A buffer solution contains 0.235 M C6H5NH3 Br and 0.385 M C6H5NH2 (aniline). Determine the pH change when 0.112 mol HI is added to 1.00 L of the buffer. (Assume K₂ (C6H5NH₂) = 7.4 × 10-¹⁰.) pH after addition - pH before addition = pH change = Submit Answer

A buffer solution contains 0.235 M C6H5NH3 Br and 0.385 M C6H5NH2 (aniline). Determine the pH change when 0.112 mol HI is added to 1.00 L of the buffer. (Assume K₂ (C6H5NH₂) = 7.4 × 10-¹⁰.) pH after addition - pH before addition = pH change = Submit Answer

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter14: Acid- Base Equilibria

Section: Chapter Questions

Problem 100CWP: Consider 1.0 L of a solution that is 0.85 M HOC6H5 and 0.80 M NaOC6H5. (Ka for HOC6H5 = 1.6 1010.)...

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Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

A buffer solution contains 0.235 M C6H5NH3 Br and 0.385 M C6H5NH₂ (aniline).
Determine the pH change when 0.112 mol HI is added to 1.00 L of the buffer.
(Assume K₂ (C6H5NH₂) = 7.4 × 10-¹⁰.)
pH after addition - pH before addition = pH change =
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Step 1: Determine the pH of the buffer solution from the given data:

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Step 2: Calculation for pH of the solution before add any HI:

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Step 3: Calculation for pH after addition of HI:

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