**Question:**What is the pH of a buffer containing 0.11 M HClO (aq) and 0.57 M NaClO (aq)?**Options:**- 12.70- 8.23- 7.52- 2.34- 6.81**Explanation:**To find the pH of a buffer solution containing hypochlorous acid (HClO) and its conjugate base sodium hypochlorite (NaClO), you can use the Henderson-Hasselbalch equation:\[ \text{pH} = \text{pKa} + \log \left( \frac{[\text{A}^-]}{[\text{HA}]} \right) \]Where:- \([\text{A}^-]\) is the concentration of the conjugate base, NaClO.- \([\text{HA}]\) is the concentration of the acid, HClO.- pKa is the negative log of the acid dissociation constant (Ka) for HClO, which is typically around 7.5.Substitute the given concentrations into the equation and solve for the pH.

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What is the pH of a buffer containing .11 M HCIO (aq) and .57 M NaCIO (aq)?

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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