background theory for synthesising aspirin?
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phosphoric acid is the catalyst used in the synthesis.    Its a one to one molar ratio reaction.
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take a carboxylic acid and couple under normal conditions with an O-alkylated/acylated hydroxylamine.\n\nBy normal conditions, I mean normal peptide coupling conditions usined EDC, DIC/HOBt, CDI, PyBOP, PyBrOP, TBTU etc etc etc
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Grignard Synthesis of Benzoic Acid\n\n\nPreparation:  McMurry, sections 10.8 and 20.6.\n\nConversion of an organic halide into a Grignard reagent completely transforms the reactive character of the organic compound. Carbon bears partial positive charge when bonded to halogen but partial negative charge when the carbon is bonded to magnesium. The Grignard reagent is a very reactive nucleophile and base. \n\nIn this experiment you will make the Grignard reagent phenyl magnesium bromide; this reagent will then be treated with carbon dioxide to form benzoic acid. The sequence (Equation I) is explained in McMurry Sect 20.6.\n\n\nAs in any work, this experiment may not succeed the first time; be prepared to repeat it from the beginning. On the second try, you should be able to work much more efficiently and with more understanding. \n\n\nProcedure: Obtain a 150 mm piece of magnesium ribbon. Hold one end with forceps and with the other hand remove the residue on the ribbon by scraping it with a spatula, scissors or pliers to obtain a shiny surface. Cut at least 0.12 g of the shiny ribbon into 2-3 mm pieces (do not handle the pieces) and place on a folded piece of paper to obtain the mass on the balance. Transfer the magnesium pieces to the 5 mL conical vial, add the dry spin vane, add one small crystal of iodine and add 300 µL (0.3 mL) of anhydrous ether. Be prepared to add more ether as necessary to maintain the liquid level at a minimum of 300 µL.\n\nAssemble the rest of the apparatus as in Mayo, et al., Fig 3.24. Clamp the apparatus firmly to a stand.\n\nIn the hood, prepare a solution of 510 µL of bromobenzene in 700 µL of anhydrous ether in the 3 mL vial using the delivery pipettes provided. Cap this vial with a polyethylene top. \n\n(*Note:  Be certain the dry ice is ready before you initiate the reaction below.)\n\nDraw half of the bromobenzene solution into the syringe and insert the needle through the polyethylene cap in the Claisen head as in the figure. While stirring the mixture below, add 6-8 drops of the bromobenzene solution. Evidence of reaction is the formation of tiny bubbles. When the reaction has started, add the remainder of the bromobenzene solution slowly over 3-5 min. The temperature should be maintained at about 40 oC to allow gentle refluxing (Mayo, et al., p. 29) of the ether. To the 3 mL vial add an extra 300 µL of ether, then transfer this to the reaction via the syringe. Adjust the total volume to 3 mL with the addition of more anhydrous ether. Reflux the mixture for 10 minutes, then allow the gray-brown solution of the Grignard reagent to cool to room temperature. What do you observe?\n\nThe Dry Ice (at least 1.0 g) is added in small chunks to the Grignard solution. Note the reaction as this is added. To convert the C6H5C(=O)-OMgBr, to benzoic acid (last step, Equation I), use a pipet to VERY SLOWLY add 1 mL of 6 N HCl and again observe the result. Test the aqueous layer with pH paper; it should be acidic. Remove the ether by gently heating the vial for 5 minutes on the steam bath. Cap the vial, mark it and set it in your drawer until the next laboratory period. \n\nPreparation for the 2nd laboratory period:  The benzoic acid has been synthesized, but it must be purified. Water soluble magnesium salts are removed by extracting away the water layer; but, a number of organic side products remain with the benzoic acid.  These are side products of the Grignard reaction; small amounts of benzene are formed (Equation II), unreacted bromobenzene remains, and biphenyl, H5C6-C6H5, is formed from the reaction (Equation III). \n\nThe benzoic acid can be isolated from this mixture by taking advantage of its property as an acid. Only it can dissolve in aqueous NaOH (Equation IV) while the side products remain in the ether. After the ether-soluble side products have been removed, strong acid is again added to reverse this reaction in order to restore the benzoic acid.\n\nRecrystallization of the crude product in
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Hey my research topic also includes it. I use Smethyl thiourea for doing so. check out my site\nGoto projects and then goto view documents. there you will find various patents. goto oxadiazine synthesis patent
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Chemexper.com its super cool , type in the name of the compound and it will give you a ton of info about the thing you are looking at. I order chemicals off of it but it was really useful in researching for my Ochem labs as well.
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if you are really interested in in organic chemistry, go ahead with some synthetic work.but as per as your knowledge in organic chemistry, i don't know you would be able to do this kind of projects. anyway here i am suggesting you some synthesis.\n\n1) conversion of benzene to acetaminophen.\n2) conversion of aniline to acetanilide.\n3) synthesis of isonicotinic acid hydrazide from gamma picoline.
