Copper ( II ) sulfate - wikipedia Copper ( II ) sulfate Copper ( II ) sulfate Structure of pentahydrate Crystals of CuSO 5H O Names IUPAC name Copper ( II ) sulfate Other names Cupric sulphate Blue vitriol ( pentahydrate ) Bluestone ( pentahydrate ) Bonattite ( trihydrate mineral ) Boothite ( heptahydrate mineral ) Chalcanthite ( pentahydrate mineral ) Chalcocyanite ( mineral ) Identifiers CAS Number 7758 - 98 - 7 7758 - 99 - 8 ( pentahydrate ) 16448 - 28 - 5 ( trihydrate ) 19086 - 18 - 1 ( heptahydrate ) 3D model ( JSmol ) Interactive image ChEBI CHEBI : 23414 ChEMBL ChEMBL604 ChemSpider 22870 ECHA InfoCard 100.028. 952 EC Number 231 - 847 - 6 E number E519 ( acidity regulators,... ) KEGG C18713 PubChem CID 24462 RTECS number GL8800000 ( anhydrous ) GL8900000 ( pentahydrate ) UNII KUW2Q3U1VV InChI InChI = 1S / Cu. H2O4S / c ; 1 - 5 ( 2, 3 ) 4 / h ; ( H2, 1, 2, 3, 4 ) / q + 2 ; / p - 2 Key : ARUVKPQLZAKDPS - UHFFFAOYSA - L InChI = 1 / Cu. H2O4S / c ; 1 - 5 ( 2, 3 ) 4 / h ; ( H2, 1, 2, 3, 4 ) / q + 2 ; / p - 2 Key : ARUVKPQLZAKDPS - NUQVWONBAI SMILES ( O - ) S ( = O ) ( = O ) ( O - ). ( Cu + 2 ) Properties Chemical formula CuSO ( anhydrous ) CuSO 5H O ( pentahydrate ) Molar mass 159.609 g / mol ( anhydrous ) 249.685 g / mol ( pentahydrate ) Appearance gray - white ( anhydrous ) blue ( pentahydrate ) Density 3.60 g / cm ( anhydrous ) 2.286 g / cm ( pentahydrate ) Melting point 110 ° C ( 230 ° F ; 383 K ) decomposes ( 5H O ) < 560 ° C decomposes Solubility in water 1.055 molal ( 10 ° C ) 1.26 molal ( 20 ° C ) 1.502 molal ( 30 ° C ) Solubility anhydrous insoluble in ethanol pentahydrate soluble in methanol 10.4 g / L ( 18 ° C ) insoluble in ethanol, insoluble in acetone Magnetic susceptibility ( χ ) + 1330 10 cm / mol Refractive index ( n ) 1.724 -- 1.739 ( anhydrous ) 1.514 -- 1.544 ( pentahydrate ) Structure Crystal structure Orthorhombic ( anhydrous, chalcocyanite ), space group Pnma, oP24, a = 0.839 nm, b = 0.669 nm, c = 0.483 nm. Triclinic ( pentahydrate ), space group P1, aP22, a = 0.5986 nm, b = 0.6141 nm, c = 1.0736 nm, α = 77.333 °, β = 82.267 °, γ = 72.567 ° Thermochemistry Std molar entropy ( S ) 5 J K mol Std enthalpy of formation ( Δ H ) − 769.98 kJ / mol Pharmacology ATC code V03AB20 ( WHO ) Hazards Safety data sheet anhydrous pentahydrate GHS pictograms NFPA 704 0 Flash point Non-flammable Lethal dose or concentration ( LD, LC ) : LD ( median dose ) 300 mg / kg ( oral, rat ) US health exposure limits ( NIOSH ) : PEL ( Permissible ) TWA 1 mg / m ( as Cu ) REL ( Recommended ) TWA 1 mg / m ( as Cu ) IDLH ( Immediate danger ) TWA 100 mg / m ( as Cu ) Related compounds Other cations Iron ( II ) sulfate Manganese ( II ) sulfate Nickel ( II ) sulfate Zinc sulfate Except where otherwise noted, data are given for materials in their standard state ( at 25 ° C ( 77 ° F ), 100 kPa ). verify ( what is ? ) Infobox references Copper ( II ) sulfate, also known as cupric sulfate, or copper sulphate, is the inorganic compound with the chemical formula Cu SO ( H O ), where x can range from 0 to 5. The pentahydrate ( x = 5 ) is the most common form. Older names for this compound include blue vitriol, bluestone, vitriol of copper, and Roman vitriol. The pentahydrate ( CuSO 5H O ), the most commonly encountered salt, is bright blue. It exothermically dissolves in water to give the aquo complex ( Cu ( H O ) ), which has octahedral molecular geometry. The structure of the solid pentahydrate reveals a polymeric structure wherein copper is again octahedral but bound to four water ligands. The Cu ( II ) ( H O ) centers are interconnected by sulfate anions to form chains. Anhydrous copper sulfate is a white powder. Contents 1 Preparation and occurrence 2 Chemical properties 2.1 Chemistry education 3 Uses 3.1 As a fungicide and herbicide 3.2 Analytical reagent 3.3 Organic synthesis 3.4 Niche uses 3.4. 