**Determining Hydroxide Ion Concentration in Aqueous Trimethylamine Solution**The hydroxide ion concentration, $[OH^{-}]$, of an aqueous solution of 0.591 M trimethylamine (a weak base with the formula $(CH_{3})_{3}N$), $K_b = 6.3 \times 10^{-5} $, is:\[[OH^{-}] = \underline{\hspace{5cm}} \, M.\]In this problem, we are required to find the hydroxide ion concentration ($[OH^-]$) in a 0.591 M aqueous solution of trimethylamine. Trimethylamine is a weak base and its base dissociation constant $(K_b)$ is given as $6.3 \times 10^{-5}$. To solve for $[OH^{-}]$, we typically use the base dissociation constant formula related to weak bases:\[K_b = \frac{[CH_3]_3 NH^+][OH^-]}{[CH_3]_3 N]\]Where:- $[CH_3]_3 NH^+$ is the concentration of the conjugate acid.- $[OH^-]$ is the concentration of hydroxide ions.- $[CH_3]_3 N$ is the initial concentration of the weak base (trimethylamine), which will slightly decrease due to dissociation.Given the initial concentration and the $ K_b $ value, we can set up an ICE table (Initial, Change, Equilibrium) to solve for $[OH^{-}]$.This type of analysis is foundational for understanding equilibrium in weak base solutions in Chemistry.

Trimethylamine dissolved in H2O and since it is a weak base so it dissociates partially as follows

Answered: The hydroxide ion concentration, [OH*],…

The hydroxide ion concentration, [OH*], of an aqueous solution of 0.591 M trimethylamine (a weak base with the formula (CH3)3N) , Kp = 6.3×10$, is: М. =[.HO)

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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