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When five drops of 0.10 M NaOH were added to 20 mL of the buffer in question 4, the pH went from 3.25 to 3.31. Write a net ionic equation to explain why the pH did not go up more than this.

When five drops of 0.10 M NaOH were added to 20 mL of the buffer in question 4, the pH went from 3.25 to 3.31. Write a net ionic equation to explain why the pH did not go up more than this.

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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  1. When five drops of 0.10 M NaOH were added to 20 mL of the buffer in question 4, the pH went from 3.25 to 3.31. Write a net ionic equation to explain why the pH did not go up more than this. 

4. Formic acid, HFor, has a K value of 1.8 x 10-4. You need to prepare 150 mL of a buffer hav- ing a pH of 3.25 from 0.10 M HFor solution and a 0.10 M NaFor solution. How many mL of NaFor and HFor should be mixed to make the desired buffer? 36.42 113.58 mL NaFor mL HFor 5. When five drops of 0.10 M NaOH were added to 20 mL of the buffer in question 4, the pH went from 3.25 to 3.31. Write a net ionic equation to explain why the pH did not go up more than this. H+ + OH- ----> H2O
Transcribed Image Text:4. Formic acid, HFor, has a K value of 1.8 x 10-4. You need to prepare 150 mL of a buffer hav- ing a pH of 3.25 from 0.10 M HFor solution and a 0.10 M NaFor solution. How many mL of NaFor and HFor should be mixed to make the desired buffer? 36.42 113.58 mL NaFor mL HFor 5. When five drops of 0.10 M NaOH were added to 20 mL of the buffer in question 4, the pH went from 3.25 to 3.31. Write a net ionic equation to explain why the pH did not go up more than this. H+ + OH- ----> H2O
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