Answer :

The [OH-] of a 1.10M solution of pyridine (C5H5N, Kb=1.70×10^-9) can be calculated by using the Kb expression and the concept of equilibrium.

Pyridine (C5H5N) is a weak base that reacts with water to produce hydroxide ions (OH-) through the process of ionization. The Kb value represents the base dissociation constant for pyridine.

The Kb expression for pyridine can be written as follows:

Kb = [OH-][C5H5N] / [C5H5NH+]

Given that the initial concentration of pyridine is 1.10M, and assuming that x represents the concentration of hydroxide ions formed, we can set up an equilibrium expression:

Kb = x * (1.10 - x) / (1.10)

Since the value of x is expected to be small compared to 1.10, we can approximate the expression as follows:

Kb = x * (1.10) / (1.10)

Simplifying the equation gives:

Kb = x

Solving for x, we find that the concentration of hydroxide ions [OH-] is equal to the Kb value, which is 1.70×10^-9 in this case.

Therefore, the [OH-] of the 1.10M pyridine solution is 1.70×10^-9.

To learn more about equilibrium, you can refer to the following link:

https://brainly.com/question/30694482

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