HBr (strong acid) will react with C5H5N (weak base).
C5H5N(aq) + HBr(aq) → C5H5NH+(aq) + Br-(aq)
Step 1: Calculate the initial amount (in moles) of each species:
moles C5H5N = 0.00525 mol C5H5N
moles HBr = 0.00672 mol HBr
Step 2: Construct an ICF chart to determine the final amount of each species.
After the reaction is complete the solution contains:
• 0.00147 mol HBr → strong acid
• 0.00525 mol C5H5NH+ → conjugate acid
• pH will depend on the strong acid
Step 3: Calculate the pH of the solution
final volume of solution = 0.057 L
Calculate the pH for each of the following cases in the titration of 25.0 mL of 0.210 M pyridine, C5H5N(aq) with 0.210 M HBr(aq) (Kb = 1.7 x 10-9)
after addition of 32.0 mL of HBr
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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 Base Strong Acid Titrations concept. You can view video lessons to learn Weak Base Strong Acid Titrations. Or if you need more Weak Base Strong Acid Titrations practice, you can also practice Weak Base Strong Acid Titrations practice problems.
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