Reliable values for the thermodynamic functions associated with the solvati
on of a water molecule in its own liquid phase and in cyclohexane, at 25 de
greesC, are obtained using experimental data from different investigations.
They are successfully rationalized by means of a general theory of solvati
on. The standard Gibbs energy change is given by the balance of two contras
ting terms: the work to create a cavity in the solvent suitable to host the
water molecule; and the work to turn on the water-solvent interactions. It
proves that the work of cavity creation is largely overwhelmed by the form
ation of two H-bonds in liquid water, whereas it is almost exactly counterb
alanced by the establishment of van der Waals interactions in liquid cycloh
exane.