Introduction
Nickel Sulfate is a crystalline inorganic compound that is yellow, green or blue coloured and produces toxic gasses upon heating. It is used in electroplating and as a chemical intermediate to produce other types of nickel compounds. Nickel Sulfate is a by-product of copper refining and it naturally occurs as a rare mineral which is retgersite. Retgersite is a type of chemical that is useful in utensils, jewellery, coins, metal buttons, and eyeglasses. Nickel Sulfate is also used for making paper clips, keys, enamel dyes, and electrical wiring. Nickel Sulfate hexahydrate is also known as blue salt. And it may be produced by the dissolution of nickel metal or nickel oxides in the sulfuric acid.
What is Nickel Sulfate?
Nickel sulfate or Nickel (II) sulfate is an inorganic compound. It is highly soluble in aqueous solutions.
This sulfate compound is a green coloured salt or ester of sulphuric acid.
It is formed by replacing one or both hydrogen atoms with Nickel (metal) atoms.
The chemical formula for Nickel Sulfate is NiSO4.
Nickel (II) Sulfate is available naturally in the form of mineral morenosite. It is usually unstable in the air.
It is also called,
Nickel (II) Sulfate,
Nickel monosulphate,
Nickelous Sulfate.
Nickel Sulfate hexahydrate.
Nickel (2+) Sulfate.
Nickel Sulfate can be formed in laboratories by dissolving Nickel oxide in Sulphuric acid. The reaction gives a concentrated solution of Nickel Sulfate Heptahydrate. On heating the concentrated solution, crystalline Nickel Sulfate hexahydrate is derived for commercial use.
It is a carcinogenic compound as exposure to its fumes can cause cancer.
Production of Nickel Sulfate
The production of Nickel Sulfate includes: It is made by dissolving nickel oxide in hot, dilute sulfuric acid. Nickel is basically delivered in a sealed reactor, with a sulphuric acid solution. This sealed reactor is then filled with oxygen. The temperature and the amount of pressure in the sealed reactor are kept constant during the whole operation. The oxidation process produces concentrated Nickel Sulfate solution in an enclosed environment. After heating and increasing the pressure in the sealed reactor, it results in the formation of blue crystalline Nickel Sulfate. The impurities of it are then removed from the crystals by treating them with a diluted solution of Barium carbonate. And this whole method is widely used to produce Nickel Sulfate in large quantities.
The Nickel Sulfate is usually prepared by dissolving nickel oxide into hot, dilute Sulphuric acid. The general steps involved in the process are,
The metal, Nickel, is supplied in an enclosed reactor along with Sulphuric acid solution.
Oxygen is introduced into the reactor.
During this process, temperature and pressure in the reactor are kept constant.
In an enclosed environment, the chemical process (oxidation) gives rise to concentrated Nickel Sulfate solution.
On further heating and increasing the pressure in the reactor, blue crystalline Nickel Sulfate is formed.
By treating the crystals with a diluted solution of Barium carbonate, elimination of impurities takes place.
This process is widely used for the mass production of Nickel Sulfate.
Physical Properties of NiSO4
It occurs in yellow solid when in anhydrous form, green-blue crystals when in heptahydrate form and in blue crystals when in hexahydrate state.
It is odourless.
Its molecular weight is 154.75 g/mol.
It is having a density of 3.68 g/cm3
Its boiling point is 840 °C
Its Melting point is > 100 °C in an anhydrous state and >53 °C for hexahydrate form.
The linear chemical formula is given as NiSO4(H2O)6.
It is soluble in water and methanol. Solubility in water is 293 g/L at 0°C.
Its CAS registration number is 7786-81-4.
Though it has a sweet, astringent taste, it is recommended not to taste.
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Nickel Sulfate is a yellow solid when it is anhydrous, Nickel Sulfate is a green-blue crystal when it is heptahydrate, and Nickel Sulfate is a blue crystal when it is hexahydrate.
Nickel Sulfate’s weight is 3.68 g/cm3 and its density is 3.68 g/cm3.
Nickel Sulfate’s molecular mass is 154.75 g/mol.
Nickel Sulfate’s boiling point is 840 degrees Celsius.
Nickel Sulfate is odourless.
Nickel Sulfate’s melting point is more than 100 °C in anhydrous form and more than 53 °C in hexahydrate form.
