月: 2023年1月

What Is Lead Nitrate?

Lead nitrate, known as lead(II) nitrate, is an inorganic compound with the chemical formula Pb(NO₃)₂. Its molecular weight is 331.2 g/mol. This compound decomposes upon heating, releasing toxic nitrogen oxides and lead oxides.

It is regulated under several laws due to its hazardous nature.

Uses of Lead Nitrate

Lead nitrate is utilized in the manufacturing of matches, as an oxidizing agent in black powder for fireworks, and in explosives. It also finds applications as a heat stabilizer in polyester and nylon, a coating agent for thermal paper, rat poison, a mordant in dyeing chintz, and as a precursor for pigments such as yellow lead and Naples yellow. Additionally, it serves as a stabilizer in electroless plating solutions, in the production of optical glass, and as a reagent in purity tests for ferricyanide.

Properties of Lead Nitrate

Lead nitrate is a white or colorless solid, soluble in water with a solubility of 56.5 g per 100 g of water at 20°C and 135 g at 100°C. Its specific gravity is 4.53 at 20°C. It decomposes to lead(II) oxide when heated and can synthesize insoluble lead salts. Its solubility leads to the formation of various basic salts depending on the pH. Lead nitrate can cause lead poisoning, with symptoms including bowel dysfunction, loss of appetite, abdominal pain, vomiting, and nausea.

Structure of Lead Nitrate

The crystal structure of solid lead nitrate, determined by neutron diffraction, is a face-centered cubic system. Each lead atom is centrally bonded to 12 oxygen atoms, with a bond length of 281 pm and all N-O bonds measuring 127 pm.

Other Information on Lead Nitrate

1. Synthesis of Lead Nitrate

Discovered by Andreas Libavius in 1597, lead nitrate is produced by dissolving metallic lead or lead(II) oxide in nitric acid. It can also result from evaporating a solution obtained from reacting metallic lead with dilute nitric acid or from processing lead and bismuth waste from lead refineries.

2. Reaction of Lead Nitrate

When solutions of lead nitrate and potassium iodide are mixed, lead(II) iodide forms as a bright yellow precipitate, demonstrating the precipitation reaction. Lead nitrate also forms coordination complexes with electron-donating nitrogen and oxygen ligands. For example, a complex with pentaethylene glycol demonstrates the ability of lead to form extensive coordination structures.

What Is Iron Nitrate?

Iron nitrate is an inorganic compound represented by the formulas Fe(NO₃)₃ (trivalent) and Fe(NO₃)₂ (divalent). The trivalent form is more stable and commonly produced compared to the divalent form.

Uses of Iron Nitrate

1. Iron Nitrate (III)

Iron nitrate (III) is utilized primarily for its solubility in alcohol, making it suitable for reactions with organic compounds. It serves as a starting material in the synthesis of metal catalysts and as a reagent in organic compound reactions, such as the nitration of benzene rings. Additionally, it is employed as a mordant in dyes, silk thickeners, tanning agents, and various analytical reagents.

2. Iron Nitrate (II)

Iron nitrate (II) hexahydrate is less stable and not commonly used, often appearing as a byproduct in the production of iron nitrate (III). Upon heating, it emits nitric oxide and precipitates hydroxide salts, enabling the production of iron nitrate (III).

Properties of Iron Nitrate

1. Iron Nitrate (III)

Iron nitrate (III) appears as a light purple solid at room temperature, with a molecular weight of 241.86 g/mol, a melting point of 47.2°C, and a specific gravity of 1.68. It decomposes at 125°C, is soluble in water and alcohols, and has a CAS number of 10421-48-4. The nonahydrate form absorbs moisture from the air, turning into a brown liquid due to its hygroscopic nature. Upon heating, it decomposes to iron oxide (Fe₂O₃).

2. Iron Nitrate (II)

The hexahydrate form of iron nitrate (II) is green, with a molecular weight of 287.95 g/mol, a melting point of 60.5°C, and a CAS number of 14013-86-6. It dissolves easily in water and displays acidity in aqueous solution. At temperatures below -12℃, it can precipitate as a nonahydrate.

Other Information on Iron Nitrate

1. Production Process of Iron Nitrate (III)

Iron nitrate (III) is synthesized by dissolving iron in nitric acid, resulting in either a hexahydrate or nonahydrate form depending on the concentration of the solution. The hexahydrate can be converted to the nonahydrate by treatment with fuming nitric acid or anhydrous nitric acid.

