Question

(NH4)2 SO4(aq) + Pb(C2H3O2)2 (aq) ---> 2NH4C2H3O2 (aq) + PbSO4 (s). I need to find the total ionic equation, and the net ionic equation.

Answer 1

You have to remember how to create the total ionic equation to get the net ionic equation. Net ionic is the total ionic minus the spectator ions (the ones who don't do anything or change during the reaction.)

You need to write out the same equation but separate everything into ions!

Answer 2

How do I find the charges on the periodic table and apply them to the equation once it is balanced as it is?

Answer 3

You can find the charges based on their location on the table for singular elements. The column that they are in indicates the charge. Transition metals don't always fit there, so you need to figure out their charge by the compound that they are in. Remember that a compound needs to have a net charge of 0, unless you're explicitly told otherwise.

Some charges you just need to start memorizing, like polyatomic ions. SO4 has a charge of 2-.
Since SO4 has a charge of 2- and Pb is attached to it, the charge of Pb would be 2+.
Written form: lead (II) = Pb[2+]

The picture I attached is the charges of the columns in the periodic table. The transition metals in the middle section are cut out because those charges vary.

Answer 4

to confirm, is the total ionic EQ: SO4[2-] + NH4[+] + Pb[2+] + 2(C2H3O2)]1-] --> NH[4+] + 2(C2H3O2)[1-] + Pb[2+] + SO4[2-] ?

Answer 5

I believe so, but it's missing a few balanced areas. Like... NH4[+] needs to be 2NH4[+] !

Answer 6

What would the net ionic equation be? It looks like everything cancels out on both sides.