Question 1

The concentration of HCl in a solution that is prepared by dissolving 5.5 g of HCl in 200 g of C2H6O is ________ molal.

Accepted Answer

A) 27.5 
B) 7.5 × 10-4 
C) 3.3 × 10-2 
D) 0.75 
E) 1.3

Question 2

Calculate the mole fraction of HCl in a 7.20% (by mass)aqueous solution.

Accepted Answer

A) 0.0369 
B) 0.0383 
C) 0.0739 
D) 0.0185 
E) The density of the solution is needed to solve the problem.

Question 3

Calculate the molarity of phosphoric acid (H3PO4)in a 38.4% (by mass)aqueous solution.

Accepted Answer

A) 0.115 m 
B) 0.206 m 
C) 0.0514 m 
D) 0.103 m 
E) The density of the solution is needed to solve the problem.

Question 4

What is the freezing point (°C)of a solution prepared by dissolving 11.3 g of Ca(NO3)2 (formula weight = 164 g/mol)in 115 g of water? The molal freezing point depression constant for water is 1.86 °C/m.

Accepted Answer

A) -3.34 
B) -1.11 
C) 3.34 
D) 1.11 
E) 0.00

Question 5

A supersaturated solution ________.

Accepted Answer

A) is one with more than one solute 
B) is one that has been heated 
C) is one with a higher concentration than the solubility 
D) must be in contact with undissolved solid 
E) exists only in theory and cannot actually be prepared

Question 6

A solution contains 150.8 grams of NaCl in 678.3 grams of water. Calculate the vapor pressure lowering (in torr)of the solution at 25.0 °C. (Note: The vapor pressure of pure water at 25.0 °C is 23.76 torr.)

Accepted Answer

The answer of A solution contains 150.8 grams of NaCl...

Question 7

A solution is prepared by dissolving 15.0 g of NH3 in 250.0 g of water. The density of the resulting solution is 0.974 g/mL. The molality of NH3 in the solution is ________ m.

Accepted Answer

A) 0.00353 
B) 0.882 
C) 60.0 
D) 3.24 
E) 3.53

Question 8

Calculate the molality of a 10.0% (by mass)aqueous solution of hydrochloric acid.

Accepted Answer

A) 2.40 m 
B) 87.4 m 
C) 0.791 m 
D) 1.20 m 
E) The density of the solution is needed to solve the problem.

Question 9

A solution is prepared by dissolving calcium chloride in water and diluting to 500.0 mL. If this solution contains 44 ppm chloride ions, the concentration of calcium ions is ________ ppm.

Accepted Answer

A) 44 
B) 88 
C) 22 
D) 11 
E) 500

Question 10

-A sample of potassium chlorate (15.0 g)is dissolved in 201 g of water at 70 °C, with precautions taken to avoid evaporation of any water. The solution is cooled to 30.0 °C and no precipitate is observed. This solution is ________.

Accepted Answer

A) hydrated 
B) miscible 
C) saturated 
D) unsaturated 
E) supersaturated

Question 11

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

Accepted Answer

A) 4.56 
B) 370 
C) 1.51 
D) 2.28 
E) The density of the solution is needed to solve the problem.

Question 12

Which of the following substances is more likely to dissolve in water?

Accepted Answer

A) HOCH2CH2OH 
B) CHCl3 
C)  O  CH3(CH2)9CH 
D) CH3(CH2)8CH2OH 
E) CCl4

Question 13

A solution contains 30 ppm of benzene. The density of the solution is 1.00 g/mL. This means that ________.

Accepted Answer

A) there are 30 mg of benzene in 1.0 L of this solution 
B) 100 g of the solution contains 30 g of benzene 
C) 100 g of the solution contains 30 mg of benzene 
D) the solution is 30% by mass of benzene 
E) the molarity of the solution is 30 M

Question 14

-A sample of potassium nitrate (49.0 g)is dissolved in 101 g of water at 100 °C, with precautions taken to avoid evaporation of any water. The solution is cooled to 30.0 °C and a small amount of precipitate is observed. This solution is ________.

