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A 300 mg sample of caffeine was dissolved in 10.0 g of camphor (Kf 39.7C/m) , decreasing the freezing point of camphor by 3.07C. What is the molar mass of caffeine?


A) 47.0 g/mol
B) 194 g/mol
C) 388 g/mol
D) 94.0 g/mol
E) 97.0 g/mol

F) A) and E)
G) C) and D)

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Rank the following compounds in order of increasing attraction between their ions: KBr, SrBr2, and CsBr.


A) CsBr KBr SrBr2
B) SrBr2 CsBr KBr
C) KBr SrBr2 CsBr
D) CsBr SrBr2 KBr
E) SrBr2 KBr CsBr

F) B) and D)
G) None of the above

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Ion interaction energies are determined by Coulomb's law given by the equation: Ion interaction energies are determined by Coulomb's law given by the equation: Based on this equation, what two factors dictate the strength of ion-ion interactions? Based on this equation, what two factors dictate the strength of ion-ion interactions?

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The magnitude of the charges o...

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Indicate which aqueous solution has the fastest evaporation rate.


A) 0.10 M CaCO3
B) 0.20 M NaNO3
C) 0.15 M KBr
D) 0.30 M Li2SO4
E) 0.10 M MgCl2

F) D) and E)
G) B) and E)

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Why would you expect or predict sodium fluoride to have the lowest solubility in water compared to the other sodium halide salts?


A) Fluoride has the largest (most negative) enthalpy of hydration of all the halide ions.
B) Fluoride has the smallest (least negative) enthalpy of hydration of all the halide ions.
C) Sodium fluoride has the largest (most negative) lattice energy of all the sodium halides.
D) Sodium fluoride has the smallest molar mass of all the sodium halides.
E) Fluoride is the most basic of all the halide ions and forms HF in aqueous solution.

F) A) and D)
G) A) and E)

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Which of the solutions shown here will have the lowest vapor pressure? White circles indicate solvent molecules; black circles indicate molecules of a nonvolatile solute.


A) Which of the solutions shown here will have the lowest vapor pressure? White circles indicate solvent molecules; black circles indicate molecules of a nonvolatile solute. A) B) C) D)
B) Which of the solutions shown here will have the lowest vapor pressure? White circles indicate solvent molecules; black circles indicate molecules of a nonvolatile solute. A) B) C) D)
C) Which of the solutions shown here will have the lowest vapor pressure? White circles indicate solvent molecules; black circles indicate molecules of a nonvolatile solute. A) B) C) D)
D) Which of the solutions shown here will have the lowest vapor pressure? White circles indicate solvent molecules; black circles indicate molecules of a nonvolatile solute. A) B) C) D)

E) All of the above
F) None of the above

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Rank the following ionic compounds in order of increasing lattice energy (largest lattice energy is the most negative): MgF2, MgCl2, MgBr2, and MgI2.

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All of these consist of 2F1F1F1...

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The freezing point of a 0.0925 m solution of ammonium chloride was found to be 0.325C. What is the actual van't Hoff factor for this salt at this concentration compared to the ideal one of 2? Kf (water) 1.86C/m


A) 1.89
B) 1.95
C) 1.90
D) 1.80
E) 1.97

F) A) and D)
G) C) and D)

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A medical company separates methanol (CH3OH) ) and ethanol (CH3CH2OH) by distillation. In one run, the starting solution was 25% methanol and 75% ethanol by mass at 25C. In the liquid, the mole ratio of methanol to ethanol was ________, and in the vapor it was ________. The vapor pressures for methanol and ethanol at this temperature are 92 torr and 45 torr, respectively.


A) 0.48; 2.0
B) 2.0; 0.48
C) 0.33; 2.0
D) 0.48; 0.33
E) 2.3; 0.55

F) B) and D)
G) None of the above

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Which of the following is a colligative property? I. osmotic pressure II. molar mass III. density IV. freezing point depression V. boiling point


A) I, II, IV, and V only
B) I and IV only
C) II and IV only
D) II, III, and V only
E) I, II, and V only

F) C) and E)
G) None of the above

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Eugenol is a nonelectrolyte that contributes to the flavor of spices such as clove, nutmeg, cinnamon, and basil. A 328 mg sample of eugenol was dissolved in 10.0 g of chloroform (Kb 3.63C/m) , increasing the boiling point of the chloroform by 0.726C. What is the molar mass of eugenol?


