MadSci Network: Chemistry |
Dear User, Extraction is one of the oldest chemical procedures known to mankind. Extraction and concentration of pharmaceutically active substances , dyes, etc. date back to ancient Egypt and Mesopotamia and probably earlier than that. Your question touches a very broad area of basic chemistry, and I am afraid that I would only be able to provide a very basic set of concepts and hints - for full explaination you should refer to any decent textbook on basic chemistry. Solubility of substances in solvents depends on how efficiently the solvent molecules break interactions between molecules of the solute (i.e. substance to be dissolved) and how efficiently the solvent molecules form new interactions with the solute molecules. Roughly, substances can be divided into two very general classes - polar and non-polar, depending on their dipole moments. Also, very roughly, substances may be divided into hydrophilic and hydrophobic i.e. "loving water" and "hating water". These sets overlap but are not identical. Solvents, of course, also fall into these categories. Polar substances readily form interactions with polar substances. These interactions are based chiefly on Coulomb - type forces, i.e. on interaction of partial charges which result from polarization of the molecules. Non-polar molecules, likewise, interact with non-polar ones, mostly via surface-surface type of interactions (van der Waals etc.). This is of course a very broad generalization, but it will suffice. As an example, it is easy to observe water droplets sliding around on teflon-covered pan, without even wetting the pan - due to the fact that water is highly polar whereas teflon is not. Oil, on the contrary, spreads nicely over teflonized surfaces due to the fact that both oil and teflon are hydrophobic, relatively non-polar substances. Of course, molecules generally can be assigned to both classes, partially. And thus, caffeine is a polar molecule, which has a significant hydrophobic portion (look at the structure). In water, caffeine dissolves chiefly via formation of hydrogen bonds involving atoms with free electron pairs (N and O). In Ch2Cl2, these interactions give way to generalized hydrophobic interactions of the nonpolar dichloromethane with hydrophobic parts of the molecule, such as -CH3 etc. Likewise, caffeine readily dissolves in chloroform and several other organic solvents. http://www.scimedia.com/chem-ed/sep/extract/extract.htm http://www.uwec.edu/Academic/Curric/cheniepj/CAFFEIN2.htm Solubility of caffeine in water is about 9 times less than in dichlorometane - thus when a solution of caffeine in water is brought in contact with dichloromethane, most of the caffeine will migrate into the organic layer (see partition theory in your textbook). In order to complete the extraction, fresh solvent is used twice (i leave it as an excercise for you to calculate the percentage of caffeine extracted from a given volume of solution using one, two, three etc. portions of organic solvent but it can be easily seen that two changes will extract most and three - practically all of the alkaloid). Once again, the above is a very general and incomplete explaination. The fact that you feel "muddled" about this procedure may indicate incomplete understanding of the basic chemistry principles (polarity, solubility, intermolecular interactions) which may be vital for you to pass the necessary exams. Often, this condition may be remedied by reading appropriate literature - such as university-grade textbooks on general chemistry, which may be found in any decent library. Feel free to contact me if you need assistence. Hope it helps. A.G.E.
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