Natrium Produkt Beschreibung
- Englisch Name:Sodium
- Synonyma:Natrium;Sodium (engl.)
sodio;Sodium;NA 1421;Nametal;Natrium;sodium-23;SODIUM LUMP;sodium atom;COCKTAIL NA;SODIUM LUMPS
Natrium physikalisch-chemischer Eigenschaften
- Schmelzpunkt: :97.8 °C(lit.)
- Siedepunkt: :883 °C(lit.)
- Dichte :1.04 g/mL at 20 °C
- Dampfdruck :1 mm Hg ( 440 °C)
- Flammpunkt: :128 °F
- storage temp. :water-free area
- Löslichkeit :H2O: soluble
- Aggregatzustand :pieces (large)
- Farbe :White to off-white
- Wichte :0.97
- Widerstand (resistivity) :4.69 μΩ-cm, 20°C
- Wasserlöslichkeit :REACTS
- Sensitive :Air & Moisture Sensitive
- Merck :14,8570
- Stabilität: :Reacts violently with water, liberating and possibly igniting hydrogen. Flammable solid. Incompatible with water, strong oxidizing agents. Do not store near oxidants. Store under oil, or dry inert gas. Air sensitive.
- InChIKey :MPMYQQHEHYDOCL-UHFFFAOYSA-N
- CAS Datenbank :7440-23-5(CAS DataBase Reference)
- NIST chemische Informationen :Sodium(7440-23-5)
- EPA chemische Informationen :Sodium(7440-23-5)
- Kennzeichnung gefährlicher :C,F,T
- R-Sätze: :34-14/15-45-65
- S-Sätze: :26-8-6A-45-43D-43-36/37/39-22-7/8-62-5
- RIDADR :UN 3264 8/PG 3
- WGK Germany :1
- RTECS-Nr. :VY0686000
- Selbstentzündungstemperatur :>115 °C in air
- TSCA :Yes
- HS Code :2805 11 00
- HazardClass :4.3
- PackingGroup :I
- Giftige Stoffe Daten :7440-23-5(Hazardous Substances Data)
Sodium Chemische Eigenschaften,Einsatz,Produktion Methoden
- ERSCHEINUNGSBILD SILBERNER FESTSTOFF IN VERSCHIEDENEN FORMEN
- CHEMISCHE GEFAHREN Reagiert heftig mit Wasser, Feuer- und Explosionsgefahr. Schnelle Zersetzung unter Einfluss von Luftund Feuchtigkeit, unter Bildung brennbarer/explosionsfähiger Gase (z.B. Wasserstoff, ICSC-Nr. 0001).
TLV nicht festgelegt (ACGIH 2005).
MAK nicht festgelegt (DFG 2006).
- AUFNAHMEWEGE Schwerwiegende lokale Wirkungen auf allen Aufnahmewegen.
WIRKUNGEN BEI KURZZEITEXPOSITION
WIRKUNGEN BEI KURZZEITEXPOSITION:
Siehe ICSC 0360 (Natriumhydroxid)
- LECKAGE Gefahrenbereich verlassen! Fachmann zu Rate ziehen! Chemikalienschutzanzug mit umgebungsluftunabhängigem Atemschutzgerät. Verschüttetes Material mit trockenem Pulver abdecken.
R14/15:Reagiert heftig mit Wasser unter Bildung hochentzündlicher Gase.
R45:Kann Krebs erzeugen.
S26:Bei Berührung mit den Augen sofort gründlich mit Wasser abspülen und Arzt konsultieren.
S8:Behälter trocken halten.
S45:Bei Unfall oder Unwohlsein sofort Arzt zuziehen (wenn möglich, dieses Etikett vorzeigen).
S43:Zum Löschen . . . (vom Hersteller anzugeben) verwenden (wenn Wasser die Gefahr erhöht, anfügen: "Kein Wasser verwenden").
S53:Exposition vermeiden - vor Gebrauch besondere Anweisungen einholen.
- Aussehen Eigenschaften Na; wachsweiches, an frischen Schnittstellen silberweißes Metall, meist mit einer graubraunen Kruste überzogen.
