Calculate the maximum amount of ethyl salicylate that could form from the amounts of starting material you used. Report the amount in mol and g units. That amount is called theoretical yield, use it to determine the percent yield you obtained. Observations and measurements Salicylic acid (g) Ethanol (mL) Weight flask and stir bar (g) Weight flask, stir bar and product (g) Ferric hydroxamate test color Observations or measurements 0.2354 4mL 26. 35959 26.89649 Purple €

Calculate the maximum amount of ethyl salicylate that could form from the amounts of starting material you used. Report the amount in mol and g units. That amount is called theoretical yield, use it to determine the percent yield you obtained. Observations and measurements Salicylic acid (g) Ethanol (mL) Weight flask and stir bar (g) Weight flask, stir bar and product (g) Ferric hydroxamate test color Observations or measurements 0.2354 4mL 26. 35959 26.89649 Purple €

EBK A SMALL SCALE APPROACH TO ORGANIC L

4th Edition

ISBN:9781305446021

Author:Lampman

Publisher:Lampman

Chapter80: Crystallization: Purification Of Solids

Section: Chapter Questions

Problem 4P

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CREATE A SCHEMATIC DIAGRAM USING THE PROCEDURE: Weighing of standard reagents 1. Make an improvised weighing dish for solid samples (i.e. aluminum foil). Put the foil inside the analytical balance. 2. Press TARE. 3. Weigh accurately 0.4000 grams of NaCl powder in the foil. The reading of the weight must not exceed + 0.0030 g. Note that unused or excess chemicals should never be returned to the stock bottle. 4. Close the balance glass door. Note the actual weight of the NaCl powder that is reflecting on the analytical balance. 5. Transfer carefully the contents in a 150-ml beaker.
On a paper, draw a schematic diagram on the Extraction of Saponins from Gugo by Lead Method using the procedures stated below. Procedures (Stas-Otto Method): Extraction of Saponins from the Gugo Bark by Lead Method Extract saponins from gugo by boiling about 10g of small pieces of gugo bark in water. (If necessary, extract first with ether or petroleum ether). Filter and add a neutral lead acetate solution to the aqueous solution; acid saponins, if present, are precipitated as lead salts. To the filtrate (including the washings, concentrated by evaporation), add basic lead acetate to precipitate neutral saponins. Wash the lead precipitate and suspend in water. Decompose by passing H2S Filter PbS and absorbed impurities. Concentrate the filtrate and finally allow to evaporate to dryness or in vacuum over H2SO4. Purify the saponins by CHCl3 and precipitate with ether. Weigh the residue and compute the percentage yield.
1. Which of the following may cause an increase in the calculated percent recovery of the recrystallized benzoic acid? a.Adding too much solvent in the receiving flask during hot filtrationb.Using cold water in rinsing the residue from the flask during hot filtration c.Using fluted filter paper during hot filtrationd.Not adding animal charcoal to the solution2. Which set of reagents can confirm that sulfate ions are present in two unkown solutions? a.1.0 M NaOH and excess NH3 b.0.1 M Ba(NO3)2 and 0.01 M KMnO4 c.1.0 M NaOH and 0.1 M K2Zn3[Fe(CN)6]2d.0.1 M Ba(NO3)2 and 1.0 M CH3COOH
If this is the procedure that we used to adapt a new reaction, what is the mass, molecular weiht, volume, mole equiv, moles of the all the reagents and products of the new reaction? Below is the procedure and attached is the new reaction 5-Amino-2-chlorophenol To a 250 mL Erlenmeyer flask containing a Teflon coated magnetic stirring bar was added 85% sodium hydrosulfite (14.0 g), water (80 mL), and 20% (mass/vol) sodium hydroxide solution (16 mL). The mixture was magnetically stirred until a clear solution was obtained, then solid 2-chloro-5-nitrophenol (2.75 g) is added in one portion. The mixture was stirred at room temperature for 20 minutes then heated to a gentle boil for about two minutes during which time the yellow color of the solution disappeared, indicating complete reduction of the nitro function. The reaction mixture was cooled to room temperature and then placed in an ice-water bath for about 10 minutes. The crude product was collected by vacuum filtration, washed with a…
