After filtering your final product, you find that your product is still wet, but you proceed to take a melting point anyways. The literature melting point of luminol is 319 °C. What do you expect the melting point of your luminol to be? What would you expect the yield to be? Would it be an accurate yield?
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After filtering your final product, you find that your product is still wet, but you proceed to take a melting point anyways. The literature melting point of luminol is 319 °C. What do you expect the melting point of your luminol to be? What would you expect the yield to be? Would it be an accurate yield?
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- Each of the student statements below is wrong. Explain why they are not correct. (a) All my compound dissolved right away in the small amount of solvent I added at room temperature, and I didn’t need to heat it at all. This means I’m going to get lots of pure compound out. (b) I did a recrystallization of naphthalene and my percent recovery was very high (99%), so I must have pure product. (c) When you’ve dissolved all your compound in hot solvent, and you’re in a hurry, it’s ok to just place it straight into the ice bath.1.Each of the student statements below is wrong. You will need to explain why they are not correct. (a) All my compound dissolved right away in the small amount of solvent I added at room temperature, and I didn’t need to heat it at all. This means I’m going to get lots of pure compound out. (b) I did a recrystallization of naphthalene and my percent recovery was very high (99%), so I must have pure product. (c) When you’ve dissolved all your compound in hot solvent, and you’re in a hurry, it’s ok to just place it straight into the ice bath.If 80% of a desired compound is extracted into the organic phase in each step (leaving 20% in the aqueous layer), how many extractions are necessary to ensure that at least 99% of the compound has been recovered in the organic phase? 1 extraction 2 extractions 3 extractions 4 extractions
- Which of the following should be done if there is no recrystallization due to the unsaturation of the solution? (mixed solvent recrystallization) a. Crystal seeding b. Scratching the inner walls or bottom of container c. Further boiling of solvent d. Adding small amount of sampleA student rushed through this experiment. Describe the effect that the following procedural changes would have on the percent recovery of acetanilide. Briefly explain the basis of each answer.(a) Rather than adding 0.5-mL portions of boiling solvent to the acetanilide, the student added 5-mL portions of boiling solvent.(b) The student did not pre-heat the gravity filtration apparatus.(c) The student forgot to cool 5 mL of solvent in Part 5 and washed the crystals with room-temperature solvent.please answer the question based on the information below Why is toluene used as the solvent for the recrystallization here? Day 2: Recrystallization and analysis of the o-chlorobenzoic acid Recrystallize the product using hot toluene. Be sure to add enough toluene so that the solid dissolves at a higher temperature, but some of the solid stays undissolved at room temperature. Do not add too much toluene, as you may not be able to crystallize your product. If you believe you added too much toluene, or if o-chlorobenzoic acid crystals do not appear upon cooling the solution on ice, you will need to evaporate some of the toluene in the hood. The crystals should be suspended fully in toluene before filtration. After drying the solids, determine the melting point of the product. Acquire the infrared spectrum and the 1H-NMR spectrum in DMSO-d6. Cleanup Notes: Solid MnO2 often sticks to the glassware and is difficult to remove, even with soapy water and scrubbing. You can easily clean…
- PREPARATION OF n-PROPYL PROPANOATE Q1) How can you tell, by looking at the refluxing set-up, that the reaction between n-propanol and propionic acid is over? Q2) When assembling the distillation set-up, why is it important to place the tip of the thermometer at the same height as the exit to the side arm of the round-bottom flask?Please create a flow chart for this experiment. ( the images are steps 1 through five, the steps 6-9 are in the description below.) Steps 6-9: —> Cautiously add concentrated hydrochloric acid dropwise to Flask 1 until the contents are acidic to litmus and then cool the flask in ice. 7) Decant the ether from Flask 3 into a tared flask, taking care to leave all of the drying agent behind. Wash the drying agent with additional ether to ensure complete transfer of the product. If decantation is difficult then remove the drying agent by gravity filtration. Put a boiling stick in the flask, and evaporate the ether in the hood. 8) Isolate the compound in Flask 2 by vacuum filtration on a Hirsch funnel, and wash it on the filter with a small quantity of ice water. 9) Isolate, weight the product in Flask 1 by suction filtration.Q2. What does “crude” product mean? Q3. What is the advantage of using Buchner filtration in filtering crystals? Q4. Briefly explain how scratching the wall of the glass flask can help formation of crystals. Q5. Briefly explain why crystals form as the solvent cools during recrystallization.
- If you do not heat your crucible strongly enough to remove all volatile impurities when you heat the crucible empty, what will be the result if those impurities are completely volatilized when heating your sample?Based on the readings and lecture on emulsions, and the procedures for this lab answer the following question. What is the dispersed phase in the simple vinaigrette? Air Oil Water Egga student performed a recrystallization on 515 mg of impure compound using ethanol. After isolating the crystals, he obtained only 215 mg of pure product. Knowing that his sample was only slightly impure, he concluded that a significant amount of product was lost. Explain what likely happened and what he can do to recover his product.