月: 2023年7月

What Is Isobutyl Vinyl Ether?

Isobutyl vinyl ether is an organic compound with the chemical formula C6H12O and contains an ether bond.

It is also known as 1-etheneoxy-2-methylpropane, isobutoxyethene, vinyl isobutyl ether, etc. The CAS number is 109-53-5.

It has a molecular weight of 100.16, a melting point of -132°C, and a boiling point of 83°C. It is a clear, colorless liquid at room temperature. It is characterized by a sweet aroma characteristic of ethers. It has a density of 0.77 g/mL and is virtually insoluble in water. It is soluble in ether, benzene, acetone, and alcohol.

Uses of Isobutyl Vinyl Ether

Isobutyl vinyl ether is a substance used primarily as an organic synthetic raw material. Its products are used in a variety of fields, including pharmaceuticals, plasticizers, and corrosion inhibitors.

Polymers produced by polymerization are also used in industrial applications. Homopolymers are used in adhesives, paints, varnishes, lubricants, greases, and elastomers. Copolymers with copolymerization components such as olefins, siloxanes, and diisocyanates are used in applications such as adhesives, coatings, textile finishing agents, and lubricant additives. They impart affinity, hydrophilicity, plasticity, etc., and improve workability, dyeability, strength, flexibility, transparency, luster, etc.

Copolymers with vinyl chloride are often used in paint resins, which are used in a wide range of applications, including ships, anti-corrosion, stone and concrete, and polyolefins. Otherwise, copolymers with allyl vinyl ether and ternary copolymers with methyl acrylate and acrylonitrile are also commercially available and used.

Properties of Isobutyl Vinyl Ether

Isobutyl vinyl ether contains an olefinic structure in its molecule and may polymerize under the influence of heat, light, or other agents, or when in contact with initiators of polymerization, such as peroxides.

Although stable against alkalis, they are subject to hydrolysis by acids and polymerization reactions in the presence of Lewis acids. When reacting with alcohols under acidic conditions, acetals are produced.

The flash point is as low as -15°C, and the spontaneous combustion point is 195°C. When stored, it should be avoided under conditions of heat, sparks, open flames, electrostatic discharge, and light, and it should be avoided in contact with oxidizing agents.

Types of Isobutyl Vinyl Ether

Isobutyl vinyl Ether is sold as an industrial chemical and R&D reagent product. As a reagent product for research and development, it is offered in a variety of capacities, including 5mL, 25mL, 250mL, 500mL, 5g, and 25g. These reagent products are stored at room temperature or refrigerated and are handled differently by different manufacturers. It may contain trihexylamine as a stabilizer.

For industrial use, it is available in different types of capacities such as 100 g, 1 kg, 25 kg, 150 kg, etc., and is supplied in drums. Industrial applications are mainly organic synthetic raw materials and coating agents.

Other Information on Isobutyl Vinyl Ether

1. Synthesis of Isobutyl Vinyl Ether

Isobutyl vinyl ether can be synthesized by the REPPE reaction of isobutanol and acetylene.

2. Handling and Regulatory Information for Isobutyl Vinyl Ether

As mentioned above, isobutyl vinyl ether has a low flash point and is highly flammable. 

In addition to keeping the product away from naked flames and other sources of fire, it is necessary to take measures such as using explosion-proof electrical equipment, ventilation equipment, and lighting equipment. The substance is also known to be a skin and eye irritant. It should be handled using appropriate protective equipment such as protective gloves and protective eyewear.

What Is Oxalic Acid Dihydrate?

Oxalic acid dihydrate is an organic compound represented by C2H2O4-2H2O.

The CAS number is 6153-56-6. It has a molecular weight of 126.07 and a melting point of 104-106°C. It is a white crystal or crystalline powder at room temperature. The compound is soluble in water and ethanol and insoluble in diethyl ether.

Oxalic acid dihydrate is hygroscopic, and therefore, when left in moist air, it will assume the dihydrate state. Dihydrate also precipitates from aqueous solutions.

