Adipic Acid In Chemical

Adipic Acid is a mildly toxic, white, crystalline compound. The C6 straight-chain dicarboxylic acid is slightly soluble in water and soluble in alcohol and acetone. Nearly all commercial adipic acid is produced from cyclohexane.

The Adipic acid is an organic compound with the formula C6H10O4. The IUPAC name of this chemical is hexanedioic acid. With the CAS registry number 124-04-9, it is also named as Adipinsaure. The product’s categories are Industrial/Fine Chemicals; alpha,omega-Alkanedicarboxylic Acids; alpha,omega-Bifunctional Alkanes; Monofunctional & alpha,omega-Bifunctional Alkanes. Besides, it is a white crystalline powder, which should be stored in a closed and dry place at temperature of 4 °C.

1. Preparation of Adipic acid

currently adipic acid is produced from a mixture of cyclohexanol and cyclohexanone called “KA oil”, the abbreviation of “ketone-alcohol oil.” The KA oil is oxidized with nitric acid to give adipic acid, via a multistep pathway. Early in the reaction the cyclohexanol is converted to the ketone, releasing nitrous acid:

HOC6H11 + HNO3 → OC6H10 + HNO2 + H2O

Among its many reactions, the cyclohexanone is nitrosated, setting the stage for the scission of the C-C bond:

HNO2 + HNO3 → NO+NO3- + H2O

OC6H10 + NO+ → OC6H9-2-NO + H+

Side products of the method include glutaric and succinic acids.

2. Uses of Adipic acid

the majority of adipic acid is used as monomer for the production of nylon by a polycondensation reaction with hexamethylene diamine forming 6,6-nylon. Other major applications also involve polymers: it is a monomer for production of Polyurethane and its esters are plasticizers, especially in PVC.

Almost 90 percent of adipic acid produced is used in the production of nylon 66. The nylon, which has a protein-like structure, is further processed into fibers for applications in carpeting, automobile tire cord, and clothing. Adipic acid is also used to manufacture plasticizers and lubricant components.

In medicine, adipic acid has been incorporated into controlled-release formulation matrix tablets to obtain pH-independent release for both weakly basic and weakly acidic drugs. It has also been incorporated into the polymeric coating of hydrophilic monolithic systems to modulate the intragel pH, resulting in zero-order release of a hydrophilic drug. The disintegration at intestinal pH of the enteric polymer shellac has been reported to improve when adipic acid was used as a pore-forming agent without affecting release in the acidic media. Other controlled-release formulations have included adipic acid with the intention of obtaining a late-burst release profile. Small but significant amounts of adipic acid are used as a food ingredient as a flavorant and gelling aid. It is used in some calcium carbonate antacids to make them tart.

3. Safety of Adipic acid

Adipic acid, like most carboxylic acids, is a mild skin irritant. It is mildly toxic, with an LD50 of 3600 mg/kg for oral ingestion by rats.

When you are using this chemical, please be cautious about it, This chemical is irritating to eyes.  In case of contact with eyes, rinse immediately with plenty of water and seek medical advice.

Hydrogen peroxide’s Application And Structure

Hydrogen peroxide, With the CAS registry number 7722-84-1,  is also named as Albone. The product’s categories are Oxidative Stress Proteins and Reagents Synthetic Reagents; Cell Stress; Nitric Oxide and Cell Stress; Oxidation; Peroxides; Synthetic Reagents; Peroxides Micro / Nanoelectronics; Electronic Chemicals; Semiconductor Grade Chemicals; Analytical Reagents; Pure Reagents for Wet Digestion (Trace SELECT)Analytical/Chromatography; etc. Besides, it is colourless liquid, which should be stored in a cool, clean, ventilated warehouse at 2-8 °C. it is slightly unstable – will very slowly decompose. And the decomposition is promoted by catalysts and heating. It also reacts with rust, brass, zinc, nickel, finely powdered metals, copper and iron and their alloys. In addition, its molecular formula is H2O2 and molecular weight is 34.01.

