Abstract
The apparent first dissociation constant of carbonic acid has been defined in different ways in the literature. Harned and co-workers (8-10) have defined it in terms of molalities of the participating species, including H ions: K s = m H mH CO3 /m CO2 . In contrast, Hastings and Sendroy have defined an apparent constant in which acidity is expressed as H ion activity: K' 1 = a H m HCO3 /m CO2 . These constants differ by a factor γ H , the activity coefficient of H ions at the prevailing ionic strength. Therefore, pK' 1 is greater than pK s by an amount equal to -log γ H , which, at µ = 0.16 M, is approximately 0.1. It is important that the correct value for the apparent dissociation constant or its logarithmic form be entered in the mass action expression or in the Henderson-Hasselbalch equation in order to prevent significant errors in the computation by means of these equations of quantities that cannot be directly measured. Specifically, for the derivation of bicarbonate concentration from P CO2 and pH (-log a H ), pK' 1 is to be used and not an uncorrected pK s .
Original language | American English |
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Journal | American Journal of Physiology - Cell Physiology |
Volume | 260 |
State | Published - May 1 1991 |
Disciplines
- Medical Cell Biology
- Medical Neurobiology
- Medical Physiology
- Medical Sciences
- Medicine and Health Sciences
- Neurosciences
- Physiological Processes