in an acidbase titration, 10.0 mL (VB)of NH3 (Ka(NH+) = 5.8*10^ - 19) 0.18 M (CB) are titrated at the equivalence point (EP) with 10.0 ml (VA) of HCI 0.18 M (CA). Calculate (to two decimal places) the pH of the solution at the equivalence point.
in an acidbase titration, 10.0 mL (VB)of NH3 (Ka(NH+) = 5.8*10^ - 19) 0.18 M (CB) are titrated at the equivalence point (EP) with 10.0 ml (VA) of HCI 0.18 M (CA). Calculate (to two decimal places) the pH of the solution at the equivalence point.
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter15: Acid–base Equilibria
Section: Chapter Questions
Problem 57P
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in an acidbase titration, 10.0 mL (VB)of NH3 (Ka(NH+) = 5.8*10^ - 19) 0.18 M (CB) are titrated at the equivalence point (EP) with 10.0 ml (VA) of HCI 0.18 M (CA). Calculate (to two decimal places) the pH of the solution at the equivalence point.
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