Question 1

Of the following, a 0.2 M aqueous solution of ________ will have the highest freezing point.

Accepted Answer

A) RbBr 
B) K2SO4 
C) Sr(NO3)2 
D) (NH4)2SO4 
E) Fe(NO3)2 
A) RbBr 
B) K2SO4 
C) Sr(NO3)2 
D) (NH4)2SO4 
E) Fe(NO3)2

Question 2

Which one of the following substances would be the most soluble in CCl4?

Accepted Answer

A) C4H10 
B) Li2O 
C) NH3 
D) HCl 
E) CH3CH2CH2OH 
A) C4H10 
B) Li2O 
C) NH3 
D) HCl 
E) CH3CH2CH2OH

Question 3

Calculate the freezing point of a 0.05500 m aqueous solution of NaNO3. The molal freezing-point-depression constant of water is 1.86 °C/m.

Accepted Answer

A) 0.0286 
B) -0.106 
C) 0.106 
D) -0.0562 
E) -0.205 
A) 0.0286 
B) -0.106 
C) 0.106 
D) -0.0562 
E) -0.205

Question 4

An unsaturated solution is one that ________.

Accepted Answer

A) has no double bonds 
B) contains the maximum concentration of solute possible, and is in equilibrium with undissolved solute 
C) has a concentration lower than the solubility 
D) contains more dissolved solute than the solubility allows 
E) contains no solute 
A) has no double bonds 
B) contains the maximum concentration of solute possible, and is in equilibrium with undissolved solute 
C) has a concentration lower than the solubility 
D) contains more dissolved solute than the solubility allows 
E) contains no solute

Question 5

Of the concentration units below, only ________ uses kg of solvent in its calculation.

Accepted Answer

A) mass % 
B) ppm 
C) ppb 
D) molarity 
E) molality 
A) mass % 
B) ppm 
C) ppb 
D) molarity 
E) molality

Question 6

A solution contains 150.8 grams of NaCl in 678.3 grams of water. Calculate the vapor pressure of water (in torr)over the solution at 25.0 °C. (Note: The vapor pressure of pure water at 25.0 °C is 23.76 torr.)

Accepted Answer

The answer of A solution contains 150.8 grams of NaCl...

Question 7

The process of solute particles being surrounded by solvent particles is known as ________.

Accepted Answer

A) salutation 
B) agglomeration 
C) solvation 
D) agglutination 
E) dehydration 
A) salutation 
B) agglomeration 
C) solvation 
D) agglutination 
E) dehydration

Question 8

A solution is prepared by dissolving 2.00 g of glycerin (C3H8O3)in 201 g of ethanol (C2H5OH). The freezing point of the solution is ________°C. The freezing point of pure ethanol is -114.6 °C at 1 atm. The molal-freezing-point-depression constant (Kf)for ethanol is 1.99 °C/m. The molar masses of glycerin and of ethanol are 92.1 g/mol and 46.1 g/mol, respectively.

Accepted Answer

A) -116.6 
B) 0.215 
C) -112.6 
D) -114.4 
E) -114.8 
A) -116.6 
B) 0.215 
C) -112.6 
D) -114.4 
E) -114.8

Question 9

Which one of the following substances would be the least soluble in CCl4?

Accepted Answer

A) Na2SO4 
B) C4H10 
C) F2 
D) HCl 
E) CH3CH2CH2CH2OH 
A) Na2SO4 
B) C4H10 
C) F2 
D) HCl 
E) CH3CH2CH2CH2OH

Question 10

A saturated solution ________.

Accepted Answer

A) contains dissolved solute in equilibrium with undissolved solute 
B) has the capacity to dissolve more solute 
C) will rapidly precipitate if a seed crystal is added 
D) contains no double bonds 
E) cannot be attained 
A) contains dissolved solute in equilibrium with undissolved solute 
B) has the capacity to dissolve more solute 
C) will rapidly precipitate if a seed crystal is added 
D) contains no double bonds 
E) cannot be attained

Question 11

What is the molarity of sodium chloride in solution that is 13.0% by mass sodium chloride and that has a density of 1.10 g/mL?

Accepted Answer

A) 143 
B) 2.45 
C) 2.56 
D) 2.23 
E) 1.43 × 10-2 
A) 143 
B) 2.45 
C) 2.56 
D) 2.23 
E) 1.43 × 10-2

Question 12

Which of the following substances is more likely to dissolve in CH3OH?

Accepted Answer

A) CCl4 
B) Kr 
C) N2 
D) CH3CH2OH 
E) H2 
A) CCl4 
B) Kr 
C) N2 
D) CH3CH2OH 
E) H2

Question 13

A solution is prepared by adding 40.00 g of lactose (milk sugar)to 110.0 g of water at 55 °C The partial pressure of water above the solution is ________ torr. The vapor pressure of pure water at 55 °C is 118.0 torr. The MW of lactose is 342.3 g/mol.

Accepted Answer

A) 2.216 
B) 125.5 
C) 225.9 
D) 115.8 
E) 86.5 
A) 2.216 
B) 125.5 
C) 225.9 
D) 115.8 
E) 86.5

Question 14

The concentration (M)of HCl in a solution prepared by dissolving 5.5 g of HCl in 200 g of C2H6O is ________ M. The density of the solution is 0.79 g/mL.

