Sodium Sulfide Nonahydrate Formula

Sodium sulfide nonahydrate is a commonly used chemical compound with the formula Na2S·9H2O. It is a white crystalline solid that contains both sodium ions (Na+) and sulfide ions (S2-).

One common use of sodium sulfide nonahydrate is in the production of paper pulp, where it is used as a pulping agent. It helps to break down the lignin in wood chips, which separates the fibers and allows them to be processed into paper.

Another use of this compound is in the leather industry, where it is used during the dehairing process to remove hair from animal hides. Sodium sulfide nonahydrate acts as a reducing agent, breaking down the disulfide bonds in keratin, the protein that makes up hair and nails.

Sodium sulfide nonahydrate is also used in the mining industry to separate ores from rocks. It is added to water along with other chemicals to create a frothy mixture that can then be separated into its component parts.

In addition, this compound is used as a source of sulfide ions in organic chemistry reactions and as a reducing agent in certain chemical processes.

It is important to handle sodium sulfide nonahydrate with care, as it is a hazardous substance that can cause skin and eye irritation, and can release toxic hydrogen sulfide gas when exposed to acid.

Sodium sulfide nonahydrate is a hazardous chemical compound that poses several risks when handled. Firstly, it can cause severe skin and eye irritation on contact, which may lead to burns or chemical injuries. Furthermore, sodium sulfide nonahydrate can emit toxic fumes when exposed to heat or acids, which can cause respiratory problems and even death in extreme cases.

It is also highly reactive with other chemicals, including acids, oxidizing agents, and metals, which can result in dangerous chemical reactions and the release of flammable or explosive gases. Therefore, proper precautions must be taken when handling sodium sulfide nonahydrate, such as wearing protective clothing and gloves, working in a well-ventilated area, and avoiding contact with other substances. Additionally, it should be stored in a dry and cool place away from any potential sources of ignition or incompatible materials.

Sodium sulfide nonahydrate can be synthesized by dissolving sodium sulfide in water and then crystallizing the compound from the solution in the presence of water. The resulting crystals will contain nine molecules of water for every molecule of sodium sulfide. Alternatively, the nonahydrate can be obtained by reacting sodium hydroxide with sulfur in the presence of hydrogen gas at high temperature and pressure. The resulting product is then dissolved in water and the nonahydrate precipitated out by adding alcohol or acetone to the solution. It is important to handle sodium sulfide and its solutions with care, as they can be highly toxic and corrosive.

Sodium sulfide can form several hydrates, including:

1. Sodium sulfide pentahydrate (Na2S·5H2O)

2. Sodium sulfide nonahydrate (Na2S·9H2O)

3. Sodium sulfide decahydrate (Na2S·10H2O)

4. Sodium sulfide undecahydrate (Na2S·11H2O)

The exact hydrate formed depends on the conditions of preparation and the relative humidity of the environment. Sodium sulfide pentahydrate is the most commonly encountered hydrate, but all four hydrates have been reported in the literature. These hydrates are used in various industrial processes, such as paper pulp processing, ore flotation, and wastewater treatment. It should be noted that sodium sulfide is hygroscopic, meaning it readily absorbs moisture from the air, which can lead to changes in the hydration state of the compound over time.

The melting point of sodium sulfide nonahydrate is 54.5°C. It is a white to yellow crystalline solid with the chemical formula Na2S·9H2O. The compound is soluble in water and has a strong odor of hydrogen sulfide. It is commonly used in the production of paper pulp, dyes, and pharmaceuticals. When heated, it decomposes and releases toxic fumes, so proper ventilation and safety precautions should be taken.

The boiling point of sodium sulfide nonahydrate is not applicable because this compound undergoes thermal decomposition before it reaches its boiling point. The compound begins to decompose at around 50°C and releases hydrogen sulfide gas, which has a strong odor and can be harmful if inhaled. Therefore, it is important to handle this compound with care and avoid heating it above room temperature.

