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What is the pH of a 1.0 L solution that is 0.50 M PO4³- and 0.50 M HPO4²-? a. If 0.01 moles of OH is added to the above buffer, what will the new pH be? Change of volume is negligible. b. If 0.01 moles of OH- is added to 1.0 L of water, what will the new pH be? Change of volume is negligible.

What is the pH of a 1.0 L solution that is 0.50 M PO4³- and 0.50 M HPO4²-? a. If 0.01 moles of OH is added to the above buffer, what will the new pH be? Change of volume is negligible. b. If 0.01 moles of OH- is added to 1.0 L of water, what will the new pH be? Change of volume is negligible.

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
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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### Problem Statement **1. What is the pH of a 1.0 L solution that is 0.50 M PO₄³⁻ and 0.50 M HPO₄²⁻?** **a. If 0.01 moles of OH⁻ is added to the above buffer, what will the new pH be? Change of volume is negligible.** **b. If 0.01 moles of OH⁻ is added to 1.0 L of water, what will the new pH be? Change of volume is negligible.** ### Explanation: - **Given Buffers and their Concentrations:** - The solution contains 1.0 L of 0.50 M PO₄³⁻ and 0.50 M HPO₄²⁻. - **Scenarios to Consider:** 1. Addition of OH⁻ to the buffer solution and its impact on the pH. 2. Addition of OH⁻ to pure water and its impact on the pH. **Note:** The calculations require the use of the acid-base equilibrium principles and appropriate formulas to deduce the new pH levels in both scenarios. Further details and step-by-step calculations should be provided in the educational content for comprehensive learning.
Transcribed Image Text:### Problem Statement **1. What is the pH of a 1.0 L solution that is 0.50 M PO₄³⁻ and 0.50 M HPO₄²⁻?** **a. If 0.01 moles of OH⁻ is added to the above buffer, what will the new pH be? Change of volume is negligible.** **b. If 0.01 moles of OH⁻ is added to 1.0 L of water, what will the new pH be? Change of volume is negligible.** ### Explanation: - **Given Buffers and their Concentrations:** - The solution contains 1.0 L of 0.50 M PO₄³⁻ and 0.50 M HPO₄²⁻. - **Scenarios to Consider:** 1. Addition of OH⁻ to the buffer solution and its impact on the pH. 2. Addition of OH⁻ to pure water and its impact on the pH. **Note:** The calculations require the use of the acid-base equilibrium principles and appropriate formulas to deduce the new pH levels in both scenarios. Further details and step-by-step calculations should be provided in the educational content for comprehensive learning.
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