Glycine has pK 2 values of 2.34 and 9.60. At what pH does glycine exist in the forms shown?

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Answer 1

Textbook Question

Chapter 21, Problem 49P

Glycine has pK₂ values of 2.34 and 9.60. At what pH does glycine exist in the forms shown?

Chapter 21, Problem 49P, Glycine has pK2 values of 2.34 and 9.60. At what pH does glycine exist in the forms shown?

(a)

Expert Solution

Interpretation Introduction

Interpretation:

The pH at which glycine exists at the given form has to be calculated.

Concept introduction:

The isoelectric point $(pI)$ is the $pH$ at which the amount of positive charge and negative charge on an amino acid becomes balanced.

The value of $pI$ is depends upon the $pKa$ value of protonated amino group and $pKa$ value of carboxyl group of an amino acid.

Protons are released when the $pH$ becomes $pKa$ of species.

Answer to Problem 49P

The pH of the glycine for the given form is $9.60.$

Explanation of Solution

In the given form of glycine,

EBK ORGANIC CHEMISTRY, Chapter 21, Problem 49P , additional homework tip 1

The $50%$ of amino group of the glycine are released their protons, so the pH of the system becomes $pKa$ .

The $pKa$ of the amino group of glycine is $9.60.$

Therefore,

The pH of the glycine for the given form is $9.60.$

(b)

Expert Solution

Interpretation Introduction

Interpretation:

The pH at which glycine exists at the given form has to be calculated.

Concept introduction:

The isoelectric point $(pI)$ is the $pH$ at which the amount of positive charge and negative charge on an amino acid becomes balanced.

The value of $pI$ is depends upon the $pKa$ value of protonated amino group and $pKa$ value of carboxyl group of an amino acid.

Protons are released when the $pH$ becomes $pKa$ of species.

Explanation of Solution

In the given form of glycine,

EBK ORGANIC CHEMISTRY, Chapter 21, Problem 49P , additional homework tip 2

The amount of positive charge and negative charge are equal or balanced for 100% system.

The isoelectric point ( $pI$ ) is the $pH$ at which the amount of positive charge and negative charge on an amino acid becomes balanced.

Therefore,

The pH of the glycine for the given form is $6.02.$

(c)

Expert Solution

Interpretation Introduction

Interpretation:

The $pH$ at which glycine exists at the given form has to be calculated.

Concept introduction:

The isoelectric point $(pI)$ is the $pH$ at which the amount of positive charge and negative charge on an amino acid becomes balanced.

The value of $pI$ is depends upon the $pKa$ value of protonated amino group and $pKa$ value of carboxyl group of an amino acid.

Protons are released when the $pH$ becomes $pKa$ of species.

Answer to Problem 49P

The pH of the glycine for the given form is $2.34.$

Explanation of Solution

In the glycine form of glycine,

EBK ORGANIC CHEMISTRY, Chapter 21, Problem 49P , additional homework tip 3

The $50%$ of $–OH$ group of the glycine are released their protons, so the pH of the system becomes $pKa$ of the $–OH$ of glycine.

The $pKa$ of the $–OH$ group of glycine is $2.34.$

Therefore,

The pH of the glycine for the given form is $2.34.$

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04:58

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Answer 2

Textbook Question

Chapter 21, Problem 49P

Glycine has pK₂ values of 2.34 and 9.60. At what pH does glycine exist in the forms shown?

Chapter 21, Problem 49P, Glycine has pK2 values of 2.34 and 9.60. At what pH does glycine exist in the forms shown?

(a)

Expert Solution

Interpretation Introduction

Interpretation:

The pH at which glycine exists at the given form has to be calculated.

Concept introduction:

The isoelectric point $(pI)$ is the $pH$ at which the amount of positive charge and negative charge on an amino acid becomes balanced.

The value of $pI$ is depends upon the $pKa$ value of protonated amino group and $pKa$ value of carboxyl group of an amino acid.

Protons are released when the $pH$ becomes $pKa$ of species.

Answer to Problem 49P

The pH of the glycine for the given form is $9.60.$

Explanation of Solution

In the given form of glycine,

EBK ORGANIC CHEMISTRY, Chapter 21, Problem 49P , additional homework tip 1

The $50%$ of amino group of the glycine are released their protons, so the pH of the system becomes $pKa$ .