Accepted Answer

A) 21 
B) 0.93 
C) 0.58 
D) 6.0 × 10-4 
E) 1.72 
A) 21 
B) 0.93 
C) 0.58 
D) 6.0 × 10-4 
E) 1.72

Question 15

The vapor pressure of pure water at 25 °C is 23.8 torr. What is the vapor pressure (torr)of water above a solution prepared by dissolving 18.0 g of glucose (a nonelectrolyte, MW = 180.0 g/mol)in 95.0 g of water?

Accepted Answer

A) 24.3 
B) 23.4 
C) 0.451 
D) 0.443 
E) 23.8 
A) 24.3 
B) 23.4 
C) 0.451 
D) 0.443 
E) 23.8

Question 16

Calculate the molality of a 10.0% (by mass)aqueous solution of hydrochloric acid.

Accepted Answer

A) 3.32 m 
B) 121 m 
C) 1.10 m 
D) 1.66 m 
E) The density of the solution is needed to solve the problem. 
A) 3.32 m 
B) 121 m 
C) 1.10 m 
D) 1.66 m 
E) The density of the solution is needed to solve the problem.

Question 17

-A sample of potassium nitrate (49.0 g)is dissolved in 101 g of water at 100 °C, with precautions taken to avoid evaporation of any water. The solution is cooled to 30.0 °C and no precipitate is observed. This solution is ________.

Accepted Answer

A) hydrated 
B) placated 
C) saturated 
D) unsaturated 
E) supersaturated 
A) hydrated 
B) placated 
C) saturated 
D) unsaturated 
E) supersaturated

Question 18

As the concentration of a solute in a solution increases, the freezing point of the solution ________ and the vapor pressure of the solution ________.

Accepted Answer

A) increases, increases 
B) increases, decreases 
C) decreases, increases 
D) decreases, decreases 
E) decreases, is unaffected 
A) increases, increases 
B) increases, decreases 
C) decreases, increases 
D) decreases, decreases 
E) decreases, is unaffected

Question 19

Which of the following will have an ideal van't Hoff factor (i)value of 1?

Accepted Answer

A) sucrose 
B) NaF 
C) LiNO3 
D) NH4NO3 
E) Li2PO4 
A) sucrose 
B) NaF 
C) LiNO3 
D) NH4NO3 
E) Li2PO4

Question 20

What is the molality of sodium chloride in solution that is 13.0% by mass sodium chloride and that has a density of 1.10 g/mL?

Accepted Answer

A) 2.23 
B) 1.30 
C) 2.56 
D) 2.03 
E) 1.10 
A) 2.23 
B) 1.30 
C) 2.56 
D) 2.03 
E) 1.10

Exam 13: Properties of Solutions

Of the following, a 0.2 M aqueous solution of ________ will have the highest freezing point.

Which one of the following substances would be the most soluble in CCl4?

Calculate the freezing point of a 0.05500 m aqueous solution of NaNO3. The molal freezing-point-depression constant of water is 1.86 °C/m.

An unsaturated solution is one that ________.

Of the concentration units below, only ________ uses kg of solvent in its calculation.

A solution contains 150.8 grams of NaCl in 678.3 grams of water. Calculate the vapor pressure of water (in torr)over the solution at 25.0 °C. (Note: The vapor pressure of pure water at 25.0 °C is 23.76 torr.)

The process of solute particles being surrounded by solvent particles is known as ________.

Which one of the following substances would be the least soluble in CCl4?

A saturated solution ________.

What is the molarity of sodium chloride in solution that is 13.0% by mass sodium chloride and that has a density of 1.10 g/mL?

Which of the following substances is more likely to dissolve in CH3OH?

A solution is prepared by adding 40.00 g of lactose (milk sugar)to 110.0 g of water at 55 °C The partial pressure of water above the solution is ________ torr. The vapor pressure of pure water at 55 °C is 118.0 torr. The MW of lactose is 342.3 g/mol.

The concentration (M)of HCl in a solution prepared by dissolving 5.5 g of HCl in 200 g of C2H6O is ________ M. The density of the solution is 0.79 g/mL.

The vapor pressure of pure water at 25 °C is 23.8 torr. What is the vapor pressure (torr)of water above a solution prepared by dissolving 18.0 g of glucose (a nonelectrolyte, MW = 180.0 g/mol)in 95.0 g of water?

Calculate the molality of a 10.0% (by mass)aqueous solution of hydrochloric acid.

-A sample of potassium nitrate (49.0 g)is dissolved in 101 g of water at 100 °C, with precautions taken to avoid evaporation of any water. The solution is cooled to 30.0 °C and no precipitate is observed. This solution is ________.

As the concentration of a solute in a solution increases, the freezing point of the solution ________ and the vapor pressure of the solution ________.

Which of the following will have an ideal van't Hoff factor (i)value of 1?

What is the molality of sodium chloride in solution that is 13.0% by mass sodium chloride and that has a density of 1.10 g/mL?

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 substances would be the most soluble in CCl₄?

Calculate the freezing point of a 0.05500 m aqueous solution of NaNO₃. The molal freezing-point-depression constant of water is 1.86 °C/m.

Which one of the following substances would be the least soluble in CCl₄?

Which of the following substances is more likely to dissolve in CH₃OH?

The concentration (M)of HCl in a solution prepared by dissolving 5.5 g of HCl in 200 g of C₂H₆O is ________ M. The density of the solution is 0.79 g/mL.

As the concentration of a solute in a solution increases, the freezing point of the solution and the vapor pressure of the solution .