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ChemDraw from CambridgeSoft Corporation may be help you. Look at www.cambridgesoft.com
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http://www-ec.njit.edu/~skawinsk/chem243/chap11/chap11.htm\nthis may help–near the bottom
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In order to increase shell life, aspirin are usually stored in cool place because aspirin contains salicylic acid which deteriorates in warm condition which in thus would result in loose the effectiveness of the drug. \n    The reason for it to be stored in dark place because aspirin contains light sensitive ingredients which in the presence of light causes these ingredients to alter its conformation at molecular level which in thus would result in drug to loose its effectiveness. \n\nOverall just keep them in dark and at room temperature places and dont mess with them.
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ag, aspirin is itself an ester, though. The para hydroxy group is esterified to reduce the acidity of the molecule.\n\nThe best way to determine it, in my book, would probably be by HPLC (High Performance liquid chromatography). We did an experiment in undergraduate analytical chemistry for this purpose ... to figure out ASA in Aspirin.\n\nThe main problem, analytically, with aspirin is that the ester group could react with the base. This would create an interference in your result, because you'll use more NaOH than you would otherwise and you'll think the aspirin concentration is higher than it actually is.\n\nIgnoring the ester, the way to recover the ASA is to pulverize (grind up) the aspirin tablet and dissolve it in chloroform (or dichloromethane). Then filter off the insoluble material and evaporate off the chloroform. You could then dissolve the resulting white powder in (pre-boiled) water and titrate with NaOH. The NaOH should be standardized with KHP.\n\nTo get rid of the ester, ag is correct. You'd need to react it with concentrated acid (or Lithium aluminium hydride, but I somehow doubt you have that lying around). Then you'd need to use TLC (thin layer chromatography) to make sure that all the ester was converted (by doing a comparison spot with salicylic acid). Then,  you'd need to remove the salicylic acid with a separation (chloroform or dichloromethane), evaporate it off, and titrate.\n\nAssuming all of that worked (organic procedures aren't truely analytical, all the time), you could then figure it out.
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Synthesis - a compound forms from simpler reactants
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this is called the bioavailability of a drug. the aspirin is absorbed into the blood stream after being ingested, it enters the liver where it is broken down this is called 1st pass metabolism.  the remainder is utilised by the body the active ingredient.  the kidneys should not be excreting aspirin so u can not find out by this method.  most drugs have a certain calculated bioavailability so this is what you should be looking 4
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This might help :)\nhttp://www.chemicalforums.com/index.php?board=8;action=display;threadid=3263
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Look up the site chemfinder.com.  its a good website if you have not heard of it already.
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Key points to look for include:\n\nInfrared\n-NO2 bonds: 1515-1560, 1345-1385\nAlkenes: C-H: 3020-3080 (moderate), 675-1000\n         C=C: 1640-1680(variable) \nIf wet: Large OH hump in the 3500 area... should obliterate most other peaks in the area.\n\nI am not as up to scratch with NMR.\n\nThis is a common compound and an IR and NMR spectra should be easily found on the internet. I recommend chaecking them carefully as jus tlooking for the peaks above will probably not be highly useful.\n\nEven better than the internet is a resource book, any laboratory or university library should have such resource books.\n\nPersonally I recommend that if you are doing much organic chemistry to get 'Organic CHemistry' by Morrison R.T. and Boyd R.N., published by Prentice Hall.\nThis book has an excellent guide for spectra.
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Use the Arrhenius equation to predict the rate:\n\nhttp://en.wikipedia.org/wiki/Arrhenius_equation\n\nK = Ae -E/RT\n\nIt all boils down to your reactants, the activation of energy, and the product that is being synthesized.
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There are too many challenges in this molecule to come up with a synthesis in a few minutes.....1 chiral centre, 2 quartenary carbon centres next to each other, and geometrically specific double bonds.  However many syntheses have been completed.  The references below will direct you to published syntheses of analogues.  The first two are probably the most useful.\n\nTetrahedron, 1992, 8229-8238\nTetrahedron Letters, 1972, 2521-2524\nTetrahedron Letters, 1999, 6347-6351\nTetrahedron Letters, 1997, 1797-1800\nPhytochemistry, 1996, 23-28\nBioorganic and Medicinal Chemistry Letters, 1995, 275-278\nTetrahedron Letters, 1989, 1741-1744\nTetrahedron Letters, 1988, 5339-5342\n\nyou can access the journals through www.sciencedirect.com, but you may need to pay for them if your institution doesn't have access.\n\nhttp://cbr-rbc.nrc-cnrc.gc.ca/abscisicacid/\n\nAlso try the link above - gives you some more information.\n\nHope this helps.