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  Water Solubility Homework Help - K-12 Grade Level, College Level Chemistry

Introduction to Water Solubility

Water has been known as "universal solvent" and widespread distribution of it on this planet and essential role in life make it the discussions point of solubility. The Water can dissolve many ionic salts due to its high dielectric constant and its ability to solvate ions. The former reduces attraction among oppositely charged ions and after that stabilizes the ions by binding to them and delocalizing charge density. Various organic compounds mainly alkanes and the other hydrocarbons are almost insoluble in water. The Organic compounds that are water soluble usually have donor groups and hydrogen bond acceptor. Least soluble compounds is diethyl ether, which can serve only as the hydrogen bond acceptor and is 75% hydrocarbon in nature.

The most important characteristic of water which affects these solubilities is the extensive hydrogen bonded association of its molecules with each other. The hydrogen bonded network is become stable by the sum of all the hydrogen bond energies and if nonpolar molecules like hexane were inserted into the network they destroy local structure without contributing any hydrogen bonds of their own. Obviously, the hexane molecules experience important van der Waals attraction to neighbouring molecules, but the hydrogen bond is stronger than these attractive forces. Consequently, when the hexane or other nonpolar compounds are mixed with water, the strong association forces of water network exclude the nonpolar molecules, that must then exist in the separate part. This is shown in the following picture, and because the hexane is less dense than water, hexane phase floats on the water phase.

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It should be remember that this tendency of water to exclude nonpolar molecules and groups, since it is a factor in the behaviour and structure of many complex molecular systems. A common nomenclature that is used to depict molecules and regions within molecules is hydrophobic for nonpolar, hydrogen bonding moieties and hydrophilic for polar species.

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