CHAPTER 12. SAMPLE TEST 1
SAMPLE TEST 1. CHAPTER 1 2
1. A solution is a
a. homogeneous mixture of two or more substances.
b. heterogeneous mixture of at least three substances.
c. mixture of two or more substances in which the heavier
particles can "settle out."
d. homogeneous mixture of an element with a compound.
e. homogenous mixture containing two or more compounds.
2. Which of the following is not an example of a true solution?
a. a cola drink
b. gasoline
c. orange juice
d. brass
e. seawater
3. If two liquids are miscible, they _____ because _____.
a. do not mix together; their intermolecular interactions
are dissimilar
b. do not mix together; their intermolecular interactions are similar
c. do not mix together; their densities are dissimilar
d. mix together; their intermolecular interactions are similar
e. mix together; their intermolecular interactions are dissimilar
4. If two liquids are immiscible, they _____ because _____.
a. do not mix together; their intermolecular interactions
are dissimilar
b. do not mix together; their intermolecular interactions are similar
c. do not mix together; their densities are dissimilar
d. mix together; their intermolecular interactions are similar
e. mix together; their intermolecular interactions are dissimilar
5. If a liquid is miscible with water, some portion of the molecule is _____, which means that it is _____.
a. polar; hydrophobic
b. polar; hydrophilic
c. nonpolar; hydrophobic
d. nonpolar; hydrophilic
e. bipolar; insoluble
6. Sand is insoluble in both polar and nonpolar solvents because
a. its atoms are held together by a three-dimensional network
of strong covalent bonds.
b. the interactions between the particles of sand are much
stronger than the interactions between polar molecules.
c. the interactions between the particles of sand are much
weaker than the interactions between polar molecules.
d. the interactions between the particles of sand are much
stronger than the interactions between nonpolar molecules.
e. the interactions between the particles of sand are much
weaker than the interactions between nonpolar molecules.
7. In considering the enthalpy changes involved in the process of dissolving, the process of separating
solvent molecules is _____; separating solute particles is _____, and the process of forming
new solute-solvent associations is _____.
a.
b.
c.
d.
e.
endothermic; endothermic; endothermic
exothermic; exothermic; exothermic
endothermic; endothermic; exothermic
exothermic; exothermic; endothermic
endothermic; exothermic; endothermic
8. The overall process of forming a solution is endothermic if
a. ∆ H ° so lute + ∆ H ° so lve nt = ∆ H ° so lutio n
b. ∆ H ° so lute + ∆ H ° so lve nt < ∆ H ° so lutio n
c. ∆ H ° so lute + ∆ H ° so lve nt > ∆ H ° so lutio n
d. ∆ H ° solute + ∆ H ° solvent = 0
e. ∆ H ° solution = 0
9. The maximum amount of a substance that dissolves in a given amount of solvent at a
specified temperature is the _____ of the substance.
a.
b.
c.
d.
e.
concentration
molarity
solubility
lattice energy
density
10. When a solution is saturated the concentration of the solute is _____ the solubility, and _____
solute will dissolve.
a.
b.
c.
d.
e.
greater than; more
greater than; no more
equal to; no more
less than; no more
less than; more
11. When a solution is unsaturated the concentration of the solute is _____ the solubility, and _____
solute will dissolve.
a. greater than; more
b. greater than; no more
c. equal to; no more
d. less than; no more
e. less than; more
12. When a solution is supersaturated the concentration of the solute is _____ the solubility, and
_____ solute will dissolve.
a.
b.
c.
d.
e.
greater than; more
greater than; no more
equal to; no more
less than; no more
less than; more
13. The energy released when water molecules surround positive and negative ions is called
a. lattice energy
b. hydration energy
c. heat of mixing
d. entropy
e. solubility
14. Thermal pollution affects fish and other marine wildlife by
a. increasing the solubility of toxic ionic compounds.
b. decreasing the solubility of oxygen.
c. raising the body temperature of fish to a dangerous
level.
d. hindering the growth of marine plants.
e. preventing sunlight from reaching marine plants.
