Consider the titration of 25.00mL of 0.200M methylamine (CH3NH2). The titrant is 0.120M HCl. (Calculate each below using ICE and ICF tables.) Note you should NOT use M1V1=M2V2 (a) the initial pH of base? (b) the pH at 5.00mL added? (c) the pH at 1/2 the HCl needed to reach the equivalence point. (d) the volume of added acid required to reach the equivalence point? (e) the pH at equivalence point.
Consider the titration of 25.00mL of 0.200M methylamine (CH3NH2). The titrant is 0.120M HCl. (Calculate each below using ICE and ICF tables.) Note you should NOT use M1V1=M2V2 (a) the initial pH of base? (b) the pH at 5.00mL added? (c) the pH at 1/2 the HCl needed to reach the equivalence point. (d) the volume of added acid required to reach the equivalence point? (e) the pH at equivalence point.
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter14: Equilibria In Acid-base Solutions
Section: Chapter Questions
Problem 50QAP: Morphine, C17H19O3N, is a weak base (K b =7.4107). Consider its titration with hydrochloric acid. In...
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Consider the titration of 25.00mL of 0.200M methylamine (CH3NH2). The titrant is 0.120M HCl.
(Calculate each below using ICE and ICF tables.)
Note you should NOT use M1V1=M2V2
(a) the initial pH of base?
(b) the pH at 5.00mL added?
(c) the pH at 1/2 the HCl needed to reach the equivalence point.
(d) the volume of added acid required to reach the equivalence point?
(e) the pH at equivalence point.
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