Chemical Properties of NiSO4
It is non-flammable.
It is insoluble in alcohol and ether.
It is not compatible with strong acids.
After dissolving in water, it forms an acidic corrosive solution. On corrosion, it emits fumes of oxides of sulfur.
When it is dissolved in water, and the solution is heated to decompose, it liberates fumes of nitrous oxide. Fumes of Nickel Sulphate are highly toxic.
As its aqueous solution is acidic, the pH value is 4.5.
On heating at 103°C, aqueous Nickel Sulfate loses the water molecules. And heating up to 848°C, the anhydrous form decomposes to form sulfur trioxide and nickel oxide. The chemical expression is
\[ NiSO_{4} \rightarrow NiO + SO_{3} \]
Nickel Sulfate gives double by-products of salts on reacting with alkali metals or ammonium sulfates. These sulfates are isomorphous.
Reacting with hydrochloric acid gives Sulphuric acid and Nickel Chloride. The chemical reaction is as shown,
\[ NiSO_{4} + HCl \rightarrow NiCl + HSO_{4} \]
While reacting with sodium hydroxide, it forms Sodium Sulfate and Nickel hydroxide. The chemical equation is
\[ NiSO_{4} + NaOH \rightarrow Ni(OH)_{2} + Na_{2}SO_{4} \]
Nickel Sulfate is non-combustible.
Nickel Sulfate has a pH value of 4.5 because its aqueous solution is of acidic nature.
Nickel Sulfate is incompatible with strong acids.
Nickel Sulfate generates an acidic corrosive solution when dissolving in water, producing sulfur dioxide emissions when it corrodes.
Alcohol and ether do not dissolve in Nickel Sulfate.
Nickel Sulfate is dissolved in water and the solution is heated to decompose, nitrous oxide emissions are released and its fumes are extremely poisonous.
Uses of Nickel Sulfate
Nickel Sulfate is widely used
As the electrolyte for surface finishing processes of metals such as metal plating and electrorefining.
In the preparations of many Nickel catalysts and compounds.
As a reducing agent for flashing on steel surfaces, imparting Nickel coating from the surface.
For blackening Brass and Zinc.
As a mordant in dyeing and printing metals, textiles and ceramics.
As a coating for many metals.
In the production of driers that are used in protective shields.
They are occasionally used as calibrants to measure magnetic susceptibility.
Nickel sulfate is used as an electrolyte in metal surface finishing operations like plating and electrorefining.
Nickel sulfate is also used as a protective layer for a variety of metals.
Different types of Nickel catalysts and compounds are made by this process.
Brass and zinc can be blackened with Nickel sulfate.
Various Metals, fabrics, and pottery are dyed and printed with Nickel sulfate as a mordant.
Nickel sulfate is used as a flashing reducer on steel surfaces, providing a nickel covering to the surface.
Effects of NiSO4 on Human Health
Nickel Sulfate can be assimilated into the human body by inhalation or ingestion. Once it is absorbed in the body, it concentrates in the lungs, gut, kidneys and liver. Exposure to NiSO4 causes :
Skin irritations
Giddiness
Lassitude
Headache
Myalgia
Gastrointestinal effects such as abdominal pain, nausea, vomiting, diarrhoea
Hemorrhagic gastritis
Transient hyperbilirubinemia and albuminuria
Bronchial asthma
Dyspnoea
Mild cyanosis
Chronic obstructive airways syndrome
Chronic urticaria
Dermatitis
Effects of Nickel Sulfate
Effects of Nickel Sulfate Include: Nickel sulfate can be incorporated into the human body by inhaling or ingesting it. Nickel sulfate concentrates in the lungs, intestines, kidneys, and liver once it is taken into the body. Nickel sulfate causes poisoning by being exposed to it. Nickel Sulfate causes Chronic obstructive pulmonary disease, Dyspnoea, Mild cyanosis, Chronic urticaria, Dermatitis. Nickel Sulfate also causes Irritation of the skin, giddiness, lassitude, headache, myalgia, abdominal pain, nausea, vomiting, diarrhoea, hemorrhagic gastritis, transient hyperbilirubinemia, and albuminuria are some of the gastrointestinal side effects.
