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Answer :
It will take approximately 93.6 mL of 0.0411 M NaOH to reach the equivalence point when titrating the 36.3 mL aliquot of 0.0529 M H2SO4.
To determine the volume of base (NaOH) required to reach the equivalence point when titrating a 36.3 mL aliquot of 0.0529 M H2SO4 (aq) with 0.0411 M NaOH (aq), we need to use the concept of stoichiometry and the balanced chemical equation for the reaction.
The balanced chemical equation for the reaction between sulfuric acid (H2SO4) and sodium hydroxide (NaOH) is as follows:
H2SO4 + 2NaOH -> Na2SO4 + 2H2O
From the equation, we can see that 1 mole of sulfuric acid reacts with 2 moles of sodium hydroxide to reach the equivalence point. This means that the stoichiometric ratio between H2SO4 and NaOH is 1:2.
First, we need to calculate the number of moles of H2SO4 in the aliquot. We can do this by multiplying the concentration (0.0529 M) by the volume (36.3 mL) and converting the volume to liters: 0.0529 M * 36.3 mL * (1 L / 1000 mL) = 0.00192 moles of H2SO4.
Since the stoichiometric ratio between H2SO4 and NaOH is 1:2, we need twice the number of moles of NaOH to react with the H2SO4. Therefore, the number of moles of NaOH required is 2 * 0.00192 moles = 0.00384 moles.
To calculate the volume of 0.0411 M NaOH needed to reach this number of moles, we divide the moles by the concentration: 0.00384 moles / 0.0411 M = 0.0936 liters.
Finally, we convert the volume from liters to milliliters: 0.0936 liters * (1000 mL / 1 liter) ≈ 93.6 mL.
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