 Okay, so let's attempt to do this last portion of the problem. So again, we're finding the pH during a weak acid strong base titration, but this is after the equivalence point, so we have more base than acid, like more moles of base than moles of acid at this point in time. So we'll just reread it says calculate the pH during the titration of 40 mils of 0.100 molar propanoic acid, Ka1.3 times 10 to the negative 5 after each, or after the following volume 50 mils of 0.100 molar NaOH has been added. So from these volumes and concentrations, we should be able to get the number of moles. So if you remember from our last calculation, the number of moles of the propanoic acid here 0.005000 moles, okay, so remember what I was saying, you want to compare moles to moles on all of these things. So we'll do a quick ice table, okay, even though I know you guys can see that all of the moles of acid are used up, we'll just show it explicitly, okay. So first ice table you guys have been writing down here, 0.004000, and we're going to, oh we started out here, 0.005000, and zero there. So with this being the limiting reagent now, we can only subtract that much of this. Does that make sense to everybody? Okay, so we're going to subtract 0.004, like that, to get zero there, and back to get 0.001, zero, zero, zero, like that. Is everybody okay with that number of moles? Okay, so we could now figure out what the molarity of the hydroxide ion concentration is, okay. Why? Because we have the number of moles of hydroxide, right, this is moles? Sodium hydroxide or hydroxide ions, okay, so the concentration of the hydroxide is going to be, well, the number of moles divided by what, the total volume, right? So what's the total volume? 50 plus 40 mils, so 90 mils for 0.0900 liters, like that, okay. So moles divided by liters, that equals molarity, right, so 1, 1, 1, 1, molar, NaOH or OH minus. So we could do this a number of ways. I'm just going to use the KW, since that's my favorite way of doing it. So remember, KW equals the concentration of H3O plus times the concentration of OH minus. Is that okay? So H3O plus equals KW divided by concentration of OH minus. Do we have both of those things? Yes, right, so that equals 1.0 times 10 to the negative 14 divided by 0.01111. The negative 13th molar, okay, so how do I get the pH from that? The pH is going to be the negative log of the H3O plus concentration. So negative log, 12.05. Easy enough, right? That one, hopefully you think was easier than the other ones. Are there any questions on this one before I let you guys go? Okay, wonderful. Thank you. Okay, have a good one, guys. Have a good weekend. I'll see you next time.