This is a huge amount of work. Show what you know about it up to the point you don't know where to go next and include a short description of your problem in getting there. We can help you through it.
In general, this is what you do.
1. Write the molecular equation.
2. Convert the molecular equation to the ionic equation using the following guidlines. Write everything as ions EXCEPT
a. insoluble precipitaters.
3. weak electrolytes.
I guess getting started is the hard part for me here,
I figured out that sodium phosphate and barium chloride are the reactant and look like this
But then I do not know how to convert to a ionic equation or what the product would be??
It said sodium phosphate, not monosodium dihydrogen phosphate.
Na3PO4 + BaCl2 ==> Ba3(PO4)2 + NaCl (you balance)
My assumption is that these reagents are in solution although the problem doesn't say that. It should if your prof want labels put on it. So assuming the chemicals are solutions, we would write
Na3PO4(aq) + BaCl2(aq) ==> Ba3(PO4)2(s) + NaCl(aq) (again, you balance).
Now you look at the aq (stands for aqueous) and convert to ions.
Na3PO4(aq) becomes 3Na^+(aq) + PO4^-3(aq). BaCl2 similarly. Ba3(PO4)2 stays as the molecule since it is a solid and doesn't dissolve appreciably. NaCl converts to ions (put the labels on the ions, too).
The last step is to look at the ions on both sides of the arrow and mark out anything that is common to both sides. At the end you should have this as the net ionic equation.
3Ba^+2(aq) + 2PO4^-3(aq) ==> Ba3(PO4)2(s). This is the MEAT of the reaction. All of the other stuff is superfluous.
I hope this gets you started.