Sodium sulfide nonahydrate sigma is a white crystalline solid with the chemical formula Na2S∙9H2O. It is also known as sodium sulfide enneahydrate or sodium sulfide nona. The compound is highly soluble in water and has a strong odor of hydrogen sulfide.

In terms of its chemical composition, sodium sulfide nonahydrate contains two sodium ions (Na+) and one sulfide ion (S2-) for every formula unit. The nine water molecules in the crystal structure are held in place by hydrogen bonds with the sulfide and sodium ions.

Sodium sulfide nonahydrate is commonly used in a variety of industrial applications such as ore flotation, leather tanning, and the production of sulfur dyes. It is also used as a reducing agent in organic chemistry reactions.

It is important to handle sodium sulfide nonahydrate with caution as it can be corrosive to skin and eyes. Protective equipment such as gloves and goggles should be worn when handling the compound. Additionally, it should be stored in a cool, dry place away from incompatible materials such as acids and oxidizers.

Sodium sulfide nonahydrate SDS is a compound with the chemical formula Na2S·9H2O. It is a white to yellowish crystalline solid that is highly soluble in water. The compound is commonly used in the chemical industry as a reducing agent and as a source of sulfur for the production of other chemicals.

The structure of sodium sulfide nonahydrate consists of Na+ cations and S2- anions, which are arranged in a cubic crystal lattice. Each Na+ ion is surrounded by six S2- ions, and each S2- ion is coordinated to six Na+ ions. The nine water molecules in the compound are attached to the sodium cations through hydrogen bonding.

When sodium sulfide nonahydrate is heated, it decomposes to form sodium sulfide heptahydrate (Na2S·7H2O), which in turn decomposes further to form sodium sulfide anhydrous (Na2S). This reaction releases water and sulfur dioxide gas.

Sodium sulfide nonahydrate is a strong reducing agent and can react violently with oxidizing agents. It can also be corrosive to metals and may cause severe burns and eye damage upon contact with skin or eyes. Therefore, appropriate safety measures should be taken when handling this compound.

Sodium sulfide nonahydrate is a compound with the chemical formula Na2S·9H2O. Its solubility in water varies depending on the temperature, as well as the concentration of other ions present in the solution. At room temperature (25°C), the solubility of sodium sulfide nonahydrate in water is approximately 20 grams per 100 milliliters of water.

However, as the temperature increases, the solubility of sodium sulfide nonahydrate also increases. For example, at 50°C, its solubility in water is approximately 33 grams per 100 milliliters, while at 100°C, it can dissolve up to approximately 70 grams per 100 milliliters of water.

It should be noted that the presence of other ions in the solution can also affect the solubility of sodium sulfide nonahydrate. For instance, the presence of certain cations, such as calcium or magnesium, can reduce the solubility of the compound in water, while the presence of certain anions, such as sulfide or hydroxide, can increase its solubility.

Sodium sulfide nonahydrate is a compound that is typically stored in a cool, dry place to prevent it from decomposing or reacting with other substances. It should be kept away from sources of heat or flame, as it is flammable and can ignite if exposed to high temperatures. Additionally, sodium sulfide nonahydrate should be kept out of reach of children and pets, as it can be harmful if ingested or inhaled.

When storing sodium sulfide nonahydrate, it is important to ensure that its container is tightly sealed to prevent moisture from entering. Sodium sulfide nonahydrate has a tendency to absorb water from the air, which can cause it to form lumps or clumps. This can make it difficult to measure and use the compound accurately.

If sodium sulfide nonahydrate does become damp or clumped, it can be dried by spreading it out on a flat surface and allowing it to air-dry for several hours. However, it is important to handle the compound carefully during this process, as it can release hydrogen sulfide gas, which is toxic and has a strong odor.

Overall, proper storage and handling of sodium sulfide nonahydrate is essential to ensure its effectiveness and safety.

The chemical compound sodium sulfide nonahydrate (CAS number 1313-84-4) is a white, crystalline solid with the formula Na2S·9H2O. It is a hydrate of sodium sulfide and contains nine water molecules per unit of sodium sulfide.

