**Consider the following table:** | Name | Formula | Conjugate Acid | \( K_b \) | |-------------|-----------|----------------|--------------------| | Ammonia | \( NH_3 \) | \( NH_4^+ \) | \( 1.8 \times 10^{-5} \) | | Methylamine | \( CH_3NH_2 \) | \( CH_3NH_3^+ \) | \( 4.38 \times 10^{-4} \) | | Ethylamine | \( C_2H_5NH_2 \) | \( C_2H_5NH_3^+ \) | \( 5.6 \times 10^{-4} \) | | Aniline | \( C_6H_5NH_2 \) | \( C_6H_5NH_3^+ \) | \( 3.8 \times 10^{-10} \) | | Pyridine | \( C_5H_5N \) | \( C_5H_5NH^+ \) | \( 1.7 \times 10^{-9} \) | **Which base would be the best choice for preparing a pH = 5.00 buffer?** - o ethylamine - o aniline - o ammonia - o pyridine - o methylamine **Submit Answer** | **Try Another Version** | *1 item attempt remaining* **Explanation:** This table compares different bases along with their formulas, conjugate acids, and base dissociation constants (\( K_b \)). For selecting a base to prepare a buffer with a pH of 5.00, one must consider the \( K_b \) values. A base with a \( K_a \) (related through \( K_w/K_b \) where \( K_w \) is the ion product of water) close to the desired pH will be preferable in order to create an effective buffer.

Consider the following table: | Name | Formula | Conjugate Acid | \( K_b \) | |-------------|-----------|----------------|--------------------| | Ammonia | \( NH_3 \) | \( NH_4^+ \) | \( 1.8 \times 10^{-5} \) | | Methylamine | \( CH_3NH_2 \) | \( CH_3NH_3^+ \) | \( 4.38 \times 10^{-4} \) | | Ethylamine | \( C_2H_5NH_2 \) | \( C_2H_5NH_3^+ \) | \( 5.6 \times 10^{-4} \) | | Aniline | \( C_6H_5NH_2 \) | \( C_6H_5NH_3^+ \) | \( 3.8 \times 10^{-10} \) | | Pyridine | \( C_5H_5N \) | \( C_5H_5NH^+ \) | \( 1.7 \times 10^{-9} \) | Which base would be the best choice for preparing a pH = 5.00 buffer? - o ethylamine - o aniline - o ammonia - o pyridine - o methylamine Submit Answer | Try Another Version | 1 item attempt remaining Explanation: This table compares different bases along with their formulas, conjugate acids, and base dissociation constants (\( K_b \)). For selecting a base to prepare a buffer with a pH of 5.00, one must consider the \( K_b \) values. A base with a \( K_a \) (related through \( K_w/K_b \) where \( K_w \) is the ion product of water) close to the desired pH will be preferable in order to create an effective buffer.

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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