In a volumetric analysis experiment,a solution of sodium oxalate (Na₂C₂O₄) in acidic solution is titrated with a solution of potassium permanganate (KMnO₄) according to the following balanced chemical equation:
2KMnO₄(aq) + 8H₂SO₄(aq) + 5Na₂C₂O₄(aq) → 2MnSO₄(aq) + 8H₂O(l) + 10CO₂(g) + 5Na₂SO₄(aq) + K₂SO₄(aq)
What volume of 0.0262 M KMnO₄ is required to titrate 0.170 g of Na₂C₂O₄ dissolved in 45.0 mL of solution?

Question

Quizplus · Accepted Answer

1) Determine the moles of Na2C2O4 in the 45.0 mL solution:
Moles Na2C2O4 = (0.170 g Na2C2O4) / (128.01 g/mol Na2C2O4) = 0.001328 mol Na2C2O4
2) Calculate the number of moles of KMnO4 needed to react with the Na2C2O4:
2 mol KMnO4 : 5 mol Na2C2O4
0.001328 mol Na2C2O4 x (2 mol KMnO4 / 5 mol Na2C2O4) = 0.0005312 mol KMnO4
3) Use the molarity of KMnO4 to calculate the required volume:
Moles = Molarity x Volume (L)
0.0005312 mol KMnO4 = (0.0262 mol/L) x Volume (L)
Volume = 0.0203 L = 20.3 mL
Therefore, the answer is C) 19.3 mL (rounded to 2 decimal places).

In a Volumetric Analysis Experiment,a Solution of Sodium Oxalate (Na2C2O4)in

In a Volumetric Analysis Experiment,a Solution of Sodium Oxalate (Na₂C₂O₄)in