Just need answers 1-10. As you can see I attempted them but want to make sure on everything. I believe the odor was odorless but I'm not sure? If aspirin was created would we expect vinegar smell due to acetic acid?

4. Collect the crystals using vacuum filtration. Turn the vacuum off temporarily, pour just enough COLD water to thoroughly wet the crystals, and then turn the vacuum on. Let the vacuum draw air through the crystals for 2 minutes, making certain that the seal with the rubber ring is a good one. Place a small stals on a clean watch glass and spread them thinly to facilitate drying. Using a marker rme on the watch glass and heat the crystals for 15 minutes in an oven set at a temperature of70-80 â Determine the melting point of both your dried aspirin product and pure salicylic acid. Refer to Appendix 4 for instructions on how to take a melting point. *Pure aspirin melts at 135â and pure salicylic acid melts at 156-158 â DATA SHEET/ Questions I. Record the experimental melting ranges for your recrystallized aspirin and the starting material, salicylic acid Recrystallized aspirin Salicylic acid 2. A small melting range usually indicates that: a) The compound generally has a high melting point. 6) The compound has few impurities. c) The compound is highly impure d) The compound is likely to be soluble in water e) The compound is likely to be very unreactive. f) The compound will be difficult to recrystallize. 3. Describe the appearance of your final, recrystallized product. 4. Does the aspirin have a very strong odor, suggesting that it is a very volatile substance? 5. If all of the 2.0 g of the salicylic acid that you started with was converted to aspirin and 100% of the aspirin was recovered, the expected yield of aspirin would be 2.6 g. The isolated yield is always less than this because: (choose all that are appropriate.) Water is trapped inside the crystals. A substantial amount of the aspirin evaporates. Some aspirin remains dissolved in the solvent from the first filtration. Some aspirin remains dissolved in the solvent from the recrystallization. e) The reaction used to create the aspirin does not go to completion. 1 The acetic acid formed in the reaction adversely affects the yield of aspirin. Chem 162-Aspirin tab

Just need answers 1-10. As you can see I attempted them but want to make sure on everything. I believe the odor was odorless but I'm not sure? If aspirin was created would we expect vinegar smell due to acetic acid?

4. Collect the crystals using vacuum filtration. Turn the vacuum off temporarily, pour just enough COLD water to thoroughly wet the crystals, and then turn the vacuum on. Let the vacuum draw air through the crystals for 2 minutes, making certain that the seal with the rubber ring is a good one. Place a small stals on a clean watch glass and spread them thinly to facilitate drying. Using a marker rme on the watch glass and heat the crystals for 15 minutes in an oven set at a temperature of70-80 â Determine the melting point of both your dried aspirin product and pure salicylic acid. Refer to Appendix 4 for instructions on how to take a melting point. *Pure aspirin melts at 135â and pure salicylic acid melts at 156-158 â DATA SHEET/ Questions I. Record the experimental melting ranges for your recrystallized aspirin and the starting material, salicylic acid Recrystallized aspirin Salicylic acid 2. A small melting range usually indicates that: a) The compound generally has a high melting point. 6) The compound has few impurities. c) The compound is highly impure d) The compound is likely to be soluble in water e) The compound is likely to be very unreactive. f) The compound will be difficult to recrystallize. 3. Describe the appearance of your final, recrystallized product. 4. Does the aspirin have a very strong odor, suggesting that it is a very volatile substance? 5. If all of the 2.0 g of the salicylic acid that you started with was converted to aspirin and 100% of the aspirin was recovered, the expected yield of aspirin would be 2.6 g. The isolated yield is always less than this because: (choose all that are appropriate.) Water is trapped inside the crystals. A substantial amount of the aspirin evaporates. Some aspirin remains dissolved in the solvent from the first filtration. Some aspirin remains dissolved in the solvent from the recrystallization. e) The reaction used to create the aspirin does not go to completion. 1 The acetic acid formed in the reaction adversely affects the yield of aspirin. Chem 162-Aspirin tab

Organic chemistry question about extraction lab...?
Procedure:
Place 2.0 g of the mixture of sucrose, acetylsalicylic acid and acetanilide into a 125 mL Erlenmeyer flask.
Add 50 mL of methylene chloride (dichloromethane) and dissolve as much of the solid as possible.
Remove the insoluble sucrose via gravity filtration using fluted filter paper. Allow to dry until the next lab period.
Add the methylene chloride solution to the separatory funnel and extract it with two 25 mL portions of 5 % sodium bicarbonate (aqueous).
Place the combined aqueous layers into a 400 mL beaker and add enough concentrated hydrochloric acid to make it very acidic (less than pH of 2) â approximately 10 mL
Allow the solid to crystallize from the aqueous layer. Chilling in an ice bath may be required.
When lots of solid has been formed, collect the solid by vacuum filtration. Wash the solid with approximately 5 mL of cold water
Allow the solid to dry open until the next lab period.
Dry the organic layer (methylene chloride) over anhydrous sodium sulfate.
Decant the solvent from the drying agent (or gravity filter through fluted filter paper) into a clean, dry a pre-weighed 100 mL round-bottom flask.
Evaporate the solvent using rotary evaporation and allow the residue to dry open over the week.
The following lab period, weigh all 3 solids, take the melting points of all 3 solids and calculate the percent composition of the original solid.

Drying agents:
Equations for drying agents:
MgSO4 (s) + 7 H2O(l) ï MgSO4.7H2O(s)
CaSO4(s) + 2 H2O(l) ï CaSO4.2H2O(s)
CaCl2(s) + 6 H2O(l) ï CaCl2.6H2O(s)
Na2SO4(s) + 7 H2O(l) ï Na2SO4.7H2O(s)

1. The original organic solution was extracted two times with aqueous sodium bicarbonate. After the extraction, what compound(s) were in the organic layer? What compound(s) were in the aqueous layer?

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2. Assume that both acetylsalicylic acid and acetanilide are soluble in diethyl ether, and that diethyl ether was used in place of the methylene chloride. Would the ether layer be the bottom layer in the separatory funnel or the top layer? Explain your answer.

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3. Assume that both acetylsalicylic acid and acetanilide are soluble in methanol, and that methanol was used in place of the methylene chloride. What problem(s) might occur during the extractions? (Careful, this is a trick question.)

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4. Historically, the solid residue that is left after the methylene chloride solution is evaporated has a lower melting point that its literature value, due to impurities. Explain what impurities are present and why.

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CHEM 3341 Lecture Notes - Lecture 1: Katie Nolan, Ethyl Acetate, Naphthalene

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