Question 1

Assuming that the volumes are additive, what volume of water must be added to 35.0 mL of 15.0%(w/v) KOH to make a 10.0%(w/v) solution?

Accepted Answer

A)  15.0 mL 
B)  17.5 mL 
C)  23.3 mL 
D)  52.5 mL 
A)  15.0 mL 
B)  17.5 mL 
C)  23.3 mL 
D)  52.5 mL

Question 2

To which of the following does thermal pollution generally refer?

Accepted Answer

A)  the decrease in the O2 content of warm water as compared with cold water 
B)  the increase in the O2 content of cold water as compared with warm water 
C)  both the decrease in the O2 content of warm water as compared with cold water, and the increase in the O2 content of cold water as compared with warm water 
D)  neither the decrease in the O2 content of warm water as compared with cold water, and the increase in the O2 content of cold water as compared with warm water 
A)  the decrease in the O2 content of warm water as compared with cold water 
B)  the increase in the O2 content of cold water as compared with warm water 
C)  both the decrease in the O2 content of warm water as compared with cold water, and the increase in the O2 content of cold water as compared with warm water 
D)  neither the decrease in the O2 content of warm water as compared with cold water, and the increase in the O2 content of cold water as compared with warm water

Question 3

Which of the following is a weak electrolyte?

Accepted Answer

A)  KCl 
B)  CH3COOH 
C)  both KCI and CH3COOH 
D)  neither KCI or CH3COOH 
A)  KCl 
B)  CH3COOH 
C)  both KCI and CH3COOH 
D)  neither KCI or CH3COOH

Question 4

Which of the following is a description of a hydrated salt?

Accepted Answer

A)  a salt that is insoluble in water 
B)  a salt that is soluble in water 
C)  a salt with no water incorporated in its crystal structure 
D)  a salt with water incorporated in its crystal structure 
A)  a salt that is insoluble in water 
B)  a salt that is soluble in water 
C)  a salt with no water incorporated in its crystal structure 
D)  a salt with water incorporated in its crystal structure

Question 5

A typical sample of brass is 67%(w/w) copper and 33%(w/w) zinc. How many moles of zinc are dissolved in 67 grams of copper?

Accepted Answer

A)  0.33 mol 
B)  0.50 mol 
C)  0.67 mol 
D)  1.0 mol 
A)  0.33 mol 
B)  0.50 mol 
C)  0.67 mol 
D)  1.0 mol

Question 6

A solution is prepared by dissolving 53.5 grams of ammonium chloride, NH4Cl, in 4000.0 grams of water. What is the freezing point of the solution? (The freezing point depression constant for water is 1.86°C/mole solute in 1000 g of water.)

Accepted Answer

A)  -0.37°C 
B)  -0.47°C 
C)  -0.93°C 
D)  -1.86°C 
A)  -0.37°C 
B)  -0.47°C 
C)  -0.93°C 
D)  -1.86°C

Question 7

If we wish to prepare a 0.50 M solution of NaCl, how much of water should we add to 1.0 mole of NaCl?

Accepted Answer

A)  We need to add 2.0 mol of water. 
B)  We need to add 2.0 L of water. 
C)  We need to add 2.0 × 103 g of water. 
D)  We need to add enough water to make 2.0 L of solution. 
A)  We need to add 2.0 mol of water. 
B)  We need to add 2.0 L of water. 
C)  We need to add 2.0 × 103 g of water. 
D)  We need to add enough water to make 2.0 L of solution.

Question 8

Which of the following solutions will have the highest electrical conductance?

Accepted Answer

A)  0.1 M NaCl 
B)  0.1 M BaCl2 
C)  0.1 M AlCl3 
D)  All of these will have the same electrical conductance. 
A)  0.1 M NaCl 
B)  0.1 M BaCl2 
C)  0.1 M AlCl3 
D)  All of these will have the same electrical conductance.

Question 9

Which of the following is a weak electrolyte?

Accepted Answer

A)  NaCl 
B)  CH3COOH 
C)  both NaCI and CH3COOH 
D)  neither NaCI or CH3COOH 
A)  NaCl 
B)  CH3COOH 
C)  both NaCI and CH3COOH 
D)  neither NaCI or CH3COOH

Question 10

A solution of acetic acid is labeled 15%(w/v). How much of water must be added to 30.0 mL of this solution to reduce the concentration to 5.0%(w/v)? (Assume volumes are additive.)

