Deck 12: Solutions

Question 1

Which of the following statements is correct?

A) Energy is needed to overcome the solute-solute attractive forces.
B) Energy is needed to overcome the solvent-solvent attractive forces.
C) Solvation releases energy.
D) All the above statements are correct.

Answer 1

All the above statements are correct.

Question 2

Solutions are considered to be which general type of matter?

A) homogeneous mixtures
B) heterogeneous mixtures
C) pure substances
D) pure elements

Answer 2

homogeneous mixtures

Question 3

Which of the following is not a solution?

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

Answer 3

ice in water

Question 4

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

A) Gases are more soluble in liquids when the 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 the pressure is increased.
D) Gases are more soluble in liquids when the pressure is increased.

Question 5

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 6

Which of the following is a solution?

A) air
B) amalgam
C) metal alloys
D) All of the above are solutions.

Question 7

Which of the following has the lowest hydration energy?

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

Question 8

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.

Question 9

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 10

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 11

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 12

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 13

Sterling silver is a solution (ALLOY) of ________.

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

Question 14

Which of the following examples demonstrates a net decrease in entropy?

A) melting an ice cube
B) adding cream to hot coffee
C) ripping a finished jigsaw puzzle into a thousand pieces
D) assembling a 1000-piece jigsaw puzzle
E) All of the preceding are examples of net increases in entropy.

Question 15

Which of the following has the highest hydration energy?

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

Question 16

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 17

The solute in a saline solution is ________.

A) water
B) salt
C) the salt solution
D) One cannot say unless the exact concentration is known.

Question 18

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 19

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.

Question 20

Which of the following is the least water soluble at 50°C?

A) Ce₂(SO₄)3
B) KBr
C) NaNO₃
D) CH₃COONa

Question 21

200. mL of a 0.100 M NaCl solution contains ________ g of NaCl.

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

Question 22

25 mL of a 0.1 M NaCl solution contains ________ g of NaCl.

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

Question 23

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

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

Question 24

10.0 mL of 0.50 M hydrochloric acid neutralizes ________ mL of 0.50 M magnesium hydroxide solution.

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

Question 25

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 26

500 mL of a 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 27

Soap consists of a long ________ head and a long ________ tail.

A) polar; polar
B) polar; nonpolar
C) nonpolar; polar
D) nonpolar; nonpolar

Question 28

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 29

Which of the following is the most water soluble at 50°C?

A) CH₃COONa
B) NaNO₃
C) Ce₂(SO₄)3
D) KBr

Question 30

10.0 mL of 0.50 M sulfuric acid neutralizes ________ mL of 0.50 M ammonium hydroxide solution.

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

Question 31

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 32

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 33

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

A) 2.93 M
B) 0.050 M
C) 5.0 M
D) 0.29 M

Question 34

500 mL of a 0.4 M sodium nitrate contains ________ moles of sodium ions and ________ moles of nitrate ions.

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

Question 35

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

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

Question 36

10.0 mL of 0.50 M HCl solution neutralizes ________ mL of 0.50 M NaOH solution.

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

Question 37

To prepare 500. mL of 0.5 M NaCl from a stock of 2.0 M NaCl one needs to ________.

A) dilute 125 mL 2.0 M NaCl with enough water to a total of 500. mL solution
B) dilute 125 mL 2.0 M NaCl with 500. mL water
C) dilute 375 mL 2.0 M NaCl with enough water to a total of 500. mL solution
D) dilute 375 mL 2.0 M NaCl with 500. mL water

Question 38

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

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

Question 39

10.0 mL of 0.50 M sulfuric acid neutralizes ________ mL of 0.50 M magnesium hydroxide solution.

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

Question 40

500 mL of a 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 41

A solid solution is a solution of two metals that are not necessarily evenly distributed in each other.

Question 42

A 2.00 g sample of a non-electrolyte (molar mass = 118) is dissolved in 55.0 g of benzene (Kf 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 43

Transparent solutions are examples of homogeneous matter.

Question 44

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 45

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

Question 46

If the empirical formula is C₄H₃N and the molecular weight is 130 g/mole, then the molecular formula is ________.

A) C₁₆H₁₂N₄
B) C₁₂H₉N₃
C) C₄H₃N
D) C₈H₆N₂

Question 47

Phenolphthalein turns ________ when the solution is basic.

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

Question 48

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 49

4.173 g of an organic compound (non-electrolyte) lowered the freezing point of 100.0 g of nitrobenzene by 2.6 °C. If the Kf of nitrobenzene is 8.1 °C∙ kg solvent/mol solute, the molecular mass of the non-electrolyte is ________.

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

Question 50

Which of the following is not a colligative property?

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

Question 51

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

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

Question 52

How many grams of NaCl are in 200 g of a 10 percent-by-mass salt solution?

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

Question 53

Alloys are solid solutions.

Question 54

The solvent in a saline solution is water.

Question 55

The percent composition of a solution made by dissolving 5.0 g NaOH in 20. g of water is ________.

A) 4.0%
B) 5.0%
C) 20.%
D) 25%

Question 56

A 2.154 g sample of an unknown non-electrolyte is dissolved in 50. g of water (Kf of water = 1.86 °C∙ kg solvent/mol solute). 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 57

The solute in a sugar solution is water.

Question 58

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 59

How many grams of water are in 100 g of a 30 percent-by-mass sugar solution?

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

Question 60

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

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

Question 61

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

Question 62

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

Question 63

A mixture of sand, sodium carbonate, and calcium oxide is a homogeneous solution.

Question 64

If a liquid is volatile it evaporates readily.

Question 65

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

Question 66

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

Question 67

Air is a gas solution where oxygen is the solvent.

Question 68

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

Question 69

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

Question 70

A hydrophobic group will be attracted to water.

Question 71

Nonpolar solutes will usually dissolve in polar solvents.

Question 72

C₈H₁₈ will dissolve in CCl4.

Question 73

NH₃ will dissolve in BF3.

Question 74

A mixture is not necessarily a solution.

Question 75

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

Question 76

Polar solutes will usually dissolve in polar solvents.

Question 77

A solution prepared by dissolving 24 g potassium sulfate in 150 mL total solution has a molarity of 0.92 M.

Question 78

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

Question 79

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

Question 80

Hydrocarbons, such as pentane C₅H₁₂, are water soluble.