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Chapter 15: Problem 32

How would you select an indicator for a particular acid-base titration?

Short Answer

Expert verified
The selection of an indicator for a particular acid-base titration depends upon the nature of the reaction taking place. The indicator's color change should correspond to the pH at the equivalence point of the titration. Indicator such as phenolphthalein is apt for weak acid-strong base titrations and methyl orange for strong acid-weak base titrations.

Step by step solution

01

Understand Acid-Base Titration

Acid-base titration is a way to find out the concentration of an acid or base by neutralising it with an acid or base of known concentration. During this process, an indicator is used that changes its color at a specific pH range.
02

Determine the pH at the Equivalence Point

The equivalence point of a titration is the point at which exactly enough titrant has been added to the analyte to fully neutralise it. The pH at the equivalence point depends on the nature of the acid and base being used. For a strong acid-strong base titration, it is at pH 7, for a strong acid-weak base it's less than 7 and for a weak acid-strong base it's greater than 7.
03

Select Appropriate Indicator

The indicator should be chosen such that its color change occurs over the pH range of the equivalence point. For instance, phenolphthalein has a range from 8.2 - 10.0 making it appropriate for titrations of weak acids with strong bases, while methyl orange with a range 3.1 - 4.4 is suitable for titrations of strong acids with weak bases.

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