Answer :
The volume of KOH required to reach the equivalence point by titration is 109.04 mL.
When performing a titration, it is important to understand the concept of the equivalence point. This is the point at which the number of moles of the titrant (the substance being added) is equal to the number of moles of the analyte (the substance being titrated). At the equivalence point, the reaction is complete and all of the analytes have been consumed by the titrant. In order to calculate the volume of the titrant needed to reach the equivalence point, we need to know the initial volume of the analyte, the molarity of the titrant, and the molarity of the analyte.
The volume of KOH required to reach the equivalence point for titration of 100.8 mL of 0.397 M HNO₃ with 0.367 M KOH can be calculated using the equation:
Equivalence point (V) = (Moles of acid x Volume of acid) / Moles of base
Substituting the given values, we have:
Equivalence point (V) = (0.397 x 100.8) / 0.367
Equivalence point (V) = 109.88 mL
Therefore, the volume of KOH required to reach the equivalence point is 109.04 mL.
The calculation shown above assumes that the titration is done at a constant temperature and pressure. Additionally, it is important to make sure that the burette (the instrument used to dispense the titrant) is properly calibrated.
It is essential to understand the concepts of equivalence point and titration, as well as properly calibrate the equipment when performing this type of experiment.
In conclusion, the volume of KOH required to reach the equivalence point for titration of 100.8 mL of 0.397 M HNO₃ with 0.367 M KOH is 109.04 mL.
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