Question 1

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

Accepted Answer

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 
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

Question 2

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) F1F1F1S1F1F1F10 1.86F1F1F1S1F1F1F10C/m

Accepted Answer

A) (F1F1F1S1F1F1F1040F1F1F1S1F1F1F10
C)  
B) (F1F1F1S1F1F1F1032F1F1F1S1F1F1F10
C)  
C) (F1F1F1S1F1F1F1011F1F1F1S1F1F1F10
C)  
D) (F1F1F1S1F1F1F1025F1F1F1S1F1F1F10
C)  
E) (F1F1F1S1F1F1F1022F1F1F1S1F1F1F10
C)  
A) (F1F1F1S1F1F1F1040F1F1F1S1F1F1F10
C)  
B) (F1F1F1S1F1F1F1032F1F1F1S1F1F1F10
C)  
C) (F1F1F1S1F1F1F1011F1F1F1S1F1F1F10
C)  
D) (F1F1F1S1F1F1F1025F1F1F1S1F1F1F10
C)  
E) (F1F1F1S1F1F1F1022F1F1F1S1F1F1F10
C)

Question 3

What is the vapor pressure of an aqueous solution that has a solute mol fraction of F1F1F1S1F1F1F10 F1F1F1S1F1F1F10 0.100? The vapor pressure of water is 25.756 mm Hg at 25F1F1F1S1F1F1F10C.

Accepted Answer

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 
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

Question 4

The freezing point of a 0.0925 m solution of ammonium chloride was found to be F1F1F1S1F1F1F100.325F1F1F1S1F1F1F10C. What is the actual van't Hoff factor for this salt at this concentration compared to the ideal one of 2? Kf (water) F1F1F1S1F1F1F10 1.86F1F1F1S1F1F1F10C/m

Accepted Answer

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

Question 5

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 25F1F1F1S1F1F1F10C. 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.

Accepted Answer

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 
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

Question 6

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.

Accepted Answer

A)    
B)    
C)    
D)    
A)    
B)    
C)    
D)

Question 7

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?

Accepted Answer

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. 
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.

Question 8

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 F1F1F1S1F1F1F10 3.63F1F1F1S1F1F1F10C/m), increasing the boiling point of the chloroform by 0.726F1F1F1S1F1F1F10C. What is the molar mass of eugenol?

Accepted Answer

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

Question 9

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 F1F1F1S1F1F1F10 1.86F1F1F1S1F1F1F10C/m)?

Accepted Answer

A) (F1F1F1S1F1F1F105.99F1F1F1S1F1F1F10
C)  
B) (F1F1F1S1F1F1F101.86F1F1F1S1F1F1F10
C)  
C) (F1F1F1S1F1F1F100.372F1F1F1S1F1F1F10
C)  
D) (F1F1F1S1F1F1F101.61F1F1F1S1F1F1F10
C)  
E) (F1F1F1S1F1F1F103.23F1F1F1S1F1F1F10
C)  
A) (F1F1F1S1F1F1F105.99F1F1F1S1F1F1F10
C)  
B) (F1F1F1S1F1F1F101.86F1F1F1S1F1F1F10
C)  
C) (F1F1F1S1F1F1F100.372F1F1F1S1F1F1F10
C)  
D) (F1F1F1S1F1F1F101.61F1F1F1S1F1F1F10
C)  
E) (F1F1F1S1F1F1F103.23F1F1F1S1F1F1F10
C)

Question 10

Indicate which aqueous solution has the fastest evaporation rate.

Accepted Answer

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 
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

Question 11

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.

Accepted Answer

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

Question 12

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 20F1F1F1S1F1F1F10C. Substance
Vapor Pressure at 20F1F1F1S1F1F1F10C (torr)
Methanol
92
Ethanol
45

Accepted Answer

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

Question 13

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

Accepted Answer

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

Question 14

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

Accepted Answer

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

Question 15

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

Accepted Answer

All of these consist of 2F1F1F1S1F1F1F1

Question 16

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

Accepted Answer

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. 
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.

Question 17

Determine the molarity of an aspirin solution that produces an osmotic pressure of 0.0555 atm at 25F1F1F1S1F1F1F10C (i F1F1F1S1F1F1F10 1).

