Deck 13: Solutions

Question 1

To increase solubility of a gas into a liquid the most,then

A) increase the temperature and lower the pressure.
B) increase the temperature and raise the pressure.
C) decrease the temperature and raise the pressure.
D) decrease the temperature and lower the pressure.
E) neither pressure or temperature affects solubility.

Answer 1

decrease the temperature and raise the pressure.

Question 2

________ is the gas dissolved in carbonated drinks.

A) Carbon dioxide
B) Nitrogen
C) Helium
D) Hydrogen
E) Oxygen

Answer 2

Carbon dioxide

Question 3

A solution containing less than the equilibrium amount is called

A) an unsaturated solution.
B) a dilute solution.
C) a supersaturated solution.
D) a concentrated solution.
E) a saturated solution.

Answer 3

an unsaturated solution.

Question 4

To make rock candy,sugar is dissolved in hot water until no more can dissolve,then the solution is allowed to cool.A stick is placed in the sugar solution and crystals form on the stick.Describes what happens in terms of unsaturation,saturation,and supersaturation.

A) The hot solution is saturated and the cooled solution is unsaturated.
B) The hot solution is supersaturated and the cooled solution is saturated.
C) The hot solution is unsaturated and the cooled solution is saturated.
D) The hot solution is saturated and the cooled solution is supersaturated.
E) The hot solution is supersaturated and the cooled solution is unsaturated.

Question 5

Identify the major force between molecules of pentane.

A) dipole-dipole
B) dispersion
C) hydrogen bonding
D) ion-ion
E) ion-dipole

Question 6

A solution in which the dissolved solute is in dynamic equilibrium with the solid solute is called

A) an unsaturated solution.
B) a dilute solution.
C) a supersaturated solution.
D) a concentrated solution.
E) a saturated solution.

Question 7

Which of the following statements is generally TRUE?

A) The solubility of a solid is not dependent on either temperature or pressure.
B) The solubility of a solid is highly dependent on pressure.
C) The solubility of a solid is highly dependent on both pressure and temperature.
D) The solubility of a solid is highly dependent on temperature.
E) None of the above.

Question 8

Choose the situation below that would result in a ΔH_solution near 0.

A) When >>

B) When >

C) When <

D) When is close to

E) There isn't enough information to determine.

Question 9

Give the major force between acetone and chloroform.

A) dipole-dipole
B) dispersion
C) hydrogen bonding
D) ion-ion
E) ion-dipole

Question 10

Define solubility.

A) a solid that does not dissolve in a gas
B) the amount of a substance that will dissolve in a given amount of solvent
C) the amount of a substance that will dissolve in a given amount of solute
D) a solid mixed with another solid
E) a liquid that does not dissolve in another liquid

Question 11

Which of the following compounds is most soluble in hexane (CH₃CH₂CH₂CH₂CH₂CH₂CH₃)?

A) methanol
B) ethanol
C) 1-propanol
D) 1-butanol
E) 1-pentanol

Question 12

Describe what happens when seawater is consumed to quench thirst.

A) Seawater can quench thirst once it is boiled.
B) Seawater quenches thirst when directly ingested.
C) Seawater draws water out of the body resulting in further dehydration and diarrhea.
D) Seawater helps diarrhea.
E) Seawater must be ingested at twice the volume to quench thirst.

Question 13

If two substances are soluble in all proportions then they are ________ in each other.

A) miscible
B) nonpolar
C) immiscible
D) neutral
E) polar

Question 14

Determine ΔH_solute for KBr if the ΔH_solution (KBr)= +19.9 kJ/mol and the ΔH_hydration(KBr)= -670.kJ/mol.

A) +650 kJ/mol
B) -650 kJ/mol
C) +690 kJ/mol
D) -710 kJ/mol
E) -690 kJ/mol

Question 15

Choose the situation below that would result in an exothermic ΔH_solution.

A) When >

B) When is close to

C) When <

D) When >>

E) There isn't enough information to determine.

Question 16

A solution containing more than the equilibrium amount is called

A) an unsaturated solution.
B) a dilute solution.
C) a supersaturated solution.
D) a concentrated solution.
E) a saturated solution.

Question 17

Which of the following compounds will be most soluble in ethanol (CH₃CH₂OH)?

