Question 1

What is the mole fraction of ethanol in a solution made by dissolving 29.2 g of ethanol,C2H5OH,in 53.6 g of water?

Accepted Answer

A) 0.176 
B) 0.213 
C) 0.352 
D) 0.545 
A) 0.176 
B) 0.213 
C) 0.352 
D) 0.545 A

Question 2

Which of the following compounds is most soluble in hexane (CH3CH2CH2CH2CH2CH2CH3)?

Accepted Answer

A) methanol 
B) ethanol 
C) 1-propanol 
D) 1-butanol 
E) 1-pentanol 
A) methanol 
B) ethanol 
C) 1-propanol 
D) 1-butanol 
E) 1-pentanol E

Question 3

Give the intermolecular force that is responsible for the solubility of ethanol in water.

Accepted Answer

A) dispersion forces 
B) dipole-dipole forces 
C) hydrogen bonding 
D) ion-dipole forces 
E) ionic forces 
A) dispersion forces 
B) dipole-dipole forces 
C) hydrogen bonding 
D) ion-dipole forces 
E) ionic forces C

Question 4

Calculate the mass of oxygen (in mg)dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 atm of air.Assume the mole fraction of oxygen in air to be 0.21 and the Henry's law constant for oxygen in water at this temperature to be 1.3 × 10-3 M/atm.

Accepted Answer

A) 49.4 mg 
B) 23.5 mg 
C) 9.87 mg 
D) 27.3 mg 
E) 13.7 mg 
A) 49.4 mg 
B) 23.5 mg 
C) 9.87 mg 
D) 27.3 mg 
E) 13.7 mg

Question 5

Choose the situation below that would result in a ΔHsolution near 0.

Accepted Answer

A) When >> B) When > C) When < D) When Is close to E) There isn't enough information to determine. A) When >> B) When > C) When < D) When Is close to E) There isn't enough information to determine.

Question 6

Calculate the osmotic pressure,in torr,of a solution containing 3.00 mg of a sugar (342 g/mole)in 15.0 mL of water at 25°C.

Accepted Answer

The answer of Calculate the osmotic pressure,in torr,of a solution...

Question 7

Give the reason that antifreeze is added to a car radiator.

Accepted Answer

A) The freezing point is lowered and the boiling point is elevated. 
B) The freezing point is elevated and the boiling point is lowered. 
C) The freezing point and the boiling point are elevated. 
D) The freezing point and the boiling point are lowered. 
E) None of the above 
A) The freezing point is lowered and the boiling point is elevated. 
B) The freezing point is elevated and the boiling point is lowered. 
C) The freezing point and the boiling point are elevated. 
D) The freezing point and the boiling point are lowered. 
E) None of the above

Question 8

How many grams of KBr are required to make 350.mL of a 0.115 M KBr solution?

Accepted Answer

A) 0.338 g 
B) 3.04 g 
C) 4.79 g 
D) 40.3 g 
A) 0.338 g 
B) 3.04 g 
C) 4.79 g 
D) 40.3 g

Question 9

Which of the following should have the largest Henry's law constant (kH)in water?

Accepted Answer

A) Ar 
B) CO 
C) Xe 
D) CH3CH3 
E) CO2 
A) Ar 
B) CO 
C) Xe 
D) CH3CH3 
E) CO2

Question 10

What volume of 3.00 M CH3OH solution is needed to provide 0.220 mol of CH3OH?

Accepted Answer

A) 1.52 mL 
B) 13.6 mL 
C) 73.3 mL 
D) 660 mL 
A) 1.52 mL 
B) 13.6 mL 
C) 73.3 mL 
D) 660 mL

Question 11

Determine the boiling point of a solution that contains 78.8 g of naphthalene (C10H8,molar mass = 128.16 g/mol)dissolved in 722 mL of benzene (d = 0.877 g/mL).Pure benzene has a boiling point of 80.1°C and a boiling point elevation constant of 2.53°C/m.

Accepted Answer

A) 2.2°C 
B) 2.5°C 
C) 82.3°C 
D) 80.4°C 
E) 82.6°C 
A) 2.2°C 
B) 2.5°C 
C) 82.3°C 
D) 80.4°C 
E) 82.6°C

Question 12

Which of the following statements is true?

Accepted Answer

A) The solubility of a solid is not dependent on either temperature or pressure. 
B) The solubility of a solid is highly dependent on pressure. 
C) The solubility of a solid is highly dependent on both pressure and temperature. 
D) The solubility of a solid is highly dependent on temperature. 
E) None of the above. 
A) The solubility of a solid is not dependent on either temperature or pressure. 
B) The solubility of a solid is highly dependent on pressure. 
C) The solubility of a solid is highly dependent on both pressure and temperature. 
D) The solubility of a solid is highly dependent on temperature. 
E) None of the above.

Question 13

A solution contains 45g of KNO3 per 100.0 g of water at 25°C.The solubility of KNO3 at this temperature is 37.5 g per 100.0 g of water.The solution is ________.

