Q: Which equation correctly represents the relationship for molarity ($$M$$)?

$$M = \frac{\text{amount\;solute\;(in\;mol)}}{\text{volume\;solution\;(in\;L)}}$$

Q: Which equation represents Henry's Law for the solubility of a gas?

$$C = k_P \cdot P_{\text{gas}}$$

Q: Which equation correctly expresses Raoult's Law for a solution with a nonvolatile solute?

$$P_{\text{solution}} = X_{\text{solvent}} \cdot P$$^{\circ}$$_{\text{solvent}}$$

Q: A solution is made by dissolving 1.0 mol of NaCl in 1.0 kg of water. If the van't Hoff factor ($$i) $$for NaCl is 1.9, what is the expected freezing point depression ($$\Delta T_f) $$given $$K_f = 1.86\;\text{°C kg/mol}$$?

$$\Delta T_f = 3.53\;\text{°C}$$

Question 1

Which statement best describes the difference between a solvent and a solute in a solution?

Accepted Answer

The solvent is the component present in the largest amount, and the solute is present in a smaller amount.

Question 2

Which intermolecular forces are present in seawater (a solution of salt in water)?

Accepted Answer

Ion-dipole interactions between salt ions and water, and hydrogen bonding between water molecules.

Question 3

Which of the following pairs of substances are miscible?

Accepted Answer

Ethanol and water

Question 4

Why do ideal gases mix spontaneously when placed in the same container?

Accepted Answer

Because mixing increases the system's entropy, lowering the system's energy.

Question 5

Which statement best explains the rule 'like dissolves like'?

Accepted Answer

Solutes dissolve best in solvents with similar intermolecular forces.

Question 6

Consider the dissolution of NaCl in water. Which step is exothermic?

Accepted Answer

Forming ion-dipole interactions between Na+ and Cl- ions and water molecules.

Question 7

Which equation correctly represents the relationship for molarity ($$M$$)?

Accepted Answer

$$M = \frac{	ext{amount\;solute\;(in\;mol)}}{	ext{volume\;solution\;(in\;L)}}$$

Question 8

A solution is prepared by dissolving 25.0 g of a solute (molar mass = 50.0 g/mol) in 100.0 g of solvent. What is the molality ($$m) of $$the solution?

Accepted Answer

$$m = 0.5\;	ext{mol/kg}$$

Question 9

Which of the following best describes a saturated solution?

Accepted Answer

A solution in which the rate of dissolution equals the rate of crystallization.

Question 10

Which law describes the relationship between the solubility of a gas in a liquid and the pressure of the gas above the liquid?

Accepted Answer

Henry's Law

Question 11

Which equation represents Henry's Law for the solubility of a gas?

Accepted Answer

$$C = k_P \cdot P_{	ext{gas}}$$

Question 12

Which of the following is a colligative property?

Accepted Answer

Boiling point elevation

Question 13

What is the effect of adding a nonvolatile solute to a solvent on the vapor pressure of the solution?

Accepted Answer

The vapor pressure decreases.

Question 14

Which equation correctly expresses Raoult's Law for a solution with a nonvolatile solute?

Accepted Answer

$$P_{	ext{solution}} = X_{	ext{solvent}} \cdot P$$^{\circ}$$_{	ext{solvent}}$$

Question 15

A solution is made by dissolving 1.0 mol of NaCl in 1.0 kg of water. If the van't Hoff factor ($$i) $$for NaCl is 1.9, what is the expected freezing point depression ($$\Delta T_f) $$given $$K_f = 1.86\;	ext{°C kg/mol}$$?

Accepted Answer

$$\Delta T_f = 3.53\;	ext{°C}$$

Question 16

Which equation gives the osmotic pressure ($$\Pi) of a $$solution?

Accepted Answer

$$\Pi = MRT$$

Question 17

What happens to a cell placed in a hyperosmotic solution?

Accepted Answer

Water flows out of the cell, causing it to shrivel.

Question 18

Which of the following best explains why drinking seawater is dangerous for humans?

Accepted Answer

Seawater is hyperosmotic compared to body fluids, causing cells to lose water and dehydrate.

Question 19

Which statement about colloids is correct?

Accepted Answer

Colloids are heterogeneous mixtures that scatter light (Tyndall effect).

Solutions: Structure, Properties, and Types

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