A) trimethylamine (N(CH₃)₃)
B) acetone (CH₃COCH₃)
C) ethylene glycol (HOCH₂CH₂OH)
D) hexane (CH₃CH₂CH₂CH₂CH₂CH₃)
E) None of these compounds should be soluble in ethanol.

Question 18

A solution is formed at room temperature by vigorously dissolving enough of the solid solute so that some solid remains at the bottom of the solution.Which statement below is TRUE?

A) The solution is considered unsaturated.
B) The solution is considered supersaturated.
C) The solution is considered saturated.
D) The solution would be considered unsaturated if it were cooled a bit to increase the solubility of the solid.
E) None of the above is true.

Question 19

Choose the statement below that is TRUE.

A) A solution will form between two substances if the solute-solvent interactions are of comparable strength to the solute-solute and solvent-solvent interactions.
B) A solution will form between two substances if the solute-solvent interactions are small enough to be overcome by the solute-solute and solvent-solvent interactions.
C) A solution will form between two substances if the solute-solute interactions are strong enough to overcome the solvent-solvent interactions.
D) A solution will form between two substances only if the solvent-solvent interactions are weak enough to overcome the solute-solvent interactions.
E) None of the above is true.

Question 20

Choose the situation below that would result in an endothermic ΔH_solution.

A) When >

B) When <

C) When is close to

D) When >>

E) There isn't enough information to determine.

Question 21

Commercial grade HCl solutions are typically 39.0% (by mass)HCl in water.Determine the molarity of the HCl,if the solution has a density of 1.20 g/mL.

A) 7.79 M
B) 10.7 M
C) 12.8 M
D) 9.35 M
E) 13.9 M

Question 22

The Dirty Dozen refer to twelve chemicals that are harmful for the environment.Identify the compound that was not used as an insecticide.

A) Chlordane
B) DDT
C) Aldrin
D) polychlorinated biphenyl
E) Heptachlor

Question 23

A solution is prepared by dissolving 76.3 g NaI in 545 g of water.Determine the mole fraction of NaI if the final volume of the solution is 576 mL.

A) 6.04 × 10^-3
B) 1.65 × 10^-2
C) 1.40 × 10^-3
D) 1.32 × 10^-2
E) 8.84 × 10^-2

Question 24

Which of the following concentration units is temperature dependent?

A) mole fraction
B) molality
C) mass percent
D) molarity
E) none of the above

Question 25

______ is burped up from the bottom of a water-filled volcanic crater.

A) Carbon monoxide
B) Oxygen
C) Nitrogen
D) Hydrogen
E) Carbon dioxide

Question 26

Give the term for the amount of solute in moles per liter of solution.

A) molality
B) molarity
C) mole fraction
D) mole percent
E) mass percent

Question 27

A solution is prepared by dissolving 38.6 g sucrose (C₁₂H₂₂O₁₁)in 495 g of water.Determine the mole fraction of sucrose if the final volume of the solution is 508 mL.

A) 4.09 × 10^-3
B) 7.80 × 10^-2
C) 1.28 × 10^-3
D) 7.23 × 10^-2
E) 2.45 × 10^-3

Question 28

Which of the following statements is TRUE?

A) In general, the solubility of a solid in water decreases with increasing temperature.
B) In general, the solubility of a gas in water decreases with increasing temperature.
C) The solubility of a gas in water usually increases with decreasing pressure.
D) The solubility of an ionic solid in water decreases with increasing temperature.
E) None of the above statements is true.

Question 29

Calculate the mass of oxygen (in mg)dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 atm of air.Assume the mole fraction of oxygen in air to be 0.21 and the Henry's law constant for oxygen in water at this temperature to be 1.3 × 10^-3 M/atm.

A) 49.4 mg
B) 23.5 mg
C) 9.87 mg
D) 27.3 mg
E) 13.7 mg

Question 30

A solid can be purified through what technique?

A) recrystallization
B) dilution
C) dissolution
D) boiling
E) melting

Question 31

What mass (in g)of NH₃ must be dissolved in 475 g of methanol to make a 0.250 m solution?

A) 2.02 g
B) 4.94 g
C) 1.19 g
D) 8.42 g
E) 1.90 g

Question 32

Identify the colligative property.

A) vapor pressure lowering
B) freezing point depression
C) boiling point elevation
D) osmotic pressure
E) all of the above

Question 33

0.300 moles of sodium nitrite are needed for a reaction.The solution is 0.450 M.How many mL are needed?