FAQs on Nickel Sulfate
1. What are the safety and packaging specifications while handling NiSO4?
While treating Nickel Sulphate, toxic fumes and heat are generated. It has hazardous effects on health. To avoid its adverse effects on health, it should be handled, packed and shipped cautiously. Following are the Safety measures while handling NiSO4,
Proper training should be given before handling NiSO4.
The area where treatment, storage of NiSO4 is going to take place should be marked and isolated from other activities.
As it is not compatible with oxidising agents, it should not be treated or kept near them.
Use masks, gloves, goggles and aprons while handling NiSO4.
In case containers catch fire, use a fire extinguisher and use water sprays to keep them cool.
For storage and shipping of Nickel Sulphate cold, tightly closed, made up of antioxidant material containers should be used.
2. How to dispose of nickel sulphate waste?
As Nickel Sulphate is a carcinogenic compound, it can not be disposed of in water drains. Following methods are used to dispose of,
It can be destroyed by introducing into the strong solution of sodium dichromate and sulphuric acid. It takes one to two days to destroy Nickel Sulphate completely. The residue is later flushed with a large amount of water to the sewer.
Another method to destroy it is by reacting it with nucleophiles such as ammonia, thiosulphate and hydroxyl ions. Dissolving Nickel Sulphate in ethanol before the treatment accelerates the process.
By adding a saturated solution of potassium permanganate with acetone destroys Nickel Sulphate.
Potassium hydroxide dissolved in methanol destroys NiSO4.
By using sodium dichromate and sulphuric acid solution, Nickel Sulphate is decomposed. Further, the waste is disposed of in a large water body.
3. Is nickel sulfate harmful?
Nickel Sulfate basically is a crystalline inorganic compound. Nickel Sulfate acts as a by-product of copper refining. It naturally occurs as a rare mineral which is retgersite. Nickel Sulfate is a Carcinogen, so it is always suggested to handle it with extreme caution. Nickel sulfate also includes causes related to male infertility and testicular damage. While coming in contact with the skin and eyes Nickel sulfate might irritate and burn them. Inhalation of Nickel sulfate can irritate the nose, throat, and lungs, resulting in cough, mucus, and shortness of breath.
4. What are the physical properties of Nickel Sulfate?
The physical properties of Nickel Sulfates includes :
Nickel Sulfate’s boiling point is 840 degrees Celsius.
Nickel Sulfate is odourless.
Nickel Sulfate’s melting point is more than 100 °C in anhydrous form and more than 53 °C in hexahydrate form.
Nickel Sulfate is water and methanol soluble. It is 0°C, solubility in water is 293 g/L.
The CAS number for Nickel Sulfate is 7786-81-4.
5. How is the Nickel Sulfate prepared?
Nickel Sulfate is prepared by several methods. Scientists prepare Nickel Sulfate by dissolving nickel metal, its oxide, or its carbonate in sulfuric acid. In this method, powdered metal or black nickel oxide is added to hot dilute sulfuric acid, or nickel carbonate is added to dilute sulfuric acid.
The equations are:
\[ NiO + H_{2}SO_{4} \rightarrow NiSO_{4}+ H_{2}O \]
And,
\[ NiCO_{3} + H_{2}SO_{4} \rightarrow NiSO_{4} + CO_{2} + H_{2}O \]
\[ Ni(CO)_{4} + SO_{2} + O_{2} \rightarrow NiSO_{4} + 4CO \]
6. What are the Chemical properties of Nickel Sulfate?
The chemical properties of Nickel Sulfate include:
When Aqueous Nickel Sulfate is heated to 103°C, it loses water molecules and the anhydrous form, when heated to 848°C, decomposes to form sulfur trioxide and nickel oxide when. Its chemical formula is :
\[ NiSO_{4} \rightarrow NiO + SO_{3} \]
When reacting with hydrochloric acid, Sulphuric acid and Nickel Chloride are produced. Its chemical reaction is :
\[NiSO_{4} + HCl \rightarrow NiCl + HSO_{3} \]
If Nickel sulfate reacts with alkali metals or ammonium sulfates, two salt by-products are produced and these sulfates are identical in nature.
When reacted with sodium hydroxide, it produces sodium sulfate and nickel hydroxide. Its chemical formula is :
\[ NiSO_{4} + NaOH \rightarrow Ni(OH)_{2} + Na_{2}SO_{4} \]
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