Question 1

Coulomb's law states that the interaction energy between ions depends ________

Accepted Answer

A) only on the ionic charges. 
B) only on the distance between the ions. 
C) directly on both the ionic charges and the distance between the ions. 
D) on the temperature. 
E) directly on the ionic charges and inversely on the distance between the ions. 
A) only on the ionic charges. 
B) only on the distance between the ions. 
C) directly on both the ionic charges and the distance between the ions. 
D) on the temperature. 
E) directly on the ionic charges and inversely on the distance between the ions.

Question 2

Rank the following ionic compounds based on their expected solubility. Provide a brief rationale for your rankings.
MgF2, KCl, and Al2S3

Accepted Answer

Al₂S₃ F1F1F1S1F1F1F10 MgF₂ F1F1F1S1F1F1F1

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

The answer of A solution is prepared by adding 0.250...

Question 4

Which graph best describes how the vapor pressure of a substance varies with temperature according to the Clausius-Clapeyron equation? ln(P) is plotted on the y-axis, and 1/T is plotted on the x-axis. The origin (0, 0) is not necessarily located where the axes cross.

Accepted Answer

A) I 
B) II 
C) III 
D) IV 
A) I 
B) II 
C) III 
D) IV

Question 5

What is the molarity of a 0.923 m NaF (41.99 g/mol) solution prepared using 234 g of water? The density of the solution is 1.13 g/mL.

Accepted Answer

A) 0.654 M 
B) 0.923 M 
C) 1.00 M 
D) 1.04 M 
E) 3.94 M 
A) 0.654 M 
B) 0.923 M 
C) 1.00 M 
D) 1.04 M 
E) 3.94 M

Question 6

In the following Born-Haber cycle for the formation of sodium chloride from its elements, which step (A-E) corresponds to the lattice energy for NaCl?

Accepted Answer

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

Question 7

A newspaper article suggested using a fertilizer such as ammonium sulfate or ammonium nitrate to lower the melting point of ice on sidewalks because many of the deicing salts can damage lawns and sidewalks. Which of the following compounds would give the largest freezing point depression when 100 g of the compound are dissolved in 1 kg of solvent?

Accepted Answer

A) NH4NO3 (80.1 g/mol) 
B) (NH4)2SO4 (132.1 g/mol) 
C) MgSO4 (120.4 g/mol) 
D) CaCl2 (111.0 g/mol) 
E) MgCl2 (95.2 g/mol) 
A) NH4NO3 (80.1 g/mol) 
B) (NH4)2SO4 (132.1 g/mol) 
C) MgSO4 (120.4 g/mol) 
D) CaCl2 (111.0 g/mol) 
E) MgCl2 (95.2 g/mol)

Question 8

In the following Born-Haber cycle for the formation of sodium chloride from its elements, which step (A-E) corresponds to the electron affinity of one of the intermediate species?

Accepted Answer

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

Question 9

A solution is prepared by adding 1.50 mol glucose, which is not volatile, to 3.50 mol diethyl ether. What is the vapor pressure of this solution at 25F1F1F1S1F1F1F10C given that the vapor pressure of pure diethyl ether is 23.8 torr?

Accepted Answer

A) 7.00 torr 
B) 16.7 torr 
C) 10.2 torr 
D) 7.14 torr 
E) 34.0 torr 
A) 7.00 torr 
B) 16.7 torr 
C) 10.2 torr 
D) 7.14 torr 
E) 34.0 torr

Question 10

What would be the boiling point of a 0.52 m solution of KBr in water (Kb F1F1F1S1F1F1F10 0.52F1F1F1S1F1F1F10C)?

