Anti-Inflammatories

Pulverizing an aspirin tablet is a physical change (it is not a property at all). The chemical nature of the aspirin does not change when it is pulverized.

Salicylic acid is more polar than aspirin because it has a higher solubility in water due to the presence of a hydroxyl group that enhances its polarity. Aspirin, on the other hand, has an ester functional group, which reduces its overall polarity compared to salicylic acid.

The common paracetamol tablet is approximately 1cm long anyway. Depending on the manufacturer, aspirin may come in different shapes, but I think it's a fair assumption to say the longer end is approx 1cm

Aspirin purity can be tested using acid-base indicators such as phenolphthalein or bromothymol blue. These indicators change color based on the pH of the solution, allowing for a qualitative assessment of purity. However, more precise quantitative methods such as spectrophotometry or chromatography are typically used for accurate purity testing of aspirin.

Asprin is not an element, so it is not found on the periodic table.

Aspirin is a white crystalline powder with a melting point of 135°C.

The common chemical name for aspirin is acetylsalicylic acid. Its systematic name is 2-(acetyloxy)benzoic acid. The chemical formula of aspirin is C9H8O4.

It is generally safe to take ibuprofen with Alka-Seltzer Cold, but it's always best to consult with a healthcare provider or pharmacist before combining medications to ensure there are no potential interactions or contraindications.

melting point- 136 degree C boiling point- 140 degree C

The active medical ingredient in Aspirin is acetylsalicylic acid, or A.S.A.

To determine the number of molecules in a 500 mg tablet of acetaminophen (C8H9NO2), follow these steps:

1. Calculate the molar mass of acetaminophen (C8H9NO2) by adding the atomic masses of each element present (C: 12.01, H: 1.01, N: 14.01, O: 16.00). This gives a molar mass of 151.17 g/mol.
2. Convert the mass of the tablet (500 mg) to grams (0.5 g).
3. Use the molar mass to calculate the number of moles in 0.5 g of acetaminophen.
4. Finally, use Avogadro's number (6.022 x 10^23 molecules/mol) to convert moles to the number of molecules in the tablet.

Water-aspirin can potentially enhance plant growth by acting as a stress reliever and stimulating the plant's natural defense mechanisms. Aspirin contains salicylic acid, which can help plants fight off diseases and increase their resilience to environmental stressors. However, it is important to use water-aspirin solutions in moderation to avoid negative effects on plant health.

Aspirin is hydrolyzed in the body to salicylic acid by esterases in the liver. This process involves cleaving the acetyl group from the salicylate molecule to form salicylic acid, which is then further metabolized to various metabolites. Salicylic acid is the active metabolite responsible for the anti-inflammatory and analgesic effects of aspirin.

It is possible to extract salicylic acid, a precursor to aspirin, from certain plants like willow bark; however, most aspirin is now synthesized in a laboratory setting. Harvesting aspirin from plants is not common practice due to efficiency and cost considerations.

Yes it will be weakly acidic. Aspirin's scientific name is acetylsalicylic acid, with a pKa of 3.5. This would mean that for a solution of 0.1 M aspirin, the pH of the solution would be approximately 2.26.

Givens for question above: If the aspirin tablet is 0.4635g. it was titrated with 18.23mL of 0.1000M NaOH to neutralize. Then 33mL of NaOH was added to hydrolyze. then it was back titrated w/13.59mL HCl. what is mass of acetylsalicylic acid? what is the percent w/w?

Caffeine > Acetaminophen > Ibuprofen > ASA

Actually ASA is more polar than Ibuprofen. In ethanol ASA rf value is around .7 and Ibuprofen is around .77.

Should be Caffeine > Acetaminophen > ASA > Ibuprofen

Rf in ethanol Caffeine < Acetaminophen < ASA < Ibuprofen

Aspirin is classified under antipyretic (decreases temperature) and a non-opioid analgesic (reduces pain). It can also be used as a anti-thrombolytic (anti-clotting agent- 81mg) It makes the platelets (blood component responsible for clotting) slippery so they don't stick to anything in the vessels, which decreases your risk of DVT (blood clots).

Vacuum filtration was used instead of gravity filtration in the isolation of aspirin to speed up the filtration process by applying negative pressure to draw the solvent through the filter paper more quickly. This helps to separate the solid product from the solvent more efficiently and saves time in the isolation process.

Phosphoric acid is used in the synthesis of aspirin as a catalyst to facilitate the esterification reaction between salicylic acid and acetic anhydride. It helps increase the reaction rate and yield of aspirin.

