salicyclic acid + acetic anhydride -> aspirin and acetic acid\n\nlaws, uses of catalysts, mostly theory and background info
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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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Vinegar is an acid and is also a catalyst for corrosion of iron\n\nOil is hydrophobic and will prevent oxidation from occurring, therefor preserving the iron\n\nWater will promote oxidation and in turn degrade the iron to iron oxide (rust)
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not aspirin but it's parent compound salicylic acid. it reacts with iron and turns purple. it's a test for impurities in aspirin.
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go to\nwww.chemistry.com
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understanding the reaction meachanism \neffect of catalysts etc....\ndetermining the amounts needed
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I am not a chemistry student but I make this research for you and maybe it helps you http://www.chem.latech.edu/~deddy/chem104/104Antacid.htm\nhttp://www.chemcool.com/regents/acidsbasessalts/aim3.htm\n\njust copy those links and you should be on your way to solve ur problem.
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K2IC4H6 + HNO3 ---  K2HI + NO3C4H6
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CO2. and you can also use vinegar.
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It's an acid catalysed hydrolysis. The oxygen attached to the 2-carbon is protonated, then acetic acid is displaced from the ring by water, which is deprotonated to give salicylic acid. The vinegar smell is acetic acid. Note that the reaction cannot occur without water.
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mix vinegar and baking soda.  a chemical reaction will take place.
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Two things:\n\nThe aspirin is coated with a substance so as to dissolve in the gut instead of the stomach.\n\nThe aspirin is mixed with the basic ingredients, Calcium Carbonate and Magnesium carbonate, a small amount.
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Below is the spectrum for acetasalicylic acid.  There will only be a small difference between the chemicals shifts in the aromatic hydrogens between the two compounds.  Also, you will obviously not have the singlet from the 3 methyl hydrogens.\n\nThe second link shows the spectrum in methanol, but its kinda hard to see.
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It smells like vinegar b/c it has decomposed into salicylic acid and acetic acid. Acetic acid is essentially vinegar. It will still work as an analgesic (pain reliever) but it will no longer have an effect on platelet aggregation - blood clotting. Aspirin will normally  (when not expired) help "thin" the blood - an important role when someone is having a heart attack.  If you give someone an expired aspirin that is having a heart attack, it will not help to save thier life.  Also, since the tablet is now more acidic from decomposition, it can (and most likely will) cause stomach upset.
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1. AgCl(s) + NaNO3\n\n2. AgOH(s) + NaNO3\n\n3. They would not react as both are nitrates already
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that depends upon wheather you are going to design experiments for bulk product aspirin or formulations like aspirin tablets.\nfor bulk products tests like melting point, assay(percentage purity), solubility testing .... etc,.\nif that is a tablet you have to proceed with release rate, tablet weight, frightness test,etc.....
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The Lewis or Brønstedt acid-catalyzed esterification of carboxylic acids with alcohols to give esters is a typical reaction in which the products and reactants are in equilibrium.\n\nThe equilibrium may be influenced by either removing one product from the reaction mixture (for example, removal of the water by azeotropic distillation or absorption by molecular sieves) or by employing an excess of one reactant.\n\nIf you want to reverse the equilibrium, add water or remove the alcohol.
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To esterify a carboxylic acid (including oleic acid), you need to add the appropriate alcohol (polyethylene glycol) and an acid to catalyze the reaction.  However, to drive the reaction to completion, you must remove water that is produced as a coproduct.  You can do this by heating (boiling off the water).\n\nAlternatively, you can convert the acid to an acid chloride (using, for instance, thionyl chloride) and then reacting the acid chloride with the alcohol.  This is usually done in a non-nucleophillic base, such as pyridine, to react with the HCl that is produced during esterification.