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Lena772

  • one year ago

. In Trial 1 0.435grams of KHP were dissolved in 100 mL of water and titrated with 21.06mL of NaOH that was later determined to be 0.101M. Calculate the [C8H4O42-]Eq Pt, [OH-]eq, kb, pOH and pH values for the solution at the Equivalence Point. At the Equivalence Point the KHP has been completely converted into the phthalate ion (C8H4O42-) - use the volume of base at the End Point (when the solution just turns pink) to be equivalent to the volume of base at the Equivalence Point.

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  1. Lena772
    • one year ago
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    First calculate the concentration of the phthalate ion at the Equivalence Point, then use this concentration as the "starting" concentration in the following equilibrium: C8H4O42- + H2O ←→ HC8H4O4- + OH- Let "x" be the [OH-]eq and set up an equation where kb = x2 / ([C8H4O42-] - x) Of course you're only given the ka of KHP (3.89 x 10-6), but you know how to convert it to the kb. Finally, from the [OH-]eq, you can find the pOH and the pH. [C8H4O42-]Eq Pt - calculate this answer from the 0.435grams of KHP used initially

  2. Lena772
    • one year ago
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    @aaronq

  3. Lena772
    • one year ago
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    @Timo86m @Photon336

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