Question 1

If the density of a solution is less than 1.0 g/mL, its molarity will be greater than its molality.

Accepted Answer

A) True 
 B)False  False

Question 2

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 these choices are correct. 
A)  2.272 M 
B)  4.056 M 
C)  4.216 M 
D)  4.666 M 
E)  None of these choices are correct. A

Question 3

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 these choices are correct. 
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 these choices are correct. B

Question 4

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

Question 5

Which of the following statements describes the correct method of preparation of 1.00 L of a 2.0 M urea solution?   urea = 60.06 g/mol

Accepted Answer

A)  Dissolve 120 g of urea in 1.00 kg of distilled water. 
B)  Dissolve 120 g of urea in 880 g of distilled water. 
C)  Dissolve 120 g of urea in enough distilled water to produce 1.00 L of solution. 
D)  Dissolve 120 g of urea in 1.00 liter of distilled water. 
E)  The density of urea is needed in order to do this calculation. 
A)  Dissolve 120 g of urea in 1.00 kg of distilled water. 
B)  Dissolve 120 g of urea in 880 g of distilled water. 
C)  Dissolve 120 g of urea in enough distilled water to produce 1.00 L of solution. 
D)  Dissolve 120 g of urea in 1.00 liter of distilled water. 
E)  The density of urea is needed in order to do this calculation.

Question 6

What is the mole fraction of Ne in a mixture containing 10.1 g of Ne, 79.9 g of Ar, and 83.8 g of Kr?

Accepted Answer

A)  0.40 
B)  0.25 
C)  0.20 
D)  0.14 
E)  0.058 
A)  0.40 
B)  0.25 
C)  0.20 
D)  0.14 
E)  0.058

Question 7

The Tyndall effect

Accepted Answer

A)  is observed in concentrated solutions. 
B)  is observed only in dilute solutions. 
C)  is observed in colloidal dispersions. 
D)  is caused by Brownian motion. 
E)  is used to determine the osmotic pressure of solutions. 
A)  is observed in concentrated solutions. 
B)  is observed only in dilute solutions. 
C)  is observed in colloidal dispersions. 
D)  is caused by Brownian motion. 
E)  is used to determine the osmotic pressure of solutions.

Question 8

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

Accepted Answer

A) True 
 B)False

Question 9

How many moles of sulfate ions are present in 1.0 L of 0.5 M Li2SO4?

Accepted Answer

A)  0.5 mol 
B)  1.0 mol 
C)  1.5 mol 
D)  2.0 mol 
E)  3.0 mol 
A)  0.5 mol 
B)  1.0 mol 
C)  1.5 mol 
D)  2.0 mol 
E)  3.0 mol

Question 10

Dimethylglyoxime, DMG, is an organic compound used to test for aqueous nickel(II) ions. A solution prepared by dissolving 65.0 g of DMG in 375 g of ethanol boils at 80.3°C. What is the molar mass of DMG? Kb = 1.22°C/m, boiling point of pure ethanol = 78.5°C

Accepted Answer

A)  44.1 g/mol 
B)  65.8 g/mol 
C)  117 g/mol 
D)  131.6 g/mol 
E)  553 g/mol 
A)  44.1 g/mol 
B)  65.8 g/mol 
C)  117 g/mol 
D)  131.6 g/mol 
E)  553 g/mol

Question 11

A saturated solution of carbon dioxide in water contains 3.00 g of CO2 when the CO2 partial pressure is 8.0 atm. What mass of CO2 will escape if the partial pressure is lowered to 3.2 atm?

Accepted Answer

A)  0.90 g 
B)  1.20 g 
C)  1.40 g 
D)  1.80 g 
E)  2.20 g 
A)  0.90 g 
B)  1.20 g 
C)  1.40 g 
D)  1.80 g 
E)  2.20 g

Question 12

The vapor pressure of pure acetone (propanone) is 266 torr. When a non-volatile solute is added, the vapor pressure of acetone above the solution falls to 232 torr. What is the mole fraction of acetone in the solution?

