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Compare The Solubility Of Oils Fats And Detergents

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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

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In the “Drops of Water on a Penny” lab, I used the pipette to place 30 drops of regular water on the penny. As I was placing the drops of water on the penny, the water began to form a bubble on the penny, sticking together tightly so that it had risen above the penny. This occurred because of the high surface tension water has due to its hydrogen bonding. On the other penny with the soapy water, I was only able to place 24. Soap is a surfactant to water by interfering the hydrogen bonding and decreasing the surface tension so that the water does not stick to each as well as would have.

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Our hypothesis was partially correct, the property changing substances did have the weakest coherency with the lowest drop counts of 23(carbonated), and 14(soap), and pure water did have the strongest bond. What we also found was the the salt also dampened the liquid’s ability to hold onto a penny in large volumes, as all the different salts had a drop average of 24(28x2 & 16), five less than Tap water’s drop count (30). This led us to conclude that pure water has the strongest bond and that all foreign materials weaken the coherency of water. This evidence has led me to believe that similar substances are attracted and are more coherent towards themselves, in this case the water pieces get separated and generally less connected on a really small level due to the obstruction of foreign objects, this is why the different salts perform better than the huge air bubbles or the slippery properties of soap since the latter is more obstructive and the former dissolves with the water and blocks less. When studying a few other groups’ conclusions and data we did indeed find differences: some groups had differing data where a solution had better coherence than water itself which led to differing conclusions.

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Objective: In this lab, students learned the different methods there is to separate substances from one another. They practiced the process of decantation, extraction, filtration, and sublimation. Introduction: Theory: Before being able to isolate the components in a mixture, the students should’ve become familiar with the physical properties of each of the substances. The students were given an unknown sample which has a combination of three different components.

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The purpose of this experiment was to determine the amount of each compound is found in the original mixture. Starting with a mixture of substances the components of the mixture should be able to separate. During this separation all of the components together should have the same mass as that of the starting mass of the mixture.

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Comparing the boiling point temperature ranges of the fractions containing pure product to the literature values, the results obtained from this experiment seem to be consistent with the reported literature values. The first fraction, most likely containing methyl acetate was collected when the boiling point stabilized at 56 C, until it started changing more rapidly at 58C. The literature reports that methyl acetate has a boiling point of 56.7 C1, which is directly in this range. The fifth fraction, most likely containing ethyl acetate was collected when the boiling point stabilized at 75 C and until the temperature reading started changing again more rapidly at 77 C. The literature boiling point of ethyl acetate is 77.1C2, which while not exactly in this range, is very close to the boiling point range obtained in this experiment, suggesting that a pure sample of ethyl acetate was obtained in the fifth fraction. One limitation of this experiment was the fact

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