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EC / List no.: 221-838-5
CAS no.: 3251-23-8
Mol. formula: Cu.2HNO3
Copper nitrate, Cu(NO3)2, is an inorganic compound that forms a blue crystalline solid.
Anhydrous copper nitrate forms deep blue-green crystals and sublimes in a vacuum at 150-200 °C.
Copper nitrate also occurs as five different hydrates, the most common ones being the hemipentahydrate and trihydrate.
Synthesis and reactions for copper nitrate
Hydrated copper nitrate can be prepared by hydration of the anhydrous material or by treating copper metal with an aqueous solution of silver nitrate or concentrated nitric acid:
Cu + 4 HNO3 → Cu(NO3)2 + 2 H2O + 2 NO2
Anhydrous Cu(NO3)2 forms when copper metal is treated with N2O4:
Cu + 2 N2O4 → Cu(NO3)2 + 2 NO
Attempted dehydration of any of the hydrated copper nitrates by heating instead affords the oxides, not Cu(NO3)2.
At 80 °C, the hydrates convert to "basic copper nitrate" (Cu2(NO3)(OH)3), which converts to CuO at 180 °C.
Exploiting this reactivity, copper nitrate can be used to generate nitric acid by heating it until decomposition and passing the fumes directly into water.
This method is similar to the last step in the Ostwald process.
The equations are as follows:
2 Cu(NO3)2 → 2 CuO + 4 NO2 + O2
3NO2 + H2O → 2HNO3 + NO
Natural basic copper nitrates include the rare minerals gerhardtite and rouaite, both being polymorphs of Cu2(NO3)(OH)3 substance.
A much more complex, basic, hydrated and chloride-bearing natural salt is buttgenbachite.
Structure
Anhydrous copper nitrate
Anhydrous copper nitrate has been crystallized in two solvate-free polymorphs.
α- and β-Cu(NO3)2 are fully 3D coordination polymer networks. The alpha form has only one Cu environment, with [4+1] coordination, but the beta form has two different copper centers, one with [4+1] and one that is square planar.
The nitromethane solvate also features "[4+ 1] coordination", with four short Cu-O bonds of approximately 200 pm and one longer bond at 240 pm.
They are coordination polymers, with infinite chains of copper centers and nitrate groups.
In the gas phase, copper(II) nitrate features two bidentate nitrate ligands (see image at upper right).
Thus, evaporation of the solid entails "cracking" to give the copper nitrate molecule.
Hydrated copper nitrate
Five hydrates have been reported: the monohydrate (Cu(NO3)2·H2O), the sesquihydrate (Cu(NO3)2·1.5H2O), the hemipentahydrate (Cu(NO3)2·2.5H2O), a trihydrate (Cu(NO3)2·3H2O), and a hexahydrate ([Cu(H2O)6](NO3)2).
The hexahydrate is interesting because the Cu-O distances are all equal, not revealing the usual effect of Jahn-Teller distortion that is otherwise characteristic of octahedral Cu(II) complexes.
This non-effect is attributed to the strong hydrogen bonding that limits the elasticity of the Cu-O bonds.
Applications
Copper nitrate finds a variety of applications, the main one being its conversion to copper, oxide, which is used as catalyst for a variety of processes in organic chemistry.
Its solutions are used in textiles and polishing agents for other metals.
Copper nitrates are found in some pyrotechnics.
It is often used in school laboratories to demonstrate chemical voltaic cell reactions.
It is a component in some ceramic glazes and metal patinas.
Organic synthesis
Copper nitrate, in combination with acetic anhydride, is an effective reagent for nitration of aromatic compounds, known as the Menke nitration in honor of the Dutch chemist who discovered that metal nitrates are effective reagents for nitration.
Hydrated copper nitrate adsorbed onto clay affords a reagent called "Claycop".
The resulting blue-colored clay is used as a slurry, for example for the oxidation of thiols to disulfides.
Claycop is also used to convert dithioacetals to carbonyls.
A related reagent based on montmorillonite has proven useful for the nitration of aromatic compounds.
Physical Properties
Blue-green orthorhombic crystals; deliquescent; sublimes; readily dissolves in water, alcohols and dioxane.
The trihydrate and hexahydrate are blue rhombohedral crystals; hygroscopic; density 2.32 g/cm3 (trihydrate), 2.07 g/cm3 (hexahydrate); melts at 114°C (trihydrate); trihydrate decomposes at 170°C; hexahydrate decomposes to trihydrate at 26.4°C; both the hydrates are very soluble in water and ethanol.
