Question 1

What is the mole fraction of urea,CH4N2O,in an aqueous solution that is 49% urea by mass?

Accepted Answer

A)  0.22 
B)  0.78 
C)  0.49 
D)  0.42 
E)  0.76 
A)  0.22 
B)  0.78 
C)  0.49 
D)  0.42 
E)  0.76 A

Question 2

Which of the following solutions has the lowest osmotic pressure?

Accepted Answer

A)  0.10 M Al(NO3)3 
B)  0.20 M C6.0H12O6 
C)  0.15 M Ba(NO3)2 
D)  0.10 M CaBr2 
E)  0.15 M Na2Cl 
A)  0.10 M Al(NO3)3 
B)  0.20 M C6.0H12O6 
C)  0.15 M Ba(NO3)2 
D)  0.10 M CaBr2 
E)  0.15 M Na2Cl B

Question 3

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 C

Question 4

A concentrated hydrochloric acid solution is 37.2% HCl by mass and has a density of 1.19 g/mL at 25°C.What is the molarity of HCl?

Accepted Answer

A)  12.1 M 
B)  0.0434 M 
C)  8.57 M 
D)  11.7 M 
E)  0.0857 M 
A)  12.1 M 
B)  0.0434 M 
C)  8.57 M 
D)  11.7 M 
E)  0.0857 M

Question 5

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 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 equilibrium partial pressure of water vapor above a mixture of 37.5 g H2O and 62.5 g HOCH2CH2OH at 55 °C.The partial pressure of pure water at 55.0 °C is 118.0 mm Hg.Assume ideal behavior for the solution.

Accepted Answer

A)  3.54 mm Hg 
B)  31.7 mm Hg 
C)  38.5 mm Hg 
D)  79.5 mm Hg 
E)  175 mm Hg 
A)  3.54 mm Hg 
B)  31.7 mm Hg 
C)  38.5 mm Hg 
D)  79.5 mm Hg 
E)  175 mm Hg

Question 8

_____ are colloidal dispersions of one liquid in another.

Accepted Answer

The answer of _____ are colloidal dispersions of one liquid...

Question 9

Calculate the molarity of a solution of magnesium chloride with a concentration of 27.0 mg/mL.

Accepted Answer

A)  0.142 M 
B)  3.53 M 
C)  0.567 M 
D)  0.452 M 
E)  0.284 M 
A)  0.142 M 
B)  3.53 M 
C)  0.567 M 
D)  0.452 M 
E)  0.284 M

Question 10

The osmotic pressure of blood is 7.65 atm at 37 °C.What mass of glucose (C6H12O6,molar mass = 180.2 g/mol)is needed to prepare 2.25 L of solution for intravenous injection? The osmotic pressure of the glucose solution must equal the osmotic pressure of blood.(R = 0.08206 L⋅atm/mol⋅K)

Accepted Answer

A)  0.676 g 
B)  0.698 g 
C)  5.67 g 
D)  122 g 
E)  1.02 × 103 g 
A)  0.676 g 
B)  0.698 g 
C)  5.67 g 
D)  122 g 
E)  1.02 × 103 g

Question 11

Assuming ideal behavior,which of the following aqueous solutions should have the highest boiling point?

Accepted Answer

A)  1.00 m LiBr 
B)  0.75 m K2SO4 
C)  0.50 m Ca(NO3)2 
D)  0.75 m NaCl 
E)  1.25 m C6H12O6 
A)  1.00 m LiBr 
B)  0.75 m K2SO4 
C)  0.50 m Ca(NO3)2 
D)  0.75 m NaCl 
E)  1.25 m C6H12O6

Question 12

Which of the following compounds is not miscible with water?

Accepted Answer

A)  CH3NH2 
B)  CH3COOH 
C)  CCl4 
D)  CH3CN 
E)  HOCH2CH2OH 
A)  CH3NH2 
B)  CH3COOH 
C)  CCl4 
D)  CH3CN 
E)  HOCH2CH2OH

Question 13

The change in energy accompanying the equation below is the _____ of MX. MX(s)→ M+(aq)+ X−(aq)

Accepted Answer

A)  enthalpy of hydration 
B)  enthalpy of solution 
C)  lattice energy 
D)  enthalpy of formation 
E)  electron attachment enthalpy 
A)  enthalpy of hydration 
B)  enthalpy of solution 
C)  lattice energy 
D)  enthalpy of formation 
E)  electron attachment enthalpy

Question 14

What is the freezing point of a 0.29 m solution of glucose (C6H12O6)in water? (Kfp for water is 1.858 °C/m.)

Accepted Answer

A)  0.27 °C 
B)  0.54 °C 
C)  -0.54 °C 
D)  -0.27 °C 
E)  -1.08 °C 
A)  0.27 °C 
B)  0.54 °C 
C)  -0.54 °C 
D)  -0.27 °C 
E)  -1.08 °C

Question 15

What mass of an aqueous 18.8% glucose solution contains 85.5 g of water?

