Phosphorus trichloride

Names
IUPAC name

Phosphorus trichloride

Systematic IUPAC name

Trichlorophosphane

Other names

Phosphorus(III) chloride
Phosphorous chloride

Identifiers

CAS Number

* 7719-12-2 Y

3D model (JSmol)

* Interactive image

ChEBI |

* CHEBI:30334 Y

ChemSpider |

* 22798 Y

EC Number |

* 231-749-3

PubChem CID

* 24387

RTECS number |

* TH3675000

UNII |

* M97C0A6S8U N

UN number | 1809

InChI

* InChI=1S/Cl3P/c1-4(2)3 Y

Key: FAIAAWCVCHQXDN-UHFFFAOYSA-N Y

SMILES

* ClP(Cl)Cl

Properties

Chemical formula

| PCl3
Molar mass | 137.33 g/mol
Appearance  | Colorless to yellow fuming liquid[1]
Odor | unpleasant, acrid, like hydrochloric acid[1]
Density | 1.574 g/cm3
Melting point |  −93.6 °C (−136.5 °F; 179.6 K)
Boiling point |  76.1 °C (169.0 °F; 349.2 K)

Solubility in water

| hydrolyzes
Solubility in other solvents  | soluble[vague] in benzene, CS2, ether, chloroform, CCl4, halogenated organic solvents
reacts with ethanol
Vapor pressure | 13.3 kPa

Magnetic susceptibility (χ)

| −63.4·10−6 cm3/mol

Refractive index (nD)

| 1.5122 (21 °C)
Viscosity | 0.65 cP (0 °C)
0.438 cP (50 °C)

Dipole moment

| 0.97 D
Thermochemistry

Std enthalpy of
formation (ΔfH⦵298)

| −319.7 kJ/mol
Hazards
Main hazards | Highly toxic,[2] corrosive
Safety data sheet | ICSC 0696
GHS pictograms |
GHS Signal word | Danger

GHS hazard statements

| H300, H301, H330, H314, H373

GHS precautionary statements

| P260, P273, P284, P305+351+338, P304+340+310, P303+361+353
NFPA 704 (fire diamond)  |

~~W~~

Lethal dose or concentration (LD, LC):

LD50 (median dose)

| 18 mg/kg (rat, oral)[3]

LC50 (median concentration)

| 104 ppm (rat, 4 hr)
50 ppm (guinea pig, 4 hr)[3]
NIOSH (US health exposure limits):

PEL (Permissible)

| TWA 0.5 ppm (3 mg/m3)[1]

REL (Recommended)

| TWA 0.2 ppm (1.5 mg/m3) ST 0.5 ppm (3 mg/m3)[1]

IDLH (Immediate danger)

| 25 ppm[1]
Related compounds

Related phosphorus chlorides

| Phosphorus pentachloride
Phosphorus oxychloride
Diphosphorus tetrachloride

Related compounds

| Phosphorus trifluoride
Phosphorus tribromide
Phosphorus triiodide

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

N verify (what is YN ?)
Infobox references

Tracking categories (test):

* SizeSet

Phosphorus trichloride is an inorganic compound with the chemical formula PCl3. A colorless liquid when pure, it is an important industrial chemical, being used for the manufacture of phosphites and other organophosphorus compounds. It is toxic and reacts readily with water to release hydrogen chloride.

## Contents

* 1 History
* 2 Preparation
* 3 Structure and spectroscopy
* 4 Reactions
* 4.1 Oxidation
* 4.2 PCl3 as an electrophile
* 4.3 Conversion of alcohols to alkyl chlorides
* 4.4 Redox reactions
* 4.5 PCl3 as a nucleophile
* 4.6 PCl3 as a ligand
* 5 Uses
* 6 Safety
* 7 See also
* 8 References

## History

Phosphorus trichloride was first prepared in 1808 by the French chemists Joseph Louis Gay-Lussac and Louis Jacques Thénard by heating calomel (Hg2Cl2) with phosphorus.[5] Later during the same year, the English chemist Humphry Davy produced phosphorus trichloride by burning phosphorus in chlorine gas.[6]

## Preparation

World production exceeds one-third of a million tonnes.[7] Phosphorus trichloride is prepared industrially by the reaction of chlorine with white phosphorus, using phosphorus trichloride as the solvent. In this continuous process PCl3 is removed as it is formed in order to avoid the formation of PCl5.

