36. 10.0 mL of 1.0 M NaOH is added to 1.0 L of the above 0.15 MHCOOH and 0.20MHCOONa solution. Calculate the pH of the resulting mixture. The K₂ of formicacid is K₂ = 1.8×10-4. (Note: you may ignore the change in volume that occurs whenyou 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

we have to calculate the pH of solution

36. 10.0 mL of 1.0 M NaOH is added to 1.0 L of the above 0.15 MHCOOH and 0.20 MHCOONa solution. Calculate the pH of the resulting mixture. The K₂ of formic acid is Ka 1.8x10-4. (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

36. 10.0 mL of 1.0 M NaOH is added to 1.0 L of the above 0.15 MHCOOH and 0.20 MHCOONa solution. Calculate the pH of the resulting mixture. The K₂ of formic acid is Ka 1.8x10-4. (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

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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36. 10.0 mL of 1.0 M NaOH is added to 1.0 L of the above 0.15 MHCOOH and 0.20
MHCOONa 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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