Use the volume at the equivalence point of 16 mL from the second titration to determine the Molarity of the H2O2 solution.
the volume of equivalence point= 16 mL = 0.16L
the density of H2O2 = 1.1 g/ml
from electrochemcial series, the standard reduction potential in aqueous solution at 25oC = 1.763 V
i.e, H2O2 (aq) + 2H+(aq) + 2e- 2H2O(l)
so , number of moles = 2
the molarity of H2O2 = number of moles X volume of equivalence point (in Liters)
= 2 X 0.16
= 0.32 mols/L
hence , the Molarity of the H2O2 solution = 0.32 M
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