Final answer:
To find the volume of NaOH needed to neutralize 55.2 mL of H₂SO₄, the molarity of both the acid and the base is required, as the molar ratio of NaOH to H₂SO₄ is 2:1.
Step-by-step explanation:
To determine how many milliliters of NaOH are needed to neutralize 55.2 mL of H₂SO₄, we must know the molarity of the H₂SO₄ and the NaOH solutions, as this is stoichiometry and involves molar relationships. Without the molarity, it's not possible to provide an exact answer. Generally, the neutralization reaction between H₂SO₄ and 2NaOH would give us Na₂SO₄ and 2H₂O, indicating that the molar ratio of NaOH to H₂SO₄ is 2:1.
To determine the volume of NaOH needed to neutralize 55.2 ml of H2SO4, we can use the balanced chemical equation:
H2SO4 (aq) + 2NaOH (aq) → Na2SO4 (aq) + 2H2O (l)
From the equation, we can see that for every mole of H2SO4, 2 moles of NaOH are needed. Since the concentrations of H2SO4 and NaOH are not given, we cannot determine their exact molarities. Therefore, we cannot calculate the volume of NaOH needed to neutralize the H2SO4. Additional information is required to solve the problem.