Gefahren für Mensch und Umwelt
Natrium reagiert mit Wasser stürmisch unter Bildung von wasserstoff und Natronlauge, wobei es schmilzt und den Wasserstoff u.U. entzündet. Es reagiert äußerst heftig bis explosionsartig mit Halogenen, Halogeniden des Zinns, Silbers Schwefels, Phosphors und Siliciums, ferner mit Halogenwasserstoffen,Schwermetalloxiden, Säuren, Säurechloriden, Aktivkohle und Graphit, Ammoniumnitrat, Nitroverbindungen, Schwefelkohlenstoff und allen Peroxiden, Chloraten und Perchloraten. Die Oxide und Hydroxide, sowie Salze der meisten Schwermetalle werden beim Erhitzen mit Natrium, teilweise explosionsartig, zuden Metallen reduziert.
Petroleum sollte, wegen möglicher reaktiver Verunreinigungen, als Inertflüssigkeit vermieden werden.
Hautkontakt mit Natriummetall führt zu Verbrennungen bzw. extrem tiefgreifenden Verätzungen durch Natronlauge. Letztere sind eine in die Tiefe fortschreitene Quellung und Auflösung betroffener Gewebe (daher gefährlicher als Säureverätzungen). Am Auge durch Laugenspritzer oder Natriumpartikel schwereReizerscheinungen oder Verätzungen an der Bindehaut sowie Trübung und Geschwürbildung an der Hornhaut.
Durch Verschlucken entstehen schwerste Verätzungen der Speiseröhre und der Magenschleimhaut.
Wassergefährnder Stoff (WGK 2).
Schutzmaßnahmen und Verhaltensregeln
Reines Natrium wird unter Petrolether oder Paraffinöl aufbewahrt.
Trockene Schutzhandschuhe nur als kurzfristigen Schutz verwenden.
Verhalten im Gefahrfall
Metallstücke mit Pinzette aufsammeln. Kleine Krümel mit Propanol oder Wasser aufwischen.
Trockener Sand, Kalksteinpulver, Soda. Auf keinen Fall wasserhaltige Mittel oder CO2 zum Löschen verwenden.
Nach Hautkontakt: Metallteile trocken entfernen, dann mit Wasser gründlich abwaschen. Arzt aufsuchen.
Nach Augenkontakt: Mit Wasser mind. 10 Min. bei geöffnetem Augenlid spülen. Augenarzt aufsuchen.
Nach Verschlucken: Erbrechen vermeiden. Viel Wasser oder sauren Wein, Zitronensaft, Essigsäurelösung (stark verdünnt!) trinken lassen. Sofort zum Arzt!
Nach Kleidungskontakt: Verunreinigte Kleidung sofort ausziehen.
Ersthelfer: siehe gesonderten Anschlag
- Sachgerechte Entsorgung Kleine Reste vorsichtig in Propanol oder Ethanol geben, danach mit Wasser versetzen und neutralisieren. Das Gemisch wird im Sammelbehälter für neutrale wässrige Lösungen entsorgt. Größere Mengen als Sondermüll entsorgen.
- Chemische Eigenschaften Soft, silver-white solid oxidizing rapidly in air; waxlike at room temperature, brittle at low temperatures. Store in airtight containers or in naph- tha or similar liquid that does not contain water or free oxygen. Decomposes water on contact, with evolution of hydrogen to form sodium hydroxide; insoluble in benzene, kerosene, and naphtha. Has excellent elec- trical conductivity and high heat-absorbing capac- ity.
- Chemische Eigenschaften Sodium is a soft silvery white metallic element. Pyrophoric solid or molten liquid. Odorless
- Physikalische Eigenschaften Sodium is a soft, wax-like silver metal that oxidizes in air. Its density is 0.9674 g/cm3, andtherefore it floats on water as it reacts with the water releasing hydrogen. It has a rather lowmelting point (97.6°C) and a boiling point of 883°C. Sodium is an excellent conductor ofheat and electricity. It looks much like aluminum but is much softer and can be cut with aknife like butter. Its oxidation state is +1.
- Isotopes Sodium has 14 isotopes. The only stable isotope of sodium has an averageatomic weight of 23 (23Na) and makes up about 100% of all the isotopes of the element sodium found on Earth. All the other 13 isotopes (from 19Na to 31Na) are radioactive with relatively short half-lives and thus are unstable.
- Origin of Name The Latin name for the symbol for “sodium” (Na) is natrium, and the name “sodium” in Latin is sodanum, which was known as an ancient headache remedy and was called “soda” in English.
