Introduction of 1-Bromopropane

1-Bromopropane with CAS number of 106-94-5 is also named as Bromopropane .It is an organic solvent used for the cleaning of metal surfaces, removal of soldering residues from electronic circuit boards, and as an adhesive solvent. It has quite a potent smell. 1-Bromopropane is an organic solvent used for the cleaning of metal surfaces, removal of soldering residues from electronic circuit boards, and as an adhesive solvent. It has a characteristic hydrocarbon odor.

1. Use of 1-Bromopropane

1-Bromopropane is used as alkylating agents to introduce the alkyl groups to form carbon-carbon bonds in organic synthesis. They are also used as intermediate to form alkylated amines and alkylated metallic compounds. The end products include pharmaceuticals, insecticides, quaternary ammonium compounds, flavours and fragrances.

1-Bromopropane is also used as solvent for industrial cleaning (degreasing, metal processing and finishing, electronics, aerospace and aviation), aerosols, textiles, adhesives , inks and coatings.

2. Properties of 1-Bromopropane

Name:1-Bromopropane

EINECS:203-445-0

Molecular Formula:C3H7Br

CAS Registry Number:106-94-5 

Synonyms:n-Propyl bromide; Bromopropane,98%; 1-bromo-propan; 1-Brompropan; bromo propane; Bromopropane; Brompropan; n-C3H7Br; n-propyl; n-propylbromide(1-bromopropane); Propyl bromide

InChI:InChI=1/C3H7Br/c1-2-3-4/h2-3H2,1H3

HS Code:29033036

Appearance:Colorless transparent liquid

Molecular Weight:122.99

Density:1.353

Boiling Point:71℃

Melting Point:-110℃

Flash Point:-4.5℃

Storage Temperature:Flammables area

Refractive index:1.4326-1.4346

Solubility:2.5 g/L (20 oC)

Stability:Stability Flammable - note low flash point. Incompatible with strong oxidizing agents, strong bases.

Usage:Use is as a solvent, generally for fats, waxes, or resins, or as an intermediate in the synthesis of other compounds.

Chemical Properties: colourless liquid 

General Description: A colorless liquid. Slightly denser than water and slightly soluble in water. Flash point below 75°F. When heated to high temperatures may emit toxic fumes. 

Air & Water Reactions: Highly flammable. Slightly soluble in water. 

Reactivity Profile: Halogenated aliphatic compounds, such as 2-Bromopropane, are moderately or very reactive. Reactivity generally decreases with increased degree of substitution of halogen for hydrogen atoms. Low molecular weight haloalkanes are highly flammable and can react with some metals to form dangerous products. Materials in this group are incompatible with strong oxidizing and reducing agents. Also, they are incompatible with many amines, nitrides, azo/diazo compounds, alkali metals, and epoxides. Emits toxic fumes of bromine when burned. 

Health Hazard: Irritating to the eyes, nose, throat, upper respiratory tract, and skin. 

3. Safety Information of 1-Bromopropane

Hazard Codes: F,T

Risk Statements: 60-11-36/37/38-48/20-63-67

60: May impair fertility

11: Highly Flammable

36/37/38: Irritating to eyes, respiratory system and skin

48/20: Harmful: danger of serious damage to health by prolonged exposure through inhalation

63: Possible risk of harm to the unborn child

67: Vapors may cause drowsiness and dizziness

Safety Statements: 53-45

53: Avoid exposure - obtain special instruction before use

45: In case of accident or if you feel unwell, seek medical advice immediately (show label where possible)

RIDADR: UN 2344 3/PG 2

WGK Germany: 2

F: 8: Photosensitive.

HazardClass: 3

PackingGroup: II

HS Code: 29033036

Sodium pyrophosphate anhydrous

Sodium pyrophosphate anhydrous, also called sodium pyrophosphate, tetrasodium phosphate or TSPP, is a colorless transparent crystalline chemical compound with the formula Na4P2O7. It is a salt composed of pyrophosphate and sodium ions. Toxicity is approximately twice that of table salt when ingested orally. There is also a hydrated form, Na4P2O7 · 10(H2O).

Sodium pyrophosphate anhydrous is White powder or crystal. Melting point 880℃. Density 2.534g/cm3. Soluble in water and insoluble in alcohol. It's aqueous solution is alkaline and stable below 70℃, hydrolyzes into sodium hydrogen phosphate after boiling. Can form complex with alkaline earth metal ion, liable to deliquesce.

