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Assume that the normal blood buffer contains 0.00080 M carbonic acid and 0.0085 M hydrogen carbonate;...

Assume that the normal blood buffer contains 0.00080 M carbonic acid and 0.0085 M hydrogen carbonate; the pKa = 6.35 for carbonic acid and the volume of blood in the body is 7.00 L. The blood pH, due to disruption, is now 7.20. What is the ratio of [HCO3 − ]/[H2CO3] now that the blood has been challenged? How many moles of hydrogen carbonate must be added to the blood to bring the carbonic acid/hydrogen carbonate ratio back to a normal pH = 7.4? How many milliliters of 0.10 M hydrogen carbonate must be added to the blood?

H2CO3(aq) + H2O(l) ⇄ HCO3 − (aq) + H3O+ (aq)

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