PRODUCTS

COPPER(II) CARBONATE

Copper(II) carbonate is also used as a reagent in organic synthesis and as a precursor to other copper compounds.
Copper(II) carbonate is utilized in a variety of applications.
Copper(II) carbonate is frequently used to produce compounds for the treatment of wood.

CAS number(s): 1184-64-1 (CuCO₃) and 12069-69-1 (copper(II) carbonate–copper(II) hydroxide basic mixture)
EC number(s): common registry entries include 214-671-4 and the basic copper carbonate REACH entry 235-113-6 (for the CuCO₃·Cu(OH)₂ material).
Molecular formula (neutral): CuCO₃.
Basic copper carbonate formulas: CuCO₃·Cu(OH)₂ or Cu₂(OH)₂CO₃ or CH6Cu2O5 depending on notation.
Molar mass: ~123.55 g·mol⁻¹ (neutral CuCO₃).

SYNONYMS:
Cupric carbonate, copper carbonate, copper(II) carbonate, neutral copper carbonate, cupric carbonate (basic), basic copper carbonate, copper carbonate hydroxide, malachite (mineral form — basic carbonate), azurite (related basic carbonate), CuCO3, CuCO₃·Cu(OH)₂, Copper(II) carbonate, Other names, Cupric carbonate, neutral copper carbonate, Copper carbonate, 1184-64-1, Copper(II) carbonate, Copper monocarbonate, Copper carbonate (1:1), Cupric carbonate (1:1), Copper carbonate (CuCO3), Carbonic acid, copper(2+) salt (1:1), 9AOA5F11GJ, DTXSID6034471, RefChem:127899, copper(2+) ion carbonate, DTXCID4014471, DTXSID6058473, 214-671-4, CUPRIC CARBONATE, copper, carbonate, MFCD00051038, 7492-68-4, Carbonic acid, copper salt, Cupromaag, HSDB 258, EINECS 214-671-4, UNII-9AOA5F11GJ, CUPRICCARBONATE, CCuO3, Copper (II) carbonate, Carbonic acid,copper salt, cupric carbonate, AldrichCPR, SCHEMBL29678, COPPER (AS CARBONATE), COPPER(II) CARBONATE [HSDB], SY347833, DB-208425, NS00078651, D78271, F494383, F988213, Q409630, Cupric carbonate basic, Copper carbonate (1:1), Copper monocarbonate, Cupric carbonate, Carbonic acid, copper(2+) salt (1:1), Kop karb, Cheshunt compound, Basic copper carbonate, Basic cupric carbonate, Caswell No. 235, Copper carbonate, basic, Cupric carbonate, basic, Copper carbonate hydroxide, Dicopper dihydroxycarbonate, (Carbonato)dihydroxydicopper, Basic copper(II) carbonate, Carbonic acid, copper complex, Copper(II) carbonate hydroxide, Copper, (carbonato)dihydroxydi-, (Carbonato(2-))dihydroxydicopper, EINECS 235-113-6, EPA Pesticide Chemical Code 022901, Copper hydroxy carbonate (Cu2(OH)2CO3), Copper hydroxide carbonate (Cu2(OH)2CO3), Copper hydroxide carbonate (CuCO3.Cu(OH)2

Copper(II) carbonate or cupric carbonate is a chemical compound with formula CuCO3.
At ambient temperatures, Copper(II) carbonate is an ionic solid (a salt) consisting of copper(II) cations Cu2+ and carbonate anions CO2−3.
Copper(II) carbonate is rarely encountered because it is difficult to prepare and readily reacts with water moisture from the air.

The terms "copper carbonate", "copper(II) carbonate", and "cupric carbonate" almost always refer (even in chemistry texts) to a basic copper carbonate (or copper(II) carbonate hydroxide), such as Cu2(OH)2CO3 (which occurs naturally as the mineral malachite) or Cu3(OH)2(CO3)2 (azurite).