The $pKa$ of the amino group of glycine is $9.60.$

Therefore,

The pH of the glycine for the given form is $9.60.$

(b)

Expert Solution

Interpretation Introduction

Interpretation:

The pH at which glycine exists at the given form has to be calculated.

Concept introduction:

The isoelectric point $(pI)$ is the $pH$ at which the amount of positive charge and negative charge on an amino acid becomes balanced.

The value of $pI$ is depends upon the $pKa$ value of protonated amino group and $pKa$ value of carboxyl group of an amino acid.

Protons are released when the $pH$ becomes $pKa$ of species.

Explanation of Solution

In the given form of glycine,

EBK ORGANIC CHEMISTRY, Chapter 21, Problem 49P , additional homework tip 2

The amount of positive charge and negative charge are equal or balanced for 100% system.

The isoelectric point ( $pI$ ) is the $pH$ at which the amount of positive charge and negative charge on an amino acid becomes balanced.

Therefore,

The pH of the glycine for the given form is $6.02.$

(c)

Expert Solution

Interpretation Introduction

Interpretation:

The $pH$ at which glycine exists at the given form has to be calculated.

Concept introduction:

The isoelectric point $(pI)$ is the $pH$ at which the amount of positive charge and negative charge on an amino acid becomes balanced.

The value of $pI$ is depends upon the $pKa$ value of protonated amino group and $pKa$ value of carboxyl group of an amino acid.

Protons are released when the $pH$ becomes $pKa$ of species.

Answer to Problem 49P

The pH of the glycine for the given form is $2.34.$

Explanation of Solution

In the glycine form of glycine,

EBK ORGANIC CHEMISTRY, Chapter 21, Problem 49P , additional homework tip 3

The $50%$ of $–OH$ group of the glycine are released their protons, so the pH of the system becomes $pKa$ of the $–OH$ of glycine.

The $pKa$ of the $–OH$ group of glycine is $2.34.$

Therefore,

The pH of the glycine for the given form is $2.34.$

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04:58

Answer 3

Textbook Question

Chapter 21, Problem 49P

Glycine has pK₂ values of 2.34 and 9.60. At what pH does glycine exist in the forms shown?

Chapter 21, Problem 49P, Glycine has pK2 values of 2.34 and 9.60. At what pH does glycine exist in the forms shown?

(a)

Expert Solution

Interpretation Introduction

Interpretation:

The pH at which glycine exists at the given form has to be calculated.

Concept introduction:

The isoelectric point $(pI)$ is the $pH$ at which the amount of positive charge and negative charge on an amino acid becomes balanced.

The value of $pI$ is depends upon the $pKa$ value of protonated amino group and $pKa$ value of carboxyl group of an amino acid.

Protons are released when the $pH$ becomes $pKa$ of species.

Answer to Problem 49P

The pH of the glycine for the given form is $9.60.$

Explanation of Solution

In the given form of glycine,

EBK ORGANIC CHEMISTRY, Chapter 21, Problem 49P , additional homework tip 1

The $50%$ of amino group of the glycine are released their protons, so the pH of the system becomes $pKa$ .

The $pKa$ of the amino group of glycine is $9.60.$

Therefore,

The pH of the glycine for the given form is $9.60.$

(b)

Expert Solution

Interpretation Introduction

Interpretation:

The pH at which glycine exists at the given form has to be calculated.

Concept introduction:

The isoelectric point $(pI)$ is the $pH$ at which the amount of positive charge and negative charge on an amino acid becomes balanced.

The value of $pI$ is depends upon the $pKa$ value of protonated amino group and $pKa$ value of carboxyl group of an amino acid.

Protons are released when the $pH$ becomes $pKa$ of species.

Explanation of Solution

In the given form of glycine,

EBK ORGANIC CHEMISTRY, Chapter 21, Problem 49P , additional homework tip 2

The amount of positive charge and negative charge are equal or balanced for 100% system.

The isoelectric point ( $pI$ ) is the $pH$ at which the amount of positive charge and negative charge on an amino acid becomes balanced.

Therefore,

The pH of the glycine for the given form is $6.02.$

(c)

Expert Solution

Interpretation Introduction

Interpretation:

The $pH$ at which glycine exists at the given form has to be calculated.

Concept introduction:

The isoelectric point $(pI)$ is the $pH$ at which the amount of positive charge and negative charge on an amino acid becomes balanced.

The value of $pI$ is depends upon the $pKa$ value of protonated amino group and $pKa$ value of carboxyl group of an amino acid.

