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Calculate the pH of the solution after the addition of the following amounts of 0.0649 M...

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Chemistry

Calculate the pH of the solution after the addition of thefollowing amounts of 0.0649 M HNO3 to a 70.0 mL solution of 0.0750M aziridine. The pKa of aziridinium is 8.04.

a) 0.00 mL of HNO3

b) 7.30 mL of HNO3

c) Volume of HNO3 equal to half the quivalence point volume

d) 77.5 mL of HNO3

e) Volume of HNO3 equal to the equivalence point

f) 85.8 mL of HNO3

Please answer all parts of the question detailed with work. Iwill know if you are wrong, so please answer to the best of yourability.

Hint:

Aziridine (C2H5N), a weak base, reacts with a strong acid suchas HNO3 to form its conjugate acid aziridinium (C2H5NH ). A strongacid reacts completely with a stoichiometric amount of weak baseafter each addition of the strong acid. In the titration of a weakbase with a strong acid, there are four regions of the titrationcurve that require different calculations when determining the pHof the solution. 1) Before any strong acid is added to thesolution. 2) Between the initial addition and the equivalencepoint. 3) At the equivalence point. 4) After the equivalencepoint.

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