I found betaine in my face wash. I think it is there because it has a hydrophobic (non-polar) end that can pick up grease, and a hydrophilic (polar) end that means it is attracted to polar solvents, such as water.

My question is why are betaines used over other detergents? What are the factors that contribute to the which detergents are used in face wash (or indeed shampoo/shower gels)?

  • $\begingroup$ Good question. To get you started on some background you might want to read the answers to this question: chemistry.stackexchange.com/questions/4188/… $\endgroup$
    – Michiel
    Jun 2 '13 at 15:31
  • $\begingroup$ I am guessing that you or the manufacturer mean Cocamidopropyl betaine, which is a surfactant. some points are mentioned here en.wikipedia.org/wiki/Cocamidopropyl_betaine such as producing more foam and being less irritating to the eyes and skin $\endgroup$
    – Daniel
    Jun 16 '13 at 4:58

If it's polar, then it won't pick up grease because lipids (fats and oils) are generally non-polar. I don't know specifically how a detergent is chosen, but soaps are chemically the salts of a fatty acid. When choosing a detergent, you want a molecule with a polar head with a long, nonpolar tail.

Recall that water is polar and polar substances dissolve polar substances, and nonpolar dissolve nonpolar. The detergent in a sense forms a "bridge" between the water and the nonpolar substances (dirt, grease, oil, etc.) which would not dissolve in pure water. The detergent molecules form little "cells" (my choice of this word is not a coincidence - this is also how your cell membranes work) with the polar heads facing out and the nonpolar tails mingling with nonpolar dirt molecules inside. This allows the dirt be washed away by water.

As to why certain detergents are chosen, it is probably a balance struck between safety, effectiveness, cost to mass-produce, possibly environmental considerations associated with production, etc.

  • $\begingroup$ Geeze. A detergent is always some sort of "long" chain with a hydrophobic (non-polar) group on one end and a hydrophilic (polar) group on the other. So the molecule has one side of the molecule in water and the other side in oil. $\endgroup$
    – MaxW
    Oct 31 '15 at 5:40

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