Henderson-Hasselbalch Equation

The Henderson-Hasselbalch equation is described and an example problem of how to calculate the pH of a buffer solution using the equation is given. Also in this video are some Tips & Tricks, including a word on pH and buffer capacity of buffer solutions.

[@luxtertales7210]

Man i am arabian
And i understood your explaining
Better that arabian teachers
Keep going

[@CB_10775]

This genuinely helped me. Thanks Dr. T!

[@alcd6333]

Good refresher course in analytical chemistry: well-presented and concise.

[@kingvon3483]

This explanation was really helpful 🙌

[@jivarnejoseph7448]

Great explanation . Made it clear to understand.

[@mrjean913]

Awesome your explanation is a lot easier to understand thank you.

[@azzahranabilah7272]

That's awesome Dr.T!!!
I have a question... Can we calculate the volume of those base and acids to add on the solution by using this equation according to pH we wanted?

[@backseatkisses]

Thank you Dr. T(errific)!!

[@FartunBishar-rt1du]

Where does that 4.202 came from please 🙏

[@salvebartolome8433]

Its -log(Ka)
The Ka is already given so it's 6.3×10^-5
So to get that 4.202, do the equation, which is -log(6.3×10^-5)
Solve it to see

[@palulaylalaineale.7837]

​@@salvebartolome8433and the answer is 4.200

[@mototsumi]

what it you aren't given a salt value or second volume in a question?

[@princessparty44]

How do you calculate -log without a calculator?

[@harmony8623]

You can’t 💀 unless ur a mega genius ig or The numbers are very specific

[@ميميشان-ع2ث]

How do I calculate the logarithm 10 s- six point three in ten s-negative5 without calculator

[@唐以沫]

why does my calculator says 4.2006 not 4.202 :'((

[@hailgerald2060]

Very helpful

[@valtallica]

Thank youuuuuu!!!

[@janealacantara4388]

Thankyou!

[@annaschusser9661]

Why is the [H+] equal to 0?

[@sethkempe7675]

its not its 10^-7
but its negligible

[@K8tJayne]

Thankyou

[@canadianhaitian]

I didn't get 4.202 for pka???

[@itzjackie9091]

-log(6.3*10^-5)=4.201

[@palulaylalaineale.7837]

​@@itzjackie9091it's 4.200

[@nomindashtsengel9218]

i don`t understand the pH=4.202+log how did 0.301 come out?

[@vivekpatel4661]

because log(0.1/0.2) = 0.301

[@nazgulwraith2281]

and it is less than 1 so -0.301

[@hailgerald2060]

Hahaha

[@dylanpointon8131]

Yeah but ph = 4.202 + log (-0.301) = 3.9

[@anonanonymous1248]

Think it's supposed to be CONCENTRATION of base/CONCENTRATION of acid. The square brackets mean concentration. So concentration instead of just using number of moles given into the log (_/_). So it was supposed to be log (of 0.1 divided by 1000ml / 0.2 divided by 1000ml) .because Concentration = no. Of moles/ volume and there is 1 litre=1000 ml . You use the number of moles to calculate concentration and then use that amount in the log

[@hajernt7833]

👏👏👏

[@aryaa3998]

Thanks, ^^

[@shawnguerra2047]

Great explanation thanks dr.T!

[@danb4717]

"Henderson Hastleback"

[@streamleazefishhouse]

How do you change this to find the pH of solution in a titration if you have the moles and find your pH?

[@vibhavk8843]

+streamleazefishhouse molarity or normality would be given and the volume

[@kylepham5842]

Dr. T W

[@kaciemarie9859]

Thank you! This is amazing 🙌🏻💚