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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

Fundamentals Of Analytical Chemistry
Fundamentals Of Analytical Chemistry
9th Edition
ISBN:9781285640686
Author:Skoog
Publisher:Skoog
Chapter14: Principles Of Neutralization Titrations
Section: Chapter Questions
Problem 14.30QAP
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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
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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