05 CTR ch19 7/12/04 8:16 AM Page 487 ACID-BASE THEORIES 19hs.pequannock.org/ourpages/auto/2012/9/6/56236270/Chapter 19 St… · In the Lewis theory, an acid is an 5. acceptor. A Lewis

Chapter 19 Acids, Bases, and Salts 487

Section Review

Objectives• Define the properties of acids and bases

• Compare and contrast acids and bases as defined by the theories of Arrhenius,Brønsted-Lowry, and Lewis

Vocabulary

Part A CompletionUse this completion exercise to check your understanding of the concepts and termsthat are introduced in this section. Each blank can be completed with a term, shortphrase, or number.

Compounds can be classified as acids or bases according to 1.

different theories. An acid yields hydrogen ions 2.

in aqueous solution. An Arrhenius base yields in aqueous 3.

solution. A Brønsted-Lowry acid is a donor. A Brønsted- 4.

Lowry base is a proton . In the Lewis theory, an acid is an 5.

acceptor. A Lewis base is an electron-pair . 6.

An acid with one ionizable hydrogen atom is called a 7

acid, while an acid with two ionizable hydrogen atoms is called a 8.

acid. 9.

A is a pair of substances related by the gain or loss of 10.

a hydrogen ion. A substance that can act as both an acid and a base 11.

is called .11

10

9

8

76

5

4

3

21

• monoprotic acids

• diprotic acids

• triprotic acids

• conjugate acid

• conjugate base

• conjugate acid–base pair

• hydronium ion (H3O�)

• amphoteric

• Lewis acid

• Lewis base

Name ___________________________ Date ___________________ Class __________________

ACID-BASE THEORIES19.1

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488 Core Teaching Resources

Part B True-FalseClassify each of these statements as always true, AT; sometimes true, ST; or never true, NT.

________ 12. Hydrochloric acid is a strong acid that is diprotic.

________ 13. The ammonium ion, NH4�, is a Brønsted-Lowry base.

________ 14. A Brønsted-Lowry base is a hydrogen-ion acceptor.

________ 15. A compound can act as both an acid and a base.

________ 16. PBr3 is a Lewis base.

Part C MatchingMatch each description in Column B to the correct term in Column A.

Part D ProblemAnswer the following in the space provided.

26. Identify the Lewis acid and Lewis base in the following reaction. Explain.

dimethyl ether boron trifluoride

F F

F

� B uy HO

H 2 C 2 H

H H

H H

H 2 C C 2 H%^

%F

%

^

HC B 2 F

H

O

%

%^ ^

^@

F@

@ @

@ @

H

@

@

Column B

a. tastes sour and will change the color of an acid-baseindicator

b. an electron-pair donor

c. a water molecule that gains a hydrogen ion

d. acids that contain three ionizable hydrogens

e. particle that remains when an acid has donated ahydrogen ion

f. an electron-pair acceptor

g. acids that contain one ionizable hydrogen

h. tastes bitter and feels slippery

i. particle formed when a base gains a hydrogen ion

Column A

________ 17. monoprotic acids

________ 18. triprotic acids

________ 19. acid properties

________ 20. base properties

________ 21. conjugate base

________ 22. conjugate acid

________ 23. hydronium ion (H3O�)

________ 24. Lewis acid

________ 25. Lewis base

Name ___________________________ Date ___________________ Class __________________©

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Section Review

Objectives• Classify a solution as neutral, acidic, or basic, given the hydrogen-ion or

hydroxide-ion concentration

• Convert hydrogen-ion concentrations into values of pH and hydroxide-ionconcentrations into values of pOH

• Describe the purpose of pH indicators

Vocabulary

Key Equations• Kw � [H�] � [OH�] � 1.0 � 10�14M 2 • pOH � � log [OH�]

• pH � � log [H�] • pH � pOH � 14


Water molecules can to form hydrogen ions (H�) and 1.

hydroxide ions (OH�). The concentrations of these ions in pure 2.

water at 25°C are both equal to mol/L. 3.

The pH scale, which has a range from , is used to 4.

denote the concentration of a solution. On this scale, 0 is 5.

strongly , 14 is strongly , and 7 is . Pure 6.

water at 25°C has a pH of . 7.

The constant for water has a value of 1.0 � 10�14. 8.

