Chemistry Name __________________________

Hour _______

Chemistry

Approximate Timeline

Students are expected to keep up with class work when absent.

CHAPTER 8 – REACTIONS IN AQUEOUS SOLUTIONS

Day Plans for the day Assignment(s) for the day

1 Begin Chapter 8

8.3 – Classifying Reactions

o Synthesis

o Decomposition

o Single Displacement

o Double Displacement

o Combustion

o Acid-Base

Assignment 8.0

Assignment 8.3a

Read section(s) 8.1

2 8.1 – Understanding Reactions in Aqueous

Solutions

o Predicting whether a reaction will occur

o Reactions in which a solid forms

How to decide what product forms

o Describing Reactions in Aqueous Solutions

Molecular equations

Assignment 8.1a

3 8.1 – Understanding Reactions in Aqueous

Solutions

o Predicting whether a reaction will occur

o Reactions in which a solid forms

How to decide what product forms

o Describing Reactions in Aqueous Solutions

Molecular equations

Net ionic equations

Assignment 8.1b

Read section(s) 8.2

4 8.2 – Other Reactions in Aqueous Solutions

o Acids & Bases

Arrhenius definitions

Strong acids & strong bases

Acid-base reactions

Assignment 8.2a

5 8.2 – Other Reactions in Aqueous Solutions

o Oxidation-reduction (redox)

Definitions

Recognizing redox reactions

Assignment 8.2b

6 Discuss Types of Reactions Lab

Begin Types of Reactions lab

7 Finish Types of Reactions Lab

Finished lab write-up due at the end of the hour

Assignment 8.3b

8 Work on Assignment 8.4 Assignment 8.4

9 Grade & discuss Assignment 8.4

Review for chapter 8 Test

10 Chapter 8 Test Read section(s) 9.1

Chemistry Name __________________________

Hour _______

Study Guides

Chapter 8 Quizzes

Quiz 8.1 Understanding Reactions in Aqueous Solutions 1. Define the following terms.

a. Precipitate

b. Strong electrolyte

c. Soluble solid

d. Insoluble solid

e. Spectator ions

2. Know the factors that cause a chemical reaction to occur.

3. In chemistry, the word “precipitate” is given a specialized meaning. What does

“precipitate” mean when discussing chemical reactions?

4. Complete and balance several precipitation reactions.

5. Write net ionic equations based on your answers to number 4.

Quiz 8.2 Other Reactions in Aqueous Solutions 6. Define the following terms.

a. (Arrhenius) acid

b. (Arrhenius) base

c. Oxidation-reduction reaction

d. Strong

e. Weak

7. What are the two products of an acid-base reaction?

8. Complete and balance acid base reactions.

Quiz 8.3 Classifying Reactions 9. Classify chemical reactions by type.

a. acid-base

b. combustion

c. decomposition

d. double displacement

e. single displacement

f. synthesis

Study Guide

Chapter 8 Test

At the completion of chapter 8 you should…

1. Know the definitions of the following terms.

a. Precipitation

b. Precipitate

c. Precipitation reaction

d. Strong electrolyte

e. Soluble solid

f. Insoluble (slightly soluble) solid

g. Molecular equation

h. Complete ionic equation

i. Net ionic equation

j. Spectator ions

k. Acid (Arrhenius model)

l. Base (Arrhenius model)

m. Strong acid

n. Strong base

o. Salt

p. Oxidation-Reduction reaction (redox)

2. Know some of the factors that cause a chemical reaction to occur.

3. Be able to identify the solid that forms in a precipitation reaction.

4. Be able to write and balance molecular, complete ionic, and net ionic equations for a

chemical reaction.

5. Be able to write a balanced chemical equation for the reaction between an acid and a

base.

6. Be able to write a balanced chemical equation for the reaction between a metal and a

nonmetal.

7. Be able to classify a chemical reaction as a(n)…

a. synthesis reaction

b. decomposition reaction

c. single displacement reaction

d. double displacement reaction

e. combustion reaction

f. acid-base reaction

Chemistry Name __________________________

Hour _______

Assignment 8.0 – Vocabulary (2 pages)

Define each of the following terms.

