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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.
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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Lena772
 one year ago
Best ResponseYou've already chosen the best response.0First 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 106), 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
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