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Iron(III) oxide
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2. $NH_3$ or $KOH$ |
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$Fe^{3+}$ $+$ $3OH^-$ $\longrightarrow$ $Fe(OH)_3$ - Brown, flaky precipitate - Soluble in dilute mineral acids - Insoluble in excess reagent |
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2. $H_2S$ |
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Reduction of $Fe^{3+}$ to $Fe^{2+}$: $16Fe^{3+}$ $+$ $8S ^{2-}$ $\longrightarrow$ $16Fe^{2+}$ $+$ $S_8$ - sulfur precipitate |
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3. $(NH_4)_2S$ |
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Reduction followed by sulfide precipitation $16Fe^{3+}$ $+$ $8S ^{2-}$ $\longrightarrow$ $16Fe^{2+}$ $+$ $S_8$ $16Fe^{2+}$ $+$ $16S^{2-}$ $\longrightarrow$ $16FeS$ - Black precipitate |
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4. $K_4Fe(CN)_6$ Potassium hexacyanoferrate(II) |
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$4Fe^{3+}+3[Fe(CN)_6]^{4-}\longrightarrow Fe_4[Fe(CN)_6)]_3$ - Blue precipitate, Prussian blue, Iron(III) hexacyanoferrate(II) |
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5. $K_3Fe(CN)_6$ Potassium hexacyanoferrate(III) |
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$Fe^{3+}+[Fe(CN)_6]^{3-}\longrightarrow Fe[Fe(CN)_6)]$ - Dark brown soluble complex, iron(III) hexacyanoferrate(III), |
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6. $KSCN$ |
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7. $NaF$ |
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$Fe^{3+}$ $+$ $6F^-$ $\longrightarrow$ $FeF_6^{3-}$ - Soluble complex, colorless anion hexafluoroferrate(III) - Masking iron to $KSCN$ , but not to $KOH$, $NH_3$ and $K_4Fe(CN)_6$ |
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8. $CH_3COONa$ Sodium acetate |
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Formation of a red soluble complex $[Fe_3(CH_3COO)_6(OH)_2]^+$, by boiling one observes decomplexing and formation of $Fe(OH)_3$ |
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9. Tartarate |
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Formation of a soluble brown iron complex masking it to $KOH$ and $NH_3$ |