1 Art 3.4. 2 Etching 3.4. 3 Dyeing 4 Medical and public health issues 5 Other form of copper sulfates 6 Toxicological effects 6.1 Environmental toxicity 7 See also 8 References 9 Bibliography 10 External links Preparation and occurrence Preparation of copper ( II ) sulfate by electrolyzing sulfuric acid, using copper electrodes Copper sulfate is produced industrially by treating copper metal with hot concentrated sulfuric acid or its oxides with dilute sulfuric acid. For laboratory use, copper sulfate is usually purchased. Copper sulfate can also be produced by slowly leaching low grade copper ore in air ; bacteria may be used to hasten the process. Commercial copper sulfate is usually about 98 % pure copper sulfate, and may contain traces of water. Anhydrous Copper sulfate is 39.81 percent copper and 60.19 percent sulfate by mass, and in its blue, hydrous form, it is 25.47 % copper, 38.47 % sulfate ( 12.82 % sulfur ) and 36.06 % water by mass. Four types of crystal size are provided based on its usage : large crystals ( 10 -- 40 mm ), small crystals ( 2 -- 10 mm ), snow crystals ( less than 2 mm ), and windswept powder ( less than 0.15 mm ). Chemical properties Copper ( II ) sulfate pentahydrate decomposes before melting. It loses two water molecules upon heating at 63 ° C ( 145 ° F ), followed by two more at 109 ° C ( 228 ° F ) and the final water molecule at 200 ° C ( 392 ° F ). Dehydration proceeds by decomposition of the tetraaquacopper ( 2 + ) moiety, two opposing aqua groups are lost to give a diaquacopper ( 2 + ) moiety. The second dehydration step occurs with the final two aqua groups are lost. Complete dehydration occurs when the only unbound water molecule is lost. At 650 ° C ( 1,202 ° F ), copper ( II ) sulfate decomposes into copper ( II ) oxide ( CuO ) and sulfur trioxide ( SO ). Copper sulfate reacts with concentrated hydrochloric acid to give tetrachlorocuprate ( II ) : Cu + 4 Cl → CuCl Chemistry education Copper sulfate is commonly included in children 's chemistry sets. It is often used to grow crystals in schools and in copper plating experiments, despite its toxicity. Copper sulfate is often used to demonstrate an exothermic reaction, in which steel wool or magnesium ribbon is placed in an aqueous solution of CuSO. It is used to demonstrate the principle of mineral hydration. The pentahydrate form, which is blue, is heated, turning the copper sulfate into the anhydrous form which is white, while the water that was present in the pentahydrate form evaporates. When water is then added to the anhydrous compound, it turns back into the pentahydrate form, regaining its blue color, and is known as blue vitriol. Copper ( II ) sulfate pentahydrate can easily be produced by crystallization from solution as copper ( II ) sulfate is quite hygroscopic. In an illustration of a `` single metal replacement reaction '', iron is submerged in a solution of copper sulfate. Iron reacts producing iron ( II ) sulfate and copper precipitates. Fe + CuSO → FeSO + Cu In high school and general chemistry education, copper sulfate is used as electrolyte