Life as we know it, having started in a marine environment, is strongly dependent on water. Water, in turn, is a very reactive substance, and even when no net chemical reactions take place, it tends to interact with most substances by solvating them. The solvation can be very strong, as is the case with highly charged cations, where, for example, the hydration Gibbs free energy is very negative: -6800kJmol-' for Zr4+ ions.' It can be rather weak, as is the case for nonpolar organic molecules, where the group interaction Gibbs free energy CH2/water is only 2.7 kJ mol-' .2 In the first case, strong coordination bonds are formed by the oxygen electron-pair-donor atoms of several water molecules and the positively charged ion. In the second case weak van-der-Waals interactions take place between the not very polarizable CH2 and H 2 0 moieties. This attractive interaction cannot overcome the intermolecular water/water attractions, which accounts for the positive (unfavourable) value. For polar organic molecules, however, the main form of interaction is the formation of hydrogen bonds between one or more water molecules and the organic one. Water molecules can both donate and accept hydrogen bonds, not only to and from organic molecules but also to and from other water molecules. This gives rise to the well known three-dimensional network of liquid water.3 Solutes in liquid water must compete with water molecules for the formation of hydrogen bonds. Therefore the binding of water to organic molecules is a complicated phenomenon, unless both the organic molecule and the water molecule are in very dilute solution in some inert (nonpolar) solvent. In order to understand this binding it is necessary to determine first how much total water is available for this binding, then how much of this water is bound and how much is free, and lastly the mode of the binding of the water. This review deals with these three problems.