@@augustinematthew2055 Well, do it without any expectation. Practise. Get a hang of things. Satisfy your curiosity. You'll never get truly good at it unless it's less of a chore and more of something you can appreciate
What a great explanation! It was easy to understand, and included the background concepts along with the technique. It's wonderful to find good explanations to share with my chemistry tutoring students. Thank you.
wow so adding too much titrant doesnt have to be a tragedy as it has always been in my analitycal chemistry classes.... why u didnt teach me those haha it would be much less stress
How do you account for the fact that phenolphthalein turns pink at a pH of 10 and back to clear at a pH of 8.3. When you reach the end point, the solution is still basic. It would seem that the measured molarity of HCl is the amount it took to make the solution 8.3. None of the titration formulas I've seen seem to account for the fact that it's still basic (and not 7 and not exactly 1:1). What am I missing here?
Hello! Thank you for your question! It was a very good question, and so I made a video response, and posted it tonight. I hope it helps you and anyone else with the same question. You can find it in my new videos, in the description of this video, or at the link below. ua-cam.com/video/0n_F-QPoZiM/v-deo.html
Thank you so much for the video! I don't understand why it doesn't matter if the conical flask has water left inside it? Does that not dilute the solution?
If there is water left in the flask, as long as it is distilled water, it does not change the moles of analyte in the flask or the moles of titrant needed to react with it. It is just extra water. Be sure you are measuring with an accurate instrument (like a buret or a grad cylinder) and NOT the flask itself. Flasks are terrible for accuracy. If you are measuring with the flask, it will be off from the start, and yes, drops of water will affect it. But if you measure the analyte separately and add it to the flask, no error should occur with the extra drops.
So he knows what the exact volume of the acid he's starting with. Normally you'd use a graduated cylinder to measure that, but a burette is more precise. The second burette is for the actual titration.
I got shamed by chem sir for not getting it right the first time 😭. Now I'm traumatized to even look at an pipette
Don't worry about it, you'll get it right after some practice, not much time if you get the hang of it soon enough, you likely will
Each time I attempt a titration, my hands becomes so shaky
@@augustinematthew2055 Well, do it without any expectation. Practise. Get a hang of things. Satisfy your curiosity. You'll never get truly good at it unless it's less of a chore and more of something you can appreciate
What a great explanation! It was easy to understand, and included the background concepts along with the technique. It's wonderful to find good explanations to share with my chemistry tutoring students. Thank you.
surely it is great
Master titration class of 2018 returning! Miss ya, teach! -SD
Great explanations! Very helpful
Amazing sir, Last min prep. for tomorrow's exam.
you explained this so well!! thank you
❤ u are indeed a life saver
I didn't know the indicator would turn that clear and that pink with only one drop. You're right, it is satisfying :) 10:20
Bright pink is overshooting the endpoint. The endpoint should be a light pink that fades after 15-30 sec due to CO2 from the air.
from Alexandria,Egypt thanks❤
very satisfying video I got enough information from the video
wow so adding too much titrant doesnt have to be a tragedy as it has always been in my analitycal chemistry classes.... why u didnt teach me those haha it would be much less stress
my teacher bet me $5 i can't get a perfect titration and i'm so determined to prove him wrong
How did it go with the bet? 🤔
@@crowdedbeaker7980 ended up winning the 5 bucks thanks to you
@@vltseth1835 awesome! 😎
@@vltseth1835 Chad
Great Job
Good explained
How do you account for the fact that phenolphthalein turns pink at a pH of 10 and back to clear at a pH of 8.3. When you reach the end point, the solution is still basic. It would seem that the measured molarity of HCl is the amount it took to make the solution 8.3. None of the titration formulas I've seen seem to account for the fact that it's still basic (and not 7 and not exactly 1:1). What am I missing here?
Hello! Thank you for your question! It was a very good question, and so I made a video response, and posted it tonight. I hope it helps you and anyone else with the same question.
You can find it in my new videos, in the description of this video, or at the link below.
ua-cam.com/video/0n_F-QPoZiM/v-deo.html
Thank you sir
how to perform the titration experiment on a solution which is already of pink colour..??
Why did I see acid drip from your hands when you demonstrated tipping the beaker into the pipette from below your eyeline jnstead of above
It was water left over from the rinsing stage.
Thank you so much for the video!
I don't understand why it doesn't matter if the conical flask has water left inside it? Does that not dilute the solution?
youre right it shouldnt be wet if you want to be precise
If there is water left in the flask, as long as it is distilled water, it does not change the moles of analyte in the flask or the moles of titrant needed to react with it. It is just extra water. Be sure you are measuring with an accurate instrument (like a buret or a grad cylinder) and NOT the flask itself. Flasks are terrible for accuracy. If you are measuring with the flask, it will be off from the start, and yes, drops of water will affect it. But if you measure the analyte separately and add it to the flask, no error should occur with the extra drops.
hello fellow and future hca students in ap chem
my dude forgot the filter
I've never needed a filter for a naoh with hcl titration
Sorry but that was not a percent titration :d
It should have been a much more pale of a pink, right?
give
why is man using 2 burretes
So he knows what the exact volume of the acid he's starting with. Normally you'd use a graduated cylinder to measure that, but a burette is more precise. The second burette is for the actual titration.
@@elisecurran9497 I've always known that titrands are measured with pippetes