2007-10-18 12:37:25 · 0 answers · asked by Anonymous in Science & Mathematics ➔ Chemistry
They are both, and that is the reason why they work. The most common soap is the sodium salt of stearic acid:
CH3(CH2)16COO-Na+
The CH3(CH2)16)- part is like gasoline or diesel oil. It has an affinity for grease and oil stains. The other part is -COO-Na+. That has an affinity for water. So the two of them, working together, solubilize grease and oil in water and wash them away.
In particular, they form a structure in the water called a micelle. Supposedly, the hydrocarbon tails all dip into the center of the spherical micelle. Then, the -COO-Na+'s all cover the surface of the micelle. Any oil or greasy dirt gets dissolved in the center of the micelle. The -COO-Na+'s carry the micelle into water solution.
The problem is that there is too little room in the center of the spherical micelle to firt all those hydrocarbon chains. So the micelle cannot be exactly like that. But whatever it is, there are micelles, and they look and function a lot like that.
2007-10-18 12:53:00 · answer #1 · answered by steve_geo1 7 · 2⤊ 0⤋
Is Soap Polar Or Nonpolar
2016-10-06 11:48:37 · answer #2 · answered by ? 4 · 0⤊ 0⤋
I believe has a polar and nonpolar end - therefore binding to both the grease and the water. This allows the grease to be washed off by the water. Look it up on google for a better answer.
2016-03-13 23:41:14 · answer #3 · answered by Anonymous · 0⤊ 0⤋
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It deteremines which side will bond so the soap/ detergent can bond with grease molecules to remove from clothes/ whatever. Only one side will of the soap/detergent will create that bond
2016-03-29 03:50:40 · answer #4 · answered by Anonymous · 0⤊ 0⤋
They are both. They have a polar head and non polar tail. They are amphipathic.
2007-10-18 12:42:27 · answer #5 · answered by Anonymous · 0⤊ 0⤋