Acuarey
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Registered: 7-10-2015
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How dangerous is it? How should it be done?
Ok, after doing this one:
http://www.sciencemadness.org/talk/viewthread.php?tid=63872#...
I´ve managed to get my hand into some H2SO4(Cars´batteries)
CaO(Any contruction site)
Na2CO3
(Decomposing Sodium bicarbonate{NaHCO3}and water[Bye, bye CO2])
And I´d like to mix them up to get CaCO3 and CaSO4
CaO + 2H2O --> Ca(OH)2
Ca(OH)2 + H2SO4 --> CaSO4 + 2H2O
Ca(OH)2 + Na2CO3 --> CaCO3 + 2NaOH
So, how can I do it?
Which equipment would I need?
How can I handle sulfuric acid? Where can I place it for the reaction?
Where should I do it?
What if it goes wrong?
How do I get rid of of the NaOH Ill get?
Just add water, boil, add water and boil... Over and over, since the two salts Ill be getting are insoluble?
Any suggestions?
Sorry for the bad english and the bad Chemestry(Still in High school)
Thx for the help :3
[Edited on 9-10-2015 by Acuarey]
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Hawkguy
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Just use glass to handle the acid. Always wear PPE, and don't let the CO2 produced foam the Acid all over your kitchen. Huh congrats on finding the
Calcium Oxide, if I were you I would personally save it for something better.
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j_sum1
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Check your stoichiometry.
Reaction 1 is unbalanced. No H2 produced.
Reaction 2 is a simple acid base reaction. Your problem will be getting your Ca(OH)2 to dissolve -- it is not really soluble. (Seems this particular
question has cropped up a dozen times in the last 48 hours.) If it is dissolved you will get a precipitate -- probably very fine and a pain to try to
separate. But in principle, it should work. If you just add dilute H2SO4 to your calcium hydroxide powder then you will need excess acid and you
will need to wash thoroughly to get your CaSO4. Do-able, but I wonder why. Just buy some plaster of Paris and be done with it. I would not waste
the sulfuric acid.
Reaction 3 -- again this seems to have come up quite a bit lately. It should work, but again you have fun with solubilities and separation. neither
of your two calcium compounds are particularly soluble. I am not sure off the top of my head which is more soluble and whether you will get a
precipitate. It will be pH dependent in both cases. There are easier ways of getting calcium carbonate.
Getting CaO from a building site? I would not vouch for its purity in any way. Building materials are what they are to achieve the functionality
they need. there is no reason for manufacturers to aim for purity. There is likely to be all manner of crap in there.
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bluamine
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Quote: Originally posted by Acuarey  | Ok, after doing this one:
http://www.sciencemadness.org/talk/viewthread.php?tid=63872#...
I´ve managed to get my hand into some H2SO4(Cars´batteries)
CaO(Any contruction site)
Na2CO3
(Decomposing Sodium bicarbonate{NaHCO3}and water[Bye, bye CO2])
And I´d like to mix them up to get CaCO3 and CaSO4
CaO + 2H2O --> Ca(OH)2 + H2
Ca(OH)2 + H2SO4 --> CaSO4 + 2H2O
Ca(OH)2 + Na2CO3 --> CaCO3 + 2NaOH
So, how can I do it?
Which equipment would I need?
How can I handle sulfuric acid? Where can I place it for the reaction?
Where should I do it?
What if it goes wrong?
How do I get rid of of the NaOH Ill get?
Just add water, boil, add water and boil... Over and over, since the two salts Ill be getting are insoluble?
Any suggestions?
Sorry for the bad english and the bad Chemestry(Still in High school)
Thx for the help :3 |
It is not so dangerous to do that.. but Calcium oxide is hard to get & it is not practical because you'll get a rid of NaOH
The dangerous thing is that you may think you need a concentrated sulphuric acid so keep away of this please.
You should instead try to make your mercury cell.. I am trying to do that too. Otherwise you can buy NaOH. I wish good luck for you, & hope to
hear from you soon..
Reagards Amine
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bluamine
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| Quote: Originally posted by Hawkguy | Just use glass to handle the acid. Always wear PPE, and don't let the CO2 produced foam the Acid all over your kitchen. Huh congrats on finding the
Calcium Oxide, if I were you I would personally save it for something better.
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He just has to do that outdoor, or in an open & ventilated area, which doesn't contain any thing can react whith the acid.
Also, he has to wear a kind of safety glasses, of course with gloves, & may be a gas mask.. the last thing to mention, that he should make a
diluted sodium bicarbonate solution as a precaution..
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ave369
Eastern European Lady of Mad Science
Posts: 596
Registered: 8-7-2015
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Don't see why concentrated sulfuric acid might be required. Ordinary Bat will do. It is somewhat corrosive, but its main danger is not burned flesh:
it's ruined pants. Every little drop of battery acid that ends up on your clothes will eventually turn into a big hole. The only treatment is washing
your clothes in washing soda immediately after exposure.
Smells like ammonia....
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