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### Course: AP®︎/College Chemistry > Unit 13

Lesson 2: Titrations- Acid–base titrations
- Worked example: Determining solute concentration by acid–base titration
- 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)
- 2015 AP Chemistry free response 3b
- 2015 AP Chemistry free response 3c
- 2015 AP Chemistry free response 3d
- 2015 AP Chemistry free response 3e
- 2015 AP Chemistry free response 3f
- Titration curves and acid-base indicators
- Redox titrations

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# 2015 AP Chemistry free response 3b

Calculating the concentration of weak base using information about equivalence point in a titration. From 2015 AP Chemistry free response 3b.

## Want to join the conversation?

- why isn't the 45 mL added to the 29.95 mL of HCl?(2 votes)
- That wouldn’t help solve the question at hand.

It asks for the concentration of the stock solution, ie before mixing them.(1 vote)

- In case of a Diprotic or Any Acid which isnt Monoprotic, we will need to equate no. of Equivalents, right?(2 votes)
- How do you find out how many digits to round to?(1 vote)
- Relevant KhanAcademy information is here:

https://www.khanacademy.org/math/arithmetic-home/arith-review-decimals#arithmetic-significant-figures-tutorial(4 votes)

- Instead of calculating for moles with three sig figs before dividing by the total volume, can you just calculate for everything in the same equation like [(29.95 mL)(1L/1000 mL)(1 mol KC6H7O2/1mol HCl)]/(.02995 L) to get a four sig fig answer? If not, why?(1 vote)
- Where's the molarity of HCl in your equation? That's why it is to 3sf not 4sf.(1 vote)

- Titration- Good day khanacad, please teach me on how to prepare for example 0.5M HCl acid solution for titration purpose(0 votes)

## Video transcript

- [Voiceover] A total of 29.95 milliliters of 1.25 molar hydrochloric
acid is required to reach the equivalence point. Calculate the concentration
of potassium sorbate, we put the brackets, so we're
talking about concentration, in the stock solution. So let's juts remind ourselves what the equivalence point is. The equivalence point
is the point at which all of the potassium sorbate has reacted with the acid, with the titrate. So, we have just gotten
to the right-hand side of this net ionic equation. So, another way to think about it is, it's the point in which,
because we are reacting, for every mole of the potassium sorbate that we want to turn into sorbic acid, we're adding a mole of
the hydrochloric acid. So, one way to think about
the equivalence point is if I've added a certain number of moles of hydrochloric acid, that must the exact number of moles of the potassium sorbate
that we started out with. We've added the exact number of molecules of hydrochloric acid as they originally were of potassium sorbate, so they can completely
cancel out with each other. So if we can figure out
the number of moles, if we can figure out the number of moles of hydrochloric acid here, then we could say, "Well,
the equivalence point", or if you needed that number of moles of hydrochloric acid to
reach the equivalent point, then that means your
original stock solution had that many moles of potassium sorbate, and then we can use that to calculate the actual concentration. So let's do the first part, let's think about how many
moles of hydrochloric acid, this is right over here, so I'll just write HCl, and so, if we have 29.95 milliliters, and let's just convert it into liters, because if we have, if our concentration is
given in terms of molarity, this is moles per liter, so let's make sure we get our units right, so let's multiply this times, so we wanna convert this to liters, so we want liters in the numerator, and milliliters in the
denominator, so these cancel out, so one liter's equal to 1000 milliliters, and that makes sense, if you wanna go from
milliliters to liters, you would multiply by
1000, or divide by 1000. So this would give us the total amount of hydrochloric acid solution
we've added in liters, and now let's figure out
how many moles that will be. Well, we multiply that times the molarity, times 1.25, instead of writing molar capital M, I'm gonna write 1.25 moles per liter, and what is this going to give us? Well, let me get my calculator out, and so, I'm gonna have 29.95 divided by 1000, (mumbling) right there, times 1.25, times 1.25 is equal to, and let's see, I have three significant
figures here, four over here, so the product, I'm gonna have three, so 0.0374, 0.0374, and the unit is all work out, milliliters cancels out with milliliters, liters cancel out with liters, and I have 0.0374 moles, and remember this is moles
of hydrochloric acid, so when they say that a
total of 29.95 milliliters of 1.25 molar solution of
hydrochloric acid is added, they really added this many
moles of hydrochloric acid. So, that means our original solution had that many moles of potassium sorbate. So it had that many moles
of potassium sorbate, we can now figure out the
original concentration of potassium sorbate. The concentration of our potassium sorbate C6H7O2 is going to be equal
to the number of moles of potassium sorbate our stock
solution starts off with, so that's going to be the
same number right over here, 0.0374 moles divided by what was our original volume
of our original solution? Let's see. A student titrates 45.00, so we have four significant figures here, a student titrates 45 milliliters
of the stock solution. So the stock solution originally has a volume of 45 milliliters. So 45 milliliters, if we wanted to write
that in terms of liters, remember, the concentration,
the molarity here, we wanted it in terms of mole per liter, 45 milliliters is the same thing as 0.045, I can write zero there so that I have four
significant figures here, liters of solution, and what is this going to be equal to, and I just divided this by 1000, 45 milliliters is the same thing
as 45 thousands of a liter. And so, what do we have? We'll take that number we just had, and then we divided it by .045, and I can add two more zeros there, but form the calculator point of view it doesn't make a difference, and that's going to be equal to, all right, how many
significant figures do we have? We have three significant figures, so 0.832, 0.832, 0.832 moles per liter, or we could say 0.832 molar,
did I write that right? Yeah, 832, and there you have it, that's the initial concentration
of the potassium sorbate in our stock solution.