ZINC CHLORIDE SOLUTION 60% (NKO KLORR 60%)

ZINC CHLORIDE SOLUTION 60% / ÇNKO KLORÜR 60%

CAS Number:7646-85-7

EC Number:231-592-0

SYNONYMS:

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ZNC CHLORDE SOLUTON 60%

Zinc chloride

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For the battery type, see Zinc-chloride battery.

Zinc chloride

Zinc chloride hydrate

Kristallstruktur Zinkchlorid.png

Names

IUPAC name

Zinc chloride

Other names

Zinc(II) chloride

Zinc dichloride

Butter of zinc

Identifiers

CAS Number

7646-85-7 Anhydrous ☑

29426-92-4 Tetrahydrate ☒

3D model (JSmol)

Interactive image

ChEBI

CHEBI:49976 ☑

ChEMBL

ChEMBL1200679 ☒

ChemSpider

5525 ☑

ECHA InfoCard 100.028.720

EC Number

231-592-0

PubChem CID

3007855

RTECS number

ZH1400000

UNII

86Q357L16B ☑

UN number 2331

CompTox Dashboard (EPA)

DTXSID2035013 Edit this at Wikidata

InChI[show]

SMILES[show]

Properties

Chemical formula ZnCl2

Molar mass 136.315 g/mol

Appearance white crystalline solid

hygroscopic and very deliquescent

Odor odorless

Density 2.907 g/cm3

Melting point 290 °C (554 °F; 563 K)[1]

Boiling point 732 °C (1,350 °F; 1,005 K)[1]

Solubility in water 432.0 g/ 100 g (25 °C)

Solubility soluble in ethanol, glycerol and acetone

Solubility in alcohol 430.0 g/100ml

Magnetic susceptibility (χ) -65.0·10-6 cm3/mol

Structure

Coordination geometry Tetrahedral, linear in the gas phase

Pharmacology

ATC code B05XA12 (WHO)

Hazards

Safety data sheet External MSDS

EU classification (DSD) (outdated) Harmful (Xn)

Corrosive (C)

Dangerous for the environment (N)

R-phrases (outdated) R22, R34, R50/53

S-phrases (outdated) (S1/2), S26, S36/37/39, S45, S60, S61

NFPA 704 (fire diamond)

NFPA 704 four-colored diamond

030

Lethal dose or concentration (LD, LC):

LD50 (median dose) 350 mg/kg (rat, oral)

350 mg/kg (mouse, oral)

200 mg/kg (guinea pig, oral)

1100 mg/kg (rat, oral)

1250 mg/kg (mouse, oral)[3]

LC50 (median concentration) 1260 mg/m3 (rat, 30 min)

1180 mg-min/m3[3]

NIOSH (US health exposure limits):

PEL (Permissible) TWA 1 mg/m3 (fume)[2]

REL (Recommended) TWA 1 mg/m3 ST 2 mg/m3 (fume)[2]

IDLH (Immediate danger) 50 mg/m3 (fume)[2]

Related compounds

Other anions Zinc fluoride

Zinc bromide

Zinc iodide

Other cations Cadmium chloride

Mercury(II) chloride

Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

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Infobox references

Zinc chloride is the name of chemical compounds with the formula ZnCl2 and its hydrates. Zinc chlorides, of which nine crystalline forms are known, are colorless or white, and are highly soluble in water.[citation needed] ZnCl2 itself is hygroscopic and even deliquescent. Samples should therefore be protected from sources of moisture, including the water vapor present in ambient air. Zinc chloride finds wide application in textile processing, metallurgical fluxes, and chemical synthesis. No mineral with this chemical composition is known aside from the very rare mineral simonkolleite, Zn5(OH)8Cl2·H2O.

Structure and properties

Four crystalline forms (polymorphs) of ZnCl2 are known: α, β, γ, and δ, and in each case the Zn2+ ions are tetrahedrally coordinated to four chloride ions.[4]

Form Symmetry Pearson symbol Group No a (nm) 　b (nm) c (nm) Z ρ (g/cm3)

α tetragonal tI12 I42d 122 0.5398 0.5398 0.64223 4 3.00

β tetragonal tP6 P42/nmc 137 0.3696 0.3696 1.071 2 3.09

γ monoclinic mP36 P21/c 14 0.654 1.131 1.23328 12 2.98

δ orthorhombic oP12 Pna21 33 0.6125 0.6443 0.7693 4 2.98

Here a, b, and c are lattice constants, Z is the number of structure units per unit cell, and ρ is the density calculated from the structure parameters.[5][6][7]

The pure anhydrous orthorhombic form (δ) rapidly changes to one of the other forms on exposure to the atmosphere, and a possible explanation is that the OH- ions originating from the absorbed water facilitate the rearrangement.[4] Rapid cooling of molten ZnCl2 gives a glass.[8]

The covalent character of the anhydrous material is indicated by its relatively low melting point of 275 °C.[9] Further evidence for covalency is provided by the high solubility of the dichloride in ethereal solvents, where it forms adducts with the formula ZnCl2L2, where L = ligand such as O(C2H5)2. In the gas phase, ZnCl2 molecules are linear with a bond length of 205 pm.[10]

Molten ZnCl2 has a high viscosity at its melting point and a comparatively low electrical conductivity, which increases markedly with temperature.[10][11] A Raman scattering study of the melt indicated the presence of polymeric structures,[12] and a neutron scattering study indicated the presence of tetrahedral {ZnCl4} complexes.[13]

Hydrates

Five hydrates of zinc chloride are known: ZnCl2(H2O)n with n = 1, 1.5, 2.5, 3 and 4.[14] The tetrahydrate ZnCl2(H2O)4 crystallizes from aqueous solutions of zinc chloride.[14]

Preparation and purification

Anhydrous ZnCl2 can be prepared from zinc and hydrogen chloride:

Zn(s) + 2 HCl → ZnCl2 + H2(g)

Hydrated forms and aqueous solutions may be readily prepared similarly by treating Zn metal with hydrochloric acid. Zinc oxide and zinc sulfide react with HCl:

ZnS(s) + 2 HCl(aq) → ZnCl2(aq) + H2S(g)

Unlike many other elements, zinc essentially exists in only one oxidation state, 2+, which simplifies purification of the chloride.

Commercial samples of zinc chloride typically contain water and products from hydrolysis as impurities. Such samples may be purified by recrystallization from hot dioxane. Anhydrous samples can be purified by sublimation in a stream of hydrogen chloride gas, followed by heating the sublimate to 400 °C in a stream of dry nitrogen gas. Finally, the simplest method relies on treating the zinc chloride with thionyl chloride.[15]

Reactions

Molten anhydrous ZnCl2 at 500-700 °C dissolves zinc metal, and, on rapid cooling of the melt, a yellow diamagnetic glass is formed, which Raman studies indicate contains the Zn2+

2 ion.[14]

A number of salts containing the tetrachlorozincate anion, ZnCl2-

4, are known.[10] “Caulton’s reagent”, V2Cl3(thf)6Zn2Cl6 is an example of a salt containing Zn2Cl2-

6.[16][17] The compound Cs3ZnCl5 contains tetrahedral ZnCl2-

4 and Cl- anions.[4] No compounds containing the ZnCl4-

6 ion have been characterized.[4]

Whilst zinc chloride is very soluble in water, solutions cannot be considered to contain simply solvated Zn2+ ions and Cl- ions, ZnClxH2O(4-x) species are also present.[18][19][20] Aqueous solutions of ZnCl2 are acidic: a 6 M aqueous solution has a pH of 1.[14] The acidity of aqueous ZnCl2 solutions relative to solutions of other Zn2+ salts is due to the formation of the tetrahedral chloro aqua complexes where the reduction in coordination number from 6 to 4 further reduces the strength of the O-H bonds in the solvated water molecules.[21]

In alkali solution in the presence of OH- ion various zinc hydroxychloride anions are present in solution, e.g. Zn(OH)3Cl2-, Zn(OH)2Cl2-

2, ZnOHCl2-

3, and Zn5(OH)8Cl2·H2O (simonkolleite) precipitates.[22]

When ammonia is bubbled through a solution of zinc chloride, the hydroxide does not precipitate, instead compounds containing complexed ammonia (ammines) are produced, Zn(NH3)4Cl2·H2O and on concentration ZnCl2(NH3)2.[23] The former contains the Zn(NH3)62+ ion [4], and the latter is molecular with a distorted tetrahedral geometry.[24] The species in aqueous solution have been investigated and show that Zn(NH3)42+ is the main species present with Zn(NH3)3Cl+ also present at lower NH3:Zn ratio.[25]

Aqueous zinc chloride reacts with zinc oxide to form an amorphous cement that was first investigated in the 1855 by Stanislas Sorel. Sorel later went on to investigate the related magnesium oxychloride cement, which bears his name.[26]

When hydrated zinc chloride is heated, one obtains a residue of Zn(OH)Cl e.g.[27]

ZnCl2·2H2O → ZnCl(OH) + HCl + H2O

The compound ZnCl2·1⁄2HCl·H2O may be prepared by careful precipitation from a solution of ZnCl2 acidified with HCl. It contains a polymeric anion (Zn2Cl5-)n with balancing monohydrated hydronium ions, H5O2+ ions.[4][28]

The formation of highly reactive anhydrous HCl gas formed when zinc chloride hydrates are heated is the basis of qualitative inorganic spot tests.[29]

The use of zinc chloride as a flux, sometimes in a mixture with ammonium chloride (see also Zinc ammonium chloride), involves the production of HCl and its subsequent reaction with surface oxides. Zinc chloride forms two salts with ammonium chloride: (NH4)2ZnCl4 and (NH4)3ClZnCl4, which decompose on heating liberating HCl, just as zinc chloride hydrate does. The action of zinc chloride/ammonium chloride fluxes, for example, in the hot-dip galvanizing process produces H2 gas and ammonia fumes.[30]

Cellulose dissolves in aqueous solutions of ZnCl2, and zinc-cellulose complexes have been detected.[31] Cellulose also dissolves in molten ZnCl2 hydrate and carboxylation and acetylation performed on the cellulose polymer.[32]

Thus, although many zinc salts have different formulas and different crystal structures, these salts behave very similarly in aqueous solution. For example, solutions prepared from any of the polymorphs of ZnCl2, as well as other halides (bromide, iodide), and the sulfate can often be used interchangeably for the preparation of other zinc compounds. Illustrative is the preparation of zinc carbonate:

ZnCl2(aq) + Na2CO3(aq) → ZnCO3(s) + 2 NaCl(aq)

Applications

As a metallurgical flux

Zinc chloride has the ability to react with metal oxides (MO) to give derivatives of the formula MZnOCl2.[33][additional citation(s) needed] This reaction is relevant to the utility of ZnCl2 solution as a flux for soldering – it dissolves oxide coatings, exposing the clean metal surface.[33] Fluxes with ZnCl2 as an active ingredient are sometimes called “tinner’s fluid”. Typically this flux was prepared by dissolving zinc foil in dilute hydrochloric acid until the liquid ceased to evolve hydrogen; for this reason, such flux was once known as “killed spirits”. Because of its corrosive nature, this flux is not suitable for situations where any residue cannot be cleaned away, such as electronic work.[citation needed] This property also leads to its use in the manufacture of magnesia cements for dental fillings and certain mouthwashes as an active ingredient.

