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

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

Question 1

Which of the following best describes the process of hydration in the dissolution of an ionic solid in water?

Accepted Answer

The attraction between water molecules and the ions of the solid, resulting in the ions being surrounded and stabilized by water molecules.

Question 2

A solution is prepared by dissolving 10.0 g of NaCl in 100.0 g of water. Which term best describes this solution?

Accepted Answer

Unsaturated

Question 3

Which equation correctly represents the relationship between molarity $(M)$, moles of solute $(n)$, and volume of solution $(V)$ in liters?

Accepted Answer

$$ M = \frac{n}{V} $$

Question 4

Which of the following statements about colligative properties is correct?

Accepted Answer

They depend only on the number of solute particles present.

Question 5

A student needs to prepare 250 mL of a 0.100 M NaCl solution from a 1.00 M stock solution. What volume of the stock solution should be used?

Accepted Answer

$$ 25.0 	ext{ mL} $$

Question 6

Which of the following best explains why the vapor pressure of a solution is lower than that of a pure solvent?

Accepted Answer

The solute particles increase the entropy of the system, reducing the tendency of solvent molecules to escape into the vapor phase.

Question 7

Which of the following is an example of an exothermic dissolution process?

Accepted Answer

Dissolving NaOH in water

Question 8

Which of the following equations correctly represents Raoult's Law for the vapor pressure of a solution?

Accepted Answer

$$ P_{solution} = X_{solvent} P^0_{solvent} $$

Question 9

A solution is made by dissolving 1.00 mol of glucose (a non-electrolyte) in 1.00 kg of water. What is the expected van't Hoff factor $(i)$ for this solution?

Accepted Answer

$$ i = 1 $$

Question 10

Which of the following best describes the effect of increasing temperature on the solubility of most solid solutes in water?

Accepted Answer

Solubility increases

Question 11

Which of the following is a correct statement about the entropy change $(\Delta S)$ during the dissolution of a solid in a solvent?

Accepted Answer

$$ \Delta S $$ is usually positive because the system becomes more disordered.

Question 12

A 0.10 m aqueous solution of NaCl has a lower freezing point than pure water. Which equation describes this phenomenon?

Accepted Answer

$$ \Delta T_f = i K_f m $$

Question 13

Which of the following is NOT a colligative property?

Accepted Answer

Enthalpy of solution

Question 14

Which of the following best describes a supersaturated solution?

Accepted Answer

A solution that contains more solute than is present in a saturated solution at a given temperature.

Question 15

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

Accepted Answer

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

Question 16

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

Accepted Answer

Oil is nonpolar and water is polar, so the intermolecular forces between them are weak.

Question 17

Which of the following is a practical example of reverse osmosis?

Accepted Answer

Desalination of seawater to produce drinking water.

Question 18

Which of the following equations is used to calculate the osmotic pressure $(\Pi)$ of a dilute solution?

Accepted Answer

$$ \Pi = iMRT $$

Question 19

A solution is prepared by mixing 50.0 mL of 0.20 M HCl with 50.0 mL of 0.20 M NaOH. What is the pH of the resulting solution?

Accepted Answer

7

Question 20

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.

Solutions: Chapter 14

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