Our first goal of this experiment was to determine the solubility of oils, fats, soaps, and detergents that we created in the first week. The process of making these substances can be seen in our experimental design. In order to find the solubility of these substances, we used H20, Acetone, Ethyl Acetate, and Ethanol (Table 3). Using these, we were able to find the physical properties of each, and determine their solubility in different compounds and see how they reacted. We would compare these results to each soap and detergent, and see how they differed. Looking at Table 3, you can observe the differences of the physical properties such as the amount of bubbles, soap formed, and whether it remained a solid or not. Our next goal was to examine any environmental impact these …show more content…
The soap micelles will only take up oil particles using the hydrocarbon ends, while the negatively charged groups remain attached to the water that was used. This process describes how soaps and detergents are used to clean dirt and oil of certain surfaces. As we learned in lab and lecture “like dissolves in like.” The hydrophobic ends of our detergent and soap molecules emulsify the oil, and hydrophilic end will remain with the water molecules, breaking apart any dirt and potential grease. During our lab we tested the ability of each soap and detergent to see if it could remove grime off a dirty counter top. After mixing each with water, the hydrophilic ends kept with the water, while any dirt or grime was removed from the hydrophobic side, exemplifying the molecular benefits of these products. The intermolecular forces involved in these processes would be Dipole-Dipole (opposite charge attraction) and Hydrogen Bonding; Hydrogen molecules are covalently bonded to the electronegative