Question

1. Titrations are very common in the determination of substances in solutions. What are the criteria for using titration analysis for a chemical reaction?

2. Explain why we used titration analysis for this reaction rather than the previous technique of gravimetric analysis.

3. What is the purpose of using an indicator in a reaction?

4. The end point of a titration is generally considered to be the stoichiometric equivalence point for the reaction. What error is inherent in this assumption?

Answer 1

1) there must be stoichiometric relation between the reactants. and reaction proceed via stable and defined equilent point.

equilent point must be observable. no side reactions and 100 % convertion of reaction. finally reaction comleted in practical time.

2) compared to volumetric titrations in gravimetry errors are more and all the compounds are not solids.

3) its not possible to observe the equivalnce point by nacked eye. for the completion of the reaction can be identified by colour changes using indicater. so indicater purpuse to find the end point by giving signal.

4) end point and equilence point are nearly same but not. equelence point is where the reaction completed, end point is where the signal genarated. genarally after completion of the reaction further adiition of titrant give signal. so it cause minute errror its depends on person how carfully observed the end point.