For this reason, the qualifier neutral may be used instead of "basic" to refer specifically to CuCO3.
Copper(II) Carbonate is generally immediately available in most volumes, including bulk orders.
Copper(II) carbonate, commonly encountered in its basic form with the chemical formula Cu₂(OH)₂CO₃, is a blue-green to green inorganic solid that occurs naturally as the mineral malachite.

Copper(II) carbonate is characterized by its insolubility in water and solubility in dilute acids, such as acetic acid and hydrochloric acid, and it decomposes upon heating above 200 °C to yield copper(II) oxide (CuO), carbon dioxide (CO₂), and water (H₂O).
The pure anhydrous form, Copper(II) carbonate, is thermodynamically unstable under standard conditions and decomposes to copper(II) oxide and carbon dioxide, or forms basic copper carbonate in moist air, making the basic variant the predominant stable phase in practice.

Copper(II) carbonate has a monoclinic crystal structure and a density ranging from 3.7 to 4.0 g/cm³, appearing as a fine powder with low toxicity under normal handling but requiring precautions due to its irritant properties and environmental persistence.
Copper(II) carbonate is synthesized industrially by reacting copper(II) sulfate with sodium carbonate or through precipitation from copper salts in alkaline conditions, often as a byproduct in copper refining processes.

Copper(II) carbonate's vibrant green hue stems from d-d transitions in the copper(II) ion coordinated within a distorted octahedral environment involving carbonate and hydroxide ligands, rendering it a valued pigment in historical and modern applications.
Key uses of Copper(II) carbonate include as a colorant in ceramics, glass, and paints; in pyrotechnics for green flares; and as a precursor for other copper compounds in bronze plating and electroplating baths.

Cupric Carbonate is another name for Copper(II) carbonate.
Furthermore, Copper(II) carbonate is a chemical substance.
Copper(II) carbonate is also an ionic solid compound composed of copper (II) cations Cu2+ and carbonate anions CO2-3.

The term Copper(II) carbonate is most usually used to refer to a basic copper carbonate such as Cu2(OH)2CO3.
Copper(II) carbonate can be found in nature in the form of the mineral malachite or the azurite mineral Cu3(OH)2(CO3)2.
As a result, the qualifier neutral can be used in place of basic, which specifically refers to Copper(II) carbonate.

Copper(II) carbonate is a chemical compound with the formula CuCO3.
Copper(II) carbonate is a blue-green solid that is often found in nature as the mineral malachite.
Copper(II) carbonate is characterised by its distinctive colour and plays a crucial role in various applications.

Copper(II) carbonate consists of copper ions Cu2+ bonded to carbonate ions CO2−3 through ionic bonding.
Copper(II) carbonate finds application as a pigment in ceramics and paints, as a fungicide in agriculture, and as a catalyst in organic synthesis.

The unique properties of copper(II) carbonate make it a valuable compound in several industries.
Copper(II) carbonate is a blue-green powder; Insoluble in water.
Copper(II) carbonate is a green-blue chemical.

You might also hear Copper(II) carbonate called cupric carbonate.
Copper(II) carbonate is a chemical compound made of copper and carbonate parts.
Copper(II) carbonate's chemical formula is CuCO3.

Copper(II) carbonate is a solid that looks blue-green.
You often see Copper(II) carbonate as part of the green coating on old copper statues or roofs.
This green layer forms when copper is exposed to air for a long time.

The other part of this coating is copper(II) hydroxide.
Copper(II) carbonate can dissolve in acids.
When it does, Copper(II) carbonate creates carbon dioxide gas and a copper salt.

If you heat copper(II) carbonate, it breaks down.
Copper(II) carbonate turns into copper(II) oxide and also releases carbon dioxide gas.

Copper(II) carbonate is a grey colour ionic solid compound that contains copper (II) cations Cu2+, and carbonate CO32- anions.
Copper(II) carbonate is a non-flammable compound.

USES and APPLICATIONS of COPPER(II) CARBONATE:
Copper(II) carbonate has many uses due to its properties:
As a pigment: Copper(II) carbonate is used as a blue pigment in paints, inks, plastics and ceramics.
In agriculture: Copper(II) carbonate is used as a fungicide on crops and plants.

