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Yemelyan Rodionov
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Where Do You Buy Sulfuric Acid

Introducing our premium-grade sulfuric acid 96%, the perfect solution for a wide range of industrial applications. Sulfuric acid, also known as oil of vitriol, is a highly corrosive, dense, and oily liquid that is widely used in various industries. Our sulfuric acid is of the highest quality and purity, making it an ideal choice for use in chemical processing, mining, and other applications. One of the key benefits of our sulfuric acid is its exceptional chemical properties. It is an extremely strong acid, capable of dissolving a wide range of substances, including metals, minerals, and organic compounds. This makes it an invaluable tool in many industrial processes, such as the production of fertilizers, dyes, and detergents. Our sulfuric acid is also highly versatile, and can be used in a range of applications. It is commonly used as a catalyst in chemical reactions, and can also be used to remove rust and scale from metals. Additionally, it is used in the petroleum industry to refine crude oil into gasoline, diesel fuel, and other products. Another key benefit of our sulfuric acid is its high purity. We use only the finest raw materials and employ state-of-the-art manufacturing processes to ensure that our product meets the strictest quality standards. This ensures that our sulfuric acid is free from impurities that could compromise its effectiveness or safety. We understand that every customer has unique needs and requirements, which is why we offer a range of packaging options to suit your specific needs. From bulk tankers to 55-gallon drums and smaller quantities, we can provide the right packaging solution for your business. In addition to its industrial applications, our sulfuric acid is also used in a variety of other applications. For example, it is commonly used in the production of batteries, where it plays a key role in the chemical reactions that power these devices. It is also used in the production of textiles, where it is used to remove impurities from fabrics and to create dyes. Despite its powerful chemical properties, our sulfuric acid is safe to use when handled and stored correctly. We provide detailed safety information and guidelines to ensure that our customers can use our product safely and effectively. In conclusion, our sulfuric acid 96% is a versatile, high-quality acid that is perfect for a wide range of industrial and other applications. Whether you are in the chemical industry, mining, or producing batteries or textiles, our sulfuric acid is the perfect choice for your business. With our commitment to quality and customer service, you can be confident that you are getting the best product on the market.

where do you buy sulfuric acid

Sulfuric acid (American spelling and the preferred IUPAC name) or sulphuric acid (Commonwealth spelling), known in antiquity as oil of vitriol, is a mineral acid composed of the elements sulfur, oxygen, and hydrogen, with the molecular formula H2SO4. It is a colorless, odorless, and viscous liquid that is miscible with water.[6]

Pure sulfuric acid does not occur naturally due to its strong affinity to water vapor; it is hygroscopic and readily absorbs water vapor from the air.[6] Concentrated sulfuric acid is highly corrosive towards other materials, from rocks to metals, since it is an oxidant with powerful dehydrating properties. Phosphorus pentoxide is a notable exception in that it is not dehydrated by sulfuric acid but, to the contrary, dehydrates sulfuric acid to sulfur trioxide. Upon addition of sulfuric acid to water, a considerable amount of heat is released; thus, the reverse procedure of adding water to the acid should not be performed since the heat released may boil the solution, spraying droplets of hot acid during the process. Upon contact with body tissue, sulfuric acid can cause severe acidic chemical burns and even secondary thermal burns due to dehydration.[7][8] Dilute sulfuric acid is substantially less hazardous without the oxidative and dehydrating properties; however, it should still be handled with care for its acidity.

Sulfuric acid is a very important commodity chemical; a country's sulfuric acid production is a good indicator of its industrial strength.[9][non-primary source needed] It is widely produced with different methods, such as contact process, wet sulfuric acid process, lead chamber process, and some other methods.[which?][10] Sulfuric acid is also a key substance in the chemical industry. It is most commonly used in fertilizer manufacture[11] but is also important in mineral processing, oil refining, wastewater processing, and chemical synthesis. It has a wide range of end applications, including in domestic acidic drain cleaners,[12] as an electrolyte in lead-acid batteries, in dehydrating a compound, and in various cleaning agents.Sulfuric acid can be obtained by dissolving sulfur trioxide in water.

