Anyone wondering why the conjugate acid SO4^-2 is H2SO4, remember that it is reacting with two NH4+ which both give it 1 H+. Consequently it's conjugate acid is H2SO4, which is one of the 6 simple, strong acids. You can find a chart of all six of these thru google (there a good thing to memorize).
No no no. Just memorize the small list of strong acids. Everything else is weak. ^^ This isn't 100% true but works for most students in high school / university :)
this helped so much !! i've been struggling with this concept all semester, and our final exam is tomorrow. it makes so much more sense now, thank you !!
The first example is incorrect. The conjugate acid of sulfate is HSO4-. While H2SO4 is a strong acid, HSO4- is not. The second proton in sulfuric acid only partially dissociates. For this problem you need to consider the Ka of NH4+ and the Kb of sulfate. You would have to solve this problem like his part c).
For the second example, is the solution basic because its salt of a weak acid and a strong base (spectator ion only)? A lot of other people seem to get fuzzy on that part...
Thank you, Mr. chemistNATE. Your explanation was 200% better than how my book tried to explain it. Again, thank you very much, and I've only skim your other videos, but I'd like to encourage you to keep up the good work :)
dumb questions incoming. we saw in the first example that clearly NH4+ could donate a proton, allowing for the salt (NH4)2SO4 to be acidic. and given that the SO4^2- ion will not accept protons because it is the conjugate base of a strong acid. but how can a salt like CuSO4 be acidic if it has no protons to donate? and if you want to be technical, only the first proton in H2SO4 is strong. the second proton dissociates less easily, making the second one weak. wouldn't that allow SO4^2- to accept at least one proton (making it slightly basic)?
The Cu+2 ion of CuSO4 is acidic for a special reason. In water in becomes Cu(H2O)6(2+) which is a “complex” (H2O are ligands) and so it does actually have an H to donate
HSO4- donates more H than it accepts (you are correct that it can accept). Overall it will be acidic because a higher % of the H’s are donated vs accepted back
Oh my flippin god! You have a gift for instruction. This has been a mystery to me until you explained it. Thank you Thank you Thank you!!! Subd and liked !!
Hi! uhhh I would like to know the reactions happen when salts dissolve in acids such as calcium oxalate dissolve in certain acids? Could you explain please? I was searching for it ages online
For example a: Couldn't you just take the Ka of NH4+ (which is in the order of 2*10^-5), compute the Kb of the sulphate ion (which, given the Ka of HSO4, puts the Kb in the order of 10^-12), and argue that, given the relative magnitudes, such a solution would be acidic?
lol unfortunately in the IB Chemistry higher level exams they don't give you the Ka/Kb values so if you get a nasty one like the last one you did in the video we can't really tell which dissociate more and thus whether the solution would be basic or acidic. Oh well... Good concept though. It works
what the actual is being said here. like. i feel like chemistry at this point just says things happen and expect that everyone taking chem is jsut going to educated guess. " yup this is the point where we seperate into different things"
It explained the concepts very well and walked us through several typical questions relating to the topic and provided the answer. What is wrong with it?
Anyone wondering why the conjugate acid SO4^-2 is H2SO4, remember that it is reacting with two NH4+ which both give it 1 H+. Consequently it's conjugate acid is H2SO4, which is one of the 6 simple, strong acids. You can find a chart of all six of these thru google (there a good thing to memorize).
No no no. Just memorize the small list of strong acids. Everything else is weak.
^^ This isn't 100% true but works for most students in high school / university :)
this helped so much !! i've been struggling with this concept all semester, and our final exam is tomorrow. it makes so much more sense now, thank you !!
How
I am from India and I suddenly found this vdo..which clear my concept easily.thanks a lot
This video somehow explained the salt thing in a way I understand. Thank You
THANK YOU!!!! I have MCAT coming up.....Your videos literally helps 24/7
🎉🎉🎉 thank you for helping me study for my MCAT ❤
The first example is incorrect. The conjugate acid of sulfate is HSO4-. While H2SO4 is a strong acid, HSO4- is not. The second proton in sulfuric acid only partially dissociates. For this problem you need to consider the Ka of NH4+ and the Kb of sulfate. You would have to solve this problem like his part c).
studying for an exam and this helped a ton! You rock!
I like how you explained it more instead of just saying well this is acidic because that is blah blah blah
So..... was B a basic solution???
Yup!
This was awesome! I got an exam tomorrow and this is going to be on it. Very helpful and informative. Thanks for posting :D
Very well explained, and loved how you weren't speaking too fast. Thank you!
And THIS didnt help at all.
i love this chemistNATE guy...
Thanks brother. Made it so much simpler and shorter than my prof did.
Wow bro
For the second example, is the solution basic because its salt of a weak acid and a strong base (spectator ion only)? A lot of other people seem to get fuzzy on that part...
literally only video that helped...thank god
Im in med school and this video is still super helpful.. Thank you Nate.
Thank you, Mr. chemistNATE. Your explanation was 200% better than how my book tried to explain it. Again, thank you very much, and I've only skim your other videos, but I'd like to encourage you to keep up the good work :)
Thanks, Nate.
Thank you for your time. This video is great.
