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Alright /sci/ Chemist needing some help here, trying to make up some crystals due to the cool orange look. Something has gone wrong obviously, I think I know what it is but if anyone has any other ideas they would be appreciated.
I melted a Stainless Steel spoon in 1 mol/liter HCl. This produced a mixture of FeOH, CrOH and NiOH, evidenced by a green colour of the Cr3+ ions. After this I added Sodium Carbonate to precipitate the Chromium Hydroxide then filtered, the dried slurry was then but in a container and I added concentrated H2O2 and then filtered again producing a yellow solution, this, I believed, was Chromate in solution. As I believed that the Iron would be left behind and the chromate would filter through into the flask. however on acidifying no orange colour was observed. I now believe I may have made FeCl3 aswell as Chromate but I cannot be sure. It would make sense as the Iron Chloride would over power the colour change of Chromate regardless of pH due to higher concentration. Any thoughts ? If this is not the case, what have i made? Also is there anyway to remove the FeCl3 or should i restart the process instead using Sulfuric Acid?
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>>7800704
trichloro chromium III is supposedly green as a hydrate too, and certainly water stable. How does the carbonate work?
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>>7800704
Couldn't you try adding some silver nitrate to a sample portion see if any silver chromate falls out of solution?
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I believe upon the addition of sodium carbonate you also precipitated out Iron(II) carbonate,making with the other salts.
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Evaporate a portion of the solution off, and note the colour of the crystals. Mix them in with magnesium powder and heat them up with a blowtorch in a spoon. When the salt melts, if you are still alive then it's probably not dichromate.
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