| Pages:
1
2 |
budullewraagh
Hazard to Others
Posts: 168
Registered: 1-8-2004
Location: new york
Member Is Offline
Mood: Aliphatic
|
|
i could imagine that it was released as either HCl or Cl2
|
|
|
mick
Hazard to Others
Posts: 338
Registered: 3-10-2003
Member Is Offline
Mood: No Mood
|
|
KMnO4
About what you can do with KMnO4
This is from a book first published in 1931 and this is from my1961 reprint
In solution it is the most powerful common oxisising agent available.
The substances oxidised include nascent hydrogen, unsaturated hydrocarbons, ammonia (only slowly in solution) and ammonium salts, nitrites, hydrogen
sulpide, sulphur dioxide, sulphites, thiosulphates, phosphine, phosphites, hypophosphites, phosphorous acid, hydrochloric acid, chlorides, hydrobromic
acid and hydroiodic acid and their salts, arsenites, organic matter of most kind, the lower salts of most metals, such as ferrous, cuprous, manganous,
titanous, stannous salts and metals.
It has then got a page and a half on how to work out the relevant equation for what you want to do eg if you are doing it in suphuric acid, write down
the oxidising equation for what you are doing and subtract this equation.
The other thing is, if its fairly pure, you can use it to find out the purity of some things that can be oxidised in water because it is self
indicating, the colour changes or MnO2 is formed.
Mick
|
|
|
JohnWW
International Hazard
Posts: 2849
Registered: 27-7-2004
Location: New Zealand
Member Is Offline
Mood: No Mood
|
|
More powerful (but mostly more expensive except the last group) oxidizing agents in aqueous solution than MnO4- are:
alkali metal salts of plumbate(IV), PbO3--, and bismuthate(V), BiO3-; acid solutions of Ce(IV) salts e.g. Ce(NO3)4; and alkaline solutions of Cl2,
NaOCl and NaClO2. These are capable of oxidizing Mn(II) to MnO4-, and most of them can also oxidize Fe(III) to FeO4--.
John W.
|
|
|
tom haggen
Hazard to Others
Posts: 488
Registered: 29-11-2003
Location: PNW
Member Is Offline
Mood: a better mood
|
|
Just exactly how safe is it to mix KMn04 with concentrated sulphuric acid?
[Edited on 18-8-2004 by tom haggen]
N/A
|
|
|
budullewraagh
Hazard to Others
Posts: 168
Registered: 1-8-2004
Location: new york
Member Is Offline
Mood: Aliphatic
|
|
i'd think it would be not so dangerous as long as you added the KMnO4 slowly
|
|
|
Twospoons
International Hazard
Posts: 1282
Registered: 26-7-2004
Location: Middle Earth
Member Is Offline
Mood: A trace of hope...
|
|
If you see green crystals forming you're in trouble - I've been told they're extremely unstable.
(Oh Joy! Primary explosive in a jar of sulphuric acid!)
|
|
|
JohnWW
International Hazard
Posts: 2849
Registered: 27-7-2004
Location: New Zealand
Member Is Offline
Mood: No Mood
|
|
At low temperatures, the product would be Mn2O7, as a dark oily liquid.
John W.
|
|
|
unionised
International Hazard
Posts: 5103
Registered: 1-11-2003
Location: UK
Member Is Offline
Mood: No Mood
|
|
Question "Just exactly how safe is it to mix KMn04 with concentrated sulphuric acid?"
Answer; not safe.
|
|
|
Hang-Man
Hazard to Self
Posts: 70
Registered: 16-1-2004
Location: Canada
Member Is Offline
Mood: Wasted
|
|
I seem to remember reading somewhere that KMNO4 + H2SO4 produces O3 among other nasty things.
|
|
|
blazter
Hazard to Self
Posts: 71
Registered: 3-9-2002
Member Is Offline
Mood: No Mood
|
|
I have a friend who has a well that produces what they call "sulfur water". Based on the smell, I think it contains a small amount of H2S
dissolved in it. The odor is pretty strong, like fresh shit sitting in the sun. I was talking with him and he mentioned seeing a treatment system
that used a pink or purple liquid that gets injected at the water pump. Knowing that KMnO4 has that characteristic color in solution, and having a
vague idea that it might oxidize the H2S I plan on making up a dilute solution and adding a couple drops to a gallon of that water. Titration should
be simple if it does react since the pink will become clear.
The only possible problem is that if it isn't H2S or if the KMnO4 doesn't oxidize it. Anyone else ever experience this "sulfur
water" or can verify that it is H2S? Better yet, will adding dilute KMnO4 actually do something, or do I just have a wild hair up my ass?
|
|
|
budullewraagh
Hazard to Others
Posts: 168
Registered: 1-8-2004
Location: new york
Member Is Offline
Mood: Aliphatic
|
|
last i checked, conc H2SO4+2KMnO4 -> HMnO4+K2SO4
|
|
|
chemoleo
Biochemicus Energeticus
Posts: 3005
Registered: 23-7-2003
Location: England Germany
Member Is Offline
Mood: crystalline
|
|
JohnWW, you mentioned organic permanganyl esters.
Do you have more details? I always wondered whether such esters exist, and u seem to have heard about them. Please post details on a well-known/stable
one if you have it (partiuclalry if it is easily made - then it probably warrants its own thread anyway) - thanks 
[Edited on 21-8-2004 by chemoleo]
Never Stop to Begin, and Never Begin to Stop...
Tolerance is good. But not with the intolerant! (Wilhelm Busch)
|
|
|
S.C. Wack
bibliomaster
Posts: 2419
Registered: 7-5-2004
Location: Cornworld, Central USA
Member Is Offline
Mood: Enhanced
|
|
blazter, I don't know about any injection systems, but I get my KMnO4 for "greensand" filter regeneration. This sort of system takes
out the H2S by precipitating it as S.
I've heard that an O2/O3 mix can be made from sulfuric and KMnO4, too. Probably not much.
The reaction between KMnO4 and H2SO4 is dependant on conditions. How concentrated, whats added to what, the temp, etc. There are several possibilities
and products.
Adding hot sulfuric to the solid will just give sulfates, water, and O.
Adding the solid to conc. H2SO4 can give Mn2O7. This may not be something that you want to make much of.
|
|
|
JohnWW
International Hazard
Posts: 2849
Registered: 27-7-2004
Location: New Zealand
Member Is Offline
Mood: No Mood
|
|
| Quote: | Originally posted by chemoleo
JohnWW, you mentioned organic permanganyl esters.
Do you have more details? I always wondered whether such esters exist, and u seem to have heard about them. Please post details on a well-known/stable
one if you have it (partiuclalry if it is easily made - then it probably warrants its own thread anyway) - thanks
[Edited on 21-8-2004 by chemoleo] |
I think I said that organic permanganate esters may possibly exist, not that they do for a fact. Like chromate, perchlorate and nitrate esters, they
would be highly explosive, if they could be made. It would be possible to make them only at low temperatures, by the reaction of alcohols with Mn2O7
or with HMnO4, plus a small amount of H2SO4. Like those other esters, they would depend for their formation on their auto-decomposition into explosion
products being kinetically slow at low temperatures, although highly thermodynamically favorable.
John W.
|
|
|
| Pages:
1
2 |
![[*]](images/xpblue/default_icon.gif){kind=icon}
