Question 1

What is the Henry's law constant for O2 if the solubility of O2 in water is 0.590 g/L at a pressure of 15.5 atm?

Accepted Answer

A)  3.81 × 10-2 L·atm/mol 
B)  8.41 × 102 L·atm/mol 
C)  2.86 × 10-1 L·atm/mol 
D)  1.19 × 10-3 L·atm/mol 
E)  None of these 
A)  3.81 × 10-2 L·atm/mol 
B)  8.41 × 102 L·atm/mol 
C)  2.86 × 10-1 L·atm/mol 
D)  1.19 × 10-3 L·atm/mol 
E)  None of these

Question 2

All of the following are colloidal dispersions EXCEPT ____.

Accepted Answer

A)  marshmallow 
B)  white wine 
C)  milk 
D)  whipped cream 
E)  cheese 
A)  marshmallow 
B)  white wine 
C)  milk 
D)  whipped cream 
E)  cheese

Question 3

Which of the following statements is INCORRECT?

Accepted Answer

A)  The solubility of a gas in water decreases with increasing temperature. 
B)  The solubility of a gas in water is proportional to the partial pressure of the gas above the water. 
C)  The dissolution of a gas in water is usually an exothermic process. 
D)  The relationship between the solubility of a gas and its partial pressure is known as Henry's law. 
E)  The solubility of a gas in water is inversely proportional to the molar mass of the gas. 
A)  The solubility of a gas in water decreases with increasing temperature. 
B)  The solubility of a gas in water is proportional to the partial pressure of the gas above the water. 
C)  The dissolution of a gas in water is usually an exothermic process. 
D)  The relationship between the solubility of a gas and its partial pressure is known as Henry's law. 
E)  The solubility of a gas in water is inversely proportional to the molar mass of the gas.

Question 4

Which of the following liquids are miscible with water in any proportion?

Accepted Answer

A)  Ethanol (CH3CH2OH) and carbon tetrachloride (CCl4) 
B)  Carbon tetrachloride (CCl4) and hexane (C6H14) 
C)  Ethanol (CH3CH2OH) and formic acid (HCO2H) 
D)  Ethanol (CH3CH2OH), carbon tetrachloride (CCl4), and hexane (C6H14) 
E)  Carbon tetrachloride (CCl4) and formic acid (HCO2H) 
A)  Ethanol (CH3CH2OH) and carbon tetrachloride (CCl4) 
B)  Carbon tetrachloride (CCl4) and hexane (C6H14) 
C)  Ethanol (CH3CH2OH) and formic acid (HCO2H) 
D)  Ethanol (CH3CH2OH), carbon tetrachloride (CCl4), and hexane (C6H14) 
E)  Carbon tetrachloride (CCl4) and formic acid (HCO2H)

Question 5

The Henry's law constant for N2 in water at 25 °C is 6.0 × 10-4 mol/kg⋅bar. What is the equilibrium concentration of N2 in water when the partial pressure of N2 is 586 mm Hg? (760 mm Hg = 1 atm = 0.9869 bar)

Accepted Answer

A)  1.4 × 10-9 M 
B)  1.8 × 10-5 M 
C)  4.6 × 10-4 M 
D)  7.7 × 10-4 M 
E)  7.9 × 10-4 M 
A)  1.4 × 10-9 M 
B)  1.8 × 10-5 M 
C)  4.6 × 10-4 M 
D)  7.7 × 10-4 M 
E)  7.9 × 10-4 M

Question 6

Which of the following solutions would have the highest osmotic pressure?

Accepted Answer

A)  0.2 M C6H12O6, glucose 
B)  0.15 M MgCl2, magnesium chloride 
C)  0.15 M KCl, potassium chloride 
D)  0.2 M CH3OH, methanol 
E)  0.2 M C12H22O11, sucrose 
A)  0.2 M C6H12O6, glucose 
B)  0.15 M MgCl2, magnesium chloride 
C)  0.15 M KCl, potassium chloride 
D)  0.2 M CH3OH, methanol 
E)  0.2 M C12H22O11, sucrose

Question 7

What is the mole fraction of calcium chloride in 3.35 m CaCl2(aq)? The molar mass of CaCl2 is 111.0 g/mol and the molar mass of water is 18.02 g/mol.

