🤓 Based on our data, we think this question is relevant for Professor Dixon's class at UCF.
We are asked for the ratio of HCO3- to H2CO3 in blood of pH 7.4.
Since the solution is a buffer, we can use the Henderson-Hasselbalch Equation to calculate the ratio of [HCO3-]/[H2CO3] to have a pH of 7.4:
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 H2CO3 in blood of pH 7.4?