Question 1

Which aqueous solution listed below would be expected to have the highest boiling point?

Accepted Answer

A)   0.300 m glucose (C6H12O6) 
B)   0.150 m KBr
C)   0.100 m Na2SO4
D)   0.075 m Al(NO3) 3
E)   All of these solutions are expected to have identical boiling points.

Question 2

Which of the following concentration terms below represents moles of solute per kilogram of solvent?

Accepted Answer

A)   Molarity
B)   Molality
C)   Molar mass
D)   Mole fraction
E)   Mole percent

Question 3

After carefully noting the orientation in which the dipoles of water molecules surround the solute particles, which choice below best represents the true nature of how Mg(NO3) 2 exists in an aqueous solution?

Accepted Answer

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Question 4

Consider the following three statements about azeotropic mixtures and pick the correct answer.
I. An azeotropic mixture distills at a constant temperature.
II. An azeotropic mixture has a boiling point that is either higher or lower than the boiling points of the two components.
III. The compositions of the vapor and liquid phases are both the same for an azeotropic mixture.

Accepted Answer

A)   I is true, II and III are false
B)   I and III are true, II is false
C)   only II is true
D)   I, II, and III are all true
E)   I, II, and III are all false

Question 5

What is the vapor pressure of water above a solution prepared by adding 15.0 grams of lactose (C12H22O11)  to 100.0 grams of water at 338 K?
The vapor pressure of pure water at 338 K equals 187.5 torr. Molar Mass(C12H22O11)  = 342.30 g/mol and Molar Mass(H2O)  = 18.015 g/mol.

Accepted Answer

A)   1.47 torr
B)   24.5 torr
C)   28.1 torr
D)   163 torr
E)   186 torr

Question 6

After carefully noting the orientation in which water surrounds each solute particle, which choice below best represents the true nature of how CaCl2 exists in aqueous solution?

Accepted Answer

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Question 7

How many grams of KBr are required to prepare 1.50 L of 0.257 M aqueous solution?
MM(KBr)  = 119.00 g/mol

Accepted Answer

A)   3.24×10 - 3 g KBr
B)   20.4 g KBr
C)   45.9 g KBr
D)   309 g KBr
E)   695 g KBr

Question 8

At 25 ° C, 13.0 mg of CO dissolves in 500 g of water when the partial pressure of CO is 0.968 atm. What is the Henry's law constant (in molal/atm)  for CO at this temperature?

Accepted Answer

A)   4.48×10 - 2
B)   9.28×10 - 4
C)   9.59×10 - 4
D)   2.68×10 - 2
E)   none of these

Question 9

How many grams of Na2CO3 are required to prepare 25.0 mL of a 2.00% (m/v)  Na2CO3 solution?

Accepted Answer

A)   0.0800 g Na2CO3
B)   0.500 g Na2CO3
C)   2.00 g Na2CO3
D)   12.5 g Na2CO3
E)   50.0 g Na2CO3

Question 10

A research worker has only 300 g of a valuable solvent and wishes to use all of it to make up a 10.0 mass percent solution of solute A. How many grams of A should be weighed out?

Accepted Answer

A)   30.0 g
B)   22.2 g
C)   33.3 g
D)   10.0 g
E)   cannot calculate without knowing molar masses

Question 11

Which of the following aqueous solutions would have the greatest osmotic pressure?

Accepted Answer

A)   0.050 M CO(NH2) 2, (urea) 
B)   0.040 M NaCl
C)   0.030 M CaCl2
D)   0.020 M ScCl3
E)   0.010 M KCl

Question 12

A solution is prepared by mixing 22 g ethylene glycol [C2H4(OH) 2, molar mass = 62 g/mol] with 108 g of water. What is the mole fraction of ethylene glycol in the solution?

Accepted Answer

A)   0.056
B)   0.17
C)   0.35
D)   6.3
E)   none of these

Question 13

How many grams of glucose (C6H12O6)  must be dissolved in 750 g of ethanol (C2H5OH)  to prepare a 0.545 m solution?
MM(C6H12O6)  = 180.15 g/mol

Accepted Answer

A)   2.27×10 - 3 g glucose
B)   73.6 g glucose
C)   131 g glucose
D)   248 g glucose
E)   441 g glucose

Question 14

What is the vapor pressure of a solution of 30.0 g glycerol (C3H8O3)  in 504.5 grams of water at 25 ° C. The vapor pressure of pure water at 25 ° C is 23.76 torr and Molar Mass(C3H8O3)  = 92.09 g/mol.

