Q: Which of the following is the correct formula for calculating mass percent of a solute in a solution?

$$\text{Mass percent} = \frac{\text{mass of solute}}{\text{mass of solution}} \times 100\%$$

Question 1

Which of the following best describes a homogeneous mixture?

Accepted Answer

A mixture that is uniform in composition throughout, such as salt water.

Question 2

When NaCl dissolves in water, which type of interaction is primarily responsible for the dissolution process?

Accepted Answer

Solvent–solute attraction

Question 3

According to the solubility graph, which salt shows the greatest increase in solubility as temperature rises from 0°C to 100°C?

Accepted Answer

KNO3

Question 4

A solution is prepared by dissolving 15.5 g of NaCl in enough water to make 1.50 L of solution. What is the molarity of the solution? (Molar mass of NaCl = 58.44 g/mol)

Accepted Answer

$$0.177\ M$$

Question 5

Which of the following statements about saturated solutions is correct?

Accepted Answer

A saturated solution contains the maximum amount of solute that can dissolve under the given conditions.

Question 6

What is the effect of increasing temperature on the solubility of most solid solutes in water?

Accepted Answer

Solubility increases with increasing temperature.

Question 7

Why does warm soda pop fizz more than cold soda pop when opened?

Accepted Answer

The solubility of carbon dioxide gas decreases with temperature.

Question 8

According to Henry’s law, what happens to the solubility of a gas in a liquid as the pressure of the gas above the liquid increases?

Accepted Answer

The solubility increases.

Question 9

How many grams of sucrose ($$C_{12}H$$_{22}$$O_{11}$, molar mass = 342.34 g/mol) are contained in 1.72 L of a 0.758 M sucrose solution?

Accepted Answer

$$446\ g$$

Question 10

Which equation is used to calculate the volume of stock solution needed to prepare a diluted solution?

Accepted Answer

$$M_1V_1 = M_2V_2$$

Question 11

A chemist wants to prepare 5.00 L of a 1.50 M KCl solution from a 12.0 M stock solution. What volume of the stock solution is required?

Accepted Answer

$$0.625\ L$$

Question 12

In a reaction between $$H_2SO_4$$ and $$NaOH$$, how much 0.125 M NaOH solution is needed to completely neutralize 0.225 L of 0.175 M $$H_2SO_4$$ solution? (Reaction: $$H_2SO_4(aq) + 2 NaOH(aq) \rightarrow Na_2SO_4(aq) + 2 H_2O(l))$$

Accepted Answer

$$0.630\ L$$

Question 13

Which of the following is a colligative property?

Accepted Answer

Boiling point elevation

Question 14

What is the freezing point of a 1.7 m ethylene glycol solution? ($$K_f$$ for water = $$1.86\ ^\circ C\cdot kg/mol$$; freezing point of pure water = $$0.00\ ^\circ C)$$

Accepted Answer

$$-3.2\ ^\circ C$$

Question 15

A solution is made by dissolving a nonvolatile solute in water. What happens to the boiling point of the solution compared to pure water?

Accepted Answer

It increases.

Question 16

Which formula is used to calculate the change in boiling point for a solution?

Accepted Answer

$$\Delta T_b = m 	imes K_b$$

Question 17

What is osmosis?

Accepted Answer

The net flow of water across a semi-permeable membrane from a dilute solution (or pure water) to a more concentrated solute solution.

Question 18

Which of the following best explains why fish are more likely to die in warm water than in cold water?

Accepted Answer

Warm water contains less dissolved oxygen.

Question 19

Which of the following is the correct formula for calculating mass percent of a solute in a solution?

Accepted Answer

$$	ext{Mass percent} = \frac{	ext{mass of solute}}{	ext{mass of solution}} 	imes 100\%$$

Chapter 13: Solutions – Properties, Preparation, and Calculations

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