molecular equation is
2Na3PO4(aq) + 3MgCl2(aq) ==>Mg3(PO4)2(s) + 6NaCl(aq)
total ionic BUT you add the phases.
6Na^+ + 2PO4^3- + 3Mg^2+ + 6Cl^- ==> Mg3(PO4)2(s) + 6Na^+ + 6 Cl^-
net ionic. cancel those ions that appear on both sides of th equation and you will be left with
2PO4^3-(aq) + 3Mg^2+(aq) ==> Mg3(PO4)2(s)
please help! I don't understand any of this.
Using the Solubility Rules, write the balanced molecular, total ionic, and net ionic equations (including physical states) for the following:
Hints: There is no such thing as an Na3+. Na is in group 1A, so you know it can only form a +1 charge. It will form 3 Na+ ions for each Na3PO4. There is a diatomic molecule Cl2. But when ionic compounds are dissolved in water, they form ions so the dissociation is to 2 Cl- from the MgCl2.
1. Na3PO4 (aq) + MgCl2 (aq) ->
2. Al(CH3COO)3 (aq) + KOH (aq) ->
1 answer
1 answer