preparation of cynide?
956370
Oil of bitter almonds contains Hydrocyanic acid combined in the form of amygdalin.\nYou need to hydrolise it( acidic hydrolisis) in order to separate HCN.\nTreat it with KOH soln to get KCN.\nAlchoholis KCN on reaction with Alkyl halides to yield Alkyl cyanides.\nYou may also produce Alkyl cyanides by dehydrating Acid amides or acid oximes.\n\nThe most difficult process of the whole procedure is to separate HCN from the hydrolysis product of amygdalin. But I will not tell you that because I dont know your intention.
265334
look here\n\nhttp://webbook.nist.gov/chemistry/
506807
I'm guessing this is a question for class. In practice, working with acetylene gas as a synthetic reagent isn't a good idea. It's a flammable, explosive gas and most synthetic labs really don't have the necessary safety equipment to handle it. It's much safer to buy the butyne you need and work from there.\n\nHowever, on paper you would first make the 2-butyne. You would react 1 eq of acetylene with 2 eq of n-BuLi followed by quenching with 2 eq of MeI and standard workup and purification. If you want the 1-butyne, you can isomerize 2-butyne to 1-butyne with an amide base like NaNH2 or KHMDS.  The reason you can't just alkylate with iodoethane is that you are going to end up with a mix of acetylene, 1-butyne and 3-hexyne since you can't selective monodeprotonate every acetylene molecule. \n\nHope this helps.
42193
http://www.itt.edu/staff/boyter/links/index.html\n\nLook under chemistry equipment.  There are some chemicals you will not be able to get.  Posting what you are looking for would help.
236330
u can prepare prontosil from meta-phenylene diamine and sulphanilamide.
615612
1.  Oxidise toluene to benzoic acid using strong oxidising agents.  KMnO4 (aq) is strong enough to do this.\n\n2.  Convert you benzoic acid to benzoyl chloride, using (COCl)2 - oxalyl chloride/DMF(cat.) or SOCl2 or Ghosezs reagent or PPh3/CCl4 or PPh3/NCS etc - the former two being by far the most common methods.\n\n3.  Nitrate your malonic ester in the 2 position using isoamyl nitrate in the presence of a base, ie NaH or NaOMe.\n\n4.   Reduce your nitro to an amine (H2-Pd/C)\n\n5.  Acylate your amine with your prepared benazoyl chloride (DIPEA as a base, DCM as a solvent for example)\n\n6.  Saponify both your esters with 1M NaOH.\n\n7.  Acidify your sodium carboxylates to the free carboxylic acids and heat for a couple of hours to promote de-carboxylation.  This is a standard procedure so will work well\n\n8.  Isolate your prepared hippuric acid!\n\nThere will be many other methods - especially to prepare your methyl 2-aminomalonate.  You don;t need to form the acid chloride also.  You could just perform an amidation between your amine and benzoic acid in the presence of a coupling agent such as DIC/HOBt, CDI, HATU, PyBrOP etc etc - there are too many to mention.\n\nYou could also brominate your methyl malonate with Br2, to give methyl 2-bromomalonate.  Treat your benzoyl chloride with ammonia gas to give benzamide.  Then treating your benzamide with NaH to de-protonate your amide, and then treat with your methyl 2-bromomalonate will generate the same product as described in step 5 above.  Following the rest will give you your product.\n\nThere are more methods but hopefully this has given you some useful information.
1037670
I think you'll need to go to a university library or get a subscription to some online chemistry journals. Emil White, D. Mead Johnson Professor of Chemistry and faculty member in the Krieger School of Arts and Sciences at John's Hopkins was the first to synthesize it. Here's one promising reference:\nWhite, E.H., F. McCapra, G.F. Field, and W.D. McElroy, J.Am.Chem.Soc., 83,2402 (1961).\n\nHere's some leads:\nhttp://www.modares.ac.ir/sci/saman_h/Pages/Firefly.htm\nhttp://cas.bellarmine.edu/chem117a/lab/luminol.htm\nhttp://www.jbc.org/cgi/reprint/233/6/1528\nhttp://phot.allenpress.com/photonline/?request=get-document&doi=10.1562%2F0031-8655(2002)076%3C0153:TTMFPP%3E2.0.CO%3B2\nhttp://www3.interscience.wiley.com/cgi-bin/jhome/10009400\nhttp://www3.interscience.wiley.com/cgi-bin/jhome/4087
663581
NH4NO2 --------------> N2 + 2H20 \n\nYOU NEED TO HEAT THE SOLUTION IN ORDER TO DECOMPOSE THE COMPOUND \n \nHOPE THIS HELPS
874059
I think that isolating potassium is the wrong approach.  Potassium metal reacts with atmospheric water to form KOH and hydrogen gas.  If you accidentally get water on the metal the reaction is so vigourous that the metal will catch fire, which will be dangerous.  \n\nTry a different approach.  Dissolve KCl in water and add a molar equivalence of Silver iodide, AgI, also dissolved in water..  AgCl is nearly insoluble in water (~0.9 mg/L at 10C)  and will precipitate out, leaving KI in solution.  Filter out the AgCl and evaporate the water, leaving solid KI.  \n\nThe two biggest problems starting with KNO3 are:  It will be nearly impossible to salt out the nitrate because of its high solubility in salt form, and two, many nitrate salts, particularlyof metals, are highly explosive and dangerous.  KCl is cheap and plentiful, so why not just buy some?
