Copper dinitrate Chemical Properties

Melting point:

115°C

Density 

1.00 g/mL at 20 °C

vapor pressure 

0Pa at 25℃

solubility 

soluble in dioxane; reacts with ethyl ether

form 

blue-green orthorhombic crystals

color 

blue-green orthorhombic crystals, crystalline; hygroscopic

Water Solubility 

Soluble

Merck 

13,2671

Stability:

Stable. Oxidant. Incompatible with combustible materials.

Surface tension

73.2mN/m at 1.3g/L and 20.2℃

CAS DataBase Reference

3251-23-8(CAS DataBase Reference)

EPA Substance Registry System

Cupric nitrate (3251-23-8)

Safety Information

Hazard Codes 

O,C,Xi,N,Xn

Risk Statements 

8-20/21/22-34-22-36/38-20-45-51/53-41-38-50/53-37/38-52/53

Safety Statements 

53-17-26-36/37/39-45-36-61-39

RIDADR 

UN 3085 5.1/PG 3

WGK Germany 

3

HazardClass 

5.1

PackingGroup 

II

Hazardous Substances Data

3251-23-8(Hazardous Substances Data)

MSDS

• Language:English Provider:SigmaAldrich

Copper dinitrate Usage And Synthesis

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(II) 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(II) 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(II) nitrate which can be sublimed in vacuum at 150°C and collected.

Reactions

Thermal decomposition of copper(II) nitrate produces copper oxides and nitrogen oxides.
In aqueous solutions, copper(II) 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(II) nitrate reacts with ether forming a complex.

Hazard

Copper(II) nitrate is moderately toxic by ingestion. Skin or eye contact can cause irritation.
LD50 oral (rat): 940 mg/kg.
Copper(II) nitrate, being an oxidizing agent, can undergo violent reactions with readily oxidizable substances. Reaction with acetic anhydride is violent, and heating with potassium or ammonium ferrocyanide at 220°C may cause an explosion. It can ignite paper on prolonged contact.

Description

Cupric nitrate is a blue crystalline solid.Molecular weight=187.55; Boiling point=170℃ (decomposes below this point); Freezing/Melting point=115℃.Soluble in water. Hazard Identification (based on NFPA-704 M Rating System): Health 1, Flammability 0,Reactivity 3 (Oxidizer). Soluble in water;solubility=135 g/100 mL (trihydrate).

Chemical Properties

Cupric nitrate is a Blue crystalline solid.

Uses

Light-sensitive papers; analytical reagent; mordant in textile dyeing; nitrating agent; insecticide for vines; coloring copper black; electroplating; production of burnished effect on iron; paints; varnishes, enamels; pharmaceutical preparations; catalyst.

Definition

ChEBI: An inorganic nitrate salt having copper(2+) as the couterion.

General Description

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.

Air & Water Reactions

Deliquescent. Water soluble.

Reactivity Profile

Mixtures of Copper dinitrate with alkyl esters may explode, owing to the formation of alkyl nitrates. Mixtures with phosphorus, tin(II) chloride or other reducing agents may react explosively [Bretherick, 1979 p. 108-109]. A finely divided mixture of potassium ferrocyanide and Copper dinitrate exploded when dried at 220°C [Chem. Abst. 77:1343 (1972)]. Noncombustible, but Copper dinitrate will accelerate the burning of combustible materials. If large quantities of the material are involved in a fire or the material is finely divided, an explosion may result. Prolonged exposure to fire or heat may result in an explosion.

Hazard

Oxidizer, causes violent combustion or explosion with organic materials.

Health Hazard

Inhalation causes irritation of throat and lungs. Ingestion of large amounts causes violent vomiting and purging, intense pain, collapse, coma, convulsions, and paralysis. Solutions irritate eyes; contact with solid causes severe eye surface injury and skin irritation.

Safety Profile

Moderately toxic by ingestion. A severe eye and skin irritant. Potentially explosive reaction above 22OOC with ammonium or potassium hexacyanoferrate(I1). Reaction with ammonia + potassium amide gives explosive product. Violent reaction with acetic anhydride. May ignite on prolonged contact with paper. Concentrated solutions may ipte in contact with tin or aluminum foil. Used as a fungicide, herbicide, and as a catalyst component in solid rocket fuel. When heated to decomposition it emits toxic fumes of NOx. See also COPPER COMPOUNDS and NITRATES.

Potential Exposure

Cupric nitrate is used as an insecticide, in paint, varnish, enamel, and in wood preservatives. Metal compounds are often used in “hot” operations in the work-place. These may include, but are not limited to, welding, brazing, soldering, plating, cutting, and metallizing. At the high temperatures reached in these operations, metals often form metal fumes which have different health effects and exposure standards than the original metal compound and require specialized controls.

First aid

If this chemical gets into the eyes, remove anycontact lenses at once and irrigate immediately for at least15 min, occasionally lifting upper and lower lids. Seek medical attention immediately. If this chemical contacts theskin, remove contaminated clothing and wash immediatelywith soap and water. Seek medical attention immediately. Ifthis chemical has been inhaled, remove from exposure,begin rescue breathing (using universal precautions, including resuscitation mask) if breathing has stopped and CPR ifheart action has stopped. Transfer promptly to a medicalfacility. When this chemical has been swallowed, get medical attention. Give large quantities of water and inducevomiting. Do not make an unconscious person vomit.Medical observation is recommended for 24-48 h afterbreathing overexposure, as pulmonary edema may bedelayed. As first aid for pulmonary edema, a doctor orauthorized paramedic may consider administering a corticosteroid spray.
Note to physician: In case of fume inhalation, treat for pulmonary edema. Give prednisone or other corticosteroid orally to reduce tissue response to fume. Positive pressureventilation may be necessary. Treat metal fume fever withbed rest, analgesics, and antipyretics. The symptoms ofmetal fume fever may be delayed for 4-12 h followingexposure: it may last less than 36 h.

Shipping

UN1479 Oxidizing solid, n.o.s., Hazard Class: 5.1; Labels: 5.1-Oxidizer, Technical Name Required.

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

Copper dinitrate(3251-23-8)Related Product Information

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