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Iron is by far the most reactive element in its group; it is pyrophoric when finely divided and dissolves easily in dilute acids, giving Fe 2+. However, it does not react with concentrated nitric acid and other oxidizing acids due to the formation of an impervious oxide layer, which can nevertheless react with hydrochloric acid. [10]
Nitric acid can oxidize non-active metals such as copper and silver. With these non-active or less electropositive metals the products depend on temperature and the acid concentration. For example, copper reacts with dilute nitric acid at ambient temperatures with a 3:8 stoichiometry: 3 Cu + 8 HNO 3 → 3 Cu(NO 3) 2 + 2 NO + 4 H 2 O
The most reactive metals, such as sodium, will react with cold water to produce hydrogen and the metal hydroxide: 2 Na (s) + 2 H 2 O (l) →2 NaOH (aq) + H 2 (g) Metals in the middle of the reactivity series, such as iron , will react with acids such as sulfuric acid (but not water at normal temperatures) to give hydrogen and a metal salt ...
When dissolved, iron(III) nitrate forms yellow solutions. When this solution is heated to near boiling, nitric acid evaporates and a solid precipitate of iron(III) oxide Fe 2 O 3 appears. [7] Another method for producing iron oxides from this nitrate salt involves neutralizing its aqueous solutions. [8]
Iron(II) nitrate can be produced in multiple ways, such as the reaction of iron metal with cold dilute nitric acid: 3 Fe + 8 HNO 3 + 12 H 2 O → 3 Fe(NO 3) 2 (H 2 O) 6 + 2 NO. If this reaction is conducted below -10 °C, nonahydrate is produced. It readily releases water to give the hexahydrate. [1] The above reaction can also co-produce ...
However, it does not react with concentrated nitric acid and other oxidizing acids due to the formation of an impervious oxide layer, which can nevertheless react with hydrochloric acid. [11] High-purity iron, called electrolytic iron, is considered to be resistant to rust, due to its oxide layer.
4, which forms a more protective, stable coating than the red oxide; the boiling water also removes any remaining residue from the applied acid solution (often nitric acid and hydrochloric acid diluted in water). The loose oxide was then carded (scrubbed) off, using a carding brush – a wire brush with soft, thin (usually about 0.002 in (0.051 ...
In the 1830s, Michael Faraday and Christian Friedrich Schönbein studied that issue systematically and demonstrated that when a piece of iron is placed in dilute nitric acid, it will dissolve and produce hydrogen, but if the iron is placed in concentrated nitric acid and then returned to the dilute nitric acid, little or no reaction will take ...