The amphiprotic character of HCO 3 − has to be demonstrated using chemical equations and also the conjugate acid‑base pair has to be identified. Concept Introduction: A species that can acts as both proton donor or and also as a proton acceptor is known as amphiprotic. This reacts with both acid and base. Important character of the amphiprotic species is that it has hydrogen atoms which can be donated. Proton donor is referred as Bronsted acid while proton acceptor is referred as Bronsted base. In a reaction, where a proton is alone transferred from one species to another species is known as Proton-transfer reaction. Generally acid donates proton to form conjugate base. As donation of proton takes place, the conjugate base will have fewer hydrogen ions than that is present in acid. Base accepts protons to form conjugate acid. As proton is accepted, the conjugate acid will have more hydrogen ions than that of the base from which it is formed.

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Answer 1

Question

Chapter 6, Problem 6A.11E

(a)

Interpretation Introduction

Interpretation:

The amphiprotic character of HCO3− has to be demonstrated using chemical equations and also the conjugate acid‑base pair has to be identified.

Concept Introduction:

A species that can acts as both proton donor or and also as a proton acceptor is known as amphiprotic. This reacts with both acid and base. Important character of the amphiprotic species is that it has hydrogen atoms which can be donated.

Proton donor is referred as Bronsted acid while proton acceptor is referred as Bronsted base. In a reaction, where a proton is alone transferred from one species to another species is known as Proton-transfer reaction.

Generally acid donates proton to form conjugate base. As donation of proton takes place, the conjugate base will have fewer hydrogen ions than that is present in acid. Base accepts protons to form conjugate acid. As proton is accepted, the conjugate acid will have more hydrogen ions than that of the base from which it is formed.

(b)

Interpretation Introduction

Interpretation:

The amphiprotic character of HPO42− has to be demonstrated using chemical equations and also the conjugate acid‑base pair has to be identified.

Concept Introduction:

Refer part (a).

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Answer 2

Question

Chapter 6, Problem 6A.11E

(a)

Interpretation Introduction

Interpretation:

The amphiprotic character of HCO3− has to be demonstrated using chemical equations and also the conjugate acid‑base pair has to be identified.

Concept Introduction:

A species that can acts as both proton donor or and also as a proton acceptor is known as amphiprotic. This reacts with both acid and base. Important character of the amphiprotic species is that it has hydrogen atoms which can be donated.

Proton donor is referred as Bronsted acid while proton acceptor is referred as Bronsted base. In a reaction, where a proton is alone transferred from one species to another species is known as Proton-transfer reaction.

Generally acid donates proton to form conjugate base. As donation of proton takes place, the conjugate base will have fewer hydrogen ions than that is present in acid. Base accepts protons to form conjugate acid. As proton is accepted, the conjugate acid will have more hydrogen ions than that of the base from which it is formed.

(b)

Interpretation Introduction

Interpretation:

The amphiprotic character of HPO42− has to be demonstrated using chemical equations and also the conjugate acid‑base pair has to be identified.

Concept Introduction:

Refer part (a).

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Answer 3

Question

Chapter 6, Problem 6A.11E

(a)

Interpretation Introduction

Interpretation:

The amphiprotic character of HCO3− has to be demonstrated using chemical equations and also the conjugate acid‑base pair has to be identified.

Concept Introduction:

A species that can acts as both proton donor or and also as a proton acceptor is known as amphiprotic. This reacts with both acid and base. Important character of the amphiprotic species is that it has hydrogen atoms which can be donated.

Proton donor is referred as Bronsted acid while proton acceptor is referred as Bronsted base. In a reaction, where a proton is alone transferred from one species to another species is known as Proton-transfer reaction.

Generally acid donates proton to form conjugate base. As donation of proton takes place, the conjugate base will have fewer hydrogen ions than that is present in acid. Base accepts protons to form conjugate acid. As proton is accepted, the conjugate acid will have more hydrogen ions than that of the base from which it is formed.

(b)

Interpretation Introduction

Interpretation:

The amphiprotic character of HPO42− has to be demonstrated using chemical equations and also the conjugate acid‑base pair has to be identified.

Concept Introduction:

Refer part (a).

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Answer 4

Question

Chapter 6, Problem 6A.11E

(a)

Interpretation Introduction

Interpretation:

The amphiprotic character of HCO3− has to be demonstrated using chemical equations and also the conjugate acid‑base pair has to be identified.

Concept Introduction:

A species that can acts as both proton donor or and also as a proton acceptor is known as amphiprotic. This reacts with both acid and base. Important character of the amphiprotic species is that it has hydrogen atoms which can be donated.

Proton donor is referred as Bronsted acid while proton acceptor is referred as Bronsted base. In a reaction, where a proton is alone transferred from one species to another species is known as Proton-transfer reaction.

Generally acid donates proton to form conjugate base. As donation of proton takes place, the conjugate base will have fewer hydrogen ions than that is present in acid. Base accepts protons to form conjugate acid. As proton is accepted, the conjugate acid will have more hydrogen ions than that of the base from which it is formed.