Thus, the product of the concentrations of ions and 9.

ions in aqueous solution will always equal 1.0 � 10�14. 10.

11.

11

10

9

8

765

4

3

2

1

• self-ionization

• neutral solution

• ion-product constant forwater (Kw)

• acidic solution

• basic solution

• alkaline solutions

• pH

Name ___________________________ Date ___________________ Class __________________

HYDROGEN IONS AND ACIDITY19.2

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________ 12. In an acidic solution, [H�] is greater than [OH�].

________ 13. pH indicators can give accurate pH readings for solutions.

________ 14. If the [H�] in a solution increases, the [OH�] must decrease.

________ 15. The [OH�] is less than 10�7M in a basic solution.

________ 16. The definition of pH is the negative logarithm of the hydroxide-ionconcentration.


Part D ProblemsAnswer the following in the space provided.

24. Calculate the hydroxide-ion concentration, [OH�], for an aqueous solution inwhich [H�] is 1 � 10�10 mol/L. Is this solution acidic, basic, or neutral?

25. Determine the hydrogen-ion concentrations for aqueous solutions that havethe following pH values.

a. 3 b. 6 c. 10

Column B

a. aqueous solution in which [H�] and [OH�] are equal

b. product of hydrogen ion and hydroxide ionconcentrations for water

c. base solutions

d. solution in which [H�] is less than [OH�]

e. reaction in which two water molecules produce ions

f. the negative logarithm of the hydrogen-ionconcentration

g. solution in which [H�] is greater than [OH�]

Column A

________ 17. alkaline solutions

________ 18. pH

________ 19. self-ionization

________ 20. neutral solution

________ 21. ion-product constantfor water (Kw)

________ 22. acidic solution

________ 23. basic solution

Name ___________________________ Date ___________________ Class __________________©


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Section Review

Objectives• Define strong acids and weak acids

• Calculate an acid dissociation constant (Ka) from concentration and pH measurements

• Order acids by strength according to their acid dissociation constants (Ka)

• Order bases by strength according to their base dissociation constants (Kb)

Vocabulary


The strength of an acid or a base is determined by the 1.

of the substance in solution. The acid dissociation constant, 2.

, is a quantitative measure of acid strength. A strong acid 3.

has a much Ka than a weak acid. The Ka of an acid is 4.

determined from measured values. 5.

Hydrochloric acid and sulfuric acid are ionized in 6.

solution and are acids. Ethanoic acid, which is only about 7.

1 percent ionized, is a acid. Magnesium hydroxide and 8.

calcium hydroxide are strong . 9.

Weak bases react with to form the hydroxide ion and 10.

the conjugate of the base. Concentration in solution does 11.

not affect whether an acid or a base is or weak.11

10

9

8

7

6

5

4

3

2

1

• strong acids

• weak acids

• acid dissociation constant (Ka)

• strong bases

• weak bases

• base dissociation constant (Kb)

Name ___________________________ Date ___________________ Class __________________

STRENGTHS OF ACIDS AND BASES19.3

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________ 12. Acids are completely dissociated in aqueous solution.

________ 13. Diprotic acids lose both hydrogens at the same time.

________ 14. Acid dissociation constants for weak acids can be calculated fromexperimental data.

________ 15. Bases react with water to form hydroxide ions.



22. A 0.35M solution of a strong acid, HX, has a [H�] of 4.1 � 10�2. What is the valueof Ka for this acid?

Column B

a. ratio of the concentration of the dissociated (or ionized) formof an acid to the concentration of the undissociated acid

b. bases that dissociate completely into metal ions andhydroxide ions in aqueous solution

c. acids that ionize completely in aqueous solution

d. bases that do not dissociate completely in aqueous solution

e. acids that are only partially ionized in aqueous solution

f. ratio of concentration of conjugate acid times concentrationof hydroxide ion to the concentration of conjugate base

Column A

________ 16. strong acids

________ 17. weak acids

________ 18. acid dissociationconstant (Ka)

________ 19. strong bases

________ 20. weak bases

________ 21. base dissociationconstant (Kb)

Name ___________________________ Date ___________________ Class __________________©


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Section Review

Objectives• Explain how acid–base titration is used to calculate the concentration of an acid

or a base

• Explain the concept of equivalence in neutralization reactions

Vocabulary

Key Equations• Acid � Base y Salt � Water

• Gram equivalent mass �

• Normality (N) � equiv/L

• N1 � V1 � N2 � V2

• NA � VA � NB � VB


In the reaction of a(n) with a base, hydrogen ions 1.

and ions react to produce . This reaction, called 2.