Accepted Answer

A) 99.7F1F1F1S1F1F1F10C 
B) 100.0F1F1F1S1F1F1F10C 
C) 100.3F1F1F1S1F1F1F10C 
D) 100.5F1F1F1S1F1F1F10C 
E) 101.1F1F1F1S1F1F1F10C 
A) 99.7F1F1F1S1F1F1F10C 
B) 100.0F1F1F1S1F1F1F10C 
C) 100.3F1F1F1S1F1F1F10C 
D) 100.5F1F1F1S1F1F1F10C 
E) 101.1F1F1F1S1F1F1F10C

Question 11

Calculate the lattice energy of magnesium chloride from the following data: First ionization energy of Mg: 738 kJ/mol
Second ionization energy of Mg: 1,451 kJ/mol
Electron affinity of Cl: F1F1F1S1F1F1F10349 kJ/mol
Energy to vaporize Mg: 147.1 kJ/mol
Cl2 bond energy: 243 kJ/mol
Energy change for the reaction:

Accepted Answer

A) 1,246 kJ/mol 
B) (F1F1F1S1F1F1F10779 kJ/mol) 
C) (F1F1F1S1F1F1F102,492 kJ/mol) 
D) 2,492 kJ/mol 
E) (F1F1F1S1F1F1F101,246 kJ/mol) 
A) 1,246 kJ/mol 
B) (F1F1F1S1F1F1F10779 kJ/mol) 
C) (F1F1F1S1F1F1F102,492 kJ/mol) 
D) 2,492 kJ/mol 
E) (F1F1F1S1F1F1F101,246 kJ/mol)

Question 12

Which of the following ionic compounds would you predict to have the lowest solubility in water?

Accepted Answer

A) MgF2 
B) MgCl2 
C) CaBr2 
D) SrI2 
E) BaI2 
A) MgF2 
B) MgCl2 
C) CaBr2 
D) SrI2 
E) BaI2

Question 13

What would be the freezing point of a 1 m solution of HCl in water (Kf F1F1F1S1F1F1F10 1.86F1F1F1S1F1F1F10C)?

Accepted Answer

A) 0.0F1F1F1S1F1F1F10C 
B) (F1F1F1S1F1F1F101.86F1F1F1S1F1F1F10
C)  
C) (F1F1F1S1F1F1F103.72F1F1F1S1F1F1F10
C)  
D) 1.86F1F1F1S1F1F1F10C 
E) (F1F1F1S1F1F1F100.93F1F1F1S1F1F1F10
C)  
A) 0.0F1F1F1S1F1F1F10C 
B) (F1F1F1S1F1F1F101.86F1F1F1S1F1F1F10
C)  
C) (F1F1F1S1F1F1F103.72F1F1F1S1F1F1F10
C)  
D) 1.86F1F1F1S1F1F1F10C 
E) (F1F1F1S1F1F1F100.93F1F1F1S1F1F1F10
C)

Question 14

Click, Clack, and Jim have identical icy driveways. Click buys 10 lb of NaCl, Clack buys 10 lb of CaCl2, and Jim buys 10 lb of MgCl2. They spread these salts on their driveways. Which driveway will deice more effectively? (Assume that ideal dissociation of the salts occurs, and that colligative properties are the only consideration.)

Accepted Answer

A) Click's driveway will deice best. 
B) Clack's driveway will deice best. 
C) Jim's driveway will deice best. 
D) The three driveways will deice to the same extent. 
E) Clack and Jim's driveways will deice better than Click's. 
A) Click's driveway will deice best. 
B) Clack's driveway will deice best. 
C) Jim's driveway will deice best. 
D) The three driveways will deice to the same extent. 
E) Clack and Jim's driveways will deice better than Click's.

Question 15

Which one of the ionic compounds below would you expect to have the largest (most 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

Question 16

A solution of 5.00 g of sodium chloride in 1.00 kg of water has a freezing point of F1F1F1S1F1F1F100.299F1F1F1S1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) 1.88 
B) 1.98 
C) 1.93 
D) 1.83 
E) 1.94 
A) 1.88 
B) 1.98 
C) 1.93 
D) 1.83 
E) 1.94

Question 17

You are working as an intern in a biochemistry lab. Your advisor just isolated an enzyme and asks you to determine its molar mass using osmosis. You dissolve 1.0 g of the enzyme in water to make 250 mL of solution. You measure the osmotic pressure and find it to be 3.5 torr at 298 K. You report that the molar mass is ________ g/mol.