(b)

Interpretation Introduction

Interpretation:

The amphiprotic character of HPO42− has to be demonstrated using chemical equations and also the conjugate acid‑base pair has to be identified.

Concept Introduction:

Refer part (a).

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Answer 5

Chapter 6, Problem 6A.11E

(a)

Interpretation Introduction

Interpretation:

The amphiprotic character of HCO3− has to be demonstrated using chemical equations and also the conjugate acid‑base pair has to be identified.

Concept Introduction:

A species that can acts as both proton donor or and also as a proton acceptor is known as amphiprotic. This reacts with both acid and base. Important character of the amphiprotic species is that it has hydrogen atoms which can be donated.

Proton donor is referred as Bronsted acid while proton acceptor is referred as Bronsted base. In a reaction, where a proton is alone transferred from one species to another species is known as Proton-transfer reaction.

Generally acid donates proton to form conjugate base. As donation of proton takes place, the conjugate base will have fewer hydrogen ions than that is present in acid. Base accepts protons to form conjugate acid. As proton is accepted, the conjugate acid will have more hydrogen ions than that of the base from which it is formed.

(b)

Interpretation Introduction

Interpretation:

The amphiprotic character of HPO42− has to be demonstrated using chemical equations and also the conjugate acid‑base pair has to be identified.

Concept Introduction:

Refer part (a).

Answer 6

Chapter 6, Problem 6A.11E

(a)

Interpretation Introduction

Interpretation:

The amphiprotic character of HCO3− has to be demonstrated using chemical equations and also the conjugate acid‑base pair has to be identified.

Concept Introduction:

A species that can acts as both proton donor or and also as a proton acceptor is known as amphiprotic. This reacts with both acid and base. Important character of the amphiprotic species is that it has hydrogen atoms which can be donated.

Proton donor is referred as Bronsted acid while proton acceptor is referred as Bronsted base. In a reaction, where a proton is alone transferred from one species to another species is known as Proton-transfer reaction.

Generally acid donates proton to form conjugate base. As donation of proton takes place, the conjugate base will have fewer hydrogen ions than that is present in acid. Base accepts protons to form conjugate acid. As proton is accepted, the conjugate acid will have more hydrogen ions than that of the base from which it is formed.

Answer 7

Chapter 6, Problem 6A.11E

(a)

Interpretation Introduction

Interpretation:

The amphiprotic character of HCO3− has to be demonstrated using chemical equations and also the conjugate acid‑base pair has to be identified.

Concept Introduction:

A species that can acts as both proton donor or and also as a proton acceptor is known as amphiprotic. This reacts with both acid and base. Important character of the amphiprotic species is that it has hydrogen atoms which can be donated.

Proton donor is referred as Bronsted acid while proton acceptor is referred as Bronsted base. In a reaction, where a proton is alone transferred from one species to another species is known as Proton-transfer reaction.

Generally acid donates proton to form conjugate base. As donation of proton takes place, the conjugate base will have fewer hydrogen ions than that is present in acid. Base accepts protons to form conjugate acid. As proton is accepted, the conjugate acid will have more hydrogen ions than that of the base from which it is formed.

Answer 8

(b)

Interpretation Introduction

Interpretation:

The amphiprotic character of HPO42− has to be demonstrated using chemical equations and also the conjugate acid‑base pair has to be identified.

Concept Introduction:

Refer part (a).

Answer 9

(b)

Interpretation Introduction

Interpretation:

The amphiprotic character of HPO42− has to be demonstrated using chemical equations and also the conjugate acid‑base pair has to be identified.

Concept Introduction:

Refer part (a).

Answer 10

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Answer 11

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Answer 12

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Answer 13

Ch. 6 - Prob. 6A.1AST Ch. 6 - Prob. 6A.1BST Ch. 6 - Prob. 6A.2AST Ch. 6 - Prob. 6A.2BST Ch. 6 - Prob. 6A.3AST Ch. 6 - Prob. 6A.3BST Ch. 6 - Prob. 6A.1E Ch. 6 - Prob. 6A.2E Ch. 6 - Prob. 6A.3E Ch. 6 - Prob. 6A.4E

Solution Summary: The author explains the amphiprotic character of HCO_ 3- and the conjugate acidbase pair.

Interpretation:

The amphiprotic character of HPO42− has to be demonstrated using chemical equations and also the conjugate acid‑base pair has to be identified.

Concept Introduction:

Refer part (a).

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Chapter 6 Solutions

Solution Summary: The author explains the amphiprotic character of HCO_ 3- and the conjugate acidbase pair.

Interpretation: The amphiprotic character of HPO42− has to be demonstrated using chemical equations and also the conjugate acid‑base pair has to be identified. Concept Introduction: Refer part (a).

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Chapter 6 Solutions

Interpretation:

The amphiprotic character of HPO42− has to be demonstrated using chemical equations and also the conjugate acid‑base pair has to be identified.

Concept Introduction:

Refer part (a).