How To Do Titration Calculations | Chemical Calculations | Chemistry | FuseSchool
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- Опубліковано 21 сер 2024
- How To Do Titration Calculations | Chemical Calculations | Chemistry | FuseSchool
You should already know how to carry out titration experiments, but if you are unsure you may want to watch this video first: • How To Do Titrations |...
Titration experiments enable you to work out the concentration of an unknown solute, when you know the concentration of another solute.
After carrying out the experiment, you have to do some calculations. In this video, we run through these calculations.
There is an easy formula but learning this does not mean you necessarily understand the process and in your exam you may not get full marks when using the formula. In this video, we take you through the calculations step-by-step to make sure you understand how to do titration calculations.
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NOTE: at 2:00 concentration calculation should say 0.01 / 0.025 = 0.4 mol/dm^3
I checked the answer 10 times
@@HZrelaxview same
Yes, I got 0.4 as well.
In approximately 2 minutes, I finally understood what I couldn't in a month of class.
Glad we could help!
Really true
In a frigging nutshell😂
you sir are a living legend and life saviour to us chemistry failures, thanks a bunch, looks like im not failing anymore! :D
Happy to help!
Idk how you did it but FuseSchool, after a year of doing titrations and just having to copy other people’s answers and calculations, I have finally understood what a titration does and how to calculate such in just 5 minutes. That’s a feat of a great teacher.
That's great! So glad to hear that 🙌
I want fuse schools to be given an award for services towards humanity
Thank you!!
This tbh I agree
I honestly can't articulate how much I appreciate this, I know the vid was posted five years ago but I was so frustrated with this I was about to quit chemistry and now I have a good grasp of this! thank you so much :))))
So great to hear that! Glad it helped!
one of the easiest videos I have ever seen!
Thank you sooo much for these 2 videos!!! They really helped me! You guys are amazing!
Glad they helped 🙂
Ok, this just saved my grade. THANK YOU
Idk why was everyone teaching this topic was making more confused and fuse school just explained it with just 2 examples 👏👏
After 2 years, I can proudly say that I can work out titration and its calculations, thank you!
Amazing, an actual video that straight to the point, shows formulas and explains everything. You just saved my grade on my midterm
Glad to hear that!
For Step 3: Calculate concentration of unknown solution, where did you get 0.5 x 0.02 from for the known solution and where did you get 0.01 divided bt 0.04 from?
This 5 minute video taught me more than the month of titrations I did thank you now I have some hope for my test
No problem! And good luck! 🙌
Thank you so much my school was not helping very much but now I actually understand I was gonna cry in the lab
You just saved me from not passing in just 5 mins. Why can't all lectures make it this easy?!
Thank you!!!
Thanks so much for the positive feedback!
Thanks,, the visualised calculations are totally helpful
Teacher teached this for like 2 damn weeks and I couldn't get a damn. This video was easy to understand and I learnt the calculation almost right after the video. 🙄🙄🙄 Wish I found this dude earlier
thank you i have a titration practical after few hours and after struggling to understand moles for whole night i just found your video and it really helped me...i think im gonna pass.
Glad it was helpful!
and that is how I passed my 30 marks Titration test, boys. Thank you so much FuseSchool!!
Awesome! Glad we could help 🙌
So helpful and easy to understand
my teacher uses a long method called the box where u do a lot of fractions multiplied by each other and i don't even know how to do it this is way simpler thanks
Wonderful!!! Lovely!!! Understood what I couldn't in 3 years of classes. Thanks!
Thank you I finally understand. My chemistry teacher is terrible at explaining things
For the question at 4:30, if the molarity of HCl was wanted while the molarity of Ba(OH)2 had been given, would we multiply the result by 2??
This was really helpful thanks, you make it so easy!
Hi there is an error in the first titration calculation. 0.01/ 0.025 is not 0.04. Also one of the annotations is incorrect in the sulphuric acid titration (same annotation as the first titration). Nice videos though.
Gareth Marks love your corrections its good to be alert
I disagree .01/.025=.04
the answer is 0.4
@@bernardmukenye5863 lol "concentration" how punny
Thanks, I thought I was going mad
Thank you so much I watched so many videos and didn’t understand anything... you broke down everything simple in 5 mins .. thanks for giving me the confidence and understanding to smash these questions now !!
