Question 1

Which of the following would be least soluble in a nonpolar solvent?

Accepted Answer

A) NaNO3 
B) C5H12 
C) NH3 
D) HF 
E) CH3CH2OH 
A) NaNO3 
B) C5H12 
C) NH3 
D) HF 
E) CH3CH2OH

Question 2

Which of the following choices has the compounds correctly arranged in order of increasing solubility in water? (least soluble to most soluble)

Accepted Answer

A) CCl4 3 3 
B) CH3OH 4 4 3 3 
D) LiF 3 3 
E) CH3OH 4 3 
A) CCl4 3 3 
B) CH3OH 4 4 3 3 
D) LiF 3 3 
E) CH3OH 4 3

Question 3

291.5 grams of calcium chloride is dissolved in 1974.3 grams of water.Calculate the vapor pressure lowering (in mm Hg)of the solution at 25.0 °C.(Note: The vapor pressure of pure water at 25.0 °C is 23.76 mm Hg.)

Accepted Answer

The answer of 291.5 grams of calcium chloride is dissolved...

Question 4

The osmotic pressure of a solution formed by dissolving 45.0 mg of aspirin   in 0.250 L of water at 25 °C is ________ atm.

Accepted Answer

A) 24.5 
B) 2.05 ×   
C) 0.0245 
D) 4.41 
E) 2.48 
A) 24.5 
B) 2.05 ×   
C) 0.0245 
D) 4.41 
E) 2.48

Question 5

What is the osmotic pressure (in atm)of a 0.015 M calcium chloride solution at 28 °C?

Accepted Answer

The answer of What is the osmotic pressure (in atm)of...

Question 6

Calculate the molality of a 27.0% (by mass)aqueous solution of nitric acid.

Accepted Answer

A) 5.87 
B) 222 
C) 0.906 
D) 1.37 
E) The density of the solution is needed to solve the problem. 
A) 5.87 
B) 222 
C) 0.906 
D) 1.37 
E) The density of the solution is needed to solve the problem.

Question 7

Determine the freezing point (°C)of a 0.015 molal aqueous solution of MgSO4.Assume i = 2.0 for MgSO4.The molal freezing-point-depression constant of water is

Accepted Answer

A) -0.056 
B) -0.028 
C) -0.17 
D) -0.084 
E) 0.000 
A) -0.056 
B) -0.028 
C) -0.17 
D) -0.084 
E) 0.000

Question 8

What is the molarity of a 7.00% by mass ammonium chloride aqueous solution at 20 °C? Density of the solution is

Accepted Answer

A) 1.33 
B) 1.41 
C) 0.133 
D) 0.146 
E) 6.86 
A) 1.33 
B) 1.41 
C) 0.133 
D) 0.146 
E) 6.86

Question 9

Molality is defined as the ________.

Accepted Answer

A) moles solute/moles solvent 
B) moles solute/liters solution 
C) moles solute/kg solution 
D) moles solute/kg solvent 
E) none (dimensionless) 
A) moles solute/moles solvent 
B) moles solute/liters solution 
C) moles solute/kg solution 
D) moles solute/kg solvent 
E) none (dimensionless)

Question 10

Of the following,a 0.1 M aqueous solution of ________ will have the lowest freezing point.

Accepted Answer

A) NaCl 
B) Al(NO3)3 
C) K2CrO4 
D) Na2SO4 
E) sucrose 
A) NaCl 
B) Al(NO3)3 
C) K2CrO4 
D) Na2SO4 
E) sucrose

Question 11

A solution with a concentration higher than the solubility allows is ________.

Accepted Answer

A) not possible 
B) unsaturated 
C) supercritical 
D) saturated 
E) supersaturated 
A) not possible 
B) unsaturated 
C) supercritical 
D) saturated 
E) supersaturated

Question 12

An aqueous solution with a concentration of 18 ppm indicates that there is ________ per liter of solution.

Accepted Answer

The answer of An aqueous solution with a concentration of...

Question 13

Which of the following liquids will have the lowest freezing point?

Accepted Answer

A) pure H2O 
B) aqueous glucose (0.050 m) 
C) aqueous CoI2 (0.030 m) 
D) aqueous FeI3 (0.030 m) 
E) aqueous NaI (0.030 m) 
A) pure H2O 
B) aqueous glucose (0.050 m) 
C) aqueous CoI2 (0.030 m) 
D) aqueous FeI3 (0.030 m) 
E) aqueous NaI (0.030 m)

Question 14

Which one of the following substances would be the most soluble in C   ?

Accepted Answer

A) C4H10 
B) Li2O 
C) NH3 
D) HCl 
E) CH3CH2CH2OH 
A) C4H10 
B) Li2O 
C) NH3 
D) HCl 
E) CH3CH2CH2OH

Question 15

A solution containing 10.0 g of an unknown liquid and 90.0 g water has a freezing point of -3.33 °C.Given   for water,the molar mass of the unknown liquid is

Accepted Answer

A) 69.0 
B) 333 
C) 619 
D) 161 
E) 62.1 
A) 69.0 
B) 333 
C) 619 
D) 161 
E) 62.1

Question 16

The mole fraction of urea (MW = 60.0 g/mol)in a solution prepared by dissolving 16 g of urea in   of H2O is ________.

