pH and Buffers
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- เผยแพร่เมื่อ 5 ก.พ. 2025
- 069 - pH and Buffers
In this video Paul Andersen explains how buffer solutions maintain pH in a solution. A buffer solution is made up of a weak acid and its conjugate base. As strong acids or bases are added the pH remains stable. A good buffer solution has a pKa value equivalent to the pH and equal amounts of the weak acid and the conjugate base.
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6 hours of studying this chapter and two two hour lectures. didn't get it. One TH-cam video later and it makes perfect sense
can anyone please explain me this sentence . in metabolic acidosis , one mechanism is incresed acid buffer excretion--- ph changes rapidly with relatively small change in H concentration , limiting the amount of acid that can be secreted as free H in the urine
your body has to produce more buffer if the amount of acid secretion is increased
Literally same...
story of my life
You're only able to understand the video because of the studying you did. You just needed someone to put it in an understandable language.
You taught a 30+ year career geophysicist more in an hour than I learned in college. Hats off.
From undergrad, to my masters, I keep coming back to this video. You're godsent
Video 69. I'm feeling some chemistry here...
+Adam Leach HAAAAAAAAA
i was just going to comment the same thing. G fucking G
Nice
@@retinaz2220 nice
Adam Leach holy crap that was 4 years ago
It's amazing how the videos I need come out exactly as my professor begins lecturing on it. The timing couldn't have been any better.
You sir deserve a round of applause for this video. Thank you.
I wish as a student I could give something more than just like, share, subscribe things to such great videos.
Some people deserve enormous peace, happiness and loving people around.
I'm learning a whole lot on TH-cam, unlike in class where my professor doesn't even understand what he/she is even talking about; just reads directly from textbooks without any rationalizing
Your voice is so good.. understood everything so clearly
I just got kicked out of my chemistry class because I forgot my handout, I’m glad this makes more sense than the class
your videos are easy to understand. Thank you sir
@Cristopher Ray
Over there you have a weak acid and its salt. Notice how it's the same thing as having a weak acid and its conjugate base.
It's like having H2CO3 and HCO3- (beacuse NaHCO3 ionizes into Na+ and HCO3-)
still don't understand XD. Maybe you can add definations of pKa or other words every now and then. It will help greatly :)
Really helpful! Frm my childhood I found these theses topics cause of my head ache.. Bt now I really feeling I should learn more its too much easy.. 😍Thanku
Thank you so much. You are the best. I wish I can like this video ten thousand times!
Awesome videos :-D I'm studying for the mcat and your videos help a lot conceptualizing certain topics :-) god bless
How did you do on the mcat?
How did you do on the mcat?
You are really good at explaining. Thank you.
Best teacher in the world 💙💙
thanks man....much needed video
Thank you very much , you can't imagine how that was helpful !
Thank you sooo much ....spent an entire day trying to figure it out my self and couldn't bt there you r, in just 5 min ..thank you .
Love your videos. Could you show a video that explains acidity in the body. Maybe show the flow to keep balance after drinking soda?
thank you for saving me during chem and bio. cheers.
yes that was very helpful Mr Anderson. U D MAN
Very good video. 10/10 would recommend to fellow students
U r a much better presenter than mr khan how u utilize visual devices and showing ur face that actually makes us think u r talking to us. You are our life savior for ap sciences
but mr khan teaches more intuitively
I wish I could like this video to infinity
another great job mr. andersen
Smh this is better than khan academy
no
Parth Shorey what is smh?
@@jon-paulplacencio775 Shake my head
@@jon-paulplacencio775 Smiling much happier
@@jon-paulplacencio775 Shops must halt
Nitpick: Your seesaw diagram is incorrect. The "more acid" and "more base" should be swapped, because if base increases, pH should increase, and if acid increases, pH should decrease. Your diagram implies that more acid will increase pH and more base will decrease pH, which is incorrect.
great explanation
does OH+H2CO3->H2O+HCO3? 0:51 How does it push hydroxide ions to the right if it's not the same equation?
this is super super late and you probably either know this already or your test is long gone, but adding a base to an acid will make water and a salt. ie, the hyroxide ions from the base and the hydrogen ions from an acid will combine to form water: OH- + H+ -> H2O Therefore H+ Ions are consumed and equilibrium shifts to the right to replenish loss of H+. Hope this helps!
thank you so much, these lessons are life saving!!!
Very nice one Mr Anderson :-)
Awesome Video. Succinct and straight forward.
My bio teacher never has a lesson plan so you’ve basically thought me every thing I know
Mr Andersen, hi. I have a question regarding the shift of equilibrium at 2:19. Why adding hydroxide ions will cause the equilibrium shift to the right? Thanks.
I was wondering that too. I think its because the hydroxides bind to the H+ ions (on the products side of the reaction) and form water. This removes some of the H+ products so the reaction shifts right to create more of them.
Thankyou so much you are the best!!!😭😭
best video ever,nice!
so nice comment man,shiiiiit
Very nice video
Too helpful 🙂. Thanks 🙏🏻
Very informative, understood a lot.
Ty so much for these videos!
very helpfull .....thank you so much
This is just what I needed
Well explained!
Thanks a lot, that's just what I needed!! Love your videos :)
Awesome video!
WAY FUCKING HELPFULL! I LOVE YOU, MAN!! YOU'RE THE BEST!!!
haha Mr. Andersen like from matrix (took me 3 videos to finally realize why that name sounded familiar) also THANK YOU SO MUCH these are great
What I don't understand is how the solution is more acidic if the concentration of the H ions are less than concentration equilibrium. Shouldn't it be the other way around????? I thought it should be more basic because the concentration of H is less so OH should be favorable. I'm referring to 4:30
Amazing vids!
