Question 1

From the following list of aqueous solutions and water, select the one with the lowest freezing point.

Accepted Answer

A)  0.75 m (NH4)3PO4 
B)  1.0 m CaSO4 
C)  1.0 m LiClO4 
D)  1.5 m CH3OH, methyl alcohol 
E)  pure water 
A)  0.75 m (NH4)3PO4 
B)  1.0 m CaSO4 
C)  1.0 m LiClO4 
D)  1.5 m CH3OH, methyl alcohol 
E)  pure water A

Question 2

Saccharin, one of the first non-nutritive sweeteners used in soft-drinks, is 500 times sweeter than sugar in dilute aqueous solutions. The solubility of saccharin is 1.00 gram per 290 mL of solution. What is the molarity of a saturated saccharin solution? (   saccharin = 183.2 g/mol)

Accepted Answer

A)  0.0188 M 
B)  0.632 M 
C)  1.58 M 
D)  3.45 M 
E)  none of the above 
A)  0.0188 M 
B)  0.632 M 
C)  1.58 M 
D)  3.45 M 
E)  none of the above A

Question 3

What concentration of aqueous FeCl3 would have the same osmotic pressure as a 0.20 M solution of CaCl2 at the same temperature, assuming ideal behavior?

Accepted Answer

A)  0.60 M 
B)  0.40 M 
C)  0.30 M 
D)  0.15 M 
E)  0.10 M 
A)  0.60 M 
B)  0.40 M 
C)  0.30 M 
D)  0.15 M 
E)  0.10 M D

Question 4

Two aqueous are prepared: 1.00 m Na2CO3 and 1.00 m LiCl. Which of the following statements is true?

Accepted Answer

A)  The Na2CO3 solution has a higher osmotic pressure and higher vapor pressure than the LiCl solution. 
B)  The Na2CO3 solution has a higher osmotic pressure and higher boiling point than the LiCl solution. 
C)  The Na2CO3 solution has a lower osmotic pressure and lower vapor pressure than the LiCI solution. 
D)  The Na2CO3 solution has a lower osmotic pressure and higher boiling point than the LiCl solution. 
E)  None of the above statements is true. 
A)  The Na2CO3 solution has a higher osmotic pressure and higher vapor pressure than the LiCl solution. 
B)  The Na2CO3 solution has a higher osmotic pressure and higher boiling point than the LiCl solution. 
C)  The Na2CO3 solution has a lower osmotic pressure and lower vapor pressure than the LiCI solution. 
D)  The Na2CO3 solution has a lower osmotic pressure and higher boiling point than the LiCl solution. 
E)  None of the above statements is true.

Question 5

Ideal solutions do not conform to Raoult's Law.

Accepted Answer

A) True 
 B)False

Question 6

Calculate the vapor pressure of a solution prepared by dissolving 0.500 mol of a non-volatile solute in 275 g of hexane (   = 86.18 g/mol) at 49.6°C. P°hexane = 400.0 torr at 49.6°C.

Accepted Answer

A)  54 torr 
B)  154 torr 
C)  246 torr 
D)  346 torr 
E)  400. torr 
A)  54 torr 
B)  154 torr 
C)  246 torr 
D)  346 torr 
E)  400. torr

Question 7

A solution of ethanol (C2H6O) in water is sometimes used as a disinfectant. 1.00 L of this solution contains 553 g of ethanol and 335 g of water. What is the molality of the ethanol in this solution?

Accepted Answer

A)  0.392 m 
B)  0.608 m 
C)  13.5 m 
D)  33.6 m 
E)  35.8 m 
A)  0.392 m 
B)  0.608 m 
C)  13.5 m 
D)  33.6 m 
E)  35.8 m

Question 8

Cinnamaldehyde (   = 132.15 g/mol) is used as a flavoring agent. What mass of cinnamaldehyde must be added to 175 g of ethanol to give a solution whose boiling point is 82.7°C? Kb = 1.22°C/m, boiling point of pure ethanol = 78.5°C

Accepted Answer

A)  62.4 g 
B)  67.8 g 
C)  76.2 g 
D)  78.5 g 
E)  79.6 g 
A)  62.4 g 
B)  67.8 g 
C)  76.2 g 
D)  78.5 g 
E)  79.6 g

Question 9

Carbon tetrachloride, once widely used in fire extinguishers and as a dry cleaning fluid, has been found to cause liver damage to those exposed to its vapors over long periods of time. What is the boiling point of a solution prepared by dissolving 375 g of sulfur (S8,   = 256.5 g/mol) in 1250 g of CCl4? Kb = 5.05°C/m, boiling point of pure CCl4 = 76.7°C?