Uses of Oxalic Acid Dihydrate

Oxalic acid dihydrate is mainly used in the chemical field as a reagent, metal surface treatment agent, reducing agent, and intermediate raw material for pharmaceuticals. Specific examples are the production of persistent sulfa drugs, cerium oxalate, amino acid preparations, and alpha-keto acids. Due to its reducing properties, it can also be used in reductive titrations.

The compound is also approved as a food additive. However, when used as a food additive, the oxalic acid must be removed from the final product. Examples include the manufacture of glucose syrup and the refining of vegetable oils.

Other uses include raw materials for dyes and bleaching agents, and it is widely used.

Characteristics of Oxalic Acid Dihydrate

Oxalic acid dihydrate becomes anhydrous when placed in a desiccator containing diphosphorus pentoxide or heated to 100°C. It has two carboxyl groups. It is a divalent carboxylic acid with two carboxyl groups and acts as an ionized acid in an aqueous solution.

The acid dissociation constants pKa are 1.27 and 4.27. Because of its property as a reducing agent, it is used as a primary standard in redox titration in analytical chemistry.

Types of Oxalic Acid Dihydrate

Oxalic acid dihydrate is mainly available as a reagent for research and development and as an industrial chemical. R&D reagents are available in 25g, 100g, 500g, 2.5kg, etc., and are supplied in volumes that are easy to handle in the laboratory. These reagent products can be stored at room temperature.

As industrial chemicals, they are available in large capacities that are easy to handle in factories, such as 20 kg. Main applications include metal surface treatment agents and raw materials for pharmaceutical intermediates.

Other Information on Hydroperoxides

1. Production and Synthesis of Oxalic Acid Dihydrate

Oxalic acid is abundantly contained in plants, and is the origin of its naming. Industrially, it is produced by extracting wood chips after treating them with alkali.

Oxalic acid dihydrate is hygroscopic and becomes dihydrate when left in moist air. It also precipitates from aqueous solution in the dihydrate state.

Typical synthesis methods are as follows:

• Sodium oxalate is synthesized by thermal decomposition of sodium formate, isolated as calcium oxalate using calcium hydroxide, and then decomposed with sulfuric acid.
• Method of oxidizing ethylene glycol and glyoxal with potassium dichromate, etc.

2. Oxalic Acid and Health

Oxalic acid has the property (deleterious) of strongly binding to calcium ions. When it enters the bloodstream of a living body, it is believed to form oxalates with calcium, reducing the amount of calcium available to the body and inhibiting the coagulation and coagulation action of blood. The substance is also thought to cause some stones if taken in excess.

Some vegetables, such as spinach and ginger, contain oxalic acid, but it is water soluble and can be reduced by boiling in cooking. In addition, when taken with calcium at the same time, oxalic acid combines with calcium in the intestines to form oxalates, which are less likely to be absorbed by the body.

What Is Calcium Oxalate?

Calcium oxalate is the oxalate of calcium.

It is found in plants and also occurs as an intermediate in the production of oxalic acid. At room temperature, it is a colorless needle-like crystal that is virtually insoluble in water.

It exists not only in anhydrous form but also in monohydrate and dihydrate (weddellite) forms. In plants, it is found in rhubarb leaves, yams, taros, capsicum, untreated konjac, and unripe pineapple.

In high concentrations, it causes skin irritation and a strong gustatory taste, and is toxic to the human body.

Uses of Calcium Oxalate

Calcium oxalate alone is used as a standard solution for qualitative and quantitative analysis of calcium and oxalate ions, as a glaze for ceramics, and in other applications. Calcium oxalate is generated as an intermediate in the production of oxalic acid.

When sulfuric acid is added to calcium oxalate, calcium sulfate precipitates and the oxalate ion is released. Calcium oxalate crystals precipitate when calcium sulfate is removed by filtration and the filtrate is evaporated.