In organic synthesis

An early use of zinc chloride (Silzic) was in building carbon skeletons by condensation of methanol molecules. Unsaturated hydrocarbons are the major products, with reaction conditions influencing the distribution of products, though some aromatic compounds were formed.[34] In 1880, it was found that molten zinc chloride catalyses an aromatization reaction generating hexamethylbenzene. At the melting point of ZnCl2 (283 °C), the reaction has a ΔG = -1090 kJ/mol and can be idealised as[35]

15 CH

3OH → C

6(CH

6 + 3 CH

4 + 15 H

The discoverers of this reaction rationalized it as involving condensation of methylene units followed by complete Friedel-Crafts methylation of the resulting benzene ring with chloromethane generated in situ.[35] Such an alkylation transformation is an application of zinc chloride’s moderate strength as a Lewis acid, which is its principal role in laboratory synthesis. Other examples include catalyzing (A) the Fischer indole synthesis,[36] and also (B) Friedel-Crafts acylation reactions involving activated aromatic rings[37][38]

ZnCl2 aromatics.gif

Related to the latter is the classical preparation of the dye fluorescein from phthalic anhydride and resorcinol, which involves a Friedel-Crafts acylation.[39] This transformation has in fact been accomplished using even the hydrated ZnCl2 sample shown in the picture above.

ZnCl2 fluorescein.png

Hydrochloric acid alone reacts poorly with primary alcohols and secondary alcohols, but a combination of HCl with ZnCl2 (known together as the “Lucas reagent”) is effective for the preparation of alkyl chlorides. Typical reactions are conducted at 130 °C. This reaction probably proceeds via an SN2 mechanism with primary alcohols but SN1 pathway with secondary alcohols.

ZnCl2 Lucas.gif

Zinc chloride also activates benzylic and allylic halides towards substitution by weak nucleophiles such as alkenes:[40]

ZnCl2 benzylation.gif

In similar fashion, ZnCl2 promotes selective NaBH3CN reduction of tertiary, allylic or benzylic halides to the corresponding hydrocarbons.

Zinc chloride is also a useful starting reagent for the synthesis of many organozinc reagents, such as those used in the palladium catalyzed Negishi coupling with aryl halides or vinyl halides.[41] In such cases the organozinc compound is usually prepared by transmetallation from an organolithium or a Grignard reagent, for example:

ZnCl2 Negishi.gif

Zinc enolates, prepared from alkali metal enolates and ZnCl2, provide control of stereochemistry in aldol condensation reactions due to chelation on to the zinc. In the example shown below, the threo product was favored over the erythro by a factor of 5:1 when ZnCl2 in DME/ether was used.[42] The chelate is more stable when the bulky phenyl group is pseudo-equatorial rather than pseudo-axial, i.e., threo rather than erythro.

ZnCl2 aldol.gif

In textile and paper processing

Concentrated aqueous solutions of zinc chloride (more than 64% weight/weight zinc chloride in water) have the interesting property of dissolving starch, silk, and cellulose. Thus, such solutions cannot be filtered through standard filter papers. Relevant to its affinity for these materials, ZnCl2 is used as a fireproofing agent and in fabric “refresheners” such as Febreze. Vulcanized fibre is made by soaking paper in concentrated zinc chloride.

Smoke grenades

The zinc chloride smoke mixture (“HC”) used in smoke grenades contains zinc oxide, hexachloroethane and granular aluminium powder, which, when ignited, react to form zinc chloride, carbon and aluminium oxide smoke, an effective smoke screen.[43]

Fingerprint detection

Ninhydrin reacts with amino acids and amines to form a colored compound “Ruhemann’s purple” (RP). Spraying with a zinc chloride solution forms a 1:1 complex RP:ZnCl(H2O)2, which is more readily detected as it fluoresces better than Ruhemann’s purple.[44]

Disinfectant

Historically, a dilute aqueous solution of zinc chloride was used as a disinfectant under the name “Burnett’s Disinfecting Fluid”. [45] It is also used in some commercial brands of antiseptic mouthwash.

Skin cancer treatment

Zinc chloride has been used in alternative medicine to cause eschars, scabs of dead tissue, in an attempt to cure skin cancers.[46] Various products, such as Cansema or “black salve”, containing zinc chloride and sold as cancer cures have been listed by the U.S. Food and Drug Administration (FDA) as fake [47] with warning letters being sent to suppliers.[48]

Numerous reports in medical literature describe serious scarring and damage to normal skin by escharotic substances. Given these side-effects, its use in treatment is not warranted as there are much safer and more effective alternatives, such as radiation therapy and Mohs surgery.[49][50]

Safety

Zinc chloride is a skin irritant. After contact of the skin, immediate removal is necessary using soap and plenty of water. After contact of the eyes, adequate measures are rinsing with plenty of water or other eye rinse and contacting an ophthalmologist as soon as possible.[51]

Zinc chloride is caustic to the gastrointestinal tract, occasionally leading to hematemesis. Symptoms of acute intoxication are gastrointestinal distress, diarrhea, nausea, and abdominal pain. Vomiting occurs almost universally. The lethal dose in humans is 3-5 g.[citation needed] Decontamination of the gastrointestinal tract after oral uptake of zinc compounds is mostly unnecessary, since patients usually vomit sufficiently. Milk may be administered to decrease absorption of the metal. Zinc levels may be normalized with EDTA salts.[51]

Zinc chloride is extremely detrimental to the lungs, and pulmonary exposure to zinc chloride smoke has previously resulted in fatalities.[citation needed] Inhalation of fumes of zinc, zinc oxide, or zinc chloride leads to pulmonary edema and metal fume fever. Onset occurs within 4-6 h and may be delayed up to 8 h. Symptoms include rapid breathing, dyspnea, cough, fever, shivering, sweating, chest and leg pain, myalgias, fatigue, metallic taste, salivation, thirst, and leukocytosis, which can last from 24 to 48 h. In cases of fume inhalation, cortisone preparations should be applied immediately (e.g., by inhalation of Auxiloson) to avoid development of lung edema

About Zinc Chloride

High purity Zinc ChlorideChloride IonZinc Chloride is an excellent water soluble crystalline Zinc source for uses compatible with chlorides. Chloride compounds can conduct electricity when fused or dissolved in water. Chloride materials can be decomposed by electrolysis to chlorine gas and the metal. They are formed through various chlorination processes whereby at least one chlorine anion (Cl-) is covalently bonded to the relevant metal or cation. Ultra high purity and proprietary formulations can be prepared. The chloride ion controls fluid equilibrium and pH levels in metabolic systems. They can form either inorganic or organic compounds. Zinc Chloride is generally immediately available in most volumes. High purity, submicron and nanopowder forms may be considered. We also produce Zinc Chloride Solution. American Elements produces to many standard grades when applicable, including Mil Spec (military grade); ACS, Reagent and Technical Grade; Food, Agricultural and Pharmaceutical Grade; Optical Grade, USP and EP/BP (European Pharmacopoeia/British Pharmacopoeia) and follows applicable ASTM testing standards. Typical and custom packaging is available. Additional technical, research and safety (MSDS) information is available as is a Reference Calculator for converting relevant units of measurement.

Properties

vapor pressure 1 mmHg ( 428 °C)

assay ≥98%

mp 293 °C (lit.)

General description

Electrodeposition of zinc on glassy carbon and nickel substrates in zinc chloride-1-ethyl-3-methylimidazolium chloride molten salt is studied.[4]

Application

Zinc Chloride may be used:

• as catalyst in knoevenagel condensation of carbonyl substrates with acidic methylene reagents[3]

• in the preparation of porous carbon nanofibers, useful in the fabrication of efficient electrodes for supercapacitors[5]

• as a catalyst in preparation of poly(propylene fumarate)[6]

• in the low temperature synthesis of nanocrystalline zinc oxide films[1]

• in the synthesis of zinc oxide nanoparticles with low agglomeration. Aqueous suspensions of the nanoparticles displayed high transmittance in the visible light range, but exhibited strong absorption in the UV range.[2]

Compounds

In chemical compounds, zinc exhibits almost exclusively a +2 oxidation state. A few compounds of zinc in the +1 state have been reported, but never any compounds of zinc in the +3 state or higher.

Zinc chloride is a chemical compound whose formula is ZnCl2, with a molecular weight of 136.3 g / mol. This product is hygroscopic and deliquescent and therefore must be protected from moisture, even that contained in the atmosphere.

Applications:

One of the main applications of zinc chloride is to act as an electrolyte in dry batteries (zinc-carbon). Zinc chloride has the ability to attack the metal oxides, this property allowing its use as flux in the weld metal, dissolving the oxide layers, and leaving the metal surface clean. Zinc chloride is used in various fields such as water treatment, as a fireproofing agent in textile processing and in the manufacture of bactericides, fungicides and stabilizers for plastics.

This product can be manufactured in liquid form at any concentration up to 65% in solid form as a dry powder. The anhydrous material is packed in polyethylene valve bags of 25 or 50 Kgs, in big bags of 1.000 Kgs and in metal drums of 250 Kgs. The liquid material can be delivered in tankers or IBC’S of 1.000 lts. All the packaging we use is UN approved.

Zinc Chloride is an excellent water soluble crystalline Zinc source for uses compatible with chlorides. Chloride compounds can conduct electricity when fused or dissolved in water. Chloride materials can be decomposed by electrolysis to chlorine gas and the metal. They are formed through various chlorination processes whereby at least one chlorine anion (Cl-) is covalently bonded to the relevant metal or cation. Ultra high purity and proprietary formulations can be prepared. The chloride ion controls fluid equilibrium and pH levels in metabolic systems. They can form either inorganic or organic compounds. Zinc Chloride is generally immediately available in most volumes. High purity, submicron and nanopowder forms may be considered. We also produce Zinc Chloride Solution. American Elements produces to many standard grades when applicable, including Mil Spec (military grade); ACS, Reagent and Technical Grade; Food, Agricultural and Pharmaceutical Grade; Optical Grade, USP and EP/BP (European Pharmacopoeia/British Pharmacopoeia) and follows applicable ASTM testing standards. Typical and custom packaging is available.

Additional technical, research and safety (MSDS) information is available as is a Reference Calculator for

converting relevant units of measurement.

Butter of zinc

Zinc (chlorure de)

Zinc butter

Zinc chloride

EC Inventory, C&L Inventory, Pre-Registration process, Other, EU. Cosmetics Regulation, Annex III, Restricted Substances, EU. Worker Protection-Hazardous (98/24), EU. Dangerous Substances – Eco-Labels, EU. Workplace Signs, EU. Hazardous Waste Properties: Annex III (2008/98/EC), EU. Young People at Work (94/33)

Zinc chloride (ZnCl2)

Zinc chloride in plastic container

ZINC CHLORIDE SOLUTION

EU. ADN Dangerous Goods Lists, Directive 2008/68/EC, EU. ADR Dangerous Goods Lists, Directive 2008/68/EC, EU. RID Dangerous Goods Lists, Directive 2008/68/EC

Zinc chloride, (solution)

PROPERTIES of zinc chloride

-Physical Data of zinc chloride: mp 293 °C; bp 732 °C; d 2.907 g mL-1.

-Solubility of zinc chloride: sol H2O (432 g/100 g at 25 °C), EtOH (1 g/1.3 mL), glycerol (1 g/2 mL).

-Form Supplied in of zinc chloride:white, odorless, very deliquescent granules; principal impurities are H2O and zinc oxychloride.

-Analysis of Reagent Purity of zinc chloride: melting point

-Purification reflux (50 g) in dioxane (400 mL) in the presence of Zn0 dust, then filter hot and allow to cool to precipitate purified ZnCl2. Also, anhydrous material may be sublimed under a stream of dry HCl, followed by heating to 400 °C in a stream of dry N2.

-Handling, Storage, and Precautions: very hygroscopic; store under anhydrous conditions; moderately irritating to skin and mucous membranes.

The chemical formula of this material with bluish light gray ZnCl2, is a metal which is brittle white crystalline solid. Spilled although hard and brittle. Having a boiling temperature of water easily çözünür.düük makes widespread use of these substances. This value is pyro metallurgical especially in metal production is a very decisive factor. The world, in terms of the amount of iron use a year, aluminum, and comes after copper. available sources of zinc containing 48% zinc in the structure and in particular the local blood breaker.

Molecular Structure

Cl – Zn – Cl

Production and Reactions

Solid reaction of zinc with hydrochloric acid produced so as to be exposed hydrogen gas.