P4 \+ 6 Cl2 → 4 PCl3

## Structure and spectroscopy

It has a trigonal pyramidal shape. Its 31P NMR spectrum exhibits a singlet around +220 ppm with reference to a phosphoric acid standard.[citation needed]

## Reactions

The phosphorus in PCl3 is often considered to have the +3 oxidation state and the chlorine atoms are considered to be in the −1 oxidation state. Most of its reactivity is consistent with this description.[8]

### Oxidation

PCl3 is a precursor to other phosphorus compounds, undergoing oxidation to phosphorus pentachloride (PCl5), thiophosphoryl chloride (PSCl3), or phosphorus oxychloride (POCl3).

### PCl3 as an electrophile

PCl3 reacts vigorously with water to form phosphorous acid (H3PO3) and hydrochloric acid:

PCl3 \+ 3 H2O → H3PO3 \+ 3 HCl

Phosphorus trichloride is the precursor to organophosphorus compounds. It reacts with phenol to give triphenyl phosphite:

3 PhOH + PCl
3 → P(OPh)
3 \+ 3 HCl (Ph = C

Alcohols such as ethanol react similarly in the presence of a base such as a tertiary amine:[9]

PCl
3 \+ 3 EtOH + 3 R
3N → P(OEt)
3 \+ 3 R
3NH+Cl−

With one equivalent of alcohol and in the absence of base, the first product is alkoxyphosphorodichloridite:[10]

PCl
3 \+ EtOH → PCl
2(OEt) + HCl

In the absence of base, however, with excess alcohol, phosphorus trichloride converts to diethylphosphite:[11][12]

PCl3 \+ 3 EtOH → (EtO)2P(O)H + 2 HCl + EtCl

Secondary amines (R2NH) form aminophosphines. For example, bis(diethylamino)chlorophosphine, (Et2N)2PCl, is obtained from diethylamine and PCl3. Thiols (RSH) form P(SR)3. An industrially relevant reaction of PCl3 with amines is phosphonomethylation, which employs formaldehyde:

R2NH + PCl3 \+ CH2O → (HO)2P(O)CH2NR2 \+ 3 HCl

The herbicide glyphosate is also produced this way.

The reaction of PCl3 with Grignard reagents and organolithium reagents is a useful method for the preparation of organic phosphines with the formula R3P (sometimes called phosphanes) such as triphenylphosphine, Ph3P.

3 RMgBr + PCl
3 → R
3P + 3 MgBrCl

Triphenylphosphine is produced industrially by the reaction between phosphorus trichlorid, chlorobenzene, and sodium:[13]

PCl
3 \+ 3 PhCl + 6 Na → PPh
3 \+ 6 NaCl, where Ph = C

Under controlled conditions or especially with bulky R groups, similar reactions afford less substituted derivatives such as chlorodiisopropylphosphine.

### Conversion of alcohols to alkyl chlorides

Phosphorus trichloride is commonly used to convert primary and secondary alcohols to the corresponding chlorides.[14] As discussed above, the reaction of alcohols with phosphorus trichloride is sensitive to conditions. The mechanism for the ROH →RCl conversion involves the reaction of HCl with phosphite esters:

P(OR)
3 \+ HCl ⇌ HP(OR)+
3Cl−
HP(OR)+
3Cl− → RCl + HOP(OR)

HOP(OR)
2 \+ HCl ⇌ H
2OP(OR)+
2Cl−

2OP(OR)+
2Cl− → RCl + (HO)
2P(OR)

(HO)
2P(OR) + HCl ⇌ H(HO)
2P(OR)+Cl−
H(HO)
2P(OR)+Cl− → RCl + (HO)

The first step proceeds with nearly ideal stereochemistry but the final step far less so owing to an SN2 pathway.

### Redox reactions

Phosphorus trichloride undergoes a variety of redox reactions:[13]

3PCl
3 \+ 2 CrO
3 → 3POCl
3 \+ Cr

PCl
3 \+ SO
3 → POCl
3 \+ SO

3 PCl
3 \+ SO
2 → 2POCl
3 \+ PSCl

### PCl3 as a nucleophile

Phosphorus trichloride has a lone pair, and therefore can act as a Lewis base,[15] e.g., forming a 1:1 adduct Br3B-PCl3. Metal complexes such as Ni(PCl3)4 are known, again demonstrating the ligand properties of PCl3.

