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Blood is buffered with CO(2) " and " HCO...

Blood is buffered with `CO_(2) " and " HCO_(3)^(-)`. What is the ratio of the base concentration to the acid ( i.e., `CO_(2) (aq) " plus " H_(2)CO_(3))` concentration to maintain the pH of blood at 7.4 ? The first dissociation constant of `H_(2)CO_(3) (H_(2)CO_(3) hArr H^(+) + HCO_(3)^(-)) " is " 4.2xx10^(-7)` where the `H_(2)CO_(3)` is assumed to include `CO_(2)(aq)` i.e., dissolved `CO_(2)`. [ log 4.2=0.6232]

A

10.6

B

1.8

C

180

D

31

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a
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The pH of the a solution containing 0.4 M HCO_(3)^(-) is : [K_(a_(1)) (H_(2)CO_(3)) = 4 xx 10^(-7), K_(a_(2)) (HCO_(3)^(-)) = 4 xx 10^(-11)]

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