Copper (II) hydroxide Cu(OH)₂ – product information, price, where to buy | Manufacturer and distributor

Copper (II) hydroxide Cu(OH)₂ – high purity, CoA/SDS documentation, technical support. Copper(II) hydroxide is an inorganic chemical compound with the formula Cu(OH)₂, available in our product line in high purity, designed for research laboratories, universities, the chemical and ceramics industries, and manufacturing companies. As an experienced distributor of chemical raw materials, we offer copper hydroxide in analytical grade (p.a.) and pro analysi (p.a.) purity, with complete technical documentation included with every shipment.

We include a Certificate of Analysis (CoA), a Safety Data Sheet (SDS), and technical specifications with every order. We guarantee consistent quality across batches, competitive wholesale prices, and technical support at every stage of our partnership.

Basic Specifications – Copper Hydroxide Cu(OH)₂

Copper hydroxide – price and pricing factors

The price of copper(II) hydroxide depends on several key factors:

• Chemical purity: p.a. (pro analysis) products are more expensive than c.d.a. due to higher quality requirements and additional analytical testing.
• Order size: The price per kilogram decreases with larger quantities; volume discounts are available starting at 5 kg.
• Product form: dry powder vs. ready-to-use suspension; different forms may be more cost-effective for specific applications.
• Packaging: standard packaging vs. specialized containers for moisture-sensitive products.
• Documentation: Additional certifications (e.g., GMP) may affect the final product price.

Retail orders (250 g – 1 kg): price available upon request.

Wholesale orders (5 kg and up): customized pricing with volume discounts.

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Copper hydroxide—where to buy? Ask for a quote!

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We offer the option to order a sample of copper(II) hydroxide before placing a larger order. For B2B customers, we prepare customized quotes that take into account:

• Order volume and frequency
• Documentation and certification requirements
• Special technical requirements (purity, packaging)

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What is copper (II) hydroxide?

Copper(II) hydroxide is an inorganic chemical compound belonging to the group of transition metal hydroxides, in which the copper ion Cu²⁺ is bonded to two hydroxyl groups OH⁻. Under normal conditions, this substance occurs as a blue, gelatinous precipitate or a fine-grained powder with a characteristic color—typical of divalent copper compounds. The compound is practically insoluble in water, which causes it to precipitate as a sediment when it comes into contact with aqueous solutions.

Copper hydroxide is one of the most important chemical reagents used in both analytical laboratories and industry. Its properties—reactivity with acids and bases and its ability to form complexes—make it a compound with a wide range of applications, from analytical chemistry to ceramics and plant protection.

Chemical Formula and Structure of Cu(OH)₂

The molecular formula of copper(II) hydroxide is Cu(OH)₂, where Cu represents copper in the +2 oxidation state, and OH represents two hydroxyl groups. The molar mass of the compound is 97.56 g/mol. The compound is registered under CAS number 20427-59-2 and EC number 243-815-9. In IUPAC nomenclature, the full name is dihydroxocopper(II) or copper(2+) hydroxide.

In the crystal structure, Cu²⁺ ions are surrounded by OH⁻ groups, forming a characteristic lattice. The compound is thermally unstable—decomposition into copper oxide (CuO) and water begins as early as 80–100°C, and complete decomposition occurs at higher temperatures. It is precisely this reaction: Cu(OH)₂ → CuO + H₂O that is of practical importance in ceramics and glazing. Copper hydroxide also tends to form complexes with ammonia—the product of this reaction, the tetraamminediaqua copper(II) [Cu(NH₃)₄(H₂O)₂]²⁺, has an intense blue color and is known as Schweitzer’s liquid.

Basicity and Reactivity of Cu(OH)₂

Copper(II) hydroxide is classified in the chemical literature primarily as a weak inorganic base. It reacts with acids to form copper salts and water—this is its dominant and defining characteristic. For example, a reaction with sulfuric acid leads to the formation of copper(II) sulfate: Cu(OH)₂ + H₂SO₄ → CuSO₄ + 2H₂O.

In a concentrated NaOH solution and at elevated temperatures, Cu(OH)₂ may exhibit weak acidic behavior, forming tetrahydroxocopper anions [Cu(OH)₄]²⁻. However, this reaction proceeds much more slowly than in the case of classic amphoteric hydroxides, such as Al(OH)₃ or Zn(OH)₂, and is not considered a dominant property of the compound. For this reason, describing Cu(OH)₂ as an amphoteric compound—although found in some sources—should be treated with caution: its acidic character is very weak here and is significant mainly under laboratory conditions, not industrial ones.

