Homework answers / question archive / Chapter 15 Acids and Bases: A Second Look Multiple Choice 1)The conjugate acid of HPO42- is H2PO4 H3PO4 PO43- PO42- e

Chapter 15 Acids and Bases: A Second Look Multiple Choice 1)The conjugate acid of HPO42- is H2PO4 H3PO4 PO43- PO42- e

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Chapter 15 Acids and Bases: A Second Look

Multiple Choice

1)The conjugate acid of HPO₄^2- is

1. 1. H₂PO₄
  2. H₃PO₄
  3. PO₄^3-
  4. PO₄^2- e. H₂PO₄^-

The conjugate base of HPO₄^2- is

1. 1. H₂PO₄
  2. H₃PO₄

c. PO₄^3- d. PO₄^2-

1. 1. H₂PO₄^-

The conjugate base of H₂SO₄ is

1. 1. SO₄^2-
  2. H₃O⁺
  3. OH^- d. HSO₄^-

e. H₂SO₃

The conjugate base of H₂AsO₄^- is

1. 1. H₂AsO₄
  2. H₃AsO₄
  3. HAsO₄^- d. HAsO₄^2- e. AsO₄^3-

The conjugate acid of NH₃ is

1. 1. NH₄
  2. NH₃⁺
  3. H⁺
  4. H₃O⁺ e. NH₄⁺
The conjugate acid of H₂AsO₄^- is

a. H₂AsO₄ b. H₃AsO₄ c. HAsO₄^-

1. 1. HAsO₄^2-
  2. AsO₄^3-

Which species is amphiprotic?

1. 1. PO₄^3-(aq)
  2. HCl(g) c. HSO₄^-(aq) d. Cl^-(aq)

e. CO₃^2-(aq)

Which species is amphoteric?

1. 1. HNO₃(aq)
  2. Cl^-(g)
  3. CO₃^2-(aq) d. HSO₃^-(aq) e. PO₄^3-(aq)

Which species is amphiprotic?

1. 1. AsO₄^3-(aq)
  2. HBr(aq)
  3. HF(aq)
  4. SO₄^2-(aq)
2. e. HCO₃^-(aq)

Which species does not have a conjugate base?

1. 1. H₂O
  2. H₃O⁺
  3. NH₂^-
  4. OH^- e. F^-

Which species has a conjugate base?

1. 1. Cl^-
  2. SO₄^2-
  3. CN^- d. OH^-

e. CO₃^2-

In the reaction, HClO₃ + N₂H₄ ClO₃^- + N₂H₅⁺, which species are an acid-base pair?

1. 1. HClO₃, N₂H₄
  2. N₂H₄, ClO₃^-
  3. HClO₃, N₂H₅⁺
2. d. N₂H₄, N₂H₅⁺
  1. ClO₃^-, N₂H₅⁺

In the reaction, HClO₃ + N₂H₄ ClO₃^- + N₂H₅⁺, two species are both acids?

1. 1. HClO₃, N₂H₄
  2. HClO₃, ClO₃^- c. HClO₃, N₂H₅⁺ d. N₂H₄, N₂H₅⁺

e. ClO₃^-, N₂H₅⁺

In the reaction, HClO₃ + N₂H₄ ClO₃^- + N₂H₅⁺, which two species are both bases?

1. 1. HClO₃, N₂H₄
  2. HClO₃, ClO₃^-
  3. HClO₃, N₂H₅⁺
  4. N₂H₄, N₂H₅⁺
2. e. ClO₃^-, N₂H₄

In the reaction, H₂PO₄^- + HAsO₄^2- HPO₄^2- + H₂AsO₄^-, which species are a conjugate acidbase pair?