Accepted Answer

A) hydrated 
B) placated 
C) saturated 
D) unsaturated 
E) supersaturated

Question 15

The concentration of urea (MW = 60.0 g/mol)in a solution prepared by dissolving 16 g of urea in 39 g of H2O is ________ molal.

Accepted Answer

A) 96 
B) 6.8 
C) 0.68 
D) 6.3 
E) 0.11

Question 16

A solution is prepared by dissolving 6.00 g of an unknown nonelectrolyte in enough water to make 1.00 L of solution. The osmotic pressure of this solution is 0.750 atm at 25.0 °C. What is the molecular weight (g/mol)of the unknown solute?

Accepted Answer

A) 16.4 
B) 196 
C) 110 
D) 30.6 
E) 5.12 × 10-3

Question 17

A solution is prepared by adding 1.10 mol of KCl to 889 g of water. The concentration of KCl is ________ molal.

Accepted Answer

A) 1.24 × 10-3 
B) 808 
C) 0.808 
D) 978 
E) 1.24

Question 18

A solution is prepared by dissolving 2.60 g of a strong electrolyte (formula weight = 101 g/mol)in enough water to make 1.00 L of solution. The osmotic pressure of the solution is 1.25 atm at 25.0 °C. What is the van't Hoff factor (i)for the unknown solute?

Accepted Answer

A) 0 
B) 0.99 
C) 1.98 
D) 2.98 
E) 0.630

Question 19

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)

Question 20

The value of the boiling-point-elevation constant (Kb)depends on the identity of the solvent.

Accepted Answer

A) True 
 B)False

Exam 13: Properties of Solutions

The concentration of HCl in a solution that is prepared by dissolving 5.5 g of HCl in 200 g of C₂H₆O is ________ molal.

Calculate the mole fraction of HCl in a 7.20% (by mass) aqueous solution.

Calculate the molarity of phosphoric acid (H₃PO₄) in a 38.4% (by mass) aqueous solution.

What is the freezing point (°C) of a solution prepared by dissolving 11.3 g of Ca(NO₃) ₂ (formula weight = 164 g/mol) in 115 g of water? The molal freezing point depression constant for water is 1.86 °C/m.

A supersaturated solution ________.

A solution contains 150.8 grams of NaCl in 678.3 grams of water. Calculate the vapor pressure lowering (in torr)of the solution at 25.0 °C. (Note: The vapor pressure of pure water at 25.0 °C is 23.76 torr.)

A solution is prepared by dissolving 15.0 g of NH₃ in 250.0 g of water. The density of the resulting solution is 0.974 g/mL. The molality of NH₃ in the solution is ________ m.

Calculate the molality of a 10.0% (by mass) aqueous solution of hydrochloric acid.

A solution is prepared by dissolving calcium chloride in water and diluting to 500.0 mL. If this solution contains 44 ppm chloride ions, the concentration of calcium ions is ________ ppm.

-A sample of potassium chlorate (15.0 g) is dissolved in 201 g of water at 70 °C, with precautions taken to avoid evaporation of any water. The solution is cooled to 30.0 °C and no precipitate is observed. This solution is ________.

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

Which of the following substances is more likely to dissolve in water?

A solution contains 30 ppm of benzene. The density of the solution is 1.00 g/mL. This means that ________.

-A sample of potassium nitrate (49.0 g) is dissolved in 101 g of water at 100 °C, with precautions taken to avoid evaporation of any water. The solution is cooled to 30.0 °C and a small amount of precipitate is observed. This solution is ________.

The concentration of urea (MW = 60.0 g/mol) in a solution prepared by dissolving 16 g of urea in 39 g of H₂O is ________ molal.

A solution is prepared by dissolving 6.00 g of an unknown nonelectrolyte in enough water to make 1.00 L of solution. The osmotic pressure of this solution is 0.750 atm at 25.0 °C. What is the molecular weight (g/mol) of the unknown solute?

A solution is prepared by adding 1.10 mol of KCl to 889 g of water. The concentration of KCl is ________ molal.

