General Chemistry
General Chemistry
7th Edition
ISBN: 9780073402758
Author: Chang, Raymond/ Goldsby
Publisher: McGraw-Hill College
bartleby

Concept explainers

bartleby

Videos

Question
Book Icon
Chapter 16, Problem 16.3QP

(a)

Interpretation Introduction

Interpretation:

Given set of species has to be classified as Bronsted acid or base, or both.

Concept Introduction:

Bronsted's definition is based on the chemical reaction that occurs when both acids and bases are added with each other.  In Bronsted's theory acid donates proton, while base accepts proton from acid resulting in the formation of water.

Example: Consider the following reaction.

  HCl+NH3NH4++Cl-

Hydrogen chloride donates a proton, and hence it is a Bronsted acid.  Ammonia accepts a proton, and hence it is a Bronsted base.

Bronsted base accepts a proton to give a protonated species known as conjugate acid and Bronsted acid loses a proton deprotonated species is known as conjugate base.  When a proton is removed the resulting species will have a negative charge and when a proton is added the resulting species will have a positive charge.

(a)

Expert Solution
Check Mark

Answer to Problem 16.3QP

The species (a) is both Bronsted acid and Bronsted base.

Explanation of Solution

To classify: H2O as Bronsted acid or base, or both.

To identify the species as Bronsted acid.

  H2OH++OH-

Water molecule loses a proton to form a conjugate base as shown above.  Therefore, water can act as Bronsted acid.

To identify the species as Bronsted base.

  H2O+H+H3O+

  Water molecule accepts a proton to form hydronium ion.  Therefore, water can act as Bronsted base.

From this we can conclude that water can act as both Bronsted acid and Bronsted base.

(b)

Interpretation Introduction

Interpretation:

Given set of species has to be classified as Bronsted acid or base, or both.

Concept Introduction: Bronsted's definition is based on the chemical reaction that occurs when both acids and bases are added with each other.  In Bronsted's theory acid donates proton, while base accepts proton from acid resulting in the formation of water.

Example: Consider the following reaction.

  HCl+NH3NH4++Cl-

Hydrogen chloride donates a proton, and hence it is a Bronsted acid.  Ammonia accepts a proton, and hence it is a Bronsted base.

Bronsted base accepts a proton to give a protonated species known as conjugate acid and Bronsted acid loses a proton deprotonated species is known as conjugate base.  When a proton is removed the resulting species will have a negative charge and when a proton is added the resulting species will have a positive charge.

(b)

Expert Solution
Check Mark

Answer to Problem 16.3QP

The species (b) is Bronsted base.

Explanation of Solution

To classify: OH- as Bronsted acid or base, or both.

To identify the species as Bronsted acid.

Hydroxide ion cannot lose a proton to form a conjugate base.  Therefore, hydroxide ion cannot act as Bronsted acid.

To identify the species as Bronsted base.

  OH-+H+H2O

Hydroxide ion accepts a proton to form water molecule.  Therefore, hydroxide ion can act as Bronsted base.

From this we can conclude that hydroxide ion can only act as Bronsted base.

(c)

Interpretation Introduction

Interpretation:

Given set of species has to be classified as Bronsted acid or base, or both.

Concept Introduction: Bronsted's definition is based on the chemical reaction that occurs when both acids and bases are added with each other.  In Bronsted's theory acid donates proton, while base accepts proton from acid resulting in the formation of water.

Example: Consider the following reaction.

  HCl+NH3NH4++Cl-

Hydrogen chloride donates a proton, and hence it is a Bronsted acid.  Ammonia accepts a proton, and hence it is a Bronsted base.

Bronsted base accepts a proton to give a protonated species known as conjugate acid and Bronsted acid loses a proton deprotonated species is known as conjugate base.  When a proton is removed the resulting species will have a negative charge and when a proton is added the resulting species will have a positive charge.

(c)

Expert Solution
Check Mark

Answer to Problem 16.3QP

The species (c) is Bronsted acid.

Explanation of Solution

To classify: H3O+ as Bronsted acid or base, or both.

To identify the species as Bronsted acid.

  H3O+H2O+H+

The hydronium ion can lose a proton to form a conjugate base as shown above.  Therefore, hydronium ion can act as Bronsted acid.

