why soap is collidal in solution? how it does ion-ion repultion?
Asked by kamalnayansingh7 | 13th Jan, 2020, 08:35: AM
Colloidal state of matter: The state in which the size of the particle is such that it can pass through filter paper but not through the animal or vegetable membrane.
Consider the example of soap. Soap is the sodium salt of higher fatty acids and represented as RCOONa.
Examples: Sodium stearate, sodium palmitate
When soap is dissolved in water, it dissociates into RCOO− and Na+ ions.
The RCOO− consists of two parts—a non-polar, long hydrocarbon chain R (which is hydrophobic and called the tail) and the polar group COO− (which is hydrophilic and called the head).
The RCOO− ions are present on the surface with their polar group in water and their non-polar group away from water and remain at the surface.
At higher concentration, these ions do not remain on the surface but are pulled into the bulk of solution. Because of this, RCOO− ions coagulate to form a spherical shape with their hydrocarbon chains pointing towards the centre and the COO− part outwards on the surface of the sphere. This coagulate formed is called ionic micelle.
Each of these micelles contains up to 100 ions.
Answered by Ramandeep | 14th Jan, 2020, 12:32: PM
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