Very rusty with chemistry and looking to review some basics. Came across the following:
Iron(II) chloride and potassium phosphate react. Write and balance the molecular, ionic, and net ionic equations.
What I have so far (guessing, basically):
$$\ce{FeCl2 + K(H2PO4) -> KCl + Fe(H2PO4)2}$$ [still need to balance but correct right hand side?]
I can't remember the exact rules for forming the right hand side. I just put this in place to match ion charges. What prevents me from writing the right hand side as something else entirely (not sure what but I'm asking, "well, couldn't I figure something out if I break everything apart and re-arrange into another option?").
EDIT: Additional Question Below
Ok, so assume the above reaction was balanced (it's not) and valid. Then, my question is does the reaction go both ways ($\ce{<-->}$)? If so, when/why/how? I'm trying to think back many years ago and it has something to do with "reactivity" and the row of the elements on the periodic table, correct? I'm going to look into it more myself but if someone has a quick "30 second" answer I'm sure it'd be of help to me!
[Assuming this is OK and valid in the forward direction. Again, needs to be balanced.]
$$\ce{FeCl2 + K(H2PO4) -> KCl + Fe(H2PO4)2}$$
[Is this ever ok/possible?]
$$\ce{KCl + Fe(H2PO4)2 -> FeCl2 + K(H2PO4)}$$
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