Hydrogen peroxide is a combination of hydrogen and oxygen. Its chemical description is H2O2. In high concentrations, it can be unstable and even poisonous. In lower concentrations, such as the types found in many homes, it works well as a disinfectant and antiseptic.

1. Uses of Hydrogen peroxide

This chemical is mainly used for pulp- and paper-bleaching. It can also be used for the manufacture of sodium percarbonate, sodium perborate, certain organic peroxidessuch as dibenzoyl peroxide, epoxides such as propylene oxide. Moreover, it can be used as mild bleaches in laundry detergents. And it has been used as the microetch chemical for copper surface roughening preparation. It can also be also used to oxidize rock matrix in preparation for micro-fossil analysis in the oil and gas exploration industry. Furthermore, it is used as propellant. And it is used as an antiseptic and anti-bacterial agent in iatrology.

Hydrogen peroxide has many other uses as well. When diluted, it can be used to clean and whiten teeth, and it can be used as a gargle or mouthwash to kill germs in the mouth. It should never be swallowed. The residue from it should be rinsed from the mouth after use.

2. Structure of Hydrogen peroxide

Hydrogen peroxide (H2O2), also known as hydroperoxic acid, is a nonplanar molecule with a (twisted) structure of C2 symmetry. Although chiral (the twist can be left or right-handed), the molecule undergoes rapid racemization, the result of which is that the left and right-handed twist forms cannot be isolated as they can quickly “flip” their handed-ness. The observed anticlinal “skewed” shape is a compromise between two conformers, called syn and anti. If the molecule had the flat shape of the anti conformer, it would minimize steric repulsions. However, if it had the 90° torsion angle of the syn conformer, there would be optimized mixing between the filled p-type orbital of the oxygen (one of the lone pairs) and the LUMO of the vicinal O-H bond. The compromise angle has the lowest energy state. The bond angles can also be affected by hydrogen bonding between molecules. As the molecules in gasses are too far apart for hydrogen bonding, the molecular structure of the gaseous and crystalline forms is different; indeed a wide range of values is seen in crystals containing Hydrogen peroxide.

Although the O−O bond is a single bond, the molecule has a relatively high barrier to rotation, of 29.45 kJ/mol; for comparison, the rotational barrier for ethane is 12.5 kJ/mol. The increased barrier is ascribed to repulsion between nonbonding electrons (lone pairs) of the adjacent oxygen atoms.

3. Safety information of Hydrogen peroxide

When you are using this chemical, please be cautious about it as the following: it may cause fire in contact with combustible material. It also may cause burns. Please keep away from combustible material. Moreover, it is harmful by inhalation and if swallowed. And it is irritating to respiratory system and skin. It is also risk of serious damage to the eyes. In case of contact with eyes, rinse immediately with plenty of water and seek medical advice. Additionally, you should wear suitable protective clothing, gloves and eye/face protection. After contact with skin, wash immediately with plenty of soap-suds. And in case of accident or if you feel unwell, seek medical advice immediately (show the label whenever possible.)

Ethylene glycol’s Uses And Preparation

Ethylene glycol, also known as ethylene glycol, is clear, colorless, syrupy, liquid with sweet taste. It is used as an antifreeze in cooling and heating systems. In organic synthesis, it is used as a protecting group for carbonyl groups. Ethylene glycol is miscible with water, ethanol, acetone, acetic acid, glycerol, pyridine, but difficultly soluble in chloroform, ether, benzene, carbon disulfide, and insoluble in hydrocarbons, chlorinated hydrocarbons, oils, rubber, natural resin. It also can dissolve table salt, zinc chloride, potassium carbonate, potassium chloride, potassium iodide, potassium hydroxide and other inorganic compounds.

