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BARIUM CARBONATE

EC / List no.: 208-167-3
CAS no.: 513-77-9
Mol. formula: CH2O3.Ba

Barium carbonate is the inorganic compound with the formula BaCO3.
Like most alkaline earth metal carbonates, it is a white salt that is poorly soluble in water.
Barium carbonate occurs as the mineral known as witherite.
In a commercial sense, it is one of the most important barium compounds.

Preparation
Barium carbonate is made commercially from barium sulfide with by treatment with sodium carbonate at 60 to 70 °C (soda ash method) or, more commonly carbon dioxide at 40 to 90 °C:

In the soda ash process, an aqueous solution of barium sulfide is treated with sodium carbonate:

BaS + H2O + CO2 → BaCO3 + H2S
Reactions
Barium carbonate reacts with acids such as hydrochloric acid to form soluble barium salts, such as barium chloride:

BaCO3 + 2 HCl → BaCl2 + CO2 + H2O
Pyrolysis of barium carbonate gives barium oxide.

Uses
Barium carbonate is mainly used to remove sulfate impurities from feedstock of the chlor-alkali process.
Otherwise it is a common precursor to barium-containing compounds such as ferrites.

Other uses
Barium carbonate is widely used in the ceramics industry as an ingredient in glazes.
Barium carbonate acts as a flux, a matting and crystallizing agent and combines with certain colouring oxides to produce unique colours not easily attainable by other means.
Its use is somewhat controversial since some claim that it can leach from glazes into food and drink.
To provide a safe means of use, BaO is often used in fritted form.

In the brick, tile, earthenware and pottery industries barium carbonate is added to clays to precipitate soluble salts (calcium sulfate and magnesium sulfate) that cause efflorescence.

Barium carbonate is a white powder.
Barium carbonate is insoluble in water and soluble in most acids, with the exception of sulfuric acid.
Barium carbonate has a specific gravity of 4.275.
Barium carbonate is toxic by ingestion.

Used in brick and clay products, production of photographic paper ... In the oil well drilling industry, the barite suspension used as drilling mud can be destabilized by the presence of sol materials such as gypsum. Addition of barium carbonate renders the gypsum insoluble, inhibits the coagulation, and thus permits the mud to retain the desired consistency and dispersion.

Barium carbonate is an additive in oil-well drilling muds. The barite suspensions used in the oil well drilling industry can destabilize when soluble materials such as gypsum are present in the mud. The presence of gypsum leads to coagulation and a loss of consistency in the drilling muds. When added to the muds, barium carbonate precipitates the gypsum and prevents destabilization of the barite suspension.

Industry Uses
Catalyst for Detergent Alcohol
Fillers
Intermediates
Paint additives and coating additives not described by other categories
Processing aids, not otherwise listed
bonding agent

Consumer Uses
Building/construction materials - wood and engineered wood products
Building/construction materials not covered elsewhere
Detergent Alcohol
Paints and coatings
Tire Adhesion

Methods of Manufacturing
Barium carbonate is made from barium sulfide soln by one of two methods.
In the first, the soda ash method, the barium sulfide soln is treated with sodium carbonate, either dissolved or in solid form, producing barium carbonate and sodium disulfide.
The usual operating temp is 60-70 °C.
The resulting slurry is filtered and the barium carbonate is washed, dried, ground, and packaged. This process is thought to be used by about half of the industry.
In the second main method, carbon dioxide gas is passed through a barium sulfide soln, either batchwise or on a continuous basis, at 40-90 °C.
Temp and other operating conditions have a pronounced effect on the size and characteristics of the particles formed.
To obtain a satisfactory product, the barium sulfide must react with slightly less than the stoichiometric amt of carbon dioxide; the carbon dioxide may be supplied in pure form, or may be obtained from the combustion gases of barium sulfide reduction kilns.

General Manufacturing Information
Industry Processing Sectors
All other chemical product and preparation manufacturing
Construction
Electrical equipment, appliance, and component manufacturing
Nonmetallic mineral product manufacturing (includes clay, glass, cement, concrete, lime, gypsum, and other nonmetallic mineral product manufacturing.
Paint and coating manufacturing
Petrochemical manufacturing
Plastic material and resin manufacturing
Plastics product manufacturing
Primary metal manufacturing
Rubber product manufacturing

IDENTIFICATION: In nature barium occurs in a combined state, the principal forms being barite (barium sulfate) and witherite (barium carbonate).
Barium carbonate has a very low water solubility.
Barium and its compounds are used in diverse industrial products ranging from ceramics to lubricants.
Barium carbonate is used in the manufacture of alloys, as a loader for paper, soap, rubber and linoleum, in the manufacture of valves and as an extinguisher for radium, uranium and plutonium fires.
Anthropogenic sources of barium are primarily industrial.
Emissions may result from mining, refining or processing barium minerals and the manufacture of barium products.
Mining and processing of barite ore releases particulates into the air and from fugitive dists from the use of barite in oil drilling and oil related industries.

