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.
4) 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) ionized.
B) homogenized.
C) hybridized.
D) hydrated.
5) Which cation in each set is expected to have the larger (more negative) hydration energy?
I. Li+ or Na+
II. Rb+ or Cu2+
A) Li+ in set I and Rb+ in set II
B) Li+ in set I and Cu2+ in set II
C) Na+ in set I and Rb+ in set II
D) Na+ in set I and Cu2+ in set II
6) Which cation in each set would be expected to have the larger (more negative) hydration energy?
I. Cu+or Cu2+
II. Li+ or NH4+
A) Cu+ in set I and Li+ in set II
B) Cu+ in set I and NH4+ in set II
C) Cu2+ in set I and Li+ in set II
D) Cu2+ in set I and NH4+ in set II
7) Arrange the following compounds in order of their expected increasing solubility in water:
NaF, CH3CH2-O-CH2CH3, CH3CH2CH2CH2-OH, CH3CH2CH2CH3.
A) CH3CH2CH2CH3 < NaF < CH3CH2–O-CH2CH3 < CH3CH2CH2CH2–OH
B) NaCl < CH3CH2-O-CH2CH3 < CH3CH2CH2CH2-OH < CH3CH2CH2CH3
C) CH3CH2CH2CH3 < CH3CH2-O-CH2CH3 < NaF < CH3CH2CH2CH2–OH
D) CH3CH2CH2CH3 < CH3CH2-O-CH2CH3 < CH3CH2CH2CH2-OH < NaF
8) What are the major solute-solvent interactions created when LiF dissolves in water?
A) dipole-ion
B) dispersion
C) hydrogen bonding
D) ion-dipole
9) What are the major solute-solvent interactions created when HOCH2CH2OH dissolves in water?
A) dipole-dipole
B) dispersion
C) hydrogen bonding
D) ion-dipole
10) 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:
A) Fe2(SO4)3 > Li2SO4 > KBr > LiCl
B) Fe2(SO4)3 > Li2SO4 > LiCl > KBr
C) KBr > LiCl > Li2SO4 > Fe2(SO4)3
D) LiCl > KBr > Li2SO4 > Fe2(SO4)3
11) What is the mole fraction of ethanol in a solution made by dissolving 7.30 g of ethanol, C2H5OH, in
53.6 g of water?
A) 0.0505
B) 0.0531
C) 0.120
D) 0.136
12) What is the mole fraction of I2 in a solution made by dissolving 139 g of I2 in 245 g of hexane, C6H14?
A) 0.161
B) 0.193
C) 0.278
D) 0.385
13) What is the mole fraction of oxygen in a gas mixture that is 27% oxygen and 73% nitrogen by volume?
A) 0.24
B) 0.27
C) 0.32
D) 0.37
14) 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%
15) What is the weight percent of a caffeine solution made by dissolving 4.35 g of caffeine, C8H10N4O2,
in 75 g of benzene, C6H6?
A) 0.055%
B) 0.058%
C) 5.5%
D) 5.8%
16) What volume of a 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
17) What volume of 3.00 M CH3OH solution is needed to provide 0.320 mol of CH3OH?
A) 1.04 mL
B) 9.38 mL
C) 107 mL
D) 960 mL
18) How much water must be added to 36.0 g of CaCl2 to produce a solution that is 35.0 wt% CaCl2?
A) 48.6 g
B) 66.9 g
C) 97.2 g
D) 103 g
19) To make a 0.125 M solution, one could take 0.125 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.
20) To make a 0.125 m solution, one could take 0.125 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.
21) What molality of pentane is obtained by dissolving 25 g pentane, C5H12, in 245.0 g hexane, C6H14?
A) 0.093 m
B) 0.11 m
C) 1.4 m
D) 100 m
22) A solution is 2.25% by weight NaHCO3. How many grams of NaHCO3 are in 250.0 g of solution?
