Asked by Bree
Based on equation:
2MnO4¬¬(-) + 6H(+) +5H2O2 → 2Mn(2+) +8H2O + 5O2
A 50.0 mL solution of hydrogen peroxide of unknown concentration was diluted with 1.00L of water. 25mL of this diluted solution was then titrated with acidified potassium permanganate; 20.25mL 0f 0.02 mol/L permanganate was needed to completely neutralise this sample. Fine the concentration of the original hydrogen peroxide solution in mol/L.
2MnO4¬¬(-) + 6H(+) +5H2O2 → 2Mn(2+) +8H2O + 5O2
A 50.0 mL solution of hydrogen peroxide of unknown concentration was diluted with 1.00L of water. 25mL of this diluted solution was then titrated with acidified potassium permanganate; 20.25mL 0f 0.02 mol/L permanganate was needed to completely neutralise this sample. Fine the concentration of the original hydrogen peroxide solution in mol/L.
Answers
Answered by
DrBob222
I don't go along with the "to completely neutralize this sample" since this is a redo reaction and not an acid/base reaction. But I know what you mean.
mols KMnO4 = M x L = ?
mols H2O2 = mols KMnO4 x (5/2) = ?
That = mols in the 25 mL H2O2 and that times 40 = mols H2O2 in the 1.00L and that's the same as the mols in the 50 mL of the original solution.
(H2O2) = mols/0.05 = ?
mols KMnO4 = M x L = ?
mols H2O2 = mols KMnO4 x (5/2) = ?
That = mols in the 25 mL H2O2 and that times 40 = mols H2O2 in the 1.00L and that's the same as the mols in the 50 mL of the original solution.
(H2O2) = mols/0.05 = ?
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