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Author: Subject: Reduction of TiO2
sternman318
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[*] posted on 25-7-2011 at 15:10
Reduction of TiO2


Is it possible? I have not found any information at all

EDIT: In other words, aside from reduction with carbon, is it possibly to generate Ti(3+) from Titanium dioxide?

[Edited on 25-7-2011 by sternman318]
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DDTea
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[*] posted on 25-7-2011 at 16:04


I do this all the time at work using aluminum foil. The part that would be relevant to you:

~1 g TiO2 powder (usually >90%) is mixed with 10g Sodium Peroxide in a zirconium crucible. The mixture is fused over a Bunsen burner. The contents of the crucible are then leached with a mixture of hydrochloric and sulfuric acids (~20% acid total). This mixture is heated until it goes from a dark burgundy to an orange or even yellowish color to drive off any lingering sodium peroxide. The result liquid is transferred to a florence flask. The florence flask is kept under CO2 atmosphere by way of rubber tubing through a stopper. After purging for about a minute (really, it's good to go once you're confident that the atmosphere inside the flask is all CO2), add 3g of loosely-rolled aluminum foil. The flask is then placed on a hot plate at medium heat.
As the liquid heats up, the activation energy of the reaction will be overcome and the redox reaction will proceed. It is important not to have the heat too high or the CO2 flowing too violently, or you're guaranteed an eruption. The solution will go from the original orange (or yellow, depending on how long you heated it in the earlier step) to foggy grey to dark purple and finally, to transparent, light purple. At this point, the reduction is complete.

That's how we do it at least, but it's part of a larger method we use. You may have to adapt the procedure to your own needs.

[Edited on 7-26-11 by DDTea]




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sternman318
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[*] posted on 26-7-2011 at 09:41


Thanks DDTea!

Ive done some more reading and that, plus the procedure you gave, has given me the impression that TiO2 is not an easily reduced or altered compound! I will experiment with it, but I think it is unlikely that I will get any results. Too bad I dont have any sodium peroxide :P
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plante1999
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[*] posted on 28-7-2011 at 04:21


Ading sodium bisulfate to TiO2 and melting it , extracting the melt with metanol and than ad aluminium piece to precipitate Ti , witch can be used for making TiCl3.

TiO2 + 2NaHSO4 -) Na2SO4 + H2O + TiOSO4

If your are looking for TiTAnium look to my Youtube chanel.

http://www.youtube.com/user/plante1999?feature=mhee




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[*] posted on 14-10-2011 at 07:48


Would this work or not?
TiO<sub>2</sub> +4HCl = TiCl<sub>4</sub> + 2H<sub>2</sub>O
TiCl<sub>4</sub> + 2Mg = Ti + 2MgCl<sub>2</sub>?

Or doesnt Hydrochloric Acid react with Titanium Dioxide?




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plante1999
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[*] posted on 14-10-2011 at 08:09


no



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[*] posted on 14-10-2011 at 08:26


Could i substitute Sodium Bisulfate with Sulfuric Acid?



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plante1999
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[*] posted on 15-10-2011 at 08:10


Yes but it would be very dangerous, simply ad the rigth molar mass of sodium hydrogen carbonate (NaHCO3) and sulfuric acid (H2SO4) together to make sodium hydrogen sulfate (NaHSO4) but you can simply buy it as PH- for pool...



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[*] posted on 15-10-2011 at 08:18


what would make it dangerous with the acid? doesnt it react just my its self?



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