aqua regia (without hydrochloric acid)

[butcher]

This seems to me to be a waste of a good mind; He seems intelligent, just think if he spent his time on something practical, and for good.

Acids so concentrated, high oxidizers, and metals, and the chemistry was interesting to read, I agree with Harold, GSP, and Lou, this guy is going to get someone hurt, seriously.

Recovery and refining is dangerous enough, with the processes we use, but some of the processes he was speaking of sounds like a disaster waiting to happen.

Well He had plenty of chances to contribute on the forum, even after repeated warnings; he was bent on posting the dangerous babbling chemistry.
Thank goodness we have moderators who catch these dangers and eliminate them before a member is dismembered or killed by trying some of the things he posted.

We could come up with most anything in theory, but in practice, none of our theory may work.

 

[eeTHr]

One other interesting aspect of this guy---it would appear that he has never actually tried any of what he suggests....

 

[Lou]

That is my chief issue with him. He's a smart fellow but his armchair speculation that he spreads as gospel can/will lead someone to disaster.

 

[shinedown389]

Good job Harold, and well said. I got a head apin just read that stuff. lol

 

[Anonymous]

I have a history with him somehow,but I don't remember.I will have do some research tomorrow and figure out how I know him(his name).

 

[butcher]

I have been reading where they have used MnO2 (manganese dioxide) and NaCl table salt (sodium chloride) and few drops of sulfuric acid in mining Ore to dissolve gold into solution.

well the NaCl and sulfuric acid makes HCl (hydrchloric acid) so to dissolve gold the manganese dioxide acts as an oxidizer generating chlorine gas in solution this chlorine is what dissolves the gold.

generating chlorine gas

MnO2 + 4HCl --> MnCl2 + Cl2 (gas) + 2H20

MnO2 (Manganese dioxide) is in alkaline battery's the black stuff that looks like grafite carbon, the white/greenish material wraped in paper membrane of battery core is zink salts, alkaline usually used is KOH (pottasium hydroxide).

I do not know how reactive the manganese dioxide would be in this equation so all precautions should be taken if expieriments are done.

 

[notch]

It appears that Manganese dioxide and sulfuric acid is used to process Molybdenite rather than gold from what I found about the reaction. That reaction appears to pretty safe. Mixing concentrated sulfuric acid with Potassium Permanganate however gives Mn2O7, which can be explosive! Not safe!

Don't try it. Contact with organic materials causes a violent reaction. I have in the past. It's a very dangerous mix.

 

[butcher]

Thanks for the warning Notch on the danger, but can you clarify your answer, which reaction you have tried the maganese oxide and HCL (a common way to geneate chlorine gas), or the permanganate and sulfric acid?


I feel most anything with permanganate would pose dangers it is such a powerful oxidizer, and mixed with organics and concentrated sulfuric sounds like a recipee for explosives.

 

[notch]

Thanks for the warning Notch on the danger, but can you clarify your answer, which reaction you have tried the maganese oxide and HCL (a common way to geneate chlorine gas), or the permanganate and sulfric acid?


I feel most anything with permanganate would pose dangers it is such a powerful oxidizer, and mixed with organics and concentrated sulfuric sounds like a recipee for explosives.

I was referring to the Permanganate in Sulfuric Acid. I won't go into any details but, yes, it will explode in only a few seconds, depending on the type of Organic compound. I wouldn't want to be standing there. Even a small pop will spray it all over the work area and anyone standing close. It will literally set you on fire, with you and your clothing being the fuel.

 

[butcher]

Thanks Notch, something I have found out about the MnO2 (manganese dioxide ) in batteries is that as the cell is used it forms an manganese hydroxide, this could be converted back to the dioxide but takes several steps to do this, also the MnO2 is mixed with carbon or grafite and this could be filtered out from an MnCl2 solution as on of the steps to convert MnO(OH) back into MnO2, this seems like a lot of trouble,

I now need get back to my study to find out if the manganese hydroxide could be used directly to generate chlorine gas, (old battery's would make finding reagent easier) as this gas if properly handled can be very useful in recovery or refining, (but like a most other things if improperly handled can also be very dangerous), but here again the carbon would most likely grind this notion to a halt, looks like as usual there are no shortcuts to doing things the right way, maybe one day I will learn.