Although nearly 100% sulfuric acid solutions can be made, the subsequent loss of SO3 at the boiling point brings the concentration to 98.3% acid. The 98.3% grade is more stable in storage, and is the usual form of what is described as "concentrated sulfuric acid". Other concentrations are used for different purposes. Some common concentrations are:[13][14]

In the solid state, sulfuric acid is a molecular solid that forms monoclinic crystals with nearly trigonal lattice parameters. The structure consists of layers parallel to the (010) plane, in which each molecule is connected by hydrogen bonds to two others.[3] Hydrates H2SO4nH2O are known for n = 1, 2, 3, 4, 6.5, and 8, although most intermediate hydrates are stable against disproportionation.[18]

Because the hydration reaction of sulfuric acid is highly exothermic, dilution should be performed by adding the acid to the water rather than the water to the acid, to avoid acid splashing.[19] Because the reaction favors the rapid protonation of water, addition of acid to the water ensures that the acid is the limiting reagent. This reaction may be thought of as the formation of hydronium ions:

Concentrated sulfuric acid has a powerful dehydrating property, removing water (H2O) from other chemical compounds such as table sugar (sucrose) and other carbohydrates, to produce carbon, steam, and heat. Dehydration of table sugar (sucrose) is a common laboratory demonstration.[21] The sugar darkens as carbon is formed, and a rigid column of black, porous carbon called a carbon snake may emerge[22] as shown in the figure.

Similarly, mixing starch into concentrated sulfuric acid gives elemental carbon and water that is absorbed by the sulfuric acid, slightly diluting it. The effect of this can be seen when concentrated sulfuric acid is spilled on paper, which is composed of cellulose; the cellulose reacts to give a burnt appearance in which the carbon appears much like soot that results from fire.Although less dramatic, the action of the acid on cotton, even in diluted form, destroys the fabric.

As an acid, sulfuric acid reacts with most bases to give the corresponding sulfate. For example, the blue copper salt copper(II) sulfate, commonly used for electroplating and as a fungicide, is prepared by the reaction of copper(II) oxide with sulfuric acid:

Similarly, reacting sulfuric acid with potassium nitrate can be used to produce nitric acid and a precipitate of potassium bisulfate. When combined with nitric acid, sulfuric acid acts both as an acid and a dehydrating agent, forming the nitronium ion NO+2, which is important in nitration reactions involving electrophilic aromatic substitution. This type of reaction, where protonation occurs on an oxygen atom, is important in many organic chemistry reactions, such as Fischer esterification and dehydration of alcohols.

Even dilute sulfuric acid reacts with many metals via a single displacement reaction, like other typical acids, producing hydrogen gas and salts (the metal sulfate). It attacks reactive metals (metals at positions above copper in the reactivity series) such as iron, aluminium, zinc, manganese, magnesium, and nickel.

Sulfuric acid is formed naturally by the oxidation of sulfide minerals, such as iron sulfide. The resulting water can be highly acidic and is called acid mine drainage (AMD) or acid rock drainage (ARD). This acidic water is capable of dissolving metals present in sulfide ores, which results in brightly colored, toxic solutions. The oxidation of pyrite (iron sulfide) by molecular oxygen produces iron(II), or Fe2+:

ARD can also produce sulfuric acid at a slower rate, so that the acid neutralizing capacity (ANC) of the aquifer can neutralize the produced acid. In such cases, the total dissolved solids (TDS) concentration of the water can be increased from the dissolution of minerals from the acid-neutralization reaction with the minerals.

In the stratosphere, the atmosphere's second layer that is generally between 10 and 50 km above Earth's surface, sulfuric acid is formed by the oxidation of volcanic sulfur dioxide by the hydroxyl radical:[27]

Because sulfuric acid reaches supersaturation in the stratosphere, it can nucleate aerosol particles and provide a surface for aerosol growth via condensation and coagulation with other water-sulfuric acid aerosols. This results in the stratospheric aerosol layer.[27]

The permanent Venusian clouds produce a concentrated acid rain, as the clouds in the atmosphere of Earth produce water rain.[28] Jupiter's moon Europa is also thought to have an atmosphere containing sulfuric acid hydrates.[29]

Directly dissolving SO3 in water, called the "wet sulfuric acid process", is rarely practiced because the reaction is extremely exothermic, resulting in a hot aerosol of sulfuric acid that requires condensation and separation.

A method that is the less well-known is the metabisulfite method, in which metabisulfite is placed at the bottom of a beaker and 12.6 molar concentration hydrochloric acid is added. The resulting gas is bubbled through nitric acid, which will release brown/red vapors of nitrogen dioxide as the reaction proceeds. The completion of the reaction is indicated by the ceasing of the fumes. This method does not produce an inseparable mist, which is quite convenient. 041b061a72


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