We are asked to find the ratio of HCO3- to H2CO3 in an exhausted marathon runner whose blood pH is 7.2
Since the solution is a buffer, we can use the Henderson-Hasselbalch Equation to calculate the ratio of
In the solution, identify the weak acid and the conjugate base.
Recall from the Bronsted-Lowry definition that an acid is a proton (H+) donor and the base is a proton (H+) acceptor.
What is the ratio of HCO3- to H2 CO3 in an exhausted marathon runner whose blood pH is 7.2?
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What scientific concept do you need to know in order to solve this problem?
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Based on our data, we think this problem is relevant for Professor Billman's class at Abilene Christian University.