# HH Equation to calculate [HCO3-]

by Wek
Tags: equation, hco3
 P: 18 I'm given the following values: pH = 7.48, PO2 = 120mmHg, and PCO2 = 18mmHg. I have to find the [HCO3] using these values. There's one thing I don't understand about the Henderson-Hasselbalch equation and that is how to calculate the [CO2]. I found out that [CO2] = 0.03*PCO2. My question is, what is the 0.03 that is multiplied to the PCO2 to get the [CO2] value? One last thing, the pKa in the HH equation, is it of the HCO2? Thanks
 Admin P: 21,696 As far as I can tell pO2 is irrelevant. You need to find concentration of H2CO3 (could be you are to assume it is identical with concentration of dissolved CO2, that's a common approximation). Then you should use HH equation, pKa1 describes equilibrium of the reaction H2CO3 <-> H+ + HCO3- and you have it either in your textbook or in any tables with Ka values.
 P: 18 Yes, I used the HH equation to find the [HCO3] and it came out to be 13. I' not given any concentration for CO2 or H2CO3. In this case, how would you be able to find the concentration of CO2 or even H2CO3, if its possible at all? The value I used for [CO2] was something I found on Cornell's website but it was not explain why they used that, which is what I'm asking.
P: 21,696

## HH Equation to calculate [HCO3-]

Concentration of CO2 is something that can be calculated - for known partial pressure - using Henry's law.
P: 617
 Quote by Wek Yes, I used the HH equation to find the [HCO3] and it came out to be 13. I' not given any concentration for CO2 or H2CO3. In this case, how would you be able to find the concentration of CO2 or even H2CO3, if its possible at all? The value I used for [CO2] was something I found on Cornell's website but it was not explain why they used that, which is what I'm asking.
0.037 represents the solubility coefficient of C02 in plasma under physiological conditions. Units are mmol/mmHg/cc

Amount of C02 is a linear function of the product P(C02) and aforementioned solubility coefficient.
I believe pK is 6.1 in this case.