I could never get a good grasp of acids and bases, even throughout college, but the way you explained this has been extremely helpful. I wish I had teachers like you when I was learning chemistry basics in school
You are literally the reason as to why I understand chemistry. My professor has made these concepts out to be so difficult and you make it so simple and explain it so well! You are a LIFESAVER! Definitely coming back for Organic chem help! Thank you!
Hey Chad, I'm from India your lecture are very helpful for my preparation of NEET and JEE I would absolutely love it if you would look into these examinations and give a comprehensive guide on the prepration of these exams it will surely increase the exposure of this channel and help many more😊❤
I wish I could have you as my professor. Out of all the chemistry professors I have delt with. you seem informed, organised, and able to communicate effectively...As a student that is all i am asking for.
Hey Dhruv! If you explore the channel you'll see an old Gen Chem playlist with buffers and titrations covered in chapter 17. This lesson is part of an updated playlist and I'll be remaking and releasing these analogous chapter 17 videos week after next. But the old ones are also embedded in a free course on my site often with some extra content and organized with a dropdown menu that you might appreciate. You'll find the lessons here: www.chadsprep.com/chads-general-chemistry-videos/buffer-chemistry/ www.chadsprep.com/chads-general-chemistry-videos/titration-curves/ www.chadsprep.com/chads-general-chemistry-videos/titration-calculations/ Lots of extra content for titration calculations on that last page. Hope this helps!
Thank you so much for the amazing lesson! I was just wondering if you have any plans on teaching inorganic or analytical chemistry and making videos in those fields? Because you're the best teacher i've EVER had
Just an observation. Arrhenius in the reaction HCl+H2O can only classify HCl as an acid. Water according to him cannot be considered a base. So even in aqueous solutions these two theories don't cover each other completely .
27:23 how does increasing the concentration of weak acid makes the acid dissociate less? I mean according to les Châtelier's principle if you increase the concentration of a reactant the reaction will move in a way to lower that increase, so it will move to the right in order to produce more products.
We have to be specific about whether we are talking in 'absolute' terms or 'percentage' terms. You are correct in stating that increasing the concentration of weak acid will result in a shift right producing more products...in an 'absolute' sense. This means that a higher concentration of weak acid molecules will result in more weak acid molecules that dissociate overall. The tricky part is that a higher concentration of weak acid molecules will mean that a lower 'percentage' will have dissociated. These two claims are true at the same time. A higher concentration of weak acid will have a lower percent dissociation, though you will end up with higher overall concentrations of the dissociated products. And this is something that is difficult to explain conceptually. But the math bears it out. Ultimately, you could think of it as being due to the fact that a single weak acid molecule dissociates to produce 2 product molecules/ions. That is not very satisfying conceptually, but it is what it is. Hope this helps!
I have a question, isn't it true that weak acids correspond to strong conjugate bases? Why is it that, for example, if NH4 is a weak acid, its conjugate base, NH3+, is also a weak base?
You are looking at it as "H2O accepting a H+ and calling H3O+ a conjugate base" That's all good but now for a sec accept that's what every acid does in water i.e. donate it's H+ to water and form H3O+ ion. now the ultimate H+ donor in aqueous solution would only be this H3O+ ion right??? And particularly "Strong acids" tend to **completely** give out their H+ to water so every strong acid would ultimately exist as H3O+ in their aqueous solutions
Water accepting H+ ion and forming H3O+ ion it surely is conjugate base but it's the conjugate base of the acid which donated H+ being a conjugate base is a relatively term it doesn't mean H3O+ can't donate it's H+ to any other base
Hi Chad, can you explain why acids only donate 1 H+ to become a base? For example, why isn't the base of acid CH3COOH then CH2-COO- for example, or why not donate all the H to become C(3negative)COO-? Or NH4+ then N(4negative) instead of NH3?
Not all of those H's in CH3COOH are acidic. The H-C bonds are not polar so it is not easy to break the bond and lose the H. The O-H bond in a carboxylic acid is much weaker due to high polarity of the O-H bond and further charge delocalization from the carbonyl group which stabilizes the conjugate base CH3COO- making that H acidic (dissociation occurs in solution). In order to break the C-H bond we would have to put energy in, it wouldn't freely dissociate in solution. Hope that helps!
sir may you please assist in solving the following problem A 25ml sample of 0,10M sodium benzoate is titrated with 0,10 M of HCl what is the pH of after the addition of of 32,0ml of HCl (kb of C6H5CO2- =1,6X10^-10)
I cover titrations in this playlist in chapter 17. I specifically cover weak acid/strong base and weak base/strong acid in this lesson: th-cam.com/video/3Y9TaxwcQGs/w-d-xo.html Tune in around 21:16 for how to calculate the pH when you are past the equivalence point. Hope this helps!
