Recent content by Melvincalvin

thank you for the help btw :) !

I can setup my ice table like that fine, but where does [NaF] come into play, do I just add 0.50M to F- when I have equilibrium concentrations??

So the if it all dissociates then the initial concentration for F- should be 0.5M. I use that molarity but it still doesn't seem to work out. I can't seem to get anything to equal the equilibrium constant.

HF(aq) ↔ H+ + F- Determine equilibirum concentrations with Initital concentrations and Kc. Kc = 7.2 x 10-4 [HF] = 1.00M [NaF] = 0.50M I understand how to do an ICE table and put together questions, but what do you do with [NaF] when it is not part of the chemical equation? How to I factor it...