 Okay, so let's do the second part of that problem now. So it says what is the molarity of the potassium ions in this solution? So we figured out what the molarity of potassium phosphate was. So I'm going to erase all of this up here. Is that okay? So in order to do this problem, we're going to have to recall that both, of course, potassium and phosphate are both strong electrolytes dissociate completely in solution. So A3P04, when you put it into solution, goes to 3K plus AQS plus B043 minus AQS. Okay? Is that okay? Let's put that first. Okay, so remember, this is a mole to mole ratio. Okay? And remember, this is moles per liter here. Okay? Concentration. So if I'm wondering what's the molarity of K plus ions, remember we can break that down into its constituent parts. Right? Say, moles of K3PO4 divided by solution. Right? And we have a mole to mole conversion there. Right? Is everybody okay with that? So for every one mole of potassium and phosphate, we've got three moles, very good, of K plus ions. So, cancel, cancel. So 3, 1.57 times 3, I got one molar. Asked you, what, what, that's, that's the number of moles. Yeah, that's the moles. Yeah. Oh, but it's moles, moles per liter. Well, it's mostly five liters over there. How many molars do you have in the answer one? That was the last problem, right? So we figured out the molarity from the last problem. It's okay though, it's good, it's good to do that stuff. Yeah. So what, you're saying moles, right? But what we're saying is we never cancel that, the liters of solution here. So that's a good point. What if I asked you, I guess, just to continue this problem a little bit, what's the molarity of phosphate ions? 1.57 molar, okay, 1.57 molar of phosphate. So molar and molarity, you have the same, like the molars. Yeah, the same thing, yeah. Molarity, if you say molarity or molar, that's the way to, yeah, yeah, doing it. Any other questions?