Welcome to UNICORN CHEMICALS CO. Unicorn Chemicals Co. is a leading name in manufacturing and trading an extensive range of chemicals which find wide application in different industrial sectors. Based in Kolkata, our company was established in the year 2010. Using our wide domain expertise and in-depth market knowledge we have been able to set up an organized infrastructure and network which are aiding us to escalate our business to new heights. Our products are all manufactured using the most authentic and top quality ingredients which are formulated in their correct ratio to bring out the most desired results. All these chemicals are appreciated for their environment friendly and non-toxic nature which do not cause any adverse impact on the human body. These chemicals find effective application like dehumidification, fluid purification operations, air separation and other chemical treatment. We are backed by a team of highly qualified scientists and professionals who hold extensive insight on the specific industry. Strictly adhering to the rules and norms of the specific industry, we are producing the most authentic brands of chemicals within an affordable market rate. Our sheer dedication, ethical business policies and utmost professionalism have helped us to create a niche not only in the domestic market but we have also formed a renowned client base in the international arena.

1. Aluminium sulfate
Aluminium sulfate is a chemical compound with the formula Al2(SO4)3. It is
soluble in water and is mainly used as a flocculating agent in the purification of
drinking water[3][4] and waste water treatment plants, and also in paper
manufacturing.
Aluminium sulfate is sometimes referred to as a type of alum. Alums are double
sulfatesalts,withtheformulaAM(SO
4)2·12H 2O, where A is a monovalent cation such as potassium or ammonium
and M is a trivalent metal ion such as aluminium.[5] The anhydrous form occurs
naturally as a rare mineral millosevichite, found e.g. in volcanic environments
and on burning coal-mining waste dumps. Aluminium sulfate is rarely, if ever,
encountered as the anhydrous salt. It forms a number of different hydrates, of
which the hexadecahydrate Al2(SO4)3•16H2O and octadecahydrate
Al2(SO4)3•18H2O are the most common.The heptadecahydrate, whose formula
can be written as [Al(H2O)6]2(SO4)3•5H2O, occurs naturally as the mineral
alunogen.
Aluminium sulfate may be made by adding aluminium hydroxide, Al(OH)3, to
sulfuric acid, H2SO4:
2 Al(OH)3 + 3 H2SO4 → Al2(SO4)3+6H2O
or by heating aluminum metal in a sulfuric acid solution:
2 Al(s) + 3 H2SO4 → Al2(SO4)3 + 3 H2 (g)
Uses
Aluminium sulfate is used in water purification and as a mordant in dyeing and
printing textiles. In water purification, it causes impurities to coagulate into
larger particles and then settle to the bottom of the container (or be filtered out)
more easily. This process is called coagulation or flocculation. Research
suggests that in Australia, aluminium sulfate used this way in drinking water
treatment is the primary source of hydrogen sulfide gas in sanitary sewer
systems.[6] Improper and excess application polluted the water supply of
CamelfordinCornwall.
When dissolved in a large amount of neutral or slightly alkaline water,
aluminium sulfate produces a gelatinous precipitate of aluminium hydroxide,
Al(OH)3. In dyeing and printing cloth, the gelatinous precipitate helps the dye
adheretotheclothingfibersbyrenderingthepigmentinsoluble.

