Deck 6: Solutions and Colloids

Question 1

Which of the following is a solution?

A) blood plasma
B) cigarette smoke
C) milk
D) none of these

Answer 1

D

Question 2

Rainwater is naturally slightly acidic. Which gas causes this?

A) N₂
B) O₂
C) CO₂
D) NH₃

Answer 2

C

Question 3

Which term is used to refer to the liquid component of a solid-in-liquid solution?

A) concentrate
B) dissolver
C) solute
D) solvent

Answer 3

D

Question 4

A student is preparing a sugar-water solution to make rock candy. When the student continues to add sugar to the solution, no additional sugar dissolves. Which kind of solution is the student preparing?

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 5

Which of the following terms is used to refer to a gas dissolved in a liquid?

A) concentrate
B) precipitate
C) solute
D) solvent

Question 6

Which of the following combinations will always result in a solution?

A) gas + gas
B) liquid + liquid
C) solid + solid
D) none of these

Question 7

Which of the following cannot serve as a solvent in a solution?

A) a gas
B) a liquid
C) a solid
D) none of these

Question 8

Which of the following cannot serve as a solute in a solution?

A) a gas
B) a liquid
C) a solid
D) none of these

Question 9

A chemist has a sample that is known to be a solution. Which of the following processes can be used to separate the components of the solution?

A) chromatography
B) distillation
C) either chromatography or distillation
D) neither chromatography or distillation

Question 10

What is the solute when alcohol is dissolved in water?

A) the alcohol
B) the water
C) the compound present in a larger amount
D) the compound present in a smaller amount

Question 11

When a certain clear red-brown liquid is distilled, we recover a clear liquid and a red-brown solid. What can be said about the red-brown liquid?

A) It is an element.
B) It is a compound.
C) It is a solution.
D) We cannot determine if it is an element, a compound, or a solution.

Question 12

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

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

Question 13

A chemist has a sample that is known to be a solution. Which of the following processes can be used to separate the components of the solution?

A) chromatography
B) filtration
C) either chromatography or filtration
D) neither chromatography or filtration

Question 14

A chemist has a sample that is known to be a solution. Which of the following processes can be used to separate the components of the solution?

A) distillation
B) filtration
C) distillation and filtration
D) neither distillation or filtration

Question 15

A beaker of salt water contains some solid salt at the bottom. What type of solution is in the beaker?

A) It is a saturated solution.
B) It is a supersaturated solution.
C) It is an unsaturated solution.
D) We cannot tell if it is a saturated, a supersaturated, or an unsaturated solution.

Question 16

Which of the following is true of a solution?

A) The components of a solution can be separated by filtration.
B) The components of a solution separate on standing.
C) The separation of a solution into its components is a chemical change.
D) The separation of a solution into its components is a physical change.

Question 17

Which of the following are intermediates between homogenous and heterogeneous mixtures?

A) alloys
B) suspensions
C) plastics
D) solutions

Question 18

To which of the following solvent-solute combinations does the term "alloy" apply?

A) liquid-solid
B) liquid-liquid
C) solid-solid
D) none of these

Question 19

Which term is used to refer to the solid component of a solid-in-liquid solution?

A) concentrate
B) precipitate
C) solute
D) solvent

Question 20

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?

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 21

To which of the following solvent-solute combinations does the term "miscible" apply?

A) liquid-gas
B) liquid-liquid
C) liquid-solid
D) none of these

Question 22

For which of the following types of molecules is water likely to be a poor solvent?

A) molecules that can form hydrogen bonds with water
B) nonpolar molecules
C) polar molecules
D) none of these

Question 23

Which of the following is soluble in water?

A) benzene
B) gasoline
C) sodium chloride
D) carbon tetrachloride

Question 24

For which of the following types of compounds is water generally a good solvent?

A) nonpolar compounds
B) polar compounds
C) both nonpolar and polar compounds
D) neither nonpolar or polar compounds

Question 25

Which of the following solvents can dissolve appreciable amounts of sugar?

A) benzene (C₆H₆)
B) water
C) both benzene (C₆H₆) and water
D) neither benzene (C₆H₆)

Question 26

For which of the following types of compounds is water generally a good solvent?

A) ionic compounds
B) polar compounds
C) both ionic and polar compounds
D) neither ionic or polar compounds

Question 27

Which of the following properties does the expression "like dissolves like" generally refer to when considering the solubility of a solute in a solvent?

A) formula weight
B) molecular shape
C) both formula weight and molecular shape
D) neither formula weight or molecular shape

Question 28

Which of the following is true regarding the solubility of liquids and solids in solutions?

A) Solubility always decreases as temperature increases.
B) Solubility always increases as temperature increases.
C) Solubility usually decreases as temperature increases.
D) Solubility usually increases as temperature increases.

