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Calculate the pH of a 0.177 M aqueous solution of pyridine (C5H5N, Kb = 1.5×10-9) and the equilibrium concentrations...

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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=   
[C5H5N]equilibrium=   M
[C5H5NH+]equilibrium=   M

Answer & Explanation Solved by verified expert
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    See Answer
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