Q: What is the molarity of a solution prepared by dissolving 25.5 g of KBr (molar mass = 119.00 g/mol) in enough water to make 1.75 L of solution?

$$M = \frac{0.214\ \text{mol}}{1.75\ \text{L}} = 0.122\ \text{M}$$

Q: Which of the following equations correctly relates molarity, moles, and volume?

$$M = \frac{\text{mol}}{\text{L}}$$

Q: Which of the following is the net ionic equation for the reaction between Pb(NO$$_3$$)$$_2(aq) $$and 2 KCl(aq)?

$$\text{Pb}^{2+}(aq) + 2\ \text{Cl}^-(aq) \rightarrow \text{PbCl}_2(s)$$

Q: Which of the following is the correct net ionic equation for the neutralization of HCl(aq) with NaOH(aq)?

$$\text{H}^+(aq) + \text{OH}^-(aq) \rightarrow \text{H}_2\text{O}(l)$$

Q: Which of the following reactions is a redox reaction?

$$4\ \text{Fe}(s) + 3\ \text{O}_2(g) \rightarrow 2\ \text{Fe}_2\text{O}_3(s)$$

Question 1

Which of the following best describes a concentrated solution?

Accepted Answer

A solution with a relatively large amount of solute compared to solvent.

Question 2

What is the molarity of a solution prepared by dissolving 25.5 g of KBr (molar mass = 119.00 g/mol) in enough water to make 1.75 L of solution?

Accepted Answer

$$M = \frac{0.214\ 	ext{mol}}{1.75\ 	ext{L}} = 0.122\ 	ext{M}$$

Question 3

Which of the following is the correct sequence for preparing 1.00 L of a 1.00 M NaCl solution?

Accepted Answer

Add 1.00 mol NaCl to a flask, add water to dissolve, then add water until the total volume is 1.00 L.

Question 4

How many moles of solute are required to make 3.0 L of a 2.0 M solution?

Accepted Answer

6.0 mol

Question 5

A student wants to prepare 500.0 mL of a 2.80 M CaCl$$_2$$ solution. How many grams of CaCl$$_2 ($$molar mass = 110.984 g/mol) are needed?

Accepted Answer

155 g

Question 6

Which of the following equations correctly relates molarity, moles, and volume?

Accepted Answer

$$M = \frac{	ext{mol}}{	ext{L}}$$

Question 7

Which of the following best explains why NaCl(aq) conducts electricity but C$$_{12}H$_{22}O$_{11}(aq) $$does not?

Accepted Answer

NaCl dissociates into ions in water, while C$$_{12}H$_{22}O$_{11}$$ does not.

Question 8

Which of the following is a strong electrolyte?

Accepted Answer

NaCl(aq)

Question 9

Which of the following compounds is insoluble in water?

Accepted Answer

AgCl

Question 10

A precipitation reaction occurs when:

Accepted Answer

An insoluble solid forms upon mixing two aqueous solutions.

Question 11

Which of the following is the net ionic equation for the reaction between Pb(NO$$_3$$)$$_2(aq) $$and 2 KCl(aq)?

Accepted Answer

$$	ext{Pb}^{2+}(aq) + 2\ 	ext{Cl}^-(aq) ightarrow 	ext{PbCl}_2(s)$$

Question 12

Which of the following best describes the role of a spectator ion in a chemical reaction?

Accepted Answer

It does not participate in the chemical change and remains unchanged on both sides of the equation.

Question 13

Which of the following is the correct net ionic equation for the neutralization of HCl(aq) with NaOH(aq)?

Accepted Answer

$$	ext{H}^+(aq) + 	ext{OH}^-(aq) ightarrow 	ext{H}_2	ext{O}(l)$$

Question 14

A 10.0 mL sample of 0.20 M HBr is titrated with 0.10 M NaOH. What volume of NaOH is required to reach the equivalence point?

Accepted Answer

20.0 mL

Question 15

Which of the following reactions is a redox reaction?

Accepted Answer

$$4\ 	ext{Fe}(s) + 3\ 	ext{O}_2(g) ightarrow 2\ 	ext{Fe}_2	ext{O}_3(s)$$

Question 16

Which of the following statements about oxidation and reduction is correct?

Accepted Answer

Oxidation is the loss of electrons, and reduction is the gain of electrons.

Question 17

Which metal is most easily oxidized according to the activity series?

Accepted Answer

Na

Question 18

In the reaction $$	ext{Mg}(s) + 2\ 	ext{H}_2	ext{O}(l) ightarrow 	ext{Mg(OH)}_2(s) + 	ext{H}_2(g)$$, which element is oxidized and which is reduced?

Accepted Answer

Mg is oxidized, H in H$$_2O is $$reduced.

Question 19

Which of the following best describes the role of water in an aqueous solution?

Accepted Answer

Water acts as the solvent, dissolving the solute.

Introduction to Solutions and Aqueous Reactions: Solution Concentration, Preparation, and Types of Reactions

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