# Question #8d583

May 27, 2015

That happens because of the structure of the two molecules, i.e. the atoms to which those acidic hydrogens are bonded to.

Take acetic acid, for example. Its Lewis structure looks like this

The acidic hydrogen in acetic acid is the one bonded to the pxygen atom. Because oxygen is a very electronegative atom, the bond is forms with hydrogen will be quite polar.

That implies that the bonding electrons will spend most of the time around the oxygen atom, leaving the hydrogen atom electron deficient nad causing it to be less tightly held.

The partial positive charge that arises on the hydrogen atom can be easily attacked by a water molecule, which is a polar molecule. Moreover, the negative charge that gets created after the hydrogen is picked off can be easily stabilized by resonance.

On the other hand, the other three hydrogen atoms are bonded to a carbon. As you know, the $\text{C-H}$ bond is considered to be nonpolar, which implies that the hydrogen atom will not develop a partial positive charge.

This means that its bond with carbon will be strong enough to stop a water molecule from being able to pluck it off.

Now take a look at phosphoric acid's Lewis structure

This time, all three hydrogens are bonded to oxygen atoms, which is what ultimately makes them ionizable.

All three can be easily attacked by water molecules and removed from the phosphoric acid molecule.

So, as a conclusion, hydrogen atoms that are attached to carbon atoms are not acidic, while hydrogen atoms attached to oxygen atoms are quite acidic.