Q: Which equation correctly represents the dissociation of potassium chloride (KCl) in water?

$$\text{KCl} \rightarrow \text{K}^+ + \text{Cl}^-$$

Q: Which of the following equations represents the net ionic equation for the precipitation reaction between BaCl$$_2 (aq) $$and Na$$_2SO$_4 (aq$$)?

$$\text{Ba}^{2+} (aq) + \text{SO}_4$$^{2-}$$ (aq) \rightarrow \text{BaSO}_4 (s)$$

Question 1

Which of the following best describes the process shown in the first image, where a solute is added to a solvent to form a solution?

Accepted Answer

The solute is physically combined with the solvent, resulting in a homogeneous mixture.

Question 2

A student dissolves 45 g of KNO$$_3 in 100 g of $$water at 30$$^	ext{o}C. $$According to the solubility curve, is the solution saturated, unsaturated, or supersaturated?

Accepted Answer

Saturated

Question 3

Which equation correctly represents the dissociation of potassium chloride (KCl) in water?

Accepted Answer

$$	ext{KCl} ightarrow 	ext{K}^+ + 	ext{Cl}^-$$

Question 4

Which of the following substances is a strong electrolyte when dissolved in water?

Accepted Answer

Sodium chloride

Question 5

A solution of acetic acid in water conducts electricity weakly. This is because:

Accepted Answer

Acetic acid is a weak electrolyte and only partially dissociates.

Question 6

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

Accepted Answer

Gas molecules escape more easily from the solvent at higher temperatures.

Question 7

Which term describes a solution in which more solute is dissolved than would normally be possible at a given temperature?

Accepted Answer

Supersaturated

Question 8

A student mixes two aqueous solutions and observes the formation of a solid. What type of reaction has occurred?

Accepted Answer

Precipitation reaction

Question 9

Which of the following pairs of solutions will form a precipitate when mixed?

Accepted Answer

BaCl$$_2 (aq) + Na$_2SO$_4 (aq)$$

Question 10

What is the molarity of a solution prepared by dissolving 56.9 g of KNO$$_3 in 0.550 L of $$solution? (Molar mass of KNO$$_3 = 101.1 g/$$mol)

Accepted Answer

$$1.02\ 	ext{M}$$

Question 11

Which of the following statements about colligative properties is correct?

Accepted Answer

Colligative properties depend on the number of solute particles.

Question 12

A nurse must dilute a stock solution of morphine sulfate (120 mg/mL) to prepare 25.0 mL of a solution at 8.0 mg/mL. How many mL of stock solution should be used?

Accepted Answer

$$1.67\ 	ext{mL}$$

Question 13

Which of the following best describes the effect of adding salt to water when cooking pasta?

Accepted Answer

The boiling point of the water increases.

Question 14

Which solution will cause red blood cells to shrink due to water leaving the cells?

Accepted Answer

Hypertonic solution

Question 15

A researcher dissolves 2.50 g of sodium acetate in 47.50 g of water. What is the percent by mass of sodium acetate in the solution?

Accepted Answer

$$5.00\%$$

Question 16

Which of the following equations represents the net ionic equation for the precipitation reaction between BaCl$$_2 (aq) $$and Na$$_2SO$_4 (aq$$)?

Accepted Answer

$$	ext{Ba}^{2+} (aq) + 	ext{SO}_4$$^{2-}$$ (aq) ightarrow 	ext{BaSO}_4 (s)$$

Question 17

Which of the following best explains why saltwater evaporates more slowly than pure water?

Accepted Answer

Saltwater has a lower vapor pressure because dissolved ions reduce the number of water molecules that can escape from the surface.

Question 18

Which compound is a nonelectrolyte when dissolved in water?

Accepted Answer

C$$_6H$_{12}O$_6$$

Question 19

Which of the following best describes a miscible pair of liquids?

Accepted Answer

They dissolve completely in each other.

Solutions, Solubility, and Electrolytes: Core Concepts in General Chemistry

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