A solution contains Ce(SO4)3 2- at a concentration of 0.0150 M. It was found tha
ID: 896858 • Letter: A
Question
A solution contains Ce(SO4)3 2- at a concentration of 0.0150 M. It was found that in a titration, 25.00 mL of this solution reacted completely with 23.44 mL of 0.032 M FeSO4 solution. The reaction gave me Fe 3+ as a product in the solution. In this reaction, what is the final oxidation state of Ce? A solution contains Ce(SO4)3 2- at a concentration of 0.0150 M. It was found that in a titration, 25.00 mL of this solution reacted completely with 23.44 mL of 0.032 M FeSO4 solution. The reaction gave me Fe 3+ as a product in the solution. In this reaction, what is the final oxidation state of Ce? A solution contains Ce(SO4)3 2- at a concentration of 0.0150 M. It was found that in a titration, 25.00 mL of this solution reacted completely with 23.44 mL of 0.032 M FeSO4 solution. The reaction gave me Fe 3+ as a product in the solution. In this reaction, what is the final oxidation state of Ce?Explanation / Answer
Solution :-
Lets first calculate the moles of the each reagent
moles = molarity * volume in liter
moles of Ce(SO4)3^2- = 0.0150 mol per L * 0.025 L = 0.000375 mol
moles of FeSO4 = 0.032 mol per L * 0.02344 L = 0.00075 mol FeSO4
mole ratio = moles of FeSO4 / moles of Ce(SO4)3^2-
= 0.00075 mol / 0.000375 mol
= 2
therefore mole ratio of the reaction is 1 mol Ce(SO4)3^2- : 2 mol FeSO4
the oxidation state of the Fe changes from +2 to +3 means its oxidizing
thereofore
initial oxidation state of the Ce in Ce(SO4)3^2-
(1*Ce) + (-2*3) = -2
Ce +(-6) = -2
Ce = -2+6
Ce =+4
now after reacting with the FeSO4
FeSO4 it gives 0.00075 mol electrons
therefore the oxidation state of the Ce in the final solution will change by 0.00075/0.000375 = 2
so the oxidation state of the Ce in the final state is +2
(Ce changes from +4 to +2 means its reduced)
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