Question 1

Which of the following statements is generally 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 2

Choose the statement below that is TRUE.

Accepted Answer

A)  A solution will form between two substances if the solute-solvent interactions are of comparable strength to the solute-solute and solvent-solvent interactions. 
B)  A solution will form between two substances if the solute-solvent interactions are small enough to be overcome by the solute-solute and solvent-solvent interactions. 
C)  A solution will form between two substances if the solute-solute interactions are strong enough to overcome the solvent-solvent interactions. 
D)  A solution will form between two substances only if the solvent-solvent interactions are weak enough to overcome the solute-solvent interactions. 
E)  None of the above is true. 
A)  A solution will form between two substances if the solute-solvent interactions are of comparable strength to the solute-solute and solvent-solvent interactions. 
B)  A solution will form between two substances if the solute-solvent interactions are small enough to be overcome by the solute-solute and solvent-solvent interactions. 
C)  A solution will form between two substances if the solute-solute interactions are strong enough to overcome the solvent-solvent interactions. 
D)  A solution will form between two substances only if the solvent-solvent interactions are weak enough to overcome the solute-solvent interactions. 
E)  None of the above is true.

Question 3

Why isn't pentanol (CH3CH2CH2CH2CH2OH)very soluble in water?

Accepted Answer

Even though the pentanol molecule contai

Question 4

Solutions having osmotic pressures more than those of body fluids are called

Accepted Answer

A)  isosmotic. 
B)  hyperosmotic. 
C)  hyposmotic. 
D)  neosmotic. 
E)  magnosmotic. 
A)  isosmotic. 
B)  hyperosmotic. 
C)  hyposmotic. 
D)  neosmotic. 
E)  magnosmotic.

Question 5

Identify the major force between molecules of pentane.

Accepted Answer

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

Question 6

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

Question 7

A solution is formed at room temperature by vigorously dissolving enough of the solid solute so that some solid remains at the bottom of the solution.Which statement below is TRUE?

Accepted Answer

A)  The solution is considered unsaturated. 
B)  The solution is considered supersaturated. 
C)  The solution is considered saturated. 
D)  The solution would be considered unsaturated if it were cooled a bit to increase the solubility of the solid. 
E)  None of the above is true. 
A)  The solution is considered unsaturated. 
B)  The solution is considered supersaturated. 
C)  The solution is considered saturated. 
D)  The solution would be considered unsaturated if it were cooled a bit to increase the solubility of the solid. 
E)  None of the above is true.

Question 8

Determine the molality of an aqueous solution prepared by dissolving 0.224 moles of LiBr in 27.4 moles of H2O.

Accepted Answer

A)  0.454 m 
B)  0.220 m 
C)  0.818 m 
D)  0.122 m 
E)  0.153 m 
A)  0.454 m 
B)  0.220 m 
C)  0.818 m 
D)  0.122 m 
E)  0.153 m

Question 9

Calculate the freezing point of a solution of 500.0 g of ethylene glycol (C2H6O2)dissolved in 500.0 g of water.Kf = 1.86°C/m and Kb = 0.512°C/m.

Accepted Answer

A)  30.0°C 
B)  -30.0°C 
C)  8.32°C 
D)  -8.32°C 
E)  70.2°C 
A)  30.0°C 
B)  -30.0°C 
C)  8.32°C 
D)  -8.32°C 
E)  70.2°C

Question 10

A solution is prepared by dissolving 76.3 g NaI in 545 g of water.Determine the mole fraction of NaI if the final volume of the solution is 576 mL.

Accepted Answer

A)  6.04 × 10-3 
B)  1.65 × 10-2 
C)  1.40 × 10-3 
D)  1.32 × 10-2 
E)  8.84 × 10-2 
A)  6.04 × 10-3 
B)  1.65 × 10-2 
C)  1.40 × 10-3 
D)  1.32 × 10-2 
E)  8.84 × 10-2

Question 11

Choose the solvent below that would show the greatest boiling point elevation when used to make a 0.10 m nonelectrolyte solution.

Accepted Answer

A)  bromobenzene, Kb = 6.20°C/m 
B)  benzene, Kb = 2.53°C/m 
C)  carbon disulfide, Kb = 2.34°C/m 
D)  water, Kb = 0.512°C/m 
E)  methanol, Kb = 0.83°C/m 
A)  bromobenzene, Kb = 6.20°C/m 
B)  benzene, Kb = 2.53°C/m 
C)  carbon disulfide, Kb = 2.34°C/m 
D)  water, Kb = 0.512°C/m 
E)  methanol, Kb = 0.83°C/m

Question 12

How does a solution of two volatile components with strong solute-solvent attractions deviate from Raoult's law? Why?

Accepted Answer

The vapor pressure of the solution will

Question 13

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 14

Identify the gas that is dissolved in carbonated sodas.

