Carbonic Acid Buffers and the case of the child that drinks 1L of Cherry Coke® 10 Reasons to NEVER Let Your Kid Drink Soda 19. Carbonic Acid is also found in blood plasma. It is there because of respiration in the muscle tissue creates carbon dioxide that gets absorbed in the blood. H2CO/HCO, in the blood plasma makes a buffer. MAMAVATKN HCO5 (0) + + H,O°ca9) where pK, = 6.1 H;CO3loa) + H;O() What is a buffer and what is its function? In a healthy human the carbonic acid and bicarbonate concentrations in the blood plasma are • [H,CO3] = 0.0024M • [HCO;] = 0.048M %3D %3D Calculate the pH of blood if this buffer system is the only source of pH Calculate the number of moles of H,CO, in the blood of a child with 4.5L of blood Calculate the number of moles of HCO; in the blood of the child (assuming 4.5L of blood)

Carbonic Acid Buffers and the case of the child that drinks 1L of Cherry Coke® 10 Reasons to NEVER Let Your Kid Drink Soda 19. Carbonic Acid is also found in blood plasma. It is there because of respiration in the muscle tissue creates carbon dioxide that gets absorbed in the blood. H2CO/HCO, in the blood plasma makes a buffer. MAMAVATKN HCO5 (0) + + H,O°ca9) where pK, = 6.1 H;CO3loa) + H;O() What is a buffer and what is its function? In a healthy human the carbonic acid and bicarbonate concentrations in the blood plasma are • [H,CO3] = 0.0024M • [HCO;] = 0.048M %3D %3D Calculate the pH of blood if this buffer system is the only source of pH Calculate the number of moles of H,CO, in the blood of a child with 4.5L of blood Calculate the number of moles of HCO; in the blood of the child (assuming 4.5L of blood)

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

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 2ALQ: A friend asks the following: Consider a buffered solution made up of the weak acid HA and its salt...

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Similar questions

. When sodium hydroxide, NaOH, is added dropwise to a buffered solution, the _______ component of the butter consumes the added hydroxide ion.
8-71 Explain why you do not need to know the chemical formula of a buffer compound to use it.
What concentration of NH4NO3 is required to make [OH]=1.0105 in a 0.200-M solution of NH3?
A solution has a pH of 4.5. What would be the color of the solution if each of the following indicators were added? (See Fig. 14-8.) a. methyl orange b. alizarin c. bromcresol green d. phenolphthalein
A solution is prepared from 0.150 mol of formic acid and enough water to make 0.425 L of solution. a Determine the concentrations of H3O+ and HCOO in this solution. b Determine the H3O+ concentration that would be necessary to decrease the HCOO concentration above by a factor of 10. How many milliliters of 2.00 M HCl would be required to produce this solution? Consider that the solution was made by combining the HCl, the HCOOH, and enough water to make 0.425 L of solution. c Qualitatively, how can you account for the differences in the percentage dissociation of formic acid in parts a and b of this problem?
Find the values of Kb for the conjugate bases of the following organic acids: (a) glycolic acid, used by dermatologists as a chemical peel; K a =1.5104 (b) butyric acid, responsible for the odor of rancid butter; K a =1.5105
State which of the following species are amphiprotic and write chemical equations illustrating the amphiprotic character of these species: (a) H2O. (b) H2PO4-. (c) S2-. (d) CO32-. (e) HSO4-
Consider a solution prepared by mixing a weak acid HA. HCl, and NaA. Which of the following statements best describes what happens? a. The H+ from the HCl reacts completely with the A from the NaA. Then the HA dissociates somewhat. b. The H+ from the HCl reacts somewhat with the A from the NaA to make HA, while the HA is dissociating. Eventually you have equal amounts of everything. c. The H+ from the HCl reacts somewhat with the A from the NaA to make HA while the HA is dissociating. Eventually all the reactions have equal rates. d. The H+ from the HCl reacts completely with the A from the NaA. Then the HA dissociates somewhat until too much H+ and A are formed, so the H+ and A react to form HA, and so on. Eventually equilibrium is reached. Justify your choice, and for choices you did not pick, explain what is wrong with them.
A friend asks the following: Consider a buffered solution made up of the weak acid HA and its salt NaA. If a strong base like NaOH is added, the HA reacts with the OH to form A. Thus the amount of acid (HA) is decreased, and the amount of base (A) is increased. Analogously, adding HCI to the buffered solution forms more of the acid (HA) by reacting with the base (A). Thus how can we claim that a buffered solution resists changes in the pH of the solution? How would you explain buffering to this friend?

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