Protons are released when the $pH$ becomes $pKa$ of species.

Answer to Problem 49P

The pH of the glycine for the given form is $2.34.$

Explanation of Solution

In the glycine form of glycine,

EBK ORGANIC CHEMISTRY, Chapter 21, Problem 49P , additional homework tip 3

The $50%$ of $–OH$ group of the glycine are released their protons, so the pH of the system becomes $pKa$ of the $–OH$ of glycine.

The $pKa$ of the $–OH$ group of glycine is $2.34.$

Therefore,

The pH of the glycine for the given form is $2.34.$

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04:58

Answer 4

Textbook Question

Chapter 21, Problem 49P

Glycine has pK₂ values of 2.34 and 9.60. At what pH does glycine exist in the forms shown?

Chapter 21, Problem 49P, Glycine has pK2 values of 2.34 and 9.60. At what pH does glycine exist in the forms shown?

(a)

Expert Solution

Interpretation Introduction

Interpretation:

The pH at which glycine exists at the given form has to be calculated.

Concept introduction:

The isoelectric point $(pI)$ is the $pH$ at which the amount of positive charge and negative charge on an amino acid becomes balanced.

The value of $pI$ is depends upon the $pKa$ value of protonated amino group and $pKa$ value of carboxyl group of an amino acid.

Protons are released when the $pH$ becomes $pKa$ of species.

Answer to Problem 49P

The pH of the glycine for the given form is $9.60.$

Explanation of Solution

In the given form of glycine,

EBK ORGANIC CHEMISTRY, Chapter 21, Problem 49P , additional homework tip 1

The $50%$ of amino group of the glycine are released their protons, so the pH of the system becomes $pKa$ .

The $pKa$ of the amino group of glycine is $9.60.$

Therefore,

The pH of the glycine for the given form is $9.60.$

(b)

Expert Solution

Interpretation Introduction

Interpretation:

The pH at which glycine exists at the given form has to be calculated.

Concept introduction:

The isoelectric point $(pI)$ is the $pH$ at which the amount of positive charge and negative charge on an amino acid becomes balanced.

The value of $pI$ is depends upon the $pKa$ value of protonated amino group and $pKa$ value of carboxyl group of an amino acid.

Protons are released when the $pH$ becomes $pKa$ of species.

Explanation of Solution

In the given form of glycine,

EBK ORGANIC CHEMISTRY, Chapter 21, Problem 49P , additional homework tip 2

The amount of positive charge and negative charge are equal or balanced for 100% system.

The isoelectric point ( $pI$ ) is the $pH$ at which the amount of positive charge and negative charge on an amino acid becomes balanced.

Therefore,

The pH of the glycine for the given form is $6.02.$

(c)

Expert Solution

Interpretation Introduction

Interpretation:

The $pH$ at which glycine exists at the given form has to be calculated.

Concept introduction:

The isoelectric point $(pI)$ is the $pH$ at which the amount of positive charge and negative charge on an amino acid becomes balanced.

The value of $pI$ is depends upon the $pKa$ value of protonated amino group and $pKa$ value of carboxyl group of an amino acid.

Protons are released when the $pH$ becomes $pKa$ of species.

Answer to Problem 49P

The pH of the glycine for the given form is $2.34.$

Explanation of Solution

In the glycine form of glycine,

EBK ORGANIC CHEMISTRY, Chapter 21, Problem 49P , additional homework tip 3

The $50%$ of $–OH$ group of the glycine are released their protons, so the pH of the system becomes $pKa$ of the $–OH$ of glycine.

The $pKa$ of the $–OH$ group of glycine is $2.34.$

Therefore,

The pH of the glycine for the given form is $2.34.$

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04:58

Answer 5

Textbook Question

Answer 6

Textbook Question

Answer 7

(a)

Expert Solution

Interpretation Introduction

Interpretation:

The pH at which glycine exists at the given form has to be calculated.

Concept introduction:

The isoelectric point $(pI)$ is the $pH$ at which the amount of positive charge and negative charge on an amino acid becomes balanced.

The value of $pI$ is depends upon the $pKa$ value of protonated amino group and $pKa$ value of carboxyl group of an amino acid.

Protons are released when the $pH$ becomes $pKa$ of species.

Answer to Problem 49P

The pH of the glycine for the given form is $9.60.$

Explanation of Solution

In the given form of glycine,

EBK ORGANIC CHEMISTRY, Chapter 21, Problem 49P , additional homework tip 1

The $50%$ of amino group of the glycine are released their protons, so the pH of the system becomes $pKa$ .