1. 1. H₂PO₄^-, HAsO₄^2-
  2. H₂PO₄^-, H₂AsO₄^-
2. c. H₂PO₄^-, HPO₄^2-
  1. HAsO₄^2-, HPO₄^2-
  2. HPO₄^2-, H₂AsO₄^-

16. In the reaction, H₂PO₄ + HAsO₄

a. H₂PO₄^-, HAsO₄^2- b. H₂PO₄^-, H₂AsO₄^- c. H₂PO₄^-, HPO₄^2-

HAsO₄^2-, HPO₄^2-
HPO₄^2-, H₂AsO₄^-

HPO₄ + H₂AsO₄, which two species are both acids?

- - - ^2- ^{2- -}

17. In the reaction, H₂PO₄ + HAsO₄

H₂PO₄^-, HAsO₄^2-
H₂PO₄^-, H₂AsO₄^-
H₂PO₄^-, HPO₄^2- d. HAsO₄^2-, HPO₄^2- e. HPO₄^2-, H₂AsO₄^-

HPO₄ + H₂AsO₄, which two species are both bases?

- - - ^2- ^{2- -}

18. In the reaction, HSO₄ + HS

1. HSO₄^-, HS^-
2. HSO₄^-, H₂S

c. HS^-, H₂S

HS^-, SO₄^2-
H₂S, SO₄^2-

H₂S + SO₄, which species are a conjugate acid-base pair?

- - - ^- ^2-
In the reaction, HSO₄^- + HS^- H₂S + SO₄^2-, which two species are both acids?

a. HSO₄^-, HS^- b. HSO₄^-, H₂S c. HS^-, H₂S

1. HS^-, SO₄^2-
2. H₂S, SO₄^2-

In the reaction, HSO₄^- + HS^-

1. HSO₄^-, HS^--
2. HSO₄^-, H₂S
3. HS^-, H₂S d. HS^-, SO₄^2-

e. H₂S, SO₄^2-

H₂S + SO₄^2-, two species are both bases?

In the reaction, HSO₄^- + CN^-HCN + SO₄^2-, which species are a conjugate acid-base pair?

a. HSO₄^-, CN^- b. CN^-, HCN c. CN^-, SO₄^2-

1. HCN, SO₄^2-
2. HCN, HSO₄^-

In the reaction, HSO₄^- + CN^- ≡ HCN + SO₄^2-, which two species are both acids?

a. HSO₄^-, CN^- b. HSO₄^-, HCN c. CN^-, HCN

1. CN^-, SO₄^2-
2. SO₄^2-, HCN

In the reaction, HSO₄^- + CN^-HCN + SO₄^2-, which two species are both bases?

1. HSO₄^-, CN^-
2. HSO₄^-, HCN
3. SO₄^2-, HCN
4. CN^-, HCN e. CN^-, SO₄^2-

Which is the strongest oxyacid?

1. O

H?O?X?O?H

1. O ?

H?O?X?O?H

O?H

c. O

X?O?H

? O

d. O

? H?O?X?O?H

? H

e. O ?

H?O?X?H

? H

25. Which is the strongest oxyacid?

H?O?X?O?H

X?O?H

? O

H?O?X?O?H

? O

d. O

H?O?X?O

? O

e. O

H?O?X?O?H

? H

26. For the system

NH₂OH + CH₃NH₃⁺CH₃NH₂ + NH₃OH⁺

the position of the equilibrium lies to the left. Which is the strongest acid in the system?

NH₂OH
CH₃NH₃⁺
CH₃NH₂

d. NH₃OH⁺

e. NH₂OH and CH₃NH₃⁺ are equal in acid strength, and are the strongest acids in the system

Which is the weakest oxyacid?

a. O

H?O?X?O?H

b. O?H

H?O?X?O?H

O?H

1. O

X?O?H

? O

1. O ?

H?O?X?O?H

1. O

H?O?X?O

For the system

NH₂OH + CH₃NH₃⁺CH₃NH₂ + NH₃OH⁺

the position of the equilibrium lies to the left. Which is the weakest base in the system?

a. NH₂OH

CH₃NH₃⁺
CH₃NH₂
NH₃OH⁺
CH₃NH₂ and NH₃OH⁺ are equal in base strength and are the weakest bases in the system

Which is the strongest oxyacid?