1. Uses of Ethylene glycol

Ethylene glycol(CAS.NO:107-21-1) is a chemical commonly used in many commercial and industrial applications including antifreeze and coolant.  Ethylene glycol helps keep your car’s engine from freezing in the winter and acts as a coolant to reduce overheating in the summer. Other important uses of ethylene glycol include heat transfer fluids used as industrial coolants for gas compressors, heating, ventilating, and air-conditioning systems, and ice skating rinks.

Ethylene glycol also is used as a raw material in the production of a wide range of products including polyester fibers for clothes, upholstery, carpet and pillows; fiberglass used in products such as jet skis, bathtubs, and bowling balls; and polyethylene terephthalate resin used in packaging film and bottles.  Many of these products are energy saving and cost efficient as well as recyclable.

Ethylene glycol is used as antifreeze in cooling and heating systems, in hydraulic brake fluids, as an industrial humectant, as an ingredient of electrolytic condensers, as a solvent in the paint and plastics industries, in the formulations of printers’ inks, stamp pad inks, and inks for ballpoint pens, as a softening agent for cellophane, and in the synthesis of safety explosives, plasticizers, synthetic fibers (Terylene, Dacron), and synthetic waxes.

Ethylene glycol is also used to de-ice airport runways and aircraft.

2. Preparation of Ethylene glycol

In industrial, Ethylene glycol can be produced by chlorohydrin method, oxirane hydration and direct ethylene hydration.

1). Chlorohydrin method: Use chlorohydrin as raw material which hydrolyzes in the alkaline medium at 100 °C. It can generate oxirane first, and then hydrolyze to produce Ethylene glycol at pressure of 1.01 MPa.

2). Oxirane hydration: This method has catalytic hydration and direct hydration. The hydration process can be carried out both at atmospheric pressure and under pressure. Ordinary pressure uses a small amount of inorganic acid as catalyst and reacts at 50 ~ 70 °C. The molar ratio of oxirane and water of pressurized hydration is higher in the 1:6 or more, in order to reduce the side effect of generating ether. The reaction temperature is 150 °C and pressure is 147kPa. Ethylene glycol can be obtained by hydration. Now, there is gas-phase catalytic hydration, which uses silver oxide as catalyst, alumina as carrier, and reacts at 150 ~ 240 °C to produce 1,2-ethanediol.

3). Direct ethylene hydration: First, the single-acetate or diacetate can be produced by oxidation from ethylene in the presence of catalyst (such as antimony oxide TeO2, palladium catalyst) in acetic acid solution. Then, Ethylene glycol is obtained by further hydrolysis.

When you are using this chemical, please be cautious about it , Due to the sweet taste of 1,2-ethanediol, children and animals are more inclined to consume large quantities of it than of other poisons. It is harmful if swallowed and it is irritating to eyes. It and its toxic byproducts first affect the central nervous system, then the heart, and finally the kidneys. In case of contact with eyes, please rinse immediately with plenty of water and seek medical advice.

Sodium benzoate As A Compounds

Sodium benzoate has the chemical formula NaC7H5O2; it is a widely used food preservative, with E number E211. It is the sodium salt of benzoic acid and exists in this form when dissolved in water. It can be produced by reacting sodium hydroxide with benzoic acid. Benzoic acid occurs naturally at low levels in cranberries, prunes, greengage plums, cinnamon, ripe cloves, and apples.

Sodium benzoate with the CAS Number 532-32-1. Though benzoic acid is a more effective preservative, it isn’t very soluble in cold water compared to sodium benzoate which dissolves easily in water.

1. Properties of Sodium benzoate

Name:Sodium benzoate

EINECS:208-534-8

Molecular Formula:C7H5NaO2

CAS Registry Number:532-32-1 

InChI:InChI=1/C7H6O2.Na/c8-7(9)6-4-2-1-3-5-6;/h1-5H,(H,8,9);/q;+1/p-1

HS Code:29163100

Appearance:White crystalline powder.

