One more query please? Why does cupelled button go from a bright red , ( think I know this one ) , to a bright golden sheen , then it cools completely to a dull lead/ silver finish?
Thanks again
Thanks again
Assuming the temperature is not way above gold m.p., this means you have 30% or more silverOne more query please? Why does cupelled button go from a bright red , ( think I know this one ) , to a bright golden sheen , then it cools completely to a dull lead/ silver finish?
Thanks again
I have moved your post here, it belongs here, do not spread threads around when they are a continuation of something else.hello again, we cupelled a lead collector button, we had two actually, which were a bright yellow/ golden colour, once they cooled down , both were placed in some muriatic acid , as well as some of the cupel crust sections which had some beads imbedded, after about twelve hours, there was no sediment/ dust or solids left in the container that had the acid in it, but the acid is a bright yellow colour. Any thoughts as to what occurred? Thanks once more.
I knew I had a reply missing but it is only today I see your message.Lead usually does not hang out in puddles, but in solid state.
What do you mean 'found a puddle of lead'? I'm almost thinking mercury.
I also think it's a translation thing, but please clarify.
How have you vaporized lead? Have you scrubbed the fumes?
How did you 'dispose' of it?
"The acid"? Which one?
Don't blame the lead, it didn't do anything wrong, you gave it wrong instructions.
TO ALL NEWBIES: before you do anything, ask us first!!!! for your own sake and everything around you.
That is completely insane!I knew I had a reply missing but it is only today I see your message.
By puddle i simply meant a big solid piece of lead with a weight of 23 kg +-500g.
I didn't fully vaporize it i done it in a tiny mould for precious metals with a hand torch.
I tossed it along another piece after i reduced it's size by 75% in hcl with some peroxide.
Not blaming the lead i were simply uncertain if it contains any other metal but it reacted and behaved just like the other one.
Additionally, it's worth noting that the presence of palladium can cause gold to turn white in color. One way to gain more information is by dissolving a small piece of the material and performing a Stannous Chloride test.
To COMPLETELY get lead out of an aqueous solution, he'd need to add sulfuric acid. Lead sulfate is virtually insoluble in acidic aqueous solutions. It's a step that's essential for gold purification, for example; one that Sreetips has demonstrated many times.He could try to cement it out first. Check the Redoc Metal Series for a suitable precipitant:
Any other ideas, or comments?
@andu: Chose a pure metal that is below Lead like Nickel f.e.:
Even H2O is supposed to precipitate Lead in solution, but I am unsure if that really works in this case.
Worth a try. Please report back.
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No copyright problem here, this is from my own book "Gold Hunter´s Guide"
Did you read what that poster did?To COMPLETELY get lead out of an aqueous solution, he'd need to add sulfuric acid. Lead sulfate is virtually insoluble in acidic aqueous solutions. It's a step that's essential for gold purification, for example; one that Sreetips has demonstrated many times.
But he would also have to know how to handle sulfuric acid. It's very dangerous to anyone not familiar with the methods of storing and handling it.
If he could form lead carbonate, that's a full order of magnitude LOWER in solubility than even lead sulfate. Only 0.00011g/L.Did you read what that poster did?
He more or less dissolved 75% of 23Kg of Lead in HCl.
It have to be a massive amount of LeadChloride, and as Alondro says, maybe the best is to drop it as Sulfate and hand it in as Special waste.
I think he don't need Sulfuric acid, Magnesium Sulfate will do I think.
Easy is best here, the poster is fresh and has not worked up much lab skills yet.If he could form lead carbonate, that's a full order of magnitude LOWER in solubility than even lead sulfate. Only 0.00011g/L.
But it's tricky. One must add chilled ammonium carbonate solution and keep the reaction cold.
With summer coming on, the sulfate should dry pretty quickly too. The issue with letting ALL the solution remain is that the chloride will still be in there. Then he wouldn't want to use magnesium sulfate, because that would yield a large amount of magnesium chloride, which is quite deliquescent (due to MgCl2 being a Lewis acid) and will never dry.Easy is best here, the poster is fresh and has not worked up much lab skills yet.
The sulfate is the easiest and after initial drop he can let it evaporate naturally which will drop even more over time.
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