Question 1

Which of the following best explains why drinking seawater can cause dehydration in humans?

Accepted Answer

Seawater contains a higher concentration of salts than the salt content of human cells, causing water to move out of the cells by osmosis.

Question 2

A red blood cell is placed in a solution and it shrivels. Which type of solution is it most likely in?

Accepted Answer

Hypertonic solution

Question 3

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

Accepted Answer

Ion-dipole interactions

Question 4

Which of the following statements about the enthalpy change of solution ($\Delta H_{solution}$) is correct?

Accepted Answer

$\Delta H_{solution}$ can be either positive or negative depending on the relative magnitudes of $\Delta H_{solute}$, $\Delta H_{solvent}$, and $\Delta H_{mix}$.

Question 5

Which equation correctly relates the heat of hydration ($\Delta H_{hydration}$), lattice energy ($\Delta H_{lattice\ energy}$), and the enthalpy of solution ($\Delta H_{solution}$) for an ionic compound dissolving in water?

Accepted Answer

$\Delta H_{solution} = \Delta H_{hydration} - \Delta H_{lattice\ energy}$

Question 6

According to Henry’s Law, what happens to the solubility of a gas in a liquid if the partial pressure of the gas above the liquid is doubled?

Accepted Answer

The solubility of the gas also doubles.

Question 7

Which of the following best describes a saturated solution?

Accepted Answer

A solution in which the solute and solvent are in dynamic equilibrium and no more solute will dissolve at that temperature.

Question 8

Which of the following will increase the solubility of a solid solute in water if the dissolution process is endothermic?

Accepted Answer

Increasing the temperature

Question 9

A solution is prepared by dissolving 2.0 moles of NaCl in 1.0 kg of water. What is the molality ($m$) of the solution?

Accepted Answer

$2.0\ m$

Question 10

Which of the following best explains why the vapor pressure of a solvent decreases when a nonvolatile solute is added?

Accepted Answer

The solute particles occupy surface positions, reducing the number of solvent molecules able to escape into the vapor phase.

Question 11

Which formula correctly expresses Raoult’s Law for the vapor pressure of a solution?

Accepted Answer

$P_{solution} = X_{solvent} P_{solvent}$

Question 12

A 1.0 m solution of NaCl will have a higher boiling point than a 1.0 m solution of glucose because:

Accepted Answer

NaCl dissociates into more particles in solution, increasing the van’t Hoff factor ($i$).

Question 13

Which equation is used to calculate the osmotic pressure ($\Pi$) of a solution?

Accepted Answer

$\Pi = iMRT$

Question 14

If a red blood cell is placed in pure water, what will happen to the cell and why?

Accepted Answer

The cell will swell and possibly burst because water enters the cell by osmosis.

Question 15

Which of the following statements about colligative properties is correct?

Accepted Answer

Colligative properties depend only on the number of solute particles, not their identity.

Question 16

A solution is made by dissolving 0.5 moles of KBr in 1.0 kg of water. Assuming complete dissociation, what is the expected van’t Hoff factor ($i$) for KBr?

Accepted Answer

$2$

Question 17

Which of the following will decrease the solubility of a gas in water?

Accepted Answer

Increasing the temperature

Question 18

Which of the following best describes a miscible pair of liquids?

Accepted Answer

Two liquids that are mutually soluble in all proportions

Question 19

Which of the following equations is used to calculate the freezing point depression of a solution?

Accepted Answer

$\Delta T_f = i 	imes m 	imes K_f$

Chapter 13: Solutions – Structure, Properties, and Effects

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