Accepted Answer

A)   0.273 torr
B)   0.988 torr
C)   22.43 torr
D)   23.49 torr
E)   72.93 torr

Question 15

Calculate the osmotic pressure of a solution that contains 0.0010 mole of KCl and 0.0010 mole of BaCl2 per liter of solution at 298 K.

Accepted Answer

A)   0.049 atm
B)   6.2×10 - 3 atm
C)   0.12 atm
D)   0.073 atm
E)   over 25 atm

Question 16

What mass of KCl is required to prepare 500 mL of a 2.50 M aqueous solution of KCl?
MM(KCl)  = 74.55 g/mol.

Accepted Answer

A)   0.0168 g KCl
B)   0.0671 g KCl
C)   14.9 g KCl
D)   93.2 g KCl
E)   373 g KCl

Question 17

Arrange the following three aqueous solutions in order of decreasing freezing point. 0.50 M C6H12O6 0.20 M KNO 3 0.25 M MgCl2

Accepted Answer

A)   (highest fp)  0.20 M KNO3 > 0.50 M C6H12O6 > 0.25 M MgCl2 (lowest fp) 
B)   (highest fp)  0.50 M C6H12O6 > 0.20 M KNO3 > 0.25 M MgCl2 (lowest fp) 
C)   (highest fp)  0.50 M C6H12O6 > 0.25 M MgCl2 > 0.20 M KNO3 (lowest fp) 
D)   (highest fp)  0.25 M MgCl2 > 0.20 M KNO3 > 0.50 M C6H12O6 (lowest fp) 
E)   (highest fp)  0.25 M MgCl2 > 0.50 M C6H12O6 > 0.20 M KNO3 (lowest fp)

Question 18

What is the van't Hoff factor, " i ", for an aqueous solution of Calcium Nitrate?

Accepted Answer

A)   i = 1
B)   i = 2
C)   i = 3
D)   i = 5
E)   i = 9

Question 19

Benzene boils at 80.10 ° C and has a molal boiling constant, kb, of 2.53 C/m. When 2.15 g of a compound is dissolved in 20.0 g of benzene, the resulting solution has a boiling point of 81.10 ° C. What is the molar mass of the solute?

Accepted Answer

A)   272 g/mol
B)   108 g/mol
C)   78 g/mol
D)   2.15 g/mol
E)   93 g/mol

Question 20

The solubility limit for Sodium Chloride at 50 ° C is 37.0 grams of NaCl per 100 grams of water. What type of solution exists if 9.25 grams of NaCl is dissolved in 25 grams of water at 50 ° C?

Accepted Answer

A)   Supersaturated solution
B)   Dilute solution
C)   Saturated solution
D)   Heterogeneous solution
E)   Unsaturated solution

Exam 12: Solutions

Which aqueous solution listed below would be expected to have the highest boiling point?

Correct Answer
verified

A research worker has only 300 g of a valuable solvent and wishes to use all of it to make up a 10.0 mass percent solution of solute A. How many grams of A should be weighed out?

Correct Answer
verified

Benzene boils at 80.10 ° C and has a molal boiling constant, k_b, of 2.53 C/m. When 2.15 g of a compound is dissolved in 20.0 g of benzene, the resulting solution has a boiling point of 81.10 ° C. What is the molar mass of the solute?

Correct Answer
verified

Which of the following aqueous solutions would have the greatest osmotic pressure?

Correct Answer
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Correct Answer
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How many grams of glucose (C₆H₁₂O₆) must be dissolved in 750 g of ethanol (C₂H₅OH) to prepare a 0.545 m solution? MM(C₆H₁₂O₆) = 180.15 g/mol

Correct Answer
verified

What is the vapor pressure of a solution of 30.0 g glycerol (C₃H₈O₃) in 504.5 grams of water at 25 ° C. The vapor pressure of pure water at 25 ° C is 23.76 torr and Molar Mass(C₃H₈O₃) = 92.09 g/mol.

Correct Answer
verified

How many grams of Na₂CO₃ are required to prepare 25.0 mL of a 2.00% (m/v) Na₂CO₃ solution?

