Henderson-Hasselbalch equation | Acids and bases | AP Chemistry

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

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2 жыл бұрын

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One way to determine the pH of a buffer is by using the Henderson-Hasselbalch equation, which is pH = pKₐ + log([A⁻]/[HA]). In this equation, [HA] and [A⁻] refer to the equilibrium concentrations of the conjugate acid-base pair used to create the buffer solution. When [HA] = [A⁻], the solution pH is equal to the pKₐ of the acid. View more lessons or practice this subject at www.khanacademy.org/science/a...
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Пікірлер: 28

@Bedlaminhavana 3 ай бұрын

What an amazing, short concept video. Thank you!

@n.k.3405 2 жыл бұрын

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

@L_Lawliet1907 2 жыл бұрын

They’re one of the biggest education platforms lol

@yourlocalscribe948 2 жыл бұрын

@@L_Lawliet1907 los santos

@Protimonride 2 жыл бұрын

Thank You. 🖤

@MrBoomington 2 жыл бұрын

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

@randomvideos4296 2 жыл бұрын

What exam board?

@yaminaboub-jo2lb 2 ай бұрын

Thank you , this is really helpful

@azca. 2 жыл бұрын

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

@arthurchan4277 2 жыл бұрын

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

@divyasingh8147 2 жыл бұрын

Such a good explanation I hve ever seen.

@reginakatilo7032 Жыл бұрын

The lesson was cool... Thanks 😊

@LINKJW Жыл бұрын

thank you!

@mothman663 2 ай бұрын

Thank God for Khan Academy...

@reemalzubaidy6037 2 жыл бұрын

U sound like Sheldon from Big Bang theory thank u

@charliebrett7510 2 жыл бұрын

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 2 жыл бұрын

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 2 жыл бұрын

@@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!

@syedashobnam2573 9 ай бұрын

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

@subhamkarmakar3320 2 жыл бұрын

Nice

@sapphireherkimere128 2 жыл бұрын

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 2 жыл бұрын

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

@L_Lawliet1907 2 жыл бұрын

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

@eliasnakhle8534 2 жыл бұрын

MATH

@Logan-tg5we 10 ай бұрын

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 8 ай бұрын

dont be a debby downer

@micaelawillet8760 4 ай бұрын

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