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Calculate the pH of a 0.117 M solution of formic acid.

Calculate the pH of a 0.117 M solution of formic acid.

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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**Text:** Calculate the pH of a 0.117 M solution of formic acid. **Explanation:** The text requests the calculation of the pH for a given concentration of formic acid. To determine the pH, you'll need to use the acid dissociation constant (Ka) for formic acid and set up an equilibrium expression. This involves: 1. Writing the dissociation equation for formic acid: \[ \text{HCOOH} \rightleftharpoons \text{H}^+ + \text{HCOO}^- \] 2. Setting up an ICE table (Initial, Change, Equilibrium) to find the concentrations at equilibrium. 3. Using the Ka value for formic acid to solve for the hydrogen ion concentration \([\text{H}^+]\). 4. Calculating the pH using the formula: \[ \text{pH} = -\log[\text{H}^+] \] There are no graphs or diagrams associated with this text.
Transcribed Image Text:**Text:** Calculate the pH of a 0.117 M solution of formic acid. **Explanation:** The text requests the calculation of the pH for a given concentration of formic acid. To determine the pH, you'll need to use the acid dissociation constant (Ka) for formic acid and set up an equilibrium expression. This involves: 1. Writing the dissociation equation for formic acid: \[ \text{HCOOH} \rightleftharpoons \text{H}^+ + \text{HCOO}^- \] 2. Setting up an ICE table (Initial, Change, Equilibrium) to find the concentrations at equilibrium. 3. Using the Ka value for formic acid to solve for the hydrogen ion concentration \([\text{H}^+]\). 4. Calculating the pH using the formula: \[ \text{pH} = -\log[\text{H}^+] \] There are no graphs or diagrams associated with this text.
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