nguyenvannam2904
Harmless
Posts: 6
Registered: 10-2-2019
Member Is Offline
|
|
Lead compound
Can PbCl2 react with HNO3 to form Pb(NO3)2 ?
If yes, what product can be formed beside Pb(NO3)2?
|
|
|
woelen
Super Administrator
Posts: 7977
Registered: 20-8-2005
Location: Netherlands
Member Is Offline
Mood: interested
|
|
Using PbCl2 for making Pb(NO3)2 is not impossible, but the reaction and workup is not easy.
PbCl2 is only very sparingly soluble in aqueous solution. In hot concentrated HNO3, this slowly reacts to form Pb(NO3)2, ONCl and Cl2. The Pb(NO3)2
also does not dissolve easily, especially if the acid is more concentrated. On the other hand, if the acid is not that concentrated, then the redox
reaction in which the chloride is converted to ONCl and Cl2 hardly occurs. I expect that you will have a hard time getting Pb(NO3)2 in decent amounts
and of decent purity with HNO3.
If you want Pb(NO3)2, then dissolve lead metal in nitric acid. That reaction works much better. On cooling down, crystals of Pb(NO3)2 separate from
the acid. These crystals still contain quite some trapped acid, but when you dissolve them in hot water and allow the solid to crystallize again (let
the water evaporate in a dish over a few days), then your product is quite pure.
|
|
|
RogueRose
International Hazard
Posts: 1585
Registered: 16-6-2014
Member Is Offline
|
|
Do you already have the PbCl2?
I think I got some kind of hydroxide or hydroxide/carbonate when I was trying to neutralize a solution of lead chloride and I'm guessing I would have
used sodium carbonate, possibly with a little NaOH in it as well. IIRC, I do remember it being a difficult product to work with but I can't remember
if it was making it or neutralizing it when I wanted to dispose of it.
If you already have the chloride and want the nitrate, then maybe you can make the carbonate/hydroxide and then add the nitric acid.?
IDK where you got the lead, but I've had some very trying times working with lead from batteries and even after conversion to a salt (acetate in this
case), it didn't turn back to a very usable form of lead when I either decomposed it or did a displacement reaction. The lead remained in a very
strange form that seemed resistant to melting in the metal form w/o oxidizing at an incredibly high rate.
|
|
|
nguyenvannam2904
Harmless
Posts: 6
Registered: 10-2-2019
Member Is Offline
|
|
I use soldier wire which has about 37% Lead and 63% tin. Then I put the soldier wire in the solution of 30% HCl + 30% H2O2 in equavalent amount. The
reaction happened in about 2 hours. Then in the reaction flask, I see a bunch of solid white stuff. I boil of the flask to recrystalize PbCl2 then
filtered the solution and collected PbCl2. This method give the high yield of PbCl2 
|
|
|
nguyenvannam2904
Harmless
Posts: 6
Registered: 10-2-2019
Member Is Offline
|
|
I tried to dissolve the soldier wire into concentrated HNO3 but I don't have any idea to seperate Sn(NO3)2 and Pb(NO3)2 
|
|
|
AgCollector
Harmless
Posts: 24
Registered: 31-7-2018
Member Is Offline
|
|
I've never done this personally but from what I've read it should form an insoluble tin(IV) compound "metastannic acid", and the lead(II) nitrate
stays in solution.
|
|
|
Bedlasky
International Hazard
Posts: 1219
Registered: 15-4-2019
Location: Period 5, group 6
Member Is Offline
Mood: Volatile
|
|
Quote: Originally posted by AgCollector  |
I've never done this personally but from what I've read it should form an insoluble tin(IV) compound "metastannic acid", and the lead(II) nitrate
stays in solution. |
I once dissolved some tin/lead solder in analytical labs. Tin precipitated out as hydrous SnO2 and lead remained in solution.
Btw. tin(IV) nitrate does exist, but it's quite unstable and hydrolyze in to hydrous SnO2:
http://tin.atomistry.com/stannic_nitrate.html
|
|
|
![[*]](images/xpblue/default_icon.gif){kind=icon}