1. 1. O

X?O?H

? O

1. 1. O ?

H?O?X?O?H

? O

c. O ?

H?O?X?O

? O

1. 1. O ?

H?O?X?O?H

? H

1. 1. O ?

H?O?X?H

? H

Which species is the most acidic?

1. 1. HClO
  2. HClO₂
  3. HClO₃ d. HClO₄ e. Cl^-
Given the following substances in order of increasing acid strength,

HOCl(aq) < HC₂H₃O₂(aq) < HC₂O₄^-(aq) < HOCN(aq) < HNO₂(aq) < HCl(aq)

Which species listed below is the strongest base?

a. Cl^-(aq) b. OCl^-(aq)

1. 1. H₂C₂O₄(aq)
  2. NO₂^-(aq)
  3. OCN^-(aq)

Given the following substances in order of increasing acid strength,

HOCl(aq) < HC₂H₃O₂(aq) < HC₂O₄^-(aq) < HOCN(aq) < HNO₂(aq) < HCl(aq)

Which species listed below is the weakest base of that set?

1. 1. C₂H₃O₂^-(aq)
  2. OCl^-(aq)
  3. H₂C₂O₄(aq)

d. Cl^-(aq)

1. 1. OCN^-(aq)

Given the following substances in order of increasing acid strength,

HOCl(aq) < HC₂H₃O₂(aq) < HC₂O₄^-(aq) < HOCN(aq) < HNO₂(aq) < HCl(aq)

Which species listed below is the strongest base of that set?

1. 1. Cl^-(aq)
  2. HOCl(aq) c. C₂O₄^2-(aq) d. NO₂^-(aq)

e. OCN^-(aq)

Given the following substances in order of increasing acid strength,

HOCl(aq) < HC₂H₃O₂(aq) < HC₂O₄^-(aq) < HOCN(aq) < HNO₂(aq) < HCl(aq)

Which species listed below is the weakest base of that set?

1. 1. C₂H₃O₂^-(aq)
  2. OCl^-(aq)
  3. HC₂O₄^-(aq)
  4. HNO₂(aq)

e. OCN^-(aq)

Which species is the weakest acid?

1. 1. HBr
  2. HCl c. HF d. HI

Which species is the strongest acid?

1. 1. H₂O
  2. H₂S
  3. H₂Se

d. H₂Te

NH₃ can react with BF₃, forming NH₃?BF₃. In this reaction,

1. 1. the NH₃ acts as a Brønsted base, accepting a proton from the BF₃ molecule.
  2. the NH₃ acts as a Lewis base, donating a proton to the BF₃ molecule.
  3. the NH₃acts as a Brønsted acid, donating a proton to the BF₃ molecule.

d. the BF₃ molecule acts as a Lewis acid, accepting an electron pair from the NH₃ molecule to form a coordinate covalent bond.

1. 1. the BF₃ molecule acts as a Lewis base, donating an electron pair to the NH₃ molecule to form a coordinate covalent bond.

SO₂ can react with OH^-, forming HSO₃^-. In this reaction,

1. 1. the SO₂ acts as a Brønsted acid, accepting a proton from the OH^- ion.
  2. the SO₂ acts as a Lewis acid, accepting a proton from the OH^- ion.
  3. the OH^- ion acts as a Brønsted base, donating a proton to the SO₂ molecule.

d. the OH^- ion acts as a Lewis base, donating an electron pair to the SO₂ molecule to form a coordinate covalent bond.

1. 1. the OH^- ion acts as a Lewis acid, accepting an electron pair from the SO₂ molecule to form a coordinate covalent bond.

F^- ion can react with BF₃, forming the BF₄^- anion. In this reaction,

1. 1. the F^- ion acts as a Brønsted base, accepting a proton from the BF₃ molecule.
  2. the F^- ion acts as a Lewis base, donating a proton to the BF₃ molecule.