Great vid. Thank you.
Thank you . this was very helpful.
What software so you use to make your videos?
great vid
I was under the impression that to create a buffer, you need both the acid and a salt of the acid? So, for example, a solution of H2CO3 mixed with NaHCO3. Could you explain?
really really very useful, but :( you speak very fast!!!! thanks a lot
Nice video
Thanks!!!
thank you!!! I finally get its... its video is very usefulll :)
at 3:18 he says that the [H+] is the pH. Isn't the pH -log of [H+] and not just the hydronium concentration?
At 2:58 he mentioned "if you we take the -log of[H+] we have the pH
1:41 that is what lacks in science and mathematics education in India. Its more about equations and definitions and exam patterns here.
So is HCO3 a conjugate base in the H2CO3 H + HCO3 ?
The correct way to take the negative logarithm of each side, and we get pH = pKa + log [A-]/[HA]
how long does it take for buffer control of blood pH
Thank you...nice one
why dilute aqueous ammonia alone will
not act as a buffer solution.
Ha' Ha'! Min 1:00 Caught you saying "protein" instead of "proton"! The you said proton. Busted!
+agent008chico ok?
+Faith :3 Just having a little fun Miss Faith! Non raunchy silly fun!
agent008chico I know, I love the name of faith, even tho isn't my name. My real name means love with being generous._.
+Faith :3 Hasani?
What
Please help me know, if there is any effect on the buffer of blood if small amount of acid or base is added in it ?!
really help a lot！
Nice
Mr Anderson... this is Mr Smith, I want to have a word with you
Have you got any vidoe on Diabities
you are improving my grades
nice.
why does adding protons push it to the left? the H2CO3 cant accept more protons?
Chemical equilibria always resist the change in a reaction. It's Le Chatelier's principle- look it up! it's integral to all chemistry. Think why would more product form when its reactant concentration increases? it acts to reverse the change by forming product and using up reactant
thank you sir
can someone give me a reason why a scientist would want to use a buffer in his/her experiment? I understand how it works, but I don't know why they would need to do it. Also, why wouldn't it work if it was a strong acid and a weak base?
buffers can be used to maintain blood ph for injectables because change in the ph of blood can cause denaturation and hyper/hypo acidosis in blood and they can also be used as a natural defense of freshwater against acid rain
good one !!
Amazing!
thank u 😊😊😊
Can someone help? :( I can't seem to find a video on titrations that shows the calculations and I don't get this problem.
Two drops of indicator HIn (Ka = 1.0 * 10^-9), where HIn is yellow and In- is blue, are placed in 100.0mL of 0.10 M HCl.
The solution is titrated with 0.10 M NaOH. at what pH will the color change (yellow to greenish yellow) occur?
The answer is supposed to be 8.0 but I need help on how to do it.
I looked online and found a source that showed:
The color change occurs when the concentration of the more dominant
form is approximately ten times as great as the less dominant form of
the indicator
[HIn]/[In-] = 10/1
Ka = 1x10-9= (1/10) [H+]
[H+] = 10 Ka = 1x10-9x 10 = 1x10-8
pH = 8.00
At pH 8.00 color change occurs.
I'm confused. How could you tell that it occurs when the dominant form is approximately ten times as great? HELP? D:
Danny Huang I don't know if you need this any more but here goes....
Firstly, you have to know the pH formula involving indicators. The formula is pH= pKa + log (In (aq)/HIn(aq)). One thing to note here is that HIn is referring to a weak acid indicator and In represents the indicator after it has lost a proton (which is why we have a change in colour).
We know in this instance that Ka=1x10^9 therefore, pKa= -log(1x10^9) = -9
In the case of indicators pH=pKa. So we can say that the pH is equal to 9.
We then have an equation that looks like this: 9= log(In/HIn).
You have to know that the concentration of HIn is equal to 10x In. So we can write in place that 9= log (10/1). This 10/1 is just the ratio between the In and HIn and unless stated otherwise will always be the case. pH would therefore be equal to 8.
good stuff
Carbonic acid isn’t really weak in relation to the trillions of cells involved in respiration and the fact as you add carbonic acid the ph lowers I defiantly believe there is a huge link between burning fuel and cancer
Thank u!! :D
But I wish I could like it 10,000,000 times
What does the A stand for in HAH+ + A-?
it is a conjugate base
What happens if you add water to a buffer?
Hi. I'm putting a request for tissue and membranes video.. Thank you :)
But why does adding OH- to the acid make it dissociate .....????
Jenny Wilson The example in the video is carbonic acid (H2CO3) which is an unstable compound that can break down ( this reaction is reversible) into H(+) + HCO3- (which may make it simpler). If we add OH- ions they will react with the H+ ions to form H20 and so the equilibrium would shift to the right. This is applicable in most if not all cases.
thanks ! I must re-watch it as I should have known that so i wonder why the video made me think otherwise. thanks for the clear explanation though.
No problem 😊
so that's why H and OH =H2O (water) is good to maintain body's pH
What exactly is the conjugate base?
When an acid looses H+ ion, an anion is formed which wants to take H+ ion or proton. So, according to the Bronsted Lowry concept, it will be considered as a base. The stronger the acid, the weaker is the conjugate and vice-versa
I would like to thank BUFFER solutions for saving my life.😥😥😥😥😥😂😂😂🤣🤣🤣
Nice.
Can you please explain Common ion effect. It's a humble request. please. :)
amazing
thanks
Thanks
1:41 "Big pitcher" idk why this was funny
nice