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please explain the results from these thin layer chromatograms......we did an experiment with 6 different compounds in 100% ethylacetate, 100% hexane and another compound

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In order from left to right. acetaminophen, aspirin, caffeine, ibuprofen, Excedrin, and Tylenol. what does the results suggest.

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Related questions

These questions are from an experiment where we had a mixture of Ferrocene, acetylferrocene and diacetyl ferrocene and we separated each by using column chromatography. Before doing the column chromatography we did TLC analysis to ensure that we did, in fact, have a mixture of these 3 compounds.

During the column chromatography we first eluted the ferrocene using pure hexane. Then we eluted the acetylferrocene using a 1:1 mixture of hexane and methylene chloride. Then we eluted the diacetylferrocene using a 9:1 mixture of hexane and methylene chloride.

1. Rank ferrocene, acetylferrocene, and diacetylferrocene in order of increasing polarity. Do the TLC results from your fractions support this ranking? Explain.

2. Rank the solvents used in the experiment in order of increasing polarity.

3. Why do you start with the least polar solvent/solvent mixture and progress to increasing polar solvent/solvent mixtures when eluting the ferrocene compounds from the column rather than starting with more polar solvent system and progressing to less polar solvents?

4. How do the thin layer and column chromatography for this experiment compare in regard to stationary and mobile phases?

5. What key feature in the IR spectrum of acetylferrocene distinguishes it from the spectrum of ferrocene?

If you were to run the experiment without using any celite 545, what would happen to the purity of your sample and why? Be specific.

Why is Celite 545 labeled as 545? What makes it special?

If you were to use THF, or tetrahydrofuran instead of dicholormethane for this experiment, could you still successfully extract your caffeine? Why or why not? (Consider what is necessary for an extraction to work) Why is dichloromethane different from THF

Only answer what is above. The experiment is written below.

Introduction Caffeine is one of three legal, mind-altering drugs available in the U.S without a prescription. Two common sources of this drug are tea and coffee, both of which are prepared via extraction of the solid foodstuff with liquid water. In this lab you will extract caffeine from food samples with liquid solvents and quantify the amount obtained. Laborator Hypothesis: We can rank various tea and coffee samples by caffeine content by performing a solid-liquid extraction from the foodstuff, followed by analysis via thin-layer chromatography. Experiment: In a 50 mL Erlenmeyer flask were placed 2.0 g of black tea. Dichloromethane (15 mL) and 0.2 M NaOH (5 mL) were added successively, and the stoppered flask was swirled gently by hand for 10 minutes (note: avoid vigorous shaking, as it will cause an emulsion to form). The dicloromethane layer was separated from the leaves and the aqueous layer by vacuum filtration through 7 g Celite 545, and the leaves were washed with a further 15 mL dichloromethane. The combined dichloromethane solution was placed in a 50 mL round bottom flask and concentrated to a minimal volume (ca. 1 mL) via simple distillation. The remaining dichloromethane solutions was transferred to a watch glass via pipet, and the solvent was evaporated in a fume hood. The sample was evaluated by TLC (a mixture of methanol and ethyl acetate as the mobile phase, co-spotted with authentic caffeine). Data: What was your crude yield of caffeine? What was the mass percentage of caffeine in your food source'? Given that the materials we are interested in are UV active, compared to the TLC standard how would you characterize the purity of your caffeine extracts? Conclusions: Can you comment on the purity of your caffeine sample? For all samples your class worked with where does your foodstuff rank in terms of caffeine content? How much caffeine is reported for the typical serving of coffee or tea? How did your extraction and isolation compare with the typical serving?

Hi Iâve been struggling with my lab report and in need of some help. Here is everything you might need the lab report and data recorded in my notebook. I need help in the report questions please

QUALITATIVE STUDIES OF OXIDATION-REDUCTION REACTIONS Your objectives in this experiment include determining the products means of experimental tests, experimentally determining the relative ability of chlorine, and iodine to act as oxidizing agents, and designing an experiment to test an of a chemical reaction by bromine d rank a group of in order of their strength as reducing agents. All these objectives will require you to think logically in both your approach and your analysis of the results. Pre-Lab Questions: 1. In this lab you will be mixing hexane with aqueous (water) solutions. Which layer will be the water layer - top or bottom? Explain what property allows you to determine this. 2. Write a balanced chemical equation for the reaction of calcium metal with hydrochloric acid. What visible changes do you expect to see? Safety and Disposal: 1. Hexane is a volatile and flammable solvent. No open flames during this laboratory. When corked test tubes are shaken, pressure may develop, especially when a volatile solvent is one of the components. Remember to release the pressure intermittently by removing the cork slowly 2. Hydrochloric acid is corrosive. Wash your hands well with soap and water after working with it. 3. All solutions containing hexane must be placed in a container for recovery. Do not discard hexane down the sink. Do not put metals in the hexane recovery container. Part 1: The halogens Non-metals, such as the halogens, have relatively high electron affinities and as a result tend to react by gaining electrons, which we call becoming reduced, to form anions. In this experiment we will use the difference in solubility of the halogens (Cl2, Br2, and 12) as compared to the halides (Cr'. Br, and I') to test the reactivity of the elements The elemental halogens are non-polar and therefore are not very soluble in water. As a resul solutions of the halogen s in water are not very brightly colored. However, if an aqueous solution is mixed with a non-polar solvent, such as hexane, C&H14, the halogen is usually ferentially extracted into the non-polar solvent. Since the non-polar solvent is water, the halogen color is easily visible as a not miscible with separate colored layer

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