2. Production Method of Iron Nitrate (II)

Iron nitrate (II) is produced through the double decomposition of iron nitrate (II) with nitric acid or barium nitrate, or by reducing iron nitrate (III) with silver, typically resulting in a light green hexahydrate that turns dark red under dry conditions.

3. Hazards of Iron Nitrate

Both divalent and trivalent forms of iron nitrate are oxidizing and can cause irritation; hence, protective gear such as rubber gloves, safety glasses, and a lab coat are recommended during handling. Iron nitrate (II) is especially sensitive to air and should be kept in a saturated solution to avoid decomposition.

What Is Zinc Nitrate?

Zinc nitrate is an inorganic compound with the chemical formula Zn(NO₃)₂. It commonly exists as a hexahydrate (Zn(NO₃)₂·6H₂O) and less frequently as an anhydrous form or a tetrahydrate (Zn(NO₃)₂·4H₂O).

The CAS registry numbers are as follows: anhydrous form 7779-88-6, tetrahydrate form 9154-63-3, and hexahydrate form 10196-18-6.

Uses of Zinc Nitrate

Zinc nitrate is used in various applications, including as a raw material in pharmaceuticals, a mordant in dyeing processes, and a catalyst in resin processing. It also serves as an analytical reagent, a metal surface treatment agent, and in rechargeable batteries. While zinc nitrate is nonflammable, it can cause combustible materials to ignite and is hazardous to human health.

Properties of Zinc Nitrate

1. Basic Information on Zinc Nitrate (Anhydrous)

The anhydrous form of zinc nitrate has a molecular weight of 189.36, melts at 110°C, and appears as colorless crystals at room temperature. It reacts violently with flammable substances, metal sulfides, and reducing agents, and is deliquescent.

2. Basic Information on Zinc Nitrate (Hexahydrate)

The hexahydrate form has a molecular weight of 297.49, a melting point of 36.4°C, a decomposition boiling point of 105°C, and appears as colorless flaky crystals at room temperature. It is highly soluble in water and ethanol but not in ether, with a water solubility of 184.3g/100mL at 20°C, and a density of 2.065g/mL.

Types of Zinc Nitrate

Zinc nitrate is primarily sold as a hexahydrate for both research and industrial use.

1. Reagent Products for Research and Development

For research and development, zinc nitrate is available in convenient sizes such as 10g, 25g, and 500g, often requiring refrigerated storage. It is used in methods like plasma emission spectrometry and atomic absorption spectrometry to quantify impurity metal ions.

2. Industrial Chemicals

As an industrial chemical, it is supplied in larger quantities, such as 20 kg PE bags and 25 kg paper bags, and is available in both solution and crystalline forms. Its versatility as an analytical reagent, metal surface treatment agent, catalyst in resin processing, and mordant makes it widely available from several manufacturers.

Other Information on Zinc Nitrate

1. Synthesis of Zinc Nitrate

Zinc nitrate can be synthesized by reacting zinc or zinc oxide with nitric acid. The anhydrous form can also be produced by reacting zinc chloride with nitrogen dioxide.

2. Hazards of Zinc Nitrate and Regulatory Information

Although nonflammable, zinc nitrate is an oxidizing agent that can contribute to fires. Hazardous decomposition products include nitrogen oxides and zinc oxides. Ingestion can lead to symptoms like stomach cramps and cyanosis. It may also cause skin and eye irritation, and respiratory irritation. Zinc nitrate is regulated under various laws due to its hazards. Proper handling in compliance with these regulations is essential.

What Is Lithium Nitrate?

Lithium nitrate is an inorganic compound that appears as a white crystalline or powdered solid. It is chemically represented as LiNO3, with a molecular weight of 68.95 and a CAS registration number of 7790-69-4.

This compound has a melting point of 264°C (507°F) and is highly soluble in water, with slight solubility in ethanol.

As a safety classification, lithium nitrate is categorized as a Category 3 oxidizing solid.

Uses of Lithium Nitrate

In the industrial sector, lithium nitrate is utilized as a raw material in the manufacturing of fireworks, and ceramic products, and for its heat transfer properties in various applications.

It also serves as a valuable source of lithium ions in analytical chemistry and is used in experimental settings, including as an oxidant in sample preparation for X-ray fluorescence analysis and battery research.

Moreover, lithium nitrate is being explored for its potential to enhance the performance of lithium-ion batteries, which are increasingly important for electric vehicles and other emerging technologies.

What Is Magnesium Nitrate?

Magnesium nitrate is a chemical compound with the formula Mg(NO₃)₂. It is commonly available as magnesium nitrate hexahydrate, a colorless or white deliquescent crystal.

