Zinc nitrate (Zn(NO3)2) is a compound containing zinc and nitrate ions. It is soluble in water and commonly used in industries for various applications, including as a catalyst and in the production of dyes and pigments.
| IUPAC Name | Zinc nitrate |
| Molecular Formula | Zn(NO3)2 |
| CAS Number | 7779-88-6 |
| Synonyms | Zinc dinitrate, Nitric acid zinc salt, Celloxan, Nitrate de zinc |
| InChI | InChI=1S/2NO3.Zn/c22-1(3)4;/q2-1;+2 |
Zinc Nitrate Properties
Zinc Nitrate Formula
The formula for zinc dinitrate is Zn(NO3)2. It consists of one zinc ion (Zn2+) and two NO3- ions held together by ionic bonds. The formula represents the ratio of elements present in the compound.
Zinc Nitrate Molar Mass
The molar mass of zinc dinitrate can be calculated by adding the atomic masses of its constituent elements. The atomic mass of zinc (Zn) is approximately 65.38 grams per mole, and the atomic mass of nitrogen (N) and oxygen (O) in NO3- ions is about 14.01 and 16.00 grams per mole, respectively. Therefore, the molar mass of zinc dinitrate is approximately 189.38 grams per mole.
Zinc Nitrate Boiling Point
Zinc dinitrate does not have a specific boiling point since it decomposes before reaching its boiling point. However, when heated, it decomposes into zinc oxide, nitrogen dioxide, and oxygen. This decomposition reaction occurs around 140°C (284°F), releasing brown fumes of nitrogen dioxide.
Zinc Nitrate Melting Point
The melting point of zinc dinitrate depends on its hydration state. The anhydrous form of zinc dinitrate (Zn(NO3)2) melts at around 238°C (460°F). However, the hexahydrate form (Zn(NO3)2·6H2O) has a lower melting point of approximately 36°C (97°F) as it contains water molecules within its crystal structure.
Zinc Nitrate Density g/mL
The density of zinc dinitrate varies depending on its concentration and temperature. However, under standard conditions, the density of the anhydrous form is approximately 2.065 grams per milliliter (g/mL). The density of the hexahydrate form is slightly higher due to the presence of water molecules.
Zinc Nitrate Molecular Weight
The molecular weight of zinc dinitrate is calculated by summing the atomic masses of its constituent elements. The molecular weight of zinc dinitrate is approximately 189.38 grams per mole, as mentioned earlier.
Zinc Nitrate Structure
Zinc dinitrate has an ionic structure, with the zinc cation (Zn2+) surrounded by six water molecules in the hexahydrate form. The nitrate ions (NO3-) are present as discrete entities in the crystal lattice.
Zinc Nitrate Solubility
Zinc dinitrate is highly soluble in water. The solubility increases with temperature. At room temperature, approximately 118 grams of zinc dinitrate can dissolve in 100 grams of water, resulting in a saturated solution.
| Appearance | Colorless crystals |
| Specific Gravity | 2.065 g/mL |
| Color | Colorless |
| Odor | Odorless |
| Molar Mass | 189.38 g/mol |
| Density | 2.065 g/mL |
| Melting Point | 238°C (460°F) (anhydrous) |
| Boiling Point | Decomposes (~140°C/284°F) |
| Flash Point | Not applicable |
| Water Solubility | Highly soluble in water |
| Solubility | Soluble in water |
| Vapour Pressure | Not available |
| Vapour Density | Not available |
| pKa | Not applicable |
| pH | ~4 (aqueous solution) |
Zinc Nitrate Safety and Hazards
Zinc dinitrate poses certain safety hazards that should be considered. It is important to handle it with care to prevent potential risks. Contact with the compound can cause skin and eye irritation. Ingestion or inhalation of zinc dinitrate can lead to gastrointestinal disturbances and respiratory discomfort. It is advisable to use appropriate protective measures, such as gloves and goggles, when working with zinc dinitrate. Furthermore, it should be stored in a well-ventilated area, away from incompatible substances. In case of accidental exposure or ingestion, seeking medical attention is recommended. Adhering to proper safety protocols ensures the safe handling and use of zinc dinitrate.
| Hazard Symbols | Oxidizing Agent |
| Safety Description | Causes skin and eye irritation. Avoid ingestion and inhalation. Handle with appropriate protective measures. |
| UN IDs | UN 1514 (anhydrous), UN 1515 (hexahydrate) |
| HS Code | 28342990 |
| Hazard Class | 5.1 (Oxidizing Substances) |
| Packing Group | II (anhydrous), III (hexahydrate) |
| Toxicity | Moderately toxic |
Zinc Nitrate Synthesis Methods
There are various methods for synthesizing zinc dinitrate. One common approach is the reaction between zinc metal and nitric acid. In this method, zinc reacts with nitric acid to produce zinc dinitrate and release hydrogen gas. Operators carefully control the reaction to maintain safety.