- Occurrence Sodium is the sixth most abundant of the Earth’s elements. Since it is a highly electropositive metal and so reactive with nonmetals, it is not found in its pure elemental form on Earth.Rather, it is found in numerous compounds in relatively abundant quantities. About 2.83%of the Earth’s crust consists of sodium in compounds.Sodium is produced by an electrolytic process, similar to the other alkali earth metals. (Seefigure 4.1). The difference is the electrolyte, which is molten sodium chloride (NaCl, common table salt). A high temperature is required to melt the salt, allowing the sodium cationsto collect at the cathode as liquid metallic sodium, while the chlorine anions are liberated aschlorine gas at the anode: 2NaCl (salt) + electrolysis → Cl2↑ (gas) + 2Na (sodium metal). Thecommercial electrolytic process is referred to as a Downs cell, and at temperatures over 800°C,the liquid sodium metal is drained off as it is produced at the cathode. After chlorine, sodiumis the most abundant element found in solution in seawater.
- Charakteristisch On the periodic table sodium is located between lithium and potassium. A fresh cut intosodium looks silvery but turns gray as sodium oxidizes rapidly in air, forming sodium oxideon its surface.Sodium is extremely reactive. It reacts explosively in water as it releases hydrogen fromthe water with enough heat to ignite the hydrogen. The resulting compound of this reactionis sodium hydroxide (2Na + 2H2O → 2NaOH + H2↑). Due to its extremely electropositivereactivity, there are few uses for the pure metallic form of sodium. Because of its reactivity,hundreds of sodium compounds are found on the Earth’s surface.Guide to the Elements | 51An unusual characteristic of several alkali metals is that a mixture of two or more has alower melting point than the melting point of the separate metals. This is referred to as aeutectic system of metallic alloys. For instance, sodium has a melting point of 97.6°C, andpotassium’s melting point is 63.25°C, but when the two are mixed, the eutectic melting point(turning into a liquid phase) of the combined Na-K system is below zero degrees Celsius(–10°C). If cesium metal (melting point of 38.89°C) is added to the Na and K mixture, themelting point of this eutectic alloy (Na-K-Cs) is the lowest of any eutectic alloy at –78°C.
- History Long recognized in compounds, sodium was first isolated by Davy in 1807 by electrolysis of caustic soda. Sodium is present in fair abundance in the sun and stars. The D lines of sodium are among the most prominent in the solar spectrum. Sodium is the sixth most abundant element on earth, comprising about 2.6% of the Earth’s crust; it is the most abundant of the alkali group of metals of which it is a member. The most common compound is sodium chloride, but it occurs in many other minerals, such as soda niter, cryolite, amphibole, zeolite, sodalite, etc. It is a very reactive element and is never found free in nature. It is now obtained commercially by the electrolysis of absolutely dry fused sodium chloride. This method is much cheaper than that of electrolyzing sodium hydroxide, as was used several years ago. Sodium is a soft, bright, silvery metal that floats on water, decomposing it with the evolution of hydrogen and the formation of the hydroxide. It may or may not ignite spontaneously on water, depending on the amount of oxide and metal exposed to the water. It normally does not ignite in air at temperatures below 115°C. Sodium should be handled with respect, as it can be dangerous when improperly handled. Metallic sodium is vital in the manufacture of sodamide and esters, and in the preparation of organic compounds. The metal may be used to improve the structure of certain alloys, to descale metal, to purify molten metals, and as a heat transfer agent. An alloy of sodium with potassium, NaK, is also an important heat transfer agent. Sodium compounds are important to the paper, glass, soap, textile, petroleum, chemical, and metal industries. Soap is generally a sodium salt of certain fatty acids. The importance of common salt to animal nutrition has been recognized since prehistoric times. Among the many compounds that are of the greatest industrial importance are common salt (NaCl), soda ash (Na2CO3), baking soda (NaHCO3), caustic soda (NaOH), Chile saltpeter (NaNO3), diand tri-sodium phosphates, sodium thiosulfate (hypo, Na2S2O3 · 5H2O), and borax (Na2B4O7 · 10H2O). Seventeen isotopes of sodium are recognized. Metallic sodium is priced at about $575/kg (99.95%). On a volume basis, it is the cheapest of all metals. Sodium metal should be handled with great care. It should be kept in an inert atmosphere and contact with water and other substances with which sodium reacts should be avoided.
- Verwenden manufacture of sodium Compounds, such as the cyanide, azide, peroxide, etc.; manufacture of tetraethyllead; manufacture of refractory metals; in org syntheses; for photoelectric cells; in sodium lamps; as catalyst for many polymerization reactions. Alloyed with potassium in heat transfer media.
