Question 1

A solution containing less than the equilibrium amount is called

Accepted Answer

A)  an unsaturated solution. 
B)  a dilute solution. 
C)  a supersaturated solution. 
D)  a concentrated solution. 
E)  a saturated solution. 
A)  an unsaturated solution. 
B)  a dilute solution. 
C)  a supersaturated solution. 
D)  a concentrated solution. 
E)  a saturated solution.

Question 2

How does a solution of two volatile components with strong solute-solvent attractions deviate from Raoult's law?
 Why?

Accepted Answer

The vapor pressure of the solution will

Question 3

A solution is prepared by dissolving 40.0 g of sucrose,C12H22O11,in 250.g of water at 25°C.What is the vapor pressure of the solution if the vapor pressure of water at 25°C is 23.76 mm Hg?

Accepted Answer

A)  0.198 mm Hg 
B)  20.5 mm Hg 
C)  23.6 mm Hg 
D)  24.0 mm Hg 
A)  0.198 mm Hg 
B)  20.5 mm Hg 
C)  23.6 mm Hg 
D)  24.0 mm Hg

Question 4

Choose the aqueous solution that has the highest boiling point.These are all solutions of nonvolatile solutes and you should assume ideal van't Hoff factors where applicable.

Accepted Answer

A)  0.100 mKNO2 
B)  0.100 m Li2SO4 
C)  0.200 m C3H8O3 
D)  0.060 m Li3PO4 
E)  They all have the same boiling point. 
A)  0.100 mKNO2 
B)  0.100 m Li2SO4 
C)  0.200 m C3H8O3 
D)  0.060 m Li3PO4 
E)  They all have the same boiling point.

Question 5

Place the following solutions in order of increasing osmotic pressure. I.0.15 M C2H6O2 II.0.15 M BaCl2 III.0.15 M Na I

Accepted Answer

A)  III < I < II 
B)  II < III < I 
C)  I < II < III 
D)  II < I < III 
E)  I < III < II 
A)  III < I < II 
B)  II < III < I 
C)  I < II < III 
D)  II < I < III 
E)  I < III < II

Question 6

Which of the following statements is TRUE?

Accepted Answer

A)  In general, the solubility of a solid in water decreases with increasing temperature. 
B)  In general, the solubility of a gas in water decreases with increasing temperature. 
C)  The solubility of a gas in water usually increases with decreasing pressure. 
D)  The solubility of an ionic solid in water decreases with increasing temperature. 
E)  None of the above statements are true. 
A)  In general, the solubility of a solid in water decreases with increasing temperature. 
B)  In general, the solubility of a gas in water decreases with increasing temperature. 
C)  The solubility of a gas in water usually increases with decreasing pressure. 
D)  The solubility of an ionic solid in water decreases with increasing temperature. 
E)  None of the above statements are true.

Question 7

The boiling point of an aqueous 1.83 m (NH4)2SO4 (molar mass = 132.15 g/mol)solution is 102.5°C.Determine the value of the van't Hoff factor for this solute if the Kb for water is 0.512°C/m.

Accepted Answer

A)  3.0 
B)  3.6 
C)  1.8 
D)  2.7 
E)  2.3 
A)  3.0 
B)  3.6 
C)  1.8 
D)  2.7 
E)  2.3

Question 8

Explain why water does not dissolve in gasoline.

Accepted Answer

Water is polar and gasoline is

Question 9

What is the osmotic pressure of a solution of 55.8 g of sucrose (C12H22O11)in 200 mL of water at room temperature?

Accepted Answer

A)  19.9 atm 
B)  1.67 atm 
C)  6.27 atm 
D)  11.5 atm 
E)  14.4 atm 
A)  19.9 atm 
B)  1.67 atm 
C)  6.27 atm 
D)  11.5 atm 
E)  14.4 atm

Question 10

Determine the freezing point of a solution that contains 62.8 g of urea (CH4N2O)dissolved in 275 g of water (Kf= 1.86°C/m).

Accepted Answer

A)  -7.07°C 
B)  -4.82°C 
C)  -13.1°C 
D)  -3.01°C 
E)  -9.12°C 
A)  -7.07°C 
B)  -4.82°C 
C)  -13.1°C 
D)  -3.01°C 
E)  -9.12°C

Question 11

Give the reason that antifreeze is added to a car radiator.

Accepted Answer

A)  The freezing point is lowered and the boiling point is elevated. 
B)  The freezing point is elevated and the boiling point is lowered. 
C)  The freezing point and the boiling point are elevated. 
D)  The freezing point and the boiling point are lowered. 
E)  None of the above. 
A)  The freezing point is lowered and the boiling point is elevated. 
B)  The freezing point is elevated and the boiling point is lowered. 
C)  The freezing point and the boiling point are elevated. 
D)  The freezing point and the boiling point are lowered. 
E)  None of the above.

