\"Balancing a Limiting reagent Reaction and Determining the Formula of a product
ID: 1061976 • Letter: #
Question
"Balancing a Limiting reagent Reaction and Determining the Formula of a product by finding the molar ratio of the reactants"
Context-
In this lab we titrated 0.02M KMNo4 into a flask containing 10.0 mL of 0.05M NH3OH+ , 18.0mL of FeNH4(SO4)2 , and 10mL of 6M H3PO4 (to help eliminate any interference from chloride ions). The titration is complete and the molar ratio discovered but a secondary question is holding me back. I will do my best to provide enough information.
This was done to determine the moles of F2+ made by this reaction
The FeNH4(SO4)2 is the source of Fe3+ with moles of KMnO4 revealing the moles of Fe2+ titrated which equal the moles of Fe3+
Balanced Equations-
5Fe2+ + MnO4- + 8H+ = 5Fe3+ + Mn2+ + 4H2O
3Fe3+NH3OH+ = 3Fe2+ + NO +4H+
Question-
What would be observed in these reactions if the stockroom had prepared 0.2M Fe(NH4)2(SO4)2 instead of 0.2M FeNH4(SO4)2 ?
Explanation / Answer
If we will take 0.2M FeNH4(SO4)2, then here the oxidation state of Fe is +3 (ferric ion)
However If we will take mohr's salt, which is (NH4)2Fe(SO4)2 then there will be no source of ferric ion and the NH3OH+ will not react with with it.
It will be confusing to get Fe+2 moles formed as already we have taken salt of Fe+2 so no NH3OH+ will gets consumed.
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