Accepted Answer

A)  carbon dioxide 
B)  ammonia 
C)  helium 
D)  carbon monoxide 
E)  xenon 
A)  carbon dioxide 
B)  ammonia 
C)  helium 
D)  carbon monoxide 
E)  xenon

Question 15

Choose the aqueous solution that has the highest boiling point.These are all solutions of nonvolatile solutes and you should assume ideal van't Hoff factors where applicable.

Accepted Answer

A)  0.100 mKNO2 
B)  0.100 m Li2SO4 
C)  0.200 m C3H8O3 
D)  0.060 m Li3PO4 
E)  They all have the same boiling point. 
A)  0.100 mKNO2 
B)  0.100 m Li2SO4 
C)  0.200 m C3H8O3 
D)  0.060 m Li3PO4 
E)  They all have the same boiling point.

Question 16

Define colloid.

Accepted Answer

A colloid is a mixtu

Question 17

Define solubility.

Accepted Answer

A)  a solid that does not dissolve in a gas 
B)  the amount of a substance that will dissolve in a given amount of solvent 
C)  the amount of a substance that will dissolve in a given amount of solute 
D)  a solid mixed with another solid 
E)  a liquid that does not dissolve in another liquid 
A)  a solid that does not dissolve in a gas 
B)  the amount of a substance that will dissolve in a given amount of solvent 
C)  the amount of a substance that will dissolve in a given amount of solute 
D)  a solid mixed with another solid 
E)  a liquid that does not dissolve in another liquid

Question 18

Choose the aqueous solution that has the highest boiling point.These are all solutions of nonvolatile solutes and you should assume ideal van't Hoff factors where applicable.

Accepted Answer

A)  0.100 m AlCl3 
B)  0.100 m LiBr 
C)  0.100 m BaCl2 
D)  0.100 m C6H12O6 
E)  They all have the same boiling point. 
A)  0.100 m AlCl3 
B)  0.100 m LiBr 
C)  0.100 m BaCl2 
D)  0.100 m C6H12O6 
E)  They all have the same boiling point.

Question 19

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

Accepted Answer

A)  Xe 
B)  CO 
C)  H2 
D)  CH3CH3 
E)  CO2 
A)  Xe 
B)  CO 
C)  H2 
D)  CH3CH3 
E)  CO2

Question 20

Light beams that are visible in a dusty room is an example of

Accepted Answer

A)  an emulsion. 
B)  an aerosol. 
C)  micelle repulsion. 
D)  Brownian motion. 
E)  Tyndall effect. 
A)  an emulsion. 
B)  an aerosol. 
C)  micelle repulsion. 
D)  Brownian motion. 
E)  Tyndall effect.

Exam 13: Solutions

Which of the following statements is generally TRUE?

Choose the statement below that is TRUE.

Why isn't pentanol (CH3CH2CH2CH2CH2OH)very soluble in water?

Solutions having osmotic pressures more than those of body fluids are called

Identify the major force between molecules of pentane.

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.

A solution is formed at room temperature by vigorously dissolving enough of the solid solute so that some solid remains at the bottom of the solution.Which statement below is TRUE?

Determine the molality of an aqueous solution prepared by dissolving 0.224 moles of LiBr in 27.4 moles of H2O.

Calculate the freezing point of a solution of 500.0 g of ethylene glycol (C2H6O2)dissolved in 500.0 g of water.Kf = 1.86°C/m and Kb = 0.512°C/m.

A solution is prepared by dissolving 76.3 g NaI in 545 g of water.Determine the mole fraction of NaI if the final volume of the solution is 576 mL.

Choose the solvent below that would show the greatest boiling point elevation when used to make a 0.10 m nonelectrolyte solution.

How does a solution of two volatile components with strong solute-solvent attractions deviate from Raoult's law? Why?

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.

Identify the gas that is dissolved in carbonated sodas.

Choose the aqueous solution that has the highest boiling point.These are all solutions of nonvolatile solutes and you should assume ideal van't Hoff factors where applicable.

Define colloid.

Define solubility.

Choose the aqueous solution that has the highest boiling point.These are all solutions of nonvolatile solutes and you should assume ideal van't Hoff factors where applicable.

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

Light beams that are visible in a dusty room is an example of

Matter, measurement, and Problem Solving

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Chemical Quantities and Aqueous Reactions

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Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding Ii: Molecular Shapes,valence Bond Theory,

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Filters

Why isn't pentanol (CH₃CH₂CH₂CH₂CH₂OH)very soluble in water?

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.

Determine the molality of an aqueous solution prepared by dissolving 0.224 moles of LiBr in 27.4 moles of H₂O.

Calculate the freezing point of a solution of 500.0 g of ethylene glycol (C₂H₆O₂)dissolved in 500.0 g of water.K_f = 1.86°C/m and K_b = 0.512°C/m.

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