CHEMISTRY COMMUNITY

Hello! I saw that during the lecture (this was from like week 2), Dr. Lavelle mentioned that the weaker the base, the higher its Kb value is, which is seen when he compared two different Kb values. Although I feel like I understand that, I'd like to know if there were any key conceptual points that I missed about when I was writing this down. Can someone explain to me the concept of why this came to be, if any? Thank you!

the equilibrium constant is calculated as products/reactants. since weak acids/bases only slightly dissociate in water, they'd only form a bit of products. Whereas for strong acids/bases they would completely dissociate, where products >> reactants. from the Kb, the greater the value, the lower the pkb, and the stronger the base. (and vice versa)

the bigger the kb, the lower the pkb (log properties) which also means the stronger the base

Veronica Lu 2H wrote:the bigger the kb, the lower the pkb (log properties) which also means the stronger the base

so then did Lavelle mean to say that the higher the kb, the stronger the base? because the original post here says that he stated that the higher the kb, the weaker the base. now I'm confused.

Lower pKb indicates a stronger base. We know that pKb is the -log(Kb) so if the value of Kb is large, pKb will be lower. The greater the value of Kb, the lower the value of pKb (stronger base).