Problem: Pyridine (C5H5N) is a base with a Kb of 1.7 x 10–9. What is the pH of 0.10 M pyridine?               C5H5N + H2O ↔ C5H5NH+ + OH–a) 7.87b) 8.56c) 9.89d) 9.12e) 10.32

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Step 1

Step 2

Kb =[C5H5NH+][OH-][C5H5N]Kb =(x)(x)0.10 - xKb =x20.10 - x


[C5H5N]Kb = 0.101.7×10-9 >>> 500


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Problem Details

Pyridine (C5H5N) is a base with a Kb of 1.7 x 10–9. What is the pH of 0.10 M pyridine?

               C5H5N + H2O ↔ C5H5NH+ + OH

a) 7.87

b) 8.56

c) 9.89

d) 9.12

e) 10.32

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Weak Bases concept. If you need more Weak Bases practice, you can also practice Weak Bases practice problems.