- Verwenden This soft silvery metal occurring as chlorine in seawater was first isolated as an element by Humphry Davy in 1807. Sodium is one of the essential elements required by living organisms and it is highly reactive oxidizing in air and reacting with water. Sodium chloride was the first halide to be combined with silver for photographic purposes. Many of the sodium compounds were also used in gold toning baths. Some of them are included here.
- Verwenden Sodium is used in both low-pressure and high-pressure sodium vapor lamps. The low-pressure arc uses just a small amount of Na along with some neon for a starter. The lamp is economical and bright. The illumination with its single yellow color (electromagnetic frequency) makes it difficult for us to recognize other colors. In addition to sodium, the high-pressure lamp uses mercury, which provides a more natural color rendition of light. The very bright light of sodium-mercury lamps makes them ideal for use in sports stadiums and highways. Because the melting point of sodium metal is about 98 C (a bit lower than the boiling point of water), it is heated into a liquid phase and then transported in rail tank cars, where it cools and solidifies. Because sodium has a high specific heat rating, a major use is as a liquid coolant for nuclear reactors. Even though sodium (both solid and liquid) is extremely reactive with water, it has proven safe as a coolant for nuclear reactors in submarines. The natural deposits are located in northern Chile, which was the original source for many years. Of course, the most common use is everyday table salt, sodium chloride (NaCl).
- Verwenden Sodium is a metal element that performs bodily functions.
- Verwenden Sodium is used in the manufacture ofmany highly reactive sodium compounds andtetraethyllead, as a reducing agent in organicsynthesis, and as a catalyst in the productionof synthetic rubber. It is also used in makingsodium lamp and photovoltaic cells.
- Definition sodium: Symbol Na. A soft silveryreactive element belonging to group1 (formerly IA) of the periodic table(see alkali metals); a.n. 11; r.a.m.22.9898; r.d. 0.97; m.p. 97.8°C; b.p.882–889°C. Sodium occurs as thechloride in sea water and in the mineralhalite. It is extracted by electrolysisin a Downs cell. The metal isused as a reducing agent in certainreactions and liquid sodium is also acoolant in nuclear reactors. Chemically,it is highly reactive, oxidizingin air and reacting violently withwater (it is kept under oil). It dissolvesin liquid ammonia to formblue solutions containing solvatedelectrons. Sodium is a major essentialelement required by living organisms.The element was first isolatedby Humphry Davy in 1807.
- Definition Metallic element, atomic number 11, group IA of periodic table, aw 22.98977, valence = 1, no stable isotopes but several radioactive forms, extremely reactive.
- Allgemeine Beschreibung Sodium,Na, melts at 97.8°C and boils at 892°C. It is silver-white in color, is soft and malleable, and oxidizes in air. When exposed to air, a silvery soft metal that becomes grayish white upon. It occurs naturally only in the forms of its salts. Shipped as a solid or molten liquid. Burns violently with explosions that may spatter the material. Sodium is used as a chemical intermediate. and in pharmaceuticals, petroleum refining and metallurgy, electric power cable, Sodium lamps, other chemicals.
- Air & Water Reaktionen May ignite spontaneously in air. Reacts violently with water to give Sodium hydroxide and hydrogen, which ignites spontaneously [Merck, 11th ed. 1989)]. The ignition temperature of Sodium in air depends on the area of surface exposed: vapor ignites at room temperature; droplets at about 250°F; an agitated pool at 400°F. In the absence of moisture and hydrogen, the reaction is insignificant [Mellor 2 Supp. 2:440 1961].
