Which Solvent Or Solvent Mixture Did You Decide To Use For Your TLC? Why?

In this investigation, a TLC plate and ethyl acetate (solvent) were used to measure the Rf values of four different solutions of Tylenol, Anacin, Acetaminophen, and Acetylsalicylic acid. The value of Rf depends on the strength of the intermolecular forces that exists in molecules. The stronger the intermolecular forces are, the harder the solvent moves the molecule up, resulting a small Rf value. In contrast, molecules with weak intermolecular forces tend to have a high Rf value.

The unknown sample was identified to contain Acetaminophen, Aspirin, and caffeine based on comparison of known Rf values (Table 1). When comparing the traveled UV lit spots (figure 1), Aspirin and Ibuprofen traveled the same distance from the start line. Unknown sample 16 contains Aspirin not Ibuprofen, due to the intensity of the spot under UV light. Aspirin and the unknown shared that same intensity, whereas Ibuprofen did not share that same strength of brightness. The distance traveled by the samples was dependent upon their affinity for the mobile phase 200:1 ethyl acetate – acetic acid. The samples that traveled the furthest like the Aspirin and Ibuprofen were the most soluble in the mobile phase. The samples that traveled the shortest

The purpose of this lab is to separate a mixture and determine the percentages of each of the ingredients. Each substance will have a different boiling point due to its intrinsic properties and from that, we will be able to determine the purity of different products as we evaporate off the next level of product.

The purpose of this experiment was to synthesize t-pentyl chloride from the reaction of t-pentyl alcohol and concentrated HCl. This reaction occurred through an SN1 reaction, a unimolecular nucleophilic substitution reaction. This was a First Order Rate Reaction where the rate of t-pentyl chloride was dependent only on the concentration of t-pentyl alcohol. After the reaction was completed, the products were achieved via 3 liquid-liquid extractions and then after by simple distillation. In the liquid- liquid extractions a solute was transferred from one solvent to another. Then in the simple distillation the miscible liquids or the solution, was separated by differences in boiling points. After this the product was determined through infrared spectroscopy.

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 first TLC plate showed that the fractions collected during the experiment that appeared to be the purest were fractions 4 and 6. These two fractions and fractions number 5 were combined for the final product. The Rf values for the standard carvone, fraction 4, and fraction 6 were all 0.32 indicating that these compounds were

1. The 1% saltwater solution was easy to create, however there was a greater amount of this solution than the alcohol. The saltwater solution worked better and had more effect on each of the colors on the strip of paper than the alcohol solution because the colors began

The goal of the experiment was to identify Unknown 33A and 33B. Unknown 33A was a white, crystalline solid that had a sweet cherry smell and Unknown 33B was a beige, yellowish color liquid that was translucent and had a viscosity similar to water. Also, the liquid was homogenous and smelled sour, similar to mildew.

First thing we did in this lab was to add HCl to the t-pentyl alcohol. We did this because by adding the HCl, we are creating what we wanted, t-pentyl chloride. Then, due to the difference in density, layers will form. The top layer and less dense is the organic layer, the t-pentyl chloride and the bottom layer is the aqueous layer. The purpose of shaking vigourously is to make sure that the 2 liquids mix properly, giving us the desired product t-pentyl chloride.

The Materials that were used to measure the experiment where a pen and paper to record the reactions of the subjects being tested, and the subjects themselves.

1. What medium were you told to use in the explanation of the task at the end of your case?

In 1863, Professor Paul-Jean Coulier, published his observations that latent prints can be developed on paper by iodine fuming and how to preserve the impressions. However, with the discovery of latent print process in 1863, the first official use of latent prints wasn’t until 1933 with the Hamm Kidnapping case. To solve the Hamm Kidnapping case, a Silver Nitrate Method was used. In the Hamm Kidnapping case, the use of the Silver Nitrate Method was the first time this method was successful in obtaining latent prints. Since

The “E” solution ended up having the most spots because it was the pigment fragments. The Rf values could be calculated for all of the spots by taking the distance traveled by the spot and dividing it by the total distance traveled by the solvent front. The calculations are as shown:

There are many advance techniques that are used to detect a fraudulent document and among the best are inks of different types, both covert and overt in nature. Covert inks are known to a few people within a specific organization, and overt inks are

4. Spot the solution on a TLC plate and check with UV light to see