1. Precipitation

2. Precipitate

3. Precipitation reaction

4. Strong electrolyte

5. Soluble solid

6. Insoluble (slightly soluble) solid

7. Molecular equation

8. Complete ionic equation

9. Net ionic equation

10. Spectator ions

11. Acid (Arrhenius model)

12. Base (Arrhenius model)

13. Strong acid

14. Strong base

15. Salt

16. Oxidation-Reduction reaction (redox)

Chemistry Name __________________________

Hour _______

Assignment 8.1a – Understanding Reactions in Aqueous Solutions #1

For each of the following, predict whether or not a precipitate (solid) forms. If no precipitate

forms write “no reaction. If a precipitate does form write A) the molecular equation, and B) the

net ionic equation.

1. _____ Pb(NO3)2 (aq) + _____ NaCl (aq)

2. _____ Ba(NO3)2 (aq) + _____ K2SO4 (aq)

3. _____ KNO3 (aq) + _____ NH4Cl (aq)

4. _____ CaCl2 (aq) + _____ K2CO3 (aq)

5. _____ NaOH (aq) + _____ FeBr2 (aq)

Chemistry Name __________________________

Hour _______

Assignment 8.1b – Understanding Reactions in Aqueous Solutions #2

1) What are the driving forces that indicate a chemical reaction is likely to occur?

2) Use the solubility rules in Table 8.1 (page 245) or the information in Figure 8.3 (page

245) to predict whether the following compounds are soluble or insoluble in water.

A) potassium nitrate

B) zinc(II) hydroxide

C) calcium carbonate

D) ammonium chloride

3) Consider two separate beakers, one containing an aqueous solution of hydrochloric acid,

the second an aqueous solution of lead (II) nitrate.

A) Write and balance the chemical equation for any reaction that occurs.

B) Write and balance the net ionic equation for the reaction.

4) A) What is a spectator ion and B) What happens to it in a net ionic equation?

5) Consider the following reaction: aqueous sodium sulfate is added to aqueous barium

bromide to form solid barium sulfate and aqueous sodium bromide.

A) Write and balance the molecular equation.

B) List the spectator ions.

C) Write and balance the net ionic equation.

Chemistry Name __________________________

Hour _______

Assignment 8.2a – Acids and Bases and Acid-Base Reactions (2 pages)

1) Define the following terms.

A) Acid

B) Base

2) List both the chemical name and chemical formula for all six strong acids.

Name Formula

A) _______________________________________ ____________

B) _______________________________________ ____________

C) _______________________________________ ____________

D) _______________________________________ ____________

E) _______________________________________ ____________

F) _______________________________________ ____________

3) List both the chemical name and chemical formula for all six strong bases.

Name Formula

A) _______________________________________ ____________

B) _______________________________________ ____________

C) _______________________________________ ____________

D) _______________________________________ ____________

E) _______________________________________ ____________

F) _______________________________________ ____________

4) Complete and balance each of the following acid-base reactions. Write the net ionic

equation beneath each molecular equation.

A) _____ NaOH (aq) + _____ HCl (aq)

B) _____ H2SO4 (aq) + _____ KOH (aq)

C) _____ Ca(OH)2 (aq) + _____ HNO3 (aq)

Chemistry Name __________________________

Hour _______

Assignment 8.2b – Oxidation and Reduction and Redox Reactions

1) Define the following terms.

A) oxidation

B) reduction

2) Balance each of the following redox reactions. Identify the atom/molecule that is

oxidized and the atom/molecule that is reduced.

A) _____ Mg (s) + _____ N2 (g) _____ Mg3N2 (s)

B) _____ K (s) + _____ N2 (g) _____ K3N (s)

C) _____ Al (s) + _____ O2 (g) _____ Al2O3 (s)

D) _____ Na (s) + _____ S (s) _____ Na2S (s)

Chemistry Name __________________________

Hour _______

Assignment 8.2c – Other Reactions in Aqueous Solutions

1) What are the products in a reaction between an acid and a base?