for galvanic cells, usually as a cathode solution. For example, in a zinc / copper cell, copper ion in copper sulfate solution absorbs electron from zinc and forms metallic copper. Cu + 2e → Cu ( cathode ) E ° cell = 0.34 V Uses As a fungicide and herbicide Copper sulfate pentahydrate is used as a fungicide. However, some fungi are capable of adapting to elevated levels of copper ions. Bordeaux mixture, a suspension of copper ( II ) sulfate ( CuSO ) and calcium hydroxide ( Ca ( OH ) ), is used to control fungus on grapes, melons, and other berries. It is produced by mixing a water solution of copper sulfate and a suspension of slaked lime, a suspension of copper ( II ) hydroxide Cu ( OH ) and calcium sulfate, which is used to control fungus on grapes, melons, and other berries. Cheshunt compound, a commercial mixture of copper sulfate and ammonium carbonate ( discontinued ), is used in horticulture to prevent damping off in seedlings. As a non-agricultural herbicide, is it used to control invasive aquatic plants and the roots of plants situated near water pipes. It is used in swimming pools as an algicide. A dilute solution of copper sulfate is used to treat aquarium fishes for parasitic infections, and is also used to remove snails from aquariums. Copper ions are highly toxic to fish, however. Most species of algae can be controlled with very low concentrations of copper sulfate. Analytical reagent Several chemical tests utilize copper sulfate. It is used in Fehling 's solution and Benedict 's solution to test for reducing sugars, which reduce the soluble blue copper ( II ) sulfate to insoluble red copper ( I ) oxide. Copper ( II ) sulfate is also used in the Biuret reagent to test for proteins. Copper sulfate is used to test blood for anemia. The blood is tested by dropping it into a solution of copper sulfate of known specific gravity -- blood which contains sufficient hemoglobin sinks rapidly due to its density, whereas blood which does not sink or sinks slowly has insufficient amount of hemoglobin. In a flame test, its copper ions emit a deep green light, a much deeper green than the flame test for barium. Organic synthesis Copper sulfate is employed at a limited level in organic synthesis. The anhydrous salt is used as a dehydrating agent for forming and manipulating acetal groups. The hydrated salt can be intimately mingled with potassium permanganate to give an oxidant for the conversion of primary alcohols. Niche Uses Copper ( II ) sulfate has attracted many niche applications over the centuries. In industry copper sulfate has multiple applications. In printing it is an additive to book binding pastes and glues to protect paper from insect bites ; in building it is used as an additive to concrete to provide water resistance and disinfectant qualities. Copper sulfate can be used as a coloring ingredient in artworks, especially glasses and potteries. Copper sulfate is also used in firework manufacture as a blue coloring agent, but it is not safe to mix copper sulfate with chlorates when mixing firework powders. It corrects copper deficiencies in the soil and animals and stimulates farm animals ' growth. In decoration, copper sulfate adds color to cement, metals and ceramic. Some batteries, electrodes and wire contain copper sulfate. It is used in printing ink and hair dye and it creates a green color in fireworks. Lowering a copper etching plate into the copper sulfate solution. Copper sulfate was once