Chris it still amazes me how the views of your videos aren't in the hundred-thousands! your clarity and presentation is unsurpassed and I cannot thank you enough for helping me through my A Levels. I told my whole class about you and they love your videos as well! My sincerest thanks man honestly.
Peter Haddad Wow! What a compliment. Thanks very much, I am pleased they are helping. I would love them to reach hundreds of thousands of people as I make them to help people understand Chemistry that little bit better and partly because I love what I do. Sharing videos like you have done helps to get the message out there so I thank you for your efforts! I am twitter @allerytutors so you can follow me for pre release information on future videos and news on a podcast project that I would like to explore next.
honestly I was stressed out in the midst of studying chemistry until I found your playlists, sir. I hope it is not too late to say thank you for being an absolute life-saver! I wish you all the happiness in the world :D
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
Yes! They certainly are! I didn't even bother reading my text book for my mock exam. You're videos were more than enough for me! And thanks to you, my exam was so easy. So I sent your videos to about 40 or so of my friends! oh! thank you sooooo much...
Hi there, I have a question not directly related to buffer calculations but still relevant. A buffer solution has a constant pH even when diluted. Use a mathematical expression to explain this. I saw this question on a past paper and I do not quite understand the answer in the mark scheme which states : concentration of acid/concentration of salt is almost constant. Where did this come from and why is it true?
when the weak acid in a buffer dissociates it forms the equilibrium CH3COOH --> H+ + CH3COO- , when diluted, the OH- concentration increases, which reacts with the H+, reducing the H+ concentration. This causes the equilibrium to shift to the right hand side, causing greater dissociation of CH3COOH to balance out the effect. The opposite happens when acid is added. I think this is correct...
Chris it still amazes me how the views of your videos aren't in the hundred-thousands! your clarity and presentation is unsurpassed and I cannot thank you enough for helping me through my A Levels. I told my whole class about you and they love your videos as well! My sincerest thanks man honestly.
Peter Haddad Wow! What a compliment. Thanks very much, I am pleased they are helping. I would love them to reach hundreds of thousands of people as I make them to help people understand Chemistry that little bit better and partly because I love what I do. Sharing videos like you have done helps to get the message out there so I thank you for your efforts! I am twitter @allerytutors so you can follow me for pre release information on future videos and news on a podcast project that I would like to explore next.
honestly I was stressed out in the midst of studying chemistry until I found your playlists, sir. I hope it is not too late to say thank you for being an absolute life-saver! I wish you all the happiness in the world :D
Chris you are the best Chemistry teacher ever
Bless you! You're the reason I'm passing A2 chemistry
Pleased you found them helpful!
you are a life saver. thanks for this video
Thanks, I’m finding your videos very helpful in revising for my A2 exam
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
GOD BLESS YOU!!!!
Thanks! Hope the videos are helping you.
Yes! They certainly are! I didn't even bother reading my text book for my mock exam. You're videos were more than enough for me! And thanks to you, my exam was so easy. So I sent your videos to about 40 or so of my friends! oh! thank you sooooo much...
Thanks very much for that. The more people that use them the better!
first off, thankyou so muchh for tthis video, cleared up one of the hardest Qs of chem for me :')
my teacher forgot to teach us that we have to assume that moles of base = moles of salt in the buffer... thanks a lot!
Got it now! Thank you!!!
you saved me, thank you so much
if they gave you volumes of the acid and salt would that affect the calculation?
Hi there, I have a question not directly related to buffer calculations but still relevant.
A buffer solution has a constant pH even when diluted.
Use a mathematical expression to explain this.
I saw this question on a past paper and I do not quite understand the answer in the mark scheme which states : concentration of acid/concentration of salt is almost constant. Where did this come from and why is it true?
when the weak acid in a buffer dissociates it forms the equilibrium CH3COOH --> H+ + CH3COO- , when diluted, the OH- concentration increases, which reacts with the H+, reducing the H+ concentration. This causes the equilibrium to shift to the right hand side, causing greater dissociation of CH3COOH to balance out the effect. The opposite happens when acid is added. I think this is correct...
What about calculating the concentration of the salt from the pH and concentration of acid?
Thanks sir
Welcome
Those 4 dislikes are worser than mr cambridge
My guy !!
😘😘
You’re so cute 🥰