Barium Carbonate is a water insoluble Barium source that can easily be converted to other Barium compounds, such as the oxide by heating (calcination).
Carbonate compounds also give off carbon dioxide when treated with dilute acids.
Barium Carbonate is generally immediately available in most volumes.
Ultra high purity and high purity compositions improve both optical quality and usefulness as scientific standards.
Nanoscale elemental powders and suspensions, as alternative high surface area forms, may be considered.
American Elements produces to many standard grades when applicable, including Mil Spec (military grade); ACS, Reagent and Technical Grade; Food, Agricultural and Pharmaceutical Grade; Optical Grade, USP and EP/BP (European Pharmacopoeia/British Pharmacopoeia) and follows applicable ASTM testing standards.
Typical and custom packaging is available.
Additional technical, research and safety (MSDS) information is available as is a Reference Calculator for converting relevant units of measurement.

Barium carbonate powder is dense and white and is manufactured either from the mineral barite (BaSO4) or from barium chloride.
Subsequently a precipitation process is used to get the carbonate form.
There are several crystalline forms of BaCO3, alpha is the most stable.

Barium carbonate is very stable thermally and does not readily disassociate unless at least some CO is available in the kiln atmosphere (i.e. reduction).
BaCO3 is reduced to the unstable BaCO2 in the reaction:

BaCO3 + CO -> BaCO2 + CO2

While BaCO2 has a high melting temperature, it will break down much readily in a glaze melt (liberating the BaO for glass building).
Barium carbonate decomposes even more readily during glaze melting in a reduction atmospheres.
The dissolution process happens most quickly if BaCO3 is present in small amounts (e.g. 5% or less).
Even if present in larger amounts, the glaze matrix can solidify with both types, one participating in the glass microstructure and the other acting as a refractory filler, opacifier and matting agent (especially in low temperature glazes).
Effects produced when baria is acting as a filler are sometimes mistaken for those of a true baria crystal matte.
Such will likely leach toxic BaO (other oxides will opacify or produce a low fire matte i.e. CaO, MgO, Alumina, Zircon).

Barium carbonate produces gases as it decomposes and these can sometimes cause many pinholes or blisters in glazes.
There are barium frits available (e.g. Fusion F-403 has 35% BaO), incorporating one of them to source it instead is a classic application of glaze chemistry calculations. The resultant glaze will be more fusible and will have better clarity and fewer defects.

In art ceramics barium carbonate is popular for the production of classic barium crystal mattes, BaO readily forms crystalline phases during cooling.
These are dependent on adequate kiln temperatures, cooling cycle and the chemistry of the host glaze (a slightly reducing atmosphere is also beneficial).
Some have observed that in some formulations, barium crystallizes so well that it will occur even with very rapid cooling.
Barium can act to initiate crystal development in other chemistries, for example metallic glazes can benefit by the addition of some barium carbonate.

BaO can often be sourced from a barium frit (like Ferro CC-257) instead of raw barium carbonate, provided that the percentage is not too high.
Do not assume that BaO is necessary in every glaze in which it appears.
In some recipes BaO can be substituted for SrO or CaO and even MgO (using glaze chemistry software of course) without losing the color or surface (bright glossy blues, for example).

Barium carbonate is commonly added to clay bodies in small amounts (0.2-0.8%) to halt fired surface scumming or efflorescence Barium carbonate is slightly soluble in water and provides Ba++ ions to link with SO4-- ions in the water to form BaSO4 (barium sulfate).
This new sulfate molecular form is much less soluble (2-3 mg/L), so it stays internal (rather than migrating to the surface during drying).
However companies try minimize the use of barium (or even high clays with high soluble salts) because the barium sulphate generates sulphuric acid during firing and it corrodes kiln refractories.
To get the best dissolution it is best to add the barium to the water first and mix as long as possible, then either add the water to the other dry ingredients (for plastic bodies) or add the other ingredients to the water (for slips).