, is usually carried out by . The in a 3.

titration is the point at which the solution is neutral. At the 4.

point of a titration, the number of equivalents of acid 5.

equals the number of equivalents of base. 6.

7.

7

654

32

1

molar mass��number of ionizable hydrogens

• neutralization reactions

• equivalence point

• standard solution

• titration

• end point

Name ___________________________ Date ___________________ Class __________________

NEUTRALIZATION REACTIONS19.4

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________ 8. A solution of known concentration is called a standard solution.

________ 9. The end point of a titration of a strong base with a strong acid occurswhen [H�] � [OH�].

________ 10. The point of neutralization is the end point of titration.

________ 11. The reaction of an acid and a base produces only water.



17. Complete and balance the equations for the following acid–base reactions.

a. H3PO4 � Al(OH)3

b. HI � Ca(OH)2

Column B

a. when the number of moles of hydrogen ions equalsthe number of moles of hydroxide ions

b. a solution of known concentration

c. a process for determining the concentration of asolution by adding a known amount of a standardsolution

d. point of neutralization

e. reactions between acids and bases to produce a saltand water

Column A

________ 12. titration

________ 13. neutralizationreactions

________ 14. equivalence point

________ 15. standard solution

________ 16. end point

Name ___________________________ Date ___________________ Class __________________©


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Section Review

Objectives• Define when a solution of a salt is acidic or basic

• Demonstrate with equations how buffers resist changes in pH

Vocabulary


A forms when an acid is neutralized by a base. Salts 1.

can be neutral, , or in solutions. Salts of strong 2.

acid–strong base reactions produce solutions with water. 3.

Salts formed from the neutralization of weak acids or weak bases 4.

water. They produce solutions that are acidic or basic. 5.

For example, the pH of a solution at the equivalence point is 6.

greater than 7 for a base- acid titration. Solutions 7.

that resist changes in pH are called solutions. The buffer 8.

is the amount of acid or base that can be added to a buffer 9.

without changing the pH greatly.

9

8

76

5

4

32

1

• salt hydrolysis

• buffers

• buffer capacity

Name ___________________________ Date ___________________ Class __________________

SALTS IN SOLUTION19.5

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________ 10. An aqueous solution of NH4Cl is basic.

________ 11. HCl–NaCl would be a good buffer system.

________ 12. A buffer is a solution of a weak acid and one of its salts.

________ 13. A strong acid and a weak base produce an acidic solution.


Part D QuestionAnswer the following in the space provided.

18. Predict whether an aqueous solution of each salt will be acidic, basic, or neutral.

a. NH4Cl

b. Na2CO3

c. NH4NO3

Column B

a. the cations or anions of a dissociated salt removehydrogen ions from or donate hydrogen ions to water

b. the amount of acid or base that can be added to abuffer solution before a significant change in pH canoccur

c. the salt produced by the titration of ammonia withhydrochloric acid.

d. a solution in which the pH remains relativelyconstant when small amounts of acid or base areadded

Column A

________ 14. salt hydrolysis

________ 15. buffer

________ 16. buffer capacity

________ 17. NH4Cl

Name ___________________________ Date ___________________ Class __________________©


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Practice ProblemsIn your notebook, solve the following problems.

SECTION 19.1 ACID–BASE THEORIES1. Identify the hydrogen ion donor(s) and hydrogen ion acceptor(s) for ionization

of H2SO4 in water. Label the conjugate acid�base pairs.

2. Identify all of the ions that may be formed when H3PO4 ionizes in water.

3. Classify the following acids as monoprotic, diprotic, or triprotic.

a. HCOOH b. HBr c. H2SO3 d. H3ClO4

4. What would you expect to happen when lithium metal is added to water? Showthe chemical reaction.

5. In the following chemical reaction, identify the Lewis acid and base.

BF3 � F� 1 BF4�

6. Describe some distinctive properties of acids.

7. Describe some distinctive properties of bases.

SECTION 19.2 HYDROGEN IONS AND ACIDITY1. A solution has a hydrogen ion concentration of 1 � 10�6M. What is its pH?

