Question 1

What is the molarity of ions in an aqueous 0.50 M Na2SO4 solution?

Accepted Answer

A)   0.50 M
B)   1.0 M
C)   1.5 M
D)   3.0 M
E)   3.5 MF) B) and C)
G) None of the above

Question 2

A solution is prepared by mixing 4.00 grams of benzene (molar mass = 78.1 g/mol) , 4.00 grams of CCl4 (molar mass = 153.8 g/mol) , and 4.00 grams of C S2 (molar mass = 76.1 g/mol) . The mole fraction of benzene in this solution is:

Accepted Answer

A)   0.051
B)   0.200
C)   0.333
D)   0.395
E)   0.605F) A) and C)
G) A) and B)

Question 3

What is the molarity of ions in an aqueous 0.25 M Na3PO4 solution?

Accepted Answer

A)   0.25 M
B)   0.50 M
C)   1.0 M
D)   1.5 M
E)   2.0 MF) C) and D)
G) A) and D)

Question 4

What mass of CsCl must be added to 0.55 liters of water to produce a 0.430 m solution?
Molar Mass(CsCl)  = 168.35 g/mol and Density(H2O)  = 1.00 g/mL

Accepted Answer

A)   0.237 g CsCl
B)   0.782 g CsCl
C)   39.8 g CsCl
D)   132 g CsCl
E)   215 g CsClF) A) and E)
G) B) and C)

Question 5

A quantity of 7.85 g of a compound having the empirical formula C5H4 is dissolved in 301 g of benzene. The freezing point is 1.05 ° C below that of pure benzene (kf = 5.12 ° C/m) . The molar mass of the species in solution in benzene is:

Accepted Answer

A)   64.0 g/mol
B)   38.3 g/mol
C)   11.5 g/mol
D)   127 g/mol
E)   194 g/molF) A) and B)
G) None of the above

Question 6

Which aqueous solution is predicted to have the highest boiling point?

Accepted Answer

A)   0.03 m CO(NH2) 2, (urea) 
B)   0.02 m KCl
C)   0.02 m CaCl2
D)   0.02 m La(NO3) 3
E)   insufficient data are givenF) A) and B)
G) None of the above

Question 7

How many grams of NH3 are present in 2.50 L of 3.00 M NH3 solution?
MM(NH3)  = 17.03 g/mol

Accepted Answer

A)   0.0705 g NH3
B)   7.50 g NH3
C)   14.2 g NH3
D)   20.4 g NH3
E)   128 g NH3F) A) and B)
G) D) and E)

Question 8

Which aqueous solution would be predicted to have the lowest freezing point?

Accepted Answer

A)   0.01 m methanol (CH3OH) 
B)   0.01 m NaCl
C)   0.01 m KOH
D)   0.01 m Ca(NO3) 2
E)   all are the sameF) C) and D)
G) A) and E)

Question 9

A solution contains 1.00 mole of NaCl in 500 g of water. What is the molal concentration of NaCl?

Accepted Answer

A)   10.5 m
B)   2.00 m
C)   1.00 m
D)   0.0347 m
E)   none of theseF) D) and E)
G) A) and D)

Question 10

Arrange the following aqueous solutions in order of increasing osmotic pressure . 0.1 M NaCl 0.1 M glucose 0.1 M BaCl2

Accepted Answer

A)   (lowest)  0.1 M NaCl 2 (highest) 
B)   (lowest)  0.1 M NaCl 2 
C)   (lowest)  0.1 M glucose 2 
D)   (lowest)  0.1 M glucose 2 (highest) 
E)   0.1 M BaCl2 = 0.1 M glucose = 0.1 M NaClF) C) and D)
G) A) and B)

Question 11

Lysozyme is an enzyme that breaks bacterial cell walls. A solution containing 0.150 g of this enzyme in 210 mL of solution has an osmotic pressure of 0.953 torr at 25 ° C. What is the molar mass of lysozyme?

Accepted Answer

A)   1.40×104 g/mol
B)   2.94×103 g/mol
C)   1.17×103 g/mol
D)   18.3 g/mol
E)   14.0 g/molF) None of the above
G) C) and D)

Question 12

After carefully noting the orientation in which water molecules surround each solute particle, which choice below best represents the true nature of how Na2SO4 exists in an aqueous solution?

