Problem: A. What is the ratio of HCO3- to H2CO3 in the blood of pH 7.4?B. What is the ratio of HCO3-- to H2CO3 in an exhausted marathon runner whose blood pH is 7.2?

FREE Expert Solution

We are being asked to determine the ratio of HCO3- to H2CO3 in

a. the blood of pH 7.4

b. an exhausted marathon runner whose blood pH is 7.2

H2CO3 is a weak acid (and based on the Bronsted-Lowry definition, an acid is a proton (H+) donor. Once H2CO3 loses its proton, its conjugate base is formed)

H2CO3 + H2 HCO3- + H3O+

Whenever we have a conjugate base and weak acid, we have a buffer.

We will use the Henderson-Hasselbalch equation

Derive the ratio of HCO3- to H2CO3

where HCO3- is the conjugate base and H2CO3 is the weak acid

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Problem Details

A. What is the ratio of HCO3- to H2CO3 in the blood of pH 7.4?

B. What is the ratio of HCO3-- to H2CO3 in an exhausted marathon runner whose blood pH is 7.2?

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Henderson Hasselbalch Equation (IGNORE) concept. If you need more Henderson Hasselbalch Equation (IGNORE) practice, you can also practice Henderson Hasselbalch Equation (IGNORE) practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Young's class at UCSD.