Zn (s) + 2HCl —- ZnCl2 + H2

Zinc chloride is the name of chemical compounds with the formula ZnCl2 and its hydrates. Zinc chlorides, of which nine crystalline forms are known, are colorless or white, and are highly soluble in water.ZnCl2 itself is hygroscopic and even deliquescent. Samples should therefore be protected from sources of moisture, including the water vapor present in ambient air. Zinc chloride finds wide application in textile processing, metallurgical fluxes, and chemical synthesis. No mineral with this chemical composition is known aside from the very rare mineral simonkolleite.

Zinc chloride chemical formula is ZnCl2 and its molar mass is 136.15 g mol-1. The zinc chloride molecule is a binary salt formed by the zinc cation Zn+2 and chloride anion Cl- and it can be found as anhydrous or tetrahydrated form. The structure may be tetrahedral or orthorhombic depended on the hydration state. Its chemical structure can be written as below, in the common representations used for organic molecules.Zinc chloride is a white hygroscopic crystalline solid. Its density is 1.01 g mL-1. Zinc chloride melting point is 162-172 ºC and its boiling point is 220 ºC. It is soluble in water, ethanol, glycerol and acetone. Zinc chloride is mostly thought as a ionic compound, however it has been determinate it has a behavior more covalent. The difference of electro-negativity between Zinc and Chloride is 1.3, which is not enough to form a strong ionic bond. For that reason the melting point (energy required to break the bonds) is lower than ionic salts as sodium chloride. The zinc chloride can react in diverse ways, all of them are similar to the reaction showed by the covalent compounds, for example: the formation of complex with water molecule or in the presence of alkali solution when are formed complex species.

Zinc chloride (ZnCl2) is an important compound and it is exists in its nine crystalline forms which are either colorless or white. It is actually a granular powder which we get by heating calcium chloride and zinc sulfate together. It has a specific gravity of 2.75, a pH of 4 and a burning taste. The anhydrous zinc chloride which is white is known for its solubility in water. This compound, which is deliquescent has several applications and the main uses include chemical synthesis and textile processing.

All those who use this compound should be aware of the safety measures which are to be followed for its daily use. Experts suggest that it should be kept in air tight containers and stored in cool and dry place. Also, while you use this chemical, you should use protective rubber gloves and goggles for your personal safety.

Zinc Chloride is a chemical compound that is constituted of zinc and chlorine. It is a granular crystalline powder that is also highly hygroscopic in nature. It is soluble in many mediums, like water, alcohol, glycerol, and ether.Zinc Chloride has numerous applications in different industries, including health care, pharmaceuticals, and paper manufacturing industry. It is also used in the chemical products formulation and manufacturing industry too.

Zinc chloride is a crystalline, hydroscopic powder of white or slightly greyish colour. The substance is odourless, well soluble in water, in alcohols, ether, glycerine and acetone. This high quality product can be made in anhydrous form (i.e. free flowing) or in solution at a concentration of at least 45 %.

Zinc Chloride is a white crystalline solid. In cosmetics and personal care products, Zinc Chloride is used in the formulation of dentifrices, mouthwashes, skin care products, hair conditioners and bath products.Zinc Chloride polishes the teeth, reduces oral odor, or otherwise cleanses or deodorizes the teeth and mouth. It is also applied topically for use in properly caring for the oral cavity. Zinc Chloride induces a tightening or tingling sensation of the skin and helps to cleanse the skin or to prevent odor by destroying or inhibiting the growth of microorganisms.

While the use of triphenylphosphine as a reductant is common in organic synthesis, the resulting triphenylphosphine oxide (TPPO) waste can be difficult to separate from the reaction product. While a number of strategies to precipitate TPPO are available, none have been reported to work in more polar solvents. We report here that mixing ZnCl2 with TPPO precipitates a TPPO-Zn complex in high yield in several common polar organic solvents. The solvent compatibility of this procedure and the reliability of the precipitation in the presence of polar functional groups were examined to show the utility and limitations of this method.

Zinc Chloride is also used by various chemical industries: for example, for making nylon, for the vulcanisation of cellulose fibres in paper making, for water treatment, for pharmaceuticals, and for surface treatment.It is also used as raw material for the production of other Zinc salts, for PVC and Calcium-Zinc stabilizers in particular.The zinc salt of hydrochloric acid, ZnCl2, a white crystalline solid with a number of industrial applications.

Intraperitoneal administration of zinc chloride (ZnCl2) to Swiss albino mice in vivo induced a significant (p≤0.05) increase in the frequencies of chromosomal aberrations of the bone-marrow cells at all concentrations used following acute (7.5, 10, 15 mg/kg body weight) and chronic (2.0, 3.0 mg/kg body wt) treatment. The degree of clastogenicity was directly proportional to the concentrations (p≤0.05, trend test) and indirectly to the period of treatment (p≤0.05, ANOVA test). It induced a dose-dependent, statistically significant increase (Mann-Whitney U statistics, student’st-test) in sperm-head abnormalities. The data designate ZnCl2 as a potent clastogen and as a toxic chemical at the concentrations used.

In its aqueous state, such as in a mouthwash, zinc chloride neutralizes the odor caused by bad breath germs for long-lasting fresh breath. It also works by controlling the growth of bad breath bacteria. It is also used in other temporary breath fresheners such as mints, sprays, lozenges and even chewing gum.

When zinc is burned in chlorine a solid substance is formed of a whitish gray colour, and semi-transparent. This is the only compound known of zinc and chlorine. It may likewise be made by heating together zinc filings and corrosive sublimate; it is as soft as wax, fuses at a temperature a little above 212 degrees, and rises in the gaseous form as heat much below the red heat. Its taste is acrid, and it corrodes the skin; it acts upon water and dissolves in it, producing much heat, and its solution decomposed by an alkali affords the white hydrated oxide of zinc. The compound of zinc and chlorine has been called butter of zinc and muriate of zinc; following the nomenclature already proposed its name will be zincane; from the experiments of my brother, Dr. John Davy, it consists of nearly equal parts of zinc and chlorine

In a simple and convenient way, mesoporous germanium nanoparticles (mp-Ge NPs) are prepared by a “metathesis” reaction of magnesium germanide (Mg2Ge) and zinc chloride (ZnCl2) in an autoclave at 300 °C. Investigated as anode materials for lithium-ion batteries, the prepared mp-Ge NPs exhibit a high capacity retention of 1048 mA h g-1 at 1 C after 1000 cycles and a high rate capacity of 727.1 mA h g-1 at 10 C in Li-Ge half cells. Additionally, a 3.4 V lithium-ion full cell (Ge-LiCoO2) with an energy retention of 85% (∼268.8 W h kg-1) over 100 cycles is achieved.

Also known as zinc dichloride or zinc (II) chloride, this chemical compound appears in nine different forms, all of them crystalline and either colorless or white. Its appearance in nature is very rare.Zinc chloride has a simple molecular formula consisting of a single zinc atom in an ionic bond with two chlorine atoms. However, this apparently simple arrangement can manifest various symmetries, such as tetragonal, monoclinic and orthorhombic forms.This compound is excellent for attacking most metal oxides. Therefore, it is used to clean metal surfaces. Mouthwash companies also make use of this substance as an active ingredient. However, it is corrosive and should only be used when it is possible to clean it off completely.Since this compound is an irritant on the skin and in the human respiratory system, users must take great care with it. It acts as an acid in concentrated form.

Fixation with zinc chloride is probably similar to that with mercuric chloride, They are both group 12 elements in the periodic table, along with cadmium, but the mechanism does not appear to have been commented on apart from that.

It had been recommended long ago as a fixing agent, but was not popular. Most likely this was because it is inferior to mercuric chloride and microscopists preferred the results from using that. Recently, however, as mercuric chloride began to be criticised as a fixing agent because of its toxicity and the effect of disposal on the environment, a search for possible substitutes led to zinc chloride which, it was claimed at first, was as good as the former and a lot less toxic. It is true that it is a lot less toxic, but it does not live up to the claims initially made in its favour. It is a good fixing agent but it falls short of what has been claimed for it. What is needed is a thorough, objective evaluation of its fixation characteristics so that some definitive information is available.

Physicians, military and civilian alike, may be called upon to recognize, treat, and provide long-term care to patients who have suffered a zinc chloride (smoke bomb) inhalational injury. Pathologic changes described in the literature include laryngeal, tracheal, and bronchial mucosal edema and ulceration; interstitial edema; interstitial fibrosis; alveolar obliteration; and bronchiolitis obliterans. Acute injury is associated with a high mortality. Following is a report of a patient with a zinc chloride smoke injury which resulted in subpleural emphysematous blebs complicated by pneumothorax and abnormal exercise physiology. Gradual recovery occurred over several months. However, the chest roentgenogram remains abnormal with emphysematous blebs.

White deliquescent granules or fused pieces. Zinc chloride acts an astringent and antiseptic and has been used to deodorize, disinfect, and embalm specimens. It is used on wood for preservation and fireproofing. With metals, zinc chloride can act as a flux, etchant, cement, and colorant. For textiles, it has been used to mercerize cotton, weight fabrics, mordant dyes, and vulcanize rubber. It is also used in the manufacture of artificial silk, dyes, cold-water glue, and magnesia cements. As a microscopy reagent, zinc chloride is used to separate silk, wool, and plant fibers

APPLICATIONS

·Organic product synthesis – Synthesis of organic products in the laboratory, mainly as a moderate strength Lewis acid reaction, and several other reactions.

·Textile processing industry – 64% zinc chloride in water is used to dissolve starch, silk, and cellulose. It has many other applications in textile processing industry.

·Dry cell: It is used in dry cell batteries as an electrolyte.

·Petroleum: It is a powerful emulsion breaker. It separates oil from water

·Chemical industryit is used to prepare ethyl acetate. It is also used in the manufacturing of dyes, and many other industrial intermediate chemicals.

·Medicine: It located in the composition of some ointment that can be sold without a prescription.

·Health: It is also used in the treatment of very small amounts will come out of the skin using the redness and irritation of connecting glands önlemektedir.bebek önleyebilir.göz disease in the dehydrated skin when applied as a thin layer.

·Rubber:In the rubber industry it is used as activator.

·Textile: This sector is used as a mordant in textile dyeing.

·Chemistry: water is used in chemical synthesis as attractive.

·Battery: Batteries are used as components in the construction of housing help.

ÇNKO KLORÜR

Görünümü : Beyaz Kristal Haldedir, Higroskopiktir.

Çinko klorür Kimyasal Ad : Zinc Chloride

Çinko klorür Kimyasal Formülü : ZnCl2

Çinko klorür Özellikleri : Suda ÇOK RAHAT ÇÖZÜNÜR.

Çinko klorür Ambalaj ekli : 25 Kg. lk Torbalarda

Çinko klorür Tanm ve Kullanm Alanlar :

Çinko tereya olarak da bilinen çinko (II) klorür, suda çok çözünen ve çounlukla katalizör olarak ve dezenfektan olarak organik sentezde kullanlan inorganik bir tuzdur.

Çinko klorür çounlukla iyonik bir bileik olarak düünülür ancak daha kovalent bir davrana sahip olduu belirlenmitir. Çinko klorür, çeitli ekillerde reaksiyona girebilir, hepsi de kovalent bileikler tarafndan gösterilen reaksiyona benzer: örnein su molekülü ile kompleks oluumu veya alkali çözeltinin varlnda aadaki gibi kompleks türler oluur: Zn ( OH) 3 Cl 2- , Zn (OH) 2 Cl 2- veya ZnOHCl 2- .

Çinko, dünyada yllk kullanm miktar açsndan demir, alüminyum, ve bakrdan sonra gelir.

Çinko klorür Kullanm Alanlar

Korozyondan korunma amacyla, çelik gibi dier metallerin galvanize edilmesinde,

Pirinç, nikelli gümü, deiik lehimler, alman gümüü gibi alamlarn yapmnda,

Genellikle otomotiv endüstrisinde döküm kalplarnda,

Pillerin gövdelerinin yapmnda kullanlr.

