Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
9th Edition
ISBN: 9781133949640
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
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Chapter 16, Problem 8PS

In each of the following acid-base reactions, identify the Brønsted acid and base on the left and their conjugate partners on the right.

  1. (a) C2H5N(aq) + CH3CO2H(aq) ⇄ C5H5NH+(aq) + CH3CO2(aq)
  2. (b) N2H4(aq) + HSO4(aq) ⇄ N2H5+(aq) + SO42−(aq)
  3. (c) [Al(H2O)6]3+ (aq) + OH(aq) ⇄ [Al(H2O)5OH]2+ (aq) + H2O+()

(a)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

Bronsted acid and base on the left and their conjugate partners on the right has to be identified.

C5H5N (aq) + CH3CO2H (l) C5H5NH+(aq) + CH3CO2-(aq)

Concept Introduction:

Bronsted –Lowry definitions:

A Bronsted –Lowry acid is a proton donor, it donates a hydrogen ion, H+

A Bronsted-Lowry base is a proton acceptor, it accepts a hydrogen ion H+.

Chemistry & Chemical Reactivity, Chapter 16, Problem 8PS , additional homework tip  1

Bronsted –Lowry conjugate acid-Base pairs:

When an acid is dissolved in water, the acid (HA) donates a proton to water to form a new acid (conjugate acid) and a new base (conjugate base).

Chemistry & Chemical Reactivity, Chapter 16, Problem 8PS , additional homework tip  2

Answer to Problem 8PS

C5H5N (aq) + CH3CO2H (l) C5H5NH+(aq) + CH3CO2-(aq)

From the reaction the Bronsted acid and Bronsted base is as follows.

CH3COOH - Bronsted acidC5H5N        - Bronsted baseC5H5NH+   - Conjugate acidCH3COO-  - Conjugate base

Explanation of Solution

C5H5N (aq) + CH3CO2H (l) C5H5NH+(aq) + CH3CO2-(aq)

In the above reaction,

CH3COOH is donated a proton to C5H5N. Therefore, CH3COOH is a Bronsted acid.

C5H5N is accepted a proton from CH3COOH. Therefore,C5H5NH is a Bronsted base.

The conjugate base of CH3COOH is CH3COO- because it has one proton less than CH3COOH.

The conjugate acid of C5H5N is C5H5NH+ because it has one proton is more than C5H5N.

Therefore, from the reaction the Bronsted acid and Bronsted base is as follows.

CH3COOH - Bronsted acidC5H5N        - Bronsted baseC5H5NH+   - Conjugate acidCH3COO-  - Conjugate base

(b)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

Bronsted acid and base on the left and their conjugate partners on the right has to be identified.

 N2H4(aq) + HSO4- (aq) N2H5+ (aq) + SO42-(aq)

Concept Introduction:

Bronsted –Lowry definitions:

A Bronsted –Lowry acid is a proton donor, it donates a hydrogen ion, H+

A Bronsted-Lowry base is a proton acceptor, it accepts a hydrogen ion H+.

Chemistry & Chemical Reactivity, Chapter 16, Problem 8PS , additional homework tip  3

Bronsted –Lowry conjugate acid-Base pairs:

When an acid is dissolved in water, the acid (HA) donates a proton to water to form a new acid (conjugate acid) and a new base (conjugate base).

Chemistry & Chemical Reactivity, Chapter 16, Problem 8PS , additional homework tip  4

Answer to Problem 8PS

N2H4(aq) + HSO4- (aq) N2H5+ (aq) + SO42-(aq)

From the reaction the Bronsted acid and Bronsted base is as follows.

HSO4   - Bronsted acidN2H4      - Bronsted baseN2H5+    - Conjugate acidSO42     - Conjugate base

Explanation of Solution

N2H4(aq) + HSO4- (aq) N2H5+ (aq) + SO42-(aq)

In the above reaction,

HSO4- is donated a proton to N2H4. Therefore, HSO4- is a Bronsted acid.

N2H4 is accepted a proton from N2H5+. Therefore, N2H4 is a Bronsted base.

The conjugate base of HSO4- is SO42- because SO42- has one proton less than HSO4-.

The conjugate acid of N2H4 is N2H5+ because N2H4 has one more proton than N2H5+.

Therefore, From the reaction the Bronsted acid and Bronsted base is as follows.

HSO4   - Bronsted acidN2H4      - Bronsted baseN2H5+    - Conjugate acidSO42     - Conjugate base

(c)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

Bronsted acid and base on the left and their conjugate partners on the right has to be identified.

[Al(H2O)6]3+(aq) + OH- (aq) [Al(H2O)5OH]2+(aq) + H2O (l)

Concept Introduction:

Bronsted –Lowry definitions:

A Bronsted –Lowry acid is a proton donor, it donates a hydrogen ion, H+

A Bronsted-Lowry base is a proton acceptor, it accepts a hydrogen ion H+.

Chemistry & Chemical Reactivity, Chapter 16, Problem 8PS , additional homework tip  5

Bronsted –Lowry conjugate acid-Base pairs:

When an acid is dissolved in water, the acid (HA) donates a proton to water to form a new acid (conjugate acid) and a new base (conjugate base).

Chemistry & Chemical Reactivity, Chapter 16, Problem 8PS , additional homework tip  6

Answer to Problem 8PS

[Al(H2O)6]3+(aq) + OH- (aq) [Al(H2O)5OH]2+(aq) + H2O (l)

From the reaction the Bronsted acid and Bronsted base is as follows.

[Al(H2O)6]3+   - Bronsted acidOH-                 - Bronsted base[Al(H2O)5]2+   - Conjugate acidH2O                - Conjugate base

Explanation of Solution

[Al(H2O)6]3+(aq) + OH- (aq) [Al(H2O)5OH]2+(aq) + H2O (l)

In the above reaction,

[Al(H2O)6]3+ is donated a proton to OH-. Therefore, [Al(H2O)6]3+ is a Bronsted acid.

OH- is accepted a proton from [Al(H2O)6]3+. Therefore, OH- is a Bronsted base.

The conjugate base of [Al(H2O)6]3+ is [Al(H2O)5]32+ because [Al(H2O)6]3+ has one proton less than [Al(H2O)6]3+.

The conjugate acid of OH- is H2O because H2O has one more proton than OH-.

Therefore, form the reaction the Bronsted acid and Bronsted base is as follows.

[Al(H2O)6]3+   - Bronsted acidOH-                 - Bronsted base[Al(H2O)5]2+   - Conjugate acidH2O                - Conjugate base

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Chapter 16 Solutions

Chemistry & Chemical Reactivity

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