Question 1

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

Accepted Answer

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

Question 2

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

Question 3

A solution contains 15 ppm of benzene. The density of the solution is 1.00 g/mL. This means that

Accepted Answer

A)  there are 15 mg of benzene in 1.0 L of this solution 
B)  100 g of the solution contains 15 g of benzene 
C)  100 g of the solution contains 15 mg of benzene 
D)  the molarity of the solution is 15 
E)  the solution is 15% by mass of benzene 
A)  there are 15 mg of benzene in 1.0 L of this solution 
B)  100 g of the solution contains 15 g of benzene 
C)  100 g of the solution contains 15 mg of benzene 
D)  the molarity of the solution is 15 
E)  the solution is 15% by mass of benzene

Question 4

An aqueous solution of a soluble compound (anonelectrolyte) is prepared by dissolving 33.2 g of the compound in sufficient water to form 250 mL of solution. The solution has an osmotic pressure of 1.2 atm at 25 °C. What is the molar mass (g/mL) of the compound?

Accepted Answer

A)  2.3 × 102  
B)  1.0 × 103  
C)  2.7 × 103  
D)  6.8 × 102  
E)  28 
A)  2.3 × 102  
B)  1.0 × 103  
C)  2.7 × 103  
D)  6.8 × 102  
E)  28

Question 5

Which one of the following concentration units varies with temperature?

Accepted Answer

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

Question 6

Formation of solutions where the process is endothermic can be spontaneous provided that
)

Accepted Answer

A)  they are accompanied by an increase in order 
B)  the solvent is a gas and the solute is a solid 
C)  they are accompanied by an increase in disorder 
D)  the solvent is water and the solute is a gas 
E)  they are accompanied by another process that is exothermic 
A)  they are accompanied by an increase in order 
B)  the solvent is a gas and the solute is a solid 
C)  they are accompanied by an increase in disorder 
D)  the solvent is water and the solute is a gas 
E)  they are accompanied by another process that is exothermic

Question 7

Pairs of liquids that will mix in all proportions are called liquids.

Accepted Answer

A)  miscible 
B)  saturated 
C)  unsaturated 
D)  polar liquids 
E)  supersaturated 
A)  miscible 
B)  saturated 
C)  unsaturated 
D)  polar liquids 
E)  supersaturated

Question 8

The osmotic pressure of a solution formed by dissolving 25.0 mg of aspirin (C9H8O4) in 0.250 L of water at 25 °C is atm.

Accepted Answer

A)  1.14 × 10- 3 
B)  0.0136 
C)  1.38 
D)  13.6 
E)  2.45 
A)  1.14 × 10- 3 
B)  0.0136 
C)  1.38 
D)  13.6 
E)  2.45

Question 9

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

Accepted Answer

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

Question 10

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 a small amount of precipitate is observed. This solution is .

Accepted Answer

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

Question 11

A 0.15 m aqueous solution of a weak acid has a freezing point of - 0.31 °C. What is the percent ionization of this weak acid at this concentration? The molal freezing- point- depression constant of water is 1.86 °C/m.

Accepted Answer

A)  35 
B)  31 
C)  89 
D)  17 
E)  11 
A)  35 
B)  31 
C)  89 
D)  17 
E)  11

Question 12

A solution is prepared by dissolving calcium chloride in water and diluting to 500.0 mL. If this solution contains 44 ppm chloride ions, the concentration of calcium ions is ppm.

Accepted Answer

A)  11 
B)  44 
C)  88 
D)  500 
E)  22 
A)  11 
B)  44 
C)  88 
D)  500 
E)  22

Question 13

The magnitudes of Kf and of Kb depend on the identity of the .

Accepted Answer

A)  solvent and on temperature 
B)  solute and solvent 
C)  solvent 
D)  solute 
E)  solution 
A)  solvent and on temperature 
B)  solute and solvent 
C)  solvent 
D)  solute 
E)  solution

Question 14

The concentration of KBr in a solution prepared by dissolving 2.21 g of KBr in 897 g of water is
Molal.

Accepted Answer

A)  0.0207 
B)  0.0167 
C)  2.46 
D)  0.0186 
E)  2.07 × 10- 5 
A)  0.0207 
B)  0.0167 
C)  2.46 
D)  0.0186 
E)  2.07 × 10- 5

Question 15

The solubility of nitrogen gas in water at 25 °C and a nitrogen pressure of 1.0 atm is 6.9 × 10- 4 M. The solubility of nitrogen in water at a nitrogen pressure of 0.80 atm is M.

Accepted Answer

A)  5.5 × 10- 4  
B)  1.2 × 103  
C)  8.6 × 10- 4  
D)  0.80 
E)  3.7 × 10- 3 
A)  5.5 × 10- 4  
B)  1.2 × 103  
C)  8.6 × 10- 4  
D)  0.80 
E)  3.7 × 10- 3

Question 16

Ammonium nitrate (NH4NO3) dissolves readily in water even though the dissolution is endothermic by 26.4 kJ/mol. The solution process is spontaneous because _.