2) What is meant by the term strong acid?

3) What is meant by the term strong base?

4) A) What is an oxidation-reduction reaction? B) How can you identify this type of

reaction?

Chemistry Name __________________________

Hour _______

Assignment 8.3a – Classifying Reactions

Balance each of the following reactions and identify the type of reaction.

1. ____ Al + ____ N2 ____ AlN

Type of reaction: __________________________________

2. ____ HCl + _____NaOH ____ H2O + ____ NaCl

Type of reaction: __________________________________

3. ____ C6H10 + ____ O2 ____ CO2 + ____ H2O

Type of reaction: __________________________________

4. ____ Hg2(NO3)2 + ____ NaCl ____ Hg2Cl2 + ____ NaNO3

Type of reaction: __________________________________

5. _____ KOH + _____ HNO3 _____ KNO3 + _____ H2O

Type of reaction: __________________________________

6. ____ NH4NO3 ____ N2O + ____ H2O

Type of reaction: __________________________________

7. ____ Pb(NO3)2 + ____ HCl ____ PbCl2 + ____ HNO3

Type of reaction: __________________________________

8. ____ NO2 ____ N2 + ____ O2

Type of reaction: __________________________________

9. ____ Fe2O3 + ____Al ____Al2O3 + ____ Fe

Type of reaction: __________________________________

10. ____ Na + ____ O2 ____ Na2O2

Type of reaction: __________________________________

11. ____ Al + ____ H2SO4 ____Al2(SO4)3 + ____ H2

Type of reaction: __________________________________

12. ____ Fe + ____ O2 ____Fe2O3

Type of reaction: __________________________________

13. ____ H2SO4 + _____ Ca(OH)2 _____ H2O + _____ CaSO4

Type of reaction: __________________________________

14. ____ AgNO3 + ____ H2S ____ Ag2S + ____ HNO3

Type of reaction: __________________________________

15. ____ BaO2 ____ BaO + ____O2

Type of reaction: __________________________________

16. ____ C4H10 + ____ O2 ____ CO2 + ____ H2O

Type of reaction: __________________________________

17. ____ AgNO3 + ____ Zn ____Zn(NO3)2 + ____ Ag

Type of reaction: __________________________________

18. ____ C2H4 + ____ O2 ____ CO2 + ____ H2O

Type of reaction: __________________________________

Chemistry Name __________________________

Hour _______

Assignment 8.3b – Classifying Reactions

1) Why are precipitation reactions also called double displacement reactions?

2) What are three other ways to classify oxidation-reduction reactions?

3) Classify the following unbalanced equations as: precipitation, acid-base, or oxidation-

reduction (redox).

A) Fe (s) + H2SO4 (aq) Fe3(SO4)2 (s) + H2 (g)

B) HClO4 (aq) + RbOH (aq) RbClO4 (aq) + H2O (l)

C) K2SO4 (aq) + CaCl2 (aq) KCl (aq) + CaSO4 (s)

D) Ni (s) + Cl2 (g) NiCl2 (s)

4) One of the reactants in a combustion reaction must always be ___.

5) Classify the reaction of hydrogen gas with oxygen gas to form water in three different

ways.

6) Balance the following equations and classify them in as many ways as possible.

A) ____ Al (s) + ____ O2 (g) ____ Al2O3 (s)

B) ____ Ba(OH)2 (aq) + ____ H2SO4 (aq) ____ BaSO4 (s) + ____ H2O (l)

C) ____ H2O2 (aq) ____ H2O (l) + ____ O2 (g)

Chemistry Name __________________________

Hour _______

Assignment 8.4 – Chapter Review (4 pages)

1) A) When two solutions of ionic substances are mixed and a precipitate forms, what is the

net charge of the precipitate? B) Why?

2) What is meant by the term strong electrolyte? Give two examples of substances that are

strong electrolytes.

