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Calculate: if you have 40.0ml of 0.100mol/l acetic acid and you titrate it with 0.100 mol/l NaOH (aq), what would be the p of the solution at the equivalence point? ka for acetic acid is 1.8x10-5.
Accepted Answer
At the equivalence point, the number of moles of acetic acid is equal to the number of moles of NaOH added. So, 0.100 mol/L x 40.0 mL = 0.004 mol of acetic acid = 0.004 mol of NaOH. Thus, the total volume of the solution is 40.0 mL + 40.0 mL = 80.0 mL. The molarity of NaOH is 0.004 mol/80.0 mL = 0.0500 mol/L. The pOH of the solution is -log(0.0500) = 1.30. The pH of the solution is 14.00 - 1.30 = 12.70.
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