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

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wcaprarBest ResponseYou've already chosen the best response.1
Writing 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?
 2 years ago

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

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

PreethaBest ResponseYou've already chosen the best response.1
You 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.
 2 years ago

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