A chemist titrates 250.0 mL of 0.5849 M aniline C6H5NH2 solution with 0.4070 M HNO3 solution at 25 °C Calculate the pH at equivalence. The pKb of aniline is 4.87
Round your answer to 2 decimal places.
Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of HNO3
Note for advanced students: you may assume the total volume of the solution equals to the initial plus the volume of HNO3 solution added.
Calculating the exact pH is, as usual in titration problems, a solution stoichiometry (moles/molarity/volume) problem followed by an equilibrium composition problem.
- First, you need to calculate the molarity of C6H5NH2 after the titration reaction has run. This is the stoichiometry problem.
- Then you can set up a reaction table and use the K
- a equation for C6H5NH2 to calculate the equilibrium molarity of HNO3This is the equilibrium problem