Suppose you titrate NH3 with HC1. With 25.00 mL of NH3 in the flask, it takes 25.00 mL of 0.100 M HCl to reach the equivalence point. Calculate the molarity of ammonia. a. At this equivalence point, what is the pH? (Hint: the Ka for NH4* is 5.6×10-10).

Suppose you titrate NH3 with HC1. With 25.00 mL of NH3 in the flask, it takes 25.00 mL of 0.100 M HCl to reach the equivalence point. Calculate the molarity of ammonia. a. At this equivalence point, what is the pH? (Hint: the Ka for NH4* is 5.6×10-10).

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Suppose you titrate NH3 with HC1. With 25.00 mL of NH3 in the flask, it takes 25.00 mL of
0.100 M HCl to reach the equivalence point. Calculate the molarity of ammonia.
a. At this equivalence point, what is the pH? (Hint: the Ka for NH4* is 5.6×10-10).

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