Molecular Weight:144.1

Density:1,44 g/cm3

Boiling Point:249.3 °C at 760 mmHg

Melting Point:>300 °C(lit.)

Flash Point:111.4 °C

Storage Temperature:Store at RT.

Solubility:H2O: 1 M at 20 °C, clear, colorless

Stability:Stable, but may be moisture senstive. Incompatible with strong oxidizing agents, alkalis, mineral acids.

Usage:Food preservative, antiseptic, medicine, tobacco, pharmaceutical preparations, intermediate for manufacture of dyes, rust and mildew inhibitor.

2. Preparation of Sodium benzoate

Sodium benzoate is created by adding benzoic acid to a hot concentrated solution of sodium carbonate until effervescence ceases. The solution is then evaporated, cooled and allowed to crystallize or evaporate to dryness, and then granulated.

3. Uses of Sodium benzoate

Sodium benzoate is a preservative. It is bacteriostatic and fungistatic under acidic conditions. It is used most prevalently in acidic foods such as salad dressings (vinegar), carbonated drinks (carbonic acid), jams and fruit juices (citric acid), pickles (vinegar), and condiments. Besides, it is also used in fireworks as a fuel in whistle mix, a powder which emits a whistling noise when compressed into a tube and ignited.

4. Mechanism of food preservation

The mechanism starts with the absorption of benzoic acid into the cell. If the intracellular pH falls to 5 or lower, the anaerobic fermentation of glucose through phosphofructokinase decreases sharply which inhibits the growth and survival of micro-organisms that cause food spoilage.

 

Sodium formate Application And Production

Sodium formate, HCOONa, is the sodium salt of formic acid, HCOOH. It usually appears as a white deliquescent powder.

The Sodium formate, with the CAS registry number 141-53-7,is also known as Thionyl dichloride. It belongs to the product categories of Salachlor; Formic acid sodium salt. This chemical’s molecular formula is CHNaO2 and molecular weight is 68.01. What’s more,Its systematic name is Sodium formate. It is white crystals,which is stable,incompatible with strong oxidizing agents,strong acids,protect from moisture. Its storage temperature is 2-8°C.The Sodium formate is irritating to eyes, respiratory system and skin. When you use it ,wear suitable protective clothing, gloves and eye/face  protection. In case of contact with eyes, rinse immediately with plenty of water and seek medical advice .

1. Application

Sodium formate is used in several fabric dyeing and printing processes. It is also used as a buffering agent for strong mineral acids to increase their pH, as a food additive (E237), and as a de-iceing agent.

Sodium formate is used:

*As a buffering agent

*In printing processes

*In fabric dyeing industry

*As an animal feed additive

2. Production of Sodium formate

Reacting chloroform with an alcoholic solution of sodium hydroxide produces sodium formate; neutralizeing formatic acid with sodium carbonate also produces Sodium formate. The formular is as following:

CHCl3 + 4NaOH → HCOONa + 3NaCl + 2H2O

by reacting sodium hydroxide with chloral hydrate:

2HCl3(OH)2 + NaOH → CHCl3 + HCOONa + H2O

The latter method is better than the former, since the low aqueous solubility of CHCl3 makes it easier to separate out from the sodium formate solution than the soluble NaCl would be by fractional crystallization.

The commercial way to produce sodium formate is to bsorbing carbon monoxide under pressure in solid sodium hydroxide at 160 °C, showing below:

CO + NaOH → HCOONa

Ferric oxide

Iron oxides are chemical compounds composed of iron and oxygen. All together, there are sixteen known iron oxides and oxyhydroxides. Iron oxides and oxide-hydroxides are widespread in nature, play an important role in many geological and biological processes, and are widely utilized by humans, e.g., as iron ores, pigments, catalysts, in thermite , Hemoglobin. Common rust is a form of iron(III) oxide. Iron oxides are widely used as inexpensive, durable pigments in paints, coatings and colored concretes. Colors commonly available are in the “earthy” end of the yellow/orange/red/brown/black range.

