I'm having a hard time getting the right answer to this question A buffer solution contains 0.237 M C6H5NH3 Cl and 0.366 M C6H5NH2 (aniline). Determine the pH change when0.090 mol HCl is added to 1.00 L of the buffer. (Assume Kb (C6H5NH₂) = 7.4 × 10−¹⁰.)=pH after addition - pH before addition = pH change :

Volume of buffer solution V = 1.00 L Number of moles of HCl added = 0.090 mole Concentration of…

A buffer solution contains 0.237 M C6H5NH3 Cl and 0.366 M C6H5NH₂ (aniline). Determine the pH change when 0.090 mol HCl is added to 1.00 L of the buffer. (Assume K₁ (C6H5NH₂) = 7.4 × 10−¹⁰.) pH after addition - pH before addition = pH change =

A buffer solution contains 0.237 M C6H5NH3 Cl and 0.366 M C6H5NH₂ (aniline). Determine the pH change when 0.090 mol HCl is added to 1.00 L of the buffer. (Assume K₁ (C6H5NH₂) = 7.4 × 10−¹⁰.) pH after addition - pH before addition = pH change =

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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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.

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I'm having a hard time getting the right answer to this question

A buffer solution contains 0.237 M C6H5NH3 Cl and 0.366 M C6H5NH2 (aniline). Determine the pH change when
0.090 mol HCl is added to 1.00 L of the buffer. (Assume Kb (C6H5NH₂) = 7.4 × 10−¹⁰.)
=
pH after addition - pH before addition = pH change :

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