Question 1

Liquid A has vapor pressure x. Liquid B has vapor pressure y, and x > y. What is the mole fraction of A in the liquid mixture if the vapor above the solution is 50% A?

Accepted Answer

A)  y/(2x + 2y) 
B)  y/(x + y) 
C)  x/(2x + 2y) 
D)  x/(x + y) 
E)  none of these 
A)  y/(2x + 2y) 
B)  y/(x + y) 
C)  x/(2x + 2y) 
D)  x/(x + y) 
E)  none of these

Question 2

A 54.4-g sample of glucose (a nondissociated, nonvolatile solute with the formula C6H12O6) is dissolved in 154.4 g of water. What is the vapor pressure of this solution at 100°C?

Accepted Answer

A)  734 torr 
B)  562 torr 
C)  25.9 torr 
D)  760 torr 
E)  198 torr 
A)  734 torr 
B)  562 torr 
C)  25.9 torr 
D)  760 torr 
E)  198 torr

Question 3

An aqueous solution contains 48.6 g of KNO3 in 290.6 mL of solution. What is the molarity of the solution?

Accepted Answer

A)  0.140 M KNO3 
B)  0.167 M KNO3 
C)  1.65 M KNO3 
D)  0.00716 M KNO3 
E)  0.0591 M KNO3 
A)  0.140 M KNO3 
B)  0.167 M KNO3 
C)  1.65 M KNO3 
D)  0.00716 M KNO3 
E)  0.0591 M KNO3

Question 4

The solubility of O2 in water is 0.590 g/L at an oxygen pressure of 15 atm. What is the Henry's law constant for O2 (in units of L atm/mol)?

Accepted Answer

A)  3.93 F1F1F1S1F1F1F10 10-3 
B)  1.23 F1F1F1S1F1F1F10 10-3 
C)  8.14 F1F1F1S1F1F1F10 102 
D)  1.26 
E)  None of the above is within 5% of the correct answer. 
A)  3.93 F1F1F1S1F1F1F10 10-3 
B)  1.23 F1F1F1S1F1F1F10 10-3 
C)  8.14 F1F1F1S1F1F1F10 102 
D)  1.26 
E)  None of the above is within 5% of the correct answer.

Question 5

Which of the following concentration measures will change in value as the temperature of a solution changes?

Accepted Answer

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

Question 6

At a given temperature, you have a mixture of benzene (Pvap = 745 torr) and toluene (Pvap = 290 torr). The mole fraction of benzene in the solution is 0.590. Assuming ideal behavior, calculate the mole fraction of toluene in the vapor above the solution.

Accepted Answer

A)  0.778 
B)  0.641 
C)  0.355 
D)  0.213 
E)  0.590 
A)  0.778 
B)  0.641 
C)  0.355 
D)  0.213 
E)  0.590

Question 7

What is the boiling-point change for a solution containing 0.360 mol of naphthalene (a nonvolatile, nonionizing compound) in 258.0 g of liquid benzene? (Kb = 2.53°C/m for benzene)

Accepted Answer

A)  1.81°C 
B)  8.60°C 
C)  0.552°C 
D)  0.235°C 
E)  3.53°C 
A)  1.81°C 
B)  8.60°C 
C)  0.552°C 
D)  0.235°C 
E)  3.53°C

Question 8

You have a 10.40-g mixture of table sugar (C12H22O11) and table salt (NaCl). When this mixture is dissolved in 150. g of water, the freezing point is found to be -2.24°C. Calculate the percent by mass of sugar in the original mixture. (Assume that the NaCl is completely dissociated.)

Accepted Answer

A)  61.0% 
B)  53.8% 
C)  46.2% 
D)  39.0% 
E)  none of these 
A)  61.0% 
B)  53.8% 
C)  46.2% 
D)  39.0% 
E)  none of these

Question 9

What is the mole percent of ethanol (C2H5OH) in the 180 proof vodka, which consists of 71.0 g of ethanol for every 10.0 g of water present?