Another method involves the reaction between zinc oxide and nitric acid. Zinc oxide is dissolved in nitric acid, leading to the formation of zinc dinitrate and water. This method is useful when zinc oxide is readily available.
Additionally, zinc carbonate can be reacted with nitric acid to produce zinc dinitrate. The carbonate reacts with the nitric acid, forming carbon dioxide gas, water, and zinc dinitrate.
It is important to note that these reactions should be conducted in appropriate laboratory conditions with the necessary safety precautions. Proper protective equipment, such as gloves and goggles, should be worn, and the reactions should be carried out in a well-ventilated area.
Overall, these methods provide effective ways to synthesize zinc dinitrate, allowing for its use in various industrial applications.
Zinc Nitrate Uses
Zinc dinitrate finds application in various industries due to its versatile properties. Here are some key uses of zinc dinitrate:
- Catalyst: Zinc dinitrate catalyzes various chemical reactions, facilitating the production of dyes, pharmaceuticals, and polymers.
- Electroplating: In electroplating processes, zinc dinitrate deposits a zinc layer onto metal surfaces, imparting corrosion resistance and enhancing appearance.
- Pigments and Dyes: Zinc dinitrate acts as a precursor in producing zinc-based pigments and dyes, crucial for paints, coatings, and textiles.
- Fertilizers: Zinc dinitrate serves as a zinc source in fertilizers, ensuring plants receive sufficient nutrients for growth and development.
- Glass Manufacturing: Zinc dinitrate is instrumental in glass manufacturing, enhancing optical properties such as transparency and refractive index.
- Water Treatment: Zinc dinitrate plays a vital role in water treatment systems, controlling algae and bacterial growth, and maintaining water quality.
- Laboratory Reagent: In various laboratory experiments, zinc dinitrate actively functions as a reagent, particularly in analytical chemistry and research.
- Medicine and Pharmaceuticals: Zinc dinitrate actively contributes to certain pharmaceutical formulations and topical medications due to its antimicrobial properties.
- Fire Retardants: Zinc dinitrate is a key component of fire-retardant formulations, actively reducing the flammability of materials.
- Textile Industry: In textile dyeing and printing processes, zinc dinitrate actively improves color fastness and enhances dye uptake.
These diverse applications highlight the significance of zinc dinitrate across multiple industries, contributing to a range of products and processes.
Questions:
Q: Is zinc nitrate soluble?
A: Yes, zinc dinitrate is soluble in water.
Q: How do you precipitate zinc carbonate from zinc nitrate?
A: To precipitate zinc carbonate from Zn(NO3)2, add a solution of sodium carbonate or sodium bicarbonate to the zinc dinitrate solution, resulting in the formation of zinc carbonate as a precipitate.
Q: Does zinc react with silver nitrate?
A: Yes, Zn reacts with silver nitrate, displacing silver metal and forming zinc dinitrate.
Q: Is zinc nitrate a salt?
A: Yes, zinc nitrate is a salt composed of zinc cations (Zn2+) and NO3- ions.
Q: What forms when zinc nitrate reacts with potassium hydroxide?
A: When Zn(NO3)2 reacts with potassium hydroxide, Zn(OH)2 precipitates, and potassium nitrate is formed.
Q: What is the formula for lithium zinc nitrate?
A: The formula for lithium zinc dinitrate is LiZn(NO3)3.
Q: How to standardize magnesium nitrate and zinc nitrate solution?
A: To standardize magnesium nitrate and Zn dinitrate solutions, titration methods can be employed with a suitable standardized reagent.
Q: What is the acid and metal oxide used to produce zinc nitrate?
A: Nitric acid (HNO3) and zinc oxide (ZnO) are used to produce zinc dinitrate.
Q: What are the products when zinc is added to lead nitrate solution?
A: When Zn is added to a lead nitrate solution, zinc dinitrate and metallic lead are formed.
Q: What is zinc nitrate?
A: Zinc dinitrate is a chemical compound composed of zinc cations (Zn2+) and NO3- anions, often found as a crystalline solid.
Q: How many oxygen atoms are present in 1.50 mol of Zn(NO3)2?
A: In 1.50 mol of Zn(NO3)2, there are 9.00 mol or 27.00 atoms of oxygen.
Q: What mass of Zn(NO3)2 must be diluted to a mass of 1.00 kg with H2O to prepare 97 ppm Zn2+(aq)?
A: To prepare a solution with 97 ppm of Zn2+(aq), approximately 97 mg of Zn(NO3)2 must be diluted with water to a mass of 1.00 kg.