Write the reaction that occurs when sodium phosphate and barium chloride react. Be sure to include the phase labels. Then write the total ionic reaction and the net ionic reaction including proper phase labels.

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

NaH2PO4+BaCl2-->

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.

To determine the reaction that occurs when sodium phosphate and barium chloride react, we will first write the balanced chemical equation. Then, we will write the total ionic equation by breaking down all soluble ionic compounds into their individual ions. Finally, we will write the net ionic equation by removing the spectator ions, which are ions that appear on both sides of the equation and do not participate in the reaction.

The balanced chemical equation can be written as follows:

Na3PO4 (aq) + 3BaCl2 (aq) → Ba3(PO4)2 (s) + 6NaCl (aq)

In this equation, the reactants are sodium phosphate (Na3PO4) and barium chloride (BaCl2), while the products are barium phosphate (Ba3(PO4)2) and sodium chloride (NaCl).

Now, let's write the total ionic equation by breaking down the soluble ionic compounds into their individual ions:

3Na+ (aq) + PO4^3- (aq) + 3Ba^2+ (aq) + 6Cl- (aq) → Ba3(PO4)2 (s) + 6Na+ (aq) + 6Cl- (aq)

Note that NaCl is soluble and remains as individual ions. Ba3(PO4)2 is insoluble and forms a solid precipitate.

Next, let's write the net ionic equation by removing the spectator ions:

PO4^3- (aq) + 3Ba^2+ (aq) → Ba3(PO4)2 (s)

In the net ionic equation, only the phosphate ion (PO4^3-) and the barium ion (Ba^2+) remain as they participate in the actual reaction. Sodium and chloride ions are spectator ions and do not contribute to the reaction.

So, the net ionic equation for the reaction between sodium phosphate and barium chloride is:

PO4^3- (aq) + 3Ba^2+ (aq) → Ba3(PO4)2 (s)

Please note that the phase labels, (aq) for aqueous and (s) for solid, have been included as shown in the equations.

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.
b. gases
3. weak electrolytes.

barium chloride + sodium phosphate →