Problem: A certain indicator HIn has a pKa of 3.00 and a color change becomes visible when 7.00% of the indicator has been converted to In-. At what pH is this color change visible?

FREE Expert Solution

To solve for pH, we use the Henderson-Hasselbalch equation:

pH=pKa+log(conjugate baseweak acid)

We are given the following:

pKa = 3.00
In- = 7.00%
HIn = 93.00%

Since in the equation, we just need to compare the ratio of conjugate and weak acid present, we can directly plug-in the given percentages to the equation, thus we solve for pH:

pH=pKa+log(conjugate baseweak acid)pH=3.00+log(7.00%93.00%)pH=3.00+(-1.123)pH=3.00-1.123

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Problem Details

A certain indicator HIn has a pKa of 3.00 and a color change becomes visible when 7.00% of the indicator has been converted to In-. At what pH is this color change visible?

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Acid Base Indicators concept. If you need more Acid Base Indicators practice, you can also practice Acid Base Indicators practice problems.

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl 2nd Edition practice problems.