Titration calculation 2 - calculating volume
Summary
TLDRIn this educational video, Chris Harris from Adobe teachers.com guides viewers through a titration calculation involving a solid sample, calcium carbonate, and sulfuric acid. He meticulously explains the process of determining the volume of acid required for neutralization. Key steps include calculating moles of calcium carbonate from its mass and molecular weight, using the molar ratio to find moles of sulfuric acid, and then calculating the volume of acid needed. The video also touches on unit conversion from decimeters cubed to centimeters cubed, emphasizing the importance of understanding mole equations and molar ratios in chemistry.
Takeaways
- 🔍 Chris Harris introduces a video on titration calculations, focusing on a specific example involving a solid sample.
- 🧪 The example involves titrating solid calcium carbonate with sulfuric acid to determine the volume of acid required.
- 📚 A previous video, 'Titration Calculation One', covers calculating the concentration of a known volume of solution.
- 📉 The reaction between calcium carbonate and sulfuric acid produces calcium sulfate, water, and carbon dioxide.
- 🔬 The practical setup includes a burette with sulfuric acid and a conical flask containing calcium carbonate.
- 🧮 The first step in the calculation is to determine the moles of calcium carbonate from its mass and molecular weight.
- 📐 The molar ratio between calcium carbonate and sulfuric acid is 1:1, simplifying the calculation of moles of sulfuric acid needed.
- 📘 The volume of sulfuric acid is calculated using the formula: volume = moles / concentration.
- 🔄 Conversion from decimeters cubed to centimeters cubed is necessary to match the units requested in the problem.
- 📝 The final calculation results in a volume of 30 centimeters cubed of sulfuric acid needed to neutralize the calcium carbonate.
Q & A
What is the main topic of the video?
-The main topic of the video is titration calculation, specifically focusing on calculating the volume of acid required to neutralize a solid amount of calcium carbonate.
Who is the presenter of the video?
-The presenter of the video is Chris Harris from Adobe teachers.com.
What is the chemical reaction between calcium carbonate and sulfuric acid?
-Calcium carbonate reacts with sulfuric acid to form calcium sulfate, water, and carbon dioxide.
What is the molar mass of calcium carbonate used in the calculation?
-The molar mass of calcium carbonate (CaCO3) is 100 grams per mole.
How many moles of calcium carbonate are present in 0.75 grams?
-The number of moles of calcium carbonate in 0.75 grams is 7.5 times by 10 to the minus 3 moles.
What is the molar ratio of calcium carbonate to sulfuric acid in this reaction?
-The molar ratio of calcium carbonate to sulfuric acid in this reaction is 1:1.
What is the concentration of sulfuric acid used in the titration?
-The concentration of sulfuric acid used in the titration is 0.25 moles per decimeter cubed.
How is the volume of sulfuric acid calculated?
-The volume of sulfuric acid is calculated by dividing the number of moles by the concentration of the acid.
What is the volume of sulfuric acid needed to neutralize 0.75 grams of calcium carbonate?
-The volume of sulfuric acid needed to neutralize 0.75 grams of calcium carbonate is 0.03 decimeters cubed.
How is the volume converted from decimeters cubed to centimeters cubed?
-To convert the volume from decimeters cubed to centimeters cubed, multiply by 1000 or shift the decimal point three places to the right.
What is the final volume of sulfuric acid required in centimeters cubed?
-The final volume of sulfuric acid required to neutralize the calcium carbonate is 30 centimeters cubed.
What is the importance of knowing mole equations in titration calculations?
-Knowing mole equations is crucial in titration calculations as it allows you to determine the number of moles of reactants and products, which is essential for calculating volumes and concentrations.
Outlines
🧪 Introduction to Titration Calculation
Chris Harris from Adobe teachers.com introduces a video on titration calculations, focusing on a specific example involving a solid sample, calcium carbonate, reacting with sulfuric acid. The video aims to provide a detailed walkthrough of the titration process, explaining the calculations involved in determining the volume of acid required to neutralize the solid calcium carbonate. The reaction equation is provided, showing the formation of calcium sulfate, water, and carbon dioxide. The setup includes a conical flask with calcium carbonate and a burette containing sulfuric acid. The process involves adding sulfuric acid until a neutral solution is reached, indicating the volume of acid used. The first step in the calculation is to determine the moles of calcium carbonate from its mass and molecular weight.
📏 Calculating Moles and Volume of Acid
The second paragraph delves into the calculation of moles of calcium carbonate, using the mass of 0.75 grams and its molecular weight to find 7.5 x 10^-3 moles. It then explains the use of the molar ratio to determine the moles of sulfuric acid, which is the same as that of calcium carbonate due to the 1:1 ratio in the reaction. The final step is to calculate the volume of sulfuric acid required, using the formula volume = moles / concentration. With 7.5 x 10^-3 moles and a concentration of 0.25 moles per decimeter cubed, the volume is calculated to be 0.03 decimeters cubed. The video then covers the conversion of this volume to centimeters cubed, resulting in 30 centimeters cubed. The importance of understanding mole equations for solids and solutions, as well as the use of molar ratios, is emphasized.