15. Solubility of a gas in a liquid increases if the pressure of the gas is increased because
a. the pressure increase is always accompanied by a temperature
increase.
b. a decrease in temperature is the cause of the pressure increase.
c. the probability of collisions between the gas and the liquid
surface is increased.
d. the energy released from the dissolving process heats the gas.
e. the volume of the system must decrease if the pressure
increases.
f.
16. The relationship between pressure and solubility of a gas is called
a. the Law of Conservation of Mass.
b. the First Law of Thermodynamics.
c. the Second Law of Thermodynamics.
d. Henry's Law.
e. the solubility rules.
17..Which description of solution concentration is quantitative?
a. saturated
b. unsaturated
c. concentrated
d. immiscible
e. molar
18. Which description of solution concentration is qualitative?
a. molarity
b. mole fraction
c. molality
d. saturated
e. weight %
19. The weight percent of sugar in a solution prepared by mixing 85.0 g of sucrose, C12H22O11, with 450. g
of water is
a. 5.52 × 10 -2 %
b. 4.65 × 10 -2 %
c. 15.9%
d. 18.9%
e. 84.1%
20. The weight percent of sugar in a solution prepared by mixing 125.0 g of sucrose, C12H22O11, with 550. g
of water is
a. 0.0541%
b. 18.5%
c. 22.7%
d. 77.3%
e. 81.5%
21. The measuring unit one part per million is equivalent to
a. one mg solute/kg solution
b. one ng solute/kg solution
c. one µ g solute/kg solution
d. one kg solute/ng solution
e. one kg solute/mg solution
22. The unit M means _____, which is defined as _____.
a. molality; moles solute/mole solvent
b. molality; moles solute/kg solvent
c. molarity; mass solute/mass solution
d. molarity; moles solute/mole solvent
e. molarity; moles solute/liter solution
23. The unit m means _____, which is defined as _____.
a. molality; moles solute/mole solvent
b. molality; moles solute/kg solvent
c. molarity; mass solute/mass solution
d. molarity; moles solute/mole solvent
e. molarity; moles solute/liter solution
24. Which unit of concentration is dependent on temperature?
a. mass %
b. molality
c. molarity
d. mole %
e. parts per thousand
25. The molality of a solution is defined as
a. moles of solute per liter of solution.
b. grams of solute per liter of solution.
c. moles of solute per kilogram of solution.
d. moles of solute per kilogram of solvent.
e. the gram molecular weight of solute per kilogram of solvent.
26. What is the molarity of a NH 3 solution which contains 4.25 g of NH 3 in 2.00 L of solution?
a. 0.125 M
b. 0.250 M
c. 0.500 M
d. 1.00 M
e. 2.80 M
27. What is the percent NaCl by mass in a 1.00 molal aqueous solution?
a. 5.52
b. 5.84
c. 5.85
d. 8.35
e. 9.21
28. How many moles of ethanol, must be dissolved in one hundred grams of water to give a 1.5 molal
solution?
a. 15
b. 1.5
c. 0.15
d. 0.015
e. 0.0015
29. When one mole of a nonvolatile nonelectrolyte is dissolved in three moles of a solvent, the vapor
pressure of the solution compared to that of the pure solvent is
a. 1/4.
b. 1/3.
c. 1/2.
d. 2/3.
e. 3/4.
30. Using Raoult's law, given that the pure vapor pressure of water (M.W. 18.0 g/mol) at 75oC is
290mmHg, the vapor pressure of an aqueous solution at 75oC containing 60g of urea (M.W. 60.0
g/mol), a nonelectrolyte, in 180g of water is
a. 29 mmHg.
b. 100 mmHg.
c. 130 mmHg.
d. 190 mmHg.
e. 264 mmHg.
31. According to Henry's Law, the concentration of a gas in solution at a constant temperature is
directly proportional to
a. the pressure of the gas above the solution.
b. the vapor pressure of the pure solvent.
c. the mole fraction of solvent present.
d. Each of these statements is true.
32. A 60.0-g sample of NaOH ( F.W. 40.0 g/mol) is dissolved in water, and the solution is diluted to give a
final volume of 3.00 L. The molarity of the final solution is
a. 0.500 M.
b. 0.750 M.
c. 1.00 M.
d. 2.00 M.
e. 3.00 M.