3) On the basis of the solubility rules in Table 8.1 (page 245), predict which of the following

will be soluble or insoluble in water. (circle one)

A) barium nitrate Soluble Insoluble

B) potassium carbonate Soluble Insoluble

C) sodium sulfate Soluble Insoluble

D) copper(II) hydroxide Soluble Insoluble

E) mercury(I) chloride Soluble Insoluble

F) ammonium phosphate Soluble Insoluble

G) chromium(III) sulfide Soluble Insoluble

H) lead(II) sulfate Soluble Insoluble

4) On the basis of the solubility rules in Table 8.1 (page 245), write a balanced molecular

equation for the precipitation reactions that take place when the following aqueous

solutions are mixed. If no precipitate is formed write “no reaction.”

A) nitric acid and barium chloride

B) ammonium sulfide and cobalt (II) chloride

C) sulfuric acid and lead (II) nitrate

D) calcium chloride and potassium carbonate

E) sodium acetate and ammonium nitrate

F) sodium phosphate and chromium (III) chloride

5) Write balanced net ionic equations for the reactions that occur when the following

aqueous solutions are mixed.

A) potassium sulfate and calcium nitrate

B) iron (III) nitrate and sodium carbonate

C) silver (I) nitrate and calcium iodide

D) ammonium phosphate and cobalt (II) sulfate

Chemistry Name __________________________

Hour _______

E) strontium chloride and mercury (I) nitrate

F) barium bromide and lead (II) nitrate

6) If 1000 NaOH molecules were dissolved in water, the NaOH would produce ___ Na+

ions and ___ OH- ions.

7) Complete and balance each of the following acid-base reactions. Circle the formula of the

salt produced.

A) ____ HCl (aq) + ____ RbOH (aq)

B) ____ HClO4 (aq) + ____ NaOH (aq)

C) ____ HBr (aq) + ____ NaOH (aq)

D) ____ H2SO4 (aq) + ____ CsOH (aq)

8) If atoms of a metallic element (such as sodium) react with atoms of a nonmetallic

element (such as sulfur), which element loses electrons and which element gains them?

9) A) If potassium atoms were to react with atoms of sulfur, how many electrons would

each potassium atom lose? B) How many electrons would each sulfur atom gain? C) How

many potassium atoms would have to react to provide enough electrons for one sulfur

atom? D) What charges would the resulting potassium and sulfur ions have?

10) Balance each of the following oxidation-reduction reactions.

A) ____ Fe (s) + ____ S (s) ____ Fe2S3 (s)

B) ____ Zn (s) + ____ HNO3 (aq) ____ Zn(NO3)2 (aq) + ____ H2 (g)

C) ____ Sn (s) + ____ O2 (g) ____ SnO (g)

D) ____ K (s) + ____ H2 (g) ____ KH (s)

E) ____ Cs (s) + ____ H2O (l) ____ CsOH (s) + ____ H2 (g)

11) Identify, but do not balance, each of the following unbalanced equations as belonging to

one or more of the following categories: precipitation, acid-base, or oxidation-reduction

(redox).

A) K2SO4 (aq) + Ba(NO3)3 (aq) BaSO4 (s) + KNO3 (aq)

B) HCl (aq) + Zn (s) ZnCl2 (aq) + H2 (g)

C) HCl (aq) + AgNO3 (aq) AgCl (s) + HNO3 (aq)

D) HCl (aq) + KOH (aq) H2O (l) + KCl (aq)

E) Zn (s) + CuSO4 (aq) ZnSO4 (aq) + Cu (s)

F) NaH2PO4 (aq) + NaOH (aq) Na3PO4 (aq) + H2O (l)

G) Ca(OH)2 (aq) + H2SO4 (aq) CaSO4 (s) + H2O (l)

H) ZnCl2 (aq) + Mg (s) Zn (s) + MgCl2 (aq)

I) BaCl2 (aq) + H2SO4 (aq) BaSO4 (s) + HCl (aq)