Introduction to Buffer Solutions

[@binlo9959]

I really appreciate you taking your time to make all these, they're incredibly helpful!

[@MaChemGuy]

Dario T You're very welcome. Thanks for the comment.

[@Bilal626339]

Currently on at university doing Chemical Engineering and I use your videos, they're brilliant! Keep up the good work!

[@abiipass9465]

Thank you for all the videos, that are enabling me the revise the entire unit in a night! Really appreciated

[@Remedium96]

Best explanation I've seen yet! Thanks!

[@maazahmed2341]

Agreed

[@mohfa1806]

I salute you from lebanon...you are a wonderfull talented chemistry teacher...thank you again

[@atulsingh6262]

avoid yellow colour marker...

[@theshadeofjett]

YOU CLEARED UP A LOT OF STUFF! NOW I CAN MOVE ONTO THE CALCULATIONS THANKS

[@salemy300]

Can't thank you enoughfor all of these videos!

[@chinrxhh6707]

I can understand for your explanation and I always struggle for this buffer topic last year and now I can understand better for the concept behind it.Thank you so much.🙏🙏🙏😁😁😁😁.Big thump from Malaysia.❤️❤️❤️❤️.

[@hemanth.0716]

When I was taught about buffers I thought that the subject was very difficult & after watching this Video it's so easy . Thx you . This helped me a lot .

[@hemanth.0716]

Better avoid using yellow marker because it's of poor visibility

[@rahma4043]

This video really helped, was struggling with the topic, many thx ☺️

[@mrsangelatie2623]

Thank you so much for this video. It saved me the effort to record one myself. I just put this link into my students' notes. :-)

[@MaChemGuy]

Excellent. That's what they're there for.

[@fredriklarsson6254]

Phenomenal explanation!

[@gyrojomo]

Thanks; educational, informative and enjoyable.

[@kgomotsozamaswazitshabalal8055]

Hurrah for buffers :), Thank you Sir.

[@salins.3285]

Thank you for the video this is so helpful!

[@alil8419]

shout out to awesome accent

[@danielche2349]

you give a very logical explanation. thanks!

[@EpicEditsBySaz]

Thanks, this helped a lot.

[@nnekaude]

Really great, thanks!

[@rubenboswell4663]

I was the 1000 like 🎉

[@aarishhanif1837]

youre a true genius

[@Malak-io2bq]

it was really helpful! thank you very much =)

[@TheHammond101]

where would u recommend me to get the definitions for A2 chem? great vid also, really appreciate these- they are great!

[@MaChemGuy]

alex h If you go to www.chemnotes.org.uk/ then click on either OCR or AQA depending on which spec you're doing. The definitions for each module are in the separate module folders. Thanks for the positive comment btw!!

[@samreenkhanzada6746]

Great Great help 👍God bless you

[@MaChemGuy]

Thanks, you too!

[@sydneychishimba2506]

Thanks for this helpful video.

[@yumnabarhamji1700]

Brilliant thanks

[@sarahzaatar7367]

this vedio helped me very much thank you

[@Cobenis_Kar]

Awesome video!

[@cocoa8830]

your videos are try helpful, thank you. Will you be making videos on KC, Neutralisation titration curves and pH/

[@georgelee6783]

Thank you for the videos! They're really helpful as I'm not very good at chemistry. I have one question though, surely for the dissociation of H2CO3 would form H2O + CO2, as dissociating it with just H+ and CO2 would have the reverse effect, as your trying to lower the acid(H+) concentration in the first place.

[@1234whipcream]

for the weak acid buffer, wouldn't adding acid raise the concentration of the weak acid since it shifts to the left? if you're raising the concentration of ch3cooh, how would that regulate ph? would making more weak acid lower the pH resulted from the addition of more h+?

[@feruzebrahim9535]

Hello Sir Thank you sooo much for all of these vidoes. They are lifesavers. I just wondering if you did any videos on titration curve and choosing an indicators.😊

[@soroushpaziresh3271]

Wouldn't the formula introduced @14:10 counteract the purpose increasing pH levels when low, since H+ are being dissociated? Couldn't the products be Carbon dioxide and water?

[@BatoulSaadd]

Thank you so much 🥺🤝

[@gulzarabutt]

Really helpful!🙃

[@BilalAhmed-fg7nl]

Hi when you showed the dissociation of carbonic acid, surely since it is a diprotic acid it should dissociate to co32- and 2H+ rather than what you have shown Regardless the video was helpful thanks

[@MaChemGuy]

You are correct that it can donate both protons but these occur one at a time. The dissociation which takes place in the blood is the one I have shown. If you want to know more, check out acid dissociation constants. Thanks for the comment

[@theodo2617]

MaChemGuy Hello have you got any videos on strong and weak acids and strong and weak base calculations? :) Thank you

[@MaChemGuy]

Not yet tommihay greene. Hoping to have them done by Easter

[@MaChemGuy]

tommihay greene All done now :)

[@mohfa1806]

I have a question please : when the enzyme breaks the H2CO3 into H+ and CO2 wouldnt that also shift the 1st reaction to the left to produce more H2CO3 ? ... thank you

[@himanshusoni6096]

I couln't get how the initial part of the video cohesively gets along with the later; you didn't explain why one needs CH3COOH, CH3COONa and h+. *high concentrations of acetic acid, sodium acetate and low of hydronium ions. How did this affects the overall equilibria? Thanks for posting though!

