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

Calculate the pH of the solution after the addition of the following amounts of 0.0649 M HNO3 to a 70.0 mL solution of 0.0750 M 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. I will know if you are wrong, so please answer to the best of your ability.

Hint:

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

Expert Solution

queen_honey_blossom answered 1 year ago

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