Accepted Answer

A)  87.7% 
B)  71.0% 
C)  73.5% 
D)  26.5% 
E)  22.1% 
A)  87.7% 
B)  71.0% 
C)  73.5% 
D)  26.5% 
E)  22.1%

Question 10

When a 18.4-g sample of an unknown compound is dissolved in 522.0 g of benzene, the freezing point of the resulting solution of 3.82°C. The freezing point of pure benzene is 5.48°C, and Kf for benzene is 5.12°C/m. Calculate the molar mass of the unknown compound.

Accepted Answer

A)  9.20 F1F1F1S1F1F1F10 103 g/mol 
B)  4.72 F1F1F1S1F1F1F10 101 g/mol 
C)  8.85 F1F1F1S1F1F1F10 102 g/mol 
D)  2.96 F1F1F1S1F1F1F10 101 g/mol 
E)  1.09 F1F1F1S1F1F1F10 102 g/mol 
A)  9.20 F1F1F1S1F1F1F10 103 g/mol 
B)  4.72 F1F1F1S1F1F1F10 101 g/mol 
C)  8.85 F1F1F1S1F1F1F10 102 g/mol 
D)  2.96 F1F1F1S1F1F1F10 101 g/mol 
E)  1.09 F1F1F1S1F1F1F10 102 g/mol

Question 11

A cucumber is placed in a concentrated salt solution. What is most likely to happen?

Accepted Answer

A)  Salt will precipitate out. 
B)  Water will flow from the solution to the cucumber. 
C)  Salt will flow into the cucumber. 
D)  Water will flow from the cucumber to the solution. 
E)  No change will occur. 
A)  Salt will precipitate out. 
B)  Water will flow from the solution to the cucumber. 
C)  Salt will flow into the cucumber. 
D)  Water will flow from the cucumber to the solution. 
E)  No change will occur.

Question 12

What is the molality of an HCl solution made by dissolving 150.0 g of HCl in 450.0 g of water?

Accepted Answer

The answer of What is the molality of an HCl...

Question 13

A chemist is given a white solid that is suspected of being pure cocaine. When 1.22 g of the solid is dissolved in 15.60 g of benzene, the freezing point is lowered by 1.32°C. Calculate the molar mass of the solid. The molal freezing-point constant (Kf) for benzene is 5.12°C/m.

Accepted Answer

@#LAT-DLM&T = K_fm = 1.32 = 5.

Question 14

Calculate the molality of a solution containing 21.0 g of C6H12O6 in 271.0 mL of water (assume a density of 1.00 g/mL).

Accepted Answer

A)  0.399 m 
B)  0.0719 m 
C)  0.000430 m 
D)  0.430 m 
E)  0.00768 m 
A)  0.399 m 
B)  0.0719 m 
C)  0.000430 m 
D)  0.430 m 
E)  0.00768 m

Question 15

A liquid-liquid solution is called an ideal solution if 
I. it obeys PV = nRT.
II. it obeys Raoult's law.
III. solute-solute, solvent-solvent, and solute-solvent interactions are very similar.
IV. solute-solute, solvent-solvent, and solute-solvent interactions are quite different.

Accepted Answer

A)  II, IV 
B)  II, III 
C)  I, II 
D)  I, II, III 
E)  I, II, IV 
A)  II, IV 
B)  II, III 
C)  I, II 
D)  I, II, III 
E)  I, II, IV

Question 16

If a solution exhibits a negative deviation from Raoult's law, the vapor pressure of the solution is __________ what would be expected ideally.

Accepted Answer

A)  equal to 
B)  greater than 
C)  less than 
A)  equal to 
B)  greater than 
C)  less than

Question 17

A solution contains 1 mol of liquid A and 3 mol of liquid B. The vapor pressure of this solution is 314 torr at 25°C. At 25°C, the vapor pressure of liquid A is 265 torr and the vapor pressure of liquid B is 355 torr. Which of the following is true?

