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)
View Complete Written Solution
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.