It is applied in industries of detergents as detergent auxiliary, paper production to bleach electroplating; In food industry it is used as buffering agent, emulsifier, nutrition ingredients quality improver

Name:Sodium pyrophosphate anhydrous

EINECS:231-767-1

Molecular Formula:Na4P2O7

CAS Registry Number:7722-88-5 

Synonyms:Sodium pyrophosphate; Tetrasodium pyrophosphate; TSPP; Tetra Sodium Pyrophosphate; Tetrasodium Diphosohate

InChI:InChI=1S/H4O7P2/c1-8(2,3)7-9(4,5)6/h(H2,1,2,3)(H2,4,5,6)

Appearance:white crystalline powder or colourless crystals

Molecular Weight:177.975082

Density:2.53

Boiling Point:93.8 °C

Melting Point:880℃

Storage Temperature:Keep tightly closed in a cool place in a tightly closed container.

Solubility:H2O: 0.1 M at 20 °C, clear, colorless

Stability:Stable. Incompatible with strong oxidizing agents.

Usage:The active ingredient is no longer contained in any registered products.

Chemical Properties: white crystalline powder or colourless crystals 

General Description: Odorless, white powder or granules. Mp: 995°C. Density: 2.53 g cm-3. Solubility in water: 3.16 g / 100 mL (cold water); 40.26 g / 100 mL boiling water. Used as a wool de-fatting agent, in bleaching operations, as a food additive. The related substance Tetrasodium pyrophosphate decahydrate (Na4P2O7 0H2O) occurs as colorless transparent crystals. Loses its water when heated to 93.8°C. 

Reactivity Profile: Tetrasodium pyrophosphate is basic. Reacts exothermically with acids. Incompatible with strong oxidizing agents. Decomposes in ethyl alcohol. 

The History of Captopril

Captopril is an oral drug and a member of a class of drugs called angiotensin converting enzyme (ACE) inhibitors. Captopril is used to treat high blood pressure and heart failure. It decreases certain chemicals that tighten the blood vessels, so blood flows more smoothly and the heart can pump blood more efficiently.

Captopril(CAS.NO:62571-86-2) was developed in 1975 by three researchers at the U.S. drug company Squibb (now Bristol-Myers Squibb): Miguel Ondetti, Bernard Rubin and David Cushman. Squibb filed for U.S. patent protection on the drug in February 1976 and U.S. Patent 4,046,889 was granted in September 1977. Captopril gained FDA approval on April 6, 1981. The drug went generic in the U.S. in February 1996 as a result of the end of market exclusivity for Bristol-Myers Squibb.

The development of captopril was amongst the earliest successes of the revolutionary concept of ligand-based drug design. The renin-angiontensin-aldosterone system had been extensively studied in the mid-20th century and it had been decided that this system presented several opportune targets in the development of novel treatments for hypertension. The first two targets that were attempted were renin and ACE. Captopril was the culmination of efforts by Squibb's laboratories to develop an ACE inhibitor.

Ondetti, Cushman and colleagues built on work that had been done in the 1960s by a team of researchers led by John Vane at the Royal College of Surgeons of England. The first breakthrough was made by Kevin K.F. Ng in 1967, when he found the conversion of angiotensin I to angiotensin II took place in the pulmonary circulation instead of in the plasma. In contrast, Sergio Ferreira found bradykinin disappeared in its passage through the pulmonary circulation. The conversion of angiotensin I to angiotensin II and the inactivation of bradykinin were thought to be mediated by the same enzyme.

In 1970, using bradykinin potentiating factor (BPF) provided by Sergio Ferreira, Ng and Vane found the conversion of angiotensin I to angiotensin II was inhibited during its passage through the pulmonary circulation. BPF was later found to be a peptide in the venom of a lancehead viper (Bothrops jararaca), which was a “collected-product inhibitor” of the converting enzyme. Captopril was developed from this peptide after it was found via QSAR-based modification that the terminal sulfhydryl moiety of the peptide provided a high potency of ACE inhibition.

Captopril gained FDA approval on April 6, 1981. The drug became a generic medicine in the U.S. in February 1996, when the market exclusivity held by Bristol-Myers Squibb for captopril expired.