2. What is the pH of a solution if the [H�] � 7.2 � 10�9M?

3. What is the pOH of a solution if the [OH�] � 3.5 � 10�2M?

4. What is the pOH of a solution that has a pH of 3.4?

5. Classify each solution as acidic, basic, or neutral.

a. [H�] � 2.5 � 10�9M d. [H�] � 1 � 10�7M

b. pOH � 12.0 e. pH � 0.8

c. [OH�] � 9.8 � 10�11M

6. Calculate the pH of each solution.

a. [H�] � 1 � 10�5M c. [OH�] � 2.2 � 10�7M

b. [H�]� 4.4 � 10�11M d. pOH � 1.4

7. Classify the solutions in problem 6 as acidic or basic.

8. Why is there a minus sign in the definition of pH?

9. A solution has a pOH of 12.4. What is the pH of this solution?

10. What is the pH of a solution with [H�] � 1 � 10�3M?

Name ___________________________ Date ___________________ Class __________________

ACIDS, BASES, AND SALTS19

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SECTION 19.3 STRENGTHS OF ACIDS AND BASES1. Rank 1M of these compounds in order of increasing hydrogen ion

concentration: weak acid, strong acid, strong base, weak base.

2. Write the expression for the acid dissociation constant of the strong acidhydrofluoric acid, HF.

3. Write the expression for the base dissociation constant for hydrazine, N2H4, aweak base. Hydrazine reacts with water to form the N2H5

� ion.

4. Use Table 19.8 in your textbook to rank these acids from weakest to strongest:HOOCCOOH, HCO3

�, H2PO4�, HCOOH.

5. Write the equilibrium equation and the acid dissociation constant for thefollowing weak acids.

a. H2S b. NH4� c. C6H5COOH

6. Match each solution with its correct description.

a. dilute, weak acid (1) 18M H2SO4(aq)

b. dilute, strong base (2) 0.5M NaOH(aq)

c. concentrated, strong acid (3) 15M NH3(aq)

d. dilute, strong acid (4) 0.1M HC2H3O2(aq)

e. concentrated, weak base (5) 0.1M HCl(aq)

7. Write the base dissociation constant expression for the weak base analine,C6H5NH2.

C6H5NH2(aq) � H2O(l) 1 C6H5NH3�(aq) � OH�(aq)

8. A 0.10M solution of formic acid has an equilibrium [H�] � 4.2 � 10�3M.

HCOOH(aq) → H�(aq) � HCOO�(aq)

What is the Ka of formic acid?

9. The Ka of benzoic acid, C6H5COOH, is 6.3 � 10�5. What is the equilibrium [H�]in a 0.20M solution of benzoic acid?

10. A 0.10M solution of hydrocyanic acid, HCN, has an equilibrium hydrogen ionconcentration of 6.3 � 10�6M. What is the Ka of hydrocyanic acid?

Name ___________________________ Date ___________________ Class __________________©


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SECTION 19.4 NEUTRALIZATION REACTIONS1. What is the molarity of a sodium hydroxide solution if 38 mL of the solution is

titrated to the end point with 14 mL of 0.75M sulfuric acid?

2. If 24.6 mL of a Ca(OH)2 solution is needed to neutralize 14.2 mL of 0.0140MHC2H3O2, what is the concentration of the calcium hydroxide solution?

3. A 12.4 mL solution of H2SO4 is completely neutralized by 19.8 mL of 0.0100MCa(OH)2. What is the concentration of the H2SO4 solution?

4. What volume of 0.12M Ba(OH)3 is needed to neutralize 12.2 mL of 0.25M HCl?

5. A 55.0-mg sample of Al(OH)3 is reacted with 0.200M HCl. How many milliters ofthe acid are needed to neutralize the Al(OH)3?

SECTION 19.5 SALTS IN SOLUTION1. A buffer solution is prepared by mixing together equal quantities of formic acid,

HCHO2, and sodium formate, NaCHO2. Write equations that show what happenswhen first acid, and then base, is added to this buffer solution.

2. Complete the following rules.

a. strong acid � strong base y c. weak acid � strong base y

b. strong acid � weak base y

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Figure 1 The pH curve for the titration of a benzoic acid (C6H5COOH) solutionwith a standard solution of 0.10M sodium hydroxide (NaOH).