This compound is produced via the neutralization method, where magnesium nitrate reacts with magnesium oxide. The resulting aqueous solution is cooled and precipitated as magnesium nitrate hexahydrate.

The melting point of magnesium nitrate hexahydrate is 88.9°C. It is crucial to store and use magnesium nitrate hexahydrate at or below this temperature to prevent it from converting to basic magnesium nitrate above 88.9°C.

Uses of Magnesium Nitrate

1. Fertilizer

Magnesium nitrate serves as an essential fertilizer for plants, providing magnesium, a critical component of chlorophyll necessary for photosynthesis. Its water solubility ensures rapid absorption by plants, offering an immediate effect. However, its solubility can also lead to loss during heavy rainfall.

2. Raw Material for Gunpowder

As a raw material for gunpowder, magnesium nitrate acts as an oxidizer, releasing oxygen during combustion to support the burning of other fuels, thereby enhancing the explosive power and speed of gunpowder.

3. Manufacture of Fireworks

In fireworks manufacturing, magnesium nitrate contributes to the bright white light emitted by magnesium when it burns, adding to the visual appeal of fireworks displays.

4. Other Uses

Additional applications include its role as a dehydrating agent for concentrated nitric acid and as a precursor for various magnesium chemicals.

Properties of Magnesium Nitrate

Magnesium nitrate hexahydrate is a white crystalline solid that dissolves in water (233g/100g at 0°C), with its aqueous solution being alkaline. It is also soluble in organic solvents like ethanol and methanol, as well as in dilute nitric acid, but not in aqueous alkaline solutions.

Despite its high affinity for water, magnesium nitrate hexahydrate does not dehydrate when heated but decomposes into magnesium oxide, oxygen, and nitrogen oxides:

4Mg(NO₃)₂・6H₂O + heat → 4MgO + 2NO₂ + 2N₂O + O₂ + 6H₂O

Other Information on Magnesium Nitrate

1. Production Methods

Industrial magnesium nitrate is synthesized through various reactions, including:

• 2HNO₃ + Mg → Mg(NO₃)₂ + H₂
• 2HNO₃ + MgO → Mg(NO₃)₂ + H₂O
• Mg(OH)₂ + 2NH₄NO₃ → Mg(NO₃)₂ + 2NH₃ + 2H₂O

2. Safety Information

Magnesium nitrate is a strong oxidizer, and its reaction with flammable or reducing substances may lead to fire or explosion. Special care is required when handling magnesium nitrate, including the use of protective gear such as masks, goggles, and gloves. Store in an airtight container to prevent moisture absorption and avoid contact with combustible materials.

In case of skin contact, wash with soap and water. If magnesium nitrate enters the eyes, rinse thoroughly with water. Seek medical attention immediately if inhaled or ingested.

What Is Barium Nitrate?

Barium nitrate, also known as barium dinitrate or barium bisnitrate, is a nitrate of barium. It is represented by the chemical formula Ba(NO₃)₂ and has a molecular weight of 261.34 g/mol. It is assigned the CAS registration number 10022-31-8, a unique identifier for chemical substances.

At room temperature and pressure, barium nitrate exists as a white crystal or crystalline powder and is odorless. Its solubility in water is 90 g/L at 20°C, but it is almost insoluble in ethanol and acetone.

Uses of Barium Nitrate

Barium nitrate is a relatively stable oxidizing agent, used in manufacturing carlit, pyrotechnics (fireworks, smoke bombs, etc.), optical glass, glazes, pharmaceuticals, rubber chemicals, and many other fields. Carlit, an explosive composed mainly of ammonium perchlorate, was invented overseas and patented in 1918. It has been utilized in a wide range of fields, including civil engineering.

Optical glass, primarily made from silica stone and silica sand, contains very few impurities that impair transparency, making it ideal for optical elements that transmit light, such as lenses, prisms, optical filters, and detector window plates, as well as for light propagation, such as light guides. They are also used as qualitative analysis samples to determine the substances contained in a sample.

Pyrotechnics, known as processed gunpowder and explosives, are widely used in space exploration, including fireworks, airbags in automobiles, and rockets. 

Properties of Barium Nitrate

Barium nitrate is classified under various safety laws. Although barium nitrate itself is noncombustible, it can ignite and burn violently when mixed with combustibles and must be handled with care. It is a strong oxidizer, reacting with combustible and reducing substances. When heated, it decomposes, producing nitrogen oxides, which can react with metal powders, posing a fire and explosion hazard.