MAKE A METHODOLOGY : MATERIALS/ REAGENTS WITH SCHEMATIC DIAGRAM . THE PICTURE UPLOADED SERVES AS A GUIDE, DO THE SAME THING BASED FROM THE PIC. Procedure: Place 20 drops of each of 0.2M CuSO4 in a centrifuge tube. Then add 5 drops of freshly prepared 6M (NH4)2S to each centrifuge tube. Record your observation. Centrifuge the mixtures for 3 mins. and decant the supernatant liquid. Add 10 drops of DI water and 10 drops of 6M HNO3. Stir and boil the mixture in a hot water bath for 5 mins. centrifuge the mixture for 3 mins. Decant the supernatant solution from procedure 3. Discard the To each of the supernatant liquid, add 6 drops of 6M H2SO4. Allow themixtures to cool and 5 drops of DI water. To the mixtures in procedure 4, add few drops of concentrated NH3 until the solution becomes basic. Confirm using a litmus paper. Record your observation. Add 1 drop of 5M NaOH and 1 drop of 0.1 M SnCl2 to the centrifuge tube containing Bi3+ ion , centrifuge and decant the supernatant liquid. To…
After reacting two liquid reactants with eachother and allowing them to reflux for 2 hours. There was very poor percentage yield of product. Why?
What is/are the limiting reagent(s) for this three-step procedure? Why is sodium borohydride not the limiting reagent even though a smaller number of moles of this reagent are used? Mass/volume used in experiment: O-vanillin = 0.760g P-toluidine = 0.535g Ethanol = 15 ml Sodium borohydride = 0.1 g Glacial acetic acid = 2 ml Acetic anhydride = 2 ml
Please provide explanation1. Which of the following techniques help prevent premature recrystallization? a.Immediate cooling of the hot filtration to room temperatureb.Collecting the hot filtrate in a receiving flask with hot solventc.Filtering the filtrate through a long and narrow funnel d.Using a conventional conical filter paper for hot filtration2. Which of the following may cause an increase in the calculated percent recovery of the recrystallized benzoic acid? a.Adding too much solvent in the receiving flask during hot filtrationb.Using cold water in rinsing the residue from the flask during hot filtration c.Using fluted filter paper during hot filtrationd.Not adding animal charcoal to the solution3. Which set of reagents can confirm that sulfate ions are present in two unkown solutions? a.1.0 M NaOH and excess NH3 b.0.1 M Ba(NO3)2 and 0.01 M KMnO4 c.1.0 M NaOH and 0.1 M K2Zn3[Fe(CN)6]2d.0.1 M Ba(NO3)2 and 1.0 M CH3COOH
What could have gone wrong in the separation and purification process to result in the disparity from the observed and expected yields? Select all that apply A) Both the benzoic acid and sand may have been wet before the student recorded the masses, hence the increase in expected masses. B) The student may have filtered the benzoic acid while cold. Hence the sand could have been contaminated with benzoic acid and resulted in a higher mass for sand. C) The sand may have dissolved in the hot water along with the benzoic acid, hence, the recorded mass for benzoic acid was more. D)The benzoic acid may have been cooled down too quickly on ice thereby allowing other soluble impurities to crystallize with benzoic acid causing the increase in the expected mass
Which of the following could result in a loss in yield in a mixed solvent recrystallization? i. Use of fluted filter paper in hot filtration ii. No heated solvent in the receiving flask iii.Rapid cooling iv. Both ii and iii
1.063 g of p-acetamidophenol was measured out into a 50 mL round bottom flask along with 8 mL of 1M NaOH in ethanol and a stir bar. This mixture was heated at reflux for 15 min. It was allowed to cool and then 0.80 mL of bromoethane was added to the reaction. The mixture was then heated at reflux for another 15 min. After heating, the solution was poured onto a mixture of ice and water and further cooled on ice and then the solid was collected by vacuum filtration. This solid was then recrystallized from ethanol and water. The final mass of the purified phenacetin was 0.42250 g and it had a melting point of 127 - 130 C. The TLC plate shows (from left to right) pure p-acetamidophenol, the reaction mixture before pouring it on ice/water, phenacetin after recrystallization. The solvent used was a mixture of 80% ethyl acetate and 20% heptane with 0.5% acetic acid added. QUESTION: Using the given TLC plate can you describe the results and what does the TCL plate tell about the purity?
While performing the formula of hydrate laboratory experiment, the lid accidently slips over the crucible to completely seal the crucible. Whould your calculated percentage water of hydration be high low or unaffected? explain your answer