Accepted Answer

A)  This solution exhibits a positive deviation from Raoult's law. 
B)  This solution is ideal. 
C)  This solution exhibits a negative deviation from Raoult's law. 
A)  This solution exhibits a positive deviation from Raoult's law. 
B)  This solution is ideal. 
C)  This solution exhibits a negative deviation from Raoult's law.

Question 18

When 200.0 mL of 0.200 M H2SO4 is diluted with 155.0 mL of water, what is the molarity of the solution?

Accepted Answer

A)  0.258 M 
B)  0.155 M 
C)  0.124 M 
D)  0.113 M 
E)  none of these 
A)  0.258 M 
B)  0.155 M 
C)  0.124 M 
D)  0.113 M 
E)  none of these

Question 19

The destruction of a colloid is called

Accepted Answer

A)  denaturation. 
B)  reconfiguration. 
C)  coagulation. 
D)  degeneration. 
E)  none of these 
A)  denaturation. 
B)  reconfiguration. 
C)  coagulation. 
D)  degeneration. 
E)  none of these

Question 20

What is the expected osmotic pressure, in torr, of a 0.0100 M solution of NaCl in water at 25°C?

Accepted Answer

A)  186 torr 
B)  0.245 torr 
C)  372 torr 
D)  15.6 torr 
E)  none of these 
A)  186 torr 
B)  0.245 torr 
C)  372 torr 
D)  15.6 torr 
E)  none of these

Liquid A has vapor pressure x. Liquid B has vapor pressure y, and x > y. What is the mole fraction of A in the liquid mixture if the vapor above the solution is 50% A?

A 54.4-g sample of glucose (a nondissociated, nonvolatile solute with the formula C₆H₁₂O₆) is dissolved in 154.4 g of water. What is the vapor pressure of this solution at 100°C?

An aqueous solution contains 48.6 g of KNO₃ in 290.6 mL of solution. What is the molarity of the solution?

The solubility of O₂ in water is 0.590 g/L at an oxygen pressure of 15 atm. What is the Henry's law constant for O₂ (in units of L atm/mol)?

Which of the following concentration measures will change in value as the temperature of a solution changes?

At a given temperature, you have a mixture of benzene (P_vap = 745 torr) and toluene (P_vap = 290 torr). The mole fraction of benzene in the solution is 0.590. Assuming ideal behavior, calculate the mole fraction of toluene in the vapor above the solution.

What is the boiling-point change for a solution containing 0.360 mol of naphthalene (a nonvolatile, nonionizing compound) in 258.0 g of liquid benzene? (K_b = 2.53°C/m for benzene)

You have a 10.40-g mixture of table sugar (C₁₂H₂₂O₁₁) and table salt (NaCl). When this mixture is dissolved in 150. g of water, the freezing point is found to be -2.24°C. Calculate the percent by mass of sugar in the original mixture. (Assume that the NaCl is completely dissociated.)

What is the mole percent of ethanol (C₂H₅OH) in the 180 proof vodka, which consists of 71.0 g of ethanol for every 10.0 g of water present?

When a 18.4-g sample of an unknown compound is dissolved in 522.0 g of benzene, the freezing point of the resulting solution of 3.82°C. The freezing point of pure benzene is 5.48°C, and K_f for benzene is 5.12°C/m. Calculate the molar mass of the unknown compound.

A cucumber is placed in a concentrated salt solution. What is most likely to happen?

What is the molality of an HCl solution made by dissolving 150.0 g of HCl in 450.0 g of water?

A chemist is given a white solid that is suspected of being pure cocaine. When 1.22 g of the solid is dissolved in 15.60 g of benzene, the freezing point is lowered by 1.32°C. Calculate the molar mass of the solid. The molal freezing-point constant (K_f) for benzene is 5.12°C/m.

Calculate the molality of a solution containing 21.0 g of C₆H₁₂O₆ in 271.0 mL of water (assume a density of 1.00 g/mL).

