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Guide to Solving Titration Problems explained by Alex Honnold 

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Guide to Solving Titration Problems explained by Alex Honnold 

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Slow is fast, fast is slow. Read and analyze the problem given, a strong start can help you finish strong

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A student titrates 35.0 mL of 0.200 M methylamine (CH₃NH₂), a weak base (Kb = 4.4 × 10⁻⁴), with 0.100 M hydrochloric acid (HCl), a strong acid. After the student adds 10.0 mL of 0.100 M HCl to the base solution, calculate the pH of the solution. Determine the pH at the equivalence point, where just enough HCl has been added to fully neutralize the methylamine. If the student continues adding HCl and reaches a total of 80.0 mL of 0.100 M HCl added, calculate the pH of the resulting solution.

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Identify what you're being given and asked

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Identify what you're being given and asked

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The problem is asking you to find ph at certain stages. First is buffer, then at equivalence, and lastly excess. You're also given volumes of the solution, concentrations, and kb. This will come in handy.

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Being prepared is essential, just jumping into the problem could prove a fatal mistake

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Being prepared is essential, just jumping into the problem could prove a fatal mistake

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So far, so good

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You're almost done!!

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Was that really so hard ?

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Practicing titration problems will build up your confidence and engrave the concepts into your mind. You'll will no longer fear titration problems but look forward to aceing them!!