**Problem: Calculate the pH of a Solution**Calculate the pH of a solution that contains 150 mL of 0.25 M NaF and 252 mL of 0.30 M HF.Given:\[ K_a = 3.5 \times 10^{-4} \]**Solution Explanation:**To solve this problem, you need to determine the concentration of hydrogen ions (\([H^+]\)) in the solution to find the pH. This involves using the concept of a buffer solution since the solution contains both a weak acid (HF) and its conjugate base (NaF).1. **Convert Volume to Liters:** - Volume of NaF: \(0.150 \, \text{L}\) - Volume of HF: \(0.252 \, \text{L}\)2. **Calculate the Number of Moles:** - Moles of NaF: \(0.150 \, \text{L} \times 0.25 \, \text{M} = 0.0375 \, \text{moles}\) - Moles of HF: \(0.252 \, \text{L} \times 0.30 \, \text{M} = 0.0756 \, \text{moles}\)3. **Calculate Concentrations in the Mixture:** - Total Volume \(= 0.150 \, \text{L} + 0.252 \, \text{L} = 0.402 \, \text{L}\) - Concentration of NaF: \(\frac{0.0375 \, \text{moles}}{0.402 \, \text{L}} \approx 0.0933 \, \text{M}\) - Concentration of HF: \(\frac{0.0756 \, \text{moles}}{0.402 \, \text{L}} \approx 0.188 \, \text{M}\)4. **Apply the Henderson-Hasselbalch Equation:**\[\text{pH} = \text{pK}_a + \log\left(\frac{[\text{A}^-]}{[\text{HA}]}\right)\] - \(\text{pK}_a = -\

Given volume of HF is 252 mL and strength is 0.30 M Given volume of NaF is 150 mL and strength is…

Answered: 2. Calculate the pH of a solution that…

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2. Calculate the pH of a solution that contains 150 mL of 0.25 M NaF and 252 ml of 0.30 M HF. K, = 3.5 x 104

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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