Final answer:
To titrate 1.65 L of 0.500 M sulfuric acid with sodium hydroxide, 1.65 moles of NaOH are required, since sulfuric acid is diprotic and reacts with NaOH in a 1:2 ratio.
Step-by-step explanation:
To determine the number of moles of sodium hydroxide (NaOH) required to react with 1.65 L of 0.500 M sulfuric acid (H2SO4) to reach the titration endpoint, we must first understand the stoichiometry of the reaction. Sulfuric acid is a diprotic acid, meaning it can donate two protons (H+) per molecule. The balanced chemical equation for the reaction is:
H2SO4 (aq) + 2NaOH(aq) → Na2SO4 (aq) + 2H2O(l)
From the equation, we see that each mole of sulfuric acid reacts with two moles of sodium hydroxide. To find out how many moles of sulfuric acid we have, we multiply the volume of the solution by its molarity:
Moles of H2SO4 = 1.65 L × 0.500 M = 0.825 mol
Since it takes 2 moles of NaOH to neutralize 1 mole of H2SO4, we multiply the moles of sulfuric acid by 2:
Moles of NaOH required = 0.825 mol H2SO4 × 2 = 1.65 mol
Therefore, the correct answer is a. 1.65 mol of sodium hydroxide, which is necessary to reach the endpoint of the titration.