 Okay, yeah, so let's try this on the, why does one mole of calcium chloride lower the freezing point of water more than one mole of sodium chloride? Well, in this problem, you're going to have to figure out the osmolarity of these two compounds, right? So the osmolarity of calcium chloride is, well, we got one mole, and we'll just pretend it's per liter, okay, per the molarity. So one mole per liter. So we've got to do the osmolarity of calcium chloride smaller, because the Ca2 plus aqueous plus 2Ci minus aqueous. So that's a one to three, right? So we're going to have three moles of the particles, product particles, to one mole, calcium chloride. Of course, calcium chloride cancels, and we've got three osmolar particles for the first solution. And if we calculate the osmolarity of sodium chloride, we say one mole of sodium chloride to one liter. And if we look at sodium chloride, it's NaCl solid goes to Na plus aqueous plus Cl minus aqueous. So that's a one to two ratio of particles. So we're going to have two mole particles here for every one mole NaCl. Small NaCl cancels. And we get two osmolar particles. So the higher osmolarity is going to lower the freezing point more. So this one has a higher osmolarity. So that's why one mole of calcium chloride lowers the freezing point of water more than one mole of sodium chloride, since this has to be lower. So you can check that out. Thank you, sir.