#18. The sample of 25.00 mL of 0.020 M NH3 is titrated with 0.016 M HCl. (a) Show the reaction between NH3 and H+. (b) Find the volume of 0.016 M HCl needed to reach the equivalence point. (c)Show the reaction of hydrolysis of product from the step (a). (d) Calculate the pH at the equivalence point(Ka of NH4+ is 5.6 x 10–10)
#18. The sample of 25.00 mL of 0.020 M NH3 is titrated with 0.016 M HCl. (a) Show the reaction between NH3 and H+. (b) Find the volume of 0.016 M HCl needed to reach the equivalence point. (c)Show the reaction of hydrolysis of product from the step (a). (d) Calculate the pH at the equivalence point(Ka of NH4+ is 5.6 x 10–10)
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter14: Acid- Base Equilibria
Section: Chapter Questions
Problem 110CP: A 0.400-M solution of ammonia was titrated with hydrochloric acid to the equivalence point, where...
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#18. The sample of 25.00 mL of 0.020 M NH3 is titrated with 0.016 M HCl. (a) Show the reaction between NH3 and H+. (b) Find the volume of 0.016 M HCl needed to reach the equivalence point. (c)Show the reaction of hydrolysis of product from the step (a). (d) Calculate the pH at the equivalence point(Ka of NH4+ is 5.6 x 10–10)
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