Accepted Answer

A)  0.87 
B)  0.69 
C)  0.32 
D)  0.13 
E)  0.045 
A)  0.87 
B)  0.69 
C)  0.32 
D)  0.13 
E)  0.045

Question 13

Which, if any, of the following features is common to soaps, detergents, phospholipids, and channel-forming antibiotics?

Accepted Answer

A)  They all contain fatty acids. 
B)  They all contain phosphate groups. 
C)  They all contain polypeptide chains. 
D)  Their function depends on the dual polarity of their molecules. 
E)  None of these choices are correct. 
A)  They all contain fatty acids. 
B)  They all contain phosphate groups. 
C)  They all contain polypeptide chains. 
D)  Their function depends on the dual polarity of their molecules. 
E)  None of these choices are correct.

Question 14

A 2.0% (w/v) solution of sodium hydrogen citrate, Na2C6H6O7, which also contains 2.5% (w/v) of dextrose, C6H12O6, is used as an anticoagulant for blood which is to be used for transfusions. What is the molarity of the sodium hydrogen citrate in the solution?

Accepted Answer

A)  0.085 M 
B)  0.19 M 
C)  0.53 M 
D)  1.2 M 
E)  1.3 M 
A)  0.085 M 
B)  0.19 M 
C)  0.53 M 
D)  1.2 M 
E)  1.3 M

Question 15

For a given solution, which of the following concentration values will change as temperature changes?

Accepted Answer

A)  mass percent 
B)  molality 
C)  mole fraction 
D)  molarity 
E)  None of these choices are correct. 
A)  mass percent 
B)  molality 
C)  mole fraction 
D)  molarity 
E)  None of these choices are correct.

Question 16

Which one of the following pairs of dispersed phases and dispersing media can never form a colloid?

Accepted Answer

A)  solid and gas 
B)  liquid and gas 
C)  solid and solid 
D)  liquid and liquid 
E)  gas and gas 
A)  solid and gas 
B)  liquid and gas 
C)  solid and solid 
D)  liquid and liquid 
E)  gas and gas

Question 17

The shape of a protein molecule is determined completely by

Accepted Answer

A)  hydrogen bonding. 
B)  ion-dipole attractions. 
C)  dispersion forces. 
D)  disulfide bridges. 
E)  the sequence of amino acids in the chain. 
A)  hydrogen bonding. 
B)  ion-dipole attractions. 
C)  dispersion forces. 
D)  disulfide bridges. 
E)  the sequence of amino acids in the chain.

Question 18

Soda drinks bubble when the bottle is opened because

Accepted Answer

A)  the temperature of the soda increases. 
B)  exposure to atmospheric pressure squeezes the carbon dioxide from solution. 
C)  the partial pressure of carbon dioxide above the solution is reduced. 
D)  atmospheric nitrogen molecules displace carbon dioxide molecules. 
E)  the Henry's law constant changes due to the change in pressure. 
A)  the temperature of the soda increases. 
B)  exposure to atmospheric pressure squeezes the carbon dioxide from solution. 
C)  the partial pressure of carbon dioxide above the solution is reduced. 
D)  atmospheric nitrogen molecules displace carbon dioxide molecules. 
E)  the Henry's law constant changes due to the change in pressure.

Question 19

Which of the following ions will be expected to have the most negative heat of hydration, ΔHhydr?

Accepted Answer

A)  Na+ 
B)  Cs+ 
C)  Ca2+ 
D)  F- 
E)  I- 
A)  Na+ 
B)  Cs+ 
C)  Ca2+ 
D)  F- 
E)  I-

Question 20

Which of the following sets of conditions could exist when two liquids which are completely miscible in one another are mixed?

