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11 Dec 2019
Consider the titration of 30.0 mL of 0.0700 M (CH3)2NH (a weak base; Kb = 0.000540) with 0.100 M HClO4. Calculate the pH after the following volumes of titrant have been added:
(a) 0.0 mL
pH =
(b) 5.3 mL
pH =
(c) 10.5 mL
pH =
(d) 15.8 mL
pH =
(e) 21.0 mL
pH =
(f) 33.6 mL
pH =
Consider the titration of 30.0 mL of 0.0700 M (CH3)2NH (a weak base; Kb = 0.000540) with 0.100 M HClO4. Calculate the pH after the following volumes of titrant have been added:
(a) 0.0 mL
pH =
(b) 5.3 mL
pH =
(c) 10.5 mL
pH =
(d) 15.8 mL
pH =
(e) 21.0 mL
pH =
(f) 33.6 mL
pH =
Irving HeathcoteLv2
13 Dec 2019
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