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The concentration of carbonic acid, H2CO3 is approximately 0.0012 M, and the concentration of the hydrogen carbonate ion, HCO3 −, is around 0.024 M. Using the Henderson-Hasselbalch equation and the pKa of carbonic acid (6.4) at body temperature, calculate the pH of the blood.

Sagot :

SOLUTION:

[tex]\begin{aligned} \text{pH} & = \text{p}K_{\text{a}} + \text{log} \left(\frac{[\text{conjugate base}]}{[\text{acid}]}\right) \\ & = \text{p}K_{\text{a}} + \text{log} \left(\frac{[\text{HCO}_3^-]}{[\text{H}_2\text{CO}_3]}\right) \\ & = 6.4 + \text{log} \left(\frac{0.024}{0.0012}\right) \\ & = \boxed{7.7} \end{aligned}[/tex]

Hence, the pH of the blood is 7.7

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