A liquid-liquid solution is called an ideal solution if I. it obeys PV = nRT. II. it obeys Raoult's law. III. solute-solute, solvent-solvent, and solute-solvent interactions are very similar. IV. solute-solute, solvent-solvent, and solute-solvent interactions are quite different.

If a solution exhibits a negative deviation from Raoult's law, the vapor pressure of the solution is __________ what would be expected ideally.

A solution contains 1 mol of liquid A and 3 mol of liquid B. The vapor pressure of this solution is 314 torr at 25°C. At 25°C, the vapor pressure of liquid A is 265 torr and the vapor pressure of liquid B is 355 torr. Which of the following is true?

When 200.0 mL of 0.200 M H₂SO₄ is diluted with 155.0 mL of water, what is the molarity of the solution?

The destruction of a colloid is called

What is the expected osmotic pressure, in torr, of a 0.0100 M solution of NaCl in water at 25°C?

Atoms, Molecules, and Ions

Stoichiometry

Chemical Reactions and Solutions Stoichiometry

Gases

Chemical Equilibrium

Acids and Bases

Applications of Aqueous Equilibria

Energy, Enthalpy, and Thermochemistry

Spontaneity, Entropy, and Free Energy

Electrochemistry

Quantum Mechanics and Atomic Theory

Bonding: General Concepts

Covalent Bonding: Orbitals

Chemical Kinetics

Liquids and Solids

The Representative Elements

Transition Metals and Coordination Chemistry

The Nucleus: a Chemists View

Organic and Biochemical Molecules

Filters

Exam 17: Properties of Solutions

Liquid A has vapor pressure x. Liquid B has vapor pressure y, and x > y. What is the mole fraction of A in the liquid mixture if the vapor above the solution is 50% A?

A 54.4-g sample of glucose (a nondissociated, nonvolatile solute with the formula C6H12O6) is dissolved in 154.4 g of water. What is the vapor pressure of this solution at 100°C?

An aqueous solution contains 48.6 g of KNO3 in 290.6 mL of solution. What is the molarity of the solution?

The solubility of O2 in water is 0.590 g/L at an oxygen pressure of 15 atm. What is the Henry's law constant for O2 (in units of L atm/mol)?

Which of the following concentration measures will change in value as the temperature of a solution changes?

At a given temperature, you have a mixture of benzene (Pvap = 745 torr) and toluene (Pvap = 290 torr). The mole fraction of benzene in the solution is 0.590. Assuming ideal behavior, calculate the mole fraction of toluene in the vapor above the solution.

What is the boiling-point change for a solution containing 0.360 mol of naphthalene (a nonvolatile, nonionizing compound) in 258.0 g of liquid benzene? (Kb = 2.53°C/m for benzene)

You have a 10.40-g mixture of table sugar (C12H22O11) and table salt (NaCl). When this mixture is dissolved in 150. g of water, the freezing point is found to be -2.24°C. Calculate the percent by mass of sugar in the original mixture. (Assume that the NaCl is completely dissociated.)

What is the mole percent of ethanol (C2H5OH) in the 180 proof vodka, which consists of 71.0 g of ethanol for every 10.0 g of water present?

When a 18.4-g sample of an unknown compound is dissolved in 522.0 g of benzene, the freezing point of the resulting solution of 3.82°C. The freezing point of pure benzene is 5.48°C, and Kf for benzene is 5.12°C/m. Calculate the molar mass of the unknown compound.

A cucumber is placed in a concentrated salt solution. What is most likely to happen?

What is the molality of an HCl solution made by dissolving 150.0 g of HCl in 450.0 g of water?

A chemist is given a white solid that is suspected of being pure cocaine. When 1.22 g of the solid is dissolved in 15.60 g of benzene, the freezing point is lowered by 1.32°C. Calculate the molar mass of the solid. The molal freezing-point constant (Kf) for benzene is 5.12°C/m.