Glad it helped!
2:00
0.01 / 0.025 = 0.04
Nani?
There's an error in that calculation. Well noticed!
@@fuseschool Have you fix the calculation now?
@@karinaroosvita once a video’s out. They won’t be able to fix that calculation without losing lots of views.
@@aquiIa_chrysaetos so ur just gonna leave wrong information published
@@tasangerbakes yeah that’s kinda a really shitty thing to do. Makes me wonder what else they swept under the rug
Thanks for explaining
hey i have the background picture that is your prfile pic
hit like if u have your chemistry practical tomorrow and its already 12.30 AM
no but it is 10pm and I have a test tomorrow
Man.. They have explained this so well compared to my teacher who did but however, used too many incomprehensive terminologies that made it seem more like a set of floating Chinese characters. They also have awesome diction and this dude is an awesome narrator like really.
Wow, thank you so much! Glad you liked it 🙂
Why did you put 0.01 as the moles for the unknown solution? Are the moles of the known and unkown solution same?
We have assumed that in the equation for the reaction, 1 mole of known reacts with 1 mole of unknown. But it could have been 2 to 1 etc.
I feel like i'm the only one who is even more confused now than before I watched the video
Thanks this helped a lot!
thank you lord. I understand more than what our teacher taught us
I COME BACK TO THIS VIDEO ALL THE TIME FOR TITRATION EXERCISES IT'S AMAZING!!!!!
Awesome 😃
teaching nicely in 3 mins mad lad
Cheers 🙌
u explained in 5 mins what i couldn't understand in a whole year
Happy to help ❤️
Uhh the explaining is great! What app do you use to edit your videos? 😉😊😎
Thanks! We use After Effects.
@@fuseschool Np. It really helps me improve. Oh and yes AE is a real game changer for motion designers
Thanks. This was of great help.
Does this apply to ALL types of titrations? Like double titration and redox and everything else?
Thank you very much understood everything. Easier than it was given in my book
Glad it helped!
It was help ful to me
Absolutely amazing videos. Thank you so much :-)
Thank you too! Glad you like them!
my saviour
The most helpful video thank you so much
Glad you think so!
Isnt it 0.4 mol/dm3
Yes it is
You are right. There's an error in that calculation. Well noticed!
this really helped me, my teacher was terrible at explaining to me
Fantastic class
Thanks alot ❤
Always welcome 😊
this guys voice is big brain
This acctually helped
Awesome!
I’m still slightly confused on why the known solution has the same amount of moles than the unknown. That makes zero sense
That is what confused me also
Sometimes the two solutions react one to one, and thus has the same amount of moles.
Thank you so much very helpful!
You're welcome! Glad it helped!
hi guyz that was perfect to me and now I'm charged up with these calculations
This helped a lot, thanks : )
Glad it helped!
Pls check ba(0h)2 is in one mile only so no need of dividing with 2 pls confirm this
you are amazing. thank you
Thank you too!
You can directly give a formula instead of this much explanation (N-a×V-a)=(N-b×V-b) dilution law
Wow perfect 👍👍👍❤
Thank you 😃💜
Thank you
Welcome!
Thank you so so much
You're welcome 😊
You may have forgotten to mention that the first example assumes that you have a 1:1 ratio btw :)
To calculate mass of Na₂CO, in solution, if for titration analysis used 22.00 ml of solution H₂C₂O4 which equivalent concentration is 0.1000 mol/L. Solve it
Can u please make a video on titration for finding alkalinity of water sampla
Too good👍🏻♥️
Thanks a lot 😊
NICE VIDEO
What about when the concentration is given in Normality?
2:02 there is an error it is 0.4
Yes, you are right. Thanks for noticing!
Like your videos
Step 3 tells us to find the molarity of the unknown solution by dividing the moles of the known solution, by the volume of the unknown solution. How does this make sense?
lol at the moment i am wondering that too ?
maybe they assumed that they already know what exactly the substance is in the unknown solution (like in the 2nd example). Therefore, they can write the equation and know the moles ratio of the reactants. So maybe the reactants moles ratio is 1:1. But in the second example, the ratio of sodium hydroxide to sulfuric acid is 2:1 and they still plug the moles of NaOH to H2S04. which is incorrect i think.
