Acid-Base Reactions and pH Calculations - AP Chem Unit 8, Topic 4

[@rafansyed8420]

Jeremy Krug you are my Jeremy King ✊👑

[@JeremyKrug]

Thank you for the kind compliment!

[@user-il1vx7kx8o]

common krug w

[@-neda-n]

real

[@JeremyKrug]

Thanks!

[@JonahTeng]

great video again sir! you're really helping me through AP Chem this year; I think I'll mention you in my graduation speech 😆 😆 😆 😆

[@JeremyKrug]

That would be a great honor. I'm so glad you're finding success in AP Chem this year!

[@latencies2586]

This is so real Jonah Teng!

[@Mortgage-Rates]

all hail king krug

[@JeremyKrug]

Thanks!

[@Taengoo007]

5:05 here, why cant I get the H+ and subtract 14 from it?

[@JeremyKrug]

Mainly because the H+ from the strong acid is reacting with the OH- from the strong base. Since the OH- is in excess, we have to calculate the pOH first, and only then can we subtract it from 14. Thanks for watching!

[@Taengoo007]

@JeremyKrug omg!! THANK YOU SM!! I didn't expect a response from you lol

[@insightx4786]

Hey Mr. Krug! Love your videos for AP Chem but I came across a question. So when having a mixture of an acid and a base and needing to do an ICE table with the molarities, wouldn't you need to use M1V1=M2V2 to dilute each acid and base before putting the molarities in an ICE table? In an AP Classroom video, another teacher recommended me to use the dilution formula if you have a mixture of an acid and base so I was wondering if you need to do it or does it end up with the same result without the dilution formula?

[@polishjerry6389]

You carried me for this unit ngl

[@JeremyKrug]

So glad to hear you're having success thanks in part to my videos. Keep working hard and you will do great!

[@dennisli4437]

So concentrated I can hear the police sirens at 16:01

[@DhruvPalla]

i dont think log(0.053) is 2.28 i get 1.27? vid 10:07

[@JeremyKrug]

Check the video again. We're taking the log of 0.0053, not 0.053.

[@kayleekoffi406]

why did we subtract the moles this time rather than add like we did in 8.2?

[@JeremyKrug]

In 8.2, we were finding the [H+] and pH of a strong acid mixture, so we had to find the total moles of H+, so we had to add. In this video for 8.4, we were finding the limiting reactant between the acid and base; since they were reacting with each other, we had to subtract to determine the limiting reactant. Great question, and thanks for watching!

[@ZaidAbuhijleh-w5n]

so if i know this along side all the other unit 8 vids ill be fine?

[@JeremyKrug]

Yes, you should be in good shape!

[@ZaidAbuhijleh-w5n]

@@JeremyKrug TY!

[@pattah451]

Thanks for the video Mr. Krug, but I don't really understand the last section of the video which talks about determining stronger bases using proton acceptance. Would you be so kind as to re-explain this (dumb it down) to me?🙃

[@owoowo5302]

(not Mr. Krug here, but I'll try to explain it the best I can as a fellow student ;-;). 1) First thing you gotta know is that H2O is kinda special since it can act as both an acid OR a base depending on what it's dissolving. In this case, we have a weak acid, HCNO, which means that the H2O will act as a BASE. You might've heard of the Bronsted-Lowrey definition of acids and bases, and according to that, acids act as PROTON-DONORS, meaning that the H+ will attach to the substance acting a base (H2O) and thus ACCEPTS the proton to form H3O+. Since the HCNO LOSES or DONATES its H+/proton, it becomes CNO- upon mixing with the water, forming a conjugate base. * So, basically, the job of a base is to accept the protons (H+) that the acids donate! It's just a definition for a base- that's all :D! If it's a GOOD base, it'll be super good at accepting those protons. 2) If your Ka

[@JeremyKrug]

@owoowo5302 did a great job explaining. I'll add that when you have a stronger base dissociating, the acid that it's reacting with is also acting as a stronger acid . Likewise, when you have a weaker base dissociating, the acid that it's reacting with is also acting as a weaker acid.

[@simonleka19]

w Krug

[@JeremyKrug]

Thanks!