Characteristics of Calcium Oxalate

Calcium oxalate is the oxalate of calcium and has the chemical formula CaC2O4. It can form monohydrate or dihydrate by coordination bonding with water.

Some laboratory reagents are sold in the monohydrate state, so it is necessary to check the labeling when using calcium oxalate in experiments. When calcium oxalate hydrate is heated to 200°C, it loses its crystalline species and becomes anhydrous.

The basic properties of calcium oxalate (molecular weight, specific gravity, and solubility) are as follows:

• Molecular weight: 146.11
• Density: 2.2 g/cm3
• Solubility: Almost insoluble in water and ethanol. Soluble in dilute hydrochloric acid and dilute sulfuric acid.

Other Information on Calcium Oxalate

1. Toxicity to Humans

Calcium oxalate is highly irritating and corrosive to skin and mucous membranes. Wear protective equipment, such as nitrile gloves and protective glasses, to prevent contact with hands and eyes.

If calcium oxalate adheres to the skin, wash thoroughly with soap while rinsing under running water. Soap is used because the solubility of calcium oxalate is increased by raising the pH level, making it easier to wash off.

If it gets into the eye, wash the eye with running water with the face on the side so that the crystals of calcium oxalate can easily flow out of the eye. At this time, spread the eyelids with your fingers and move the eyeballs slowly while washing well behind the eyelids. If irritation persists in the eyes, medical attention is required. 

2. Regulation as a Deleterious Substance

Calcium oxalate is a skin irritant and is therefore designated as a “deleterious substance.” 

3. Calcium Oxalate in Food

Calcium oxalate is also found in foods because it accumulates as a secondary metabolite in plants. Spinach, yams, and black tea are particularly rich in calcium oxalate.

Eating yam may cause itchy lips, because the calcium oxalate in the yam irritates the mucous membranes of the lips. Untreated konjak yam has even higher calcium oxalate content, so it is treated with strong alkali before being crushed, mixed, and coagulated into the food “konjac.”

Touching a raw konnyaku potato with bare hands can cause irritation due to the calcium oxalate and may require hospital treatment. Some wild plants that grow in the mountains and fields also contain large amounts of calcium oxalate, such as the tenkansho plant, which grows wild.

It is important for risk management to know the forms of these plants from an illustrated book so that you do not accidentally touch them with your bare hands when camping or climbing mountains.

4. Urinary Tract Stones

Calcium oxalate ingested from food is hardly excreted in urine because it is almost insoluble in water, and gradually accumulates in the body. Calcium oxalate in the body is deposited as crystals in the kidneys and urinary tract.

5. Decomposition by Heating

Calcium oxalate itself is nonflammable, but decomposition occurs when heated or exposed to strong oxidizing agents. Since toxic carbon monoxide is produced as a decomposition product, care must be taken to avoid inadvertent contact of calcium oxalate with heating elements or oxidizing agents.

What Is Nitrogen Oxide?

Nitrogen oxide is a general term for oxides of nitrogen.

There are different types of nitrogen oxide, ranging from I to V in oxidation number. Examples include nitrogen monoxide (NO), nitrogen dioxide (NO2), nitrogen trioxide (NO3), dinitrogen monoxide (N2O), dinitrogen trioxide (N2O3), dinitrogen tetroxide (N2O4), and dinitrogen pentoxide (N2O5).

Uses of Nitrogen Oxide

Nitrogen oxide is the general term for nitrogen oxides, of which nitrogen monoxide (NO), nitrogen dioxide (NO2), and dinitrogen monoxide (N2O) are the most commonly used.

1. Nitric Oxide

Nitric oxide is used as a bleaching agent in rayon and as a raw material in the manufacture of semiconductors. It is also used as an intermediate in the production of nitric acid.

2. Nitrogen Dioxide

Nitrogen dioxide is used as a dissolving and decomposing agent for analytical samples, as well as a bleaching agent, catalyst, and nitrosating agent for organic machine compounds. It is also used as an oxidizing agent in raw materials for explosives, rocket fuel, and polymerization inhibitors.

