Chemical Forums
Specialty Chemistry Forums => Citizen Chemist => Topic started by: science2000 on December 21, 2005, 11:20:56 PM
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Does anyone know of a way to reduce magnanese(IV) dioxide to manganese(II), besides adding HCl to it? What would it do if I attempted to dissolve it in dilute acetic acid?
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"MnO2 particles are unstable in anoxic environments, and will be reduced to dissolved Mn2+" (from Joceline Boucher's Ocean Studies 212 Lectures (http://bell.mma.edu/~jbouch/OS212Lecture16/tsld008.htm)).
If you can obtain an 'anoxic environment' - i.e. one with no oxygen...as in water with 0.00% dissolved oxygen - then that should do the trick nicely.
Two notes, is that anoxic water is probably hard to come by. I know you can get rid of most dissolved gases in liquids by freezing then melting, refreezing and melting, over and over...
Second thing is that "Mn2+ is thermodynamically unstable and can eventual oxidize to MnO2(s) in the presence of oxygen" (Same source). So if you have an anoxic aqueous environment that is open to the atmosphere, be prepared for an amount of reoxidation at the surface of the solution.
Best of luck!
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Acidify and add some reducing agent. Acetic acid will be probably too weak, I would rather try sulphuric with reducing agent like Fe2+, or some organic - like ascorbic acid.
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"MnO2 particles are unstable in anoxic environments, and will be reduced to dissolved Mn2+" (from Joceline Boucher's Ocean Studies 212 Lectures (http://bell.mma.edu/~jbouch/OS212Lecture16/tsld008.htm)).
If you can obtain an 'anoxic environment' - i.e. one with no oxygen...as in water with 0.00% dissolved oxygen - then that should do the trick nicely.
Not questioning the lectures, but are you sure it read the information correctly? Lack of oxygen is not enough for the reduction to take place - you need some kind of reductor to do the trick. I believe sea water contains lots of organic reducing agents (lots meaning many different, not very large quantities).
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Not questioning the lectures, but are you sure it read the information correctly? Lack of oxygen is not enough for the reduction to take place - you need some kind of reductor to do the trick. I believe sea water contains lots of organic reducing agents (lots meaning many different, not very large quantities).
Noted; thanks for the clarification!
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Theres nothing complicated here. Just add your MnO2 to a little hydrogen peroxide and any acid. Vinegar works fine. I found this out trying to get rid of those nasty stains KMnO4 leaves behind.
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Wouldn't the oxygen produced from the decomposing peroxide oxidize the water and prevent the reduction? I don't know if I understand.
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An acidified solution of H2O2 will cause the Mn to go all the way to the +2 oxidation state from +4. Make sure the acid is added first and little or no oxygen will evolve from the solution
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Keep in mind, that not all MnO2 reacts in this way easily. Strongly calcined MnO2 (very fine crystalline stuff) hardly dissolves and even in concentrated acids it hardly is capable to react. This is a problem with many oxides. When they are calcined and become crystalline, then they dissolve with great difficulty.
Freshly precipitated amorphous MnO2 indeed quickly dissolves in an acidified solution of H2O2, forming colorless Mn(2+) ions.
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What about MnO2 from a dry-cell battery? That's the stuff I'd use.
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What about MnO2 from a dry-cell battery? That's the stuff I'd use.
Probably that dissolves quite well, because it also needs to react easily in the battery. The only problem is that this MnO2 is terribly impure. Mostly it is mixed with carbon as far as I remember and it also contains a lot of other stuff (it is humid, due to some electrolyte).
A good source of MnO2 are ceramics and pottery supplies. These also have many other interesting metal salts (e.g. salt of Co, Fe, Cu, Ni, Bi, Cr).
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It must contain electrolyte to conduct electric current.
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It must contain electrolyte to conduct electric current.
Many times that electrolyte is sodium hydroxide.
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What are some impurities in battery MnO2? Any heavy metals or things I should be warned about?
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What are some impurities in battery MnO2? Any heavy metals or things I should be warned about?
An impurity could be Zn2+
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What are some impurities in battery MnO2? Any heavy metals or things I should be warned about?
I have already answered this, although without quoting so it was probably not clear. MnO2 in battery must be soaked with strong electrolyte to pesent as small resistance to current as possible. Depending on battery type this may be NaOH as jdurg wrote (in alkalic batteries) or some chloride solution in "standard" batteries (although I am not sure about details).
Note that not all types of batteries contain MnO2.
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As you may have concluded, MnO2 from batteries is not a very good source. It is impure, not all batteries contain this. It really is a hell of a mess to take it out (I once did this, it is TERRIBLE).
If you can find some at a ceramics and pottery shop, pick up that stuff. That is MUCH better and of quite good purity. They also carry MnCO3, which is even better. The MnCO3 usually contains a little Mn(III) and Mn(IV) species also, but with a few drops of H2O2 in acidic solution, you get easily rid of that.
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It seems the best way to get manganese without making a special order is buying "Clear Water" from Walmart or where ever, this stuff is used to clear organic material from fish tanks. It's a very dilute solution of potassium permanganate, like under 1%. But it's very pure. but still, for $2.50, a bottle is kinda expensive. Anyone know of a better version of this that's more concentrated?
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Pond supply usually sells big canisters of KMnO4, and its used in water softeners, so if you live in the country or know of a specialty hardware shop you should be able to get loads of the stuff.