A sample weighing 1.25 g of the diprotic acid potassium acid phthalate (KHP) is dissolved in 50.0 ml of water. Consider the titration of this solution with 0.100 M NaOH. The two Ka's for KHP are 1.12 x 10-3 and 3.90 x 10-6. a. Calculate the pH of this solution before adding any NaOH. b. How many ml of NaOH must be added to reach the equivalence point? What is the pH at the equivalence point? c. Calculate the pH of the solution after 100. ml of NaOH have been added.
A sample weighing 1.25 g of the diprotic acid potassium acid phthalate (KHP) is dissolved in 50.0 ml of water. Consider the titration of this solution with 0.100 M NaOH. The two Ka's for KHP are 1.12 x 10-3 and 3.90 x 10-6. a. Calculate the pH of this solution before adding any NaOH. b. How many ml of NaOH must be added to reach the equivalence point? What is the pH at the equivalence point? c. Calculate the pH of the solution after 100. ml of NaOH have been added.
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Chapter16: Acid-base Equilibria
Section: Chapter Questions
Problem 16.144QP
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Transcribed Image Text:A sample weighing 1.25 g of the diprotic acid
potassium acid phthalate (KHP) is dissolved in
50.0 ml of water. Consider the titration of this
solution with 0.100 M NaOH. The two Ka's for
KHP are 1.12 x 10¯3 and 3.90 x 10
a. Calculate the pH of this solution before
adding any NaOH.
b. How many ml of NaOH must be added to
reach the equivalence point? What is the pH
at the equivalence point?
c. Calculate the pH of the solution after 100.
ml of NaOH have been added.
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