4. Formic acid, HFor, has a K, value of 1.8 x 10-4. You need to prepare 100 mL of a buffer hay- 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? mL NaFor mL HFor
4. Formic acid, HFor, has a K, value of 1.8 x 10-4. You need to prepare 100 mL of a buffer hay- 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? mL NaFor mL HFor
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
Chapter15: Acid-base Equilibria
Section: Chapter Questions
Problem 7ALQ: You have a solution of the weak acid HA and add some HCl to it. What are the major species in the...
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Help with 4 and 5 please.
![3. The pH of a 0.10 M HCN solution is 5.1.
What is the [H*]?
What is the [CN-]?
What is the K?
4 Formic acid, HFor, has a K, value of 1.8X 10". You need to prepare 100 mL of a buffer hay-
ing a pH of 3.25 from 0.10 M HFO solution and a 0.10 M NaFor solution. How many ml.
of NaFor and HFor should be mixed to make the desired buffer?
mL NaFor
mL HFor
5. When five drops of 0.10M 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.
ai noam noo noi](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F0959128f-1417-4f4f-bd20-8f81c7fe5d61%2Ff9b8e04a-66b4-4cee-b5ca-9014ba4ffbd8%2Fv64o3bs.jpeg&w=3840&q=75)
Transcribed Image Text:3. The pH of a 0.10 M HCN solution is 5.1.
What is the [H*]?
What is the [CN-]?
What is the K?
4 Formic acid, HFor, has a K, value of 1.8X 10". You need to prepare 100 mL of a buffer hay-
ing a pH of 3.25 from 0.10 M HFO solution and a 0.10 M NaFor solution. How many ml.
of NaFor and HFor should be mixed to make the desired buffer?
mL NaFor
mL HFor
5. When five drops of 0.10M 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.
ai noam noo noi
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