Copper nitrate (Cu(NO3)2) is a blue crystalline compound used in various industries. It serves as a catalyst, oxidizing agent, and precursor for copper-based materials in chemical processes.
| IUPAC Name | Copper(II) nitrate |
| Molecular Formula | Cu(NO3)2 |
| CAS Number | 3251-23-8 |
| Synonyms | Cupric nitrate; Copper dinitrate; Dicopper nitrate; Nitric acid, copper(2+) salt |
| InChI | InChI=1S/2NO3.Cu/c22-1(3)4;/q2-1;+2 |
Copper Nitrate Properties
Copper Nitrate Formula
The chemical formula of cupric nitrate is Cu(NO3)2. It indicates that each cupric nitrate molecule contains one copper (Cu) ion and two nitrate (NO3) ions. The presence of copper(II) ions denotes a +2 oxidation state of copper.
Copper Nitrate Molar Mass
Cupric nitrate’s molar mass can be calculated by adding the atomic masses of its constituent elements. Copper (Cu) has a molar mass of approximately 63.55 g/mol, while nitrate (NO3) has a molar mass of around 62.00 g/mol. Thus, the molar mass of cupric nitrate is about 187.55 g/mol.
Copper Nitrate Boiling Point
Cupric nitrate’s boiling point refers to the temperature at which it changes from a liquid to a gaseous state under standard atmospheric pressure. The boiling point of cupric nitrate is typically above 100°C (212°F). However, it’s important to note that cupric nitrate usually decomposes before reaching its boiling point.
Copper Nitrate Melting Point
Cupric nitrate’s melting point is the temperature at which it transforms from a solid to a liquid state. The melting point of cupric nitrate is usually around 256°C to 260°C (493°F to 500°F). It is essential to handle this substance carefully to avoid decomposition.
Copper Nitrate Density g/mL
The density of cupric nitrate refers to its mass per unit volume. The density of solid cupric nitrate is typically around 2.32 g/mL, while the density of its aqueous solutions can vary based on concentration.
Copper Nitrate Molecular Weight
The molecular weight of cupric nitrate is the sum of the atomic weights of all the atoms in its chemical formula. For Cu(NO3)2, the molecular weight is approximately 187.55 g/mol.
Copper Nitrate Structure
Cupric nitrate exists as a blue crystalline solid with a hexagonal crystalline structure. Each copper ion (Cu2+) is surrounded by six oxygen atoms from two nitrate ions, creating a coordinated arrangement. The structure contributes to its stability and reactivity in various chemical processes.
Copper Nitrate Solubility
Cupric nitrate is moderately soluble in water. It forms an aqueous solution when dissolved in water, which can be utilized in various applications like electroplating and as a reagent in chemical reactions. However, its solubility decreases with lower temperatures.
| Appearance | Blue crystalline solid |
| Specific Gravity | N/A |
| Color | Blue |
| Odor | Odorless |
| Molar Mass | 187.55 g/mol |
| Density | 2.32 g/mL (solid) |
| Melting Point | 256-260°C (493-500°F) |
| Boiling Point | Decomposes before boiling |
| Flash Point | N/A |
| Water Solubility | Moderately soluble, forms an aqueous solution |
| Solubility | Soluble in water |
| Vapour Pressure | N/A |
| Vapour Density | N/A |
| pKa | N/A |
| pH | Acidic |
Copper Nitrate Safety and Hazards
Cupric nitrate poses certain safety and hazards concerns. It is essential to handle this compound with caution. Direct contact with the skin or eyes may cause irritation or burns. Inhalation of dust or fumes can lead to respiratory irritation. When heated, it can release toxic nitrogen oxides. The substance is also an oxidizing agent and may ignite flammable materials upon contact. Proper protective equipment, like gloves and goggles, should be worn when working with cupric nitrate. It should be stored away from combustible materials and incompatible substances to minimize potential risks. Always follow safety guidelines and use in a well-ventilated area.
| Hazard Symbols | Oxidizing agent, Corrosive, Irritant |
| Safety Description | Handle with caution. Avoid contact with skin and eyes. Use in a well-ventilated area. Keep away from combustible materials. |
| UN IDs | UN3085 |
| HS Code | 28342910 |
| Hazard Class | 5.1 (Oxidizing Agent) |
| Packing Group | III |
| Toxicity | Harmful if ingested. May cause skin and eye irritation. Inhalation of dust or fumes can cause respiratory irritation. |
Copper Nitrate Synthesis Methods
There are several methods for synthesizing cupric nitrate.