Çinko oksit, sulu boyalarda beyaz pigment olarak ve lastik sanayinde aktivatör olarak kullanlr.

Reçetesiz satlabilen baz merhemlerin bileiminde bulunur ve ince bir tabaka halinde uygulandnda cildin su kaybetmesini önler. Yazn güne, kn da souk yanklarna kar koruyucudur. Bebeklerin bez balanan bölgelerinde çok az miktarda kullanlarak ciltte meydana gelebilecek kzarklklar önlenebilir.

Yaa bal göz hastalklarnn tedavisinde de kullanlr.

Çinko klorür, deodorantlarda ve ahap koruyucu olarak kullanlr.

Çinko sülfür, karanlkta parlayan pigment olarak saatlerin akrep ve yelkovanlarnda kullanlr.

Çinko metil, (Zn(CH3)2) pek çok organik maddenin sentezinde kullanlr.

Çinko, dünyada yllk kullanm miktar açsndan demir, alüminyum, ve bakrdan sonra gelir.

Çinko klorür Kullanm Alanlar

Çinko klorür Korozyondan korunma amacyla, çelik gibi dier metallerin galvanize edilmesinde,

Çinko klorür Pirinç, nikelli gümü, deiik lehimler, alman gümüü gibi alamlarn yapmnda,

Çinko klorür Genellikle otomotiv endüstrisinde döküm kalplarnda,

Çinko klorür Pillerin gövdelerinin yapmnda kullanlr.

Çinko oksit, sulu boyalarda beyaz pigment olarak ve lastik sanayinde aktivatör olarak kullanlr.

Yaa bal göz hastalklarnn tedavisinde de kullanlr.

Çinko klorür, deodorantlarda ve ahap koruyucu olarak kullanlr.

Çinko sülfür, karanlkta parlayan pigment olarak saatlerin akrep ve yelkovanlarnda kullanlr.

Çinko klorür addr kimyasal bileikler ile , formül ZnC 2 ve hidratlar. Dokuz kristal formu bilinen çinko klorürler renksiz veya beyazdr ve suda oldukça çözünürdür . ZnC 2 kendisidir higroskopik ve hatta nem alabilen . Bu nedenle numuneler, ortam havasnda bulunan su buhar dahil olmak üzere nem kaynaklarndan korunmaldr. Çinko klorür, tekstil ilemede, metalurjik aklarda ve kimyasal sentezde geni uygulama alan bulur . Çok nadir bulunan simonkolleit minerali Zn 5 (OH) 8 Cl 2 · H 2 O dnda bu kimyasal bileime sahip hiçbir mineral bilinmemektedir .

Çinko klorür Hazrlama ve saflatrma

Susuz ZnCl 2 çinko ve hazrlanabilir hidrojen klorür :

Zn (k) + 2 HCl → ZnCl 2 + H 2 (g)

Hidratlanm formlar ve sulu çözeltiler, Zn metalinin hidroklorik asit ile ilenmesiyle benzer ekilde kolayca hazrlanabilir. Çinko oksit ve çinko sülfür , HCl ile reaksiyona girer:

ZnS ( k ) + 2 HCl (sulu) → ZnCl 2 (sulu) + H 2 S ( g )

Dier birçok elementten farkl olarak, çinko esasen yalnzca bir oksidasyon durumunda bulunur, 2+, bu da klorürün saflatrlmasn basitletirir.

Ticari çinko klorür numuneleri tipik olarak su ve hidrolizden elde edilen ürünleri safszlk olarak içerir. Bu tür numuneler, scak dioksandan yeniden kristalletirme ile saflatrlabilir . Susuz numuneler, bir hidrojen klorür gaz aknda süblimasyon yoluyla saflatrlabilir , ardndan süblimasyon bir kuru nitrojen gaz ak içinde 400 ° C’ye stlabilir . Son olarak, en basit yöntem çinko klorürün tiyonil klorür ile ilenmesine dayanr .

Çinko klorür Tepkiler

ZnCl susuz Erimi 2 eriyik soutma hzl üzerinde, 500-700 ° C çözünene çinko metali de, ve san bir diyamanyetik cam Raman çalmalar içerir göstermektedir oluturulmaktadr ki, Zn2+

2 iyon.

Tetraklorozinkate anyon, Zn Cl içeren bir dizi tuz2-

4biliniyor. “Caulton reaktifi”, V 2 Cl 3 (thf) 6 Zn 2 Cl 6 , Zn 2 Cl içeren bir tuz örneidir2-

6. Bileik Cs 3 ZnCl 5 tetrahedral Zn içeren Cl2-

4ve Cl – anyonlar. Zn Cl içeren bileik yok4-

6 iyon karakterize edilmitir.

Çinko klorür suda çok çözünür olmasna ramen, çözeltilerin basitçe çözülmü Zn 2+ iyonlar ve Cl – iyonlar içerdii düünülemez , ZnCl x H 2 O (4- x ) türleri de mevcuttur. ZnCI ‘nin sulu çözeltiler 2 asidik olan bir 6: M sulu çözelti olan pH , sulu ZnC asiditesi 1 olarak 2 dier Zn çözeltilerine göre çözümler 2+ seviyesinin olumas nedeni tuzlar tetrahedral kloro su kompleksleri burada azalma 6’dan 4’e kadar koordinasyon says, çözülmü su moleküllerindeki O – H balarnn gücünü daha da azaltr.

OH varlnda alkali çözeltisi içinde – iyon çeitli çinko hidroksiklorit anyonlar, örnein, Zn (OH) çözeltisi içinde mevcut olan 3 C 2- , Zn (OH) 2 Cl2-

2, ZnOH Cl2-

3Ve Zn 5 (OH) 8 C 2 -h 2 O (simonkolleite) çökelir.

Amonyak bir çinko klorür çözeltisi içinden kabarcklar halinde olduunda, hidroksit yerine, Zn (NH üretilen kompleks amonyak (ammines) ihtiva eden bileikler, çökelti yapan 3 ) 4 CI 2 -h 2 O ve konsantrasyona ZnC 2 (NH 3 ) 2 . lki, Zn (NH 3 ) 6 2+ iyonunu içerir ve ikincisi, bozulmu bir tetrahedral geometriye sahip molekülerdir. Sulu çözelti içerisindeki türler aratrlm ve Zn (NH 3 ) 4 2+ ‘ nin, daha düük NH 3 : Zn orannda da bulunan Zn (NH 3 ) 3 Cl + ile birlikte bulunan ana tür olduunu göstermitir .

Sulu çinko klorür, ilk kez 1855’te Stanislas Sorel tarafndan aratrlan amorf bir çimento oluturmak için çinko oksit ile reaksiyona girer . Sorel daha sonra kendi adn tayan ilgili magnezyum oksiklorür çimentosunu aratrmaya devam etti.

Hidratl çinko klorür stldnda, bir Zn (OH) Cl kalnts elde edilir, örn.

ZnCl 2 · 2H 2 O → ZnCl (OH) + HCl + H 2 O

Bileik ZnCl 2 · 1 / 2 HCI · H 2 O ZnCI ‘nin bir çözeltiden dikkat çökeltme ile hazrlanabilir 2 HCI ile asidifiye edilmitir. Dengeleyici monohidratl hidronyum iyonlar, H 5 O 2 + iyonlar ile polimerik bir anyon (Zn 2 Cl 5 – ) n içerir .

Çinko klorür hidratlar stldnda oluan yüksek reaktif susuz HCl gaznn oluumu, kalitatif inorganik spot testlerinin temelini oluturur.

Çinko klorürün bir ak olarak, bazen amonyum klorür ile bir karm halinde kullanlmas (ayrca bkz. Çinko amonyum klorür ), HCl üretimini ve bunun ardndan yüzey oksitlerle reaksiyonunu içerir. Çinko klorür formlar amonyum klorür ile iki tuzlar (NH 4 ) 2 ZnCI 4 ve (NH 4 ) 3 ClZnCl 4 , çinko klorür hidrat yapt gibi, serbest HCl stma üzerine ayrmaktadr. Aksiyonu çinko klorür / amonyum klorit tozlar, örnein, scak daldrma galvaniz ileminde H üretir 2 gaz ve amonyak duman.

ZnCI ‘nin sulu çözeltiler içinde Selüloz çözünür 2 ve çinko-selüloz kompleksleri tespit edilmitir. Selüloz da erimi ZnCl içinde çözülür 2 hidrat ve karboksilasyon ve asetilasyon selüloz polimeri ile yaplmtr.

Bu nedenle, birçok çinko tuzunun farkl formüllere ve farkl kristal yaplara sahip olmasna ramen , bu tuzlar sulu çözelti içinde çok benzer ekilde davranr. Örnein, çözeltiler ZnCI polimorflann her hazrlanan 2 , hem de dier halojenürler (bromür, iyodür) ve sülfat genellikle dier çinko bileiklerinin hazrlanmas için birbirlerinin yerine kullanlabilir. Örnek, çinko karbonatn hazrlanmasdr:

Metalurjik bir ak olarak

Çinko klorür, MZnOCl 2 formülünün türevlerini vermek için metal oksitlerle (MO) reaksiyona girme yeteneine sahiptir . Bu reaksiyon, ZnCl yarar alakal 2 bir ekilde çözelti ak için lehimleme – temiz bir metal yüzeye aça oksit kaplamalarn çözer. ZnCI ile Cerayanlar 2 aktif madde olarak bazen “kalayc en akkan” olarak adlandrlr. Tipik olarak bu fluks, çinko folyonun , sv hidrojeni gelitirmeyi brakana kadar seyreltik hidroklorik asit içinde çözülmesiyle hazrland ; bu nedenle, bu tür bir ak bir zamanlar “öldürülmü ruhlar” olarak biliniyordu. Korozif yaps nedeniyle bu ak, elektronik iler gibi herhangi bir kalntnn temizlenemedii durumlar için uygun deildir. Bu özellik ayrca di dolgular için magnezya simanlarnn ve aktif bileen olarak baz az gargaralarnn imalatnda kullanlmasna yol açar .

Çinko klorür Organik sentezde

Çinko klorürün (Silzic) ilk kullanmlarndan biri, metanol moleküllerinin younlamasyla karbon iskeletlerini oluturmakt . Doymam hidrokarbonlar , baz aromatik bileikler olumasna ramen, ürünlerin dalmn etkileyen reaksiyon koullar ile ana ürünlerdir . 1880’de, erimi çinko klorürün, heksametilbenzen üreten bir aromatizasyon reaksiyonunu katalize ettii bulundu . ZnCI erime noktasnda 2 (283 ° C) reaksiyon, bir yer alr Δ G = -1090 kJ / mol olarak temsil edilebilir

Cilt kanseri tedavisinde Çinko klorür

Çinko klorür, alternatif tpta , cilt kanserlerini iyiletirmek amacyla eskarlara , ölü doku kabuklarna neden olmak için kullanlmtr . Cansema veya “siyah merhem” gibi çinko klorür içeren ve kanser tedavisi olarak satlan çeitli ürünler ABD Gda ve laç Dairesi (FDA) tarafndan tedarikçilere uyar mektuplar gönderilerek sahte olarak listelendi .

Tbbi literatürdeki çok sayda rapor, eskarotik maddeler tarafndan normal ciltte ciddi yara izi ve hasar tanmlar. Bu yan etkiler göz önüne alndnda, radyasyon tedavisi ve Mohs cerrahisi gibi çok daha güvenli ve daha etkili alternatifler olduu için tedavide kullanm garanti edilmez .

Emniyet

Çinko klorür cildi tahri edicidir. Ciltle temas ettikten sonra derhal sabun ve bol su ile uzaklatrlmas gerekir. Gözlerle temastan sonra, yeterli önlemler bol su ile ykamak veya baka bir göz ykamak ve mümkün olan en ksa sürede bir göz doktoruna bavurmaktr .

