COPPER CARBONATE

Cas No. : 1184-64-1

EC / List No.: 214-671-4

Copper carbonate basic is naturally found in azurite and malachite. On heating, it undergoes decomposition to form copper(II) oxide, carbon dioxide and water. Due to its high initial discharge capacity, copper carbonate (basic) is being considered as a promising candidate as anode materials for lithium-ion batteries. Copper  carbonate basic along with different ligands form an efficient catalytic system for ′on water′ β-borylation of Michael acceptors, alkenes and alkynes. Copper carbonate basic (Cupric carbonate basic, Copper basic carbonate) may be used in the preparation of colloidal copper.

 

Copper carbonate is light blue powder with density of 3.85,and a melting point of 200ºC Copper carbonate in soluble in cold water and alcohol, but soluble in acid to form that correspond copper salt, and soluble in cyanide, sodium hydroxide, ammonium salt and aqueous solution of alkali carbonates to form a copper complex.  the mainly used for pigment,insecticide electroplating and so on. When a copper atom loses one or two of its electrons Copper carbonate forms positively charged ions known as Cu+1 and Cu+2. Whilst ordinary copper carbonate contains cupric ion (or Cu+2), it may sometimes contain a chemically similar alkaline component. This substance can actually serve a number of applications around industry and life in general; you probably haven’t realized how many purposes it is utilized in today

 

Aesthetic and Practical:  This substance has a number of aesthetic purposes, most notably in jewellery. Copper carbonate can also be converted into the metal version of copper, which is highly valuable and serves a number of its own applications. This is achieved through a process of pulverization, sizing, conversion and electrolysis.

 

Copper Salts: The substance can be converted into copper salts by mixing Copper carbonate with a stronger acid. The resulting salt is complemented with water and carbon dioxide gas. Mixing the carbonate with acetic acid (otherwise known as vinegar) will produce cupric acid, water and carbon dioxide.

 

Pigments and Colorants: This substance, when pure, should have a mint green colour. When alkaline components have been added, a tinge of blue will be added to the colour. This is often added to paints, varnishes, pottery glazes and even fireworks to impart some of the colour.

 

Miscellaneous: Small amounts of copper carbonates are used in a variety of animal feeds and fertilizers.Copper carbonate also plays a major role in the creation of pesticides and fungicides. Copper carbonate can also be used to control the growth and spread of aquatic weeds. Copper carbonate also a common ingredient in the ammonia compounds that are used to treat timber.

 

The preparation of porous metal–organic frameworks (MOFs) at industrial scales requires careful selection of the metal precursor to ensure the sustainability of the synthetic process, in terms of both the environmental impact and cost. The use of earth abundant minerals is attractive for this purpose, provided that they are sufficiently reactive under the conditions of MOF formation.  In this work, we investigate the use of copper carbonate and its naturally occurring counterparts, malachite and azurite, as precursors for the synthesis of Cu3(BTC)2 (HKUST-1; BTC3– = 1,3,5-benzenetricarboxylate).

 

 Using a water/ethanol solution of copper carbonate and H3BTC, HKUST-1 was obtained at room temperature within 3 h, as confirmed by a suite of characterization techniques. The identity of the products was determined by the reaction conditions, highlighting the importance of optimizing the synthetic parameters.  When prepared under optimized conditions, HKUST-1 synthesized here showed analogous performance characteristics to materials obtained by traditional solvothermal methods; thus, our results confirm that high-quality samples of MOFs can be easily derived from mineral precursors.

 

Copper Carbonate (CuCO3) is formed after copper loses its electrons. The copper carbonate typically contains Cu + 2, known as the cupric ion. However, at times it may have an alkaline component as the content. Copper carbonate is a water-insoluble chemical compound. Copper carbonate can be converted into other copper compounds by different methods such as calcination, where on the application of heat, the chemical compound gives oxide. Copper carbonate is used in several applications.

 

Metals and salt conversions:

Copper carbonate is very commonly used to convert the compound into copper salts. In the process, the mixture is first treated with a more vital acid. In the next step, water along with the carbon dioxide gas is added. Vinegar, known as acetic acid, is mixed with carbonate to produce water, cupric acid, and carbon dioxide. It is also used for various aesthetics and practical purposes. One of the prominent application areas is jewelry. The metal conversion of copper carbonate is highly sought after in the industry. Copper carbonatet is precious and has numerous applications. Several processes are used to obtain the desired result, such as pulverization, conversion, sizing, and electrolysis.