Correct Answer
verified

What mass of KCl is required to prepare 500 mL of a 2.50 M aqueous solution of KCl? MM(KCl) = 74.55 g/mol.

Correct Answer
verified

Calculate the osmotic pressure of a solution that contains 0.0010 mole of KCl and 0.0010 mole of BaCl₂ per liter of solution at 298 K.

Correct Answer
verified

A solution is prepared by mixing 22 g ethylene glycol [C₂H₄(OH) ₂, molar mass = 62 g/mol] with 108 g of water. What is the mole fraction of ethylene glycol in the solution?

Correct Answer
verified

Which of the following concentration terms below represents moles of solute per kilogram of solvent?

Correct Answer
verified

How many grams of KBr are required to prepare 1.50 L of 0.257 M aqueous solution? MM(KBr) = 119.00 g/mol

Correct Answer
verified

Arrange the following three aqueous solutions in order of decreasing freezing point. 0.50 M C₆H₁₂O₆ 0.20 M KNO₃ 0.25 M MgCl₂

Correct Answer
verified

The solubility limit for Sodium Chloride at 50 ° C is 37.0 grams of NaCl per 100 grams of water. What type of solution exists if 9.25 grams of NaCl is dissolved in 25 grams of water at 50 ° C?

Correct Answer
verified

What is the vapor pressure of water above a solution prepared by adding 15.0 grams of lactose (C₁₂H₂₂O₁₁) to 100.0 grams of water at 338 K? The vapor pressure of pure water at 338 K equals 187.5 torr. Molar Mass(C₁₂H₂₂O₁₁) = 342.30 g/mol and Molar Mass(H₂O) = 18.015 g/mol.

Correct Answer
verified

After carefully noting the orientation in which water surrounds each solute particle, which choice below best represents the true nature of how CaCl₂ exists in aqueous solution?

Correct Answer
verified

At 25 ° C, 13.0 mg of CO dissolves in 500 g of water when the partial pressure of CO is 0.968 atm. What is the Henry's law constant (in molal/atm) for CO at this temperature?

Correct Answer
verified

What is the van't Hoff factor, " i ", for an aqueous solution of Calcium Nitrate?

Correct Answer
verified

After carefully noting the orientation in which the dipoles of water molecules surround the solute particles, which choice below best represents the true nature of how Mg(NO₃) ₂ exists in an aqueous solution?

Correct Answer
verified

Exam 12: Solutions

Which aqueous solution listed below would be expected to have the highest boiling point?

Correct AnswerverifiedShow Answer

A research worker has only 300 g of a valuable solvent and wishes to use all of it to make up a 10.0 mass percent solution of solute A. How many grams of A should be weighed out?

Correct AnswerverifiedShow Answer

Benzene boils at 80.10 ° C and has a molal boiling constant, kb, of 2.53 C/m. When 2.15 g of a compound is dissolved in 20.0 g of benzene, the resulting solution has a boiling point of 81.10 ° C. What is the molar mass of the solute?

Correct AnswerverifiedShow Answer

Which of the following aqueous solutions would have the greatest osmotic pressure?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

How many grams of glucose (C6H12O6) must be dissolved in 750 g of ethanol (C2H5OH) to prepare a 0.545 m solution? MM(C6H12O6) = 180.15 g/mol

Correct AnswerverifiedShow Answer

What is the vapor pressure of a solution of 30.0 g glycerol (C3H8O3) in 504.5 grams of water at 25 ° C. The vapor pressure of pure water at 25 ° C is 23.76 torr and Molar Mass(C3H8O3) = 92.09 g/mol.

Correct AnswerverifiedShow Answer

How many grams of Na2CO3 are required to prepare 25.0 mL of a 2.00% (m/v) Na2CO3 solution?

Correct AnswerverifiedShow Answer

What mass of KCl is required to prepare 500 mL of a 2.50 M aqueous solution of KCl? MM(KCl) = 74.55 g/mol.

Correct AnswerverifiedShow Answer

Calculate the osmotic pressure of a solution that contains 0.0010 mole of KCl and 0.0010 mole of BaCl2 per liter of solution at 298 K.

Correct AnswerverifiedShow Answer

A solution is prepared by mixing 22 g ethylene glycol [C2H4(OH) 2, molar mass = 62 g/mol] with 108 g of water. What is the mole fraction of ethylene glycol in the solution?

