Question 1

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

Accepted Answer

A) 0.200 m Ca(ClO4)2 
B) 0.200 m K3PO3 
C) 0.200 m HOCH2CH2OH 
D) 0.200 m Ba(NO3)2 
E) These all have the same freezing point. 
A) 0.200 m Ca(ClO4)2 
B) 0.200 m K3PO3 
C) 0.200 m HOCH2CH2OH 
D) 0.200 m Ba(NO3)2 
E) These all have the same freezing point.

Question 2

What is the molality of a glucose solution prepared by dissolving 18.0 g of glucose,C6H12O6,in 125.9 g of water?

Accepted Answer

A) 7.94 × 10-4 m 
B) 0.143 m 
C) 0.695 m 
D) 0.794 m 
A) 7.94 × 10-4 m 
B) 0.143 m 
C) 0.695 m 
D) 0.794 m

Question 3

Which is not a colligative property?

Accepted Answer

A) freezing point depression in a solution 
B) vapor pressure lowering in a solution 
C) boiling point elevation in a solution 
D) boiling point of a solvent 
A) freezing point depression in a solution 
B) vapor pressure lowering in a solution 
C) boiling point elevation in a solution 
D) boiling point of a solvent

Question 4

Determine the molality of a solution prepared by dissolving 0.500 moles of CaF2 in 11.5 moles H2O.

Accepted Answer

A) 1.88 m 
B) 4.35 m 
C) 5.31 m 
D) 4.14 m 
E) 2.41 m 
A) 1.88 m 
B) 4.35 m 
C) 5.31 m 
D) 4.14 m 
E) 2.41 m

Question 5

The osmotic pressure of a solution formed by dissolving 25.0 mg of aspirin (C9H8O4)in 0.250 L of water at 25°C is ________ atm.

Accepted Answer

A) 13.6 
B) 1.14 × 10-3 
C) 0.0136 
D) 2.45 
E) 1.38 
A) 13.6 
B) 1.14 × 10-3 
C) 0.0136 
D) 2.45 
E) 1.38

Question 6

Choose the situation below that would result in an endothermic ΔHsolution.

Accepted Answer

A) When  >   
B) When  >  
E) There isn't enough information to determine. 
A) When  >   
B) When  >  
E) There isn't enough information to determine.

Question 7

Define osmosis.

Accepted Answer

Osmosis is the flow of solvent

Question 8

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 9

What is the weight percent of vitamin C in a solution made by dissolving 6.50 g of vitamin C,C6H8O6,in 55.0 g of water?

Accepted Answer

A) 0.547% 
B) 1.21% 
C) 10.6% 
D) 11.8% 
A) 0.547% 
B) 1.21% 
C) 10.6% 
D) 11.8%

Question 10

What mass of ethane (CH3CH3)is contained in 50.0 mL of a 13.9% by mass solution of ethane in hexane? The density of the solution is 0.611 g/mL.

Accepted Answer

A) 2.35 g 
B) 8.49 g 
C) 11.8 g 
D) 6.95 g 
E) 4.25 g 
A) 2.35 g 
B) 8.49 g 
C) 11.8 g 
D) 6.95 g 
E) 4.25 g

Question 11

Determine the molality of an aqueous solution prepared by dissolving 0.112 moles of LiCl in 13.7 moles of H2O.

Accepted Answer

A) 0.454 m 
B) 0.220 m 
C) 0.818 m 
D) 0.122 m 
E) 0.153 m 
A) 0.454 m 
B) 0.220 m 
C) 0.818 m 
D) 0.122 m 
E) 0.153 m

Question 12

Match the following.
-0.050 m NaCl

Accepted Answer

A) largest van't Hoff factor 
B) solution of ionic compound with highest freezing point 
C) solution with ΔTb = 0.026°C 
D) highest boiling point 
E) solution that is most strongly dependent upon pressure 
A) largest van't Hoff factor 
B) solution of ionic compound with highest freezing point 
C) solution with ΔTb = 0.026°C 
D) highest boiling point 
E) solution that is most strongly dependent upon pressure

Question 13

Determine the freezing point of a solution that contains 78.8 g of naphthalene (C10H8,molar mass = 128.16 g/mol)dissolved in 722 mL of benzene (d = 0.877 g/mL).Pure benzene has a melting point of 5.50°C and a freezing point depression constant of 4.90°C/m.

