 Okay, so this one's a molarity problem, the first molarity problem that you guys saw on some sort of quiz or exam this semester, but it says what volume of a 12.0 molar HCl solution is needed to provide 0.60 moles of HCl? So it gives us the concentration of HCl solution, molar HCl, and it also says that you want to have 0.60 moles of HCl. So it's wondering what is the volume of this HCl solution that you're going to need to get 0.6 moles in? Does everybody understand the question? So when we do that, all we got to remember is what we're going to be doing is using these kind of conversion factors. Okay, so I'm going to start with that moles of HCl that the problem gives us. Okay, but here we got to remember that big M is moles per liter, right? So this means 12.0 moles of HCl per one liter of HCl solution. Okay, so when we look at that, right, so we're looking for a volume, so liters, or I think in this case we're going to get it in milliliters. We've got the conversion factor that we need to do that already. So what we're going to do is put the moles, of course, on the bottom to cancel that. One liter of the HCl solution on top, and then again, like I said, it gives you a few options, but one of the option that is the right answer is in milliliters. So one liter of the HCl solution is 1000 mls of the HCl solution. Just go ahead, in terms of 1000. I guess we're going to take a look at that. To two sig figs, right? So you're going to put the decimal point there. Mls of the 12.0 mole or HCl solution. So again, you're just using that polarity as another conversion factor from moles per liter of your particular solution. Any questions going on?