A) 164 g/mol
B) 328 g/mol
C) 363 g/mol
D) 182 g/mol
E) 82 g/mol

F) None of the above
G) A) and B)

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Predict which of the following ionic compounds has the highest melting point.


A) NaF
B) KCl
C) RbCl
D) BeF2
E) NaCl

F) A) and D)
G) C) and E)

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Determine the molarity of an aspirin solution that produces an osmotic pressure of 0.0555 atm at 25C (i 1).

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2.26 F1F1F...

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Magnesium chloride is often used to melt ice on sidewalks. Considering that the solubility of magnesium chloride (95.21 g/mol) in water is 54.3 g per 100.0 g of water, what is the lowest temperature that you would expect to be able to melt ice with magnesium chloride? Assume ideal behavior. Kf (water) 1.86C/m


A) (40C)
B) (32C)
C) (11C)
D) (25C)
E) (22C)

F) A) and B)
G) None of the above

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A solution is prepared by mixing 50 g of methanol (CH3OH) with 50 g of ethanol (CH3CH2OH) . Use the following data to determine the vapor pressure of this solution at 20C. Substance Vapor Pressure at 20C (torr) Methanol 92 Ethanol 45


A) 69 torr
B) 57 torr
C) 80 torr
D) 73 torr
E) 83 torr

F) B) and E)
G) C) and D)

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A solution is made by dissolving 100 g of essentially nonvolatile ethylene glycol (C2H6O2) in 500 g of water. What is the resulting freezing point of the solution (Kf 1.86C/m) ?


A) (5.99C)
B) (1.86C)
C) (0.372C)
D) (1.61C)
E) (3.23C)

F) C) and D)
G) A) and E)

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Which solution, if either, would create the higher osmotic pressure (compared to pure water) : one prepared from 1.0 g of NaCl in 10 mL of water or 1.0 g of CsBr in 10 mL of water?


A) They would have the same osmotic pressures.
B) NaCl would give the higher pressure.
C) CsBr would give the higher pressure.
D) It is impossible to tell.
E) These compounds are salts and do not produce an osmotic pressure.

F) C) and E)
G) All of the above

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In the diagram below, one beaker contains pure water and the other contains an equal volume of seawater. Seawater has various salts dissolved in it. The beakers are sitting in a totally enclosed chamber, and the outside temperature and pressure are held constant. Identify the statements below about this situation that are not correct. In the diagram below, one beaker contains pure water and the other contains an equal volume of seawater. Seawater has various salts dissolved in it. The beakers are sitting in a totally enclosed chamber, and the outside temperature and pressure are held constant. Identify the statements below about this situation that are not correct. I. Water will be transferred from the pure water beaker to the seawater beaker. II. Water will be transferred from the seawater beaker to the pure water beaker. III.The vapor pressure of the pure water is higher than the vapor pressure of the seawater. IV. Pure water evaporates at a faster rate than seawater. V. Water in the gas phase condenses into both beakers at the same rate. A) II only B) II and V C) II, IV, and V D) II, III, and IV E) I, III, and IV I. Water will be transferred from the pure water beaker to the seawater beaker. II. Water will be transferred from the seawater beaker to the pure water beaker. III.The vapor pressure of the pure water is higher than the vapor pressure of the seawater. IV. Pure water evaporates at a faster rate than seawater. V. Water in the gas phase condenses into both beakers at the same rate.


A) II only
B) II and V
C) II, IV, and V
D) II, III, and IV
E) I, III, and IV

F) A) and E)
G) B) and C)

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Which intermolecular interactions are likely to result in the highest vapor pressure of a substance?


A) dispersion interactions
B) dipole-dipole interactions
C) hydrogen bonds
D) ion-dipole interactions
E) ion-ion interactions

F) A) and E)
G) D) and E)

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What is the vapor pressure of an aqueous solution that has a solute mol fraction of 0.100? The vapor pressure of water is 25.756 mm Hg at 25C.


A) 23.2 mm Hg
B) 2.58 mm Hg
C) 25.8 mm Hg
D) 0.900 mm Hg
E) 22.3 mm Hg

F) None of the above
G) B) and D)

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