The $pKa$ of the amino group of glycine is $9.60.$

Therefore,

The pH of the glycine for the given form is $9.60.$

(b)

Expert Solution

Interpretation Introduction

Interpretation:

The pH at which glycine exists at the given form has to be calculated.

Concept introduction:

The isoelectric point $(pI)$ is the $pH$ at which the amount of positive charge and negative charge on an amino acid becomes balanced.

The value of $pI$ is depends upon the $pKa$ value of protonated amino group and $pKa$ value of carboxyl group of an amino acid.

Protons are released when the $pH$ becomes $pKa$ of species.

Explanation of Solution

In the given form of glycine,

EBK ORGANIC CHEMISTRY, Chapter 21, Problem 49P , additional homework tip 2

The amount of positive charge and negative charge are equal or balanced for 100% system.

The isoelectric point ( $pI$ ) is the $pH$ at which the amount of positive charge and negative charge on an amino acid becomes balanced.

Therefore,

The pH of the glycine for the given form is $6.02.$

(c)

Expert Solution

Interpretation Introduction

Interpretation:

The $pH$ at which glycine exists at the given form has to be calculated.

Concept introduction:

The isoelectric point $(pI)$ is the $pH$ at which the amount of positive charge and negative charge on an amino acid becomes balanced.

The value of $pI$ is depends upon the $pKa$ value of protonated amino group and $pKa$ value of carboxyl group of an amino acid.

Protons are released when the $pH$ becomes $pKa$ of species.

Answer to Problem 49P

The pH of the glycine for the given form is $2.34.$

Explanation of Solution

In the glycine form of glycine,

EBK ORGANIC CHEMISTRY, Chapter 21, Problem 49P , additional homework tip 3

The $50%$ of $–OH$ group of the glycine are released their protons, so the pH of the system becomes $pKa$ of the $–OH$ of glycine.

The $pKa$ of the $–OH$ group of glycine is $2.34.$

Therefore,

The pH of the glycine for the given form is $2.34.$

Answer 8

(a)

Expert Solution

Interpretation Introduction

Interpretation:

The pH at which glycine exists at the given form has to be calculated.

Concept introduction:

The isoelectric point $(pI)$ is the $pH$ at which the amount of positive charge and negative charge on an amino acid becomes balanced.

The value of $pI$ is depends upon the $pKa$ value of protonated amino group and $pKa$ value of carboxyl group of an amino acid.

Protons are released when the $pH$ becomes $pKa$ of species.

Answer to Problem 49P

The pH of the glycine for the given form is $9.60.$

Explanation of Solution

In the given form of glycine,

EBK ORGANIC CHEMISTRY, Chapter 21, Problem 49P , additional homework tip 1

The $50%$ of amino group of the glycine are released their protons, so the pH of the system becomes $pKa$ .

The $pKa$ of the amino group of glycine is $9.60.$

Therefore,

The pH of the glycine for the given form is $9.60.$

Answer 9

(a)

Expert Solution

Answer 10

(a)

Expert Solution

Answer 11

Expert Solution

Answer 12

Interpretation Introduction

Interpretation:

The pH at which glycine exists at the given form has to be calculated.

Concept introduction:

The isoelectric point $(pI)$ is the $pH$ at which the amount of positive charge and negative charge on an amino acid becomes balanced.

The value of $pI$ is depends upon the $pKa$ value of protonated amino group and $pKa$ value of carboxyl group of an amino acid.

Protons are released when the $pH$ becomes $pKa$ of species.

Answer 13

Answer to Problem 49P

The pH of the glycine for the given form is $9.60.$

Answer 14

Explanation of Solution

In the given form of glycine,

EBK ORGANIC CHEMISTRY, Chapter 21, Problem 49P , additional homework tip 1

The $50%$ of amino group of the glycine are released their protons, so the pH of the system becomes $pKa$ .

The $pKa$ of the amino group of glycine is $9.60.$

Therefore,

The pH of the glycine for the given form is $9.60.$

Answer 15

(b)

Expert Solution

Interpretation Introduction

Interpretation:

The pH at which glycine exists at the given form has to be calculated.

Concept introduction:

The isoelectric point $(pI)$ is the $pH$ at which the amount of positive charge and negative charge on an amino acid becomes balanced.