Question 29

Which of the following properties does the expression "like dissolves like" generally refer to when considering the solubility of a solute in a solvent?

A) formula weight
B) molecular polarity
C) both formula weight and molecular polarity
D) neither formula weight or molecular polarity

Question 30

Which of the following terms can be used to quantitatively describe the concentration of a solution?

A) parts per million
B) percent concentration
C) molarity
D) all of these

Question 31

A salt water solution is 3.0%(w/w). How much of salt is there in a sample that weighs 250 g?

A) 1.2 g
B) 1.5 g
C) 3.0 g
D) 7.5 g

Question 32

Which of the following gases is associated with the bends?

A) CO₂
B) NO₂
C) N₂
D) O₂

Question 33

500 mL of salt water is prepared by dissolving 20 g of salt in water. What is the %(w/v) of this solution?

A) 0.04%
B) 0.4%
C) 4.0%
D) 40.0%

Question 34

Which of the following laws describes the relationship between pressure and the solubility of gases in liquids?

A) Avogadro's law
B) Boyle's law
C) Dalton's law
D) Henry's law

Question 35

Which of the following pairs of liquids is miscible in all proportions?

A) ethanol and water
B) ethanol and oil
C) gasoline and water
D) none of these

Question 36

What is the solubility of table salt in water at 30°C?

A) 16.2 g per 100.0 g of water
B) 26.2 g per 100.0 g of water
C) 36.2 g per 100.0 g of water
D) 46.2 g per 100.0 g of water

Question 37

Which statement is true of the solubility of a gas in a liquid?

A) The solubility of the gas in the liquid always decreases as pressure increases.
B) The solubility of the gas in the liquid always increases as pressure increases.
C) The solubility of the gas in the liquid usually decreases as pressure increases.
D) The solubility of the gas in the liquid usually increases as pressure increases.

Question 38

To which of the following does thermal pollution generally refer?

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 39

Which of the following is true regarding the solubility of gases in liquids?

A) Solubility decreases as temperature increases.
B) Solubility increases as temperature increases.
C) Solubility is unaffected by changes in temperature.

Question 40

Which of the following is true regarding the solubility of liquids and solids?

A) Pressure has virtually no effect on the solubility of liquids or solids.
B) Solubility always decreases as pressure decreases.
C) Solubility always increases as pressure decreases.
D) Solubility usually decreases as pressure decreases.

Question 41

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

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

Question 42

Which of the following does not change in a solution post dilution?

A) the number of moles of solvent
B) the number of moles of solute
C) the volume of the solution
D) the molarity of the solution

Question 43

What is the mass of salt in a 400-gram sample of salt water that is 1.50%(w/w)?

A) 1.50 g
B) 2.67 g
C) 3.00 g
D) 6.00 g

Question 44

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

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

Question 45

Saline solutions (NaCl in water) used to deliver intravenous drugs are 0.89%(w/v). What mass of NaCl is found in 500.0 mL of such a solution?

A) 0.45 g
B) 0.89 g
C) 4.5 g
D) 8.9 g

Question 46

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

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 47

A solution is prepared by dissolving 7.7 g of lithium iodide, LiI, in enough water to make 400.0 mL of solution. What is the %(w/v) of LiI?

A) 0.96%
B) 1.9%
C) 3.9%
D) 7.7%

Question 48

For which of the following types of solutions is the concentration unit %(v/v) used?

A) solid in solid
B) liquid in liquid
C) solid in liquid
D) gas in gas

Question 49

Which of the following is the definition of molarity?

A) moles of solute/1000 grams of solvent
B) moles of solute/liter of solution
C) moles of solute/liter of solvent
D) moles of solvent/1000 grams of solute

Question 50

What happens to a solution post dilution?

A) The number of moles of solute increases.
B) The number of moles of solute decreases.
C) The number of moles of solvent increases.
D) The number of moles of solvent decreases.

Question 51

What is the mass of glycine in a 400-g sample of a solution that is 2.5%(w/w)?

A) 1.0 g
B) 2.5 g
C) 10.0 g
D) 25.0 g

Question 52

If we know the solute mass and the molarity of a solution, which other concentration unit can we readily determine without needing any other measurement?

A) (w/w)%
B) (w/v)%
C) (v/v)%
D) all of these

Question 53

What is the %(w/w) of a salt solution prepared by dissolving 7.5 g of salt in 242.5 g of water?

A) 0.030%
B) 0.30%
C) 0.75%
D) 3.0%

Question 54

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

Question 55

A bottle of vodka is labeled as 60 proof. What is its alcohol content in terms of (v/v)%?

A) 7.5%
B) 15%
C) 30.0%
D) 60.0%

Question 56

The label on a 750-mL bottle of wine states that its alcohol content is 12%(v/v). What volume of alcohol is present in the bottle?

