BIOS 20188 Lecture Notes - Lecture 21: Carbonic Anhydrase, Buffer Solution, Partial Pressure
3 Apr 2020
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Acids: essentially a molecule with a h proton that it is willing to give up. Strong acids vs. weak acids: level of dissociation of a moleculre into its proton and conjugate base. K = [h + ][a - ]/[ha] ph: measure of h ion concentration. Henderson- hasselbalch equation ph is -log[h + ] pk a = -log of dissociation constant (strong acid = low pka) Allows us to calculate ph in any buffered solution. Uses the h/h equation, but included the partial pressure of co 2 gas. There is no carbonic acid in the body, as due to the carbonic anhydrase it is usually replaced with carbon dioxide . Therefore, we use this to calculate physiologic ph. 2)use the acid-base map and the henderson-hasselbalch equation to demonstrate how abnormal concentrations of hco 3 . And pco 2 can produce a normal ph. Acidemia : produced by pathophysiologic process of acidosis (too low of a ph)
