So in this video, we're going to take a look at strong base strong acid titrations. Now we're going to say here that in a strong base strong acid titration, we're going to see that the initial compound represents our analyte and we're going to make this second structure our hydrate. Now we're going to say whenever we have a strong acid or strong base, we never use an ICE chart. Remember, ICE charts are used predominantly for weak acids and weak bases because they don't dissociate 100%. We use an ICE chart to determine what their concentrations are at equilibrium. And from there, we can figure out pH or pOH.

Now whenever we titrate 2 species, like in this case, a strong acid and a strong base, then we use what's called an ICF chart, and it uses the units of moles. Now remember, an ICE chart stands for Initial Change Equilibrium. And when we have 2 strong species titrating one another, we're going to use an ICF and this stands for Initial Change Final. Now the following roadmap is what we're going to use whenever we have a strong acid to strong base titration.

So first, we start out with the equivalence volume, the volume that's necessary to get to the equivalence point between these two substances. Now we're going to say we calculate the equivalence volume, \(v_e\), in order to determine the amount of titrant or volume of titrant required to reach the equivalence point. Here we have the titration of 150 ml of 0.100 molar NaOH, which is a strong base, with 0.050 molar nitric acid. Here, nitric acid is acting as our titrant. We're adding it to the NaOH.

Now remember, at the equivalence point, we have equal moles of our acid and our base. At the equivalence point, we could say that molarity of the acid times the volume of the acid equals molarity of the base times the volume of the base. Remember we said at the equivalence point our moles are equal? Well, remember moles equals molarity times volume. So by multiplying these two, that's giving me the moles of acid and by multiplying these two, that's giving me the moles of base. This equation is saying that our moles of acid equals our moles of base, which is true at the equivalence point. We're going to plug in these values. So the molarity of our base NaOH is 0.100. The volume of our base is 150. The molarity of our acid is 0.050 molar, and we don't know what its volume is. Divide both sides by 0.050 molar. See here that our molarities will cancel out and we'll be left with mls, which are the units for our volume. So when we plug that in, that gives us an answer of 300 milliliters. That means it'll take 300 milliliters of our nitric acid in order to reach the equivalence point in terms of this titration. Now we determine the equivalence volume.

Now let's talk about before we've added any strong acid to our mixture. We're going to say here before any of the strong acid titrant is added, we only have a strong base initially. Remember, strong acid strong base dissociate completely. So their concentrations can help us determine the amount of \(H^+\) or \(OH^-\) present. So here we have the titration of 150 ml of 0.100 molar sodium hydroxide with 0 ml of 0.050 molar nitric acid. Notice here we have no strong acid volume being added. So all we have within our jar, within our container, is strong base. Now remember, because it's a strong base, it dissociates completely. So it's going to break up into \(Na^+\) and \(OH^-\) completely. Because it's a strong electrolyte, the concentration of NaOH is equal to the concentration of each ion. So now we have the concentration of \(OH^-\), our hydroxide ion. If you know the concentration of your hydroxide ion, you can calculate pOH because remember pOH equals negative log of \(OH^-\). We plug in this concentration of 0.100. That gives me a pOH of 1. If we know what pOH is, we know what pH is because pH equals 14 minus pOH. So we plug in this one that was for pOH and what we'll see is that our pH equals 13. So here, we're just going through the different steps of our titration between this strong base and this strong acid. At this point, all we have is strong base, so we can easily find the pOH of that solution. Now, as we move on to the next video, we'll talk about what starts to happen as I slowly add my strong acid to my strong base.