Question 1

Which of the following best explains why NaCl dissolves readily in water but not in hexane (C6H14)?

Accepted Answer

NaCl forms ion-dipole interactions with water, but only weak dispersion forces with hexane.

Question 2

A solution is prepared by dissolving 43.0 g of KClO3 in enough water to make 100.0 mL of solution. If the density of the solution is 1.76 g/mL, what is the molality of KClO3 in the solution? (Molar mass KClO3 = 122.55 g/mol)

Accepted Answer

$3.51\ \mathrm{m}$

Question 3

Which of the following solutes will most readily dissolve in water?

Accepted Answer

HOCH2CH2OH

Question 4

A 2.4 L sample of an aqueous solution contains 0.012 mL of NH3. What is the concentration of NH3 in the solution, expressed as parts per billion (ppb)?

Accepted Answer

$5000\ \mathrm{ppb}$

Question 5

Which of the following statements about colligative properties is correct?

Accepted Answer

Adding a solute to a solvent raises the boiling point and lowers the freezing point.

Question 6

Calculate the mole fraction of citric acid in a 2.4 m aqueous solution of citric acid (C6H8O7). (Molar mass of citric acid = 192.12 g/mol)

Accepted Answer

$0.041$

Question 7

A solution was prepared by dissolving 51.0 g of KBr in 310 mL of water. Calculate the mass percent of KBr in the solution. (Density of water = 1.00 g/mL)

Accepted Answer

$14.1\%$

Question 8

Which of the following best describes a supersaturated solution?

Accepted Answer

A solution that contains more dissolved solute than the equilibrium concentration at a given temperature.

Question 9

The solubility of O2 in water at 25°C is 1.2 mM. Based on the trend for nonpolar gases, what is the most likely solubility value of F2 in water at 25°C?

Accepted Answer

$0.01\ \mathrm{mM}$

Question 10

Which of the following compounds will have the largest value for the van’t Hoff factor ($i$)?

Accepted Answer

AlCl3

Question 11

A red blood cell placed in pure water will swell because:

Accepted Answer

The osmotic pressure is greater in the cell than in the water.

Question 12

Which of the following best describes the direction of water flow between two solutions separated by a semipermeable membrane, where Solution A has a lower solute concentration than Solution B?

Accepted Answer

Water will flow from Solution A to Solution B due to higher osmotic pressure on Solution B.

Question 13

Which of the following compounds will have the highest boiling point when dissolved in water?

Accepted Answer

0.25 M NH4NO3

Question 14

A solution contains 24.8 g of sucrose (C12H22O11) dissolved in 550.0 g of water. Calculate the molality of the solution. (Molar mass of sucrose = 342.3 g/mol)

Accepted Answer

$0.13\ \mathrm{m}$

Question 15

Which of the following is true for the solubility of KBr (s) and CH3(CH2)3CH3 (g) in water?

Accepted Answer

Decreasing the temperature will decrease the solubility of CH3(CH2)3CH3.

Question 16

Which type of intermolecular force is most important for the solvation of methanol (CH3OH) in ethanol (CH3CH2OH)?

Accepted Answer

Hydrogen bonding

Question 17

A solution is prepared by dissolving 0.400 moles of Pb(NO3)4 in 750.0 g of water. What is the osmolality of total ions in the solution?

Accepted Answer

$2.67\ \mathrm{m}$

Question 18

Which of the following best describes a hypotonic solution relative to a red blood cell?

Accepted Answer

It has a lower solute concentration and lower osmotic pressure than the cell.

Question 19

Which of the following is the correct formula for calculating the change in boiling point ($\Delta T_b$) of a solution?

Accepted Answer

$\Delta T_b = i \cdot K_b \cdot m$

Ch.13 - Solutions: Properties, Concentrations, and Colligative Effects

Study Guide - Practice Questions

Study Guide - Flashcards