Final answer:
The calculation of the percentage of pyridine that forms Pyridinium ion involves understanding the concept of acid-base equilibrium. Pyridine acts as a base and upon reacting with water, turns into Pyridinium ion. The percent ionisation can be calculated using the base ionisation constant of Pyridine and the concentration of hydroxide ions.
Step-by-step explanation:
To calculate the percentage of pyridine that forms pyridinium ion in a 0.10m aqueous pyridine solution, you need to understand the concept of acid-base equilibrium. Pyridine (C5H5N) acts as a base and, when it reacts with water, converts to its protonated form, Pyridinium ion (C5H5NH+), leaving hydroxide ions (OH-) in solution.
This reaction is governed by an equilibrium constant Kb (base ionization constant). The percent ionization for a base is calculated by the formula: percent ionization = ([OH-]/Initial concentration of the base) * 100%
The amount of OH- equals the amount of Pyridinium ion produced, which comes from the base ionization of pyridine. You should look up the value of Kb for pyridine in a reference source, use it to calculate [OH-], and then use that to find the percent ionization.
Please note that this is a simplified explanation and in reality, the calculation would require more steps involving the understanding of acid-base equilibrium, ICE tables (Initial Change, Equilibrium) and the quadratic formula.
Learn more about Acid-Base Equilibrium