Other uses include synthetic raw materials and intermediates for other compounds, such as nitric acid.

3. Dinitrogen Monoxide

Dinitrogen monoxide is widely used for anesthesia in dentistry, surgery, and obstetrics and gynecology. It is also used in industry as a semiconductor material and carrier gas for atomic absorption analysis, as well as for leak detection, refrigerants, and filling balloons and tires with gas.

Characteristics of Nitrogen Oxide

Nitrogen oxide has different characteristics depending on its type. The characteristics of typical types are as follows:

1. Nitric Oxide

It is a colorless gas at room temperature with a melting point of -164°C and a boiling point of -152°C. Its liquid and solid forms are blue. It is immediately oxidized to nitrogen oxide upon contact with air.

Nitric oxide is also produced in the body and is transported to the smooth muscle of arteries. Nitric oxide increases the flexibility of smooth muscle and prevents atherosclerosis.

By keeping blood vessels flexible it prevents fatty deposits in the blood vessels and blood flow from deteriorating.

2. Nitrogen Dioxide

A reddish-brown gas produced when heavy metal nitrates are heated, with a melting point of -9.3°C and a boiling point of 21.3°C. The liquid is yellow, and the solid is colorless. It dissolves in water to form corrosive nitric acid, so moisture must be strictly controlled during storage and use.

It is produced by mixing air (oxygen) with nitrogen monoxide, which is produced by the catalytic oxidation of ammonia.

3. Nitrogen Oxide

Nitrogen oxide is an unstable, dark blue gas. It is produced by the reaction of nitrogen oxide and ozone, and is extremely unstable.

4. Dinitrogen Monoxide

Also called nitrogen oxide, this colorless gas has a melting point of -91°C and a boiling point of -89°C. It is nonflammable and stable. It is a stable, nonflammable gas. It is called laughing gas because it is characterized by its anesthetic and analgesic effects, and when inhaled causes facial muscles to twitch, giving the appearance of laughing.

It is industrially produced by decomposing the raw material, 80% ammonium nitrate solution, in a reaction tank maintained at approximately 250°C by dropping the solution at a constant flow rate, or by directly oxidizing ammonia with a catalyst.

5. Dinitrogen Oxide

A brown gas at room temperature, it has a melting point of -102°C, a boiling point of 3.5°C, and a blue color in liquid and solid form. When dissolved in water, it becomes nitrous acid, which further decomposes into nitric acid, nitric oxide, and water.

6. Dinitrogen Tetroxide

It is a pale yellow gas with a melting point of -9.3°C and a boiling point of 21.2°C. Nitrogen oxide can be cooled to yield dinitrogen tetroxide solid.

7. Dinitrogen Pentoxide

A colorless, deliquescent solid with a melting point of 30°C. It decomposes at 47°C to nitrogen oxide and oxygen, but is stable when stored below 0°C in the dark. It reacts violently with water to form nitric acid.

Other Information on Nitrogen Oxide

Effects of Nitrogen Oxide on the Environment and Living Organisms

Among nitrogen oxides, nitrogen monoxide and nitrogen dioxide have been reduced in terms of air pollution, as they cause photochemical smog and acid rain. Sources of nitrogen oxide include factories, thermal power plants, automobiles, and homes.

Nitrogen in petroleum, coal, and chemical raw materials can be generated by combining with oxygen, or it can be generated by nitrogen in the air reacting with oxygen when exposed to high temperatures. Nitrogen monoxide is gradually oxidized to nitrogen dioxide by oxygen in the air, so that even if nitrogen monoxide is present immediately after generation, most of it is considered to be nitrogen dioxide in the ambient air.

High concentrations of nitrogen oxide will increase the risk of coughing, sputum production, and respiratory illness. Nitrogen oxide also reacts with moisture in the atmosphere to form nitric acid, which, when mixed with rain and snow, causes acid rain.