Uses:
Copper nitrate is used in light-sensitive reproduction papers; as a mordant in dyeing and printing of fabrics; as a coloring reagent for ceramics; for coloring copper black; as a burnishing agent for iron; in nickel-plating baths; in pyrotechnic compositions; and in paints, varnishes, and enamels. Other applications are as an oxidizing agent; nitrating agent for aromatics; as a catalyst; and an analytical standard for copper.
Copper nitrate trihydrate occurs in nature as the mineral gerhardite.
Preparation
Copper nitrate is made by action of copper or copper(II) oxide with nitric acid.
The solution is evaporated and the product is obtained by crystallization CuO + 2HNO3 → Cu(NO3)2 + H2O
The nitrate salt prepared by this method is hydrated.
It cannot be dehydrated fully without decomposition.
Anhydrous CuNO3 may be prepared by dissolving copper metal in a solution of dinitrogen tetroxide, N2O4, in ethyl acetate.
Upon crystallization, an N2O4 adduct of Cu(NO3)2 that probably has the composition [NO+][Cu(NO3)3] is obtained.
This adduct, on heating at 90°C, yields blue anhydrous Copper nitrate which can be sublimed in vacuum at 150°C and collected.
Reactions
Thermal decomposition of Copper nitrate produces copper oxides and nitrogen oxides.
In aqueous solutions, Copper nitrate undergoes many double decomposition reactions with soluble salts of other metals, forming precipitates of insoluble copper salts.
When H2S is passed through its aqueous solution, black CuS precipitates.
Copper nitrate reacts with ether forming a complex.
Obtained as a trihydrate and as a hexahydrate.
Both are blue crystalline solids.
Used in medicine, as an insecticide, in chemical analysis, in making light sensitive papers.
Toxic oxides of nitrogen are produced in fires involving Copper dinitrate.
Purification Methods
Crystallise it from weak aqueous HNO3 (0.5mL/g) by cooling from room temperature.
The anhydrous salt can be prepared by dissolving copper metal in a 1:1 mixture of liquid NO2 and ethyl acetate and purified by sublimation [Evans et al. J Chem Soc, Faraday Trans 1 75 1023 1979].
The hexahydrate dehydrates to the trihydrate at 26o, and the anhydrous salt sublimes between 150 and 225o, but melts at 255-256o and is deliquescent.
Incompatibilities
A strong oxidizer.
Aqueous solution is acidic; incompatible with bases.
Violent reaction with potassium hexacyanoferrate; ammonia and potassium amide mixtures; acetic anhydrides, cyanides, ethers.
Forms explosive materials with nitromethanes, sodium hypobromite; acetylene; chemically active metals, such as potassium, sodium, etc. May ignite on contact with aluminum foil or tin.
Risk of spontaneous combustion with combustibles (wood, cloth, etc.) organics, or reducing agents and readily oxidizable materials. Attacks metals in the presence of moisture.
Waste Disposal
Copper-containing soluble wastes can be concentrated through the use of ion exchange, reverse osmosis, or evaporators to the point where copper can be electrolytically removed and sent to a reclaiming firm.
If recovery is not feasible, the copper can be precipitated through the use of caustics and the sludge deposited in a chemical waste landfill.
Add slowly to water; stir in excess soda ash.
Let stand, then neutralize. Decant solution and flush to sewer; landfill sludge
Obtained as a trihydrate and as a hexahydrate. Both are blue crystalline solids.
Used in medicine, as an insecticide, in chemical analysis, in making light sensitive papers.
Toxic oxides of nitrogen are produced in fires involving this material.
Use and Manufacturing
Household & Commercial/Institutional Products
• Auto Products
• Commercial / Institutional
• Inside the Home
• Pet Care
For Copper nitrate(USEPA/OPP Pesticide Code: 076102) there are 0 labels match.
In light sensitive reproductive papers; as ceramic color;
as mordant and oxidant in textile dyeing and printing; as reagent for burnishing iron, for giving a black "antique" finish to copper; for coloring zinc brown;
in nickel plating baths; in aluminum brighteners;
in wood preservatives, fungicides, herbicides; in pyrotechnic compositions; as catalyst component in solid rocket fuel;
as nitrating agent for aromatic organosilicon cmpd; as catalyst for organic reactions.
