(1) The three (3) component mixture of fluorenone, ferrocene, and 2-acetyloxybenzoic acid (aka aspirin) shown below was loaded on the column and eluted with 95:5 petroleum ether: diethyl ether. Using the Molecular View of the column provided: (a) draw one (1) molecule of each analyte in the correct relative position in the column, and (b) clearly show the relevant intermolecular forces that explain the column elution order. You do not need to include solvent molecules. (8 points) buret wall AI top of column H Al- AI- H H IIIII -0-H -Ö-H bottom of column -‒‒‒‒‒‒‒. buret wall OH
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- A spot of crude plant extract was placed on a glass plate coated with C18 silica gel. The chromatogram was developed using an appropriate solvent. The result is shown below. Which of the following spot is the most soluble in water?Volume of an unknown used was 30 mL, Initial Buret volume was 0 and the Final Buret volume was 8.5 mL. What is the molarity of the unknown solution if the Net volume of NaOH being used was 8.5 mL and Millimoles (mmoles) NaOH reacted was 0.791? Then, what is the Mass (g) of Acetic Acid in unknown sample and thr average percent (%) Acetic Acid? (assume density = 1g/mL)I would need help with these questions. The method referenced above was followed by a student and she got the following results: Caffeine Std. Conc. (ppm) Absorbance 100 1.806 50 0.899 40 0.724 30 0.545 20 0.365 10 0.183 Further, she analyzed an unknown sample and she got the following results: Sample # Absorbance 1 0.398 1. Graphically find the concentration in ppm and then calculate in mol/L of Caffeine in Sample #1? 2. Which solvent was used to extract Caffeine and why? Why is it necessary to do extraction three times? 3. Cuvettes used in this experiment were made from which material and why? 4. At what wavelength the Absorbance was measured?
- A 18 g of unknown organic sample was dissolve in 756 mL of benzene. The boiling point of benzene was increased by 3.36oC. As the first step of analysis, determine the moecular weight of the unknow sample? Kb of benzene= 2.64oC/m Bb of benzene = 80.09 oC density of benzene = 0.874 g/mL at 25 °C Answer in whole number, no units required.Chromatography question A student properly sets up a column chromatography experiment. Although the mixture is soluble i the mobile phase, the sample appears "stuck" at the top of the column and will not elute eregardless of how much solvet is pplaied. what could bee the cause of this issue and what could teh student try to achieve a successful separation?Using dimensional analysis, find the mass of acetylalicylic acid in one tablet of aspirin. The grams of aspirin used in a titration is .325g before being dissolved in 10mL of water and then added to a base, NaOH, with a molarity of .01M and a volume of 10.1 mL. In Chem2.png, the actual question is boxed in red Video used for titration assignment (Not needed for question): https://www.youtube.com/watch?v=x9jgjdizTaY
- Calculate the mass percent of the ascorbic acid in the same show full solution Situation: The pounded Vitamin C tablet was half into two below are the calculated data in the experiment. Each of the half are transfered in a 250ml erlen meyer flask and added 75ml of deionized water for the vitamin C to dissolve. Then it was prepared for titration where the burette was filled with 0.09794M standardize NaOH solution then a total of with 3 drops 2% phenolphthalein indicator was added to each erlen meyer flask l, swrill it and begin the titration. below are the following data gathered: Vitamins used: Nature Made vitamin C 500mg tablet Trial 1 Mass: 0.3108g of Vitamin C tablet Initial volume: 1.6mL Final volume: 15.4mL Trial 2 Mass: 0.3349g Initial volume: 15.4 mL Final volume: 30.2 mLDensity of solution:Trial 1: 1.2 g/mLTrial 2: 1.2 g/mLTrial 3: 1.2 g/mL Average density = 1.2 g/mL What is the relative average deviaion, %?You run the chromatography system with paper as the stationary phase and 70% isopropanol as the mobile phase. You determine the Rf of a polar analyte to be 0.40. If you use 100% isopropanol (a less polar solvent) instead of isopropanol as the mobile phase what would you expect to happen to the Rf value? No value effect on Rf higher lower could be higher or lower
- How would the following errors change the calculated value of the percent oxalic acid in the radiator cleaner, that is would the calculated value of the percentage be high, low, or unchanged? Give a brief explanation of your reasoning. a. The experimenter consistently overshot the endpoint (i.e. added too much NaOH solution), of the titrations used to standardize the sodium hydroxide solution. b. The KHP used to standardize the NaOH was not pure, but contained approximately 10% by mass of the inert ionic compound potassium chloride, KCl. 3) Oxalic acid exists in the solid state as the monohydrate, H2C2O4•H2O. What would you use to calculate the percent oxalic acid monohydrate in the cleaner?A spot of crude plant extract was placed on a glass plate coated with C18 silica gel. The chromatogram was developed using an appropriate solvent. The result is shown below. Which of the following spot is the most soluble in water? Choices: Spot C Spot M Spot E Spot HLouie performed paper chromatography to identify which among the four availablereference mixtures — WAR, OFF, YIN, MEW — have the same components as hisunknown sample, GUN. He spotted the standards and the sample in a Whatman No. 1filter paper, which he placed in a developing chamber containing 3% KCl. After 20minutes, Louie obtained the chromatogram below, immediately noting that the distancetravelled by the solvent from the origin is 79.0 mm. On the other hand, the distances (incm) traveled by the developed spots were tabulated as follows.(see attached) Questions: 1. Is the type of paper chromatography performed normal or reversed? Why?2. Calculate the Rf of the spots from the samples. Report your answers in four decimal places.