Deck 6: Solutions and Colloids

Question 1

When alcohol is dissolved in water which is the solute?

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

Answer 1

D

Question 2

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

A) a gas
B) a liquid
C) a solid
D) None, all can serve as solutes.

Answer 2

D

Question 3

In a solution of a solid in a liquid, the solid is called which of the following?

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

Answer 3

C

Question 4

When a certain clear red-brown liquid passes through a filtering apparatus no material is collected on the filter. What can be said about this 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 5

A chemist has a sample which is known to be a solution. Which of the following might be used to separate the components of the solution?

A) chromatography
B) distillation
C) either a or b
D) neither a nor b

Question 6

Rainwater is naturally slightly acidic. Which gas causes this?

A) N₂
B) O₂
C) CO₂
D) SO₂

Question 7

A chemist has a sample which is known to be a solution. Which of the following might be used to separate the components of the solution?

A) distillation
B) filtration
C) either a or b
D) neither a nor b

Question 8

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 does the student have?

A) a saturated solution
B) a supersaturated solution
C) an unsaturated solution
D) We cannot tell.

Question 9

The term solution is synonymous with which of the following?

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

Question 10

Which of the following is a solution?

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

Question 11

Which of the following is intermediate between homogenous and heterogeneous mixtures?

A) alloys
B) colloidal dispersions
C) plastics
D) polymers

Question 12

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 13

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 14

In a solution of a gas in a liquid, the gas is called which of the following?

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

Question 15

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

A) a gas
B) a liquid
C) a solid
D) None, all can serve as solvents.

Question 16

A chemist has a sample which is known to be a solution. Which of the following might be used to separate the components of the solution?

A) chromatography
B) filtration
C) either a or b
D) neither a nor b

Question 17

The term alloy is applied to which of the following solvent/solute combinations?

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

Question 18

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

A) a saturated solution
B) a supersaturated solution
C) an unsaturated solution
D) We cannot tell.

Question 19

In a solution of a solid in a liquid, the liquid is called which of the following?

A) concentrate
B) dissolver
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 does the student have?

A) a saturated solution
B) a supersaturated solution
C) an unsaturated solution
D) We cannot tell.

Question 21

Appreciable amounts of sugar can be dissolved in which of the following solvents?

A) benzene (C₆H₆)
B) water
C) both a and b
D) neither a nor b

Question 22

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 23

Suppose you prepare a solution by mixing a known volume of ethanol (density = 0.789 g/mL) with a known volume of water (density = 1.00 g/mL). Which of the following can be determined from the information given?

A) %(w/w)
B) %(w/v)
C) Both a and b can be determined.
D) Neither a nor b can be determined.

Question 24

Water is generally a good solvent for which of the following types of compounds?

A) nonpolar compounds
B) polar compounds
C) both a and b
D) neither a nor b

Question 25

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

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 26

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

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

Question 27

Appreciable amounts of solid iodine, I₂, can be dissolved in which of the following solvents?

A) benzene
B) water
C) both a and b
D) neither a nor b

Question 28

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

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

Question 29

Water is likely to be a poor solvent for which types of molecules?

A) molecules which can form hydrogen bonds
B) nonpolar molecules
C) polar molecules
D) None, water is considered a universal solvent.

Question 30

Which of the following gases is associated with the bends?

A) CO₂
B) NO₂
C) N₂
D) O₂

Question 31

Thermal pollution generally refers to which of the following?

A) the decrease in the O₂ content of warm water as compared to cold water
B) the increase in the O₂ content of cold water as compared to warm water
C) both a and b
D) neither a nor b

Question 32

Water is generally a good solvent for which of the following types of compounds?

A) ionic compounds
B) polar compounds
C) both a and b
D) neither a nor b

Question 33

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 34

The term miscible is applied to which of the following solvent/solute combinations?

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

Question 35

A student is preparing a sugar water solution to make rock candy. When the student adds some sugar to the solution a large amount of sugar crystallizes. Which kind of solution does the student have?

A) a saturated solution
B) a supersaturated solution
C) an unsaturated solution
D) We cannot tell.

Question 36

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

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

Question 37

When considering the solubility of a particular solute in a particular solvent the term "like dissolves like" generally refers to which of the following properties?

A) formula weight
B) molecular shape
C) both a and b
D) neither a nor b

Question 38

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

A) concentrated
B) dilute
C) molarity
D) all of these

Question 39

When considering the solubility of a particular solute in a particular solvent the term "like dissolves like" generally refers to which of the following properties?

A) formula weight
B) molecular polarity
C) both a and b
D) neither a nor b

Question 40

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

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

Question 41

A glycine solution is 2.50%(w/w). How much glycine is there in a sample which has a mass of 250. g?