This Lewis basicity is exploited in the Kinnear–Perren reaction to prepare alkylphosphonyl dichlorides (RP(O)Cl2) and alkylphosphonate esters (RP(O)(OR')2). Alkylation of phosphorus trichloride is effected in the presence of aluminium trichloride give the alkyltrichlorophosphonium salts, which are versatile intermediates:[16]

PCl3 \+ RCl + AlCl3 → RPCl+3 \+ AlCl−4

The RPCl+3 product can then be decomposed with water to produce an alkylphosphonic dichloride RP(=O)Cl2.

### PCl3 as a ligand

PCl3, like the more popular phosphorus trifluoride, is a ligand in coordination chemistry. One example is Mo(CO)5PCl3.[17]

## Uses

PCl3 is important indirectly as a precursor to PCl5, POCl3 and PSCl3, which are used in many applications, including herbicides, insecticides, plasticisers, oil additives, and flame retardants.

For example, oxidation of PCl3 gives POCl3, which is used for the manufacture of triphenyl phosphate and tricresyl phosphate, which find application as flame retardants and plasticisers for PVC. They are also used to make insecticides such as diazinon. Phosphonates include the herbicide glyphosate.

PCl3 is the precursor to triphenylphosphine for the Wittig reaction, and phosphite esters which may be used as industrial intermediates, or used in the Horner-Wadsworth-Emmons reaction, both important methods for making alkenes. It can be used to make trioctylphosphine oxide (TOPO), used as an extraction agent, although TOPO is usually made via the corresponding phosphine.

PCl3 is also used directly as a reagent in organic synthesis. It is used to convert primary and secondary alcohols into alkyl chlorides, or carboxylic acids into acyl chlorides, although thionyl chloride generally gives better yields than PCl3.[18]

## Safety

* 600 ppm is lethal in just a few minutes.[19]
* 25 ppm is the US NIOSH "Immediately Dangerous to Life and Health" level[20]
* 0.5 ppm is the US OSHA "permissible exposure limit" over a time-weighted average of 8 hours.[21]
* 0.2 ppm is the US NIOSH "recommended exposure limit" over a time-weighted average of 8 hours.[22]
* Under EU Directive 67/548/EEC, PCl3 is classified as very toxic and corrosive , and the risk phrases R14, R26/28, R35 and R48/20 are obligatory.

Industrial production of phosphorus trichloride is controlled under the Chemical Weapons Convention, where it is listed in schedule 3, as it can be used to produce mustard agents.[23]

## See also

* Phosphorus pentachloride
* Phosphoryl chloride
* Phosphorus trifluorodichloride

## References

1. ↑ 1.0 1.1 1.2 1.3 1.4 NIOSH Pocket Guide to Chemical Hazards. "#0511". National Institute for Occupational Safety and Health (NIOSH). https://www.cdc.gov/niosh/npg/npgd0511.html.
2. ↑ Phosphorus trichloride toxicity
3. ↑ 3.0 3.1 "Phosphorus trichloride". Immediately Dangerous to Life and Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH). https://www.cdc.gov/niosh/idlh/7719122.html.
4. ↑ Sigma-Aldrich Co., Phosphorus trichloride.
5. ↑ Gay-Lussac; Thénard (27 May 1808). "Extrait de plusieurs notes sur les métaux de la potasse et de la soude, lues à l'Institut depuis le 12 janvier jusqu'au 16 mai" (in fr). Gazette Nationale, Ou le Moniteur Universel 40 (148): 581–582. https://books.google.com/books?id=GRROAAAAcAAJ&pg=PA581. From p. 582: "Seulement ils ont rapporté qu'en traitant le mercure doux par le phosphure, dans l'espérance d'avoir de l'acide muriatique bien sec, il ont trouvé une liqueur nouvelle très limpide, sans couleur, répandant de fortes vapeurs, s'enflammant spontanément lorsqu'on en imbibe le papier joseph; laquelle ne paraît être qu'une combinaison de phosphore, d'oxigène et d'acide muriatique, et par conséquent analogue à cette qu'on obtient en traitant le soufre par le gas acide muriatique oxigèné." (Only they reported that by treating calomel with phosphorus, in the hope of obtaining very dry hydrogen chloride, they found a new, very clear liquid, colorless, giving off strong vapors, spontaneously igniting when one soaks filter paper in it; which seems to be only a compound of phosphorus, oxygen, and hydrochloric acid, and thus analogous to what one obtains by treating sulfur with chlorine gas.)
6. ↑ Davy, Humphry (1809). "The Bakerian Lecture. An account of some new analytical researches on the nature of certain bodies, particularly the alkalies, phosphorus, sulphur, carbonaceous matter, and the acids hitherto undecomposed; with some general observations on chemical theory". Philosophical Transactions of the Royal Society of London 99: 39–104. doi:10.1098/rstl.1809.0005. https://babel.hathitrust.org/cgi/pt?id=mdp.39015034564347;view=1up;seq=53. On pp. 94–95, Davy mentioned that when he burned phosphorus in chlorine gas ("oxymuriatic acid gas"), he obtained a clear liquid (phosphorus trichloride) and a white solid (phosphorus pentachloride).
7. ↑ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
8. ↑ "Phosphorus trichloride (PCl3)". https://www.simply.science/images/content/chemistry/metals_and_non_metals/nitrogen_family/conceptmap/Phosphorus_chloride.html.
9. ↑ A. H. Ford-Moore; B. J. Perry (1963). "Triethyl Phosphite". Organic Syntheses. http://www.orgsyn.org/demo.aspx?prep=CV4P0955. ;  Collective Volume, 4, pp. 955
10. ↑ Gerrard, W.; Isaacs, M. J. D.; Machell, G.; Smith, K. B.; Wyvill, P. L. (1953). "394. Interaction of phosphorus trichloride with alcohols and with hydroxy-esters". Journal of the Chemical Society (Resumed): 1920. doi:10.1039/JR9530001920.
11. ↑ Malowan, John E. (1953). "Diethyl phosphite". Inorganic Syntheses. 4. pp. 58–60. doi:10.1002/9780470132357.ch19. ISBN 9780470132357.
12. ↑ Pedrosa, Leandro (2011). "Esterification of Phosphorus Trichloride with Alcohols; Diisopropyl phosphonate". ChemSpider Synthetic Pages (Royal Society of Chemistry): 488. doi:10.1039/SP488. http://cssp.chemspider.com/488.
13. ↑ 13.0 13.1 Corbridge, D. E. C. (1995). Phosphorus: An Outline of its Chemistry, Biochemistry, and Technology (5th ed.). Amsterdam: Elsevier. ISBN 0-444-89307-5.
14. ↑ Brown, Geoffrey W. (1971). "Displacement of Hydroxyl Groups". The Hydroxyl Group (1971). PATai's Chemistry of Functional Groups. pp. 593–639. doi:10.1002/9780470771259.ch11. ISBN 9780470771259.
15. ↑ R. R. Holmes (1960). "An examination of the basic nature of the trihalides of phosphorus, arsenic and antimony". Journal of Inorganic and Nuclear Chemistry 12 (3–4): 266–275. doi:10.1016/0022-1902(60)80372-7.
16. ↑ Svara, J.; Weferling, N.; Hofmann, T.. "Ullmann's Encyclopedia of Industrial Chemistry". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a19_545.pub2.
17. ↑ Frenking, Gernot; Wichmann, Karin; Fröhlich, Nikolaus; Grobe, Joseph; Golla, Winfried; Van, Duc Le; Krebs, Bernt; Läge, Mechtild (2002). "Nature of the Metal−Ligand Bond in M(CO)5PX3 Complexes (M = Cr, Mo, W; X = H, Me, F, Cl): Synthesis, Molecular Structure, and Quantum-Chemical Calculations". Organometallics 21 (14): 2921–2930. doi:10.1021/om020311d.
18. ↑ L. G. Wade Jr. (2005). Organic Chemistry (6th ed.). Upper Saddle River, New Jersey, USA: Pearson/Prentice Hall. p. 477.
19. ↑ A. D. F. Toy (1973). The Chemistry of Phosphorus. Oxford, UK: Pergamon Press.
20. ↑ Documentation for Immediately Dangerous To Life or Health Concentrations (IDLHs)
21. ↑ OSHA: Phosphorus Trichloride
22. ↑ CDC - NIOSH Pocket Guide to Chemical Hazards
23. ↑ M. C. Forbes; C. A. Roswell; R. N. Maxson (2007). "Phosphorus(III) Chloride". Inorganic Syntheses. 2. 145–7. doi:10.1002/9780470132333.ch42. ISBN 9780470132333.

* v
* t
* e

Phosphorus compounds

* PBr3
* PBr5
* PCl3
* PCl5
* PF3
* PF5
* PI3
* InP
* PH3
* PN
* P3N5
* P2O3
* P2O4
* P2O5
* P4S3
* P4S10
* AlP
* Ca3P2
* Zn3P2
* CuP2
* HfP
* FeP
* Fe3P
* BP
* YP

* v
* t
* e

Salts and covalent derivatives of the chloride ion

HCl |  |  |  | He

|
|
|
|

LiCl | BeCl2 | BCl3
B2Cl4 | CCl4 | NCl3
ClN3 | Cl2O
ClO2
Cl2O7 | ClF
ClF3
ClF5 | Ne
NaCl | MgCl2 | AlCl
AlCl3 | SiCl4 | P2Cl4
PCl3
PCl5 | S2Cl2
SCl2
SCl4 | Cl2 | Ar
KCl | CaCl
CaCl2 | ScCl3 | TiCl2
TiCl3
TiCl4 | VCl2
VCl3
VCl4
VCl5 | CrCl2
CrCl3
CrCl4 | MnCl2 | FeCl2
FeCl3 | CoCl2
CoCl3 | NiCl2 | CuCl
CuCl2 | ZnCl2 | GaCl2
GaCl3 | GeCl2
GeCl4 | AsCl3
AsCl5 | Se2Cl2
SeCl4 | BrCl | KrCl
RbCl | SrCl2 | YCl3 | ZrCl3
ZrCl4 | NbCl4
NbCl5 | MoCl2
MoCl3
MoCl4
MoCl5
MoCl6 | TcCl4 | RuCl3 | RhCl3 | PdCl2 | AgCl | CdCl2 | InCl
InCl2
InCl3 | SnCl2
SnCl4 | SbCl3
SbCl5 | Te3Cl2
TeCl4 | ICl
ICl3 | XeCl
XeCl2
CsCl | BaCl2 |  | HfCl4 | TaCl5 | WCl2
WCl3
WCl4
WCl5
WCl6 | Re3Cl9
ReCl4
ReCl5
ReCl6 | OsCl4 | IrCl2
IrCl3
IrCl4 | PtCl2
PtCl4 | AuCl
AuCl3 | Hg2Cl2,
HgCl2 | TlCl | PbCl2,
PbCl4 | BiCl3 | PoCl2,
PoCl4 | AtCl  | RnCl2
FrCl | RaCl2 |  | Rf  | Db  | Sg  | Bh  | Hs  | Mt  | Ds  | Rg  | Cn  | Nh  | Fl  | Mc  | Lv  | Ts  | Og
| ↓  |  |
LaCl3 | CeCl3 | PrCl3 | NdCl2,
NdCl3 | PmCl3 | SmCl2,
SmCl3 | EuCl2,
EuCl3 | GdCl3 | TbCl3 | DyCl2,
DyCl3 | HoCl3 | ErCl3 | TmCl2
TmCl3 | YbCl2
YbCl3 | LuCl3
AcCl3 | ThCl4 | PaCl5 | UCl3
UCl4
UCl5
UCl6 | NpCl4 | PuCl3 | AmCl2
AmCl3 | CmCl3 | BkCl3 | CfCl3 | EsCl3 | Fm  | Md  | No  | LrCl3

* v
* t
* e

* Agents used in chemical warfare
* incapacitation
* riot control

Blood|

* Cyanogen
* Cyanogen bromide
* Cyanogen chloride (CK)
* Hydrogen cyanide (AC)
* Arsine
* Vinyl arsine

Blister|

* Arsenicals
* Ethyldichloroarsine (ED)
* Methyldichloroarsine (MD)
* Phenyldichloroarsine (PD)
* Lewisite (L)
* Mustard gas (HD H HT HL HQ)
* Nitrogen mustard
* HN1
* HN2
* HN3
* TL-301
* Nitrosocarbamates
* KB-16

Nerve|

| G-agents|

* Tabun (GA)
* Sarin (GB)
* Chlorosarin (GC)
* Soman (GD)
* Ethylsarin (GE)
* Cyclosarin (GF)
* GH
* GJ
* GK
* GL
* GM
* GN
* GO
* GP
* GQ
* GR
* GS
* GT
* GU
* Fluorotabun
* GV
* GV1
* GV2
* GV3
* GV4
* GV5
* GV6
* EA-1356
* EA-3534
* EA-4352
* EA-5414
* EA-5488
* Thiosarin
* Thiosoman
* Thiocyclosarin
* Crotylsarin

|

V-agents|

* EA-2192
* EA-3148
* EA-3317
* VD
* VE
* VF
* VG
* VH
* VJ
* VK
* VL
* VM
* VN
* VO
* VP
* VQ
* VR
* VS
* VT
* VU
* VV
* VW
* VY
* VZ
* VX
* V1
* V2
* V3
* V4
* V5
* V6
* IVX
* IIVx
* Chinese VX
* V-sub x (GD-7)

Novichok agents|

* A-230
* A-232
* A-234
* A-242
* A-262
* C01-A035
* C01-A039
* C01-A042

Carbamates|

* EA-3887
* EA-3887A
* EA-3948
* EA-3966
* EA-3990
* EA-4026
* EA-4038
* EA-4048
* EA-4056
* EA-4057
* EA-4181
* T-1123
* Octamethylene-bis(5-dimethylcarbamoxyisoquinolinium bromide)

Other|

* EA-2012
* EA-2054
* EA-2098
* EA-2613
* 2-Ethoxycarbonyl-1-methylvinyl cyclohexyl methylphosphonate
* Neopentylene fluorophosphate

Precursors|

* Chlorosarin
* Chlorosoman
* Cyclohexanol
* 1,8-Dibromooctane
* N,N-Diisopropylaminoethanol
* Dimethylamidophosphoric dichloride
* Dimethylamidophosphoric dicyanide
* Isopropyl alcohol
* Methyldichlorophosphine
* Methylphosphonic acid dichloride
* Methylphosphonyl difluoride
* Pinacolone
* Pinacolyl alcohol
* QL
* 3,3,5-Trimethylcyclohexanol

Neurotoxins|

* Saxitoxin (TZ)
* Botulinum toxin (BTX)
* Tetanospasmin (TeNT)
* Chlorophenylsilatrane
* Tetrodotoxin

Nettle|

* Phosgene oxime (CX)

Pulmonary/Choking agent|

* Chlorine
* Phosgene (CG)
* Perfluoroisobutene
* Chloropicrin (PS)
* Diphosgene (DP)
* Disulfur decafluoride
* Acrolein
* Ethyl bromoacetate
* Perchloromethyl mercaptan

Vomiting agent|

* Adamsite
* Chloropicrin
* Diphenylchlorarsine
* Diphenylcyanoarsine
* Diphenylaminecyanoarsine

Incapacitating|

* Agent 15 (BZ)
* Dimethylheptylpyran (DMHP)
* EA-3167
* EA-3443
* EA-3580
* EA-3834
* Kolokol-1
* LSD-25
* PAVA spray
* Sleeping gas

Riot control|

* Xylyl bromide
* Pepper spray (OC)
* Mace (spray)
* CN
* CS
* CR
* CNS

Other|

* Methyl fluoroacetate
* Fluoroethyl fluoroacetate
* Ricin
* Abrin
* Enterotoxin type B
* Depleted uranium
* post-combustion uranium oxides

* List of chemical warfare agents
* CB military symbol

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*[CID]: Compound ID
*[H300]: Fatal if swallowed
*[H301]: Toxic if swallowed
*[H330]: Fatal if inhaled
*[H314]: Causes severe skin burns and eye damage
*[H373]: May cause damage to organs through prolonged or repeated exposure
*[P260]: Do not breathe dust/fume/gas/mist/vapours/spray
*[P273]: Avoid release to the environment
*[P284]: Wear respiratory protection
*[P305+351+338]: IF IN EYES: Rinse continuously with water for several minutes. Remove contact lenses if present and easy to do – continue rinsing
*[P304+340+310]: IF INHALED: Remove victim to fresh air and keep at rest in a position comfortable for breathing. Immediately call a POISON CENTER or doctor/physician
*[P303+361+353]: IF ON SKIN (or hair): Remove/Take off immediately all contaminated clothing. Rinse skin with water/shower
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