The copper ions have toxicity to fungi and inhibit their growth.
As a feed additive: Copper carbonate is added to feeds for livestock as a source of copper.
Copper is an essential element for enzymes, haemoglobin formation and immunity in animals.

Copper carbonate provides supplemental copper in the feeds.
As a mineral supplement: Copper(II) carbonate is used as a source of copper for mineral supplements in tablets and powders.
Other uses: Finely crushed Copper(II) carbonate finds applications as an abrasive in polishing and cleaning due to its hardness.

Copper(II) carbonate is combined with arsenic to generate acetoarsenite, often known as Paris green.
Copper(II) carbonate is used to preserve the wood.
Copper(II) carbonate is an active element in animal feeds and is in high demand in animal fodder.

Copper(II) carbonate is a popular method for converting the chemical into copper salts.
The combination is initially treated with a more vital acid during the procedure.
Water and carbon dioxide gas are then introduced in the next stage.

Vinegar (acetic acid) is combined with carbonate to produce water, cupric acid, and carbon dioxide.
Copper(II) carbonate is also utilized for a variety of esthetical functions.
Jewelry is one of the most prominent application areas of Copper(II) carbonate.

Due to the sheer unique color of each component, they are utilized as colorants and pigments.
In Copper(II) carbonate's purest form, the combination is mint green.
The inclusion of alkaline components results in a blue tint.

These hues are excellent coloring agents.
They are utilized as a pigment in a variety of applications, including paints and varnishes.
Copper(II) carbonate is used in artist paints to get the desired hues, and it is also known by other names such as verditer and mountain green.

Copper(II) carbonate is a popular pigment and colorant in fireworks and ceramic glazes.
Copper(II) carbonate is a byproduct of the production of Copper Chromite catalysts.
The hydrogenolysis of fatty methyl esters in the formation of fatty alcohol is the greatest (industrial scale) application of copper chromite catalysts.

Copper Chromite has a high hydrogenation activity for aldehydes and ketones to their corresponding alcohols, as well as nitro-compounds to primary amines.
To minimize reaction rate and regulate synthesis in the reactor, some applicators use Copper Oxide Black instead of Copper Carbonate.

Copper(II) carbonate dihydroxide is used as pigments and in treatment for copper deficiency in ruminants.
Copper(II) carbonate is also used in pyrotechnics, in sweetening of petrol sour crude stock and animal and poultry feeds.
Copper(II) carbonate finds application in some types of make-up such as lipstick.

In analytical chemistry, Copper(II) carbonate is used as a reagent for analysis.
Pigments & ceramics: Copper(II) carbonate is used as a green/blue pigment and glaze colorant in ceramics and glass (ceramic stains / glazes).
Laboratory reagent / chemical intermediate: source of Cu²⁺ after acid treatment; Copper(II) carbonate is used in preparative inorganic chemistry.

Algaecide / biocide (limited): Copper(II) carbonate is historically used in some algaecidal formulations; usage depends on formulation and regulations.
Metal finishing / metallurgy (limited): Copper(II) carbonate is used in some copper-containing processes or as a precursor to other copper compounds.

Educational & demonstration reagent: Copper(II) carbonate is used in teaching to demonstrate carbonate–acid reactions producing CO₂.
Copper(II) carbonate is used in pigments, pyrotechnics, insecticides, to make other copper salts, for coloring brass black, as an astringent in pomade preparations, as an antidote for phosphorus poisoning, smut preventive, fungicide for seed treatment, in animal and poultry feeds as readily absorbable source of copper, and as a veterinary medication (anthelmintic aid in sheep).

In agriculture, Copper(II) carbonate serves as an algaecide, fungicide, and micronutrient supplement in animal feeds to prevent copper deficiencies, while emerging research explores its role as an anode material in lithium-ion batteries due to its high discharge capacity.
Additionally, Copper(II) carbonate acts in catalytic systems for organic reactions, such as β-borylation of alkenes, highlighting its versatility in chemical synthesis.