The compound is soluble in water and its aqueous solution is highly alkaline. It reacts with acids to produce hydrogen sulfide gas, which has a characteristic rotten egg odor. Sodium sulfide nonahydrate is commonly used in the production of dyes, leather, and paper.

In terms of safety, sodium sulfide nonahydrate is corrosive and can cause severe skin and eye irritation. It should be handled with care, using appropriate protective equipment such as gloves and goggles. It is also important to avoid inhalation or ingestion of the compound. Proper storage and disposal procedures should be followed to prevent environmental contamination.

Sodium sulfide nonahydrate Merck is a chemical compound with the molecular formula Na2S·9H2O. It appears as colorless or white crystals that are highly soluble in water and have a strong odor of hydrogen sulfide.

The compound is commonly used as a reducing agent, as well as in the preparation of other chemicals such as sodium hydrosulfide and sulfur dyes. It also has applications in the leather industry for dehairing hides and in the pulp and paper industry for bleaching wood pulp.

When handling sodium sulfide nonahydrate Merck, it is important to take proper safety precautions due to its corrosive and toxic nature. Protective clothing, gloves, and eye protection should be worn, and the compound should only be handled in a well-ventilated area. It should also be stored in a cool, dry place away from incompatible materials such as acids, oxidizers, and metals.

Overall, sodium sulfide nonahydrate Merck is a useful but potentially hazardous compound that should be handled with care and caution to ensure safety and accuracy in its use.

Sodium sulfide (anhydrous) is an inorganic compound with the chemical formula Na2S. It is a colorless to yellowish solid that is highly soluble in water, but insoluble in organic solvents.

The compound can be prepared by reacting sodium with sulfur at high temperatures or by treating sodium hydroxide with hydrogen sulfide gas. Sodium sulfide is commonly used in a variety of industrial applications, including paper production, leather processing, and as a reducing agent in chemical reactions.

It is important to handle sodium sulfide with care as it is corrosive and can cause severe skin and eye irritation. When handling, protective clothing, gloves, and goggles should be worn. Additionally, sodium sulfide should be stored in a cool, dry place away from incompatible substances such as acids and oxidizers.

In aqueous solutions, sodium sulfide undergoes hydrolysis to produce hydrogen sulfide gas and sodium hydroxide. This reaction results in the characteristic odor of rotten eggs associated with the compound.

Overall, sodium sulfide plays an important role in various industrial processes and must be handled with care due to its corrosiveness and potential health hazards.

The chemical formula for sodium sulfide nonahydrate is Na2S·9H2O. This indicates that it contains two sodium (Na) atoms, one sulfur (S) atom, nine water (H2O) molecules, and a total of 18 hydrogen (H) and 9 oxygen (O) atoms.

The molar mass of sodium sulfide nonahydrate can be calculated by adding the molar masses of its individual components. Sodium sulfide has a molar mass of 78.045 g/mol (22.99 g/mol for sodium and 55.96 g/mol for sulfur), while nonahydrate means there are nine water molecules (H2O) per formula unit, each with a molar mass of 18.015 g/mol. Therefore, the molar mass of sodium sulfide nonahydrate is:

Molar mass = [molar mass of Na2S] + ([molar mass of H2O] x 9)

Molar mass = (22.99 g/mol x 2) + (18.015 g/mol x 9)

Molar mass = 126.04 g/mol

Therefore, the molar mass of sodium sulfide nonahydrate is 126.04 g/mol.

Sodium sulfide nonahydrate appears as a colorless to white crystalline solid. It is usually found as large transparent to translucent crystals, although it may sometimes appear as a powder. The compound is highly soluble in water and has a characteristic odor of hydrogen sulfide. Its chemical formula is Na2S·9H2O.

The solubility of sodium sulfide nonahydrate in water is approximately 47 grams per 100 milliliters of water at 20°C. However, it should be noted that solubility can vary depending on factors such as temperature and pressure. When dissolved in water, sodium sulfide nonahydrate dissociates into the Na+ and S2- ions.