Final answer:
To calculate the volume of NaOH solution needed to reach the final equivalence point, first determine the moles of ascorbic acid and the moles of NaOH required to react with it. Then use stoichiometry and the molarity of the NaOH solution to calculate the volume of NaOH solution needed.
Step-by-step explanation:
In order to calculate the volume of NaOH solution needed to reach the final equivalence point, we need to determine the moles of ascorbic acid and the moles of NaOH required to react with it.
First, we need to calculate the moles of ascorbic acid. We are given that 0.412 g of ascorbic acid is weighed out into a 250 mL volumetric flask and diluted to the mark with distilled water. Since the molar mass of ascorbic acid is 176.13 g/mol, we can calculate:
Moles of ascorbic acid = mass of ascorbic acid / molar mass of ascorbic acid
Moles of ascorbic acid = 0.412 g / 176.13 g/mol = 0.00234 mol
Next, we can use stoichiometry to determine the moles of NaOH required to react with the ascorbic acid. The balanced chemical equation for the reaction between ascorbic acid and NaOH is:
H2C6H6O6 + 2NaOH -> 2H2O + Na2C6H6O6
From the equation, we can see that 1 mole of ascorbic acid reacts with 2 moles of NaOH. Therefore, the moles of NaOH required can be calculated as:
Moles of NaOH = 2 * moles of ascorbic acid = 2 * 0.00234 mol = 0.00468 mol
Finally, we can calculate the volume of NaOH solution needed using the molarity of the NaOH solution, which is 0.1600 M:
Volume of NaOH solution = Moles of NaOH / Molarity of NaOH = 0.00468 mol / 0.1600 M = 0.02925 L = 29.25 mL