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ercdndrs

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About ercdndrs

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    Quark

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    ON, Canada
  • Favorite Area of Science
    Chemistry
  1. If H2O2 is a stronger oxidiser than bromine (I'm not sure it is)you could do the following. We'll assume you're using sodium bromide. 1) add HCl to an aqueous solution of NaBR so you have: Na+, Cl-, H+, Br- in solution 2) add H2O2 to the solution. The peroxide will oxidise the H+ to H2O and Br- will turn to Br2. Bromine will form over chlorine because it is a weaker oxidising agent.
  2. Not sure if this is the right thread, but I was wondering if concentrated (98%) H2SO4 will degrade a HDPE container. Thanks in advance!
  3. Ok thank you! Have yet to conduct the experiment because I've decided against using acetone as the resulting ketazine is soluble in water and I don't want to bother with distillation of it. Will post my results as soon as I can get some MEK.
  4. Iron chloride solution is yellow; I don't know if the little bit of iron in your solution could cause that drastic a colour change though.
  5. I don't so much have any special use for the hydrazine sulfate; I just think the reaction would be interesting and good practise. In any case I could just sell the product on ebay or something. I do have acess to a large backyard, and yes I am aware of the toxic fumes. Obviously I wouldn't be trying this on a large scale, but something small just for curiosity's sake.
  6. Hey all, So I am looking to make some hydrazine sulfate through the ketazine process. However, I don't have acess to the ideal ingredients so I am wondering if my subsitutions would work: 65%Calcium hypochlorite powder susbtituted for NaClO solution 10% concentrated ammonia acetone instead of 2-butanone I would carry out the reaction with excess ammonia and then distill off the dimethyl ketazine from the solution before reacting it with sulfuric acid to get hydrazine sulfate. Are there any problems with this? Thanks in advance!
  7. Hello All, I'm also interested in making nitric acid. I do have ammonium nitrate and sulfuric acid, but my acid is very impure (buffering agents and colliodal carbon). So, I am thinking of trying this alternate route, requiring few special materials (get ammonium nitrate from disposable cold packs): 1) Electrolyse ammonium nitrate solution with copper anode: 2 NO3- + Cu(s) - 2e = Cu(NO3)2(aq) 2 NH4+ + 2 H2O + 2e = H2(g) + 2 NH4OH(aq) NH4OH(aq) =NH3(g) + H2O 2) Electrolyse again with graphite electrodes: 2 Cu(NO3)2(aq) + 2 H2O = 2 Cu(s) + 4 HNO3(aq) + O2(g) As far as I know copper will only react with concentrated or hot oxidising acids. I know sulfuric acid can be prepared in the same way as step 2 from copper (II) sulfate, so I am wondering if nitric acid can be produced this way and if this process will work in general. Are there any problems with anything I've done here? Thanks!
  8. Just that, can a solution of chlorate be converted to perchlorate using hydrogen peroxide? ClO3- + H2O2 = H2O + ClO4- Guess this is just a question of H2O2's strength as an oxidiser compared to chlorate? Or to perchlorate, because the product, perchlorate, is more stable than chlorate, would this drive the reaction to completion? Thanks
  9. Hey all, I am considering making a cell for the production of perchlorates, and I am stuck on finding a suitable material for my anode. Obviously I need something that is conductive but won't react with the chloride/ up to perchlorate ions present during electrolyis. I do have carbon (graphite) electrodes but I've read they are messy and are slowly eaten away. Platinum is always an option but it is expensive, so I am wondering if I can just use nickel or a nickel based alloy instead? Thanks
  10. You'll only be able to reach ~20% concentration through boiling the acid. http://en.wikipedia.org/wiki/Hydrochloric_acid
  11. The title states it all: a) Would the 2 chemicals react B) If so, what would the products be? A few things i could guess: 1) CH3-CH3 + H2O2 -> 2 H2O + CH2=CH2 2) CH3-CH3 + 2 H2O2 -> 2 H2O + HO-CH2-CH2-OH 3) CH3-CH3 + H2O2 -> H2O + CH3-CH2-OH Thanks in advance!
  12. Unfortunately I can't accurately answer your questions, but I have some things I'd like to point out. 1. If you want to do this efficiently/ inexpensively, batteries aren't the gratest choice. I use a car battery charger, preferrably with a low (~2V) voltage/high current setting. 2. make sure you use an inert anode, or you'll have a metal sulfate, magnesium hydroxide, and H2 gas forming instead of H2 and O2.
  13. So it seems cracking = breaking of C-C bonds in a hydrocarbon; dehydrogenation = breaking of C-H bonds.
  14. The iron will decompose the peroxide to water and oxygen gas, which will bubble up, though some will dissolve in the water and make the iron rust. I don't know what you have the sodium chloride in there for but I doubt it will do much.
  15. In the original question: "...semi safe to breathe...." Most people wouldn't consider iodine/HI vapor even remotely safe to inhale, being a halogen/strong acid and all ; )
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