Q: A face-centered cubic (FCC) unit cell contains 4 particles. If the molar mass of the substance is 60 g/mol, what is the mass of one unit cell? (Use Avogadro’s number $N_A = 6.022 \times 10^{23}$ mol$^{-1}$)

The mass of one unit cell is $\frac{4 \times 60}{6.022 \times 10^{23}}$ g.

Q: Which of the following is a correct expression for freezing point depression?

$\Delta T_f = K_f \times m \times i$

Q: A body-centered cubic (BCC) unit cell contains 2 particles. If the mass of one particle is $1.66 \times 10^{-22}$ g, what is the mass of the unit cell?

Mass $= 2 \times 1.66 \times 10^{-22}$ g

Q: Which formula correctly represents the calculation of molality ($m$) for a solution?

$m = \frac{\text{moles of solute}}{\text{kg of solvent}}$

Q: A solution is made by dissolving 0.5 mol of glucose in 1.0 kg of water. If the freezing point depression constant ($K_f$) for water is $1.86$ °C·kg/mol, what is the expected freezing point depression?

$\Delta T_f = 1.86 \times 0.5 = 0.93$ °C

Question 1

Which of the following best describes the classification of NaCl as a crystalline solid?

Accepted Answer

NaCl is an ionic solid because it is composed of ions held together by electrostatic forces.

Question 2

A face-centered cubic (FCC) unit cell contains 4 particles. If the molar mass of the substance is 60 g/mol, what is the mass of one unit cell? (Use Avogadro’s number $N_A = 6.022 	imes 10^{23}$ mol$^{-1}$)

Accepted Answer

The mass of one unit cell is $\frac{4 	imes 60}{6.022 	imes 10^{23}}$ g.

Question 3

Which property is NOT characteristic of molecular crystalline solids?

Accepted Answer

High melting points

Question 4

A solution is prepared by dissolving 10 g of NaCl (molar mass = 58.44 g/mol) in 100 g of water. What is the mole fraction of NaCl in the solution?

Accepted Answer

Mole fraction $= \frac{10/58.44}{(10/58.44)+(100/18.02)}$

Question 5

Which equation correctly represents the calculation of density for a unit cell?

Accepted Answer

$D = \frac{m}{v}$

Question 6

Which of the following statements about the effect of temperature on solubility is correct?

Accepted Answer

The solubility of gases in water decreases as temperature increases.

Question 7

Which of the following is a correct expression for freezing point depression?

Accepted Answer

$\Delta T_f = K_f 	imes m 	imes i$

Question 8

A body-centered cubic (BCC) unit cell contains 2 particles. If the mass of one particle is $1.66 	imes 10^{-22}$ g, what is the mass of the unit cell?

Accepted Answer

Mass $= 2 	imes 1.66 	imes 10^{-22}$ g

Question 9

Which of the following best explains why ionic solids have high melting points?

Accepted Answer

Because they are composed of ions held together by strong electrostatic forces.

Question 10

Which formula correctly represents the calculation of molality ($m$) for a solution?

Accepted Answer

$m = \frac{	ext{moles of solute}}{	ext{kg of solvent}}$

Question 11

Which of the following is a colligative property?

Accepted Answer

Vapor pressure lowering

Question 12

A solution is made by dissolving 0.5 mol of glucose in 1.0 kg of water. If the freezing point depression constant ($K_f$) for water is $1.86$ °C·kg/mol, what is the expected freezing point depression?

Accepted Answer

$\Delta T_f = 1.86 	imes 0.5 = 0.93$ °C

Question 13

Which of the following best describes addition polymerization?

Accepted Answer

It involves the addition of monomers without the loss of any atoms.

Question 14

Which equation correctly represents osmotic pressure ($\pi$) for a dilute solution?

Accepted Answer

$\pi = MRT$

Question 15

Which factor most strongly affects whether a solute will dissolve in a solvent?

Accepted Answer

The intermolecular forces between solute and solvent

Question 16

A solution contains 0.2 mol of NaCl in 500 mL of water. What is the molarity of the solution?

Accepted Answer

Molarity $= \frac{0.2}{0.5} = 0.4$ M

Question 17

Which of the following is the correct expression for vapor pressure lowering in a solution?

Accepted Answer

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

Question 18

Which of the following best describes the energetics of solution formation?

Accepted Answer

Solution formation involves both endothermic and exothermic steps.

Question 19

A sample of oxygen gas is dissolved in water at 25°C. If the partial pressure of oxygen above the water is doubled, what happens to the solubility of oxygen in water?

Accepted Answer

The solubility doubles.

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

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