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Author: Subject: Preparation of titanium nanoparticles
ninhydric1
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[*] posted on 22-11-2017 at 21:34
Preparation of titanium nanoparticles


I have recently taken an interest in nanoparticles and their versatile applications and developments. Preparing silver nanoparticles is well documented but I wanted to prepare a more obscure metal nanoparticle. During my research, I happened to stumble on an article describing the synthesis of titanium dioxide nanoparticles and another article describing its uses and possible improvements (both articles attached below).

The article about TiO2 nanoparticles states that by adding TiCl4 to chilled distilled water and then adding urea will create a colloid of TiO2 in water. From what I understand, TiCl4 is hydrolyzed to TiO2 and the urea somehow complexes with the TiO2 to form a suspension. Is this the correct mechanism and will it work?

Upon researching the synthesis of TiCl4, I came upon a synthesis developed by plante1999, as quoted below:

Quote: Originally posted by plante1999  
Simply melt pyrosulphate with the ore in presence of NaCl, it will make HCl + TiCl4

Sources: my own work

In fact I already made most inorganic titanium compounds and many organic ones, I think that I have some(a lot) knowledge in this field.

[Edited on 17-5-2012 by plante1999]

[Edited on 17-5-2012 by plante1999]


Has anyone tried this (besides plante1999 himself) and can confirm the reaction occurs? If it does, is a paint can an acceptable reaction vessel?

(Anders Hoveland was an interesting member too)



Attachment: tinanoparticles.pdf (531kB)
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Attachment: Nanoparticles.pdf.pdf (2.3MB)
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[Edited on 11-23-2017 by ninhydric1]




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VSEPR_VOID
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[*] posted on 25-11-2017 at 03:57


I wonder if you could use them for solar cells. I remember NerdRage had a video about producing simple solar cells using TiO2, carbon, and raspberries. You should try it if you can produce enough nano particles.

https://www.youtube.com/watch?v=WHTbw5jy6qU




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ninhydric1
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[*] posted on 25-11-2017 at 09:43


TiO2 is often used in photocatalyzing specific reactions so it would make sense that it is an experimental component for solar cells.



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[*] posted on 25-11-2017 at 12:21


TiO2 mp is 1840 C

Na2S2O7 decomposes starting at 400 C

Pardon my incredulity but I think we're going to need to see some extraordinary evidence to believe these compounds are in the same melt




[Edited on 04-20-1969 by clearly_not_atara]
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[*] posted on 25-11-2017 at 13:26


I assume plante1999 meant that the reaction takes place when Na2S2O7 starts melting. I'm pretty sure I won't be able to reach temperatures up to 1840 degrees Celsius. It would be best for him to clarify, but he hasn't been online for a while.



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