Soluble In Methanol

Methanol, ethanol, 1-propanol, and 1-butanol are alcohols that contain both London-dispersion forces and hydrogen bonds. Hydrogen

My hypothesis was that the water will have the most amount of drops and the soapy water will have the least amount of drops.

This reaction is spontaneous for almost all esters but can be very slow under typical conditions of temperature and pressure. The reaction occurs at a much faster rate if there is a significant amount of base (OH-) in the solution. In this lab experiment, the rate of this reaction will be studied using an ester called para-nitrophenyl acetate (PNA), which produces an alcohol,

This was concluded by combining information on melting points and TLC; melting range narrowed when filtered product was mixed with the standard product. Also, the Rf value of the pure product is closely related to the Rf value of the standard. TLC of filtrate showed no movement of the substance in the mixture under 9:1 ratio declaring the substance to be extremely polar. Of the three potential unknown reactants, 4-methoxyphenol would be the most polar and therefore would travel least up the TLC plate. (Q14:Yield) 81.2% product yield was collected. “Matter cannot be created nor destroyed”, therefore some product could have filtered through. TLC of filtrate confirmed remnants of product present. Filtering the filtrate could have increased the yield. (Q15:Recovery) The percent recovery of the product makes sense because it is the mass of the crystallized product divided by the crude product: 94.9%. The percentage reflects the mass of pure product (without the presence of impurities). (Q16:MP) Melting point coincides with the unknown nucleophile being 4-methoxyphenol because when the standard product was combined with our pure product, the melting range narrowed. When compared to the melting ranges obtained when mixed with the other two possible products the melting ranges significantly decreased and widened. This is often an indication of impurities being present, but because this was a

- If you use 10 drops of Oregano Oil with two tablespoons of coconut oil, you can create a natural hand sanitizer!

The purpose of this experiment was to determine the molar solubility, the solubility constant, and the effect of a common ion on the molar solubility of calcium hydroxide. To accomplish this the experiment was split into two parts; part A and Part B. in Part A of the experiment a standardized 0.05 M solution of HCl was titrated into a 25 mL solution of saturated Ca(OH)2 which contained 2 drops of orange methyl identifier. Once the titration began, the HCl was added until the methyl orange endpoint was reached, and as a result the volume of the HCl needed for the endpoint to be reached could be used in

The reaction took place in a conical vial and .2mL of each of the reactant samples were added to it along with some 95% ethanol. Two drops of NaOH were added shortly after and stirred at room temperature for fifteen minutes. The vial was cooled in and ice bath and crystallized. Vacuum filtration was performed to filter the crude product. The crude product was recrystallized using methanol and filtered again. We made one change to the procedure and instead of using .7mL of ethanol we

organic compound to dissolve (increase in entropy), a decrease in heat will then allow that

Would you be up for having the largest methanol plant in the world next to your city? Most people wouldn’t. This would be a bigger con than pro for Tacoma. It would cause environmental issues, and can be dangerous. One reason this would be a bad idea is because it would cause a lot of pollution, and more than Tacoma already has. Another reason this would be bad idea is because if something goes wrong, it can cause a lot of problems and can potentially be dangerous. This is why a methanol plant in Tacoma, WA would be a bad idea.

Determining how a mechanism comes to be is crucial as a scientist and arriving to conclusions is a crucial component which lead to examining and determining which mechanism takes place when two or more substrates are made to react. At the end of the experiment a mechanism was determined based on the purified product’s melting point. This was accomplished by having the reaction take place but also through acquiring the melting point and comparing the number to the melting point which was already established by the scientific community. (Q1) When 0.252 g of trans-cinnamic acid was mixed in 2.5 mL glacial acetic acid and 0.434g pyridinium tribromide was added, the resulting product reflects an addition reaction. In general, reactions take place to achieve its lowest Gibb’s free energy because it’s at

In order to achieve isoborneol from camphor, a mixture of camphor with methanol and sodium borohydride was heated for about two minutes. Data Table 1 demonstrates the measurements that were taken to prepare the reaction mixture. The addition of sodium borohydride caused the reaction to fizzed.

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.

As shown in Table 3.0, it was difficult to stir and combine the shortening and the lard with the sodium hydroxide and glycerol. Though the oil-based soaps were easy to make, they did not yield as much compared to the fat-based soaps. Table 6.0 shows that Soap 3 which was shortening based and Soap 4 which was lard based produced 11.18 g and 11.22 g, respectively. This was a much greater yield than the oil based soaps. Soap 1 which used olive oil yielded 3.154 grams and soap 2 using vegetable oil yielded 1.319 grams. This was something to consider when choosing which starting material to use and depends on whether ease of synthesis or greater yield is more important. The detergent synthesis methods were very similar but method 2 took less steps and was a bit easier than method 1. Table 6.0 shows that detergent 2 had a greater yield, 5.143 grams whereas detergent 1 had a yield of about 4 grams. The lathering test showed that though soaps 3 and 4 produced the most product of the soaps, they did not create many bubbles or a good lather according to Table 7.0. The soaps/detergents that produced the most bubbles were soap 1 which used olive oil followed by detergent 1 and then soap 2

1. Obtain a sample of the mixture. The mixture you will separate contains three components: NaCl, NH4Cl, and SiO2. Their separation will be accomplished by heating the mixture to sub-lime the NH4Cl, extracting the NaCl with water, and drying the remaining SiO2.

The purpose of this lab was to create soaps and detergents and test their cleaning ability. We created four different soaps and two detergents using different starting materials composed of oils and fats for the soaps and lauryl alcohol and sulfuric acid for the detergents. Soaps are created by a process called saponification, which is the formation of a salt by combing an acid and a base.1 Soap and detergent are effective cleaning agents because they have hydrophilic and hydrophobic ends.1 The hydrophobic ends interact with the dirt and oil while the hydrophilic ends interact with the water molecules effectively washing the dirt and oil away.2 While soaps and detergents are very similar in their cleaning ability, they have a major difference being that soaps are made from natural products and detergents are made from synthetic materials.3 In order to make the soaps, we used four different starting materials including lard, shortening, olive oil, and vegetable oil.