### Problem Statement:Calculate the hydroxide ion concentration, $[OH^-]$, in a solution of 0.138 M $CH_3NH_2$.### Reaction and Given Values:The chemical reaction and the base dissociation constant ($K_b$) are given below:\[ CH_3NH_2 \, (\text{aq}) + H_2O \, (\ell) \leftrightharpoons CH_3NH_3^+ \, (\text{aq}) + OH^- \, (\text{aq}) \]\[ K_b = 4.4 \times 10^{-4} \]### Instructions:Enter your answer in scientific notation with 2 significant digits (e.g., 2.3E-2).### Answer:\[ \boxed{\text{ }} \]### Explanation:In this problem, you are asked to determine the hydroxide ion concentration in a methylamine solution. The dissociation of methylamine in water and the given base dissociation constant $K_b$ will help you in this calculation. Remember to express your final answer in scientific notation with two significant digits.

Answered: Image /qna-images/answer/ab1a70d0-d88e-4b77-ad59-7a05801bf9b3.jpg

What is [OH] in a solution of 0.138 M CH3NH2 ? The reaction and Kp are given below. CH3NH2 (aq) + H20 (1)= CH3NH3+(aq) + OH (aq) Kp = 4.4x10-4 13D Enter your answer in scientific notation with 2 significant digits (2.3E-2).

What is [OH] in a solution of 0.138 M CH3NH2 ? The reaction and Kp are given below. CH3NH2 (aq) + H20 (1)= CH3NH3+(aq) + OH (aq) Kp = 4.4x10-4 13D Enter your answer in scientific notation with 2 significant digits (2.3E-2).

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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### Problem Statement:
Calculate the hydroxide ion concentration, $[OH^-]$, in a solution of 0.138 M $CH_3NH_2$.

### Reaction and Given Values:
The chemical reaction and the base dissociation constant ($K_b$) are given below:
\[ CH_3NH_2 \, (\text{aq}) + H_2O \, (\ell) \leftrightharpoons CH_3NH_3^+ \, (\text{aq}) + OH^- \, (\text{aq}) \]
\[ K_b = 4.4 \times 10^{-4} \]

### Instructions:
Enter your answer in scientific notation with 2 significant digits (e.g., 2.3E-2).

### Answer:
\[ \boxed{\text{ }} \]

### Explanation:
In this problem, you are asked to determine the hydroxide ion concentration in a methylamine solution. The dissociation of methylamine in water and the given base dissociation constant $K_b$ will help you in this calculation. Remember to express your final answer in scientific notation with two significant digits.

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