Mindmap
Keywords
💡Titration
💡Moles
💡Calcium Carbonate
💡Sulfuric Acid
💡Molar Ratio
💡Concentration
💡Neutralization
💡Volume
💡Buret
💡Molecular Mass
💡Unit Conversion
Highlights
Introduction to titration calculation with a solid sample
Detailed explanation of titration calculation process
Example of titration with calcium carbonate and sulfuric acid
Equation for the reaction between calcium carbonate and sulfuric acid
Practical setup for titration with a solid sample
Importance of calculating moles in titration
Explanation of mole calculation for calcium carbonate
Use of molar mass to calculate moles
Calculation of moles of calcium carbonate
Molar ratio and its application in titration
Calculation of moles of sulfuric acid
Conversion of moles to volume using concentration
Calculation of volume of sulfuric acid needed
Conversion of volume from decimeters cubed to centimeters cubed
Final volume of acid required to neutralize calcium carbonate
Emphasis on understanding mole equations for solids and solutions
Summary of key steps in titration calculation
Transcripts
[Music]
thank you
hi there my name is Chris Harris and I'm
from Adobe teachers.com and welcome to
this video on titration calculation 2.
so in this video we're going to go
through another example of a titration
calculation uh we're going to go through
a worked example and I'm going to try to
go through in as much detail as I can to
explain how we calculate it and why we
calculate it as well okay so um this
example we're going to be actually
looking at a titration with a solid
sample in the conical flask
um instead of a a quite traditional
solution that you might have in there
and we're actually going to be
calculating
as you can see on here we're going to be
calculating what volume of acid is
required to neutralize a solid amount of
calcium carbonate now the there is
another video called titration
calculation one uh that looks into
calculating the concentration of an a
known volume of solution in the conical
flask so if you want to have a look at
that video we just click on the link
below and you can have a look at it
there okay so let's get started so it
says 0.75 grams of calcium carbonate
reacts with 0.25 moles per DM cubed of
sulfuric acid what volume and I've got
in centimeters cubed our acid will be
needed to neutralize calcium carbonate
and we've got the equation written down
here for us which is nice and handy so
CaCO3 calcium carbonate plus sulfuric
acid will form calcium sulfate water and
carbon dioxide so just a standard uh
acid base reaction reacting with the
carbonate to form carbon dioxide as well
so we've got our practical setup here
just to see how it would look and we've
got our type our buret so which is over
here and the buret contains 0.25 moles
per DM cubed of sulfuric acid
and this is contains in Opus in an
iconic or fast Square 0.75 grams of
calcium carbonate and it's really simple
all we're going to do is add the
sulfuric acid and we would have some
kind of indicator in there as well to
keep adding it until we get a neutral
solution in which case we work out the
volume of acid that we needed to add so
and the first thing we need to do is to
work out moles and with all titrations
you need to work out the moles first and
I've got a saying where if in doubt work
out the moles because from the moles you
can work out loads of different things
now if you don't know how to calculate
moles you're not confident on the
equations to do with moles then I have
done a video looking at mole equations
so we just click on the link below and
you can have a look at that video then
but for this video we're going to assume
you know how to do them so the first
thing we need to do is work out the
number of moles of calcium carbonate and
the reason why we do that is because we
have a mass of calcium carbonate
um
and we know it's Mr as well we can work
out it's Mr and from that we can work
out the moles so let's get started so
we'll write this in blue I think so we
do the number of moles of calcium
carbonate is the mass which is
0.75 grams and we're going to divide
that by the molecular mass which is 100
and you calculate that from the periodic
table and then if you put that into your
calculator you should get 7.5 Times by
10 to the minus 3 moles
thank you
okay so that's the amount of moles of
calcium carbonate now we need to work
out the number balls of calcium
carbonate because actually from this we
can work up the moles of anything on
this equation by using the molar ratio
now we need to work out the volume of
sulfuric acid so actually we need to
work out the number of moles of sulfuric
acid in this reaction and because it's a
one-to-one ratio it's the same number of
moles so we're just going to put 7.5
Times by 10 to the minus 3 moles
okay so this is the number of moles of
sulfuric acid
okay now we've worked out the number of
moles we now then need to work out the
volume now we need to use a different
mole equation here and the different
mole equation is actually
um the solution one because we're
dealing with a solution so to work out
the volume and we'll write this down
here so the volume
is actually the number of moles divided
by the concentration
um
okay and so this is to do with sulfuric
acid so we know the moles and we know
the concentration because we've been
told the concentration of sulfuric acid
is 0.25 moles per decimeters cubed and
then from that obviously we can work out
our volume so if we put them numbers in
so our moles is 7.5 Times by 10 to the
minus 3 divide that by the concentration
which is 0.25
okay and then if we put that in our
calculator and we should get a value of
0.03
okay now the volume of this is
decimeters cubed and all volumes in
these calculations are in decimeters
cubed so we're just going to put that on
there
okay so you can see that this is
obviously
um not the final answer not quite
because it did say what volume in
centimeters cubed we need to do so we
need to be able to convert this back
into centimeters cubed now if you're not
sure on how to convert units which is a
very very important skill that you need
to be able to do in chemistry now I have
done a video looking at converting units
so we just click on the link below and
you can have a look at that one but um
basically you should convert this in
centimeters cubed we just need to
multiply by 1000 and we should get it in
centimeters cubed so we don't need a
calculator for this really just shift
the decimal point to the right three
places and we get 30 centimeters cubed
okay so that is the volume of
um that is the volume of acid that we
needed to average 30 centimeters cubes
to neutralize our carbonate but um there
we go it's pretty much as simple as that
just I suppose the important things are
you need to know your mole equations
both solid and for Solutions as well and
you need to know how to use your molar
ratio in your equation but that's it
bye-bye
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