Question 1

Which of the following intermolecular forces is primarily responsible for the solubility of sodium chloride (NaCl) in water?

Accepted Answer

Ion-dipole interactions between Na\^+ and H\_2O

Question 2

Which factor would most likely increase the solubility of a gas in a liquid?

Accepted Answer

Increasing the partial pressure of the gas above the liquid

Question 3

Which of the following best describes the energy changes during the solution process?

Accepted Answer

Energy is released when solute-solvent interactions form.

Question 4

Given the partial pressure of argon in air is 9.85 mmHg and $$k = 1.4 	imes 10$$^{-3}$$ mol/L·atm, what is the concentration of argon gas dissolved in water? (1 atm = 760 mmHg)

Accepted Answer

$$1.8 	imes 10$$^{-5}$$ mol/L

Question 5

A fish tank is bubbled with air at 1.34 atm. The air contains 336 g O\_2 and 1107 g N\_2. If $$k_{O_2$} = 1.3 	imes 10$$^{-3}$$ mol/L·atm, what is the molarity of dissolved O\_2? (Molar mass O\_2 = 32.0 g/mol, N\_2 = 28.0 g/mol)

Accepted Answer

$$0.0016$$ mol/L

Question 6

Which equation correctly expresses Raoult's Law for calculating the vapor pressure of a solution?

Accepted Answer

$$P_{solution} = X_{solvent} \cdot P^0$_{solvent}$$

Question 7

How many grams of sucrose ($$C_{12}H$$_{22}$$O_{11}$, molar mass = 342 g/mol) must be added to 500.0 g of water to lower the vapor pressure from 23.8 mmHg to 23.4 mmHg at 25°C? (Assume ideal solution behavior)

Accepted Answer

Approximately 146 g

Question 8

What is the boiling point of a solution made by adding 23.5 g of glucose ($$C_6H_{12}O_6$, molar mass = 180 g/mol) to 325 mL of water? (K_b = 0.52$ °C/m, density of water = 1.00 g/mL)

Accepted Answer

100.22 °C

Question 9

A solution is made by dissolving 167 g of NaCl (molar mass = 58.5 g/mol) in 1500 g of ice. What is the expected freezing point of the mixture? ($$K_f = 1.86$$ °C/m, $$i = 2$$ for NaCl)

Accepted Answer

-3.56 °C

Question 10

If 25.0 g of an unknown molecular solute lowers the freezing point of 343 g of water to -4.56°C ($$K_f = 1.86$$ °C/m), what is the molar mass of the solute?

Accepted Answer

150 g/mol

Question 11

What is the osmotic pressure of a 750.0 mL solution containing 34.5 g of glucose ($$C_6H_{12}O_6$, molar mass = 180 g/mol) at 27.6°C? (R = 0.0821$ L·atm/mol·K)

Accepted Answer

3.8 atm

Question 12

A 500.0 mL solution contains 24.5 g of a molecular solute and has an osmotic pressure of 16.7 atm at 30.0°C. What is the molar mass of the solute? ($$R = 0.0821 L$$·atm/mol·K)

Accepted Answer

98 g/mol

Question 13

A 0.453 M solution of an unknown ionic salt X\_3Y has an osmotic pressure of 40.2 atm at 26.1°C. What is the van’t Hoff factor ($$i) $$for this salt? ($$R = 0.0821 L$$·atm/mol·K)

Accepted Answer

3.7

Question 14

What is the freezing point of a 250.0 mL sample of ethanol (density = 0.789 g/mL, $$K_{fp} = 1.99$$ °C/m, freezing point = -114.6°C) with 34.5 g of NaCl (molar mass = 58.5 g/mol) dissolved in it? ($$i = 2$$ for NaCl)

Accepted Answer

-116.2 °C

Question 15

Which of the following best explains how the wood frog survives hibernation in freezing temperatures?

Accepted Answer

It increases the concentration of glucose in its cells, lowering the freezing point of its body fluids.

Question 16

Which of the following statements about colligative properties is correct?

Accepted Answer

They depend only on the number of solute particles present.

Question 17

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

Accepted Answer

$$\Pi = iMRT$$

Question 18

Which of the following would NOT increase the boiling point of water?

Accepted Answer

Decreasing atmospheric pressure

Question 19

A solution is prepared by dissolving a nonvolatile solute in water. Which of the following is a correct consequence?

Accepted Answer

The boiling point of the solution increases.

General Chemistry II: Solutions, Colligative Properties, and Intermolecular Forces Study Guide

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