Accepted Answer

A)   2SO4 exists in an aqueous solution? 
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G) A) and E)

Question 13

The molarity and molality of a solution:

Accepted Answer

A)   may never be equal.
B)   are equal for all solutions.
C)   both express the quantity of solute in moles.
D)   are equal for all solutions having water as the solvent.
E)   are equal for all concentrated solutions.F) B) and C)
G) C) and D)

Question 14

The solubility of a gas in water is highest for:

Accepted Answer

A)   low pressure and low temperature.
B)   low pressure and high temperature.
C)   high pressure and low temperature.
D)   high pressure and high temperature.
E)   neither pressure nor temperature changes gas solubility.F) A) and B)
G) C) and D)

Question 15

At 10 ° C the Henry's law constant for O2 is 1.7×10 - 3 molal/atm. What is the molal concentration of O2 in solution that is in equilibrium with air (20 mole % O2)  at 10 ° C?

Accepted Answer

A)   3.4×10 - 4 m
B)   1.7×10 - 3 m
C)   1.1×10 - 2 m
D)   3.4×10 - 2 m
E)   none of theseF) B) and E)
G) B) and D)

Question 16

What is the mole fraction of NH3 for a 5.00% (m/m)  aqueous solution of NH3?

Accepted Answer

A)   c NH3 = 0.0527
B)   c NH3 = 0.190
C)   c NH3 = 0.294
D)   c NH3 = 0.810
E)   c NH3 = 0.947F) C) and D)
G) A) and E)

Question 17

The solubility of potassium sulfate in water is 6.85 g/100 mL at 0 ° C and 24.1 g/100 mL at 100C. From this we can conclude that:

Accepted Answer

A)   potassium sulfate is an electrolyte.
B)   the enthalpy of solution is less than zero.
C)   potassium sulfate is insoluble in CH3OH.
D)   the enthalpy of solution is positive.
E)   none of theseF) B) and C)
G) A) and E)

Question 18

Which of the following is soluble in H2O?

Accepted Answer

A)   Fe(OH) 3
B)   AgI
C)   PbSO4
D)   NaCl
E)   all of themF) C) and D)
G) B) and C)

Question 19

Arrange the following solutions in order of increasing boiling point . 0.25 m KCl 0.15 m AlCl3 0.55 m ethanol (CH3CH2OH)

Accepted Answer

A)   (lowest bp)  0.55 m Ethanol m KCl m AlCl3 (highest bp) 
B)   (lowest bp)  0.15 m AlCl3 m KCl m Ethanol (highest bp) 
C)   (lowest bp)  0.55 m Ethanol m AlCl3 m KCl (highest bp) 
D)   (lowest bp)  0.25 m KCl m Ethanol m AlCl3 (highest bp) 
E)   (lowest bp)  0.25 m KCl m AlCl3 m Ethanol (highest bp) F) D) and E)
G) C) and E)

Question 20

An aqueous solution of hydrochloric acid contains 36.0% (m/m) . What is the molality of this same solution?
MM(HCl)  = 36.46 g/mol and MM(H2O)  = 18.015 g/mol

Accepted Answer

A)   0.217 m
B)   0.563 m
C)   9.87 m
D)   15.4 m
E)   98.7 mF) All of the above
G) A) and E)

Exam 12: Solutions

Arrange the following solutions in order of increasing boiling point . 0.25 m KCl 0.15 m AlCl3 0.55 m ethanol (CH3CH2OH)

Correct AnswerverifiedShow Answer

A solution is prepared by mixing 4.00 grams of benzene (molar mass = 78.1 g/mol) , 4.00 grams of CCl4 (molar mass = 153.8 g/mol) , and 4.00 grams of C S2 (molar mass = 76.1 g/mol) . The mole fraction of benzene in this solution is:

Correct AnswerverifiedShow Answer

What is the mole fraction of NH3 for a 5.00% (m/m) aqueous solution of NH3?