used to kill bromeliads, which serve as mosquito breeding sites. Copper sulfate is used as a molluscicide to treat bilharzia in tropical countries. Copper sulfate is used as an anti-fungal agent to protect seeds against fungus and to protect horse hooves from infection. It inhibits growth of bacteria such as Escherichia coli. Art In 2008, the artist Roger Hiorns filled an abandoned waterproofed council flat in London with 75,000 liters of copper sulfate solution. The solution was left to crystallize for several weeks before the flat was drained, leaving crystal - covered walls, floors and ceilings. The work is titled Seizure. Since 2011, it has been on exhibition at the Yorkshire Sculpture Park. Etching Copper sulfate is used to etch zinc or copper plates for intaglio printmaking. It is also used to etch designs into copper for jewelry, such as for Champlevé. Dyeing Copper sulfate can be used as a mordant in vegetable dyeing. It often highlights the green tints of the specific dyes. Medical and public Health issues Copper sulfate was used in the past as an emetic. It is now considered too toxic for this use. It is still listed as an antidote in the World Health Organization 's Anatomical Therapeutic Chemical Classification System. Other form of copper sulfates Anhydrous copper ( II ) sulfate is a white solid. It can be produced by dehydration of the normally available pentahydrate copper sulfate. In nature, it found as the very rare mineral known as chalcocyanite. The pentahydrate also occurs in nature as chalcanthite. Two other copper sulfates comprise the remaining of these rare minerals : bonattite ( trihydrate ) and boothite ( heptahydrate ). Anhydrous copper ( II ) sulfate Picture of anhydrous CuSO. Space - filling model anhydrous CuSO. The rare ( bluish ) mineral boothite ( CuSO 7H O ) Toxicological effects Copper sulfate is an irritant. The usual routes by which humans can receive toxic exposure to copper sulfate are through eye or skin contact, as well as by inhaling powders and dusts. Skin contact may result in itching or eczema. Eye contact with copper sulfate can cause conjunctivitis, inflammation of the eyelid lining, ulceration, and clouding of the cornea. Upon oral exposure, copper sulfate is moderately toxic. According to studies, the lowest dose of copper sulfate that had a toxic impact on humans is 11 mg / kg. Because of its irritating effect on the gastrointestinal tract, vomiting is automatically triggered in case of the ingestion of copper sulfate. However, if copper sulfate is retained in the stomach, the symptoms can be severe. After 1 -- 12 grams of copper sulfate are swallowed, such poisoning signs may occur as a metallic taste in the mouth, burning pain in the chest, nausea, diarrhea, vomiting, headache, discontinued urination, which leads to yellowing of the skin. In cases of copper sulfate poisoning, injury to the brain, stomach, liver, or kidneys may also occur. Environmental toxicity Copper sulfate is highly soluble in water and therefore is easy to distribute in the environment. Copper in the soil may be from industry, motor vehicle, and architectural materials. According to studies, copper sulfate exists mainly in the surface soil and tends to bind organic matter. The more acidic the soil is, the less binding occurs. See also Chalcanthum References ^ Jump up to : Haynes, p. 4.62 Jump up ^ Haynes, p. 5.199 Jump up ^ Anthony, John W. ; Bideaux, Richard A. ; Bladh, Kenneth W. ; Nichols, Monte C., eds. ( 2003 ). `` Chalcocyanite ''. Handbook of Mineralogy ( PDF ). V. Borates, Carbonates, Sulfates. Chantilly, VA, US : Mineralogical Society of America. ISBN 0962209740. Jump up ^ Haynes, p. 10.240 Jump up ^ Kokkoros, P.A. ; Rentzeperis, P.J. ( 1958 ). `` The crystal structure of the anhydrous sulphates of copper and zinc ''. Acta Crystallographica. 