5. Using what you've learned in class about the buffering system of the blood, derive an equation for the [H] concentration in terms of the concentration of dissolved CO₂, the blood bicarbonate concentration, the K, of carbonic acid, and K for the reaction: CO, (0)+H_O (0)=H_CO, (0) K 6. Hyperventilation (very rapid and deep breathing, which reduces the concentration of CO₂ in the blood) causes dizziness. a. How does hyperventilation affect the pH of the blood (i.e., is the pH increased or decreased as a result of hyperventilation)? Briefly, explain your answer in terms of equilibrium shifts. b. The normal first-aid treatment for hyperventilation is to have the patient breathe into a paper bag. Briefly, explain why this treatment works and tell what effect the paper-bag treatment has on the pH of the blood. 7. Soap is an example of an amphoteric substance. a. How does soap work? b. Why do amphoteric substances such as soap foam?

5. Using what you've learned in class about the buffering system of the blood, derive an equation for the [H] concentration in terms of the concentration of dissolved CO₂, the blood bicarbonate concentration, the K, of carbonic acid, and K for the reaction: CO, (0)+H_O (0)=H_CO, (0) K 6. Hyperventilation (very rapid and deep breathing, which reduces the concentration of CO₂ in the blood) causes dizziness. a. How does hyperventilation affect the pH of the blood (i.e., is the pH increased or decreased as a result of hyperventilation)? Briefly, explain your answer in terms of equilibrium shifts. b. The normal first-aid treatment for hyperventilation is to have the patient breathe into a paper bag. Briefly, explain why this treatment works and tell what effect the paper-bag treatment has on the pH of the blood. 7. Soap is an example of an amphoteric substance. a. How does soap work? b. Why do amphoteric substances such as soap foam?

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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Enough water is added to the buffer in Question 29 to make the total volume 10.0 L. Calculate (a) the pH of the buffer. (b) the pH of the buffer after the addition of 0.0500 mol of HCl to 0.600 L of diluted buffer. (c) the pH of the buffer after the addition of 0.0500 mol of NaOH to 0.600 L of diluted buffer. (d) Compare your answers to Question 29(a)-(c) with your answers to (a)-(c) in this problem. (e) Comment on the effect of dilution on the pH of a buffer and on its buffer capacity.
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Methyl orange, HMO, is a common acid-base indicator. In solution it ionizes according to the equation: HMOaqH+aq+MO-aqredyellow If methyl orange is added to distilled water, the solution turns yellow. If 1 drop or two of 6 M HCl is added to the yellow solution, it turns red. If to that solution one adds a few drops of 6 M NaOH, the color reverts to yellow. a. Why does adding 6 M HCl to the yellow solution of methyl orange tend to cause the color to change to red? Note that in solution HCl exists as H+ and Cl- ions. b. Why does adding 6 M NaOH to the red solution tend to make it turn back to yellow? Note that in solution NaOH exists as Na+ and OH- ions. How does increasing OH- shift Reaction 3 in the discussion section? How would the resulting change in H+ affect the dissociation reaction of HMO?
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