Q: Which of the following equations correctly relates the vapor pressure lowering ($\Delta P$) to the mole fraction of solute ($X_{\text{solute}}$) and the vapor pressure of pure solvent ($P^0_{\text{solvent}}$)?

$\Delta P = X_{\text{solute}} P^0_{\text{solvent}}$

Q: Which of the following is the correct formula for calculating the mass of a single particle in a unit cell?

$\text{mass of one particle} = \dfrac{\text{molar mass}}{N_A}$

Question 1

Which of the following best describes the type of crystalline solid formed by sodium chloride (NaCl)?

Accepted Answer

Ionic solid

Question 2

A face-centered cubic (FCC) unit cell of silver has an edge length of $4.09\ 	ext{\AA}$ and contains 4 atoms per unit cell. If the molar mass of silver is $107.87\ 	ext{g/mol}$, what is the density of silver in $	ext{g/cm}^3$? ($1\ 	ext{cm} = 10^8\ 	ext{\AA}$, $N_A = 6.022 	imes 10^{23}\ 	ext{mol}^{-1}$)

Accepted Answer

$10.5\ 	ext{g/cm}^3$

Question 3

Which of the following statements about the energetics of solution formation is correct?

Accepted Answer

The process can be either endothermic or exothermic depending on the relative magnitudes of lattice energy and hydration energy.

Question 4

A solution is prepared by dissolving $10.0\ 	ext{g}$ of glucose ($C_6H_{12}O_6$, molar mass $180\ 	ext{g/mol}$) in $90.0\ 	ext{g}$ of water. What is the mole fraction of glucose in the solution?

Accepted Answer

$0.055$

Question 5

Which of the following best explains why the solubility of gases in water decreases as temperature increases?

Accepted Answer

Gas molecules have higher kinetic energy and escape from the solution more easily.

Question 6

Which of the following is a correct expression for the osmotic pressure ($\pi$) of a dilute solution at temperature $T$?

Accepted Answer

$\pi = iMRT$

Question 7

Which of the following substances is most likely to form a molecular crystalline solid?

Accepted Answer

CO$_2$

Question 8

A solution is made by dissolving $0.50\ 	ext{mol}$ of NaCl in $1.0\ 	ext{kg}$ of water. If the van't Hoff factor ($i$) for NaCl is $2$, and $K_f$ for water is $1.86\ ^\circ	ext{C}\cdot	ext{kg/mol}$, what is the freezing point of the solution?

Accepted Answer

$-1.86\ ^\circ	ext{C}$

Question 9

Which of the following best describes addition polymerization?

Accepted Answer

Monomers with double bonds react to form long chains without the loss of small molecules.

Question 10

A body-centered cubic (BCC) unit cell contains how many atoms per unit cell?

Accepted Answer

2

Question 11

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

Accepted Answer

Increasing the partial pressure of the gas above the solution

Question 12

A solution is prepared by dissolving $5.00\ 	ext{g}$ of KNO$_3$ (molar mass $101\ 	ext{g/mol}$) in enough water to make $250.0\ 	ext{mL}$ of solution. What is the molarity of the solution?

Accepted Answer

$0.198\ 	ext{M}$

Question 13

Which of the following is NOT a colligative property?

Accepted Answer

Color

Question 14

Which of the following equations correctly relates the vapor pressure lowering ($\Delta P$) to the mole fraction of solute ($X_{	ext{solute}}$) and the vapor pressure of pure solvent ($P^0_{	ext{solvent}}$)?

Accepted Answer

$\Delta P = X_{	ext{solute}} P^0_{	ext{solvent}}$

Question 15

Which of the following best explains why NaCl dissolves in water but not in hexane ($C_6H_{14}$)?

Accepted Answer

Water can stabilize Na$^+$ and Cl$^-$ ions through ion-dipole interactions, but hexane cannot.

Question 16

A sample of a crystalline solid is hard, has a high melting point, and does not conduct electricity in the solid state but does conduct when melted. What type of solid is it most likely to be?

Accepted Answer

Ionic solid

Question 17

Which of the following is the correct formula for calculating the mass of a single particle in a unit cell?

Accepted Answer

$	ext{mass of one particle} = \dfrac{	ext{molar mass}}{N_A}$

Question 18

A solution is made by dissolving $20.0\ 	ext{g}$ of NaOH (molar mass $40.0\ 	ext{g/mol}$) in $180.0\ 	ext{g}$ of water. What is the percent by mass of NaOH in the solution?

Accepted Answer

$10.0\%$

Question 19

Which of the following statements about the effect of temperature on the solubility of solids and gases in water is correct?

Accepted Answer

The solubility of most solids increases with increasing temperature, while the solubility of gases decreases.

Question 20

Which of the following is a property of atomic (metallic) crystalline solids?

Accepted Answer

They conduct electricity in the solid state.

Chapter 13 & 14 Study Guide: Solids, Solutions, and Colligative Properties

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