Question 1

Which of the following best describes the mixture shown in the first image (oil and water in a glass)?

Accepted Answer

A suspension

Question 2

Which of the following is the major intermolecular force between acetone and chloroform?

Accepted Answer

hydrogen bonding

Question 3

Which compound will be most soluble in water ($$\mathrm{H_2O}$$)?

Accepted Answer

ethylene glycol ($$\mathrm{HOCH_2CH_2OH})$$

Question 4

The structure shown in the sixth image is Vitamin C. Based on its structure, is Vitamin C water-soluble or fat-soluble?

Accepted Answer

Water-soluble, because it has many polar $$\mathrm{OH}$$ groups

Question 5

Which of the following best explains why oil and water do not mix?

Accepted Answer

Oil is nonpolar and water is polar

Question 6

Which of the following statements about solubility is correct?

Accepted Answer

The solubility of most solids in water increases with increasing temperature.

Question 7

According to Henry’s Law, what is the solubility of methyl bromide ($$\mathrm{CH_3Br}) in $$water at 25°C and a partial pressure of 280 mm Hg? ($$k = 0.159\ \mathrm{mol/(L\cdot atm)})$$

Accepted Answer

$$0.417\ \mathrm{mol/L}$$

Question 8

Which of the following best describes the process of osmosis as shown in the diagram?

Accepted Answer

Solvent moves from low to high solute concentration through a semipermeable membrane

Question 9

Which of the following solutions would have the highest boiling point elevation?

Accepted Answer

0.50 M NaCl (strong electrolyte)

Question 10

A solution is prepared by dissolving 50.0 g of sucrose ($$\mathrm{C$$_{12}$$H_{22}O$$_{11}}$) in 250. g of water at 25°C. If the vapor pressure of pure water at 25°C is 23.76 mm Hg, what is the vapor pressure of the solution? (Molar mass of sucrose = 342 g/mol)

Accepted Answer

22.9 mm Hg

Question 11

Which of the following best describes a colloid?

Accepted Answer

A heterogeneous mixture with particles that do not settle out and cannot pass through a semipermeable membrane

Question 12

Which of the following is a correct application of the 'like dissolves like' rule?

Accepted Answer

Polar solutes are more soluble in polar solvents

Question 13

Which of the following best explains why the vapor pressure of a solvent decreases when a nonvolatile solute is added?

Accepted Answer

The solute decreases the rate of vaporization by occupying surface sites

Question 14

A solution contains 0.10 moles of $$\mathrm{$$MgCl_2$$} in 750 mL of $$water. What is the freezing point depression? ($$K_f$$ for water = $$1.86\ ^\circ\mathrm{C}/m$$, use the theoretical van’t Hoff factor for $$\mathrm{$$MgCl_2$$})$$

Accepted Answer

$$-0.99\ ^\circ\mathrm{C}$$

Question 15

Which of the following best describes the effect of temperature on the solubility of gases in water?

Accepted Answer

Solubility decreases with increasing temperature

Question 16

Which of the following is true about the van’t Hoff factor ($$i) $$for strong electrolytes?

Accepted Answer

It is usually less than the theoretical value due to ion pairing

Question 17

Which of the following best describes the process of recrystallization?

Accepted Answer

Dissolving a solid in a hot solvent and then cooling the solution slowly

Question 18

Which of the following is the correct formula for calculating the molality ($$m) of a $$solution?

Accepted Answer

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

Question 19

Which of the following best describes the effect of adding a solute to a solvent on the freezing point of the solution?

Accepted Answer

The freezing point decreases

General Chemistry Study Guidance: Solutions, Solubility, and Intermolecular Forces

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