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platedish29
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Quote: Originally posted by blogfast25  | | Quote: Originally posted by platedish29 | EDIT 2: yea ammonium iron phosphate is really grey-green. But when it was first prepared starting through iron hydroxide, thats green in color, and
phosphoric acid, it first dissolved completely and turn red-brown? Then uppon addition of ammonium hydroxide it turned to the final color.
[Edited on 19-3-2013 by platedish29] |
Take us through what you did precisely? |
Uh?! what? I successfully reproduced the experiment for a green variety of the phosphate, showed for that procedures. What I got after filtering
indicates that the original poster have gone tricky in his affairs, and that the blue variety must be more of a valuable than we may dink + I added
absolutely extra ammnonia so it may enhance the facts about stoichometry mentioned earlier. The solution smells ammonia but it still managed to yield
the very green product at the same time. Interesting is also the gelly green hydroxide changing into a brown colloidal suspension in the rist acid
addition showed how iron behaves in this particular situation...
nevethless practically showed everything about iron there is to be shown.
Thanks.
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rstar
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Can Ca(ClO)2 do it cleanly ?
"A tidy laboratory means a lazy chemist "
- Jöns Jacob Berzelius
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platedish29
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Do you mean calcium hypochlorite? I know calcium when added to iron III sulphate switches its colors from brown to red, an indicative it would somehow
contribute iron III formation. Is it commonly believed Fe3+ ions would survive alone in the solution? I mean, not sticking to something else?
Fe(HOH)3 + Fe(HOH)3 + HCl + H2O --> Fe2(OH)(HOH)5Cl + H2OH+
*****Dear rstar,
not into the assurance (that posts that it is you the owner) producing it too are clearly demeriting...but if I posed a photo of them in the internet?
I kicked a weird glitter which is so beautiful!
[Edited on 20-3-2013 by platedish29]
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elementcollector1
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| Quote: Originally posted by platedish29 |
Do you mean calcium hypochlorite? I know calcium when added to iron III sulphate switches its colors from brown to red, an indicative it would somehow
contribute iron III formation. Is it commonly believed Fe3+ ions would survive alone in the solution? I mean, not sticking to something else?
Fe(HOH)3 + Fe(HOH)3 + HCl + H2O --> Fe2(OH)(HOH)5Cl + H2OH+
*****Dear rstar,
not into the assurance posts that its you the owner producing it too are clearly demeriting if I posed a photo of them in the internet? I kicked weird
glitter which is so beautiful!
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This post is unacceptable.
Fe(OH)3, not Fe(HOH)3.
"Fe2(OH)(HOH)5Cl" and "H2OH" do not exist.
Compounds do not react with themselves, just put "2 Fe(OH)3" if that's what you meant.
Calcium ions, when added to iron sulfate, precipitate out *white* calcium sulfate, leaving an iron salt (likely also in the +3 oxidation state).
As for just Fe ions, not technically true, even if you used stoichiometry: some small amount of CaSO4 does dissolve in water.
As for the last paragraph... What? Are you high or something? Or just trolling?
Elements Collected:52/87
Latest Acquired: Cl
Next in Line: Nd
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platedish29
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| Quote: Originally posted by elementcollector1 | | Quote: Originally posted by platedish29 |
Do you mean calcium hypochlorite? I know calcium when added to iron III sulphate switches its colors from brown to red, an indicative it would somehow
contribute iron III formation. Is it commonly believed Fe3+ ions would survive alone in the solution? I mean, not sticking to something else?
Fe(HOH)3 + Fe(HOH)3 + HCl + H2O --> Fe2(OH)(HOH)5Cl + H2OH+
*****Dear rstar,
not into the assurance posts that its you the owner producing it too are clearly demeriting if I posed a photo of them in the internet? I kicked weird
glitter which is so beautiful!
|
This post is unacceptable.
Fe(OH)3, not Fe(HOH)3.
"Fe2(OH)(HOH)5Cl" and "H2OH" do not exist.
Compounds do not react with themselves, just put "2 Fe(OH)3" if that's what you meant.
Calcium ions, when added to iron sulfate, precipitate out *white* calcium sulfate, leaving an iron salt (likely also in the +3 oxidation state).
