By the way, worth mentioning is to always roll out as thin as possible the alloy button or metal and make a "cone" before digesting with acids, as this really helps the precious metals left to stay together instead of having just a fine powder laying all about.
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Bullion.Forum
Non-Chemical Iodine/Iodide & Rhodium
- Thread starter Comanche
- Start date
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My deepest apologies. I know better than to post when I am give out and not half thinking! 
In the first place, I don't always do everything a certain way! :lol: That was a really dumb statement! :lol:
What I did inadvertently, was get into some methods done on just a small assay type scale, not a larger type scale that I would use to extract and separate the precious metals out of. :wink:
I let this topic get way out in left field from what I originally intended it to do. Like I did say, this topic was only for the express purpose of discovering if any of you knew if Iodine/Iodine leach would dissolve the rhodium minerals.....and since I do not think that we really came to a real conclusion or answer to that question.....my best option now is to get out in my lab, grind up some ore and start testing myself! :lol:
In the second place, when I say it works for me, that does not necessarily mean that the entire process works for me, but the part that I I wanted to accomplish works for me! :lol:
Irons, I believe that if you will try putting some copper wire or any copper in some concentrated hot sulfuric acid and bring to almost boiling , you may discover that indeed the copper will dissolve very neatly into the Hot, Saturated H2SO4 quite rapidly. Different strengths of sulfuric acid and temps will dissolve copper at different rates. This is also one of the reasons that sulfuric acid is the accepted electrolyte for making purified copper cathodes, of course again a certain strengths, temps, amps, etc.!
Anyhow, my apologies to all, if I have offended any or such. Which I never try to do intentionally.
I am now ready to move on to another subject, at least until I have the answers to this I/I problem that I will pursue shortly in my lab work! :lol:
In the first place, I don't always do everything a certain way! :lol: That was a really dumb statement! :lol:
What I did inadvertently, was get into some methods done on just a small assay type scale, not a larger type scale that I would use to extract and separate the precious metals out of. :wink:
I let this topic get way out in left field from what I originally intended it to do. Like I did say, this topic was only for the express purpose of discovering if any of you knew if Iodine/Iodine leach would dissolve the rhodium minerals.....and since I do not think that we really came to a real conclusion or answer to that question.....my best option now is to get out in my lab, grind up some ore and start testing myself! :lol:
In the second place, when I say it works for me, that does not necessarily mean that the entire process works for me, but the part that I I wanted to accomplish works for me! :lol:
Irons, I believe that if you will try putting some copper wire or any copper in some concentrated hot sulfuric acid and bring to almost boiling , you may discover that indeed the copper will dissolve very neatly into the Hot, Saturated H2SO4 quite rapidly. Different strengths of sulfuric acid and temps will dissolve copper at different rates. This is also one of the reasons that sulfuric acid is the accepted electrolyte for making purified copper cathodes, of course again a certain strengths, temps, amps, etc.!
Anyhow, my apologies to all, if I have offended any or such.
Which I never try to do intentionally.I am now ready to move on to another subject, at least until I have the answers to this I/I problem that I will pursue shortly in my lab work! :lol:
lazylightning
Well-known member
Hi All!
As I see this subject has been untouched for a while, I would still like to put my question forward here because I think someone here could steer me right.
So I went to the labshop today and instead of potassium bisulfate they accidently sold me something a little different. Actually, on one German chemistry forum I accidently ran accross a reference about dissolving Rh with the help of the stuff I accidently got which is K2S2O7. Below is a qoute of the reference:
**********************************************************
"The dissolution of rhodium in an acidic salt melt functions quite well, if you let react the metal with a mixture of potassiumdisulfate; K2S2O7 and sodium chloride; NaCl. This mixture melts at fairly deep temperatures, so you actually can use pyrex-beakers as reaction containers. Another possibility is, to use porcelain dishes. Reaction is best done in an oven at 500-550o C. Usually in 1-2 hours about 80% of the metal has dissolved in the molten mixture. Prolonged reaction does not lead to significant more dissolution, because the salt melt itself decomposes slowly at these temperatures, probably by releasing gaseous SO3 and/or SO2Cl2. The presence of chloride in abundance leads to the formation of Rh(III)-chloro-complexes, clearly evident by the deep red color of the resolidified melt after cooling down. The combined effects of a molten mixture of NaCl and K2S2O7 on platinum group metals can be compared to the combined effects of HCl and HNO3 in aqua regia on metallic gold. So even metallic iridium, which does not react with molten K2S2O7 alone, is dissolved in a similar way by the molten salt-mixture.
Here an example for a rhodium batch of 20 grams, which I did myself for a few times: 20 g of rhodium powder, 136 g NaCl and 296 g K2S2O7 are intimately ground together in a mortar. The grey powdery mixture is placed in a porcelain dish or into wide Pyrex or Jenaer-glass beakers. The beaker(s) or dish(es) should only be half filled. They are put in an oven, heated to 500-550oC and held at this temperature for about 1-2 hours. After cooling down the deep red solids are dissolved in a mixture of 1600 ml water and 400 ml of concentrated HCl. Any undissolved rhodium metal, usually about 4 grams, is filtered off and can be reused again. The deep red filtered liquid contains about 16 grams of rhodium and can be treated further to precipitate Rh(OH)3."