 

Coloring pigment:

Owing to the specific color of different compounds, they are used as colorants and pigments. In pure form, the combination is of mint green color. A tinge of blue is obtained after the addition of alkaline components. These colors act as great coloring agents. They are used as a pigment in products, paints, and varnishes. Copper carbonate is used in artist paints to obtain desired colors for which it is also known with different names such as verditer and mountain green. Copper carbonate is highly demanded in fireworks and pottery glazes as pigment and colorant.

 

Agriculture and aquaculture:

Copper carbonate is used across a wide range of applications. Copper carbonate commonly used to develop compounds for the treatment of timber. Copper carbonate is added to arsenic to produce acetoarsenite, which is popularly known as Paris green. Copper carbonate  is used as a wood preservative. Copper carbonate is actively used as an ingredient in animal feeds and is demanded continuously in animal fodder. Fertilizer is the other product where the demand for copper carbonate is very high. Copper carbonate used to create different pesticides, insecticides, and fungicides. Acetoarsenite is used as an insecticide. Besides agriculture, aquaculture is also one of the major application areas. Copper carbonate used in controlling the unnecessary spreading of weeds.

 

Copper Chromite Catalysts Manufacturing:

Copper Carbonate is used in manufacturing Copper Chromite catalysts. The largest field (industrial scale) of applying copper chromite catalysts is the hydrogenolysis of fatty methyl esters in fatty alcohol production. Copper Chromite is very active for the hydrogenation of aldehydes and ketones to their corresponding alcohols, as well as nitro-compounds to the primary amines. Some applicators use Copper Oxide Black instead of Copper Carbonate to reduce reaction rate and control synthesis in the reactor.

 

Boiling Point             333.6ºC at 760mmHg

Melting Point             200ºC

Molecular Formula CCuO3

Molecular Weight       123.555

Flash Point           169.8ºC

Exact Mass           122.914345

PSA                       63.19000

Vapour Pressure 2.58E-05mmHg at 25°C

Stability             Stable. Incompatible with strong acids.

Water Solubility insoluble H2O

Laboratory Grade - Intermediate purity. Suitable for educational laboratories. Use for qualitative analysis, not quantitative analysis.

Reagent Grade - High purity. Often equal to purity standards set by the American Chemical Society (ACS). Use for quantitative analysis

 

Copper Carbonate is a water-insoluble Copper source that can easily be converted to other Copper compounds, such as oxide by heating (calcination). Carbonate compounds also give off carbon dioxide when treated with dilute acids. Copper Carbonate is generally immediately available in most volumes. High purity, submicron and nanopowder forms may be considered.

Both malachite and azurite can be found in the verdigris patina that is found on weathered brass, bronze, and copper. The composition of the patina can vary, in a maritime environment depending on the environment a basic chloride may be present, in an urban environment basic sulfates may be present. This compound is often improperly called (even in chemistry articles) copper carbonate, cupric carbonate, and similar names. 

The true (neutral) copper  carbonate CuCO3 is not known to occur naturally. Copper carbonate decomposed by water or moisture from the air and was synthesized only in 1973 by high temperature and very high pressures.

All pigments for ceramics are intermixable so why not get creative and experiment by missing your own completely fresh color. During the firing process, the colors fuse extra vigorously creating purity, intensity, and brilliance. The colors are stronger, therefore, significantly less percentage is needed to create vivid colors making them excessively cost-effective.

 

How to use Iron Oxide in the pottery: 

Both malachite and azurite, as well as basic copper carbonate have been used as pigments. One example of the use of both azurite and its artificial form blue verditer is the portrait of the family of Balthasar Gerbier by Peter Paul Rubens. The green skirt of Deborah Kip is painted in azurite, smalt, blue verditer (an artificial form of azurite), yellow ochre, lead-tin-yellow and yellow lake. The green color is achieved by mixing blue and yellow pigments. It has also been used in some types of make-up, like lipstick, although it can also be toxic to humans. It also has been used for many years as an effective algaecide in farm ponds and in aquaculture operations.

