Titration calculation 2 - calculating volume

Summary

In 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

00:00

🧪 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.

05:01

📏 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.

Keywords

💡Titration

Titration is a laboratory method used to find the concentration of an unknown solution by reacting it with a solution of known concentration. In the video, titration is the main focus as the presenter explains how to calculate the volume of acid needed to neutralize a solid sample of calcium carbonate. The example provided is a titration involving a solid sample, which is a deviation from the more common liquid titrants.

💡Moles

Moles are a fundamental concept in chemistry, representing the amount of a substance in terms of its quantity of atoms or molecules. In the video, the presenter calculates the moles of calcium carbonate from its mass and molecular weight, which is essential for determining the reaction's stoichiometry and calculating the required volume of acid.

💡Calcium Carbonate

Calcium carbonate is a chemical compound with the formula CaCO3. It is the main reactant in the titration example discussed in the video. The presenter calculates the moles of calcium carbonate to determine how much acid is needed to neutralize it completely.

💡Sulfuric Acid

Sulfuric acid is a strong mineral acid with the molecular formula H2SO4. In the video, sulfuric acid is the titrant used to react with calcium carbonate. The concentration of sulfuric acid is given as 0.25 moles per decimeter cubed, which is crucial for calculating the volume needed to neutralize the calcium carbonate.

💡Molar Ratio

The molar ratio is the ratio of the amounts of substances reacting in a chemical reaction. In the video, the molar ratio is used to determine the stoichiometry of the reaction between calcium carbonate and sulfuric acid, which is a 1:1 ratio, meaning one mole of calcium carbonate reacts with one mole of sulfuric acid.

💡Concentration

Concentration in chemistry refers to the amount of a substance in a given volume of solution. The video explains how to use the concentration of sulfuric acid to calculate the volume required to neutralize a known mass of calcium carbonate.

💡Neutralization

Neutralization is a chemical reaction in which an acid and a base react to form a salt and water. In the context of the video, neutralization refers to the reaction between sulfuric acid and calcium carbonate to form calcium sulfate, water, and carbon dioxide.

💡Volume

Volume in the context of the video refers to the amount of space occupied by a substance, specifically the volume of sulfuric acid needed to neutralize calcium carbonate. The presenter calculates the volume of acid in decimeters cubed and then converts it to centimeters cubed.

💡Buret

A buret is a piece of laboratory equipment used to dispense precise volumes of a solution. In the video, the buret contains the sulfuric acid solution that is added to the calcium carbonate until neutralization is achieved.

💡Molecular Mass

Molecular mass is the mass of one mole of a substance and is calculated by summing the atomic masses of all atoms in a molecule. In the video, the presenter uses the molecular mass of calcium carbonate to convert its mass to moles.

💡Unit Conversion

Unit conversion is the process of changing the units of a measurement to a different type of unit. In the video, the presenter demonstrates how to convert the volume of sulfuric acid from decimeters cubed to centimeters cubed, which is a common practice in scientific calculations.

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