Thanks for the video. One note: for your half-reactions shown at 5:50, the potentials should be the same as one another (+0.222 V vs. SHE). Just because you flip the way you write the equation, doesn't mean you need to put a negative sign on the potential! The equation describes an equilibrium so can be written in either direction. Convention is to use the Standard Hydrogen Electrode (SHE) as the anode in some theoretical cell against whatever reaction you're referring to - in this case Ag/AgCl - thus it's a Standard Reduction Potential of Ag/AgCl.
Hands-down the best explanation I have found. I will be borrowing your approach to teach my students. Thanks!
Thank you very much. We're glad you like it!
Thank you for this! This is the only explanation I’ve been able to find that allowed me to understand what exactly is going on.
THANK YOU❤
Great explanation!
What a video... thanks man!
Thanks for the video. One note: for your half-reactions shown at 5:50, the potentials should be the same as one another (+0.222 V vs. SHE). Just because you flip the way you write the equation, doesn't mean you need to put a negative sign on the potential! The equation describes an equilibrium so can be written in either direction. Convention is to use the Standard Hydrogen Electrode (SHE) as the anode in some theoretical cell against whatever reaction you're referring to - in this case Ag/AgCl - thus it's a Standard Reduction Potential of Ag/AgCl.
Thank you very much for the correction! Hopefully we can get that corrected shortly.