| Pages:
1
2 |
blogfast25
International Hazard
Posts: 10562
Registered: 3-2-2008
Location: Neverland
Member Is Offline
Mood: No Mood
|
|
Hmmm.. I seriously wonder if such a Ti(SO4)2 can exist, and how it would be synthesised. Surely a Ti<sup>4+</sup> must have too strong a
central electric field to be able to exist in watery solution and would hydrolyse immediately?
[Edited on 1-10-2013 by blogfast25]
|
|
|
watson.fawkes
International Hazard
Posts: 2793
Registered: 16-8-2008
Member Is Offline
Mood: No Mood
|
|
Here's what Kirk-Othmer
says.
| Quote: | | Titanium(IV) sulfate can be prepared by the reaction if titanium tetrachloride with sulfur trioxide dissolved in sulfuryl chloride. [...] It is
readily hydrolyzed by moisture and, when heated, changes first to titanyl sulfate [...] and then to TiO2. |
|
|
|
blogfast25
International Hazard
Posts: 10562
Registered: 3-2-2008
Location: Neverland
Member Is Offline
Mood: No Mood
|
|
I was thinking of treating anhydrous TiF4 with anhydrous H2SO4 as a displacement reaction.
One thing's for sure: there are other references to Ti(SO4)2 but so far I haven't found any references to its properties. One mentions a nonahydrate
but that's GOTTA be nonsense.
Hydrothermal hydrolysis of titanyl sulphate is the basis of the 'sulphate process' for the production of TiO2 from Ilmenite and H2SO4.
And I remain deeply sceptical re the cited green colour: not a single (IV) compound in Group IV b is coloured.
[Edited on 2-10-2013 by blogfast25]
|
|
|
Chemosynthetic
Harmless
Posts: 19
Registered: 12-11-2013
Member Is Offline
Mood: No Mood
|
|
Well, I lost my old password, so I haven't been able to post, but I was hoping plante1999 would share more of his experiences about the pyrosulfate,
titanium dioxide, and sodium chloride method of TiCl4 production. I am curious if he could offer advice on estimation of the mixed melting point, or
how he came to conclusion that TiCl4 was produced rather than the liberation of SO3 from the pyrosulfate, which decomposes near its MP.
http://www.inorganicventures.com/advice/fusion-titanium-diox...
I just have not found a reference to this technique and would like to try it, but would prefer a citation of some kind or more info first.
Edit- spoke too soon:
www.sciencemadness.org/talk/viewthread.php?tid=20234
[Edited on 12-11-2013 by Chemosynthetic]
|
|
|
bismuthate
National Hazard
Posts: 803
Registered: 28-9-2013
Location: the island of stability
Member Is Offline
Mood: self reacting
|
|
Would Al or Ga trichlorides (or monochlorides) react with TiO2 to form TiCl4?
[Edited on 5-12-2013 by bismuthate]
|
|
|
blogfast25
International Hazard
Posts: 10562
Registered: 3-2-2008
Location: Neverland
Member Is Offline
Mood: No Mood
|
|
Not at RT, no. TiO2 has a very high Enthalpy of Formation, it is, in other words, very, very stable. At high temperatures and with continuous removal
of the TiCl4 it might be possible:
4 AlCl3 + 3 TiO2 < === > 2 Al2O3 + 3 TiCl4 would be pulled to the right if you distilled off the TiCl4, continuously. Not for the faint of
heart...
Neither AlCl nor GaCl are particularly stable or practical to work with.
|
|
|
NAILA2
Harmless
Posts: 1
Registered: 17-11-2015
Member Is Offline
Mood: No Mood
|
|
Anyone please send to paper or journal about synthesis of titanium tetracloride ?
|
|
|
blogfast25
International Hazard
Posts: 10562
Registered: 3-2-2008
Location: Neverland
Member Is Offline
Mood: No Mood
|
|
Look up 'Kroll Process'.
|
|
|
Chemi Pharma
Hazard to Others
Posts: 349
Registered: 5-5-2016
Location: Latin America
Member Is Offline
Mood: Quarantined
|
|
I found a patent that uses any titanium salt to produce an alkali chlorotitanate that are thermally decomposed at relative low temperatures producing
TICl4. Probably a easier method of synthesis, I guess. I have attached the patent below.
Attachment: Titanium tetrachloride from alkali chlorotitanates.PDF (475kB)
This file has been downloaded 401 times
|
|
|
rockyit98
Hazard to Others
Posts: 283
Registered: 12-4-2019
Location: The Known Universe
Member Is Offline
Mood: no mood is a good mood
|
|
4NaCl + 2SiO2 +2CaSO4+TiO2 ------> TiCl4 + 2CaSiO3 + 2Na2SO4 Temp>1000C
or
2CaCl2 + 2SiO2 +TiO2 ------> TiCl4 + 2CaSiO3 Temp>1000C
second one is better, no CaTio3
|
|
|
| Pages:
1
2 |
![[*]](images/xpblue/default_icon.gif){kind=icon}