- Reaktivität anzeigen Sodium is a powerful reducing agent. Reacts with incandescence with boron trifluoride [Merck 11th ed. 1989]. Reacts explosively with maleic anhydride [Chem Safety Data Sheet SD-88 1962; Chem. Haz. Info. Series C-71 1960]. Explodes on contact with bromoazide. Mixtures with any of the following produce a strong explosion on impact: aluminum bromide, aluminum chloride, aluminum fluoride, ammonium chloride, antimony(III) bromide, antimony(III) chloride, antimony(III) iodide, arsenic(III) chloride, arsenic(III) iodide, bismuth(III) bromide, bismuth(III) chloride, bismuth(III) iodide, boron tribromide, carbon tetrachloride, chromium(IV) chloride, cobalt(II) bromide, cobalt(II) chloride, copper(II) chloride, iron(II) chloride, iron(III) bromide, iron(II) iodide, iodine bromide, manganese(II) chloride, mercury(II) bromide, mercury(II) chloride, mercury(II) fluoride, mercury(II) iodide, mercury(I) chloride, silicon tetrachloride, silver fluoride, tin(IV) chloride, tin(IV) iodide (with sulfur), tin(II) chloride, sulfur dibromide, sulfur dichloride, thallium(I) bromide, vanadium pentachloride, phosphorus pentachloride, phosphorus tribromide, and zinc bromide [Mellor 2 Supp. 2:497 1961]. Reacts with ammonium nitrate to form a yellow explosive substance, thought to be diSodium nitrite [Mellor 8: Supp. 1 546 1964]. Reduces heated bismuth(III) oxide to the metal; the reaction is accompanied by incandescence [Mellor 9:649 1946-47]. Reacts, if finely divided, with bromine with luminescence. Burns spontaneously in moist chlorine. Reacts at room temperature with iodine [Mellor 2 Supp. 1:848 1956]. Reacts explosively with Dry Ice if the two are brought together by impact [Mellor 2 Supp. 2:468 1961]. Forms explosive mixtures with chlorinated hydrocarbons [Chem. Eng. News 26:2604 1948]. Explodes on contact with hydrochloric acid [Mellor 2:469 1946-47]. Explodes with aqueous hydrofluoric acid [Mellor 2:469 1946-47]. Ignites spontaneously in contact with dilute nitric acid [Mellor 2:470 1946-47]. Reacts with dilute sulfuric acid with explosive violence [Mellor 2:470 1946-47]. Sodium ignites on contact with hydroxylamine. (Mellor, 1940, Vol. 8, 292.)
- Hazard Severe fire risk in contact with water in any form, ignites spontaneously in dry air when heated; to extinguish fires use dry soda ash, salt, or lime. Forms strong caustic irritant to tissue.
Sodium as the elemental metal is very dangerous because of its extreme electropositivenature, particularly when it comes in contact with moist air, water, snow, or ice or otheroxidizing agents. It readily gives up electrons to electronegative atoms (nonmetals). In thesereactions, it releases hydrogen gas with enough heat to explosively ignite the hydrogen.
Numerous sodium compounds are hazardous as carcinogens (cancer-causing) and astoxins (poisons) in plants and animals. On the other hand, we benefit greatly from the manycompounds containing the element sodium. We could not live without it.
- Health Hazard Sodium is highly corrosive and can causeburns on the skin. Its fumes are highlyirritating to the skin, eyes, and mucousmembranes.
- Health Hazard Sodium reacts with the moisture on skin and other tissues to form highly corrosive sodium hydroxide. Contact of metallic sodium with the skin, eyes, or mucous membranes causes severe burns; thermal burns may also occur due to ignition of the metal and liberated hydrogen.
- Health Hazard Severe burns caused by burning metal or by caustic soda formed by reaction with moisture on skin.
- Brandgefahr Special Hazards of Combustion Products: Fumes of burning Na are highly irritating to skin, eyes, and mucous membranes.
- Brandgefahr Sodium spontaneously ignites when heated above 115 °C in air that has even modest moisture content, and any sodium vapor generated is even more flammable. Sodium reacts violently on contact with water and often ignites or explodes the hydrogen formed. Sodium fires must be extinguished with a class D dry chemical extinguisher or by the use of sand, ground limestone, dry clay or graphite, or ''Met- L-X ? " type solids. Water or CO 2 extinguishers must never be used on sodium fires.
- Flammability and Explosibility Sodium spontaneously ignites when heated above 115 °C in air that has even modest moisture content, and any sodium vapor generated is even more flammable. Sodium reacts violently on contact with water and often ignites or explodes the hydrogen formed. Sodium fires must be extinguished with a class D dry chemical extinguisher or by the use of sand, ground limestone, dry clay or graphite, or "Met- L-X ?" type solids. Water or CO2 extinguishers must never be used on sodium fires.
Sodium (Na) is a silvery reactive element belonging to
Group 1 (formerly IA) of the Periodic Table.
It is not an essential element for any crop (including salt
marsh plants), but it is useful in certain biological
processes. Some crops grow better with sodium which is
absorbed as an ion.