Mate thank you so much that was really good love ya !
dumb questions incoming.
we saw in the first example that clearly NH4+ could donate a proton, allowing for the salt (NH4)2SO4 to be acidic. and given that the SO4^2- ion will not accept protons because it is the conjugate base of a strong acid.
but how can a salt like CuSO4 be acidic if it has no protons to donate? and if you want to be technical, only the first proton in H2SO4 is strong. the second proton dissociates less easily, making the second one weak. wouldn't that allow SO4^2- to accept at least one proton (making it slightly basic)?
The Cu+2 ion of CuSO4 is acidic for a special reason. In water in becomes Cu(H2O)6(2+) which is a “complex” (H2O are ligands) and so it does actually have an H to donate
HSO4- donates more H than it accepts (you are correct that it can accept). Overall it will be acidic because a higher % of the H’s are donated vs accepted back
Thanks for a great video! I have had a hard time finding anything on the intrenet about this topic but luckily I found your video! :)
Oh my flippin god! You have a gift for instruction. This has been a mystery to me until you explained it. Thank you Thank you Thank you!!! Subd and liked !!
Sulfuric acid is a strong acid; HSO3 is the weak conjugate acid for the base SO3.
Nice explanation
I wonder how CN- can have its own Kb since it has no OH- to dissociate into.
you're good, no you're great actually
absolutely useful and clear!
you are a life saver! I understand this now
I used two of your videos so far and i understood both concepts completely after watching! Thank you so much!
P.s. can you be my chemistry teacher?
Thank you. I finally understand something.
what was first one ? neutral?
How do we know an acid is weak or strong??
So was the solution for B) basic or neutral?
Nooo
Hi! uhhh I would like to know the reactions happen when salts dissolve in acids such as calcium oxalate dissolve in certain acids? Could you explain please? I was searching for it ages online
Finally i understood this, thank you so much.
Thank you that was incredible! Really helped me so much!!!!!! THANK YOU!!
how do you determine the conjugate pairs that you hv written in orange ? pls help ! :(
dammit missed this question on the test. The question was worth 20% of the test!!!!!
Why NaHSO 4 is a salt however it is slightly acidic?
For example a:
Couldn't you just take the Ka of NH4+ (which is in the order of 2*10^-5), compute the Kb of the sulphate ion (which, given the Ka of HSO4, puts the Kb in the order of 10^-12), and argue that, given the relative magnitudes, such a solution would be acidic?
thanks Nate!!!
Are you Canadian? And was the second one basic or acidic?
so i have to memorize weak bases/acids tooo?
@ 3:28 you said H2SO4 is a weak acid, the example you did right before it had H2SO4 as a STRONG acid with SO4 as a weak base... Im confused.
H2SO3 was the second example :)) not H2SO4
you're my hero :)
How can H2SO4^-2 be a strong acid in the first formula and then be a weak acid in the second?
+Benjamin Thomas That's because in the second formula it was SO3^2- and not SO4^2-
What? Cool thanks
Very well put, thank you!
Thanks dude.
LMFAOOO
It was all professional then you were like, "That's a legit equilibrium that happens"
I laughed so hard. Keep it up this helped me a lot!
legit is a word, but how people use it now makes it like "unprof"
Thank you!
Welp. Further confused me.
lol unfortunately in the IB Chemistry higher level exams they don't give you the Ka/Kb values so if you get a nasty one like the last one you did in the video we can't really tell which dissociate more and thus whether the solution would be basic or acidic. Oh well... Good concept though. It works
Very helpful, thank you!
THANK YOU SO MUCH FOR THIS. NOW I SHALL PASS.
this dude literally saves my GPA
Is he Irish!? Great video keep up the awesome videos!
Thanks -- Very very helpful
Spanishiwa liked it, so i thought it's bout Starcraft. x)
But nice guide. ;)
what the actual is being said here. like. i feel like chemistry at this point just says things happen and expect that everyone taking chem is jsut going to educated guess. " yup this is the point where we seperate into different things"
Let’s figure out where you’re lost.
* do you know what HF does in water ?
thanks, helped very much
So what did b. make?
thanks bestie
👍🏽U really goo at explaining chemistry topic/ but this one I still don get it/ is there's a easy way
To explain it.
you have the same accent as my physics lecturer
Thought i got it....till i came here.
King fr
protone sucking up ability :D
super helpful! thanks :)
chemistNate: saving my ass since my freshman year of HS to my first year in college :P.
great job thanks
Ka for HSO4- is 1.2 x 10^-2. It does not dissociate completely.
Thanks
Thanks.
Thank you so much!
thank you
thanks!
and btw nice watch!
Its difficult to understand
There was a lot of "sucking".... haha
could I just borrow your brain for my midterm?
awesome !!!!
Thanks *w*
Aur chotta page nhi mila tha
"proton sucking up ability" love that man. I need layman terms not some stuffy professor's explanation!
terrible video, doesn't even answer the questions
wrong
It explained the concepts very well and walked us through several typical questions relating to the topic and provided the answer. What is wrong with it?
lol wat r u on about
Did not get this at all!!!
thank you for the information but I have to let you know your tone of voice sounds unbearably condescending in this
Oh :/ I thought he was just being excited
if u increase speed up to *2 then he sounds nice and enthusiastic
Not helpful. I got even more confused after watching this.
New drinking game: take a shot after every time he says "this"
Ummmm.......
Nvm great vid :)
Bkwas video hai.....koi kabhi mat dekna .
terrible...
Thanks -- Very very helpful