 So, let's do that same problem now, but instead of figuring out the molarity of the two ions, we'll figure out the equivalence per liter of the two ions, okay? So equivalence is the same thing as moles, but it's moles of charge, okay? So, if we think about, like, our ions here, right, when we say we've got one mole of sodium ions, that means we have one equivalent of charge, okay? Why? Because sodium only has one charge per ion, is that cool with everybody? So we say we have one equivalent of charge. Say we have one mole of phosphate ions, phosphate ions, we have three charges, okay? Three equivalence charges, you can further identify things if you want to, okay? But for right now, we're just wondering about equivalence altogether. Instead of the molarity of the two ions, what are the equivalence of charge of those two ions? So, in this case, concentration of those things, but the equivalence of charge of sodium, right, and the equivalence of the charge of phosphate. And we still use this, we still use this, and we still, and now we need to use this too, okay? But are you okay? Can you see the step, step, step, okay? So, to figure out the equivalence of sodium ions, we have to figure, we have to know the concentration of sodium phosphate to begin with. We know that one mole of sodium phosphate here of solution. We also know the number of moles of sodium phosphate to the number of moles of sodium ions that was given to us from the reaction equation that you had to figure out. All of this was based on you knowing the charge of this phosphate on it, okay? So, remember that. Okay? So, just another conversion factor, on the bottom, what's going to be on the bottom? One mole of sodium phosphate, right, and on the top, three moles, no, we still will need one more step, right? So, for every, I'm kind of getting into that, but, so for every one equivalent of charge, one mole can handle with that, right now. We get these units now that are equivalents of charge per liter. Do you guys see that? Okay? And then we just do one times three times one, which is three divided by one. So, this equals three equivalents per liter. Okay? So, that's the way to say that. And if you want to even further emphasize that, okay, it's the same thing, okay? It's what we've done here because I don't have very much room on this board, okay? You guys can watch the video. Equivalents of sodium, we're going to do equivalents of phosphate. And we have to start with the same concentration, right? We'll write it again. We'll do the whole step by step by step again. Okay? And remember, so we're looking for equivalents of charge, so we've got to get there. But we've got to start here. One mole of phosphate, liter of solution, right, multiply that by the conversion factor because we're looking for, eventually, equivalents of charge from the phosphate amount. So, we don't have that other conversion factor up here. What is it? One mole. So, we just got to do it one more time because we've got the conversion factor that changes one to the other and it's also going to be what? That makes sense, hopefully, in three equivalents per liter you want to think about. It makes sense because the charges always have to balance, right? But you knew that all the way from, are there any questions on this stuff? Okay, so the next step is, you know, just keep going to the next step, you know, like molarity, molality or whatever, you know? So, you just got to keep finding these step by step by step things, you know, in order to convert one to the other. So, you just got to keep remembering, you know, this step will convert this to this and not this to this. Okay?