Question 1

Which one of the following is most soluble in hexane (C6H14)?

Accepted Answer

A) CH3OH 
B) CH3CH2CH2OH 
C) CH3CH2OH 
D) CH3CH2CH2CH2OH 
E) CH3CH2CH2CH2CH2OH 
A) CH3OH 
B) CH3CH2CH2OH 
C) CH3CH2OH 
D) CH3CH2CH2CH2OH 
E) CH3CH2CH2CH2CH2OH

Question 2

Which one of the following solutes has a limiting van't Hoff factor (i)of 3 when dissolved in water?

Accepted Answer

A) KNO3 
B) CH3OH 
C) CCl4 
D) Na2SO4 
E) sucrose 
A) KNO3 
B) CH3OH 
C) CCl4 
D) Na2SO4 
E) sucrose

Question 3

A solution is prepared by dissolving 27.7 g of CaCl2 in 375 g of water. The density of the resulting solution is 1.05 g/mL. The concentration of CaCl2 is ________% by mass.

Accepted Answer

A) 6.88 
B) 7.22 
C) 0.0722 
D) 0.0688 
E) 6.24 
A) 6.88 
B) 7.22 
C) 0.0722 
D) 0.0688 
E) 6.24

Question 4

The formula weight of FeCl3∙6H2O is ________.

Accepted Answer

Question 5

Calculate the mole fraction of nitric acid of a 18.6% (by mass)aqueous solution of nitric acid.

Accepted Answer

A) 0.0484 
B) 0.0508 
C) 0.0967 
D) 0.0242 
E) The density of the solution is needed to solve the problem. 
A) 0.0484 
B) 0.0508 
C) 0.0967 
D) 0.0242 
E) The density of the solution is needed to solve the problem.

Question 6

Calculate the mole fraction of HCl in a 9.45% (by mass)aqueous solution.

Accepted Answer

A) 0.0491 
B) 0.0516 
C) 0.0981 
D) 0.0245 
E) The density of the solution is needed to solve the problem. 
A) 0.0491 
B) 0.0516 
C) 0.0981 
D) 0.0245 
E) The density of the solution is needed to solve the problem.

Question 7

Calculate the mole fraction of nitric acid of an 8.37% (by mass)aqueous solution of nitric acid.

Accepted Answer

A) 0.0199 
B) 0.0203 
C) 0.0398 
D) 0.00995 
E) The density of the solution is needed to solve the problem. 
A) 0.0199 
B) 0.0203 
C) 0.0398 
D) 0.00995 
E) The density of the solution is needed to solve the problem.

Question 8

Which of the following liquids will have the highest freezing point?

Accepted Answer

A) pure H2O 
B) aqueous glucose (0.050 m) 
C) aqueous CoI2 (0.030 m) 
D) aqueous FeI3 (0.030 m) 
E) aqueous NaI (0.030 m) 
A) pure H2O 
B) aqueous glucose (0.050 m) 
C) aqueous CoI2 (0.030 m) 
D) aqueous FeI3 (0.030 m) 
E) aqueous NaI (0.030 m)

Question 9

The vapor pressure of pure water at 25 °C is 23.8 torr. Determine the vapor pressure (torr)of water at 25 °C above a solution prepared by dissolving 25 g of urea (a nonvolatile, non-electrolyte, MW = 60.0 g/mol)in 75 g of water.

Accepted Answer

A) 2.9 
B) 0.42 
C) 22 
D) 27 
E) 0.91 
A) 2.9 
B) 0.42 
C) 22 
D) 27 
E) 0.91

Question 10

Calculate the vapor pressure of a solution made by dissolving 109 grams of glucose (molar mass = 180.2 g/mol)in 920.0 ml of water at 25 °C. The vapor pressure of pure water at 25 °C is 23.76 mm Hg. Assume the density of the solution is 1.00 g/ml.