A) 0.667 mL
B) 1500 mL
C) 1.5 mL
D) 667 mL
E) 135 mL

Question 34

Give the term for the amount of solute in moles per kilogram of solvent.

A) molality
B) molarity
C) mole fraction
D) mole percent
E) mass percent

Question 35

Calculate the number of moles of sulfuric acid that is contained in 0.250 mL of 0.500 M sulfuric acid solution.

A) 0.125 moles
B) 2.00 moles
C) 0.500 moles
D) 8.00 moles
E) 0.600 moles

Question 36

Calculate the molality of a solution that is prepared by mixing 25.5 mL of CH₃OH (d = 0.792 g/mL)and 387 mL of CH₃CH₂CH₂OH (d = 0.811 g/mL).

A) 0.630 m
B) 0.812 m
C) 1.57 m
D) 2.01 m
E) 4.98 m

Question 37

Choose the solvent below that would show the greatest freezing point lowering when used to make a 0.20 m nonelectrolyte solution.

A) carbon tetrachloride, K_f = 29.9°C/m
B) chloroform, K_f = 4.70°C/m
C) benzene, K_f = 5.12°C/m
D) ethanol, K_f = 1.99°C/m
E) diethyl ether, K_f = 1.79°C/m

Question 38

Commercial grade HCl solutions are typically 39.0% (by mass)HCl in water.Determine the molality of the HCl,if the solution has a density of 1.20 g/mL.

A) 39.0 m
B) 17.5 m
C) 6.39 m
D) 10.7 m
E) 9.44 m

Question 39

Determine the Henry's law constant for ammonia in water at 25°C if an ammonia pressure of 0.022 atm produces a solution with a concentration of 1.3 M.

A) 59 M/atm
B) 0.017 M/atm
C) 0.029 M/atm
D) 35 M/atm
E) 0.038 M/atm

Question 40

Determine the vapor pressure of a solution at 25°C that contains 76.6 g of glucose (C₆H₁₂O₆)in 250.0 mL of water.The vapor pressure of pure water at 25°C is 23.8 torr.

A) 70.8 torr
B) 72.9 torr
C) 23.1 torr
D) 22.9 torr
E) 7.29 torr

Question 41

Identify the classification of milk.

A) aerosol
B) solid aerosol
C) foam
D) emulsion
E) solid emulsion

Question 42

Identify the classification of opal.

A) aerosol
B) solid aerosol
C) foam
D) emulsion
E) solid emulsion

Question 43

Define colloid.

A) a mixture in which a substance floats on the dispersing medium
B) a mixture in which a substance is dissolved in a solute
C) a mixture in which a substance is dissolved in a solvent
D) a mixture in which a substance settles to the bottom of a dispersing medium
E) a mixture in which a dispersed substance is finely divided in a dispersing medium

Question 44

Solutions having osmotic pressures more than those of body fluids are called

A) isosmotic.
B) hyperosmotic.
C) hyposmotic.
D) neosmotic.
E) magnosmotic.

Question 45

The boiling point elevation of an aqueous sucrose solution is found to be 0.39°C.What mass of sucrose (molar mass= 342.30 g/mol)would be needed to dissolve in 500.0 g of water? K_b (water)= 0.512°C/m.

A) 261 g sucrose
B) 528 g sucrose
C) 762 g sucrose
D) 223 g sucrose
E) 130. g sucrose

Question 46

Calculate the freezing point of a solution of 500.0 g of ethylene glycol (C₂H₆O₂)dissolved in 500.0 g of water.K_f = 1.86°C/m and K_b = 0.512°C/m.

A) 30.0°C
B) -30.0°C
C) 8.32°C
D) -8.32°C
E) 70.2°C

Question 47

Determine the vapor pressure of a solution at 55°C that contains 34.2 g NaCl in 375 mL of water.The vapor pressure of pure water at 55°C is 118.1 torr.The van't Hoff factor for NaCl is 1.9.

A) 115 torr
B) 87.1 torr
C) 108 torr
D) 112 torr
E) 92.8 torr

Question 48

Identify the classification of whipped cream.

A) aerosol
B) solid aerosol
C) foam
D) emulsion
E) solid emulsion

Question 49

A compound is found to have a molar mass of 598 g/mol.If 35.8 mg of the compound is dissolved in enough water to make 175 mL of solution at 25°C,what is the osmotic pressure of the resulting solution?

