1.)Write the Balanced net ionic equation for the reaction between MnO4- ion and Fe2+ ion in acidic solution.2.) How many moles of Fe2+ ion can be iodized by .0014 moles of MnO4- ion in the reaction in question 1.3.) A solid sample containing some Fe 2+ ion weighs 1.062g. It requires 24.12 mL 0.01562 M KMno4 to titrate the Fe2+ in the dissolved sample to a pink end point.a) How many moles Mno4- ion are required?b) How many moles Fe2+ are there in the sample?c) How many grams of iron are there in the sample?d) What is the percentage of Fe in the sample?4.)What is the percentage of Fe in iron(II) ammonium sulfate hexahydrate, Fe(NH4)2(SO4)2*H2O
Adding the halfequations:OXIDATION: Fe2+(aq) → Fe3+(aq) + e‾REDUCTION: MnO4(aq) + 8H++(aq) + 5e‾ → Mn2+(aq) + 4H2O(l)so as to eliminate electrons (ie 5 * OXIDATION + REDUCTION) we…
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