Copper(II) carbonate is a versatile compound widely recognized for its applications in various industries, including ceramics, agriculture, and chemical manufacturing.
This inorganic salt, often encountered as a blue-green powder, Copper(II) carbonate serves as a key ingredient in the production of pigments and glazes, providing vibrant colors in ceramic and glass applications.

Additionally, Copper(II) carbonate is utilized as a precursor in the synthesis of other copper compounds, making it invaluable in the field of materials science.
In agriculture, Copper(II) carbonate acts as a fungicide and herbicide, contributing to crop protection and soil health.

Copper(II) carbonate's unique properties, such as thermal stability and solubility in acids, enhance its functionality in diverse formulations, offering significant advantages over similar compounds.

Researchers and industry professionals appreciate its effectiveness and reliability, making Copper(II) carbonate a preferred choice for applications requiring high-performance materials.

Copper(II) carbonate is used as seed treatment fungicide; in pyrotechnics; as paint and varnish pigment; in animal and poultry feeds; in sweetening of petrol sour crude stock; in manufacture of other Cu salts.

BENEFITS / NOTABLE CHARACTERISTICS of COPPER(II) CARBONATE:
Copper(II) carbonate provides a stable, relatively non-volatile source of Cu²⁺ in solid form.
Copper(II) carbonate produces characteristic green/blue color in glazes and pigments.
Low solubility gives slow release of copper ions in some formulations (useful or limiting depending on application).

WHAT IS COPPER(II) CARBONATE USED FOR?
Copper(II) carbonate has a few important uses:
Copper(II) carbonate can be used to kill algae, which are tiny plant-like organisms that can grow in water.
Copper(II) carbonate is also used as a pigment, which means it gives color to things like paints or dyes.

RELATED COMPOUNDS of COPPER(II) CARBONATE:
Other anions
*Copper(II) sulfate

Other cations
*Nickel(II) carbonate
*Zinc carbonate

HOW IS COPPER(II) CARBONATE MADE?
Copper(II) carbonate can form naturally when copper(II) hydroxide is left in the air.
People can also make Copper(II) carbonate in a lab.
One way is to mix copper sulfate with sodium carbonate.
This reaction creates copper(II) carbonate and also leaves sodium sulfate dissolved in the water.

STRUCTURAL FORMULA of COPPER(II) CARBONATE:
The structural representation of Copper(II) carbonate is as shown in the figure below.
The Copper(II) carbonate can react immediately with water and air and is a tedious process practically to prepare.

PREPARATION of COPPER(II) CARBONATE:
In ambient circumstances, solutions of Copper II Sulfate CuSO4 and sodium carbonate Na2CO3 are mixed.
This results in the formation of a basic carbonate and the release of CO2.

This is due to the Cu2+ ion's high reactivity for the hydroxide anion HO.
The basic carbonate is then thermally decomposed at air pressure to generate Copper II oxide CuO instead of the carbonate.

W. F. T. Pistorius claimed in 1960 that synthesis could be accomplished by heating basic copper carbonate at 180 °C for 36 hours in a carbon dioxide CO2 (450 atm) atmosphere and water (50 atm).
The obtained bulk was well-crystallized malachite Cu2CO3(OH)2.

However, a little amount of a rhombohedral material, which was claimed to be Copper(II) carbonate, was also recovered.
Because this synthesis was not particularly reliable, it was terminated.
The reliable synthesis of genuine Copper(II) carbonate was reported in 1973 by Hartmut Ehrhardt and coworkers.

The resulting chemical compound, Copper(II) carbonate, was grey in color and was formed when basic copper carbonate was heated in a carbon dioxide atmosphere produced by the breakdown of silver oxalate Ag2C2O4 at 500°C and 2 GPa (20,000 atm).
Copper(II) carbonate obtained was described as having a monoclinic structure.

FORMULA of COPPER(II) CARBONATE:
Copper(II) carbonate has the chemical formula CuCO3.
The "Cu" in the formula represents copper atoms.
Each copper atom has 29 electrons and an atomic number of 29.
The "2+" shows that each copper atom has lost two electrons, giving it a 2+ charge.
The "CO3" in the formula represents carbonate ions.
Each carbonate ion contains one carbon atom joined to three oxygen atoms to form a triangular-shaped ion.
The carbonate ion has a 2- charge.

