I could never get a good grasp of acids and bases, even throughout college, but the way you explained this has been extremely helpful. I wish I had teachers like you when I was learning chemistry basics in school
You are literally the reason as to why I understand chemistry. My professor has made these concepts out to be so difficult and you make it so simple and explain it so well! You are a LIFESAVER! Definitely coming back for Organic chem help! Thank you!
Trust in the Lord with all your heart and lean not on your own understanding. In all your ways acknowledge Him and he shall make your paths straight. Proverbs 3:5+6
Hey Dhruv! If you explore the channel you'll see an old Gen Chem playlist with buffers and titrations covered in chapter 17. This lesson is part of an updated playlist and I'll be remaking and releasing these analogous chapter 17 videos week after next. But the old ones are also embedded in a free course on my site often with some extra content and organized with a dropdown menu that you might appreciate. You'll find the lessons here: www.chadsprep.com/chads-general-chemistry-videos/buffer-chemistry/ www.chadsprep.com/chads-general-chemistry-videos/titration-curves/ www.chadsprep.com/chads-general-chemistry-videos/titration-calculations/ Lots of extra content for titration calculations on that last page. Hope this helps!
Thank you so much for the amazing lesson! I was just wondering if you have any plans on teaching inorganic or analytical chemistry and making videos in those fields? Because you're the best teacher i've EVER had
sir may you please assist in solving the following problem A 25ml sample of 0,10M sodium benzoate is titrated with 0,10 M of HCl what is the pH of after the addition of of 32,0ml of HCl (kb of C6H5CO2- =1,6X10^-10)
I cover titrations in this playlist in chapter 17. I specifically cover weak acid/strong base and weak base/strong acid in this lesson: ru-vid.com/video/%D0%B2%D0%B8%D0%B4%D0%B5%D0%BE-3Y9TaxwcQGs.html Tune in around 21:16 for how to calculate the pH when you are past the equivalence point. Hope this helps!
I wish I could have you as my professor. Out of all the chemistry professors I have delt with. you seem informed, organised, and able to communicate effectively...As a student that is all i am asking for.
Hi Chad, can you explain why acids only donate 1 H+ to become a base? For example, why isn't the base of acid CH3COOH then CH2-COO- for example, or why not donate all the H to become C(3negative)COO-? Or NH4+ then N(4negative) instead of NH3?
Not all of those H's in CH3COOH are acidic. The H-C bonds are not polar so it is not easy to break the bond and lose the H. The O-H bond in a carboxylic acid is much weaker due to high polarity of the O-H bond and further charge delocalization from the carbonyl group which stabilizes the conjugate base CH3COO- making that H acidic (dissociation occurs in solution). In order to break the C-H bond we would have to put energy in, it wouldn't freely dissociate in solution. Hope that helps!