A solution is prepared by dissolving 2.60 g of a strong electrolyte (formula weight = 101 g/mol) in enough water to make 1.00 L of solution. The osmotic pressure of the solution is 1.25 atm at 25.0 °C. What is the van't Hoff factor (i) for the unknown solute?

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

The value of the boiling-point-elevation constant (K_b)depends on the identity of the solvent.

Exam 13: Properties of Solutions

The concentration of HCl in a solution that is prepared by dissolving 5.5 g of HCl in 200 g of C2H6O is ________ molal.

Calculate the mole fraction of HCl in a 7.20% (by mass) aqueous solution.

Calculate the molarity of phosphoric acid (H3PO4) in a 38.4% (by mass) aqueous solution.

What is the freezing point (°C) of a solution prepared by dissolving 11.3 g of Ca(NO3) 2 (formula weight = 164 g/mol) in 115 g of water? The molal freezing point depression constant for water is 1.86 °C/m.

A supersaturated solution ________.

A solution contains 150.8 grams of NaCl in 678.3 grams of water. Calculate the vapor pressure lowering (in torr)of the solution at 25.0 °C. (Note: The vapor pressure of pure water at 25.0 °C is 23.76 torr.)

A solution is prepared by dissolving 15.0 g of NH3 in 250.0 g of water. The density of the resulting solution is 0.974 g/mL. The molality of NH3 in the solution is ________ m.

Calculate the molality of a 10.0% (by mass) aqueous solution of hydrochloric acid.

A solution is prepared by dissolving calcium chloride in water and diluting to 500.0 mL. If this solution contains 44 ppm chloride ions, the concentration of calcium ions is ________ ppm.

-A sample of potassium chlorate (15.0 g) is dissolved in 201 g of water at 70 °C, with precautions taken to avoid evaporation of any water. The solution is cooled to 30.0 °C and no precipitate is observed. This solution is ________.

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

Which of the following substances is more likely to dissolve in water?

A solution contains 30 ppm of benzene. The density of the solution is 1.00 g/mL. This means that ________.

-A sample of potassium nitrate (49.0 g) is dissolved in 101 g of water at 100 °C, with precautions taken to avoid evaporation of any water. The solution is cooled to 30.0 °C and a small amount of precipitate is observed. This solution is ________.

The concentration of urea (MW = 60.0 g/mol) in a solution prepared by dissolving 16 g of urea in 39 g of H2O is ________ molal.

A solution is prepared by dissolving 6.00 g of an unknown nonelectrolyte in enough water to make 1.00 L of solution. The osmotic pressure of this solution is 0.750 atm at 25.0 °C. What is the molecular weight (g/mol) of the unknown solute?

A solution is prepared by adding 1.10 mol of KCl to 889 g of water. The concentration of KCl is ________ molal.

A solution is prepared by dissolving 2.60 g of a strong electrolyte (formula weight = 101 g/mol) in enough water to make 1.00 L of solution. The osmotic pressure of the solution is 1.25 atm at 25.0 °C. What is the van't Hoff factor (i) for the unknown solute?

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

The value of the boiling-point-elevation constant (Kb)depends on the identity of the solvent.

The concentration of HCl in a solution that is prepared by dissolving 5.5 g of HCl in 200 g of C₂H₆O is ________ molal.

Calculate the molarity of phosphoric acid (H₃PO₄) in a 38.4% (by mass) aqueous solution.

What is the freezing point (°C) of a solution prepared by dissolving 11.3 g of Ca(NO₃) ₂ (formula weight = 164 g/mol) in 115 g of water? The molal freezing point depression constant for water is 1.86 °C/m.

A solution is prepared by dissolving 15.0 g of NH₃ in 250.0 g of water. The density of the resulting solution is 0.974 g/mL. The molality of NH₃ in the solution is ________ m.

The concentration of urea (MW = 60.0 g/mol) in a solution prepared by dissolving 16 g of urea in 39 g of H₂O is ________ molal.

The value of the boiling-point-elevation constant (K_b)depends on the identity of the solvent.