Final answer:
The results of a titration provide the concentrations of samples A and B using stoichiometric calculations based on the volume and concentration of the titrant. Common errors in a titration can include misreading volumes, incorrect indicator use, and incomplete reactions. A practical application of titration is in measuring the acidity of acid rain.
Step-by-step explanation:
Results of a Titration and Concentration of Samples
The results of a titration provide the concentrations of the acid or base in the samples A and B. To determine these concentrations, the volume of titrant (the solution of known concentration) added to reach the end point is measured, and this information is used in stoichiometric calculations alongside the known concentration of the titrant and the balanced chemical equation.
Sources of Error in a Titration Experiment
Three possible sources of error in a titration experiment include misreading the volume on the burette, not adding the indicator properly, or incomplete reactions due to insufficient mixing. Such errors can affect the accuracy of the titration results.
Real World Application of Titrations
A real world example of a problem that could be solved using titration is determining the concentration of sulfuric acid in a sample of acid rain. The titration process would involve adding a known concentration of a base (like NaOH) to the acid rain until the end point is reached, indicated by a pH indicator or meter.