Accepted Answer

A)  70.8°C 
B)  75.2°C 
C)  78.2°C 
D)  82.6°C 
E)  >85°C 
A)  70.8°C 
B)  75.2°C 
C)  78.2°C 
D)  82.6°C 
E)  >85°C

Question 10

Procaine hydrochloride (   = 272.77 g/mol) is used as a local anesthetic. Calculate the molarity of a 4.666 m solution which has a density of 1.1066 g/mL.

Accepted Answer

A)  2.272 M 
B)  4.056 M 
C)  4.216 M 
D)  4.666 M 
E)  none of the above 
A)  2.272 M 
B)  4.056 M 
C)  4.216 M 
D)  4.666 M 
E)  none of the above

Question 11

The most abundant molecules in the cell membranes of most species are

Accepted Answer

A)  proteins. 
B)  sugars. 
C)  phospholipids. 
D)  fatty acids. 
E)  steroids. 
A)  proteins. 
B)  sugars. 
C)  phospholipids. 
D)  fatty acids. 
E)  steroids.

Question 12

A 0.100 m MgSO4 solution has a freezing point of -0.23°C. What is the van't Hoff factor for this solution? Kf = 1.86°C/m

Accepted Answer

A)  0.62 
B)  1.0 
C)  1.2 
D)  2.0 
E)  4.0 
A)  0.62 
B)  1.0 
C)  1.2 
D)  2.0 
E)  4.0

Question 13

In general, water is a good solvent for both polar and non-polar compounds.

Accepted Answer

A) True 
 B)False

Question 14

Electrolyte solutions generally behave less ideally as the solute concentration increases.

Accepted Answer

A) True 
 B)False

Question 15

Select the strongest electrolyte from the following set.

Accepted Answer

A)  CH3CH2OH, ethanol 
B)  LiNO3 
C)  C6H12O6, glucose 
D)  CCl4 
E)  HF 
A)  CH3CH2OH, ethanol 
B)  LiNO3 
C)  C6H12O6, glucose 
D)  CCl4 
E)  HF

Question 16

The solubility of gases in water increases with increase in the pressure of the gas.

Accepted Answer

A) True 
 B)False

Question 17

A 0.89% (w/v) sodium chloride solution is referred to as physiological saline solution because it has the same concentration of salts as human blood. What is the molarity of a physiological saline solution?

Accepted Answer

A)  0.0028 M 
B)  0.015 M 
C)  0.15 M 
D)  0.30 M 
E)  0.35 M 
A)  0.0028 M 
B)  0.015 M 
C)  0.15 M 
D)  0.30 M 
E)  0.35 M

Question 18

Which of the following pairs of ions is arranged so that the ion with the larger (i.e., more negative) heat of hydration is listed first?

Accepted Answer

A)  Br-, K+ 
B)  Mg2+, Sr 2+ 
C)  Ca2+, Sc3+ 
D)  Na+, Li+ 
E)  None of the above are arranged in this way. 
A)  Br-, K+ 
B)  Mg2+, Sr 2+ 
C)  Ca2+, Sc3+ 
D)  Na+, Li+ 
E)  None of the above are arranged in this way.

Question 19

Select the type of interaction which best describes the attraction between Mg2+ ions and water molecules.

Accepted Answer

A)  dipole-dipole 
B)  dipole-induced dipole 
C)  ion-dipole 
D)  ion-induced dipole 
E)  ion-hydrogen bond 
A)  dipole-dipole 
B)  dipole-induced dipole 
C)  ion-dipole 
D)  ion-induced dipole 
E)  ion-hydrogen bond

Question 20

An emulsion is a dispersion consisting of a

Accepted Answer

A)  solid in a liquid. 
B)  liquid in a liquid. 
C)  gas in a liquid. 
D)  liquid in a solid. 
E)  gas in a solid. 
A)  solid in a liquid. 
B)  liquid in a liquid. 
C)  gas in a liquid. 
D)  liquid in a solid. 
E)  gas in a solid.

Exam 13: The Properties of Mixtures: Solutions and Colloids

From the following list of aqueous solutions and water, select the one with the lowest freezing point.

Saccharin, one of the first non-nutritive sweeteners used in soft-drinks, is 500 times sweeter than sugar in dilute aqueous solutions. The solubility of saccharin is 1.00 gram per 290 mL of solution. What is the molarity of a saturated saccharin solution? ( saccharin = 183.2 g/mol)

What concentration of aqueous FeCl3 would have the same osmotic pressure as a 0.20 M solution of CaCl2 at the same temperature, assuming ideal behavior?

