making sulfuric acid
Posted 4 October 2006 - 08:54 PM
Posted 5 October 2006 - 06:18 AM
Posted 5 October 2006 - 09:15 AM
Just pick up a few liters of this at the local hardware store and try it with your flowers of sulphur
Posted 9 October 2006 - 09:22 PM
Posted 10 October 2006 - 02:24 AM
Irgendwann fällt jede Mauer.
flammis acribus addictis:
voca me cim benedictis.
Posted 10 October 2006 - 08:37 AM
Air 21% Oxygen btw.
you must also take into account the temprature this reaction takes place at, the Sulpher actualy Burns with a blue flame.
the other stuff would probably oxidise it too if it were 1000+c
Posted 16 February 2007 - 05:16 AM
Posted 18 February 2007 - 05:21 PM
No…sulfur is an odd chemical being in the same periodic group as oxygen it is an oxidizer as in the classic reaction of powdered sulfur with iron filings(S + Fe + ->FeS). But it can also act as a reducer when exposed to a more powerful oxidizer such as KClO3 the reaction there being 2KClO3+3S->3SO2 + 2KCl. When you talk about a “secondary oxidizer” your probably thinking of the simplified explanation of black powder.
I thought sulfur helped the oxidiser activate as a secondary oxidiser
Posted 13 July 2007 - 11:34 AM
I just made my first concetrated sulfuric acid from car battery fluid.
I condacted the experiment outside but during the process and just about before the fumes turn white i sensed a weird burn in my nose and my throat and i started coughing for 5minutes.
I was 5-6m away from the boiling mixture !
Does anyone know what is the white smoke that come out when you boil H2SO4 ?
Is there a way to prevent the release of fumes into the atmosphere... by bubbling the fumes through a NaOH solution for example ?
I also threw some Copper into concentrated H2SO4 but i didnt get the blue color that you get when you add copper into HNO3.
Why so ? does anyone know ?
H2SO4 cant oxidise copper ?
Posted 13 July 2007 - 11:58 AM
the "fumes" were vaporised H2SO4 and other oxides of sulpher.
Odd that you should mention about the copper in H2SO4, I`ve never got it to react either, and was having a discussion with someone the other day that said he can do it, apparently Ariel oxygen in the acid will assist the reaction, however I`ve never managed to accomplish this either without either passing a current through it or using the Oxide of copper CuO and heating them together.
Posted 29 July 2007 - 02:03 AM
Posted 12 November 2007 - 11:16 PM
Has anyone tried the method where you layer equal parts Sulfur and KNO3 (or NaNO3) and bubble the gases through water? That seems to be a really simple way, provided you have the right labware, and doesn't require temperatures higher than what a basic alcohol lamp can provide.
I've tried that method before. I suspended a copper endcap with the NaNO3 and sulfur inside a 3-liter soda bottle (2-liter should work just as well). I put about a cup of water in the bottom. I used a propane torch to light the S/NaNO3 mixture a placed the endcap into the bottle and screwed the cap on tightly. The bottle filled up with SO2 and NO2 gas. After about two hours, I removed the liquid and tested the pH, getting somewhere around a 2.
Posted 18 April 2008 - 03:31 PM
so much time attacking a curious 13-year-old who wants to make H2S04, pfftt... If you were
a true chemist you would never even think about trying to tell somebody something is impossible,
you would extract joy from telling people how to do things, no matter how dangerous, the only
reason i can think of in terms of you people telling someone not to try and make sulfuric acid
is because you yourselves once tried to make up a batch but failed miserably, now in your worthless
freetime you spend your fatass days sitting on a computer typing away insults at people who want to
try and accomplish something that you failed at. You make me sick.
And for the record, making sulfuric acid is not that difficult at all, you simply need hydrogen
peroxide, and an appropriate setup where you can pump Sulfur Dioxide gas into the liquid, and you
will get sulfuric acid, the purity obtained depends on the purity of the Peroxide, but if you have
a low purity peroxide then you can increase the purity in many ways, my favorite way is by sparging.
Sulfuric acid was first synthesized in around 800ad i think, by a Persian chemist, if you morons can't
emulate a 1200 year old procedure in your own modern living-enviroment then i wouldn't even consider
your chemical-knowledge to be on par with a first grader. Stupid old men. But i forgot, if anybody tries
the experiments that you so miserably failed at all your life they will blow there eye out or cause
themselves immense damage, because they too are retards like yourselves, right? You just continue
sitting there living your fatass-days away by believing that your something, spitting out words that
are designed to try and make you look like you are actually something, something other than the nothing
that you are and always will be, unlike people who aren't afraid to try, and put there life at risk in
Furthermore, for the record, i have not tried this, but if you look at the MSDS for Sodium Bisulphate
you will see that according to it when Sodium Bisulphate is dissolved in Ethanol it disintegrates into
free Sulfuric acid and Sodium Sulfate.
Posted 19 April 2008 - 02:33 PM
Posted 19 April 2008 - 11:59 PM
The production of sulphuric as goes as it follows.
You first need [LaTeX Error: Syntax error] which you can get by:
[LaTeX Error: Syntax error] or
[LaTeX Error: Syntax error]
then you need [LaTeX Error: Syntax error] which you get from:
[LaTeX Error: Syntax error] in this case you need a catalyst which is [LaTeX Error: Syntax error]
and the third phase is getting the acid, but you do not directly put into reaction [LaTeX Error: Syntax error] with [LaTeX Error: Syntax error] due to loss of [LaTeX Error: Syntax error] (AFAIK). It goes like this:
[LaTeX Error: Syntax error] and then 'tame' it with water
[LaTeX Error: Syntax error] and this way [LaTeX Error: Syntax error] is highly concentrated.
Posted 29 April 2008 - 09:09 AM
Ok, back to sulfuric acid.
I heated acid from battery until it starts smell ( SO3 came out, right?), i tried it on some tissue and did not burn it (guess around 90%~), so i used some chunks of anhydrous magnesium sulfate in a liebig distiller which sits on top of a small flask with the acid and starts to heating it, hoped to extract the water so i dont lose the SO3. it didnt work out well, so i just did a test batch and added anhydrous magnesium sulfate directly to the acid. it did fuzzed a bit and i think its the water crystallisation of mgso4...
So now i ended up around 96%~ acid since it slightly burns tissue when cooled down. But how do i separate the MgSO4.7H2O??
Do i distill the mixture to like 330~C and bubble it through another batch of 90% acid?
or is there otherways.
it taste like, burning.
-Дафиoсo Иваноски [D]
Posted 19 September 2008 - 11:31 PM
Would someone elaborate the setup appature for bubbling SO2 in to H2O2?
How would you burn the sulfur and direct the sulfuric dioxide into H2O2?
Posted 20 September 2008 - 03:23 PM
Have an earlenmeyer flask or similar flask with your sulfur in it. You are then going to want an inlet for a small pencil torch to fit through the stopper and into the flask. Have an outlet of your tubing through the same stopper that will lead to another erlenmeyer flask (glass tubing needed here) and have your glass tubing going through the stopper and down toward the very bottom of your H2O2 sample. In this same stopper, you will need to have an outlet (second open hole in the stopper) incase some of the gas does not react for some reason like low concentration of H2O2 or similar.
What's the most important thing to learn in chemistry?
--Never lick the spoon.
0 user(s) are reading this topic
0 members, 0 guests, 0 anonymous users