0.156 liters (156 mL) of NaOH are required to reach the second equivalence point.
How to find volume?
To find the volume of NaOH required to reach the second equivalence point, we first need to determine the moles of oxalic acid dihydrate (H₂C₂O₄･2H₂O) present in the solution.
Given concentration of H₂C₂O₄･2H₂O = 0.400 M
Moles of H₂C₂O₄･2H₂O = (Concentration) x (Volume)
= (0.400 mol/L) x (65.0 mL / 1000 mL/L)
= 0.026 mol
The balanced chemical equation shows that 1 mol of H₂C₂O₄･2H₂O reacts with 2 moles of NaOH.
So, moles of NaOH required = 2 x moles of H₂C₂O₄･2H₂O
= 2 x 0.026 mol
= 0.052 mol
Now, use the concentration and moles to find the volume of NaOH:
Volume of NaOH = Moles / Concentration
= 0.052 mol / 0.333 mol/L
≈ 0.156 L
Therefore, approximately 0.156 liters (156 mL) of NaOH are required to reach the second equivalence point.
Complete question:
A solution of oxalic acid dihydrate (H₂C₂O₄･2H₂O) with a known concentration of 0.400 MH₂C₂O₄ 2H₂0 is titrated with a 0.333 M NaOH solution. How many LNaOH are required to reach the second equivalence point with a starting volume of 65.0 ML H₂C₂O₄ 2H₂0, according to the following balanced chemical equation: H₂C₂0₄.2H₂0 + 2NaOH → Na₂C₂0₄ + 4 H₂O