There is a weak acid, Butyric acid (C3H7COOH), with a Ka of 2.2 x 10-5. You will be titrating 25.0 mL
of this with the strong base, Ca(OH)2 which is 0.100 M and it takes 15.0 mL to get it to it’s
equivalence point. Please note that the base has 2 basic units.
A. Before titrating, what is the pH of the solution of HBut? B. What is the net ionic equation of this acid in water? C. What is the concentration of this acid? D. What is the % ionization before starting to titrate? E. What is the pH at the equivalence point? F. What is the pH 1/2 way to the equivalence point? G. Where does it buffer? H. Draw an approximate titration curve. I. Look at figure 16.8 on page 684 of your textbook and determine which indicator would be
useful?