Çinko klorür gastrointestinal sistem için kostiktir ve bazen hematemeze yol açar . Akut zehirlenmenin belirtileri mide-barsak rahatszl, ishal, bulant ve karn arsdr. Kusma neredeyse evrensel olarak gerçekleir. nsanlarda öldürücü doz 3-5 gramdr. Çinko bileiklerinin oral almndan sonra gastrointestinal sistemin dekontaminasyonu çounlukla gereksizdir, çünkü hastalar genellikle yeterince kusarlar. Metalin emilimini azaltmak için süt verilebilir. Çinko seviyeleri EDTA tuzlar ile normalize edilebilir .

Çinko klorür akcierler için son derece zararldr ve akcierlerin çinko klorür dumanna maruz kalmas daha önce ölümlerle sonuçlanmtr. Çinko, çinko oksit veya çinko klorür dumanlarnn solunmas akcier ödemine ve metal duman ateine yol açar . Balangç 4-6 saat içinde olur ve 8 saate kadar gecikebilir. Semptomlar hzl nefes alma, nefes darl , öksürük, ate, titreme, terleme, göüs ve bacak ars, miyalji , yorgunluk, metal tad, tükürük, susuzluk ve 24 ila 48 saat sürebilen lökositozu içerir. Duman inhalasyonu durumlarnda , akcier ödeminin gelimesini önlemek için kortizon preparatlar hemen uygulanmaldr (örn. Auxiloson inhalasyonu ile ).

Çinko klorür, ZnCl2 formülü ve hidratlar ile kimyasal bileiklerin addr. Dokuz kristalin formunun bilindii çinko klorürler renksiz veya beyazdr ve suda çok çözünürler. ZnCl2’nin kendisi higroskopik ve hatta kesindir. Bu nedenle numuneler, ortam havasnda bulunan su buhar da dahil olmak üzere nem kaynaklarndan korunmaldr. Çinko klorür, tekstil ileme, metalurjik akkanlar ve kimyasal sentezlerde geni bir uygulama alan bulur. Bu kimyasal bileime sahip hiçbir mineral, çok nadir mineral simonkolleitinden bilinmemektedir.

Çinko klorür kimyasal formülü ZnCl2’dir ve molar kütlesi 136.15 g mol-1’dir. Çinko klorür molekülü, Zn + 2 ve klorür anyonu Cl- ile oluturulan ikili bir tuz olup, susuz veya tetrahidlenmi formda bulunabilir. Yap, hidrasyon durumuna bal olarak tetrahedral veya ortorombik olabilir. Kimyasal yaps, aadaki gibi, organik moleküller için kullanlan ortak sunumlarda yazlabilir.Zinc klorür, beyaz higroskopik kristal bir katdr. Younluu 1.01 g mL-1’dir. Çinko klorür erime noktas 162-172 ºC’dir ve kaynama noktas 220 ºC’dir. Su, etanol, gliserol ve asetonda çözünür. Çinko klorür çounlukla iyonik bir bileik olarak düünülür, ancak daha kovalent bir davrana sahip olduu belirlenmitir. Çinko ve Klorür arasndaki elektro-negatifliin fark, güçlü iyonik ba oluturmak için yeterli olmayan 1.3’dür. Bu nedenle erime noktas (balar krmak için gereken enerji) sodyum klorür gibi iyonik tuzlardan daha düüktür. Çinko klorür çeitli yollarla reaksiyona girebilir, hepsi kovalent bileikler tarafndan gösterilen reaksiyona benzerdir, örnein: kompleks moleküller oluturulduunda su molekülü veya alkali çözeltisinin varlnda kompleks oluumu.

Çinko klorür (ZnCl2) önemli bir bileiktir ve renksiz veya beyaz olan dokuz kristal formunda bulunur. Aslnda kalsiyum klorür ve çinko sülfatn birlikte stlmasyla elde edilen granül bir tozdur. 2.75 özgül arl, pH deeri 4 ve yanan tad vardr. Beyaz olan susuz çinko klorür, suda çözünürlüü için bilinir. arküteri olan bu bileiin çeitli uygulamalar vardr ve ana kullanmlar arasnda kimyasal sentez ve tekstil ileme yer alr.

Bu bileii kullananlarn tümü, günlük kullanm için izlenecek güvenlik önlemlerinin farknda olmaldr. Uzmanlar, hava geçirmez kaplarda tutulmasn ve serin ve kuru yerde saklanmasn önermektedir. Ayrca, bu kimyasal maddeyi kullanrken, kiisel güvenliiniz için koruyucu lastik eldiven ve gözlük kullanmalsnz.

Çinko Klorür, çinko ve klorden oluan kimyasal bir bileiktir. Doada oldukça higroskopik olan granüler kristal bir tozdur. Su, alkol, gliserol ve eter gibi birçok ortamda çözünür. Zink Chloride, salk, eczaclk ve kat imalat endüstrisi dahil olmak üzere farkl endüstrilerde çok sayda uygulamaya sahiptir. Ayn zamanda kimyasal ürün formülasyonu ve imalat sanayinde de kullanlmaktadr.

Çinko klorür beyaz veya hafif grimsi renkli kristalin, hidroskopik bir tozdur. Madde kokusuzdur, suda iyi çözünür, alkol, eter, gliserin ve asetonda bulunur. Bu yüksek kaliteli ürün susuz formda (yani serbest akl) veya solüsyonda en az% 45’lik bir konsantrasyonda yaplabilir.

Çinko Klorür beyaz kristal bir katdr. Kozmetik ve kiisel bakm ürünlerinde, Çinko Klorür, di bakm ürünleri, az gargaralar, cilt bakm ürünleri, saç kremleri ve banyo ürünlerinin formüle edilmesinde kullanlr. Zink Chloride dileri parlatr, az kokusunu azaltr veya dileri ve az temizler veya deodorize eder. Ayn zamanda az boluu için uygun bakmda kullanlmak üzere topikal olarak uygulanr. Çinko Klorür cildin sklaan veya karncalanma hissini uyandrr ve mikroorganizmalarn büyümesini yok ederek veya engelleyerek cildi temizlemeye veya kokuyu önlemeye yardmc olur.

Organik sentezde trifenilfosfinin bir indirgeyici olarak kullanlmas yaygn olmasna ramen, ortaya çkan trifenilfosfin oksit (TPPO) atnn reaksiyon ürününden ayrlmas zor olabilir. TPPO’yu çökeltmek için bir takm stratejiler mevcut olmasna ramen, hiçbiri daha polar çözücülerde çallmad bildirilmitir. Burada ZnCl2’nin TPPO ile kartrlmasnn bir çok yaygn polar organik çözücü içinde yüksek verimde bir TPPO-Zn kompleksi çökeltiini bildiriyoruz. Bu yöntemin çözücü uyumluluu ve polar fonksiyonel gruplarn varlnda çökelme güvenilirlii, bu yöntemin fayda ve snrlarn gösterecek ekilde incelendi.

Çinko Klorür ayrca çeitli kimyasal endüstriler tarafndan da kullanlr: örnein, naylon yapmnda, kat yapmnda selüloz liflerinin vulkanizasyonu, su artma, ilaç ve yüzey ilemleri için kullanlr. Özellikle PVC ve Kalsiyum-Çinko stabilizatörleri için dier çinko tuzlar. Hidroklorik asitin çinko tuzu, ZnCl2, bir dizi endüstriyel uygulama ile beyaz kristal bir kat.

Çinko Klorür, klorürlerle uyumlu kullanm için mükemmel bir suda çözünür kristal Çinko kaynadr. Klorür bileikleri, su içinde kaynatnda veya çözündüklerinde elektrik yapabilirler. Klorür materyalleri elektrolizle klor gazna ve metale ayrlabilir. En az bir klor anyonunun (Cl-) ilgili metal veya katyona kovalent olarak baland çeitli klorinasyon ilemleriyle oluturulurlar. Ultra yüksek saflk ve tescilli formülasyonlar hazrlanabilir. Klorür iyonu metabolik sistemlerde sv dengesini ve pH seviyelerini kontrol eder. norganik veya organik bileikler oluturabilirler. Çinko Klorür genellikle çou ciltte hemen mevcuttur. Yüksek saflk, mikron alt ve nanopowder formlar düünülebilir. Ayrca Çinko Klorür Çözeltisi üretiyoruz. American Elements, Mil Spec (askeri snf) dahil olmak üzere, uygulanabilir olduunda birçok standart kaliteye; ACS, Reaktif ve Teknik Snf; Gda, Tarm ve laç Snf; Optik Snf, USP ve EP / BP (Avrupa Farmakopesi / ngiliz Farmakopesi) ve geçerli ASTM test standartlarn takip eder. Tipik ve özel ambalajlar mevcuttur. Ek teknik, aratrma ve güvenlik (MSDS) bilgileri, ilgili ölçüm birimlerini dönütürmek için bir Referans Hesaplayc olarak mevcuttur.

Çinko klorürün (ZnCl2), in vivo olarak sviçre albino farelerine intraperitonal uygulanmas, akut (7.5, 10, 15 mg / kg) takiben kullanlan tüm konsantrasyonlarda kemik ilii hücrelerinin kromozomal anormallikleri frekanslarnda anlaml (p <0.05) bir arta neden oldu. vücut arl) ve kronik (2.0, 3.0 mg / kg vücut arl) tedavisi. Klastojenisitenin derecesi, konsantrasyonlarla (p = 0.05, trend testi) ve dolayl olarak tedavi periyodu ile doru orantlyd (p≤0.05, ANOVA testi). Sperm ba anormalliklerinde doz baml, istatistiksel olarak anlaml bir art (Mann-Whitney U istatistikleri, student’st-test) indüklemitir. Veriler, ZnCl2’yi güçlü bir klastojen olarak ve kullanlan konsantrasyonlarda toksik bir kimyasal olarak tanmlar.

Bir gargarada olduu gibi sulu durumunda, çinko klorür uzun süreli taze nefes için kötü nefes mikroplarnn neden olduu kokuyu etkisiz hale getirir. Ayrca kötü nefes bakterilerinin büyümesini kontrol ederek çalr. Ayn zamanda darphane, sprey, pastil ve hatta sakz gibi dier geçici soluma tatlandrclarnda da kullanlr.

Çinko klor içinde yakldnda, kat bir madde beyazms gri bir renkten oluur ve yar saydamdr. Bu çinko ve klorun bilinen tek bileiidir. Ayn ekilde çinko kaplamalar ve andrc süblimasyonu birlikte stmak suretiyle de yaplabilir; balmumu kadar yumuaktr, 212 derecenin biraz üzerinde bir scaklkta füzyonlar ve krmz sdan çok daha fazla s olarak gaz biçiminde yükselir. Tad acur ve cildi korozyona uratr; suyun üzerine hareket eder ve içinde erir, fazla s üretir ve bir alkali tarafndan ayrtrlan çözeltisi, beyaz hidratl çinko oksitini verir. Çinko ve klorin bileiine çinko tereya ve çinko çürüü denir; isimlendirmeyi takiben ad daha önce ad zinkan olacaktr; kardeim Dr. John Davy’in deneylerinden, neredeyse eit çinko ve klor parçalarndan oluuyor

Çinko diklorür veya çinko (II) klorür olarak da bilinen bu kimyasal bileik, hepsi kristalli ve renksiz veya beyaz olmak üzere dokuz farkl biçimde ortaya çkar. Doada görünümü çok nadirdir. Zink klorür, iki klor atomu ile iyonik bada tek bir çinko atomundan oluan basit bir moleküler formüle sahiptir. Bununla birlikte, bu görünüte basit bir düzenleme, tetragonal, monoklinik ve ortorombik formlar gibi çeitli simetriler gösterebilir. Bu bileik, çou metal okside saldran için mükemmeldir. Bu nedenle, metal yüzeylerin temizlenmesi için kullanlr. Az sular irketleri de bu maddeyi aktif bir bileen olarak kullanrlar. Ancak, andrcdr ve sadece tamamen temizlenebilir olduunda kullanlmaldr. Bu bileiin ciltte ve insan solunum sisteminde tahri edici olmas nedeniyle, kullanclar buna büyük özen göstermelidir. Konsantre olarak bir asit gibi davranr.

