Chemistry, 6e (McMurry/Fay)
Chapter 11 Solutions and Their Properties
11.1 Multiple-Choice Questions
1) Which of the following mixtures have components which can be separated by filtration?
A) colloids
B) solutions
C) suspensions
D) All of these
2) Stainless steel is an example of a ________ solution.
A) gas/solid
B) liquid/liquid
C) solid/liquid
D) solid/solid
3) In most liquid solutions, the component present in the larger amount is called the
A) dispersed medium.
B) emulsifying agent.
C) solute.
D) solvent.
4) The rubbing alcohol sold in drug stores often is composed of 70% isopropyl alcohol and 30% water.
In this solution
A) isopropyl alcohol is the solvent.
B) water is the solvent.
C) both water and isopropyl alcohol are solvents.
D) neither water nor isopropyl alcohol is a solvent.
5) Which is not a solution?
A) brass
B) fog
C) hydrochloric acid
D) wine
6) For a liquid solution made by dissolving a solid or a gas in a liquid, the
A) liquid is the solute.
B) liquid is the solvent.
C) solute is the component present in the greatest amount.
D) solvent is the component present in the greatest amount.
7) Iodine, I2(s), is more soluble in dichloromethane, CH2Cl2(l), than in water because
A) both iodine and dichloromethane have strong ion-dipole interactions.
B) the dipole-dipole forces in dichloromethane are much stronger than the dispersion forces in iodine.
C) the intermolecular forces are similar in both iodine and dichloromethane.
D) iodine is polar and dichloromethane has a large number of hydrogen bonds.
8) For which case would ΔHsoln be expected to be negative?
A) if solute-solute interactions are much greater than solvent-solvent and solute-solvent interactions
B) if solvent-solvent interactions are much greater than solute-solvent and solute-solute interactions
C) if solute-solvent interactions are much greater than solvent-solvent and solute-solute interactions
D) if solute-solvent interactions are the same as solvent-solvent and solute-solute interactions
9) KBr does not dissolve well in nonpolar solvents because
A) solute-solute interactions are much larger than solvent-solvent or solute-solvent interactions.
B) solvent-solvent interactions are much larger than solute-solvent or solute-solute interactions.
C) solute-solvent interactions are much larger than solvent-solvent or solute-solute interactions.
D) solute-solvent interactions are similar to solvent-solvent and solute-solute interactions.
10) Commercial cold packs often contain solid NH4NO3 and a pouch of water. The temperature of the
pack drops as the NH4NO3 dissolves in water. Therefore, for the dissolving of NH4NO3 in water,
A) ΔHsoln is negative and ΔSsoln may be negative or positive.
B) ΔHsoln is negative and ΔSsoln is positive.
C) ΔHsoln is positive and ΔSsoln may be negative or positive.
D) ΔHsoln is positive and ΔSsoln is positive.
11) When a particular solid begins to dissolve in water, the temperature rises dramatically. For the
dissolving of this solid in pure water
A) ΔHsoln is always negative and ΔSsoln may be negative or positive.
B) ΔHsoln is always negative and ΔSsoln is always positive.
C) ΔHsoln is always positive and ΔSsoln may be negative or positive.
D) ΔHsoln is always positive and ΔSsoln is always positive.
12) In the process of dissolving ionic compounds, the cations and anions are separated from the crystal
lattice and surrounded by an ordered shell of solvent molecules. If the solvent is water, the dissolved
ions are said to be
A) halogenated.
B) homogenized.
C) hybridized.
D) hydrated.
13) One reason ionic compounds do not dissolve well in nonpolar solvents is that
A) ion-dipole interactions are too large for effective solvation to occur.
B) ion-solvent interactions are not strong enough to solvate the ions in solution.
C) not all cations and anions have the same magnitude of charge and therefore do not form neutral ion
pairs.
D) there are no forces of attraction between ions and nonpolar molecules.
14) Which cation in each set is expected to have the larger (more negative) hydration energy?
I. Mg2+ or Ba2+
II. K+ or Al3+
A) Mg2+ in set I and K+ in set II
B) Mg2+ in set I and Al3+ in set II
C) Ba2+ in set I and K+ in set II
D) Ba2+ in set I and Al3+ in set II
15) Which cation in each set would be expected to have the larger (more negative) hydration energy?
