00:01
For this question, we've got two different reactions.
00:03
We first have a reaction between sodium phosphate and iron three nitrate, and we need to determine the molecular equation, the complete ionic equation, and the net ionic equation.
00:12
And then we have a reaction between iron three nitrate and sodium hydroxide.
00:16
And again, we want to determine the molecular equation, the complete ionic, and the net ionic equations as well.
00:22
So starting with our sodium phosphate and iron three nitrate, this is a double replacement reaction.
00:28
So our elements are going to switch partners.
00:31
And so one of our products is going to be sodium nitrate.
00:34
So we'll have n -a -n -o -3.
00:36
And that's an aqueous compound.
00:40
And then we're going to get ironed -3 -phosphate, which is f -e -p -o -3, or excuse me, p -o -4.
00:47
And this is going to be insoluble, so that'll be our precipitate.
00:51
To balance this particular reaction, we just need to put a -3 in front of the sodium nitrate, and we'll be balanced.
00:58
For the complete ionic equation, anything that's aqueous is going to break up into its ions.
01:05
So both of our reactants will break up into their ions, and then our product of sodium nitrate will break up into its ions.
01:12
Anything that's not aqueous, so if it's a solid liquid or gas, it stays as is, and we don't break it up.
01:18
So we're going to have three sodium ions on the left side of our arrow.
01:24
We'll have one phosphate ion, one iron ion, and three nitrate.
01:33
Nitrate ions.
01:38
And then we go over to our products and we're going to break up sodium nitrate because it's aqueous.
01:42
So we'll have three sodium ions again.
01:46
And then we'll have three nitrate ions.
01:49
And then our iron three phosphate is going to stay as a complete compound...