Deck 12: Solutions

Question 1

In a solution made by dissolving 50 grams of calcium chloride (CaCl₂)in 1000 grams of water, which component is considered to be the solute?

A)Water is the solute.
B)Both water and calcium chloride are solutes in this example.
C)Calcium chloride is the solute.
D)The solute cannot be determined from the information given.

Answer 1

Calcium chloride is the solute.

Question 2

Which of the following is not a solution?

A)ice in water
B)vinegar in water
C)sugar in water
D)metal alloys

Answer 2

ice in water

Question 3

Which of the following solutions are possible?

A)Both the solvent and solute are liquids.
B)Both the solvent and solute are solids.
C)The solvent is a liquid and the solute is a gas.
D)All of them are possible.

Answer 3

All of them are possible.

Question 4

Which of the following has the lowest hydration energy?

A)sodium chloride
B)magnesium chloride
C)aluminum chloride
D)silicon tetrachloride

Question 5

Henry's law gives the relationship between ________.

A)colligative properties and the freezing point
B)solubility of a gas and concentration
C)solubility of a gas and pressure
D)hydrophobic and hydrophilic solutions

Question 6

In a solution made by dissolving 200 grams of sugar in 1000 grams of water, which component is considered to be the solvent?

A)Water is the solvent.
B)Both water and sugar are solvents in this example.
C)Sugar is the solvent.
D)The solvent cannot be determined from the information given.

Question 7

What is the molarity of 3.68 mL of a solution containing 0.0025 moles of calcium chloride?

A)6.8 × 10^-4 M
B)0.68 M
C)1.5 M
D)6.8 × 10^-3 M

Question 8

Under what conditions would a gas be most soluble in a liquid?

A)high temperature and high pressure
B)high temperature and low pressure
C)low temperature and high pressure
D)low temperature and low pressure

Question 9

Sterling silver is a solution (ALLOY)of ________.

A)silver and zinc
B)silver and gold
C)silver and copper
D)silver and iron

Question 10

The spherical structure of a soap molecule that is formed when in contact with water is called ________.

A)detergent
B)hydrophobic end
C)hydrophilic end
D)micelle

Question 11

Which end, the polar end or the nonpolar end, of a detergent molecule is attracted to water?

A)the polar end
B)both the polar and the nonpolar end
C)neither the polar nor the nonpolar end
D)the nonpolar end

Question 12

In a dilute saline solution the solute is in the form of ________.

A)Na⁺ and Cl^-
B)NaCl (s)
C)NaCl (ℓ)
D)both A and B

Question 13

Which of the following statements is correct?

A)Temperature usually increases the solubility of a solid in water.
B)Pressure usually increases the solubility of a gas in water.
C)Solubility involves the statement "like dissolves like".
D)All of the above statements are correct.

Question 14

The statement "like dissolves like" justifies why ________.

A)water will dissolve ethyl alcohol
B)octane will dissolve methane
C)water will not dissolve fats
D)All of the above statements are correct.

Question 15

Which end, the polar end or the nonpolar end, of a detergent molecule is attracted to dirt particles?

A)the polar end
B)both the polar and the nonpolar end
C)neither the polar nor the nonpolar end
D)the nonpolar end

Question 16

How are solubility and temperature generally related in a system consisting of a solid solute and a liquid solvent?

A)Solubility generally increases with increasing temperature.
B)Solubility generally increases with decreasing temperature.
C)Changing the temperature has no effect on solubility.
D)Solubility generally decreases with increasing temperature.

Question 17

If a solute is to be soluble in a given solvent, which step in the solution-making process must have a negative value for its energy?

A)the physical separation of solvent particles
B)the physical separation of solute particles
C)the formation of solvent/solute interactions
D)All three of the preceding steps must be negative for a solute to be soluble.

Question 18

Which of the following statements is correct?

A)Difference in energy attributed to solvent separation consumes energy.
B)Difference in energy attributed to solute separation consumes energy.
C)Solvation releases energy.
D)All the above statements are correct.

Question 19

Which of the following has the highest hydration energy?

