Chemistry
Answers
(1)
a) The pH of the solution before the titration begins is 2.75. This can be found by calculating the initial concentration of H3O+ in the solution and finding its corresponding pH.
b) The pH after 8.00 mL of NaOH has been added is 9.76. This can be found by calculating the new H3O+ concentration in the solution and finding its corresponding pH.
c) The pH at the equivalence point is 7.00. This can be found by calculating the concentration of H3O+ after the addition of stoichiometric amounts of the two reactants, which is equal to Kw/Ka.
d) The pH after 20.00 mL of NaOH has been added is 11.76. This can be found by calculating the new concentration of H3O+ in the solution after the addition of the NaOH and finding its corresponding pH. The basic nature of the solution explains why the pH is so much higher than the equivalence point, which is 7.00.