 

When using ceramic pigments in glazes, usually in concentrations of 1–10%, a little more care must be taken because some pigment systems react with materials in a glaze. Copper Carbonate (CuCo3) - May yield green & turquoise in oxidation or red in reduction with a slight fluxing reaction.  Copper glazes may tend to volitize at higher temperatures & affect the color of the pieces around them.  Carbonate form is more toxic than the oxide.  Conceptually, copper carbonate is CuCO3, however this form is not normally available in the market (copper carbonate basic is the article of commerce) so the powder should be viewed as a family of compounds.

 

As with other metallic colouring carbonates, copper carbonate is green in colour and bulkier than the oxide form, thus it tends to disperse better to give more even results. Copper carbonate also more reactive chemically and thus melts better. As such, it is ideal for use in brush work where minimal speck is required. However it produces gases as it decomposes and these can cause pinholes or blisters in glazes. Also the carbonate form contains less copper per gram, therefore colours are less intense than the oxide form.

 

The hydroxyl component is an important aid in dispersing the powder throughout the glaze slurry and thus avoid specks in the fired glaze.The raw powder begins to melt between 1950 and 2000F. At around 1500F it gases and will discolour nearby items in the kiln A compound, CuCO3, that was used as a sulfide scavenger for water-base muds. However, Copper carbonate was found to be corrosive due to spontaneous plating of metallic copper onto metal surfaces, causing pitting corrosion; it has largely been replaced by zinc compounds.

 

Cupric carbonate is also called Copper carbonate with chemical formula CuCO3. With the CAS registry number 1184-64-1, Copper carbonate a blue-green compound. The substance has the EINECS registry number 214-671-4. Copper carbonate stable that incompatible with strong acids. In addition,Copper carbonate insoluble in water, found effective in melting ice, soluble in ethanoic acid. Cupric carbonate is non-hazardous for air, sea and road freight.

 

Properties: Copper can slowly acquire a dull green coating in moist air. The green material is a 1:1 mole mixture of Cu(OH)2 and CuCO3. Basic copper carbonate occurs naturally as malachite (Cu2(OH)2CO3) and azurite (Cu3(OH)2(CO3)2). Cupric carbonate reacts with acids and gives carbon dioxide and corresponding copper(II) salts of that acid. Otherwise. Cupric carbonate will decompose at 290°C and form copper oxide. The response equations are as the following:

 

CuCO3 + 2 HCl → CuCl2 + H2O + CO2 (g)

CuCO3 + H2SO4 → CuSO4 + H2O + CO2 (g)

CuCO3 → CuO + CO2(g)

 

Preparation: Pure Cupric carbonate is obtained from basic copper carbonate in the presence of carbon dioxide at 180 °C and 4.6 MPa (46 atm) pressure. Cupric carbonate is prepared by combining aqueous solutions of copper sulfate and sodium carbonate. Finally, Basic cupric carbonate will precipitate from the solution:

 

2 CuSO4 + 2 Na2CO3 + H2O → Cu2(OH)2CO3 + 2 Na2SO4 + CO2

 

Uses: Cupric carbonate was formerly much used as a pigment, and is still in use for artist's colours. Copper carbonate has also been used in some types of make-up, like lipstick, although Copper carbonate can also be toxic to humans.Copper carbonate also has been used for many years as an effective algaecide in farm ponds and in aquaculture operations. Copper carbonate can be used to copper plate a metallic surface by adding sulfuric acid and heat it then passing a charge through it with the metal in the liquid. This process is known as electroplating. Cupric carbonate can also be used to manufacture signal flare, fireworks, paint, other copper salt and so on.

 

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).

 

Copper  Carbonate is also referred to as Cupric Carbonate. Further, it is essentially a chemical compound.  The Copper Carbonate Formula is CuCO 3. Further, it is an ionic solid compound which consists of copper (II) cations Cu2+ and carbonate anions CO2− 3. It is not that easy to be found because it is quite difficult to prepare. 

 

Most commonly, the term of copper carbonate or cupric carbonate is referred to as a basic copper carbonate like Cu2(OH)2CO3. This occurs in nature in the form of the mineral malachite or Cu3(OH)2(CO3)2 which is azurite. It is because of this reason that the qualifier neutral can be utilized in place of basic which refers particularly to CuCO3.

