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5. 50.0mL of 0.10M HCl solution is mixed with 80.0mL 0.035M NH, aqueous solution. What is the pH of the resulting solution?

5. 50.0mL of 0.10M HCl solution is mixed with 80.0mL 0.035M NH, aqueous solution. What is the pH of the resulting solution?

Chemistry
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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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A Calculating the pH of a Buffer: pH = pk + log HA This equation is known as the Henderson-Hasselbalch equation. This applies only to buffers.
Transcribed Image Text:A Calculating the pH of a Buffer: pH = pk + log HA This equation is known as the Henderson-Hasselbalch equation. This applies only to buffers.
5. 50.0mL of 0.10M HCl solution is mixed with 80.0mL 0.035M NH, aqueous solution. What is the pH of the resulting solution?
Transcribed Image Text:5. 50.0mL of 0.10M HCl solution is mixed with 80.0mL 0.035M NH, aqueous solution. What is the pH of the resulting solution?
Expert Solution
Step 1: Determine the pH of the resulting solution after mix given aqueous solutions:

Given,

The molarity of HCl solution = 0.10 M

Volume of HCl solution = 50.0 mL

The molarity of NH3 solution = 0.035 M

Volume of NH3 solution = 80.0 mL

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