STRUCTURE of COPPER(II) CARBONATE:
The CuCO3 formula of Copper(II) carbonate shows that each copper ion is bonded to three bidentate carbonate ions.
The bonding between Cu2+ and CO2−3 ions is ionic due to the electrostatic attraction between the positively charged copper ions and negatively charged carbonate ions.

Here are some additional details about the structure of Copper(II) carbonate:
The carbonate ion has a resonance structure, with the unshared pair of electrons on any of the three O atoms.
This delocalises the negative charge and adds to the stability of the CO2−3 ion.

The Cu2+ - CO2−3 interaction is dominated by ionic or electrostatic bonding due to the large difference in their electronegativities.
There is no significant covalent character.

copper-ii-carbonate-formula
In the monoclinic crystal structure, the Copper(II) carbonate layers are stacked along the c-axis.
The CO2−3 ions occupy the ab plane while Cu2+ ions occupy the spaces between them.

In the orthorhombic structure, the stacking of Copper(II) carbonate layers is less ordered.
The CO2−3 ions still form layers that Cu2+ ions fit in between.

PREPARATION of COPPER(II) CARBONATE:
Copper(II) carbonate can be prepared through various methods, and here are two common reactions used for its synthesis:

*Reaction of Copper(II) Sulfate with Sodium Carbonate:
In this reaction, copper (II) sulphate reacts with sodium carbonate to yield Copper(II) carbonate and sodium sulphate as a byproduct.
The reaction takes place in an aqueous solution.
CuSO4+Na2CO3→CuCO3+Na2SO4

*Precipitation Method using Sodium Bicarbonate:
Here, copper (II) chloride reacts with sodium bicarbonate to form Copper(II) carbonate, sodium chloride, water, and carbon dioxide.
This reaction is carried out in an aqueous medium.
CuCl2+2NaHCO3→CuCO3+2NaCl+H2O+CO2

CHEMICAL PROPERTIES of COPPER(II) CARBONATE:
Chemical Properties of Copper(II) carbonate are as follows:

*Decomposition:
Copper(II) carbonate is thermally unstable and readily decomposes upon heating, releasing carbon dioxide and leaving behind copper (II) oxide.
CuCO3(s)→CuO(s)+CO2(g)

*Acid-Base Reactions:
Copper(II) carbonate acts as a base and reacts with acids to form copper (II) salts and carbon dioxide.
CuCO3(s)+2HCl(aq)→CuCl2(aq)+H2O(l)+CO2(g)

*Reaction with Ammonia:
Copper(II) carbonate reacts with ammonia to form a complex, deep blue compound called copper (II) tetraamine carbonate.
CuCO3(s)+4NH3(aq)→Cu(NH3)4(s)

*Redox Reactions:
Copper(II) carbonate can undergo redox reactions, where it can be reduced to copper (I) compounds or oxidized to copper(II) compounds.
2CuCO3(s)+C→2CuO(s)+2CO2(g)

CHEMICAL FORMULA of COPPER(II) CARBONATE:
CuCO3 is the formula for Copper(II) carbonate.
When heated in the air, Copper(II) carbonate decomposes into copper oxide, water, and carbon dioxide.
Copper(II) carbonate is also acid-soluble and produces the corresponding copper salt.

To produce a copper complex, Copper(II) carbonate is also soluble in an aqueous solution of cyanide, ammonium salt, and an alkali metal carbonate.
When boiled in water or heated in an alkaline solution, Copper(II) carbonate produces brown oxide.

(II) carbonate is extremely unstable in a hydrogen sulfide atmosphere and can react with it to form copper sulfide.
Being in the air for an extended period of time causes it to emit CO2 by absorbing moisture.

Copper(II) carbonate then gradually transforms into a green malachite composition.
The stability of dry Copper(II) carbonate is highly dependent on the partial pressure of carbon dioxide (PCO2).
Copper(II) carbonate can be stable in dry air for months, but it decomposes slowly into CuO and CO2 if PCO2 is less than 0.11 atm.

