Soap
Soap is a salt of a fatty acid used in a variety of cleansing and lubricating products.[1] In a domestic setting, soaps are surfactants usually used for washing, bathing, and other types of housekeeping. In industrial settings, soaps are used as thickeners, components of some lubricants, and precursors to catalysts.
When used for cleaning, soap solubilizes particles and grime, which can then be separated from the article being cleaned. In hand washing, as a surfactant, when lathered with a little water, soap kills microorganisms by disorganizing their membrane lipid bilayer and denaturing their proteins. It also emulsifies oils, enabling them to be carried away by running water.[2]
Soap is created by mixing fats and oils with a base,[3] as opposed to detergent which is created by combining chemical compounds in a mixer.
Humans have used soap for millennia. Evidence exists for the production of soap-like materials in ancient Babylon around 2800 BC.
Since they are salts of fatty acids, soaps have the general formula (RCO2−)nMn+ (Where R is an alkyl, M is a metal and n is the charge of the cation). The major classification of soaps is determined by the identity of Mn+. When M is Na (Sodium) or K (Potassium), the soaps are called toilet soaps, used for handwashing. Many metal dications (Mg2+, Ca2+, and others) give metallic soap. When M is Li, the result is lithium soap (e.g., lithium stearate), which is used in high-performance greases.[4] A cation from an organic base such as ammonium can be used instead of a metal; ammonium nonanoate is an ammonium-based soap that is used as an herbicide.[5]
Unlike detergents, when used in hard water soap does not lather well and a scum of stearate, a common ingredient in soap, forms as an insoluble precipitate.[6]
