Your first post's reasoning is correct. The protonated decanoic acid will be able to form hydrogen bonds. Yet, you need to consider both the deprotonated and protonated states.
You need to consider them in relation to the molecules pka:
pH<pKa - the molecule will be protonated
pH=pKa- molecule will be neutral (half will be protonated and half unprotonated)
pH>pka- the molecule will be mostly deprotonated
In the case for decanoic acid, when the hydroxyl group is deprotonated it will mostly bear a negative charge. The charged the molecule will be able to make stronger intermolecular bonds. Remember, as the strength of intermolecular bonds increases, the volatility decreases.
Meanwhile, if you being to lower the pH, the proportion of protonated decanoic acid increases and it eliminates the negative charge, making it neutral. You have to note that electrostatic interactions are much stronger than hydrogen bonds. As a result, intermolecular bond strength decreases and volatility increases.