[mercenary_sg]

I am task to recover the Pb from lead II sulfate without using electro-chemistry. But i am given limited tools though. I have search through the net, and this is what i am thinking.

Adding Sodium Hydroxide at high quantities and maintain at high pH level to extract the lead from sulphate.

Or by adding PbS to PbSO4 to obtain 2Pb(l) and 2SO2(g)

Or adding PbSO4 to 4CH3COONH$ to get [Pb(CH3COO0)4]2-

Which is a better feasible way to extract lead. The lead content i am having is only 3%. Or is there a better way of extraction? Do advice too.
This is for a project i am doing. Now seeking advice from fellow forumers before i proceed to carry on the testing.
Thanks in advance

[DevaDevil]

it all depends on if you need to extract lead as a metal, or ion.

If you need lead to become metallic; you need electrochemistry - if only because you need to reduce your lead, which is in the 2+ oxidation state. (adding metallic Zinc would make the lead crystallize out for example:
Zn --> Zn²⁺ + 2 e^- E= 0.76
PbSO₄ + 2 e^- --> Pb + SO₄^2-
-----------------------------------------------------------------------
Zn + PbSO₄ ---> Pb + Zn²⁺ + SO₄^2-

just an example (this is the basis of old batteries), but you get the picture.


If you are allowed to get lead out as an ion, lead acetate sounds fine

[Borek]

If you are allowed to get lead out as an ion, lead acetate sounds fine

How? Sulfate is weakly soluble, pK_so about 7.8 if I am not mistaken, IMHO acetic acid is not that strong complexing agent to dissolve PbSO₄.

[DevaDevil]

lol Borek, that could actually be true enough.
I am not experienced enough with complexing agents, as I like to keep my metals in metallic form.

[AWK]

Concentrated ammonium acetate gently solubilizes PbSO4. This is a common test allowing differentiating PbSO4 from BaSO4 during qualitative inorganic analysis.

PbSO4 can be  converted to metal by reduction with carbon at high temperature. Usually addition of Na2CO3 is used in the lab.