Question 1

What physical property is used to separate the hydrocarbon components in petroleum (crude oil)?

Accepted Answer

A) melting point 
B) density 
C) boiling point 
D) molar mass 
E) viscosity 
A) melting point 
B) density 
C) boiling point 
D) molar mass 
E) viscosity C

Question 2

Which of the following aqueous solutions will have the lowest freezing point?

Accepted Answer

A) 0.1 m magnesium sulfate, MgSO4 
B) 0.1 m potassium chloride, KCl 
C) 0.08 m magnesium chloride, MgCl2 
D) 0.04 m sodium sulfate, Na2SO4 
E) 0.05 m sodium chloride, NaCl 
A) 0.1 m magnesium sulfate, MgSO4 
B) 0.1 m potassium chloride, KCl 
C) 0.08 m magnesium chloride, MgCl2 
D) 0.04 m sodium sulfate, Na2SO4 
E) 0.05 m sodium chloride, NaCl C

Question 3

Which one of the ionic compounds below would you expect to have the smallest (least negative) lattice energy?

Accepted Answer

A) MgO 
B) CaO 
C) SrO 
D) BaO 
E) BeO 
A) MgO 
B) CaO 
C) SrO 
D) BaO 
E) BeO D

Question 4

A solution of 5.00 g of lithium chloride in 1.00 kg of water has a freezing point of F1F1F1S1F1F1F100.410F1F1F1S1F1F1F10C. What is the actual van 't Hoff factor for this salt at this concentration? Kf (water) F1F1F1S1F1F1F10 1.86F1F1F1S1F1F1F10C/m

Accepted Answer

Question 5

Which intermolecular interactions are likely to result in the lowest 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 6

Arrange the three ionic compounds sodium chloride, magnesium chloride, and aluminum chloride in order of increasing melting point.

Accepted Answer

A) NaCl F1F1F1S1F1F1F10 MgCl2 F1F1F1S1F1F1F10 AlCl3 
B) MgCl2 F1F1F1S1F1F1F10 NaCl F1F1F1S1F1F1F10 AlCl3 
C) AlCl3 F1F1F1S1F1F1F10 MgCl2 F1F1F1S1F1F1F10 NaCl 
D) AlCl3 F1F1F1S1F1F1F10 NaCl F1F1F1S1F1F1F10 MgCl2 
E) NaCl F1F1F1S1F1F1F10 AlCl3 F1F1F1S1F1F1F10 MgCl2 
A) NaCl F1F1F1S1F1F1F10 MgCl2 F1F1F1S1F1F1F10 AlCl3 
B) MgCl2 F1F1F1S1F1F1F10 NaCl F1F1F1S1F1F1F10 AlCl3 
C) AlCl3 F1F1F1S1F1F1F10 MgCl2 F1F1F1S1F1F1F10 NaCl 
D) AlCl3 F1F1F1S1F1F1F10 NaCl F1F1F1S1F1F1F10 MgCl2 
E) NaCl F1F1F1S1F1F1F10 AlCl3 F1F1F1S1F1F1F10 MgCl2

Question 7

The arrow in the diagram below indicates the direction of solvent flow through a membrane in osmosis. Which solution, A or B, is more concentrated? Explain your reasoning.

Accepted Answer

In osmosis the solvent flows from the re

Question 8

How many moles of solute are there in a 0.155 m glucose solution prepared with 50.0 kg of water?

Accepted Answer

A) 15.5 mol 
B) 15.0 mol 
C) 0.155 mol 
D) 31.0 mol 
E) 7.75 mol 
A) 15.5 mol 
B) 15.0 mol 
C) 0.155 mol 
D) 31.0 mol 
E) 7.75 mol

Question 9

Does the temperature of the vapors in a still head increase or decrease as a fractional distillation progresses? Explain.

Accepted Answer

The temperature increases. The

Question 10

Arrange the following compounds in order of increasing attraction between their ions:
MgO, CaO, BaO.

Accepted Answer

BaO F1F1F1

Question 11

Which of the following aqueous solutions will have the highest freezing point?

Accepted Answer

A) 0.03 m potassium perchlorate, KClO4 
B) 0.05 m sodium iodide, NaI 
C) 0.03 m calcium nitrate, Ca(NO3)2 
D) 0.02 m lithium phosphate, Li3PO4 
E) 0.05 m magnesium sulfate, MgSO4 
A) 0.03 m potassium perchlorate, KClO4 
B) 0.05 m sodium iodide, NaI 
C) 0.03 m calcium nitrate, Ca(NO3)2 
D) 0.02 m lithium phosphate, Li3PO4 
E) 0.05 m magnesium sulfate, MgSO4

Question 12

Which of the following must be true if the dissolution of an ionic solid in water is endothermic?

