# Question #940b6

Sep 28, 2017

The blood's Bicarbonate weak-acid/conjugated-base buffer system.

#### Explanation:

Since the pH of Blood has to be maintained in the narrow range of $\left(7.35 - 7.45\right)$, a suitable buffer system is in order. That buffer system is the Bicarbonate Buffer System.

$C {O}_{2}$ and ${H}_{2} O$ are catalyzed by an enzyme called Carbonic Anhydrase to form ${H}_{2} C {O}_{3}$ (Carbonic Acid) which dissociates back and forth into $H C {O}_{3}^{-}$ (Bicarbonate) and ${H}^{+}$ (Hydrogen Proton).

Here is the complete reaction:

$C {O}_{2} + {H}_{2} O r i g h t \le f t h a r p \infty n s {H}_{2} C {O}_{3} r i g h t \le f t h a r p \infty n s H C {O}_{3}^{-} + {H}^{+}$

Just like any Buffer, Bicarbonate Buffer works by neutralizing any extra acid or base introduced into the system by keeping its Weak Acid, then it'll fail to balance the pH and result in cases of Acidosis or Alkalosis.