The plot shown in Figure 1 shows how the pH of a benzoic acid solution of unknownconcentration changes as a function of the volume of 0.10M NaOH added. Thestarting volume of benzoic acid solution was 25 mL. Use this titration curve to answerthe following questions.

1. Write the chemical equation for the reaction of benzoic acid (C6H5COOH) withNaOH. Note that the acidic hydrogen atom in benzoic acid is shown in bold.How many moles of benzoic acid are neutralized per mole of NaOH added?

2. Estimate the pH of the solution at the equivalence point of the titration. Is thesolution acidic, neutral, or basic at the equivalence point?

3. Based on your estimate of the pH at the equivalence point, characterize benzoicacid as a weak acid or a strong acid. Explain your answer.

4. How many moles of NaOH were needed to reach the equivalence point?

2

4

6

8

10

12

14

0 5 10 15 20 25 30 35 40 45 50

pH

0.10M NaOH added (mL)

Name ___________________________ Date ___________________ Class __________________©


INTERPRETING GRAPHICSUse with Section 19.5

19

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5. Define the equivalence point in this reaction. What are [NaOH], [C6H5COOH],and [C6H5COONa] at the equivalence point?

6. What is the concentration of benzoic acid in the original “unknown” solution?

7. Refer to Figure 19.8 in your textbook. Which of the acid–base indicators shownwould be most appropriate for this particular titration? Label the titration curvein Figure 1 to indicate the range of pH values for which your chosen indicator ismost effective.

8. At the equivalence point, the pH of the solution is determined by the hydrolysisof the sodium benzoate salt, C6H5COONa. Write the chemical equation showingthe hydrolysis of water by the benzoate ion (C6H5COO�). How does thisequation support your answer to question 2?

9. Use your answer to question 8 to write the base dissociation constant (Kb)expression for the reaction of benzoate ion with water.

10. Based on your estimate of the pH at the equivalence point and using theexpression for Kb, determine the numerical value of Kb for the benzoate ion(C6H5COO�).

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Name ___________________________ Date ___________________ Class __________________

Vocabulary ReviewFrom each group of terms, choose the term that does not belong and then explain your choice.

1. basic, neutral, acidic, hydronium ion

2. acidic solution, hydroxide ion, basic solution, alkaline solution

3. Arrhenius, Brønsted-Lowry, Lewis, amphoteric

4. conjugate acid, Brønsted-Lowry, Lewis acid, conjugate base

5. weak bases, weak acids, strong acids, dissociation constant

Choose the term from the following list that best matches each description.

equivalence point neutral

hydrolyzing salts buffer

______________________ 6. compounds derived from the reaction of a strong base with a weak acid or from the reaction of a strong acid with a weak base

______________________ 7. a term used to describe the pH of a solution that results when one equivalent of a strong acid is mixed with one equivalent of a strong base

______________________ 8. the point of neutralization in a titration

______________________ 9. a solution that consists of a weak acid and one of its salts, or a solution of a weak base and one of its salts

© Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved.


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Chapter QuizChoose the best answer and write its letter on the line.

________ 1. A solution in which the hydroxide-ion concentration is 1 � 10�2 is 19.2a. acidic. c. neutral.b. basic. d. none of the above

________ 2. What is the pH of a solution in which [OH�] � 1 � 10�5? 19.2a. 5.0 c. �5.0b. 9.0 d. �9.0

________ 3. If the [H�] in a solution is 1 � 10�3 mol/L, then the [OH�] is 19.2a. 1 � 10�11 mol/L. c. 1 � 10�13 mol/L.b. 1 � 10�17 mol/L. d. cannot be determined

________ 4. In the reaction: 19.1

CO32� � H2O 1 HCO3

� � OH�

the carbonate ion is acting as a(n)a. Arrhenius base. c. Brønsted-Lowry base.b. Arrhenius acid. d. Brønsted-Lowry acid.

_________ 5. Identify the Brønsted-Lowry base and conjugate base in this reaction. 19.1

H2S � H2O 1 H3O� � HS�

a. H2S and H2O c. HS� and H2Ob. H2S and H3O� d. HS� and H3O�

________ 6. For the reaction HX 1 H� � X�, the equilibrium concentrations 19.3are as follows.

[HX] � 1 � 10�1; [H�] , [X�] � 1 � 10�5

Ka would be:a. 1 � 109. c. 1 � 10�7.b. 1 � 10�11. d. 1 � 10�9.

