 OK, so this one's a titration problem. Again, I've recorded more titration problems, but this one's a nice one. It says 25.0 mill sample of vinegar, which is dilute acetic acid. And then it gives you the molecular formula of vinegar. It's titrated and found to react with 94.7 mills of a 0.2 molar NaOH solution. What is the molarity of the acetic acid solution? And then it goes on to give you the double displacement reaction equation, or the acid base. Remember, acid base are always double displacements. So it goes on to give you the balanced reaction equation, which is that. If this wasn't balanced for us, we would have to balance it first. But since it is, we're not going to. So the first thing I guess we want to remember is that when we're titrating something, it takes a multiple ratio of the things that are presented in the balanced chemical equation to reach that equivalence point. So what we see here is that we've got a molarity of NaOH, a volume of NaOH. So we should, from those two things, be able to get the moles of NaOH. We've got the volume of acetic acid, but we don't have the moles. And it's looking for the molarity of the acetic acid solution. So what is that? So that's what we're looking for. We've got the volume. All we need is the number of moles. So let's go about figuring this out. So the first thing I like to do is change this molarity symbol to moles per liter. So if you want to, moles of NaOH per liter. And this is the number of mils of NaOH. So we want to convert that to liters, or this to milliliters. I like to convert things to, how do we do that? 1,000 milliliters. So the molarity of NaOH we've got here. So let's figure out how many moles are in this many liters of NaOH that we're doing next. So how do I do that? I've got per liter here. I've got liter there. So all I've got to do is take this number and multiply it by that thing. Because this is, of course, liters of NaOH. Doing that should give us the number of moles. So this one's going to be a 3. So 0.0. Does everybody OK to that point? We've got the moles. So from here, we've got moles of NaOH. We've got the reaction equation, and we've got the moles or volume of acetic acid. So remember, to get the molarity of acetic acid, we need moles of acetic acid. So from here, we should be able to get the moles of acetic acid using some conversion factor. That conversion factor, of course, you all are about to tell me is the reaction equation. I know, so I'll save you the trouble. So 1 mole of NaOH from the reaction equation gives 1 mole of C2H4O2, which is acetic acid. So what are the 6 mils here? So how do I figure out what the molarity is? So remember, the molarity is the number of moles of C2H4O2 divided by the number of liters of C2H4O2. And we have both of those numbers now. Correct? Yes. Thank you. So 0.0250 liters, 0.018, the C2H4O2, because that's a different problem. It's a different problem. So this gives you the number. This starts you with the molarity of NaOH. The thing is, if you don't have, you haven't converted from acetic acid to NaOH. The only reason they're the same, as you're putting the same, is because the reaction equation is a one-to-one mole of ratio. So if you do that for every one of these problems, you'll get them wrong, because you need to use that balanced reaction equation. I would say, yes, it does matter a lot, because you're not converting the units. So if you want to think it doesn't matter, then yes, for a one-to-one balanced equation, it doesn't matter at all. But it does matter a lot. Yes. What do you use other equations for? So when you're not in touch. So let's say something to the effect of, like, the other M1A1 equation, like, if you have this concentration of HCl, what, how many mills of H concentrated HCl would you need to have this other dilute concentration of HCl? So it's the same molecule, if you understand. As opposed to this, as you're talking about the acid referring to the base, right? So you have to titrate them. OK, so it's a totally, totally different problem. Like, I promise you, I know you want it to be the same problem, but I promise you, it's a way different. It just happens to work out to be the same in this particular problem. Promise.