Project 17 Soaps Lab Report

6. The solubility of the solids were tested using a micro tray, by placing them in water and oil to observe their polarity,

The topic is: The cleanest cleaner. In this experiment, the scientists will be testing which brand of detergents cause a better cleaning effect on one stain on multiple white shirts. The independent variable in this experiment consists of the different detergents, while the dependent variable consists of the amount by which the stain faded (using the purple light scale), and or removed, others include the white t shirts, washing cycle, and drying cycle, staining agent, and cycle of drying and washing. The control variable in this experiment will be the 1 trial run with water only per experiment. The unit while measuring the amount of detergent is mL, and a scale which the is going to use to measure the amount of stain faded.

Water (H2O) is a good solvent because it is partially polarized. The hydrogen ends of the water molecule have a partial positive charge, and the oxygen end of the molecule has a partial negative charge. This is because the oxygen atom holds on more tightly to the electrons it shares with the hydrogen atoms. The partial charges make it possible for water molecules to arrange themselves around charged atoms (ions) in solution, like the sodium (Na+) and chloride (Cl−) ions that dissociate when table salt dissolves in water.

The goal of this project was to make, and test four soaps, and two detergents. The purpose of making four different soaps and two detergents was needed in order to decide which one would be best for the environmental group to use in the future that would allow for the safest cleanup of an oil spill while not harming the animals or the environment in the process. It was necessary to test the impact of the four soaps and two detergents by analyzing their different properties based off of their specific characteristics and the wastewater left over from the vacuum filtration procedure. This procedure had to be undertaken in order to confirm which of the soaps and detergents synthesized is most

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The purpose of this experiment was to determine which solvent (water or 70% isopropyl alcohol) is better at dissolving salt. The hypothesis for this experiment was, “If we pour a spoonful of salt into water and a spoonful of salt into isopropyl alcohol, then the salt will dissolve faster in the water than the isopropyl alcohol because water is polar and can break apart the salt molecules (NaCl) to cause it to dissolve faster. In this experiment, salt was poured into each solvent and stirred for a specific time until the salt dissolved. The time it took for the salt to dissolve in each solvent was recorded and compared.

An ice bath was prepared in a large beaker and a small cotton ball was obtained. 0.5 g of acetanilide, 0.9 g of NaBr, 3mL of ethanol and 2.5 mL acetic acid was measured and gathered into 50mL beakers. In a fume hood, the measured amounts of acetanilide, NaBr, ethanol and acetic acid were mixed in a 25mL Erlenmeyer flask with a stir bar. The flask was plugged with the cotton ball and placed in an ice bath on top of a stir plate. The stir feature was turned on a medium speed. 7mL of bleach was obtained and was slowly added to the stirring flask in the ice bath. Once all the bleach was added, stirring continued for another 2 minutes and then the flask was removed from the ice bath and left to warm up to room temperature. 0.8mL of saturated sodium thiosulfate solution and 0.5mL of NaOH solution were collected in small beakers. The two solutions were added to the flask at room temperature. The flask was gently stirred. Vacuum filtration was used to remove the crude product. The product was weighed and a melting point was taken. The crude product was placed into a clean 25mL Erlenmeyer flask. A large beaker with 50/50 ethanol/water

If soap was added to the experiment, I think that they would mix because soap is what breaks the oil when washing dishes because they have around the same densities. The mixture was a heterogeneous mixture because you could see the dissimilar parts (the oil and the water). The hypothesis was correct because the oil never mixed with the water and the oil was always on top of the water. If I could do this experiment again, I would use seawater to see how the oil would react with

Purpose: The purpose of this experiment is to learn about and use the Scientific Method. The discussion of physical properties such as density, color, texture, smell, and solubility will take place.

For example lipids are insoluble in water whereas carbohydrates are soluble in water. This is because lipids contain non - polar hydrocarbon units whereas water contains polar hydrocarbon units. So when the two are mixed together there is no attraction between particles so no breakdown is possible. But lipids care soluble in non - polar solvents, e.g. alcohol. Carbohydrates have polar hydroxyl groups, so there

In one of our research we found out that last October 2005 the FDA’s Non-Prescription Drug Advisory Committee was tasked to discuss and investigate the benefits as well as the possible risks relating to the antibacterial products. The FDA’s discussion commence in a request for further research regarding specific antibacterial product being sold in the market. The debate regarding different antiseptic products has focused mainly on the antibacterial bath soap in which most of these products contain triclosan or triclocarban. Although the FDA did not announce any formal regulations regarding the right percentage concentration of triclosan used in antibacterial products most of these products has a triclosan concentration raging from 0.1% to 0.45%. Triclocarban which is said to be a “cousin” of triclosan is also used in some antibacterial bath soap.

Samples of benzophenone, malonic acid, and biphenyl were each tested with water, methyl alcohol, and hexane. Benzophenone was insoluble in water as it is nonpolar while water is highly polar. Benzophenone was soluble in methyl alcohol, dissolving in 15 seconds, because methyl alcohol is intermediately polar as benzophenone is nonpolar. Methyl alcohol is polar but not as much as water. Thus, the nonpolar benzophenone was soluble in methyl alcohol. Benzophenone was partially soluble in hexane because hexane is nonpolar as is benzophenone. Thus, benzophenone was dissolved in hexane. Malonic acid was soluble in water because both malonic acid and water are polar. It took 25 seconds for malonic acid to dissolve in water. Malonic acid was soluble in methyl alcohol because malonic acid is polar and methyl alcohol is intermediately polar, allowing malonic acid to dissolve in the methanol in 15 seconds. Malonic acid was insoluble in hexane because hexane is nonpolar while malonic acid is polar. Biphenyl was insoluble in water as water is highly polar whilst biphenyl is nonpolar. Biphenyl was partially soluble in methanol which is intermediately polar whilst biphenyl is nonpolar, allowing it to dissolve a little. Biphenyl was soluble in hexane because both biphenyl and hexane are nonpolar molecules. Biphenyl dissolved in hexane in 10 seconds.

In week one we performed a qualitative solubility test of our fats and oils, synthesized our soaps and detergents, and performed a solubility test and lathering test for the soaps and detergents. We wanted to test the solubility of our starting materials of the soap making process to understand the properties of the materials. In our initial solubility test of the starting materials, we found that most of the materials were insoluble. As you can see in Table 2.0, olive oil and vegetable oil were only soluble in toluene and the shortening and lard were only partially soluble in acetone. In order to understand the solubility of the soaps and detergents, after our synthesis and filtration, we performed a qualitative solubility test with each of

As mentioned in the discussion, olive oil, vegetable oil, crisco, and lard were soluble in nonpolar solvents and insoluble in polar solvents. This is due to the chemical composition of polar and nonpolar substances which results from the molecular shape as well as properties of dissolving solutes in solution. Polar substances are hydrophilic and contain polar Van Der Waals interactions (intermolecular forces) such as dipole-dipole forces, ion-dipole forces, and hydrogen bonding. Nonpolar substances are hydrophobic and contain non-polar Van Der Waals interactions. ‘Like dissolve like’ is the reason only polar solutes dissolve in polar solvents and why nonpolar solutes dissolve in nonpolar solvents. Molecules with similar polarity have similar intermolecular forces and therefore, can interact with each, or in this case dissolve9. Additionally, the solubility of a compound is determined by the length of the hydrocarbon chain. Long hydrocarbon chains such as the one found in oleic acid makes a compound more insoluble10. Therefore, since the lipids used in this experiment were hydrophobic substances and each lipid has long hydrocarbon chains, the results were consistent with the scientific literature and principles.

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