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5. An Indicator Molecule Br Br OH HO, -Br Br = 4.89 pK. Yellow pH < 3.7 Blue pH > 5.5 Shown above is a molecule that acts as an acid/base indicator. Suppose a solution has a pH of 5.1 and this indicator is used. Describe its color appearance at that point and explain. a. b. Which species of the molecule, the protonated molecule (HInd) or the deprotonated ion (Ind-'), is yellow-colored in solution? Justify.

5. An Indicator Molecule Br Br OH HO, -Br Br = 4.89 pK. Yellow pH < 3.7 Blue pH > 5.5 Shown above is a molecule that acts as an acid/base indicator. Suppose a solution has a pH of 5.1 and this indicator is used. Describe its color appearance at that point and explain. a. b. Which species of the molecule, the protonated molecule (HInd) or the deprotonated ion (Ind-'), is yellow-colored in solution? Justify.

Chemistry
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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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5. An Indicator Molecule Br Br OH HO, -Br Br pK, = 4.89 Yellow pH < 3.7 Blue pH > 5.5 Shown above is a molecule that acts as an acid/base indicator. Suppose a solution has a pH of 5.1 and this indicator is used. Describe its color appearance at that point and explain. a. b. Which species of the molecule, the protonated molecule (HInd) or the deprotonated ion (Ind-'), is yellow-colored in solution? Justify.
Transcribed Image Text:5. An Indicator Molecule Br Br OH HO, -Br Br pK, = 4.89 Yellow pH < 3.7 Blue pH > 5.5 Shown above is a molecule that acts as an acid/base indicator. Suppose a solution has a pH of 5.1 and this indicator is used. Describe its color appearance at that point and explain. a. b. Which species of the molecule, the protonated molecule (HInd) or the deprotonated ion (Ind-'), is yellow-colored in solution? Justify.
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