________ 7. The reaction that takes place when an acid is added to an ethanoic 19.5acid-ethanoate (CH3COOH/CH3COO�) buffer isa. CH3COO� � H� 1 CH4 � CO2

b. CH3COOH � H� 1 CH3COO� � H�

c. CH3COO� � H� 1 CH3COOHd. CH3COOH � OH� 1 CH3COO� � H2O

________ 8. Which salt hydrolyzes water to form a solution that is acidic? 19.5a. LiBr c. NaBrb. NH4Br d. KBr

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Chapter Test A

A. MatchingMatch each term in Column B with the correct description in Column A. Write theletter of the correct term on the line.

B. Multiple ChoiceChoose the best answer and write its letter on the line.

________ 11. A solution in which the hydroxide-ion concentration is 1 � 10�5M isa. acidic. c. neutral.b. basic. d. none of the above

________ 12. In a neutral solution, the [H�] isa. 10�14. c. 1 � 107M.b. zero. d. equal to [OH�].

________ 13. The products of the self-ionization of water area. H3O7

� and H2O. c. OH� and H�.b. HO� and OH�. d. OH� and H�.

Column B

a. acidic solution

b. conjugate acid–base pair

c. amphoteric

d. alkaline solution

e. Kw

f. end point

g. neutral solution

h. hydronium ion

i. Ka

j. salt hydrolysis

Column A

________ 1. acid dissociation constant

________ 2. [H�] greater than [OH�]

________ 3. The cations or anions of a dissociated salt removehydrogen ions from or donate hydrogen ions towater.

________ 4. point of neutralization of the titration

________ 5. H3O�

________ 6. [OH�] and [H�] � 1 � 10�7

________ 7. [OH�] greater than [H�]

________ 8. ion-product constant for water

________ 9. describes a substance that can act as both an acidand a base

________ 10. two substances that are related by the loss or gainof a single hydrogen ion

Name ___________________________ Date ___________________ Class __________________©



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________ 14. Which of these solutions is most basic?a. [H�] � 1 � 10�11 c. [H�] � 1 � 10�2

b. [OH�] � 1 � 10�4 d. [OH�] � 1 � 10�13

________ 15. The formula of the hydrogen ion is often written asa. H2O�. c. H�.b. OH�. d. H3O�.

________ 16. What is the pH of a solution in which the [H�] � 1 � 10�12?a. �1.0 c. 2.0b. �2.0 d. 12.0

________ 17. What is the pH of a 0.01M hydrochloric acid solution?a. 10�2 c. 2.0b. 12.0 d. 10�12

________ 18. The Ka of carbonic acid is 4.3 � 10�7.

H2CO3 1 H� � HCO3�

This means that H2CO3 is aa. good hydrogen-ion acceptor.b. poor hydrogen-ion acceptorc. good hydrogen-ion donor.d. poor hydrogen-ion donor.

________ 19. Which of the following pairs consist of a weak acid and a strong base?a. ethanoic acid, sodium hydroxideb. ethanoic acid, calcium hydroxidec. sulfuric acid, sodium hydroxided. ethanoic acid, ammonia

________ 20. In the reaction NH4� � H2O 1 NH3 � H3O�, water is acting as a(n)

a. Arrhenius acid. c. Brønsted-Lowry acid.b. Brønsted-Lowry base. d. Arrhenius base.

________ 21. A solution with a pH of 5.0a. is basic.b. has a hydrogen-ion concentration of 5.0M.c. is neutral.d. has a hydroxide-ion concentration of 1 � 10�9M.

________ 22. With solutions of strong acids and strong bases, the word strong refers toa. molality. c. solubility.b. molarity. d. degree of ionization.

________ 23. The hydrolysis of water by the salt of a weak base and a strong acidshould produce a solution that isa. weakly basic. c. strongly basic.b. neutral. d. acidic.

________ 24. Which of these is an Arrhenius base?a. KOH c. H2PO4

�

b. NH3 d. CH3COOH

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________ 25. Which of these acids is monoprotic?a. CH3COOH c. H2SO4

b. H2CO3 d. H3PO4

________ 26. A solution that contains one mole of Ca(OH)2 and one mole of H2SO4 isa. CaSO4 � H3O� � H2O. c. CaH2 � H3SO4. b. CaSO4 � H3O� � OH�. d. CaSO4 � 2H2O.