A) 0.900 g
B) 5.62 g
C) 117 g
D) 225 g
23) How many grams of KBr are required to make 250. mL of a 0.115 M KBr solution?
A) 0.242 g
B) 2.17 g
C) 3.42 g
D) 28.8 g
24) What is the molality of a glucose solution prepared by dissolving 27.0 g of glucose, C6H12O6, in 125.9
g of water?
A) 1.19 × 10-3 m
B) 0.214 m
C) 0.981 m
D) 1.19 m
25) A solution of LiCl in water has XLiCl = 0.0800. What is the molality?
A) 4.01 m LiCl
B) 4.44 m LiCl
C) 4.83 m LiCl
D) 8.70 m LiCl
26) A solution of LiCl in water is 22.0 wt% LiCl. What is the mole fraction of LiCl?
A) 0.107
B) 0.120
C) 0.519
D) 4.33
27) 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) 1408 ppm
C) 550 ppm
D) 818 ppm
28) 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
29) The dose of amoxicillin given to a young child is 40.0 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 30.0 pounds?
A) 3.00 mL
B) 6.82 mL
C) 16.0 mL
D) 9.9 mL
30) Molarity is defined as moles of solute per
A) kilogram of solvent.
B) liter of solution.
C) mole of solute.
D) total moles present.
31) Molality is defined as moles of solute per
A) kilogram of solvent.
B) liter of solvent.
C) mole of solvent.
D) total moles present.
32) Which concentration becomes smaller as the temperature is increased from 25°C to 60°C?
A) mass %
B) molality
C) molarity
D) mole fraction
33) What is the molality of ethanol in a solution made by dissolving 7.30 g of ethanol, C2H5OH, in 53.6 g
of water?
A) 0.00550 m
B) 0.500 m
C) 2.96 m
D) 400 m
34) A 1.40 M solution of CaCl2 in water has a density of 1.11 g/mL. What is the molality?
A) 1.90 m CaCl2
B) 2.30 m CaCl2
C) 1.47 m CaCl2
D) 1.44 m CaCl2
35) Calculate the molality of a solution with 53 grams of KCl in 2000 mL of water. (density of water is 1.00
g/mL).
A) 0.027
B) 0.27
C) 0.00071
D) 0.0027
36) 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 0.4 atm.
B) The total pressure is 3 atm and the partial pressure of CO2 is 0.6 atm.
C) The total pressure is 1 atm and the partial pressure of CO2 is 0.3 atm.
D) The total pressure is 1 atm and the partial pressure of CO2 is 0.5 atm.
37) 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 290. mm Hg?
A) 0.0607 mol/L
B) 0.382 mol/L
C) 0.417 mol/L
D) 46.1 mol/L
38) A saturated solution is defined as
A) a concentrated solution.
B) a solution that is in equilibrium with pure solute.
C) a solution than is in equilibrium with undissolved solute.
D) a solution that is not in equilibrium with both pure solvent and undissolved solute.
39) Which of the following does not affect the solubility of a solute in a given solvent?
A) hydrogen bonding of the solute
B) nonpolarity of the solvent
C) rate of stirring
D) temperature of the solvent and solute
40) In which case should CO2(g) be more soluble in water?
A) The total pressure is 6 atm and the partial pressure of CO2 is 1 atm.
B) The total pressure is 4 atm and the partial pressure of CO2 is 3 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 0.4 atm.
41) A solution is prepared by dissolving 50.0 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) 0.247 mm Hg
B) 19.8 mm Hg
C) 23.5 mm Hg
D) 24.0 mm Hg
42) A KCl solution is prepared by dissolving 25.0 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) 21.6 mm Hg
B) 22.7 mm Hg
C) 23.2 mm Hg
D) 24.9 mm Hg
43) 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 =
0.520.
A) 95.2 mm Hg
B) 121 mm Hg
C) 124 mm Hg
D) 242 mm Hg
44) If one mole of each is dissolved in 1.00 L of water, which will lower the vapor pressure the most?
