For a reaction between sodium phosphate and strontium nitrate write out the following:

a) The balanced molecular equation
b) The ionic equation
c) The net ionic equation

a) I think I have this one:
2 Na3PO4 (aq) + 3 Sr(NO3)2 (aq) --> 6 NaNO3 (aq) + Sr(PO4)2 (s)

b) Should I just take apart the unbalanced equation?

3Na^+(aq) + PO4^3-(aq) + 2NO3^-(aq) --> Na+(aq) + NO3^-(aq) + Sr3(PO4)2(s)

c) If the above is the ionic equation then I have no idea how to make the net ionic equation. I don't see anything canceling out.

for part a, i think you forgot to put Sr3(PO4)2 (since you used that for part b). So, part a's balanced equation should be: 2 Na3PO4 (aq) + 3 Sr(NO3)2 (aq) <--> 6 NaNO3 (aq) + Sr3(PO4)2 (s)

Oh, sorry, I meant Sr3(PO4)2. That's what I wrote down but I didn't type it properly.

The Na^+ cancels on both sides and the NO3^- cancels on both sides (you omitted the 6 coefficient for the rigght side for both Na+ and NO3-).

So the net ionic equation is
PO4^-3(aq) + Sr^+2(aq) ==> Sr3(PO4)2(s)

To determine the net ionic equation, we need to identify the spectator ions. Spectator ions are ions that remain the same on both sides of the equation and do not participate in the actual reaction.

Let's break down the ionic equation into its individual ions:

3Na^+(aq) + PO4^3-(aq) + 2NO3^-(aq) --> Na+(aq) + NO3^-(aq) + Sr3(PO4)2(s)

In this equation, the sodium ion (Na^+) and the nitrate ion (NO3^-) appear on both sides of the equation and do not change. Therefore, they are spectator ions.

Now, let's rewrite the equation by removing the spectator ions:

PO4^3-(aq) + Sr^2+(aq) --> Sr3(PO4)2(s)

This is the net ionic equation. It represents the actual reaction occurring between sodium phosphate and strontium nitrate.

Net ionic equation: PO4^3-(aq) + Sr^2+(aq) --> Sr3(PO4)2(s)