Question 1

Which of the following best describes a colloid?

Accepted Answer

A homogeneous mixture with particles ranging from 2 to 500 nm in diameter.

Question 2

A nurse needs to prepare 250 mL of a 2.0% (m/v) saline solution for a patient. How many grams of NaCl are required?

Accepted Answer

Question 3

Which of the following pairs of substances is most likely to form a solution?

Accepted Answer

Hexane and carbon tetrachloride

Question 4

A solution is prepared by dissolving 1.8 g of heparin sodium in enough water to make 15 mL of solution. What is the (m/v)% concentration of heparin sodium?

Accepted Answer

$$12\%$$

Question 5

Which statement best explains why the solubility of gases in water decreases as temperature increases?

Accepted Answer

Increased temperature gives gas molecules more kinetic energy, making them more likely to escape from the solution.

Question 6

A 0.75 mol sample of KBr is dissolved in 1.0 kg of water. What is the boiling point of the resulting solution? (Assume normal boiling point of water is $$100^\circ	ext{C}$$ and $$\Delta T_b = 0.51^\circ	ext{C}$$ per mole of particles per kg water.)

Accepted Answer

$$100.77^\circ	ext{C}$$

Question 7

Which of the following best describes a strong electrolyte?

Accepted Answer

A substance that ionizes completely in water, producing a solution that conducts electricity well.

Question 8

A 5.0% (m/v) glucose solution is commonly used intravenously. If the molar mass of glucose is $$180 	ext{ g/mol}$$, what is the osmolarity of this solution?

Accepted Answer

$$0.28 	ext{ osmol/L}$$

Question 9

A solution is prepared by diluting 75 mL of a 3.5 M glucose solution to a final volume of 450 mL. What is the final concentration?

Accepted Answer

$$0.58 	ext{ M}$$

Question 10

Which of the following statements about osmosis is correct?

Accepted Answer

Osmosis is the movement of solvent molecules through a semipermeable membrane from a region of lower solute concentration to higher solute concentration.

Question 11

A patient receives an intravenous solution that is hypertonic relative to their blood plasma. What is the most likely effect on their red blood cells?

Accepted Answer

Water will leave the cells, causing them to shrink (crenate).

Question 12

According to Henry’s Law, what happens to the solubility of a gas in a liquid if the partial pressure of the gas above the liquid is doubled (at constant temperature)?

Accepted Answer

The solubility of the gas doubles.

Question 13

A solution is made by dissolving 2.355 g of $$\mathrm{H_2SO_4} in $$water and diluting to a final volume of 50.0 mL. The molar mass of $$\mathrm{H_2SO_4} is$$ $$98.1 	ext{ g/mol}. $$What is the molarity of the solution?

Accepted Answer

$$0.480 	ext{ M}$$

Question 14

Which of the following is a colligative property of solutions?

Accepted Answer

Boiling point elevation

Question 15

A 1.0 M NaCl solution is to be diluted to prepare 750 mL of 0.32 M NaOH. What volume of the 1.0 M NaOH solution is needed?

Accepted Answer

$$240 	ext{ mL}$$

Question 16

Which of the following best describes the process of dialysis as used in hemodialysis?

Accepted Answer

Small waste molecules pass through a semipermeable membrane, while larger molecules like proteins remain in the blood.

Question 17

A solution contains 0.065 M ethyl alcohol ($$\mathrm{C_2H_5OH}) in 5.6 L of $$blood. The molar mass of ethyl alcohol is $$46.0 	ext{ g/mol}. $$What is the total mass of alcohol in the blood?

Accepted Answer

$$17 	ext{ g}$$

Question 18

Which of the following statements about the freezing point of a solution is correct?

Accepted Answer

The freezing point of a solution is lower than that of the pure solvent.

Question 19

A solution is prepared by dissolving NaCl in water to make 1.50 L of a 0.300 osmol/L solution. The molar mass of NaCl is $$58.44 	ext{ g/mol}. $$What mass of NaCl is needed?

Accepted Answer

$$13.1 	ext{ g}$$

Chapter 9: Solutions – Study Notes for GOB Chemistry

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