Sodium influences water retention in sugar beet and increases drought resistance. The supportive role of sodium is not clear in some plants; however, in crops like celery, marigold, sugar beet, turnip, etc., it increases the amount of water held by a unit dry weight of the leaf tissue and increases the succulence of the plant (which is why these plants have a greater drought resistance and increased leaf area.) Sugar beet and marigold in western Europe, for instance, need a good supply of sodium for satisfactory yields. In potassium deficient soils, sodium helps the growth of crops like barley and prevents the accumulation of other toxic cations, because deficiency of one cation leads to accumulation of the other. Sodium concentration varies widely from 0.01 to 10% in leaves. Sugar beet petioles frequently contain the upper end of the range. In low-sodium soils, beet leaves are dark green, thin and dull in hue and exhibit interveinal necrosis similar to that resulting from potassium deficiency.
Sodium is essential for halophytic plants. Plants that possess the C4 dicarboxylic acid photosynthetic pathway, require sodium as an essential nutrient. Sodium has a role in inducing crassulacean acid metabolism that is responsible for water stress. The lack of sodium causes certain plant species to shift their carbon dioxide fucation pathway from C4 to C3. Water economy in plants seems to be related to the C4 dicarboxylic photosynthetic pathway of plants in fine textured soils. The benefits of sodium are high when potassium is deficient.
The sodium demand of the crops is independent of, and perhaps greater than, their potassium demand. The important sodium-containing fertilizers are potassium fertilizers with a wide ranging content of sodium chloride, sodium nitrate, rhenania phosphate and multiple nutrient fertilizers with sodium salts. Sodium nitrate is available as a natural product, Chile saltpeter, which contains trace amounts of micronutrients, like boron. Synthetically, it is made from nitric acid and sodium hydroxide.
The presence of sodium in soils is restricted to arid and semi-arid regions. It is one of the most loosely held metallic ions and is readily lost in leaching water. In fine textured soils, sodium accumulation inhibits plant growth. A high concentration of sodium is undesirable in water as sodium is adsorbed on cation exchange sites, causing soil aggregates to break down, sealing the soil pores, and making it impermeable to water flow. Sodium adsorption ratio (SAR) is used to estimate the exchangeable percent sodium of soil; a low value indicates low sodium content.
In sodic soils, exchangeable sodium is above 15 % and its adsorption rate (SAR) is 13. The permeability is the limiting factor in the reclamation of sodic soil. A high salt content in water keeps sodic soils flocculated (joining of colloidal particles to form clusters) and the floccules are highly porous and allow penetration of the leaching waters. Thus, the first water used for leaching may be moderately salty. Sodic soil with low salt concentrations readily loses its structure because it allows soil colloids (clay and humus) to disperse into individual hydrated particles.
Some of the effects ascribed to sodium may also be due to the chloride ion in sodium chloride. In addition to toxicity due to high concentrations of sodium and chloride, sodium chloride affects plant growth because of the osmotic effect which increases the potential forces that hold water in the soil and makes it difficult for the plant roots to extract moisture.
Fine textured clayey soils with low exchangeable sodium (10%) and sandier soils with 20% exchang
Sodium has atomic number 11 and has the symbol Na, derived from the Latin name natrium. Sodium ions (Na+) are soluble in water and therefore present in large quantities in the oceans. Na+ is also part of minerals and an essential element for all animal life. The main biological roles of sodium ions are the maintenance of body fluids in humans and the functioning
of neurons and transmission of nerve impulses. Na+ is an important electrolyte and a vital component of the
extracellular fluid. Therefore, one of its roles is to maintain the fluid in the human body via osmoregulation,
a passive transport mechanism. Na+ ions also play a crucial role in the contraction of muscles
and in the mode of action of several enzymes. In the human body, Na+ is often used to actively build up an
electrostatic potential across membranes, with potassium ions (K+) being the counter-ion.
The build-up of an electrostatic potential across cell membranes is important to allow the transmission of
Sodium is an essential mineral for the human body and crucial for the regulation of the body fluid via its osmosis activity. Sodium ions account for over 90% of all ions in the plasma and in the interstitial fluid, which are involved in osmosis processes. Furthermore, it is the most abundant cation in the extracellular fluid, and therefore the Na+ content controls the extracellular volume. In particular, the kidneys play an important role in regulating the fluid level of the body as well as the filtration, secretion and re-absorption of Na+ in the nephrons, the functional unit of the kidney. Na+ ions are used in the human body to establish osmotic gradients, which in turn is crucial to control the water balance. Furthermore, decreases in blood pressure and in Na+ concentrations are sensed by the kidneys, and hormones (e.g. renin, antidiuretic hormones (ADHs), atrial natriuretic peptide) are released that control the blood pressure, osmotic balances and water-retaining mechanisms.