How to Obtain Copper Hydroxide? Synthesis Methods

Copper(II) hydroxide can be prepared using several laboratory and industrial methods. The most commonly used are precipitation reactions involving a base and the reaction of copper salts with a suitable alkaline reagent. Each method yields a product with slightly different properties—varying degrees of crystallinity, particle size, and reactivity.

Precipitation reaction—sodium or potassium hydroxide

The simplest and most commonly used laboratory method for obtaining copper(II) hydroxide (II) is the reaction of a copper salt solution (e.g., copper sulfate, CuSO₄) with a solution of sodium hydroxide (NaOH) or potassium hydroxide (KOH). The reaction proceeds as follows:

CuSO₄ + 2 NaOH → Cu(OH)₂↓ + Na₂SO₄

The reaction produces a characteristic blue, gel-like precipitate of Cu(OH)₂. The product precipitates immediately after the solutions are mixed. The precipitate must be filtered off, washed with distilled water to remove sulfate and sodium ions, and then dried at a low temperature (well below 80°C) to prevent thermal decomposition into CuO. This method is used in both analytical laboratories and industrial processes.

Reaction of copper nitrate or copper sulfate with a base

Copper(II) hydroxide can also be obtained from other copper salts—copper nitrate Cu(NO₃)₂ or copper chloride CuCl₂—by treating them with a dilute base. The reaction of copper nitrate with sodium hydroxide proceeds as follows:

Cu(NO₃)₂ + 2 NaOH → Cu(OH)₂↓ + 2 NaNO₃

The method using copper sulfate is most commonly used due to the availability and low cost of the substrate. Using copper nitrate yields a product with a slightly different precipitate morphology, which may be important for further processing. Important process parameters include the concentration of the substrate solutions, the reaction temperature, and the rate at which the base is added—these parameters affect the particle size and purity of the product.

Physicochemical Properties of Copper Hydroxide

Copper(II) hydroxide in its solid state takes the form of a blue, fine-grained powder or a gel-like precipitate. The compound’s color is characteristic of Cu²⁺ ions and results from the absorption of visible light by the d orbitals of the copper electron.

Solubility: The compound is practically insoluble in water (approx. 2.9 mg/L at 25°C), and the pH of an aqueous suspension is approximately 8–9, reflecting the compound’s basic nature. It dissolves well in acids (diluted sulfuric, hydrochloric, and nitric acids) to form copper salts, and in excess ammonia—forming a deep blue tetraamminediaqua-copper(II) complex.

Thermal stability: Cu(OH)₂ is thermally unstable—decomposition into black copper oxide (CuO) and water begins in the range of 80–100°C (decomposition onset temperature), and complete decomposition occurs at higher temperatures. The product should be stored and dried well below this limit.

Density: approx. 3.37 g/cm³ (for the crystalline form); the value may vary depending on the degree of hydration and the method of preparation.

Reactivity: Reacts with acids (forming copper salts) and with ammonia water (forming a tetraamminediacopper(II) complex); undergoes thermal decomposition in the range of 80–100°C. In concentrated NaOH and at elevated temperatures, it may exhibit weak acidic properties.

Applications of Copper Hydroxide

Copper(II) hydroxide is a compound with a wide range of applications—from analytical and laboratory chemistry, through the ceramics industry and glazing, to plant protection in agriculture. Below, we present the most important areas of use for Cu(OH)₂.

Laboratory and analytical applications

In chemistry laboratories, copper hydroxide is used as a substrate in biuret assays—a method for detecting and quantitatively determining proteins and peptide bonds. The reaction mechanism is as follows: in a strongly basic environment (in the presence of NaOH), Cu(OH)₂ releases Cu²⁺ ions, which form a characteristic violet-blue coordination complex with peptide bonds. The actual reactant is therefore the Cu²⁺ ion in an alkaline environment, not Cu(OH)₂ itself—this compound acts as a substrate from which active copper ions are released. The method is widely used in biochemistry, analytical chemistry, and the food industry.

Cu(OH)₂ is also used as a substrate in the synthesis of other copper compounds—copper oxide (CuO), copper salts, and coordination complexes. As a laboratory reagent, it is used to detect aldehydes and reducing sugars—in Fehling’s and Benedict’s reagents, Cu²⁺ ions (released from Cu(OH)₂ in a basic environment) act as an oxidizing agent, reducing to Cu₂O.