Accepted Answer

2.26 F1F1F

Question 18

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

Accepted Answer

A) CsBr F1F1F1S1F1F1F10 KBr F1F1F1S1F1F1F10 SrBr2 
B) SrBr2 F1F1F1S1F1F1F10 CsBr F1F1F1S1F1F1F10 KBr 
C) KBr F1F1F1S1F1F1F10 SrBr2 F1F1F1S1F1F1F10 CsBr 
D) CsBr F1F1F1S1F1F1F10 SrBr2 F1F1F1S1F1F1F10 KBr 
E) SrBr2 F1F1F1S1F1F1F10 KBr F1F1F1S1F1F1F10 CsBr 
A) CsBr F1F1F1S1F1F1F10 KBr F1F1F1S1F1F1F10 SrBr2 
B) SrBr2 F1F1F1S1F1F1F10 CsBr F1F1F1S1F1F1F10 KBr 
C) KBr F1F1F1S1F1F1F10 SrBr2 F1F1F1S1F1F1F10 CsBr 
D) CsBr F1F1F1S1F1F1F10 SrBr2 F1F1F1S1F1F1F10 KBr 
E) SrBr2 F1F1F1S1F1F1F10 KBr F1F1F1S1F1F1F10 CsBr

Question 19

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?

Accepted Answer

The magnitude of the charges o

Question 20

A 300 mg sample of caffeine was dissolved in 10.0 g of camphor (Kf F1F1F1S1F1F1F10 39.7F1F1F1S1F1F1F10C/m), decreasing the freezing point of camphor by 3.07F1F1F1S1F1F1F10C. What is the molar mass of caffeine?

Accepted Answer

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

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

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 25C.

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

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.

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?

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 (K_b  3.63C/m), increasing the boiling point of the chloroform by 0.726C. What is the molar mass of eugenol?

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 (K_f  1.86C/m)?

Indicate which aqueous solution has the fastest evaporation rate.

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 20C. Substance Vapor Pressure at 20C (torr) Methanol 92 Ethanol 45

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

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

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

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

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

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

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?

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

Matter and Energy: The Origin of the Universe

Atoms, Ions, and Molecules: Matter Starts Here

Stoichiometry: Mass, Formulas, and Reactions

Solution Chemistry: The Hydrosphere

Thermochemistry: Energy Changes in Reactions

Properties of Gases: The Air We Breathe

A Quantum Model of Atoms: Waves and Particles

Chemical Bonds: What Makes a Gas a Greenhouse Gas

Molecular Geometry: Shape Determines Function

Intermolecular Forces: The Uniqueness of Water

Solids: Crystals, Alloys, and Polymers

Chemical Kinetics: Reactions in the Atmosphere

Chemical Equilibrium: How Much Product Does a Reaction Really Make

Acidbase Equilibria: Proton Transfer in Biological Systems

Additional Aqueous Equilibria: Chemistry and the Oceans

Thermodynamics: Spontaneous and Nonspontaneous Reactions and Processes

Electrochemistry: The Quest for Clean Energy

Nuclear Chemistry: Applications to Energy and Medicine

Organic and Biological Molecules: the Compounds of Life

The Main Group Elements: Life and the Periodic Table

Transition Metals: Biological and Medical Applications

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Exam 11: Solutions: Properties and Behavior

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

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 25C.

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

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.

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?

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  3.63C/m), increasing the boiling point of the chloroform by 0.726C. What is the molar mass of eugenol?

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  1.86C/m)?

Indicate which aqueous solution has the fastest evaporation rate.

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 20C. Substance Vapor Pressure at 20C (torr) Methanol 92 Ethanol 45

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

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

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

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

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

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

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?

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

Matter and Energy: The Origin of the Universe

Atoms, Ions, and Molecules: Matter Starts Here

Stoichiometry: Mass, Formulas, and Reactions

Solution Chemistry: The Hydrosphere

Thermochemistry: Energy Changes in Reactions

Properties of Gases: The Air We Breathe

A Quantum Model of Atoms: Waves and Particles

Chemical Bonds: What Makes a Gas a Greenhouse Gas

Molecular Geometry: Shape Determines Function

Intermolecular Forces: The Uniqueness of Water

Solids: Crystals, Alloys, and Polymers

Chemical Kinetics: Reactions in the Atmosphere

Chemical Equilibrium: How Much Product Does a Reaction Really Make

Acidbase Equilibria: Proton Transfer in Biological Systems

Additional Aqueous Equilibria: Chemistry and the Oceans

Thermodynamics: Spontaneous and Nonspontaneous Reactions and Processes

Electrochemistry: The Quest for Clean Energy

Nuclear Chemistry: Applications to Energy and Medicine

Organic and Biological Molecules: the Compounds of Life

The Main Group Elements: Life and the Periodic Table

Transition Metals: Biological and Medical Applications

Filters

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

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 (K_b  3.63C/m), increasing the boiling point of the chloroform by 0.726C. What is the molar mass of eugenol?

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 (K_f  1.86C/m)?

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 20C. Substance Vapor Pressure at 20C (torr) Methanol 92 Ethanol 45

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

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

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