The value of $pI$ is depends upon the $pKa$ value of protonated amino group and $pKa$ value of carboxyl group of an amino acid.

Protons are released when the $pH$ becomes $pKa$ of species.

Explanation of Solution

In the given form of glycine,

EBK ORGANIC CHEMISTRY, Chapter 21, Problem 49P , additional homework tip 2

The amount of positive charge and negative charge are equal or balanced for 100% system.

The isoelectric point ( $pI$ ) is the $pH$ at which the amount of positive charge and negative charge on an amino acid becomes balanced.

Therefore,

The pH of the glycine for the given form is $6.02.$

Answer 16

(b)

Expert Solution

Answer 17

(b)

Expert Solution

Answer 18

Expert Solution

Answer 19

Interpretation Introduction

Interpretation:

The pH at which glycine exists at the given form has to be calculated.

Concept introduction:

The isoelectric point $(pI)$ is the $pH$ at which the amount of positive charge and negative charge on an amino acid becomes balanced.

The value of $pI$ is depends upon the $pKa$ value of protonated amino group and $pKa$ value of carboxyl group of an amino acid.

Protons are released when the $pH$ becomes $pKa$ of species.

Answer 20

Explanation of Solution

In the given form of glycine,

EBK ORGANIC CHEMISTRY, Chapter 21, Problem 49P , additional homework tip 2

The amount of positive charge and negative charge are equal or balanced for 100% system.

The isoelectric point ( $pI$ ) is the $pH$ at which the amount of positive charge and negative charge on an amino acid becomes balanced.

Therefore,

The pH of the glycine for the given form is $6.02.$

Answer 21

(c)

Expert Solution

Interpretation Introduction

Interpretation:

The $pH$ at which glycine exists at the given form has to be calculated.

Concept introduction:

The isoelectric point $(pI)$ is the $pH$ at which the amount of positive charge and negative charge on an amino acid becomes balanced.

The value of $pI$ is depends upon the $pKa$ value of protonated amino group and $pKa$ value of carboxyl group of an amino acid.

Protons are released when the $pH$ becomes $pKa$ of species.

Answer to Problem 49P

The pH of the glycine for the given form is $2.34.$

Explanation of Solution

In the glycine form of glycine,

EBK ORGANIC CHEMISTRY, Chapter 21, Problem 49P , additional homework tip 3

The $50%$ of $–OH$ group of the glycine are released their protons, so the pH of the system becomes $pKa$ of the $–OH$ of glycine.

The $pKa$ of the $–OH$ group of glycine is $2.34.$

Therefore,

The pH of the glycine for the given form is $2.34.$

Answer 22

(c)

Expert Solution

Answer 23

(c)

Expert Solution

Answer 24

Expert Solution

Answer 25

Interpretation Introduction

Interpretation:

The $pH$ at which glycine exists at the given form has to be calculated.

Concept introduction:

The isoelectric point $(pI)$ is the $pH$ at which the amount of positive charge and negative charge on an amino acid becomes balanced.

The value of $pI$ is depends upon the $pKa$ value of protonated amino group and $pKa$ value of carboxyl group of an amino acid.

Protons are released when the $pH$ becomes $pKa$ of species.

Answer 26

Answer to Problem 49P

The pH of the glycine for the given form is $2.34.$

Answer 27

Explanation of Solution

In the glycine form of glycine,

EBK ORGANIC CHEMISTRY, Chapter 21, Problem 49P , additional homework tip 3

The $50%$ of $–OH$ group of the glycine are released their protons, so the pH of the system becomes $pKa$ of the $–OH$ of glycine.

The $pKa$ of the $–OH$ group of glycine is $2.34.$

Therefore,

The pH of the glycine for the given form is $2.34.$

Answer 28

Ch. 21.1 - a. Explain why, when the imidazole ring of...Ch. 21.2 - a. Which isomer(R)-alanine or (S)-alanineis...Ch. 21.2 - Prob. 4P Ch. 21.3 - Prob. 5P Ch. 21.3 - Prob. 6P Ch. 21.3 - Draw the predominant form for glutamate in a...Ch. 21.3 - a. Why is the pKa of the glutamate side chain...Ch. 21.4 - Calculate the pI of each of the following amino...Ch. 21.4 - a. Which amino acid has the lowest pI value? b....Ch. 21.4 - Prob. 12P

Glycine has pK 2 values of 2.34 and 9.60. At what pH does glycine exist in the forms shown?

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Answer to Problem 49P

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