The development of captopril has been claimed as an instance of 'biopiracy' (commercialization of traditional medicines), since no benefits have flowed back to the indigenous Brazilian tribe who first used pit viper venom as an arrowhead poison.

Mercury In Chemical

Mercury is a chemical element with the symbol Hg and atomic number 80. It is commonly known as quicksilver and was formerly named hydrargyrum (from Greek "hydr-" water and "argyros" silver). A heavy, silvery d-block element, mercury is the only metallic element that is liquid at standard conditions for temperature and pressure; the only other element that is liquid under these conditions is bromine, though metals such as caesium, gallium, and rubidium melt just above room temperature.

With the CAS registry number 7439-97-6 and EINECS registry number 231-106-7, this chemical of Mercury is also named as Mercuryelement. In addition, the molecular formula is Hg and the molecular weight is 200.59. It is a kind of silvery liquid metal and belongs to the classes of Metals; Inorganics; Essential Chemicals; Chemical Synthesis; Volumetric Solutions; Analytical Reagents for General Use; Electrochemistry; Trace Analysis Reagents; I-N, Puriss p.a. Metal and Ceramic Science. It is the only one liquid metal at the normal temperature, free exist in nature and exist in the cinnabar, calomel and several other mines.

1. Properties of Mercury

Name:Mercury

EINECS:231-106-7

Molecular Formula:Hg

CAS Registry Number:7439-97-6 

Synonyms:Quicksilver; Mercury metal 99.99+ % for analysis; Mercuryredistilled; Mercury solution 1000 ppm; Mercury solution 10 000 ppm

InChI:InChI=1/Hg

Appearance:silver liquid

Molecular Weight:200.59

Density:13.54

Boiling Point:356.5℃

Melting Point:-38.9℃

Storage Temperature:Poison room

Solubility:insoluble in water

Stability:Stable. Incompatible with strong acids, sodium thiosulfate, ammonium hydroxide.

Chemical Properties :silvery liquid metal 

General Description: An odorless, silvery metallic liquid. Insoluble in water. Toxic by ingestion, absorption and inhalation of the fumes. Corrosive to aluminum. Used as a catalyst in instruments, boilers, mirror coatings. 

Air & Water Reactions: Insoluble in water. 

Reactivity Profile: Mercury forms an explosive acelylide when mixed with acetylene. Can form explosive compounds with ammonia (a residue resulting from such a reaction exploded when an attempt was made to clean Mercury off a steel rod . Chlorine dioxide (also other oxidants, such as: chlorine, bromine, nitric acid, performic acid), and Mercury explode when mixed . Methyl azide in the presence of Mercury is potentially explosive . Ground mixtures of sodium carbide and Mercury can react vigorously . Ammonia forms explosive compounds with gold, Mercury, or silver. 

Health Hazard: No immediate symptoms. As poisoning becomes established, slight muscular tremor, loss of appetite, nausea, and diarrhea are observed. Psychic, kidney, and cardiovascular disturbances may occur. 

Fire Hazard: Behavior in Fire: Not flammable 

2. Preparation of Mercury

It can be purified by maens of electrolysis.The electrolytic process needs electrolytic solution dilute nitric acid. In addition, the electrolysis voltage is 2-3V and the current is 3-4A. 

3. Uses of Mercury

It can be used to make tubes, mercury rectifiers and electrodes in the electronics industry. And it also be used in a variety of gauges and thermometers, polarographic analysis dropping mercury electrode, etc.

4. Toxicity and safety

Mercury and most of its compounds are extremely toxic and must be handled with care; in cases of spills involving mercury (such as from certain thermometers or fluorescent light bulbs), specific cleaning procedures are used to avoid exposure and contain the spill. Protocols call for physically merging smaller droplets on hard surfaces, combining them into a single larger pool for easier removal with an eyedropper, or for gently pushing the spill into a disposable container. Vacuum cleaners and brooms cause greater dispersal of the mercury and should not be used. Afterwards, fine sulfur, zinc, or some other powder that readily forms an amalgam (alloy) with mercury at ordinary temperatures is sprinkled over the area before itself being collected and properly disposed of. Cleaning porous surfaces and clothing is not effective at removing all traces of mercury and it is therefore advised to discard these kinds of items should they be exposed to a mercury spill.

