Nickel sulfate (NiSO4) is a compound that consists of nickel, sulfur, and oxygen atoms. It is commonly used in electroplating, catalysts, and as a nutrient in some fertilizers.
| IUPAC Name | Nickel(II) sulfate |
| Molecular Formula | NiSO4 |
| CAS Number | 7786-81-4 |
| Synonyms | Nickelous sulfate, Sulfuric acid nickel salt, Nickel(II) sulfate, Nickel(2+);sulfate |
| InChI | InChI=1S/Ni.H2O4S/c;1-5(2,3)4/h;(H2,1,2,3,4)/q+2;/p-2 |
Nickel Sulfate Properties
Nickel Sulfate Formula
The chemical formula of nickel sulfate is NiSO4. It represents the combination of one nickel atom (Ni) and one sulfate group (SO4). The formula clearly indicates the presence of nickel and sulfur, along with oxygen in the sulfate group.
Nickel Sulfate Molar Mass
The molar mass of nickelous sulfate (NiSO4) is calculated by summing the atomic masses of its constituent elements. Nickel (Ni) has an atomic mass of approximately 58.69 grams per mole, while sulfur (S) has an atomic mass of about 32.07 grams per mole, and oxygen (O) has an atomic mass of roughly 16 grams per mole. By adding these values, the molar mass of nickelous sulfate is determined to be around 154.76 grams per mole.
Nickel Sulfate Boiling Point
Nickelous sulfate does not have a specific boiling point because it decomposes when heated. However, it is important to note that its decomposition temperature is influenced by factors such as pressure and the presence of other substances. Therefore, it is advisable to handle nickelous sulfate with caution when exposed to high temperatures.
Nickel Sulfate Melting Point
The melting point of nickelous sulfate is approximately 100 degrees Celsius (212 degrees Fahrenheit). At this temperature, the solid form of nickelous sulfate transitions into a liquid state. It is worth mentioning that variations in the purity and crystal structure of nickelous sulfate can slightly affect its melting point.
Nickel Sulfate Density g/mL
The density of nickelous sulfate refers to its mass per unit volume. The density of nickelous sulfate is typically around 3.68 grams per milliliter (g/mL). It is worth noting that the density may vary depending on the temperature and purity of the sample.
Nickel Sulfate Molecular Weight
The molecular weight of nickelous sulfate (NiSO4) is the sum of the atomic weights of its constituent elements. As previously mentioned, the molecular weight of nickelous sulfate is approximately 154.76 grams per mole.
Nickel Sulfate Structure
Nickelous sulfate possesses a crystal structure in its solid state. It forms monoclinic crystals with each nickel ion (Ni2+) surrounded by six oxygen atoms from sulfate groups. The sulfate groups are arranged in a way that allows for the efficient packing of the crystal lattice.
Nickel Sulfate Solubility
Nickelous sulfate exhibits moderate solubility in water. It dissolves readily in water, with the solubility increasing as temperature rises. The presence of other ions and substances can influence its solubility. Furthermore, nickelous sulfate can form hydrates when combined with water molecules, leading to the formation of various nickelous sulfate hydrates.
| Appearance | Blue/green crystals |
| Specific Gravity | 3.68 g/mL |
| Color | Blue/green |
| Odor | Odorless |
| Molar Mass | 154.76 g/mol |
| Density | 3.68 g/mL |
| Melting Point | 100 °C (212 °F) |
| Boiling Point | Decomposes |
| Flash Point | Not applicable |
| Water Solubility | Highly soluble |
| Solubility | Soluble in water, and organic solvents such as ethanol |
| Vapour Pressure | Not applicable |
| Vapour Density | Not applicable |
| pKa | -1.1 (Sulfuric acid) |
| pH | Acidic (around 4) |
Nickel Sulfate Safety and Hazards
Nickelous sulfate poses certain safety hazards that need to be addressed. It is essential to handle it with care to avoid potential risks. Direct skin contact should be minimized, as it may cause skin irritation or sensitization. Ingestion or inhalation of nickelous sulfate should be avoided, as it can lead to adverse health effects. When working with nickelous sulfate, appropriate personal protective equipment, such as gloves and goggles, should be worn to prevent contact with the substance. Nickelous sulfate should be stored in a cool, dry place, away from incompatible materials. Proper ventilation is necessary when working with nickelous sulfate to minimize the concentration of airborne particles.
| Hazard Symbols | None |
| Safety Description | – Avoid skin contact – Avoid ingestion and inhalation – Wear appropriate personal protective equipment |
| Un IDs | Not applicable |
| HS Code | 2833.25 |
| Hazard Class | Not classified |
| Packing Group | Not applicable |
| Toxicity | May cause skin irritation or sensitization |
Nickel Sulfate Synthesis Methods
There are various methods for synthesizing nickelous sulfate.