11 ( 5 ) : 361 -- 364. doi : 10.1107 / S0365110X58000955. Jump up ^ Bacon, G.E. ; Titterton, D.H. ( 1975 ). `` Neutron - diffraction studies of CuSO 5H O and CuSO 5D O ''. Z. Kristallogr. 141 ( 5 -- 6 ) : 330 -- 341. doi : 10.1524 / zkri. 1975.141. 5 - 6.330. ^ Jump up to : `` NIOSH Pocket Guide to Chemical Hazards # 0150 ''. National Institute for Occupational Safety and Health ( NIOSH ). Jump up ^ Cupric sulfate. US National Institutes of Health Jump up ^ `` Copper ( II ) sulfate MSDS ''. Oxford University. Retrieved 2007 - 12 - 31. Jump up ^ Antoine - François de Fourcroy, tr. by Robert Heron ( 1796 ) `` Elements of Chemistry, and Natural History : To which is Prefixed the Philosophy of Chemistry ''. J. Murray and others, Edinburgh. Page 348. Jump up ^ Oxford University Press, `` Roman vitriol '', Oxford Living Dictionaries. Accessed on 2016 - 11 - 13 Jump up ^ Ting, V.P. ; Henry, P.F. ; Schmidtmann, M. ; Wilson, C.C. ; Weller, M.T. `` In situ neutron powder diffraction and structure determination in controlled humidities ''. Chem. Commun. 2009 : 7527 -- 7529. doi : 10.1039 / B918702B. ^ Jump up to : `` Uses of Copper Compounds : Copper Sulphate ''. copper.org. Copper Development Association Inc. Retrieved 10 May 2015. Jump up ^ Andrew Knox Galwey ; Michael E. Brown ( 1999 ). Thermal decomposition of ionic solids. Elsevier. pp. 228 -- 229. ISBN 0 - 444 - 82437 - 5. Jump up ^ Wiberg, Egon ; Nils Wiberg ; Arnold Frederick Holleman ( 2001 ). Inorganic chemistry. Academic Press. p. 1263. ISBN 0 - 12 - 352651 - 5. Jump up ^ `` Process for the preparation of stable copper ( II ) sulfate monohydrate applicable as trace element additive in animal fodders ''. Retrieved 2009 - 07 - 07. Jump up ^ Zumdahl, Steven ; DeCoste, Donald ( 2013 ). Chemical Principles. Cengage Learning. pp. 506 -- 507. ISBN 978 - 1 - 285 - 13370 - 6. Jump up ^ Johnson, George Fiske ( 1935 ). `` The Early History of Copper Fungicides ''. Agricultural History. 9 ( 2 ) : 67 -- 79. JSTOR 3739659. Jump up ^ Parry, K.E. ; Wood, R.K.S. ( 1958 ). `` The adaption of fungi to fungicides : Adaption to copper and mercury salts ''. Annals of Applied Biology. 46 ( 3 ) : 446 -- 456. doi : 10.1111 / j. 1744 - 7348.1958. tb02225. x. Jump up ^ `` Uses of Copper Compounds : Copper Sulfate 's Role in Agriculture ''. Copper.org. doi : 10.1111 / j. 1744 - 7348.1933. tb07770. x. Retrieved 2007 - 12 - 31. Jump up ^ Coutts, J, Edwards, A, Osborn, A, & Preston, GH, The Complete Book of Gardening, p. 533, Ward Lock, London ( 1954 ) Jump up ^ `` All About Copper Sulfate ''. National Fish Pharmaceuticals. Retrieved 2007 - 12 - 31. Jump up ^ Estridge, Barbara H. ; Anna P. Reynolds ; Norma J. Walters ( 2000 ). Basic Medical Laboratory Techniques. Thomson Delmar Learning. p. 166. ISBN 0 - 7668 - 1206 - 5. Jump up ^ Hoffman, R.V. ( 2001 ). Copper ( II ) Sulfate, in Encyclopedia of Reagents for Organic Synthesis. John Wiley & Sons. doi : 10.1002 / 047084289X. rc247. Jump up ^ Philip J. Kocienski ( 2005 ). Protecting Groups. Thieme. p. 58. ISBN 978 - 1 - 58890 - 376 - 1. Jump up ^ Jefford, C.W. ; Li, Y. ; Wang, Y. `` A