Q: A $$75.0\ \mathrm{mL}$$ sample of $$0.0150\ \mathrm{M}$$ KNO$$_3$$ contains how many moles of solute?

$$1.13 \times 10$$^{-3}$$\ \mathrm{mol}$$

Question 1

A hospital pharmacist prepares an intravenous (IV) saline solution by dissolving 0.90 mol of NaCl in enough water to make 1.00 L of solution. What is the molarity of the IV saline solution?

Accepted Answer

$$0.90\ \mathrm{M}$$

Question 2

Which of the following best describes why potassium nitrate (KNO$$_3) is $$classified as an electrolyte when dissolved in water?

Accepted Answer

It dissociates into ions that conduct electricity.

Question 3

A solution is prepared by diluting $$0.200\ \mathrm{L} of$$ $$1.00\ \mathrm{M}$$ HCl to a final volume of $$0.800\ \mathrm{L}. $$What is the final molarity?

Accepted Answer

$$0.25\ \mathrm{M}$$

Question 4

Which of the following mixtures is best classified as a colloid?

Accepted Answer

Milk

Question 5

A student needs to prepare $$250\ \mathrm{mL} of$$ $$0.100\ \mathrm{M}$$ NaOH from a $$1.00\ \mathrm{M}$$ stock solution. What volume of the stock solution should be used?

Accepted Answer

$$25.0\ \mathrm{mL}$$

Question 6

Which of the following statements about suspensions is correct?

Accepted Answer

Suspensions contain large particles that settle out and can be separated by filtration.

Question 7

A solution contains $$0.0250$$ moles of NaCl in $$500\ \mathrm{mL} of $$solution. What is the molarity?

Accepted Answer

$$0.0500\ \mathrm{M}$$

Question 8

Which of the following best explains why a supersaturated solution is unstable?

Accepted Answer

It contains more solute than can be dissolved at the current temperature, so crystals can form easily.

Question 9

A nurse must prepare an IV bag with a glucose concentration of $$0.30\ \mathrm{M}. If $$the stock solution is $$1.20\ \mathrm{M}$$, how much stock solution is needed to make $$500\ \mathrm{mL} of $$the IV bag?

Accepted Answer

$$125\ \mathrm{mL}$$

Question 10

Which of the following is a property of a solution but NOT of a suspension?

Accepted Answer

Particles do not settle and cannot be separated by filtration.

Question 11

A $$0.500\ \mathrm{L}$$ solution contains $$0.200$$ moles of HCl. What is the molarity of the solution?

Accepted Answer

$$0.400\ \mathrm{M}$$

Question 12

Which of the following best describes the difference between a colloid and a solution?

Accepted Answer

Colloids have larger particles that can be separated by semipermeable membranes, while solutions cannot.

Question 13

A student adds $$0.00500$$ moles of NaCl to a beaker and wants a final concentration of $$0.0250\ \mathrm{M}. $$What volume of solution (in mL) should they prepare?

Accepted Answer

$$200\ \mathrm{mL}$$

Question 14

Which of the following is a real-life example of a suspension?

Accepted Answer

Muddy water

Question 15

A $$75.0\ \mathrm{mL}$$ sample of $$0.0150\ \mathrm{M}$$ KNO$$_3$$ contains how many moles of solute?

Accepted Answer

$$1.13 	imes 10$$^{-3}$$\ \mathrm{mol}$$

Question 16

Which of the following best describes the process of dilution?

Accepted Answer

The amount of solute remains the same, but the volume increases and concentration decreases.

Question 17

A solution is classified as unsaturated. What does this mean?

Accepted Answer

More solute can still be dissolved in the solution.

Question 18

Which of the following equations is used to calculate the final concentration after dilution?

Accepted Answer

$$M_1V_1 = M_2V_2$$

Question 19

Which of the following substances, when dissolved in water, will NOT conduct electricity?

Accepted Answer

Methane ($$\mathrm{CH}_4)$$

Chapter 9: Solutions – Properties, Calculations, and Types of Mixtures

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