Explain the cleansing action of soap. 

D cleansing action of soap is as follws-

The soap molecules form micelles around the soap in such a way dat  d hyprophilic (d ionic part or d polar part) part is in water n the hydrophobic (the hydrocarbon part or d nonpolar) part is surrounding the dirt. Being polar the hydrophilic part is attracted to the water. It starts pulling the hydrophobic part vich in turn pulls d dirt away from the surface of the cleaning material. This way  the cleaning material is no more dirty.Normally for dis to occur der is a need of extra force n lot of water. The extra force is provided by scrubbing the cleaning mateial.

Hope dis helps

Cleansing Action of Soap

Unimolecular film of soap molecules on water surface

A soap has two dissimilar ends. At one end is the hydrocarbon chain that is non-polar and hydrophobic (oil soluble). At the other end there is the carboxylate ion that is polar and hydrophilic (water soluble).

 When soap is added to water, its molecules make a unimolecular film on the surface of water with their carboxyl groups dissolved in water and the hydrocarbon chains standing on end to form a hydrocarbon layer as shown in the figure below.

Cleaning Action of a Soap

When a dirty cloth is soaked in soap solution, soap dissolves dirt (fat or oil with dust absorbed in it) by micelle formation. The oil or fat is at the centre of the sphere with fat-soluble hydrocarbon chains of soap dissolved in it. The water soluble carboxylate ions make a hydrophilic surface around this sphere and render the miscelles of oil or fat water-soluble. Thus the micelle is dissolved in water and is washed away.

Soap tends to concentrate on the solution surface and therefore lowers its surface tension, causing foaming. This helps it to penetrate the fabric. It emulsifies fat in dirt to form micelles render all the micelles water-soluble. Thus the water washes the dirt away.

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 Because soap is a salt, it partially separates into its component ions in water. The active ion of the soap molecule is the RCOO^-. The two ends of this ion behave in different fashions. The carboxylate end (-COO^-) is hydrophilic (water-loving), and is said to be the "head" of the ion. The hydrocarbon portion is lipophilic (oil-loving) and is called the "tail" of the molecule. This unusual molecular structure is responsible for the unique surface and solubility characteristics of soaps and other surfactants (agents affecting the surface of a material).
In a mixture of soap and water, soap molecules are uniformly dispersed. This system is not a true solution , however, because the hydrocarbon portions of the soap's ions are attracted to each other and form spherical aggregates known as micelles. The molecules tails that are incompatible with water are in the interior of these micelles, while the hydrophilic heads remain on the outside to interact with water. When oil is added to this system, it is taken into these micelles as tiny particles. Then it can be rinsed away.