Question 1

Arrange the following solutions in order of increasing freezing point depression.

Accepted Answer

CH₃CO₂H < KC

Question 2

An aqueous solution of fructose, C6H12O6, has an osmotic pressure of 10.50 atm at 25.0°C. What is the boiling point of this solution? Kf = 1.86 °C m−1 and Kb = 0.512 °C m−1. The density of the solution is 1.077 g mL−1.Hint: You will need to convert molarity to molality before finding the boiling point elevation.

Accepted Answer

Question 3

A dilute aqueous solution of CaCl2 contains 0.159 grams of solute per liter of solution. It is fully dissociated. What is its osmotic pressure at 20.0°C?Hint: CaCl2 is an ionic compound.

Accepted Answer

A) 1.79 torr 
B) 3.49 torr 
C) 26.2 torr 
D) 78.6 torr 
E) 2.65 × 103 torr 
A) 1.79 torr 
B) 3.49 torr 
C) 26.2 torr 
D) 78.6 torr 
E) 2.65 × 103 torr

Question 4

Pure benzene, C6H6, has a freezing point of 5.45°C. Its freezing point depressionconstant is: Kf = 5.07 °C m-1. A solution was made by taking 24.20 g of an unknown nonelectrolyte and dissolving it in 125.0 g of benzene. The measured freezing point of the solution was -1.65°C. Calculate the molecular weight of the unknown substance.Hint: Find molality, then moles, then molar mass, being sure to keep track of units.

Accepted Answer

A) 138 g mol-1 
B) 145 g mol-1 
C) 258 g mol-1 
D) 272 g mol-1 
E) 595 g mol-1 
A) 138 g mol-1 
B) 145 g mol-1 
C) 258 g mol-1 
D) 272 g mol-1 
E) 595 g mol-1

Question 5

An aqueous solution of ethanol, C2H5OH, is 19.00% ethanol by mass and has a density of 0.9700 g mL-1. Calculate the molarity of the ethanol solution.

Accepted Answer

A) 4.001 M 
B) 4.124 M 
C) 4.252 M 
D) 5.092 M 
E) 14.48 M 
A) 4.001 M 
B) 4.124 M 
C) 4.252 M 
D) 5.092 M 
E) 14.48 M

Question 6

During osmosis,

Accepted Answer

A) pure solvent passes through a membrane but solutes do not. 
B) pure solute passes through a membrane but solvent does not. 
C) pure solvent moves in one direction through the membrane while the solution moves through the membrane in the other direction. 
D) pure solvent moves in one direction through the membrane while the solute moves through the membrane in the other direction. 
E) pure solute moves in one direction through the membrane while the solution moves through the membrane in the other direction. 
A) pure solvent passes through a membrane but solutes do not. 
B) pure solute passes through a membrane but solvent does not. 
C) pure solvent moves in one direction through the membrane while the solution moves through the membrane in the other direction. 
D) pure solvent moves in one direction through the membrane while the solute moves through the membrane in the other direction. 
E) pure solute moves in one direction through the membrane while the solution moves through the membrane in the other direction.

Question 7

A glucose solution is prepared by dissolving 5.10 g of glucose, C6H12O6, in 110.5 g of water. What is the molality of the glucose solution?

Accepted Answer

A) 0.283 m 
B) 0.000256 m 
C) 0.245 m 
D) 0.256 m 
E) 0.351 m 
A) 0.283 m 
B) 0.000256 m 
C) 0.245 m 
D) 0.256 m 
E) 0.351 m

Question 8

The higher the concentration of an ionic substance in solution, the ________ the van't Hoff factor deviates from its predicted value. Hint: Dilute solutions behave closer to expectations than concentrated solutions.

Accepted Answer

The answer of The higher the concentration of an ionic...

Question 9

At 28.0°C, the vapor pressure of pure carbon disulfide, CS2, is 378.7 torr, while that of acetone, C3H6O, is 228.9 torr. What is the vapor pressure, at 28.0°C, of a solution made by mixing 0.250 moles of carbon disulfide and 0.450 moles of acetone, if Raoult's Law is obeyed?Hint: Organizing the given information into moles and mole fraction of each component will help in solving this problem.

