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Ferrous sulfate and copper sulfate suspension
Wanderer0:
I am to make a suspension of equal parts of Fe(II)SO4 and CuSO4 in equal proportion to a total of 4% (w/v)
I am making the suspension from ferrous sulfate heptahydrate and copper sulfate pentohydrate. The solvent will be water, but the final solution has to be basic pH~9.0.
How can I achieve stability of the ferrous sulphate in such pH?
I would ideally be able to retain stability for several hours.
Thanks in advance
Mitch:
Have you tried yet? Are you seeing the ferrous sulfate crash out?
chenbeier:
I think that will not work, at alcaline pH both will precipitate as hydroxide.
Wanderer0:
Yes, I did see precipitation. However I am not sure if Fe2+ has oxidased to Fe3+ and then reacted (it most probably has).
Is there any way of making a suspension of the two salts to render it stable for several hours?
If both salt hydrates were dissolved in water in equal amounts, would Fe2+ oxidise to Fe3+ or would it bind copper out of its sulfate?
Thank you very much for your help.
Wanderer0:
To clarify:
I need to spread FeSO4 and CuSO4 on an area that will be moist and contain organic compounds to observe the effect for several hours - up to 8.
I will obtain salts from their heptahydrate and pentahydrate forms.
Is there another solvent that would allow me to spread these salts on the test area and that would allow the active components (iron- ferrous and copper) to be released during the period?
I am basically observing the effects of these specific metals on an area, and they must be spread out in their sulphate form.
The test area will be moist, and there will be organic compounds on it, but this is not my interest.
Is there a better solvent or medium for distributing these salts on an even surface? Would a glycerol/aqueous/alcohol composition reduce Fe2+ oxidation?
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