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Calculate the percent ionization of a 0.15 formic acid solution in a solution containing 0.11 potassium formate.

I have the formic acid Ka=1.8 *10^-4
When I solve for "x" I'm getting 1.1.44*10^-2 When I plug that into equation (x/0.15-x)*100, I'm getting 10.6% which is incorrect. I getting lost in the math, plz help. Thanks

Question ID
523630

Created
April 1, 2011 12:24am UTC

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0

URL
https://questions.llc/questions/523630

Answers
2

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2848

2 answers

  1. I don't believe it's the math. Let's simplify the formic acid and call it HF (I know that isn't right but it saves typing).
    HF ==> H^+ + F^- and KF ==>K^+ + F^-
    HF = 0.15M at the start. F^- from KF = 0.11
    (H^+)(F^-)/(HF) = Ka
    (H^+) = x
    (F^-) = x + 0.11 but since x is small we can make this equal to 0.11.
    (HF) = 0.15-x but since x is small we can make this equal 0.15.
    Solve for x = (H^+). I get an answer of 2.45E-4 = (H^+). By the way, I solved the quadratic we get if we keep x+0.11 and 0.15-x and I get 2.445E-4 so there is almost no error in making the assumptions.
    Then % ion = (ions/0.15)*100 = (2.45E-4/0.15)*100 =??
    Note that I've carried too many significant figures, you should correct that, especially if you are keying the answer into a database.

    Answer ID
    523802

    Created
    April 1, 2011 4:55am UTC

    Rating
    1

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  2. Thank you so much! I see what I was doing wrong now. I need more practice with these type problems.

    Answer ID
    523951

    Created
    April 1, 2011 5:42pm UTC

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    0

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