Using the table of the weak base below, you have chosen Pyridine as your weak base in the buffer solution. You have already added enough of theconjugate acid salt to make the buffer solution concentration at 0.62 M in this salt. The desired pH of the buffer should be equal to 4.5.Values of K, for Some Common Weak BasesConjugateNameFormulaAcidKbAmmoniaNH3NH4+1.8 x 10-5Methylamine CH3NH2CH3NH3 +4.38 x 10-4EthylamineC₂H5NH₂C₂H5NH3+5.6 x 10-4AnilineC6H5NH3 +3.8 x 10-10CH;NH,C,H,NPyridineCH;NH*1.7 x 10-⁹1. Compute the poH of the buffer solution. (Supply answer up to the 1st decimal point)

Answered: Image /qna-images/answer/8804df55-a5c6-4299-9f9b-44f824310855.jpg

Methylamine Ethylamine H3NH₂ C₂H5NH₂ H₂NH3 C₂H5NH3+ 4.38 X 10 5.6 x 10-4 Aniline CH;NH, C6H5NH3 + 3.8 x 10-10 Pyridine C,H,N CH;NH* 1.7 x 10-⁹ 1. Compute the poH of the buffer solution. (Supply answer up to the 1st decimal point)

Methylamine Ethylamine H3NH₂ C₂H5NH₂ H₂NH3 C₂H5NH3+ 4.38 X 10 5.6 x 10-4 Aniline CH;NH, C6H5NH3 + 3.8 x 10-10 Pyridine C,H,N CH;NH* 1.7 x 10-⁹ 1. Compute the poH of the buffer solution. (Supply answer up to the 1st decimal point)

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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