Problem: A 1.0L buffer solution contains 0.100 mol of HC2H3O2 and 0.100 mol of NaC2H3O2. The value of Ka for HC2H3O2 is 1.8×10−5. Calculate the pH of the solution upon the addition of 10.0 mL of 1.00 M  HCl to the original buffer.

FREE Expert Solution

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

Step 1. Determine the moles of acid added

  • Use the formula for molarity to determine the moles of H+ or H3O+
  • Recall that HCl is a monoprotic acid (produces one H+ per molecule)
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Problem Details

A 1.0L buffer solution contains 0.100 mol of HC2H3O2 and 0.100 mol of NaC2H3O2. The value of Ka for HC2H3O2 is 1.8×10−5. Calculate the pH of the solution upon the addition of 10.0 mL of 1.00 M  HCl to the original buffer.

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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.