33. How many grams of Na 2SO4 (F.W. 142 g/mol) are contained in 0.400 L of 0.250 M Na 2SO4 solution?
a. 14.2
b. 18.3
c. 27.6
d. 35.5
e. 68.4
34. Using Raoult's law, given that the pure vapor pressure of water (M.W. 18.0 g/mol) at 75oC is
290mmHg, the vapor pressure of an aqueous solution at 75oC containing 60g of urea (M.W. 60.0
g/mol), a nonelectrilyte, in 180g of water is
a. 29 mmHg.
b. 100 mmHg.
c. 130 mmHg.
d. 190 mmHg.
e. 264 mmHg.
35. The solubility of a gas in a liquid can always be increased by
a. increasing the temperature of the solvent.
b. decreasing the polarity of the solvent.
c. decreasing the temperature of the gas above the solvent.
d. decreasing the pressure of the gas above the solvent.
e. increasing the pressure of the gas above the solvent.
36. Which one of the following is not a colligative property?
a. osmotic pressure.
b. boiling point elevation.
c. density
d. vapor pressre lowering.
e. freezing-point depression
37. If 0.100 mol of napthalene is dissolved in 100.0 g of benzene (C6H6 ), what is the molality?
a. 0.100
b. 0.900
c. 1.00
d. 1.28
e. 12.8
38. What is the mole fraction of methanol, CH3OH (M.W. 32 g/mol), in an ethanol, C2H5OH (M.W. 46
g/mol), solution that is 60.0% ethanol by mass?
a. 0.40
b. 0.46
c. 0.49
d. 0.54
e. 0.60
39. What is the molality of ethyl alcohol, C2H5OH (M.W. 46.0 g/mol), in an aqueous solution that is 50.0%
ethyl alcohol by mass?
a. 10.9
b. 21.7
c. 25.9
d. 28.1
e. 71.9
40. Which of the following solutions made up of soluble salts has the highest osmotic pressure?
a. 0.15 M NaCl
b. 0.10 M CaCl2
c. 0.15 M Ba(NO3)2
d. 0.10 M Al(NO3)3
41. Calculate the MOLALITY of C2H5OH in a water solution which is prepared by mixing 50.0 mL of
C2H5OH with 100.0 mL of H2O at 20 °C. The density of the C2H5OH is 0.789 g/mL at 20 °C.
a.
b.
c.
d.
0.086 m
0.094 m
1.24 m
8.56 m
e. none of these
42. A solution of two liquids, A and B, shows negative deviation from Raoult's Law. This means that
a. the molecules of A interact strongly with other A-type molecules.
b. the two liquids have a positive heat of solution.
c. molecules of A interact weakly, if at all, with B molecules.
d. the molecules of A hinder the strong interaction between B molecules.
e. molecules of A interact more strongly with B than A with A or B with B.
43. Which of the following is NOT a colligative property?
a. freezing point depression
b. boiling point elevation
c. osmotic pressure
d. solubility
e. two of the above
44. The molal freezing point depression constants for benzene and water are 5.12 and 1.86 respectively.
When 4.6 g of formic acid (HCOOH) is dissolved in 1.0 kg of benzene, the observed freezing point
lowering is 0.26C. When the same amount of formic acid is dissolved in 1.0 kg of water, the freezing
point is lowered by 0.19C. To explain these results, we must assume that:
a. formic acid is ASSOCIATED in benzene and MONOMERIC in water.
b. formic acid is MONOMERIC in benzene and DISSOCIATED in water.
c. formic acid is MONOMERIC in benzene and ASSOCIATED in water.
d. formic acid is DISSOCIATED in benzene and MONOMERIC in water.
e. none of these is true.
