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What volume of a 0.452 M NaOH solution is needed to neutralize 85 mL of a 0.176 M solution of H₂SO₄?

A. 218.3 mL
B. 66.2 mL
C. 38.4 mL
D. 436.6 mL

Answer :

Final answer:

The correct answer is (b) Approximately 66.2 mL of the 0.452 M NaOH solution is required to neutralize 85 mL of a 0.176 M H2SO4 solution due to the 1:2 stoichiometric relationship between sulfuric acid and sodium hydroxide in the neutralization reaction.

Explanation:

Neutralization of H2SO4 with NaOH

To determine the volume of a NaOH solution required to neutralize an H2SO4 solution, we can use the stoichiometry of the reaction and molarity concentration of the solutions. The balanced equation for the reaction is:

Chemical Reaction

H2SO4 + 2NaOH
ightarrow Na2SO4 + 2H2O

This shows that each mole of H2SO4 is neutralized by 2 moles of NaOH. Using the given molarities, we can calculate:

  1. Moles of H2SO4 = 0.176 M imes 0.085 L = 0.01496 moles
  2. Moles of NaOH needed = 0.01496 moles of H2SO4 imes 2 = 0.02992 moles
  3. Volume of NaOH = 0.02992 moles / 0.452 M = 0.0662 L

Thus, 0.0662 L or 66.2 mL of the 0.452 M NaOH solution is needed to neutralize 85 mL of a 0.176M solution of H2SO4.

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