A) C12H22O11
B) KNO3
C) C3H7OH
D) MgCl2
45) Which of the following solutions will have the lowest freezing point?
A) 0.010 m Rb I
B) 0.010 m K2SeO4
C) 0.035 m CH3OH
D) 0.015 m SrBr2
46) What is the expected freezing point of a 0.50 m solution of K2SO4 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
47) Calculate the freezing point of a solution of 30.0 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) -1.56°C
B) 1.56°C
C) 3.93°C
D) 7.06°C
48) What is the freezing point of a solution of 2.86 g MgCl2 in 100 g of water? Kf for water is 1.86°C/m.
A) -0.0558°C
B) -0.558°C
C) -1.12°C
D) -1.67°C
49) An aqueous solution has a normal boiling point of 102.5°C. What is the freezing point of this solution?
For water Kb = 0.51°C/m and Kf = 1.86°C/m.
A) -0.69°C
B) -2.5°C
C) -3.6°C
D) -9.1°C
50) 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) paradichlorobenzene, Kf = 7.10.
B) tert-butanol, Kf = 9.1.
C) water, Kf = 1.86.
D) All are expected to have the same freezing point.
51) A 0.50 m solution of which solute has the largest van’t Hoff factor?
A) CaF2
B) Li3PO4
C) K2CO3
D) NaNO3
52) A 0.020 m aqueous solution containing which solute will have the lowest freezing point?
A) LiCl
B) NaF
C) KCl
D) All will have approximately the same freezing point.
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53) A 0.35 m aqueous solution of an unknown solute has a boiling point elevation of 0.79°C. The boiling
point elevation of a 0.35 m solution of a nonionizing molecular solute in water is 0.33°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
54) Chloroform has a boiling point of 61.1°C and dichloromethane has a boiling point of 40.0°C. When
0.250 mol of dichloromethane is added to 0.750 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.
55) Which of the following pairs of solutions have roughly the same boiling point elevation?
A) 0.100 m C6H12O6 and 0.0333 m CuF2
B) 0.100 m KF and 0.100 m C6H12O6
C) 0.200 m KCl and 0.300 m Li2SO4
D) 0.100 m LiBr and 0.0500 m MgBr2
56) Calculate the freezing point of a solution when 370 grams of Ca3(PO4) is added to 3000mL of water.
(density of water is 1.00 g/mL). The Kf for water is 1.86°C/m and normal freezing point of water is 0.00°C.
A) -0.74
B) -0.0030
C) -3.70
D) -1.27
57) A solution is made by dissolving 19.5 g of sucrose, C12H22O11, in 117 g of water, producing a
55
solution with a volume of 125 mL at 20°C. What is the expected osmotic pressure at 20°C?
A) 11.0 atm
B) 23.2 atm
C) 50.0 atm
D) 58 atm
1) In a solution that is 75% ethyl alcohol and 25% water, the solute is ________ and the solvent is
________.
2) According to the rule of thumb “like dissolves like” ionic solids like LiF or polar substances like glucose
are more soluble in ________ solvents, whereas nonpolar substances like I2 are more soluble in ________
solvents.
3) When KI is dissolved in water, the major forces overcome are ________ forces in the solute and
________ forces in the solvent, and the major forces created between solute and solvent particles are
________ forces.
4) A person is considered legally intoxicated with a blood alcohol level of 80 mg/dL. Assuming that blood
plasma has a density of 1.025 g/mL, what is this concentration expressed in parts per million?
5) Amphetamines in urine can be confirmed by mass spectroscopy at a concentration of 500 ng/mL.
Assuming a urine density of 1.025 g/mL, what is this concentration in parts per million?
6) Molarity is defined as ________, whereas molality is defined as ________.
7) The number of moles of ions in 35.0mL of 4.00 M Na2SO4 is ________ moles.
8) The volume of 0.200 M H2SO4 that contains 5.00 mmol of H+ is ________ mL.