To identify the species as Bronsted base.

Hydronium ion cannot accept proton to form a conjugate acid.

From this we can conclude that hydronium ion can act only as Bronsted acid.

(d)

Interpretation Introduction

Interpretation:

Given set of species has to be classified as Bronsted acid or base, or both.

Concept Introduction: Bronsted's definition is based on the chemical reaction that occurs when both acids and bases are added with each other.  In Bronsted's theory acid donates proton, while base accepts proton from acid resulting in the formation of water.

Example: Consider the following reaction.

  HCl+NH3NH4++Cl-

Hydrogen chloride donates a proton, and hence it is a Bronsted acid.  Ammonia accepts a proton, and hence it is a Bronsted base.

Bronsted base accepts a proton to give a protonated species known as conjugate acid and Bronsted acid loses a proton deprotonated species is known as conjugate base.  When a proton is removed the resulting species will have a negative charge and when a proton is added the resulting species will have a positive charge.

(d)

Expert Solution
Check Mark

Answer to Problem 16.3QP

The species (d) is Bronsted base.

Explanation of Solution

To classify: NH3 as Bronsted acid or base, or both.

To identify the species as Bronsted acid.

Ammonia cannot lose a proton to form a conjugate base.  Therefore, ammonia cannot act as Bronsted acid.

To identify the species as Bronsted base.

  NH3+H+NH4+

Ammonia accepts a proton to form ammonium ion.  Therefore, ammonia ion can act as Bronsted base.

From this we can conclude that ammonia can act only as Bronsted base.

(e)

Interpretation Introduction

Interpretation:

Given set of species has to be classified as Bronsted acid or base, or both.

Concept Introduction: Bronsted's definition is based on the chemical reaction that occurs when both acids and bases are added with each other.  In Bronsted's theory acid donates proton, while base accepts proton from acid resulting in the formation of water.

Example: Consider the following reaction.

  HCl+NH3NH4++Cl-

Hydrogen chloride donates a proton, and hence it is a Bronsted acid.  Ammonia accepts a proton, and hence it is a Bronsted base.

Bronsted base accepts a proton to give a protonated species known as conjugate acid and Bronsted acid loses a proton deprotonated species is known as conjugate base.  When a proton is removed the resulting species will have a negative charge and when a proton is added the resulting species will have a positive charge.

(e)

Expert Solution
Check Mark

Answer to Problem 16.3QP

The species (e) is Bronsted acid.

Explanation of Solution

To classify: NH4+ as Bronsted acid or base, or both.

To identify the species as Bronsted acid.

  NH4+NH3+H+

The ammonium ion can lose a proton to form a conjugate base as shown above.  Therefore ammonium ion can act as Bronsted acid.

To identify the species as Bronsted base.

Ammonium ion cannot accept proton to form a conjugate acid.

From this we can conclude that ammonium ion can act only as Bronsted acid.

(f)

Interpretation Introduction

Interpretation:

Given set of species has to be classified as Bronsted acid or base, or both.

Concept Introduction: Bronsted's definition is based on the chemical reaction that occurs when both acids and bases are added with each other.  In Bronsted's theory acid donates proton, while base accepts proton from acid resulting in the formation of water.

Example: Consider the following reaction.

  HCl+NH3NH4++Cl-

Hydrogen chloride donates a proton, and hence it is a Bronsted acid.  Ammonia accepts a proton, and hence it is a Bronsted base.

Bronsted base accepts a proton to give a protonated species known as conjugate acid and Bronsted acid loses a proton deprotonated species is known as conjugate base.  When a proton is removed the resulting species will have a negative charge and when a proton is added the resulting species will have a positive charge.

(f)

Expert Solution
Check Mark

Answer to Problem 16.3QP

The species (f) is Bronsted base.

Explanation of Solution

To classify: NH2 as Bronsted acid or base, or both.

To identify the species as Bronsted acid.

NH2 cannot lose a proton to form a conjugate base.  Therefore, NH2 cannot act as Bronsted acid.

To identify the species as Bronsted base.

  NH2+H+NH3

NH2 accepts a proton to form ammonia.  Therefore, NH2 ion can act as Bronsted base.

