Question 1

The concentration unit of molality is symbolized as ________

Accepted Answer

A) M. 
B) m. 
C) M.. 
D) mol. 
E) mo. 
A) M. 
B) m. 
C) M.. 
D) mol. 
E) mo.

Question 2

What is the molality of 153 mL of a 1.10 M NaF (41.99 g/mol) solution? The density of the solution is 1.23 g/mL.

Accepted Answer

A) 0.894 m 
B) 0.929 m 
C) 1.10 m 
D) 2.34 m 
E) 5.85 m 
A) 0.894 m 
B) 0.929 m 
C) 1.10 m 
D) 2.34 m 
E) 5.85 m

Question 3

A solution is prepared by adding 0.250 mol napthalene, which is not volatile, to 2.25 mol diethyl ether. What is the vapor pressure of this solution at 25F1F1F1S1F1F1F10C given that the vapor pressure of pure diethyl ether is 532 torr?

Accepted Answer

A) 53.2 torr 
B) 59.1 torr 
C) 473 torr 
D) 479 torr 
E) 591 torr 
A) 53.2 torr 
B) 59.1 torr 
C) 473 torr 
D) 479 torr 
E) 591 torr

Question 4

Which of the following is not typically needed to calculate the lattice energy of an ionic compound?

Accepted Answer

A) enthalpy of vaporization 
B) bond enthalpy 
C) enthalpy of solution 
D) electron affinity 
E) ionization energy 
A) enthalpy of vaporization 
B) bond enthalpy 
C) enthalpy of solution 
D) electron affinity 
E) ionization energy

Question 5

Calculate the lattice energy of sodium fluoride from the following data: Ionization energy of Na: 496 kJ/mol
Electron affinity of F: F1F1F1S1F1F1F10328 kJ/mol
Energy to vaporize Na: 108 kJ/mol
F2 bond energy: 160 kJ/mol
Energy change for the reaction:

Accepted Answer

A) 931 kJ/mol 
B) (F1F1F1S1F1F1F10931 kJ/mol) 
C) (F1F1F1S1F1F1F101,011 kJ/mol) 
D) 1,011 kJ/mol 
E) (F1F1F1S1F1F1F10851 kJ/mol) 
A) 931 kJ/mol 
B) (F1F1F1S1F1F1F10931 kJ/mol) 
C) (F1F1F1S1F1F1F101,011 kJ/mol) 
D) 1,011 kJ/mol 
E) (F1F1F1S1F1F1F10851 kJ/mol)

Question 6

Which of the solutions shown here will have the highest 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

What mass of a 0.66 m ammonium nitrate (80.04 g/mol) solution will contain 0.15 mol of solute?

Accepted Answer

A) 227 g 
B) 239 g 
C) 440 g 
D) 493 g 
E) 4,453 g 
A) 227 g 
B) 239 g 
C) 440 g 
D) 493 g 
E) 4,453 g

Question 8

Isopropyl alcohol has a boiling point of 82.3F1F1F1S1F1F1F10C. Solutions of isopropyl alcohol in water have normal boiling points less than 100F1F1F1S1F1F1F10C. Is this observation consistent with the following equation? Explain.F1F1F1S1F1F1F10Tb F1F1F1S1F1F1F10 iKbm

Accepted Answer

A) No, boiling point elevation only pertains to ionic solutes. 
B) No, boiling point elevation only pertains to nonvolatile solutes. 
C) Yes, boiling point depression occurs for all solutions. 
D) Yes, the boiling point depression constant for isopropyl alcohol is large. 
E) No, isopropyl alcohol can hydrogen bond with water. 
A) No, boiling point elevation only pertains to ionic solutes. 
B) No, boiling point elevation only pertains to nonvolatile solutes. 
C) Yes, boiling point depression occurs for all solutions. 
D) Yes, the boiling point depression constant for isopropyl alcohol is large. 
E) No, isopropyl alcohol can hydrogen bond with water.

Question 9

Which of the following requires the smallest energy to separate the ions?

Accepted Answer

A) CaF2 
B) KF 
C) NaF 
D) MgF2 
E) LiF 
A) CaF2 
B) KF 
C) NaF 
D) MgF2 
E) LiF

Question 10

Which arrangement below orders the cations from smallest to largest hydration energy? Smallest to largest means least negative hydration energy to most negative hydration energy.