Furthermore, nitrogen oxide is exposed to ultraviolet light, causing a photochemical reaction that produces photochemical oxidants (Ox). When the concentration of these photochemical oxidants in the atmosphere increases, a white, hazy fog-like condition known as photochemical smog occurs. Photochemical oxidants can cause eye pain, headaches, and nausea.

What Is Sodium Oxide?

Sodium oxide is a compound formed by mixing sodium with an appropriate amount of oxygen in a chemical reaction.

Under normal conditions, sodium oxide exists in the form of white crystals. It is well soluble in water and changes to sodium hydroxide after dissolution. Sodium oxide reacts violently when exposed to water, so it must be stored and handled with care.

Sodium oxide is generally used in the state of sodium hydroxide after reacting with water. 

Uses of Sodium Oxide

Sodium oxide is usually used in the form of sodium hydroxide reacted with water. Sodium hydroxide, also called caustic sodium, is used in a wide range of applications, including synthetic fibers, paper, pulp, chemicals, food industry, and soap.

Otherwise, sodium oxide can absorb carbon dioxide and change to sodium carbonate, or it can be heated in air and change to sodium peroxide. In its stand-alone state, sodium oxide is often used as an ingredient in a variety of compounds.

Properties of Sodium Oxide

Sodium oxide has a melting point of 1,132°C and a decomposition temperature of 1,950°C. When heated above 400°C, sodium oxide decomposes to sodium peroxide (Na2O2) and sodium (Na).

During the weathering of rocks, atmospheric carbon dioxide dissolves into water, which reacts with the sodium oxide in the feldspar contained in the rock, turning it into sodium bicarbonate. Sodium oxide also becomes sodium carbonate when it absorbs carbon dioxide.

Sodium oxide is hygroscopic. Therefore, when sodium oxide is dissolved in water, it reacts violently with water to form sodium hydroxide. When sodium oxide is heated in air, it becomes sodium peroxide.

Structure of Sodium Oxide

Sodium oxide is an inorganic compound that is an oxide of sodium. The chemical formula of sodium oxide is Na2O, its molar mass is 61.979, and its density is 2.27 g/cm3.

Sodium oxide crystals are white crystals belonging to the cubic crystal system. It has an inverted fluorite-type structure, with sodium oxide ions in the position of fluoride ions in calcium fluoride and calcium oxide ions in the position of calcium ions. The lattice constant of sodium oxide is a = 5.55 Å.

Other Information About Sodium Oxide

1. Formation of Sodium Oxide

Sodium oxide can be formed by a chemical reaction involving an appropriate amount of oxygen and sodium. When sodium is heated in excess air, about 20% sodium peroxide is produced as well as sodium oxide.

Relatively pure sodium oxide can be obtained by chemically reacting sodium with sodium hydroxide at 300°C and removing the unreacted sodium using distillation.

In addition, the chemical reaction of liquid sodium with sodium nitrate also produces sodium oxide, along with nitrogen.

2. Other Sodium Oxides

In addition to sodium oxide (Na2O), the composition of sodium oxides includes sodium peroxide (Na2O2) and sodium superoxide (NaO2), both of which contain peroxide ions (O22-).

For example, sodium oxide (Na2O2), also called sodium peroxide, is a yellowish-white granular or powdery substance. Sodium oxide is a strong oxidizing agent that reacts violently with water, breaking it down into hydrogen peroxide and sodium hydroxide. Sodium oxide is therefore also a raw material for the production of hydrogen peroxide.

Sodium superoxide (NaO2), on the other hand, is a superoxide of sodium. It is obtained by reacting sodium oxide with oxygen at high temperature and pressure. Alternatively, sodium superoxide can be obtained by the reaction of an ammonia solution of sodium with oxygen.

Sodium superoxide is easily hydrolyzed to a mixture of sodium peroxide and sodium hydroxide.

What Is Potassium Oxide?