Accepted Answer

A) between 0 and 1,000 
B) between 1,000 and 5,000 
C) between 5,000 and 10,000 
D) between 10,000 and 20,000 
E) between 20,000 and 50,000 
A) between 0 and 1,000 
B) between 1,000 and 5,000 
C) between 5,000 and 10,000 
D) between 10,000 and 20,000 
E) between 20,000 and 50,000

Question 18

Determine the molal concentration of a sugar solution in water that has a freezing point of F1F1F1S1F1F1F102.1F1F1F1S1F1F1F10C. Kf F1F1F1S1F1F1F10 1.86F1F1F1S1F1F1F10C/m for water.

Accepted Answer

A) 1.13 m 
B) (F1F1F1S1F1F1F101.13 m) 
C) 3.91 m 
D) (F1F1F1S1F1F1F103.91 m) 
E) 0.113 m 
A) 1.13 m 
B) (F1F1F1S1F1F1F101.13 m) 
C) 3.91 m 
D) (F1F1F1S1F1F1F103.91 m) 
E) 0.113 m

Question 19

Which statement about how the vapor pressure (P) of a liquid depends on temperature is correct?

Accepted Answer

A) The larger the enthalpy of vaporization, the smaller the change in vapor pressure for a given change in temperature. 
B) A graph of P versus 1/T is linear with a slope F1F1F1S1F1F1F10Hvap /R. 
C) The smaller the intermolecular interactions, the greater the change in vapor pressure for a given change in temperature. 
D) A graph of ln(P) versus T is linear with a slope F1F1F1S1F1F1F10Hvap /R. 
E) A graph of ln(P) versus 1/T is linear with a slope F1F1F1S1F1F1F10Hvap /R. 
A) The larger the enthalpy of vaporization, the smaller the change in vapor pressure for a given change in temperature. 
B) A graph of P versus 1/T is linear with a slope F1F1F1S1F1F1F10Hvap /R. 
C) The smaller the intermolecular interactions, the greater the change in vapor pressure for a given change in temperature. 
D) A graph of ln(P) versus T is linear with a slope F1F1F1S1F1F1F10Hvap /R. 
E) A graph of ln(P) versus 1/T is linear with a slope F1F1F1S1F1F1F10Hvap /R.

Question 20

Describe how the data obtained by a measurement of osmotic pressure can be used to determine the molar mass of a compound.

Accepted Answer

The concentration (molarity) of particle

Coulomb's law states that the interaction energy between ions depends ________

Rank the following ionic compounds based on their expected solubility. Provide a brief rationale for your rankings. MgF₂, KCl, and Al₂S₃

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 graph best describes how the vapor pressure of a substance varies with temperature according to the Clausius-Clapeyron equation? ln(P) is plotted on the y-axis, and 1/T is plotted on the x-axis. The origin (0, 0) is not necessarily located where the axes cross.

What is the molarity of a 0.923 m NaF (41.99 g/mol) solution prepared using 234 g of water? The density of the solution is 1.13 g/mL.

In the following Born-Haber cycle for the formation of sodium chloride from its elements, which step (A-E) corresponds to the lattice energy for NaCl?

In the following Born-Haber cycle for the formation of sodium chloride from its elements, which step (A-E) corresponds to the electron affinity of one of the intermediate species?

A solution is prepared by adding 1.50 mol glucose, which is not volatile, to 3.50 mol diethyl ether. What is the vapor pressure of this solution at 25C given that the vapor pressure of pure diethyl ether is 23.8 torr?

What would be the boiling point of a 0.52 m solution of KBr in water (K_b 0.52C)?

