In the laboratory, a general chemistry student measured the pH of a 0.589 M aqueous solution of triethylamine, (C₂H₅)₃N, to be 12.202.Use the information she obtained to determine the Kb for this base.\[ K_b(\text{experiment}) = \]**Explanation for Learners:**To determine the Kb (base dissociation constant) for triethylamine, use the pH value to find the concentration of hydroxide ions (OH⁻) produced. Then use the formula for Kb:\[ K_b = \frac{[OH^-]^2}{[Base] - [OH^-]} \]**Steps:**1. Calculate the pOH from the pH: \[ \text{pOH} = 14 - \text{pH} \]2. Convert pOH to [OH⁻]: \[ [OH^-] = 10^{-\text{pOH}} \]3. Substitute [OH⁻] and the initial concentration of the base into the Kb equation to solve for Kb.

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In the laboratory, a general chemistry student measured the pH of a 0.589 M aqueous solution of triethylamine, (C₂H5)3N to be 12.202. Use the information she obtained to determine the K₁ for this base. K(experiment) = Submit Answer Retry Entire Group 9 more group attempts remaining

In the laboratory, a general chemistry student measured the pH of a 0.589 M aqueous solution of triethylamine, (C₂H5)3N to be 12.202. Use the information she obtained to determine the K₁ for this base. K(experiment) = Submit Answer Retry Entire Group 9 more group attempts remaining

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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