00:01
For this question, we have a reaction between aqueous barium hydroxide and aqueous phosphoric acid.
00:07
And that's going to give us barium phosphate and water.
00:11
And we want to determine the complete ionic equation for this reaction.
00:15
And then also what the spectator ions are.
00:17
So we already have the balanced reaction.
00:19
The states were given to us.
00:21
If the states of each of the different compounds hadn't been given to us, you would just use the solubility rules to determine that.
00:28
But now what we're going to do is get into the.
00:30
Complete ionic equation.
00:32
So when doing a complete ionic equation, anything that's aqueous is going to break up into its ions.
00:40
And so since we've got water here, water can also be considered to be hoh.
00:46
That'll just make a little bit more sense when we get to the ionic equation.
00:50
But anything that's aqueous gets broken up into its ions.
00:52
And then anything that's not aqueous, we just leave alone and it stays as is.
00:58
So when we do that, we're we're going to have three barium ions, and the three just comes from the coefficient.
01:08
We're going to have six hydroxide ions.
01:11
This comes from the coefficient multiplied by the subscript for the hydroxide, and then we'll do the same thing, because next we'll have six hydrogens, hydrogen ions, and then we'll have two phosphate ions on our left side of the arrow...