Sodium chloride Chemical Properties

Melting point:

801 °C (lit.)

Boiling point:

1465 °C/1 atm (lit.)

Density 

1.199 g/mL at 20 °C

vapor pressure 

1 mm Hg ( 865 °C)

refractive index 

n20/D 1.378

Flash point:

1413°C

storage temp. 

+15C to +30C

solubility 

H₂O: soluble

form 

tablets

color 

White

Specific Gravity

2.165

PH

5.5-6.5(1 tablet in 100 mL purified water)

Water Solubility 

360 g/L (20 ºC)

Sensitive 

Hygroscopic

λmax

λ: 260 nm Amax: 0.02
λ: 280 nm Amax: 0.01

Crystal Structure

NaCl type

crystal system

Cube

Merck 

14,8599

BRN 

3534976

Space group

Fm3m

Lattice constant

a/nm	b/nm	c/nm	α/o	β/o	γ/o	V/nm3
0.564	0.564	0.564	90	90	90	0.17942

Dielectric constant

5.9（Ambient）

BCS Class

1

Stability:

Stable. Incompatible with strong oxidizing agents.

InChIKey

FAPWRFPIFSIZLT-UHFFFAOYSA-M

CAS DataBase Reference

7647-14-5(CAS DataBase Reference)

NIST Chemistry Reference

Sodium chloride(7647-14-5)

EPA Substance Registry System

Sodium chloride (7647-14-5)

Safety Information

Hazard Codes 

Xi

Risk Statements 

36-36/37/38-22

Safety Statements 

24/25-26-36

WGK Germany 

1

RTECS 

VZ4725000

F 

3-10

TSCA 

Yes

HS Code 

38220000

Hazardous Substances Data

7647-14-5(Hazardous Substances Data)

Toxicity

LD50 orally in rats: 3.75 ±0.43 g/kg (Boyd, Shanas)

MSDS

• Language:English Provider:Sodium chloride
• Language:English Provider:SigmaAldrich
• Language:English Provider:ACROS
• Language:English Provider:ALFA

Sodium chloride Usage And Synthesis

Crystal System

​The space lattice of NaCl belongs to the cubic system, and its rock salt structure has a lattice constant of a=0.55870 nm and Na–Cl=0.27935 nm. The cleavage plane is (100).

Description

Sodium chloride is widely distributed in nature. Oceans are the vast source of sodium chloride. It occurs in seawater at an average concentration of 2.68 wt%. It also occurs in many inland saline waters and in salt deposits in sedimentary rocks, as the mineral halite.
Sodium chloride is probably the most important salt of both sodium and chlorine. Sodium chloride, common table salt, is an essential component of most food preparation, imparting flavor to food and providing the sodium nutritional requirement. Also, it is used for preserving food. Therapeutically, NaCl solution is used to combat dehydration as an electrolyte replenisher, and it is an emetic.
The most important applications of sodium chloride in the chemical industry are in making a number of important industrial chemicals such as hydrochloric acid, sodium hydroxide, sodium carbonate, and metallic sodium. It is the starting material in manufacturing these substances. Other uses are in dyeing and printing fabrics, glazing pottery, in making soap, and for curing hides. Sodium chloride is a component of many freezing mixtures.

Chemical Properties

Sodium chloride, NaCl, also known as common salt and halite, is a white crystalline solid.It is soluble in water,slightly soluble in alcohol, and melts at 804 °C (1480 °F). Sodium chloride is the most important sodium mineral and occurs naturally in seawater, underground deposits, and brine wells.Sodiumchlorideis a basic raw material for the production of chlorine,sodium hypochlorite, sodium bisulfate,soda ash, and hydrogen chloride. Sodium chloride is also used in food preparation, fertilizers, and by highway departments to control icy road conditions.

Chemical Properties

Sodium chloride occurs as a white crystalline powder or colorless crystals; it has a saline taste. The crystal lattice is a face-centered cubic structure. Solid sodium chloride contains no water of crystallization although, below 0℃, salt may crystallize as a dihydrate.

Physical properties

Sodium chloride is the familiar compound commonly referred to as salt or table salt. Th e mineral form of sodium chloride is halite and is found in natural deposits throughout the world. It accounts for approximately 2.7% by weight of the dissolved minerals in seawater. Sodium chloride is an ionic compound existing as a white crystalline cubic structure of alternating sodium and chloride ions. Sodium chloride is essential for life, with the average adult requiring about 1 to 2 grams per day. Salt supplies sodium and provides numerous essential functions such as maintaining water balance in cells, taking part in nerve signal transmission and muscle contraction.

