4) Calculate how much 1.00 M CH3COONA solution, in mL, you would need to add to 10.00 mL of a 1.00 M CH3COOH solution that will then be diluted to 100.00 mL to make a 100.00 mL of a buffer with a pH of 4.85. The Ka of CH3COOH is 1.8 x 105) udn 5) If 25.00 mL of a buffer solution is prepared to be 0.10M of both formic acid (HCOOH) and sodium formate (HCOONA). (HCOOH K, = 1.77 x 104) Calculate the pH when: a. 0.00 mL of 0.10 M HCI is added wol hst e 2e1/264 nomme Ng wol s iislgse b. 10.00 mL of 0.10 M HCI is added с. 25.00 mL of 0.10 M HCI is added
4) Calculate how much 1.00 M CH3COONA solution, in mL, you would need to add to 10.00 mL of a 1.00 M CH3COOH solution that will then be diluted to 100.00 mL to make a 100.00 mL of a buffer with a pH of 4.85. The Ka of CH3COOH is 1.8 x 105) udn 5) If 25.00 mL of a buffer solution is prepared to be 0.10M of both formic acid (HCOOH) and sodium formate (HCOONA). (HCOOH K, = 1.77 x 104) Calculate the pH when: a. 0.00 mL of 0.10 M HCI is added wol hst e 2e1/264 nomme Ng wol s iislgse b. 10.00 mL of 0.10 M HCI is added с. 25.00 mL of 0.10 M HCI is added
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter16: Reactions Between Acids And Bases
Section: Chapter Questions
Problem 16.36QE
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Please help asap
![4) Calculate how much 1.00 M CH3COONA solution, in mL, you would need to add to 10.00 mL
of a 1.00 M CH3COOH solution that will then be diluted to 100.00 mL to make a 100.00 mL of
a buffer with a pH of 4.85. The Ka of CH3COOH is 1.8 x 105)
trudnA
5) If 25.00 mL of a buffer solution is prepared to be 0.10M of both formic acid (HCOOH) and
sodium formate (HCOONA). (HCOOH K, = 1.77 x 104) Calculate the pH when:
a. 0.00 mL of 0.10 M HCl is added
wol bet a 2s12mal ma
Juen to Ha
omme
b. 10.00 mL of 0.10 M HCI is added
C. 25.00 mL of 0.10 M HCI is added](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc3f56dff-0b60-49cc-8c03-28401888e8a6%2Fad903bb9-d34f-41b3-8b07-1e25508adf9c%2Flc9phjr_processed.jpeg&w=3840&q=75)
Transcribed Image Text:4) Calculate how much 1.00 M CH3COONA solution, in mL, you would need to add to 10.00 mL
of a 1.00 M CH3COOH solution that will then be diluted to 100.00 mL to make a 100.00 mL of
a buffer with a pH of 4.85. The Ka of CH3COOH is 1.8 x 105)
trudnA
5) If 25.00 mL of a buffer solution is prepared to be 0.10M of both formic acid (HCOOH) and
sodium formate (HCOONA). (HCOOH K, = 1.77 x 104) Calculate the pH when:
a. 0.00 mL of 0.10 M HCl is added
wol bet a 2s12mal ma
Juen to Ha
omme
b. 10.00 mL of 0.10 M HCI is added
C. 25.00 mL of 0.10 M HCI is added
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