From this we can conclude that NH2 can act only as Bronsted base.

(g)

Interpretation Introduction

Interpretation:

Given set of species has to be classified as Bronsted acid or base, or both.

Concept Introduction: Bronsted's definition is based on the chemical reaction that occurs when both acids and bases are added with each other.  In Bronsted's theory acid donates proton, while base accepts proton from acid resulting in the formation of water.

Example: Consider the following reaction.

  HCl+NH3NH4++Cl-

Hydrogen chloride donates a proton, and hence it is a Bronsted acid.  Ammonia accepts a proton, and hence it is a Bronsted base.

Bronsted base accepts a proton to give a protonated species known as conjugate acid and Bronsted acid loses a proton deprotonated species is known as conjugate base.  When a proton is removed the resulting species will have a negative charge and when a proton is added the resulting species will have a positive charge.

(g)

Expert Solution
Check Mark

Answer to Problem 16.3QP

The species (g) is Bronsted base.

Explanation of Solution

To classify: NO3 as Bronsted acid or base, or both.

To identify the species as Bronsted acid.

NO3 does not have a proton at all.  Therefore, this cannot lose a proton to form a conjugate base.  Hence, NO3 cannot act as Bronsted acid.

To identify the species as Bronsted base.

  NO3+H+HNO3

NO3 accepts a proton to form nitric acid.  Therefore, NO3 ion can act as Bronsted base.

From this we can conclude that NO3 can act only as Bronsted base.

(h)

Interpretation Introduction

Interpretation:

Given set of species has to be classified as Bronsted acid or base, or both.

Concept Introduction: Bronsted's definition is based on the chemical reaction that occurs when both acids and bases are added with each other.  In Bronsted's theory acid donates proton, while base accepts proton from acid resulting in the formation of water.

Example: Consider the following reaction.

  HCl+NH3NH4++Cl-

Hydrogen chloride donates a proton, and hence it is a Bronsted acid.  Ammonia accepts a proton, and hence it is a Bronsted base.

Bronsted base accepts a proton to give a protonated species known as conjugate acid and Bronsted acid loses a proton deprotonated species is known as conjugate base.  When a proton is removed the resulting species will have a negative charge and when a proton is added the resulting species will have a positive charge.

(h)

Expert Solution
Check Mark

Answer to Problem 16.3QP

The species (h) is Bronsted base.

Explanation of Solution

To classify: CO32 as Bronsted acid or base, or both.

To identify the species as Bronsted acid.

Explanation:  CO32 does not have a proton at all.  Therefore, this cannot lose a proton to form a conjugate base.  Hence, CO32 cannot act as Bronsted acid.

To identify the species as Bronsted base.

  CO32+H+HCO3

CO32 accepts a proton to form HCO3 ion.  Therefore, CO32 ion can act as Bronsted base.

From this we can conclude that CO32 can act only as Bronsted base.

(i)

Interpretation Introduction

Interpretation:

Given set of species has to be classified as Bronsted acid or base, or both.

Concept Introduction: Bronsted's definition is based on the chemical reaction that occurs when both acids and bases are added with each other.  In Bronsted's theory acid donates proton, while base accepts proton from acid resulting in the formation of water.

Example: Consider the following reaction.

  HCl+NH3NH4++Cl-

Hydrogen chloride donates a proton, and hence it is a Bronsted acid.  Ammonia accepts a proton, and hence it is a Bronsted base.

Bronsted base accepts a proton to give a protonated species known as conjugate acid and Bronsted acid loses a proton deprotonated species is known as conjugate base.  When a proton is removed the resulting species will have a negative charge and when a proton is added the resulting species will have a positive charge.

(i)

Expert Solution
Check Mark

Answer to Problem 16.3QP

The species (i) is Bronsted acid.

Explanation of Solution

To classify: HBr as Bronsted acid or base, or both.

To identify the species as Bronsted acid.

  HBrBr-+H+

The HBr can lose a proton to form a conjugate base as shown above.  Therefore, HBr can act as Bronsted acid.

To identify the species as Bronsted base.

HBr cannot accept proton to form a conjugate acid.

