4 Chlorophenol Synthesis Lab Report

Atoms are the basic units of matter and all life is based on them. Life on earth is based on the element carbon. It is a highly versatile atom able to form four covalent bonds with itself or other atoms such as hydrogen and water. Atoms combine to form molecules and those that are carbon based are referred to as organic molecules. Organic molecules occur in four different types in living cells; carbohydrates, lipids, proteins and nucleic acids. They are also known as hydrocarbons due to the presence of both hydrogen and carbon. Carbohydrates are made up of carbon, hydrogen and oxygen in the ratio 1:2:1. They are important sources of energy and are classified in three main groups; monosaccharides, disaccharides and polysaccharides.

A chemical reaction is when substances (reactants) change into other substances (products). The five general types of chemical reactions are synthesis (also known as direct combination), decomposition, single replacement (also known as single displacement), double replacement (also known as double displacement), and combustion. In this lab, the five general types of chemical reactions were conducted and observations were taken before, during, and after the reaction. Then the reactants and observations were used to determine the products to form a balanced chemical equation. The purpose of this lab was to learn and answer the question: How can observations be used to determine the identity of substances produced in a chemical reaction?

We used TLC analysis to identify each product obtained from the dihydroxylation reactions by spotting a TLC plate with the product of our reaction, a solution of cis-cyclohexane, trans-cyclohexane, and a 50:50 mixture of the two. We then placed the plate in a beaker with ethyl acetate saturating the atmosphere to allow the TLC plate to develop. Finally, we compared Rf values of the components of the mobile phase, after the phase was completed. 100% ethyl acetate was used instead of 100% Hexane or a mixture of Ethyl Acetate, because ethyl acetate has high polarity and can separate the components of a mixture to elution, unlike hexane, which is non-polar, and therefore unable to separate the components of the mixture. A 50:50 mixture of both would not work, because the polar and non-polar compounds would neutralize the mixture, and thereby not separate the components of the mixture.

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.

The wet, crude product was placed into the 50 mL Erlenmeyer flask. Small amounts of CaCl2 were added to dry the solution. The flask was sealed and the mixture was swirled and left to settle. Once

The reduction of nitro compounds consists of a two step reaction in which m-nitroacetophenone was reduced to 3-aminoacetophenone using tin and the acid, hydrochloric acid, and 3-aminoacetophenone was reduced to 3-(1-hydroxyethylaniline) using sodium borohydride and ethanol as a solvent. The former reduction was performed with granular tin and concentrated hydrochloric acid, stopped with the addition of sodium hydroxide, and the product separated using gravity filtration. The latter reduction was performed with granular sodium borohydride and ethanol, stopped with the addition of hydrochloric acid and water, and separated using ether as a solvent in a separatory funnel. Both products were evaluated using NMR spectroscopy, IR spectroscopy, thin-layer

The purpose of this lab report is to synthesize luminol and then test its chemiluminescent properties. 5-nitro-2,3-dihydrophtalazine-1,4-dione was reduced using sodium hydrosulfite in a solution of 3 M sodium hydroxide in water to form luminol. The product was then used to chemically generate light by reacting luminol with 3 M sodium hydroxide, hydrogen peroxide, and potassium ferricyanide. The reaction created a bright, blue light emission. From glow sticks to revealing remnants of blood samples in crime scene investigations, luminol, C8H7N3O2, has a wide variety of real world applications.

to compare the results, and neither solution was expected to produce an observable chemical reaction. The procedure was the same as used for the test with 6M HNO3 and 0.1M AgNO3 solution and the test with 6M HCl and 0.1M BaCl2 solution. A third experiment used was the flame test. First, a scoopula was used to place 0.1 grams of the unknown compound in a test tube, and a wash bottle was used to add approximately 2 mL of deionized water to create a solution.

Purpose: The purpose of this experiment was to observe the many physical and chemical properties of copper as it undergoes a series of chemical reactions. Throughout this process, one would also need to acknowledge that even though the law of conservation of matter/mass suggests that one should expect to recover the same amount of copper as one started with, inevitable sources of error alter the results and produce different outcomes. The possible sources of error that led to a gain or loss in copper are demonstrated in the calculation of percent yield (percent yield= (actual yield/theoretical yield) x 100.

Dispense .5 mL water into the already weighed conical vial, replace cap and face insert on its down side.

The hypothesis, “If the mass of solid CaCl2 and NH4Cl increases, then the qsolution (J) and ΔHsolution (kJ/mol) will increase proportionally.” is partially rejected. For CaCl2, the q solution does increase, but the ΔH is constant, not proportional. In the NH4Cl, the q solution decreases proportionally, while the ΔH is constant. In the calcium chloride reaction, the data is precise because the R squared value is .894 when the outlier is included which is relatively high considering the outlier. The ΔH data is relatively precise as well. The standard deviation of the ΔH without the outlier is only 3.38, but with the outlier the standard deviation rockets up to 15.9. Although the the data is precise, the accuracy is somewhat subpar. The percent error for ΔH is a strong 29.8%, which is far too high to be considered accurate.

Zhang et al23 (2013) reported the removal of tetrabromobisphenol A (TBBPA) from aqueous solution by GO. The effects of contact time, pH, and temperature, and the presence of coexisting anions as well as humic acid, were studied through batch experiments. The adsorption capacity decreased with an increase in temperature as well as solution pH. The presence of coexisting anions such as NO-3 SO4 -2 −, HPO4 -2 and HCO 3 2- reduced TBBPA adsorption in the order NO3 - < SO4 2- < HPO4 2- < HCO3 2-The presence of humic acid also significantly reduced the adsorption of TBBPA onto GO. The adsorption reaction followed the pseudo-second-order kinetics, while the adsorption isotherm was well described by the Langmuir model with a maximum adsorption capacity of 115.77 mg g−1 at 298 K. Thermodynamic studies indicated that the adsorption of TBBPA onto GO was feasible and spontaneous at all temperatures and was exothermic in nature. Both π–π stacking interactions and hydrogen bonding were proposed to be responsible for the adsorption of TBBPA by GO.

As a conclusion, we were not able to recover a final product due to misreading the experimental procedure. To avoid this problem in the future, I am planning on double checking my work and being completely positive before disposing of any solution or substance. However, if we would have successfully synthesized resacetophenone, we would have analyzed the identity of the compound by obtaining a melting point range. Then we would have calculated percent yield to see how much product was recovered in comparison to the beginning amount of chemicals present.

Solvent extraction is dependent on the two liquids having different polarities so that they do not mix with each other (Example Crude oil and water). When these two liquids are mixed together they form separate layers, these two liquids would therefore be described as immiscible.

In this lab, solutions are mixed with an indicator (red cabbage juice), which can be able to identify whether it is an acid, base or neutral.