Accepted Answer

A) 198 torr 
B) 228 torr 
C) 282 torr 
D) 325 torr 
E) 425 torr 
A) 198 torr 
B) 228 torr 
C) 282 torr 
D) 325 torr 
E) 425 torr

Question 10

Oxygen has a solubility in water of 0.0043 g/100 mL at 20°C, but CO2 has a solubility of 0.169 g/100 mL at 20°C. What is the main reason for this large difference in solubilities between these gases?

Accepted Answer

Carbon dioxide will form strong interact

Question 11

A scientist looking to remove oxygen from above a liquid sample pumps nitrogen into a sealed compartment to displace the oxygen, then places his liquid sample into the compartment. If the nitrogen pressure (partial pressure)were 1.8 atm, what would be the concentration of dissolved nitrogen gas if the Henry's Law constant for nitrogen gas was 6.8 × 10−4 M atm−1 at this temperature?

Accepted Answer

Question 12

Which of the following will always cause an increase in the solubility of a gas in a solvent in which the gas does not react with the solvent to form a new substance?

Accepted Answer

A) increasing the temperature of the solvent and simultaneously decreasing the pressure of the gas in the space above the solvent 
B) decreasing the temperature of the solvent and simultaneously increasing the pressure of the gas in the space above the solvent 
C) increasing the temperature of the solvent and simultaneously increasing the pressure of the gas in the space above the solvent 
D) decreasing the temperature of the solvent and simultaneously decreasing the pressure of the gas in the space above the solvent 
E) increasing the temperature of the solvent while maintaining the pressure of the gas in the space above the solvent at a set value 
A) increasing the temperature of the solvent and simultaneously decreasing the pressure of the gas in the space above the solvent 
B) decreasing the temperature of the solvent and simultaneously increasing the pressure of the gas in the space above the solvent 
C) increasing the temperature of the solvent and simultaneously increasing the pressure of the gas in the space above the solvent 
D) decreasing the temperature of the solvent and simultaneously decreasing the pressure of the gas in the space above the solvent 
E) increasing the temperature of the solvent while maintaining the pressure of the gas in the space above the solvent at a set value

Question 13

Concerning the process of separating of a solid substance into its component units (molecules or ions),

Accepted Answer

A) the process is exothermic and the potential energy increases. 
B) the process is exothermic and the potential energy decreases. 
C) the process is endothermic and the potential energy increases. 
D) the process is endothermic and the potential energy decreases. 
E) the process is endothermic and occurs with no change in potential energy. 
A) the process is exothermic and the potential energy increases. 
B) the process is exothermic and the potential energy decreases. 
C) the process is endothermic and the potential energy increases. 
D) the process is endothermic and the potential energy decreases. 
E) the process is endothermic and occurs with no change in potential energy.

Question 14

Pure cyclohexane, C6H12, has a freezing point of 6.53°C. Its freezing point depression constant is: Kf = 20.0 °C m-1. A solution was made by taking 18.55 g of an unknown nonelectrolyte and dissolving it in 150.0 g of cyclohexane. The measured freezing point of the solution was -4.28°C. Calculate the molecular weight of the unknown substance.Hint: Find molality, then moles, then molar mass, being sure to keep track of units.

Accepted Answer

A) 61.8 g mol-1 
B) 66.8 g mol-1 
C) 229 g mol-1 
D) 578 g mol-1 
E) 1099 g mol-1 
A) 61.8 g mol-1 
B) 66.8 g mol-1 
C) 229 g mol-1 
D) 578 g mol-1 
E) 1099 g mol-1

Question 15

A solution is made by dissolving 0.840 moles of sodium hydroxide in 300.0 g of water. If the van't Hoff factor, i, for this particular concentration is 1.70, what is the expected freezing point of this solution? Kf = 1.86 °C m-1.

Accepted Answer

A) +0.80°C 
B) -2.66°C 
C) +3.06°C 
D) -8.85°C 
E) -9.97°C 
A) +0.80°C 
B) -2.66°C 
C) +3.06°C 
D) -8.85°C 
E) -9.97°C

Question 16

Which property of a solution is not a colligative property?

Accepted Answer

A) solubility of a solute 
B) freezing point depression 
C) boiling point elevation 
D) osmotic pressure 
E) vapor pressure lowering 
A) solubility of a solute 
B) freezing point depression 
C) boiling point elevation 
D) osmotic pressure 
E) vapor pressure lowering

Question 17

Which aqueous solution will have the highest freezing point temperature?Hint: be sure to closely read the question.

