[hanson]
FeCl2 + HCl + 1/2 H2O2 ----> FeCl3 + H2O
....c) add a Cl2/water solution to the FeCl2 soln,
which you make on the side from diluted
2 HCl + H2O2 ---> Cl2 + 2 H2O
2 FeCl2 + Cl2 ----> 2 FeCl3
[Farooq]
> 2 HCl + H2O2 ---> Cl2 + 2 H2O
> Does this actually occur?
>
[Hanson]
It seems so to me, as long as HCl is in stochiometric excess
over H2O2, else you'd get HClOx, where x = 1 to 4.
But even then it wouldn't matter, because HClOx, with Fe2+ and
Fe present, will be reduced to the Cl- in the oxidized FeCl3.
[Farooq]
I think Hydrogen peroxide is unable to oxidize HCl to OCl- or
chlorite, or perchlorate ion, keeping in mind the chemical properties
of H2O2 and electrode potentials of hydrogen peroxide.
Hypochlorite ion is more powerful oxidizing agent than peroxide ion ,
and both are not compatable with each other, the final reaction being
OCl- +H2O2--> O2 +Cl +H2O. I remember this reaction produces light
when a suitable dye is used.
[hanson]
Interesting. When I get back into the labs, I'll asked them to play
with your assertion and find out. Don't hold your breath though.
It'll take time.
-------------
I finally got to it and it turned out that both of us were right.
Here are the quick and dirty fly by nite experiments I did.
2 HCl + H2O2 --//--> Cl2 + 2 H2O
Mix of ~10% HCl/H2O + ~10% w/w H2O2/H2O both ~ 50 ml each
stayed colorless. --- Even upon heating to 50-60°C still colorless
and a little foaming of colorless bubbles evolved. No smell: --> O2
but no trace of any chlorine smell or yellow fumes.
***** Just as Farooq predicted ****
FeCl2 + HCl + 1/2 H2O2 ----> FeCl3 + H2O
Mix of ~ 50 ml each ~10% HCl/H2O with 1/2 tsp FeCl2 turned
light green and upon addition of ~10% w/w H2O2/H2O the solution
turned immediately deep yellow indicating Fe2+ ---> Fe3+ oxidation.
***** Just as hanson said it would ****
Farooq, thanks a million! You showed me something.
You are a good man, dude.
hanson
-------------
Hanson,
You would not believe it, just yesterday I was thinking of asking you
whether you checked the very same reaction mentioned above but I
thought that you must have long forgotten it.
I was more interested in the chemiluminescent reaction between
hypochlorite ion and hydrogen peroxide in presence of a suitable dye,
you mentioned that you would check that reaction also, since you seem
to have an excellent background in organic chemistry, you might be
able make a better dye or something.
BTW, I am not very active in the lab any more ....for decades now.
But, I still have extremely fond memories from working on the
bench, orchestrating & mastering the "play of matter and molecules".
So, these days, I mostly post from and during my long, long boring
flights.... while the interns and juniors tell me about the laughs they have
with other use-net morons... on this same handle.....and in concert,
I just returned from a long flight, probably having traveled some 5-6
miles over your domicile to/fro my destination north of the Karakoram-
Pamir.....engaging with you subconsciously on a bio-el resonance due
to the rather "small" 1/r^2 differential of induction intensity.
Take care man,
hanson
>Mix of ~10% HCl/H2O + ~10% w/w H2O2/H2O both ~ 50 ml each
>stayed colorless. --- Even upon heating to 50-60°C still colorless
>and a little foaming of colorless bubbles evolved. No smell: --> O2
>but no trace of any chlorine smell or yellow fumes.
> ***** Just as Farooq predicted ****
People have the tendency to think that H2O2 is a great oxidizing agent ... It
is ... but its relative greatness is many times higher in basic solution than
acidic solutions ...
The half cell reaction is
H2O2 = O2 + 2H+ +2e E = -0.682
Be seeing you
In the Village
Number 6