Accepted Answer

A) 0.278 mm Hg 
B) 0.605 mm Hg 
C) 22.98 mm Hg 
D) 23.48 mm Hg 
E) 23.76 mm Hg 
A) 0.278 mm Hg 
B) 0.605 mm Hg 
C) 22.98 mm Hg 
D) 23.48 mm Hg 
E) 23.76 mm Hg

Question 11

The phenomenon used to differentiate colloids and true solutions is called the ________ effect.

Accepted Answer

The answer of The phenomenon used to differentiate colloids and...

Question 12

Calculate the freezing point of a 0.09500 m aqueous solution of glucose. The molal freezing-point-depression constant of water is 1.86 °C/m.

Accepted Answer

A) 0.0475 
B) 0.106 
C) -0.0562 
D) -0.177 
E) -0.354 
A) 0.0475 
B) 0.106 
C) -0.0562 
D) -0.177 
E) -0.354

Question 13

Which one of the following concentration units varies with temperature?

Accepted Answer

A) molarity 
B) mass percent 
C) mole fraction 
D) molality 
E) all of the above 
A) molarity 
B) mass percent 
C) mole fraction 
D) molality 
E) all of the above

Question 14

Determine the freezing point (°C)of a 0.015 molal aqueous solution of MgSO4. Assume i = 2.0 for MgSO4. The molal freezing-point-depression constant of water is 1.86 °C/m.

Accepted Answer

A) -0.056 
B) -0.028 
C) -0.17 
D) -0.084 
E) 0.000 
A) -0.056 
B) -0.028 
C) -0.17 
D) -0.084 
E) 0.000

Question 15

A solution is prepared by dissolving 23.7 g of CaCl2 in 375 g of water. The density of the resulting solution is 1.05 g/mL. The concentration of Cl- in this solution is ________ M.

Accepted Answer

A) 0.214 
B) 0.562 
C) 1.12 
D) 1.20 
E) 6.64 × 10-2 
A) 0.214 
B) 0.562 
C) 1.12 
D) 1.20 
E) 6.64 × 10-2

Question 16

Hydrophobic colloids ________.

Accepted Answer

A) are those that contain water 
B) can be stabilized by adsorption of ions 
C) are those that do not contain water 
D) can be stabilized by coagulation 
E) will separate into two phases if they are stabilized 
A) are those that contain water 
B) can be stabilized by adsorption of ions 
C) are those that do not contain water 
D) can be stabilized by coagulation 
E) will separate into two phases if they are stabilized

Question 17

Which of the following liquids will have the highest freezing point?

Accepted Answer

A) pure H2O 
B) aqueous glucose (0.60 m) 
C) aqueous sucrose (0.60 m) 
D) aqueous FeI3 (0.24 m) 
E) aqueous KF (0.50 m) 
A) pure H2O 
B) aqueous glucose (0.60 m) 
C) aqueous sucrose (0.60 m) 
D) aqueous FeI3 (0.24 m) 
E) aqueous KF (0.50 m)

Question 18

Which one of the following substances is more likely to dissolve in benzene (C6H6)?

Accepted Answer

A) CH3CH2OH 
B) NH3 
C) NaCl 
D) CCl4 
E) HBr 
A) CH3CH2OH 
B) NH3 
C) NaCl 
D) CCl4 
E) HBr

Question 19

The process of a substance sticking to the surface of another is called

Accepted Answer

A) absorption 
B) diffusion 
C) effusion 
D) adsorption 
E) coagulation 
A) absorption 
B) diffusion 
C) effusion 
D) adsorption 
E) coagulation

Question 20

Which of the following liquids will have the lowest freezing point?

Accepted Answer

A) pure H2O 
B) aqueous glucose (0.60 m) 
C) aqueous sucrose (0.60 m) 
D) aqueous FeI3 (0.24 m) 
E) aqueous KF (0.50 m) 
A) pure H2O 
B) aqueous glucose (0.60 m) 
C) aqueous sucrose (0.60 m) 
D) aqueous FeI3 (0.24 m) 
E) aqueous KF (0.50 m)

Exam 13: Properties of Solutions

Which one of the following is most soluble in hexane (C6H14)?