A) 3.42 torr
B) 6.36 torr
C) 5.01 torr
D) 5.99 torr
E) 8.36 torr

Question 50

The boiling point of an aqueous 1.83 m (NH₄)₂SO₄ (molar mass = 132.15 g/mol)solution is 102.5°C.Determine the value of the van't Hoff factor for this solute if the K_b for water is 0.512°C/m.

A) 3.0
B) 3.6
C) 1.8
D) 2.7
E) 2.3

Question 51

Give the reason that antifreeze is added to a car radiator.

A) The freezing point is lowered and the boiling point is elevated.
B) The freezing point is elevated and the boiling point is lowered.
C) The freezing point and the boiling point are elevated.
D) The freezing point and the boiling point are lowered.
E) None of the above

Question 52

Determine the freezing point depression of a solution that contains 30.7 g glycerin (C₃H₈O₃,molar mass = 92.09 g/mol)in 376 mL of water.Some possibly useful constants for water are K_f = 1.86°C/m and K_b = 0.512°C/m.

A) 0.887°C
B) 1.65°C
C) 3.33°C
D) 4.98°C
E) 0.654°C

Question 53

Calculate the boiling point of a solution of 500.0 g of ethylene glycol (C₂H₆O₂)dissolved in 500.0 g of water.K_f = 1.86°C/m and K_b = 0.512°C/m.Use 100°C as the boiling point of water.

A) 108°C
B) 92°C
C) 130°C
D) 70°C
E) 8.3°C

Question 54

Fluids used for an intravenous transfusion must be ________ with bodily fluids.

A) isosmotic
B) hyperosmotic
C) hyposmotic
D) neosmotic
E) magnosmotic

Question 55

Determine the freezing point of a solution that contains 78.8 g of naphthalene (C₁₀H₈, molar mass = 128.16 g/mol)dissolved in 722 mL of benzene (d = 0.877 g/mL).Pure benzene has a melting point of 5.50°C and a freezing point depression constant of 4.90°C/m.

A) 4.76°C
B) 4.17°C
C) 0.74°C
D) 1.33°C
E) 1.68°C

Question 56

Solutions having osmotic pressures less than those of body fluids are called

A) isosmotic.
B) hyperosmotic.
C) hyposmotic.
D) neosmotic.
E) magnosmotic.

Question 57

Determine the boiling point of a solution that contains 78.8 g of naphthalene (C₁₀H₈, molar mass = 128.16 g/mol)dissolved in 722 mL of benzene (d = 0.877 g/mL).Pure benzene has a boiling point of 80.1°C and a boiling point elevation constant of 2.53°C/m.

A) 2.2°C
B) 2.5°C
C) 82.3°C
D) 80.4°C
E) 82.6°C

Question 58

Soap has an ionic and a polar end.It works well to remove oil by

A) surrounding the oil with the nonpolar end, and the water interacts with the polar end.
B) surrounding the oil with the polar end, and the water interacts with the nonpolar end.
C) surrounding the oil and water with the polar end.
D) surrounding the oil and water with the nonpolar end.

Question 59

A 150.0 mL sample of an aqueous solution at 25°C contains 15.2 mg of an unknown nonelectrolyte compound.If the solution has an osmotic pressure of 8.44 torr,what is the molar mass of the unknown compound?

A) 223 g/mol
B) 294 g/mol
C) 341 g/mol
D) 448 g/mol
E) 195 g/mol

Question 60

Light beams that are visible in a dusty room is an example of

A) an emulsion.
B) an aerosol.
C) micelle repulsion.
D) Brownian motion.
E) Tyndall effect.

Question 61

Determine the solubility of CO₂ in soda water at 25°C if the pressure of CO₂ is 5.6 atm.The Henry's law constant for carbon dioxide in water at this temperature is 3.4 × 10^-2 M/atm.

A) 0.16 M
B) 0.53 M
C) 0.61 M
D) 0.19 M
E) 0.78 M

Question 62

Dissolving of a salt can be defined as

A) solvation of ions, with no change in the amount of solid.
B) solvation of ions, with increase in the amount of solid.
C) solvation of ions, with decrease in the amount of solid.
D) rate of bubbling > rate of dissolving.
E) rate of condensing > rate of bubbling.

Question 63

Determine the partial pressure of oxygen necessary to form an aqueous solution that is 7.1 × 10^-4 M O₂ at 25°C.The Henry's law constant for oxygen in water at 25°C is
1)3 × 10^-3 M/atm.