Accepted Answer

A)  30.0 mL 
B)  60.0 mL 
C)  90.0 mL 
D)  120.0 mL 
A)  30.0 mL 
B)  60.0 mL 
C)  90.0 mL 
D)  120.0 mL

Question 11

Isotonic saline is 0.89% NaCl (w/v). Suppose you want to prepare 1.0 L of isotonic solution of NH4Cl. What mass of NH4Cl would you need?

Accepted Answer

A)  1.6 g 
B)  8.1 g 
C)  8.9 g 
D)  54 g 
A)  1.6 g 
B)  8.1 g 
C)  8.9 g 
D)  54 g

Question 12

A student is preparing a sugar-water solution to make rock candy. When the student continues to add sugar to the solution, the sugar dissolves. Which kind of solution is the student preparing?

Accepted Answer

A)  The student is preparing a saturated solution. 
B)  The student is preparing a supersaturated solution. 
C)  The student is preparing an unsaturated solution. 
D)  We cannot tell if the student is preparing a saturated, a supersaturated, or an unsaturated solution. 
A)  The student is preparing a saturated solution. 
B)  The student is preparing a supersaturated solution. 
C)  The student is preparing an unsaturated solution. 
D)  We cannot tell if the student is preparing a saturated, a supersaturated, or an unsaturated solution.

Question 13

Which of the following statements is true?

Accepted Answer

A)  Suspensions are homogeneous. 
B)  Solutions are heterogeneous. 
C)  Colloids are borderline homogeneous. 
D)  Colloids are always transparent. 
A)  Suspensions are homogeneous. 
B)  Solutions are heterogeneous. 
C)  Colloids are borderline homogeneous. 
D)  Colloids are always transparent.

Question 14

A solution contains 1.0 g of solute dissolved in 100 mL of water. Which of the following solutes will cause the solution to have the lowest freezing point?

Accepted Answer

A)  Ribose, C5H10O5, will cause the solution to have the lowest freezing point. 
B)  Glucose, C6H12O6, will cause the solution to have the lowest freezing point. 
C)  Sucrose, C12H22O11, will cause the solution to have the lowest freezing point. 
D)  All of these will cause the solution to have the same freezing point. 
A)  Ribose, C5H10O5, will cause the solution to have the lowest freezing point. 
B)  Glucose, C6H12O6, will cause the solution to have the lowest freezing point. 
C)  Sucrose, C12H22O11, will cause the solution to have the lowest freezing point. 
D)  All of these will cause the solution to have the same freezing point.

Question 15

A solution is prepared by dissolving 215 grams of methanol, CH3OH, in 1000.0 grams of water. What is the freezing point of the solution? (The freezing point depression constant for water is 1.86°C/mole solute in 1000 g of water.)

Accepted Answer

A)  -6.72°C 
B)  -12.5°C 
C)  -25.0°C 
D)  -40.3°C 
A)  -6.72°C 
B)  -12.5°C 
C)  -25.0°C 
D)  -40.3°C

Question 16

Which of the following is a synonym of the term "solution"?

Accepted Answer

A)  compound 
B)  element 
C)  heterogeneous mixture 
D)  homogeneous mixture 
A)  compound 
B)  element 
C)  heterogeneous mixture 
D)  homogeneous mixture

Question 17

Which laboratory equipment is best suited to prepare 100 mL of a 0.2 M solution of sodium chloride?

Accepted Answer

A)  a 50-mL volumetric flask 
B)  a 100-mL volumetric flask 
C)  a 50-mL volumetric pipet 
D)  a 100-mL volumetric pipet 
A)  a 50-mL volumetric flask 
B)  a 100-mL volumetric flask 
C)  a 50-mL volumetric pipet 
D)  a 100-mL volumetric pipet

Question 18

Which ions among Cl-, Na+, NH4+, and NO3- will move toward a cathode?

Accepted Answer

A)  only the chloride ions 
B)  only the sodium ions 
C)  both the chloride and nitrate ions 
D)  both the sodium and ammonium ions 
A)  only the chloride ions 
B)  only the sodium ions 
C)  both the chloride and nitrate ions 
D)  both the sodium and ammonium ions

Question 19

The following photograph shows the laboratory apparatus required for preparing an aqueous solution of the hypothetical compound AB (150.5 g/mol). Which of the following correctly describes the process followed during the preparation of the solution?

