The surface tension of a dilute soap solution is lower than that of pure water because Answer: surface tension of soap solution...

The surface tension of a dilute soap solution is lower than that of pure water because

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soap molecules accumulate more at the surface than in the bulk solution

साबुन के अणु का संचय समष्टि विलयन की अपेक्षा सतह पर अधिक होता है।, Option ID :- 3225,

 
soap molecules accumulate more in the bulk of the solution than on the surface
साबुन के अणु सतह की अपेक्षा समष्टि विलयन में अधिक संचित होते हैं। , Option ID :- 3226,

 
the soap molecules aggregate uniformly in the bulk and the surface.
साबुन के अणु सतह तथा समष्टि विलयन दोनों में एकसमान पुंजित होते हैं।, Option ID :- 3227,

 
soap molecules form micellar structures at low concentration.
साबुन के अणु न्‍यून सांद्रता में मिसेली संरचना बनाते हैं।, Option ID :- 3228,

Answer: surface tension of soap solution is less than pure water because pure water have no impurity and behave as strong streched strong bond but when soap is added the bond become loose due to presence of stiarate ion and hydrogen ion

Soap molecules are composed of long chains of carbon and hydrogen atoms. This separates the water molecules from each other. Since the surface tension forces become smaller as the distance between water molecules increases, the intervening soap molecules decrease the surface tension.

Soap molecules are composed of long chains of carbon and hydrogen atoms. At one end of the chain is a configuration of atoms which likes to be in water (hydrophilic). The other end shuns water (hydrophobic) but attaches easily to grease. In washing, the "greasy" end of the soap molecule attaches itself to the grease on your dirty plate, letting water seep in underneath. The particle of grease is pried loose and surrounded by soap molecules, to be carried off by a flood of water.

In a soap-and-water solution the hydrophobic (greasy) ends of the soap molecule do not want to be in the liquid at all. Those that find their way to the surface squeeze their way between the surface water molecules, pushing their hydrophobic ends out of the water. This separates the water molecules from each other. Since the surface tension forces become smaller as the distance between water molecules increases, the intervening soap molecules decrease the surface tension. If that over-filled cup of water mentioned earlier were lightly touched with a slightly soapy finger, the pile of water would immediately spill over the edge of the cup; the surface tension "skin" is no longer able to support the weight of the water because the soap molecules separated the water molecules, decreasing the attractive force between them.