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Posts posted by Cesium

  1. Binary cyanides, thiocyanides, carbides, and compounds with similar anions are usually classified as inorganic compounds even though they contain carbon. Semantics, I guess. And even so they would not meet our definition of "metal organic" because they are just salts.


    Ferrocene is a great example though.

  2. I know of no method with the mechanism you suggest. However, napthalene can be oxidized to phthalic acid with KMnO4. Then, with NaOH or lime you can decarboxylate the phthalic acid to benzoic acid, and finally to benzene. Sure sounds like a pain to me...but it should be possible.

  3. In order to perform decarboxylation you need to reflux with NaOH or Ca(OH)2 IIRC. I'm not sure how hard it would be to make sure you didn't decarboxylate all the way to benzene. Somebody here probably knows.

  4. Uh...almost any alcohol; methyl, ethyl, isopropyl phthalates. Both the di and mono esters exist. They are not particularly interesting; phthalate esters are used as an additives to plastics. Common ones are benzyl butyl phthalate and diisobutyl phthalate. Where did you get phthalic acid?


    As for chloric to perchloric acid, electrolysis may work.

  5. It's just more hassle than is really necessary. SO2 is soluble in water so you shouldn't loose much if you take it slow.


    Woelen, how do you prevent that suck back from occuring? The exact some problem happened to me several times when I was dissolving NO2 in water (from the decomposition of Mg(NO3)2). As soon as I stopped heating, my liquid would get sucked back into the Mg(NO3)2. I quickly learned to remove the tube from the beaker before I stopped heating. I also tried to clamp the tube after heating, but this didn't work too well (the suction was quite powerful).

  6. Do the copper salt thing in solution as suggested. If you don't have CuSO4 or CuCl2 on hand, add some copper (from wire, old parts, etc.) to a mixture of HCl and H2O2 (3% is fine). This will give you a solution of CuCl2- dilute it and then add to zinc.

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