Accepted Answer

A) 4.76°C 
B) 4.17°C 
C) 0.74°C 
D) 1.33°C 
E) 1.68°C 
A) 4.76°C 
B) 4.17°C 
C) 0.74°C 
D) 1.33°C 
E) 1.68°C

Question 14

A solution is prepared by dissolving 38.6 g sucrose (C12H22O11)in 495 g of water.Determine the mole fraction of sucrose if the final volume of the solution is 508 mL.

Accepted Answer

A) 4.09 × 10-3 
B) 7.80 × 10-2 
C) 1.28 × 10-3 
D) 7.23 × 10-2 
E) 2.45 × 10-3 
A) 4.09 × 10-3 
B) 7.80 × 10-2 
C) 1.28 × 10-3 
D) 7.23 × 10-2 
E) 2.45 × 10-3

Question 15

Calculate the molality of a solution that is prepared by mixing 25.5 mL of CH3OH (d = 0.792 g/mL)and 387 mL of CH3CH2CH2OH (d = 0.811 g/mL).

Accepted Answer

A) 0.630 m 
B) 0.812 m 
C) 1.57 m 
D) 1.89 m 
E) 4.98 m 
A) 0.630 m 
B) 0.812 m 
C) 1.57 m 
D) 1.89 m 
E) 4.98 m

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

How many moles of KF are contained in 244 mL of 0.135 m KF solution? The density of the solution is 1.22 g/mL.

Accepted Answer

A) 4.31 × 10-2 mol KF 
B) 4.02 × 10-2 mol KF 
C) 3.29 × 10-2 mol KF 
D) 2.32 × 10-2 mol KF 
E) 1.67 × 10-2 mol KF 
A) 4.31 × 10-2 mol KF 
B) 4.02 × 10-2 mol KF 
C) 3.29 × 10-2 mol KF 
D) 2.32 × 10-2 mol KF 
E) 1.67 × 10-2 mol KF

Question 18

A solution is prepared by adding 30.00 g of lactose (milk sugar)to 110.0 g of water at 55°C.The partial pressure of water above the solution is ________ torr.The vapor pressure of pure water at 55°C is 118.0 torr.The MW of lactose is 342.3 g/mol.

Accepted Answer

A) 1.670 
B) 94.1 
C) 169.4 
D) 116.3 
E) 92.7 
A) 1.670 
B) 94.1 
C) 169.4 
D) 116.3 
E) 92.7

Question 19

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 20

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

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

What is the molality of a glucose solution prepared by dissolving 18.0 g of glucose,C₆H₁₂O₆,in 125.9 g of water?

Which is not a colligative property?

Determine the molality of a solution prepared by dissolving 0.500 moles of CaF₂ in 11.5 moles H₂O.

The osmotic pressure of a solution formed by dissolving 25.0 mg of aspirin (C₉H₈O₄)in 0.250 L of water at 25°C is ________ atm.

Choose the situation below that would result in an endothermic ΔH_solution.

Define osmosis.

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

What is the weight percent of vitamin C in a solution made by dissolving 6.50 g of vitamin C,C₆H₈O₆,in 55.0 g of water?

What mass of ethane (CH₃CH₃)is contained in 50.0 mL of a 13.9% by mass solution of ethane in hexane? The density of the solution is 0.611 g/mL.

Determine the molality of an aqueous solution prepared by dissolving 0.112 moles of LiCl in 13.7 moles of H₂O.

Match the following. -0.050 m NaCl

Determine the freezing point of a solution that contains 78.8 g of naphthalene (C₁₀H₈,molar mass = 128.16 g/mol)dissolved in 722 mL of benzene (d = 0.877 g/mL).Pure benzene has a melting point of 5.50°C and a freezing point depression constant of 4.90°C/m.

A solution is prepared by dissolving 38.6 g sucrose (C₁₂H₂₂O₁₁)in 495 g of water.Determine the mole fraction of sucrose if the final volume of the solution is 508 mL.

Calculate the molality of a solution that is prepared by mixing 25.5 mL of CH₃OH (d = 0.792 g/mL)and 387 mL of CH₃CH₂CH₂OH (d = 0.811 g/mL).

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?

How many moles of KF are contained in 244 mL of 0.135 m KF solution? The density of the solution is 1.22 g/mL.