I. Fe2+ or Fe3+
II. Li+ or NH4+
A) Fe2+ in set I and Li+ in set II
B) Fe2+ in set I and NH4+ in set II
C) Fe3+ in set I and Li+ in set II
D) Fe3+ in set I and NH4+ in set II
16) Although there are exceptions, which is most likely to be true for the dissolving of a solid in a
liquid?
A) ΔHsoln is positive.
B) ΔHsoln is negative.
C) ΔSsoln is positive.
D) ΔSsoln is negative.
17) When two similar liquids mix to form a solution, the entropy of solution (ΔSsoln) is expected to be
A) negative.
B) zero.
C) positive.
D) negative at low temperatures but positive at high temperatures.
18) When an ionic solute dissolves in water to form an unsaturated solution, the free energy change
(ΔGsoln) is
A) negative.
B) zero.
C) positive.
D) either A or C, depending on the ionic compound
19) The change in the Gibbs free energy for dissolving more solute in a supersaturated solution is
A) negative.
B) zero.
C) positive.
D) positive at low temperatures and negative at high temperatures.
20) The change in the Gibbs free energy for dissolving solute in a saturated solution is
A) negative.
B) zero.
C) positive.
D) positive at low temperatures and negative at high temperatures.
21) For the process of dissolving a solid in a liquid, which of the following statements is true?
A) ΔHsoln is always negative and ΔSsoln is usually positive.
B) ΔHsoln is always positive and ΔSsoln is usually negative.
C) ΔHsoln is either positive or negative and ΔSsoln is usually positive.
D) ΔHsoln is either positive or negative and ΔSsoln is usually negative.
22) Most gases become less soluble in water as the temperature increases. What can be concluded about
the signs of ΔHsoln and ΔSsoln in this case?
A) ΔHsoln is negative and ΔSsoln is negative.
B) ΔHsoln is negative and ΔSsoln is positive.
C) ΔHsoln is positive and ΔSsoln is negative.
D) ΔHsoln is positive and ΔSsoln is positive.
23) Arrange the following compounds in order of their expected increasing solubility in water:
KCl, CH3CH2-O-CH2CH3, CH3CH2CH2CH2-OH, CH3CH2CH2CH2CH3.
A) CH3CH2CH2CH2CH3 < KCl < CH3CH2-O-CH2CH3 < CH3CH2CH2CH2–OH
B) KCl < CH3CH2-O-CH2CH3 < CH3CH2CH2CH2-OH < CH3CH2CH2CH2CH3
C) CH3CH2CH2CH2CH3 < CH3CH2-O-CH2CH3 < KCl < CH3CH2CH2CH2–OH
D) CH3CH2CH2CH2CH3 < CH3CH2-O-CH2CH3 < CH3CH2CH2CH2-OH < KCl
24) Which of the following should most favor the solubility of an ionic solid in water?
A) a low lattice energy for the solid and a low hydration energy for its ions
B) a low lattice energy for the solid and a high hydration energy for its ions
C) a high lattice energy for the solid and a low hydration energy for its ions
D) a high lattice energy for the solid and a high hydration energy for its ions
25) Which should be least soluble in water?
A)
B)
C)
D)
26) What are the major solute-solvent interactions created when KBr dissolves in water?
A) dipole-dipole
B) dispersion
C) hydrogen bonding
D) ion-dipole
27) What are the major solute-solvent interactions created when HOCH2CH2OH dissolves in water?
A) dipole-dipole
B) dispersion
C) hydrogen bonding
D) ion-dipole
28) Substances with high lattice energies tend to be less soluble than substances with low lattice
energies. On that basis predict the relative aqueous solubility at 20°C, from highest to lowest, of the
following ionic compounds: Ce2(SO4)3, K2SO4, KBr, NaCl.
A) Ce2(SO4)3 > K2SO4 > KBr > NaCl
B) Ce2(SO4)3 > K2SO4 > NaCl > KBr
C) KBr > NaCl > K2SO4 > Ce2(SO4)3
D) NaCl > KBr > K2SO4 > Ce2(SO4)3
29) A solution has a density of 1.023 g/mL and a concentration of 0.0800 g/dL. What is the
concentration in parts per million?
A) 700 ppm
B) 782 ppm
C) 800 ppm
D) 818 ppm
30) Fresh air contains approximately 400 ppm CO2, whereas the breath of an intoxicated person
contains about 4 percent CO2. The amount of CO2 in the breath of an intoxicated person is ________
times the amount of CO2 in fresh air.