Çinko klorür ile fiksasyon muhtemelen mercurik klorür ile benzerdir, her ikisi de periyodik tabloda, kadmiyum ile birlikte grup 12 elementlerdir, ancak mekanizmann bundan ayr yorumlanm gibi görünmemektedir.

Bir tamirci olarak uzun zaman önce önerilmiti, ancak popüler deildi. Muhtemelen bunun nedeni, mermik klorürden daha düük olmas ve mikroskobistlerin sonuçlar kullanmasn tercih etmeleriydi. Bununla birlikte, son zamanlarda, merhem klorürün toksisitesi ve bertarafn çevre üzerindeki etkisi nedeniyle bir sabitleme maddesi olarak eletirilmeye balamasyla, muhtemel ikame maddelerinin aranmas, ilk bata olduu iddia edilen çinko klorürün ortaya çkmasna neden olmutur. eski ve çok daha az zehirli. Çok daha az toksik olduu dorudur, ancak balangçta kendi lehine yaplan iddialara kadar yaamaz. yi bir sabitleme maddesidir ancak bunun için talep edilenin yetersiz kalmasdr. htiyaç duyulan ey, baz kesin bilginin mevcut olmas için sabitleme özelliklerinin kapsaml, objektif bir deerlendirmesidir.

Çinko klorürlü (duman bombas) inhalasyon yaralanmasna maruz kalan hastalara uzun süreli bakm, tan ve tedavi için doktorlar, askeri ve sivil olarak çarlabilirler. Literatürde tarif edilen patolojik deiiklikler arasnda laringeal, trakeal ve broniyal mukozal ödem ve ülserasyon; interstisyel ödem; interstisyel fibroz; alveoler obliterasyon; ve broniyolit obliterans. Akut yaralanma, yüksek mortalite ile ilikilidir. Aada, çinko klorürlü duman yaralanmas olan bir hastann pnömotoraks ve anormal egzersiz fizyolojisi ile komplike olan subplevral amfizematöz kabarcklara neden olduu bildirilmitir. Kademeli iyileme birkaç ay içinde meydana geldi. Bununla birlikte, göüste roentgenogram, amfizematöz blebler ile anormal kalr.

Beyaz parçal granüller veya kaynam parçalar. Çinko klorür, bir büzücü ve antiseptik etki eder ve örnekleri deodorize etmek, dezenfekte etmek ve embalmek için kullanlr. Koruma ve atee dayankllk için ahap üzerinde kullanlr. Metaller ile, çinko klorür bir ak, erozyon, çimento ve renklendirici olarak hareket edebilir. Tekstil için pamuk, arlk kumalar, mordan boyalar ve vulkanize kauçuun merserize edilmesi için kullanlmtr. Yapay ipek, boyalar, souk su tutkal ve magnezya çimentolarnn üretiminde de kullanlr. Mikroskopi reaktifi olarak, ipek, yün ve bitki liflerini ayrmak için çinko klorür kullanlr.

Çinko klorür, ZnCl2 formülüne ve hidratlarna sahip kimyasal bileiklerin addr. Dokuz kristalli formu bilinen

çinko klorürler renksiz veya beyazdr ve suda oldukça çözünürdür. ZnCl2’nin kendisi higroskopiktir ve hatta

svlar. Bu nedenle numuneler, ortam havasnda bulunan su buhar dahil olmak üzere nem kaynaklarndan

korunmaldr. Çinko klorür, tekstil ilemede, metalurjik aklarda ve kimyasal sentezde geni uygulama alan

bulur. Çok nadir bulunan simonkolleit minerali Zn5 (OH) 8Cl2 · H2O dnda bu kimyasal bileime sahip hiçbir

mineral bilinmemektedir.

Çinko Klorür, klorürlerle uyumlu kullanmlar için mükemmel bir suda çözünür kristalli Çinko kaynadr. Klorür bileikleri, suda kaynatnda veya çözündüünde elektrik iletebilir. Klorid malzemeleri elektroliz yoluyla klor gazna ve metale ayrtrlabilir. En az bir klor anyonunun (Cl-) ilgili metale veya katyona kovalent olarak baland çeitli klorlama ilemleriyle oluturulurlar. Ultra yüksek saflkta ve tescilli formülasyonlar hazrlanabilir. Klorür iyonu, metabolik sistemlerde sv dengesini ve pH seviyelerini kontrol eder. norganik veya organik bileikler oluturabilirler. Çinko Klorür, çou ciltte genellikle hemen bulunur. Yüksek saflk, mikron alt ve nano toz formlar düünülebilir. Ayrca Çinko Klorür Çözeltisi üretiyoruz. American Elements, uygulanabilir olduunda, Mil Spec (askeri snf) dahil olmak üzere birçok standart snfta üretim yapar; ACS, Reaktif ve Teknik Snf; Gda, Tarm ve laç Derecesi; Optik Snf, USP ve EP / BP (Avrupa Farmakopesi / ngiliz Farmakopesi) ve ilgili ASTM test standartlarn takip eder. Tipik ve özel paketleme mevcuttur. lgili ölçüm birimlerini dönütürmek için bir Referans Hesaplayc olduu gibi ek teknik, aratrma ve güvenlik (MSDS) bilgileri mevcuttur.

Susuz ZnCl2 çinko ve hidrojen klorürden hazrlanabilir:

Zn (k) + 2 HCl → ZnCl2 + H2 (g)

Hidratlanm formlar ve sulu çözeltiler, Zn metalinin hidroklorik asit ile ilenmesiyle benzer ekilde kolayca

hazrlanabilir. Çinko oksit ve çinko sülfür, HCl ile reaksiyona girer:

ZnS (k) + 2 HCl (sulu) → ZnCl2 (sulu) + H2S (g)

Dier birçok elementten farkl olarak, çinko esasen yalnzca bir oksidasyon durumunda bulunur, 2+, bu da klorürün

saflatrlmasn kolaylatrr.

Ticari çinko klorür numuneleri tipik olarak su ve hidrolizden elde edilen ürünleri safszlk olarak içerir. Bu tür

numuneler, scak dioksandan yeniden kristalletirme ile saflatrlabilir. Susuz numuneler, bir hidrojen klorür

gaz aknda süblimasyon yoluyla saflatrlabilir, ardndan süblimasyon bir kuru nitrojen gaz ak içinde

400 ° C’ye stlabilir. Son olarak, en basit yöntem çinko klorürün tiyonil klorür ile ilenmesine dayanr.

Çinko klorür suda çok çözünür olsa da, çözeltilerin basitçe çözülmü Zn2 + iyonlar ve Cl- iyonlar içerdii düünülemez, ZnClxH2O (4 – x) türleri de mevcuttur. Sulu ZnCl2 çözeltileri asidiktir: 6 M sulu çözeltinin pH deeri 1’dir. Dier Zn2 + tuzlarnn çözeltilerine göre sulu ZnCl2 çözeltilerinin asitlii, koordinasyon saysnn 6’dan düürüldüü dört yüzlü kloro aqua komplekslerinin oluumundan kaynaklanr. çözülmü su moleküllerindeki O – H balarnn kuvvetini 4’e daha da düürür.

OHy iyonu varlnda alkali çözeltide, çözelti içinde çeitli çinko hidroksiklorür anyonlar mevcuttur; Zn (OH) 3Cl2-, Zn (OH) 2Cl2-

2, ZnOHCl2-

3 ve Zn5 (OH) 8Cl2 · H2O (simonkolleit) çökelir.

Bir çinko klorür çözeltisinden amonyak köpürtüldüünde, hidroksit çökelmez, bunun yerine kompleks amonyak (amminler) içeren bileikler, Zn (NH3) 4Cl2 · H2O ve konsantrasyonda ZnCl2 (NH3) 2 üretilir. [23] lki, Zn (NH3) 62+ iyonunu [4] içerir ve ikincisi, bozulmu tetrahedral geometriye sahip molekülerdir. Sulu çözeltideki türler aratrlm ve Zn (NH3) 42 + ‘nin Zn ile mevcut ana tür olduunu göstermitir. (NH3) 3Cl + ayrca daha düük NH3: Zn orannda mevcuttur.

Sulu çinko klorür, ilk kez 1855’te Stanislas Sorel tarafndan aratrlan amorf bir çimento oluturmak için çinko oksit ile reaksiyona girer. Sorel daha sonra kendi adn tayan ilgili magnezyum oksiklorür çimentosunu aratrmaya devam etti.

Hidratl çinko klorür stldnda, bir Zn (OH) Cl tortusu elde edilir, örn.

ZnCl2 · 2H2O → ZnCl (OH) + HCl + H2O

ZnCl2 · 1⁄2HCl · H2O bileii, HCl ile asitletirilmi bir ZnCl2 çözeltisinden dikkatlice çökeltilerek hazrlanabilir. Dengeleyici monohidratl hidronyum iyonlar, H5O2 + iyonlar ile polimerik bir anyon (Zn2Cl5-) n içerir. [4

Çinko klorür hidratlar stldnda oluan yüksek reaktif susuz HCl gaznn oluumu, kalitatif inorganik spot testlerinin temelini oluturur.

Çinko klorürün bir ak olarak, bazen amonyum klorür ile bir karm halinde kullanlmas (ayrca bkz. Çinko amonyum klorür), HCl üretimini ve bunun ardndan yüzey oksitlerle reaksiyonunu içerir. Çinko klorür, amonyum klorür ile iki tuz oluturur: (NH4) 2ZnCl4 ve (NH4) 3ClZnCl4, tpk çinko klorür hidratn yapt gibi, serbest brakan HCI stldnda ayrr. Örnein scak daldrma galvanizleme ileminde çinko klorür / amonyum klorür aklarnn etkisi H2 gaz ve amonyak duman üretir.

Selüloz, sulu ZnCl2 çözeltilerinde çözünür ve çinko-selüloz kompleksleri tespit edilmitir. [31] Selüloz ayrca erimi ZnCl2 hidratta çözünür ve selüloz polimeri üzerinde gerçekletirilen karboksilasyon ve asetilasyon.

Bu nedenle, birçok çinko tuzunun farkl formüllere ve farkl kristal yaplara sahip olmasna ramen, bu tuzlar sulu çözelti içinde çok benzer ekilde davranr. Örnein, ZnCl2 polimorflarnn herhangi birinden ve dier halojenürlerden (bromür, iyodür) ve sülfattan hazrlanan çözeltiler, dier çinko bileiklerinin hazrlanmas için sklkla birbirlerinin yerine kullanlabilir. Örnek, çinko karbonatn hazrlanmasdr:

ZnCl2 (sulu) + Na2CO3 (sulu) → ZnCO3 (k) + 2 NaCl (sulu)

Bavurular

Metalurjik bir ak olarak

Çinko klorür, MZnOCl2 formülünün türevlerini vermek için metal oksitlerle (MO) reaksiyona girme kabiliyetine sahiptir. Bu reaksiyon, lehimleme için bir ak olarak ZnCl2 çözeltisinin kullanm ile ilgilidir – oksit kaplamalar çözerek temiz metal yüzeyi aça çkarr. Aktif bir bileen olarak ZnCl2 bazen “kalayc svs” olarak adlandrlr. Tipik olarak bu fluks, çinko folyonun, sv hidrojeni gelitirmeyi brakana kadar seyreltik hidroklorik asit içinde çözülmesiyle hazrland; bu nedenle, bu tür bir ak bir zamanlar “öldürülmü ruhlar” olarak biliniyordu. Korozif yaps nedeniyle, bu eritken elektronik iler gibi herhangi bir kalntnn temizlenemedii durumlar için uygun deildir. Bu özellik ayn zamanda aktif bileen olarak di dolgular için magnezya simanlarnn ve baz az gargaralarnn imalatnda kullanlmasna yol açar.

