Chemical Formula For Sodium Sulfate

Sodium sulfate SDS是指钠硫酸盐的安全数据表，包含有关这种化合物的物理、化学和毒理相关信息。下面是一些详细说明：

1. 化学性质：Sodium sulfate是一种无色晶体，其分子式为Na2SO4，相对分子质量为142.04g/mol。它具有中等溶解度，在水中可溶解度约为44 g/100 mL，在甲醇中可溶解度较小。

2. 物理性质：Sodium sulfate在室温下呈固体结晶状态，熔点为888℃。它在高温下会发生分解反应，生成二氧化硫和氧气。此外，它还具有比较低的蒸汽压和密度。

3. 毒理学信息：Sodium sulfate属于一般非毒性化学品，吞食或吸入少量粉尘不会造成严重的健康危害。但如果大量暴露于它，可能会引起眼睛和皮肤刺激。此外，它也可能对环境产生负面影响，如污染水源。

4. 安全操作：在使用Sodium sulfate时，应遵循正确的安全操作程序。建议戴上防护手套、防护眼镜和呼吸器等个人防护装备。同时，应在通风良好的环境下操作，避免直接接触到化合物。若不慎接触身体，应立即用大量清水冲洗，并及时就医治疗。

5. 储存条件：Sodium sulfate应储存在干燥、通风和避光的地方，远离火源和氧化剂。它应该与易燃物和酸性物质分开存放，以防止发生意外事故。

The chemical name of Na2SO3 is sodium sulfite.

Sodium sulfite is a white crystalline solid that is highly soluble in water and has a strong sulfurous odor. It is composed of two sodium cations (Na+) and one sulfite anion (SO32-), with a molecular weight of 126.04 g/mol.

In industry, sodium sulfite is commonly used as a reducing agent, preservative, and food additive. It can also be used in the production of paper, textiles, and photographic films.

It is important to handle and store sodium sulfite properly, as it can be hazardous if ingested, inhaled, or in contact with skin. Precautions should be taken when handling the compound, such as wearing protective clothing and avoiding direct contact with the eyes and skin.

Sodium sulfate is a white, odorless crystalline compound with a melting point of 884°C and a boiling point of 1429°C. It is soluble in water, but insoluble in alcohol. Sodium sulfate has a density of 2.68 g/cm³ and a molar mass of 142.04 g/mol. It is hygroscopic, meaning it can absorb moisture from the air. Sodium sulfate is not flammable or explosive, and it is not considered to be toxic. However, prolonged exposure to high concentrations of sodium sulfate dust may irritate the respiratory system.

Sodium sulfate has several industrial uses, including:

1. Detergent manufacturing: Sodium sulfate is used as a filler in powdered detergents to increase their bulk and improve their flow properties.

2. Glass manufacturing: Sodium sulfate is added to the mixture of raw materials used to make glass to lower its melting point and improve its workability.

3. Pulp and paper production: Sodium sulfate is used as a cooking chemical in the production of wood pulp for papermaking, helping to break down the fibers and separate the cellulose from the lignin.

4. Textile dyeing: Sodium sulfate is used as a leveling agent in textile dyeing, helping to ensure that the dye is evenly distributed across the fabric.

5. Chemical synthesis: Sodium sulfate is used as a source of sulfur in the production of various chemicals, such as sodium sulfide and sodium bisulfite.

Overall, sodium sulfate is a versatile compound with a wide range of industrial applications.

Sodium sulfate is generally considered to be a relatively safe compound, with low toxicity and minimal environmental impact. However, exposure to large amounts of sodium sulfate can cause irritation to the eyes, skin, and respiratory tract. Ingestion of large doses may cause gastrointestinal upset, including nausea, vomiting, and diarrhea.

Sodium sulfate is also a mild irritant to the lungs, and inhalation of dust or mist may result in respiratory irritation, coughing, and shortness of breath. Prolonged or repeated exposure to high levels of sodium sulfate dust may lead to lung damage and respiratory disorders.

In addition, sodium sulfate may have a corrosive effect on some metals, particularly aluminum, and should not be stored in contact with these materials. It may also react with strong acids to release sulfur dioxide gas, which is irritating to the eyes and respiratory system.

Overall, while sodium sulfate is not highly toxic, it is important to handle the compound with care and take appropriate safety precautions to minimize the risk of exposure and associated hazards.

The solubility of sodium sulfate in water varies with temperature. At 0°C, the solubility is approximately 9.6g/100mL of water. As the temperature increases, the solubility also increases and reaches a maximum of around 42g/100mL at 32.4°C. Above this temperature, the solubility decreases slightly and reaches about 39g/100mL at 100°C. It's important to note that these values are for anhydrous sodium sulfate (Na2SO4) and may differ for hydrated forms such as Na2SO4·10H2O.

The chemical reaction between sodium sulfate and hydrochloric acid can be represented by the following balanced equation:

Na2SO4 + 2HCl → 2NaCl + H2SO4

In this reaction, sodium sulfate (Na2SO4) reacts with hydrochloric acid (HCl) to produce sodium chloride (NaCl) and sulfuric acid (H2SO4).

The reaction is a double displacement reaction, where the positive ions of each compound switch places. The sodium ion (Na+) from sodium sulfate combines with the negative chloride ion (Cl-) from hydrochloric acid to form sodium chloride (NaCl), while the positive hydrogen ion (H+) from hydrochloric acid combines with the negative sulfate ion (SO42-) from sodium sulfate to form sulfuric acid (H2SO4).

This reaction is exothermic, meaning that it releases energy in the form of heat. It is also highly acidic, since sulfuric acid is a strong acid and can cause burns and other damage to skin and other materials. Care should be taken when handling these chemicals and appropriate safety precautions should always be followed.

Some common synonyms for sodium sulfate are Glauber's salt, sal mirabilis, thenardite, and mirabilite.

Sodium sulfate acts as a drying agent by its ability to absorb water molecules from a substance. When sodium sulfate is added to a wet or damp substance, it forms hydrates with the water molecules present in the substance. As a result, the sodium sulfate removes the water from the substance and forms anhydrous sodium sulfate, which is a highly effective drying agent. The anhydrous sodium sulfate can then be easily separated from the dry substance through filtration or decantation. This process is commonly used in various industries, including pharmaceuticals, food, and chemicals, to remove water from substances prior to further processing or analysis.

The molarity of a solution of sodium sulfate that contains 5 grams per liter can be calculated as follows:

1. Determine the molar mass of sodium sulfate (Na2SO4), which is 142.04 g/mol.

2. Convert the mass of the solute (5 grams) to moles by dividing by the molar mass:

5 g ÷ 142.04 g/mol = 0.0353 mol

3. Calculate the volume of the solution in liters. Since the concentration is given in terms of grams per liter, we know that there are 5 grams of sodium sulfate in each liter of solution. Therefore, the volume of the solution is also 1 liter.

4. Finally, divide the number of moles of solute by the volume of the solution in liters to obtain the molarity:

0.0353 mol ÷ 1 L = 0.0353 M

Therefore, the molarity of the solution is 0.0353 M.