Accepted Answer

A) supersaturated 
B) unsaturated 
C) saturated 
D) none of the above 
A) supersaturated 
B) unsaturated 
C) saturated 
D) none of the above

Question 14

What is the freezing point of a solution of 7.15 g MgCl2 in 100 g of water? Kf for water is 1.86°C/m.

Accepted Answer

A) -0.140°C 
B) -1.40°C 
C) -2.80°C 
D) -4.18°C 
A) -0.140°C 
B) -1.40°C 
C) -2.80°C 
D) -4.18°C

Question 15

Place the following aqueous solutions of nonvolatile,nonionic compounds in order of decreasing osmotic pressure.
I.0.011 M sucrose 
II.0.00095 M glucose 
III.0.0060 M glycerin

Accepted Answer

A) I > III > II 
B) I > II > III 
C) II > III > I 
D) III > I > II 
E) II > I > III 
A) I > III > II 
B) I > II > III 
C) II > III > I 
D) III > I > II 
E) II > I > III

Question 16

Match the following.
-0.050 m C6H12O6 (aqueous)

Accepted Answer

A) largest van't Hoff factor 
B) solution of ionic compound with highest freezing point 
C) solution with ΔTb = 0.026°C 
D) highest boiling point 
E) solution that is most strongly dependent upon pressure 
A) largest van't Hoff factor 
B) solution of ionic compound with highest freezing point 
C) solution with ΔTb = 0.026°C 
D) highest boiling point 
E) solution that is most strongly dependent upon pressure

Question 17

To make a 2.00 m solution,one could take 2.00 moles of solute and add

Accepted Answer

A) 1.00 L of solvent. 
B) 1.00 kg of solvent. 
C) enough solvent to make 1.00 L of solution. 
D) enough solvent to make 1.00 kg of solution. 
A) 1.00 L of solvent. 
B) 1.00 kg of solvent. 
C) enough solvent to make 1.00 L of solution. 
D) enough solvent to make 1.00 kg of solution.

Question 18

Which interaction(s)determine whether a solution will form?

Accepted Answer

A) solvent-solvent 
B) solute-solute 
C) solvent-solute 
D) all of the above 
A) solvent-solvent 
B) solute-solute 
C) solvent-solute 
D) all of the above

Question 19

An aqueous solution has a normal boiling point of 103.0°C.What is the freezing point of this solution? For water Kb = 0.51°C/m and Kf = 1.86°C/m.

Accepted Answer

A) -0.82°C 
B) -3.0°C 
C) -3.6°C 
D) -11°C 
A) -0.82°C 
B) -3.0°C 
C) -3.6°C 
D) -11°C

Question 20

A solution is prepared by dissolving 49.3 g of KBr in enough water to form 473 mL of solution.Calculate the mass % of KBr in the solution if the density is 1.12 g/mL.

Accepted Answer

A) 10.4% 
B) 8.57% 
C) 10.1% 
D) 11.7% 
E) 9.31% 
A) 10.4% 
B) 8.57% 
C) 10.1% 
D) 11.7% 
E) 9.31%

What is the mole fraction of ethanol in a solution made by dissolving 29.2 g of ethanol,C₂H₅OH,in 53.6 g of water?

Which of the following compounds is most soluble in hexane (CH₃CH₂CH₂CH₂CH₂CH₂CH₃)?

Give the intermolecular force that is responsible for the solubility of ethanol in water.

Calculate the mass of oxygen (in mg)dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 atm of air.Assume the mole fraction of oxygen in air to be 0.21 and the Henry's law constant for oxygen in water at this temperature to be 1.3 × 10^-3 M/atm.

Choose the situation below that would result in a ΔH_solution near 0.

Calculate the osmotic pressure,in torr,of a solution containing 3.00 mg of a sugar (342 g/mole)in 15.0 mL of water at 25°C.

Give the reason that antifreeze is added to a car radiator.

How many grams of KBr are required to make 350.mL of a 0.115 M KBr solution?

Which of the following should have the largest Henry's law constant (k_H)in water?

What volume of 3.00 M CH₃OH solution is needed to provide 0.220 mol of CH₃OH?

Determine the boiling point of a solution that contains 78.8 g of naphthalene (C₁₀H₈,molar mass = 128.16 g/mol)dissolved in 722 mL of benzene (d = 0.877 g/mL).Pure benzene has a boiling point of 80.1°C and a boiling point elevation constant of 2.53°C/m.

Which of the following statements is true?

A solution contains 45g of KNO3 per 100.0 g of water at 25°C.The solubility of KNO3 at this temperature is 37.5 g per 100.0 g of water.The solution is ________.

What is the freezing point of a solution of 7.15 g MgCl₂ in 100 g of water? K_f for water is 1.86°C/m.

