Why is cupric hydroxide insoluble in water?

Copper(II) hydroxide (chemical formula Cu(OH)2) is the hydroxide of the metal copper. The typical color of copper hydroxide is blue. Some forms of copper(II) hydroxide are sold as "stabilized" copper hydroxide, quite likely a mixture of copper(II) carbonate and hydroxide. These are often greener in color.

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History

Copper(II) hydroxide has been known to man since copper smelting began around 5000 BCE although the alchemists were probably the first to manufacture it.[1] This was easily done by mixing solutions of lye and blue vitriol, both chemicals which were known in antiquity.

It was produced on an industrial scale during the 17th and 18th centuries for use in pigments such as blue verditer and Bremen green.[2] These pigments were used in ceramics and painting.[3]

Chemical Properties

Synthesis

Copper(II) hydroxide can be produced by adding a small amount of sodium hydroxide to a dilute solution of copper(II) sulfate (CuSO4 · 5H2O). The precipitate produced in this manner, however, often contains an appreciable amount of sodium hydroxide impurity and a purer product can be attained if ammonium chloride is added to the solution beforehand. Alternatively, copper hydroxide is readily made by electrolysis of water (containing a little electrolyte such as sodium bicarbonate). A copper anode is used, often made from scrap copper.

"Copper in moist air slowly acquires a dull green coating. The green material is a 1:1 mole mixture of Cu(OH)2 and CuCO3."[4]

2Cu(s) + H2O(g) + CO2(g) + O2(g) ---> Cu(OH)2(s) + CuCO3(s)

This is the patina that forms on bronze and other copper alloy statues such as the Statue of Liberty.

Reactions

Moist samples of copper(II) hydroxide slowly turn black due to the formation of copper(II) oxide.[5] When it is dry, however, copper(II) hydroxide does not decompose unless it is heated to 185°C.[6]

Copper(II) hydroxide reacts with a solution of ammonia to form a deep blue solution consisting of the [Cu(NH3)4]2+ complex ion, but the hydroxide is reformed when the solution is diluted with water. Copper(II) hydroxide in ammonia solution, known as Schweizer's reagent, possesses the interesting ability to dissolve cellulose. This property led to it being used in the production of rayon, a cellulosic fiber.

Since copper(II) hydroxide is mildly amphoteric, it dissolves slightly in concentrated alkali, forming [Cu(OH)4]2-.[7]

Use as an organic reagent

Copper(II) hydroxide has a rather specialized role in organic synthesis. Often, when it is utilized for this purpose, it is prepared in situ by mixing a soluble copper(II) salt and potassium hydroxide.

It is sometimes used in the synthesis of aryl amines. For example, copper(II) hydroxide catalyzes the reaction of ethylenediamine with 1-bromoanthraquinone or 1-amino-4-bromoanthraquinone to form 1-((2-aminoethyl)amino)anthraquinone or 1-amino-4-((2-aminoethyl)amino)anthraquinone, respectively.

Copper(II) hydroxide also converts acid hydrazides to carboxylic acids at room temperature. This is especially useful in synthesizing carboxylic acids with other fragile functional groups. The published yields are generally excellent as is the case with the production of benzoic acid and octanoic acid.

Natural occurrence

Copper(II) hydroxide is found in several different copper minerals, most notably azurite, malachite, antlerite, and brochantite. Azurite (2CuCO3 • Cu(OH)2 ) and malachite (CuCO3 • Cu(OH)2) are carbonates while antlerite (CuSO4 • 2Cu(OH)2) and brochantite (CuSO4 • 3Cu(OH)2) are sulfates. Copper(II) hydroxide is rarely found as an uncombined mineral because it slowly reacts with carbon dioxide from the atmosphere to form a basic copper(II) carbonate.

Uses

Copper(II) hydroxide has been used as an alternative to the Bordeaux mixture, a fungicide and nematacide.[8] Nowadays, it is disfavored because of environmental contamination problems. Copper(II) hydroxide is also occasionally used as ceramic colorant.

Precautions

Copper(II) hydroxide is a skin, eye and respiratory irritant. Always wear safety glasses when handling copper hydroxide. In case of contact with eyes, rinse immediately with plenty of water and seek medical advice.

Copper(II) hydroxide is the hydroxide of copper with the chemical formula of Cu(OH)2. It is a pale greenish blue or bluish green solid. Some forms of copper(II) hydroxide are sold as "stabilized" copper(II) hydroxide, although they likely consist of a mixture of copper(II) carbonate and hydroxide. Cupric hydroxide is a strong base, although its low solubility in water makes this hard to observe directly.

Occurrence[edit]

Copper(II) hydroxide has been known since copper smelting began around 5000 BC although the alchemists were probably the first to manufacture it by mixing solutions of lye (sodium or potassium hydroxide) and blue vitriol (copper(II) sulfate).[3] Sources of both compounds were available in antiquity.