 

Copper carbonate generally expected of reactions like mixing solutions of Copper  sulfate CuSO 4 and sodium carbonate Na 2CO 3 in ambient conditions to produce CuCO 3, but instead, it produces a basic carbonate and CO2 because of the great attraction of the Cu2+ ion for the hydroxide anion HO−   When the basic carbonate thermally decomposes at atmospheric pressure, it produces Copper oxide CuO instead of the carbonate.

 

W. F. T. Pistorius in the year, 1960, claimed synthesis. He did so when he heated basic copper carbonate at 180 °C in an atmosphere containing carbon dioxide, CO 2(450 atm) and water (50 atm) up to 36 hours. The majority of these products came out to be well-crystallized malachite Cu 2CO 3(OH)2, however, there was also a small quantity of the rhombohedral substance in the result which was claimed as CuCO 3. But, it is important to note that this synthesis was actually not reproduced. If we look at the origin, we will see that the reliable synthesis of true Copper  carbonate was testified for the first time in 1973 by Hartmut Ehrhardt and others. Thus, this compound was acquired in the form of gray powder.

 

Copper carbonate was after they heated basic copper carbonate in an atmosphere containing carbon dioxide (which we produce by decomposing silver oxalate Ag 2C2O 4) at 500 °C and 2 GPa (20,000 atm). The compound was said to have a monoclinic structure. The stability of dry CuCO3 is dependent significantly on the partial pressure of carbon dioxide (pCO2). It can remain stable for months in dry air but will decompose slowly into CuO and CO2 if pCO2 is less than 0.11 atm.

 

In the company of water or moist air at 25 °C, CuCO3 is constant only for pCO2 above 4.57 atmospheres and pH between about 4 and 8. Further, below that partial pressure, it reacts with water to make a very 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)22− is formed as an alternative. Copper Carbonate is a water insoluble Copper source that can easily be converted to other Copper compounds, such as the oxide by heating (calcination). Carbonate compounds also give off carbon dioxide when treated with dilute acids. 

 

Copper Carbonate is generally immediately available in most volumes. High purity, submicron and nanopowder forms may be considered. American Elements produces to many standard grades when applicable, including Mil Spec (military grade); ACS, Reagent and Technical Grade; Food, Agricultural and Pharmaceutical Grade; Optical Grade, USP and EP/BP (European Pharmacopoeia/British Pharmacopoeia) and follows applicable ASTM testing standards. Typical and custom packaging is available.

 

 Additional technical, research and safety (MSDS) information is available as is a Reference Calculator for converting relevant units of measurement. Technical guidance for using Copper Carbonate in agriculture is also available. Copper (atomic symbol: Cu, atomic number: 29) is a Block D, Group 11, Period 4 element with an atomic weight of 63.546. The number of electrons in each of copper's shells is 2, 8, 18, 1 and its electron configuration is [Ar] 3d10 4s1. The copper atom has a radius of 128 pm and a Van der Waals radius of 186 pm. Copper was first discovered by Early Man prior to 9000 BC.

 

In its elemental form, copper has a red-orange metallic luster appearance.Of all pure metals, only silver has a higher electrical conductivity.The origin of the word copper comes from the Latin word 'cuprium' which translates as "metal of Cyprus." Cyprus, a Mediterranean island, was known as an ancient source of mined copper. 

 

When green copper carbonate{CuCO3} is heated it decomposes forming copper oxide {CuO} and carbon dioxide {CO2}. This is a decomposition reaction. Brisk effervescence of CO2 gas is released while heating. Decomposition reactions occur when heat is applied to a pure substance and the particles rearrange into two or more new products.

 

Applications

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

 

Cobalt carbonate is a fine grained material that gives more even distribution of colour than cobalt oxide. Produces an evenly textured blue glaze (1-3%) which is less intense than the oxide. Cobalt almost always produces blues, which may vary somewhat with glaze composition, high zinc glazes tending to give greenish blues (especially if titanium is present) and high magnesium glazes tending to produce lilac or pink hues. Cobalt is quite soluble in glazes, consequently it has little or no opacifying effect in the amounts normally used (rarely more than 1-2%). 

 

Cobalt is an active flux and it may be necessary to take this into account when using it in some glazes, as it may increase their fusibility quite considerably. Like other raw oxides (or carbonates) of copper, manganese and nickel, cobalt may cause blisters or bubbles in some glazes due to changing oxidation state during the firing cycle.