Which one of the following solutes has a limiting van't Hoff factor (i)of 3 when dissolved in water?

A solution is prepared by dissolving 27.7 g of CaCl2 in 375 g of water. The density of the resulting solution is 1.05 g/mL. The concentration of CaCl2 is ________% by mass.

The formula weight of FeCl3∙6H2O is ________.

Calculate the mole fraction of nitric acid of a 18.6% (by mass)aqueous solution of nitric acid.

Calculate the mole fraction of HCl in a 9.45% (by mass)aqueous solution.

Calculate the mole fraction of nitric acid of an 8.37% (by mass)aqueous solution of nitric acid.

Which of the following liquids will have the highest freezing point?

The vapor pressure of pure water at 25 °C is 23.8 torr. Determine the vapor pressure (torr)of water at 25 °C above a solution prepared by dissolving 25 g of urea (a nonvolatile, non-electrolyte, MW = 60.0 g/mol)in 75 g of water.

Calculate the vapor pressure of a solution made by dissolving 109 grams of glucose (molar mass = 180.2 g/mol)in 920.0 ml of water at 25 °C. The vapor pressure of pure water at 25 °C is 23.76 mm Hg. Assume the density of the solution is 1.00 g/ml.

The phenomenon used to differentiate colloids and true solutions is called the ________ effect.

Calculate the freezing point of a 0.09500 m aqueous solution of glucose. The molal freezing-point-depression constant of water is 1.86 °C/m.

Which one of the following concentration units varies with temperature?

Determine the freezing point (°C)of a 0.015 molal aqueous solution of MgSO4. Assume i = 2.0 for MgSO4. The molal freezing-point-depression constant of water is 1.86 °C/m.

A solution is prepared by dissolving 23.7 g of CaCl2 in 375 g of water. The density of the resulting solution is 1.05 g/mL. The concentration of Cl- in this solution is ________ M.

Hydrophobic colloids ________.

Which of the following liquids will have the highest freezing point?

Which one of the following substances is more likely to dissolve in benzene (C6H6)?

The process of a substance sticking to the surface of another is called

Which of the following liquids will have the lowest freezing point?

Introduction: Matter and Measurement

Atoms, Molecules, and Ions

Stoichiometry: Calculations With Chemical Formulas and Equations

Aqueous Reactions and Solution Stoichiometry

Thermochemistry

Electronic Structure of Atoms

Periodic Properties of the Elements

Basic Concepts of Chemical Bonding

Molecular Geometry and Bonding Theories

Gases

Liquids and Intermolecular Forces

Solids and Modern Materials

Chemical Kinetics

Chemical Equilibrium

Acid-Base Equilibria

Additional Aspects of Aqueous Equilibria

Chemistry of the Environment

Chemical Thermodynamics

Electrochemistry

Nuclear Chemistry

Chemistry of the Nonmetals

Transition Metals and Coordination Chemistry

The Chemistry of Life: Organic and Biological Chemistry

Filters

Which one of the following is most soluble in hexane (C₆H₁₄)?

A solution is prepared by dissolving 27.7 g of CaCl₂ in 375 g of water. The density of the resulting solution is 1.05 g/mL. The concentration of CaCl₂ is ________% by mass.

The formula weight of FeCl₃∙6H₂O is ________.

Determine the freezing point (°C)of a 0.015 molal aqueous solution of MgSO₄. Assume i = 2.0 for MgSO₄. The molal freezing-point-depression constant of water is 1.86 °C/m.

A solution is prepared by dissolving 23.7 g of CaCl₂ in 375 g of water. The density of the resulting solution is 1.05 g/mL. The concentration of Cl^- in this solution is ________ M.

Which one of the following substances is more likely to dissolve in benzene (C₆H₆)?