The reason for the large difference in pKa1 and pKa2 value of oxalic acid than suberic acid needs to be explained. Concept introduction: In the water, the product of concentration of OH- and H+ ions at a specific temperature is recognized as ionic product i.e. Kw of water. The Kw values increment with the increment in temperature which means the OH- and H+ ion’s concentration increments with the increment in temperature. The Kw value is 1 × 10 − 4 at 25 0 C. The p K a for an acid can be calculated as follows: p K a = − log ( K a ) Here, K a is acid dissociation constant of an acid.

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Answer 1

Question

Chapter 16, Problem 92IAE

Interpretation Introduction

Interpretation:

The reason for the large difference in pKa1 and pKa2 value of oxalic acid than suberic acid needs to be explained.

Concept introduction:

In the water, the product of concentration of OH- and H+ ions at a specific temperature is recognized as ionic product i.e. Kw of water. The Kw values increment with the increment in temperature which means the OH- and H+ ion’s concentration increments with the increment in temperature. The Kw value is 1×10−4 at 25 ⁰C. The pKa for an acid can be calculated as follows:

pKa=−log(Ka)

Here, Ka is acid dissociation constant of an acid.

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Answer 2

Question

Chapter 16, Problem 92IAE

Interpretation Introduction

Interpretation:

The reason for the large difference in pKa1 and pKa2 value of oxalic acid than suberic acid needs to be explained.

Concept introduction:

In the water, the product of concentration of OH- and H+ ions at a specific temperature is recognized as ionic product i.e. Kw of water. The Kw values increment with the increment in temperature which means the OH- and H+ ion’s concentration increments with the increment in temperature. The Kw value is 1×10−4 at 25 ⁰C. The pKa for an acid can be calculated as follows:

pKa=−log(Ka)

Here, Ka is acid dissociation constant of an acid.

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Answer 3

Question

Chapter 16, Problem 92IAE

Interpretation Introduction

Interpretation:

The reason for the large difference in pKa1 and pKa2 value of oxalic acid than suberic acid needs to be explained.

Concept introduction:

In the water, the product of concentration of OH- and H+ ions at a specific temperature is recognized as ionic product i.e. Kw of water. The Kw values increment with the increment in temperature which means the OH- and H+ ion’s concentration increments with the increment in temperature. The Kw value is 1×10−4 at 25 ⁰C. The pKa for an acid can be calculated as follows:

pKa=−log(Ka)

Here, Ka is acid dissociation constant of an acid.

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Answer 4

Question

Chapter 16, Problem 92IAE

Interpretation Introduction

Interpretation:

The reason for the large difference in pKa1 and pKa2 value of oxalic acid than suberic acid needs to be explained.

Concept introduction:

In the water, the product of concentration of OH- and H+ ions at a specific temperature is recognized as ionic product i.e. Kw of water. The Kw values increment with the increment in temperature which means the OH- and H+ ion’s concentration increments with the increment in temperature. The Kw value is 1×10−4 at 25 ⁰C. The pKa for an acid can be calculated as follows:

pKa=−log(Ka)

Here, Ka is acid dissociation constant of an acid.

Expert Solution & Answer

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Answer 5

Chapter 16, Problem 92IAE

Interpretation Introduction

Interpretation:

The reason for the large difference in pKa1 and pKa2 value of oxalic acid than suberic acid needs to be explained.

Concept introduction:

In the water, the product of concentration of OH- and H+ ions at a specific temperature is recognized as ionic product i.e. Kw of water. The Kw values increment with the increment in temperature which means the OH- and H+ ion’s concentration increments with the increment in temperature. The Kw value is 1×10−4 at 25 ⁰C. The pKa for an acid can be calculated as follows:

pKa=−log(Ka)

Here, Ka is acid dissociation constant of an acid.

Answer 6

Chapter 16, Problem 92IAE

Interpretation Introduction

Interpretation:

The reason for the large difference in pKa1 and pKa2 value of oxalic acid than suberic acid needs to be explained.

Concept introduction:

In the water, the product of concentration of OH- and H+ ions at a specific temperature is recognized as ionic product i.e. Kw of water. The Kw values increment with the increment in temperature which means the OH- and H+ ion’s concentration increments with the increment in temperature. The Kw value is 1×10−4 at 25 ⁰C. The pKa for an acid can be calculated as follows:

pKa=−log(Ka)

Here, Ka is acid dissociation constant of an acid.

Answer 7

Chapter 16, Problem 92IAE

Interpretation Introduction

Interpretation:

The reason for the large difference in pKa1 and pKa2 value of oxalic acid than suberic acid needs to be explained.

Concept introduction:

In the water, the product of concentration of OH- and H+ ions at a specific temperature is recognized as ionic product i.e. Kw of water. The Kw values increment with the increment in temperature which means the OH- and H+ ion’s concentration increments with the increment in temperature. The Kw value is 1×10−4 at 25 ⁰C. The pKa for an acid can be calculated as follows:

pKa=−log(Ka)

Here, Ka is acid dissociation constant of an acid.

Answer 8

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Answer 9

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Answer 10

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Answer 11

Ch. 16 - According to the Brønsted-Lowry theory, lebel each...Ch. 16 - Write the formula of the conjugate based in the...Ch. 16 - For each of the following, identify the acides and...Ch. 16 - Which of the following species are amphiprotic in...Ch. 16 - Why which of the following bases will the...Ch. 16 - In a manner similar to equation (16.3), represent...Ch. 16 - With the aid of Table 16.2, predict the direction...Ch. 16 - With the aid of Table 16.2, predict the direction...Ch. 16 - Calculate [H2O4] and [OH-] or each solution: (a)...Ch. 16 - What is the pH of each of the following solution?...

Solution Summary: The author explains that oxalic acid has a higher pKa1 value than suberic acid.

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