Accepted Answer

A) CsF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 KF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 Ca2F1F1F1S1F1F1F10 F1F1F1S1F1F1F10 Al3F1F1F1S1F1F1F10 
B) KF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 CsF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 Ca2F1F1F1S1F1F1F10 F1F1F1S1F1F1F10 Al3F1F1F1S1F1F1F10 
C) Al3F1F1F1S1F1F1F10 F1F1F1S1F1F1F10 Ca2F1F1F1S1F1F1F10 F1F1F1S1F1F1F10 KF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 CsF1F1F1S1F1F1F10 
D) Al3F1F1F1S1F1F1F10 F1F1F1S1F1F1F10 Ca2F1F1F1S1F1F1F10 F1F1F1S1F1F1F10 CsF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 KF1F1F1S1F1F1F10 
E) KF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 CsF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 Al3F1F1F1S1F1F1F10 F1F1F1S1F1F1F10 Ca2F1F1F1S1F1F1F10 
A) CsF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 KF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 Ca2F1F1F1S1F1F1F10 F1F1F1S1F1F1F10 Al3F1F1F1S1F1F1F10 
B) KF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 CsF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 Ca2F1F1F1S1F1F1F10 F1F1F1S1F1F1F10 Al3F1F1F1S1F1F1F10 
C) Al3F1F1F1S1F1F1F10 F1F1F1S1F1F1F10 Ca2F1F1F1S1F1F1F10 F1F1F1S1F1F1F10 KF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 CsF1F1F1S1F1F1F10 
D) Al3F1F1F1S1F1F1F10 F1F1F1S1F1F1F10 Ca2F1F1F1S1F1F1F10 F1F1F1S1F1F1F10 CsF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 KF1F1F1S1F1F1F10 
E) KF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 CsF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 Al3F1F1F1S1F1F1F10 F1F1F1S1F1F1F10 Ca2F1F1F1S1F1F1F10

The concentration unit of molality is symbolized as ________

What is the molality of 153 mL of a 1.10 M NaF (41.99 g/mol) solution? The density of the solution is 1.23 g/mL.

A solution is prepared by adding 0.250 mol napthalene, which is not volatile, to 2.25 mol diethyl ether. What is the vapor pressure of this solution at 25C given that the vapor pressure of pure diethyl ether is 532 torr?

Which of the following is not typically needed to calculate the lattice energy of an ionic compound?

Calculate the lattice energy of sodium fluoride from the following data: Ionization energy of Na: 496 kJ/mol Electron affinity of F: 328 kJ/mol Energy to vaporize Na: 108 kJ/mol F₂ bond energy: 160 kJ/mol Energy change for the reaction:

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

What mass of a 0.66 m ammonium nitrate (80.04 g/mol) solution will contain 0.15 mol of solute?

Isopropyl alcohol has a boiling point of 82.3C. Solutions of isopropyl alcohol in water have normal boiling points less than 100C. Is this observation consistent with the following equation? Explain.T_b  iK_bm

Which of the following requires the smallest energy to separate the ions?

Which arrangement below orders the cations from smallest to largest hydration energy? Smallest to largest means least negative hydration energy to most negative hydration energy.

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

The concentration unit of molality is symbolized as ________

What is the molality of 153 mL of a 1.10 M NaF (41.99 g/mol) solution? The density of the solution is 1.23 g/mL.

A solution is prepared by adding 0.250 mol napthalene, which is not volatile, to 2.25 mol diethyl ether. What is the vapor pressure of this solution at 25C given that the vapor pressure of pure diethyl ether is 532 torr?

Which of the following is not typically needed to calculate the lattice energy of an ionic compound?

Calculate the lattice energy of sodium fluoride from the following data: Ionization energy of Na: 496 kJ/mol Electron affinity of F: 328 kJ/mol Energy to vaporize Na: 108 kJ/mol F2 bond energy: 160 kJ/mol Energy change for the reaction:

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

What mass of a 0.66 m ammonium nitrate (80.04 g/mol) solution will contain 0.15 mol of solute?

Isopropyl alcohol has a boiling point of 82.3C. Solutions of isopropyl alcohol in water have normal boiling points less than 100C. Is this observation consistent with the following equation? Explain.Tb  iKbm

Which of the following requires the smallest energy to separate the ions?

Which arrangement below orders the cations from smallest to largest hydration energy? Smallest to largest means least negative hydration energy to most negative hydration energy.

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

Calculate the lattice energy of sodium fluoride from the following data: Ionization energy of Na: 496 kJ/mol Electron affinity of F: 328 kJ/mol Energy to vaporize Na: 108 kJ/mol F₂ bond energy: 160 kJ/mol Energy change for the reaction:

Isopropyl alcohol has a boiling point of 82.3C. Solutions of isopropyl alcohol in water have normal boiling points less than 100C. Is this observation consistent with the following equation? Explain.T_b  iK_bm