A) 10-2
B) 10-1
C) 101
D) 102
31) Formaldehyde is a carcinogenic volatile organic compound with a permissible exposure level of
0.75 ppm. At this level, how many grams of formaldehyde are permissible in a 6.0-L breath of air
having a density of 1.2 kg/m3?
A) 3.8 × 10-2 g formaldehyde
B) 5.4 × 10-6 g formaldehyde
C) 3.8 g formaldehyde
D) 5.4 g formaldehyde
32) The dose of amoxicillin given to a young child is 40 mg/kg of body weight/day. If the amoxicillin is
administered as a suspension having a concentration of 400 mg/5 mL, how many mL of amoxicillin
must be administered per dose for a child weighing 18 pounds?
A) 2.0 mL
B) 4.1 mL
C) 4.5 mL
D) 9.9 mL
33) Molarity is defined as moles of solute per
A) kilogram of solvent.
B) liter of solution.
C) mole of solvent.
D) total moles present.
34) Molality is defined as moles of solute per
A) kilogram of solvent.
B) liter of solution.
C) mole of solvent.
D) total moles present.
35) Which concentration becomes smaller as the temperature is increased from 20°C to 80°C?
A) mass %
B) molality
C) molarity
D) mole fraction
36) What is the mole fraction of ethanol in a solution made by dissolving 14.6 g of ethanol, C2H5OH, in
53.6 g of water?
A) 0.0964
B) 0.106
C) 0.214
D) 0.272
37) What is the molality of ethanol in a solution made by dissolving 14.6 g of ethanol, C2H5OH, in 53.6
g of water?
A) 0.00591 m
B) 0.272 m
C) 5.91 m
D) 272 m
38) What is the mole fraction of I2 in a solution made by dissolving 27.8 g of I2 in 245 g of hexane,
C6H14?
A) 0.0371
B) 0.0385
C) 0.0715
D) 0.0770
39) What is the mole fraction of oxygen in a gas mixture that is 22% oxygen and 78% nitrogen by
volume?
A) 0.20
B) 0.22
C) 0.25
D) 0.28
40) A solution is prepared by dissolving 17.75 g sulfuric acid, H2SO4, in enough water to make 100.0
mL of solution. If the density of the solution is 1.1094 g/mL, what is the mole fraction H2SO4 in the
solution?
A) 0.0181
B) 0.0338
C) 0.0350
D) 19.0
41) A solution is prepared by dissolving 17.75 g sulfuric acid, H2SO4, in enough water to make 100.0
mL of solution. If the density of the solution is 1.1094 g/mL, what is the molarity?
A) 0.1775 M H2SO4
B) 0.1810 M H2SO4
C) 1.810 M H2SO4
D) 1.940 M H2SO4
10
42) A solution is prepared by dissolving 17.75 g sulfuric acid, H2SO4, in enough water to make 100.0
mL of solution. If the density of the solution is 1.1094 g/mL, what is the molality?
A) 0.1775 m H2SO4
B) 0.1810 m H2SO4
C) 1.810 m H2SO4
D) 1.940 m H2SO4
43) A solution is prepared by dissolving 17.75 g sulfuric acid, H2SO4, in enough water to make exactly
100.0 mL of solution. If the density of the solution is 1.1094 g/mL, what is the weight % H2SO4 in the
solution?
A) 16.00%
B) 18.00%
C) 19.00%
D) 84.00%
44) A solution is prepared by dissolving 171 g of CdCl2 in enough water to make 250.0 mL of solution.
If the density of the solution is 1.556 g/mL, what is the molarity of the solution?
A) 0.440 M
B) 0.684 M
C) 0.933 M
D) 3.73 M
45) A solution is prepared by dissolving 171 g of CdCl2 in enough water to make exactly 250.0 mL of
solution. If the density of the solution is 1.556 g/mL, what is the weight percent of CdCl2 in the
solution?
A) 7.17%
B) 44.0%
C) 56.0%
D) 68.4%
46) What is the weight percent of vitamin C in a solution made by dissolving 1.30 g of vitamin C,
C6H8O6, in 55.0 g of water?
A) 0.195%
B) 0.242%
C) 2.31%
D) 2.36%
47) What is the weight percent of a caffeine solution made by dissolving 4.35 g of caffeine,
11
C8H10N4O2, in 75 g of benzene, C6H6?
A) 0.055%
B) 0.058%
C) 5.5%
D) 5.8%
48) What volume of 0.716 M KBr solution is needed to provide 10.5 g of KBr?