One common approach involves the reaction between nickel metal or nickel oxide with sulfuric acid. In this method, sulfuric acid dissolves Ni metal or nickel oxide, resulting in the formation of nickelous sulfate. You can carry out the reaction under controlled conditions, such as temperature and stirring, to ensure efficient conversion.
Another method involves sulfuric acid reacting with nickel carbonate. The sulfuric acid dissolves nickel carbonate, producing nickelous sulfate. Chemists commonly use this method when they have readily available nickel carbonate, as it offers a convenient starting material.
Furthermore, sulfuric acid can dissolve nickel hydroxide to synthesize NiSO4. The dissolution of nickel hydroxide in sulfuric acid leads to the formation of NiSO4. This method is suitable when you desire to use nickel hydroxide as the precursor for nickelous sulfate synthesis.
It’s important to note that you should follow proper safety precautions during the synthesis process. This includes using appropriate protective equipment and handling procedures. Conduct the reactions in a well-ventilated area to minimize the risk of exposure to harmful fumes. Careful control of reaction parameters, such as temperature and concentration, is crucial to ensure optimal conversion and yield of nickelous sulfate.
Nickel Sulfate Uses
Nickelous sulfate has various applications across different industries. Here are some of its common uses:
- Electroplating: Electroplating processes extensively use nickelous sulfate to create a durable and corrosion-resistant coating on metal surfaces. Nickelous sulfate enhances the appearance, hardness, and resistance of objects like jewelry, automotive parts, and kitchenware.
- Catalyst: Nickelous sulfate acts as a catalyst in numerous chemical reactions, including hydrogenation and oxidation processes. Industries employ nickelous sulfate catalysts in the production of pharmaceuticals, petrochemicals, and fine chemicals.
- Batteries: Rechargeable batteries, particularly Ni-Cd and Ni-MH batteries, contain nickelous sulfate as an essential component. Nickelous sulfate facilitates electrode reactions and ensures efficient storage and release of electrical energy.
- Fertilizers: Some fertilizers utilize soluble Ni from nickelous sulfate to supply plants with essential nutrients. Nickel plays a crucial role in various metabolic processes in plants, contributing to their growth and development.
- Textiles: The textile industry uses nickelous sulfate in dyeing and printing processes to enhance color fastness and dye uptake of fabrics. Nickelous sulfate ensures vibrant and long-lasting color results.
- Pharmaceuticals: Nickelous sulfate finds application in pharmaceutical preparations, primarily for producing medicines containing Ni as an active ingredient or formulating specific Ni complexes used in medical research.
- Research and Development: Laboratories employ nickelous sulfate for various research and development purposes, including chemical synthesis, electrochemical studies, and material science investigations.
Questions:
Q: What is the formula of nickel(II) sulfate?
A: The formula of nickel(II) sulfate is NiSO4.
Q: Chromium metal is added to a solution of nickel(II) sulfate. What is the balanced chemical reaction?
A: The balanced chemical reaction is: Cr + NiSO4 -> CrSO4 + Ni.
Q: How to make nickel ammonium sulfate?
A: Nickel ammonium sulfate can be prepared by dissolving nickelous sulfate and ammonium sulfate in water, followed by crystallization.
Q: Is nickelous sulfate soluble in water?
A: Yes, nickelous sulfate is soluble in water.
Q: Who mines nickelous sulfate?
A: Nickelous sulfate is not mined directly. Ni ores are mined, and from those, nickelous sulfate can be produced.
Q: What is the name of the compound NiSO4?
A: The compound NiSO4 is called nickelous sulfate.
Q: How many grams of NiSO4 are there in 100g hydrate? How many moles?
A: The amount of NiSO4 in 100g of the hydrate would depend on the specific hydrate compound and its molar mass.
Q: Is NiSO4 soluble in water?
A: Yes, NiSO4 is soluble in water.
Q: How many grams of NiSO4 are obtained if the yield is 76.9%?
A: The grams of NiSO4 obtained would depend on the initial amount and conditions of the reaction.
Q: Is NiSO4 hazardous?
A: NiSO4 can be hazardous if not handled properly. It is important to follow safety guidelines when working with it.
Q: What is the name of the covalent compound NiSO4?
A: NiSO4 is not a covalent compound. It is an ionic compound known as nickelous sulfate.
Q: Is NiSO4 a salt?
A: Yes, NiSO4 is considered a salt due to its ionic nature and formation from the reaction between an acid (sulfuric acid) and a base (nickel hydroxide).
Q: What is the charge in NiSO4?
A: In NiSO4, the nickel ion (Ni2+) carries a positive charge of 2+, while the sulfate ion (SO4 2-) carries a negative charge of 2-.