Two aqueous are prepared: 1.00 m Na2CO3 and 1.00 m LiCl. Which of the following statements is true?

Ideal solutions do not conform to Raoult's Law.

Calculate the vapor pressure of a solution prepared by dissolving 0.500 mol of a non-volatile solute in 275 g of hexane ( = 86.18 g/mol) at 49.6°C. P°hexane = 400.0 torr at 49.6°C.

A solution of ethanol (C2H6O) in water is sometimes used as a disinfectant. 1.00 L of this solution contains 553 g of ethanol and 335 g of water. What is the molality of the ethanol in this solution?

Cinnamaldehyde ( = 132.15 g/mol) is used as a flavoring agent. What mass of cinnamaldehyde must be added to 175 g of ethanol to give a solution whose boiling point is 82.7°C? Kb = 1.22°C/m, boiling point of pure ethanol = 78.5°C

Procaine hydrochloride ( = 272.77 g/mol) is used as a local anesthetic. Calculate the molarity of a 4.666 m solution which has a density of 1.1066 g/mL.

The most abundant molecules in the cell membranes of most species are

A 0.100 m MgSO4 solution has a freezing point of -0.23°C. What is the van't Hoff factor for this solution? Kf = 1.86°C/m

In general, water is a good solvent for both polar and non-polar compounds.

Electrolyte solutions generally behave less ideally as the solute concentration increases.

Select the strongest electrolyte from the following set.

The solubility of gases in water increases with increase in the pressure of the gas.

A 0.89% (w/v) sodium chloride solution is referred to as physiological saline solution because it has the same concentration of salts as human blood. What is the molarity of a physiological saline solution?

Which of the following pairs of ions is arranged so that the ion with the larger (i.e., more negative) heat of hydration is listed first?

Select the type of interaction which best describes the attraction between Mg2+ ions and water molecules.

An emulsion is a dispersion consisting of a

Keys to the Study of Chemistry

The Components of Matter

Stoichiometry of Formulas and Equations

The Major Classes of Chemical Reactions

Gases and the Kinetic-Molecular Theory

Thermochemistry: Energy Flow and Chemical Change

Quantum Theory and Atomic Structure

Electron Configuration and Chemical Periodicity

Models of Chemical Bonding

The Shapes of Molecules

Theories of Covalent Bonding

Intermolecular Forces: Liquids, Solids, and Phase Changes

Periodic Patterns in the Main Group Elements: Bonding, Structure, and Reactivity

Organic Compounds and the Atomic Properties of Carbon

Kinetics: Rates and Mechanisms of Chemical Reactions

Equilibrium: the Extent of Chemical Reactions

Acid-Base Equilibria

Ionic Equilibria in Aqueous Systems

Thermodynamics: Entropy, Free Energy, and the Direction of Chemical Reactions

Electrochemistry: Chemical Change and Electrical Work

The Elements in Nature and Industry

The Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

Filters

Saccharin, one of the first non-nutritive sweeteners used in soft-drinks, is 500 times sweeter than sugar in dilute aqueous solutions. The solubility of saccharin is 1.00 gram per 290 mL of solution. What is the molarity of a saturated saccharin solution? ( _saccharin = 183.2 g/mol)

What concentration of aqueous FeCl₃ would have the same osmotic pressure as a 0.20 M solution of CaCl₂ at the same temperature, assuming ideal behavior?

Two aqueous are prepared: 1.00 m Na₂CO₃and 1.00 m LiCl. Which of the following statements is true?

Calculate the vapor pressure of a solution prepared by dissolving 0.500 mol of a non-volatile solute in 275 g of hexane ( = 86.18 g/mol) at 49.6°C. P°_hexane = 400.0 torr at 49.6°C.

A solution of ethanol (C₂H₆O) in water is sometimes used as a disinfectant. 1.00 L of this solution contains 553 g of ethanol and 335 g of water. What is the molality of the ethanol in this solution?

Cinnamaldehyde ( = 132.15 g/mol) is used as a flavoring agent. What mass of cinnamaldehyde must be added to 175 g of ethanol to give a solution whose boiling point is 82.7°C? K_b = 1.22°C/m, boiling point of pure ethanol = 78.5°C

A 0.100 m MgSO₄solution has a freezing point of -0.23°C. What is the van't Hoff factor for this solution? K_f = 1.86°C/m

Select the type of interaction which best describes the attraction between Mg²⁺ions and water molecules.