At a temperature of 25°C in water or moist air, Copper(II) carbonate is only constant for PCO2 over 4.57 atmospheres and has a pH between 4 and 8.
Copper(II) carbonate is strongly reactive with water below the partial pressure and forms a basic carbonate - (azurite, Cu3(CO3)2(OH)2).
3CuCO3 + H2O → Cu3(CO3)2(OH)2 + CO2

PREPARATION of COPPER(II) CARBONATE:
Reactions that may be expected to yield Copper(II) carbonate, such as mixing solutions of copper(II) sulfate CuSO4 and sodium carbonate in ambient conditions, yield instead a basic carbonate and CO2, due to the great affinity of the Cu2+ ion for the hydroxide anion HO−.
Thermal decomposition of the basic carbonate at atmospheric pressure yields copper(II) oxide rather than the carbonate.

In 1960, C. W. F. T. Pistorius claimed synthesis by heating basic copper carbonate at 180 °C (356 °F) in an atmosphere of carbon dioxide at 450 atm (46 MPa) and water at 50 atm (5.1 MPa) for 36 hours.
The bulk of the products was well-crystallized malachite Cu2CO3(OH)2, but a small yield of a rhombohedral substance was also obtained, claimed to be Copper(II) carbonate.

However, this synthesis was apparently not reproduced.
Reliable synthesis of true copper(II) carbonate was reported for the first time in 1973 by Hartmut Ehrhardt et al.

Copper(II) carbonate was obtained as a gray powder, by heating basic copper carbonate in an atmosphere of carbon dioxide (produced by the decomposition of silver oxalate, Ag2C2O4) at 500 °C (932 °F) and 20,000 atm (2 GPa).
Copper(II) carbonate was determined to have a monoclinic structure.

CHEMICAL AND PHYSICAL PROPERTIES of COPPER(II) CARBONATE:
The stability of dry Copper(II) carbonate depends critically on the partial pressure of carbon dioxide (pCO2).
Copper(II) carbonate is stable for months in dry air, but decomposes slowly into CuO and CO2 if pCO2 is less than 0.11 atm (11 kPa).

In the presence of water or moist air at 25 °C (77 °F), Copper(II) carbonate is stable only for pCO2 above 4.57 atm (463 kPa) and pH between about 4 and 8.
Below that partial pressure, Copper(II) carbonate reacts with water to form a basic carbonate (azurite, Cu3(CO3)2(OH)2).

3 CuCO3 + H2O → Cu3(CO3)2(OH)2 + CO2
In highly basic solutions, the complex anion Cu(CO3)2−2 is formed instead.
The solubility product of the true copper(II) carbonate was measured by Reiterer and others as pKso = 11.45 ± 0.10 at 25 °C (77 °F).

STRUCTURE of COPPER(II) CARBONATE:
In the crystal structure of Copper(II) carbonate, copper adopts a distorted square pyramidal coordination environment with coordination number 5.
Each carbonate ion bonds to 5 copper centres.

Copper(II) carbonate is a chemical compound of copper.
Copper(II) carbonate is used as a pigment, in some types of make-up, as an algaecide, and for bronze plating.
Copper is a chemical element with the symbol Cu and atomic number 29.

Copper is an essential elements in plants and animals as it is required for the normal functioning of more than 30 enzymes.
Copper(II) carbonate occurs naturally throughout the environment in rocks, soil, water, and air.

PHYSICAL and CHEMICAL PROPERTIES of COPPER(II) CARBONATE:
Name: Copper(II) carbonate (also called cupric carbonate).
Common forms: “neutral” CuCO₃ (rare, poorly stable) and more commonly basic copper carbonate (often formulated as CuCO₃·Cu(OH)₂ or Cu₂(OH)₂CO₃, the green/blue mineral malachite/azurite family).
Molecular formula (neutral): CuCO₃. Basic copper carbonate formulas: CuCO₃·Cu(OH)₂ or Cu₂(OH)₂CO₃ or CH6Cu2O5 depending on notation.
Molar mass: ~123.55 g·mol⁻¹ (neutral CuCO₃).
EC number(s): common registry entries include 214-671-4 and the basic copper carbonate REACH entry 235-113-6 (for the CuCO₃·Cu(OH)₂ material).
CAS number(s): 1184-64-1 (CuCO₃) and 12069-69-1 (copper(II) carbonate–copper(II) hydroxide basic mixture)

