What is the net ionic reaction of Barium Phosphate and Phosphoric Acid? I tried
H + 2PO4 + 3Ba + OH -> Ba3(PO4)2 + H2O, and
6H + 2PO4 + 3Ba + 6OH -> Ba3(PO4)2 + 6H2O
but the homework software says both are wrong. What is wrong with it?
The net ionic equation you provided is partially correct but incomplete. The balanced net ionic equation for the reaction between barium phosphate (Ba3(PO4)2) and phosphoric acid (H3PO4) is as follows:
2H+ + 3PO4^3- + 3Ba^2+ → Ba3(PO4)2(s) + 2H2O
In this reaction, two hydrogen ions (H+) from the phosphoric acid combine with three phosphate ions (PO4^3-) from the barium phosphate to form solid barium phosphate (Ba3(PO4)2) and water (H2O).
The incorrect part of your attempt is assuming that hydroxide ions (OH-) are involved in the reaction, which is not the case as you are dealing with phosphoric acid, not a base. Additionally, you forgot to balance the charges of the ions involved.
Therefore, the correct net ionic equation is 2H+ + 3PO4^3- + 3Ba^2+ → Ba3(PO4)2(s) + 2H2O.
It seems like you are trying to write the net ionic reaction for the reaction between Barium Phosphate (Ba3(PO4)2) and Phosphoric Acid (H3PO4). However, there is an issue with the equations you provided.
First, let's write the balanced chemical equation for the reaction:
3Ba3(PO4)2 + 2H3PO4 -> 6BaPO4 + H2(PO4)2
To determine the net ionic reaction, we need to first dissociate the compounds that are strong electrolytes into their respective ions. Ba3(PO4)2 does not dissociate since it is insoluble, but phosphoric acid (H3PO4) does dissociate:
H3PO4 -> 3H+ + PO4^3-
Now, let's remove any spectator ions. Spectator ions are the ions that appear on both sides of the equation and do not participate in the actual reaction. In this case, BaPO4 is a precipitate and does not appear in its ionic form on both sides. Therefore, we can remove it from the equation.
The net ionic reaction is:
3H+ + PO4^3- -> H2(PO4)2
So, the correct net ionic reaction is 3H+ + PO4^3- -> H2(PO4)2.
It's important to double-check the solubility of compounds and the dissociation of strong electrolytes when writing net ionic reactions.
You must have written the problem incorrectly. I assume you meant you want the net ionic equation for H3PO4 and Ba(OH)2.
Ba(OH)2(s) + H3PO4(l) ==> Ba3(PO4)2(s) + H2O(l)
If the Ba(OH)2 is in solution, then
Ba^+2(aq) + 2OH^-(aq) + H3PO4(l) ==>Ba3(PO4)2(s) + H2O(l)
Neither equation is balanced. I've left that for you to do depending upon what you intended.