Potassium oxide is a compound obtained by heating potassium nitrate and potassium.

Potassium oxide exists at room temperature in the form of colorless crystals or a gray solid. It is generally used in the state of potassium hydroxide.

Related substances to potassium oxide include potassium, potassium hydroxide, and potassium peroxide.

Uses of Potassium Oxide

Potassium oxide is often used in the form of potassium hydroxide reacted with water. Specifically, potassium hydroxide is used in a wide range of applications, including as a raw material for liquid soap, detergents, and chemical fertilizers, and as an electrolyte in alkaline batteries.

Potassium hydroxide is considered to be a basic compound with strong cleaning properties among raw materials for detergents. It is often used in detergents for professional use because of its particularly strong ability to decompose and dissolve oil stains.

Properties of Potassium Oxide

Potassium oxide decomposes into potassium and potassium peroxide at 350°C. Its density is 2.35 g/cm3. It dissolves well in water, and after dissolution, it changes to potassium hydroxide. Potassium oxide is dangerous because it reacts with water in the air. It is also corrosive.

Potassium Oxide is an oxide of potassium and has the chemical formula K2O. The crystal solid of Potassium Oxide belongs to the cubic crystal system. It has an antifluorite structure, with the potassium oxide ion in the position of the fluoride ion of calcium fluoride and the oxide ion in the position of the calcium ion. The lattice constant of potassium oxide is a = 6.436 Å.

Other Information About Potassium Oxide

1. Formation of Potassium Oxide

Potassium oxide can be synthesized by reacting a small amount of air with potassium metal. Excess unreacted potassium metal can be removed by distillation.

Potassium Oxide can also be obtained by heating potassium metal and potassium nitrate. 

2. Potassium Oxide in Rocks

The composition of a rock is generally indicated in the form of an oxide. It is contained as silicate, such as orthoclase (KAlSi3O8), which has the structure KAlSi3O8. For example, if granite is listed as having a composition of 4.5% K2O, it contains approximately 26.6% orthoclase.

The same is true for potash fertilizers. In other words, the potassium content is converted to K2O even if the ingredient is potassium carbonate or potassium sulfate.

3. Potassium Characteristics

At 350°C, potassium oxide decomposes into potassium, along with potassium peroxide. Potassium is an element with atomic number 19. It is an alkali metal with the element symbol K. It is one of the typical elements and an essential element for living organisms. Potassium oxide is quickly oxidized by air.

4. Characteristics of Potassium Hydroxide

When potassium oxide is placed in water, it generates high heat and potassium hydroxide is formed. Potassium hydroxide is the hydroxide of potassium, and its chemical formula is KOH. It is an ionic crystal composed of hydroxide and potassium ions and is a hard, brittle white solid. Potassium hydroxide is also called caustic potash. 

5. Characteristics of Potassium Oxide

At 350°C, potassium oxide decomposes, along with potassium, into potassium peroxide. Potassium oxide is a peroxide of potassium, also known as potassium peroxide. Its chemical formula is K2O2.

When potassium metal is dissolved in liquid ammonia and oxygen is blown into the dark blue solution at -50°C, the reaction causes the solution to turn colorless and potassium peroxide to form as an orange precipitate.

What Is Thallium Acetate?

Thallium acetate is an odorless, tasteless, white crystalline powder.

Its IUPAC name is thallium(I) acetate, and it is also known as thallium monoacetate or thallous acetate. It is a metal salt with the chemical formula TlC2H3O2 and a molecular weight of 263.43.

Uses of Thallium Acetate

Thallium acetate was used as a depilatory in dermatology and as a cosmetic depilatory cream in the 19th and early 20th centuries. Today, it is strictly controlled as a deleterious substance due to its toxicity.

Current uses include rat poison (expired pesticides), insecticides, pesticides in general (including intermediates), firework dyes, optical materials, and electronic materials. In microbiology, it is also used as an additive for selective cultivation of bacteria.

