A 25.00 mL sample of H₂SO₄ requires 31.43 mL of 0.110 M NaOH to reach the equivalence point.What is the molarity of the H₂SO₄?

Question

Quizplus · Accepted Answer

To find the molarity of the acid, we use the titration formula: $ M_1V_1 = M_2V_2 $, where $ M_1 $ and $ V_1 $ are the molarity and volume of the acid, and $ M_2 $ and $ V_2 $ are the molarity and volume of the base. Rearranging for $ M_1 $, we get $ M_1 = \frac{M_2V_2}{V_1} $. Plugging in the given values: $ M_1 = \frac{0.110 \, \text{M} \times 31.43 \, \text{mL}}{25.00 \, \text{mL}} = 0.138 \, \text{M} $. However, since the acid is $ \text{H}_2\text{SO}_4 $ (as indicated by the subscript formatting in the question), which is a diprotic acid, we need to account for the fact that each molecule of acid can react with two molecules of NaOH. Thus, the actual molarity of the acid solution is half of the calculated value, which is $ 0.0692 \, \text{M} $.

A 2500 ML Sample of H2SO4 Requires 31

A 2500 ML Sample of H₂SO₄ Requires 31