Ferric oxide is one of the most common synonyms of Iron oxides, with the CAS NO. 1309-37-1, it has many synonyms, such as Crystalline ferric oxide, Specular hematite, fe203, Specular red iron oxide, Specularite, Alaska black diamond, Specular jeweler’s rouge, Iron oxide; Ferric oxide red. It is a red crystalline insoluble oxide of iron that occurs as haematite and rust and is made by heating ferrous sulphate: used as a pigment and metal polish.

Ferric oxide red (Fe2O3), also known as iron (III) oxide, is a coloring agent for tablets and capsules and is used in the pharmaceutical industry. Ferric oxide red occurs naturally as hematite ore and rust. Iron oxides are also commonly used in the cosmetics industry. Iron oxides for use in pharmaceutical manufacturing may also be synthetic.

Uses of Ferric oxide: The overwhelming application of Ferric oxide is as the feedstock of the steel and iron industries, e.g. the production of iron, steel, and many alloys.  It is also used to put the final polish on metallic jewelry and lenses, and historically as a cosmetic. Except for these, Ferric oxides are used as pigments in dental composites alongside titanium oxides.

Some Uses of Phosphoric acid

Phosphoric acid, also called orthophosphoric acid,  (H3PO4), the most important oxygen acid of phosphorus, used to make phosphate salts for fertilizers. It is also used in dental cements, in the preparation of albumin derivatives, and in the sugar and textile industries. It serves as an acidic, fruitlike flavouring in food products.

Pure phosphoric acid is a crystalline solid (melting point 42.35° C, or 108.2° F); in less concentrated form it is a colourless syrupy liquid. The crude acid is prepared from phosphate rock, while acid of higher purity is made from white phosphorus.

Phosphoric acid(CAS.NO:7664-38-2) forms three classes of salts corresponding to replacement of one, two, or three hydrogen atoms. Among the important phosphate salts are: sodium dihydrogen phosphate (NaH2PO4), used for control of hydrogen ion concentration (acidity) of solutions; disodium hydrogen phosphate (Na2HPO4), used in water treatment as a precipitant for highly.

1. Food additive

Food-grade phosphoric acid (additive E338) is used to acidify foods and beverages such as various colas, but not without controversy regarding its health effects.  It provides a tangy or sour taste, and being a mass-produced chemical is available cheaply and in large quantities. The low cost and bulk availability is unlike more expensive seasonings that give comparable flavors, such as citric acid which is obtainable from citrus, but usually fermented by Aspergillus niger mold from scrap molasses, waste starch hydrolysates and phosphoric acid. Various phosphates, e.g., monocalcium phosphate, are used as leavening agents.

Phosphoric acid is deliberately added to soft drinks to give them a sharper flavor. It also slows the growth of molds and bacteria, which would otherwise multiply rapidly in the sugary solution.

Almost all of the acidity of soda pop comes from the phosphoric acid and not from the carbonic acid from the dissolved CO2. You can verify this by measuring the pH of fresh and flat soda pop; there’s very little difference.

The phosphoric acid is corrosive, but actually the acid concentration in soda pop is lower than that in orange juice or lemonade.

2. In medicine

Phosphoric acid is used in dentistry and orthodontics as an etching solution, to clean and roughen the surfaces of teeth where dental appliances or fillings will be placed. Phosphoric acid is also an ingredient in over-the-counter anti-nausea medications that also contain high levels of sugar (glucose and fructose). This acid is also used in many teeth whiteners to eliminate plaque that may be on the teeth before application.

3. General Side Effects

When phosphoric acid powders are inhaled or come in contact with skin and other body tissues, it can cause dermatitis, pain, tearing, blurred vision, difficulty swallowing or breathing and gastrointestinal problems. Most of these side effects occur in industrial manufacturing plants where concentrated levels of phosphoric acid are used. The amount of phosphoric acid added to sodas and other foods by comparison is a very small amount.

