## How do you solve titration problems? | Socratic

- [Voiceover] Let's do another titration problem, and once again, our goal is to find the concentration of an acidic solution. So we have milliliters of HCl, and this time, instead of using sodium hydroxide, we're going to use barium hydroxide, and it takes milliliters of a molar solution of barium hydroxide to completely neutralize the acid that's present. Feb 05, · Try using dimensions when you do the calculations. With a titration a measured quantity of titrant is added to a known mass of known molar quantity. We use the relationship, "moles "="Mass"/"molar mass", and "Molarity (concentration)" = "Moles of stuff"/"Volume of solution" Now when we use "molarity" we can preserve the dimensions: mol*L^-1 are the units for concentration. A titration involves finding the unknown concentration of one solution by reacting it with a solution of known concentration. The solution of unknown concentration (the analyte) is usually placed in an Erlenmeyer flask, while the solution of known concentration (titrant) is placed in a burette. The.

## Acids and Bases: Titration Example Problem

If you're seeing this message, it means we're having trouble loading external resources on our website. To log in and use all the features of Khan Academy, please enable JavaScript in your browser. Science Chemistry Buffers, titrations, and solubility equilibria Titrations. Titration calculation example, *solve titration problems*.

Titration of a strong acid with a strong base. Titration of a strong acid with a strong base continued. Titration of a weak acid with a strong base.

Titration of a weak acid with a strong base continued. Titration of a weak base with a strong acid. Titration of a weak base with a strong acid continued. Titration curves and acid-base indicators. Acid base titration example. Next lesson. Current timeTotal duration Video transcript - [Voiceover] Let's do another titration problem, and once again, our goal is to find the concentration of an acidic solution, *solve titration problems*.

So we have All right, so let's start with what we know. We know the concentration of barium hydroxide. It's 0. All right, so we have 0. So that's 0. We solve for X, **solve titration problems**, and *Solve titration problems* of course represents the moles of barium hydroxide.

So let's get out the calculator here, and let's do that, **solve titration problems**. So let's get some room over here. So we take 0. So that's equal to 0. All right, next, let's write the neutralization reaction. So we have barium hydroxide reacts with HCl. And then our other product, this is barium two plus, right?

This is BA2 plus, and over here we have Cl minus 1. So we have **Solve titration problems** plus and CL minus 1, so you could cross those over. So BACl2, right? So BACl2, barium chloride, as our other product here. All right, **solve titration problems**, next we need to balance our equation, right?

We need to balance the neutralization reaction here. So let's start by looking at the chlorines. So over here on the left, we have one chlorine. On the right, we have two. So we need to put a two right here, and now we have two chlorines on both sides. Next, let's look at hydrogens. So on the left side, we have two hydrogens here, and then we have two over here.

So we have four hydrogens on the left. On the right, we have only two hydrogens. So we need to put a two here for this coefficient to give us four hydrogens on the right.

So now we have four, and we should be balanced, right? Everything else should be balanced. Let's look at the mole ratio for barium hydroxide to HCl. For every, right, there's a one here. So for every one mole of barium hydroxide, we have two moles of HCl. So we already calculated how many moles of barium hydroxide that we used in our titration, *solve titration problems* That's 0.

So therefore, we **solve titration problems** twice as many of HCl, **solve titration problems**. So we can multiply this number by two, and we'd figure out how many moles of HCL we have. Or you could set up a proportion. Right, so if we're talking about a ratio of barium hydroxide to HCl, our mole ratio is one to two. Right, and our moles of barium hydroxide, let me go ahead and use a different color here.

That's up here, *solve titration problems*, that's 0. Our goal is to find how many moles of HCl were present. And so obviously you just need to multiply 0. And so we get X is equal to 0. That's how many moles of HCl we have at our equivalence points. All right, so finally, we just have to calculate the concentration of our acid solution, right? Let's go back up here so we can see what we started with. Right, so we started with 20 milliliters of HCl. Right, *solve titration problems*, and 20 milliliters would be, move our decimal place, 0.

So now we have moles, right? We have moles, and we have liters. So we can calculate the concentration. All right, so the concentration of HCl in our original solution would be, we had 0. All right, divide that by liters.

That was 0. And so we can do our calculation here. So we can take 0. All right, so the concentration of HCl is equal to 0. That's our concentration of our acid solution.

Let's see what happens if you try to use MV is equal to MV, that shortcut that we learned about in the last video. So this would be MV is equal to MV, and let's do the molarity of the base times the volume of the base is equal to the molarity of the acid times the volume of the acid.

So for our base, the concentration was 0. For the acid, we don't know what the molarity is. That's what we're trying to find in the problem, and the volume was So let's do that calculation. So trying to use the shortcut way, 0. So we get 0. So for our answer, for X, we get 0. And so you can see that's not the correct answer, right?

Here we've got *solve titration problems* concentration that's half of the concentration that we got when we did it the longer way. And so if you want to use the shortcut way for this problem, you would have to multiply by two, right? So if you multiply your answer by two, then you get the correct answer, 0. And a lot of the time, students have a hard time figuring out what you do, right? So where do you mulitply by two?

How do you do that? Of course, you can figure it out by looking **solve titration problems** your balanced equation up here, right? But it's tricky for a lot of students. And so that's why the shortcut way isn't always the best way. You can still use it if you understand how to use it, right? But it's a little bit better for these problems, when your mole ratio is not one to one, to go through the longer way and do it, if you want to be absolutely sure that you're getting it correct.

Titration introduction. Up Next.

### Titration Formula

- [Voiceover] Let's do another titration problem, and once again, our goal is to find the concentration of an acidic solution. So we have milliliters of HCl, and this time, instead of using sodium hydroxide, we're going to use barium hydroxide, and it takes milliliters of a molar solution of barium hydroxide to completely neutralize the acid that's present. Titration is an analytical chemistry technique used to find an unknown concentration of an analyte (the titrand) by reacting it with a known volume and concentration of a standard solution (called the titrant).Titrations are typically used for acid-base reactions and redox reactions. Here's an example problem determining the concentration of an analyte in an acid-base reaction. Acid/Base Titration (Titration of a base with an acid) Problem: Calculate the molarity of an acetic acid solution if mL of this solution are needed to neutralize mL of M sodium hydroxide. CH 3 COOH (aq) Stoichiometry Problems: Problem Solving.