Deck 13: Physical Properties of Solutions

Question 1

Which is defined as the maximum amount of solute that will dissolve in a given quantity of solvent at a specific temperature?

A) precipitation
B) combustion
C) solubility
D) super saturation
E) dilution

Answer 1

solubility

Question 2

Which accurately characterizes all nonelectrolyte solutions?

A) Nonelectrolyte solutions contain molecules.
B) Nonelectrolyte solutions conduct electricity.
C) Nonelectrolyte solutions react with other solutions.
D) Nonelectrolyte solutions do not conduct electricity.
E) Nonelectrolyte solutions conduct heat.

Answer 2

Nonelectrolyte solutions do not conduct electricity.

Question 3

Which process defines how an ionic compound breaks apart into its constituent ions upon dissolution?

A) electrolysis
B) dissociation
C) division
D) ionization
E) decomposition

Answer 3

dissociation

Question 4

Which substance is present in the largest proportion in a solution?

A) salute
B) gas
C) solvent
D) solid
E) solute

Question 5

What is the name given to a solution that contains less solute than it has the capacity to dissolve?

A) Unsaturated
B) Saturated
C) Solvented
D) Oversaturated
E) Supersaturated

Question 6

Which of these compounds is a nonelectrolyte?

A) NaOH
B) HNO₃
C) C₂H₆O (ethanol)
D) KF
E) CH₃COOH (acetic acid)

Question 7

Which of these compounds is a weak electrolyte?

A) HCl
B) CH₃COOH (acetic acid)
C) C₆H₁₂O₆ (glucose)
D) O₂
E) NaCl

Question 8

Which of these compounds is a nonelectrolyte?

A) NaF
B) HNO₃
C) CH₃COOH (acetic acid)
D) NaOH
E) C₆H₁₂O₆ (glucose)

Question 9

Which of these compounds is a strong electrolyte?

A) H₂O
B) N₂
C) CH₃COOH (acetic acid)
D) C₂H₆O (ethanol)
E) KOH

Question 10

What is the name given to a solution that contains the maximum amount of solute that will dissolve in a solvent at a specific temperature?

A) Saturated
B) Unsaturated
C) Solvent
D) Solute
E) Supersaturated

Question 11

The distinguishing characteristic of all nonelectrolyte solutions is that they

A) contain ions.
B) do not conduct electricity.
C) react with other solutions.
D) always contain acids.
E) conducts heat.

Question 12

The distinguishing characteristic of all electrolyte solutions is that they

A) contain molecules.
B) conduct electricity.
C) react with other solutions.
D) always contain acids.
E) conduct heat.

Question 13

Which is the correct description of a solution?

A) A solution is a heterogeneous mixture of two or more substances.
B) A solution is a homogeneous mixture of two or more substances.
C) A solution may be a gas, solid, or liquid.
D) A solution is any mixture of two or more substances.

Question 14

Which process defines how molecular compounds form ions upon dissolution?

A) ionization
B) composition
C) division
D) dissolution
E) decomposition

Question 15

What name is given to the major component in a solution?

A) Supersaturated
B) Solute
C) Saturated
D) Unsaturated
E) Solvent

Question 16

Which of these compounds is a weak electrolyte?

A) HCl
B) NH₃
C) C₆H₁₂O₆ (glucose)
D) N₂
E) KCl

Question 17

Which of these compounds is a strong electrolyte?

A) H₂O
B) O₂
C) H₂SO₄
D) C₆H₁₂O₆ (glucose)
E) CH₃COOH (acetic acid)

Question 18

Which one of the following substances is the strongest electrolyte?

A) CO
B) CH₃Cl
C) CH₄
D) C₂H₅OH
E) HCl

Question 19

What name is given to a minor component in a solution?

A) Solvent
B) Unsaturated
C) Saturated
D) Solute
E) Supersaturated

Question 20

Which substance is present in the smallest proportion in a solution?

A) liquid
B) gas
C) solvent
D) solid
E) solute

Question 21

Which is most soluble in CCl₄?

A) NaCl
B) H₂O
C) NaOH
D) C₈H₁₈
E) CH₃OH

Question 22

Which of the following is not soluble in water?

A) Vitamin C
B) NaCl
C) CH₃CH₂OH
D) NH₃
E) Vitamin E

Question 23

What is the percent CsCl by mass in a 0.711 M aqueous CsCl solution that has a density of 1.091 g/mL?

