General Chemistry
General Chemistry
7th Edition
ISBN: 9780073402758
Author: Chang, Raymond/ Goldsby
Publisher: McGraw-Hill College
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Chapter 16, Problem 16.7QP

(a)

Interpretation Introduction

Interpretation:

For the given set of acids, formula for conjugated base has to be written.

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.

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

Example: Consider the following reaction.

HCl+NH3NH4++Cl-

Bronsted base accepts a proton to give a protonated species known as conjugate acid and Bronsted acid loses a proton to give a 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

Explanation of Solution

The conjugate base of CH2ClCOOH

To identify the conjugate base

CH2ClCOOH       CH2ClCOO-+H+

The conjugate base is CH2ClCOO-

Conjugate base is formed when a proton is removed from the Bronsted acid.  The scheme for the formation of conjugate base for the given acid is shown above.

(b)

Interpretation Introduction

Interpretation:

For the given set of acids, formula for conjugated base has to be written.

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.

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

Example: Consider the following reaction.

HCl+NH3NH4++Cl-

Bronsted base accepts a proton to give a protonated species known as conjugate acid and Bronsted acid loses a proton to give a 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

Explanation of Solution

The conjugate base of HIO4

To identify the conjugate base

HIO4      IO4+H+

The conjugate base is  IO4

Conjugate base is formed when a proton is removed from the Bronsted acid.  The scheme for the formation of conjugate base for the given acid is shown above.

(c)

Interpretation Introduction

Interpretation:

For the given set of acids, formula for conjugated base has to be written.

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.

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

Example: Consider the following reaction.

HCl+NH3NH4++Cl-

Bronsted base accepts a proton to give a protonated species known as conjugate acid and Bronsted acid loses a proton to give a 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

Explanation of Solution

The conjugate base of H3PO4

To identify the conjugate base

H3PO4      H2PO4-+H+

The conjugate base is   H2PO4-

Conjugate base is formed when a proton is removed from the Bronsted acid.  The scheme for the formation of conjugate base for the given acid is shown above.

(d)

Interpretation Introduction

Interpretation:

For the given set of acids, formula for conjugated base has to be written.

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.

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

Example: Consider the following reaction.

HCl+NH3NH4++Cl-

Bronsted base accepts a proton to give a protonated species known as conjugate acid and Bronsted acid loses a proton to give a 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

Explanation of Solution

The conjugate base of H2PO4

To identify the conjugate base

H2PO4      HPO42+H+

The conjugate base is    HPO42

Conjugate base is formed when a proton is removed from the Bronsted acid.  The scheme for the formation of conjugate base for the given acid is shown above.

(e)

Interpretation Introduction

Interpretation:

For the given set of acids, formula for conjugated base has to be written.

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.

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

Example: Consider the following reaction.

HCl+NH3NH4++Cl-

Bronsted base accepts a proton to give a protonated species known as conjugate acid and Bronsted acid loses a proton to give a 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

Explanation of Solution

The conjugate base of HPO42

To identify the conjugate base

HPO42      PO43+H+

The conjugate base is PO43

Conjugate base is formed when a proton is removed from the Bronsted acid.  The scheme for the formation of conjugate base for the given acid is shown above.

(f)

Interpretation Introduction

Interpretation:

For the given set of acids, formula for conjugated base has to be written.

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.

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

Example: Consider the following reaction.

HCl+NH3NH4++Cl-

Bronsted base accepts a proton to give a protonated species known as conjugate acid and Bronsted acid loses a proton to give a 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

Explanation of Solution

The conjugate base of H2SO4

To identify the conjugate base

H2SO4       HSO4+H+

The conjugate base is HSO4

Conjugate base is formed when a proton is removed from the Bronsted acid.  The scheme for the formation of conjugate base for the given acid is shown above.

(g)

Interpretation Introduction

Interpretation:

For the given set of acids, formula for conjugated base has to be written.

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.

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

Example: Consider the following reaction.