Accepted Answer

A)  0.000866 
B)  0.0569 
C)  0.271 
D)  37.2 
E)  59.2 
A)  0.000866 
B)  0.0569 
C)  0.271 
D)  37.2 
E)  59.2

Question 8

Which of the following statements about soaps and detergents is false?

Accepted Answer

A)  The polar end is attracted to grease and oil. 
B)  They have a polar and a nonpolar end. 
C)  They are emulsifiers for grease and oil. 
D)  Phosphate detergents can produce pollution. 
E)  They can be described as surfactants. 
A)  The polar end is attracted to grease and oil. 
B)  They have a polar and a nonpolar end. 
C)  They are emulsifiers for grease and oil. 
D)  Phosphate detergents can produce pollution. 
E)  They can be described as surfactants.

Question 9

The following equation is known as ________ law: $P _ { \text {solvent } } = X _ { \text {solvent } } P _ { \text {solvent } } ^ { \circ }$ .

Accepted Answer

The answer of The following equation is known as ________...

Question 10

Ideally, colligative properties depend only on the:

Accepted Answer

A)  relative number of solute and solvent particles in a solution. 
B)  molar masses of the solute particles in a solution. 
C)  density of a solution. 
D)  hydrated radii of the molecules or ions dissolved in a solution. 
E)  partial pressure of the gases above the surface of a solution. 
A)  relative number of solute and solvent particles in a solution. 
B)  molar masses of the solute particles in a solution. 
C)  density of a solution. 
D)  hydrated radii of the molecules or ions dissolved in a solution. 
E)  partial pressure of the gases above the surface of a solution.

Question 11

What mass of ethylene glycol, when mixed with 225 g H2O, will reduce the equilibrium vapor pressure of H2O from 1.00 atm to 0.800 atm at 100 °C? The molar masses of water and ethylene glycol are 18.02 g/mol and 62.07 g/mol, respectively. Assume ideal behavior for the solution.

Accepted Answer

A)  15.6 g 
B)  49.9 g 
C)  194 g 
D)  969 g 
E)  3.10 × 103 g 
A)  15.6 g 
B)  49.9 g 
C)  194 g 
D)  969 g 
E)  3.10 × 103 g

Question 12

Colloids are described by all of the following except:

Accepted Answer

A)  The particles in a colloid are so small that settling is negligible. 
B)  The mixture appears cloudy. 
C)  Only combinations of liquids and gases can form colloids. 
D)  Colloids are not suspensions or homogeneous mixtures. 
E)  Mayonnaise, whipped cream and fog are all examples of colloids. 
A)  The particles in a colloid are so small that settling is negligible. 
B)  The mixture appears cloudy. 
C)  Only combinations of liquids and gases can form colloids. 
D)  Colloids are not suspensions or homogeneous mixtures. 
E)  Mayonnaise, whipped cream and fog are all examples of colloids.

Question 13

What is the mass percent of an aqueous sodium hydroxide solution in which the molality of NaOH is 10.7 m?

Accepted Answer

A)  0% 
B)  69% 
C)  2% 
D)  30.0% 
E)  0%.. 
A)  0% 
B)  69% 
C)  2% 
D)  30.0% 
E)  0%..

Question 14

Henry's Law constant is 0.0013 mol/kg?bar and 0.034 mol/kg?bar for O2 and CO2 respectively at 25°C. What pressure of CO2 is required to achieve the same solubility as 0.711 bar of O2?

Accepted Answer

A)  0.0 bar 
B)  19.0 bar 
C)  $3.1 \times 10 ^ { - 5 }$ bar 
D)  $6.2 \times 10 ^ { - 5 }$ bar 
E)  37.0 bar 
A)  0.0 bar 
B)  19.0 bar 
C)  $3.1 \times 10 ^ { - 5 }$ bar 
D)  $6.2 \times 10 ^ { - 5 }$ bar 
E)  37.0 bar

Question 15

What is the mole fraction of urea, CO(NH2)2, in a solution prepared by dissolving 4.8 g of urea in 30.3 g of methanol, CH3OH?

