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Author: Subject: Putting BaSO4 to use?
Antiswat
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[*] posted on 19-9-2021 at 00:56
Putting BaSO4 to use?


it seems you cant NaOH BaSO4 nor react it with any acid
barium salts can be very useful for reactions such as
(NH4)2SO4 + Ba(ClO4)2 = NH4ClO4 + BaSO4

and seperating iodate from iodide, as with bromate/bromide
but how does one get to recycle barium sulfate? is high reaction temperatures required, such as pyrotechnic reduction using coke or metal powders even?




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Amos
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[*] posted on 19-9-2021 at 06:09


Prolonged boiling/heating (I'm talking literal days) of barium sulfate in a solution of sodium carbonate slowly converts it back into barium carbonate. Even if the product material still contains remaining sulfate, due to barium sulfate's virtual insolubility it can still be partially reacted with acids to make new water soluble barium salts, and the remaining insoluble barium sulfate can be recycled once again.

Barium sulfate is also relatively easy to reduce with carbon at temperatures that can be accomplished by a furnace, fireplace, etc. The resulting barium sulfide is water-soluble and easily leached from the remaining sulfate and carbon, which again can be recycled. This can be used as a source of sulfide ion or simply converted back to carbonate using Na2CO3. The sodium sulfide coproduct is also useful, and while difficult to isolate from solution should be purer than much of the commercial material if handled properly.
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S.C. Wack
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[*] posted on 19-9-2021 at 10:26


"It has been found that barium sulfate can be decomposed to the extent of over 99 per cent in a single operation, by boiling for 1 hour (or 2 hours in the case of barite) with a strong solution containing at least fifteen times the theoretical amount of sodium carbonate."

https://doi.org/10.1021/ac50065a014




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Antiswat
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[*] posted on 22-10-2021 at 04:25


brilliant- i suppose lead sulfate may be dealt with in the same manner, which is really cool as used car batteries arent too hard to come by

when i read carbonate, i dont see why hydroxide wouldnt work same way? and people will say, thats super corrosive- well stainless steel 316 only corrodes about 1mm a year handling boiling, liquid, NaOH

could we maybe assume boiling hydroxide would work better? very interesting turning useless stuff into useful stuff, calcium sulfate is also a major waste product around the world, its ridiculous the amounts of chemicals we pay money to bury in the ground.




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S.C. Wack
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[*] posted on 22-10-2021 at 16:59


Dead car batteries have liitle sulfate in them, as electrode failure is typically mechanical not chemical...I wouldn't count on recovering baryta, but it would be an interesting experiment.



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[*] posted on 23-10-2021 at 04:20


Quote: Originally posted by Antiswat  


when i read carbonate, i dont see why hydroxide wouldnt work same way?

could we maybe assume boiling hydroxide would work better? .

No
Barium hydroxide is soluble in water.
Barium carbonate isn't.
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[*] posted on 24-10-2021 at 18:24


Quote: Originally posted by S.C. Wack  
Dead car batteries have liitle sulfate in them, as electrode failure is typically mechanical not chemical...I wouldn't count on recovering baryta, but it would be an interesting experiment.


From the few car batteries I have dumpster dived, they often give 4 to 7 V.
So, the serial connection between the cells is ok. There is of course some mechanical damage (The grid is fragile or breaky).
If you attempt to charge them, the voltage goes up. Once you stop charging them, the voltage drops quickly on its own. In a few days, it will return to 4 to 7 V.

The good news is that the cathode has some PbO2, which is a good oxidizer.
You can also reduce it with charcoal easily and have some lead.




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[*] posted on 25-10-2021 at 08:04


Metals like stainless steel are pretty impervious to alkali hydroxides and carbonates.
Aluminum on the other hand ...
Stainless big weakness is halides.
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