Asked by Jessica
A student determines the iron (II) content of a solution by first precipitating it as iron (II) hydroxide, and then decomposing the hydroxide to iron (II) oxide by heating. How many grams of iron (II) oxide should the student obtain if her solution contains 46.0 mL of 0.426 M iron(II) nitrate?
Answers
Answered by
DrBob222
Fe(NO3)2 + 2OH^- ==> Fe(OH)2 + 2NO3^-
Then Fe(OH)2 + heat ==> FeO + H2O
mols Fe(NO3)2 = mols x L = ?
mols FeO = mols Fe(NO3)2 (look at the equation; 1 mol Fe(NO3)2 = 1 mol FeO)
Then g Fe) = mols FeO x molar mass FeO.
Then Fe(OH)2 + heat ==> FeO + H2O
mols Fe(NO3)2 = mols x L = ?
mols FeO = mols Fe(NO3)2 (look at the equation; 1 mol Fe(NO3)2 = 1 mol FeO)
Then g Fe) = mols FeO x molar mass FeO.
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