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Calculate the pH of the solution after the addition of the following amounts of 0.0656 M...

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Chemistry

Calculate the pH of the solution after the addition of thefollowing amounts of 0.0656 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; Ph=

b) 9.06 mL of HNO3; Ph=

c) Volume of HNO3 equal to half the equivalence point volume;Ph=

d) 77.0 mL of HNO3; Ph=

e) Volume of HNO3 equal to the equivalence point; Ph=

f) 83.8 mL of HNO3; Ph=

Answer & Explanation Solved by verified expert
3.7 Ratings (402 Votes)
Concentration of aziridine 00750 MpKa 804First we need to calculate Kb from the pKaWe knowpKa log KaKa 10pKa 10804 912X109Kb Kw Ka 1014 912X109 11X106a pH when 000 mL of HNO3 isaddedIt is the weak base so we need to put ICE chartC2H5N H2O C2H6N OHInitially 0075000Finally 00750x xxKb for C2H5N 11X106Kb C2H6N OH C2H5N11X106 x x 00750xThe x in the 00750x can be    See Answer
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