- Sicherheitsprofil Metahc sodtum reacts exothermally with the moisture of body or tissue surfaces, causing thermal and chemical burns. Sodium in elemental form is highly reactive. Sodium reacts violently with water to form sodium hydroxide. A very dangerous fire hazard when exposed to heat and moisture. Under the appropriate condttions, it can react violently with moisture, air, ALBr3, dcl3, AlF3, NH4 chlorocuprate, NH4NO3, SbBr3, SbCl3, SbI3, AsCl3, Ash, Bil3r3, BiCl3, BiI3, Biz03, BBr3, bromoazide, Con, CO + NH3, cCl4, Cl2, ClF3, CrCl4, Cr03, CoBr, CoCl, CuCl2, CuO，FeBrs, FeCL, FeBr2, FeCl2, FeI2, hydrazine hydrate, H202, H2S, HCl, HF, F2, 1,2dichloroethylene, dichloromethane, Brz, hydroxylamine, iodine, iodine monochloride, iodine pentafluoride, lead oxide, maleic anhydride, manganous chloride, mercuric bromide, mercuric chloride, mercuric fluoride, mercuric iodide, mercurous chloride, mercurous oxide, methyl chloride, molybdenum trioxide, monoammonium phosphate, nitric acid, nitrogen peroxide, nitrosyl fluoride, nitrous oxide, phosgene, phosphorus, phosphorus pentafluoride, phosphorus pentoxide, phosphorus tribromide, phosphorus trichloride, phosphoryl chloride, potassium oxides, potassium ozonide, potassium superoxide, selenium, silicon tetrachloride, silver bromide, silver chloride, silver fluoride, silver iodide, sodium peroxide, stannic chloride, stannic iodide with sulfur, stannic oxide, stannous chloride, sulfur, sulfur dibromide, sulfur dichloride, sulfur dioxide, sulfuric acid, tellurium, tetrachloroethane, thallous bromide, thiophosphoryl bromide, trichlorethylene, vanadium pentachloride, vanadyl chloride, zinc bromide, any oxidizing material. Decomposes moisture to evolve hydrogen and heat. Reacts exothermally with halogens, acids, and halogenated hydrocarbons. flammable in air. Can be safely stored under liquid hydrocarbons. Dangerous explosion hazard when exposed to moisture in any form!! Keep away from water at all times!! When heated in air it emits toxic fumes of sodium oxide. Reacts with water or steam to produce heat, hydrogen, and flammable vapors. Can react vigorously to explosively with oxidizing materials. To fight fEe, use soda ash, dry sodium chloride, or graphite, in order of preference. When heated to decomposition it emits toxic fumes of NazO. See also SODIUM HYDROXIDE and HYDROGEN. Heated sodium is spontaneously
- mögliche Exposition A potential danger to those involved in tetra-alkyl lead manufacture using lead-sodium alloy as a reactant; those using sodium as a liquid metal coolant, as a catalyst, or in the manufacture of sodium hydride, borohydride, or peroxide.
- Lager Safety glasses, impermeable gloves, and a fire-retardant laboratory coat should be worn at all times when working with sodium, and the metal should be handled under the surface of an inert liquid such as mineral oil, xylene, or toluene. Sodium should be used only in areas free of ignition sources and should be stored under mineral oil in tightly sealed metal containers under an inert gas such as argon.
- Versand/Shipping UN1428 Sodium, Hazard Class: 4.3; Labels: 4.3-Dangerous when wet material. Note: Finely divided sodium is pyrophoric.
- läuterung methode The metal is placed on a coarse grade of sintered-glass filter, melted under vacuum and forced through the filter using argon. The Pyrex apparatus is then re-evacuated and sealed off below the filter, so that the sodium could be distilled at 460o through a side arm and condenser into a receiver bulb which is then sealed off [Gunn & Green J Am Chem Soc 80 4782 1958]. EXPLODES and IGNITES in water.
- Inkompatibilitäten A strong reducing agent. A dangerous fire hazard when exposed to heat and moisture. Violent reaction with water, forming NaOH. Violent reaction with oxidizers (chlorates, nitrates, peroxides, permanganates, perchlorates, chlorine, bromine, fluorine, etc.); contact may cause fires or explosions. Keep away from alkaline materials, strong bases, strong acids, oxoacids, epoxides. halogenated hydrocarbons; phosphorus and phosphorus compounds; sulfur and sulfur compounds; and many other chemicals.
