Question 1

Why does drinking seawater cause dehydration in humans?

Accepted Answer

Because seawater is hyperosmotic, causing water to flow out of cells due to osmosis.

Question 2

Which of the following best describes why ideal gases mix spontaneously?

Accepted Answer

Because mixing increases their entropy.

Question 3

Which statement about the formation of a solution is correct?

Accepted Answer

Mixing can occur even if the process is endothermic, due to entropy increase.

Question 4

Which of the following pairs is most likely to be miscible?

Accepted Answer

Alcohol and water

Question 5

A solution is prepared by dissolving 25.0 grams of a solute (molar mass = 25.0 g/mol) in 100.0 grams of solvent. What is the molality of the solution?

Accepted Answer

$$1.0\ \mathrm{m}$$

Question 6

Which of the following best explains why ammonia has a larger Henry’s law constant in water than oxygen?

Accepted Answer

Because ammonia is polar and oxygen is nonpolar.

Question 7

Which of the following is true about the vapor pressure of a solution compared to the pure solvent?

Accepted Answer

The vapor pressure of the solution is always lower than that of the pure solvent.

Question 8

What is the vapor pressure of a solution in which the mole fraction of the solute is $$0.200$$ and the vapor pressure of the pure solvent is $$100.0\ \mathrm{torr}$$? (Assume a single nonvolatile, nonelectrolyte solute.)

Accepted Answer

$$80.0\ \mathrm{torr}$$

Question 9

A solution contains equal moles of two volatile liquids, A and B. The vapor pressure of pure A is $$100\ \mathrm{mmHg}$$ and pure B is $$200\ \mathrm{mmHg}. $$The measured vapor pressure of the solution is $$120\ \mathrm{mmHg}. $$What does this indicate about the interactions?

Accepted Answer

Solute–solute and solvent–solvent interactions \u003e solute–solvent interactions

Question 10

Which of the following best describes a supersaturated solution?

Accepted Answer

A solution that contains more solute than the saturation concentration and is unstable.

Question 11

Which of the following statements about colligative properties is correct?

Accepted Answer

They depend only on the number of solute particles.

Question 12

Which solution will have the highest boiling point?

Accepted Answer

$$0.50\ \mathrm{M}\ \mathrm{NaCl}$$

Question 13

What is the effect of adding a nonvolatile solute to a solvent on the freezing point of the solution?

Accepted Answer

The freezing point decreases.

Question 14

Which of the following best describes osmosis?

Accepted Answer

The flow of solvent from low solute concentration to high solute concentration through a semipermeable membrane.

Question 15

A solution is prepared by dissolving $$10.0\ \mathrm{g} of $$NaCl (molar mass $$58.44\ \mathrm{g/mol}) in$$ $$500.0\ \mathrm{g} of $$water. What is the molality of the solution?

Accepted Answer

$$0.171\ \mathrm{m}$$

Question 16

Which of the following best describes a colloid?

Accepted Answer

A heterogeneous mixture with particles that do not separate on standing and show the Tyndall effect.

Question 17

Which of the following is a real-life example of the Tyndall effect?

Accepted Answer

The scattering of headlights in fog.

Question 18

Which of the following best explains why soap can emulsify oil in water?

Accepted Answer

Soap molecules have both a hydrophilic head and a hydrophobic tail.

Chapter 14: Solutions – General Chemistry Study Notes

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