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

Question 42

If we wish to prepare a 0.50 M solution of NaCl, how much water must be added to 1.0 mole of NaCl?

A) 2.0 mol
B) 2.0 L
C) 2.0 × 10³ g
D) Enough water to make 2.0 L of solution.

Question 43

A solution is prepared by dissolving 3.50 grams of NH₄Cl in enough water to make 250. 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 44

Which laboratory equipment is needed to prepare solutions of known %(v/v)?

A) a graduated cylinder
B) a volumetric flask
C) both a and b
D) neither a nor b

Question 45

A solution is prepared by dissolving 4.40 g of KSCN in enough water to make 340. 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 46

Even if we know the solute, molarity and density of a solution, which of the following concentration units cannot be readily determined without any other measurements?

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

Question 47

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 48

If we wish to prepare 250. mL of 0.200 M BaCl₂ solution, how much solid BaCl₂ is needed?

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

Question 49

If a solution is prepared by dissolving 7.7 g of lithium iodide, LiI, in enough water to make 400. mL of solution, what is the %(w/v) of LiI?

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

Question 50

Which laboratory equipment is needed to prepare solutions of known %(w/v)?

A) a balance
B) a volumetric flask
C) both a and b
D) Neither a nor b

Question 51

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

A) molarity
B) %(w/v)
C) both a and b
D) neither a nor b

Question 52

What is the %(w/w) of a salt solution prepared by dissolving 35.0 g of NaCl in 115 g of water?

A) 2.33%
B) 3.04%
C) 23.3%
D) 30.4%

Question 53

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

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

Question 54

Which piece of glassware do we need to accurately measure the total volume of a solution of a specific molarity?

A) a graduated cylinder
B) a volumetric flask
C) a volumetric pipet
D) Any of these would be appropriate.

Question 55

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 56

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

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

Question 57

Saline solutions (NaCl in water) used to deliver intravenous drugs are 0.89%(w/v). What mass of NaCl is found in 500. mL of such a solution?

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

Question 58

Which laboratory equipment is needed to prepare solutions of known %(w/w)?

A) a balance
B) a volumetric flask
C) both a and b
D) neither a nor b

Question 59

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 60

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

A) %(w/w)
B) %(w/v)
C) both a and b
D) neither a nor b

Question 61

A certain wine contains 0.0100 M NaHSO₃ as a preservative. What mass of NaHSO₃ is in a 750 mL bottle of this wine?

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

Question 62

What is the molar mass of CuSO₄·5H₂O?

A) 90.0 g/mol
B) 177.6 g/mol
C) 159.6 g/mol
D) 249.6 g/mol

Question 63

How many moles of solute are contained in 500. mL of 0.50 M KCl?

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

Question 64

Which of the following is associated with gout?

A) anhydrous calcium sulfate
B) anhydrous sodium urate
C) calcium sulfate dihydrate
D) sodium urate monohydrate

Question 65

Which of the following is true of a solid which is hygroscopic?

A) It will gain weight when exposed to a damp environment.
B) It may change its color upon being exposed to a damp environment.
C) both a and b
D) neither a nor b

Question 66

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 solution which is 10.0%(w/v)?

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

Question 67

What volume of 12.0 M HCl must be used to make 300. mL of 0.600 M HCl?

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

Question 68

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 solution which is 3.00 M?

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

Question 69

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 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

The unit 1 ppm is equivalent to which of the following?

A) 1000 ppb
B) 0.0001%
C) both a and b
D) neither a nor b

Question 72

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 73

Which of the following is true of the formula weights of a material which exists in both anhydrous and hydrated forms?

A) They have the same formula weight.
B) The hydrated form always has a lower formula weight.
C) The hydrated form always has a higher formula weight.
D) We cannot make any general statement about the formula weights of the two forms.

Question 74

Which of these properties of water is one which makes it such a good solvent?

A) its boiling point
B) its high specific heat
C) its high surface tension
D) its hydrogen bonding ability

Question 75

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

A) a salt which is insoluble in water
B) a salt which 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 76

Which must we do when preparing a solution of specific molarity?

A) Carefully weigh the solute, carefully weigh the solvent.
B) Carefully weigh the solute, carefully measure the volume of solvent.
C) Carefully weigh the solute, fill the volumetric flask to the mark.
D) None of the above is the correct procedure.

Question 77

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 78

Which of the following is a description of an anhydrous salt?

A) a salt which is insoluble in water
B) a salt which 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 79

Which of the following is true of electrolytes?

A) All electrolytes have mobile ions.
B) All electrolytes contain equal numbers of cations and anions.
C) both a and b
D) neither a nor b

Question 80

The term water of hydration is applied to which to which of the following?

A) water molecules required to dissolve a solid
B) water molecules associated with ions in solution
C) water molecules associated with a salt in the solid state
D) none of the above