The oxidation state 4+ is not stable in PbCl4; the reaction is:
Pb4+ + 2 e---------Pb2+
A filter? Lead (II) chloride isn't very soluble (and lead (IV) chloride isn't very stable, tending to decompose into lead (II) chloride and chlorine gas), and you could use HCl to raise the chloride concentration (and therefore lower the lead concentration) even further.
Yes; lead(II) chloride is very low soluble in water.
Lead Chloride.
by adding hot water
lead IV chloride
Silver is most.
Elemental chlorine is a stronger oxidizing agent than iron (II) cations.
Tin will act as an oxidizing agent. Lead will act as a reducing agent. Tin will be reduced. Lead will be oxidized.
silver chloride is soluble in ammonia, lead chloride is only slightly soluble in ammonia
It is very simple
lead chloride is formed
PbCl2 is lead chloride, lead dichloride or lead (II) chloride. It is an important to the chemical industry because of its value as a reagent. A link to the Wikipedia article is provided. Surf on over for details.
Aluminium + Lead Chloride --> Aluminiu, Chloride + Lead Al + 3PbCl --> AlCl3 + 3Pb
Add ammonia solution to mix. Silver chloride dissolves leaving lead chloride behind.
Sodium chloride remain in solution; lead(II) chloride is practically insoluble in water.
Lead (IV) Chloride
Lead chloride is written as a formula like this: PbCl2