A) 7.52 mL
B) 14.7 mL
C) 63.2 mL
D) 123 mL
49) What volume of 3.00 M CH3OH solution is needed to provide 0.270 mol of CH3OH?
A) 1.23 mL
B) 11.1 mL
C) 90.0 mL
D) 810 mL
50) How much water must be added to 42.0 g of CaCl2 to produce a solution that is 35.0 wt% CaCl2?
A) 56.7 g
B) 78.0 g
C) 83.3 g
D) 120 g
51) To make a 2.0 M solution, one could take 2.00 moles of solute and add
A) 1.00 L of solvent.
B) 1.00 kg of solvent.
C) enough solvent to make 1.00 L of solution.
D) enough solvent to make 1.00 kg of solution.
52) To make a 2.00 m solution, one could take 2.00 moles of solute and add
A) 1.00 L of solvent.
B) 1.00 kg of solvent.
C) enough solvent to make 1.00 L of solution.
D) enough solvent to make 1.00 kg of solution.
53) What molality of pentane is obtained by dissolving 5.0 g pentane, C5H12, in 245.0 g hexane,
C6H14?
A) 0.020 m
B) 0.024 m
C) 0.28 m
D) 20. m
54) A solution is 2.25% by weight NaHCO3. How many grams of NaHCO3 are in 450.0 g of solution?
A) 0.500 g
B) 10.1 g
C) 200 g
D) 225 g
55) How many grams of KBr are required to make 650. mL of a 0.115 M KBr solution?
A) 0.628 g
B) 5.65 g
C) 8.90 g
D) 74.8 g
56) What is the molality of a glucose solution prepared by dissolving 18.0 g of glucose, C6H12O6, in
125.9 g of water?
A) 7.94 × 10-4 m
B) 0.143 m
C) 0.695 m
D) 0.794 m
57) Aqueous solutions of 30% (by weight) hydrogen peroxide, H2O2, are used to oxidize metals or
organic molecules in chemical reactions. Given that the density of the solution is 1.11 g/mL, calculate
the molarity.
A) 0.794 M
B) 6.78 M
C) 9.79 M
D) 12.6 M
58) Aqueous solutions of 30.0% (by weight) hydrogen peroxide, H2O2, are used to oxidize metals or
organic molecules in chemical reactions. Calculate the molality of this solution.
A) 0.974 m
B) 6.78 m
C) 9.79 m
D) 12.6 m
59) Sodium hydroxide is available commercially as a 50.0% by weight aqueous solution. The density of
the solution is 1.53 g/mL. Calculate the molarity of this sodium hydroxide solution.
A) 0.450 M
B) 19.1 M
C) 25.0 M
D) 125. M
60) Sodium hydroxide is available commercially as a 50.0% by weight aqueous solution. Calculate the
molality of this sodium hydroxide solution.
A) 0.450 m
B) 19.1 m
C) 25.0 m
D) 125. m
61) A 1.30 M solution of CaCl2 in water has a density of 1.11 g/mL. What is the molality?
A) 1.17 m CaCl2
B) 1.25 m CaCl2
C) 1.35 m CaCl2
D) 1.44 m CaCl2
62) A 3.17 m solution of CaCl2 in water has a density of 1.24 g/mL. What is the molarity?
A) 2.56 M CaCl2
B) 2.91 M CaCl2
C) 3.50 M CaCl2
D) 3.93 M CaCl2
63) A 2.00 M solution of CaCl2 in water has a density of 1.17 g/mL. What is the mole fraction of
CaCl2?
A) 0.0348
B) 0.0360
C) 0.0366
D) 0.0380
64) A solution of LiCl in water has XLiCl = 0.0500. What is the molality?
A) 2.60 m LiCl
B) 2.77 m LiCl
C) 2.92 m LiCl
D) 5.26 m LiCl
65) A solution of LiCl in water is 18.0 wt% LiCl. What is the mole fraction of LiCl?
A) 0.0853
B) 0.0933
C) 0.425
D) 4.56
66) At 25.0°C, a solution has a concentration of 3.179 M and a density of 1.260 g/mL. The density of
the solution at 50.0°C is 1.249 g/mL. What is the molarity of the solution at 50.0°C?
A) 2.545 M
B) 3.151 M
C) 3.179 M
D) 3.230 M
67) A saturated solution is defined as
A) a concentrated solution.
B) a solution that is in equilibrium with pure solvent.
