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10.0 mL of 1.0 M NaOH is added to 1.0 L of the above 0.15 MHCOOH and 0.20 M HCOONa solution. Calculate the pH of the resulting mixture. The K₂ of formic acid is K₂ = 1.8×10-4. (Note: you may ignore the change in volume that occurs when you add the 10 mL of base to the 1000 mL of buffer.) (A) 3.56 (B) 3.74 (C) 3.87 (D) 4.15 (E) 3.92

10.0 mL of 1.0 M NaOH is added to 1.0 L of the above 0.15 MHCOOH and 0.20 M HCOONa solution. Calculate the pH of the resulting mixture. The K₂ of formic acid is K₂ = 1.8×10-4. (Note: you may ignore the change in volume that occurs when you add the 10 mL of base to the 1000 mL of buffer.) (A) 3.56 (B) 3.74 (C) 3.87 (D) 4.15 (E) 3.92

Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter14: Equilibria In Acid-base Solutions
Section: Chapter Questions
Problem 12QAP: A buffer is prepared by dissolving 0.062 mol of sodium fluoride in 127 mL of 0.0399 M hydrofluoric...
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10.0 mL of 1.0 M NaOH is added to 1.0 L of the above 0.15 MHCOOH and 0.20 M HCOONa solution. Calculate the pH of the resulting mixture. The K₂ of formic acid is K₂ = 1.8×10-4. (Note: you may ignore the change in volume that occurs when you add the 10 mL of base to the 1000 mL of buffer.) (A) 3.56 (B) 3.74 (C) 3.87 (D) 4.15 (E) 3.92
Transcribed Image Text:10.0 mL of 1.0 M NaOH is added to 1.0 L of the above 0.15 MHCOOH and 0.20 M HCOONa solution. Calculate the pH of the resulting mixture. The K₂ of formic acid is K₂ = 1.8×10-4. (Note: you may ignore the change in volume that occurs when you add the 10 mL of base to the 1000 mL of buffer.) (A) 3.56 (B) 3.74 (C) 3.87 (D) 4.15 (E) 3.92
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