It was produced on an industrial scale during the 17th and 18th centuries for use in pigments such as blue verditer and Bremen green.[4] These pigments were used in ceramics and painting.[5]

Mineral[edit]

The mineral of the formula Cu(OH)2 is called spertiniite. Copper(II) hydroxide is rarely found as an uncombined mineral because it slowly reacts with carbon dioxide from the atmosphere to form a basic copper(II) carbonate. Thus copper slowly acquires a dull green coating in moist air by the reaction:

The green material is in principle a 1:1 mole mixture of Cu(OH)2 and CuCO3.[6] This patina forms on bronze and other copper alloy statues such as the Statue of Liberty.

Production[edit]

Copper(II) hydroxide can be produced by adding sodium hydroxide to a solution of a soluble copper(II) salt, such as copper(II) sulfate (CuSO4·5H2O):[7]

The precipitate produced in this manner, however, often contains water and an appreciable amount of sodium-containing impurities. Furthermore, this form of copper hydroxide tends to convert to black copper(II) oxide:[8]

A purer product can be attained if ammonium chloride is added to the solution beforehand to generate ammonia in situ.[9] Alternatively it can be produced in a two-step procedure from copper(II) sulfate via "basic copper sulfate:"[8]

Alternatively, copper hydroxide is readily made by electrolysis of water (containing a little electrolyte such as sodium sulfate or magnesium sulfate) with a copper anode:

Structure[edit]

The structure of Cu(OH)2 has been determined by X-ray crystallography The copper center is square pyramidal. Four Cu-O distances in the plane range are 1.96 Å, and the axial Cu-O distance is 2.36 Å. The hydroxide ligands in the plane are either doubly bridging or triply bridging.[10]

Reactions[edit]

It is stable to about 100 °C.[7]

Copper(II) hydroxide reacts with a solution of ammonia to form a deep blue solution of tetramminecopper [Cu(NH3)4]2+ complex ion.

Copper(II) hydroxide catalyzes the oxidation of ammonia solutions in presence of dioxygen, giving rise to copper ammine nitrites, such as Cu(NO2)2(NH3)n.[11][12]

Copper(II) hydroxide is mildly amphoteric. It dissolves slightly in concentrated alkali, forming [Cu(OH)4]2−.[13][7]

Reagent for organic chemistry[edit]

Copper(II) hydroxide has a rather specialized role in organic synthesis. Often, when it is utilized for this purpose, it is prepared in situ by mixing a soluble copper(II) salt and potassium hydroxide.

It is sometimes used in the synthesis of aryl amines. For example, copper(II) hydroxide catalyzes the reaction of ethylenediamine with 1-bromoanthraquinone or 1-amino-4-bromoanthraquinone to form 1-((2-aminoethyl)amino)anthraquinone or 1-amino-4-((2-aminoethyl)amino)anthraquinone, respectively:[14]

Copper(II) hydroxide also converts acid hydrazides to carboxylic acids at room temperature. This conversion is useful in the synthesis of carboxylic acids in the presence of other fragile functional groups. The yields are generally excellent as is the case with the production of benzoic acid and octanoic acid:[14]

Copper(II) hydroxide in ammonia solution, known as Schweizer's reagent, possesses the interesting ability to dissolve cellulose. This property led to it being used in the production of rayon, a cellulose fiber.

It is also used widely in the aquarium industry for its ability to destroy external parasites in fish, including flukes, marine ich, Brooklynellosis, and marine velvet, without killing the fish. Although other water-soluble copper compounds can be effective in this role, they generally result in high fish mortality.

Copper(II) hydroxide has been used as an alternative to the Bordeaux mixture, a fungicide and nematicide.[15] Such products include Kocide 3000, produced by Kocide L.L.C. Copper(II) hydroxide is also occasionally used as ceramic colorant.

Copper(II) hydroxide has been combined with latex paint, making a product designed to control root growth in potted plants. Secondary and lateral roots thrive and expand, resulting in a dense and healthy root system. It was sold under the name Spin Out, which was first introduced by Griffin L.L.C. The rights are now owned by SePRO Corp.[16] It is now sold as Microkote either in a solution you apply yourself, or as treated pots.

Other copper(II) hydroxides[edit]

Chemical structure of azurite, one of many copper(II) hydroxides (color code: red = O, green = Cu, gray = C, white = H).[17]

Together with other components, copper(II) hydroxides are numerous. Several copper(II)-containing minerals contain hydroxide. Notable examples include azurite, malachite, antlerite, and brochantite. Azurite (2CuCO3·Cu(OH)2) and malachite (CuCO3·Cu(OH)2) are hydroxy-carbonates, whereas antlerite (CuSO4·2Cu(OH)2) and brochantite (CuSO4·3Cu(OH)2) are hydroxy-sulfates.

Why is copper hydroxide insoluble in water?

Is cupric hydroxide soluble in water?

Is copper hydroxide insoluble or soluble?

Is cupric hydroxide soluble?