A) 1.53%
B) 3.87 × 10^-1%
C) 11.0%
D) 12.0%
E) 65.2%

Question 24

Which compound is the most soluble in water?

A) CH₃CH₂CH₂CH₂CH₂OH
B) CH₃CH₂CH₂CH₂OH
C) CH₃CH₂CH₂CH₂CH₂CH₂CH₂OH
D) CH₃CH₂CH₂OH
E) All of these compounds are equally soluble in water.

Question 25

If a solute dissolves in an endothermic process

A) hydrogen bonds must exist between solvent and solute.
B) strong ion-dipole forces must exist in the solution.
C) the solute must be a gas.
D) the entropy of the solution is immaterial.
E) the entropy of the solution must be greater than that of its pure components.

Question 26

Which of the following sets of conditions could exist when two liquids which are completely miscible in one another are mixed?

A) ΔH_soln > 0, entropy of system decreases
B) ΔH_soln ≈ 0, entropy of system decreases
C) ΔH_soln ≈ 0, entropy change of system ≈ 0
D) ΔH_soln ≈ 0, entropy of system increases
E) None of these choices is correct.

Question 27

The structure of Vitamin B1, thiamine, is shown here. Vitamin B1 is most soluble in ________.

A) fats
B) water
C) air
D) carbon tetrachloride
E) octane

Question 28

Which is true regarding the solvation of a solute in a solvent?

A) Separation of solute molecules from one another is an endothermic process, and separation of solvent molecules from one another is an exothermic process.
B) Separation of solute molecules from one another is an exothermic process, and separation of solvent molecules from one another is an endothermic process.
C) Separation of solute molecules from one another, and separation of solvent molecules from one another, are both endothermic processes.
D) Separation of solute molecules from one another, and separation of solvent molecules from one another, are both exothermic processes.
E) Separation of solute molecules from one another, and separation of solvent molecules from one another, both result in a decrease in entropy.

Question 29

What is the name given to a solution that contains more solute than it has the capacity to dissolve?

A) Unsaturated
B) Saturated
C) Soluted
D) Supersaturated
E) Oversaturated

Question 30

A solution of potassium hydroxide is in equilibrium with undissolved solute at 45°C. What will happen if the temperature is raised to 50°C? (ΔH_soln = -57.6 kJ/mol)

A) The mass of undissolved KOH will increase.
B) The mass of undissolved KOH will decrease.
C) The mass of undissolved KOH will be unchanged.
D) The mass of water in the solution will increase.
E) The entropy of the system will decrease.

Question 31

Which response lists all the following pairs that are miscible liquids? I. octane (C₈H₁₈) and water
II) acetic acid (CH₃COOH) and water
III) octane (C₈H₁₈) and carbon tetrachloride (CCl₄)

A) I and III
B) I and II
C) III only
D) II only
E) II and III

Question 32

What term describes the process when two liquids are completely soluble in each other in all proportions?

A) Solvation
B) Miscible
C) Unsaturated
D) Saturated
E) Oversaturated

Question 33

What is the molarity of a solution that is 26.0% by mass phosphoric acid (H₃PO₄) and that has a density of 1.155 g/mL?

A) 2.30 × 10 ^-3 M
B) 2.30 M
C) 2.65 M
D) 3.06 M
E) 0.265 M

Question 34

When two pure substances are mixed to form a solution

A) heat is released.
B) heat is absorbed.
C) there is an increase in entropy.
D) there is a decrease in entropy.
E) entropy is conserved.

Question 35

Calculate the percent by mass of potassium nitrate in a solution made from 45.0 g KNO₃ and 295 mL of water at 25ºC. At this temperature, the density of water is 0.997 g/mL.

A) 1.51%
B) 7.57%
C) 13.3%
D) 15.2%
E) 86.7%

Question 36

What is the name given to the process when solvent molecules surround the solute molecules?

A) Unsaturated
B) Solution
C) Oversaturated
D) Saturated
E) Solvation

Question 37

Which is immiscible with water?

A)
B)
C)
D)
E)

Question 38

The mixing of solvent molecules and solute molecules is usually described as

A) the separation energy.
B) the heat of solvation.
C) an endothermic process.
D) an exothermic process.
E) the heat of solution.

