Ba(OH)2 + H3PO4 = Ba3(PO4)2 + H2O When I balance it, I get .....
3Ba(OH)2 + 2H3PO4 = Ba3(PO4)2 + 6H2O ........but what about the net ionic reaction.......for some reason , I dont think there was one, because they both remained aq.
2007-11-08 22:47:24 · 3 answers · asked by dannchris@sbcglobal.net 1 in Science & Mathematics ➔ Chemistry
yes, if there was no phase change eg a prisapatate.
2007-11-08 23:02:25 · answer #1 · answered by Anonymous · 0⤊ 0⤋
Barium phosphate is insoluble. Barium hydroxide is soluble and fully ionised. Phosphoric acid is a weak acid, so it is present mainly as a molecular species. So write out the overall equation in ionic form
3Ba2+(aq) + 6 OH-(aq) + 2 H3PO4(aq) ---> Ba3(PO4)2(s) + 6 H2O(liq)
In this particular case, rather unusually, there are no spectator ions and the total ionic equation is the same thing as the net ionic equation.
2007-11-09 02:26:58 · answer #2 · answered by Facts Matter 7 · 0⤊ 0⤋
Balanced Molecular
3Ba(OH)2 + 2H3PO4 ---> Ba3(PO4)2 + 6HOH
Complete Ionic
(3Ba+2) + (6 OH-) + (6 H+) + [2(PO4)3-]
--->
(3Ba+2) + [2(PO4)3-] + (6H+) + (6OH-)
Net Ionic
Cross out species that occur on both sides of the equation. So, you're right, there's not net ionic.
2007-11-08 23:05:47 · answer #3 · answered by student2000 2 · 0⤊ 0⤋