2. Aluminium sulfate is sometimes used to reduce the pH of garden soil, as it
hydrolyzes to form the aluminium hydroxide precipitate and a dilute sulfuric acid
solution. An example of what changing the pH level of soil can do to plants is
visible when looking at Hydrangea macrophylla. The gardener can add
aluminium sulfate to the soil to reduce the pH which in turn will result in the
flowers of the Hydrangea turning a different color (blue). The aluminium is what
makes the flowers blue; at a higher pH, the aluminium is not available to the
plant.Thus,boththealuminiumandsulfurkeeptheplantsblue.
Aluminium potassium sulfate and another form of alum, aluminium ammonium
sulfate, are the active ingredients in some antiperspirants; however, beginning in
2005 the US Food and DrugAdministration no longer recognized it as a wetness
reducer. Despite this, several countries, primarily in Asia, still use the widely
available and cheap alum sulfate as a very effective cure for a medical condition
known asHyperhydrosis.
Aluminiumpotassiumsulfateisusuallyfoundinbakingpowder.
In the construction industry, it is used as waterproofing agent and accelerator in
concrete.Anotheruseisafoamingagentinfirefightingfoam.
It is also used in styptic pencils, and pain relief from stings and bites.[medical
citationneeded]
Itcanalsobeveryeffectiveasamolluscicide,killingspanishslugs.
It is used in dentistry (especially in gingival retraction cords) because of its
astringentandhemostaticproperties

3. Calcium hypochlorite
Uses
Calcium hypochlorite is an inorganic compound with formula Ca(ClO)2.As
a mixture with lime and calcium chloride, it is marketed as chlorine powder
or bleach powder for water treatment and as a bleaching agent.[1] This
compound is relatively stable and has greater available chlorine than sodium
hypochlorite (liquid bleach).[2] It is a white solid, although commercial
samples appear yellow. It strongly smells of chlorine, owing to its slow
decomposition in moist air. It is not highly soluble in water and is more
preferably used in soft to medium-hard water. It has two forms: dry and
hydrated.
Sanitation
Calcium hypochlorite is commonly used to sanitize public swimming pools
and disinfect drinking water. Generally the commercial substance is sold
with a purity of a 68% (with other additives and contaminants varying based
upon the product's intended purpose). For instance as a swimming pool
chemical it is often mixed with cyanuric acid stabilizers and anti-scaling
agents (in order to reduce the loss of chlorine from ultraviolet radiation and
to prevent calcium hardening). Calcium hypochlorite is also used in
kitchens to disinfect surfaces and equipment.[3] Other common uses
include bathroom cleansers, household disinfectant sprays, algaecides,
herbicides,andlaundrydetergents.
Organicchemistry
Calcium hypochlorite is a general oxidizing agent and therefore finds some
use in organic chemistry.[4] For instance the compound is used to cleave
glycols, α-hydroxy carboxylic acids and keto acids to yield fragmented
aldehydes or carboxylic acids.[5] Calcium hypochlorite can also be used in
thehaloformreactiontomanufacturechloroform.m
the
acid is
ypochlorite
njugate
form

4. Production
Calcium oxychloride is produced industrially by treating lime
(Ca(OH)2) with chlorine gas. The reaction can be conducted in stages to
give various compositions, each with different concentration of calcium
hypochlorite, together with unconverted lime and calcium chloride. The
fullconversionisshown[1]
2Cl
2+2Ca(OH)
2→Ca(OCl)
2+CaCl
2+2H 2O
Bleaching powder is not a simple mixture of calcium hypochlorite,
calcium chloride, and calcium hydroxide. Instead, it is a mixture
consisting principally of calcium hypochlorite Ca(OCl)2, dibasic
calcium hypochlorite, Ca3(OCl)2(OH)4, and dibasic calcium chloride,
Ca3Cl2(OH)4.[7]Itismadefromslightlymoistslakedlime.
Safety
Calcium hypochlorite is stored dry and cold, away from any organic
material and metals. The hydrated form is safer to handle.