Accepted Answer

A) The change in enthalpy for this process is negative. 
B) The process releases energy. 
C) The hydration energy exceeds the lattice energy. 
D) The ions have charges greater than 1 unit. 
E) The solubility will increase with increasing temperature. 
A) The change in enthalpy for this process is negative. 
B) The process releases energy. 
C) The hydration energy exceeds the lattice energy. 
D) The ions have charges greater than 1 unit. 
E) The solubility will increase with increasing temperature.

Question 13

Which statement regarding the fractional distillation of two substances is not correct?

Accepted Answer

A) The substance with the lower boiling point has a higher concentration in the vapor than in the liquid. 
B) The boiling point of the mixture is not constant, changing as the distillation progresses. 
C) The substance with the higher vapor pressure has a higher concentration in the vapor than in the liquid. 
D) The mole ratio of the two substances in the vapor is not the same as it is in the liquid. 
E) When the vapor at any stage of the distillation is condensed, the resulting distillate has the same composition as the original mixture of the two substances. 
A) The substance with the lower boiling point has a higher concentration in the vapor than in the liquid. 
B) The boiling point of the mixture is not constant, changing as the distillation progresses. 
C) The substance with the higher vapor pressure has a higher concentration in the vapor than in the liquid. 
D) The mole ratio of the two substances in the vapor is not the same as it is in the liquid. 
E) When the vapor at any stage of the distillation is condensed, the resulting distillate has the same composition as the original mixture of the two substances.

Question 14

Which one of the ionic compounds below would you expect to have the largest (most negative) lattice energy?

Accepted Answer

A) MgF2 
B) MgCl2 
C) MgBr2 
D) MgI2 
E) CaI2 
A) MgF2 
B) MgCl2 
C) MgBr2 
D) MgI2 
E) CaI2

Question 15

Which statement is not correct? Determination of molar mass of an unknown sample by an osmotic pressure measurement requires that ________

Accepted Answer

A) the solute dissolved in the solution is pure. 
B) the solute is a nonelectrolyte. 
C) the molecules of the solute do not pass through the semipermeable membrane. 
D) the mass of the solute dissolved in the solution is known in advance. 
E) the molar concentration of the solute in the solution is known in advance. 
A) the solute dissolved in the solution is pure. 
B) the solute is a nonelectrolyte. 
C) the molecules of the solute do not pass through the semipermeable membrane. 
D) the mass of the solute dissolved in the solution is known in advance. 
E) the molar concentration of the solute in the solution is known in advance.

Question 16

Considering that ideal behavior is not always found in nature, which of the following aqueous solutions would you expect to have the largest van 't Hoff factor?

Accepted Answer

A) 0.100 m C12H22O11 (sucrose) 
B) 0.100 m (NH4)2SO4 
C) 0.001 m (NH4)2SO4 
D) 0.100 m NH4Cl 
E) 0.001 m NH4Cl 
A) 0.100 m C12H22O11 (sucrose) 
B) 0.100 m (NH4)2SO4 
C) 0.001 m (NH4)2SO4 
D) 0.100 m NH4Cl 
E) 0.001 m NH4Cl

Question 17

Ethylene glycol is used in automobile radiators as an antifreeze. What will the freezing point of an antifreeze solution be if 2.5 L of ethylene glycol are mixed together with 2.5 L of water? The following information may be helpful to you. Ethylene glycol has a very low vapor pressure and is essentially nonvolatile. molar mass of ethylene glycol F1F1F1S1F1F1F10 62.1 g/mol
Van 't Hoff factor F1F1F1S1F1F1F10 1
Density of ethylene glycol F1F1F1S1F1F1F10 1.11 g/mL
Density of water F1F1F1S1F1F1F10 1.00 g/mL
Kf for water F1F1F1S1F1F1F10 1.86F1F1F1S1F1F1F10C kg/mol