Other Information on Barium Nitrate

1. Regulatory Information on Barium Nitrate

Barium nitrate is classified under various safety laws as hazardous material, dramatic, and oxidizing substances.

2. Handling and Storage Precautions

When handling or storing barium nitrate, adhere to the following precautions:

• Store outdoors or in a well-ventilated area.
• Avoid mixing with oxidizing agents, reducing agents, and combustibles.
• Store in a cool, dark place away from direct sunlight.
• Use sealed apparatus, equipment, or local ventilation in areas where dust is generated.

3. Manufacturing Process of Barium Nitrate

Barium nitrate is produced using various methods:

• Reaction of acid and base, e.g., 2HNO₃ + Ba(OH)₂ → Ba(NO₃)₂ + 2H₂O
• Reaction of a base with an acidic oxide, e.g., Ba(OH)₂ + N₂O₅ → Ba(NO₃)₂ + H₂O
• Reaction of basic oxides with acidic oxides, e.g., BaO + 2HNO₃ → Ba(NO₃)₂ + H₂O; BaO + N₂O₅ → Ba(NO₃)₂
• Reaction of weak salts with strong acids, e.g., BaF₂ + 2HNO₃ → Ba(NO₃)₂ + 2HF
• Reaction of a weak base salt with a strong base, e.g., Sn(NO₃)₂ + Ba(OH)₂ → Ba(NO₃)₂ + Sn(OH)₂
• Reaction of an active metal with an acid, e.g., Ba + 2HNO₃ → Ba(NO₃)₂ + H₂

What Is Nickel Nitrate?

Nickel nitrate is a chemical compound with the formula Ni(NO₃)₂, known for its use in various industrial applications. It exists both in an anhydrous form and more commonly as a hexahydrate Ni(NO₃)₂・6H₂O, with significant potential hazards including fire risk and health effects such as irritation, allergies, and possible carcinogenicity.

Uses of Nickel Nitrate

Nickel nitrate plays a crucial role in manufacturing alkaline and nickel-hydrogen rechargeable batteries, serving as a catalyst, a metal surface treatment agent, and a pigment base for ceramics. Its applications extend to secondary batteries, including nickel-cadmium and nickel-metal hydride batteries, and it is utilized in plating, polymerization catalysts for synthetic resins and fibers, and as a coloring agent for various materials.

Properties of Nickel Nitrate

The anhydrous form of nickel nitrate presents as pale greenish-yellow crystals, with significant solubility in water. The hexahydrate form, a light green crystal, exhibits high water solubility and is also soluble in ethanol but not in ether. Upon heating, it transitions through various stages of hydration to eventually form nickel oxide.

Types of Nickel Nitrate

Available mainly for research and industrial uses, nickel nitrate is typically sold in the hexahydrate form. It comes in various quantities for laboratory research and larger scales for industrial applications, emphasizing the need for careful handling due to its solubility characteristics and potential hazards.

Other Information on Nickel Nitrate

Synthesis of nickel nitrate involves the reaction of nickel oxide or hydroxide with nitric acid, predominantly producing the hexahydrate form. Its reactivity profile underscores its oxidizing nature, highlighting precautions against violent reactions with combustibles and the generation of toxic decomposition products in fire conditions.

What Is Sodium Nitrate?

Sodium nitrate is the sodium salt of nitric acid, naturally found as Chilean nitrate and primarily extracted from the Pacific coast of South America, including Chile. It is also produced by companies like Ube Industries and Nissan Chemical, with imports from Chile, Korea, and China.

Under various laws, sodium nitrate is classified as an oxidizing substance and a hazardous material due to its oxidizing properties.

Uses of Sodium Nitrate

As a food additive, sodium nitrate is used in cheese and sake fermentation and as a meat colorant, though its use is regulated due to potential carcinogenic effects. It serves as a fast-acting nitrogen fertilizer, a defoaming agent in glass manufacturing, and gunpowder, dyes, and flame retardants. Additionally, it’s used in producing other salts and as a thermal storage medium in solar power generation.

Properties of Sodium Nitrate

Sodium nitrate appears as colorless crystals, melting at 308°C, and exhibits deliquescence. It dissolves well in hot water, with solubility decreasing at lower temperatures, and shows slight solubility in methanol but is almost insoluble in ethanol. Its role in processed meats has been linked to the formation of carcinogenic nitrosamines.

Structure of Sodium Nitrate

The chemical formula for sodium nitrate is NaNO₃, with a tricrystalline structure, a formula weight of 84.99 g/mol, and a density of 2.3 g/cm³.

