Nickel nitrate (Ni(NO₃)₂) is a chemical compound with nickel and nitrate ions. It’s soluble in water and often used in catalysts, electroplating, and as a precursor in other nickel compounds.
| IUPAC Name | Nickel dinitrate |
| Molecular Formula | Ni(NO₃)₂ |
| CAS Number | 13138-45-9 |
| Synonyms | Nickel(II) nitrate, Nickelous nitrate, Dinitronickel, Nickel bis(nitrate) |
| InChI | InChI=1S/2NO3.Ni/c22-1(3)4;/q2-1;+2 |
Nickel Nitrate Properties
Nickel Nitrate Formula
The chemical formula of nickel dinitrate is Ni(NO₃)₂. It represents a compound composed of nickel (Ni) cations and nitrate (NO₃) anions. The subscript “2” in the formula indicates that there are two NO3- ions for each Ni+2 cation.
Nickel Nitrate Molar Mass
The molar mass of nickel dinitrate can be calculated by adding the atomic masses of its constituent elements. Nickel (Ni) has a molar mass of approximately 58.69 g/mol, while nitrate (NO₃) has a molar mass of around 62.00 g/mol. Adding them together, the molar mass of nickel dinitrate is approximately 182.69 g/mol.
Nickel Nitrate Boiling Point
Nickel dinitrate’s boiling point refers to the temperature at which it changes from a liquid to a gaseous state. The boiling point of nickel dinitrate is approximately 136.7 degrees Celsius (278.06 degrees Fahrenheit). However, it is essential to note that this value may vary slightly depending on the purity of the compound.
Nickel Nitrate Melting Point
Nickel dinitrate’s melting point is the temperature at which it transforms from a solid to a liquid state. The melting point of nickel dinitrate is around 56.7 degrees Celsius (134.06 degrees Fahrenheit). Similar to the boiling point, the melting point may be influenced by the compound’s purity.
Nickel Nitrate Density g/mL
The density of nickel dinitrate is a measure of its mass per unit volume. Nickel dinitrate has a density of approximately 1.68 g/mL. This value indicates that it is denser than water, which has a density of 1 g/mL.
Nickel Nitrate Molecular Weight
Nickel dinitrate’s molecular weight is the sum of the atomic weights of all the atoms present in its chemical formula. As mentioned earlier, the molecular weight of nickel dinitrate is approximately 182.69 g/mol.
Nickel Nitrate Structure
The structure of nickel dinitrate can be visualized as nickel cations (Ni²⁺) surrounded by two nitrate (NO₃⁻) anions per cation. The nitrate ions form coordinate bonds with the nickel cations, creating a stable ionic compound.
Nickel Nitrate Solubility
Nickel dinitrate is highly soluble in water, forming a clear, greenish-blue solution. Its solubility in water is an essential property, as it allows it to be easily used in various applications, such as catalysts, electroplating, and the production of other nickel compounds.
| Appearance | Greenish-blue solid |
| Specific Gravity | 1.68 g/mL |
| Color | Greenish-blue |
| Odor | Odorless |
| Molar Mass | 182.69 g/mol |
| Density | 1.68 g/mL |
| Melting Point | 56.7°C |
| Boiling Point | 136.7°C |
| Flash Point | Not applicable |
| Water Solubility | Highly soluble |
| Solubility | Soluble in water and organic solvents such as ethanol |
| Vapour Pressure | Not available |
| Vapour Density | Not available |
| pKa | Not available |
| pH | Neutral (around 7) |
Please note that some properties may not be available or relevant for nickel diitrate.
Nickel Nitrate Safety and Hazards
Nickel dinitrate poses certain safety hazards and precautions must be taken while handling it. Direct contact with the compound can cause skin and eye irritation. Inhalation of its dust or fumes may lead to respiratory irritation. It is essential to wear appropriate protective gear, such as gloves and safety goggles, when working with nickel dinitrate. Avoid ingestion as it can be harmful to health. In case of accidental exposure, seek immediate medical attention. Furthermore, proper storage in a well-ventilated area away from incompatible substances is crucial to minimize potential risks and ensure safe handling.
| Hazard Symbols | Corrosive, Irritant, Health Hazard |
| Safety Description | Causes skin and eye irritation. Harmful if inhaled or ingested. Handle with care. Avoid direct contact. Use protective equipment. |
| UN IDs | UN2724 |
| HS Code | 2834.2990 |
| Hazard Class | 5.1 (Oxidizing Substances) |
| Packing Group | II |
| Toxicity | Moderately toxic |
Nickel Nitrate Synthesis Methods
There are several methods to synthesize nickel dinitrate. One common method involves the reaction between nickel oxide (NiO) or nickel hydroxide (Ni(OH)₂) with nitric acid (HNO₃). During this process, nickel oxide or nickel hydroxide dissolves in nitric acid, leading to the formation of nickel dinitrate and water as byproducts.
