*500mg of iron (ii) complex and ferrous bisglyceride was dissolved in dilute H2SO4 and titrated...
*500mg of iron (ii) complex and ferrous bisglyceride was dissolved in dilute H2SO4 and titrated...
*500mg of iron (ii) complex and ferrous bisglyceride was dissolved in dilute H2SO4 and titrated with 0.02moldm-³ KmnO4. 18.10cm³ of KMnO4 solution was required to reach the end point. The equation for the titration reaction is as follows:*
5Fe² + MnO4 + 8H -------------> 5Fe² + Mn² + 4H20
*Calculate*
I. The number of moles of Fe² in the capsule
II. Mass of iron in the capsule
III. Molar mass of the iron(ii) complex assuming that one mole of the complex contains one mole of iron (Fe = 55.9)?
InChemistry
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Asked by Chasey on 20th December, 2021
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