One common approach involves the reaction between copper oxide (CuO) or copper hydroxide (Cu(OH)2) with nitric acid (HNO3). When preparing cupric nitrate, one can slowly add cupric oxide or cupric hydroxide to a solution of nitric acid, which leads to the formation of cupric nitrate and water.
Another method involves the reaction between copper metal (Cu) and concentrated nitric acid. Cu metal reacts with nitric acid to produce cupric nitrate, nitrogen dioxide (NO2) gas, and water. This method requires careful handling due to the formation of toxic nitrogen dioxide gas.
Alternatively, you can dissolve Cu metal or cupric oxide in a mixture of nitric acid and hydrogen peroxide (H2O2) to produce cupric nitrate. This method provides a faster reaction and yields pure cupric nitrate.
Lastly, the double displacement reaction between CuSO4 and sodium nitrate (NaNO3) can also produce cupric nitrate. By mixing these two salts in water, cupric nitrate precipitates out, and the by-product sodium sulfate remains dissolved.
Follow safety precautions during synthesis because the chemicals involved exhibit reactivity. Employ proper protective equipment and utilize appropriate lab practices to ensure a successful and safe synthesis of cupric nitrate.
Copper Nitrate Uses
Cupric nitrate finds various applications across different industries due to its unique properties. Some notable uses include:
- Catalyst: It acts as a catalyst in organic synthesis, facilitating reactions like the conversion of alcohols to aldehydes or ketones.
- Pyrotechnics: Cupric nitrate is a key component in pyrotechnic formulations, contributing to blue and green flame colors.
- Agriculture: In agriculture, it serves as a copper source in fertilizers to provide essential nutrients to plants.
- Oxidizing agent: Cupric nitrate actively oxidizes other substances in chemical processes.
- Metal plating: Cupric nitrate actively deposits a thin layer of Cu on various metal surfaces in electroplating processes.
- Pigments and dyes: Cupric nitrate actively contributes to the creation of green and blue pigments for ceramics, glass, and textiles.
- Photographic processes: Cupric nitrate actively assists in image development in some photographic solutions.
- Preservation: It finds application in preserving wood by aiding in the fixation of preservatives.
- Preparation of other copper compounds: It serves as a precursor for the synthesis of various copper-based materials and compounds.
Cupric nitrate’s versatility and reactivity make it a valuable chemical in different fields, ranging from industrial processes to artistic applications.
Questions:
Q: What happens when copper nitrate is heated?
A: When heated, cupric nitrate decomposes into cupric oxide, nitrogen dioxide gas, and oxygen.
Q: Is copper nitrate soluble in water?
A: Yes, cupric nitrate is moderately soluble in water.
Q: What is the chemical formula of copper nitrate?
A: The chemical formula of cupric nitrate is Cu(NO3)2.
Q: Is copper nitrate a strong electrolyte?
A: Yes, cupric nitrate is a strong electrolyte, dissociating into ions when dissolved in water.
Q: What is the charge of copper nitrate?
A: Cupric nitrate has a net charge of 0; it is a neutral compound.
Q: How many nitrogen atoms are in 10.2 g of copper(II) nitrate?
A: There are approximately 0.161 moles of cupric (II) nitrate, and thus, about 0.322 moles of nitrogen atoms.
Q: What mass of silver can be produced from 3.00 mol of copper and 3.85 mol of silver nitrate?
A: 342.3 g of silver can be produced, following the balanced chemical equation.
Q: Is copper nitrate soluble?
A: Yes, cupric nitrate is soluble in water.
Q: What is the formula for copper (II) nitrate?
A: The formula for cupric (II) nitrate is Cu(NO3)2.
Q: What is produced during the replacement reaction of Cu(NO3)2 and Zn?
A: Zinc nitrate (Zn(NO3)2) and cupric metal (Cu) are produced during the replacement reaction.
Q: What is Cu(NO3)2?
A: Cu(NO3)2 is the chemical formula for cupric nitrate, a blue crystalline compound.
Q: Which of the following is reduced in the following reaction? Cu(NO3)2 + Zn –> Zn(NO3)2 + Cu
A: Copper (Cu) is reduced in the reaction, gaining electrons to form copper metal.
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: No, solid Cu(OH)2 does not form since Cu(NO3)2 ionizes completely in solution, and there is an excess of OH⁻ ions from KOH.