Copper hydroxide (Cu(OH)2) is a blue solid formed by the reaction of copper salts with hydroxide ions. It’s used as a fungicide and in various chemical processes.
| IUPAC Name | Copper(II) hydroxide |
| Molecular Formula | Cu(OH)2 |
| CAS Number | 20427-59-2 |
| Synonyms | Cupric hydroxide; Copper dihydroxide; CuOH2 |
| InChI | InChI=1S/Cu.2H2O/h;2*1H2/q+2;;/p-2 |
Copper Hydroxide Properties
Copper Hydroxide Formula
The chemical formula of cupric hydroxide is Cu(OH)2. It represents the combination of one copper ion (Cu2+) and two OH- ions held together by ionic bonds. This blue solid compound is commonly used in various industries due to its unique properties.
Copper Hydroxide Molar Mass
The molar mass of cupric hydroxide (Cu(OH)2) can be calculated by adding the atomic masses of its constituent elements. Copper (Cu) has an atomic mass of approximately 63.55 g/mol, and each OH- ion has a combined atomic mass of approximately 17.01 g/mol. Therefore, the molar mass of cupric hydroxide is approximately 97.55 g/mol.
Copper Hydroxide Boiling Point
Cupric hydroxide does not have a distinct boiling point as it decomposes before reaching its boiling point. When heated, it undergoes a thermal decomposition reaction to form copper oxide and water vapor.
Copper Hydroxide Melting Point
Cupric hydroxide has a melting point of around 200°C (392°F). At this temperature, the solid undergoes a phase transition and transforms into a liquid state.
Copper Hydroxide Density g/mL
The density of cupric hydroxide is approximately 3.36 g/mL. This value represents the mass of one milliliter of cupric hydroxide, indicating its compactness and concentration.
Copper Hydroxide Molecular Weight
The molecular weight of cupric hydroxide is approximately 97.55 g/mol. It is calculated by summing the atomic weights of all atoms present in one molecule of cupric hydroxide.
Copper Hydroxide Structure
Cupric hydroxide adopts a crystalline structure, with Cu2+ ions surrounded by OH- ions in a trigonal planar arrangement. This crystal lattice arrangement contributes to its stability and distinctive properties.
Copper Hydroxide Solubility
Cupric hydroxide exhibits limited solubility in water. It forms a sparingly soluble suspension in water, meaning only a small amount of the compound dissolves in the solvent. The solubility can be influenced by factors such as temperature and pH levels.
| Appearance | Blue solid |
| Specific Gravity | ~3.36 g/mL |
| Color | Blue |
| Odor | Odorless |
| Molar Mass | ~97.55 g/mol |
| Density | ~3.36 g/mL |
| Melting Point | ~200°C (392°F) |
| Boiling Point | Decomposes |
| Flash Point | N/A |
| Water Solubility | Sparingly soluble |
| Solubility | Limited, varies with temperature and pH levels |
| Vapour Pressure | N/A |
| Vapour Density | N/A |
| pKa | N/A |
| pH | Alkaline (basic) |
Copper Hydroxide Safety and Hazards
Cupric hydroxide poses certain safety and hazard considerations. It is generally considered low in toxicity but can cause irritation to the skin, eyes, and respiratory tract upon contact or inhalation. Adequate protective measures, such as wearing gloves and safety goggles, should be taken while handling this compound. In case of accidental ingestion or exposure, immediate medical attention is necessary. Additionally, cupric hydroxide should be stored in a secure and well-ventilated area, away from incompatible substances. Proper disposal procedures must be followed to prevent environmental contamination. Adherence to safety guidelines is crucial to minimize potential risks associated with cupric hydroxide.
| Hazard Symbols | None |
| Safety Description | Low toxicity; Irritant |
| UN IDs | Not applicable |
| HS Code | 2825.90.5000 |
| Hazard Class | Not classified as hazardous |
| Packing Group | Not classified |
| Toxicity | Low |
Copper Hydroxide Synthesis Methods
Several active methods can synthesize cupric hydroxide.
