Question

aqueous sodium chloride reacts with aqueous lead (II) nitrate to yield a lead(II) chloride precipitate and aqueous sodium nitrate.

What is the net ionic equation?

What reaction type is this?
a) acid-base
b) precipitation
c) oxidation reduction
d) combination of the above

Answer 1

We are told in the problem statement that lead (II) chloride is the precipitate, so we can write the complete ionic equation as Na+(aq) + Cl-(aq) + Pb(II)2+(aq) + (NO3)-(aq) -> Pb(II)Cl2 (s) + Na+ (aq) + (NO3)-(aq)
Anything that appears in the reactants and products can be left out of the net ionic equation.

Answer 2

An acid base reaction produces water and a salt. Precipitation reactions produce an insoluble ionic compound. In an oxidation reduction reaction, the oxidation numbers must change. What do you see happening here?

Answer 3

So, I am getting:

\[2 Cl ^{-}_{(aq)} + Pb ^{2+}_{(aq)} \rightarrow PbCl _{2(s)}\]

as the net ionic equation. Is that correct?

Answer 4

Yes, good job!

Answer 5

I'm seeing an oxidation reduction reaction?

Chlorine is being oxidized and Lead is being reduced?

Answer 6

No, the oxidation number of Chlorine is -1 as a reactant and a product, and Lead is +2 as a reactant and a product.

Answer 7

I thought that elements by themselves have an OS of 0?

Answer 8

True of elements, but these are ions.

Answer 9

ohhhh I see. Not sure what the reaction type is then :/

Answer 10

Ions have an oxidation number equal to their charge.

Answer 11

This isn't acid base and its not ionic compound.

Answer 12

All the reactants are soluble, but we have produced an insoluble ionic compound. This is a precipitation reaction.

Answer 13

ok im getting mixed up between ionic and molecular compounds. Thanks for your help!

Answer 14

No problem :)