This page will give a insight to the process of Saponifacation with some important 
chemical equation which are not given in N.C.E.R.T or S. CHAND 

of class 10th Std.

      the pictorial /animated image can help you to understand it better have a look  

Key Concepts about soaps and saponification :

• Soaps are produced during the chemical reaction known as saponification.
• Saponification is the reaction between a fat or oil and a base, producing glycerol and a salt (soap) 
• fat or oil + base -----> glycerol + salt (soap)
• Soaps are usually sodium or potassium salts of long-chain fatty acids
• Soaps are cleaning agents or detergents.
• Molecules of soap are made up of two parts: 
• a non-polar , hydrophobic tail consisting of a long hydrocarbon chain 
• a hydrophilic, negatively charged, carboxylate ion (anion) head
• Hydrophobic: aversion to water, not readily wettable by water. 
• Hydrophilic: affinity for water, wettable by water

Saponification :

fat or oil (ester)	+	base	heat ----->	glycerol (alkanol)	+	salt (soap)
RCOOR'	+	NaOH	heat ----->	R'OH	+	RCOO-Na+

Example of saponification :

glyceryl tristearate (ester)	+	NaOH (base)	--->	glycerol (alkanol)	+	sodium stearate (salt, soap)
H | O || H- C - O- C -(CH2)16-CH3 | O || H- C - O- C -(CH2)16-CH3 | O || H- C - O- C -(CH2)16-CH3 | H	+	3NaOH	--->	H | H- C -OH | H- C -OH | H- C -OH | H	+	3CH3(CH2)16COO-Na+

Most soaps are made from vegetable oils such as olive oil, palm oil and coconut oil.
Some soaps are made from animal fats (tallows).

Potassium soaps tend to be softer and more water-soluble than the corresponding sodium soap.

Soaps from unsaturated fatty acids are softer than those from saturated fatty acids.

Cleaning Action of Soaps (mechanism) :

When a soap such as sodium stearate dissolves in water, carboxylate anions and metal cations are produced:

CH3(CH2)16COO-Na+

water ----->

CH3(CH2)16COO-(aq) + Na+(aq)

Action of micelles in Removal of dirt from the cloth

The non-polar, hydrophobic, long hydrocarbon chain end of the carboxylate ion attaches to non-polar dirt, grease and oil.

The hydrophilic, carboxylate anion end is attracted to polar water molecules by ion -dipole interaction 

Soap micelles, clusters of soap molecules in which the hydrocarbon chains are attracted to each other by Van der Waals forces (dispersion forces, London forces, weak intermolecular forces), surround the non-polar dirt particle, with the anion heads attracted to the surrounding water.

When agitated, the soil particle surrounded by soap micelles breaks free and remains dispersed in the washing water because the carboxylate anions repel each other.

The soil particle surrounded by soap micelles forms an emulsion in the washing water. An emulsion is a suspension of one liquid in another liquid. Soap is an emulsifying agent because it allows oil to be suspended in water.

As a cleaning agent, soap suffers from two main drawbacks :

• it does not function well in acidic solutions because of the formation of insoluble fatty acid 
  eg. CH₃(CH₂)₁₆COO^-Na⁺_(aq) + HCl_(aq) -----> CH₃(CH₂)₁₆COOH_(s) + Na⁺_(aq) + Cl^-_(aq)
• it forms insoluble precipitates with Ca²⁺ and Mg²⁺ ions present in hard water, forming a scum
  eg. 2CH₃(CH₂)₁₆COO^-Na⁺_(aq) + Ca²⁺_(aq) -----> [CH₃(CH₂)₁₆COO^-]₂Ca²⁺_(s) + 2Na⁺_(aq)

Additives such as sodium carbonate and phosphates can help offset these effects.

synthetic are increasingly being used instead of soaps because they do not suffer from these disadvantages to the same extent.