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Due to the addition of more NaOH than was necessary to reach the endpoint of the titration, the recorded data would show NaOH at a higher concentration, and whatever other chemical in solution (the analyte of the titration) to appear at a lower concentration. If recording the amount of mL of the titrant added to the analyte to reach the end-point of the titration, it would cause the recorded mL needed to be higher than the true amount needed.

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Why phenolphthalein cannot be used as an indicator for titrating a weak base against a strong acid?

Phenolphthalein is not suitable for this titration because its color change occurs over a pH range that is beyond the equivalence point of the weak base and strong acid titration. At the equivalence point of this titration, the solution is acidic, which is below phenolphthalein's color change pH range. This can lead to inaccurate results and difficulty in determining the endpoint of the titration.


Why it is quantitatively not acceptable to titrate each of the vinegar samples?

This is because the readings of the amount of NaOH needed are only valid up to the point when the color pink appears in the entire solution. Titrating beyond that point would produce erroneous values of NaOH volume and molarity of acetic acid.


What is over-titration?

Over-titration refers to the process of adding too much titrant during a titration, resulting in an endpoint that goes beyond the equivalence point. This can lead to inaccurate results as the excess titrant can skew the calculations.


Mention five precautions in titration?

-do not over-shoot the volume of the titrant beyond the equivalence point. -make sure your acid/base is pure - no impurities -Accidental dilution of the acid/base because residual water remains after rinsing. -Misjudging the change in color


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Related Questions

Would your calculated molarity of NaOH be too high too low or unaffected if you titrated to a dark pink color?

If you titrated to a dark pink color, it signifies that you have overshot the endpoint and added excessive NaOH. This would make your calculated molarity of NaOH too high due to the excess base added beyond the equivalence point, affecting the accuracy of the results.


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Why phenolphthalein cannot be used as an indicator for titrating a weak base against a strong acid?

Phenolphthalein is not suitable for this titration because its color change occurs over a pH range that is beyond the equivalence point of the weak base and strong acid titration. At the equivalence point of this titration, the solution is acidic, which is below phenolphthalein's color change pH range. This can lead to inaccurate results and difficulty in determining the endpoint of the titration.


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