9) Cocaine, C17H21NO4, in urine can be confirmed by mass spectroscopy at a concentration of 150
ng/mL. Assuming a urine density of 1.025 g/mL, what is this concentration expressed as molality?
10) Concentrations of fluoride in drinking water greater than 4.0 mg/L can cause mottled teeth in
children. What is 4.0 mg/L expressed as molality?
11) The solubility of a gas in a liquid is greatest at ________ pressures and ________ temperatures.
12) Dinitrogen monoxide is still used as a general anesthetic. The Henry’s law constant for the solubility
of N2O in water is 2.5 × 10-2 mol/L·atm. What is the molar solubility of N2O in water if the partial
pressure of N2O is 1700 mm Hg?
13) At 20°C and 0.28 atm pressure Xenon has a solubility in water of 1.4 mmol/L. What is the Henry’s
Law-constant in mol/ L·atm at 20°C?
14) Freezing point depression, boiling point elevation, vapor pressure lowering, and osmotic pressure are
examples of ________ properties, which depend on the amount but not the chemical identity of dissolved
particles.
15) When solute is added to water, the solution has a ________ freezing point than that of pure ice at 0˚C.
16) ________ properties depend only on the identity of the solute and on the number of solute particles
present.
17) At 80.0°C heptane, C7H16, has a vapor pressure of 428 mm Hg and octane, C8H18, has a vapor
pressure of 175 mm Hg. What is the vapor pressure of a solution that contains 20.0 g C7H16 and 11.4 g
C8H18?
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18) At 80.0°C benzene has a vapor pressure of 96.0 mm Hg and toluene has a vapor pressure of 30.3 mm
Hg. If a mixture of benzene and toluene has a vapor pressure of 54.6 mm Hg, what are the mole fractions
of benzene and toluene?
19) If dissociation of MgCl2 in water were 100%, the van’t Hoff factor would be ________; however, for
real solutions the van‘t Hoff factor for MgCl2 is ________ (greater than, less than) this value.
20) The vapor pressure of water at 25°C is 23.8 mm Hg. The vapor pressure lowering, ΔP, of an aqueous
solution containing 0.500 mole fraction NaCl is ________ (equal to, greater than, less than) 11.9 mm Hg?
21) At 25°C the vapor pressures of benzene and toluene are 96.0 mm Hg and 30.5 mm Hg, respectively.
The vapor pressure of a solution that has a 0.50 mole fraction of toluene will have a vapor pressure
________ (equal to, greater than, less than) 30.5 mm Hg.
22) The boiling point of a solution containing a nonvolatile solute will be ________ than the boiling point
of the pure solvent, whereas the boiling point of a solution of two volatile liquids will be ________ than
the boiling point of the more volatile liquid and ________ than the boiling point of the less volatile liquid.
23) A 1.0 m aqueous BaI2 solution will have a ________ vapor pressure, ________ freezing point, and
________ boiling point than a 1.0 m aqueous solution of LiI.
24) The osmotic pressure of a 0.10 M solution of sucrose, C12H22O11 will be ________ (equal to, greater
than, less than) the osmotic pressure of a 0.10 M solution of fructose, C6H12O6.
25) The osmotic pressure of a 100-mL solution containing 1.0 g of sucrose, C12H22O11 will be ________
(equal to, greater than, less than) the osmotic pressure of a 100-mL solution containing 1.0 g of fructose,
C6H12O6.
26) At 300 K a 500.0 mL solution containing 0.4314 g of dextrose has an osmotic pressure of 89.6 mm Hg.
What is the molar mass of dextrose?
27) At 25°C the vapor pressures of benzene and toluene are 96.0 mm Hg and 30.5 mm Hg, respectively.
When a 1:1 molar mixture of benzene and toluene is fractionally distilled, the first fraction will have a
mole fraction of benzene that is ________ (equal to, greater than, less than) 0.50.