Question 1

Which of the following best describes an aqueous solution?

Accepted Answer

A homogeneous mixture in which water is the solvent.

Question 2

Which statement correctly distinguishes between a strong electrolyte and a weak electrolyte in aqueous solution?

Accepted Answer

A strong electrolyte completely dissociates into ions, while a weak electrolyte only partially dissociates.

Question 3

Which of the following compounds is most likely to be a strong electrolyte when dissolved in water?

Accepted Answer

NaCl

Question 4

A student dissolves 0.1 mol of acetic acid (CH\_3COOH) in water. Only about 1% of the acetic acid molecules ionize. What type of electrolyte is acetic acid?

Accepted Answer

Weak electrolyte

Question 5

Which of the following best explains why pure water does not conduct electricity?

Accepted Answer

It does not contain free ions to carry electric current.

Question 6

Which equation correctly represents the dissociation of sodium chloride (NaCl) in water?

Accepted Answer

$$\mathrm{NaCl} (aq) \rightarrow \mathrm{Na}^+ (aq) + \mathrm{Cl}^- (aq)$$

Question 7

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

Accepted Answer

C\_12H\_22O\_11 (sucrose)

Question 8

A solution is prepared by dissolving 0.50 mol of KBr in enough water to make 1.0 L of solution. What is the molarity of the solution?

Accepted Answer

$$M = \frac{0.50\ \mathrm{mol}}{1.0\ \mathrm{L}} = 0.50\ \mathrm{M}$$

Question 9

Which of the following best describes the process of dilution?

Accepted Answer

Adding solvent to a solution to decrease its concentration.

Question 10

A chemist mixes solutions of AgNO\_3 and NaCl. A white precipitate forms. What is the identity of the precipitate?

Accepted Answer

AgCl

Question 11

Which of the following ionic compounds is predicted to be soluble in water?

Accepted Answer

K\_2SO\_4

Question 12

Which of the following is the correct balanced molecular equation for the reaction between HCl(aq) and NaOH(aq)?

Accepted Answer

$$\mathrm{HCl} (aq) + \mathrm{NaOH} (aq) \rightarrow \mathrm{NaCl} (aq) + \mathrm{H}_2\mathrm{O} (l)$$

Question 13

Which of the following best describes the role of water molecules in stabilizing ions in solution?

Accepted Answer

Water molecules surround ions, shielding them from interacting with each other.

Question 14

Which of the following is a correct net ionic equation for the reaction between AgNO\_3(aq) and NaCl(aq)?

Accepted Answer

$$\mathrm{Ag}^+ (aq) + \mathrm{Cl}^- (aq) \rightarrow \mathrm{AgCl} (s)$$

Question 15

A solution contains 0.20 mol of CaCl\_2 dissolved in 1.0 L of water. What is the concentration of chloride ions in the solution?

Accepted Answer

$$[\mathrm{Cl}^-] = 0.40\ \mathrm{M}$$

Question 16

Which of the following best describes a precipitation reaction?

Accepted Answer

A reaction in which an insoluble solid forms from the mixing of two solutions.

Question 17

Which of the following is the correct formula for calculating molarity?

Accepted Answer

$$M = \frac{	ext{moles of solute}}{	ext{liters of solution}}$$

Question 18

Which of the following statements is true regarding the solubility of ionic compounds in water?

Accepted Answer

All common ionic compounds of alkali metals (group 1) and ammonium (NH\_4^+) are soluble in water.

Question 19

A student needs to prepare 250 mL of a 0.10 M NaCl solution from a 1.0 M stock solution. What volume of stock solution should be used?

Accepted Answer

$$V_1$$ = \frac{$$M_2$$ $$V_2$$}{$$M_1$$} = \frac{0.10 	imes 250}{1.0} = 25\ \mathrm{mL}$$

General Properties of Aqueous Solutions and Reactions in Aqueous Solution

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