Applications
Barium carbonate has been used as brine purification chemical in the chloro-alkali industry and as an ingredient in rat poisons and enamels.
Barium carbonate is used in photographic paper manufacturing.
The chemical is used to produce the barium sulphate which gives the photographic paper its flat white appearance.
Practiced in the manufacture of barium ferrites and also in the manufacture of television picture tubes.
Barium carbonate is an additive in oil-well drilling muds.

Uses
(1) Barium carbonate is mainly used for the manufacture of optical glass, funnels, and barium magnetic materials, the manufacture of other barium salts, ceramic, enamel, paint, welding rod feed
(2) Barium carbonate is important chemical raw materials for the production of funnels, magnetic materials and advanced optical glass.
(3) Barium carbonate is used for fireworks, flares preparation, also used for auxiliary material of ceramic coatings and optical glass.
(4) Barium carbonate is used for the manufacture of electronic ceramics, PTC thermistors, capacitors and other electronic components.
(5) Barium carbonate is mainly used for the manufacture of optical glass, CRT glass, and barium magnetic materials and capacitors, it is also used for carburizing steel and metal surface treatment.
Barium carbonate is the raw material of manufacturing other barium salts and ceramic, enamel, pigments, paints, rubber, electrode.
Barium carbonate is also used as rodenticides and purifying agent, oxidation catalyst.
(6) Barium carbonate is mainly used for the manufacture of optical glass, CRT glass, and barium magnetic materials and capacitors, it is also used for carburizing steel and metal surface treatment.
Barium carbonate is the raw material of manufacturing other locks salt and ceramic, enamel, pigments, paints, rubber, electrode.
Barium carbonate is also used as purifying agent and rodenticides.
(7) Barium carbonate is used for the production of funnels, electronic ceramics and purified water, producing pigment, paint or other barium salts, it is used for the manufacture of optical glass, barium magnetic materials, it is important chemical raw material of manufacturing funnels, magnetic materials and advanced optical glass.
Barium carbonate is used for fireworks, flares preparation, it is also used as auxiliary material of ceramic coatings and optical glass, it is used for manufacturing electronic ceramics, PTC thermistor, capacitor of electronic components, it is mainly used in the manufacture of optical glass, CRT glass and barium magnetic materials and capacitors, it is also used for carburizing steel and metal surface treatment.
Barium carbonate is raw material of manufacturing other barium salts and ceramic, enamel, pigments, paints, rubber, electrode materials.
Barium carbonate is also used as rodenticides and purifying agent, oxidation catalyst.
Barium carbonate is mainly used in the manufacture of optical glass, CRT glass and barium magnetic.
Producing piezoelectric ceramic capacitors
Barium carbonate is widely used in high-voltage AC capacitors, ultrasonic transducer devices and piezoelectric ceramic capacitor manufacturing.
The piezoelectric effect was first discovered on quartz crystal by the Curie brothers in 1880, the crystal which can produce the piezoelectric effect was called piezoelectric crystal.
The class of piezoelectric crystal is single crystal, such as quartz (SiO2), sodium potassium tartrate (it is also known Luose salt, NaKC4H4O6 * H2O), BGO (Bi12GeO20) and the like.
Another class of piezoelectric crystals is called piezoelectric ceramics such as barium titanate (BaTiO3), lead zirconate titanate [Pb (ZrxTirx) O3, code PZT], magnesium niobate lead zirconate titanate of Japan made [Pb (Mg1/3Nb2/3) O3 added PZT, code PCM], manganese, antimony, lead zirconate titanate of China made [Pb (Mn1/2Sb2/3) O3 added PIT code PMS] and so on.
Piezoelectric ceramic materials have three major categories:
PZT materials (PbZrTiO3): titania, zirconia, lead oxide, strontium oxide, niobium oxide, lanthanum oxide and the like.
PMN class materials (PbNbMgO3): niobium oxide, magnesium oxide, lead oxide, strontium oxide, lanthanum oxide and the like.
Barium titanate type materials (BaTiO3): titanium dioxide, barium carbonate, strontium carbonate.
The above information is edited by ChemicalBook editor Maggie.