Occurrence

Sodium chloride is widely distributed in nature. Oceans are the vast source of sodium chloride. It occurs in seawater at an average concentration of 2.68 wt%. It also occurs in many inland saline waters and in salt deposits in sedimentary rocks, as the mineral halite.
Sodium chloride is probably the most important salt of both sodium and chlorine. Sodium chloride, common table salt, is an essential component of most food preparation, imparting flavor to food and providing the sodium nutritional requirement. Also, it is used for preserving food. Therapeutically, NaCl solution is used to combat dehydration as an electrolyte replenisher, and it is an emetic.
The most important applications of sodium chloride in the chemical industry are in making a number of important industrial chemicals such as hydrochloric acid, sodium hydroxide, sodium carbonate, and metallic sodium. It is the starting material in manufacturing these substances. Other uses are in dyeing and printing fabrics, glazing pottery, in making soap, and for curing hides. Sodium chloride is a component of many freezing mixtures.

Uses

sodium chloride (table salt) is used as a preservative, astringent, and anti-septic to treat inflamed lesions. It can also be used to mask odor, reduce product density, and control viscosity. Diluted solutions are not considered irritating.

Uses

Sodium chloride Commonly known as table salt, sodium chloride is found as the mineral halite and in brines and seawater. Sodium chloride is soluble in water but less so in alcohol. It was the first halide to be combined with silver nitrate and was also used by L. J. M. Daguerre and W. H. F. Talbot as a stabilizer before fi xing with hypo was adopted.

Uses

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

Uses

Used in biochemistry and molecular biology applications; a component of PBS and SSC buffers

Uses

Used as an electrolyte; buffers ; matrix modification.

Uses

Natural salt is the source of chlorine and of sodium as well as of all, or practically all, their Compounds, e.g., hydrochloric acid, chlorates, sodium carbonate, hydroxide, etc.; for preserving foods; manufacture of soap, to salt out dyes; in freezing mixtures; for dyeing and printing fabrics, glazing pottery, curing hides; metallurgy of tin and other metals.

Definition

ChEBI: An inorganic chloride salt having sodium(1+) as the counterion.

Production Methods

Sodium chloride occurs naturally as the mineral halite. Commercially, it is obtained by the solar evaporation of sea water, by mining, or by the evaporation of brine from underground salt deposits.

Definition

A compound with an acidic and a basic radical, or a compound formed by total or partial replacement of the hydrogen in an acid by a metal. In general terms a salt is a material that has identifiable cationic and anionic components.

Definition

saline: Describing a chemical compoundthat is a salt, or a solutioncontaining a salt.

Definition

salt: A compound formed by reactionof an acid with a base, in whichthe hydrogen of the acid has been replacedby metal or other positiveions. Typically, salts are crystallineionic compounds such as Na+Cl– andNH₄⁺NO₃^-. Covalent metal compounds,such as TiCl₄, are also oftenregarded as salts.

Preparation

Sodium chloride is produced by solar evaporation of seawater or brine from underground salt deposits. It also is produced by mining rock salt. The commercial product contains small amounts of calcium and magnesium chlorides.

brand name

Broncho Saline (Blairex).

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.

Flammability and Explosibility

Non flammable

Pharmaceutical Applications

Sodium chloride is widely used in a variety of parenteral and nonparenteral pharmaceutical formulations, where the primary use is to produce isotonic solutions.
Sodium chloride has been used as a lubricant and diluent in capsules and direct-compression tablet formulations in the past, although this practice is no longer common. Sodium chloride has also been used as a channeling agent and as an osmotic agent in the cores of controlled-release tablets. It has been used as a porosity modifier in tablet coatings, and to control drug release from microcapsules.
The addition of sodium chloride to aqueous spray-coating solutions containing hydroxypropyl cellulose or hypromellose suppresses the agglomeration of crystalline cellulose particles.(13) Sodium chloride can also be used to modify drug release from gels and from emulsions. It can be used to control micelle size, and to adjust the viscosity of polymer dispersions by altering the ionic character of a formulation.

Agricultural Uses

Halite is a naturally occurring sodium chloride (NaCl) deposit. The most abundant potash mineral deposit is sylvite (KCl). Sylvite with halite forms the common potash ore, called sylvinite.