Accepted Answer

A)  0.86 
B)  0.14 
C)  0.078 
D)  0.92 
E)  0.23 
A)  0.86 
B)  0.14 
C)  0.078 
D)  0.92 
E)  0.23

Question 16

Aqueous colloidal solutions can be classified as ________ (water-fearing), or hydrophilic (water-loving).

Accepted Answer

The answer of Aqueous colloidal solutions can be classified as...

Question 17

What is the molality of a 19.4 M sodium hydroxide solution that has a density of 1.54 g/mL?

Accepted Answer

A)  12.6 m 
B)  19.8 m 
C)  25.4 m 
D)  29.9 m 
E)  50.4 m 
A)  12.6 m 
B)  19.8 m 
C)  25.4 m 
D)  29.9 m 
E)  50.4 m

Question 18

If 11.7 g of naphthalene, C10H8, is dissolved in 104.2 g of chloroform, CHCl3, what is the molality of the solution?

Accepted Answer

A)  0.0914 m 
B)  13.4 m 
C)  0.877 m 
D)  0.101 m 
E)  0.105 m 
A)  0.0914 m 
B)  13.4 m 
C)  0.877 m 
D)  0.101 m 
E)  0.105 m

Question 19

What is the definition of molality?

Accepted Answer

A)  moles of solute per kg of solvent 
B)  grams of solute per kg of solution 
C)  grams of solute per liter of solution 
D)  moles of solute per liter of solvent 
E)  moles of solute per liter of solution 
A)  moles of solute per kg of solvent 
B)  grams of solute per kg of solution 
C)  grams of solute per liter of solution 
D)  moles of solute per liter of solvent 
E)  moles of solute per liter of solution

Question 20

For the following gas-liquid equilibrium for an aqueous system at a constant partial pressure of CO2, CO2(g)   &ensp;&ensp;&ensp;   D   &ensp;&ensp;    CO2(aq)
What is the effect on the equilibrium composition of the liquid when the temperature of the liquid is increased?

Accepted Answer

A)  The amount of CO2 dissolved in the liquid increases. 
B)  The amount of CO2 dissolved in the liquid decreases. 
C)  The amount of CO2 dissolved in the liquid does not change. 
D)  Not enough information is provided to answer the question. 
E)  Either A or B could occur. 
A)  The amount of CO2 dissolved in the liquid increases. 
B)  The amount of CO2 dissolved in the liquid decreases. 
C)  The amount of CO2 dissolved in the liquid does not change. 
D)  Not enough information is provided to answer the question. 
E)  Either A or B could occur.

Exam 14: Solutions and Their Behavior

What is the Henry's law constant for O2 if the solubility of O2 in water is 0.590 g/L at a pressure of 15.5 atm?

All of the following are colloidal dispersions EXCEPT ____.

Which of the following statements is INCORRECT?

Which of the following liquids are miscible with water in any proportion?

The Henry's law constant for N2 in water at 25 °C is 6.0 × 10-4 mol/kg⋅bar. What is the equilibrium concentration of N2 in water when the partial pressure of N2 is 586 mm Hg? (760 mm Hg = 1 atm = 0.9869 bar)

Which of the following solutions would have the highest osmotic pressure?

What is the mole fraction of calcium chloride in 3.35 m CaCl2(aq)? The molar mass of CaCl2 is 111.0 g/mol and the molar mass of water is 18.02 g/mol.

Which of the following statements about soaps and detergents is false?

The following equation is known as ________ law: Psolvent =Xsolvent Psolvent ∘P _ { \text {solvent } } = X _ { \text {solvent } } P _ { \text {solvent } } ^ { \circ }Psolvent ​=Xsolvent ​Psolvent ∘​ .

Ideally, colligative properties depend only on the:

What mass of ethylene glycol, when mixed with 225 g H2O, will reduce the equilibrium vapor pressure of H2O from 1.00 atm to 0.800 atm at 100 °C? The molar masses of water and ethylene glycol are 18.02 g/mol and 62.07 g/mol, respectively. Assume ideal behavior for the solution.

