Indicators
- Indicators are substances that change colour when they are added to acidic or alkaline solutions
- When choosing the appropriate indicator, the pH of the equivalence point is very important
- The two most common indicators that are used in titrations are methyl orange and phenolphthalein
- Both indicators change colour over a specific pH range
The diagram shows the change in colour from red to yellow of methyl orange over a pH range of 3.1-4.4 and from colourless to pink of phenolphthalein over a pH range of 8.3-10
Indicator & pH range table
Choosing indicators for titrations
- Strong acid and strong alkali
- The colour change for both indicators takes place at a pH range that falls within the vertical region of the curve
- Therefore, either indicator can be used
The diagram shows that both indicators can be used to determine the endpoint of the titration of a strong acid and strong alkali
- Strong acid and weak alkali
- Only methyl orange will change colour at a pH close to the equivalence point and within the vertical region of the curve
The diagram shows that only methyl orange can be used to determine the endpoint of the titration of a strong acid and weak alkali
- Weak acid and strong alkali
- Now, only phenolphthalein will change colour at a pH close to the equivalence point and within the vertical region of the curve
- The pH range at which methyl orange changes colour falls below the curve
The diagram shows that only phenolphthalein can be used to determine the endpoint of the titration of a weak acid and strong alkali
- Weak acid and weak alkali
- Neither indicator is useful, and a different method should be considered
The diagram shows that nether indicators can be used to determine the endpoint of the titration of a weak acid and weak alkali
