Question 1

Which of the following best describes a saturated solution of NaCl at 25 °C?

Accepted Answer

A solution in which no more NaCl can dissolve and undissolved NaCl is in dynamic equilibrium with dissolved NaCl.

Question 2

If you add more solid NaCl to a saturated solution of NaCl at constant temperature, what will happen to the concentration of dissolved NaCl?

Accepted Answer

The concentration will remain the same because the solution is already saturated.

Question 3

Which of the following changes will increase the concentration of a saturated solution of NaCl?

Accepted Answer

Increasing the temperature of the solution.

Question 4

A solution contains 40 g of NaCl in 100 mL of water at 25 °C. What type of solution is this?

Accepted Answer

Supersaturated

Question 5

Which of the following pairs is most likely to be miscible?

Accepted Answer

Ethanol (C2H5OH) and water

Question 6

Why are vitamins A, D, E, and K not soluble in water?

Accepted Answer

They are largely nonpolar molecules and water is a polar solvent.

Question 7

According to Henry’s Law, what is the relationship between the solubility of a gas ($$S_g) $$and the pressure of the gas ($$P_g) $$above the solution?

Accepted Answer

$$S_g = kP_g$$

Question 8

At 20 °C and 1 atm, the Henry’s Law constant for O$$_2 is$$ $$1.4 	imes 10$$^{-3}$$ mol/L·atm. What is the equilibrium concentration of dissolved O_2$ in water under these conditions?

Accepted Answer

$$1.4 	imes 10$$^{-3}$$ mol/L

Question 9

Which of the following statements best explains why the solubility of gases in water decreases with increasing temperature?

Accepted Answer

The entropy of the gas phase is much greater than that of the dissolved state, so higher temperatures favor the gas phase.

Question 10

Which of the following best describes the effect of increasing pressure on the solubility of CO$$_2 in a $$sealed bottle of soda?

Accepted Answer

The solubility of CO$$_2$$ increases as pressure increases.

Question 11

Which of the following compounds will be miscible with water?

Accepted Answer

Both 1-butanol and ethanol

Question 12

A student prepares a solution by dissolving 15 mg of riboflavin (vitamin B2) in 100 mL of water. Based on its solubility, what type of solution is this?

Accepted Answer

Saturated

Question 13

Which of the following best explains why hexane (C6H14) does not dissolve in water?

Accepted Answer

Hexane is nonpolar and water is polar, so there are no favorable interactions.

Question 14

Which of the following vitamins would you expect to be stored in fatty tissue rather than excreted in urine?

Accepted Answer

Vitamin A

Question 15

A solution contains dissolved sodium acetate at a concentration greater than its solubility at a given temperature. What will happen if a seed crystal of sodium acetate is added?

Accepted Answer

Excess sodium acetate will crystallize out until the solution is saturated.

Question 16

Which of the following best describes the phrase 'like dissolves like'?

Accepted Answer

Polar solutes dissolve in polar solvents, and nonpolar solutes dissolve in nonpolar solvents.

Question 17

Which of the following would increase the solubility of a solid solute in water?

Accepted Answer

Increasing the temperature of the solution.

Question 18

A sealed bottle of soda is opened and left at room temperature. What will happen to the concentration of dissolved CO$$_2$$ over time?

Accepted Answer

It will decrease as CO$$_2$$ escapes into the air.

Question 19

Which of the following gases has the highest solubility in water at 20 °C and 1 atm?

Accepted Answer

CO$$_2$$

Saturated Solutions, Solubility, and Factors Affecting Solubility

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