As shown in the graph, hemoglobin exchanges oxygen and protons due to an inverse relationship between oxygen binding and proton binding known as the Bohr effect. The binding of oxygen to hemoglobin causes a conformational change that disrupts salt bridges, making oxyhemoglobin more acidic than deoxyhemoglobin. For purposes of calculation, hemoglobin can be modeled as a simple monoprotic buffer, dissociating one proton per subunit as illustrated in the graph and equilibrium equations. pK₂=7.8 HHb — H+ + Hb pK₂=6.7 HHbO₂ H+ + HbO₂ You will now calculate the quantity (in millimoles) of protons that will be released when 1.55 mmol of oxygen binds to deoxyhemoglobin at pH 7.4 and the pH then returns to 7.4 (i.e., going from point A to point B on the curve).
As shown in the graph, hemoglobin exchanges oxygen and protons due to an inverse relationship between oxygen binding and proton binding known as the Bohr effect. The binding of oxygen to hemoglobin causes a conformational change that disrupts salt bridges, making oxyhemoglobin more acidic than deoxyhemoglobin. For purposes of calculation, hemoglobin can be modeled as a simple monoprotic buffer, dissociating one proton per subunit as illustrated in the graph and equilibrium equations. pK₂=7.8 HHb — H+ + Hb pK₂=6.7 HHbO₂ H+ + HbO₂ You will now calculate the quantity (in millimoles) of protons that will be released when 1.55 mmol of oxygen binds to deoxyhemoglobin at pH 7.4 and the pH then returns to 7.4 (i.e., going from point A to point B on the curve).
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
Related questions
Question
Please, I do not understand this question. Steps leading to the CORRECT answer would be helpful!
![As shown in the graph, hemoglobin exchanges oxygen and
protons due to an inverse relationship between oxygen binding
and proton binding known as the Bohr effect. The binding of
oxygen to hemoglobin causes a conformational change that
disrupts salt bridges, making oxyhemoglobin more acidic
than deoxyhemoglobin.
For purposes of calculation, hemoglobin can be modeled as a
simple monoprotic buffer, dissociating one proton per subunit
as illustrated in the graph and equilibrium equations.
pK₁=7.8
HHb
H+ + Hb
pK₁=6.7
HHbO₂
H+ + HbO₂
You will now calculate the quantity (in millimoles) of protons
that will be released when 1.55 mmol of oxygen binds to
deoxyhemoglobin at pH 7.4 and the pH then returns to 7.4 (i.e.,
going from point A to point B on the curve).
11.0
10.0
9.0
8.0
pH 7.0
6.0
5.0
4.0
Oxygen-Proton Exchange in Hemoglobin
Blood pH (7.4) A
HHb
HHbO₂
Tissues
H+ + HCO3
Hb
HbO₂
H* + HCO3
Lungs
H₂O
CO₂
H₂O
B
CO₂
Hb
HbO₂
0.0 0.1 0.2 0.3 0.4 0.5 0.6 0.7 0.8 0.9 1.0
Fraction Unprotonated](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F25d5c273-ce26-424b-bd36-a8a6b930ab8d%2F22374f50-40f8-4aa1-8221-4c97f43e0bb1%2Fof98aza_processed.png&w=3840&q=75)
Transcribed Image Text:As shown in the graph, hemoglobin exchanges oxygen and
protons due to an inverse relationship between oxygen binding
and proton binding known as the Bohr effect. The binding of
oxygen to hemoglobin causes a conformational change that
disrupts salt bridges, making oxyhemoglobin more acidic
than deoxyhemoglobin.
For purposes of calculation, hemoglobin can be modeled as a
simple monoprotic buffer, dissociating one proton per subunit
as illustrated in the graph and equilibrium equations.
pK₁=7.8
HHb
H+ + Hb
pK₁=6.7
HHbO₂
H+ + HbO₂
You will now calculate the quantity (in millimoles) of protons
that will be released when 1.55 mmol of oxygen binds to
deoxyhemoglobin at pH 7.4 and the pH then returns to 7.4 (i.e.,
going from point A to point B on the curve).
11.0
10.0
9.0
8.0
pH 7.0
6.0
5.0
4.0
Oxygen-Proton Exchange in Hemoglobin
Blood pH (7.4) A
HHb
HHbO₂
Tissues
H+ + HCO3
Hb
HbO₂
H* + HCO3
Lungs
H₂O
CO₂
H₂O
B
CO₂
Hb
HbO₂
0.0 0.1 0.2 0.3 0.4 0.5 0.6 0.7 0.8 0.9 1.0
Fraction Unprotonated
![Step 1: Calculate the ratio of [HHb] to [Hb] at pH 7.4.
Step 2: Calculate the millimoles of HHb in 1.55 mmol
deoxyhemoglobin at pH 7.4.
Step 3: Calculate the ratio of [HHbO₂] to [HbO₂] at pH 7.4.
Step 4: Calculate the millimoles of HHbO₂ in 1.55 mmol of
oxyhemoglobin at pH 7.4.
Step 5: Calculate the millimoles of protons that will be
released when 1.55 mmol of oxygen binds to
deoxyhemoglobin at pH 7.4.
[HHb]
[Hb]
иннь =
[HHbO₂]
[HbO₂]
иHHbO₂ =
nprotons =
2.51
2.0002
0.2
0.4648
1.54
mmol
mmol
mmol](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F25d5c273-ce26-424b-bd36-a8a6b930ab8d%2F22374f50-40f8-4aa1-8221-4c97f43e0bb1%2Fo7tprgu_processed.png&w=3840&q=75)
Transcribed Image Text:Step 1: Calculate the ratio of [HHb] to [Hb] at pH 7.4.
Step 2: Calculate the millimoles of HHb in 1.55 mmol
deoxyhemoglobin at pH 7.4.
Step 3: Calculate the ratio of [HHbO₂] to [HbO₂] at pH 7.4.
Step 4: Calculate the millimoles of HHbO₂ in 1.55 mmol of
oxyhemoglobin at pH 7.4.
Step 5: Calculate the millimoles of protons that will be
released when 1.55 mmol of oxygen binds to
deoxyhemoglobin at pH 7.4.
[HHb]
[Hb]
иннь =
[HHbO₂]
[HbO₂]
иHHbO₂ =
nprotons =
2.51
2.0002
0.2
0.4648
1.54
mmol
mmol
mmol
Expert Solution
![](/static/compass_v2/shared-icons/check-mark.png)
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 5 steps with 5 images
![Blurred answer](/static/compass_v2/solution-images/blurred-answer.jpg)
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Recommended textbooks for you
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781305957404/9781305957404_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781259911156/9781259911156_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
![Principles of Instrumental Analysis](https://www.bartleby.com/isbn_cover_images/9781305577213/9781305577213_smallCoverImage.gif)
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781305957404/9781305957404_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781259911156/9781259911156_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
![Principles of Instrumental Analysis](https://www.bartleby.com/isbn_cover_images/9781305577213/9781305577213_smallCoverImage.gif)
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
![Organic Chemistry](https://www.bartleby.com/isbn_cover_images/9780078021558/9780078021558_smallCoverImage.gif)
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
![Chemistry: Principles and Reactions](https://www.bartleby.com/isbn_cover_images/9781305079373/9781305079373_smallCoverImage.gif)
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
![Elementary Principles of Chemical Processes, Bind…](https://www.bartleby.com/isbn_cover_images/9781118431221/9781118431221_smallCoverImage.gif)
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY