PRODUCTS

ZINC CHLORIDE SOLUTION 60%

SYNONYMS:
ZINC CHLORIDE SOLUTION 60%; Chlorure de zinc; DICHLORURE DE ZINC; Butter of zinc; Zinkchloride; Zintrace;Zinc chloride fume;Zine dichloride; Zinco (cloruro di)

CAS Number:7646-85-7
EC Number:231-592-0

SYNONYMS:
ZINC CHLORIDE SOLUTION 60%;; Chlorure de zinc; DICHLORURE DE ZINC; ZINC, CHLORURE DE ; ZINC, DICHLORURE DE; BUTTER OF ZINC; ZINC BUTTER; Zinc chloride; Zinc(II) chloride;Zinc dichloride;Butter of zinc; zinc chloride;Zinc dichloride;7646-85-7;Zinc butter;Zinc chloride (ZnCl2);Zinc(II) chloride;Zinkchloride;Zintrace;Zinc chloride fume;Zine dichloride;Zinc chloride, Zinc (chlorure de);Zinco (cloruro di);Zinkchlorid;Zinkchloride;Caswell No. 910;Zinc chloride ;Chlorure de zinc ;Zinc (chlorure de);CCRIS 3509;Zinc chloride 0.1 M ;Zinco (cloruro di);HSDB 1050;EINECS 231-592-0;UN1840;UN2331;EPA Pesticide Chemical Code 087801;NSC 529648;AI3-04470;Zinc chloride (TN);ZINC CHLORIDE (ZNCL2) ; ZINC CHLORIDE; ZINC CHLORIDE; BUTTER OF ZINC; CHLORURE DE ZINC ; ZINC (CHLORURE DE) ; ZINC BUTTER; ZINC CHLORIDE FUME; ZINC CHLORIDE FUME ; ZINC DICHLORIDE; ZINCO (CLORURO DI); ZINKCHLORID;ZnCl2; Butter of zinc; Chlorure de zinc; Zinc (chlorure de); Zinc chloride (ZnCl2); Zinc dichloride; Zinc muriate; Zinc Butter; Zinco (cloruro di); Zinkchlorid; Zinkchloride; Tinning flux; UN 1840; UN 2331; Zinc chloride, anhydrous; Zinco; Zinctrace; Hydrochloric acid zinc salt (2:1);Butter of zinc;Zinc dichloride;Zinc(II) chloride;Zinc chloride; çinko; çinko klorür;çinko klorid;çinko 2 klorür;çinko(II) klorür;çinko-2-klorür;çinkoklorür;çinko 2 klorid;çinko (II) klorid;zinc klorür;Zinc(II) chloride;Zinc dichloride;Butter of zinc;Zinc dichloride;Zinc(II) chloride;Zinc chloride; çinko; çinko klorür;çinko klorid;çinko 2 klorür;çinko(II) klorür;çinko-2-klorür;çinko 2 klorid;çinko (II) klorid;zinc klorür;Zinc(II) chloride;Zinc dichloride; ZINC DICHLORIDE; ÇİNKO KLORÜR; ÇİNKO KLORİT; ÇİNKO KLORİD; ZN chlorid; zn chloride; Zn Chlorit; Zn klorit; Zn clorid; Zn clorit; ZINC CHLORIDE SOLUTION 60%;; CHLORURE DE ZİNC; DICHLORURE DE ZINC; ZINC, CHLORURE DE ; ZINC, DICHLORURE DE; BUTTER OF ZINC; ZINC BUTTER; ZİNC CHLORİDE; ZINC DICHLORIDE; ÇİNKO KLORÜR; ÇİNKO KLORİT; ÇİNKO KLORİD; Zn CHLORİD; Zn CHLORİDE; Zn CHLORİT; Zn KLORİT; Zn CLORİD; Zn CLORİT; Zn klorüre; çinko klorit; ÇİNKO KHLORİT; Zn KLORİD; Zınc Chlorıde Solutıon 60%;; Chlorure De Zinc; Dıchlorure De Zınc; Zınc, Chlorure De ; Zınc, Dıchlorure De; Butter Of Zınc; Zınc Butter; Zinc Chloride; Zınc Dıchlorıde; Çinko Klorür; Çinko Klorit; Çinko Klorid; Zn Chlorid; Zn Chloride; Zn Chlorit; Zn Klorit; Zn Clorid; Zn Clorit; Zn Klorüre; Çinko Klorit; Çinko Khlorit; Zn Klorid; zınc chlorıde solutıon 60%;; chlorure de zinc; dıchlorure de zınc; zınc, chlorure de ; zınc, dıchlorure de; butter of zınc; zınc butter; zinc chloride; zınc dıchlorıde; çinko klorür; çinko klorit; çinko klorid; zn chlorid; zn chloride; zn chlorit; zn klorit; zn clorid; zn clorit; zn klorüre; çinko klorit; çinko khlorit; zn klorid; Çinko Klorit

ZİNC CHLORİDE SOLUTİON 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
3)
6 + 3 CH
4 + 15 H
2O
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.düşük 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.