A) 9.0 mL
B) 90.0 mL
C) 120 mL
D) 180 mL

Question 57

400 g of salt solution is prepared by dissolving 30 g of salt in water. What is the %(w/w) of this solution?

A) 0.075%
B) 7.5%
C) 0.069%
D) 6.9%

Question 58

A 750-mL bottle of vodka is labeled as 60 proof. What is its alcohol content?

A) 113.0 mL
B) 225.0 mL
C) 450.0 mL
D) 600.0 mL

Question 59

Which of the following concentration units can be used when only the masses of the solute and the solution are known?

A) %(w/w)
B) %(w/v)
C) %(v/v)
D) M

Question 60

A glycine solution is 2.50%(w/w). How much of glycine is there in a sample that has a mass of 250.0 g?

A) 1.25 g
B) 5.00 g
C) 6.25 g
D) 12.5 g

Question 61

What is the mass of BaCl₂ in a 0.250-L bottle of 0.200 M BaCl₂?

A) 5.21 g
B) 10.4 g
C) 41.7 g
D) 52.1 g

Question 62

A particular wine contains 0.0100 M NaHSO₃ as a preservative. What is the mass of NaHSO₃ in a 750-mL bottle of the wine?

A) 0.39 g
B) 0.70 g
C) 0.78 g
D) 1.5 g

Question 63

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?

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

Question 64

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.)

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

Question 65

The concentration of lead in a water sample is found to be 3 ppb. To which of the following is this equivalent?

A) 0.003 mg lead per 1 kg of water
B) 0.03 mg lead per 1 kg of water
C) 0.3 mg lead per 1 kg of water
D) 3.0 mg lead per 1 kg of water

Question 66

Which of the following is the equivalent of 13 mg of arsenic in 1 kg of drinking water?

A) 0.13 ppm arsenic
B) 1.3 ppm arsenic
C) 13.0 ppm arsenic
D) 130.0 ppm arsenic

Question 67

What volume of 12.0 M HCl must be used to make 300.0 mL of 0.600 M HCl?

A) 1.50 mL
B) 2.40 mL
C) 15.0 mL
D) 24.0 mL

Question 68

A solution of iodine in carbon tetrachloride is 0.100 M. How much of carbon tetrachloride must be added to 50.0 mL of this solution to reduce the concentration to 0.0250 M? (Assume volumes are additive.)

A) 50.0 mL
B) 100.0 mL
C) 150.0 mL
D) 200.0 mL

Question 69

Assuming that the volumes are additive, what volume of water must be added to 35.0 mL of 12.0 M HCl to make a 3.00 M solution?

A) 70.0 mL
B) 87.5 mL
C) 105 mL
D) 140 mL

Question 70

What is the mass of NaCl in a 0.500-L bottle of 2.00 M NaCl?

A) 29.3 g
B) 58.5 g
C) 117 g
D) 234 g

Question 71

A stockroom attendant has a 15.0%(w/v) solution of KOH. What volume of this solution should she use if she needs to prepare 20.0 mL of a 10.0%(w/v) solution?

A) 6.67 mL
B) 7.50 mL
C) 13.3 mL
D) 15.0 mL

Question 72

A saline solution is 5.00%(w/v). How much of water must be added to 50.0 mL of this solution to reduce the concentration of the solution to 1.0%(w/v)? (Assume volumes are additive.)

A) 50.0 mL
B) 100.0 mL
C) 200.0 mL
D) 250.0 mL

Question 73

A typical sample of brass is 67%(w/w) copper and 33%(w/w) zinc and has a density of 8.40 g/mL. What is the molarity of this solution?

A) 33 M
B) 42 M
C) 88 M
D) 67 M

Question 74

Which of the following is a colligative property?

A) molarity
B) percent concentration
C) parts per million
D) osmotic pressure

Question 75

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?

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 76

A solution has a concentration of 15 ppm. Which of the following is another way to describe the concentration of this solution?

A) 0.015 ppb
B) 0.15 ppb
C) 1500 ppb
D) 15000 ppb

Question 77

A solution is prepared by dissolving 3.50 grams of NH₄Cl in enough water to make 250.0 mL of solution. What is the concentration of this solution?

A) 0.0327 M
B) 0.0654 M
C) 0.131 M
D) 0.262 M

Question 78

A solution is prepared by dissolving 4.40 g of KSCN in enough water to make 340.0 mL of solution. What is the concentration of the solution?

A) 0.0440 M
B) 0.0543 M
C) 0.119 M
D) 0.133 M

Question 79

If we wish to prepare 250.0 mL of 0.200 M BaCl₂ solution, how much of solid BaCl₂ is needed?

A) 4.17 g
B) 5.21 g
C) 10.4 g
D) 20.8 g

Question 80

How many moles of solute are contained in 500.0 mL of 0.50 M KCl?

A) 0.25
B) 0.50
C) 1.0
D) 2.0