C) a solution than is in equilibrium with undissolved solute.
D) a solution that is in equilibrium with both pure solvent and undissolved solute.
68) Which of the following does not affect the solubility of a solute in a given solvent?
A) polarity of the solute
B) polarity of the solvent
C) rate of stirring
D) temperature of the solvent and solute
69) Which of the following statements is true for a supersaturated solution?
A) The solute in the solution is at equilibrium with undissolved solute.
B) The solution contains more than the equilibrium amount of solute.
C) The solution is stable and the solute will not precipitate.
D) A supersaturated solution is more than 50% solute by mass.
70) In general, as the temperature increases, the solubility of gases in water ________ and the solubility
of most solids in water ________.
A) decreases, decreases
B) decreases, increases
C) increases, decreases
D) increases, increases
71) The solubility of gaseous solutes in liquid solvents is greater when the
A) external pressure over the solution is increased.
B) external pressure is decreased.
C) partial pressure of the gas above the solution is increased.
D) partial pressure of the solvent is increased.
72) In which case should CO2(g) be more soluble in water?
A) The total pressure is 5 atm and the partial pressure of CO2 is 1 atm.
B) The total pressure is 3 atm and the partial pressure of CO2 is 2 atm.
C) The total pressure is 1 atm and the partial pressure of CO2 is 0.03 atm.
D) The total pressure is 1 atm and the partial pressure of CO2 is 0.5 atm.
73) The Henry’s Law constant of methyl bromide, CH3Br, is k = 0.159 mol/(L ∙ atm) at 25°C. What is
the solubility of methyl bromide in water at 25°C and at a partial pressure of 250. mm Hg?
A) 0.0523 mol/L
B) 0.329 mol/L
C) 0.483 mol/L
D) 39.8 mol/L
74) The solubility of argon in water at 25°C is 0.0150 mol/L. What is the Henry’s Law constant for
argon if the partial pressure of argon in air is 0.00934 atm?
A) 1.40 × 10-4 mol/(L ∙ atm)
B) 0.623 mol/(L ∙ atm)
C) 1.61 mol/(L ∙ atm)
D) 4.10 mol/(L ∙ atm)
75) Which of the following is not an application of colligative properties?
A) adding silver to mercury to lower the vapor pressure of mercury
B) desalinating sea water by reverse osmosis
C) melting snow by application of salt
D) reduced boiling points of pure liquids at increased altitudes
76) A solution is prepared by dissolving 40.0 g of sucrose, C12H22O11, in 250. g of water at 25°C.
What is the vapor pressure of the solution if the vapor pressure of water at 25°C is 23.76 mm Hg?
A) 0.198 mm Hg
B) 20.5 mm Hg
C) 23.6 mm Hg
D) 24.0 mm Hg
77) A KCl solution is prepared by dissolving 40.0 g KCl in 250.0 g of water at 25°C. What is the vapor
pressure of the solution if the vapor pressure of water at 25°C is 23.76 mm Hg?
A) 20.5 mm Hg
B) 22.1 mm Hg
C) 22.9 mm Hg
D) 25.5 mm Hg
78) At a given temperature the vapor pressures of benzene and toluene are 183 mm Hg and 59.2 mm Hg,
respectively. Calculate the total vapor pressure over a solution of benzene and toluene with Xbenzene =
0.600.
A) 110 mm Hg
B) 121 mm Hg
C) 133 mm Hg
D) 242 mm Hg
79) At a given temperature the vapor pressures of benzene and toluene are 183 mm Hg and 59.2 mm Hg,
respectively. Calculate the mole fraction of benzene in the vapor phase over a solution of benzene and
toluene with Xbenzene = 0.600.
A) 0.600
B) 0.678
C) 0.756
D) 0.823
80) How many grams of sucrose, C12H22O11, must be added to 500. g of water at 100°C to change the
vapor pressure to 752 mm Hg?
A) 0.295 g
B) 5.32 g
C) 10.6 g
D) 101 g
81) If one mole of each is dissolved in 1.00 L of water, which will lower the vapor pressure the most?
A) C12H22O11
B) NaNO3
C) C3H7OH
D) MgCl2
82) When 2.36 g of a nonvolatile solute is dissolved in 100 g of solvent, the largest change in freezing
point will be achieved when the solvent is
A) benzene, Kf = 5.07.
B) camphor, Kf = 37.8.
C) chloroform, Kf = 4.70.