From this we can conclude that HBr can act only as Bronsted acid.

(j)

Interpretation Introduction

Interpretation:

Given set of species has to be classified as Bronsted acid or base, or both.

Concept Introduction: Bronsted's definition is based on the chemical reaction that occurs when both acids and bases are added with each other.  In Bronsted's theory acid donates proton, while base accepts proton from acid resulting in the formation of water.

Example: Consider the following reaction.

  HCl+NH3NH4++Cl-

Hydrogen chloride donates a proton, and hence it is a Bronsted acid.  Ammonia accepts a proton, and hence it is a Bronsted base.

Bronsted base accepts a proton to give a protonated species known as conjugate acid and Bronsted acid loses a proton deprotonated species is known as conjugate base.  When a proton is removed the resulting species will have a negative charge and when a proton is added the resulting species will have a positive charge.

(j)

Expert Solution
Check Mark

Answer to Problem 16.3QP

The species (j) is Bronsted acid.

Explanation of Solution

To classify: HCN as Bronsted acid or base, or both.

To identify the species as Bronsted acid.

  HCNCN-+H+

The HCN can lose a proton to form a conjugate base as shown above.  Therefore, HCN can act as Bronsted acid.

To identify the species as Bronsted base.

HCN cannot accept proton to form a conjugate acid.

From this we can conclude that HCN can act only as Bronsted acid.

