Q: Which equation correctly represents Henry’s Law for the solubility of a gas in a liquid?

$$S_{\text{gas}} = k_H P_{\text{gas}}$$

Question 1

Which of the following best describes a solution?

Accepted Answer

A homogeneous mixture of two or more substances

Question 2

According to the 'like dissolves like' rule, which solvent would best dissolve a nonpolar solute such as oil?

Accepted Answer

Hexane

Question 3

Which intermolecular force is primarily responsible for the high solubility of NaCl in water?

Accepted Answer

Ion-dipole interactions

Question 4

A solution is prepared by mixing 35.8 g of benzene (C6H6, 78.11 g/mol) and 56.7 g of toluene (C7H8, 92.13 g/mol) at 25°C. If the vapor pressure of pure benzene is 95.1 mm Hg and pure toluene is 28.4 mm Hg, what is the vapor pressure above the solution?

Accepted Answer

40.6 mm Hg

Question 5

Which equation correctly represents Henry’s Law for the solubility of a gas in a liquid?

Accepted Answer

$$S_{	ext{gas}} = k_H P_{	ext{gas}}$$

Question 6

Which of the following would be expected to have the highest solubility in water?

Accepted Answer

CH3CH2CH2OH

Question 7

What happens to the solubility of most solid solutes as temperature increases?

Accepted Answer

Solubility increases

Question 8

A 235 mL block of stainless steel contains 561 mg of sulfur. If the steel has a density of 8.03 g/mL, what is the concentration of sulfur expressed in ppm?

Accepted Answer

297 ppm

Question 9

Which concentration unit does NOT vary with temperature?

Accepted Answer

Molality (m)

Question 10

Which property is NOT a colligative property?

Accepted Answer

Color change

Question 11

A solution is prepared by dissolving 150.0 mg of caffeine in 10.0 g of camphor. The freezing point is 3.07°C lower than pure camphor (Kf = 39.7°C/m). What is the molar mass of caffeine?

Accepted Answer

194 g/mol

Question 12

Which equation is used to calculate the boiling point elevation of a solution?

Accepted Answer

$$\Delta T_b = m 	imes K_b$$

Question 13

What is the osmotic pressure ($$\pi) of a $$solution with a molarity of 0.25 M at 298 K? (R = 0.08206 L·atm/mol·K)

Accepted Answer

$$\pi = 6.11$$ atm

Question 14

Which of the following aqueous solutions is expected to have the lowest freezing point (largest deviation from pure water)? Assume complete dissociation.

Accepted Answer

1 m AlCl3

Question 15

What is the van’t Hoff factor ($$i) $$for NaCl in aqueous solution, assuming complete dissociation?

Accepted Answer

$$i = 2$$

Question 16

Which scenario best illustrates osmosis?

Accepted Answer

Solvent flows from a solution of lower solute concentration to higher concentration

Question 17

Which of the following is NOT a factor affecting the solubility of a solute in a solvent?

Accepted Answer

Color of the solute

Question 18

A red blood cell placed in pure water will:

Accepted Answer

Swell and possibly burst due to water entering the cell

Question 19

Which concentration unit is defined as the ratio of moles of a component to the total moles in the mixture?

Accepted Answer

Mole fraction

Question 20

Which of the following statements about dynamic equilibrium in a saturated solution is correct?

Accepted Answer

The rate of dissolution equals the rate of recrystallization

Chapter 14: Solutions – Properties, Types, and Colligative Effects

Study Guide - Practice Questions

Study Guide - Flashcards