Appearance: green to blue-green powder or crystalline material (basic carbonate often green — malachite-like).
Density: varies with form/crystallinity; reported data differ for neutral vs. basic forms (crystalline parameters available for synthetic and mineral forms).
Solubility: essentially insoluble in water; slight dissolution in acidic media (reacts with acids to give copper salts and CO₂).
Solubility product values reported for specific synthetic samples (very low Ksp ~10⁻¹¹.⁴⁵ for some preparations).
Melting / decomposition: decomposes on heating, giving copper(II) oxide (CuO) and CO₂;
neutral CuCO₃ is thermally unstable under normal conditions (basic carbonate typically more commonly encountered).

Color / appearance in commerce: powder ranges from pale blue to green (depending on hydration/basicity and particle size).
Oxidation state: copper in +2 oxidation state (Cu²⁺).
Acid/base behavior: reacts with acids to produce soluble copper(II) salts and carbon dioxide (CO₂) — e.g., with HCl → CuCl₂ + CO₂ + H₂O. With strong bases it can undergo complexation or conversion to hydroxide species.
Thermal behavior: on heating decomposes to CuO and CO₂; neutral CuCO₃ is not easily isolated at ambient pressure and is less common than basic carbonates.

Stability: the “neutral” CuCO₃ is metastable; the basic carbonate (CuCO₃·Cu(OH)₂) is the more stable, commonly encountered form.
Chemical formula: CuCO3
Molar mass: 123.5549 g/mol
Appearance: Green or blue powder
Solubility in water: insoluble
Solubility product (Ksp): 10−11.45 ± 0.10 at 25 °C (77 °F) for material synthesized at high pressure.
Structure
Space group: Pa-C2s

Lattice constant: a = 6.092 Å, b = 4.493 Å, c = 7.030 Å
α = 90°, β = 101,34°°, γ = 90°
Coordination geometry: 5
Molecular Weight: 123.55 g/mol
Hydrogen Bond Donor Count: 0
Hydrogen Bond Acceptor Count: 3
Rotatable Bond Count: 0
Exact Mass: 122.914341 Da
Monoisotopic Mass: 122.914341 Da

Topological Polar Surface Area: 63.2 Å²
Heavy Atom Count: 5
Formal Charge: 0
Complexity: 18.8
Isotope Atom Count: 0
Defined Atom Stereocenter Count: 0
Undefined Atom Stereocenter Count: 0
Defined Bond Stereocenter Count: 0
Undefined Bond Stereocenter Count: 0

Covalently-Bonded Unit Count: 2
Compound Is Canonicalized: Yes
Melting Point: 200.0°C
Color: Green
Physical Form: Fine Crystalline Powder
Linear Formula: CuCO3·Cu(OH)2
Fieser: 01,163
Merck Index: 15, 2621
Solubility Information: Solubility in water: insoluble.

Other solubilities: soluble in acids, ammonia, practically insoluble in alcohol
Formula Weight: 221.1
Percent Purity: 54 to 56% Cu
Grade: Pure
Packaging: Glass bottle
Density: 4
Chemical Name or Material: Copper(II) carbonate basic
CAS: 12069-69-1
Molecular Formula: CCuO3·CuO2H2
Molecular Weight (g/mol): 221.1

MDL Number: MFCD00010976
Synonym: Copper(II)hydroxide carbonate
Linear Formula: CuCO3 · Cu(OH)2
CAS Number: 12069-69-1
Molecular Weight: 221.12
EC Number: 235-113-6
MDL number: MFCD00010976
UNSPSC Code: 12352302

PubChem Substance ID: 329752028
NACRES: NA.55
Grade: reagent grade
Form: powder
Physical state: solid
Color: No data available
Odor: odourless
Melting point/freezing point