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Chapter 16 Solutions

General Chemistry

Ch. 16.4 - Prob. 1RCCh. 16.5 - Prob. 1PECh. 16.5 - Prob. 2PECh. 16.5 - Prob. 1RCCh. 16.5 - Prob. 3PECh. 16.5 - Prob. 2RCCh. 16.6 - Prob. 1PECh. 16.6 - Prob. 1RCCh. 16.7 - Prob. 1RCCh. 16.8 - Prob. 1PECh. 16.8 - Rank the following acids from strongest to...Ch. 16.9 - Prob. 1PECh. 16.9 - Practice Exercise Predict whether the following...Ch. 16.9 - Prob. 1RCCh. 16.10 - Prob. 1RCCh. 16.11 - Prob. 1PECh. 16.11 - Prob. 1RCCh. 16 - Prob. 16.1QPCh. 16 - Prob. 16.2QPCh. 16 - Prob. 16.3QPCh. 16 - Prob. 16.4QPCh. 16 - Prob. 16.5QPCh. 16 - Prob. 16.6QPCh. 16 - Prob. 16.7QPCh. 16 - Prob. 16.8QPCh. 16 - Prob. 16.9QPCh. 16 - Prob. 16.10QPCh. 16 - Prob. 16.12QPCh. 16 - Prob. 16.13QPCh. 16 - Prob. 16.14QPCh. 16 - 16.15 Calculate the hydrogen ion concentration for...Ch. 16 - 16.16 Calculate the hydrogen ion concentration in...Ch. 16 - Prob. 16.17QPCh. 16 - Prob. 16.18QPCh. 16 - 16.19 Complete this table for a...Ch. 16 - Prob. 16.20QPCh. 16 - Prob. 16.21QPCh. 16 - Prob. 16.22QPCh. 16 - Prob. 16.23QPCh. 16 - Prob. 16.24QPCh. 16 - Prob. 16.25QPCh. 16 - Prob. 16.26QPCh. 16 - Prob. 16.27QPCh. 16 - Prob. 16.28QPCh. 16 - Prob. 16.29QPCh. 16 - Prob. 16.30QPCh. 16 - Prob. 16.31QPCh. 16 - Prob. 16.32QPCh. 16 - Prob. 16.33QPCh. 16 - Prob. 16.34QPCh. 16 - Prob. 16.35QPCh. 16 - Prob. 16.36QPCh. 16 - Prob. 16.37QPCh. 16 - Prob. 16.38QPCh. 16 - Prob. 16.39QPCh. 16 - 16.40 Which of the following solutions has the...Ch. 16 - Prob. 16.41QPCh. 16 - Prob. 16.42QPCh. 16 - Prob. 16.43QPCh. 16 - Prob. 16.44QPCh. 16 - Prob. 16.45QPCh. 16 - Prob. 16.46QPCh. 16 - 16.47 A 0.040 M solution of a monoprotic acid is...Ch. 16 - Prob. 16.48QPCh. 16 - Prob. 16.49QPCh. 16 - 16.50 Write all the species (except water) that...Ch. 16 - Prob. 16.51QPCh. 16 - Prob. 16.52QPCh. 16 - Prob. 16.53QPCh. 16 - Prob. 16.54QPCh. 16 - Prob. 16.55QPCh. 16 - Prob. 16.56QPCh. 16 - 16.57 What is the original molarity of a solution...Ch. 16 - Prob. 16.58QPCh. 16 - Prob. 16.59QPCh. 16 - Prob. 16.60QPCh. 16 - Prob. 16.61QPCh. 16 - Prob. 16.62QPCh. 16 - Prob. 16.63QPCh. 16 - Prob. 16.64QPCh. 16 - Prob. 16.65QPCh. 16 - Prob. 16.66QPCh. 16 - Prob. 16.67QPCh. 16 - Prob. 16.68QPCh. 16 - Prob. 16.69QPCh. 16 - Prob. 16.70QPCh. 16 - Prob. 16.71QPCh. 16 - Prob. 16.72QPCh. 16 - Prob. 16.73QPCh. 16 - Prob. 16.74QPCh. 16 - Prob. 16.75QPCh. 16 - Prob. 16.76QPCh. 16 - Prob. 16.77QPCh. 16 - Prob. 16.78QPCh. 16 - Prob. 16.79QPCh. 16 - Prob. 16.80QPCh. 16 - Prob. 16.81QPCh. 16 - Prob. 16.82QPCh. 16 - Prob. 16.83QPCh. 16 - Prob. 16.84QPCh. 16 - Prob. 16.85QPCh. 16 - Prob. 16.86QPCh. 16 - Prob. 16.87QPCh. 16 - Prob. 16.88QPCh. 16 - Prob. 16.89QPCh. 16 - Prob. 16.90QPCh. 16 - Prob. 16.91QPCh. 16 - Prob. 16.92QPCh. 16 - 16.93 Most of the hydrides of Group 1A and Group...Ch. 16 - Prob. 16.94QPCh. 16 - Prob. 16.95QPCh. 16 - Prob. 16.96QPCh. 16 - Prob. 16.97QPCh. 16 - Prob. 16.98QPCh. 16 - Prob. 16.99QPCh. 16 - 16.100 Hydrocyanic acid (HCN) is a weak acid and a...Ch. 16 - Prob. 16.101QPCh. 16 - Prob. 16.102QPCh. 16 - Prob. 16.103QPCh. 16 - Prob. 16.104QPCh. 16 - 16.105 You are given two beakers containing...Ch. 16 - Prob. 16.106QPCh. 16 - Prob. 16.107QPCh. 16 - Prob. 16.108QPCh. 16 - Prob. 16.109QPCh. 16 - Prob. 16.110QPCh. 16 - Prob. 16.111QPCh. 16 - Prob. 16.112QPCh. 16 - Prob. 16.113QPCh. 16 - Prob. 16.114QPCh. 16 - Prob. 16.115QPCh. 16 - Prob. 16.116QPCh. 16 - Prob. 16.117QPCh. 16 - Prob. 16.118QPCh. 16 - Prob. 16.119QPCh. 16 - Prob. 16.120QPCh. 16 - Prob. 16.121SPCh. 16 - Prob. 16.122SPCh. 16 - Prob. 16.123SPCh. 16 - Prob. 16.124SPCh. 16 - Prob. 16.125SPCh. 16 - Prob. 16.126SPCh. 16 - Prob. 16.127SPCh. 16 - Prob. 16.128SPCh. 16 - Prob. 16.129SPCh. 16 - 16.130 Use the data in Appendix 2 to calculate the...
Knowledge Booster
Background pattern image
Chemistry
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Recommended textbooks for you
Text book image
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Text book image
Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
Text book image
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
Text book image
Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
Text book image
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Text book image
Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY
General Chemistry | Acids & Bases; Author: Ninja Nerd;https://www.youtube.com/watch?v=AOr_5tbgfQ0;License: Standard YouTube License, CC-BY