A solution is prepared by adding 30.00 g of lactose (milk sugar)to 110.0 g of water at 55°C.The partial pressure of water above the solution is ________ torr.The vapor pressure of pure water at 55°C is 118.0 torr.The MW of lactose is 342.3 g/mol.

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?

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.

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Molecules, Compounds and Chemical Equations

Chemical Quantities and Aqueous Reactions

Gases

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The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and

Liquids, Solids, and Intermolecular Forces

Chemical Kinetics

Chemical Equilibrium

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Exam 12: Solutions

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

What is the molality of a glucose solution prepared by dissolving 18.0 g of glucose,C6H12O6,in 125.9 g of water?

Which is not a colligative property?

Determine the molality of a solution prepared by dissolving 0.500 moles of CaF2 in 11.5 moles H2O.

The osmotic pressure of a solution formed by dissolving 25.0 mg of aspirin (C9H8O4)in 0.250 L of water at 25°C is ________ atm.

Choose the situation below that would result in an endothermic ΔHsolution.

Define osmosis.

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

What is the weight percent of vitamin C in a solution made by dissolving 6.50 g of vitamin C,C6H8O6,in 55.0 g of water?

What mass of ethane (CH3CH3)is contained in 50.0 mL of a 13.9% by mass solution of ethane in hexane? The density of the solution is 0.611 g/mL.

Determine the molality of an aqueous solution prepared by dissolving 0.112 moles of LiCl in 13.7 moles of H2O.

Match the following. -0.050 m NaCl

Determine the freezing point of a solution that contains 78.8 g of naphthalene (C10H8,molar mass = 128.16 g/mol)dissolved in 722 mL of benzene (d = 0.877 g/mL).Pure benzene has a melting point of 5.50°C and a freezing point depression constant of 4.90°C/m.

A solution is prepared by dissolving 38.6 g sucrose (C12H22O11)in 495 g of water.Determine the mole fraction of sucrose if the final volume of the solution is 508 mL.

Calculate the molality of a solution that is prepared by mixing 25.5 mL of CH3OH (d = 0.792 g/mL)and 387 mL of CH3CH2CH2OH (d = 0.811 g/mL).

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?

How many moles of KF are contained in 244 mL of 0.135 m KF solution? The density of the solution is 1.22 g/mL.

A solution is prepared by adding 30.00 g of lactose (milk sugar)to 110.0 g of water at 55°C.The partial pressure of water above the solution is ________ torr.The vapor pressure of pure water at 55°C is 118.0 torr.The MW of lactose is 342.3 g/mol.

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?

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.

Matter, Measurement, and Problem Solving

Atoms and Elements

Molecules, Compounds and Chemical Equations

Chemical Quantities and Aqueous Reactions

Gases

Thermochemistry

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and

Liquids, Solids, and Intermolecular Forces

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Free Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Filters

What is the molality of a glucose solution prepared by dissolving 18.0 g of glucose,C₆H₁₂O₆,in 125.9 g of water?

Determine the molality of a solution prepared by dissolving 0.500 moles of CaF₂ in 11.5 moles H₂O.

The osmotic pressure of a solution formed by dissolving 25.0 mg of aspirin (C₉H₈O₄)in 0.250 L of water at 25°C is ________ atm.

Choose the situation below that would result in an endothermic ΔH_solution.

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

What is the weight percent of vitamin C in a solution made by dissolving 6.50 g of vitamin C,C₆H₈O₆,in 55.0 g of water?

What mass of ethane (CH₃CH₃)is contained in 50.0 mL of a 13.9% by mass solution of ethane in hexane? The density of the solution is 0.611 g/mL.

Determine the molality of an aqueous solution prepared by dissolving 0.112 moles of LiCl in 13.7 moles of H₂O.

Determine the freezing point of a solution that contains 78.8 g of naphthalene (C₁₀H₈,molar mass = 128.16 g/mol)dissolved in 722 mL of benzene (d = 0.877 g/mL).Pure benzene has a melting point of 5.50°C and a freezing point depression constant of 4.90°C/m.

A solution is prepared by dissolving 38.6 g sucrose (C₁₂H₂₂O₁₁)in 495 g of water.Determine the mole fraction of sucrose if the final volume of the solution is 508 mL.

Calculate the molality of a solution that is prepared by mixing 25.5 mL of CH₃OH (d = 0.792 g/mL)and 387 mL of CH₃CH₂CH₂OH (d = 0.811 g/mL).

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?

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.