5. Sulfuric acid
Sulfuric acid (alternative spelling sulphuric acid) is a highly corrosive strong
mineral acid with the molecular formula H2SO4 and molecular weight
98.079 g/mol. It is a pungent-ethereal, colorless to slightly yellow viscous
liquid that is soluble in water at all concentrations.[6] Sometimes, it is dyed
dark brown during production to alert people to its hazards.[7] The historical
nameofthisacidisoilofvitriol.[8]
Sulfuric acid is a diprotic acid and shows different properties depending upon
its concentration. Its corrosiveness on other materials, like metals, living
tissues or even stones, can be mainly ascribed to its strong acidic nature and, if
concentrated, strong dehydrating and oxidizing properties. Sulfuric acid at a
high concentration can cause very serious damage upon contact, since not
only does it cause chemical burns via hydrolysis, but also secondary thermal
burns through dehydration.[9][10] It can lead to permanent blindness if
splashed onto eyes and irreversible damage if swallowed.[9] Accordingly,
safety precautions should be strictly observed when handling it. Moreover, it
ishygroscopic,readilyabsorbingwatervapourfromtheair.[6]
Sulfuric acid has a wide range of applications including in domestic acidic
drain cleaners,[11] as an electrolyte in lead-acid batteries and in various
cleaning agents. It is also a central substance in the chemical industry.
Principal uses include mineral processing, fertilizer manufacturing, oil
refining, wastewater processing, and chemical synthesis. It is widely
produced with different methods, such as contact process, wet sulfuric acid
process,leadchamberprocessandsomeothermethods.
Uses
Sulfuric acid is a very important commodity chemical, and indeed, a nation's
sulfuric acid production is a good indicator of its industrial strength.[27]
World production in 2004 was about 180 million tonnes, with the following
geographic distribution:Asia 35%, NorthAmerica (including Mexico) 24%,
Africa 11%,Western Europe 10%, Eastern Europe and Russia 10%,Australia
and Oceania 7%, South America 7%.[28] Most of this amount (~60%) is
consumed for fertilizers, particularly superphosphates, ammonium
phosphate and ammonium sulfates. About 20% is used in chemical industry
for production of detergents, synthetic resins, dyestuffs, pharmaceuticals,
petroleum catalysts, insecticides and antifreeze, as well as in various
processes such as oil well acidicizing, aluminium reduction, paper sizing,
water treatment.About 6% of uses are related to pigments and include paints,
enamels, printing inks, coated fabrics and paper, and the rest is dispersed into
a multitude of applications such as production of explosives, cellophane,
acetateandviscosetextiles,lubricants,non-ferrousmetalsandbatteries.

6. The study of vitriol, a category of glassy minerals from which the acid can be
derived, began in ancient times. Sumerians had a list of types of vitriol that
they classified according to the substances' color. Some of the earliest
discussions on the origin and properties of vitriol is in the works of the Greek
physician Dioscorides (first centuryAD) and the Roman naturalist Pliny the
Elder (23–79 AD). Galen also discussed its medical use. Metallurgical uses
for vitriolic substances were recorded in the Hellenistic alchemical works of
Zosimos of Panopolis, in the treatise Phisica et Mystica, and the Leyden
papyrusX.
Persian alchemists Jābir ibn Hayyān (c. 721 – c. 815 AD, also known as
Geber), Razi (865 – 925 AD), and Jamal Din al-Watwat (d. 1318, wrote the
book Mabāhij al-fikar wa-manāhij al-'ibar), included vitriol in their mineral
classification lists. Ibn Sina focused on its medical uses and different
varietiesofvitriol.
Sulfuric acid was called "oil of vitriol" by medieval European alchemists
because it was prepared by roasting "green vitriol" (iron (II) sulfate) in an
iron retort. There are references to it in the works of Vincent of Beauvais and
in the Compositum de Compositis ascribed to Saint Albertus Magnus. A
passage from Pseudo-Geber´s Summa Perfectionis was long considered to
bethefirstrecipeforsulfuricacid,butthiswas amisinterpretation.
In the seventeenth century, the German-Dutch chemist Johann Glauber
prepared sulfuric acid by burning sulfur together with saltpeter (potassium
nitrate,KNO
3), in thepresenceof steam.As saltpeterdecomposes,itoxidizesthesulfur to
SO
3, which combines with water to produce sulfuric acid. In 1736, Joshua
Ward, a London pharmacist, used this method to begin the first large-scale
productionofsulfuricacid.
In 1746 in Birmingham, John Roebuck adapted this method to produce
sulfuric acid in lead-lined chambers, which were stronger, less expensive,
and could be made larger than the previously used glass containers. This
process allowed the effective industrialization of sulfuric acid production.
After several refinements, this method, called the lead chamber process or
"chamber process", remained the standard for sulfuric acid production for
almosttwocenturies.[2]

