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Topic: mixed-oxide  (Read 4388 times)

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Offline samuelchan86

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mixed-oxide
« on: May 12, 2010, 10:21:37 PM »
normally to synthesized oxide particles in lab, a simple co-precipitation method using alkaline like NaOH or NH4OH to stoichiometrically precipitate out the oxides.. for example...

2Fe3+ + Fe2+ + 8OH- --> Fe3O4 + 4H2O

is it possible for me to... do the same with just other oxides.. for example.. copper oxides, tin oxides, zinc oxides... etc..
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Offline Mitch

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Re: mixed-oxide
« Reply #1 on: May 13, 2010, 09:07:56 AM »
Titanium is only +4, it doesn't have multiple oxidation states
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Offline sjb

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Re: mixed-oxide
« Reply #2 on: May 13, 2010, 09:21:47 AM »
Quote from: Mitch on May 13, 2010, 09:07:56 AM
Titanium is only +4, it doesn't have multiple oxidation states

Are you sure? What about TiCl3 - used in McMurry couplings, Nefs etc. Or do you just mean combined with oxygen - there are other oxides listed at http://en.wikipedia.org/w/index.php?title=Titanium_oxide&oldid=319697847 ?
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Offline samuelchan86

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Re: mixed-oxide
« Reply #3 on: May 13, 2010, 10:17:19 PM »
actually what i meant was... just by having a simple solution with the anion of my targeted oxide for example.. titanium dioxide... so the equation would be like...

Ti4+ + Zn2+ OH- --> ( TiO2-ZnO) + H2O

ignoring the stoichiometric no.

p/s: sorrry if there is any confusion above  :-[
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