Melting point/ range: > 400 °C - OECD Test Guideline 102 - Decomposition
Initial boiling point and boiling range: Not applicable
Flammability (solid, gas): The product is not flammable. - Flammability (solids)
Upper/lower flammability or explosive limits: No data available
Flash point: does not flash
Autoignition temperature: No data available
Decomposition temperature: 200 °C
pH: 8 - 9 at 50 g/l at 20 °C (slurry)

Viscosity
Viscosity, kinematic: No data available
Viscosity, dynamic: No data available
Water solubility: 0,002 g/l at 20 °C - OECD Test Guideline 105 - slightly soluble
Partition coefficient: n-octanol/water: Not applicable for inorganic substances
Vapor pressure: No data available
Density: 3,9 - 4,0 g/cm3 at 25 °C
Relative density: No data available

Relative vapour density: No data available
Particle characteristics: No data available
Explosive properties: No data available
Oxidizing properties: none
Other safety information: No data available
CAS Number: 12069-69-1
Purity: 50-57% (as Cu, Assay by titration)

Grade: Pure
Molecular Formula: CuCO3
Molecular Weight: 123.55
MDL Number: MFCD00051038
PubChem ID: 25503
Melting Point: 200 °C
Density: 4.00
Appearance: Blue-green, light green or aqua powder

Conditions: Store at RT
IUPAC Name: dicopper carbonate dihydroxide
InChI Key: ZMMDPCMYTCRWFF-UHFFFAOYSA-J
Boiling Point: 333.6ºC at 760 mmHg
Melting Point: 200ºC
Flash Point: 169.8ºC
Density: 4

Appearance: Fine green powder
Exact Mass: 219.84900
Hazard Statements: Xn:Harmful
H-Bond Acceptor: 5
H-Bond Donor: 2
Safety Description: S26-S36
Stability: Stable at room temperature in closed containers under normal storage and handling conditions.

FIRST AID MEASURES of COPPER(II) CARBONATE:
-Description of first-aid measures
*General advice:
Show this material safety data sheet to the doctor in attendance.
*If inhaled:
After inhalation:
Fresh air.
*In case of skin contact:
Take off immediately all contaminated clothing.
Rinse skin with
water/ shower.
*In case of eye contact:
After eye contact:
Rinse out with plenty of water.
Call in ophthalmologist.
Remove contact lenses.
*If swallowed:
After swallowing:
Immediately make victim drink water (two glasses at most).
Consult a physician.
-Indication of any immediate medical attention and special treatment needed.
No data available

ACCIDENTAL RELEASE MEASURES of COPPER(II) CARBONATE:
-Environmental precautions:
Do not let product enter drains.
-Methods and materials for containment and cleaning up:
Cover drains.
Collect, bind, and pump off spills.
Observe possible material restrictions.
Take up dry.
Dispose of properly.
Clean up affected area.

FIRE FIGHTING MEASURES of COPPER(II) CARBONATE:
-Extinguishing media:
*Suitable extinguishing media:
Carbon dioxide (CO2)
Foam
Dry powder
*Unsuitable extinguishing media:
For this substance/mixture no limitations of extinguishing agents are given.
-Further information:
Prevent fire extinguishing water from contaminating surface water or the ground water system.

EXPOSURE CONTROLS/PERSONAL PROTECTION of COPPER(II) CARBONATE:
-Control parameters:
--Ingredients with workplace control parameters:
-Exposure controls:
--Personal protective equipment:
*Eye/face protection:
Use equipment for eye protection.
Safety glasses
*Body Protection:
protective clothing
*Respiratory protection:
Recommended Filter type: Filter A
-Control of environmental exposure:
Do not let product enter drains.

HANDLING and STORAGE of COPPER(II) CARBONATE:
-Conditions for safe storage, including any incompatibilities:
*Storage conditions:
Tightly closed.
Dry.

STABILITY and REACTIVITY of COPPER(II) CARBONATE:
-Chemical stability:
The product is chemically stable under standard ambient conditions (room temperature).
-Possibility of hazardous reactions:
No data available