45. When one mole of a nonvolatile non-dissociating substance is dissolved in two moles of solvent, the
ratio of the vapor pressure of the solution to that of the pure solvent (at the same temperature) is
approximately:
a. 1/3
b. 1/2
c. 2/3
d. 3/2
e. none of these
46. How many grams of water are needed to give a 3.00 m NH 3 solution if 15 moles of NH3 are to be
dissolved in the water?
a. 5
b. 4500
c. 4.5
d. 2000
e. 5000
47. Determine the molarity of a 25.0% CaCl 2 solution that has a density of 1.228 g/mL.
a. 11.1 b. 0.25
c. 2.77 d. 5.45
e. 22.6
48. What is the MOLALITY of a solution of 50.0 g of propanol (molar mass = 60.1 g/mol) in 152 mL water,
if the density of water is 1.0 g/mL?
a) 5.47 m b) 0.00547 m
c) 0.833 m d) 0.183 m e) none of these
49. How many grams of C12H22O11 are needed to dissolve in 250g of water to give a 2.337 x 10 -1 m solution?
(M.W. C12H22O11 = 342.34)
a. 6.000g b. 2.100g
c. 11.00g
d. 20.00g e. 1600g
50. A solution is made by adding 0.100 mole of ethyl ether to 0.500 mole of ethyl alcohol. If the vapor
pressures of ethyl ether and ethyl alcohol at 20 oC are 375 torr and 20.0 torr, respectively, the vapor
pressure of the solution at 20 oC (assuming ideal behavior) is:
a) 79.2 torr b) 316 torr c) 47.5 torr d) 395 torr e) none of these
51. The term "proof" is defined as twice the percent by volume of pure ethanol in solution. Thus, a solution
that is 95% (by VOLUME) ethanol is 190 proof. What is the MOLARITY of ethanol in a 92 proof
ethanol/water solution?
density of ethanol = 0.80 g/cm3
density of water = 1.0 g/cm3
mol. wt. of ethanol = 46
a) 0.46 M b) 0.80 M c) 0.92 M d) 8.0 M e) 17 M
52. Vapor pressure (in torr) at 25 oC
benzene (C6H6)
94.4
chloroform (CH3Cl)
172.0
Using the above data, calculate the total vapor pressure of a chloroform-benzene solution at 25 oC
which contains 50.0 g CH3Cl and 50.0 g C6H6. Assume the solution behaves ideally.
a) 67.8 torr b) 125 torr
c) 141 torr d) 172 torr e) none of these
53. When a nonvolatile solute is added to a volatile solvent, the solution vapor pressure
________________ , the boiling point _______________ , the freezing point _______________ , and
the osmotic pressure across a semipermeable membrane _________________ .
a) decreases, increases, decreases, decreases.
b) increases, increases, decreases, increases.
c) increases, decreases, increases, decreases.
d) decreases, decreases, increases, decreases.
e) decreases, increases, decreases, increases.
54. A solute added to a solvent raises the boiling point of the solution because
a) the temperature to cause boiling must be great enough to boil not only the solvent but also the solute.
b) the solute particles lower the solvent's vapor pressure thus requiring a higher temperature to cause
boiling.
c) the solute particles raise the solvent's vapor pressure thus requiring a higher temperature to cause boiling.
d) the solute increases the volume of the solution, and an increase in volume requires an increase in
the temperature to reach the boiling point (derived from PV = nRT).
e) two of the above are correct.
55. At a given temperature the vapor pressures of pure liquid benzene and toluene are 745 torr and 290
torr, respectively. A solution prepared by mixing benzene and toluene obeys Raoult's law. At this
temperature the vapor pressure of benzene over a solution in which the mole fraction of benzene is
equal to 0.340 is
a) 417 torr b) 352 torr c) 98.6 torr d) 253 torr e) none of these
56. A solution of hydrogen peroxide is 30.0% H2O2 by mass and has a density of 1.11 g/cm3. The
MOLARITY of the solution is:
a) 7.94 M b) 8.82 M c) 9.79 M d) 0.980 e) none of these
57. A solution containing 296.6 g of Mg(NO3)2 per liter has a density of 1.114 g/mL. The MOLARITY of the
solution is:
a) 2.000 M
b) 2.446 M
c) 6.001 M
d) 1.805 M
e) none of these
58. The osmotic pressure, in torr, of a 0.0100 M solution of NaCl in water at 25C is APPROXIMATELY:
a) 0.245
b) 15.6
c) 372
d) 186
e) none of these
59. When 100. mL of 0.125 M HCl is diluted to 250. mL, the resulting MOLARITY of the HCl solution is:
a) 0.625 M b) 0.250 M
c) 0.0500 M
d) 0.0250 M e) none of these
60. When 1.50 g of glutamic acid is dissolved in 100.0 g H 2O, the resulting solution freezes at -0.190C. (Kf
for H2O is 1.86C kg/mol.) The molecular weight of glutamic acid is:
a) 14.7 g/mol
b) 1.50 g/mol
c) 189 g/mol
d) 28.0 g/mol e) 147 g/mol
61. Benzene and toluene form an ideal solution. At 298K, what is the mole fraction of benzene in the liquid
that is in equilibrium with a vapor that has equal partial pressures of benzene and toluene? At 298K,
the vapor pressures of pure benzene and pure toluene are 95 and 28 torr, respectively.