The uses of Acetic acid

Acetic acid  is a colorless, pungent, water-miscible liquid, C 2  H 4  O 2  , the essential constituent of vinegar, produced by oxidation of acetaldehyde, bacterial action on ethyl alcohol, the reaction of methyl alcohol with carbon monoxide, and other processes: used chiefly in the manufacture of acetate fibers and in the production of numerous esters that are solvents and flavoring agents.

Acetic acid(CAS.NO:64-19-7) is the acid most commonly associated with vinegar. Acetic acid is a two-carbon carboxylic acid. It is the most commercially important organic acid and is used in the manufacture of a broad range of chemical products, such as plastics and insecticides.

1. Used in Food

This clear, colorless acid has a distinctive sour taste, although tasting it is not recommended unless it is clearly labeled as fit for human consumption. It also has a strong, sharp odor which is familiar to many people because it smells like vinegar. Or, rather, vinegar smells like acetic acid. In food preparation, it can be used as a flavoring, with the sharp taste being desirable in some foods, and also as a food preservative. The acid inhibits bacterial growth, keeping food safe from contamination. The historic use of vinegar as a food preservative has created an acquired taste in some cultures for the distinctive tang of vinegar, so foods which no longer require preservation may have some added vinegar for flavor.

2. Industrially Use

Industrially, acetic acid is used in a wide range of processes. It is also used in chemical production and research, in settings where people have need for a weak acid. Like other acids, acetic acid is corrosive for many substances, and it can be involved in a variety of chemical reactions. Acetic acid is used as a solvent, a reagent, a catalyst, and a pesticide. It can be used in the preparation of paints, varnishes, and glazes, and in medical treatment, as for example in the treatment of jellyfish stings.

Most important carboxylic acid (CHCOOH). Pure (“glacial”) acetic acid is a clear, syrupy, corrosive liquid that mixes readily with water. Vinegar is its dilute solution, from fermentation and oxidation (see oxidation-reduction) of natural products. Its salts and esters are acetates. It occurs naturally as a metabolic intermediate in body fluids and plant juices. Industrial production is either synthetic, from acetylene, or biological, from ethanol. Industrial chemicals made from it are used in printing and as plastics, photographic films, textiles, and solvents.

3. Medical Use

Acetic acid is used to treat an outer ear infection (external otitis). It works by stopping the growth of bacteria and fungus. Treating the infection reduces pain and swelling in the ear. Wetness in the ear canal can help bacteria and fungus to grow. This medication may also contain drying ingredients such as glycerin or alcohol. Drying of the ear canal helps to cure the infection.

4. Use as solvent

Glacial acetic acid is an excellent polar protic solvent, as noted above. It is frequently used as a solvent for recrystallization to purify organic compounds. Acetic acid is used as a solvent in the production of terephthalic acid (TPA), the raw material for polyethylene terephthalate (PET). In 2006, about 20% of acetic acid was used for TPA production.

Acetic acid is often used as a solvent for reactions involving carbocations, such as Friedel-Crafts alkylation. For example, one stage in the commercial manufacture of synthetic camphor involves a Wagner-Meerwein rearrangement of camphene to isobornyl acetate; here acetic acid acts both as a solvent and as a nucleophile to trap the rearranged carbocation.

Glacial acetic acid is used in analytical chemistry for the estimation of weakly alkaline substances such as organic amides. Glacial acetic acid is a much weaker base than water, so the amide behaves as a strong base in this medium. It then can be titrated using a solution in glacial acetic acid of a very strong acid, such as perchloric acid.

Sodium chlorite As A Compounds

Sodium chlorite is a salt-based chemical that also features the element chlorine. Sodium chlorite (NaClO2) is a chemical compound used in the manufacturing of paper. It has several practical uses and is very similar to sodium chlorate, a common food additive. Most people interact with sodium chlorite frequently but do not realize it, because the chemical is rarely interacted with in large portions. While not dangerous in small amounts, large doses of sodium chlorite can be dangerous.