When you are using Mercury, please be cautious about it as the following:

This chemical can cause burns and has danger of cumulative effects. It is irritating to eyes, respiratory system and skin. And it has danger of serious damage to health by prolonged exposure in contact with skin and if swallowed. In addition, it is toxic to aquatic organisms, may cause long-term adverse effects in the aquatic environment. When you are using 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. And in case of accident or if you feel unwell, seek medical advice immediately (show label where possible). This material and its container must be disposed of as hazardous waste. You should keep container tightly closed and avoid release to the environment. At last, you can refer to special instructions safety data sheet.

About Nitric acid

Nitric acid is a colorless, highly corrosive liquid and a very powerful oxidizing agent that in the highly pure state is not entirely stable and must be prepared from its azeotrope by distillation with concentrated sulfuric acid. Nitric acid gradually yellows because of decomposition to nitrogen dioxide. Solutions containing more than 80% nitric acid are called fuming nitric acids. It also can be called Acide nitrique; Acido nitrico; Acidum nitricum; Aqua fortis; Azotic acid; Azotowy kwas; Engraver's acid; Hydrogen nitrate; Kyselina dusicne; Nital; Nitric acid; Nitrous fumes; Nitryl hydroxide; Red fuming nitric acid; Salpetersaeure; Salpetersaure; Salpeterzuuroplossingen; UNII-411VRN1TV4.

1. History

The first mention of nitric acid is in Pseudo-Geber's De Inventione Veritatis, wherein it is obtained by calcining a mixture of niter, alum and blue vitriol. It was again described by Albert the Great in the 13th century and by Ramon Lull, who prepared it by heating niter and clay and called it "eau forte" (aqua fortis).

Glauber devised the process still used today to obtain it, namely by heating niter with strong sulfuric acid. In 1776 Lavoisier showed that it contained oxygen, and in 1785 Henry Cavendish determined its precise composition and showed that it could be synthesized by passing a stream of electric sparks through moist air.

2. Preparation of Nitric acid

Nitric acid is made by reacting nitrogen dioxide (NO2) with water.

3 NO2 + H2O → 2 HNO3 + NO

For many years it was made by the reaction of sulfuric acid and saltpeter, but this method is no longer used.

NaNO3 + H2SO4 → NaHSO4 + HNO3

It is now manufactured by combusting ammonia in air in the presence of a (platinum or other noble metal) catalyst, and the nitrogen oxides thus formed are oxidized further and absorbed in water to form nitric acid.

NH3 + 2O2 → HNO3 + H2O

3. Uses of Nitric acid

1). A solution of Nitric acid and alcohol, Nital, is used for etching of metals to reveal the microstructure.Nitric acid is also used in explosives, and is key to the manufacture of Nitroglycerin and RDX.

2). In a low concentration, it is often used to artificially age pine and maple. The color produced is a grey-gold very much like very old wax or oil finished wood (wood finishing).

4. Safety

Nitric acid(CAS NO.7697-37-2) is a strong acid and a powerful oxidizing agent. The major hazard posed by it is chemical burns as it carries out acid hydrolysis with proteins (amide) and fats (ester) which consequently decomposes living tissue (e.g. skin and flesh). Concentrated nitric acid stains human skin yellow due to its reaction with the keratin. These yellow stains turn orange when neutralized. Systemic effects are unlikely, however, and the substance is not considered a carcinogen or mutagen.

The standard first aid treatment for acid spills on the skin is, as for other corrosive agents, irrigation with large quantities of water. Washing is continued for at least ten to fifteen minutes to cool the tissue surrounding the acid burn and to prevent secondary damage. Contaminated clothing is removed immediately and the underlying skin washed thoroughly.

Being a strong oxidizing agent, reactions of nitric acid with compounds such as cyanides, carbides, metallic powders can be explosive and those with many organic compounds, such as turpentine, are violent and hypergolic (i.e. self-igniting). Hence, it should be stored away from bases and organics.

Chemical Properties of L-Valine

L-Valine, with the IUPAC Name of (2S)-2-amino-3-methylbutanoic acid, is one kind of white crystalline powder. This belongs to the Product Categories which include Amino Acids;Amino Acid Derivatives;Valine ;Amino Acids and Derivatives;alpha-Amino Acids;Biochemistry;Nutritional Supplements;Amino Acids.