- Waste disposal Incineration with absorption of oxide fumes.
Sodium Upstream-Materialien And Downstream Produkte
- 3,3-Diphenylpropanol 2,4-Dimethylchinolin 2-Heptanol 2-Methoxyfuran 4-Amino-2-methylpyrimidin-5-carbonitril 4,4,4-Trifluor-1-phenylbutan-1,3-dion 4,6-Diaminopyrimidin-2-thiol Bis(2-ethylhexyl)phenylphosphit Fentin-chlorid 2,3-Epoxypropylisopropylether Dinatriumperoxid 6-Amino-1-methyl-5-nitrosouracil Octan-3-ol Di(2-pyridyl)amin 2-Methylbutan-1-thiol
Natrium Anbieter Lieferant Produzent Hersteller Vertrieb Händler.Global(0)Suppliers
7440-23-5, Sodium Verwandte Suche:
- Beryllium Dinatriumoxid Weies Mineraloel (Erdoel) Paraffinwachse und Kohlenwasserstoffwachse Natriumhydroxid Dinatrium-2,2'-(9,10-dioxoanthracen-1,4-diyldiimino)bis(5-methylsulfonat Dinatrium-2,2'-((9,10-dihydro-9,10-dioxoanthracen-1,5-diimino)bis(5-methylbenzolsulfonat) Natrium-3,3'-(9,10-dioxoanthracen-1,4-diyldiimino)bis(2,4,6-trimethylbenzolsulfonat) Sodium acetate trihydrate Natriumbenzoat Natriumcarbonat Natriumsulfat Natriumchlorid Natriumnitrat Natriumnitrit Natriumhydrogencarbonat Natriumacetat
- sodium metallic
- Sodium (99.95%)
- Sodium dispersion
- Sodium ingot (min.99.8%)
- Sodium solution 10 000 ppm
- Sodium solution 1000 ppm
- Sodium standard solution 1000 ppm
- SODIUM METAL 99.5%
- SODIUM, CUBE, IN MINERAL OIL, 99.95%
- SODIUM 30-35 WT. % DISPERSION IN PARAF&
- SODIUM 25 WT. % DISPERSION IN TOLUENE
- SODIUM, LUMP, IN KEROSENE, 99%
- Sodium, ingot, 99.95% metals basis
- SODIUM, SPHERES, 3 TO 8MM, IN ODORLESS M INERAL SPIRITS
- SODIUM, STICK, DRY, A.C.S. REAGENT (UNDE R NITROGEN)
- SODIUM, 25WT. % DISPERSION IN PARAFFIN WAX
- SODIUM, 40 WT. % DISPERSION IN NAPHTHEN&
- Sodium, 99.5%, oiled sticks
- Sodium, under mineral oil, 99.8%
- SODIUM REAGENT (ACS)
- SODIUM, 40% DISPERSION IN OIL
- SODIUM, 3N5: 99.95%
- SODIUM: 99.95%, 3N5
- SODIUM DISPERSION, GRAY SUSPENSION: 40% IN MINERAL OIL
- SODIUM INGOT: 99.8%, (ACS)
- SODIUM STICK DRY A.C.S. REAGENT &
- SODIUM, 30-35 WT. % DISPERSION IN PARAFFIN WAX
- SODIUM LUMPS
- SODIUM, LARGE PIECES, IN KEROSENE
- SODIUM LUMP
- Sodium, 30wt% dispersion in toluene, <0.1 mm particle size
- Sodium, dry stick
- Sodium, oiled sticks, wrapped in aluminium foil, 99.8%
- Sodium, Breakseal Ampoule
- Sodium, Oil based standard solution, Specpure(R), Na 1000μg/g
- Sodium, plasma standard solution, Specpure(R), Na 1000μg/ml
- Sodium, plasma standard solution, Specpure(R), Na 10,000μg/ml
- Sodium, Oil based standard solution, Specpure(R), Na 5000μg/g
- Sodium, AAS standard solution, Specpure(R), Na 1000μg/ml
- Sodium, sticks, in mineral oil
- Dupont sodium metal dispersion
- SODIUM, POWDER, DRY
- Sodium AA Standard,1000 ppm in HNO3
- BUFFERS PH 4,00(20°C) 7,00 (20°C)9,00
- THIOGLYCOLLATE MEDIUM USP 20X9ML