A 35.0 mL sample of a 0.110 M HBrO solution was titrated with 0.125 M KOH. The Ka for HBrO is 2.0 ×10^-9 a. How much volume is needed to reach the equivalence point? b. What is the pH of the solution before titration? c. What is the pH of the solution after 15.4 mL have been added?
A 35.0 mL sample of a 0.110 M HBrO solution was titrated with 0.125 M KOH. The Ka for HBrO is 2.0 ×10^-9 a. How much volume is needed to reach the equivalence point? b. What is the pH of the solution before titration? c. What is the pH of the solution after 15.4 mL have been added?
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Chapter16: Acid-base Equilibria
Section: Chapter Questions
Problem 16.135QP: A 30.0-mL sample of 0.05 M HClO is titrated by a 0.0250 M KOH solution Ka for HClO is 3.5 108....
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A 35.0 mL sample of a 0.110 M HBrO solution was titrated with 0.125 M KOH. The Ka for HBrO is 2.0 ×10^-9
a. How much volume is needed to reach the equivalence point?
b. What is the pH of the solution before titration?
c. What is the pH of the solution after 15.4 mL have been added?
d. What is the pH of the solution after 20.0 mL have been added?
e. What is the pH of the solution after 30.8 mL have been added?
f. What is the pH of the solution after 40.0 mL have been added?
g. Sketch a plot of pH vs volume added, labeling the points for
b-f.
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