Accepted Answer

A) 0.100 molal MgBr2(aq) 
B) 0.100 molal MgSO4(aq) 
C) 0.150 molal KClO3(aq) 
D) 0.150 molal MgCl2(aq) 
E) 0.250 molal C6H12O6(aq) 
A) 0.100 molal MgBr2(aq) 
B) 0.100 molal MgSO4(aq) 
C) 0.150 molal KClO3(aq) 
D) 0.150 molal MgCl2(aq) 
E) 0.250 molal C6H12O6(aq)

Question 18

Which solution has the highest osmotic pressure at 25°C?

Accepted Answer

A) 0.200 M (NH4)2SO4 
B) 0.200 M KClO3 
C) 0.200 M C2H6O, ethanol 
D) 0.200 M NiF2 
E) 0.200 M Fe(NO3)3 
A) 0.200 M (NH4)2SO4 
B) 0.200 M KClO3 
C) 0.200 M C2H6O, ethanol 
D) 0.200 M NiF2 
E) 0.200 M Fe(NO3)3

Question 19

The process, MgSO4(s). MgSO4(aq), is an endothermic process. The solubility of magnesium sulfate in water should therefore increase as the solvent temperature is increased.

Accepted Answer

A) True 
 B)False

Question 20

How many grams of glycerol (C3H8O3, a nonelectrolyte)should be dissolved in 600 g of water to prepare a solution whose freezing point is -4.65°C? For water, Kf is 1.86°C m-1 and Kb is 0.512 °C m-1.

Accepted Answer

A) 22.1 grams 
B) 93.6 grams 
C) 138 grams 
D) 384 grams 
E) 478 grams 
A) 22.1 grams 
B) 93.6 grams 
C) 138 grams 
D) 384 grams 
E) 478 grams

Arrange the following solutions in order of increasing freezing point depression.

A dilute aqueous solution of CaCl₂ contains 0.159 grams of solute per liter of solution. It is fully dissociated. What is its osmotic pressure at 20.0^°C?Hint: CaCl₂ is an ionic compound.

An aqueous solution of ethanol, C₂H₅OH, is 19.00% ethanol by mass and has a density of 0.9700 g mL^-1. Calculate the molarity of the ethanol solution.

During osmosis,

A glucose solution is prepared by dissolving 5.10 g of glucose, C₆H₁₂O₆, in 110.5 g of water. What is the molality of the glucose solution?

The higher the concentration of an ionic substance in solution, the ________ the van't Hoff factor deviates from its predicted value. Hint: Dilute solutions behave closer to expectations than concentrated solutions.

Oxygen has a solubility in water of 0.0043 g/100 mL at 20°C, but CO₂ has a solubility of 0.169 g/100 mL at 20°C. What is the main reason for this large difference in solubilities between these gases?

Which of the following will always cause an increase in the solubility of a gas in a solvent in which the gas does not react with the solvent to form a new substance?

Concerning the process of separating of a solid substance into its component units (molecules or ions),

A solution is made by dissolving 0.840 moles of sodium hydroxide in 300.0 g of water. If the van't Hoff factor, i, for this particular concentration is 1.70, what is the expected freezing point of this solution? K_f = 1.86 °C m^-1.

Which property of a solution is not a colligative property?

Which aqueous solution will have the highest freezing point temperature?Hint: be sure to closely read the question.

Which solution has the highest osmotic pressure at 25°C?

The process, MgSO₄(s). MgSO₄(aq), is an endothermic process. The solubility of magnesium sulfate in water should therefore increase as the solvent temperature is increased.

How many grams of glycerol (C₃H₈O₃, a nonelectrolyte)should be dissolved in 600 g of water to prepare a solution whose freezing point is -4.65°C? For water, K_f is 1.86°C m^-1 and K_b is 0.512 °C m^-1.

A Very Brief History of Chemistry

Scientific Measurements

Elements, Compounds, and the Periodic Table

The Mole and Stoichiometry

Molecular View of Reactions in Aqueous Solutions

Oxidation-Reduction Reactions

Energy and Chemical Change

The Quantum Mechanical Atom

The Basics of Chemical Bonding

Theories of Bonding and Structure

Properties of Gases

Intermolecular Attractions and the Properties of Liquids and Solids

Chemical Kinetics

Chemical Equilibrium

Acids and Bases, a Molecular Look

Acid-Base Equilibria in Aqueous Solutions

Solubility and Simultaneous Equilibria

Thermodynamics

Electrochemistry

Nuclear Reactions and Their Role in Chemistry

Metal Complexes

Organic Compounds, Polymers, and Biochemicals

Filters

Exam 13: Mixtures at the Molecular Level: Properties of Solutions

Arrange the following solutions in order of increasing freezing point depression.

