Using Ka vs Kb

[Connie Liang 3L]

If in one reaction you have an acid ionizing and a base gaining a proton at the same time, why would you use Ka over Kb and vice versa?

[Hannah Biju 1E]

If there is formation of an acid (H3O+), then you should use Ka. If there is formation of a base (OH-), then you should use Kb.

[Muskaan Abdul-Sattar]

Hey! As Hannah said, I believe Ka is used when dealing with the formation of acids while Kb is used when dealing with the formation of bases.

[Fiona Huang 3C]

If you have an acid dissociating or when H3O+ is formed, you would use Ka. When a base is dissociating, you would use Kb. Also, Ka x Kb = Kw = 10-14.

[Julianna Shimabukuro 1D]

As everyone else has stated, Ka is for the formation of acids and Kb is for the formation of bases. A way to memorize this is that Ka has an "a" in it for acids, and Kb has a "b" in it for bases.

[Gicelle Rubin 1E]

If there is formation of an acid (H3O+), then you should use Ka. If there is formation of a base (OH-), then you should use Kb.

Thank you for your clarification! I had totally forgotten about this!

[Rajshree 1F]

if the product formed is H3O+ then Ka should be used and if OH- is formed then Kb should be used.

[OmarArafat_2K]

With Acid dissociations/formations, you use Ka. With base dissociations/formations, use Kb.

[Sarah Huh 1K]

Ka is used for the formation of acids (H30+ in product), while Kb is used for the formation of bases (OH-)