$$0.50\,L \times \frac{8.8\,mEq}{1\,L} \times \frac{1\,Eq}{1000\,mEq} \times \frac{1\,mol}{2\,Eq} = 0.0022\,mol$$

Question 1

Which of the following best describes a solution?

Accepted Answer

A homogeneous mixture of two or more substances

Question 2

A nurse is preparing an intravenous (IV) solution for a patient. Why is it important that the IV solution is isotonic with blood plasma?

Accepted Answer

To prevent water from leaving or entering the blood cells excessively

Question 3

Which of the following compounds will NOT dissolve in water? Explain why.

Accepted Answer

Gasoline, because it is nonpolar

Question 4

When NaCl dissolves in water, what happens at the molecular level?

Accepted Answer

Na+ ions are attracted to the oxygen atoms of water, and Cl− ions are attracted to the hydrogen atoms of water

Question 5

Which of the following equations correctly represents the dissociation of K2CrO4, a strong electrolyte, in water?

Accepted Answer

$$K_2CrO_4(s) \rightarrow 2K^+(aq) + $$CrO_4$$^{2-}(aq)$$

Question 6

A solution is prepared by mixing 15.0 g of Na2CO3 and 235 g of H2O. What is the mass percent (% m/m) of Na2CO3 in the solution?

Accepted Answer

6.00%

Question 7

Which of the following best explains why fish die in water that is too warm?

Accepted Answer

The solubility of oxygen gas decreases as temperature increases

Question 8

A patient’s blood calcium level is 8.8 mEq/L. How many moles of Ca2+ are in 0.50 L of blood? (1 Eq Ca2+ = 2 moles Ca2+)

Accepted Answer

$$0.50\,L 	imes \frac{8.8\,mEq}{1\,L} 	imes \frac{1\,Eq}{1000\,mEq} 	imes \frac{1\,mol}{2\,Eq} = 0.0022\,mol$$

Question 9

Which of the following mixtures is a colloid?

Accepted Answer

A mixture with medium-sized particles that do not settle and can be separated by semipermeable membranes

Question 10

A red blood cell is placed in a 2% NaCl solution. What will happen to the cell?

Accepted Answer

It will undergo crenation

Question 11

Which of the following best describes the process of osmosis?

Accepted Answer

Water moves from a lower to a higher solute concentration through a semipermeable membrane

Question 12

Which of the following is a correct statement about the effect of temperature on solubility?

Accepted Answer

The solubility of most solids increases as temperature increases

Question 13

Which of the following equations correctly expresses mass percent (m/m)?

Accepted Answer

$$	ext{mass percent (m/m)} = \frac{	ext{g of solute}}{	ext{g of solute} + 	ext{g of solvent}} 	imes 100\%$$

Question 14

A solution contains 5.0 g of KI in 250 mL of solution. What is the mass/volume percent (% m/v) of KI?

Accepted Answer

$$\frac{5.0\,g}{250\,mL} 	imes 100\% = 2.0\%$$

Question 15

Which of the following best describes a saturated solution?

Accepted Answer

A solution that contains the maximum amount of solute and has undissolved solute at the bottom

Question 16

Which of the following is a strong electrolyte?

Accepted Answer

NaCl

Question 17

A mixture that has solute particles that do not settle out but are too large to pass through a semipermeable membrane is called a _______.

Accepted Answer

colloid

Question 18

Which of the following best explains why a bottle of carbonated drink may burst when left in the hot sun?

Accepted Answer

The solubility of CO2 decreases with temperature, causing gas to leave solution and increase pressure

Question 19

Which of the following is true about the charge balance in blood plasma?

Accepted Answer

The total number of positive charges is equal to the total number of negative charges

Chapter 9: Solutions – Structure, Properties, and Biological Relevance

Study Guide - Practice Questions