Using the table of the weak base below, you have chosen Methylamine as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.48 M in this salt. The desired pH of the buffer should be equal to 9.75. Values of K, for Some Common Weak Bases Conjugate Acid Name Formula 1.8 × 10-5 4.38 × 10-4 5.6 × 10–4 3.8 × 10-10 1.7 x 10-9 NH4 CH;NH3* NH3 CH;NH2 C¿H;NH2 CH;NH2 C;H;N Ammonia Methylamine Ethylamine Aniline C¿H§NH3* CH;NH;* C;H;NH+ Pyridine 3. Compute the concentration of the weak base in Molarity. (round off final answer to 4 decimal places)

Using the table of the weak base below, you have chosen Methylamine as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.48 M in this salt. The desired pH of the buffer should be equal to 9.75. Values of K, for Some Common Weak Bases Conjugate Acid Name Formula 1.8 × 10-5 4.38 × 10-4 5.6 × 10–4 3.8 × 10-10 1.7 x 10-9 NH4 CH;NH3* NH3 CH;NH2 C¿H;NH2 CH;NH2 C;H;N Ammonia Methylamine Ethylamine Aniline C¿H§NH3* CH;NH;* C;H;NH+ Pyridine 3. Compute the concentration of the weak base in Molarity. (round off final answer to 4 decimal places)

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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