Kullanm Alanlar

Korozyondan korunma amacyla, çelik gibi dier metallerin galvanize edilmesinde,

Pirinç, nikelli gümü, deiik lehimler, alman gümüü gibi alamlarn yapmnda,

Genellikle otomotiv endüstrisinde döküm kalplarnda,

Pillerin gövdelerinin yapmnda kullanlr.

Çinko oksit, sulu boyalarda beyaz pigment olarak ve lastik sanayinde aktivatör olarak kullanlr.

Yaa bal göz hastalklarnn tedavisinde de kullanlr.

Çinko klorür, deodorantlarda ve ahap koruyucu olarak kullanlr.

Çinko sülfür, karanlkta parlayan pigment olarak saatlerin akrep ve yelkovanlarnda kullanlr.

Çinko Klorür Görünüm

Kristal beyaz toz.

Çinko Klorür Çözünürlük

Çinko Klorür tamamen suda çözünür bir maddedir.

Çinko Klorür Kullanmlar

Çinko klorür organik sentez, kaynak ve su artmnda katalizör olarak kullanlr.

Chloride de zinc

Hydrate de Chloride de zinc

Kristallstruktur Zinkchlorid.png

Des noms

Nom IUPAC

Chloride de zinc

Autres noms

Chloride de zinc (II) DiChloride de

zinc

Beurre de zinc

Identifiants du Chloride de Zinc

Numero CAS du Chloride de Zinc

7646-85-7 anhydre ☑

29426-92-4 Tétrahydrate ☒

Modèle 3D ( JSmol )

Image interactive

ChEBI

CHEBI du Chloride de Zinc: 49976 ☑

ChEMBL

ChEMBL1200679 ☒

ChemSpider

5525 ☑

Carte Info ECHA 100.028.720

Numéro CE du Chloride de Zinc

231-592-0

PubChem CID du Chloride de Zinc

3007855

Numéro RTECS du Chloride de Zinc

ZH1400000

UNII

86Q357L16B ☑

Numéro UN 2331

Tableau de bord CompTox ( EPA )

DTXSID2035013 Modifiez ceci sur Wikidata

InChI[spectacle]

Sourires[spectacle]

Propriétés du Chloride de Zinc

Formule chimique du Chloride de Zinc ZnCl 2

Masse molaire du Chloride de Zinc 136,315 g / mol

Apparence du Chloride de Zinc solide cristallin blanc

hygroscopique et très déliquescent

Odeur du Chloride de Zinc inodore

Densité du Chloride de Zinc 2,907 g / cm 3

Point de fusion du Chloride de Zinc 290 ° C (554 ° F; 563 K) [1]

Point d’ébullition du Chloride de Zinc 732 ° C (1 350 ° F; 1 005 K) [1]

solubilité du Chloride de Zincdans l’eau 432,0 g / 100 g (25 ° C)

Solubilité du Chloride de Zinc soluble dans l’ éthanol , le glycérol et l’ acétone

Solubilité du Chloride de Zincdans l’ alcool 430,0 g / 100 ml

Susceptibilité magnétique du Chloride de Zinc (χ) -65,0 · 10 -6 cm 3 / mol

Structure du Chloride de Zinc

Géométrie de coordination Tétraédrique , linéaire en phase gazeuse

Pharmacologie

Code ATC B05XA12 ( OMS )

Dangers du Chloride de Zinc

Fiche de données de sécurité MSDS externe

Classification UE (DSD) (obsolète) Nocif ( Xn )

Corrosif ( C )

Dangereux pour l’environnement ( N )

Phrases R (obsolètes) R22 , R34 , R50 / 53

Phrases S (obsolètes) (S1 / 2) , S26 , S36 / 37/39 , S45 , S60 , S61

NFPA 704 (diamant de feu)

Diamant quatre couleurs NFPA 704

030

Dose ou concentration létale (DL, LC):

DL 50 ( dose médiane ) 350 mg / kg (rat, oral)

350 mg / kg (souris, oral)

200 mg / kg (cobaye, oral)

1100 mg / kg (rat, oral)

1250 mg / kg (souris, oral) [3]

CL 50 ( concentration médiane ) 1260 mg / m 3 (rat, 30 min)

1180 mg-min / m 3 [3]

NIOSH (limites d’exposition pour la santé aux États-Unis):

PEL (autorisé) TWA 1 mg / m 3 (fumées) [2]

REL (recommandé) TWA 1 mg / m 3 ST 2 mg / m 3 (fumée) [2]

IDLH (danger immédiat) 50 mg / m 3 (fumée) [2]

Composés apparentés

Autres anions Fluorure de

zinc Bromure de

zinc Iodure de zinc

Autres cations Chloride de cadmium Chloride de

mercure (II)

Sauf indication contraire, les données sont données pour les matériaux dans leur état standard (à 25 ° C [77 ° F], 100 kPa).

☒ vérifier ( qu’est-ce que c’est ?) ☑☒

Références Infobox

Le Chloride de zinc est le nom des composés chimiques de formule ZnCl 2 et ses hydrates. Les Chlorides de zinc , dont neuf formes cristallines sont connues, sont incolores ou blancs et sont hautement solubles dans l’eau. [la citation nécessaire ] ZnCl 2 lui-même est hygroscopique et même déliquescent . Les échantillons doivent donc être protégés des sources d’humidité, y compris de la vapeur d’eau présente dans l’air ambiant. Le Chloride de zinc trouve une large application dans le traitement du textile , les flux métallurgiqueset synthèse chimique. Aucun minéral de cette composition chimique n’est connu à part le minéral très rare simonkolleite , Zn 5 (OH) 8 Cl 2 · H 2 O.

Structure et propriétés

Quatre formes cristallines ( polymorphes ) de ZnCl 2 sont connues: α, β, γ et δ, et dans chaque cas les ions Zn 2+ sont tétraédralement coordonnés à quatre ions Chloride. [4]

Forme Symétrie Symbole Pearson Groupe Non a (nm) 　b (nm) c (nm) Z ρ (g / cm 3 )

α tétragonale tI12 I 4 2d 122 0,5398 0,5398 0,64223 4 3,00

β tétragonale tP6 P4 2 / nmc 137 0,3696 0,3696 1,071 2 3.09

γ monoclinique mP36 P2 1 / c 14 0,654 1,131 1,23328 12 2,98

δ orthorhombique oP12 Pna2 1 33 0,6125 0,6443 0,7693 4 2,98

Ici, a , b et c sont des constantes de réseau, Z est le nombre d’unités de structure par maille élémentaire et ρ est la densité calculée à partir des paramètres de structure. [5] [6] [7]

La forme orthorhombique anhydre pure (δ) se transforme rapidement en l’une des autres formes lors de l’exposition à l’atmosphère, et une explication possible est que les ions OH – provenant de l’eau absorbée facilitent le réarrangement. [4] Le refroidissement rapide du ZnCl 2 fondu donne un verre . [8]

Le caractère covalent du matériau anhydre est indiqué par son point de fusion relativement bas de 275 ° C. [9] Une autre preuve de la covalence est fournie par la solubilité élevée du diChloride dans les solvants éthérés , où il forme des adduits avec la formule ZnCl 2 L 2 , où L = ligand tel que O (C 2 H 5 ) 2 . En phase gazeuse, les molécules de ZnCl 2 sont linéaires avec une longueur de liaison de 205 pm. [dix]

Le ZnCl 2 fondu a une viscosité élevée à son point de fusion et une conductivité électrique comparativement faible, qui augmente nettement avec la température. [10] [11] Une étude de diffusion Raman de la fonte a indiqué la présence de structures polymères, [12] et une étude de diffusion de neutrons a indiqué la présence de complexes tétraédriques {ZnCl 4 }. [13]

Hydrate

On connaît cinq hydrates de Chloride de zinc: ZnCl 2 (H 2 O) n avec n = 1, 1,5, 2,5, 3 et 4. [14] Le tétrahydrate ZnCl 2 (H 2 O) 4 cristallise à partir de solutions aqueuses de Chloride de zinc. [14]

Préparation et purification

Le ZnCl 2 anhydre peut être préparé à partir de zinc et de Chloride d’hydrogène :

Zn (s) + 2 HCl → ZnCl 2 + H 2 (g)

Les formes hydratées et les solutions aqueuses peuvent être facilement préparées de manière similaire en traitant le métal Zn avec de l’acide chlorhydrique. L’oxyde de zinc et le sulfure de zinc réagissent avec HCl:

ZnS ( s ) + 2 HCl (aq) → ZnCl 2 (aq) + H 2 S ( g )

Contrairement à de nombreux autres éléments, le zinc n’existe essentiellement que dans un seul état d’oxydation, 2+, ce qui simplifie la purification du Chloride.

Les échantillons commerciaux de Chloride de zinc contiennent généralement de l’ eau et des produits d’ hydrolyse sous forme d’impuretés. Ces échantillons peuvent être purifiés par recristallisation dans du dioxane chaud . Les échantillons anhydres peuvent être purifiés par sublimation dans un courant de Chloride d’hydrogène gazeux, suivi du chauffage du sublimé à 400 ° C dans un courant d’ azote gazeux sec . Enfin, la méthode la plus simple repose sur le traitement du Chloride de zinc avec du Chloride de thionyle . [15]

Réactions

Le ZnCl 2 anhydre fondu à 500-700 ° C dissout le zinc métal et, lors du refroidissement rapide de la masse fondue, un verre diamagnétique jaune se forme, qui, d’après les études Raman, contient du Zn2+

2ion. [14]

Un certain nombre de sels contenant l’ anion tétrachlorozincate , Zn Cl2-

4, sont connus. [10] “Réactif de Caulton”, V 2 Cl 3 (thf) 6 Zn 2 Cl 6 est un exemple de sel contenant du Zn 2 Cl2-

6. [16] [17] Le composé Cs 3 ZnCl 5 contient du Zn Cl tétraédrique2-

4et Cl – anions. [4] Aucun composé contenant le Zn Cl4-

6ion ont été caractérisés. [4]

Alors que le Chloride de zinc est très soluble dans l’eau, les solutions ne peuvent pas être considérées comme contenant simplement des ions Zn 2+ solvatés et des ions Cl – , des espèces ZnCl x H 2 O (4- x ) sont également présentes. [18] [19] [20] Les solutions aqueuses de ZnCl 2 sont acides: une solution aqueuse 6 M a un pH de 1. [14] L’acidité des solutions aqueuses de ZnCl 2 par rapport aux solutions d’autres Zn 2+Les sels sont dus à la formation de complexes chloro-aqua tétraédriques où la réduction du nombre de coordination de 6 à 4 réduit encore la force des liaisons O – H dans les molécules d’eau solvatées. [21]

Dans une solution alcaline en présence d’ ion OH – divers anions d’hydroxyChloride de zinc sont présents en solution, par exemple Zn (OH) 3 Cl 2- , Zn (OH) 2 Cl2-

2, ZnOH Cl2-

3et Zn 5 (OH) 8 Cl 2 · H 2 O (simonkolleite) précipite. [22]

Lorsque l’ammoniac est barboté dans une solution de Chloride de zinc, l’hydroxyde ne précipite pas, mais des composés contenant de l’ammoniac complexé (ammines) sont produits, Zn (NH 3 ) 4 Cl 2 · H 2 O et en concentration ZnCl 2 (NH 3 ) 2 . [23] Le premier contient l’ ion Zn (NH 3 ) 6 2+ [4] , et le dernier est moléculaire avec une géométrie tétraédrique déformée. [24] Les espèces en solution aqueuse ont été étudiées et montrent que Zn (NH 3 ) 4 2+ est la principale espèce présente avec Zn (NH3 ) 3 Cl + également présent à un rapport NH 3 : Zn inférieur. [25]