________ 27. According to the Brønsted-Lowry theory, watera. acts as a base when it accepts a hydrogen ion.b. can be neither an acid nor a base.c. acts as an acid by accepting hydrogen ions.d. can accept but not donate hydrogen ions.

________ 28. What are the Brønsted-Lowry acids in this equilibrium reaction?

CN� � H2O 1 HCN � OH�

a. H2O, OH� c. H2O, HCNb. CN�, OH� d. CN�, H2O

________ 29. A solution of one of the following compounds is acidic because one ofits ions undergoes hydrolysis. The compound isa. KCl. c. CH3COOK.b. NH4Cl. d. NH3.

C. ProblemsSolve the following problems in the space provided. Show your work.

30. Calculate the pH for the following solutions. State whether each solution isacidic, basic, or neutral.

a. [H�] � 1 � 10�9

b. [OH�] � 1 � 10�10

c. [H�] � 1 � 10�7

31. Calculate the hydrogen-ion concentration [H�] for an aqueous solution inwhich [OH�] is 1 � 10�12 mol/L. Is this solution acidic, basic, or neutral?

Name ___________________________ Date ___________________ Class __________________©


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32. Write the expression for Ka for each acid. Assume that only one hydrogen isionized in each case.

a. H2SO3

b. HNO3

33. Write complete and balanced equations for each of the following acid–basereactions.

a. HBr � Mg(OH)2y

b. H2SO4 � Al(OH)3y

34. Predict whether an aqueous solution of each salt will be acidic, basic, or neutral.

a. Na2CO3 c. (NH4)SO4

b. KNO3 d. Mg(C2H3O2)2

D. EssayWrite a short essay for the following.

35. Compare and contrast the properties of acids and bases.

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Chapter Test B

A. MatchingMatch each term in Column B with the correct description in Column A. Write theletter of the correct term on the line.

B. Multiple ChoiceChoose the best answer and write its letter on the line.

________ 12. Which of the following is true about acids?a. Acids give foods a bitter taste.b. Aqueous solutions of acids conduct electricity.c. Acids have a pH value greater than 7.d. all of the above

Column B

a. the ion-productconstant for water

b. Lewis base

c. acid

d. conjugate acid

e. neutralizationreaction

f. Lewis acid

g. base

h. diprotic acid

i. amphoteric

j. titration

k. equivalence point

Column A

________ 1. a substance that can donate a pair of electrons to form acovalent bond

________ 2. a compound that produces hydroxide ions whendissolved in water

________ 3. the particle formed when a weak base gains a hydrogenion

________ 4. 1.0 � 10�14 (mol/L)2

________ 5. a substance that can accept a pair of electrons to form acovalent bond

________ 6. a compound that produces hydrogen ions whendissolved in water

________ 7. H2SO4

________ 8. when the number of moles of hydrogen ions equals thenumber of moles of hydroxide ions in titration

________ 9. describes a substance that can act as both an acid and abase

________ 10. the process of adding a known amount of solution ofknown concentration to determine the concentration ofanother solution

________ 11. reactions in which an acid and a base react in anaqueous solution to produce a salt and water

Name ___________________________ Date ___________________ Class __________________©



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________ 13. The products of the neutralization reaction between HNO2(aq) andCa(OH)2(aq) area. CaNO3 � H2O. c. CaNO3 � 2H2O.b. Ca(NO3)2 � H2O. d. Ca(NO3)2 � 2H2O.

________ 14. A solution in which the [H�] is 1.0 � 10�4 mol/L is said to bea. acidic. c. neutral.b. basic. d. none of the above

________ 15. What is the pH of the solution in question 14?a. 1.00 c. 10.00b. 4.00 d. 14.00

________ 16. A solution with a pH of 9 has a [OH�] concentration ofa. 1.0 � 10�14 mol/L. c. 1.0 � 10�5 mol/L.b. 1.0 � 10�9 mol/L. d. 1.0 � 10�7 mol/L.