Question 39

Potassium fluoride is used for frosting glass. Calculate the molarity of a solution prepared by dissolving 78.6 g of KF in enough water to produce 225 mL of solution.

A) 0.304 M
B) 0.349 M
C) 1.35 M
D) 3.29 M
E) 6.01 M

Question 40

What is the percent CdSO₄ by mass in a 1.00 molal aqueous CdSO₄ solution?

A) 0.001%
B) 0.10%
C) 17.2%
D) 20.8%
E) 24.4%

Question 41

What mass of LiOH is required to prepare 0.250 L of a 3.55 M solution?

A) 0.0371 g
B) 0.888 g
C) 21.3 g
D) 250. g
E) 340. g

Question 42

What volume of concentrated (14.7 M) phosphoric acid is needed to prepare 25.0 L of 3.0 M H₃PO₄?

A) 0.20 L
B) 0.57 L
C) 1.8 L
D) 3.6 L
E) 5.1 L

Question 43

Calcium nitrite is used as a corrosion inhibitor in lubricants. What is the molality of a solution prepared by dissolving 18.5 g of calcium nitrite in 83.5 g of distilled water?

A) 0.181 m
B) 0.222 m
C) 0.596 m
D) 1.35 m
E) 1.68 m

Question 44

The solubility of oxygen in lakes high in the Rocky Mountains is affected by the altitude. If the aqueous solubility of atmospheric O₂ is 2.67 × 10^-4 M at sea level and 25°C, what is the solubility of O₂ at an elevation of 12,000 ft where the total pressure is 0.657 atm? Assume the temperature is 25°C, and that the mole fraction of O₂ in air is 0.209 at both 12,000 ft and at sea level.

A) 1.75 × 10^-4 M
B) 2.67 × 10^-4 M
C) 3.66 × 10^-5 M
D) 4.06 × 10^-4 M
E) 5.58 × 10^-5 M

Question 45

The solubility of nitrogen gas in water at 25°C and a nitrogen pressure of 522 mmHg is 4.7 × 10^-4 mol/L. What is the value of the Henry's law constant in mol L^-1• atm^-1?

A) 6.8 × 10^-4 mol L^-1• atm^-1
B) 4.7 × 10^-4 mol L^-1• atm^-1
C) 3.2 × 10^-4 mol L^-1• atm^-1
D) 9.0 × 10^-7 mol L^-1• atm^-1
E) 1.5 × 10³ mol L^-1• atm^-1

Question 46

Cadmium bromide is used in photography and lithography. What is the molality of a solution prepared by dissolving 45.38 g of CdBr₂ in 375.0 g of water?

A) 0.03035 m
B) 0.01600 m
C) 0.1210 m
D) 0.4446 m
E) 16.00 m

Question 47

Copper(II) bromide is used as a wood preservative. What mass of CuBr₂ is needed to prepare 750.0 mL of a 1.25 M solution?

A) 134 g
B) 209 g
C) 372 g
D) 750 g
E) 938 g

Question 48

What is the molarity of a solution of 10.0% by mass cadmium sulfate, CdSO₄ (208.47 g/mol)? The density of the solution is 1.10 g/mL.

A) 0.528 M
B) 0.436 M
C) 0.479 M
D) 0.100 M
E) 1.89 M

Question 49

The density of a 20.3 M CH₃OH (methanol) solution is 0.858 g/mL. What is the molality of this solution? H₂O is the solvent.

A) 17.4 m
B) 20.8 m
C) 23.7 m
D) 70.0 m
E) 97.8 m

Question 50

Which law describes the quantitative relationship between the solubility of a gas and its partial pressure?

A) Entropy
B) Henry's law
C) Enthalpy
D) Boyle's law
E) Avogadro's law

Question 51

At 10°C one volume of water dissolves 3.10 volumes of chlorine gas at 1.00 atm pressure. What is the Henry's law constant of Cl₂ in water? (R = 0.0821 atm • L • mol^-1• K^-1 )

A) 3.8 mol • L^-1• atm^-1
B) 0.043 mol • L^-1• atm^-1
C) 36 mol • L^-1• atm^-1
D) 3.1 mol • L^-1• atm^-1
E) 0.13 mol • L^-1• atm^-1

Question 52

Which combination of a 36.0% (w/w) stock solution of acetic acid (d = 1.045 g/mL) and water will result in 1.00 kg of a 15.0% (w/w) acetic acid solution?

