   # Answers to all problems are at the end of this book. Detailed solutions are available in the Student Solutions Manual, Study Guide, and Problems Book . Polyprotic Adds: Phosphate Species Abundance at Different pHs What are the approximate fractional concentrations of the following phosphate species at pH values of 0,2, 4, 6, 8, 10, and 12? H 3 PO 4 Η 2 ΡΟ 4 - HPO 4 2- PO 4 3- ### Biochemistry

6th Edition
Reginald H. Garrett + 1 other
Publisher: Cengage Learning
ISBN: 9781305577206

#### Solutions

Chapter
Section ### Biochemistry

6th Edition
Reginald H. Garrett + 1 other
Publisher: Cengage Learning
ISBN: 9781305577206
Chapter 2, Problem 8P
Textbook Problem
396 views

## Answers to all problems are at the end of this book. Detailed solutions are available in the Student Solutions Manual, Study Guide, and Problems Book.Polyprotic Adds: Phosphate Species Abundance at Different pHs What are the approximate fractional concentrations of the following phosphate species at pH values of 0,2, 4, 6, 8, 10, and 12? H3PO4 Η2ΡΟ4- HPO42- PO43-

Interpretation Introduction

(a)

To calculate:

The approximate fractional concentrations of H3PO4 at pH values of 0,2,4,6,8,10, and 12.

Concept Introduction:

Phosphoric acid has three H+ dissociations.

H3PO4H++H2PO4     pKa1=2.15H2PO4H++HPO42     pKa2=7.20HPO42H++PO43        pKa3=12.4

The Henderson-Hasselbalch equation is as follows:

pH=pKa+log[A][HA]

### Explanation of Solution

Rearranging the Henderson-Hasselbalch equation as follows:

pH=pKa+log[ A ][HA][ A ][HA]=antilog(pHpKa)

At particular pH, [H2PO4-][H3PO4] = x, [HPO42-][H2PO4-] = y, [PO43-][HPO42-] = z

Fraction of any species at a particular pH is concentration of the species divided by the sum of the concentration of all species.

fH3PO4=[H3PO4][H3PO4]+[H2PO4-]+[HPO42-]+[PO43-]

We can rewrite the above equation as a function of x, y, and z

Interpretation Introduction

(b)

To calculate:

The approximate fractional concentrations of H2PO4- at pH values of 0,2,4,6,8,10, and 12 should be calculated

Introduction:

Phosphoric acid has three H+ dissociations.

H3PO4H++H2PO4     pKa1=2.15H2PO4H++HPO42     pKa2=7.20HPO42H++PO43        pKa3=12.4

The Henderson-Hasselbalch equation is as follows:

pH=pKa+log[A][HA]

Interpretation Introduction

(c)

To calculate:

The approximate fractional concentrations of HPO42- at pH values of 0,2,4,6,8,10, and 12.

Introduction:

Phosphoric acid has three H+ dissociations.

H3PO4H++H2PO4     pKa1=2.15H2PO4H++HPO42     pKa2=7.20HPO42H++PO43        pKa3=12.4

The Henderson-Hasselbalch equation is as follows:

pH=pKa+log[A][HA]

Interpretation Introduction

(d)

To calculate:

The approximate fractional concentrations of PO43- at pH values of 0,2,4,6,8,10, and 12.

Concept Introduction:

Phosphoric acid has three H+ dissociations.

H3PO4H++H2PO4     pKa1=2.15H2PO4H++HPO42     pKa2=7.20HPO42H++PO43        pKa3=12.4

The Henderson-Hasselbalch equation is as follows:

pH=pKa+log[A][HA]

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