DOUBLE REPLACEMENT ON ANOTHER LEVEL!!!

Remember when we only learned how to write a balance equation and then we had to balance them?
If not then let's review some!

1) silver nitrate + potassium phosphate ----->
2) aluminum iodide + mercury(II)chloride ----->
3) calcium nitrate + hydrochloric acid ---->The Solubility Table
4) copper(II)bromide + aluminum chloride ---->

ANSWERS:
1) 1AgNO4 + 1KPO4 ----> 1AgPO4 + 1KNO3
2) 2AlI3 + 3HgCl2 ----> 2AlCl3 + 3HgI2
3) 1CaNO4 + 2HCl ----> 1CaCl2 + 2HNO4
4) 3CuBr2 + 2AlCl3 ----> 3CuCl + 2AlBr3


Now that we've done that, let's take it to another level.
Let's take the same examples and sort them into states. Remember? Aqueous, solid, gas etc?

1) 1AgNO4 + 1KPO4 ----> 1AgPO4 + 1KNO3

Look at the balanced equation and then look at your list of solubility sheet. If you don't have one click on the link below: Solubility Chart
Now look at the highlighted part. First put your finger on Phosphate and slide it across to see if it is a soluble or not a soluble to silver. Do the exact same thing with KNO3.

It will look a little like this : 1AgNO4 + 1KPO4 ----> 1AgPO4(s) + 1KNO3(aq)
Looking at the balanced equation we need to separate the compounds, the easier way to do this is looking at the solid. If both compounds in the highlighted part is a aqueous that means no reaction occurred. However if one compound is a solid and the other an aqueous then a reaction occurred and the separated compound would look like.... Ag+1(aq) + PO4(aq) ----> AgPO4
**REMEMBER TO WRITE THE CHARGES!!**
Try it with the other ones and see what you come up with!