 Okay, so this question says we have a solution of sodium sulfate that has a concentration of 0.384 molar. And it wants to know, well, if we have that, what's the molarity of the total ions in solution? Okay. So here we have the molarity of sodium sulfate, and it wants the molarity of all ions. Okay? So in order to do this, you want to, you're going to have to remember kind of your solubility rules, okay? So the first thing you want to do is write out an equation of the dissolution of sodium sulfate. So when you put it into water, what happens to it? So you get this. So what you want to realize about this question is that it's saying the total number of ions. So if you look at this, right, for every one sodium sulfate, we make three ions, right, because there's two of these and one of these. So in order to do this, what you're going to use is that conversion factor, one mole of sodium sulfate equals three moles five. So let's just do that. So if you want to remember, molarity is just moles per liter, and we started with moles of sodium sulfate, one liter. And we have that conversion factor that we just figured out through the chemical equation. That one mole of sodium sulfate is three moles of ions canceled. So hopefully you can see we got moles of ions divided by liters. So that's going to be molarity of ions. So all we have to do is take our initial number, 0.384, and multiply. So the molarity of the ions to three sick things is 1.15 molar in ions. Oftentimes you'll see this when you're referring to ions as equivalents per liter. So that's another concentration unit that you might see. So in other words, since it's ions, it would be like 1.15 equivalents per liter. Does this make sense? So what I'm going to do is I'm going to start another video, and what we'll do is a very similar problem to this, but we're going to give a volume and then figure out how many moles are in that volume. So are there any questions on this one before we kill it?