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Reference no: EM131703629

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

Reference no: EM131703629

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