A)sodium chloride
B)magnesium chloride
C)aluminum chloride
D)silicon tetrachloride

Question 20

How are the solubilities of gases (solutes)in liquids (solvents)affected by changing pressure?

A)Gases are more soluble in liquids when pressure is decreased.
B)Pressure has no effect on how soluble a gas is in a liquid.
C)Gases are less soluble in liquids when pressure is increased.
D)Gases are more soluble when the pressure is increased.

Question 21

Which of the following is not a colligative property?

A)molarity
B)freezing point depression
C)vapor pressure lowering
D)boiling point elevation

Question 22

An impurity ________ the boiling point of a compound.

A)decreases
B)increases
C)has no effect on
D)One cannot say unless the physical properties of the compound are known.

Question 23

500 mL 0.4 M aluminum nitrate solution contains ________ moles of aluminum ions and ________ moles of nitrate ions.

A)0.6; 0.2
B)0.2; 0.4
C)0.2; 0.6
D)0.2; 0.2

Question 24

Which of the following is water insoluble?

A)octane, C₈H₁₈
B)ethanol, C₂H₅OH
C)sodium sulfate, Na₂SO₄
D)acetic acid, the active ingredient in vinegar, CH₃COOH

Question 25

25 mL 0.1 M NaCl contains ________ g NaCl.

A)0.0025
B)0.15
C)2.5
D)0.25

Question 26

What is the freezing point of a sugar solution prepared by dissolving 375.00 g of sucrose (342.3 g/mol)in 1500.0 g of water (K_f of water = 1.86 °C)?

A)1.36 °C
B)-1.36 °C
C)-1.86 °C
D)-0.465 °C

Question 27

500 mL 0.4 M potassium dichromate contains ________ moles of potassium ions and ________ moles of dichromate ions.

A)0.4; 0.2
B)0.2; 0.4
C)0.4; 0.6
D)0.2; 0.2

Question 28

The molarity of a solution that contains 5.85 g NaCl in 2.0 L solution is ________.

A)2.93 M
B)0.05 M
C)5.0 M
D)0.29 M

Question 29

How many grams of water are in 100 g of a 30 mass % sugar solution?

A)30
B)60
C)70
D)100

Question 30

Phenolphthalein turns ________ when the solution is basic.

A)clear
B)blue
C)pink
D)orange

Question 31

To prepare 100 mL 0.4 M HCl from a stock solution of 2 M HCl one needs to ________.

A)dilute 20 mL 2 M HCl with 100 mL HCl
B)dilute 20 mL 2 M HCl with enough water to make a total volume of 100 mL solution
C)use 500 mL 2 M HCl and boil it down to a final volume of 100 mL solution
D)dilute 80 mL 2 M HCl to a total volume of 100 mL solution

Question 32

A 0.2119 g sample of an acid, HA, was neutralized by 34.7 mL 0.0500 M NaOH solution. The molecular mass of the acid is ________.

A)61
B)92
C)122
D)244

Question 33

An impurity ________ the melting point of a compound.

A)decreases
B)increases
C)has no effect on
D)One cannot say unless the physical properties of the compound are known.

Question 34

200. mL 0.100 M NaCl contains ________ g NaCl.

A)1.17
B)11.7
C)117
D)5.85

Question 35

Which of the following is water soluble?

A)CCl₄
B)C₂H₅OH
C)C₈H₁₈
D)CH₃CH₂OCH₂CH₃

Question 36

How many grams of NaCl are in 200 g of a 10 mass % salt solution?

A)10
B)20
C)40
D)80

Question 37

4.173 g of an organic compound (non-electrolyte)lowered the freezing point of 100.0 g nitrobenzene by 2.6 °C. If the K_f of nitrobenzene is 8.1 °C, the molecular mass of the non-electrolyte is ________.

A)260
B)195
C)65
D)130

Question 38

A 2.154 g sample of an unknown non-electrolyte is dissolved in 50 g of water (K_f of water = 1.86 °C). If the solution freezes at -1.23 °C, the molecular mass of the non-electrolyte is ________.