Le Chloride de zinc aqueux réagit avec l’oxyde de zinc pour former un ciment amorphe qui a été étudié pour la première fois en 1855 par Stanislas Sorel . Sorel a ensuite enquêté sur le ciment d’oxyChloride de magnésium associé , qui porte son nom. [26]

Lorsque le Chloride de zinc hydraté est chauffé, on obtient un résidu de Zn (OH) Cl par exemple [27]

ZnCl 2 · 2H 2 O → ZnCl (OH) + HCl + H 2 O

Le composé ZnCl 2 · une / 2 HCl · H 2 O peuvent être préparés par précipitation soigneuse d’une solution de ZnCl 2 acidifié avec HCl. Il contient un anion polymère (Zn 2 Cl 5 – ) n avec des ions hydronium monohydratés d’équilibrage, des ions H 5 O 2 + . [4] [28]

La formation de gaz HCl anhydre hautement réactif formé lorsque les hydrates de Chloride de zinc sont chauffés est la base de tests ponctuels inorganiques qualitatifs. [29]

L’utilisation de Chloride de zinc comme fondant, parfois en mélange avec du Chloride d’ammonium (voir aussi Chloride de zinc-ammonium ), implique la production de HCl et sa réaction ultérieure avec les oxydes de surface. Le Chloride de zinc forme deux sels avec le Chloride d’ammonium: (NH 4 ) 2 ZnCl 4 et (NH 4 ) 3 ClZnCl 4 , qui se décomposent en chauffant en libérant du HCl, tout comme l’hydrate de Chloride de zinc. L’action des flux Chloride / Chloride d’ ammonium zinc, par exemple, dans la galvanisation à chaud procédé produit H 2 des vapeurs de gaz et d’ ammoniac. [30]

La cellulose se dissout dans des solutions aqueuses de ZnCl 2 et des complexes zinc-cellulose ont été détectés. [31] La cellulose également dissout dans fondu ZnCl 2 hydrate et carboxylation et acétylation effectuée sur le polymère de cellulose. [32]

Ainsi, bien que de nombreux sels de zinc aient des formules et des structures cristallines différentes , ces sels se comportent de manière très similaire en solution aqueuse. Par exemple, les solutions préparées à partir d’un quelconque des polymorphes de ZnCl 2 , ainsi que d’ autres halogénures (bromure, iodure), et le sulfate peuvent souvent être utilisés de manière interchangeable pour la préparation d’autres composés de zinc. La préparation du carbonate de zinc est illustrative:

ZnCl 2 ( aq ) + Na 2 CO 3 (aq) → ZnCO 3 (s) + 2 NaCl (aq)

Applications

En tant que flux métallurgique

Le Chloride de zinc a la capacité de réagir avec les oxydes métalliques (MO) pour donner des dérivés de formule MZnOCl 2 . [33] [ citation (s) supplémentaire (s) nécessaire (s) ] Cette réaction est pertinente pour l’utilité de la solution de ZnCl 2 comme flux pour le brasage – elle dissout les revêtements d’oxyde, exposant la surface métallique propre. [33] Les flux contenant du ZnCl 2 comme ingrédient actif sont parfois appelés «fluide d’étain». Typiquement, ce flux a été préparé en dissolvant une feuille de zinc dans de l’acide chlorhydrique diluéjusqu’à ce que le liquide cesse de dégager de l’hydrogène; pour cette raison, un tel flux était autrefois appelé “esprits tués”. En raison de sa nature corrosive, ce flux ne convient pas aux situations où aucun résidu ne peut être nettoyé, comme le travail électronique. [la citation nécessaire ] Cette propriété conduit également à son utilisation dans la fabrication de ciments de magnésie pour les obturations dentaires et certains bains de bouche comme ingrédient actif.

Dans la synthèse organique

Une première utilisation du Chloride de zinc (Silzic) consistait à construire des squelettes de carbone par condensation de molécules de méthanol . Les hydrocarbures insaturés sont les principaux produits, les conditions de réaction influençant la distribution des produits, bien que certains composés aromatiques se soient formés. [34] En 1880, on a découvert que le Chloride de zinc fondu catalyse une réaction d’ aromatisation générant de l’ hexaméthylbenzène . Au point de fusion du ZnCl 2 (283 ° C), la réaction a un Δ G = -1090 kJ / mol et peut être idéalisée comme [35]

15 CH

3OH → C

6(CH

6+ 3 CH

4+ 15 H

Les découvreurs de cette réaction l’ont rationalisée comme impliquant la condensation d’unités méthylène suivie d’une méthylation complète de Friedel-Crafts du cycle benzénique résultant avec du chlorométhane généré in situ . [35] Une telle transformation d’alkylation est une application de la force modérée du Chloride de zinc en tant qu’acide de Lewis , qui est son rôle principal dans la synthèse en laboratoire. D’autres exemples incluent la catalyse (A) de la synthèse d’indole de Fischer , [36] et également (B) des réactions d’acylation de Friedel-Crafts impliquant des cycles aromatiques activés [37] [38]

ZnCl2 aromatics.gif

La préparation classique du colorant fluorescéine à partir d’anhydride phtalique et de résorcinol , qui implique une acylation de Friedel-Crafts, est liée à ce dernier . [39] Cette transformation a en effet été réalisée en utilisant le même hydraté ZnCl 2 échantillon représenté sur la figure ci – dessus.

ZnCl2 fluorescéine.png

L’ acide chlorhydrique réagit seulement faiblement avec les alcools primaires et les alcools secondaires , mais une combinaison de HCl avec ZnCl 2 (connus ensemble comme le « réactif Lucas ») est efficace pour la préparation d’alkyl Chlorides. Les réactions typiques sont conduites à 130 ° C. Cette réaction se déroule probablement via un mécanisme S N 2 avec des alcools primaires mais une voie S N 1 avec des alcools secondaires.

ZnCl2 Lucas.gif

Le Chloride de zinc active également les halogénures benzyliques et allyliques vers la substitution par des nucléophiles faibles tels que les alcènes : [40]

Benzylation de ZnCl2.gif

De la même façon, ZnCl 2 favorise sélective NaBH 3 CN réduction d’halogénures tertiaires allyliques ou benzyliques des hydrocarbures correspondants.

Le Chloride de zinc est également un réactif de départ utile pour la synthèse de nombreux réactifs organozinciques , tels que ceux utilisés dans le couplage de Negishi catalysé au palladium avec des halogénures d’aryle ou des halogénures de vinyle . [41] Dans de tels cas, le composé organozincique est généralement préparé par transmétallation à partir d’un organolithium ou d’un réactif de Grignard , par exemple:

ZnCl2 Negishi.gif

Zinc énolates , préparés à partir d’ énolates de métaux alcalins et de ZnCl 2 , assurent le contrôle de la stéréochimie en aldol condensation réactions dues à la chélation sur le zinc. Dans l’exemple illustré ci – dessous, la thréo produit a été favorisée par rapport à la erythro par un facteur de 5: 1 lorsque ZnCl 2 dans du DME / éther a été utilisé. [42] Le chelate est plus stable lorsque le groupe phényle volumineux est pseudo- équatorial plutôt que pseudo- axial , c’est-à-dire thréo plutôt qu’érythro .

ZnCl2 aldol.gif

Dans le traitement des textiles et du papier

Les solutions aqueuses concentrées de Chloride de zinc (plus de 64% poids / poids de Chloride de zinc dans l’eau) ont la propriété intéressante de dissoudre l’ amidon , la soie et la cellulose . Ainsi, de telles solutions ne peuvent pas être filtrées à travers des papiers filtres standards. En raison de son affinité pour ces matériaux, le ZnCl 2 est utilisé comme agent ignifuge et dans des “rafraîchisseurs” de tissus tels que Febreze. La fibre vulcanisée est fabriquée en trempant du papier dans du Chloride de zinc concentré.

Les grenades fumigènes

Le mélange de fumée de Chloride de zinc («HC») utilisé dans les grenades fumigènes contient de l’oxyde de zinc , de l’ hexachloroéthane et de la poudre d’ aluminium granulaire qui, lorsqu’ils sont enflammés, réagissent pour former de la fumée de Chloride de zinc, de carbone et d’oxyde d’aluminium , un écran de fumée efficace . [43]

Détection d’empreintes digitales

La ninhydrine réagit avec les acides aminés et les amines pour former un composé coloré «violet de Ruhemann» (RP). La pulvérisation avec une solution de Chloride de zinc forme un complexe 1: 1 RP: ZnCl (H 2 O) 2 , qui est plus facilement détecté car il fluorescent mieux que le violet de Ruhemann. [44]

Désinfectant

Historiquement, une solution aqueuse diluée de Chloride de zinc était utilisée comme désinfectant sous le nom de “Burnett’s Disinfecting Fluid”. [45] Il est également utilisé dans certaines marques commerciales de rince-bouche antiseptique.

Le traitement du cancer de la peau

Le Chloride de zinc a été utilisé en médecine alternative pour provoquer des escarres , des croûtes de tissus morts, dans le but de guérir les cancers de la peau. [46] Divers produits, tels que Cansema ou “pommade noire”, contenant du Chloride de zinc et vendus comme remèdes contre le cancer ont été répertoriés par la Food and Drug Administration (FDA) des États-Unis comme des faux [47] avec des lettres d’avertissement envoyées aux fournisseurs. [48]

De nombreux rapports dans la littérature médicale décrivent des cicatrices graves et des lésions cutanées normales par des substances escharotiques. Compte tenu de ces effets secondaires, son utilisation dans le traitement n’est pas justifiée car il existe des alternatives beaucoup plus sûres et plus efficaces, telles que la radiothérapie et la chirurgie de Mohs . [49] [50]

Sécurité

Le Chloride de zinc est un irritant cutané. Après contact avec la peau, un retrait immédiat est nécessaire avec du savon et beaucoup d’eau. Après contact avec les yeux, des mesures adéquates consistent à rincer abondamment à l’eau ou à un autre rinçage oculaire et à contacter un ophtalmologiste dès que possible. [51]

Le Chloride de zinc est caustique au tractus gastro-intestinal, conduisant parfois à une hématémèse . Les symptômes d’intoxication aiguë sont la détresse gastro-intestinale, la diarrhée, les nausées et les douleurs abdominales. Les vomissements se produisent presque partout. La dose létale chez l’homme est de 3 à 5 g. [la citation nécessaire ] La décontamination du tractus gastro-intestinal après l’absorption orale de composés de zinc est la plupart du temps inutile, puisque les patients vomissent habituellement suffisamment. Le lait peut être administré pour diminuer l’absorption du métal. Les niveaux de zinc peuvent être normalisés avec des sels EDTA . [51]

Le Chloride de zinc est extrêmement nocif pour les poumons et l’exposition pulmonaire à la fumée de Chloride de zinc a déjà entraîné des décès. [la citation nécessaire ] L’inhalation de vapeurs de zinc, d’oxyde de zinc ou de Chloride de zinc conduit à un œdème pulmonaire et à une fièvre de fumée de métal . L’apparition se produit dans les 4 à 6 h et peut être retardée jusqu’à 8 h. Les symptômes comprennent une respiration rapide, une dyspnée , une toux, de la fièvre, des frissons, des sueurs, des douleurs à la poitrine et aux jambes, des myalgies , de la fatigue, un goût métallique, une salivation, une soif et une leucocytose , qui peut durer de 24 à 48 h. En cas d’inhalation de fumées, les préparations de cortisone doivent être appliquées immédiatement (par exemple, par inhalation deAuxiloson ) pour éviter le développement d’un œdème pulmonaire. [51]

Utilisation et sources d’émission du Chloride de Zinc

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ZINC CHLORIDE SOLUTION 60% (NKO KLORR 60%)

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ZINC CHLORIDE SOLUTION 60% (NKO KLORR 60%)

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