Solubility

Introduction:
Solubility is the measure that indicates the maximum solute that can dissolve in a determine measure of solvent in a specific temperature.
In our lives is very commonly used this property because is useful in the kitchen, in cleaning of the house, in the beverages, in some products, in beauty products, and hair products, etc.

Solubility
Solubility is the property of a solid,liquid, or gaseous chemical substance called solute to dissolve in a liquid solvent to form a homogeneous solution. The solubility of a substance fundamentally depends on the used solvent as well as on temperature and pressure. The extent of the solubility of a substance in a specific solvent is measured as the saturation concentration where adding more solute does not increase the concentrationof the solution.
Solute is the substance that is dissolves in another substance, known as a solvent.
Solvent is a liquid or a gas that dissolves a solid, liquid or gas solute, resulting in a solution
The solvent is generally a liquid, which can be a pure substance or a mixture. One also speaks of solid solution, but rarely of solution in a gas (see vapor-liquid equilibrium instead)
The extentof solubility ranges widely, from infinitely soluble (fully miscible) such as ethanol in water, to poorly soluble, such as silver chloride in water. The term insoluble is often applied to poorly or very poorly soluble compounds.
Types of solutions
There are three types of solutions:
* Saturated : the amount of the solute is equal to the values on its solubility
* Unsaturated: the amountof solute is less than that its solubility
* Supersaturated: the solute dissolve is greater than that indicated by its solubility


Molecular view
Solubility occurs under dynamic equilibrium, which means that solubility results from the simultaneous and opposing processes of dissolution and phase joining (e.g. precipitation of solids). The solubility equilibrium occurs when the twoprocesses proceed at a constant rate.
The term solubility is also used in some fields where the solute is altered by solvolysis. For example, many metals and their oxides are said to be "soluble in hydrochloric acid," whereas the aqueous acid degrades the solid to irreversibly give soluble products. It is also true that most ionic solids are degraded by polar solvents, but such processes arereversible. In those cases where the solute is not recovered upon evaporation of the solvent the process is referred to as solvolysis. The thermodynamic concept of solubility does not apply straight forwardly to solvolysis.
When a solute dissolves, it may form several species in the solution. For example, an aqueous suspension of ferrous hydroxide, Fe(OH)2, will contain the series[Fe(H2O)6 − x(OH)x](2 − x)+ as well as other oligomeric species. Furthermore, the solubility of ferrous hydroxide and the composition of its soluble components depend on pH. In general, solubility in the solvent phase can be given only for a specific solute which is thermodynamically stable, and the value of the solubility will include all the species in the solution (in the example above, all the iron-containing complexes).Factors affecting the solubility
Solubility is defined for specific phases. For example, the solubility of aragonite and calcite in water are expected to differ, even though they are both polymorphs of calcium carbonate and have the same chemical formula.
The solubility of one substance in another is determined by the balance of intermolecular forces between the solvent and solute, and theentropy change that accompanies the solvation. Factors such as temperature and pressure will alter this balance, thus changing the solubility.
Solubility may also strongly depend on the presence of other species dissolved in the solvent, for example, complex-forming anions (ligands) in liquids. Solubility will also depend on the excess or deficiency of a common ion in the solution, a...