Other Information on Sodium Nitrate

1. Production of Sodium Nitrate

Historically sourced from the Atacama Desert in Chile, sodium nitrate was primarily mined until the Haber-Bosch process reduced the demand for natural sources. Chile continues to have significant reserves, with mining operations yielding sodium nitrate among other minerals.

2. Synthesis of Sodium Nitrate

Industrially, sodium nitrate is produced by reacting sodium carbonate, bicarbonate, or hydroxide with nitric acid or by mixing these sodium compounds with ammonium nitrate.

3. Reaction of Sodium Nitrate

Reactions involving sodium nitrate can produce nitric acid or sodium nitrate through interactions with sulfuric acid or silver nitrate, respectively.

4. Dangers of Sodium Nitrate

Studies have linked nitrates to various health issues, including diabetes, Alzheimer’s, Parkinson’s, stomach, and esophageal cancer, primarily due to the formation of carcinogenic nitrosamines from nitrate and nitrite in processed meats.

What Is Cerium Carbonate?

Cerium carbonate is a compound where cerium can be either in a trivalent or tetravalent oxidation state.

Uses of Cerium Carbonate

1. Luminous Materials

Cerium carbonate was historically used in gas mantles for its luminescent properties. Today, it finds use in the light-emitting components of lanterns for outdoor activities.

2. Organic Synthesis Reaction Reagent

Ceric ammonium nitrate (CAN), a powerful oxidizing agent in organic synthesis, is often used in stoichiometric amounts and combination with sodium bromate for oxidation reactions.

3. Other Uses

Cerium carbonate(III) hexahydrate is used as an anti-tarnish agent for pigments, and in etching processes for the manufacturing of liquid crystal displays.

Properties of Cerium Carbonate

1. Cerium Carbonate

The chemical formula of cerium carbonate is Ce2(CO3)3 for its trivalent form, with a molecular weight that varies depending on its hydration state.

2. Cerium Carbonate(III) Hexahydrate

Cerium carbonate(III) hexahydrate, with the chemical formula CeH12N3O15, has a molecular weight of 434.22. It is a colorless to white, hygroscopic crystalline powder, soluble in water, alcohol, and acetone.

Types of Cerium Carbonate

In addition to its trivalent form, cerium carbonate also exists in a tetravalent state in aqueous solutions or as complex salts.

Other Information on Cerium Carbonate

1. Regulatory Information

Cerium carbonate(III) hexahydrate is classified under various national laws and regulations concerning hazardous materials and environmental protection.

2. Precautions for Handling and Storage

When handling cerium carbonate(III) hexahydrate, wear protective gloves, work clothes, and glasses to avoid contact with skin and eyes. Store in a cool, well-ventilated place, away from direct sunlight and moisture.

What Is Strontium Nitrate?

Strontium nitrate is an inorganic compound with the formula Sr(NO₃)₂ and CAS number 10042-76-9. It is notable for its oxygen-releasing properties when heated, making it a potential oxidizing agent that requires careful storage due to its ability to ignite reducing substances.

Uses of Strontium Nitrate

Strontium nitrate is extensively used in the manufacture of fireworks, phosphors, optical glass, flares, reagents, gunpowder, explosives, LCD/OLED glass, optical glass, ceramics, igniters, and in applications requiring a deep red flame coloration. It also finds application in inorganic chemical products, pharmaceuticals, and as a gas-generating agent in automotive airbags.

Properties of Strontium Nitrate

This white crystalline powder has a formula weight of 211.43, melts at 570°C, and boils at 645°C. Highly soluble in water (40 g/100 g at 0°C) and ammonia, it is insoluble in ethanol, acetone, and ether. The anhydrous form crystallizes in the cubic system, while the tetrahydrate in the monoclinic system.

Types of Strontium Nitrate

Available mainly for research and industrial use, strontium nitrate is sold in various quantities suitable for laboratory and industrial applications, typically stored at room temperature.

Other Information on Strontium Nitrate

1. Synthesis

It can be synthesized via the neutralization of strontium hydroxide, carbonate, or oxide with nitric acid. Concentrating the aqueous solution yields tetrahydrate strontium nitrate below 29.3°C.

2. Reactivity

Upon decomposition, it releases oxygen and nitrogen dioxide, forming strontium oxide, and is stable under normal conditions but hazardous with flammable materials.

3. Hazardousness and Regulatory Information

As an oxidizing solid, it poses risks of corrosion and irritation to skin and eyes, necessitating strict handling precautions, including the use of protective gear and avoiding contact with heat and flammable materials. It is regulated under multiple safety laws, emphasizing its hazardous nature.