Calculate the pH of a 0.177 M aqueous solution
of pyridine
(C5H5N, Kb =
1.5×10-9) and the equilibrium
concentrations...
70.2K
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Chemistry
Calculate the pH of a 0.177 M aqueous solutionof pyridine(C5H5N, Kb =1.5×10-9) and the equilibriumconcentrations of the weak base and its conjugate acid.
pH
= Â Â
[C5H5N]equilibrium
= Â Â
M
[C5H5NH+]equilibrium
= Â Â
M
Answer & Explanation
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3.7 Ratings (630 Votes)
Let be the dissociation of the weak base pyridine C5H5N H2O C2H5NH OH initial conc c 0 0 change c c c Equb conc c1 c
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