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

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