akcapr Posted April 21, 2005 Share Posted April 21, 2005 If i was to make nitric acid via the sulfuric acid- potassium nitrate method, how would i accurately figure out the concentration of the nitric acid knowing the amount of liquid the NO2 will dissovle in,the amount of H2so4 and its conc., and knowing amount of potassium nitrate, and assuming all the gas will dissolve? also, just making sure: the colder the water the better the gas will dissolve in it, correct? Link to comment Share on other sites More sharing options...
raivo Posted April 21, 2005 Share Posted April 21, 2005 [math]\ce{H2SO4 + KNO3 -> KHSO4 + HNO3}[/math] Link to comment Share on other sites More sharing options...
akcapr Posted April 21, 2005 Author Share Posted April 21, 2005 sometin like an equation would help. I know the reaction, just how to figure out the concentration depending on the amount of water it dissolves in. Link to comment Share on other sites More sharing options...
budullewraagh Posted April 21, 2005 Share Posted April 21, 2005 i strongly advise you to not make nitric anhydride. it comes back to haunt you later in life Link to comment Share on other sites More sharing options...
Silencer Posted April 21, 2005 Share Posted April 21, 2005 how would one remover the potassium sulfate after the above reaction? I thought all sulfates were soluble... Link to comment Share on other sites More sharing options...
akcapr Posted April 21, 2005 Author Share Posted April 21, 2005 i wasnt gonna make it purposely, how do i better make nitric acid then? and kno how to figure the conc. I was think no2 would come out due to the heat Link to comment Share on other sites More sharing options...
H2SO4 Posted April 21, 2005 Share Posted April 21, 2005 you could tr y titration. Heres a link to a page that shows procedure. Ive never performed titration but iv read about it in books. http://en.wikipedia.org/wiki/Titration Link to comment Share on other sites More sharing options...
Fortuna Posted April 23, 2005 Share Posted April 23, 2005 Actually, simply measuring the density with a good volumetric column and an accurate scale will give you a pretty good idea of the concentration you have. The titration method of course works a bit better and is admittedly more accurate. However, be sure you don;t have any unreacted H2SO4 in there. If you know the purity of the H2SO4 and KNO3 you started with, you should already have a pretty good idea of what the concentration is anyway. Link to comment Share on other sites More sharing options...
akcapr Posted April 23, 2005 Author Share Posted April 23, 2005 what about the nitric anhydride thing bulldewraagh said? Link to comment Share on other sites More sharing options...
budullewraagh Posted April 23, 2005 Share Posted April 23, 2005 it's scary and it will cause permanent respiratory failure. if you survive the initial pulmonary edema, 10 years from now you'll feel it coming back; you'll feel asthmatic, you'll be susceptible to bronchitis and pneumonia, etc. need i say more? Link to comment Share on other sites More sharing options...
akcapr Posted April 23, 2005 Author Share Posted April 23, 2005 how would i make nitric acid (w/ sulfuric acid kno3 method) without making that nasty stuff? Link to comment Share on other sites More sharing options...
budullewraagh Posted April 23, 2005 Share Posted April 23, 2005 you probably wouldnt... Link to comment Share on other sites More sharing options...
akcapr Posted April 23, 2005 Author Share Posted April 23, 2005 reallly? what about this http://www.totse.com/en/technology/science_technology/nitric.html and this http://www.skepticfiles.org/new/133doc.htm Link to comment Share on other sites More sharing options...
raivo Posted April 23, 2005 Share Posted April 23, 2005 it's scary and it will cause permanent respiratory failure. if you survive the initial pulmonary edema, 10 years from now you'll feel it coming back; you'll feel asthmatic, you'll be susceptible to bronchitis and pneumonia, etc. need i say more? May well be true but if you do not inhale it in remarkably quantities nothing will happen. Nitric anhydride is not that mysterious substance. Anyone who deals with nitric acid (like some artist for example) will inhale it occassionally. Nitirc acid, even diluted fumes, that gas. To make nitric acid safely you need good fume hood or have to synthesise it outside. You still have to be extra cautious not to inhale any fumes. Amount of H2SO4 has to be such that there would never be any dry nitrate. Otherwise you may decompose nitrate by heating and if you are especially unluky that process may decompose you. Link to comment Share on other sites More sharing options...
akcapr Posted April 23, 2005 Author Share Posted April 23, 2005 how would i get the right amount of h2so4 so theres no dry hydrate? Link to comment Share on other sites More sharing options...
budullewraagh Posted April 23, 2005 Share Posted April 23, 2005 akcapr, if you do that reaction cold with not very conc sulfuric acid, you could conceivably avoid the nitric anhydride problem. still, it's tricky and you will be left with a very impure product. raivo, nitric anhydride is just as bad as i described Link to comment Share on other sites More sharing options...
raivo Posted April 23, 2005 Share Posted April 23, 2005 I said "dry nitrate"! You just have to pour so much H2SO4 that all nitrate is wet and you have to watch it stays wet during the process. Otherwise you may decompose it by heating. Link to comment Share on other sites More sharing options...
akcapr Posted April 23, 2005 Author Share Posted April 23, 2005 so i would just add enough h2so4 too cover the nitrate and kkep it "wet"? Also, if i would heat would i heat it boiling or just below. Becasue the h2so4 could evaporate/ boil and the vapor would dissolve in the liquid and contaminate my acid, correct? and, even if i did get nitric anhydride couldnt i (safely) collect it and dissolve it in water? Link to comment Share on other sites More sharing options...
raivo Posted April 23, 2005 Share Posted April 23, 2005 H2SO4 will not evaporate below 200C (or even more). You have to heat over 100C, boiling water bath is not hot enough. Anhydride dissolves so well that you even can not put tube into water because liquid will instantly rise up by tube into your boiling flask. Experiment with few milliliters in test tube and ONLY if you get everything working go to greater amounts. Link to comment Share on other sites More sharing options...
budullewraagh Posted April 24, 2005 Share Posted April 24, 2005 yes, you could collect and dissolve your nitric anhydride, but again, it's bloody scary. if you HAVE to do this, use PTFE tubing; just about anything else will be oxidized h2so4 at high concs will fume the anhydride, SO3, a white gas. it makes you choke. i had a fun experience with that once. Link to comment Share on other sites More sharing options...
H2SO4 Posted April 24, 2005 Share Posted April 24, 2005 reallly? what about this http://www.totse.com/en/technology/science_technology/nitric.html Never listen to people on totse. There a bunch of dumbasses. Link to comment Share on other sites More sharing options...
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