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3. Write net ionic equations to show how each of the buffer mixtures below would neutralize added Ht and OH- (i.e., exclude Na* and Cl from these equations) a. C6H5COOH:C6H5COO- H+ + OH- + b. NH4*:NH3 H+ + OH- +

3. Write net ionic equations to show how each of the buffer mixtures below would neutralize added Ht and OH- (i.e., exclude Na* and Cl from these equations) a. C6H5COOH:C6H5COO- H+ + OH- + b. NH4*:NH3 H+ + OH- +

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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**Buffer Solutions and Net Ionic Equations** **3. Write net ionic equations to show how each of the buffer mixtures below would neutralize added H⁺ and OH⁻ (i.e., exclude Na⁺ and Cl⁻ from these equations):** **a. Buffer System: C₆H₅COOH / C₆H₅COO⁻** - **H⁺ +** _________ **→** __________________ - **OH⁻ +** _________ **→** __________________ **b. Buffer System: NH₄⁺ / NH₃** - **H⁺ +** _________ **→** __________________ - **OH⁻ +** _________ **→** __________________ This exercise requires you to complete the net ionic equations that demonstrate how these buffer mixtures neutralize incoming hydrogen ions (H⁺) and hydroxide ions (OH⁻). The goal is to understand the buffer action by which acids and bases are neutralized efficiently, maintaining the pH levels.
Transcribed Image Text:**Buffer Solutions and Net Ionic Equations** **3. Write net ionic equations to show how each of the buffer mixtures below would neutralize added H⁺ and OH⁻ (i.e., exclude Na⁺ and Cl⁻ from these equations):** **a. Buffer System: C₆H₅COOH / C₆H₅COO⁻** - **H⁺ +** _________ **→** __________________ - **OH⁻ +** _________ **→** __________________ **b. Buffer System: NH₄⁺ / NH₃** - **H⁺ +** _________ **→** __________________ - **OH⁻ +** _________ **→** __________________ This exercise requires you to complete the net ionic equations that demonstrate how these buffer mixtures neutralize incoming hydrogen ions (H⁺) and hydroxide ions (OH⁻). The goal is to understand the buffer action by which acids and bases are neutralized efficiently, maintaining the pH levels.
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