Calculate the molality of a solution containing 21.0 g of C6H12O6 in 271.0 mL of water (assume a density of 1.00 g/mL).

A liquid-liquid solution is called an ideal solution if I. it obeys PV = nRT. II. it obeys Raoult's law. III. solute-solute, solvent-solvent, and solute-solvent interactions are very similar. IV. solute-solute, solvent-solvent, and solute-solvent interactions are quite different.

If a solution exhibits a negative deviation from Raoult's law, the vapor pressure of the solution is __________ what would be expected ideally.

A solution contains 1 mol of liquid A and 3 mol of liquid B. The vapor pressure of this solution is 314 torr at 25°C. At 25°C, the vapor pressure of liquid A is 265 torr and the vapor pressure of liquid B is 355 torr. Which of the following is true?

When 200.0 mL of 0.200 M H2SO4 is diluted with 155.0 mL of water, what is the molarity of the solution?

The destruction of a colloid is called

What is the expected osmotic pressure, in torr, of a 0.0100 M solution of NaCl in water at 25°C?

Atoms, Molecules, and Ions

Stoichiometry

Chemical Reactions and Solutions Stoichiometry

Gases

Chemical Equilibrium

Acids and Bases

Applications of Aqueous Equilibria

Energy, Enthalpy, and Thermochemistry

Spontaneity, Entropy, and Free Energy

Electrochemistry

Quantum Mechanics and Atomic Theory

Bonding: General Concepts

Covalent Bonding: Orbitals

Chemical Kinetics

Liquids and Solids

The Representative Elements

Transition Metals and Coordination Chemistry

The Nucleus: a Chemists View

Organic and Biochemical Molecules

Filters

A 54.4-g sample of glucose (a nondissociated, nonvolatile solute with the formula C₆H₁₂O₆) is dissolved in 154.4 g of water. What is the vapor pressure of this solution at 100°C?

An aqueous solution contains 48.6 g of KNO₃ in 290.6 mL of solution. What is the molarity of the solution?

The solubility of O₂ in water is 0.590 g/L at an oxygen pressure of 15 atm. What is the Henry's law constant for O₂ (in units of L atm/mol)?

At a given temperature, you have a mixture of benzene (P_vap = 745 torr) and toluene (P_vap = 290 torr). The mole fraction of benzene in the solution is 0.590. Assuming ideal behavior, calculate the mole fraction of toluene in the vapor above the solution.

What is the boiling-point change for a solution containing 0.360 mol of naphthalene (a nonvolatile, nonionizing compound) in 258.0 g of liquid benzene? (K_b = 2.53°C/m for benzene)

You have a 10.40-g mixture of table sugar (C₁₂H₂₂O₁₁) and table salt (NaCl). When this mixture is dissolved in 150. g of water, the freezing point is found to be -2.24°C. Calculate the percent by mass of sugar in the original mixture. (Assume that the NaCl is completely dissociated.)

What is the mole percent of ethanol (C₂H₅OH) in the 180 proof vodka, which consists of 71.0 g of ethanol for every 10.0 g of water present?

When a 18.4-g sample of an unknown compound is dissolved in 522.0 g of benzene, the freezing point of the resulting solution of 3.82°C. The freezing point of pure benzene is 5.48°C, and K_f for benzene is 5.12°C/m. Calculate the molar mass of the unknown compound.

A chemist is given a white solid that is suspected of being pure cocaine. When 1.22 g of the solid is dissolved in 15.60 g of benzene, the freezing point is lowered by 1.32°C. Calculate the molar mass of the solid. The molal freezing-point constant (K_f) for benzene is 5.12°C/m.

Calculate the molality of a solution containing 21.0 g of C₆H₁₂O₆ in 271.0 mL of water (assume a density of 1.00 g/mL).

When 200.0 mL of 0.200 M H₂SO₄ is diluted with 155.0 mL of water, what is the molarity of the solution?