Accepted Answer

A)  of the increase in disorder upon dissolution of this strong electrolyte 
B)  the vapor pressure of the water decreases upon addition of the solute 
C)  of the increase in enthalpy upon dissolution of this strong electrolyte 
D)  of the decrease in enthalpy upon addition of the solute 
E)  osmotic properties predict this behavior 
A)  of the increase in disorder upon dissolution of this strong electrolyte 
B)  the vapor pressure of the water decreases upon addition of the solute 
C)  of the increase in enthalpy upon dissolution of this strong electrolyte 
D)  of the decrease in enthalpy upon addition of the solute 
E)  osmotic properties predict this behavior

Question 17

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

Question 18

Molality is defined as the .

Accepted Answer

A)  moles solute/kg solution 
B)  moles solute/Liters solution 
C)  moles solute/moles solvent 
D)  moles solute/kg solvent 
E)  none (dimensionless) 
A)  moles solute/kg solution 
B)  moles solute/Liters solution 
C)  moles solute/moles solvent 
D)  moles solute/kg solvent 
E)  none (dimensionless)

Question 19

A saturated solution .

Accepted Answer

A)  contains as much solvent as it can hold 
B)  cannot be attained 
C)  contains dissolved solute in equilibrium with undissolved solid 
D)  will rapidly precipitate if a seed crystal is added 
E)  contains no double bonds 
A)  contains as much solvent as it can hold 
B)  cannot be attained 
C)  contains dissolved solute in equilibrium with undissolved solid 
D)  will rapidly precipitate if a seed crystal is added 
E)  contains no double bonds

Question 20

The concentration of urea in a solution prepared by dissolving 16 g of urea in 39 g of H2O is % by mass. The molar mass of urea is 60.0 g/mol.

Accepted Answer

A)  0.29 
B)  0.41 
C)  29 
D)  0.48 
E)  41 
A)  0.29 
B)  0.41 
C)  29 
D)  0.48 
E)  41

Exam 13: Properties of Solutions

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

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 .

A solution contains 15 ppm of benzene. The density of the solution is 1.00 g/mL. This means that

An aqueous solution of a soluble compound (anonelectrolyte) is prepared by dissolving 33.2 g of the compound in sufficient water to form 250 mL of solution. The solution has an osmotic pressure of 1.2 atm at 25 °C. What is the molar mass (g/mL) of the compound?

Which one of the following concentration units varies with temperature?

Formation of solutions where the process is endothermic can be spontaneous provided that )

Pairs of liquids that will mix in all proportions are called liquids.

The osmotic pressure of a solution formed by dissolving 25.0 mg of aspirin (C9H8O4) in 0.250 L of water at 25 °C is atm.

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

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 a small amount of precipitate is observed. This solution is .

A 0.15 m aqueous solution of a weak acid has a freezing point of - 0.31 °C. What is the percent ionization of this weak acid at this concentration? The molal freezing- point- depression constant of water is 1.86 °C/m.

A solution is prepared by dissolving calcium chloride in water and diluting to 500.0 mL. If this solution contains 44 ppm chloride ions, the concentration of calcium ions is ppm.

The magnitudes of Kf and of Kb depend on the identity of the .

The concentration of KBr in a solution prepared by dissolving 2.21 g of KBr in 897 g of water is Molal.

The solubility of nitrogen gas in water at 25 °C and a nitrogen pressure of 1.0 atm is 6.9 × 10- 4 M. The solubility of nitrogen in water at a nitrogen pressure of 0.80 atm is M.

Ammonium nitrate (NH4NO3) dissolves readily in water even though the dissolution is endothermic by 26.4 kJ/mol. The solution process is spontaneous because _.

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?

Molality is defined as the .

A saturated solution .

The concentration of urea in a solution prepared by dissolving 16 g of urea in 39 g of H2O is % by mass. The molar mass of urea is 60.0 g/mol.

Introduction: Matter and Measurement

Atoms, Molecules, and Ions

Stoichiometry: Calculations With Chemical Formulas and Equations

Aqueous Reactions and Solution Stoichiometry

Electronic Structure of Atoms

Periodic Properties of the Elements

Basic Concepts of Chemical Bonding

Gases

Intermolecular Forces, Liquids, and Solids

Modern Materials

Chemical Kinetics

Chemical Equilibrium

Acid-Base Equilibria

Additional Aspects of Equilibria

Chemistry of the Environment

Chemical Thermodynamics

Electrochemistry

Nuclear Chemistry

Chemistry of the Nonmetals

Metals and Metallurgy

Chemistry of Coordination Compounds

The Chemistry of Life: Organic and Biological Chemistry

Filters

The osmotic pressure of a solution formed by dissolving 25.0 mg of aspirin (C₉H₈O₄) in 0.250 L of water at 25 °C is atm.

The magnitudes of K_fand of K_bdepend on the identity of the .

The solubility of nitrogen gas in water at 25 °C and a nitrogen pressure of 1.0 atm is 6.9 × 10^-⁴M. The solubility of nitrogen in water at a nitrogen pressure of 0.80 atm is M.

Ammonium nitrate (NH₄NO₃) dissolves readily in water even though the dissolution is endothermic by 26.4 kJ/mol. The solution process is spontaneous because _.

The concentration of urea in a solution prepared by dissolving 16 g of urea in 39 g of H₂O is % by mass. The molar mass of urea is 60.0 g/mol.