Question

Why does the strength of an acid affect the enthalpy of neutralization? How is this important in a biological system?

Answer 1

Strong acids --> will dissoaciate 100%

So this helps to form stronger bonds when neutralization occurs

for

Weak Acids --> will not dissoaciate 100%; therefore not all bonds are broken easily, plenty of material remains molecular (not ionic)

In general, the standard enthalpy of neutralization for organic acids is slightly less exothermic than that of mineral acids (stronger acids)

This is mainly due to the partial ionization of weak organic acids.

The bond between the proton and its conjugate base requires energy to be broken... This will "take out" some energy... therefore, expect a lower enthalpy change.

This is pretty important for biology, since the changes in pH and energy requirements are ipmortant, for instance, in the stomach where HCl will help to process material due to the enthalpy of neutralization and acidity levels