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

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)   0.058F) B) and E)
G) B) and D)

Question 3

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.F) B) and E)
G) A) and D) A

Question 4

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 gF) A) and B)
G) B) and E)

Question 5

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

Accepted Answer

A) True 
 B)False

Question 6

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.F) A) and E)
G) A) and D)

Question 7

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.F) A) and D)
G) B) and C)

Question 8

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)   0.045F) B) and D)
G) B) and C)

Question 9

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.F) B) and D)
G) A) and C)

Question 10

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 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." class="answers-bank-image d-inline" rel="preload" > 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.F) A) and C)
G) C) and D)

Question 11

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-F) C) and D)
G) A) and B)

Question 12

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.F) None of the above
G) C) and D)

Question 13

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 gasF) A) and E)
G) A) and B)

Question 14

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.F) C) and D)
G) B) and C)

Question 15

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 MF) All of the above
G) C) and E)

Question 16

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/molF) A) and B)
G) B) and E)

Question 17

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.F) B) and C)
G) C) and D)

Question 18

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 MF) A) and D)
G) A) and E)

Question 19

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.F) All of the above
G) B) and C) B

Question 20

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 molF) B) and E)
G) B) and D)

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.

Correct AnswerverifiedFalse

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?

Correct AnswerverifiedShow Answer

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.

Correct AnswerverifiedA

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?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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?

Correct AnswerverifiedShow Answer

Soda drinks bubble when the bottle is opened because

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

The Tyndall effect

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

The shape of a protein molecule is determined completely by

Correct AnswerverifiedShow Answer

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?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedB

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

Correct AnswerverifiedShow Answer

Correct Answer
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False

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A

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?

Correct Answer
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Correct Answer
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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

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

Correct Answer
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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?

Correct Answer
verified

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

Correct Answer
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Correct Answer
verified

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?

Correct Answer
verified

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

Correct Answer
verified
B

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

Correct Answer
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