 

Basic copper carbonate is a chemical compound, more properly called copper(II) carbonate hydroxide. Copper carbonate an ionic compound (a salt) consisting of the ions copper(II) Cu2+, carbonate CO2−3, and hydroxide OH− The name most commonly refers to the compound with formula Cu2CO3(OH)2. Copper carbonate a green crystalline solid that occurs in nature as the mineral malachite. Copper carbonate has been used since antiquity as a pigment, and it is still used as such in artist paints, sometimes called verditer, green bice, or mountain green.

 

Sometimes the name is used for Cu3(CO3)2(OH)2, a blue crystalline solid also known as the mineral azurite. Copper carbonate too has been used as pigment, sometimes under the name mountain blue or blue verditer. Both malachite and azurite can be found in the verdigris patina that is found on weathered brass, bronze, and copper. The composition of the patina can vary, in a maritime environment depending on the environment a basic chloride may be present, in an urban environment basic sulfates may be present.

 

This compound is often improperly called (even in chemistry articles) copper carbonate, cupric carbonate, and similar names. The true (neutral) Copper carbonate CuCO3 is not known to occur naturally. Copper carbonate decomposed by water or moisture from the air, and was synthesized only in 1973 by high temperature and very high pressures. Basic copper carbonate is prepared by combining aqueous solutions of copper(II) sulfate and sodium carbonate at ambient temperature and pressure. Basic copper carbonate precipitates from the solution, with release of carbon dioxide CO2:

 

2 CuSO4 + 2 Na2CO3 + H2O → Cu2(OH)2CO3 + 2 Na2SO4 + CO2

 

Basic copper carbonate can also be prepared by reacting aqueous solutions of copper(II) sulfate and sodium bicarbonate at ambient conditions. Basic copper carbonate precipitates from the solution, again with release of carbon dioxide:

 

2 CuSO4 + 4 NaHCO3 → Cu2(OH)2CO3 + 2 Na2SO4 + 3 CO2 + H2O

 

Reactions

Basic cop­per car­bon­ate is de­com­posed by acids, such as so­lu­tions of hy­drochlo­ric acid HCl, into the cop­per(II) salt and car­bon diox­ide. In 1794 the French chemist Joseph Louis Proust (1754–1826) ther­mally de­com­posed cop­per car­bon­ate to CO2 and CuO, cupric oxide. The basic cop­per car­bon­ates, mala­chite and azu­rite, both de­com­pose form­ing CO2 and CuO, cupric oxide.

 

Uses

 

Both mala­chite and azu­rite, as well as basic cop­per car­bon­ate have been used as pig­ments. One ex­am­ple of the use of both azu­rite and its ar­ti­fi­cial form blue verditer is the por­trait of the fam­ily of Balthasar Ger­bier by Peter Paul Rubens. The green skirt of Deb­o­rah Kip is painted in azu­rite, smalt, blue verditer (ar­ti­fi­cial form of azu­rite), yel­low ochre, lead-tin-yel­low and yel­low lake. The green color is achieved by mix­ing blue and yel­low pigments.

 

Copper carbonate has also been used in some types of make-up, like lip­stick, al­though it can also be toxic to hu­mans. It also has been used for many years as an ef­fec­tive al­gae­cide in farm ponds and in aqua­cul­ture op­er­a­tions.

 

All copper feed grade sources must comply with stringent regulation on undesirable substances. Heavy metals and dioxins are the most critical risks for the feed and food chain. The higher the copper concentration, the lower is the contribution to contamination in the  feed. Figure 2 illustrates this advantage with the example of lead.