Biochem/physiol Actions

Sodium chloride helps to stimulate the stable induction of T-helper cell 17 (TH17) cells.

Clinical Use

Treatment and prophylaxis of sodium chloride deficiency

Safety Profile

Poison by intraperitoneal and intracervical routes. Moderately toxic by ingestion, intravenous, and subcutaneous routes. An experimental teratogen. Human systemic effects by ingestion: blood pressure increase. Human reproductive effects by intraplacental route: terminates pregnancy. Experimental reproductive effects. Human mutation data reported. A skin and eye irritant. When bulk sodium chloride is heated to high temperature, a vapor is emitted that is irritating, particularly to the eyes. Ingestion of large amounts of sodium chloride can cause irritation of the stomach. Improper use of salt tablets may produce this effect. Potentially explosive reaction with dichloromaleic anhydride + urea. Electrolysis of mixtures with nitrogen compounds may form the explosive nitrogen trichloride. Reaction with burning lithmm forms the dangerously reactive sodmm. The molten salt at 11 00' reacts explosively with water. Violent reaction with BrF3. When heated to decomposition it emits toxic fumes of Cland Na2O.

Safety

Sodium chloride is the most important salt in the body for maintaining the osmotic tension of blood and tissues. About 5–12 g of sodium chloride is consumed daily, in the normal adult diet, and a corresponding amount is excreted in the urine. As an excipient, sodium chloride may be regarded as an essentially nontoxic and nonirritant material. However, toxic effects following the oral ingestion of 0.5–1.0 g/kg body-weight in adults may occur. The oral ingestion of larger quantities of sodium chloride, e.g. 1000 g in 600mL of water, is harmful and can induce irritation of the gastrointestinal tract, vomiting, hypernatremia, respiratory distress, convulsions, or death.
In rats, the minimum lethal intravenous dose is 2.5 g/kg bodyweight.
LD50 (mouse, IP): 6.61 g/kg
LD50 (mouse, IV): 0.65 g/kg
LD50 (mouse, oral): 4.0 g/kg
LD50 (mouse, SC): 3.0 g/kg
LD50 (rat, oral): 3.0 g/kg

Drug interactions

Potentially hazardous interactions with other drugs
May impair the efficacy of antihypertensive drugs in chronic renal failure.

Metabolism

Excess sodium is mainly excreted by the kidney, and small amounts are lost in the faeces and sweat.

storage

Aqueous sodium chloride solutions are stable but may cause the separation of glass particles from certain types of glass containers. Aqueous solutions may be sterilized by autoclaving or filtration. The solid material is stable and should be stored in a well-closed container, in a cool, dry place.
It has been shown that the compaction characteristics and the mechanical properties of tablets are influenced by the relative humidity of the storage conditions under which sodium chloride was kept.

Purification Methods

It is recrystallised from a saturated aqueous solution (2.7mL/g) by passing in HCl gas, or by adding EtOH or acetone. It can be freed from bromide and iodide impurities by adding chlorine water to an aqueous solution and boiling it for some time to expel free bromine and iodine. Traces of iron can be removed by prolonged boiling of solid NaCl in 6M HCl; the crystals are then washed with EtOH and dried at ca 100o. Sodium chloride has been purified by sublimation in a stream of pre-purified N2 and collected by electrostatic discharge [Ross & Winkler J Am Chem Soc 76 2637 1954]. For use as a primary analytical standard, analytical reagent grade NaCl should be finely ground, dried in an electric furnace at 500-600o in a platinum crucible, and allowed to cool in a desiccator. For most purposes, however, drying at 110-120o is satisfactory.

Incompatibilities

Aqueous sodium chloride solutions are corrosive to iron. They also react to form precipitates with silver, lead, and mercury salts. Strong oxidizing agents liberate chlorine from acidified solutions of sodium chloride. The solubility of the antimicrobial preservative methylparaben is decreased in aqueous sodium chloride solutions and the viscosity of carbomer gels and solutions of hydroxyethyl cellulose or hydroxypropyl cellulose is reduced by the addition of sodium chloride.

Regulatory Status

GRAS listed. Included in the FDA Inactive Ingredients Database (injections; inhalations; nasal, ophthalmic, oral, otic, rectal, and topical preparations). Included in nonparenteral and parenteral medicines licensed in the UK. Included in the Canadian List of Acceptable Non-medicinal Ingredients.

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