Glaze/ceramics ingredient; pyrotechnic/rocket fuel ingredient;
mordant/oxidizing agent (textile dyeing); metal surface treatments agent
Light-sensitive papers; analytical reagent; mordant in textile dyeing;
nitrating agent;
insecticide for vines;
coloring copper black;
electroplating;
production of burnished effected on iron;
paints;
varnishes, enamels;
pharmaceuticals preparations;
catalyst.
Industry Use:
Adhesives and sealant chemicals
Copper Metal
Industrial Use
Intermediates
Process regulators
Processing aids, specific to petroleum production
Consumer Uses
Fuels and related products
Methods of Manufacturing
By treating copper or copper oxide with nitric acid.
The solution is evaporated and product recovered by crystallization. /Hydrated salts/
Dissolving copper in nitric acid solution; dissolving copper(II) oxide, basic copper(II) carbonate or copper(II) hydroxide in nitric acid solution.
General Manufacturing Information
Industry Processing Sectors
All other basic inorganic chemical manufacturing
All other chemical product and preparation manufacturing
Other - Secondary Precious Metals Reclaimers
Petroleum refineries
Primary metal manufacturing
Propellant
Copper Nitrate is generally immediately available in most volumes. High purity, submicron and nanopowder forms may be considered.
Typical and custom packaging is available.
Copper nitrate is the chemical compound with the formula Cu(NO3)2.
Commonly referred to simply as copper nitrate, the anhydrous form is a blue, crystalline solid.
Hydrated forms of copper nitrate, also blue, are commonly used in school laboratories to demonstrate chemical voltaic cell reactions.
The hydrated and anhydrous species have remarkably different properties, illustrating the effect of water of crystallization.
The Roman numeral sign is to specify that the copper has an oxidation state of +2.
Properties
Hydrated and anhydrous copper nitrates behave differently.
Anhydrous form
The bright blue anhydrous material, Cu(NO3)2, is a volatile solid, subliming in a vacuum.
In the gas-phase, Cu(NO3)2 is square planar, each Cu center being surrounded by four oxygen atoms.
Upon condensation, this monomer polymerizes.
Hydrated copper nitrate
Crystalline Cu(NO3)2(H2O)2.5 features octahedral Cu centers surrounded by water and the nitrate anions.[1] This hydrate decomposes at ca. 170 °C into copper oxide, nitrogen dioxide and oxygen:
2Cu(NO3)2(s) → 2CuO(s) + 4NO2(g) + O2(g)
Copper nitrate can be used to generate nitric acid by heating it until decomposition and passing the fumes directly into water.
This method is similar to the last step in the Ostwald process.
The equations are as follows:
2Cu(NO3)2 → 2CuO + 4NO2 + O2
3NO2 + H2O → 2 HNO3 + NO
Copper nitrate soaked splints of wood burn with an emerald green flame.
Addition of Magnesium nitrate gives a lime green color.
Synthesis
Cu(NO3)2 forms when copper metal is treated with N2O4:
Cu + 2 N2O4 → Cu(NO3)2 + 2 NO
It can also be formed by reacting copper metal with an aqueous solution of silver nitrate, see this page for more info.
Use in organic synthesis
Copper nitrate, in combination with acetic anhydride, is an effective reagent for nitration of aromatic compounds, under what are known as "Menke conditions", in honor of the Dutch chemist who discovered that metal nitrates are effective reagents for nitration.
Hydrated copper nitrate absorbed onto clay affords a reagent called "claycop".
The resulting blue clay is used as a slurry, for example for the oxidation of thiols to disulfides.
Claycop is also used to convert dithioacetals to carbonyls.
A related reagent based on Montmorillonite has proven useful for the nitration of aromatic compounds
About Copper nitrate
Helpful information
Copper nitrate is registered under the REACH Regulation and is manufactured in and / or imported to the European Economic Area, at ≥ 1 000 to < 10 000 tonnes per annum.
Copper nitrate is used by consumers, in articles, by professional workers (widespread uses), in formulation or re-packing, at industrial sites and in manufacturing.
Consumer Uses
Copper nitrate is used in the following products: lubricants and greases, coating products, fillers, putties, plasters, modelling clay, fertilisers, metal surface treatment products, non-metal-surface treatment products, inks and toners, leather treatment products, polishes and waxes and cosmetics and personal care products.
Other release to the environment of Copper nitrate is likely to occur from: indoor use (e.g. machine wash liquids/detergents, automotive care products, paints and coating or adhesives, fragrances and air fresheners), outdoor use and outdoor use in close systems with minimal release (e.g. hydraulic liquids in automotive suspension, lubricants in motor oil and break fluids).