________ 17. Among the following, which solution is the most acidic?a. [H�] � 1 � 10�5 mol/L c. [OH�] � 1 � 10�7 mol/Lb. pH � 3 d. pH � 10

________ 18. The monoprotic acid from among the following isa. H2CO3. c. H3PO4.b. H2SO4. d. HCl.

________ 19. The Brønsted-Lowry theory defines an acid as a(n)a. hydrogen ion donor. c. electron-pair donor.b. hydrogen ion acceptor. d. electron-pair acceptor.

________ 20. Which of the following is true about neutralization reactions?a. They involve strong acids and strong bases.b. They result in the production of a salt and water.c. They are all double-replacement reactions.d. all of the above

________ 21. In the reaction: HCl(g) � NH3(aq) → NH4�(aq) � Cl�(aq), HCl(g) is

acting as a(n):a. Brønsted-Lowry acid. c. Lewis acid.b. Brønsted-Lowry base. d. Lewis base.

________ 22. The conjugate acid in the reaction described in question 21 isa. HCl(g). c. NH44

�(aq).b. NH3(aq). d. Cl�(aq).

________ 23. Which of the following is true about indicators?a. They are weak acids or bases.b. They are as accurate as a pH meter.c. They maintain their colors across the range of pH values for

which they are used.d. all of the above

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________ 24. What is the Lewis acid in the following reaction?

NH3 � BI3 → I3BNH3

a. NH3 c. I3BNH3

b. BI3 d. none of these

________ 25. Among the following Ka values, which represents the strongest acid?a. Ka � 1.2 � 10�3 c. Ka � 8.7 � 10�8

b. Ka � 3.4 � 10�5 d. Ka � 5.8 � 10�10

________ 26. How many moles of Mg(OH)2(aq) would be required to neutralize 3.0mol HCl(aq)?a. 1.5 mol c. 6.0 molb. 3.0 mol d. 2.0 mol

C. ProblemsSolve the following problems in the space provided. Show your work.

27. Calculate the [OH�] for an aqueous solution in which [H�] � 1.0 � 10�9 mol/L.Is the solution acidic, basic, or neutral?

28. For each of the following, fill in the concentration of the requested ion, the pH,and the type of solution (acid, base, or neutral).

29. Write the expression for Ka for each of the following acids. Assume that only onehydrogen is ionized.

a. HI

b. H2SO4

30. Write complete and balanced equations for each of the following neutralizationreactions:

a. HF(aq) � KOH(aq) y

b. H2SO4(aq) � LiOH(aq) y

31. How many moles of sulfuric acid would be required to neutralize 0.35 mol of KOH?

Name ___________________________ Date ___________________ Class __________________©


Concentration pH Solution Type

a. [H�] � 1 � 10�3 [OH�] �

b. [OH�] � 1 � 10�8 [H�] �

c. [H�] � [OH�] [H�] �

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32. If the Ksp for a CuCl solution is 3.2 � 10�7, what is the concentration of Cu and of Cl ions atequilibrium?

D. EssayWrite a short essay for the following.

33. Distinguish between the Brønsted-Lowry and Lewis theories of acids and bases.

E. Additional ProblemsSolve the following problems in the space provided. Show your work.

34. Determine the pH of a solution whose [H�] � 3.4 � 10�4 mol/L. Is the solutionacidic, basic, or neutral?

35. Use the Brønsted-Lowry definitions of acids and bases to identify the acid, base,conjugate acid, and conjugate base in each of the following reactions.

a. HF(aq) � H2O(l) 1 H3O�(aq) � F�(aq)

b. HCl(g) � H2O(l)1 H3O�(aq) � Cl�(aq)

c. HC2H3O2(aq) � H2O(l) 1 H3O�(aq) � C2H3O2�(aq)

36. Identify the Lewis acids and bases in the following reactions:

37. A 0.1000M solution of ethanoic acid (HC2H3O2) is only partially ionized so that[H�] � 2.25 � 10�3M. What is the acid dissociation constant for this acid?

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Acid Base Conjugate Acid Conjugate Base

a.

b.

c.

Lewis Acid Lewis Base

a. H� � I� → HI

b. NH3 � BCl3 → Cl3BNH3

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05 CTR ch19 7/12/04 8:16 AM Page 487 ACID-BASE THEORIES 19hs.pequannock.org/ourpages/auto/2012/9/6/56236270/Chapter 19 St… · In the Lewis theory, an acid is an 5. acceptor. A Lewis