A) 1.1 atm
B) 0.92 atm
C) 0.88 atm
D) 1.8 atm
E) 0.55 atm

Question 64

Identify the compound whose solubility decreases with increasing temperature.

A) Ce₂(SO₄)₃
B) K₂Cr₂O₇
C) NaNO₃
D) KClO₃
E) CaCl₂

Question 65

Give the major force in NaCl solution.

A) dipole-dipole
B) nonpolar forces
C) hydrogen bonding
D) ion-ion
E) ion-dipole

Question 66

Identify the compound whose solubility is least affected by temperature.

A) KCl
B) K₂Cr₂O₇
C) NaNO₃
D) Pb(NO₃)₃
E) NaCl

Question 67

What volume of a 0.716 M KBr solution is needed to provide 30.5 g of KBr?

A) 21.8 mL
B) 42.7 mL
C) 184 mL
D) 358 mL

Question 68

Calculate the molarity of a solution that contains 0.300 moles of CsBr in 0.600 L of water.

A) 0.500 M
B) 2.00 M
C) 0.125 M
D) 8.00 M
E) 0.750 M

Question 69

Identify the compounds that are soluble in both water and hexane.

A) methanol and 1-pentanol
B) ethanol and 1-butanol
C) 1-propanol and 1-butanol
D) 1-butanol and 1-pentanol
E) ethanol and 1-propanol

Question 70

Identify the most polar solvent.

A) acetone
B) octane
C) sodium chloride
D) toluene
E) carbon tetrachloride

Question 71

Which of the following compounds will be most soluble in nonane (C₉H₂₀)?

A) 1-pentanol
B) benzene
C) acetic acid
D) ethyl methyl ketone
E) ethanol

Question 72

Dynamic equilibrium can be defined as

A) rate of dissolution = rate of recrystallization.
B) rate of dissolution < rate of recrystallization.
C) rate of dissolution > rate of recrystallization.
D) rate of bubbling > rate of dissolving.
E) rate of condensing > rate of bubbling.

Question 73

Determine the solubility of N₂ in water exposed to air at 25°C if the atmospheric pressure is 2.0 atm.Assume that the mole fraction of nitrogen is 0.78 in air and the Henry's law constant for nitrogen in water at this temperature is 6.1 × 10^-4 M/atm.

A) 1.6 × 10^-4 M
B) 6.4 × 10^-4 M
C) 9.5 × 10^-4 M
D) 1.1 × 10^-4 M
E) 1.2 × 10^-4 M

Question 74

Which of the following should have the largest Henry's law constant (k_H)in water?

A) Xe
B) CO
C) H₂
D) CH₃CH₃
E) CO₂

Question 75

Which cation in each set is expected to have the larger (more negative)hydration energy? I Be²⁺ or Ca²⁺
II Rb⁺ or Zn²⁺

A) Be²⁺ in set I and Rb⁺ in set II
B) Be²⁺ in set I and Zn²⁺ in set II
C) Ca²⁺ in set I and Rb⁺ in set II
D) Ca²⁺ in set I and Zn²⁺ in set II

Question 76

The Henry's law constant for helium gas in water at 30°C is 3.70 × 10^-4 M/atm.When the partial pressure of helium above a sample of water is 0.650 atm,the concentration of helium in the water is ________ M.

A) 5.69 × 10^-4
B) 1.76 × 10³
C) 1.30
D) 2.41 × 10^-4
E) 3.70 × 10^-4

Question 77

Identify the gas that is dissolved in carbonated sodas.

A) carbon dioxide
B) ammonia
C) helium
D) carbon monoxide
E) xenon

Question 78

Give the major force between ethanol and rubbing alcohol.

A) dipole-dipole
B) ionic forces
C) hydrogen bonding
D) ion-ion
E) oxygen bonding

Question 79

Which of the following ions should have the most exothermic ΔH_hydration?

A) Rb⁺
B) Ba²⁺
C) Al³⁺
D) Sr²⁺
E) Ni²⁺

Question 80

The Henry's Law constant of methyl bromide,CH₃Br,is k = 0.159 mol/(L ∙ atm)at 25°C.What is the solubility of methyl bromide in water at 25°C and at a partial pressure of 270.mm Hg?

A) 0.0565 mol/L
B) 0.355 mol/L
C) 0.448 mol/L
D) 42.9 mol/L