How to test if sodium sulfide is oxidized 20

Pure sodium sulfide is a colorless crystalline powder. Strong moisture absorption, soluble in water. The aqueous solution has a strong alkaline reaction.

Burns can be caused when touched ** and hair. Therefore, sodium sulfide is commonly known as sulfide alkali. Sodium sulfide aqueous solution slowly oxidizes sodium thiosulfate, sodium sulfite, sodium sulfate, and sodium polysulfide in the air.

Since sodium thiosulfate is formed at a relatively fast rate, the main product of oxidation is sodium thiosulfate. Sodium sulfide is deliquescent in the air and carbonated and deteriorated, continuously releasing hydrogen sulfide gas. Industrial sodium sulfide contains impurities, and its color is pink, brownish-red, and earthy yellow.

Specific gravity, boiling point, also varies depending on the influence of impurities.

Check whether the sodium sulfide is oxidized: divide the solution into 2 parts, add copper sulfate and barium hydroxide respectively.

All are oxidized: the addition of copper sulfate does not produce a black solid, and the addition of barium hydroxide white precipitates.

Partial: Produces both black solids and white precipitates.

None: The addition of copper sulfate produces a black solid, and the addition of barium hydroxide does not have a white precipitate.

If all the sulfur ions are oxidized and hydrochloric acid is added, there will be no gas hydrogen sulfide produced, so it can be directly verified whether it is completely oxidized. If there is no complete oxidation, add acid and then add barium chloride, if there is a white precipitate, it means that sodium sulfide is oxidized.

na2s+2hcl====2nacl+h2s↑

naso4+bacl2*****baso4↓+2nacl

If there is a precipitate (sulfur) after acidification with hydrochloric acid, it indicates that it has been oxidized.

Summary. Sodium bisulfate is not easily oxidized, it is an inorganic compound that is often used to regulate pH. Sodium bisulfate is usually a white powdery solid with strong acidity and corrosiveness, but it does not spontaneously oxidize at room temperature.

However, under certain conditions, such as at high temperature, high pressure, and oxygen-containing environment, sodium bisulfate may undergo oxidation reactions, such as when sodium bisulfate is heated in an oxygen atmosphere, resulting in products such as sulfur dioxide, water, and sulfuric acid.

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Sodium bisulfate is not easily oxidized, it is an inorganic compound, and it is often used to adjust the pH of the Lingjie. Sodium bisulfate is usually a white powdered solid rot panicle, which is strongly acidic and corrosive, but it does not spontaneously oxidize at room temperature. However, under specific bib conditions, such as at high temperature, high pressure, and oxygen-containing environment, sodium bisulfate may undergo oxidation reactions, such as when sodium bisulfate is heated in an oxygen atmosphere, resulting in products such as sulfur dioxide, water, and sulfuric acid.

Summary. Sodium bisulfate, also known as sodium bisulfate, is a colorless, odorless, toxic crystal that is easily soluble in water. Sodium bisulfate can be oxidized in the air, resulting in a change in its properties, but its oxidation is relatively low.

When exposed to air, especially when the humidity is high, sodium bisulfate will become wet, producing oxidizing substances such as sulfur dioxide, nitrogen dioxide and oxygen, which trigger the oxidation reaction through chemical reactions, thereby reducing the stability of sodium bisulfate, so it needs to be sealed and stored.

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Sodium bisulfate, also known as sodium disulfide, is a colorless, odorless, toxic crystal that is easily soluble in water. Sodium bisulfate can be oxidized in the air, and its properties change due to the conduction, but its oxidation is relatively low. When exposed to air, especially when the humidity is high, sodium bisulfate will become wet, producing oxidizing substances such as sulfur dioxide, nitrogen dioxide and oxygen, which trigger the oxidation reaction through chemical reactions, thereby reducing the stability of sodium bisulfate, so it needs to be sealed and stored.

Summary. Sodium bisulfate (chemical formula NaHSO4), is a white powder that is easily soluble in water and acidic. Sodium bisulfate itself is not easily oxidized, but under certain conditions, it can also be oxidized.

For example, sodium bisulfate is susceptible to oxidation when it comes into contact with strong oxidizing agents such as hydrogen peroxide, potassium permanganate, etc. In addition, under high temperature, high pressure and other conditions, sodium bisulfate is also easy to be oxidized. In the laboratory, sodium bisulfate is often used as a neutralizer for reducing and oxidizing agents to determine the endpoint of redox reactions in solution.

Sodium bisulfate (chemical formula NaHSO4), is a white powder that is easily soluble in water and acidic. Sodium bisulfate itself is not easily oxidized, but under certain conditions, it can also be oxidized. For example, when sodium bisulfate comes into contact with strong oxidizing agents such as hydrogen peroxide, potassium permanganate, etc., it is easy to be oxidized.

In addition to this state, sodium bisulfate is also easy to be oxidized under high temperature, high pressure and other conditions. In the laboratory, sodium bisulfate is used as a neutralizer for reducing and oxidizing agents and is often used to determine the endpoint of redox reactions in hand-defined solutions.

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Sodium bisulfate (chemical formula NaHSO4), is a white powder that is easily soluble in water and acidic. Sodium bisulfate itself is not easily oxidized, but under certain conditions, it can also be oxidized. For example, when sodium bisulfate comes into contact with strong oxidizing agents such as hydrogen peroxide, potassium permanganate, etc., it is easy to be oxidized.

In addition to this state, sodium bisulfate is also easy to be oxidized under high temperature, high pressure and other conditions. In the laboratory, sodium bisulfate is used as a neutralizer for reducing and oxidizing agents and is often used to determine the endpoint of redox reactions in hand-defined solutions.

There are 3 main methods.

1. The equations that reflect the strong oxidation of concentrated sulfuric acid are all composed of SO2 raw field beams.

Cu+2H2SO4 (concentrated) = CuSO4+H2O+SO2 ZN+2H2SO4 (concentrated) = ZNSO4+H2O+SO2 2Fe + 6H2SO4 (concentrated) = Fe2(SO4)3+ 3H2O + 3SO2

2. Embody strong acid to make weak acid.

Na2SO3 + 2HCl = NaCl + SO2 + H2O (laboratory method).

Na2SO3 + H2SO4 = Na2SO4 + SO2 + H2O (laboratory method).

Ba2SO3 + H2SO4 = Ba2SO4 +SO2 +H2O3, reflecting the reduction of sulfur elements.

s + o2 = so2