Question 1

Which of the following best describes the process of solution formation for an ionic compound in water?

Accepted Answer

The solute particles are separated, the solvent particles are separated, and then the solute and solvent particles mix.

Question 2

Which of the following statements about solubility is correct?

Accepted Answer

The solubility of most solids in water increases as temperature increases.

Question 3

A solution is prepared by dissolving 25.0 g of a solute (molar mass = 25.0 g/mol) in 100.0 g of solvent. What is the molality of the solution?

Accepted Answer

$10.0\ \mathrm{m}$

Question 4

Which of the following compounds will be most soluble in water ($\mathrm{H_2O}$)?

Accepted Answer

ethylene glycol ($\mathrm{HOCH_2CH_2OH}$)

Question 5

Which of the following vitamins is most likely to be water soluble?

Accepted Answer

A vitamin with many hydroxyl ($-OH$) groups and few hydrocarbon chains.

Question 6

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

Accepted Answer

Oil is nonpolar and water is polar, so their intermolecular forces are not compatible.

Question 7

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

Accepted Answer

hydrogen bonding

Question 8

A solution is prepared by dissolving 29.0 g of $\mathrm{H_3PO_4}$ in enough water to make 500.0 mL of solution. What is the molarity of the solution? ($\mathrm{M_{H_3PO_4}} = 98.0\ \mathrm{g/mol}$)

Accepted Answer

$0.591\ \mathrm{M}$

Question 9

Which of the following statements about colligative properties is true?

Accepted Answer

Colligative properties depend only on the number of solute particles, not their identity.

Question 10

What is the vapor pressure of a solution in which the mole fraction of the solute is $0.200$ and the vapor pressure of the pure solvent is $100.0$ torr? (Assume a single nonvolatile, nonelectrolyte solute.)

Accepted Answer

$80.0$ torr

Question 11

A solution contains $478$ g of ethylene glycol ($62.07$ g/mol) in $3202$ g of water. What is the freezing point of the solution? ($K_f$ for water is $1.86\ ^\circ\mathrm{C}/m$)

Accepted Answer

$-4.48\ ^\circ\mathrm{C}$

Question 12

Which of the following best describes the effect of adding a nonvolatile solute to a solvent?

Accepted Answer

The vapor pressure of the solvent decreases.

Question 13

A solution of $6.85$ g of a carbohydrate in $100.0$ g of water has a density of $1.024$ g/mL and an osmotic pressure of $4.61$ atm at $20.0\ ^\circ\mathrm{C}$. What is the molar mass of the carbohydrate? ($R = 0.0821\ \mathrm{L\cdot atm\cdot mol^{-1}\cdot K^{-1}}$)

Accepted Answer

$171\ \mathrm{g/mol}$

Question 14

Which of the following best explains why the measured van’t Hoff factor for an electrolyte is often less than the theoretical value?

Accepted Answer

Ion pairing occurs in solution, reducing the number of effective particles.

Question 15

Which of the following mixtures is a colloid?

Accepted Answer

Milk

Question 16

Which of the following best describes the structure of a soap molecule?

Accepted Answer

A hydrophilic ionic head and a hydrophobic nonpolar tail

Question 17

Which of the following statements about Henry’s Law is correct?

Accepted Answer

The solubility of a gas in a liquid is directly proportional to its partial pressure above the liquid.

Question 18

Which of the following best describes osmosis?

Accepted Answer

The flow of solvent from a solution of low concentration into a solution of high concentration through a semipermeable membrane.

Solubility and Intermolecular Forces: Practice Questions and Guidance

Study Guide - Practice Questions

Study Guide - Flashcards