a) 0.50
b) 0.77
c) 0.23 d) 0.30
e) none of these
62. In order to calculate the freezing point of an ideal dilute solution of a single, non-dissociating solute in a
solvent, the minimum information one must know is:
a) the molality (of the solute).
b) the molality (of the solute) and the freezing point depression constant of the solvent.
c) the same quantities as in (b) plus the freezing point of the pure solvent.
d) all of the quantities in (c) plus the molecular weight of the solute.
e) all of the quantities in (c) plus the weight of the solvent.
63. The vapor pressure of water at 90C is 0.692 atm. What is the vapor pressure (in atm) of a solution made
by dissolving 1.00 mole of CsF(s) in 1.00 kg of water? Assume that Raoult's law applies.
a) 0.692 atm b) 0.680 atm c) 0.668 atm d) 0.656 atm
e) none of these
64. Pentane and hexane form an ideal solution. The components have the following properties:
- - molar mass
- density
- bp
- vapor pressure at 25oC
o
pentane 72
0.63 g/mL
36 C 511 torr
hexane
86
0.66 g/mL
69 oC 150 torr
What is the mole fraction of pentane (Xpentane) in the vapor in equilibrium at 25C with a pentanehexane solution in which Xpentane = 0.30?
a) Xpentane = 0.23 b) Xpentane = 0.29 c) Xpentane = 0.59 d) Xpentane = 0.68 e) Xpentane = 0.77
65. What is the mole fraction of ethanol, C2H5OH, in a methanol solution that is 40.%(w/w)
methanol, CH3OH, by mass?
a. 0.40
b. 0.46
c. 0.51
d. 0.54
66. Calculate the molarity (M) of a solution containing 12.0 moles of KNO3 and 5000 mL of
water. a. 2.40 x 10-3. b. 2.40. c. 2.40 x 10-2. d. 2.40x 10-1.
67. The density of a 3.54 M solution of NH4Cl is 1.0512 g/mL. What is the molality of the solution?
a. 4.51 b. 3.54 c. 4.11
d. 5.02
68. 135 grams of an aqueous KOH solution contains 18.5 grams of KOH. What is the percentage of
KOH in the solution?
a. 13.7% b. 18.5% c. 16.7% d. 15.2%
69. Which of the following solutes dissolved in 1000 g of water provide the fewest number of particles
in the solution?
a.
b.
c.
d.
e.
0.030 moles urea, CO(NH2) 2 (covalent compound)
0.030 moles acetic acid, CH3COOH(weak acid)
0.030 moles ammonium nitrate, NH4NO3
0.030 moles calcium sulfate, CaSO4 (insoluble salt)
0.030 moles barium chloride, BaCl2
70. Determine the sodium ion concentration, [Na+], in a solution with 50.0 g Na3PO4 dissolved in
750. mL of solution.
a. 0.407 M
b. 0.565 M
c. 1.22 M
d. 1.69 M
e. 3.66 M
71. What is the molarity of technical grade concentrated sulfuric acid, H2SO4, which is labeled 95%
and has a density of 1.84 g/mL?
a. 0.969 M
b. 1.84 M
c. 17.8 M
d. 51.6 M
e. 98.0 M
72. The vapor pressure of water at 90.0°C is 526 mm Hg. What is the vapor pressure of a 50.0%(w/w)
solution of glucose, C6H12O6, at 90.0°C?