Question 12

What is the change in boiling point of a solution of 31.1 g Na3PO4 in 750.g of water? Kb for water is 0.512 °C/m.Assume ideal behavior.

Accepted Answer

A)  0.103°C 
B)  3.60°C 
C)  0.515°C 
D)  1.43°C 
A)  0.103°C 
B)  3.60°C 
C)  0.515°C 
D)  1.43°C

Question 13

Calculate the mass of oxygen (in mg)dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 atm of air.Assume the mole fraction of oxygen in air to be 0.21 given that kH for O2 is 1.3 × 10-3 M/ atm at this temperature.

Accepted Answer

A)  49.4 mg 
B)  23.5 mg 
C)  9.87 mg 
D)  27.3 mg 
E)  13.7 mg 
A)  49.4 mg 
B)  23.5 mg 
C)  9.87 mg 
D)  27.3 mg 
E)  13.7 mg

Question 14

The Henry's Law constant of methyl bromide,CH3Br,is k = 0.159 mol/(L ∙ atm)at 25°C.What is the solubility of methyl bromide in water at 25°C and at a partial pressure of 270.mm Hg?

Accepted Answer

A)  0.0565 mol/L 
B)  0.355 mol/L 
C)  0.448 mol/L 
D)  42.9 mol/L 
A)  0.0565 mol/L 
B)  0.355 mol/L 
C)  0.448 mol/L 
D)  42.9 mol/L

Question 15

Which cation in each set is expected to have the larger (more negative)hydration energy?
I Be2+ or Ca2+
II Rb+ or Zn2+

Accepted Answer

A)  Be2+ in set I and Rb+ in set II 
B)  Be2+ in set I and Zn2+ in set II 
C)  Ca2+ in set I and Rb+ in set II 
D)  Ca2+ in set I and Zn2+ in set II 
A)  Be2+ in set I and Rb+ in set II 
B)  Be2+ in set I and Zn2+ in set II 
C)  Ca2+ in set I and Rb+ in set II 
D)  Ca2+ in set I and Zn2+ in set II

Question 16

A solution is formed at room temperature by vigorously dissolving enough of the solid solute so that some solid remains at the bottom of the solution.Which statement below is TRUE?

Accepted Answer

A)  The solution is considered unsaturated. 
B)  The solution is considered supersaturated. 
C)  The solution is considered saturated. 
D)  The solution would be considered unsaturated if it were cooled a bit to increase the solubility of the solid. 
E)  None of the above are true. 
A)  The solution is considered unsaturated. 
B)  The solution is considered supersaturated. 
C)  The solution is considered saturated. 
D)  The solution would be considered unsaturated if it were cooled a bit to increase the solubility of the solid. 
E)  None of the above are true.

Question 17

Choose the solvent below that would show the greatest boiling point elevation when used to make a 0.10 m nonelectrolyte solution.

Accepted Answer

A)  carbon tetrachloride, Kb = 5.03°C/m 
B)  benzene, Kb = 2.53°C/m 
C)  diethyl ether, Kb = 2.02°C/m 
D)  water, Kb = 0.512°C/m 
E)  acetic acid, Kb = 3.07°C/m 
A)  carbon tetrachloride, Kb = 5.03°C/m 
B)  benzene, Kb = 2.53°C/m 
C)  diethyl ether, Kb = 2.02°C/m 
D)  water, Kb = 0.512°C/m 
E)  acetic acid, Kb = 3.07°C/m

Question 18

Calculate the freezing point of a solution containing 5.0 grams of KCl and 550.0 grams of water.The molal-freezing-point-depression constant (Kf)for water is 1.86°C/m.

Accepted Answer

A)  -0.45 oC 
B)  +0.45 oC 
C)  -0.23 oC 
D)  +0.23 oC 
E)  1.23 oC 
A)  -0.45 oC 
B)  +0.45 oC 
C)  -0.23 oC 
D)  +0.23 oC 
E)  1.23 oC

Question 19

Which of the following compounds is most soluble in hexane (CH3CH2CH2CH2CH2CH2CH3)?

Accepted Answer

A)  methanol 
B)  ethanol 
C)  1-propanol 
D)  1-butanol 
E)  1-pentanol 
A)  methanol 
B)  ethanol 
C)  1-propanol 
D)  1-butanol 
E)  1-pentanol

Question 20

Identify the polar solvent.

Accepted Answer

A)  acetone 
B)  hexane 
C)  diethyl ether 
D)  toluene 
E)  carbon tetrachloride 
A)  acetone 
B)  hexane 
C)  diethyl ether 
D)  toluene 
E)  carbon tetrachloride

Exam 14: Solutions

A solution containing less than the equilibrium amount is called

How does a solution of two volatile components with strong solute-solvent attractions deviate from Raoult's law? Why?

