Question

Consider the reaction when aqueous solutions of lead (II) nitrate and iron chloride are combined. What is the net ionic equation for this reaction?

Answer 1

Well, all halides are soluble EXCEPT for those of `Pb^(2+)`, `Hg_2^(2+)`, and `Ag^+`...

Explanation:

And so this so-called metathesis, i.e. partner exchange gives...

`Pb(NO_3)_2(aq) + FeCl_2(aq) rarr Fe(NO_3)_2(aq)+PbCl_2(s)darr`

Or we could write the net ionic equation, which represents NET macroscopic change...

`Pb^(2+) + 2Cl^(-) rarr PbCl_2(s)darr`

Answer 2

`Pb(NO_3)_2(aq)+FeCl_2(aq)->Fe(NO_3)_2(aq)+PbCl_2(s)`

Explanation:

Combining aqueous solutions of lead (ii) nitrate and iron (ii) chloride (I'm assuming you mean iron (ii) chloride because it's simpler to mess around with) will result in an aqueous solution of lead (ii), iron (ii), nitrate and chloride ions.

By kinetic particle theory, you will end up with a solid of lead (ii) chloride which is insoluble in an aqueous solution of iron (ii) nitrate ions floating around, due to the lead (ii) ions colliding with the chloride ions and forming an insoluble solid. I hope this helps!