A dilute aqueous solution of CaCl2 contains 0.159 grams of solute per liter of solution. It is fully dissociated. What is its osmotic pressure at 20.0°C?Hint: CaCl2 is an ionic compound.

An aqueous solution of ethanol, C2H5OH, is 19.00% ethanol by mass and has a density of 0.9700 g mL-1. Calculate the molarity of the ethanol solution.

During osmosis,

A glucose solution is prepared by dissolving 5.10 g of glucose, C6H12O6, in 110.5 g of water. What is the molality of the glucose solution?

The higher the concentration of an ionic substance in solution, the ________ the van't Hoff factor deviates from its predicted value. Hint: Dilute solutions behave closer to expectations than concentrated solutions.

Oxygen has a solubility in water of 0.0043 g/100 mL at 20°C, but CO2 has a solubility of 0.169 g/100 mL at 20°C. What is the main reason for this large difference in solubilities between these gases?

Which of the following will always cause an increase in the solubility of a gas in a solvent in which the gas does not react with the solvent to form a new substance?

Concerning the process of separating of a solid substance into its component units (molecules or ions),

A solution is made by dissolving 0.840 moles of sodium hydroxide in 300.0 g of water. If the van't Hoff factor, i, for this particular concentration is 1.70, what is the expected freezing point of this solution? Kf = 1.86 °C m-1.

Which property of a solution is not a colligative property?

Which aqueous solution will have the highest freezing point temperature?Hint: be sure to closely read the question.

Which solution has the highest osmotic pressure at 25°C?

The process, MgSO4(s). MgSO4(aq), is an endothermic process. The solubility of magnesium sulfate in water should therefore increase as the solvent temperature is increased.

How many grams of glycerol (C3H8O3, a nonelectrolyte)should be dissolved in 600 g of water to prepare a solution whose freezing point is -4.65°C? For water, Kf is 1.86°C m-1 and Kb is 0.512 °C m-1.

A Very Brief History of Chemistry

Scientific Measurements

Elements, Compounds, and the Periodic Table

The Mole and Stoichiometry

Molecular View of Reactions in Aqueous Solutions

Oxidation-Reduction Reactions

Energy and Chemical Change

The Quantum Mechanical Atom

The Basics of Chemical Bonding

Theories of Bonding and Structure

Properties of Gases

Intermolecular Attractions and the Properties of Liquids and Solids

Chemical Kinetics

Chemical Equilibrium

Acids and Bases, a Molecular Look

Acid-Base Equilibria in Aqueous Solutions

Solubility and Simultaneous Equilibria

Thermodynamics

Electrochemistry

Nuclear Reactions and Their Role in Chemistry

Metal Complexes

Organic Compounds, Polymers, and Biochemicals

Filters

A dilute aqueous solution of CaCl₂ contains 0.159 grams of solute per liter of solution. It is fully dissociated. What is its osmotic pressure at 20.0^°C?Hint: CaCl₂ is an ionic compound.

An aqueous solution of ethanol, C₂H₅OH, is 19.00% ethanol by mass and has a density of 0.9700 g mL^-1. Calculate the molarity of the ethanol solution.

A glucose solution is prepared by dissolving 5.10 g of glucose, C₆H₁₂O₆, in 110.5 g of water. What is the molality of the glucose solution?

Oxygen has a solubility in water of 0.0043 g/100 mL at 20°C, but CO₂ has a solubility of 0.169 g/100 mL at 20°C. What is the main reason for this large difference in solubilities between these gases?

A solution is made by dissolving 0.840 moles of sodium hydroxide in 300.0 g of water. If the van't Hoff factor, i, for this particular concentration is 1.70, what is the expected freezing point of this solution? K_f = 1.86 °C m^-1.

The process, MgSO₄(s). MgSO₄(aq), is an endothermic process. The solubility of magnesium sulfate in water should therefore increase as the solvent temperature is increased.

How many grams of glycerol (C₃H₈O₃, a nonelectrolyte)should be dissolved in 600 g of water to prepare a solution whose freezing point is -4.65°C? For water, K_f is 1.86°C m^-1 and K_b is 0.512 °C m^-1.