A)33
B)65
C)130
D)260

Question 39

500 mL 0.4 M calcium nitrite contains ________ moles of calcium ions and ________ moles of nitrite ions.

A)0.4; 0.2
B)0.2; 0.4
C)0.4; 0.6
D)0.2; 0.2

Question 40

7.5 g calcium carbonate in a 150 mL aqueous solution will provide a ________ M solution.

A)0.10
B)0.50
C)1.0
D)2.0

Question 41

The solute in a sugar solution is water.

Question 42

C₈H₁₈ will dissolve in CCl₄.

Question 43

Amalgams are solid solutions.

Question 44

Air is a gas solution where oxygen is the solvent.

Question 45

Dry cleaning uses perchloroethane to remove grease and oil from clothes.

Question 46

NH₃ will dissolve in BF₃.

Question 47

Nonpolar solutes will usually dissolve in polar solvents.

Question 48

Polar solutes will usually dissolve in polar solvents.

Question 49

A mixture is not necessarily a solution.

Question 50

Ca²⁺ is expected to have a greater energy of hydration than K⁺.

Question 51

10.0 mL 0.5 M sulfuric acid neutralizes ________ mL 0.5 M ammonium hydroxide.

A)5.0
B)10.
C)20.
D)40.

Question 52

A 2.00 g sample of a non-electrolyte (molar mass = 118)is dissolved in 55.0 g benzene (K_f of benzene is What is the freezing point depression of the solution?

A)1.58 °C
B)3.16 °C
C)0.79 °C
D)2.33 °C

Question 53

There is no difference between the "molarity" and the "percent composition" of a given solution.

Question 54

Transparent solutions are examples of homogeneous matter.

Question 55

10.0 mL 0.5 M HCl neutralizes ________ mL 0.5 M NaOH.

A)5.0
B)10.
C)20.
D)40.

Question 56

10.0 mL 0.5 M sulfuric acid neutralizes ________ mL 0.5 M magnesium hydroxide.

A)5.0
B)10.
C)20.
D)40.

Question 57

Vinegar is a liquid solution where acetic acid serves as the solvent.

Question 58

It is not possible to make a solution in which both the solute and the solvent are gases.

Question 59

Situations of great disorder are said to have "high entropies."

Question 60

The solvent in a saline solution is water.

Question 61

100 mL of 1.0 M KOH will neutralize 100 mL of 1.0 M H₂SO₄ solution.

Question 62

The process of surrounding solute ions with solvent molecules is called solvation.

Question 63

What are two physical properties of water that make it an especially useful and common solvent?

Question 64

The bends, a condition encountered by divers, is attributed to the rapid depressurized escape of nitrogen from blood.

Question 65

A 20 mass % NaOH solution is made by dissolving 5 g NaOH in 25 g water.

Question 66

A 1 mass % saline solution contains 1 g of NaCl plus 99 g of water.

Question 67

If a liquid is volatile it evaporates readily.

Question 68

Alloys are solid solutions.

Question 69

How does the phrase "like dissolves like" help to explain why a solute like sodium chloride (NaCl)and a solvent like water should form a solution?

Question 70

A hydrophobic group will be attracted to water.

Question 71

Starting with 100 mL of water, if you then add 30 grams of sodium chloride (NaCl)to the water, will the volume of the solution you make be less than/exactly/greater than 100 mL?

Question 72

Once the temperature of 100.°C is reached, liquid water spontaneously becomes
a gas.

Question 73

Use the general rule "like dissolves like" to briefly explain why vegetable oil (nonpolar)will not dissolve in water (polar).

Question 74

For most molecular solids an increase in temperature generally causes an increase in solubility.

Question 75

A saline solution will boil at 100 °C.

Question 76

The addition of NaCl to water will decrease the freezing point.

Question 77

Molarity is defined as moles of solute per liter of solvent.

Question 78

25 mL of 0.2 M NaOH will neutralize 10 mL 0.5 M HCl solution.

Question 79

What are the three ways a given solution's "percent composition" can be described?

Question 80

Hydrocarbons, such as pentane C₅H₁₂, are water soluble.