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Chapter Presentation

Transparencies

Lesson Starters

Standardized Test Prep

Visual Concepts

Resources



Table of Contents

Chapter 14 Acids and Bases

Section 1 Properties of Acids and Bases Section 2 Acid-Base Theories

Section 3 Acid-Base Reactions



Lesson Starter

• The solutions in the beakers are different because they have a different pH.

• One beaker contains a basic solution and the other beaker contains an acidic solution

Chapter 14Section 1 Properties of Acids and Bases



Lesson Starter

• What is the meaning of the word neutralization.

• How is the word used in everyday life?

• How is it likely to apply to acids and bases?

Chapter 14 Section 3 Acid-Base Reactions



Objectives

• Describe a conjugate acid, a conjugate base, and an amphoteric compound.

• Explain the process of neutralization.

• Define acid rain, give examples of compounds that can cause acid rain, and describe effects of acid rain.




Conjugate Acids and Bases

• The species that remains after a Brønsted-Lowry acid has given up a proton is the conjugate base of that acid.

HF(aq) + H

2O(l) FĞ(aq) + H

3O(aq)


acid conjugate base



Conjugate Acids and Bases, continued

• Brønsted-Lowry acid-base reactions involve two acid-base pairs, known a conjugate acid-base pairs.


acid1 base2 base1 acid2

HF(aq) + H

2O(l) FĞ(aq) + H

3O(aq)



Neutralization Reactions




Conjugate Acids and Bases, continuedStrength of Conjugate Acids and Bases

• The stronger an acid is, the weaker its conjugate base

• The stronger a base is, the weaker its conjugate acid

HCl(g) + H2O(l) H

3O(aq) + ClĞ(aq)


strong acid base acid weak base



Conjugate Acids and Bases, continuedStrength of Conjugate Acids and Bases, continued

• Proton transfer reactions favor the production of the weaker acid and the weaker base.

HClO4(aq) + H

2O(l) H

3O(aq) + ClO

4Ğ(aq)

CH3COOH(aq) + H

2O(l) H

3O(aq) + CH

3COOĞ(aq)


stronger acid stronger base weaker acid weaker base

• The reaction to the right is more favorable

weaker acid weaker base stronger acid stronger base

• The reaction to the left is more favorable



Visual Concepts

Click below to watch the Visual Concept.

Visual Concept

Conjugated Acids and Bases

Chapter 14



Relative Strengths of Acids and Bases


Relative Strengths of Acids and Bases



Amphoteric Compounds

• Any species that can react as either an acid or a base is described as amphoteric.

• example: water• water can act as a base

H2SO

4(aq) + H

2O(l) H

3O(aq) + HSO

4Ğ(aq)

NH

3(g) + H

2O(l) NH

4(aq) OHĞ(aq)


acid1 base2 acid2 base1

• water can act as an acid

base1 acid2 acid1 base2



Amphoteric Compounds, continued–OH in a Molecule

• The covalently bonded IOH group in an acid is referred to as a hydroxyl group.

• Molecular compounds containing —OH groups can be acidic or amphoteric.

• The behavior of a compound is affected by the number of oxygen atoms bonded to the atom connected to the —OH group.




Oxyacids of Chlorine




Visual Concepts


Visual Concept

Amphoterism

Chapter 14



Neutralization ReactionsStrong Acid-Strong Base Neutralization

• In aqueous solutions, neutralization is the reaction of hydronium ions and hydroxide ions to form water molecules.

• A salt is an ionic compound composed of a cation from a base and an anion from an acid.

HCl(aq) + NaOH(aq) NaCl(aq) H2O(l)




Visual Concepts


Visual Concept

Neutralization Reaction

Chapter 14



Acid Rain

• NO, NO2, CO2, SO2, and SO3 gases from industrial processes can dissolve in atmospheric water to produce acidic solutions.

SO3(g) + H

2O(l) H

2SO

4(aq)


• example:

• Very acidic rain is known as acid rain.

• Acid rain can erode statues and affect ecosystems.



Visual Concepts

Acid Precipitation

Chapter 14



Visual Concepts


Visual Concept

Chemical Weathering

Chapter 14



End of Chapter 14 Show



Multiple Choice

1. Which of the following is not a characteristic of

an acid?

A. An acid changes the color of an indicator.

B. An acid has a bitter taste.

C. An acid ionizes in water.

D. An acid produces hydronium ions in water.

Chapter 14 Standardized Test Preparation



Multiple Choice

1. Which of the following is not a characteristic of

an acid?

A. An acid changes the color of an indicator.

B. An acid has a bitter taste.

C. An acid ionizes in water.

D. An acid produces hydronium ions in water.




Multiple Choice

2. When an acid reacts with an active metal,

A. the hydronium ion concentration increases.

B. the metal forms anions.

C. hydrogen gas is produced.

D. carbon dioxide gas is produced.




Multiple Choice

2. When an acid reacts with an active metal,

A. the hydronium ion concentration increases.

B. the metal forms anions.

C. hydrogen gas is produced.

D. carbon dioxide gas is produced.




Multiple Choice

3. Which of the following is a Brønsted-Lowry base?

A. an electron pair donor

B. an electron pair acceptor

C. a proton donor

D. a proton acceptor




Multiple Choice

3. Which of the following is a Brønsted-Lowry base?

A. an electron pair donor

B. an electron pair acceptor

C. a proton donor

D. a proton acceptor




Multiple Choice

4. Which acid is the most commonly produced industrial chemical?

A. hydrochloric acid

B. acetic acid

C. nitric acid

D. sulfuric acid




Multiple Choice

4. Which acid is the most commonly produced industrial chemical?

A. hydrochloric acid

B. acetic acid

C. nitric acid

D. sulfuric acid




Multiple Choice5. Which of the following is a conjugate pair?

