In an EAS Reaction the compounds 5.0g of acetanilide, 0.2g potassium bromate, 5ml acetic acid, 0.9 ml hydrobromic acid solution, and 5 ml saturated sodium bisulfite solution are used. Given these compound and obtaining a yield for the experiment at 6.3 grams which yields 5.3 grams after recrystallization and drying, Please find the theoretical yield and the percent yield?

In an EAS Reaction the compounds 5.0g of acetanilide, 0.2g potassium bromate, 5ml acetic acid, 0.9 ml hydrobromic acid solution, and 5 ml saturated sodium bisulfite solution are used. Given these compound and obtaining a yield for the experiment at 6.3 grams which yields 5.3 grams after recrystallization and drying, Please find the theoretical yield and the percent yield?

Macroscale and Microscale Organic Experiments

7th Edition

ISBN:9781305577190

Author:Kenneth L. Williamson, Katherine M. Masters

Publisher:Kenneth L. Williamson, Katherine M. Masters

Chapter8: Thin-layer Chromatography: Analyzing Analgesics And Isolating Lycopene From Tomato Paste

Section: Chapter Questions

Problem 10Q: A TLC plate showed two spots with Rf values of 0.25 and 0.26. The plate was removed from the...

See similar textbooks

Similar questions

The experiment wAs preformed using a recrystallization of salicylic acid. The IR was preformed using a KBR pellet method Re-state the diagnostic peaks from the results, this time with the intention of comparing the experimental to literature diagnostic values as well as fingerprint regions to provide evidence to answer your hypothesis. After comparing your values, you must discuss what conclusions you obtained (i.e. was there evidence to support that your compound is pure?)
Write the equations for the acid-base reactions involved in this experiment. Clearly show the reactants and products for each chemical equation. Experiment: seperation of caffeine and benzoic acid by acid-base extraction Things used in lab: -solid mixture of caffeine and benzoic acid -40mL of dichloromethane -20mL of 1.0 M NaOH -magnesium sulfate as drying agent for caffeine isolation -3.00 M HCl for recovery of benzoic acid
Suppose we start with 3.0g of contaminated benzoic acid. After recrystallisation we end up with 2.3g of pure benzoic acid. What is the percentage recovery of the experiment?
Read the detailed procedure of an experiment in your screen. Evaluate each step in the procedure whether it belongs to HOMOGENIZATION, EXTRACTION, PURIFICATION/CONCENTRATION, DATA TREATMENT, or INSTRUMENTAL ANALYSIS step.
A student doing this experiment had some problems with the procedure, as described below. Explain what effect each problem would have had on the magnitude of the results calculated. b) The student neglected to open the pinch clamp on the plastic tubing between the filter flask and the beaker when the Mg came in contact with the HCl solution. After the stopper popped out of the Erlenmeyer flask, the student quickly replaced the stopper, opened the clamp, and proceeded with the experiment. c) The student began titrating the unreacted HCl with standard NaOH solution and realized that there was a large air bubble in the buret tip. The bubble came out as the first few milliliters of titrant were added. d) The student forgot to add indicator to the titration mixture until 12.50 mL of titrant had been added. When the indicator was finally added, the solution was colorless.
Please type all of the parts to this question occordingly to the instructions. Here is an example of a formal procedure based off of the experiment presented in Mohrig:Sodium hydroxide (4.6 g) was dissolved in water (25 mL). This solution was added to a 100 mL round bottom flask along with methyl salicylate (2.0 mL) and a stir bar. The mixture was heated at reflux for 15 min and then progressively cooled to 5 °C. The solution was acidified with 3M sulfuric acid (15-20 mL), and the resulting solid was collected by vacuum filtration. The crude salicylic acid was recrystallized from water to yield ???? g of final solid. The melting point and IR were taken to assess purity. Calculate the molarity of the solution of sodium hydroxide that is used.a. M = b. If the original procedure is the base scale (100%), how far are we scaling down the reaction when using 0.75 mL of methyl salicylate? (Example: the original uses 2.0 mL, if we were to use 1.0 mL, we would be scaling the reaction down…
What is the effect of weighing a recrystallized organic solid which is not completely dried to the percentage yield? Elaborate.
Of Aspirin, ethanol, acetaminophen, ethyl acetate, hexane, and water which could go undetected during HPLC analysis, but could result in a lower than expected melting point, why are they not detected by HPLC analysis?
A TLC plate showed two spots with Rf values of 0.25 and 0.26. The plate was removed from the developing chamber, the residual solvent was allowed to evaporate from the plate, and then the plate was returned to the developing chamber. What would you expect to see after the second development was complete?
Despite their structural differences, separation of mixtures of organic compounds (such as the arenes benzoic acid, 4-t-butylphenol, and benzamide) often proves difficult. Silica gel chromatography, however, can be used with some success provided that an appropriate solvent is used to provide optimal separation. Consider, for example, the TLC plate pictured at right after developing and UV visualization where prior to elution, lanes A and B were spotted with 4-t-butylphenol and lanes B and C spotted with benzamide. Which of the following must be true? In the space provided, indicate the CORRECT answers (as 1, 2, and/or 3) then explain your reasoning for all three statements. Benzamide elutes faster than t-butylphenol. The Rf for t-butylphenol is less than that of benzamide. Benzamide is more polar than 4-t-butylphenol
Which of the following could DECREASE the amount of the recovered crystals in the purification by recrystallization experiment? Collecting the recrystallized benzoic acid by filtration using a pre-weighed filter paper. Using a long-stemmed funnel in the hot filtration step. Cooling the filtered solution rapidly. Washing the recovered crystals using hot solvent. a. II, III b. II, IV c. II, III, IV d. I, II, III, IV
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