L-Valine, or valine, is a proteinogenic amino acid that the body uses in the synthesis of protein. It is one of the branched chain amino acids (BCAAs) responsible for repairing and strengthening the muscle tissues. Being an essential amino acid, it must be obtained from the diet or through supplements. This amino acid can be obtained from a variety of foods, including both animal and plant foods.

1. Uses

There are many benefits of L-Valine for those who engage in regular exercise and bodybuilding. When present, it helps to increase the strength and endurance of the muscles and speeds up the recovery of fatigued muscles after workouts or competitions. A speedy recovery of the muscles can prevent them from breaking down and losing their tone. As a result of those benefits, L-Valine supplements are often taken by bodybuilders and competing athletes to maintain and improve their strength.

Other benefits include a reduced appetite, which can help to maintain a healthy weight. The metabolism of glucose, a form of sugar that the body uses for energy, is also improved. Those who have trouble sleeping can benefit due to its ability to reduce insomnia. It can also reduce nervousness and strengthen the immune system. A strong immune system in return is able to prevent a host of serious illnesses and common ailments.

2. Properties of L-Valine

Name:L-Valine

EINECS:200-773-6

Molecular Formula:C5H11NO2

CAS Registry Number:72-18-4 

InChI:InChI=1/C5H11NO2/c1-3(2)4(6)5(7)8/h3-4H,6H2,1-2H3,(H,7,8)/t4-/m0/s1

HS Code:29224995

Appearance:White crystalline powder

Molecular Weight:117.15

Density:1.23

Boiling Point:213.6 °C at 760 mmHg

Melting Point:315 °C

Flash Point:83 °C

Alpha:28 o (C=8, 6N HCL)

Storage Temperature:Store at RT

Refractive index:1.507

Solubility:85 g/L (20 °C)

3. Structure Descriptors of L-Valine

You could convert the following datas into the molecular structure:

(1)Canonical SMILES: CC(C)C(C(=O)O)N

(2)Isomeric SMILES: CC(C)[C@@H](C(=O)O)N

(3)InChI: InChI=1S/C5H11NO2/c1-3(2)4(6)5(7)8/h3-4H,6H2,1-2H3,(H,7,8)/t4-/m0/s1

(4)InChIKey: KZSNJWFQEVHDMF-BYPYZUCNSA-N

4. Safety Information of L-Valine

Hazard Codes: Xn

Risk Statements: 40

R40:Limited evidence of a carcinogenic effect.

Safety Statements: 24/25-36-22

S24/25:Avoid contact with skin and eyes.

S36:Wear suitable protective clothing.

S22:Do not breathe dust.

WGK Germany: 3

RTECS: YV9361000

HS Code: 29224995

Mutation data reported. When heated to decomposition it emits toxic fumes of NOx.

5. Production of L-Valine

Racemic valine can be synthesized by bromination of isovaleric acid followed by amination of the α-bromo derivative

HO2CCH2CH(CH3)2 + Br2 → HO2CCHBrCH(CH3)2 + HBr

HO2CCHBrCH(CH3)2 + 2 NH3 → HO2CCH(NH2)CH(CH3)2 + NH4Br

Sodium chloride's Uses And Preparation

Sodium chloride, also known as salt, common salt, table salt or halite, is an ionic compound with the formula NaCl, representing equal proportions of sodium and chlorine. Sodium chloride is the salt most responsible for the salinity of the ocean and of the extracellular fluid of many multicellular organisms. In the form of edible or table salt it is commonly used as a condiment and food preservative. Large quantities of sodium chloride are used in many industrial processes, and it is a major source of sodium and chlorine compounds used as feedstocks for further chemical syntheses. A second major consumer of sodium chloride is de-icing of roadways in sub-freezing weather.

1. Uses of Sodium chloride 

As the major ingredient in edible salt, Sodium chloride is commonly used as a condiment and food preservative. Sodium chloride can manufacture pulp and paper, to setting dyes in textiles and fabric, to producing soaps, detergents, and other bath products. Sodium chloride is sometimes used as a cheap and safe desiccant because of its hygroscopic properties.

Salt also is added to secure the soil and to provide firmness to the foundation on which highways are built. Road salt ends up in fresh water bodies and could harm aquatic plants and animals by disrupting their osmoregulation ability. The industrial uses of salt include, in descending order of quantity consumed, various applications, oil and gas exploration, textiles and dyeing, pulp and paper, metal processing, tanning and leather treatment, and rubber manufacture. It is used to flocculate and increase the density of the drilling fluid to overcome high downwell gas pressures.

