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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?

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1. wcaprar

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. bouhehad

where is NaF in your chemical formula?? You have it as one of your givens but were would you use it in your solution?

3. wcaprar

NaF would dissociate in solution with Na becoming spectator ion. So the concentration of NaF is used for the initial concentration of F-

4. Preetha

You can look up Kas. There is probably a table in the back of your book. Acid dissociation constants. 7.2 x 10-4. 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.

5. wcaprar

Aha! I see! I thought that I was supposed to calculate that somehow, lol. I found it now, thanks!

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