What if we use weak base like bicarbonate sodium to make ascorbate sodium how we can calculate the buffer cause its not gonna dissolve completely ? And thanks for the video
Definitely not. A buffer is its most effective when they are equal, but it is not necessary and in most instances, it is not possible to get the buffer at an exact pH without having the concentrations slightly different.
@@RoxiHulet Hello mam, I am a research scholar who needs your favour for my doubt. How to prepare 25 ml of 0.1 mol/L Sodium acetate buffer ( PH-6), containing 5.0mmol/L ethylenediaminetetracetic acid and 5.0 mmol /L Cysteine ? Plz clarify me as soon as possible, Bez I am struggling to get clear .🙏🏾
It gets always talked about the addition of a strong acid or strong base to a buffer... my question would be how to calculate the ph with the addition of a weak acid?. Lets say the addition of acetic acid to a phosphate buffer
Using a strong base is necessary to ensure that the last part of the ice table works out the way it does, had she used a weak one there would have been leftover base which would have messed with the pH and the reaction would have yielded different amounts of acid and conjugate base
I’m pretty frustrated with the American school system, my professor does not go through these with us in class at all and there is no way I can remember all of these steps just from watching a couple of RUclips videos. My exam is tomorrow.
That is very frustrating, I sympathize. My advice is to work out as many problems as you can to get the practice. This is a hard concept! When I was a student, I found that repetitive practice was the best way for me to learn things like this. Good luck to you!
By far the best video I've been able to find on this subject! Thank you so much!
You’re welcome!
You are awesome!!!Thank you so much!!! May god bless you.
Hi, I'm come from Vietnam. This video is useful for me. Thanks you so much and wish you have a good day!
thank you, great multi-concept problem, thumbs up
You’re welcome!!
how about if they gave you a specific Molarity for both the acid and the base, and not choose whatever you want. Would this still work?
What if we use weak base like bicarbonate sodium to make ascorbate sodium how we can calculate the buffer cause its not gonna dissolve completely ?
And thanks for the video
OMG I LOVE U SO MUCH FOR MAKING THIS VIDEO
Thanks for making it simple :)
amazing video, everything you need is within the first minute
Awesome video!
How would you prepare a 50 mL buffer using 0.5 M acetic acid and 0.4 M NaOH. Target pH is 4.3.
don't the conecntrations of weak acid and its conjugate base have to be equal though?
Definitely not. A buffer is its most effective when they are equal, but it is not necessary and in most instances, it is not possible to get the buffer at an exact pH without having the concentrations slightly different.
How to have a buffer 1x or 9x, 7x ... how to caculate ?
Good evening, is there any strategy that I can use to calculate all buffer solutions calculations?
Thank you for your kind explanation. But I have a question, how to apply this explanation to polyprotic acid?
No changes are necessary for a polyprotic acid. Just make sure you are correctly identifying the acid and base.
@@RoxiHulet Hello mam, I am a research scholar who needs your favour for my doubt.
How to prepare 25 ml of 0.1 mol/L Sodium acetate buffer ( PH-6), containing 5.0mmol/L ethylenediaminetetracetic acid and 5.0 mmol /L Cysteine ?
Plz clarify me as soon as possible, Bez I am struggling to get clear .🙏🏾
very helpful >from KFUPM
I still can't find any concise way to make a buffer with pH of 4,01...
It gets always talked about the addition of a strong acid or strong base to a buffer... my question would be how to calculate the ph with the addition of a weak acid?. Lets say the addition of acetic acid to a phosphate buffer
عاشت ايدج
Isn't the use of strong base invalidate the rule of having a buffer solution?
Using a strong base is necessary to ensure that the last part of the ice table works out the way it does, had she used a weak one there would have been leftover base which would have messed with the pH and the reaction would have yielded different amounts of acid and conjugate base
Love you ❤️❤️
I’m pretty frustrated with the American school system, my professor does not go through these with us in class at all and there is no way I can remember all of these steps just from watching a couple of RUclips videos. My exam is tomorrow.
That is very frustrating, I sympathize. My advice is to work out as many problems as you can to get the practice. This is a hard concept! When I was a student, I found that repetitive practice was the best way for me to learn things like this. Good luck to you!
Wouldn't that result in a 100 mL buffer solution because both the weak acid and the base were solved for 50mL?
Sarah Sisney no. because it just shows how much moles do you need in a 50 mL buffer solution. :)
it accounts for the total volume of the buffer solution
Thank hunny finally get it 😘😘