7. Hydrochloric acid
Hydrochloric acid is a clear, colorless, highly pungent solution of hydrogen
chloride (HCl) in water. It is a highly corrosive, strong mineral acid with many
industrial uses. Hydrochloric acid is found naturally in gastric acid. When it
reactswithanorganicbaseitformsahydrochloridesalt.
It was historicallycalled acidum salis, muriaticacid, and spirits of salt because it
was produced from rock salt and green vitriol (by BasiliusValentinus in the 15th
century) and later from the chemically similar common salt and sulfuric acid
(by Johann Rudolph Glauber in the 17th century). Free hydrochloric acid was
first formally described in the 16th century by Libavius. Later, it was used by
chemistssuchasGlauber,Priestley, andDavyintheirscientificresearch.
With major production starting in the Industrial Revolution, hydrochloric acid
is used in the chemical industry as a chemical reagent in the large-scale
production of vinyl chloride for PVC plastic, and MDI/TDI for polyurethane. It
has numerous smaller-scale applications, including household cleaning,
production of gelatin and other food additives, descaling, and leather
processing. About 20 million tonnes of hydrochloric acid are produced
worldwideannually.
a mixture consisting of hydrochloric and nitric acids, prepared by dissolving sal
ammoniac in nitric acid, was described in the works of Pseudo-Geber, a 13th-
century European alchemist. Other references suggest that the first mention of
aquaregiaisinByzantinemanuscriptsdatingtotheendof the13thcentury.
Free hydrochloric acid was first formally described in the 16th century by
Libavius, who prepared it by heating salt in clay crucibles. Other authors claim
that pure hydrochloric acid was first discovered by the German Benedictine
monk Basil Valentine in the 15th century, when he heated common salt and
green vitriol, whereas others argue that there is no clear reference to the
preparationofpurehydrochloricaciduntiltheendofthe16thcentury.
In the 17th century, Johann Rudolf Glauber from Karlstadt am Main, Germany
used sodium chloride salt and sulfuric acid for the preparation of sodium sulfate
in the Mannheim process, releasing hydrogen chloride gas. Joseph Priestley of
Leeds, England prepared pure hydrogen chloride in 1772, and by 1808
Humphry Davy of Penzance, England had proved that the chemical
compositionincludedhydrogenandchlorine.
History

8. During the Industrial Revolution in Europe, demand for alkaline substances
increased. A new industrial process developed by Nicolas Leblanc of Issoundun,
France enabled cheap large-scale production of sodium carbonate (soda ash). In
this Leblanc process, common salt is converted to soda ash, using sulfuric acid,
limestone, and coal, releasing hydrogen chloride as a by-product. Until the British
Alkali Act 1863 and similar legislation in other countries, the excess HCl was
vented into the air.After the passage of the act, soda ash producers were obliged to
absorbthewastegasinwater, producinghydrochloricacidonanindustrialscale.
In the 20th century, the Leblanc process was effectively replaced by the Solvay
process without a hydrochloric acid by-product. Since hydrochloric acid was
already fully settled as an important chemical in numerous applications, the
commercial interest initiated other production methods, some of which are still
used today. After the year 2000, hydrochloric acid is mostly made by absorbing
by-producthydrogenchloridefromindustrialorganiccompoundsproduction.
Since 1988, hydrochloric acid has been listed as a Table II precursor under the
1988 United Nations Convention Against Illicit Traffic in Narcotic Drugs and
Psychotropic Substances because of its use in the production of heroin, cocaine,
andmethamphetamine.
Hydrochloric acid is a strong inorganic acid that is used in many industrial
processes such as refining metal. The application often determines the required
productquality.
Applications