Oxidation capacity of ferrous ions, ionic equation for oxidation of ferrous ions to iron ions?

Ferrous ions are oxidized to generally give +3 valence iron. Due to the moderate oxidizing properties of +3-valent iron, ferrous iron can be oxidized by slightly stronger oxidants, such as chlorine, bromine, oxygen, potassium permanganate, potassium dichromate, nitric acid and other common oxidants. Under alkaline conditions, the extremely strong oxidant can oxidize ferrous ions into +6 potassium ferrite, such as sodium hypochlorite, etc., in fact, sodium ferrite in an acidic environment is a more oxidizing substance than O3 and KMno4.

2fe(oh)3 + 3naclo + 4naoh ==== 2na2feo4 + 3nacl + 5h2o

The more reactive metals can be oxidized by ferrous ions, such as zinc, aluminum, magnesium, etc. The reducing properties of sodium, potassium, and calcium are too strong, and they react when they are dipped in water, and can only replace the iron in the molten ferrous salts.

In high school, these two are generally available.

If it does not specifically refer to the oxidation of any substance, it is Fe2+ E- Fe3+

Ferrous ions lose one electron and are oxidized to iron ions.

1. Ferrous ions are reducible, and potassium permanganate, potassium chromate, and hydrogen peroxide oxidizer oxidize them into iron ions.

2. In an acidic solution, the oxygen in the air oxidizes ferrous ions to iron ions.

3. Ferrous ions undergo redox reaction with the branches of newly made chlorine water and oxidize into iron ions.

4. Ferrous ions and concentrated dilute nitric acid can undergo redox reaction and oxidize into iron ions.

1.Iron ions can react with metals (such as Cu and Ag) that are weaker than iron to form ferrous ions. 2fe3+

cu2fe2+

Cu2+ (iron ions are more oxidizing than copper ions).

2. Iron ions can also be associated with a small amount of metals that are more reducible than iron but do not react with water (such as. mgalzn) reaction to form ferrous ions. 2fe3+

zn2fe2+

Zn2+ (Zn as a reducing agent, which can reduce iron ions to ferrous ions) If there is an excess of these metals, it will further reduce ferrous ions to single finger iron.

3. Iron ions can also react with iron to form ferrous ions (centering reaction) 2Fe3+Fe

3fe2+

Summary. Iron ions are removed, and oxidants are added under alkaline conditions. Because ferrous hydroxide is easily oxidized to iron hydroxide under alkaline conditions, the resulting iron hydroxide will be stripped out of solution in the form of precipitation.

At the same time, iron hydroxide is not easy to redissolve under alkaline conditions, and can be quickly removed by filtration and separation. Under neutral conditions, the solubility of iron hydroxide will be relatively large, and it will be difficult to precipitate and separate, so the effect will be relatively poor.

Ferrous hydroxide is susceptible to oxidation. In chemistry, ferrous hydroxide(II) can be oxidized to iron hydroxide by oxygen and oxidants, while ferrous ion mountain clear (Fe2+) can be further oxidized to ferrous iron (III). Therefore, in some chemical reactions, ferrous hydroxide(II) hydroxide is considered to be susceptible to oxidation, while ferrous ions are relatively stable.

There are iron ions in the solution, and the removal of iron ions is good for adding oxidant under neutral conditions? Or alkaline conditions?

Iron hydroxide precipitates almost entirely in neutral conditions, while ferrous hydroxide precipitates in alkaline conditions.

Iron ions are removed, and oxidants are added under alkaline conditions. Because under alkaline conditions, ferrous hydroxide is easily oxidized to iron hydroxide, and the resulting iron hydroxide will be stripped from the solution in the form of precipitation. At the same time, iron hydroxide is easy to redissolve under alkaline conditions, and can be quickly removed by filtration and separation.

Under neutral conditions, the solubility of iron hydroxide will be relatively large, and it will be difficult to precipitate and separate, so the effect will be relatively poor.

According to the KSP of iron hydroxide, pH4-5 has almost precipitated.

If the solubility product of iron hydroxide has been reached, it is indeed easy to precipitate when the pH is in the range of 4-5. In the pH range, iron hydroxide is less soluble, so the degree of dissolution is relatively low, and precipitates are relatively easy to form. At the same time, the pH is also affected, which may cause the reed to tremble and cause uneven precipitation or color changes, so it is necessary to pay attention to the control and adjustment of pH during the experimental operation.

Divalent iron is oxidized to trivalent iron, which can be well precipitated under neutral conditions, is it necessary to adjust it to alkaline?

Under neutral conditions, iron(III) hydroxide will precipitate, but not very completely. However, under alkaline closed-bond conditions, iron(III) hydroxide is more likely to form stable precipitation, and the precipitation amount is larger. Therefore, in order to obtain better precipitation and separation purity, it is necessary to adjust the solution to alkaline conditions.

Ferrous hydroxide (Fe(OH)2) and ferrous locust ions (Fe2+) are both substances with certain reducing properties.

Ferrous hydroxide can undergo an oxidation reaction that oxidizes Fe(Oh)2 to Fe(Oh)3 or FeO(OH). At the same time, Luwei ferrous hydroxide can also be reduced to Fe2+ under certain conditions.

The ferrous ion itself is a highly reducing substance, which can often play the role of a reducing agent in chemical reactions. For example, when reacting with copper chloride, ferrous ions can reduce Cu2+ to Cu+ and oxidize themselves to Fe3+.

3fe2+ =2fe3+

Fe2+ loses an electron and is oxidized to Fe3+, for example, 2FeCl2 + Cl2 = 2FeCl3, and Cl2 is the oxidizing agent in the banquet.