Article service life
Release to the environment of Copper nitrate can occur from industrial use: industrial abrasion processing with low release rate (e.g. cutting of textile, cutting, machining or grinding of metal).
Other release to the environment of Copper nitrate is likely to occur from: indoor use in long-life materials with low release rate (e.g. flooring, furniture, toys, construction materials, curtains, foot-wear, leather products, paper and cardboard products, electronic equipment) and outdoor use in long-life materials with low release rate (e.g. metal, wooden and plastic construction and building materials).
Copper nitrate can be found in complex articles, with no release intended: machinery, mechanical appliances and electrical/electronic products (e.g. computers, cameras, lamps, refrigerators, washing machines).
Copper nitrate can be found in products with material based on: stone, plaster, cement, glass or ceramic (e.g. dishes, pots/pans, food storage containers, construction and isolation material), fabrics, textiles and apparel (e.g. clothing, mattress, curtains or carpets, textile toys) and leather (e.g. gloves, shoes, purses, furniture).
Widespread uses by professional workers
Copper nitrate is used in the following products: fertilisers, coating products, fillers, putties, plasters, modelling clay, metal surface treatment products, inks and toners, lubricants and greases, polishes and waxes and cosmetics and personal care products.
Copper nitrate is used in the following areas: formulation of mixtures and/or re-packaging and building & construction work.
Copper nitrate is used for the manufacture of: chemicals and mineral products (e.g. plasters, cement).
Other release to the environment of Copper nitrate is likely to occur from: outdoor use, indoor use (e.g. machine wash liquids/detergents, automotive care products, paints and coating or adhesives, fragrances and air fresheners) and outdoor use in close systems with minimal release (e.g. hydraulic liquids in automotive suspension, lubricants in motor oil and break fluids).
Formulation or re-packing
Copper nitrate is used in the following products: adsorbents, air care products, coating products, fillers, putties, plasters, modelling clay, fertilisers, metal surface treatment products, non-metal-surface treatment products, inks and toners, pH regulators and water treatment products, laboratory chemicals, leather treatment products, lubricants and greases, polishes and waxes, polymers and cosmetics and personal care products.
Copper nitrate has an industrial use resulting in manufacture of another substance (use of intermediates).
Release to the environment of Copper nitrate can occur from industrial use: formulation of mixtures and formulation in materials.
Uses at industrial sites
Copper nitrate is used in the following products: pH regulators and water treatment products and adsorbents.
Copper nitrate has an industrial use resulting in manufacture of another substance (use of intermediates).
Copper nitrate is used in the following areas: formulation of mixtures and/or re-packaging.
Copper nitrate is used for the manufacture of: chemicals.
Release to the environment of Copper nitrate can occur from industrial use: in the production of articles, as an intermediate step in further manufacturing of another substance (use of intermediates), as processing aid and in processing aids at industrial sites.
Manufacture
Release to the environment of Copper nitrate can occur from industrial use: manufacturing of the substance.
Description
Large green blue, deliquescent crystals. Copper nitrate is used to colorize metals.
Copper nitrategives a blackened, or antique, look to Copper and turns Zinc brown.
Additionally Copper nitrateis used to brighten Aluminum and burnish Iron.
Copper nitrate is used as a mordant and oxidizing agent in textile dyeing.
Copper nitrateis used as a pigment for Glass, enamels, and ceramics.
Because of its toxicity, it is also used as a Fungicide, and wood preservative.
Properties
Chemical
Decomposition of copper nitrate yields nitrogen dioxide gas.
2 Cu(NO3)2 → 2 CuO + 4 NO2 + O2
This reaction is a cheap source of nitrogen dioxide, which can be bubbled through water to generate nitric acid through the following reaction:
3 NO2 + H2O → 2 HNO3 + NO
Bubbling it through hydrogen peroxide is much more efficient.
2 NO2 + H2O2 → 2 HNO3
In combination with acetic anhydride, it is an effective reagent for nitration of aromatic compounds.
As with many other copper(II) salts, Copper nitrate yields a blue to green coloration in flame tests.
Unlike other copper compounds, though, the nitrate is also an oxidizer, making it useful for producing brilliantly colored flames in pyrotechnics without slowing down the reactions too much.
The resulting mixture can not be stored however, due to the hygroscopicity of copper nitrate.
Physical
Anhydrous copper nitrate is deep-blue-green.
It is highly hygroscopic and will turn into at least 5 hydrates, as it absorbs more and more water.
The hydrates are blue and hygroscopic.