1. 1. the F^- ion acts as a Brønsted acid, donating a proton to the BF₃ molecule.

d. the BF₃ molecule acts as a Lewis acid, accepting an electron pair from the F^- ion to form a coordinate covalent bond.

1. 1. the BF₃ molecule acts as a Lewis base, donating an electron pair to the F^- ion to form a coordinate covalent bond.

CO₂ can react with OH^-, forming HCO₃^-. In this reaction,

1. 1. the CO₂ acts as a Brønsted acid, accepting a proton from the OH^- ion.
  2. the CO₂ acts as a Lewis acid, accepting a proton from the OH^- ion.
  3. the OH^- ion acts as a Brønsted base, donating a proton to the CO₂ molecule.
  4. the OH^- ion acts as a Lewis acid, accepting an electron pair from the CO₂ molecule to form a coordinate covalent bond.

e. the OH^- ion acts as a Lewis base, donating an electron pair to the CO₂ molecule to form a coordinate covalent bond.

Which pair of reactants will yield H₂SO₄ as one of its products?

1. 1. SO₂ + OH^-
  2. SO₃ + OH^-
  3. SO₂ + H₂O
  4. SO₄^2- + OH^-

e. SO₃ + H₂O

Which pair of reactants will yield H₂SO₃ as one of its products?

1. 1. SO₂ + OH^-
  2. SO₃ + OH^- c. SO₂ + H₂O

1. 1. SO₄^2- + OH^-
  2. SO₃ + H₂O

Which solution will have the lowest pH?

a. Al(NO₃)₃(aq)

1. 1. Ca(NO₃)₂(aq)
  2. KNO₃(aq)
  3. Mg(NO₃)₂(aq)
  4. Zn(NO₃)₂(aq)

Which solution will have the highest pH?

1. 1. Al(NO₃)₃(aq)
  2. Ga(NO₃)₃(aq)

c. AgNO₃(aq)

1. 1. Cu(NO₃)₂(aq)
  2. Zn(NO₃)₂(aq)

Which solution will have the lowest pH?

1. 1. Zn(NO₃)₂(aq)
  2. Cd(NO₃)₂(aq)
  3. Ga(NO₃)₃(aq)
  4. Hg(NO₃)₂(aq)

e. Al(NO₃)₃(aq)

Which will have the highest pH?

1. 1. Al(NO₃)₃(aq)
  2. Cd(NO₃)₂(aq)
  3. Ga(NO₃)₃(aq)

d. KNO₃(aq)

1. 1. Zn(NO₃)₂(aq)

Five solutions were prepared by dissolving 0.00100 mole of each of the following compounds in enough water to make 1.000 liter of solution. Which one of the solutions would you expect to be the most acidic? The one made with

1. 1. CO₂
  2. P₄O₆
  3. P₄O₁₀
  4. SO₂ e. SO₃

Five solutions were prepared by dissolving 0.00100 mole of each of the following in enough water to make 1.000 liter of solution. Which one of the solutions would you expect to be the most acidic? The one made with

1. 1. Na₂O
  2. BaO
  3. Ga₂O₃
  4. Al₂O₃

e. P₄O₆

Which solution should be the most acidic?

a. Al(NO₃)₃(aq)

1. 1. Ca(NO₃)₂(aq)
  2. KNO₃(aq)
  3. Mg(NO₃)₂(aq)
  4. Zn(NO₃)₂(aq)

Which solution should be the least acidic?

1. 1. Al(NO₃)₃(aq)
  2. Ga(NO₃)₃(aq)

c. AgNO₃(aq)

1. 1. Cu(NO₃)₂(aq)
  2. Zn(NO₃)₂(aq)

Which solution should be the most acidic?

1. 1. Zn(NO₃)₂(aq)
  2. Cd(NO₃)₂(aq)
  3. Ga(NO₃)₃(aq)
  4. Hg(NO₃)₂(aq)

e. Al(NO₃)₃(aq)

Which solution should be the least acidic?

