Henderson-Hasselbalch equation | Acids and bases | AP Chemistry | Khan Academy

[@n.k.3405]

THIS CHANNEL HAS BEEN UP FOR YEARS AND YET THEY'RE STILL POSTING VIDEOS... AHHHHHHHHHH

[@L_Lawliet1907]

They’re one of the biggest education platforms lol

[@yourlocalscribe948]

@@L_Lawliet1907 los santos

[@mothman663]

Thank God for Khan Academy...

[@Cacophonyofvoices]

What an amazing, short concept video. Thank you!

[@divyasingh8147]

Such a good explanation I hve ever seen.

[@reginakatilo7032]

The lesson was cool... Thanks 😊

[@yaminaboub-jo2lb]

Thank you , this is really helpful

[@azca.]

1:50 - How did you get the Ka value?

[@arthurchan4277]

google. it should be given if you need it on an exam.

[@MrBoomington]

We actually had to prove this equation in the A-level exam. Yeah been 2 months now I kinda forgot it lol

[@randomvideos4296]

What exam board?

[@reemalzubaidy6037]

U sound like Sheldon from Big Bang theory thank u

[@Protimonride]

Thank You. 🖤

[@syedashobnam2573]

Or u can think it like this more conjugate base = more basic and higher pH, more acid= acidic solution less pH.

[@LINKJW]

thank you!

[@charliebrett7510]

At 3:50 I’m confused. I thought a weak acid partially dissociates into its ions in an equilibrium EQUALLY in a one to one ratio e.g CH3COOH->CH3COO- + H+. So the concentration of CH3COOH ALWAYS equals the conc of CH3COO- providing the volume of the buffer solution is constant. As m=cv c=m/v and so same moles/Same volume should give same conc for both CH3COOH and CH3COO- each time? Why is it 6 and 4? Can someone please explain?

[@dawsonlin5929]

Weak acids dissociate into their ions at an equilibrium based on their Ka value, so they don't always dissociate into a one-to-one ratio all the time. Furthermore, a buffer solution is formed by mixing a weak acid and its conjugate base, the concentrations of which are up to the scientist conducting the experiment. This buffer solution happens to have a ratio of 6 to 4, so he is calculating the pH in this particular scenario. Hope this helps!

[@charliebrett7510]

@@dawsonlin5929 so to recap, weak acids can dissociate into even amounts of their ions or uneven amounts of their ions based on their Ka. So in a calculation you would have to know the moles of the ions it dissociates into and the weak acid separately as there is rarely a 1:1 ratio. And thank you so much!

[@Logan-tg5we]

yet again another video I have wasted time watching that doesnt include how to calculate acid and base concentration for the equation. 7 min of my life I will never get back, thank you so much for not helping in any measurable way.

[@xinyi9118]

dont be a debby downer

[@micaelawillet8760]

you can use an ice table. There are other videos that explain how to find the h3o and oh concentrations.

[@subhamkarmakar3320]

Nice

[@sapphireherkimere128]

What to do if there is a x10 on the pKa given to us while finding the pH, example is pKa = 1.28 x 10

[@thomasrimer1611]

That just means the pKa is 12.8 1.28*10=12.8, that is scientific notation

[@L_Lawliet1907]

Like the other guy said, it’s just scientific notation. Just move the decimal place to the right by one.

[@eliasnakhle8534]

MATH

[@SD33396]

Hi sir

[@szxnv]

:)