The reaction can take the following representation:
- With Nickel Oxide: NiO + 2HNO₃ → Ni(NO₃)₂ + H₂O
- With Nickel Hydroxide: Ni(OH)₂ + 2HNO₃ → Ni(NO₃)₂ + 2H₂O
Another approach involves the reaction between nickel metal and concentrated nitric acid, which results in the formation of nickel dinitrate and nitrogen dioxide gas (NO₂) as a byproduct:
- With Nickel Metal: Ni + 4HNO₃ → Ni(NO₃)₂ + 2H₂O + 2NO₂
It is important to conduct these reactions in well-controlled conditions, as nitric acid is a strong oxidizing agent and can be hazardous. Ensure a safe and successful outcome during the synthesis process by actively employing proper safety measures and equipment. Additionally, the choice of reactants and reaction conditions may vary depending on the specific application and desired properties of the nickel dinitrate product.
Nickel Nitrate Uses
Nickel dinitrate finds multiple applications across various industries due to its unique properties. Here are some of its prominent uses:
- Electroplating: Nickel dinitrate enables the deposition of a thin layer of nickel onto various metals, enhancing their corrosion resistance and appearance during electroplating processes.
- Catalyst: It plays a crucial role as a catalyst in chemical reactions, facilitating the conversion of reactants into desired products, particularly in organic synthesis.
- Ceramics: The ceramics industry employs nickel dinitrate to impart specific coloration and enhance the performance of ceramic materials.
- Glass Industry: Manufacturers in the glass industry use nickel dinitrate to produce colored glass with desirable optical properties.
- Battery Production: Manufacturers utilize nickel dinitrate in the production of nickel-based batteries, including nickel-metal hydride (NiMH) batteries.
- Fuel Cells: Nickel dinitrate acts as a precursor in the fabrication of nickel oxide electrodes for solid oxide fuel cells (SOFCs).
- Pyrotechnics: In pyrotechnics, nickel dinitrate serves as an oxidizer, producing green flames in fireworks.
- Chemical Reagents: It functions as a reagent in various chemical reactions, especially those involving nickel complexes.
- Fertilizers: In agriculture, nickel dinitrate finds occasional use as a source of nickel in fertilizers to address nickel deficiencies in certain crops.
Nickel dinitrate’s diverse applications across different industries highlight its significance as a versatile compound with wide-ranging practical uses.
Questions:
Q: When ammonium phosphate and nickel(ii) nitrate solutions are mixed, what precipitates out?
A: Nickel(II) phosphate precipitates out.
Q: What is the molarity of a solution that contains 5.8 grams of nickel nitrate in 500 ml?
A: The molarity is 0.2 M.
Q: What wavelengths does nickel nitrate absorb?
A: Nickel dinitrate absorbs wavelengths in the ultraviolet and visible regions.
Q: Is nickel II nitrate soluble?
A: Yes, nickel(II) dinitrate is soluble in water.
Q: What is the formula for nickel II nitrate?
A: The formula is Ni(NO₃)₂.
Q: What is the color of nickel II nitrate?
A: The color of nickel(II) dinitrate is greenish-blue.
Q: How many atoms of nitrogen are in the chemical formula Ni(NO₃)₂?
A: There are four atoms of nitrogen.
Q: Is Ni(NO₃)₂ soluble in water?
A: Yes, Ni(NO₃)₂ is soluble in water.
Q: Which of the compounds C4H10, BaCl2, Ni(NO₃)₂, SF6 are expected to exist as formula units?
A: C4H10 (butane) and SF6 (sulfur hexafluoride) are expected to exist as formula units. BaCl2 and Ni(NO₃)₂ are ionic compounds.