Crystallization
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Crystallization is a solid-liquid separation technique, or the process of formation of solid crystals from a homogeneous solution.
For crystallization to occur the solution at hand ought to be supersaturated. Put simply, the solution should contain more solute molecules than it would under ordinary conditions. This can be achieved by various methods -- solvent evaporation, cooling, chemical reaction, 'drowning' being the most common ones used in industrial practice.
To make things clear we can use a simple example. We take a bowl of water to which we add sugar crystals. We keep adding sugar to it until we reach a stage when no more crystals can be dissolved. This solution so obtained is a saturated one. One can dissolve further crystals into this saturated solution, by heating it: solubility of solutes generally increases with temperature. When the temperature of the solution is allowed to attain equilibrium with the surroundings, the solubility of the solute decreases (because the temperature of the solution has decreased) and the 'excess' sugar so added crystallizes out.
This process illustrates the simplest of supersaturation techniques. 'Drowning' is the addition of a nonsolvent in the solution that decreases the solubility of the solid. Alternatively, chemical reactions can also be used to decrease the solubility of the solid in the solvent, thus working towards supersaturation.
Crystallization can be divided into stages - primary nucleation is the first. Simply defined, it's the growth of a new crystal, which in turn causes secondary nucleation - the final stage (if removal of the crystals is not an issue). Secondary nucleation requires existing crystals to perpetuate crystal growth. In our sugar example, we had obtained such nuclei when the 'excess' sugar had just about crystallized out assisting further crystal formation. Secondary nucleation is the main stage in crystallization for this is what causes the 'mass production' of crystals.