Asked by Rob
A solution of potassium permanganate (KMnO4) was standardised by titrating with 0.20 g of Na2C2O4 dissolved in 50 cm3 of acidified water. The endpoint was reached after 23.10 cm3 of solution had been added. Calculate the molar concentration of KMnO4 in the solution.
Answers
Answered by
DrBob222
1. Write and balance the equation.
2MnO4^- + 5C2O4^2- + ? ==> 2Mn^2+ + 10CO2 +?
I didn't finish the entire equation (that is I omitted the H^+, electrons, and H2O) BUT I balanced the redox part and that's all you need.
2. mols Na2C2O4 = grams/molar mass = ?
3. Using the coefficients in the balanced equation, convert mols C2O4^2- to mols MnO4^-. That's ?mols Na2C2O4 x (2 mols KMnO4/5 mols Na2C2O4) = ?
4. Then M KMnO4 = mols KMnO4/L KMnO4
2MnO4^- + 5C2O4^2- + ? ==> 2Mn^2+ + 10CO2 +?
I didn't finish the entire equation (that is I omitted the H^+, electrons, and H2O) BUT I balanced the redox part and that's all you need.
2. mols Na2C2O4 = grams/molar mass = ?
3. Using the coefficients in the balanced equation, convert mols C2O4^2- to mols MnO4^-. That's ?mols Na2C2O4 x (2 mols KMnO4/5 mols Na2C2O4) = ?
4. Then M KMnO4 = mols KMnO4/L KMnO4
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