Guys..I need some guidelines on this...It's kind of urgent...
If we add V2O5, H2O and EDTA...will EDTA reduce V5+ to V4+
If so what should be the optimal ratio of these three compounds to achieve the same...
how to decide?Praxichys - 26-1-2017 at 10:32
I think EDTA will be awfully hard to oxidize. You're looking at elimination of CO2 as the pathway which I doubt unless perhaps you're melting them
together?
What are you looking for? A V(IV)-EDTA complex or VO2?DraconicAcid - 26-1-2017 at 10:46
If you want to make a vanadium EDTA complex, it's probably easiest to reduce the vanadium first. Many reducing agents will reduce V(V) to V(IV)
(sulphite in acidic solution may be the easiest).
A stronger reducing agent can turn it into vanadium(III), which forms an EDTA complex: http://www.journal.csj.jp/doi/pdf/10.1246/bcsj.64.2629
(They make the sodium salt using an ion exchange column, but I don't see why it wouldn't work to just use sodium carbonate in the the preparation in
the first place.)
ETA: mayko nicely posted the paper in the "requested papers" thread. Thanks, mayko! Reaction of V2O5 with EDTA salts will give vanadium(V)
complexes. My German is scheisslich, but apparently the reaction o f 11.7 g NH4VO3 and 29.2 g EDTA with 20 mL conc. NH3 and 700 mL water at low
temperature (ice bath?) over several hours gave 19 g of (NH4)3VO2(EDTA). You could probably substitute 9.1 g V2O5, dissolve it in the conc ammonia
first, then add the EDTA and water.
EATA: http://npl.csircentral.net/31/1/22.pdf says that vanadium(V) will oxidize EDTA, in 2 M sulphuric acid at 50 oC.
[Edited on 26-1-2017 by DraconicAcid]
[Edited on 26-1-2017 by DraconicAcid]jyoti1234321 - 30-1-2017 at 08:45
Thanks a lot..feel obliged..MeshPL - 31-1-2017 at 08:31
Anyone can acces most such papers via www.sci-hub.cc although the site is semi-legal...
If you want to acces that German article enter DOI number (10.1002/hlca.19650480716) or direct link and fill in captcha.
[Edited on 31-1-2017 by MeshPL]Melgar - 1-2-2017 at 21:17