The functional groups of anything are the croups that aren't normal alkane (single carbon-hydrogen bonds) groups. In the case of Ibuprofen there are two functional groups. The first is the aromatic group or Benzene ring in the centre of the structure. The second is the carboxylic acid group (Oxygen double bonded to two

Maintaining the temperature at 90 degrees C in the synthesis of aspirin helps to achieve optimal reaction kinetics, ensuring the reaction proceeds at a suitable rate. This temperature also promotes the formation of the desired product while minimizing the formation of unwanted byproducts.

see there http://homechemistry.blogspot.com/2008/04/aspirin-lab.html Lesson: Acid-catalyzed hydrolysis of acetylsalicylic acid to salicylic acid and acetic acid What Happened: We dissolved the active ingredient of aspirin in water, separated it from the binder, then purified the drug using sulfuric acid as a catalyst. The World of Chemistry video series, which you can watch online at Annenberg Media, has been serving as our spine lately. We were up to the episode on catalysts this week, so I found a demonstration from The Joy of Chemistry (actually from the chapter on organic chemistry) which used dilute sulfuric acid (sold as aquarium pH lowering solution) as a catalyst to purify aspirin. FYI, another example of a catalyst at work were the pineapple enzymes we used to dissolve Jello. According to Wikipedia, the end product of this demonstration, salicylic acid, is what aspirin metabolizes into in the liver. Its name comes from the Latin word for the willow tree, Salix, from whose bark it can be obtained. Interestingly, it can also be derived from methyl salicylate (oil of wintergreen). In 1897, Felix Hoffmann, a chemist at Friedrich Bayer & Co., obtained acetylsalicylic acid by a reaction of salicylic acid and acetic anhydride; this is the basis for Bayer's claims to the discovery of aspirin. Materials: Safety glasses Rubber gloves 10-15 aspirin (plain or buffered) ½ cup (120 ml) rubbing alcohol (70% isopropyl) 2-4 large glass containers (we used a Pyrex bowl and old honey jars and canning jars) Coffee filters and rubber bands Sturdy plastic spoon Aquarium lowering solution (dilute sulfuric acid) Pipette or straw =>>>>>>>>>>>>>>>>>>>> 1.Place aspirin in glass. 2.Pour in alcohol, a little more than needed to cover the aspirin. 3.Heat the glass in the microwave on 50% power for 30 seconds until warm but not boiling. The acetylsalicyclic acid will dissolve in the alcohol, leaving the starch binder. 4.Gently crush remaining residue with spoon to extract as much acid as possible. Let sit 15-30 minutes. 5.Take coffee filter and spread it over top of second glass. Push it down slightly so it resembles a funnel. Secure with rubber band. 6.Carefully pour the solution through the filter. The liquid that drips through is called the “mother liquor.” The acetylsalicylic acid has dissolved in the water. What's left on the filter is the starch binder that holds the drug in the pill shape. 7.Wearing gloves, dispose of coffee filter. Don’t touch the wet part. 8.Run a small stream of cold tap water. Take the glass with the mother liquor and add water until it is about ¾ full. Small white flakes of acid should begin falling out of solution. Let sit for a couple hours. 9.Set up another filter on another glass. Pour mixture through filter to separate out the crystals. 10.Filter 2-3 times if needed, letting solution sit for 1-2 hours in between. 11.Allow to dry overnight, away from breezes. The crystals will become fluffy. 12.Take ¼ of wet or dry crystals and put into glass. Add aquarium solution dropwise with a pipette or straw until the entire sample is completely covered. The sulfuric acid is the catalyst and remains at the end, so be careful with the liquid. 13.Heat the mixture in the microwave for no more than 15 seconds at 50% power. It may start to steam immediately. 14.Remove glass. You should smell vinegar (acetic acid) evaporating. If not, wave your hand over the glass to waft the fumes towards your nose. The sludge that remains is salicylic acid. 15.Dispose of solids in the trash and liquids in the toilet. NOTES: We ended up doing the demonstration twice -- although, as it turned out, we probably didn't need to -- because the shopping list at the beginning of the book didn't specify that the alcohol needed was 70% concentration. I found an old bottle of the right concentration, and we did everything over. However, we discovered that letting the first solution sit and filtering it several more times yielded enough crystals to do the demonstration. In the end, we had twice as much acetylsalicylic acid as we needed. We probably used too much in the final step (as well as too much sulfuric acid, which I tried to pour slowly out of the bottle instead of using a pipette) because when we put it in the microwave, it immediately started steaming! I turned it off a few seconds short of 15 and the vinegar smell was overwhelming.

The ingredients needed to produce aspirin are salicylic acid and acetic anhydride. Acetic acid is also produced as a byproduct during the chemical reaction.

Do not be confused with alcohols nor ketones when seeing the -OH and the =O bonded. They each are really parts of either:
- the carboxylic acid group (-COOH)
- the ester link (from neighbour carbon along the ring)


Likewise, double-bonds you see constitute the benzene (aromatic) ring:
- a functional group in itself
- they are not the normal alkene double bonds
- would actually best be represented by a circle inside the ring,
- not double lines for each of 3 double bonds, as resonance occurs in benzene rings.


Therefore, aspirin (or acetylsalicylic acid) contains:
- aromatic ring
- carboxylic acid group
- ester group
and can be regarded as an acid (i.e. acetylsalicylic acid)
or the acetate ester of salicylic acid :-)


so aspirin is (if choosing from your options):
- not an alkene, nor a ketone, nor an alcohol.
- we are left with a carboxylic acid
BUT we usually only regard aspirin as an acetate ester, or a derivative of salicylic acid,
so you wouldn't generally hear one calling aspirin a carboxylic acid :-)


I hope I cleared things up a bit :-)
Cheers.