Problem: A 1.0L buffer solution contains 0.100 mol of HC2H3O2 and 0.100 mol of NaC2H3O. The value of Ka for HC2H3O2  is 1.8×10−5. Calculate the pH of the solution upon the addition of 0.015 mol of NaOH to the original buffer.

FREE Expert Solution

Determine the pH of the buffer upon addition of strong base using an ICF table and Henderson-Hasselbalch equation.

Step 1. Establish the ICF table

  • HC2H3O2 will appear as the weak acid and C2H3O2-(NaC2H3O2) as its conjugate base
  • Upon addition of the strong base, OH- will consume some of the HC2H3Oto form more C2H3O2-
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Problem Details

A 1.0L buffer solution contains 0.100 mol of HC2H3O2 and 0.100 mol of NaC2H3O. The value of Ka for HC2H3O2  is 1.8×10−5. Calculate the pH of the solution upon the addition of 0.015 mol of NaOH to the original buffer.

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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 Acid Strong Base Titrations concept. You can view video lessons to learn Weak Acid Strong Base Titrations. Or if you need more Weak Acid Strong Base Titrations practice, you can also practice Weak Acid Strong Base Titrations practice problems.