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wcaprar
 3 years ago
Buffer solution problem: Calculate the pH of a solution that is 0.30 M in HF and 0.15 M in NaF?
wcaprar
 3 years ago
Buffer solution problem: Calculate the pH of a solution that is 0.30 M in HF and 0.15 M in NaF?

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wcaprar
 3 years ago
Best ResponseYou've already chosen the best response.1Writing out the chemical formula would be HF + H20 = H30+ + F . I would do an ICE table to find out what everything is in equilibrium and thats where I get stuck. I don't have a Ka value. Where do I find it/how to I solve for it?

bouhehad
 3 years ago
Best ResponseYou've already chosen the best response.0where is NaF in your chemical formula?? You have it as one of your givens but were would you use it in your solution?

wcaprar
 3 years ago
Best ResponseYou've already chosen the best response.1NaF would dissociate in solution with Na becoming spectator ion. So the concentration of NaF is used for the initial concentration of F

Preetha
 3 years ago
Best ResponseYou've already chosen the best response.1You can look up Kas. There is probably a table in the back of your book. Acid dissociation constants. 7.2 x 104. This relationship is called the Henderson Hasselbach equation. pH = pKa + log [A]/[HA]. Use molar quantities and plug it in. ICE table will give you the same answer.

wcaprar
 3 years ago
Best ResponseYou've already chosen the best response.1Aha! I see! I thought that I was supposed to calculate that somehow, lol. I found it now, thanks!
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