Production method

(1) Carbonation method: carbon dioxide is passed through barium sulfide solution (see preparation of barium sulfide) to carbonize, the obtained barium carbonate slurry is desulfurization washed, vacuum filtration, dried at 300℃ and pulverized to obtain barium carbonate products. its
BaS + CO2 + H2O→ BaCO3↓+ H2S↑
Metathesis method: barium sulfide and ammonium carbonate proceeds metathesis reaction, and then washing, filtering and drying to obtain bismuth products. its
BaS + (NH4) 2CO3 → BaCO3 ↓ + (NH4) 2S
Poison nepheline conversion method: witherite ore reacts with ammonium salt to generate soluble barium salt, and ammonium carbonate is recycled and re-used, ammonium carbonate is added into soluble barium salt to precipitate refined barium carbonate, it is filtered and dried to obtain barium carbonate products.
The obtained mother liquor is recycled use.

(2) Carbonization method.
Reaction equation:
BaS + CO2 → BaCO3 ↓ + H2S ↑
Operational method: 1L barium sulfide aqueous solution of 180g/L reacts with carbon dioxide at 70℃ to produce barium carbonate precipitation.
Precipitation is mixed with 10ml 25% aqueous ammonia, at 60℃ desulfurization for 20min.
Filtered, and dried to obtain the precipitated barium carbonate, product contains 0.46% sulfur.

Metathesis method.
Reaction equation:
BaCl2 + NH4HCO3 + NH4OH → BaCO3 ↓ + 2NH4Cl + H2O
Operational method: At 30℃, 23.6L containing ammonium bicarbonate 56.1g /L aqueous solution and 1.36L ammonia is mixed in 50L kettle and then at 50℃, within 2h dropping 21.6L 200.3g/L barium chloride solution, it is stirred for 30min at 40℃.
Filtered, dried at 140 ℃, pulverized to obtain barium carbonate which average particle diameter d is 0.8μm, purity is 99.8%.
Witherite method.
Reaction equation:
BaCO3 + 2NH4Cl → BaCl2 + 2NH3 + H2O + CO2
BaCL2 + (NH4) 2CO3 → BaCO3 ↓ + 2NH4Cl
Operational method: 100 g 80% of toxic heavy powder (120 mesh) and 60g ammonium chloride is well mixed, it is rapidly put into 650℃ muffle furnace and reacts for 3min.
After cooling, it is flooded, filtered, removed debris to obtain barium chloride solution, 36g ammonium carbonate is added, precipitating barium carbonate, it is filtered, dried and pulverized, the conversion rate is 91%.

(3) Operational method: Dry granulation method: heavy precipitation barium carbonate is sieved, it is placed within the raw materials warehouse and stirred well, mixed, degassed, the material goes through the rotary feeder, lying vertical screw conveyor rollers press rollers compressed tablets, producer thickness is 3.7~4 mm.
The material rolled into sheet is input granulator, by adjusting its speed and aperture size sieve to adjust the particle size distribution of semi-finished products.
Semi-finished products use knife pulse pneumatic conveying method which semi-finished products input the vibration feeder to sieve, particles larger than 20 mesh is back to granulator, particle 65 mesh or less is back to raw materials warehouse, particle between 65 mesh to 20 mesh is transported to packaging warehouse for finished packaging to obtain particles of barium carbonate.
Wet granulation of barium carbonate: Precipitation system is filtered and separated to obtain cake of containing water in manufacturing process system, and the filter cake should control the water content to about 20%.
Under the action of the rotating blades, the material is rapidly mixed well, and kneaded, mediated to form dense particles, the wet pellets is put into the rotary kiln direct fire, sintered at 800~1200℃.
After whole particles, screening, iron removal, weighing and packing to obtain particles of barium carbonate.

Barium Carbonate is a water-insoluble toxic salt BaCO3 occurring in nature as witherite, made artificially by precipitation as a white powder, and used chiefly in making other barium compounds, in removing sulfates from aqueous solutions, in ceramics as a flux, and in optical glass

Widely used in the ceramics industry as an ingredient in glazes, it acts as a flux to produce unique colours not easily attainable by other means.
In the brick, earthenware and pottery industries it is added to cause efflorescence.

Synonyms: Witherite
INCI: Barium Carbonate
Chemical Formula: BaCO3
CAS Number: 25070-31-9, 513-77-9

USES AND APPLICATIONS FOR BARIUM CARBONATE
INDUSTRIES
Pharma
Cleaning
Coatings & Construction
Food and Nutrition
Polymers

A heavy white powder that occurs in nature as the mineral Witherite.
Barium carbonate is used as a pigment in the manufacture of paints, glazes and synthetic marble.
When Barium hydroxide is used as an alkalizing agent for paper, it can react with Carbon dioxide and precipitate as barium carbonate to provide an alkaline reserve.
Both barium hydroxide and barium carbonate are highly toxic.
Barium carbonate is used commercially in rat poison, bricks, cement, and mortar.

