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The easiest way is to add back some of the solution you were titrating. If phenolphthalein remains, it will react with the solution and change back to purple. Incidentally, phenolphthalein will always remain in the solution of the titration reaction - it changes color depending upon the pH of the solution, but the indicator itself is not affected by the titration reaction.
briefly discuss the errors tahat occur in the above titration and the change in the colour of the indicators.
In titrations, the end point is when you have brought the tested sample to absolute neutral. At this point, if you add one more drop of titrating solution to the sample, you would change the pH sufficient to change the color of the indicator in the sample. This is the point at which you can determine the pH of the original solution, by calculating back the amount of titrating solution you had to add to the sample to neutralize it.
The equivalence point represents a region where the amount of acid to base (or base to acid) concentration is equal. Before the equivalence point there is a greater amount of acid (or base, depending on the titration). After the titration there is a greater amount of base (or acid). This reverse in dominance results in a dramatic change in pH.
When there is a buffer present, the buffer makes it difficult to change the pH of a solution. Say for instance a buffer keeps the pH around 6.5 +/- 0.2 . The buffer only works when the pH is in this range. If too much acid or too much base is added, taking the pH out of this range the pH will change quickly, even if only a little extra base or acid is added to the solution.
the reason why a indicator is important in some titration is to show a change in the solution. for example as a solution runs from acidic to basic the indicator may turn a different color. but this is the reason why it is important inmost experiments.
1. The advantage in diluting the solution before titration is that it allows for greater accuracy in the titration; this is because the color change in the solution is easier to observe if it is a dilute solution.
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buffer solutions resists change in PH
No, because a drop of strong base can change the pH a lot and mess up titration, it has to be a moderate-weak base!
The easiest way is to add back some of the solution you were titrating. If phenolphthalein remains, it will react with the solution and change back to purple. Incidentally, phenolphthalein will always remain in the solution of the titration reaction - it changes color depending upon the pH of the solution, but the indicator itself is not affected by the titration reaction.
It makes it easier to see the colour change in the solution after it reaches its endpoint.
Titration is a chemical process.
coz the oxidation state of manganese ion changes from +7 to +4. as a result Mno2 is formed which is brown in colour hence titration colour change cannot be detected
Titration in which the end point is marked by a color change.
A potentiometric titration is one in which the end-point is detected by measuring the change in potential of a suitable electrode during the titration.
briefly discuss the errors tahat occur in the above titration and the change in the colour of the indicators.