Question 1

Which of the following best explains why drinking seawater leads to dehydration in humans?

Accepted Answer

The high concentration of salt in seawater draws water out of body cells by osmosis.

Question 2

A solution is prepared by dissolving 10.0 g of NaCl in 100.0 g of water. Which term best describes NaCl in this solution?

Accepted Answer

Solute

Question 3

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

Accepted Answer

Ion–dipole interactions

Question 4

According to the rule 'like dissolves like,' which solvent would best dissolve a nonpolar solute such as hexane ($\mathrm{C_6H_{14}}$)?

Accepted Answer

Hexane ($\mathrm{C_6H_{14}}$)

Question 5

Which of the following best describes entropy in the context of solution formation?

Accepted Answer

A measure of energy randomization or dispersal in a system.

Question 6

Which equation correctly expresses the enthalpy of solution ($\Delta H_{\mathrm{soln}}$) in terms of the steps of solution formation?

Accepted Answer

$\Delta H_{\mathrm{soln}} = \Delta H_{\mathrm{solute}} + \Delta H_{\mathrm{solvent}} + \Delta H_{\mathrm{mix}}$

Question 7

A solution is saturated with respect to a solute at a given temperature. What will happen if more solute is added?

Accepted Answer

The added solute will not dissolve and will remain as a solid.

Question 8

Which of the following statements about the solubility of gases in water is correct?

Accepted Answer

The solubility of gases decreases with increasing temperature.

Question 9

According to Henry’s law, what is the relationship between the solubility of a gas ($S_{\mathrm{gas}}$) and its partial pressure ($P_{\mathrm{gas}}$) above a liquid?

Accepted Answer

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

Question 10

Which of the following units is NOT commonly used to express solution concentration?

Accepted Answer

Joules per liter (J/L)

Question 11

A solution is made by dissolving 10.0 g of glucose ($\mathrm{C_6H_{12}O_6}$) in 100.0 g of water. What is the molality ($m$) of the solution? (Molar mass of glucose = 180.16 g/mol)

Accepted Answer

$0.556\ m$

Question 12

Which equation represents Raoult’s law for the vapor pressure of a solution?

Accepted Answer

$P_{\mathrm{solution}} = x_{\mathrm{solvent}} P^\circ_{\mathrm{solvent}}$

Question 13

Which of the following best describes a colligative property?

Accepted Answer

A property that depends only on the number of solute particles.

Question 14

What is the expected van’t Hoff factor ($i$) for a solution of $\mathrm{MgCl_2}$, assuming complete dissociation?

Accepted Answer

3

Question 15

Which of the following equations gives the freezing point depression for a solution?

Accepted Answer

$\Delta T_f = i m K_f$

Question 16

A 1.0 m aqueous solution of NaCl has a lower freezing point than a 1.0 m solution of glucose. Why?

Accepted Answer

NaCl dissociates into more particles in solution.

Question 17

Which of the following best describes a colloid?

Accepted Answer

A mixture with dispersed particles between 1 nm and 1000 nm.

Question 18

Which phenomenon is used to distinguish a colloid from a true solution?

Accepted Answer

Tyndall effect

Question 19

Which of the following best describes osmosis?

Accepted Answer

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

Solutions: Properties, Formation, and Concentration

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