Question

A patient is hyperventilating. The "blowing off" of excessive carbon dioxide causes a decrease in blood...

A patient is hyperventilating. The "blowing off" of excessive carbon dioxide causes a decrease in blood H+ concentration. How can the carbonic acid-bicarbonate buffer system function to correct this imbalance?

CO2 + H2O ↔ H2CO3 ↔ H+ + HCO3-

Science   Anatomy-And-Physiology   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

The blowing off excessive carbon dioxide from lung shifts the carbonic acid-bicarbonate buffer reactions(CO2 + H2O ↔ H2CO3 ↔ H+ + HCO3-) to the left that results into fomration of co2 by the action of the carbonic anhydrase until the blood H+ concentration normalizes.After that bicarbonate concentration get regulated via kidney compensation ,in which kidney starts producing NH4+ (ammonium) and monophosphate and releasing them through urine and thus reabsorbs  bicarbonate ions in blood plasma while clearing the acids(H+ ions) via urine flow.

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Some friends and I were working on this problem and we think we got through A....
Some friends and I were working on this problem and we think we got through A. and B. but we're having a hard time figuring out C. 5) a) What is the ratio of bicarbonate (HCO3 -) to carbonic acid (H2CO3) in blood at its normal pH of 7.4?  Ka for carbonic acid is 4.3 x 10-7. b)  After heavy exercise, an athleteʹs blood pH was detemined to be 7.1.  What is the ratio of bicarbonate (HCO3 -) to carbonic acid (H2CO3) at...
A man suffering from untreated diabetes mellitus is admitted to the hospital. Glucose is present in...
A man suffering from untreated diabetes mellitus is admitted to the hospital. Glucose is present in his urine and he exhibits shallow breathing. Analysis of his blood shows [HCO3-] of 16 mM and [CO2] of .9 mM. 1.) Write a multi-step equilibrium for bicarbonate as a buffer in blood. Your expressions should include carbon dioxide and carbonic acid. 2.) What is the approximate pH of the blood of the patient above? Use carbon dioxide as the acid. 3.) After the...
The bicarbonate buffer system is derived from carbon dioxide reacting with water in the tissues to...
The bicarbonate buffer system is derived from carbon dioxide reacting with water in the tissues to form carbonic acid. Carbonic acid then donates a proton to water to form hydronium and bicarbonate. a. What is the chemical equation for the reactions described above? Include physical states. b. What 2 components make this a buffer? c. Breathing out shifts this equilibrium in which direction? d. Why do we buffer our blood?
The interaction between carbon dioxide and water results in formation of carbonic acid, H2CO3, which lowers...
The interaction between carbon dioxide and water results in formation of carbonic acid, H2CO3, which lowers the pH of water through the reactions H2CO3(aq)+H2O(l) <---> HCO3-(aq) + H3O+(aq) Ka1= 4.3*10^-7 HCO3-(aq) +H2O(l) <---> CO3 2- (aq) + H3O+ (aq) Ka2=5.6*10^-11 This dissocociation causes "normal" rainwater to have a pH of approximately 5.7. However, H3O+(aq) can also come from other sources, particularly from acids resulting from interactions of water with industrial pollutants. Scientists studying a particular lake found that its pH...
When carbon dioxide is unloaded from the red blood cell during external respiration. Which process must...
When carbon dioxide is unloaded from the red blood cell during external respiration. Which process must occur? 1. oxygen leaves hemoglobin to to the alveolus 2. carbon dioxide combines with water to form carbonic acid 3. bicarbonate leaves the red blood cell in exchange for a chloride ion 4. carbon dioxide enters the red blood cell and binds to hemoglobin 5. hemoglobin buffers the cell by carrying H+
When carbon dioxide is unloaded form the red blood cell during external respiration, which process must...
When carbon dioxide is unloaded form the red blood cell during external respiration, which process must occur? 1. oxygen leaves hemoglobin to go to the alveolus 2. carbon dioxide combines with water to form carbonic acid 3. bicarbonate leaves the red blood cell in exchange for a chloride ion 4. carbon dioxide enters the red blood cell and bind to hemoglobin 5. hemoglobin buffers the cell by carrying h+
cccc Questions Respiratory I    J excessive carbon dioxide in the blood is called Alveoli    ...
cccc Questions Respiratory I    J excessive carbon dioxide in the blood is called Alveoli     I        Excessive stretching of the lungs is accomplished through which reflexive action Apnea     L Inadequate oxygen delivery to the cells is called Carbonic anhydrase     F labored breathing is called Cardiac notch     S Nasal hairs are also called Compliance   B sustained absence of breathing is called Dyspnea     A The actual site of gas exchange occurs at the level of Expiratory...
The solubility of carbon dioxide in water is of considerable environmental and commercial importance. Although the...
The solubility of carbon dioxide in water is of considerable environmental and commercial importance. Although the behavior of dissolved CO2 is somewhat complicated, for most purposes it can be treated as dissolving to form carbonic acid, H2CO3, according to the following equation: CO2 (g) + H2O (l) H2CO3 (aq) Keq = 0.036 (a) Carbonated sodas are typically packaged under a carbon dioxide pressure of about 5 bar. Calculate the number of moles of carbon dioxide dissolved (in the form of...
The Henderson-Hasselbalch equation relates the pH of a buffer solution to the pKa of its conjugate...
The Henderson-Hasselbalch equation relates the pH of a buffer solution to the pKa of its conjugate acid and the ratio of the concentrations of the conjugate base and acid. The equation is important in laboratory work that makes use of buffered solutions, in industrial processes where pH needs to be controlled, and in medicine, where understanding the Henderson-Hasselbalch equation is critical for the control of blood pH. Part A As a technician in a large pharmaceutical research firm, you need...
The Henderson-Hasselbalch equation relates the pH of a buffer solution to the pKa of its conjugate...
The Henderson-Hasselbalch equation relates the pH of a buffer solution to the pKa of its conjugate acid and the ratio of the concentrations of the conjugate base and acid. The equation is important in laboratory work that makes use of buffered solutions, in industrial processes where pH needs to be controlled, and in medicine, where understanding the Henderson-Hasselbalch equation is critical for the control of blood pH. Part A.) As a technician in a large pharmaceutical research firm, you need...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT