1. Consider the titration of 50.00 mL of 0.1000 M HNO2 (Ka = 7.1 x 10-4) with 0.1000 M NaOH.
a. Write the equilibrium equation that describes the analyte flask before any base is added.
b. Write the reaction that takes place in the analyte flask following the addition of base.
c. Use Le Chatelierās principle to predict how the initial equilibrium, and pH, will change following
the addition of base.
d. Calculate the pH after adding 0.00, 5.00, 20.00 and 50.00 mL of 0.100 M NaOH.
e. Sketch a detailed titration curve based on your calculations from part d. Use a dotted line to
predict the pH beyond 50 mL of titrant added. Label the equivalence point.