857379
Nitrogen triiodide is a feisty one:\n\nhttp://en.wikipedia.org/wiki/Nitrogen_triiodide
1054522
Can't see what the matches might be for, but you could quite easily make nitrogen iodide with the iodine, which is a very unstable explosive.
316857
Part 2: Synthesis of Benzil \n\nStarting with the a-hydroxyketone benzoin (prepared in Part 1), you will prepare an oxidation product, benzil, which is an a-diketone. \n\n \n\nThis oxidation can easily be done with a variety of mild oxidizing agents, including Fehling's solution (an alkaline cupric tartrate complex) or copper(II) sulfate in pyridine.  In addition, benzoin could be oxidized by sodium dichromate, but the yield of benzil is lower because some of the benzoin is converted back into benzaldehyde following cleavage of the bond between the two oxidized carbon atoms, which is activated by the phenyl rings, producing benzoic acid as the final product.  In this experiment, due to ease of use and consistent results, we will use nitric acid as the oxidizing agent. \n\nCaution: Concentrated nitric acid is highly corrosive and causes severe burns if spilled onto your skin. Nitrogen dioxide (NO2) fumes are highly toxic and can damage the lungs due to inflammation. Do not breathe NO2 fumes, and perform this part of the experiment in the hood. \n\nProcedure \n\nHeat a mixture of 4.0 g of benzoin (prepared in Part 1; save enough for analysis, but proportion reagents as needed) into a round-bottom flask with 14.0 mL of concentrated nitric acid.  Add a stirring bar and attach a condenser to the top of the flask. Set up a reflux in the hood to vent NO2 produced during the reaction. With stirring, heat the reaction mixture. Begin timing the reaction when NO2 (red-brownish colored gas) are visible above the reaction mixture and gas bubbles are present on the stir bar. Reflux for at least 30 minutes, or until no more NO2 gas is apparent. Do not stop the reaction until the reaction is complete. Stop the reaction by removing the heating mantle, and letting the reaction mixture cool for about 5 minutes.  Add about 75 mL of cold water to the reaction mixture, cool to room temperature, and swirl for a minute or two to coagulate the precipitated product: collect and wash the yellow solid using vacuum filtration.  Continue drawing air through the crystals on the funnel by suction for about 5 minutes to assist in drying the crystals..  The crude product (dry weight 3.7-3.9 grams) need not be dried but can be crystallized at once from ethanol.  Dissolve the product in 10 mL of hot ethanol, add water dropwise to the cloud point (mixture goes from clear to cloudy, or solids being formed), and set aside to crystallize.  Record the yield, crystalline form, color, and melting point of the purified, and recrystallized, benzil.   \n\nTest for the presense of unoxidized benzoin: Dissolve about 0.5 mg of crude or purified benzil in 0.5 mL of 95% ethanol or methanol and add one drop of 10% NaOH.  If benzoin is present the solution soon acquires a purplish color owing to a complex of benzil with a product of autoxidation of benzoin.  If no color develops in 2-3 min, and indication that the sample is free from benzoin, add a small amount of benzoin, observe the color that develops, and not that if the test tube is stoppered and shaken vigorously the color momentarily disappears; when the soluton is then let stand, the color reappears. \n\nCleaning up: The aqueous filtrate (containing HNO3) should be neutralized with sodium carbonate, diluted with water, and flushed down the drain.  Ethanol used in crystallization should be placed in the organic solvents container.
824314
Two types of preps.\n\nA. To make the solution you use in titrations.\n\nPreparation of Phenolphthalein Indicator (Acid/Base Indicator) \n\n1. - Weigh out 0.5 g of phenolphthalein.\n\n2. - Prepare a 50% ethanol (ethyl alcohol) solution consisting of 50ml ethanol and 50 ml water. \n\n3. - Dissolve the phenolphthalein thoroughly in the 50% ethanol solution. \n\n4. - Use from a bottle fitted with an eye dropper. Store the rest in a stoppered bottle. \n\n\nB. To synthesize the chemical you have to go back to references in the 1880s or the patent literature of the 1950s.  You will need to find a university library for that.  The basics are the condensation reaction of phenol and phthalic anhydride.  A more modern method is given in the reference.
821226
1. sodium hypochlorite\n2. hydrogen chloride\n3. concentrated sulphuric acid\n4. oxidising it, for example with potassium manganate(VII).\n\nIf you've done the other 96, well done!
264119
Aside from the fact that it boils at -33.5°C, ammonia is a polar molecule, so it's best solvent use would be with other polar molecules, and water and alcohols would be far better solvents.  I would classify it as a poor solvent since it would be hard to use because you would have to keep it very cold, and there are better solvents you could use.\n\nUses:  Fertilizer (as mentioned previously); manufacture of nitric acid, hydrozine hydrate, hydrogen cyanide, urethane, acrylonitrile and sodium carbonate (by Solvay process); refrigerant; nitriding of steel; condensation catalyst; synthetic fibers; dyeing; neutralizing agent in petroleum industry; latex preservative; sulfite cooking liquors; fuel cells; rocket fuel; yeast nutrient; developing diazo films.
788768
Just the usual stuff.  Use an electrolyte (H2SO4/HNO3), a couple of electrodes, a reduction table of half cell potentials, and some electricity.
485893
Check on the internet for the ratios used by comercial factories, then prepare a solution from glycol and water in the given proportion. That's all!!!