Accepted Answer

A) 0.58 
B) 0.37 
C) 0.13 
D) 0.11 
E) 9.1 
A) 0.58 
B) 0.37 
C) 0.13 
D) 0.11 
E) 9.1

Question 17

Of the concentration units below,only ________ uses kg of solvent in its calculation.

Accepted Answer

A) mass % 
B) ppm 
C) ppb 
D) molarity 
E) molality 
A) mass % 
B) ppm 
C) ppb 
D) molarity 
E) molality

Question 18

What is the molal concentration of a benzene (C6H6)solution prepared by mixing 13.0 g benzene with 38.0 g of carbon tetrachloride?

Accepted Answer

A) 2.40 
B) 622 
C) 4.38 
D) 0.342 
E) 0.508 
A) 2.40 
B) 622 
C) 4.38 
D) 0.342 
E) 0.508

Question 19

What is the mole fraction of LiCl in solution that is 9.0% by mass LiCl and has a density of 1.00 g/mL?

Accepted Answer

A) 0.960 
B) 2.33 
C) 0.0403 
D) 2.12 
E) 9.00 
A) 0.960 
B) 2.33 
C) 0.0403 
D) 2.12 
E) 9.00

Question 20

A 2.05 m aqueous solution of some unknown had a boiling point of 102.1 °C.Which one of the following could be the unknown compound? The boiling point elevation constant for water is

Accepted Answer

A) NaCl 
B) CH3OH 
C) C6H12O6 
D) Na2CO3 
E) CaBr2 
A) NaCl 
B) CH3OH 
C) C6H12O6 
D) Na2CO3 
E) CaBr2

Exam 13: Properties of Solutions

Which of the following would be least soluble in a nonpolar solvent?

Which of the following choices has the compounds correctly arranged in order of increasing solubility in water? (least soluble to most soluble)

291.5 grams of calcium chloride is dissolved in 1974.3 grams of water.Calculate the vapor pressure lowering (in mm Hg)of the solution at 25.0 °C.(Note: The vapor pressure of pure water at 25.0 °C is 23.76 mm Hg.)

The osmotic pressure of a solution formed by dissolving 45.0 mg of aspirin in 0.250 L of water at 25 °C is ________ atm.

What is the osmotic pressure (in atm)of a 0.015 M calcium chloride solution at 28 °C?

Calculate the molality of a 27.0% (by mass)aqueous solution of nitric acid.

Determine the freezing point (°C)of a 0.015 molal aqueous solution of MgSO4.Assume i = 2.0 for MgSO4.The molal freezing-point-depression constant of water is

What is the molarity of a 7.00% by mass ammonium chloride aqueous solution at 20 °C? Density of the solution is

Molality is defined as the ________.

Of the following,a 0.1 M aqueous solution of ________ will have the lowest freezing point.

A solution with a concentration higher than the solubility allows is ________.

An aqueous solution with a concentration of 18 ppm indicates that there is ________ per liter of solution.

Which of the following liquids will have the lowest freezing point?

Which one of the following substances would be the most soluble in C ?

A solution containing 10.0 g of an unknown liquid and 90.0 g water has a freezing point of -3.33 °C.Given for water,the molar mass of the unknown liquid is

The mole fraction of urea (MW = 60.0 g/mol)in a solution prepared by dissolving 16 g of urea in of H2O is ________.

Of the concentration units below,only ________ uses kg of solvent in its calculation.

What is the molal concentration of a benzene (C6H6)solution prepared by mixing 13.0 g benzene with 38.0 g of carbon tetrachloride?

What is the mole fraction of LiCl in solution that is 9.0% by mass LiCl and has a density of 1.00 g/mL?

A 2.05 m aqueous solution of some unknown had a boiling point of 102.1 °C.Which one of the following could be the unknown compound? The boiling point elevation constant for water is

Introduction: Matter, energy, and Measurement

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Chemical Reactions and Reaction Stoichiometry

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Electronic Structure of Atoms

Periodic Properties of the Elements

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Additional Aspects of Aqueous Equilibria

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Determine the freezing point (°C)of a 0.015 molal aqueous solution of MgSO₄.Assume i = 2.0 for MgSO₄.The molal freezing-point-depression constant of water is

The mole fraction of urea (MW = 60.0 g/mol)in a solution prepared by dissolving 16 g of urea in $The mole fraction of urea (MW = 60.0 g/mol)in a solution prepared by dissolving 16 g of urea in of H<sub>2</sub>O is .$ of H₂O is .

What is the molal concentration of a benzene (C₆H₆)solution prepared by mixing 13.0 g benzene with 38.0 g of carbon tetrachloride?