 Okay, let's do our first neutralization reaction. So we'll use this same acid, the ammonium ion, okay, so neutralization reactions happens when acids react with bases, okay. Things that have negative charges are bases, okay. Things that have positive charges are acids, almost free polymers, okay. And in this class, though, all is free, okay, introductory, all is free. Anyways, so, things, molecules don't like to have a charge, okay. They will if they have to, but they don't like it, okay. So, this guy here has a positive charge, he don't like it, right. This guy here has a negative charge, he don't like it. This guy here, as we learned before, wants, likes to give up that proton, right. And this guy here, if he got that proton, would become water, right. Become a very stable molecule. So, it's to each other's benefit to transfer this proton, okay. So what happens is a proton transfer or a neutralization reaction. A neutralization reaction happens when a base reacts with an acid, okay. So watch, base reacting with acid. That is the equilibrium is going to lie to this side, you know how it's going to go that way. Why? Because these are relatively unstable relative to the products. Why the products are not charged, okay, the reactants are charged. So what are the products going to be? Can anybody help me? In H3, with its lone pair of electrons there, right. And H2O, how many lone pairs will the oxygen have? Two. So what you want to think of is that these, this lone pair here, no, I should have done different ones. That lone pair there made that bond there, okay. So is that cool with everybody? Does everybody understand? So this thing's called an acid. So remember, an acid has a conjugate base. It's the same structure without that problem. So which one of these over here on the right or on the left is the conjugate base of the ammonium model? H3 or ammonium. So I'll put you right down here, conjugate base. And every base has a conjugate acid, okay. And that's just the base plus the proton. I'm going to erase this one. So it's the base plus the proton. So that's the conjugate acid. You could think of it the opposite way too though, right. But if we wrote this over here and this over here, right, then this would be the acid, this would be the base, this would be the conjugate base, and this would be the conjugate acid. So it all depends on which way you write the thing, okay. Acid-base reactions, because they're in equilibrium, go back and forth. I know we didn't do any problem also with Châtelier's principle, but we didn't do many problems. But what'll happen is, you know, we can push this equilibrium back and forth depending on what we put in, okay. If we put in a lot of this, it'll go this way. But if it's just like this, right, these are less stable than these. So it's going to want to push the reaction natural. Are there any questions on this? You guys get this?