2CH2CH2CH2OH
26) Which one of the following is least soluble in water?
A) CH3OH
B) CH3CH2CH2OH
C) CH3CH2OH
D) CH3CH2CH2CH2OH
E) CH3CH2CH2CH2CH2OH
27) Which one of the following is most soluble in hexane (C6H14)?
A) CH3OH
B) CH3CH2CH2OH
C) CH3CH2OH
D) CH3CH2CH2CH2OH
E) CH3CH2CH2CH2CH2OH
28) 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
29) 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
30) 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.
31) 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.
32) Pressure has an appreciable effect on the solubility of __________ in liquids.
A) gases
B) solids
C) liquids
D) salts
E) solids and liquids
33) 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.
34) 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
35) The Procter & Gamble Company product called olestraTM is formed by combining a sugar molecule
with __________.
A) alcohols
B) vitamin A
C) fatty acids
D) protein
E) cholesterol
36) 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
37) 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.
38) 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
39) 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.
40) 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.
41) 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
42) 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.
43) 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.
44) 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
45) 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.
46) 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.
47) 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
48) 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
49) 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)
50) 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
51) Of the concentration units below, only __________ is temperature dependent.
A) mass %
B) ppm
C) ppb
D) molarity
E) molality
52) 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
53) 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
54) 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
55) 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
56) 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
57) 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
58) 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
59) 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)
60) 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)
61) 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)
62) 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)
63) 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
64) Which produces the greatest number of ions when one mole dissolves in water?
A) NaCl
B) NH4NO3
C) NH4Cl
D) Na2SO4
E) sucrose
65) 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
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
67) 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
68) 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
69) 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
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
71) 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
72) The ideal value of i (van’t Hoff factor) for (NH4)3PO4.
A) 1
B) 2
C) 3
D) 4
E) 5
73) 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
74) 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
75) The process of a substance sticking to the surface of another is called
A) absorption
B) diffusion
C) effusion
D) adsorption
E) coagulation
76) 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.
77) 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