Aspirin âAspirin (Figure P15.63) is an acid substance whose pK_a = 3.50 at body temperature

(37Â°C). One standard adult aspirin contains 325 mg of the drug. If you take 1 aspirin on a full

stomach (assume a volume of 1 L and a pH of 2.0), what percent of the aspirin in your stomach

is present as the anion?

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Tod ThielLv2

13 Dec 2019

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Aspirin has the structural formula

At body temperature (37 °C), K_a for aspirin equals 3 × 10^-5. If two aspirin tablets, each having a mass of 325 mg, are dissolved in a full stomach whose volume is 1 L and whose pH is 2, what percent of the aspirin is in the form of neutral molecules?

pearprairie-dog148

Aspirin is a monoprotic weak acid with a K a of 3.98 x 10-4 and one dose of aspirin is 500mg.

Write the reaction that controls the pH of aspirin (HC9H7O4)

Given that the average stomach has a pH of 1.4 and a volume of approximately 1 liter, calculate the concentration of aspirin (HA) and its conjugate (A - ) in the stomach.

The conjugate of aspirin is the active drug, and it is absorbed from the stomach into the bloodstream. The pH of the blood stream is 7.4. Assume that all the A - you calculated in (b) is initially absorbed into the bloodstream and calculate what the new ratio of A - /HA will become at this pH.

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