As for just Fe ions, not technically true, even if you used stoichiometry: some small amount of CaSO4 does dissolve in water.
As for the last paragraph... What? Are you high or something? Or just trolling? |
Nope sier!
I just want to post a photo of the glitter I hade made and steal the credits for the idea.
Sorry for that phrase it SOUNDS confusing, or I just have a very colloquial english!
yeah, Fe(HOH)3 Should be Fe(OH2)6(3+) or Fe(OH2)4(3+) not sure, sorry, just missed the notations.
[Edited on 20-3-2013 by platedish29]
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elementcollector1
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Trying to understand here: You made ferric ammonium phosphate, or some other compound, and it was glittery. You want to sell this compound, or
otherwise "steal the idea".
...I still don't get it.
Oh, you were referring to the hydrated Fe(H2O)x +3 ions. I thought you were referring to Fe(OH)3, the compound. My bad.
Elements Collected:52/87
Latest Acquired: Cl
Next in Line: Nd
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rstar
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@platedish : LOL
FeCl2 + Ca(ClO)2 = ?
"A tidy laboratory means a lazy chemist "
- Jöns Jacob Berzelius
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blogfast25
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Calcium hypochlorite will oxidise Fe(II) very easily but you end up with an almost inseparable mixture of FeCl3 and CaCl2: fairly useless.
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platedish29
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The cause of coloration was probably just caged iron hydroxides. High heat makes them dehydrate into a bid deal of orange/ black/ brown mass.
How's going dessication of your blue stuff rstar?
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rstar
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Ok, going to heat up that blue stuff today and post the results in this space . 
[
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[Edited on 21-3-2013 by rstar]
"A tidy laboratory means a lazy chemist "
- Jöns Jacob Berzelius
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rstar
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I guess FeCl2 can be easily oxidized to FeCl3 by KMnO4, but there will be a problem of separating the Mn++ ions
"A tidy laboratory means a lazy chemist "
- Jöns Jacob Berzelius
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blogfast25
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| Quote: Originally posted by rstar | | I guess FeCl2 can be easily oxidized to FeCl3 by KMnO4, but there will be a problem of separating the Mn++ ions |
Yes. That's why H2O2, HNO3 or Cl2 are preferred: they leave no cations that would have to be separated from the Fe3+ cations, a difficult task.
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rstar
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| Quote: Originally posted by blogfast25 | | Quote: Originally posted by rstar | | I guess FeCl2 can be easily oxidized to FeCl3 by KMnO4, but there will be a problem of separating the Mn++ ions |
Yes. That's why H2O2, HNO3 or Cl2 are preferred: they leave no cations that would have to be separated from the Fe3+ cations, a difficult task.
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HNO3 ? conc or dilute ? and can you give me the equation ?
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blogfast25
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Oxidation ‘half-reaction’:
Fe2+ === > Fe3+ + e-
Reduction (‘half-reaction’):
HNO3 + 3 H+ + 3 e- === > NO + 2 H2O
(Note: NO will oxidise spontaneously to NO2 when exposed to air oxygen [NO+ ½ O2 === > NO2], these are the dangerously brown toxic fumes you would
observe)
To balance the electrons:
3 Fe2+ + HNO3 + 3 H+ === > 3 Fe3+ + NO + 2 H2O
To obtain charge neutrality:
3 FeCl2 + HNO3 + 3 HCl === > 3 FeCl3 + NO + 2 H2O
Even 35 % HNO3 will do the trick. My experience is that the oxidation reaction seems to take place all at once, so you need quite a roomy container to
avoid the reagent mix to boil over: both gas and heat are produced when the reaction takes place. BEWARE of the toxic NO2: do this outside (standing
upwind) or under a fume hood. Cold mix the reagents in a very roomy beaker, then slowly heat while stirring constantly, until quite
suddenly the reaction will proceed and much NO/NO2 will be released and the solution will heat up a lot too.
After successful reaction, simmer the solution for some time to eliminate all traces of NO. You now have a relatively pure solution of FeCl3, which
depending on concentration will be yellow (very dilute) to reddish/brown (more concentrated).
[Edited on 22-3-2013 by blogfast25]
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