Selective, Heterogeneous Oxidation using a Mixture of Potassium Permanganate and Cupric Sulfate : ( 3aS, 7aR ) - Hexahydro - ( 3S, 6R ) - Dimethyl - 2 ( 3H ) - Benzofuranone ''. Organic Syntheses. ; Collective Volume, 9, p. 462 ^ Jump up to : Copper Development Association. `` Uses of Copper Compounds : Table A - Uses of Copper Sulphate ''. copper. Copper Development Association Inc. Retrieved 12 May 2015. Jump up ^ Partin, Lee. `` The Blues : Part 2 ''. skylighter. Skylighter. Inc. Archived from the original on 21 December 2010. Retrieved 12 May 2015. Jump up ^ Despommier ; Gwadz ; Hotez ; Knirsch ( June 2005 ). Parasitic Disease ( 5 ed. ). NY : Apple Tree Production L.L.C. pp. Section 4.2. ISBN 978 - 0970002778. Retrieved 12 May 2015. Jump up ^ `` Seizure homepage ''. Artangel.org.uk. Retrieved 2009 - 09 - 21. Jump up ^ `` Roger Hiorns : Seizure ''. Yorkshire Sculpture Park. Retrieved 2015 - 02 - 22. Jump up ^ greenart.info, Bordeau etch, 2009 - 01 - 18, retrieved 2011 - 06 - 02. Jump up ^ ndiprintmaking.ca, The Chemistry of using Copper Sulfate Mordant, 2009 - 04 - 12, retrieved 2011 - 06 - 02. Jump up ^ http://mordent.com/etch-howto/, How to Electrolytically etch in copper, brass, steel, nickel silver or silver, retrieved 2015 - 05 - 2015. Jump up ^ Holtzmann, N.A. ; Haslam, R.H. ( July 1968 ). `` Elevation of serum copper following copper sulfate as an emetic ''. Pediatrics. 42 ( 1 ) : 189 -- 93. PMID 4385403. Jump up ^ Olson, Kent C. ( 2004 ). Poisoning & drug overdose. New York : Lange Medical Mooks / McGraw - Hill. p. 175. ISBN 0 - 8385 - 8172 - 2. Jump up ^ V03AB20 ( WHO ) Jump up ^ Windholz, M., ed. 1983. The Merck Index. Tenth edition. Rahway, NJ : Merck and Company. ^ Jump up to : Guidance for reregistration of pesticide products containing copper sulfate. Fact sheet no. 100., Washington, DC : U.S. Environmental Protection Agency, Office of Pesticide Programs, 1986 Jump up ^ TOXNET. 1975 -- 1986. National library of medicine 's toxicology data network. Hazardous Substances Data Bank ( HSDB ). Public Health Service. National Institute of Health, U.S. Department of Health and Human Services. Bethesda, MD : NLM. ^ Jump up to : Clayton, G.D. and F.E. Clayton, eds. 1981. Patty 's industrial hygiene and toxicology. Third edition. Vol. 2, Part 6 Toxicology. NY : John Wiley and Sons. ISBN 0 - 471 - 01280 - 7 Jump up ^ National Institute for Occupational Safety and Health ( NIOSH ). 1981 -- 1986. Registry of toxic effects of chemical substances ( RTECS ). Cincinnati, OH : NIOSH. Jump up ^ United State Environment Protection Agency. `` Reregistration Eligibility Decision ( RED ) for Coppers '' ( PDF ). www.epa.org. United State Environment Protection Agency. Retrieved 12 May 2015. Bibliography Haynes, William M., ed. ( 2011 ). CRC Handbook of Chemistry and Physics ( 92nd ed. ). Boca Raton, FL : CRC Press. ISBN 1439855110. External links Wikimedia Commons has media related to Copper ( II ) sulfate. International Chemical Safety Card 0751 International Chemical Safety Card 1416 National Pollutant Inventory -- Copper and compounds fact sheet Copper compounds Cu ( 0, I ) Cu Si Cu ( I ) CuBr CuCN CuCl CuF CuH CuI Cu C Cu Cr O Cu O CuOH CuNO Cu P Cu S CuSCN Cu ( I, II ) Cu H O S Cu ( II ) Cu ( BF ) CuBr CuC CuCO Cu ( CN ) Cu ( ClO ) CuCl CuF Cu ( NO ) Cu ( PO ) CuN CuO CuO Cu ( OH ) CuI CuS CuSO Cu ( AsO ) Cu ( III ) K CuF Cu O Cu ( IV ) Cs CuF Rb CuF hide Salts and esters of the sulfate ion H SO He Li SO BeSO esters