1. 1. Al(NO₃)₃(aq)
  2. Cd(NO₃)₂(aq)
  3. Ga(NO₃)₃(aq)

d. KNO₃(aq)

1. 1. Zn(NO₃)₂(aq)

Five solutions were prepared by dissolving 0.00100 mole of each of the following in enough water to make 1.000 liter of solution. Which one of the solutions would you expect to have the lowest pH? The one made with

1. 1. CO₂
  2. P₄O₆
  3. P₄O₁₀
  4. SO₂ e. SO₃

Five solutions were prepared by dissolving 0.00100 mole of each of the following in enough water to make 1.000 liter of solution. Which one of the solutions would you expect to have the lowest pH? The one made with

1. 1. Na₂O
  2. BaO
  3. Ga₂O₃
  4. Al₂O₃

e. P₄O₆

An aqueous solution at 25.0 ^°C has an H⁺ concentration of 4.0 x 10^-2 molar. What is the OH^- concentration in the same solution, in moles per liter?

1. 1. 4.0 x 10^-2
  2. 4.0 x 10^-9
  3. 4.0 x 10^-12

d. 2.5 x 10^-13 e. 25.0

If the H⁺ ion concentration in an aqueous solution at 25.0 ^°C has a value of 0.100 molar, then the OH^- concentration in moles per liter is

1. 1. 0.100
  2. 1.0 x 10^-7
  3. 10 x 10^-12 d. 1.0 x 10^-13 e. 4.0 x 10¹²

If the H⁺ ion concentration in an aqueous solution at 25.0 ^°C has a value of 0.100 molar, then the pOH of the solution is

1. 1. 1.00
  2. 7.00
  3. 12.00 d. 13.00 e. 11.40

If the H⁺ ion concentration in an aqueous solution at 25.0 ^°C has a value of 0.100 molar, then the pH of the solution is

1. 1. -1.00
  2. 0.100 c. 1.00 d. 6.90

e. 13.00

If the OH^- ion concentration in an aqueous solution at 25.0 ^°C is 6.6 x 10^-4 M, then the H⁺ concentration in moles per liter in the same solution is

1. 1. 1.5 x 10^-1
  2. 1.5 x 10^-4
  3. 6.6 x 10^-10 d. 1.5 x 10^-11 e. 6.6 x 10^-11

If the OH^- ion concentration in an aqueous solution at 25.0 ^°C is 3.4 x 10^-3 M, then the H⁺ concentration in moles per liter in the same solution is

a. 2.9 x 10^-3 b. 2.9 x 10^-12 c. 3.4 x 10^-17

1. 1. 5.8 x 10^-9
  2. 6.6 x 10^-10

If the H⁺ ion concentration in an aqueous solution at 25.0 ^°C is measured as 6.6 x 10^-4 M, then the pH is

a. 3.00

b. 3.18 c. 6.60

1. 1. 9.55
  2. 10.82

If the OH^- ion concentration in an aqueous solution at 25.0 ^°C is measured as 3.4 x 10^-3 M, then the pH is

1. 1. 2.47
  2. 7.22
  3. 8.24 d. 11.53 e. 16.47 Section 15.5
Calculate the pH of a mixture made by adding 50.0 mL of 0.20 M HCl(aq) to 150.0 mL of water if the temperature of the mixture is 25.0 ^°C.

1. 1. 0.70
  2. 1.00
  3. 1.18 d. 1.30

e. 13.00

Calculate the pH of a 0.020 M solution of Ca(OH)₂ whose temperature is 25.0 ^°C.

1. 1. 1.40
  2. 0.040
  3. 1.69 d. 12.60

e. 12.30

A mixture is made by adding 50.0 mL of 0.20 M NaOH(aq) to 50.0 mL of water. At 25.0 ^°C, what is its pH?

1. 1. 1.00
  2. 4.55
  3. 7.00 d. 13.00 e. 13.30

Fill in the Blanks

What is the formula for the conjugate base of NH₃(aq)? _____

What is the formula for the conjugate acid of the OH^-(aq) ion? _____

The strongest base that can exist in aqueous solution is _____.

