What's the relationship between CO2, bicarbonate (HC03- ), and carbonic acid (H2CO3)? In what form is most CO2 carried in our blood? What is the role of carbonic anhydrase in gas exchange?
The relationship between
Carbon dioxide (CO2) dissolves in with water to form carbonic acid (H2CO3) this reaction is speedup by the enzyme carbonic anhydrase, then carbonic acid dissociates in to bicarbonate (HC03-).
Overall reaction is represented as CO2 + H2O carbonic anhydrase -à H2CO3 + HCO3- + H+ (this is a reversible reaction and carbonic anhydrase can reverse this reaction – this happens in once RBC reaches lungs)
carbonic acid (H2CO3) and bicarbonate (HC03-) exist in 1:20 in the blood
CO2 / H2CO3 = 1000 / 1
H2CO3 / HCO3- = 1/20
Major form of dissolved CO2 carried in our blood is in the form of bicarbonate (HC03-), 70-75% (rest 25% dissolved in serum or combined with serum protiens and heamoglobin) of the CO2 in our blood is converted in to carbonic acid (H2CO3), which dissociate in to bicarbonate (HC03-) as we know carbonic acid (H2CO3) to bicarbonate (HC03-) ratio is 1:20, that means nearly 71.25% of carbonic acid (H2CO3) gets dissociated in to bicarbonate (HC03-)
As described above carbonic anhydrase can help H2CO3 + HCO3- formation and reverse reaction of forming CO2 + H2O , In tissues due to high CO2 concentration the reaction is forward (lowers the activation energy of combining C O2 + OH- to give HC03-), whereas in lungs because of low CO2 concentration and high O2 concentration the backward reaction is favored to release CO2 (lowers the activation energy of hydrolyzing HCO3- to CO2 + OH- and release CO2 + H2O)
What's the relationship between CO2, bicarbonate (HC03- ), and carbonic acid (H2CO3)? In what form is...
21. What are the characteristics of the carbonic acid-bicarbonate buffer system (select all that apply? a CO2 is eliminated by the lungs b. Neutralizes HCl acid to yield carbonic acid and salt c. H2CO3 formed by neutralization dissociates into H2O and CO2 d. Shifts H+ in and out of cell in exchange for other cations such as potassium and sodium e. Free basic radicals dissociate into ammonia and OH-, which combines with Ho to form water 22. What are characteristics...
One common biological buffer is the carbonic acid (H2CO3) / bicarbonate (HCO3-) buffer. Which of the following statements describes what happens when a small amount of a strong acid is added to the buffer system: A. the amount of bicarbonate increases B. the amount of bicarbonate decreases C. the amount of carbonic acid increases D. the amount of carbonic acid decreases E. both b & c
8. (4 pts) The biological catalyst carbonic anhydrase converts carbon dioxide to carbonic acid, an essential component of the bicarbonate buffer system regulating our blood pH. What mass (in me) of sodium carbonate (NaHCO, MM: 84.006 g/mol) must be added to 500.0 ml of 0.029 M carbonic acid (K. 1 4.3 x 10-7, K., 4.8 x 10-11) to produce a solution with pH = 7.40? Assume no volume change after the addition of sodium carbonate. H2CO3 + H2O=HCO3 + H20...
10.39 The first-order rate constant for the dehydration of carbonic acid, H2CO3(aq) = CO2(g) + H2O(1) is about 1 x 102 s-. In view of this rather high rate constant, explain why it is necessary to have the enzyme carbonic anhydrase to enhance the rate of dehydration in the lungs.
Carbon dioxide dissolves in water to form carbonic acid, which is primarily dissolved CO2. Dissolved CO2 satisfies the equilibrium equation CO2(gas)<------>CO2(aq) K=0.032 M*atm-1 The acid dissociation constants listed in most standard reference texts for carbonic acid actually apply to dissolved CO2. For a CO2 partial pressure of 3.1×10-4 atm in the atmosphere, what is the pH of water in equilibrium with the atmosphere?
The enzyme carbonic anhydrase catalyzes the hydration of CO2 gas in red blood cells: CO2 (g) + H2O (L) →H2CO3 (aq) Determine the ∆Ssys of this reaction at 37 °C (body temperature), and justify the sign. *Thermodynamic parameters at T=298K and 1 bar Sm (JK-1 mol-1) Cp (JK-1 MOL-1) CO2 (g) 213.7 36.8 H2O (L) 69.9 78.2 H2CO3 (aq) 187.4 19.4
2. Blood is buffered using a bicarbonate system primarily to accommodate the formation of CO2 in the tissues. The overall pK for the reaction below is 6.35: CO2 + H2O H2CO3 H+ + HCO3 During acidosis, treatment can consist of IV administration of NaHC03. If the pH of blood is typically 7.4, and the total concentration of carbonic acid/ bicarb is 0.05M, what is the concentration of conjugate base and acid in blood?
In waters affected by acid rain the concentrations of the three carbonic acid species (H2CO3, HCO3-, CO32-) are determined by concentration of the strong acid deposited by acid rain, as well as the concentration of H2CO3 which is controlled by the solubility of carbon dioxide . Under these conditions (constant H2CO3 and relatively low pH) the only carbonic acid equilbrium of importance is the conjugate base reaction of HCO3-, which is related to, but not identical to - and not...
One of the most important buffering systems in the biological realm is the carbonic acid (H2CO3)/carbonate ion (HCO3- ) system that maintains the pH of blood plasma to a relatively constant value. In blood at 37°C, the Ka of carbonic acid is 8x10-8. Suppose that the concentrations of the buffer components in the blood plasma are: [HCO3-] = 0.24 M and [H2CO3] = .12 M. Calculate the pH of blood.
You create a 1 L solution of 0.1 M H2CO3. carbonic acid, H2CO3, is a diprotic acid with Ka1 = 4.5 x 10-7 and Ka2 = 4.7 x 10-11. a) What will the initial pH of the solution be? b) What volume of 0.1 M NaOH will you need to add to reach the second equivalence point( remember carbonic acid deprotonates to bicarbonate HCO3- and then can deprotonate further to CO32-? c) At the second equivalence point, what will the...