Thallium acetate was used in ancient times as a rat poison. Rats have a keen sense of smell, and thallium acetate was often used because it is tasteless, odorless, and toxic. Nowadays, rat poison is available in safer materials such as coumarin-based rat poison.

Prussian blue (iron (II) hexacyanoferrate (III)) is used as a remedy in cases where thallium has been ingested by accidental ingestion of rat poison.

Properties of Thallium Acetate

Thallium acetate is solid at room temperature with a melting point of 130°C. It is tidally soluble. It is soluble in water, ethanol, and chloroform, and insoluble in acetone.

Thallium is one of the most toxic elements known as acute and chronic poisons. The effects of exposure are cumulative and symptoms may be delayed for 12 to 24 hours. If inhaled, ingested, or absorbed through the skin, it can be fatal.

The lethal dose in humans by ingestion is about 8 mg per kg of body weight. It is acutely toxic (orally) and toxic for reproduction, and has various hazards, including life-threatening if swallowed, suspected adverse effects on fertility and the fetus, hair (alopecia) disorders, nervous system disorders, nervous system disorders due to long-term or repeated exposure, and toxic to aquatic organisms.

Types of Thallium Acetate

There are two types of thallium acetate depending on the oxidation state: Thallium Acetate (I) and Thallium Acetate (II) (English: Thallium(III) triacetate).

Thallium acetate (II) has the chemical formula TlC6H9O6, molecular weight 381.52, and CAS No. 2570-63-0.

Other Information on Thallium Acetate

1. Production Process of Thallium Acetate

Thallium acetate is synthesized from thallium hydroxide or thallium carbonate and thallium acetate. It can be purified by recrystallization in alcohol after evaporation of the solvent. 

2. Precautions for Handling and Storage

Handling
Avoid contact with strong oxidizers and acids. It is important to use the product in a draft chamber with local exhaust ventilation. Also, wear personal protective equipment when using the product.

In Case of Fire
Thallium acetate is nonflammable and will not itself burn. However, thermal decomposition may produce corrosive and toxic vapors or gases.

Use water spray, foam, powder extinguishing media, carbon dioxide, or dry sand to extinguish fires. Do not use stick spray.

In Case of Skin Contact
It is corrosive and irritating. Care should be taken to prevent adhesion to the skin. Always wear protective clothing, such as a lab coat or work clothes and protective gloves when using the product.

Sleeves of protective clothing should never be rolled up to prevent skin exposure. In the unlikely event of skin contact, wash off with soap and copious amounts of water. If on clothing, remove all contaminated clothing and isolate. It is important to seek medical attention immediately.

In Case of Eye Contact
It is strongly irritating to the eyes. Protective eyewear or goggles must be worn during use as serious injury may occur.

In the unlikely event of eye contact, rinse the eye cautiously with water for several minutes. If you are wearing contacts and can easily remove them, take them off and rinse thoroughly. It is important to always seek medical attention.

Storage
When storing, place in a glass container and keep tightly closed. Store in a cool, well-ventilated place away from direct sunlight. It is also important that the storage unit is always locked.

What Is Sodium Tartrate?

Sodium potassium tartrate is a compound salt consisting of sodium and potassium salts in tartaric acid.

It is also known as Rochelle salt or Seignette salt. In its normal state, it exists as colorless or bluish-white crystals. It is soluble in water but insoluble in alcohol.

Uses of Sodium Tartrate

Sodium tartrate is a compound with a strong piezoelectric effect and high dielectric constant, so it can be used as an oscillator or piezoelectric element, or in microphones and handsets. Industrially, sodium potassium tartrate is synthesized by reacting sodium hydrogen tartrate with an aqueous solution of sodium carbonate.

It is also the main ingredient in other Fehling’s solutions and is registered as a food additive in the EU. It is also used in the pharmaceutical and food industries. Furthermore, because of its mild reducing action, it is used as a reducing agent in the electroless plating of silver, and was used to make mirrors from plate glass in the past.