Accepted Answer

A)  5.10 g of AB is dissolved in 100.0 mL of water, and the solution is thoroughly mixed. 
B)  5.10 g of AB is dissolved in water, and enough water is added to produce 100.0 mL of solution. 
C)  5.10 g of AB is dissolved in 94.90 mL of water, and the solution is thoroughly mixed. 
D)  5.10 g of AB is dissolved in water, and enough water is added to produce 105.1 mL of solution. 
A)  5.10 g of AB is dissolved in 100.0 mL of water, and the solution is thoroughly mixed. 
B)  5.10 g of AB is dissolved in water, and enough water is added to produce 100.0 mL of solution. 
C)  5.10 g of AB is dissolved in 94.90 mL of water, and the solution is thoroughly mixed. 
D)  5.10 g of AB is dissolved in water, and enough water is added to produce 105.1 mL of solution.

Question 20

Which of the following concentration units will not change if a solution is heated?

Accepted Answer

A)  molarity 
B)  %(w/v) 
C)  both molarity and %(w/v) 
D)  neither molarity or %(w/v) 
A)  molarity 
B)  %(w/v) 
C)  both molarity and %(w/v) 
D)  neither molarity or %(w/v)

Exam 6: Solutions and Colloids

Assuming that the volumes are additive, what volume of water must be added to 35.0 mL of 15.0%(w/v) KOH to make a 10.0%(w/v) solution?

To which of the following does thermal pollution generally refer?

Which of the following is a weak electrolyte?

Which of the following is a description of a hydrated salt?

A typical sample of brass is 67%(w/w) copper and 33%(w/w) zinc. How many moles of zinc are dissolved in 67 grams of copper?

A solution is prepared by dissolving 53.5 grams of ammonium chloride, NH4Cl, in 4000.0 grams of water. What is the freezing point of the solution? (The freezing point depression constant for water is 1.86°C/mole solute in 1000 g of water.)

If we wish to prepare a 0.50 M solution of NaCl, how much of water should we add to 1.0 mole of NaCl?

Which of the following solutions will have the highest electrical conductance?

Which of the following is a weak electrolyte?

A solution of acetic acid is labeled 15%(w/v). How much of water must be added to 30.0 mL of this solution to reduce the concentration to 5.0%(w/v)? (Assume volumes are additive.)

Isotonic saline is 0.89% NaCl (w/v). Suppose you want to prepare 1.0 L of isotonic solution of NH4Cl. What mass of NH4Cl would you need?

A student is preparing a sugar-water solution to make rock candy. When the student continues to add sugar to the solution, the sugar dissolves. Which kind of solution is the student preparing?

Which of the following statements is true?

A solution contains 1.0 g of solute dissolved in 100 mL of water. Which of the following solutes will cause the solution to have the lowest freezing point?

A solution is prepared by dissolving 215 grams of methanol, CH3OH, in 1000.0 grams of water. What is the freezing point of the solution? (The freezing point depression constant for water is 1.86°C/mole solute in 1000 g of water.)

Which of the following is a synonym of the term "solution"?

Which laboratory equipment is best suited to prepare 100 mL of a 0.2 M solution of sodium chloride?

Which ions among Cl-, Na+, NH4+, and NO3- will move toward a cathode?

The following photograph shows the laboratory apparatus required for preparing an aqueous solution of the hypothetical compound AB (150.5 g/mol). Which of the following correctly describes the process followed during the preparation of the solution?

Which of the following concentration units will not change if a solution is heated?

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A solution is prepared by dissolving 53.5 grams of ammonium chloride, NH₄Cl, in 4000.0 grams of water. What is the freezing point of the solution? (The freezing point depression constant for water is 1.86°C/mole solute in 1000 g of water.)

Isotonic saline is 0.89% NaCl (w/v). Suppose you want to prepare 1.0 L of isotonic solution of NH₄Cl. What mass of NH₄Cl would you need?

A solution is prepared by dissolving 215 grams of methanol, CH₃OH, in 1000.0 grams of water. What is the freezing point of the solution? (The freezing point depression constant for water is 1.86°C/mole solute in 1000 g of water.)

Which ions among Cl^-, Na⁺, NH₄⁺, and NO₃^- will move toward a cathode?