Sodium chlorite(CAS.NO:7758-19-2) is the product of three elements: sodium (Na), chlorine (Cl) and oxygen. In each molecule, one sodium atom and one chlorine atom bind with two oxygen atoms. The chemical equation for this composition is NaClO2. It is found in solid form as a white powder and is also water-soluble. Under high heat, it can be explosive.

In its dried state, sodium chlorite (NaClO 2 ) is a white or light yellow-green solid. The greenish tint comes from trace amounts of CdO2 or iron, which are production residuals. Sodium chlorite has a molecular weight of 90.44 and decomposes at about 392°F (200°C). It is generally soluble in water, but its solubility increases as the temperature of the water rises. Sodium chlorite is a powerful oxidizer that will not explode on percussion. The anhydrous salt does not absorb water and is stable for up to ten years.

Sodium chlorite is used for a variety of applications. It is used as a disinfectant and purification chemical for water. It is also employed as a textile-bleaching and water anti-fouling agent. Additionally, it is used in the paper and electronics manufacturing industries as a bleaching agent.

In organic synthesis, sodium chlorite is frequently used as a reagent in the Pinnick oxidation for the oxidation of aldehydes to carboxylic acids. The reaction is usually performed in monosodium phosphate buffered solution in the presence of a chlorine scavenger (usually 2-methyl-2-butene).

Recently, sodium chlorite has been used as an oxidizing agent to convert alkyl furans to the corresponding 4-oxo-2-alkenoic acids in a simple one pot synthesis.

Sodium chlorite, like many oxidizing agents, should be protected from inadvertent contamination by organic materials to avoid the formation of an explosive mixture. The chemical is highly stable in pure form and does not explode on percussive impact (unless organic contaminants are present, e.g. a greasy hammer striking the chemical on an anvil) and will also ignite if combined with a strong reducing agent.

Sodium chlorite is a strong oxidant and can therefore be expected to cause clinical symptoms similar to the well known sodium chlorate: methemoglobinemia, hemolysis, renal failure. A dose of 10-15 grams of sodium chlorate can be lethal.

While sodium chlorite is safe in low dosages, it can be harmful to your health if consumed in dosages larger than half a teaspoon. If this occurs, you should begin drinking water immediately and continue drinking to dilute the chemical. Call Poison Control for step-by-step guidance and, if needed, medical help. Health Science Spirit also recommends added half a teaspoon of soda bicarbonate with every glass drank. You can also consider inducing vomiting after drinking several glasses. Be aware that sodium chlorite can irritate the eyes and should not come in contact with them.

Memantine hydrochloride

Memantine hydrochloride (Mem-ant-een hi-droh-clor-ride) is a medicine which is used in Alzheimer’s disease.

Name:Memantine hydrochloride

EINECS:255-219-6

Molecular Formula:C12H21N.HCl

CAS Registry Number:41100-52-1

InChI:InChI=1S/C12H21N/c1-10-3-9-4-11(2,6-10)8-12(13,5-9)7-10/h9H,3-8,13H2,1-2H3

Appearance:Crystalline Solid

Molecular Weight:179.30184

Boiling Point:239.8 °C at 760 mmHg

Melting Point:292 °C

Flash Point:92.3 °C

Storage Temperature:-20°C Freezer

Solubility:soluble

Usage: Memantine hydrochloride is used as an antiparkinsonian and antispasmodic.

Memantine hydrochloride is not suitable for everyone and some people should never use it. Other people should only use it with special care. It is important that the person prescribing this medicine knows your full medical history.

The following types of medicine may interact with Memantine hydrochloride:

*anticholinergics

*antipsychotics

*barbiturates

*dopaminergics

*NMDA-antagonists

*oral anticoagulants

If you are taking Memantine hydrochloride and one of the above medicines or types of medicines, make sure your prescriber knows about it.