D) All are expected to have the same freezing point.
83) A 0.50 m solution of which solute has the largest van’t Hoff factor?
A) CaCl2
B) K3PO4
C) LiCO3
D) NaNO3
84) A 0.020 m aqueous solution containing which solute will have the lowest freezing point?
A) LiCl
B) NaCl
C) KCl
D) All will have approximately the same freezing point.
85) Which of the following solutions will have the lowest freezing point?
A) 0.0100 m NaCl
B) 0.0100 m Li2SO4
C) 0.035 m CH3CH2CH2OH
D) 0.015 m MgCl2
86) Which of the following pairs of solutions have roughly the same boiling point elevation?
A) 0.100 m C6H12O6 and 0.0333 m CuCl2
B) 0.100 m NaCl and 0.100 m C6H12O6
C) 0.200 m NaCl and 0.300 m Na2SO4
D) 0.100 m KCl and 0.0500 m MgBr2
87) What is the expected freezing point of a 0.50 m solution of Na2SO4 in water? Kf for water is
1.86°C/m.
A) -0.93°C
B) -1.9°C
C) -2.8°C
D) -6.5°C
88) Calculate the freezing point of a solution of 20.0 g methyl salicylate, C7H6O2, dissolved in 800. g
of benzene, C6H6. Kf for benzene is 5.10°C/m and the freezing point is 5.50°C for benzene.
A) -1.05°C
B) 1.05°C
C) 4.45°C
D) 6.54°C
89) What is the freezing point of a solution of 1.43 g MgCl2 in 100 g of water? Kf for water is 1.86°C/m
for water.
A) -0.0279°C
B) -0.279°C
C) -0.559°C
D) -0.838°C
90) The normal boiling point of pure benzene is found to be 80.10°C. What is the approximate
molecular weight of a nonionizing substance if a solution of 3.55 g of the substance dissolved in 100. g
of benzene has a normal boiling point of 80.19°C? Kb = 5.12°C/m for benzene, C6H6.
A) 20 amu
B) 500 amu
C) 2000 amu
D) 20,000 amu
91) An aqueous solution has a normal boiling point of 102.0°C. What is the freezing point of this
solution? For water Kb is 0.51°C/m and Kf = 1.86°C/m.
A) -0.55°C
B) -2.0°C
C) -3.6°C
D) -7.3°C
92) A solution of 0.2113 g of water dissolved in 25.0 g of a solvent freezes at 11.5°C below the freezing
point of the solvent. What is Kf for this solvent?
A) 0.735°C/m
B) 1.36°C/m
C) 5.39°C/m
D) 24.5°C/m
93) A 0.51 m aqueous solution of an unknown solute has a boiling point elevation of 0.62°C. The
boiling point elevation of a 0.51 m solution of a nonionizing molecular solute in water is 0.26°C. How
many moles of particles are formed per mole of solute when the unknown solute is dissolved in water?
A) 1.4
B) 2.0
C) 2.4
D) 3.0
94) An aqueous CsCl solution is 8.00 wt% CsCl and has a density of 1.0643 g/mL at 20°C. What is the
boiling point of this solution? Kb = 0.51°C/m for water.
A) 100.27°C
B) 100.53°C
C) 103.8°C
D) 104.3°C
95) Chloroform has a boiling point of 61.1°C and dichloromethane has a boiling point of 40.0°C. When
0.100 mol of dichloromethane is added to 0.900 mol of chloroform, the resulting solution will have a
boiling point
A) between 40.0°C and 61.1°C, but closer to 61.1°C.
B) between 40.0°C and 61.1°C, but closer to 40.0°C.
C) greater than 61.1°C.
D) less than 40.0°C.
96) Two aqueous solutions, A and B, are separated by a semipermeable membrane. The osmotic
pressure of solution A immediately begins to decrease. Which of the following statements is true?
A) Solvent molecules are moving from solution B into solution A.
B) The initial osmotic pressure of solution B is greater than that of solution A.
C) The solvent molecules are moving from the solution of higher osmotic pressure to that of lower
osmotic pressure.
D) Both B and C are true statements.
97) Red blood cells are placed into pure water. Which of the following statements is true?
A) Water molecules flow out of the red blood cells, causing them to collapse.
B) Water flows into the red blood cells, causing them to swell and burst.
C) The osmotic pressure of the cell contents increases, causing the cells to burst.
D) The osmotic pressure inside the cells equals the osmotic pressure outside.