 

There are many advantages in favour of non-water soluble compounds, under the condition that they are enough solubilized in the proximal part of the digestive tract for intestinal uptake. Copper sulphate is well known for its hygroscopicity. Metal sulphates are water soluble compounds and as such they can create negative interactions in the premix and

in the gut. Already in the early 2000’s, it had been shown that metal oxides were less aggressive on vitamin stability when mixed in vitamin/mineral premixes. Since, vitamin manufacturers have improved their stability so that they are less sensitive to negative effects from other

 

Copper is an essential trace element, a constituent of many proteins and of more than 20 enzymes. The daily intake is between 1 and 4 mg, mainly via food but in smaller amounts also via inhalation and skin contact. The toxicity of copper at the molecular level can be explained by its direct effects on the structure and function of proteins, membranes, and DNA as well as by the reactivity of the oxygen radicals formed in the copper redox cycle. During polishing work on copper plates, copper concentrations given as 0.12 mg/m3 which are, however, probably two to three times higher, produced symptoms similar to those of a common cold. In general, single oral doses of copper salts by humans primarily causes reversible gastrointestinal complaints accompanied by nausea and vomiting. The no observed adverse effect level (NOAEL) for nausea and vomiting is a copper concentration of 2 to 4 mg/l water. 

 

As a transition metal, copper is able to accept or donate one electron and thereby initiate redox reactions resulting in the formation of oxygen radicals. Copper ions are thus important catalytic co-factors for enzymatic redox reactions. Examples of copper binding enzymes are copper-zinc superoxide dismutase, cytochrome c oxidase, dopamine β-hydroxylase and ceruloplasmin (ferroxidase). 

 

Copper is an integral part of many proteins and more than 20 enzymes with important functions in cellular respiration, cellular energy metabolism, connective tissue biosynthesis, and iron metabolism. It also plays an important role in the regulation of gene transcription Ionic copper binds with a high affinity to histidine or sulfur in cysteine and methionine. Copper carbonate can lead to inactivation of proteins and enzymes. Free, unbound copper ions are present in biological matrices in the extremely small concentration of one ion per cell . Reactive Copper carbonate can oxidize thiol groups located in the membranes to form disulfides, thereby being able to disturb structural or functional properties of membranes .

 

The Copper carbonate thus formed can be oxidized again to form Copper carbonate via endogenous oxygen or via hydrogen peroxide from the respiratory chain. In this redox cycle, reactive oxygen radicals can be produced through Fenton-like reactions. Therefore,Copper carbonate assumed that reactive copper can lead to oxidative cell damage, such as lipid peroxidation, thiol oxidation, and DNA damage .

 

The mechanisms leading to the symptoms of acute and chronic toxicity of copper, which are relatively well documented for humans as well, and the concentrations capable of inducing symptoms in each specific case are hardly known. The gastrointestinal complaints occurring after acute intoxication seem to be a direct sequel of gastric irritation by the copper ions, and are probably triggered on a neuronal basis. Individual differences in sensitivity, the volume of the compounds containing copper, Copper carbonate degree of oxidation and the amount contained in the stomach play an important role .

 

Absorption of copper occurs through the gastrointestinal tract. With increasing supply absorption is reduced, and excessive amounts of copper are excreted again. The liver is the central organ for copper metabolism. It regulates the copper concentration via excretion with the bile and the faeces. Only very small amounts of copper can be detected in the urine. One half of the copper concentration in blood is found in plasma, the other half in erythrocytes. In the organs, most of the copper is contained in the liver, followed by the spleen, kidneys, and lungs

To maintain copper homeostasis, a fine balance between intake, distribution andstorage of the metal, as well as its excretion is necessary . Specific transport proteins in the mucosal cells of the small intestine control the amount of copper absorbed from the food into the blood. From the copper contained in the diet, about 15 % to 60 % are absorbed. Absorption can be influenced by other metals or complex formation in the diet, and decreases as copper levels rise. In humans, absorption was 56 % after an intake of 0.8 mg/day with the diet and 12 % after 8 mg/day (WHO 1998). The required copper intake for an adult is about 1 to 3 mg/day. 

 

Copper reaches the livermainly bound to transcuprein (Weiss and Linder 1985), histidine and high affinitybinding sites of albumin (Masuoka et al. 1993). Copper uptake by liver cells is not an entirely clear process, although one specific copper transport protein, hCTR1 (humanchymotrypsin-like protease) nevertheless does seem to play an important role (Peña etal. 1999). Since only copper(I) ions can be transported by hCTR1, copper(II) must be reduced by a reductase before being absorbed into a cell.

 

IUPAC  name. : copper(2+) carbonate, C&L Inventory, Copper(II), carbonaten copper(II) , hydroxide

Synonyms. : Carbonic acid, copper(2+) salt (1:1); Copper carbonate (CuCo3); Copper (II) carbonate; copper(2+) carbonate