# chem:ionic equations

write below the complete ionic equation for the reaction of magnesium phosphate with lead(II)nitrate. Include which ions will be aqueous and which compound will precipitate.

I understand how to balance the equation, but the example they give me is completely different from the question and I don't understand where I'm supposed to get my answer from. Can anyone help?

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1. Mg3(PO4)2 + 3Pb(NO3)2 --> 3Mg(NO3)2 (s) + Pb3(PO4)2 (aq)

I think that's how you do it, just an ordinary double displacement reaction. To be honest, I just use my instinct to say the magnesium nitrate is solid and the other is aqueous... I can't remember, if only I have your text book with me.

Anyway, Good Luck!

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2. Jake, you missed it on the products. Nitrates are soluble, but lead phosphate is not.

Mg3(PO4)2 + 3Pb(NO3)2 --> 3Mg(NO3)2 (aq) + Pb3(PO4)2 (s)

So the net ionic equation is...

2PO4-- + 3Pb++ >> Pb3(PO4)2 (s)

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3. Here are a set of rules for solubility. Memorize them.

http://www.chem.vt.edu/RVGS/ACT/notes/solubility_rules.html

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4. Oh yeah, I forgot the NET IONIC thing :(. I took this inorganic class like 4 years ago.

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