A solution is prepared by dissolving 40.0 g of sucrose,C12H22O11,in 250.g of water at 25°C.What is the vapor pressure of the solution if the vapor pressure of water at 25°C is 23.76 mm Hg?

Choose the aqueous solution that has the highest boiling point.These are all solutions of nonvolatile solutes and you should assume ideal van't Hoff factors where applicable.

Place the following solutions in order of increasing osmotic pressure. I.0.15 M C2H6O2 II.0.15 M BaCl2 III.0.15 M Na I

Which of the following statements is TRUE?

The boiling point of an aqueous 1.83 m (NH4)2SO4 (molar mass = 132.15 g/mol)solution is 102.5°C.Determine the value of the van't Hoff factor for this solute if the Kb for water is 0.512°C/m.

Explain why water does not dissolve in gasoline.

What is the osmotic pressure of a solution of 55.8 g of sucrose (C12H22O11)in 200 mL of water at room temperature?

Determine the freezing point of a solution that contains 62.8 g of urea (CH4N2O)dissolved in 275 g of water (Kf= 1.86°C/m).

Give the reason that antifreeze is added to a car radiator.

What is the change in boiling point of a solution of 31.1 g Na3PO4 in 750.g of water? Kb for water is 0.512 °C/m.Assume ideal behavior.

Calculate the mass of oxygen (in mg)dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 atm of air.Assume the mole fraction of oxygen in air to be 0.21 given that kH for O2 is 1.3 × 10-3 M/ atm at this temperature.

The Henry's Law constant of methyl bromide,CH3Br,is k = 0.159 mol/(L ∙ atm)at 25°C.What is the solubility of methyl bromide in water at 25°C and at a partial pressure of 270.mm Hg?

Which cation in each set is expected to have the larger (more negative)hydration energy? I Be2+ or Ca2+ II Rb+ or Zn2+

A solution is formed at room temperature by vigorously dissolving enough of the solid solute so that some solid remains at the bottom of the solution.Which statement below is TRUE?

Choose the solvent below that would show the greatest boiling point elevation when used to make a 0.10 m nonelectrolyte solution.

Calculate the freezing point of a solution containing 5.0 grams of KCl and 550.0 grams of water.The molal-freezing-point-depression constant (Kf)for water is 1.86°C/m.

Which of the following compounds is most soluble in hexane (CH3CH2CH2CH2CH2CH2CH3)?

Identify the polar solvent.

Essentials: Units, Measurements, and Problem Solving

Atoms

The Quantum Mechanical Model of the Atom

Periodic Properties of the Elements

Molecules and Compounds

Chemical Bonding I

Chemical Bonding Ii

Chemical Reactions and Chemical Quantities

Introduction to Solutions and Aqueous Reactions

Thermochemistry

Gases

Liquids, Solids, and Intermolecular Forces

Crystalline Solids and Modern Materials

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Free Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Organic Chemistry

Transition Metals and Coordination Compounds

Filters

A solution is prepared by dissolving 40.0 g of sucrose,C₁₂H₂₂O₁₁,in 250.g of water at 25°C.What is the vapor pressure of the solution if the vapor pressure of water at 25°C is 23.76 mm Hg?

Place the following solutions in order of increasing osmotic pressure. I.0.15 M C₂H₆O₂ II.0.15 M BaCl₂ III.0.15 M Na I

The boiling point of an aqueous 1.83 m (NH₄)₂SO₄ (molar mass = 132.15 g/mol)solution is 102.5°C.Determine the value of the van't Hoff factor for this solute if the K_b for water is 0.512°C/m.

What is the osmotic pressure of a solution of 55.8 g of sucrose (C₁₂H₂₂O₁₁)in 200 mL of water at room temperature?

Determine the freezing point of a solution that contains 62.8 g of urea (CH₄N₂O)dissolved in 275 g of water (K_f= 1.86°C/m).

What is the change in boiling point of a solution of 31.1 g Na₃PO₄ in 750.g of water? K_b for water is 0.512 °C/m.Assume ideal behavior.

Calculate the mass of oxygen (in mg)dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 atm of air.Assume the mole fraction of oxygen in air to be 0.21 given that k_H for O₂is 1.3 × 10^-3 M/ atm at this temperature.

The Henry's Law constant of methyl bromide,CH₃Br,is k = 0.159 mol/(L ∙ atm)at 25°C.What is the solubility of methyl bromide in water at 25°C and at a partial pressure of 270.mm Hg?

Which cation in each set is expected to have the larger (more negative)hydration energy? I Be²⁺ or Ca²⁺ II Rb⁺ or Zn²⁺

Calculate the freezing point of a solution containing 5.0 grams of KCl and 550.0 grams of water.The molal-freezing-point-depression constant (K_f)for water is 1.86°C/m.

Which of the following compounds is most soluble in hexane (CH₃CH₂CH₂CH₂CH₂CH₂CH₃)?