Colloids are described by all of the following except:

What is the mass percent of an aqueous sodium hydroxide solution in which the molality of NaOH is 10.7 m?

Henry's Law constant is 0.0013 mol/kg?bar and 0.034 mol/kg?bar for O2 and CO2 respectively at 25°C. What pressure of CO2 is required to achieve the same solubility as 0.711 bar of O2?

What is the mole fraction of urea, CO(NH2)2, in a solution prepared by dissolving 4.8 g of urea in 30.3 g of methanol, CH3OH?

Aqueous colloidal solutions can be classified as ________ (water-fearing), or hydrophilic (water-loving).

What is the molality of a 19.4 M sodium hydroxide solution that has a density of 1.54 g/mL?

If 11.7 g of naphthalene, C10H8, is dissolved in 104.2 g of chloroform, CHCl3, what is the molality of the solution?

What is the definition of molality?

For the following gas-liquid equilibrium for an aqueous system at a constant partial pressure of CO2, CO2(g) D CO2(aq) What is the effect on the equilibrium composition of the liquid when the temperature of the liquid is increased?

Basic Concepts of Chemistry

Lets Review: the Tools of Quantitative Chemistry

Atoms, Molecules, and Ions

Chemical Reactions

Stoichiometry: Quantitative Information About Chemical Reactions

Principles of Chemical Reactivity: Energy and Chemical Reactions

The Structure of Atoms

The Structure of Atoms and Periodic Trends

Bonding and Molecular Structure

Bonding and Molecular Structure Orbital Hybridization and Molecular Orbitals

Gases and Their Properties

Intermolecular Forces and Liquids

The Solid State

Chemical Kinetics: the Rates of Chemical Reactions

Principles of Chemical Reactivity: Equilibria

Principles of Chemical Reactivity: the Chemistry of Acids and Bases

Principles of Chemical Reactivity: Other Aspects of Aqueous Equilibria

Principles of Chemical Reactivity: Entropy and Free Energy

Principles of Chemical Reactivity: Electron Transfer Reactions

Environmental Chemistry: Earths Environment, Energy, and Sustainability

The Chemistry of the Main Group Elements

The Chemistry of the Transition Elements

Carbon: Not Just Another Element

Biochemistry

Nuclear Chemistry

Filters

The Henry's law constant for N₂ in water at 25 °C is 6.0 × 10^-4 mol/kg⋅bar. What is the equilibrium concentration of N₂ in water when the partial pressure of N₂ is 586 mm Hg? (760 mm Hg = 1 atm = 0.9869 bar)

What is the mole fraction of calcium chloride in 3.35 m CaCl₂(aq)? The molar mass of CaCl₂ is 111.0 g/mol and the molar mass of water is 18.02 g/mol.

The following equation is known as ________ law: $P _ { \text {solvent } } = X _ { \text {solvent } } P _ { \text {solvent } } ^ { \circ }$ .

What mass of ethylene glycol, when mixed with 225 g H₂O, will reduce the equilibrium vapor pressure of H₂O from 1.00 atm to 0.800 atm at 100 °C? The molar masses of water and ethylene glycol are 18.02 g/mol and 62.07 g/mol, respectively. Assume ideal behavior for the solution.

Henry's Law constant is 0.0013 mol/kg?bar and 0.034 mol/kg?bar for O₂ and CO₂ respectively at 25°C. What pressure of CO₂ is required to achieve the same solubility as 0.711 bar of O₂?

What is the mole fraction of urea, CO(NH₂)₂, in a solution prepared by dissolving 4.8 g of urea in 30.3 g of methanol, CH₃OH?

If 11.7 g of naphthalene, C₁₀H₈, is dissolved in 104.2 g of chloroform, CHCl₃, what is the molality of the solution?

For the following gas-liquid equilibrium for an aqueous system at a constant partial pressure of CO₂, CO₂(g) D CO₂(aq) What is the effect on the equilibrium composition of the liquid when the temperature of the liquid is increased?