Accepted Answer

A) (F1F1F1S1F1F1F1039F1F1F1S1F1F1F10
C)  
B) (F1F1F1S1F1F1F1016F1F1F1S1F1F1F10
C)  
C) (F1F1F1S1F1F1F101.6F1F1F1S1F1F1F10
C)  
D) (F1F1F1S1F1F1F1033F1F1F1S1F1F1F10
C)  
E) (F1F1F1S1F1F1F1024F1F1F1S1F1F1F10
C)  
A) (F1F1F1S1F1F1F1039F1F1F1S1F1F1F10
C)  
B) (F1F1F1S1F1F1F1016F1F1F1S1F1F1F10
C)  
C) (F1F1F1S1F1F1F101.6F1F1F1S1F1F1F10
C)  
D) (F1F1F1S1F1F1F1033F1F1F1S1F1F1F10
C)  
E) (F1F1F1S1F1F1F1024F1F1F1S1F1F1F10
C)

Question 18

Which statement about the vapor pressure of a liquid is not correct?

Accepted Answer

A) The vapor pressure increases with increasing temperature because more molecules have sufficient energy to overcome the attractive forces that hold them in the liquid. 
B) The vapor pressure decreases with increasing strength of intermolecular interactions. 
C) The pressure at which the rate of molecules evaporating equals the rate of molecules condensing is called the vapor pressure. 
D) Adding a nonvolatile solute to a liquid increases the vapor pressure. 
E) The enthalpy of vaporization determines how sensitive the vapor pressure of a substance is to a change in temperature. 
A) The vapor pressure increases with increasing temperature because more molecules have sufficient energy to overcome the attractive forces that hold them in the liquid. 
B) The vapor pressure decreases with increasing strength of intermolecular interactions. 
C) The pressure at which the rate of molecules evaporating equals the rate of molecules condensing is called the vapor pressure. 
D) Adding a nonvolatile solute to a liquid increases the vapor pressure. 
E) The enthalpy of vaporization determines how sensitive the vapor pressure of a substance is to a change in temperature.

Question 19

The molality of a solution is defined as ________

Accepted Answer

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) grams of solute per kilogram of solvent. 
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) grams of solute per kilogram of solvent.

Question 20

Which statement below regarding vapor pressure is not correct?

Accepted Answer

A) Vapor pressure is an intensive property. 
B) The substance with the stronger intermolecular forces has the lower vapor pressure. 
C) Vapor pressure increases with increasing temperature. 
D) Pure water has a higher vapor pressure at a given temperature than seawater. 
E) A nonvolatile solute increases the vapor pressure of the solvent. 
A) Vapor pressure is an intensive property. 
B) The substance with the stronger intermolecular forces has the lower vapor pressure. 
C) Vapor pressure increases with increasing temperature. 
D) Pure water has a higher vapor pressure at a given temperature than seawater. 
E) A nonvolatile solute increases the vapor pressure of the solvent.

Exam 11: Solutions: Properties and Behavior

What physical property is used to separate the hydrocarbon components in petroleum (crude oil)?

Which of the following aqueous solutions will have the lowest freezing point?

Which one of the ionic compounds below would you expect to have the smallest (least negative) lattice energy?

A solution of 5.00 g of lithium chloride in 1.00 kg of water has a freezing point of 0.410C. What is the actual van 't Hoff factor for this salt at this concentration? Kf (water)  1.86C/m

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

Arrange the three ionic compounds sodium chloride, magnesium chloride, and aluminum chloride in order of increasing melting point.

The arrow in the diagram below indicates the direction of solvent flow through a membrane in osmosis. Which solution, A or B, is more concentrated? Explain your reasoning.

How many moles of solute are there in a 0.155 m glucose solution prepared with 50.0 kg of water?

Does the temperature of the vapors in a still head increase or decrease as a fractional distillation progresses? Explain.

Arrange the following compounds in order of increasing attraction between their ions: MgO, CaO, BaO.

Which of the following aqueous solutions will have the highest freezing point?

Which of the following must be true if the dissolution of an ionic solid in water is endothermic?

Which statement regarding the fractional distillation of two substances is not correct?

Which one of the ionic compounds below would you expect to have the largest (most negative) lattice energy?

Which statement is not correct? Determination of molar mass of an unknown sample by an osmotic pressure measurement requires that ________

Considering that ideal behavior is not always found in nature, which of the following aqueous solutions would you expect to have the largest van 't Hoff factor?

Which statement about the vapor pressure of a liquid is not correct?

The molality of a solution is defined as ________

Which statement below regarding vapor pressure is not correct?

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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A solution of 5.00 g of lithium chloride in 1.00 kg of water has a freezing point of 0.410C. What is the actual van 't Hoff factor for this salt at this concentration? K_f(water)  1.86C/m