We’re being asked to calculate the pH of a 0.2634 M C5H5N
C5H5N is a weak base that will further react in water to form OH-
C5H5N(aq) + H2O (l) → OH- (aq) + C5H6N+ (aq)
From this, we can construct an ICE table for the reaction of C5H5N in a solution. Remember that liquids are ignored in the ICE table.
Pyridine is a weak base with the formula, C5H5N, the Kb for Pyridine is 1.8 x 10-9 In an aqueous solution, pyridine partially dissociates according to the following reaction: C5H5N + H2O ⇔ C5H5NH+ + OH-
Use the Kb equation to calculate the pH of the aqueous pyridine solution described below: Volume: 375 mL Concentration: 0.2634 M Since this is a weak base, you can assume the amount of base dissociated is << 5% of the total amount of base present. Report your answer with the correct number of significant digits.
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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.