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:
- Moles of H2SO4 = 0.176 M imes 0.085 L = 0.01496 moles
- Moles of NaOH needed = 0.01496 moles of H2SO4 imes 2 = 0.02992 moles
- 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.