a. 478 mm Hg
b. 47.9 mm Hg
c. 526 mm Hg
d. 263 mm Hg
e. 2.63 mm Hg
73. Calculate the freezing point of an aqueous solution of CaCl2 prepared by mixing 385.0 g solute
with 1.00 kg of water. The value of kf for water is 1.86°C/m.
a. 0.0 ° C
b. -1.86 ° C
c. -6.45 ° C
d. -12.9 ° C
e. -19.4 ° C
74. Calculate the boiling point of a mixture where 95.0 g of formic acid, H2CO2, is dissolved in 250. g
of acetic acid. Acetic acid has a Kb of 2.93°C/m and boils at 118°C. Assume formic acid does not
ionize when dissolved in acetic acid.
a. 115 ° C
b. 118 ° C
c. 126 ° C
d. 136 ° C
e. 142 ° C
75. Arrange the solutions in order of increasing freezing point: 0.15 m glucose, C6H12O6 0.15 m LiCl 0.25
m NH4NO3 a. C6H12O6 < LiCl < NH4NO3
b.
c.
d.
e.
C6H12O6 = LiCl < NH4NO3
NH4NO3 < C6H12O6 = LiCl
NH4NO3 < LiCl < C6H12O6
LiCl < C6H12O6 < NH4NO3
76. Osmotic pressure is the
a. pressure that must be applied to a solution in order to cause osmosis to occur from the pure solvent.
b. pressure that must be applied to a solution in order to prevent osmosis from the pure solvent.
c. decrease in vapor pressure when a solution is compared to a pure solvent.
d. increase in vapor pressure when a solution is compared to a pure solvent.
e. correction factor applied when a sample of gas is collected by water displacement.
77. Osmotic pressure is especially useful for determining _____ of a solute.
a. boiling point
b. density
c. freezing point
d. molar mass
e. solubility
78. The driving force for osmosis is
.
a. entropy
b. temperature
c. pressure
d. enthalpy
e. identity of the solute
79. An aqueous solution at 27°C contains 4.2 g of a protein in a 200. mL sample. The osmotic pressure
is 0.0237 atm. What is the molar mass of the protein?
a.
b.
c.
d.
e.
2.2 × 10 4 g/mol
870 g/mol
2.0 × 10 3 g/mol
79 g/mol
22 g/mol
80. In living systems, a solution that is ____ has a lower solute concentration than the surrounding
cells and therefore causes water to flow _____ the cells by osmosis.
a.
b.
c.
d.
e.
hypertonic; into
hypotonic; into
isotonic; into
hypertonic; out of
hypotonic; out of
81. A simple home experiment involves dissolving the shell of an egg in vinegar and placing the
remaining membrane-covered "egg" in a very concentrated salt solution. This would cause the
"egg" to _____ in size because _____.
a.
b.
c.
d.
e.
shrink; water would flow out of the "egg"
swell; water would flow out of the "egg"
remain the same; only air can penetrate the
membrane
shrink; water would flow into the "egg"
swell; water would flow into the "egg"
82. In a colloid, the large particles analogous to the solute are called the _____, and the
medium analogous to the solvent is called the _____.
a.
b.
c.
d.
e.
dispersed; continuous
continuous; dispersed
vapor; dispersed
liquid; continuous
liquid; solid
83. All of the following are types of colloids except
a. milk
b. blood
c. mayonnaise
d. filtered black coffee
e. orange juice
84. An emulsifier is a substance that
a. gets dissolved in another substance.
b. dissolves another substance.
c. coats and stabilizes particles of a dispersed
phase.
d. settles to the bottom of a container of a
heterogeneous mixture.
e. diffuses through the membrane in osmosis.
85. The chemical structure of a surfactant always contains
a. a metal ion.
b. a hydrophilic portion and a hydrophobic portion.
c. an aromatic group and an acid group.
d. one or more amino acids and a phosphate group.
e. a fatty acid and an amino acid.
86. The product of a saponification reaction is a
a. detergent
b. micelle
c. scale
d. scum
e. soap
87.Arrange the following steps of water purification in the correct order.