The text is from this forum page: http://www.mathematik-forum.de/forum/showthread.php?t=106496&page=1
**********************************************************
So judging by the text written above, if I add the table salt to the melt mix then it will dissolve the Ir too. I probably have Ir in it. Do I want to do that? Or will Ir precipitate out with the Rh when I add the alchohol? Maybe I should do it without the table salt to insure that the Ir isn't dissolved? They didn't mention whether or not the K2S2O7 will work on the Rh without the table salt, if you look at it carefully. If I add the table salt and it dissolves the Ir too, then it the Ir could precipitate out with the Rh, and then I've done all this for naught.
Also, I just noticed that they do not refer to using alchohol as a precipitant, perhaps it will not work in this case? Though I dont see why, it's still a Rh sulphate water solution.
The site is in German though they're posting in English. I'd just join that forum but all the registration process is in German. Ich nicht forschtehen.
Any ideas?
The material I have is electroprecipitated sulfides(a red color) which contains Rh, Ir and perhaps other pgm's (but no Ru or Os, they are already removed). There may be base metals also. I can roast them to get oxides, but that will make it harder to dissolve, I assume. Then I will have to reduce the oxides under hydrogen first to make it metal again and easier to dissolve. What about putting these sulfides (ground up) into this melt mix. Again, these sulfides dissolve easier in AR than the metal forms and hot AR can dissolve the Rh sulfides pretty fast too. I think they would dissolve pretty easy in any salt melt at all. Then the problem I will face again is the prospect of Ir being in the solution as a water soluble sulfate. Again, will it come out of solution as a precipitate along with the Rh when I add alchohol, or will only Rh do that? Rh is my target material of choice because it seems to be highest along with the Ir in concentration.
Thanks in advance for any thoughts on this.
As I see this subject has been untouched for a while, I would still like to put my question forward here because I think someone here could steer me right.
So I went to the labshop today and instead of potassium bisulfate they accidently sold me something a little different. Actually, on one German chemistry forum I accidently ran accross a reference about dissolving Rh with the help of the stuff I accidently got which is K2S2O7. Below is a qoute of the reference:
**********************************************************
"The dissolution of rhodium in an acidic salt melt functions quite well, if you let react the metal with a mixture of potassiumdisulfate; K2S2O7 and sodium chloride; NaCl. This mixture melts at fairly deep temperatures, so you actually can use pyrex-beakers as reaction containers. Another possibility is, to use porcelain dishes. Reaction is best done in an oven at 500-550o C. Usually in 1-2 hours about 80% of the metal has dissolved in the molten mixture. Prolonged reaction does not lead to significant more dissolution, because the salt melt itself decomposes slowly at these temperatures, probably by releasing gaseous SO3 and/or SO2Cl2. The presence of chloride in abundance leads to the formation of Rh(III)-chloro-complexes, clearly evident by the deep red color of the resolidified melt after cooling down. The combined effects of a molten mixture of NaCl and K2S2O7 on platinum group metals can be compared to the combined effects of HCl and HNO3 in aqua regia on metallic gold. So even metallic iridium, which does not react with molten K2S2O7 alone, is dissolved in a similar way by the molten salt-mixture.
Here an example for a rhodium batch of 20 grams, which I did myself for a few times: 20 g of rhodium powder, 136 g NaCl and 296 g K2S2O7 are intimately ground together in a mortar. The grey powdery mixture is placed in a porcelain dish or into wide Pyrex or Jenaer-glass beakers. The beaker(s) or dish(es) should only be half filled. They are put in an oven, heated to 500-550oC and held at this temperature for about 1-2 hours. After cooling down the deep red solids are dissolved in a mixture of 1600 ml water and 400 ml of concentrated HCl. Any undissolved rhodium metal, usually about 4 grams, is filtered off and can be reused again. The deep red filtered liquid contains about 16 grams of rhodium and can be treated further to precipitate Rh(OH)3."
The text is from this forum page: http://www.mathematik-forum.de/forum/showthread.php?t=106496&page=1
**********************************************************
So judging by the text written above, if I add the table salt to the melt mix then it will dissolve the Ir too. I probably have Ir in it. Do I want to do that? Or will Ir precipitate out with the Rh when I add the alchohol? Maybe I should do it without the table salt to insure that the Ir isn't dissolved? They didn't mention whether or not the K2S2O7 will work on the Rh without the table salt, if you look at it carefully. If I add the table salt and it dissolves the Ir too, then it the Ir could precipitate out with the Rh, and then I've done all this for naught.
Also, I just noticed that they do not refer to using alchohol as a precipitant, perhaps it will not work in this case? Though I dont see why, it's still a Rh sulphate water solution.
The site is in German though they're posting in English. I'd just join that forum but all the registration process is in German. Ich nicht forschtehen.
Any ideas?
The material I have is electroprecipitated sulfides(a red color) which contains Rh, Ir and perhaps other pgm's (but no Ru or Os, they are already removed). There may be base metals also. I can roast them to get oxides, but that will make it harder to dissolve, I assume. Then I will have to reduce the oxides under hydrogen first to make it metal again and easier to dissolve. What about putting these sulfides (ground up) into this melt mix. Again, these sulfides dissolve easier in AR than the metal forms and hot AR can dissolve the Rh sulfides pretty fast too. I think they would dissolve pretty easy in any salt melt at all. Then the problem I will face again is the prospect of Ir being in the solution as a water soluble sulfate. Again, will it come out of solution as a precipitate along with the Rh when I add alchohol, or will only Rh do that? Rh is my target material of choice because it seems to be highest along with the Ir in concentration.
Thanks in advance for any thoughts on this.
Shecker
Well-known member
Older Reed switches had a coating of gold/rhodium as the contact point. Never ones have ruthenium.
Randy in Gunnison
Randy in Gunnison