Correct AnswerverifiedShow Answer

Which of the following concentration terms below represents moles of solute per kilogram of solvent?

Correct AnswerverifiedShow Answer

How many grams of KBr are required to prepare 1.50 L of 0.257 M aqueous solution? MM(KBr) = 119.00 g/mol

Correct AnswerverifiedShow Answer

Arrange the following three aqueous solutions in order of decreasing freezing point. 0.50 M C6H12O6 0.20 M KNO 3 0.25 M MgCl2

Correct AnswerverifiedShow Answer

The solubility limit for Sodium Chloride at 50 ° C is 37.0 grams of NaCl per 100 grams of water. What type of solution exists if 9.25 grams of NaCl is dissolved in 25 grams of water at 50 ° C?

Correct AnswerverifiedShow Answer

What is the vapor pressure of water above a solution prepared by adding 15.0 grams of lactose (C12H22O11) to 100.0 grams of water at 338 K? The vapor pressure of pure water at 338 K equals 187.5 torr. Molar Mass(C12H22O11) = 342.30 g/mol and Molar Mass(H2O) = 18.015 g/mol.

Correct AnswerverifiedShow Answer

After carefully noting the orientation in which water surrounds each solute particle, which choice below best represents the true nature of how CaCl2 exists in aqueous solution?

Correct AnswerverifiedShow Answer

At 25 ° C, 13.0 mg of CO dissolves in 500 g of water when the partial pressure of CO is 0.968 atm. What is the Henry's law constant (in molal/atm) for CO at this temperature?

Correct AnswerverifiedShow Answer

What is the van't Hoff factor, " i ", for an aqueous solution of Calcium Nitrate?

Correct AnswerverifiedShow Answer

After carefully noting the orientation in which the dipoles of water molecules surround the solute particles, which choice below best represents the true nature of how Mg(NO3) 2 exists in an aqueous solution?

Correct AnswerverifiedShow Answer

Correct Answer
verified

Correct Answer
verified

Benzene boils at 80.10 ° C and has a molal boiling constant, k_b, of 2.53 C/m. When 2.15 g of a compound is dissolved in 20.0 g of benzene, the resulting solution has a boiling point of 81.10 ° C. What is the molar mass of the solute?

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

How many grams of glucose (C₆H₁₂O₆) must be dissolved in 750 g of ethanol (C₂H₅OH) to prepare a 0.545 m solution? MM(C₆H₁₂O₆) = 180.15 g/mol

Correct Answer
verified

What is the vapor pressure of a solution of 30.0 g glycerol (C₃H₈O₃) in 504.5 grams of water at 25 ° C. The vapor pressure of pure water at 25 ° C is 23.76 torr and Molar Mass(C₃H₈O₃) = 92.09 g/mol.

Correct Answer
verified

How many grams of Na₂CO₃ are required to prepare 25.0 mL of a 2.00% (m/v) Na₂CO₃ solution?

Correct Answer
verified

Correct Answer
verified

Calculate the osmotic pressure of a solution that contains 0.0010 mole of KCl and 0.0010 mole of BaCl₂ per liter of solution at 298 K.

Correct Answer
verified

A solution is prepared by mixing 22 g ethylene glycol [C₂H₄(OH) ₂, molar mass = 62 g/mol] with 108 g of water. What is the mole fraction of ethylene glycol in the solution?

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Arrange the following three aqueous solutions in order of decreasing freezing point. 0.50 M C₆H₁₂O₆ 0.20 M KNO₃ 0.25 M MgCl₂

Correct Answer
verified

Correct Answer
verified

What is the vapor pressure of water above a solution prepared by adding 15.0 grams of lactose (C₁₂H₂₂O₁₁) to 100.0 grams of water at 338 K? The vapor pressure of pure water at 338 K equals 187.5 torr. Molar Mass(C₁₂H₂₂O₁₁) = 342.30 g/mol and Molar Mass(H₂O) = 18.015 g/mol.

Correct Answer
verified

After carefully noting the orientation in which water surrounds each solute particle, which choice below best represents the true nature of how CaCl₂ exists in aqueous solution?

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

After carefully noting the orientation in which the dipoles of water molecules surround the solute particles, which choice below best represents the true nature of how Mg(NO₃) ₂ exists in an aqueous solution?

Correct Answer
verified