Question

You titrated a 21.00 mL solution of 0.0600 M oxalic acid (H2C2O4) with 0.0800 M NaOH. The balanced equation for the reaction is:H2C2O4 + 2NaOH → Na2C2O4 + 2H2O

What volume of NaOH solution was required to reach the equivalence point?
0.0126 L
0.0168 L
0.0252 L
0.0336 L

Answer 1

To find the volume of NaOH needed for titration, the moles of oxalic acid are first calculated, then, using the stoichiometric ratio of 1:2 for the reaction, the moles of NaOH required are determined. Dividing these moles by the molarity of the NaOH gives the volume required for equivalence, but the calculated value does not match the provided options.

Step-by-step explanation:

To determine the volume of NaOH solution required to reach the equivalence point when titrating with oxalic acid, we use the stoichiometry of the balanced equation:

H2C2O4 + 2NaOH → Na2C2O4 + 2H2O

First, calculate the moles of oxalic acid:

# moles H2C2O4 = 21.00 mL × 0.0600 M = 0.00126 mol

Since the reaction ratio of H2C2O4 to NaOH is 1:2, we need twice the moles of NaOH:

# moles NaOH = 2 × 0.00126 mol = 0.00252 mol

Then, calculate the volume of NaOH solution:

Volume NaOH = # moles NaOH / Molarity NaOH = 0.00252 mol / 0.0800 M = 0.0315 L = 31.50 mL

However, since this value is not one of the options given, it implies there might be a calculation error or typo in the options. Therefore, please double-check the given values and options for the correct answer.