[@trankimchi5478]

thank you so much sir

[@ummewaseem5983]

Wouldnt the large excess of CH3COO- react with the minute amount of H+ from the dissociation of the original acid and increase the pH?

[@MaChemGuy]

It reaches an equilibrium

[@xVbM1]

When making a buffer for say methyl amine with HCL, would the moles of HCL you add to methyl amine have to be half the moles of methyl amine present? This would allow allow you to get equal concentrations of methyl amine and salt?

[@PriyankaGupta-fb8uj]

thank you sir

[@MR2perfectable]

Sorry, I’m a bit confused when adding an acid to the acidic buffer. When we add H+ ions, they would react with the ethanoate ions, using them up. So, wouldn’t the equilibrium shift to the right to replenish the ethanoate ions ? Btw, thank you very much for these videos.

[@MaChemGuy]

Arian I see what you mean but the ethanoate ions are in excess compared to the H+ ions (remember that these come from slight dissociation of the weak acid). So adding extra acid means there will be more H+ than before and so some of the excess ethanoate ions react with them, sending the equilibrium to the left. Hope that clears things up. Glad you like the videos btw :)

[@MR2perfectable]

MaChemGuy Ah, I see, thank you very much !!

[@dopamineater8427]

i have a question if you please, in my book these reactions of an acid with its salt are called "common ion" but if we add a small amount of a strong base or an acid the whole solution becomes buffer, is this correct or the concepts of buffer and common ion are the same?

[@ayaali3285]

Thanks

[@cyrildim1351]

Thank you sir 😊

[@fedrom8262]

Hi Why was the CH3COONa written in yellow? Thanks for the videos, they're really helpful!

[@MaChemGuy]

+Fifitheflower Pot I was trying to get across that due to it's complete dissociation it isn't there in the form of CH3COONa

[@fedrom8262]

+MaChemGuy Thank you for the reply! Why can't buffers stop the change of pH completely instead of minimising the change?

[@MaChemGuy]

+Fifitheflower Pot They can only deal with tiny pH changes. Large addition of acid/base would render the buffer useless

[@rapunzelle21]

THANK YOUU SO MUCH

[@MaChemGuy]

Jesya Ashley You're SO welcome :)

[@mrgg336]

get this legend to 1mil subs

[@maheensamo5691]

owsum lecture it helped me alot:)

[@MaChemGuy]

Maheen Samo Glad to hear it!

[@naddn5321]

+MaChemGuy You really explained this nice! So lucky to find you! Just one question (at 12:55) How can carbonic acid disociate and form enough of HCO3- since it is a weak acid? And since there is no salt (for ex. NaHCO3) in the solution that could have created more of HCO3- as we saw in previous examples? Big thank you in advance!

[@MaChemGuy]

Naki Naki Thanks! I'll ask a doctor and get back to you :)

[@naddn5321]

+MaChemGuy That's really nice of you, thank you!!!

[@MaChemGuy]

Naki Naki Carbonic acid is constantly formed by the reaction between CO2 and H2O. This dissociates to form the HCO3- ion and H+. The H+ ion is removed as it binds to haemoglobin to form haemoglobonic acid. This removal of H+ from the equilibrium drives the equilibrium to replace the lost H+ and thus making more HCO3- too. That's from a doctor of Biology by the way. Will also ask a medical doctor. If you're studying A level Chem I wouldn't worry as this is all way beyond the spec. Very interesting none the less!!

[@thfreakin]

can u do excess weak acid and strong base

[@fedrom8262]

Also if the CH3COOH was minute and was ignored, why wasn't the minute H+ ion ignored? @ 4.58 min

[@MaChemGuy]

+Fifitheflower Pot You need H+ to calculate pH

[@arancienne]

why are they used?

[@lewiscutler489]

If I'm not mistaken basic buffers are no longer on the spec correct?

[@MaChemGuy]

Correct

[@s1xtc3nt]

I think he got the last part wrong its supposed to be carbonic acid breaks down into CO2 and water

[@sharan5857]

stop that was so helpful! thank you!

[@sarahnorman3796]

Do we need to know about basic buffers for OCR A?

[@MaChemGuy]

Nope :)

[@cherrybruce2145]

Why can’t u make. a buffer with weak acid and weak base?

[@raymanster8037]

love you bby

[@vinayshelke6740]

Thanks