Methyl orange, HMO, is a common acid-base indicator. In solution it ionizes according to the equation: HMO(a q) (red)= H* (a q) + MO minus (a q)(yellow) What color will the solution turn if OH minus is added and why?
Methyl orange, HMO, is a common acid-base indicator. In solution it ionizes according to the equation: HMO(a q) (red)= H* (a q) + MO minus (a q)(yellow) What color will the solution turn if OH minus is added and why?
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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![**Understanding Methyl Orange as an Acid-Base Indicator**
Methyl orange, denoted as HMO, is a widely used acid-base indicator. In solution, it undergoes ionization as represented by the equation:
\[ \text{HMO (aq) (red)} \rightleftharpoons \text{H}^+ \text{(aq)} + \text{MO}^- \text{(aq) (yellow)} \]
### Question:
What color will the solution turn if \(\text{OH}^-\) is added and why?
### Options:
1. **Red.** \( \text{H}^+ \) concentration decreases. Reaction moves to the right.
2. **Yellow.** \( \text{H}^+ \) concentration increases. Reaction moves to the left.
3. **Red.** \( \text{H}^+ \) concentration increases. Reaction moves to the left.
4. **Yellow.** \( \text{H}^+ \) concentration decreases. Reaction moves to the left.
5. **Red.** \( \text{H}^+ \) concentration decreases. Reaction moves to the left.
6. **Yellow.** \( \text{H}^+ \) concentration increases. Reaction moves to the right.
7. **Yellow.** \( \text{H}^+ \) concentration decreases. Reaction moves to the right.
8. **Red.** \( \text{H}^+ \) concentration increases. Reaction moves to the right. *(Selected Option)*
### Explanation:
When \(\text{OH}^-\) is added to the solution, it reacts with \( \text{H}^+ \), reducing its concentration. This drives the reaction to the right, leading to the formation of more \(\text{MO}^-\), which is yellow. However, the selected correct option indicates that the reaction moving to the right will result in a red color, due to the increase in \( \text{H}^+ \) concentration, which is the equilibrium response to the initial decrease caused by \(\text{OH}^-\). This shows a misunderstanding or correction in the logical assumption, as the equilibriums aim to counter the added base effect by eventually forming more of the red acid form.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc02bfde4-a78d-4551-93f6-03d589a5c8dc%2F4f6d1023-966e-4660-aeef-49a3da36f84b%2F045hfaj_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Understanding Methyl Orange as an Acid-Base Indicator**
Methyl orange, denoted as HMO, is a widely used acid-base indicator. In solution, it undergoes ionization as represented by the equation:
\[ \text{HMO (aq) (red)} \rightleftharpoons \text{H}^+ \text{(aq)} + \text{MO}^- \text{(aq) (yellow)} \]
### Question:
What color will the solution turn if \(\text{OH}^-\) is added and why?
### Options:
1. **Red.** \( \text{H}^+ \) concentration decreases. Reaction moves to the right.
2. **Yellow.** \( \text{H}^+ \) concentration increases. Reaction moves to the left.
3. **Red.** \( \text{H}^+ \) concentration increases. Reaction moves to the left.
4. **Yellow.** \( \text{H}^+ \) concentration decreases. Reaction moves to the left.
5. **Red.** \( \text{H}^+ \) concentration decreases. Reaction moves to the left.
6. **Yellow.** \( \text{H}^+ \) concentration increases. Reaction moves to the right.
7. **Yellow.** \( \text{H}^+ \) concentration decreases. Reaction moves to the right.
8. **Red.** \( \text{H}^+ \) concentration increases. Reaction moves to the right. *(Selected Option)*
### Explanation:
When \(\text{OH}^-\) is added to the solution, it reacts with \( \text{H}^+ \), reducing its concentration. This drives the reaction to the right, leading to the formation of more \(\text{MO}^-\), which is yellow. However, the selected correct option indicates that the reaction moving to the right will result in a red color, due to the increase in \( \text{H}^+ \) concentration, which is the equilibrium response to the initial decrease caused by \(\text{OH}^-\). This shows a misunderstanding or correction in the logical assumption, as the equilibriums aim to counter the added base effect by eventually forming more of the red acid form.
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