The strongest acid that can exist in aqueous solution is _____.

Which one of the two species, H₂Se or H₃As, is the stronger Brønsted acid? _______

Which one of the two species, HF(aq) or HI(aq), is the weaker Brønsted acid? _______

Which one of the two species, H₂S or HBr, is the stronger Brønsted acid? _______

Three oxyacids with the formulas shown are listed in order of decreasing acid strength:

HZO₃ > HYO₃ > HXO₃

What is the formula for the strongest conjugate base of these acids? ______

74. Three binary acids with the formulas shown are listed in order of decreasing acid strength:

HZ > HY > HX

What is the formula for the strongest conjugate base of these acids? ______

The sulfide ion can react with the sulfur trioxide molecule to produce a thiosulfate ion, as shown below.

? ?

S^2- + S?O → S—S—O

? ?

O O

Which reagent is the Lewis base, if any? _____

Selenium atoms can react with the sulfite ion to produce a selenosulfate ion, as shown below

2- 2-

? ?

Se + :S—O → Se—S—O

? ?

O O

Which reagent is the Lewis base, if any? _______

The oxide ion can react with the carbon dioxide molecule to produce a carbonate ion, as shown below.

O	O
?	?
O^2- + C →	O—C
?	?
O	O

Which reagent, if any, is the Lewis acid? _______

Which solution is more acidic, AlCl₃(aq) or InCl₃(aq)? _____

At a temperature of 50.0 °C, the value of the ion product constant for H₂O is 5.5 x 10^-14. What is the [H⁺] ion in pure water at this temperature? ______

True and False

The conjugate acid of HCl(aq) is H⁺(aq). ___

The conjugate base of NH₃ is NH₄OH(aq). ___

The conjugate acid of Cl^-(aq) is HCl(aq). ___

NH₄Cl(aq) is one of the conjugate bases of Cl^-(aq) ___

The H₂PO₄^-(aq) ion is amphiprotic in water solution. ___

O^2- ion is produced by the dissociation of MgO when it is dissolved in water. The O^2- ion acts as a strong acid. ___

The ion product constant for water, K_w, varies with the temperature of the water. ___

Critical Thinking Questions

At 60 ^°C the value of K_w is 9.5 x 10^-14. Considering this, what is the calculated value for the pOH of a 2.00 x 10^-3 M HCl(aq) solution at this temperature?

1. 2.70
2. 6.51 c. 10.32 d. 11.30

e. 13.02

At 60 ^°C the value of K_w is 9.5 x 10^-14. Considering this, what is the calculated value for the pH of a 5.00 x 10^-2 M Ba(OH)₂(aq) solution at this temperature?

1. 1.00
2. 1.30 c. 12.02 d. 12.70

e. 13.00

At 60 ^°C the value of K_w is 9.5 x 10^-14. Considering this, what is the calculated value for the pOH of pure water this temperature?

a. 6.02

b. 6.51

1. 7.00
2. 7.49
3. 9.50

At 60 ^°C the value of K_w is 9.5 x 10^-14. Considering this, what is the calculated value for the pH of a solution made by dissolving 1.00 g of sodium hydroxide in enough water to make 500 ml of solution at this temperature? _________

Short answer

91. Explain how NH₃ can be both a Bronsted base and a Lewis base, at the same time.

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Chapter 15 Acids and Bases: A Second Look Multiple Choice 1)The conjugate acid of HPO42- is H2PO4 H3PO4 PO43- PO42- e

Chemistry

? H

? H

? O

? O

? H

NH₂OH + CH₃NH₃⁺CH₃NH₂ + NH₃OH⁺

NH₂OH + CH₃NH₃⁺CH₃NH₂ + NH₃OH⁺

Fill in the Blanks

HZO₃ > HYO₃ > HXO₃

HZ > HY > HX

True and False

Critical Thinking Questions