A. H+ and OH

B.

C. HCl and Cl

D.


NH2Ğ and NH

4

H2SO

4 and SO

42-



Multiple Choice

5. Which of the following is a conjugate pair?

A. H+ and OH

B.

C. HCl and Cl

D.

NH2Ğ and NH

4

H2SO

4 and SO

42-




Multiple Choice

6. What is the formula for acetic acid?

A. CH3COOH

B. HNO3

C. HClO4

D. HCN




Multiple Choice

6. What is the formula for acetic acid?

A. CH3COOH

B. HNO3

C. HClO4

D. HCN




Multiple Choice

7. Which of the following species is the conjugate acid of another species in the list?

A.

B. H3PO4

C. H2O

D.


PO43-

H2PO

4Ğ



Multiple Choice

7. Which of the following species is the conjugate acid of another species in the list?

A.

B. H3PO4

C. H2O

D.

PO43-

H2PO

4Ğ




Multiple Choice

8. Identify the salt that forms when a solution of H2SO4 is titrated with a solution of Ca(OH)2.

A. calcium sulfate

B. calcium hydroxide

C. calcium oxide

D. calcium phosphate




Multiple Choice

8. Identify the salt that forms when a solution of H2SO4 is titrated with a solution of Ca(OH)2.

A. calcium sulfate

B. calcium hydroxide

C. calcium oxide

D. calcium phosphate




Multiple Choice9. Which of the following statements is true for the

reaction below?

A. HF is the base.

B.

C. F− is the conjugate base.

D.

HF(aq) + HPO

42Ğ(aq) FĞ(aq) + H

2PO

4Ğ(aq)


HPO42Ğ is the acid.

H2PO

4Ğ is the conjugate base.



Multiple Choice9. Which of the following statements is true for the

reaction below?

A. HF is the base.

B.

C. F− is the conjugate base.

D.

HPO42Ğ is the acid.

H2PO

4Ğ is the conjugate base.

HF(aq) + HPO

42Ğ(aq) FĞ(aq) + H

2PO

4Ğ(aq)




Short Answer

10. How does a strong acid differ from a weak acid? Give

one example of each.




Short Answer

10. How does a strong acid differ from a weak acid? Give

one example of each.

Answer: A strong acid is 100% ionized; a weak acid is

less than 100% ionized. Possible strong acids are HCl,

HI, HBr, HNO3, H2SO4, HClO4, and HClO3. With very

few exceptions, any other acid will be a weak acid.




Short Answer

11. Identify the conjugate acid-base pairs in the following

reaction: HClO

2(aq) + NH

3(aq) ClO

2Ğ(aq) + NH

4(aq)




Short Answer

11. Identify the conjugate acid-base pairs in the following

reaction:

Answer: HClO2(aq) acid1,

NH3(aq) base2,

ClO2Ğ(aq) base

1;

NH4(aq) acid

2

HClO

2(aq) + NH

3(aq) ClO

2Ğ(aq) + NH

4(aq)




Extended Response


12. Phosphoric acid, H3PO4, has three hydrogen atoms and is classified as a triprotic acid. Acetic acid, CH3COOH, has four hydrogen atoms and is classified as a monoprotic acid. Explain the difference, and justify your explanation by drawing the Lewis structure for both acids.



12. Phosphoric acid, H3PO4, has three hydrogen atoms and is classified as a triprotic acid. Acetic acid, CH3COOH, has four hydrogen atoms and is classified as a monoprotic acid. Explain the difference, and justify your explanation by drawing the Lewis structure for both acids.

Answer: Each of the H atoms in phosphoric acid is attached to an oxygen atom and can ionize. Only one of the H atoms in acetic acid is attached to an oxygen atom and can be ionized. The three H atoms bonded to C do not ionize; thus, acetic acid is a monoprotic acid.


Extended Response



P OH

OH

HO

O

CH

H

H

C

O

OH


Extended Response12. Phosphoric acid, H3PO4, has three hydrogen atoms and is

classified as a triprotic acid. Acetic acid, CH3COOH, has four hydrogen atoms and is classified as a monoprotic acid. Explain the difference, and justify your explanation by drawing the Lewis structure for both acids.

Answer continued:



13. Write the full equation, ionic equation, and net ionic equation for the neutralization reaction between ammonia and sulfuric acid. Identify the spectator ion(s).


Extended Response



13. Write the full equation, ionic equation, and net ionic equation for the neutralization reaction between ammonia and sulfuric acid. Identify the spectator ion(s).

Answer:

full equation:

ionic equation:

net ionic equation:

spectator ion:

2NH3(aq) + H

2SO

4(aq) (NH

4)

2SO

4(aq)

2NH3(aq) + 2H

3O(aq) + SO

42Ğ(aq)

2NH4(aq) + SO

42Ğ(aq) + 2H

2O(l)

2NH3(aq) + 2H

3O(aq) 2NH

4(aq) + 2H

2O(l)

SO42Ğ


Extended Response

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