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

I need help with all or whatever i can get help in!!! This is the synthesis of aspirin lab

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