How did you get the mole for the unknown at 1:58
For the purposes of this calculation we are assuming that one mole of the known solution reacts with one mole of the unknown, so once you have calculated the number of moles of the known solution that have reacted, this will be the number of moles of unknown. If the two solutions react differently, say 1:2 or 2:3 (it will always be a simple ratio) then you have to include this fact too.
0.01/0.025 is equal to 0.4
I think so too
You are right. There's an error in that calculation. Thanks for noticing!
rip to my homies using liters/mol
First one is wrong
Thank you so god damn much
Most welcome!
at 2:00 is it just me or is the answer wrong for the concentration of the unknown substance. 0.01/0.025 is equal to 0.4 not 0.04
It should be 0.4, you are right! Thanks for noticing!
@@fuseschool thanks for replying.... I thought i missed something out too....I spent the last half hour trying to understand why everyone in the comments were saying it was so easy. It is easy, but concept is easy to understand here, but the final answer is 0.4.
at 2:19 is it know concentration X (Volume of known/ Volume of unknown) ?
Best
I dont understand in the end how/why is it 0.6÷2
Wtf thanks man
how do we know both of them have the same moles?
like if we find the moles of know how do we know the unkown also has same mole?
ye
this is just a fancy way of saying M1V1=M2V2
Sort of... But you can only use M1V1 = M2V2 when the mole ratio is one to one...
If the mole ratio isn't one to one, it's better to go through the long way to ensure you don't make any mistakes.
What if the mole ratio is not 1:1??
how i can find average moles
I completely understand the maths behind the answer to the last calculation, but the logic doesn't make sense: if substances neutralise they must have the exact same amount of stuff in total, and since the two substances had the exact same volume they must have had the exact same amount of stuff per amount of space in order to total the same number of moles, so how can a volume with a concentration of 0.3 mol/dm^3 neutralise with an identical volume that has a concentration of 0.6 mol/dm^3?
You are nearly right, but remember that a di-basic acid, such as sulphuric acid, has two replaceable hydrogen atoms per molecule, but an alkali such as sodium hydroxide has only one -OH group per molecule. So you need two moles of NaOH to neutralise one mole of H2SO4. Check out the video at 4:00 again.
I have a test on this in 46 minutes
Hope it went well 🤞
I like ur video design but the information is not the best.
voice very low
2:00 its 0.4 not 0.04 ...
You're right! There's a mistake. Thanks for noticing!
Is it just me or is their an error in the concentration calculation of the unknown substance. 0.01/0.025=0.4 not 0.04?
nobody asked
Were did they get the 0.01 from? They seem to have carried it over from the mole value for sodium hydroxide which if you are going to do you carry it over and divide by 2 to get the mole of sulphuric acid and go from there
Yup, you are right, there's an error. Sorry about that!
Wesley Allen exactly what I thought, I’m extremly confused
But how do i find the molarity
molarity is the molar concentration given by M/L
so you might have to change units
Your wrong in that practice question. you're meant to divide 0.015 by 2 instead of mulitplying
what the hell happened to the stoichiometry?
audio is too low :(
0.01/0.025=0.4
at 2:00, there is something wrong
It should be 0.4, you are right! Thanks for noticing!
ok wtf how is cm cubed equal to ml
ua-cam.com/video/vYClOV9rXKs/v-deo.html
They are both measures of volume. Often ml is used for liquids and cm3 for solids, but cm3 also works for liquids (like in video I shared).
1000cm cubed = 1 litre
Who's here for gcse 2018?
Hi Sir would you be able to help me with this or someone else
In a titration a 125cm3 sample of nitric acid reacted exactly with 10cm3 of 0.40mol/dm3 potassium hydroxide solution. Calculate the number of moles of potassium hydroxide used?
Many thanks
No
0.032 mol/dm3 i think
@@olliecowdall4545 nice try man but it's actually 0.32mol/dm³
@@olliecowdall4545 yeah thats right
@@olliecowdall4545 HI