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deltaH

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About deltaH

  • Rank
    Quark
  • Birthday 10/16/1980

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  • Website URL
    http://www.ideashack.org

Profile Information

  • Location
    South Africa
  • Interests
    Chemistry, innovation, process design and development, sustainable technologies
  • College Major/Degree
    Chemical Engineering
  • Favorite Area of Science
    Chemistry
  1. I don't think it's as simple as that John, especially as I've already seen that dilute H2SO4 made albumin dissolve very well and not cause it to denature. As for the ammonium sulfate, I've never seen it at our nurseries here, but I will check next time I am nearby. Nevertheless, I am not happy with the denaturation test as whole anymore, it's just too neither here nor there for my liking. I think I need to concentrate on isolating the guanidine. A good friend of mine from the SM forum has made a suggestion to add excess sodium hydroxide and use that to drive off the ammonia, provided t
  2. "It's possible that some denaturing of the protein is due to the acid rather than guanidinium." Yes exactly what I suspected, which is why I did that control test with some diluted battery acid. But the egg white simply dissolved more easily (instantly). It doesn't curdle like milk does upon acidification. I'll be honest, qualitatively testing for guanidine is a tough problem and I cannot call it neither here nor there with these protein tests anymore. There is some evidence for a positive test, but it's not dramatic enough to be a resounding yes. "Try neutralising some of the product an
  3. "Congratulations, you have proved that the stuff either contains guanidinium or ammonium sulphate, both of which will precipitate proteins. http://web.mnstate.e...ateProtocol.pdf But I didn't think that was a matter of contention." Thank you for highlighting a possible problem in my guanidine test and attaching your protocol article. There is, however, a big difference between precipitating proteins and denaturing proteins. As per your article, ammonium sulfate precipitates without denaturing. This should redissolve again upon addition of large volumes of fresh water. I will repeat my test a
  4. Thank you very much for the link and advice. I was concerned because ordinarily a larger organic cation on an anionic surfactant tends to increase solubility of the surfactant. I myself have prepared choline palmitate soaps that are extremely soluble (compared to their sodium counterparts). I took some liquid dishwashing detergents and mixed it with some of the partially neutralised solution that I had sitting outside evaporating from my first successful batch experiments. In theory, there should be guanidine sulfates in there. This caused immediate precipitation upon squirting in som
  5. Indeed and thanks. Have you a reference for the guanidine precipitation you mentioned? I still cannot find info on that.
  6. "Sodium dodecyl sulphate will form a precipitate with guanidinium ions..." Intriguing and thanks for the suggestion. As I struggled to verify this, do you have a reference for me please? "Also, learn to do titrations, that will let you produce much better quantitative data." I would need a burette and at least a two decimal scale for that. This would cost me more money than I can afford at the moment. I admit it would come in very handy, but it's something that I will need to put off for a while.
  7. Sadly IR is out of the question for my means at the moment, if somebody would like to assist in this regard, it would be greatly appreciated! Failing this, I can only try a 'wet' chemical test for guanidine salts, as a matter of priority. ********************************************* Okay, I had some time today and so decided to prepare another batch because I need material for testing (I had neutralised the material from my first batch a while ago). Unfortunately, my retailer was out of the good quality battery acid I bought last time (I estimated it's H2SO4 conc. to be about 37%). I
  8. "It's clear to me that you have little or no idea what you have made." I have as far as I can tell obtained an unknown product that is not described by the literature to the best of my knowledge. So what do we do in such a case? We perform experiments and propose a theory that fits the observations. I have started this process and the current best theory I have for it is NH4•C(NH2)3•2HSO4•H2SO4 based on the experimental observations. By the scientific method, this is correct until proven otherwise, but it's not necessarily the Answer/Truth. If you dispute why my observations do not fit th
  9. Hi Phi for All, absolutely! Attack on my idea is welcome by employing scientific arguments, however, John Cuthber makes no such attempt, merely references an insult and an unrelated post (as I've explained), and yes, I've reported it almost the moment I saw it Now for those who have scientific arguments to make... I will be EXTREMELY grateful to them. ***************************************** I would like to make a correction to my original post, there is a typo in my equation: 2(NH2)2CO(s) + 4H2SO4(l) + heat => NH4•C(NH2)3•2HSO4•H2SO4(l) + CO2(g) Should read: 2(NH2)2CO(s) +
  10. Kudo's for your creative attempt to enflame by reference, it didn't work there, it doesn't work here either. How can it... it's just an insult, you don't even make a logical argument to counter? What's worse is that link pertains to my investigation to find an OTC route to prepare ammonium carbamate from urea, the discovery of the salt I discuss here is in fact one of the reasons that route I investigated is low yielding! As for your suggestion of KNO2... this is particularly dangerous, trying to get me to blow myself up with azo salts... nice The action of nitric acid (generated in s
  11. Hi mooeypoo... very interesting question! I suggest trying ordinary epsom salts, MgSO4.7H2O for your ice cube experiment (use a generous sprinkling). I will now sneeze: aah-aaaah-aaaaah-choooo-MgSO4.11H2O-ooooooo, pardon me Wow, just stared at my toast and saw an interesting image... here... I'll show you: Source: Ronald C. Peterson and Ruiyao Wang, Crystal molds on Mars: Melting of a possible new mineral species to create Martian chaotic terrain, 2006, linked to Wikipedia's article on Meridianiite on 6th November 2013.
  12. Thanks hypervalent_iodine and so true! Unfortunately I don't think MSDS' exists for my product as I believe it is novel, however, urea's and sulfuric acid's MSDS' certainly do exists and as for the product, familiarising oneself with those (particularly conc. sulfuric acid) as well as for ammonium bisulfate and guanidinium bisulfate or sulfate should come close enough! I have also found some literature that may be pertinent to this topic, namely, the known preparation of guanidine sulfates from urea and sulfamic acid. If my formula hypothesis is correct, then these studies may suggest that
  13. Pt/Ir would be great, but if you are just using a wire, then you will not be able to run very high current in your cell because the surface area of your wire is very small, however, as for durability and the especially water electrolysis, it should perform well on a small scale and for demonstration purposes.
  14. WARNING: This preparation involves boiling strong concentrated acids that would corrode flesh instantly if it lands on you and also causes terrible thermal and chemical burns. It should only be attempted while wearing a plastic apron, face shield, thick rubber gloves and labcoat while working in a fume cupboard and having a water shower source nearby and by skilled practitioners. The product when wet with attack many hydrolysable plastics such as polyesters and polyamides, as well as many metals. The use of polypropylene and glass is strongly advised. If you carry out this reaction, you do it
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