Calculate the lattice energy of magnesium chloride from the following data: First ionization energy of Mg: 738 kJ/mol Second ionization energy of Mg: 1,451 kJ/mol Electron affinity of Cl: 349 kJ/mol Energy to vaporize Mg: 147.1 kJ/mol Cl₂ bond energy: 243 kJ/mol Energy change for the reaction:

Which of the following ionic compounds would you predict to have the lowest solubility in water?

What would be the freezing point of a 1 m solution of HCl in water (K_f 1.86C)?

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

A solution of 5.00 g of sodium chloride in 1.00 kg of water has a freezing point of 0.299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

Determine the molal concentration of a sugar solution in water that has a freezing point of 2.1C. K_f  1.86C/m for water.

Which statement about how the vapor pressure (P) of a liquid depends on temperature is correct?

Describe how the data obtained by a measurement of osmotic pressure can be used to determine the molar mass of a compound.

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

Exam 11: Solutions: Properties and Behavior

Coulomb's law states that the interaction energy between ions depends ________

Rank the following ionic compounds based on their expected solubility. Provide a brief rationale for your rankings. MgF2, KCl, and Al2S3

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 graph best describes how the vapor pressure of a substance varies with temperature according to the Clausius-Clapeyron equation? ln(P) is plotted on the y-axis, and 1/T is plotted on the x-axis. The origin (0, 0) is not necessarily located where the axes cross.

What is the molarity of a 0.923 m NaF (41.99 g/mol) solution prepared using 234 g of water? The density of the solution is 1.13 g/mL.

In the following Born-Haber cycle for the formation of sodium chloride from its elements, which step (A-E) corresponds to the lattice energy for NaCl?

In the following Born-Haber cycle for the formation of sodium chloride from its elements, which step (A-E) corresponds to the electron affinity of one of the intermediate species?

A solution is prepared by adding 1.50 mol glucose, which is not volatile, to 3.50 mol diethyl ether. What is the vapor pressure of this solution at 25C given that the vapor pressure of pure diethyl ether is 23.8 torr?

What would be the boiling point of a 0.52 m solution of KBr in water (Kb  0.52C)?

Calculate the lattice energy of magnesium chloride from the following data: First ionization energy of Mg: 738 kJ/mol Second ionization energy of Mg: 1,451 kJ/mol Electron affinity of Cl: 349 kJ/mol Energy to vaporize Mg: 147.1 kJ/mol Cl2 bond energy: 243 kJ/mol Energy change for the reaction:

Which of the following ionic compounds would you predict to have the lowest solubility in water?

What would be the freezing point of a 1 m solution of HCl in water (Kf  1.86C)?

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

A solution of 5.00 g of sodium chloride in 1.00 kg of water has a freezing point of 0.299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

Determine the molal concentration of a sugar solution in water that has a freezing point of 2.1C. Kf  1.86C/m for water.

Which statement about how the vapor pressure (P) of a liquid depends on temperature is correct?

Describe how the data obtained by a measurement of osmotic pressure can be used to determine the molar mass of a compound.

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

Rank the following ionic compounds based on their expected solubility. Provide a brief rationale for your rankings. MgF₂, KCl, and Al₂S₃

What would be the boiling point of a 0.52 m solution of KBr in water (K_b 0.52C)?

Calculate the lattice energy of magnesium chloride from the following data: First ionization energy of Mg: 738 kJ/mol Second ionization energy of Mg: 1,451 kJ/mol Electron affinity of Cl: 349 kJ/mol Energy to vaporize Mg: 147.1 kJ/mol Cl₂ bond energy: 243 kJ/mol Energy change for the reaction:

What would be the freezing point of a 1 m solution of HCl in water (K_f 1.86C)?

A solution of 5.00 g of sodium chloride in 1.00 kg of water has a freezing point of 0.299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

Determine the molal concentration of a sugar solution in water that has a freezing point of 2.1C. K_f  1.86C/m for water.