Accepted Answer

A)  105 g 
B)  19.8 g 
C)  14.5 g 
D)  16.1 g 
E)  85.5 g 
A)  105 g 
B)  19.8 g 
C)  14.5 g 
D)  16.1 g 
E)  85.5 g

Question 16

If one of the factors determining the equilibrium of a system is changed,the system adjusts to counteract that change.This is known as ________ principle.

Accepted Answer

The answer of If one of the factors determining the...

Question 17

Which of the following is a colligative property?

Accepted Answer

A)  Vapor pressure addition 
B)  Boiling point depression 
C)  Freezing point depression 
D)  Osmotic pressure 
E)  Melting point elevation 
A)  Vapor pressure addition 
B)  Boiling point depression 
C)  Freezing point depression 
D)  Osmotic pressure 
E)  Melting point elevation

Question 18

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 19

A 0.20 M solution of MgSO4 has an observed osmotic pressure of 7.7 atm at 25°C.Determine the observed van't Hoff factor for this experiment.

Accepted Answer

A)  2.0 
B)  1.6 
C)  0.31 
D)  19 
E)  1.8 
A)  2.0 
B)  1.6 
C)  0.31 
D)  19 
E)  1.8

Question 20

What mass of Na2SO4 must be dissolved in 100.0 grams of water to lower the freezing point by 2.50 °C? The freezing point depression constant,Kfp,of water is -1.86 °C/m.Assume the van't Hoff factor for Na2SO4 is 2.85.

Accepted Answer

A)  3.77 g 
B)  6.36 g 
C)  6.70 g 
D)  11.3 g 
E)  19.1 g 
A)  3.77 g 
B)  6.36 g 
C)  6.70 g 
D)  11.3 g 
E)  19.1 g

Exam 14: Solutions and Their Behavior

What is the mole fraction of urea,CH4N2O,in an aqueous solution that is 49% urea by mass?

Which of the following solutions has the lowest osmotic pressure?

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

A concentrated hydrochloric acid solution is 37.2% HCl by mass and has a density of 1.19 g/mL at 25°C.What is the molarity of HCl?

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

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

What is the equilibrium partial pressure of water vapor above a mixture of 37.5 g H2O and 62.5 g HOCH2CH2OH at 55 °C.The partial pressure of pure water at 55.0 °C is 118.0 mm Hg.Assume ideal behavior for the solution.

_____ are colloidal dispersions of one liquid in another.

Calculate the molarity of a solution of magnesium chloride with a concentration of 27.0 mg/mL.

The osmotic pressure of blood is 7.65 atm at 37 °C.What mass of glucose (C6H12O6,molar mass = 180.2 g/mol)is needed to prepare 2.25 L of solution for intravenous injection? The osmotic pressure of the glucose solution must equal the osmotic pressure of blood.(R = 0.08206 L⋅atm/mol⋅K)

Assuming ideal behavior,which of the following aqueous solutions should have the highest boiling point?

Which of the following compounds is not miscible with water?

The change in energy accompanying the equation below is the _____ of MX. MX(s)→ M+(aq)+ X−(aq)

What is the freezing point of a 0.29 m solution of glucose (C6H12O6)in water? (Kfp for water is 1.858 °C/m.)

What mass of an aqueous 18.8% glucose solution contains 85.5 g of water?

If one of the factors determining the equilibrium of a system is changed,the system adjusts to counteract that change.This is known as ________ principle.

Which of the following is a colligative property?

Which of the following statements is INCORRECT?

A 0.20 M solution of MgSO4 has an observed osmotic pressure of 7.7 atm at 25°C.Determine the observed van't Hoff factor for this experiment.

What mass of Na2SO4 must be dissolved in 100.0 grams of water to lower the freezing point by 2.50 °C? The freezing point depression constant,Kfp,of water is -1.86 °C/m.Assume the van't Hoff factor for Na2SO4 is 2.85.

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

What is the mole fraction of urea,CH₄N₂O,in an aqueous solution that is 49% urea by mass?

What is the equilibrium partial pressure of water vapor above a mixture of 37.5 g H₂O and 62.5 g HOCH₂CH₂OH at 55 °C.The partial pressure of pure water at 55.0 °C is 118.0 mm Hg.Assume ideal behavior for the solution.

The osmotic pressure of blood is 7.65 atm at 37 °C.What mass of glucose (C₆H₁₂O₆,molar mass = 180.2 g/mol)is needed to prepare 2.25 L of solution for intravenous injection? The osmotic pressure of the glucose solution must equal the osmotic pressure of blood.(R = 0.08206 L⋅atm/mol⋅K)

The change in energy accompanying the equation below is the _____ of MX. MX(s)→ M⁺(aq)+ X−(aq)

What is the freezing point of a 0.29 m solution of glucose (C₆H₁₂O₆)in water? (K_fp for water is 1.858 °C/m.)

A 0.20 M solution of MgSO₄ has an observed osmotic pressure of 7.7 atm at 25°C.Determine the observed van't Hoff factor for this experiment.

What mass of Na₂SO₄ must be dissolved in 100.0 grams of water to lower the freezing point by 2.50 °C? The freezing point depression constant,K_fp,of water is -1.86 °C/m.Assume the van't Hoff factor for Na₂SO₄ is 2.85.