Trust in the Lord with all your heart and lean not on your own understanding. In all your ways acknowledge Him and he shall make your paths straight. Proverbs 3:5+6
The NH3 + CH3COOH = NH4+ + CH3COO- Example makes no sense to me as to why the acids are the acids, and the bases the bases. (based off what I learned from the previous info from this video) So lost!
So the acidic species are NH4+ and CH3COOH because they both have a 'donatable' proton, forming the conjugate bases NH3 and CH3COO-... can you let me know what you are strugglinig to understand particularly?
I could never get a good grasp of acids and bases, even throughout college, but the way you explained this has been extremely helpful. I wish I had teachers like you when I was learning chemistry basics in school
Glad the channel is helping you now.
You just took my love for chemistry to a new high,thank you for the lesson Chad
That is great to hear - you're welcome!
You are literally the reason as to why I understand chemistry. My professor has made these concepts out to be so difficult and you make it so simple and explain it so well! You are a LIFESAVER! Definitely coming back for Organic chem help! Thank you!
Glad the channel is helping you - Happy Studying!
You made comprehension of my lectures easier. Thank you, Chad; you are the GOAT.
You're welcome - and Thank You!
not LSD 😭 this man is gold
Glad you think so!
Studying for MCAT rn and your vid are amazing!! you are single-handedly helping to boost my score. Thank you!
You're welcome and Happy Studying!
You are amazing. And hopefully your channel will grow.
For now I will do my part by sharing it to my mates
Thank you - Appreciate that!
Hey Chad, I'm from India your lecture are very helpful for my preparation of NEET and JEE I would absolutely love it if you would look into these examinations and give a comprehensive guide on the prepration of these exams it will surely increase the exposure of this channel and help many more😊❤
I wish I could have you as my professor. Out of all the chemistry professors I have delt with. you seem informed, organised, and able to communicate effectively...As a student that is all i am asking for.
Thank you!
I think you are by far the best Professor I've come across. Thank you for your work!
Greetings from Cyprus!
You're welcome and Thank You from USA!
I am a chemistry student and your explanations helped me so much. Thank you!
Excellent!
Yehey! I found the best explanation about these concepts. I haven't taken Chem in my entire life, so thank you soo much. 🙏👍😊
You're welcome - glad it helped!
You made my day when you mentioned HF can dissolve dead bodies like in Breaking Bad
Yeah Science!
your videos save my AP chem grade you make it so logical and simple!! God bless you
Glad to hear that and Thank You!
the best channel to learn sciene!
Thanks for saying so!
Beautiful explanation! Cant wait for next video to come out
Awesome! It's coming in the morning and another Thursday morning.🙂
@@ChadsPrep please do a video on buffers and titrations
Hey Dhruv! If you explore the channel you'll see an old Gen Chem playlist with buffers and titrations covered in chapter 17. This lesson is part of an updated playlist and I'll be remaking and releasing these analogous chapter 17 videos week after next. But the old ones are also embedded in a free course on my site often with some extra content and organized with a dropdown menu that you might appreciate. You'll find the lessons here:
www.chadsprep.com/chads-general-chemistry-videos/buffer-chemistry/
www.chadsprep.com/chads-general-chemistry-videos/titration-curves/
www.chadsprep.com/chads-general-chemistry-videos/titration-calculations/
Lots of extra content for titration calculations on that last page. Hope this helps!
Thank you for your explanation. It has saved me so much time reading books and trying to figure out how to analyze the information.
You're welcome!
Your videos are so helpful. Thanks!
You're welcome, F.P. - and thank you!
Thank you so much for the amazing lesson! I was just wondering if you have any plans on teaching inorganic or analytical chemistry and making videos in those fields? Because you're the best teacher i've EVER had
Dear Chad. I am overwhelmed to see Trust in The Lord along side Acids and Bases. Be blessed bro
Right back at ya!
Great work sir.
Thank You
From Ghana and I completely understood it thank uuu
Excellent!
wish you were my chem professor... Thanks for this lesson!
You're welcome!
You are a wonderful Teacher
Thank you for the kind words!
super easy and useful, thank you Chad
You bet!
love the video + the shirt! thanks for all your help :)
Thank you + thank you - You're Welcome!
great as always
Thank you
Thank you for explaining things so well, so thoroughly:)
Glad it was helpful!
NIce simple explanation! Thank you!
You're welcome!
Just an observation. Arrhenius in the reaction HCl+H2O can only classify HCl as an acid. Water according to him cannot be considered a base. So even in aqueous solutions these two theories don't cover each other completely .
Absolute legend, thank you so much!!!
Very welcome!
27:23 how does increasing the concentration of weak acid makes the acid dissociate less? I mean according to les Châtelier's principle if you increase the concentration of a reactant the reaction will move in a way to lower that increase, so it will move to the right in order to produce more products.
