An aqueous solution of 6.3g oxalic acid dihydrate is made up to 250 ml...
Calculation of Volume of NaOH Required to Neutralize the Solution
Given:Mass of oxalic acid dihydrate = 6.3g
Volume of solution = 250 ml
Concentration of NaOH = 0.1N
Volume of solution to be neutralized = 10 ml
Formula:Moles of oxalic acid dihydrate = (mass of oxalic acid dihydrate) / (molar mass of oxalic acid dihydrate)
Moles of NaOH = (concentration of NaOH) x (volume of NaOH used in liters)
Moles of oxalic acid dihydrate = moles of NaOH (at equivalence point)
Calculation:Molar mass of oxalic acid dihydrate = molar mass of oxalic acid + 2 x molar mass of water
Molar mass of oxalic acid dihydrate = (2 x 1) + (2 x 16) + 2 x [1 + (2 x 16)]
Molar mass of oxalic acid dihydrate = 126 g/mol
Moles of oxalic acid dihydrate = (6.3g) / (126 g/mol) = 0.05 mol
At equivalence point, moles of NaOH = moles of oxalic acid dihydrate
Therefore, moles of NaOH = 0.05 mol
Moles of NaOH = (concentration of NaOH) x (volume of NaOH used in liters)
Volume of NaOH used in liters = moles of NaOH / concentration of NaOH
Volume of NaOH used in liters = 0.05 mol / 0.1N = 0.5 L
Volume of NaOH used in 10 ml of solution = (0.5 L / 250 ml) x 10 ml = 0.02 ml
Therefore, the volume of NaOH required to completely neutralize 10 ml of this solution is 0.02 ml.