In textiles and dyeing, salt is used as a brine rinse to separate organic contaminants, to promote “salting out” of dyestuff precipitates, and to blend with concentrated dyes to standardize them. In metal processing, salt is used in concentrating uranium ore into uranium oxide (yellow cake). It also is used in processing aluminium, beryllium, copper, steel and vanadium. In the pulp and paper industry, salt is used to bleach wood pulp. It also is used to make sodium chlorate. In rubber manufacture, salt is used to make buna, neoprene and white rubber types.

2. Preparation of Sodium chloride

Salt is currently mass-produced by evaporation of seawater or brine from other sources, such as brine wells and salt lakes, and by mining rock salt, called halite. Using sold salt dissoves in distilled water. The mixture is boiled after addition of sodium hydroxide, then is stored overnight and filtered. You should keep filtrate clean and then cool down it simultaneously put into pure HCl gas to make the mixture saturated. After that, crystal of Sodium chloride will separate out. There are also three methods of Sodium chloride production and purification: brine solution, rock salt mining, and the open pan or grainer process:

To produce Sodium chloride from brine, water is pumped into the salt deposit and the saturated salt solution containing 26% salt, 73.5% water, and 0.5% impurities, is removed. Hydrogen sulfide is removed by aeration, and oxidation with chlorine. Calcium (Ca2+), magnesium (Mg2+), and iron (Fe3+) are precipitated as the carbonates using soda ash and are removed in a settling tank. The brine solution can be sold directly or it can be evaporated to give salt of 99.8% purity.

Rock salt is produced from deep mines so that the salt is taken directly from the deposit. Salt obtained by this method is 98.5 to 99.4% pure.

In the open pan or grainer salt method, hot brine solution is held in an open pan approximately 4 to 6 meters wide, 45 to 60 meters long, and 60 cm deep at 96°C. Flat, pure sodium chloride crystals form on the surface and fall to the bottom and are raked to a centrifuge, separated from the brine, and dried. A purity of 99.98% is obtained. A vacuum pan system is also available.

Physical properties About Sodium chloride

Sodium chloride. With the CAS register number 7647-14-5. The substance is an ionic compound with the formula NaCl. Sodium chloride is soluble in water and glycerol, but insoluble in alcohol. Sodium chloride is stable. You must avoid contact with strong acids which when in contact may evolve chlorine gas. Sodium chloride will become corrosive to metals when wet. What's more, its EINECS number is 231-598-3.

Water solution of Sodium chloride is alkaline with the PH value 6.7-7.3. It is soluble in water, salty, and has low thermal conductivity. In addition, it won't conduct electricity. Sodium chloride has a strong hygroscopicity and can deliquesce easily. Rock salt is the most widely content in salt mine.

Sodium chloride is an ionic compound found in various foods and medical treatments. More commonly referred to as “salt” or “table salt,” sodium chloride is used as a seasoning in many foods.

Medically, sodium chloride solutions are used in catheter flush injections or intravenous infusions, and for cleaning objects such as contact lenses in the form of saline. Sodium chloride inhalation can remove certain bacteria in body secretions.

Name:Sodium Chloride

EINECS:231-598-3

Molecular Formula:NaCl

CAS Registry Number:7647-14-5 

InChI:InChI=1/ClH.Na/h1H;/q;+1/p-1

HS Code:3822 00 00

Appearance:colourless crystals or white powder

Molecular Weight:58.44

Density:2.165

Boiling Point:1461°C

Melting Point:801°C

Flash Point:1413°C

Storage Temperature:Store in a cool, dry, well-ventilated area away from incompatible substances.

Refractive index:n20/D 1.378

Solubility:360 g/L (20 °C)

Stability:Stable under normal shipping and handling conditions.

Chemical Properties:White crystalline powder

Usage:Facilitates the cross-coupling of organostannanes with iodides without using palladium.1

General Description:A white crystalline solid. Commercial grade usually contains some chlorides of calcium and magnesium which absorb moisture and cause caking.

Air & Water Reactions: Water soluble.

Reactivity Profile: Sodium chloride is generally unreactive. Releases gaseous hydrogen chloride if mixed with a concentrated nonvolatile acid such as sulfuric acid.

Fire Hazard: Literature sources indicate that Sodium chloride is nonflammable.