One common approach involves the reaction of a Cu salt, such as CuSO4, with a strong base like sodium hydroxide (NaOH) or potassium hydroxide (KOH). During this process, the hydroxide ions (OH-) from the base displace the sulfate ions (SO4^2-) in the CuSO4, forming cupric hydroxide (Cu(OH)2) as a blue precipitate.
Another method involves the reaction of a copper(II) salt with ammonia (NH3). By adding ammonia to a Cu(II) solution, cupric hydroxide precipitates due to the combination of Cu2+ ions with hydroxide ions from the ammonia.
Electrolysis enables the synthesis of cupric hydroxide by immersing a Cu electrode in an electrolyte solution and applying a direct electric current. The reduction of water at the cathode generates hydroxide ions, leading to the formation of cupric hydroxide.
These active synthesis methods offer controlled and efficient ways to produce cupric hydroxide for various industrial and research applications.
Copper Hydroxide Uses
Cupric hydroxide finds multiple applications across various industries due to its unique properties and versatile nature. Some notable uses include:
- Fungicide: Agriculturalists widely use it as a protective fungicide to control fungal diseases in crops such as fruits, vegetables, and ornamental plants.
- Chemical Intermediates: It serves as a valuable chemical intermediate in the synthesis of various copper compounds, like copper oxide and copper salts.
- Wood Preservative: It treats wood and offers protection against wood-boring insects and decay-causing fungi, extending the life of wooden structures.
- Antibacterial Agent: In certain formulations, it acts as an antibacterial agent, finding applications in medical and healthcare settings.
- Aquatic Treatment: It aids in managing algae and aquatic weeds in ponds, lakes, and other water bodies, maintaining ecological balance.
- Ceramics and Glass Industry: Manufacturers use it as a coloring agent to impart vibrant blue and green hues to ceramics and glass products.
- Pyrotechnics: It contributes to the coloration of fireworks and flares, playing a role in pyrotechnic applications.
- Battery Manufacturing: It finds utility in the production of batteries as an electrode material, aiding in energy storage.
- Paint and Coatings: Certain paint formulations incorporate it to provide protective and antimicrobial properties.
The diverse range of applications showcases the significance of cupric hydroxide in multiple industries, making it a valuable compound for various practical uses.
Questions:
Q: Is copper hydroxide soluble?
A: Cupric hydroxide has limited solubility in water, forming a sparingly soluble suspension.
Q: How many moles are in 68 grams of copper (II) hydroxide Cu(OH)2?
A: There are approximately 0.697 moles of Cu(OH)2 in 68 grams.
Q: Is copper II hydroxide soluble in water?
A: Cupric II hydroxide has limited solubility in water.
Q: Is sodium hydroxide and copper sulfate a chemical reaction?
A: Yes, the reaction between NaOH and CuSO4 results in the formation of cupric hydroxide and sodium sulfate.
Q: Is copper(II) hydroxide soluble?
A: Cupric(II) hydroxide has limited solubility in water.
Q: What is the color of copper hydroxide?
A: Cupric hydroxide is blue in color.
Q: Is copper hydroxide an alkali?
A: Cupric hydroxide is a base but not classified as an alkali.
Q: Is copper hydroxide a strong base?
A: Cupric hydroxide is not considered a strong base.
Q: Is Cu(OH)2 soluble in water?
A: Cu(OH)2 has limited solubility in water.
Q: How many moles are in 68 grams of copper (II) hydroxide Cu(OH)2?
A: There are approximately 0.697 moles of Cu(OH)2 in 68 grams.
Q: How many moles are present in 34 grams of Cu(OH)2?
A: There are approximately 0.3485 moles of Cu(OH)2 in 34 grams.
Q: Does any solid Cu(OH)2 form when 0.075 g of KOH is dissolved in 1.0 L of 1.0 × 10^−3 M Cu(NO3)2?
A: Yes, solid Cu(OH)2 forms as a precipitate due to the reaction between KOH and Cu(NO3)2