How does blood act like a buffer solution?

Buffer solutions resist changes in pH, how does blood achieve this? why is there a need to maintain constant pH in the blood?



(I know about the bicarbonate thing, so please go into further detail when answering)How does blood act like a buffer solution?
since you know about the CO2/bicarbonate system, you can write out the equilibrium equation:

CO2+H2O = HCO3(-) + H+

Ka=[HCO3-]*[H+]/[CO2] (since the concentration of water is constant and doesn't change much, it's often included in Ka)



so upon conversion you'll get that

pH=pKa+log([CO2]/[HCO3-])

Since CO2 and water are abundant in the blood, this system forms easily. Of course the presence of proteins and other substances also affects the pH of blood, but there are cellular mechanisms (inluding enzymes, carbonic anhydrase being one that guard the homeostasis) to keep it pretty much constantHow does blood act like a buffer solution?
The pH of human blood must stay in a relatively narrow range around pH = 7.4 (7.35-7.45) in order to ensure cellular survival. It can be maintained within these limits thanks to buffer systems utilizing plasmatic carbonates, phosphates or proteins for example.



The buffer ability of blood, in addition to its role in the metabolism, can also minimize the consequences of an accidental ingestion of acid (or base).