posted by sydney on .
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?
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!
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)
Here are a set of rules for solubility. Memorize them.
Oh yeah, I forgot the NET IONIC thing :(. I took this inorganic class like 4 years ago.