We have to be specific about whether we are talking in 'absolute' terms or 'percentage' terms. You are correct in stating that increasing the concentration of weak acid will result in a shift right producing more products...in an 'absolute' sense. This means that a higher concentration of weak acid molecules will result in more weak acid molecules that dissociate overall. The tricky part is that a higher concentration of weak acid molecules will mean that a lower 'percentage' will have dissociated. These two claims are true at the same time. A higher concentration of weak acid will have a lower percent dissociation, though you will end up with higher overall concentrations of the dissociated products.
And this is something that is difficult to explain conceptually. But the math bears it out. Ultimately, you could think of it as being due to the fact that a single weak acid molecule dissociates to produce 2 product molecules/ions. That is not very satisfying conceptually, but it is what it is. Hope this helps!
Thank you very much sir, so in the video you were referring to the percent dissociation?
Thank you so much, Chad.
You're welcome.
Super helpful! Thank you!
Very welcome!
I have a question, isn't it true that weak acids correspond to strong conjugate bases? Why is it that, for example, if NH4 is a weak acid, its conjugate base, NH3+, is also a weak base?
thank you
You're welcome
Im back to thank you again Chad :) the breaking bad comment made me check comments so..
Thank you for this ❤
You're welcome and Thanks!
Thank you Chad!
You're welcome!
i just didn't enjoy and learned from your video but also loved seeing you rock in "TRUST IN THE LORD..." tee. God Bless!
Thanks and same to you!
Why at 24:35 he says that the only acid left is H3O+ ? Isn't H3O+ in the reaction a conjugate base?
H3O+ is essentially H+ ion and the reason he says that's the only acids left is cuz all strong acids (HCl in this case) get completely ionized.
You are looking at it as "H2O accepting a H+ and calling H3O+ a conjugate base"
That's all good but now for a sec accept that's what every acid does in water i.e. donate it's H+ to water and form H3O+ ion.
now the ultimate H+ donor in aqueous solution would only be this H3O+ ion right???
And particularly "Strong acids" tend to **completely** give out their H+ to water so every strong acid would ultimately exist as H3O+ in their aqueous solutions
Water accepting H+ ion and forming H3O+ ion it surely is conjugate base but it's the conjugate base of the acid which donated H+ being a conjugate base is a relatively term it doesn't mean H3O+ can't donate it's H+ to any other base
Hopefully it's clear now
What is the difference between MCAT prep video and this?
I hope you have a good day chad. Thank you very much ♥️
Thank you - have an awesome day yourself :)
I think more examples would have done it but it was great
Thanks.
Hi Chad, can you explain why acids only donate 1 H+ to become a base? For example, why isn't the base of acid CH3COOH then CH2-COO- for example, or why not donate all the H to become C(3negative)COO-? Or NH4+ then N(4negative) instead of NH3?
Not all of those H's in CH3COOH are acidic. The H-C bonds are not polar so it is not easy to break the bond and lose the H. The O-H bond in a carboxylic acid is much weaker due to high polarity of the O-H bond and further charge delocalization from the carbonyl group which stabilizes the conjugate base CH3COO- making that H acidic (dissociation occurs in solution). In order to break the C-H bond we would have to put energy in, it wouldn't freely dissociate in solution. Hope that helps!
@@ChadsPrep yes that helps, thank you
But did you mean to say the C-H bonds are not polar? Instead of H-C?
great shirt man
Thanks!
sir may you please assist in solving the following problem
A 25ml sample of 0,10M sodium benzoate is titrated with 0,10 M of HCl what is the pH of after the addition of of 32,0ml of HCl (kb of C6H5CO2- =1,6X10^-10)
I cover titrations in this playlist in chapter 17. I specifically cover weak acid/strong base and weak base/strong acid in this lesson: th-cam.com/video/3Y9TaxwcQGs/w-d-xo.html
Tune in around 21:16 for how to calculate the pH when you are past the equivalence point. Hope this helps!
you’re everything
Glad the channel/videos are helping you!
@@ChadsPrep In my prayers you’re 🤍
@@mahra855 Thank you.
19:28 this part caught me off guard because the Super Bowl just happened and this video was filmed one year ago
What timing!
What does your shirt say?
Trust in the Lord with all your heart and lean not on your own understanding. In all your ways acknowledge Him and he shall make your paths straight. Proverbs 3:5+6
this man is literally Heisenberg. Didn't know he was still living.
Ssshhhhh - no one needs to know!
w chad
Happy Studying!
The NH3 + CH3COOH = NH4+ + CH3COO- Example makes no sense to me as to why the acids are the acids, and the bases the bases. (based off what I learned from the previous info from this video) So lost!
So the acidic species are NH4+ and CH3COOH because they both have a 'donatable' proton, forming the conjugate bases NH3 and CH3COO-... can you let me know what you are strugglinig to understand particularly?
awesome video but the shirt made me question you.
You're not suggesting I teach without a shirt, are you? Not on this channel! 😁😆
Avvont wwnasoon