HCl+NH3NH4++Cl-

Bronsted base accepts a proton to give a protonated species known as conjugate acid and Bronsted acid loses a proton to give a 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

Explanation of Solution

The conjugate base of  HSO4

To identify the conjugate base

HSO4       SO42+H+

The conjugate base of SO42

Conjugate base is formed when a proton is removed from the Bronsted acid.  The scheme for the formation of conjugate base for the given acid is shown above.

(h)

Interpretation Introduction

Interpretation:

For the given set of acids, formula for conjugated base has to be written.

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.

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

Example: Consider the following reaction.

HCl+NH3NH4++Cl-

Bronsted base accepts a proton to give a protonated species known as conjugate acid and Bronsted acid loses a proton to give a 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

Explanation of Solution

The conjugate base of HCOOH

To identify the conjugate base

HCOOH    HCOO+H+

The conjugate base of HCOO

Conjugate base is formed when a proton is removed from the Bronsted acid.  The scheme for the formation of conjugate base for the given acid is shown above.

(i)

Interpretation Introduction

Interpretation:

For the given set of acids, formula for conjugated base has to be written.

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.

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

Example: Consider the following reaction.

HCl+NH3NH4++Cl-

Bronsted base accepts a proton to give a protonated species known as conjugate acid and Bronsted acid loses a proton to give a 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

Explanation of Solution

The conjugate base of HSO3

To identify the conjugate base

HSO3      SO32+H+

The conjugate base of  SO32

Conjugate base is formed when a proton is removed from the Bronsted acid.  The scheme for the formation of conjugate base for the given acid is shown above.

(j)

Interpretation Introduction

Interpretation:

For the given set of acids, formula for conjugated base has to be written.

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.

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

Example: Consider the following reaction.

HCl+NH3NH4++Cl-

Bronsted base accepts a proton to give a protonated species known as conjugate acid and Bronsted acid loses a proton to give a 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

Explanation of Solution

The conjugate base of NH4+

To identify the conjugate base

NH4+       NH3+H+

The conjugate base is  NH3

Conjugate base is formed when a proton is removed from the Bronsted acid.  The scheme for the formation of conjugate base for the given acid is shown above.

(k)

Interpretation Introduction

Interpretation:

For the given set of acids, formula for conjugated base has to be written.

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.

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

Example: Consider the following reaction.

HCl+NH3NH4++Cl-

Bronsted base accepts a proton to give a protonated species known as conjugate acid and Bronsted acid loses a proton to give a 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.

(k)

Expert Solution
Check Mark

Explanation of Solution

The conjugate base of H2S

To identify the conjugate base

H2S      HS+H+

The conjugate base of  HS

Conjugate base is formed when a proton is removed from the Bronsted acid.  The scheme for the formation of conjugate base for the given acid is shown above.

(l)

Interpretation Introduction

Interpretation:

For the given set of acids, formula for conjugated base has to be written.

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.

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

Example: Consider the following reaction.

HCl+NH3NH4++Cl-

Bronsted base accepts a proton to give a protonated species known as conjugate acid and Bronsted acid loses a proton to give a 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.

(l)

Expert Solution
Check Mark

Explanation of Solution

The conjugate base of HS-

To identify the conjugate base

HS-      S2-+H+

The conjugate base of S2-

Conjugate base is formed when a proton is removed from the Bronsted acid.  The scheme for the formation of conjugate base for the given acid is shown above.

(m)

Interpretation Introduction

Interpretation:

For the given set of acids, formula for conjugated base has to be written.

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.

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

Example: Consider the following reaction.

HCl+NH3NH4++Cl-

Bronsted base accepts a proton to give a protonated species known as conjugate acid and Bronsted acid loses a proton to give a 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.

(m)

Expert Solution
Check Mark

Explanation of Solution

The conjugate base of HClO

To identify the conjugate base

HClO      ClO-+H+

The conjugate base of ClO-

Conjugate base is formed when a proton is removed from the Bronsted acid.  The scheme for the formation of conjugate base for the given acid is shown above.

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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...
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