A solution is prepared using a sodium salt of an unknowndiprotic base. The unknown diprotic weak base solution will beanalyzed for concentration by titration with a strong acid. Theunknown is placed in an Erlenmyer flask, and small, measuredvolumes of a standard strong acid solution are added until thefinal equivalence point is reached. Then the concentration of thebase is calculated fromthe known volumes, the one knownconcentration and stoichiometry. All solutions are kept at roomtemperature.
A. Before the titration starts, is the solution in the flaskacidic, neutral or alkaline?
B. Write a complete ionic equation for the complete(Bronsted-Lowry) acid-base neutralization reaction of a genericweak diprotic base B2- with hydrochloric acid.
C. List the most commonform of each solute species that ispresent in the reaction mixture at the final equivalence point, andlabel each as a strong acid, weak acid, neutral, weak base, orstrong base.
D. At the final equivalence point, will the overall solution bestrongly acidic, weakly acidic, neutral, weakly basic, or stronglybasic?
E. List the solute species that are present when more standardis added after the final equivalence point, and label each aseither a strong acid, weak acid, neutral, weak base or strongbase.
F. If extra titrant is added tto the flask after the finalequivalence point has been reached, will the mixture be stronglyacidic, weakly acidic, neutral, weakly basic, or stronglybasic?
