What is the pH at the equivalence point when 60.0 mL of 0.250 M N2H4 is titrated by 2.5 x 10^-2 M HI? Kb = 1.7 x 10^-6

Answered: What is the pH at the equivalence point…

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter17: Principles Of Chemical Reactivity: Other Aspects Of Aqueous Equilibria

Section17.3: Acid-base Titrations

Problem 17.6CYU: The titration of 0.100 M acetic acid with 0.100 M NaOH is described in the text. What is the pH of...

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What is the pH at the equivalence point when 60.0 mL of 0.250 M N2H4 is titrated by 2.5 x 10^-2 M HI? Kb = 1.7 x 10^-6

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Step 1

The question is based on the concept of volumetric analysis.

It involves titration of weak base, hydrazine with strong acid hydroiodic acid. at equivalence point, the salt formed is of weak base and strong acid.

So,it undergoes acidic hydrolysis to produce the acidic solution.

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