Soaps are sodium or potassium salts of long chain carboxylic acids. They contain two ends having different properties: the carboxylic acid part which is hydrophobic and the ionic end (Na+ or K+) which is hydrophilic.
Structure of a soap molecule
Dirt present in clothes is basically a hydrocarbon. When soap is used in water, the soap molecules tend to surround the dirt such that they form a cluster in which the hydrophobic tails are in the interior of the cluster and the hydrophilic part are on the surface of the cluster (see figure below). The hydrophilic part dissolves in water and the hydrophobic part dissolves in the hydrocarbon (dirt). This formation or cluster is called micelle.
Formation of micelle
Agitating the water by hand or brush forces the hydrophilic end to move along the direction of agitation of water, dragging the micelle holding the dirt out of the clothes and the dirt is rinsed away. In short, the cleansing action of soap is achieved by the formation of micelles.
