Human blood is kept at a typical pH of 7.40 mainly by the carbonic acid–carbonate ion...

Human blood is kept at a typical pH of 7.40 mainly by the carbonic acid–carbonate ion buffer system. The corresponding chemical equation describing the buffer would be: H2CO3(aq) + H2O(l) ⇌ HCO3-(aq) + H3O+(aq) The appropriate Ka value for carbonic acid is 4.3×10-7, so its pKa value is 6.37. Calculate the [base]/[acid] ratio in human blood. (Answer to 3 significant figures, no units)

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Expert Solution

According to the equilibrium reaction given for the buffer system in human blood:

$H_2CO_3_{(aq)}+H_2O_{(l)}\rightleftharpoons HCO_3^-_{(aq)}+H_3O^+_{(aq)}$

The equilibrium constant for this reaction is:

Taking logarithms in equation (1):

Rearranging this equation according from the logarithmic properties:

Multiplying this equation by -1:

According to the definition of pH and pKa:

The ratio [HCO₃^-]/[H₂CO₃] is then:

Substituting known values:

queen_honey_blossom answered 1 year ago

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