 OK, anyway, so the first one. A 500-gram sample of potassium phosphate has dissolved in enough water to make 1.5 liters of solution. What's the molarity of potassium phosphate solution? OK, so it tells us the mass of potassium phosphate. So it's asking us, what's the molarity of this solution? Could we do this? Do you guys think we could do this with this information, Ryan? The only thing we need to do is use what? There's one conversion factor. The molar mass, the molar mass. So what we need to do is figure out the molar mass of potassium phosphate. Did you do it already? OK, thanks. So 212.27, is that what you got? So let's just write it out explicitly. So 212.27. And remember, molarity, of course, it helps to formula, right? So it's going to be number of moles of solute over volume of solution, like that. And so do we have that stuff now? Yeah, we can calculate it. So let's do that. So 500 plus 5 times 212.27, would you have said, or is this thing molarity here? So what did you guys get? 1.57. 1.57, and good, because it's only the three same things, right? 1.57, molar is what you said, molar. And you could go so far as to say, K3, P1, that's it. Everybody OK with that one? And any questions on that one? It's just the conversion factors, right? This whole class, actually, you know? So if you can find the units that will cancel to give you the units that you want, just put them over each other, or multiplying by each other. And they'll cancel and give you what you want, OK? It's the last part, P1. Yeah, we'll do that in the next video, OK?