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The molarity and molality of a solution:

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How many grams of NH3 are present in 2.50 L of 3.00 M NH3 solution? MM(NH3) = 17.03 g/mol

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An aqueous solution of hydrochloric acid contains 36.0% (m/m) . What is the molality of this same solution? MM(HCl) = 36.46 g/mol and MM(H2O) = 18.015 g/mol

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At 10 ° C the Henry's law constant for O2 is 1.7×10 - 3 molal/atm. What is the molal concentration of O2 in solution that is in equilibrium with air (20 mole % O2) at 10 ° C?

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A solution contains 1.00 mole of NaCl in 500 g of water. What is the molal concentration of NaCl?

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A quantity of 7.85 g of a compound having the empirical formula C5H4 is dissolved in 301 g of benzene. The freezing point is 1.05 ° C below that of pure benzene (kf = 5.12 ° C/m) . The molar mass of the species in solution in benzene is:

Correct AnswerverifiedShow Answer

Which aqueous solution would be predicted to have the lowest freezing point?

Correct AnswerverifiedShow Answer

The solubility of potassium sulfate in water is 6.85 g/100 mL at 0 ° C and 24.1 g/100 mL at 100C. From this we can conclude that:

Correct AnswerverifiedShow Answer

After carefully noting the orientation in which water molecules surround each solute particle, which choice below best represents the true nature of how Na2SO4 exists in an aqueous solution?

Correct AnswerverifiedShow Answer

What is the molarity of ions in an aqueous 0.25 M Na3PO4 solution?

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Which aqueous solution is predicted to have the highest boiling point?

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Arrange the following aqueous solutions in order of increasing osmotic pressure . 0.1 M NaCl 0.1 M glucose 0.1 M BaCl2

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Lysozyme is an enzyme that breaks bacterial cell walls. A solution containing 0.150 g of this enzyme in 210 mL of solution has an osmotic pressure of 0.953 torr at 25 ° C. What is the molar mass of lysozyme?

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What is the molarity of ions in an aqueous 0.50 M Na2SO4 solution?

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The solubility of a gas in water is highest for:

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What mass of CsCl must be added to 0.55 liters of water to produce a 0.430 m solution? Molar Mass(CsCl) = 168.35 g/mol and Density(H2O) = 1.00 g/mL

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Which of the following is soluble in H2O?

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Arrange the following solutions in order of increasing boiling point . 0.25 m KCl 0.15 m AlCl₃ 0.55 m ethanol (CH₃CH₂OH)

Correct Answer
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A solution is prepared by mixing 4.00 grams of benzene (molar mass = 78.1 g/mol) , 4.00 grams of CCl₄ (molar mass = 153.8 g/mol) , and 4.00 grams of C S₂ (molar mass = 76.1 g/mol) . The mole fraction of benzene in this solution is:

Correct Answer
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What is the mole fraction of NH₃ for a 5.00% (m/m) aqueous solution of NH₃?

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How many grams of NH₃ are present in 2.50 L of 3.00 M NH₃ solution? MM(NH₃) = 17.03 g/mol

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An aqueous solution of hydrochloric acid contains 36.0% (m/m) . What is the molality of this same solution? MM(HCl) = 36.46 g/mol and MM(H₂O) = 18.015 g/mol

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At 10 ° C the Henry's law constant for O₂ is 1.7×10^{- 3} molal/atm. What is the molal concentration of O₂ in solution that is in equilibrium with air (20 mole % O₂) at 10 ° C?

Correct Answer
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Correct Answer
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A quantity of 7.85 g of a compound having the empirical formula C₅H₄ is dissolved in 301 g of benzene. The freezing point is 1.05 ° C below that of pure benzene (k_f = 5.12 ° C/m) . The molar mass of the species in solution in benzene is:

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After carefully noting the orientation in which water molecules surround each solute particle, which choice below best represents the true nature of how Na₂SO₄ exists in an aqueous solution?

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What is the molarity of ions in an aqueous 0.25 M Na₃PO₄ solution?

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Arrange the following aqueous solutions in order of increasing osmotic pressure . 0.1 M NaCl 0.1 M glucose 0.1 M BaCl₂

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What is the molarity of ions in an aqueous 0.50 M Na₂SO₄ solution?

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What mass of CsCl must be added to 0.55 liters of water to produce a 0.430 m solution? Molar Mass(CsCl) = 168.35 g/mol and Density(H₂O) = 1.00 g/mL

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Which of the following is soluble in H₂O?

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