Properties of Sodium Tartrate

Sodium tartrate has a molar mass of 282.1, a melting point of 75°C, and a boiling point of 220°C. Sodium tartrate crystals dissolve at a relative humidity above about 84% and dehydrate at a relative humidity below about 30%.

Sodium potassium tartrate is a salt of the divalent carboxylic acid tartrate with sodium and potassium. It usually contains four molecules of crystalline water and has the chemical formula KNaC4H4O6-4H2O.

Other Information on Sodium Potassium Tartrate

1. Formation of Sodium Potassium Tartrate

Sodium potassium tartrate can be prepared by adding 0.5 moles of sodium carbonate to a heated solution containing 1 mole of potassium hydrogen tartrate. The solution is filtered while hot and the filtrate is dried, resulting in the precipitation of solid Sodium Tartrate as crystallite.

Experiments have been conducted at Skylab under microgravity and convection conditions to study the growth of Rochelle salt into large crystals. 

2. Chelating Action of Sodium Tartrate

Sodium tartrate has high solubility in water, and in water it ionizes to form tartrate ions with chelating properties. Therefore, sodium tartrate can be widely used as a weakly basic chelating agent.

In organic synthesis, sodium tartrate is used as a post-treatment for reactions using aluminum hydride reagents, such as lithium aluminum hydride (LAH) and diisobutyl aluminum hydride (DIBAL-H). Sodium tartrate can prevent the formation of emulsions and precipitations during aliquot handling due to its chelating action.

It is also used industrially as a component of plating solutions and as a reagent in chemical analyses such as Fehling’s reaction, Biuret test, Nessler reaction, and determination of cadmium. 

3. Piezoelectric Effect of Sodium Tartrate

Single crystals of sodium tartrate will exhibit a high dielectric constant of about 4,000 as a ferroelectric material. On the other hand, it also has a lower Curie temperature limit and does not exhibit ferroelectricity only in the temperature range of 255-297K.

In the past, piezoelectric elements were widely used for crystal microphones and crystal earphones, taking advantage of this feature. Today, however, other materials such as barium titanate (BT) and potassium dihydrogen phosphate (KDP) have been discovered as piezoelectric elements, and the use of moisture-sensitive sodium tartrate is almost non-existent.

What Is Magnesium Peroxide?

Magnesium peroxide is the peroxide of magnesium, also known as magnesium dioxide.

There are several ways to synthesize the anhydrous form of magnesium peroxide: one is to add solid potassium peroxide in a solution of magnesium nitrate and ammonia. Another is to add hydrogen peroxide and alkali to ether or aqueous solutions of magnesium compounds.

Uses of Magnesium Peroxide

Magnesium peroxide is mainly used as an oxidizer, bleach, and disinfectant. Magnesium peroxide is an alkaline earth metal peroxide. As such, it is not as hazardous as alkali metal peroxides, as its reaction with water does not produce large amounts of oxygen.

Peroxides are classified as oxygen bleaches among bleaching agents.
These oxygen bleaches are sometimes used as disinfectants because they are not only bleaching agents but also have bactericidal properties.

What Is Potassium Peroxide?

Potassium peroxide is a peroxide of potassium.

It is generally synthesized by blowing oxygen into metallic potassium dissolved in liquid ammonia at -50°C until the solution turns from dark blue to colorless.

It exists in an orange powder state and is characterized by the generation of oxygen upon heating.

Uses of Potassium Peroxide

Potassium peroxide is mainly used as a bleaching agent, oxidizing agent, and in oxygen-producing gas masks.

Among bleaching agents, it is classified as an oxygen bleach.
Other oxygen bleaches include sodium percarbonate and hydrogen peroxide, which do not bleach dyes and can be used on a relatively wide range of items.

Potassium peroxide, however, is an alkali metal peroxide and is known to generate large amounts of oxygen through an exothermic reaction with water, making it prone to explosions and other problems that require caution.