Industrial Applications

In the chemical industry, copper(II) hydroxide is used as a substrate for the production of other copper compounds—primarily copper oxide (CuO), copper sulfate, copper nitrate, and copper coordination complexes used in catalysis. It is also used as a catalyst or catalyst precursor in certain organic processes. It is also used as a component of electroplating baths and as an agent for surface finishing of metals.

In the textile industry, Schweitzer’s solution—a Cu(OH)₂ complex with ammonia having the formula [Cu(NH₃)₄(H₂O)₂]²⁺—was historically used to dissolve cellulose and produce cuprammoniacal fibers (commercially known as cupro or cuprammonium rayon). Although this method is no longer widely used industrially, copper hydroxide remains an important substrate in the synthesis of copper coordination complexes.

Copper Hydroxide in Glazing and Ceramics – Alkaline Baths

Copper(II) hydroxide is a valuable pigment and refining agent used in glazing and artistic ceramics. During the firing of ceramics, Cu(OH)₂ thermally decomposes into copper oxide (CuO), which is responsible for coloring glazes. Depending on the composition of the ceramic body, the firing temperature, and the kiln atmosphere, copper oxide imparts colors to glazes ranging from intense green through turquoise and blue to black.

Of particular importance is the behavior of Cu(OH)₂ in the acidic and basic environments used in the preparation of glazing baths. In an alkaline environment (alkaline glazing baths), copper hydroxide forms complexes with hydroxyl groups, which become incorporated into the glaze structure, producing an intense, uniform color. In an acidic environment, Cu(OH)₂ dissolves to form Cu²⁺ ions, which react with the silicates in the glaze to create characteristic color effects. Ceramists and glazers value copper hydroxide for the predictability of its coloring reactions and the wide range of color effects it produces—depending on the bath pH, the concentration of the copper compound, and the firing parameters.

In glazing practice, copper hydroxide is used at a concentration of 1–5% based on the dry weight of the glaze, most often in the form of a fine-grained powder mixed directly into the ceramic body or applied as a component of immersion baths. The product, available in laboratory grade (p.a.), ensures color uniformity and reproducibility of results across production batches.

Applications in Agriculture and Plant Protection

Copper (II) hydroxide is a widely used plant protection product, registered for controlling fungal and bacterial diseases in fruit, vegetable, and agricultural crops. It acts by contact and on the surface—it forms a protective layer on plant surfaces that releases Cu²⁺ ions, which inhibit the germination of fungal spores and the proliferation of bacteria. It is used to protect apple trees (apple scab, fire blight), potatoes and tomatoes (late blight), grapevines (downy mildew), and many other crops.

In organic farming, copper hydroxide is one of the few approved fungicides and bactericides. However, it is important to be aware of the limitations—excessive use can lead to copper accumulation in the soil and phytotoxicity at too high doses or under unfavorable weather conditions.

Safety and Regulations – Copper (II) Hydroxide

Copper(II) hydroxide is a substance classified in accordance with the CLP Regulation (EC No. 1272/2008). Examples of hazard categories include harm to aquatic life (H400, H410) and skin and eye irritation. Detailed labeling information is provided in the current Safety Data Sheet (SDS) for the specific product batch.

Recommended personal protective equipment: chemical-resistant gloves (nitrile/neoprene), safety glasses or goggles, protective clothing; when working with dust—a half-mask with a P2 or P3 filter. Work in a well-ventilated area or under a fume hood. After contact with skin or eyes: rinse thoroughly with water (at least 15 minutes) and seek medical attention in accordance with the SDS.

Store tightly closed in a dry and cool place (approx. 15–25°C), away from organic materials, acids, and reducing agents. Relative humidity below 60%. Transport in accordance with applicable ADR regulations—confirm classification with the current SDS before shipment.

Technical Documentation – Copper Hydroxide

We include the following with every shipment of copper(II) hydroxide: a Safety Data Sheet (SDS) compliant with REACH, a Certificate of Analysis (CoA) for the batch with the LOT number, and technical specifications. Upon request, we can provide additional certificates for processes with specific quality standards.

CAS Number: 20427-59-2 | EC Number: 243-815-9 | Formula: Cu(OH)₂ | Molar mass: 97.56 g/mol