Place the following aqueous solutions of nonvolatile,nonionic compounds in order of decreasing osmotic pressure. I.0.011 M sucrose II.0.00095 M glucose III.0.0060 M glycerin

Match the following. -0.050 m C₆H₁₂O₆(aqueous)

To make a 2.00 m solution,one could take 2.00 moles of solute and add

Which interaction(s)determine whether a solution will form?

An aqueous solution has a normal boiling point of 103.0°C.What is the freezing point of this solution? For water K_b = 0.51°C/m and K_f = 1.86°C/m.

A solution is prepared by dissolving 49.3 g of KBr in enough water to form 473 mL of solution.Calculate the mass % of KBr in the solution if the density is 1.12 g/mL.

Matter, Measurement, and Problem Solving

Atoms and Elements

Molecules, Compounds and Chemical Equations

Chemical Quantities and Aqueous Reactions

Gases

Thermochemistry

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and

Liquids, Solids, and Intermolecular Forces

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Free Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Filters

Exam 12: Solutions

What is the mole fraction of ethanol in a solution made by dissolving 29.2 g of ethanol,C2H5OH,in 53.6 g of water?

Which of the following compounds is most soluble in hexane (CH3CH2CH2CH2CH2CH2CH3)?

Give the intermolecular force that is responsible for the solubility of ethanol in water.

Calculate the mass of oxygen (in mg)dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 atm of air.Assume the mole fraction of oxygen in air to be 0.21 and the Henry's law constant for oxygen in water at this temperature to be 1.3 × 10-3 M/atm.

Choose the situation below that would result in a ΔHsolution near 0.

Calculate the osmotic pressure,in torr,of a solution containing 3.00 mg of a sugar (342 g/mole)in 15.0 mL of water at 25°C.

Give the reason that antifreeze is added to a car radiator.

How many grams of KBr are required to make 350.mL of a 0.115 M KBr solution?

Which of the following should have the largest Henry's law constant (kH)in water?

What volume of 3.00 M CH3OH solution is needed to provide 0.220 mol of CH3OH?

Determine the boiling point of a solution that contains 78.8 g of naphthalene (C10H8,molar mass = 128.16 g/mol)dissolved in 722 mL of benzene (d = 0.877 g/mL).Pure benzene has a boiling point of 80.1°C and a boiling point elevation constant of 2.53°C/m.

Which of the following statements is true?

A solution contains 45g of KNO3 per 100.0 g of water at 25°C.The solubility of KNO3 at this temperature is 37.5 g per 100.0 g of water.The solution is ________.

What is the freezing point of a solution of 7.15 g MgCl2 in 100 g of water? Kf for water is 1.86°C/m.

Place the following aqueous solutions of nonvolatile,nonionic compounds in order of decreasing osmotic pressure. I.0.011 M sucrose II.0.00095 M glucose III.0.0060 M glycerin

Match the following. -0.050 m C6H12O6 (aqueous)

To make a 2.00 m solution,one could take 2.00 moles of solute and add

Which interaction(s)determine whether a solution will form?

An aqueous solution has a normal boiling point of 103.0°C.What is the freezing point of this solution? For water Kb = 0.51°C/m and Kf = 1.86°C/m.

A solution is prepared by dissolving 49.3 g of KBr in enough water to form 473 mL of solution.Calculate the mass % of KBr in the solution if the density is 1.12 g/mL.

Matter, Measurement, and Problem Solving

Atoms and Elements

Molecules, Compounds and Chemical Equations

Chemical Quantities and Aqueous Reactions

Gases

Thermochemistry

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and

Liquids, Solids, and Intermolecular Forces

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Free Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Filters

What is the mole fraction of ethanol in a solution made by dissolving 29.2 g of ethanol,C₂H₅OH,in 53.6 g of water?

Which of the following compounds is most soluble in hexane (CH₃CH₂CH₂CH₂CH₂CH₂CH₃)?

Calculate the mass of oxygen (in mg)dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 atm of air.Assume the mole fraction of oxygen in air to be 0.21 and the Henry's law constant for oxygen in water at this temperature to be 1.3 × 10^-3 M/atm.

Choose the situation below that would result in a ΔH_solution near 0.

Which of the following should have the largest Henry's law constant (k_H)in water?

What volume of 3.00 M CH₃OH solution is needed to provide 0.220 mol of CH₃OH?

Determine the boiling point of a solution that contains 78.8 g of naphthalene (C₁₀H₈,molar mass = 128.16 g/mol)dissolved in 722 mL of benzene (d = 0.877 g/mL).Pure benzene has a boiling point of 80.1°C and a boiling point elevation constant of 2.53°C/m.

What is the freezing point of a solution of 7.15 g MgCl₂ in 100 g of water? K_f for water is 1.86°C/m.

Match the following. -0.050 m C₆H₁₂O₆(aqueous)

An aqueous solution has a normal boiling point of 103.0°C.What is the freezing point of this solution? For water K_b = 0.51°C/m and K_f = 1.86°C/m.