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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