ROSO ( RO ) SO ( NH ) SO ( N H ) HSO ( NH OH ) SO NOHSO HOSO Ne Na SO NaHSO MgSO Al ( SO ) Al SO ( OAc ) Si SO HSO HSO ( HSO ) Cl Ar K SO KHSO CaSO Sc ( SO ) TiOSO VSO V ( SO ) VOSO CrSO Cr ( SO ) MnSO FeSO Fe ( SO ) CoSO NiSO CuSO Cu SO ( Cu ( NH ) ( H O ) ) SO ZnSO Ga ( SO ) Ge As Se Br Kr RbHSO Rb SO SrSO Y ( SO ) Zr ( SO ) Nb Mo Tc Ru Rh PdSO Ag SO CdSO In ( SO ) SnSO Sb ( SO ) Te Xe Cs SO BaSO Hf Ta Re Os Ir Pt Au Hg SO HgSO Tl SO Tl ( SO ) PbSO Bi ( SO ) Po At Rn Fr Ra Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og ↓ La Ce ( SO ) Ce ( SO ) Pr ( SO ) Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb ( SO ) Lu Ac Th Pa U ( SO ) UO SO Np Pu Am Cm Bk Cf Es Fm Md No Lr Antidotes ( V03AB ) Nervous system Nerve agent / Organophosphate poisoning Atropine Biperiden Diazepam Oximes Obidoxime Pralidoxime see also : Cholinesterase Barbiturate overdose Bemegride Ethamivan Benzodiazepine overdose Cyprodenate Flumazenil GHB overdose Physostigmine SCH - 50911 Opioid overdose Diprenorphine Doxapram Nalmefene Nalorphine Naloxone Naltrexone Reversal of neuromuscular blockade Sugammadex Circulatory system Beta blocker Glucagon Digoxin toxicity Digoxin Immune Fab Heparin Protamine Other Arsenic poisoning Dimercaprol Succimer Cyanide poisoning 4 - Dimethylaminophenol Hydroxocobalamin nitrite Amyl nitrite Sodium nitrite Sodium thiosulfate Hydrofluoric acid Calcium gluconate Methanol / Ethylene glycol poisoning Primary alcohols : Ethanol Fomepizole Paracetamol toxicity ( Acetaminophen ) Acetylcysteine Glutathione Methionine Toxic metals ( cadmium lead mercury thallium ) Dimercaprol Edetates Prussian blue Other iodine - 131 Potassium iodide Methylthioninium chloride oxidizing agent Potassium permanganate Prednisolone / promethazine Emetic Copper sulfate Ipecacuanha Syrup of ipecac WHO - EM Withdrawn from market Clinical trials : Phase III Never to phase III GND : 4166168 - 0 LCCN : sh85032394 Retrieved from `` https://en.wikipedia.org/w/index.php?title=Copper(II)_sulfate&oldid=836145948 '' Categories : Copper compounds Sulfates Desiccants Herbicides Hidden categories : Chemical articles with multiple compound IDs Multiple chemicals in an infobox that need indexing Chemical articles with multiple CAS registry numbers Articles with changed CASNo identifier ECHA InfoCard ID from Wikidata E number from Wikidata Chembox having GHS data Articles containing unverified chemical infoboxes Chembox image size set All articles with unsourced statements Articles with unsourced statements from April 2018 Pages containing citation needed template with deprecated parameters Articles with unsourced statements from January 2018 Articles with unsourced statements from May 2015 Wikipedia articles with GND identifiers Wikipedia articles with LCCN identifiers Talk Contents About Wikipedia تۆرکجه বাংলা Bân - lâm - gú Български Català Čeština Dansk Deutsch Eesti Ελληνικά Español Esperanto فارسی Français 한국어 Հայերեն हिन्दी Bahasa Indonesia Italiano עברית Кыргызча Latviešu Magyar മലയാളം Bahasa Melayu Монгол Nederlands 日本 語 Norsk Occitan ਪੰਜਾਬੀ Plattdüütsch Polski Português Română Русский Scots Simple English Slovenčina Slovenščina Српски / srpski Srpskohrvatski / српскохрватски Suomi Svenska தமிழ் తెలుగు ไทย Türkçe Українська Tiếng Việt 中文 43 more Edit links This page was last edited on 12 April 2018, at 22 : 58. 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Question: what is the molar mass of copper(ll) sulfate cuso4
Answer: 159.609 g/mol