MeshPL
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A stupid question about PbCl2
I've been messing with dissolving lead-tin solder, and have a question: does the NaCl solution redissolve lead? Or is it only NaCl? And will PbCl2
dissolve in ~30% AcOH?
Thanks!
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blogfast25
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Quote: Originally posted by MeshPL  | I've been messing with dissolving lead-tin solder, and have a question: does the NaCl solution redissolve lead? Or is it only NaCl? And will PbCl2
dissolve in ~30% AcOH?
Thanks! |
Your question isn't very clear to me but I can say this. PbCl2 solubility goes up somewhat when there's free chloride in the solution. This
is mainly due to the formation of a complex:
PbCl2 + 2 Cl- < === > PbCl42-
I don't believe it will dissolve in 30% HOAc though...
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MeshPL
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Ok, I'll formulate this question more clearly (I must have had a brain eclipse while writing the last post):
Will PbCl2 dissolve well in a concentrated NaCl solution?
Is efficient complexation of PbCl2 possible using only HCl or NaCl will also work?
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blogfast25
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| Quote: Originally posted by MeshPL | Ok, I'll formulate this question more clearly (I must have had a brain eclipse while writing the last post):
Will PbCl2 dissolve well in a concentrated NaCl solution?
Is efficient complexation of PbCl2 possible using only HCl or NaCl will also work?
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Both NaCl and HCl will work but it depends on your definition of 'well'. Solubility will remain fairly low, even at high [Cl-], IIRW.
There are data on the solubility of PbCl2 in chloride bearing solutions: I've seen graphs of solubility v. [Cl-]. I believe
there are also data on the complexation constant (Kf) of the mentioned complex. That should even allow to compute a rough estimate of
solubility v. [Cl-].
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MeshPL
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Oh yes! There is such a graph on wikipedia! It indeed seems that at high Cl- concentrations Pb 2+ is somewhat soluble, but not too much. Thanks!
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