(e) An acidic buffer solution is formed by mixing 50 mmol dm formic acid (HCOOH) with 0.8 mol dm³ of sodlum formate (HCOONa). The acid dissociation constant (K.) of formic acid is 1.78 × 104, (1) Calculate the pk, of formic acid, (1) Calculate the pH of the buffer solution described above, using the Henderson- Hasselbalch equation: pH = pk + log10 [Conjugate Base] (Acid) (III) A small amount of sodium hydroxide (NaOH) is added to the solution, but the pH does not change, Explain this observation.

(e) An acidic buffer solution is formed by mixing 50 mmol dm formic acid (HCOOH) with 0.8 mol dm³ of sodlum formate (HCOONa). The acid dissociation constant (K.) of formic acid is 1.78 × 104, (1) Calculate the pk, of formic acid, (1) Calculate the pH of the buffer solution described above, using the Henderson- Hasselbalch equation: pH = pk + log10 [Conjugate Base] (Acid) (III) A small amount of sodium hydroxide (NaOH) is added to the solution, but the pH does not change, Explain this observation.

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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