The transfer of benzene and toluene from gas phase into water is a spontane
ous process at room temperature under Ben-Naim's standard conditions. This
strongly contrasts with the behavior of aliphatic hydrocarbons, for which t
he Gibbs energy of transfer is large and positive. To understand this diffe
rence in behavior between the aromatics and aliphatics, we analyze the hydr
ation of benzene and toluene in a large temperature range using available e
xperimental and computer simulation data. We introduce a small but importan
t modification in the definition of the solvent reorganization enthalpy in
order to handle slightly polar solutes such as the aromatic hydrocarbons, w
hich form weak hydrogen-bonds with water. The analysis shows that, for arom
atic hydrocarbons, the van der Waals interaction energy overwhelms the Gibb
s energy cost for cavity creation at room temperature, thus rendering the h
ydration process spontaneous. The formation of the weak hydrogen-bonds betw
een the aromatic ring and water appears to be largely compensating and not
to contribute significantly to the hydration Gibbs energy.