A) 417 mL of 36% acetic acid in 583 mL of distilled water
B) 417 g of 36% acetic acid in 583 g of distilled water
C) 360 mL of 36% acetic acid in 640 mL of distilled water
D) 360 g of 36% acetic acid in 640 g of distilled water
E) 150 g of 36% acetic acid in 850 g of distilled water

Question 53

What is the molarity of a 17.0% by mass solution of sodium acetate, NaC₂H₃O₂ (82.0 g/mol), in water? The density of the solution is 1.09 g/mL.

A) 0.170 M
B) 0.207 M
C) 2.07 M
D) 2.26 M
E) 1.90 M

Question 54

Calculate the molality of a 20.0% by mass ammonium sulfate (NH₄)₂SO₄ solution. The density of the solution is 1.117 g/mL.

A) 0.151 m
B) 0.200 m
C) 0.223 m
D) 1.51 m
E) 1.89 m

Question 55

What volume of a 2.75 M solution of NaOH is required to make 500.0 mL of a 1.27 M solution of NaOH?

A) 231 mL
B) 1.72 L
C) 1.10 L
D) 440 mL
E) 909 mL

Question 56

What is the molality of a solution prepared by dissolving 84.7 g of KMnO₄ in 165 g of water?

A) 0.339 m
B) 0.513 m
C) 0.536 m
D) 3.25 m
E) 81.1 m

Question 57

Which of the following states that the solubility of a gas in a liquid is proportional to the pressure of the gas over the solution?

A) Entropy
B) Henry's law
C) Dissolution
D) Vapor pressure
E) Enthalpy of solvation

Question 58

What mass of water is required to dissolve 27.8 g of ammonium nitrate NH₄NO₃ in order to prepare a 0.452 m solution?

A) 0.0615 kg
B) 0.100 kg
C) 0.177 kg
D) 0.768 kg
E) 1.30 kg

Question 59

What is the molarity of a solution prepared by diluting 1.85 L of 6.5 M KOH to 11.0 L?

A) 0.28 M
B) 0.91 M
C) 1.1 M
D) 3.1 M
E) 3.9 M

Question 60

What mass of water is required to dissolve 25.31 g of potassium nitrate (KNO₃) in order to prepare a 0.1982 m solution?

A) 0.5101 kg
B) 0.1277 kg
C) 1.000. kg
D) 1.263 kg
E) 0.7917 kg

Question 61

A solution is 40.00% by volume benzene (C₆H₆) in carbon tetrachloride at 20°C. The vapor pressure of pure benzene at this temperature is 74.61 mmHg and its density is 0.87865 g/cm³; the vapor pressure of pure carbon tetrachloride is 91.32 mmHg and its density is 1.5940 g/cm³. If this solution is ideal, its total vapor pressure at 20°C is

A) 84.64 mmHg.
B) 84.30 mmHg.
C) 82.96 mmHg.
D) 81.63 mmHg.
E) 165.93 mmHg.

Question 62

Sodium hydroxide is a common ingredient in drain cleaners such as Drano^®. The mole fraction of sodium hydroxide in a saturated aqueous solution is 0.310. What is the molality of the solution?

A) 0.310 m
B) 0.690 m
C) 1.24 m
D) 12.4 m
E) 24.9 m

Question 63

Aqueous ammonia is commercially available in a solution that is 28% (w/w) ammonia. What is the mole fraction of ammonia in such a solution?

A) 0.017
B) 0.023
C) 0.012
D) 0.24
E) 0.29

Question 64

Dissolving a solute such as KOH in a solvent such as water results in

A) an increase in the melting point of the liquid.
B) a decrease in the boiling point of the liquid.
C) a decrease in the vapor pressure of the liquid.
D) no change in the boiling point of the liquid.

Question 65

A solution of chloroform, CHCl₃, and acetone, (CH₃)₂CO, exhibits a negative deviation from Raoult's law. This result implies that

A) chloroform-chloroform interactions are stronger than chloroform-acetone interactions.
B) chloroform-acetone interactions are weaker than chloroform-chloroform interactions.
C) acetone-acetone interactions are stronger than chloroform-acetone interactions.
D) acetone-acetone interactions are weaker than chloroform-acetone interactions.

Question 66

From the following list of aqueous solutions and water, select the one with the highest boiling point.