Accepted Answer

A)  ΔHsoln > 0, entropy of system decreases 
B)  ΔHsoln ≈ 0, entropy of system decreases 
C)  ΔHsoln ≈ 0, entropy change of system ≈ 0 
D)  ΔHsoln ≈ 0, entropy of system increases 
E)  None of these choices are correct. 
A)  ΔHsoln > 0, entropy of system decreases 
B)  ΔHsoln ≈ 0, entropy of system decreases 
C)  ΔHsoln ≈ 0, entropy change of system ≈ 0 
D)  ΔHsoln ≈ 0, entropy of system increases 
E)  None of these choices are correct.

Exam 13: The Properties of Mixtures Solutions and Colloids

If the density of a solution is less than 1.0 g/mL, its molarity will be greater than its molality.

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.

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

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?

Which of the following statements describes the correct method of preparation of 1.00 L of a 2.0 M urea solution? urea = 60.06 g/mol

What is the mole fraction of Ne in a mixture containing 10.1 g of Ne, 79.9 g of Ar, and 83.8 g of Kr?

The Tyndall effect

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

How many moles of sulfate ions are present in 1.0 L of 0.5 M Li2SO4?

Dimethylglyoxime, DMG, is an organic compound used to test for aqueous nickel(II) ions. A solution prepared by dissolving 65.0 g of DMG in 375 g of ethanol boils at 80.3°C. What is the molar mass of DMG? Kb = 1.22°C/m, boiling point of pure ethanol = 78.5°C

A saturated solution of carbon dioxide in water contains 3.00 g of CO2 when the CO2 partial pressure is 8.0 atm. What mass of CO2 will escape if the partial pressure is lowered to 3.2 atm?

The vapor pressure of pure acetone (propanone) is 266 torr. When a non-volatile solute is added, the vapor pressure of acetone above the solution falls to 232 torr. What is the mole fraction of acetone in the solution?

Which, if any, of the following features is common to soaps, detergents, phospholipids, and channel-forming antibiotics?

A 2.0% (w/v) solution of sodium hydrogen citrate, Na2C6H6O7, which also contains 2.5% (w/v) of dextrose, C6H12O6, is used as an anticoagulant for blood which is to be used for transfusions. What is the molarity of the sodium hydrogen citrate in the solution?

For a given solution, which of the following concentration values will change as temperature changes?

Which one of the following pairs of dispersed phases and dispersing media can never form a colloid?

The shape of a protein molecule is determined completely by

Soda drinks bubble when the bottle is opened because

Which of the following ions will be expected to have the most negative heat of hydration, ΔHhydr?

Which of the following sets of conditions could exist when two liquids which are completely miscible in one another are mixed?

Keys to Studying Chemistry Definitions, Units, and Problem Solving

The Components of Matter

Stoichiometry of Formulas and Equations

Three 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

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 Reaction Direction

Electrochemistry Chemical Change and Electrical Work

The Elements in Nature and Industry

Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

Filters

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

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?

Which of the following statements describes the correct method of preparation of 1.00 L of a 2.0 M urea solution? _urea = 60.06 g/mol

How many moles of sulfate ions are present in 1.0 L of 0.5 M Li₂SO₄?

Dimethylglyoxime, DMG, is an organic compound used to test for aqueous nickel(II) ions. A solution prepared by dissolving 65.0 g of DMG in 375 g of ethanol boils at 80.3°C. What is the molar mass of DMG? K_b = 1.22°C/m, boiling point of pure ethanol = 78.5°C

A saturated solution of carbon dioxide in water contains 3.00 g of CO₂ when the CO₂ partial pressure is 8.0 atm. What mass of CO₂ will escape if the partial pressure is lowered to 3.2 atm?

A 2.0% (w/v) solution of sodium hydrogen citrate, Na₂C₆H₆O₇, which also contains 2.5% (w/v) of dextrose, C₆H₁₂O₆, is used as an anticoagulant for blood which is to be used for transfusions. What is the molarity of the sodium hydrogen citrate in the solution?

Which of the following ions will be expected to have the most negative heat of hydration, ΔH_hydr?