Sulfuric acid (H2SO4) or oil of vitriol is a highly corrosive and strong mineral acid commonly used in various industrial processes such as fertilizer production, oil refining, and metal treatment. It is also a strong dehydrating agent.
| IUPAC Name | Sulphuric Acid |
| Molecular Formula | H2SO4 |
| CAS Number | 7664-93-9 |
| Synonyms | Oil of Vitriol, Sulfuric Acid Anhydride, Bisulfuric Acid |
| InChI | InChI=1S/H2O4S/c2-1(3)4/h(H2,2,3,4)/p-1 |
Sulfuric Acid Properties
Sulfuric Acid formula
The chemical formula of sulfuric acid is H2SO4, which represents two hydrogen atoms, one sulfur atom, and four oxygen atoms. This formula represents the composition of the sulfuric acid molecule and its chemical structure.
Sulfuric Acid molar mass
The molar mass of sulfuric acid is 98.08 g/mol. It is calculated by adding up the atomic masses of each element in the chemical formula of sulfuric acid (H2SO4).
Sulfuric Acid boiling point
Sulphuric acid has a boiling point of 337.1°C. At this temperature, the vapor pressure of the liquid reaches the atmospheric pressure and it begins to boil.
Sulfuric Acid melting point
The melting point of sulphuric acid is 10.4°C. It is a highly viscous liquid at room temperature, but can freeze to form a solid state at lower temperatures.
Sulfuric Acid density g/ml
The density of sulphuric acid ranges from 1.84 g/mL to 1.93 g/mL, depending on its concentration. As the concentration of sulphuric acid increases, its density also increases.
Sulfuric Acid molecular weight
The molecular weight of sulphuric acid is 98.08 g/mol. It is calculated by adding up the atomic masses of each element in its chemical formula (H2SO4).
Sulfuric Acid Structure
The sulphuric acid molecule consists of two hydrogen atoms (H) bonded to a sulfur atom (S) that is also bonded to four oxygen atoms (O). It has a tetrahedral molecular geometry and is a strong dehydrating agent.
| Appearance | Clear, colorless, oily liquid |
| Specific Gravity | 1.84 (water = 1) |
| Color | Colorless |
| Odor | Pungent, sulfurous odor |
| Molar Mass | 98.079 g/mol |
| Density | 1.835 g/mL |
| Melting Point | 10.5°C |
| Boiling Point | 337°C |
| Flash Point | 140°F (60°C) |
| Water Solubility | Completely miscible |
| Solubility | Soluble in water and alcohol |
| Vapour Pressure | 40 mmHg (20°C) |
| Vapour Density | 2.5 (air = 1) |
| pKa | -3 |
| pH | Less than 1 (strongly acidic) |
Sulfuric Acid Safety and Hazards
Sulfuric acid is a highly corrosive and hazardous substance. Contact with skin and eyes can cause severe burns and blindness. Inhalation of its fumes can irritate the respiratory system and cause coughing, wheezing, and shortness of breath. It is flammable and reactive, and should be handled with caution in a well-ventilated area, using protective equipment such as gloves and eye protection. Spills should be cleaned up immediately to prevent damage to surfaces and potential harm to individuals. Proper storage and labeling is necessary to ensure safe handling.
| Hazard Symbols | Corrosive, Irritant, Harmful |
| Safety Description | Keep away from heat/sparks/open flames/hot surfaces. No smoking. Store in a well-ventilated place. Keep container tightly closed. Wear protective gloves/protective clothing/eye protection/face protection. |
| UN IDs | UN1830 |
| HS Code | 2815.11.00 |
| Hazard Class | 8 |
| Packing Group | II |
| Toxicity | Oral: LD50 = 1.2 g/kg (Rat) |
Sulfuric Acid Synthesis Methods
H2SO4 can be synthesized through several methods, including the Contact Process and the Lead Chamber Process.
The Contact Process is the most widely used method for the industrial production of sulphuric acid, which involves the oxidation of sulfur dioxide to sulfur trioxide and then the reaction of sulfur trioxide with water to produce H2SO4.
The Lead Chamber Process, on the other hand, involves the oxidation of sulfur dioxide with nitrogen dioxide in the presence of a catalyst, typically lead dioxide, and then the reaction of the resulting sulfur trioxide with water. Both methods produce H2SO4 with varying levels of purity and concentration, which can be further purified and concentrated as needed.
Sulfuric Acid Uses
H2SO4 is a versatile and widely used chemical in various industries. People commonly use sulphuric acid in the production of fertilizers, detergents, dyes, and pigments. It also plays a role in refining petroleum products, processing minerals and ores, and producing chemicals such as nitric acid and sulfates. Laboratories use H2SO4 as a reagent, and it serves as a catalyst in chemical reactions. Lead-acid batteries use sulphuric acid as an electrolyte, and steel workers use it for pickling to remove rust and scale before plating or painting.
Overall, H2SO4 plays a crucial role in many industrial processes, making it one of the most important chemicals in the world.
Questions:
Is sulfuric acid a strong acid?
Yes, H2SO4 is a strong acid. A strong acid is one that completely dissociates in water to produce hydrogen ions (H+), meaning it donates all of its hydrogen ions to the solution. Considered one of the strongest acids, sulphuric acid boasts a high level of acidity, making it highly reactive and corrosive. To prevent harm to people and the environment, proper handling and storage of sulphuric acid is a must.
What is sulfuric acid used for?
Sulphuric acid is widely used in a variety of industries and applications. Some of the most common uses of H2SO4 include:
- Fertilizer production: sulphuric acid is used in the production of phosphoric acid, which is a key component of many fertilizers.
- Petroleum refining: sulphuric acid is used to remove impurities such as sulfur compounds from crude oil during the refining process.
- Metal processing: sulphuric acid is used in metal processing to remove rust and scale from iron and steel, as well as to refine metal ores.
- Manufacturing: sulphuric acid is used in the production of a variety of products, including detergents, dyes, pigments, and other chemicals.
- Automotive batteries: sulphuric acid is used as the electrolyte in lead-acid batteries, which are commonly used in cars and other vehicles.
- Laboratory reagent: sulphuric acid is commonly used as a laboratory reagent due to its high level of reactivity and ability to dissolve many substances.
What type of acid is sulfuric acid?
H2SO4 is a strong inorganic acid. Classified as a diprotic acid, H2SO4 donates two hydrogen ions (H+) to a solution, making it a strong mineral acid. With its highly reactive and corrosive nature, caution must be taken when handling and storing H2SO4 to prevent harm to people and the environment. Industries use sulphuric acid widely in their processes, including the production of fertilizers, detergents, dyes, pigments, and other chemicals, as well as in refining petroleum products and processing metal ores.
What is the formula for sulfuric acid?
The chemical formula for sulfuric acid is H2SO4.
What is oil of vitriol?
Oil of vitriol is another term for sulphuric acid, a strong and highly corrosive chemical. It is commonly used in the production of fertilizers, detergents, and dyes, as well as in the refining of petroleum and the processing of other chemicals.