A) 1.0 M KNO₃
B) 0.75 M NaCl
C) 0.75 M CuCl₂
D) 2.0 M C₁₂H₂₂O₁₁ (sucrose)
E) pure water

Question 67

What is the name for a solute that does not exert a vapor pressure when it is dissolved in a liquid?

A) Colloid
B) Amorphous solid
C) Nonvolatile
D) Crystalline solid
E) Electrolyte

Question 68

What is the vapor pressure above a solution prepared by dissolving 0.500 mol of a nonvolatile solute in 275 g of hexane (86.18 g/mol) at 49.6°C? P°_hexane = 400.0 torr at 49.6°C.

A) 54 torr
B) 154 torr
C) 246 torr
D) 346 torr
E) 400. torr

Question 69

Safrole was once used as a flavoring in root beer, until it was banned in 1960. What is the vapor pressure of a solution prepared by dissolving 0.75 mol of nonvolatile safrole in 950 g of ethanol (46.07 g/mol)? P°_ethanol = 50.0 torr at 25°C.

A) 1.8 torr
B) 11 torr
C) 15 torr
D) 40 torr
E) 48 torr

Question 70

Which of the following is not a colligative property?

A) Vapor pressure lowering
B) Atmospheric pressure
C) Boiling point elevation
D) Osmotic pressure
E) Freezing point depression

Question 71

What is the name of a solution that obeys Raoult's law?

A) Ideal solution
B) Nonideal solution
C) Suspension
D) Solute
E) Solvent

Question 72

Which statement is false?

A) The vapor pressure of a solvent over a solution decreases as its mole fraction increases.
B) The solubility of a gas increases as the temperature decreases.
C) The vapor pressure of a solvent over a solution is less than that of pure solvent.
D) The greater the pressure of a gas over a solution, the greater its solubility.
E) Ionic solutes dissociate in solution, causing an enhancement of all colligative properties.

Question 73

The mole fraction of potassium nitrate in an aqueous solution is 0.0194. The solution's density is 1.0627 g/mL. What is the molarity of KNO₃ in the solution?

A) 0.0194 M
B) 0.981 M
C) 1.05 M
D) 1.96 M
E) 19.4 M

Question 74

Which solution has the highest vapor pressure?

A) 0.75 mol of a nonvolatile compound in 750 g of ethanol
B) 0.75 mol of a volatile compound in 750 g of ethanol
C) 1.5 mol of a nonvolatile compound in 750 g of ethanol
D) Solutions A and B have the same vapor pressure and it is higher than the vapor pressure of solution C.
E) Not enough information is given to determine which solution has the highest vapor pressure.

Question 75

Which of the following aqueous solutions should demonstrate the most ideal behavior?

A) 0.1 M K₂SO₄
B) 0.1 M CaCl₂
C) 3.0 M LiF
D) 0.1 M MgSO₄
E) 0.1 M NaCl

Question 76

The solubility of the oxidizing agent potassium permanganate is 7.1 g per 100.0 g of water at 25°C. What is the mole fraction of potassium permanganate (KMnO₄) in this solution?

A) 0.0080
B) 0.0086
C) 0.066
D) 0.071
E) 0.48

Question 77

From the following list of aqueous solutions and water, select the one with the highest freezing point.

A) 1.0 M KNO₃
B) 0.75 M NaCl
C) 0.75 M CuCl₂
D) 2.0 M C₁₂H₂₂O₁₁ (sucrose)
E) 2.0 M KNO₃

Question 78

What relationship states that the partial pressure of a solvent over a solution is given by the vapor pressure of the pure solvent times the mole fraction of the solvent in the solution?

A) Henry's law
B) Law of partial pressures
C) Curie's law
D) Raoult's law
E) Vapor pressure

Question 79

Which of the following aqueous solutions should demonstrate the most nonideal behavior?

A) 0.1 M NaI
B) 0.2 M CuSO₄
C) 0.5 M KBr
D) 2.0 M CuCl₂
E) 2.5 M CsCl

Question 80

Diethyl ether has a vapor pressure of 400.0 torr at 18°C. When a sample of benzoic acid is dissolved in ether, the vapor pressure of the solution is 342 torr. What is the mole fraction of benzoic acid in the solution?

A) 0.0169
B) 0.0197
C) 0.145
D) 0.855
E) 0.045