 So, let's attempt this titration problem that we came up with, so using the reaction equation that we had from the last problem. So, you can see here that we have a volume of HCN of 15.0 mils. The molarity of HCN is 2.00 molar. And we're going to titrate that with 3.00 molar NaOH and we're wondering what is the volume of NaOH that we're going to need to reach the equivalence point, okay? So how do we do that? Well, the first thing we have to, we're going to eventually need to use this reaction equation to do a mol to mol ratio, okay? So first thing we need to do is figure out, well, how many moles of HCN do we have, okay? So how do we do that? Well, remember, this is moles per liter, okay? So let's just convert that, the moles of HCN are 1 liter of HCN and we've got 15 mils of HCN, right? So for every 1 liter of HCN, 1,000 mils of HCN, except for me, I think it is, the mils of HCN, right? So we're going to say 15.0 mils HCN, like that. That cancels out everything to give us moles of HCN. Do you see that? Does that make sense? Sure, we do, yeah. Does it? It's important that it does. And why I did it that way. Okay, so let's do it together. 2 divided by 1,000 times 15. So the number of moles is 3.00 times 10 to the negative 2, moles of HCN, like that, okay? So how many moles of NaOH are going to react completely with that many moles of HCN? 3.00. 3.00 times 10 to the negative 2. Because there's a 1 to 1 ratio here. You can't come up with that on your own. You can do this. Okay, so for every 1 mole of HCN you have, you've got 1 mole of NaOH reacting with it. So the number of moles of NaOH that we need to completely react with that many moles of HCN is going to be 3.00 times 10 to the negative 2. Moles of NaOH. Like that, does that make sense? Okay, wonderful. So, but we're not interested necessarily in that number of moles of NaOH. We're interested in the volume, right? But we've got the concentration here, the molarity. So remember what is molarity? That's moles per liter, right? Moles per liter. So moles per liter, that's just a conversion factor from moles of NaOH to liters of NaOH, okay? So we've got moles of NaOH here, right? And we want volume so we can cancel those things out using it. So we've got 3.00 moles of NaOH per one liter of NaOH. Like that, like that. So, divided by 3, 1.00 times 10 to the negative 2 liters of NaOH. Alright, so do we want to keep it in liters? Let's change it back to milliliters, okay? So what do we want to do? So for every one liter, 1,000 mils. So all we have to do is multiply that by 1,000. And we get the answer that we would have expected, of course, 10.0 mils of NaOH. We'll fully titrate 15 mils of 2.00 molar HCM, okay? So it's just a logical stepwise process. Don't make it harder than what it is, okay? Just think, what am I looking for in this part? I have like, I don't know, 10 of these online. Check them out, okay? They're in the titration section. I'll put this one in there too. Did you get for a bowl of salute? Oh, do you want? Okay. Anybody else have any questions? Questions before I kill it? Okay, I wonder.