Vanadium rapidshare

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Dow Futures 36, Nasdaq Futures 15, Russell Futures 2, Crude Oil Gold 1, Silver Vix CMC Crypto 1, FTSE 7, Nikkei 28, I was testing if a solution NaClO3 worked as an oxidant, but I got stuck on the first step. Perhaps the process is very slow, as blogfast25 said. I feel the presence of a funny smell, so something must be happening..

Yes, dissolving of ferrovanadium is very very slow. Ferrovanadium is known for its corrosion resistance and its strength for these reasons it is used in better quality tools. You could try adding some solution of NaOCl to the HCl just a few drops, no gas should escape and see if this helps. It also helps if you hit the ferrovanadium into small particles with a heavy hammer. Add the NaOCl very slowly, dropwise, while stirring.

Let us know if this helps. Beware of the nasty fumes from this boiling solution, do this outside. But in any case, patience will be needed. The only point is that if you use H2O2 that a brown peroxo complex is formed at low pH, which is not that unstable and it may require quite some time of boiling before all of it is destroyed this brown complex is much more stable than the similar deep blue chromium complex.

You must destroy this complex before adding a base, so keep on boiling until the dark redbrown color of the complex is gone and the solution has turned more yellow than brown. Thanks, woelen. And I'd forgotten how stable the perox complex can be.

Try heating and adding small amounts of H2O2 or HNO3, or do as woelen suggested using NaOCl; they are all based on getting small amounts of oxidiser into the solution but not too much at once. In all cases there will be some chlorine given off, so have good ventilation, and if you do heat it to boiling then there's the HCl fumes too.

If you heat that much then it is best to do it in a Erlenmeyer flask to keep in spray and act as a condenser. Does vanadium extract? I realise this is only useful if you can get ether but I's still like to know if the vanadium extracts too take your pick of vanadium's oxidation state, provided it's compatible with Fe III compounds.

Quote: Originally posted by unionised. That oxidation state is very strongly reducing. At very high pH around 14 , it mainly exists as colorless VO4 3- , the orthovanadate ion. When pH is lowered, this ion is hydrolyzed and species like VO2 OH 2 - are formed, which when crystallized from solution forms the metavanadate ion VO3 - , but the metavanadate ion probably is not a single simple ion, but more like a polymeric species [VO3 n] n- , very similar to the metaphosphates calgon.

When pH is reduced further, then further hydrolysis and condensation occurs, anionic species are formed with many vanadium atoms in it, with bridging O and OH groups. At pH in the range I left about an hour and a half on the magnetic stirrer, and not dissolved but the solution turned a green darker.

Today when I see the solution was blue as in the pic. Uploaded with ImageShack. When it reached the boiling point of the solution turned dark green again. I have a question: as the solution is evaporating, as it boils, can i add water to keep the solution? Yes, you can add water to maintain the volume. However the vanadium compounds formed have high solubilities, so some concentration will not cause problems. Ferrovanadium will function as a reducing agent, when the NaOCl had been consumed the vanadium in solution was being reduced, air can oxidise it.

Heat can also change the coordination sphere, changing the colour. Filter and today added sodium hypochlorite until the entire solution becomes a dark green. I read more carefully and really could not be V4O9 2 -. What is the justification for that color, then? However the solution is now dark green. I am boiling it to remove excess solvent because I have a small problem: the larger borosilicate glass I have is an mL Erlenmeyer, i need to work with small volumes. When I was adding sodium hypochlorite it formed an intense yellow color, which after dissolving turned the green.

And the foam on the topo turned yellow.. The upper dashed line marks where the stuff will oxidise water to O2, the lower dashed line where water is reduced to H2. Those reactions may be slow for various reasons, and concentrations as well as the formation of complexes can shift things, but this should give you a feel for what species may be present.

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