Dud u r such a goat! I prefer watching videos to make sure im understanding the content rather than reading the books and u really explain everything so well and make it so easy to understand! Keep up the amazing content GOAT!!
Sir I took gen chem almost 2 years ago already and I had never fully understood the theory behind chemical equilibrium. I went to a community college and didn't have the best teachers unfortunately. I was just passing the tests memorizing formulas like a robot and plugging in numbers completely oblivious to what anything really meant. You have completely enlightened my mind!!!! It may sound funny that I put so much weight into learning one single concept but trust me this makes me so happy you have no idea. You are espectacular!!
I'm so happy to hear that you've been getting a lot from my lectures! I hope it remains that way :) Make sure you share with a friend so the knowledge spreads!
Love your videos, I'm just a bit confused on where to find ur Gen Chem notes, I only see Bio, Ochem, Biochem notes on the drive. I would highly appreciate ur help
Question: when you were explaining why H2O was not included in the equilibrium constant of weak acids (Ka) I remember them teaching us that in dilute aqueous solutions, the [H2O] is effectively considered a constant because it is present in excess in the reaction. Is that not correct?
If anyone is able to help - why around 21:58 do we add HCL to the solution? are we saying the ph dropping increases H3O+, and if that's the case, we reach equilibrium by adding HCL? just dont understand the connection between adding a strong acid to increase H3O+ and shift the eq left .. thank u!
someone correct me if im wrong, but i think its this: We are adding HCl to disturb the equilibrium. Adding HCl to an aqueous solution -> HCl completely dissociates -> more H+ ions present -> causes more H2O to be protonated thus forming H3O+. This increases H3O+ concentration on the right, and the reaction now "wants" to shift back towards the left. Adding HCl, a strong acid, is basically synonymous with adding H+ ions and has the effect of dropping pH, since pH is -log[H+]. So for these problems, when they say "what happens when the lower the pH" you can think of it as "what happens when we add H+ ions to the solution" to figure it out. To answer this "are we saying the ph dropping increases H3O+," it is adding the H+ ions via HCl that drops the pH AND increases H3O+. Hope that helps!
Dud u r such a goat! I prefer watching videos to make sure im understanding the content rather than reading the books and u really explain everything so well and make it so easy to understand! Keep up the amazing content GOAT!!
Appreciate you my man !!
youre actually the goat for these. if I make the mcat cutoff on the first try you're getting a fruit basket
HAHAHA hello ninette- happy you're getting something out of it!
Sir I took gen chem almost 2 years ago already and I had never fully understood the theory behind chemical equilibrium. I went to a community college and didn't have the best teachers unfortunately. I was just passing the tests memorizing formulas like a robot and plugging in numbers completely oblivious to what anything really meant. You have completely enlightened my mind!!!! It may sound funny that I put so much weight into learning one single concept but trust me this makes me so happy you have no idea. You are espectacular!!
I'm so happy to hear that you've been getting a lot from my lectures! I hope it remains that way :) Make sure you share with a friend so the knowledge spreads!
bro you're the goat!! You, Uworld and Anki are carrying me like lebron carried 07 Cavs
So glad you're getting a lot out of it my friend! Enjoy, and don't let the UWorld wear you down
@@yusufahasan Never back down never what??
@@IAMTheDeffence NEVER GIVE UP !!!!!
@@yusufahasan yessir 🫡
Love your videos, I'm just a bit confused on where to find ur Gen Chem notes, I only see Bio, Ochem, Biochem notes on the drive. I would highly appreciate ur help
will upload those asap
Thank you for all your support and please share with friends!
Question: when you were explaining why H2O was not included in the equilibrium constant of weak acids (Ka) I remember them teaching us that in dilute aqueous solutions, the [H2O] is effectively considered a constant because it is present in excess in the reaction. Is that not correct?
your videos are so helpful! can you make a video on the gas phase chapter?
I wish! i’m so bad at that chapter
If anyone is able to help - why around 21:58 do we add HCL to the solution? are we saying the ph dropping increases H3O+, and if that's the case, we reach equilibrium by adding HCL? just dont understand the connection between adding a strong acid to increase H3O+ and shift the eq left .. thank u!
someone correct me if im wrong, but i think its this:
We are adding HCl to disturb the equilibrium. Adding HCl to an aqueous solution -> HCl completely dissociates -> more H+ ions present -> causes more H2O to be protonated thus forming H3O+. This increases H3O+ concentration on the right, and the reaction now "wants" to shift back towards the left. Adding HCl, a strong acid, is basically synonymous with adding H+ ions and has the effect of dropping pH, since pH is -log[H+]. So for these problems, when they say "what happens when the lower the pH" you can think of it as "what happens when we add H+ ions to the solution" to figure it out.
To answer this "are we saying the ph dropping increases H3O+," it is adding the H+ ions via HCl that drops the pH AND increases H3O+. Hope that helps!
Hey where can I find your notes?
they should be up on the drive now, link in the description!