00:02
Hi there.
00:03
In this question, we're reacting to aquaous ionic compounds.
00:08
So therefore, we have what's known as a double replacement or double displacement reaction.
00:13
Those two terms are used interchangeably.
00:16
And what happens in a double replacement reaction is we have those two aquaous ionic compounds and they exchange ions.
00:23
The positive ion from the first goes with the negative ion from the second and the positive ion from the second combines with the negative ion from the first.
00:31
However, there is a positive ion from the first.
00:32
However, there is a positive ion from the first.
00:32
Only a reaction if one of the products forms an insoluble product.
00:46
In other words, it forms a precipitate.
00:53
It could also be a liquid or a gas, but in this question we are looking for a precipitate.
00:58
Okay, and our rules for solubility are going to tell us if we form a precipitate.
01:04
So before we try to write our net ionic equation, i just want to write the molecular equation for this to see if we do get a precipitate.
01:12
So we're reacting.
01:15
Lead nitrate, lead to nitrate.
01:18
We know that because it's with two nitrate ions.
01:21
That's going to be aqueous and it's reacting with rubidium chloride, also aquis.
01:29
Now when we exchange ions, the lead two is going to combine with the chloride ion.
01:36
So we need to write this as pb, cl, two, because the lead has a two positive charge, the chloride has a one negative charge.
01:45
We'll look at our solubility, rule in a moment, but let's write our other product first.
01:51
We have rb with nitrate.
01:56
Rb is in the first group of the periodic table, so ribidium has one positive charge, nitrate has a one negative.
02:03
All right, looking at our solubility rules.
02:05
Actually, i'm going to start with the nitrate because i know that all nitrates are soluble...