**Buffer Solution Problem**A buffer solution contains 0.447 M hypochlorous acid and 0.236 M potassium hypochlorite.If 0.0335 moles of sodium hydroxide are added to 250 mL of this buffer, what is the pH of the resulting solution? (Assume that the volume does not change upon adding sodium hydroxide)\[ \text{pH} = \_\_\_\_ \]---**Explanation:**To solve this problem, you will need to understand how adding a strong base (sodium hydroxide) to a buffer affects its pH. You can use the Henderson-Hasselbalch equation which is given as:\[ \text{pH} = \text{p}K_a + \log \left( \frac{[\text{A}^-]}{[\text{HA}]} \right) \]Where:- \(\text{p}K_a\) is the negative base-10 logarithm of the acid dissociation constant (\(K_a\)) of the weak acid (hypochlorous acid in this case).- \([\text{A}^-]\) is the concentration of the conjugate base (hypochlorite ion).- \([\text{HA}]\) is the concentration of the weak acid (hypochlorous acid).**Steps to Calculate:**1. **Calculate the initial moles of Hypochlorous Acid (HA) and Hypochlorite Ion (A⁻)**: - Initial moles of hypochlorous acid ([\(\text{HA}\)]): \(0.447 \, M \times 0.250 \, L = 0.11175 \, \text{moles}\) - Initial moles of hypochlorite ([\(\text{A}^-\)]): \(0.236 \, M \times 0.250 \, L = 0.059 \, \text{moles}\) 2. **New concentrations after adding NaOH**: - Since NaOH is a strong base, it will react completely with the weak acid (\(\text{HA}\)). - Moles of NaOH added: \(0.0335 \, \text{moles}\) - After reaction: New \([\text{HA}]\) = Initial \([\text{HA

Given the molarity of hypochlorous acid, HClO = 0.447 M Molarity of sodium hypochlorite, NaClO =…

A buffer solution contains 0.447 M hypochlorous acid and 0.236 M potassium hypochlorite. If 0.0335 moles of sodium hydroxide are added to 250 mL of this buffer, what is the pH of the resulting solution ? (Assume that the volume does not change upon adding sodium hydroxide) pH = =

A buffer solution contains 0.447 M hypochlorous acid and 0.236 M potassium hypochlorite. If 0.0335 moles of sodium hydroxide are added to 250 mL of this buffer, what is the pH of the resulting solution ? (Assume that the volume does not change upon adding sodium hydroxide) pH = =

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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