I.
aeration
II.
addition of alum and lime
III. chlorination
IV. coarse filtration
V.
sand filtration
VI. settling
a. I-II-III-IV-V-VI
b. IV-II-VI-V-I-III
c. II-VI-I-IV-V-III
d. I-III-II-VI-IV-V
e. III-V-IV-II VI-I
88. One of the unwanted byproducts of chlorination of drinking water is _____, which may present a health
hazard.
a. alkaline earth cations, such as Mg2+
b. trihalomethanes, also called THMs
c. soap scum
d. boiler scale
e. iron discoloration
89. All of the following ions contribute to the hardness of water except
a. Ca2+
b. Fe3+ c.Mg2+ d. Mn2+ e. Na+
Answers to questions:
1. > a. homogeneous mixture of two or more substances.
2. > c. orange juice
3. > d. mix together; their intermolecular interactions are similar
4. > a. do not mix together; their intermolecular interactions are dissimilar
5. > b. polar; hydrophilic
6. > a. its atoms are held together by a three-dimensional network of strong covalent bonds
7. > c. endothermic; endothermic; exothermic
8. > c. ∆ H ° solute + ∆ H ° solvent > ∆ H ° solution.
9. > c. solubility
10. > c. equal to; no more
11. > e. less than; more
12. > b. hydration energy
13. > b. hydration energy
14. > b. decreasing the solubility of oxygen.
15. > c. the probability of collisions between the gas and the liquid surface is increased.
16. > d. Henry's Law.
17. > e. molar
18. > d. saturated
19. > c. 15.9%
20. > b. 18.5%
21. > a. one mg solute/kg solution
22. > e. molarity; moles solute/liter solution
23. > b. molality; moles solute/kg solvent
24. > c. molarity
25. > d moles of solute per kilogram of solvent.
26. > a 0.125 M
27. > a 5.52
28. > c 0.15
29. > e 3/4.
30. > e 264 mmHg.
31. > a the pressure of the gas above the solution.
32. > a 0.500 M.
33. > a 14.2
34. > e 264 mmHg.
35. > e increasing the pressure of the gas above the solvent.
36. > c density
37. > c 1.00
38. > c 0.49
39. > b 21.7
40. > c 0.15 M Ba(NO3)2
41. > d 8.56 m
42. > e molecules of A interact more strongly with B than A with A or B with B
43. > d solubility
44. > a formic acid is ASSOCIATED in benzene and MONOMERIC in water.
45. > c 2/3
46. > e 5000
47. > c. 2.77
48. > a. 11.1
49. > d. 20.00g
50. > a) 79.2 torr
51. >d) 8.0 M
52. >c) 141 torr
53. >e) decreases, increases, decreases, increases.
54. >b) the solute particles lower the solvent's vapor pressure thus requiring a higher temperature to cause
>boiling.
55. >d) 253 torr
56. >c) 9.79 M
57. >a) 2.000 M
58. >c)
59. >c) 0.0500 M
60. >e) 147 g/mol
61. >c) 0.23
62. >c) the same quantities as in (b) plus the freezing point of the pure solvent.
63. >c) 0.668 atm
64. >c) Xpentane = 0.59
65. >c) 0.51
66. > b. 2.40.
67. > c. 4.11
68. > a. 13.7%
69. > d. 0.030 moles calcium sulfate, CaSO4 (insoluble salt)
70. > c. 1.22 M
71. > c. 17.8 M
72. > a. 478 mm Hg
73. > e. -19.4°C
74. > e. 142°C
75. > d. NH4NO3 < LiCl < C6H12O6
76. > b. pressure that must be applied to a solution in order to prevent osmosis from the pure solvent.
77. > d. molar mass
78. > a. entropy
79. > a. 2.2 × 104 g/mol
80. > b. hypotonic; into
81. > a. shrink; water would flow out of the "egg"
82. > a. dispersed; continuous
83. > d. filtered black coffee
84. > c. coats and stabilizes particles of a dispersed phase.
85. > b. a hydrophilic portion and a hydrophobic portion.
86. > e. soap
87. > b. IV-II-VI-V-I-III DIF
88. > b. trihalomethanes, also called THMs
89. > e. Na+