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 0.0206 M KMnO₄ is required to titrate 0.176 g of Na₂C₂O₄ dissolved in 50.0 mL of solution?

Question

Quizplus · Accepted Answer

First, we need to calculate the number of moles of Na2C2O4:
moles Na2C2O4 = 0.176 g / (2 * 23.00 + 12.01 + 4 * 16.00) = 0.001 mol

Next, we can use stoichiometry to determine how many moles of KMnO4 are required to react with the Na2C2O4:
2 KMnO4 + 5 Na2C2O4 + 8 H2SO4 → 2 MnSO4 + 10 CO2 + 8 H2O + 5 Na2SO4 + K2SO4

From the balanced equation, we can see that 2 moles of KMnO4 react with 5 moles of Na2C2O4. Therefore, the number of moles of KMnO4 needed is:

moles KMnO4 = (0.001 mol Na2C2O4) / (5 mol Na2C2O4 / 2 mol KMnO4) = 0.0004 mol KMnO4

Finally, we can use the molarity and volume of the KMnO4 solution to determine the volume required for the titration:

moles KMnO4 = M KMnO4 x V KMnO4
V KMnO4 = moles KMnO4 / M KMnO4 = 0.0004 mol / 0.0206 M = 0.0194 L = 19.4 mL

Therefore, the best choice is C) 25.5 mL, which is the closest to the calculated volume of KMnO4 required for the titration.

A Solution of Sodium Oxalate (Na2C2O4)in Acidic Solution Is Titrated

A Solution of Sodium Oxalate (Na₂C₂O₄)in Acidic Solution Is Titrated