The hydrates cannot be dried by heating, as this will decompose the salt, leaving black copper(II) oxide and will give off nitrogen dioxide and nitric acid fumes.
Copper nitrate solutions can occasionally change their color from blue-green to green.
Availability
Copper nitrate is available as both anhydrous and hydrate at many chemical suppliers as well as on Ebay.
Preparation
Copper nitrate hydrated can be prepared by reacting copper with nitric acid.
Cu + 4 HNO3 → Cu(NO3)2 + 2 H2O + 2 NO2
It can also be prepared by mixing two concentrated solutions of calcium nitrate and copper(II) sulfate.
Calcium sulfate will precipitate, while the much more soluble copper nitrate will remain in solution.
Filter the solution (it's recommended you use vacuum filtration as gypsum tends to hold water).
The resulting solution is dried in a desiccator at room temperature, or just a bit higher, to avoid decomposing the fragile salt.
When it's dried, the resulting blue-green crystals have a fluffy aspect. They should be stored in sealed dry bottles, as they're hygroscopic.
Anhydrous copper nitrate synthesis eluded chemists for a long time, but in 1969s a method was discovered.
By adding dinitrogen tetroxide to copper metal in anhydrous conditions and then gently heating the resulting product to 80°C to get rid of the nitrogen oxides, pure anhydrous copper nitrate results.
Cu + 2 N2O4 → Cu(NO3)2 + 2 NO[1]
Projects
Nitric acid synthesis
Nitrating aromatic compounds
Blue-green flames in pyrotechnics
IUPAC NAMES:
Cobre(II) Nitrato 3-hidrato
Copper ( II ) Nitrate
copper (II) nitrate
Copper dinitrate
copper dinitrate
Copper Dinitrate
Copper dinitrate
copper dinitrate trihydrate
copper nitrate
Copper Nitrate
copper(2+) dinitrate
Copper nitrate
copper(II) nitrate
Copper(II) Nitrate 2-water
COPPER(II)NITRATE
copper;dinitrate
CUPRIC NITRATE ANHYDROUS
SYNONYMS:
cupricnitratesolution
Nitricacid,copper(2+)salt
nitricacid,copper(2++)salt
cupric nitrate, n-hydrate
Copper(Ⅱ) nitrate trihydrate
Copper nitrate on Celiteloading 30wt. %
COPPER ICP STANDARD, CU(NO3)2
CU(NO3)2
COPPER (II) NITRATE
COPPER NITRATE
Copper(II) nitrate on Celite®
Nitric acid, copper(2+) salt (2:1)
claycop
copper(2+)nitrate
Copperbis(nitrate)
coppernitrite,trihydrate
cupricdinitrate
cupricnitrate(copper(ii)
cupricnitrate(copper(ii)nitrate)
COPPER(II) NITRATE 26 WT. % ON SILICA &
COPPER ION STANDARD SOLUTION FLUKA &
copper standard for ic
copper(ii) nitrate on celite
copper(ii) nitrate solution
Kupfer(II)-nitrat
Copper dinitrate
Copper nitrate: (Cupric nitrate)
Copper(II) nitrate on Celite(R)
Copper standard for AAS
Copper atomic spectroscopy standard concentrate 1.000 g Cu
Copper(II) nitrate on silica gel
Copper ion standard solution
Copper, certified metal standard solution for atomic spectrometry
Bisnitric acid copper(II) salt
Copper(II)dinitrate
Dinitric acid copper(II) salt
Cupric nitrate
Copper solution 1000 ppm, for AAS 500ML
Cupric nitrate,Copper dinitrate
Copper dinitrate ISO 9001：2015 REACH
Copper dinitrate
CUPRIC NITRATE
Copper(II) nitrate
3251-23-8
Copper nitrate
copper;dinitrate
Cupric dinitrate
Copper(2+) nitrate
Nitric acid, copper(2+) salt
UNII-9TC879S2ZV
Copper nitrate basic
Nitric acid, copper(2+) salt (2:1)
9TC879S2ZV
10402-29-6
Claycop
Caswell No. 246
HSDB 264
Nitric acid, copper salt
EINECS 221-838-5
EPA Pesticide Chemical Code 076102
Cop-per nitrate
copper(2+) dinitrate
CuN2O6
EC 221-838-5
copper(II) nitrate (anh.)
Cu(NO3)2
copper(II) nitrate (anhydrous)
DTXSID7040314
CHEBI:78036
AKOS01590339
S627
FT-0624045
FT-0624120
Q286064