A white insoluble compound, BaCO3; r.d. 4.43.
Barium carbonate decomposes on heating to give barium oxide and carbon dioxide:BaCO3(s) → BaO(s)+CO2(g) The compound occurs naturally as the mineral witherite and can be prepared by adding an alkaline solution of a carbonate to a solution of a barium salt.
Barium carbonate is used as a raw material for making other barium salts, as a flux for ceramics, and as a raw material in the manufacture of certain types of optical glass.

Barium carbonate is an insoluble barium salt of carbonic acid with the formula BaCO3, even less soluble than barium sulfate.
Unlike BaSO4, barium carbonate reacts with acids and can serve as precursor to any barium salt.

Properties
Physical
Barium carbonate is a white chalk-like powder, insoluble in water and virtually all solvents, though it dissolves in acids, releasing carbon dioxide.
When heated to 811 °C, it undergoes polymorphic transformation and starting from 1360-1,450 °C it decomposes to release carbon dioxide.
Barium barbonate is quite dense, 4.286 g/cm3

Chemical
Heat causes it to decompose, liberating carbon dioxide and turning into the oxide BaO.

Barium carbonate reacts with all acids, resulting in barium salts and carbon dioxide. This makes it a useful precursor to all barium compounds.

Availability
Barium carbonate is sold by chemical suppliers. Some rat poisons may contain barium carbonate.

Occasionally, pottery stores may sell barium carbonate.

Barium carbonate also occurs naturally as the mineral witherite.

Preparation
Barium carbonate is prepared from barium sulfate by lengthy boiling under reflux with sodium carbonate.
This reaction is sometimes called the Curie reaction, because Marie Curie prepared radium carbonate the same way.

The reaction is very long.

Projects
Anything having to do with barium
Make barium peroxide

BaCO3 occurs in nature as the mineral witherite.
Also it can be synthesized from barite mineral by reduction barium sulphate (BaSO4) with carbon sources.
BaCO3 crystallizes in three polymorphisms such as orthorhombic and cubic.

Barium carbonate is very important chemical for brick and tile producers for solving efflorescence and scumming problems.
Barium carbonate is used for removing sulfates in phosporic acid production.
Barium carbonate with higher purity levels (> 99,5%) is usefull for electroceramic industry.
Nano-barium carbonate has several potential applications in fields of science and technology.
Barium carbonate nano particles and their composites show good catalytic activity for solid oxide fuel cathodes.
Lanthanide doped barium carbonate structures are good candidates for optical materials of photonic device with their luminescence properties.
Morphology controlled synthesis of Barium carbonate has also become attractive for different areas such as medicine, cosmetics, pigments, nano devices, etc.
Researchers have synthesized bunch-like, dumbell, double dumbell and flower like barium carbonate crystals by using natural gums in hydrothermal conditions (Sreedhar, B., Satya Vani, Ch., Keerthi Devi, D., Basaveswara Rao, M.V., Rambabu, C., “Shape controlled synthesis of barium carbonate microclusters and nanocrystallites using natural polysachharide-gum acacia” American Journal of Materials Science, 2,2012)

Another interesting application of Barium carbonate is sulphate removing from drinking water. Elevated levels of sulphate (exceeding 400 mg/l) can experience diarrhea and dehydration. BaCO3-PVC composites have potential to remove sulphates from water.

CAS Number: 513-77-9
Chemical Formula: BaCO3
Availability: R and D quantities only. Please contact ABSCO for delivery time
Description: ABSCO supplies barium carbonate as 99.9% pure material as a powder.
Hazard Class: 6.1, PGIII, UN1564
Applications: Barium carbonate is supplied as a high purity material whose uses include the manufacture of LED phosphors.

Description:
Barium carbonate is used both in white and green color compositions.
When chlorine donors are present in a composition a green color will result from the formation of BaCl+ in the flame.
Without chlorine donors BaO will be formed which emits white light.
Barium carbonate is convenient to use in chlorate based color compositions since it will neutralize residual acid which reduces the risk of spontaneous ignition.

Sources:
Barium carbonate is cheaply available in kilogram quantities from ceramic supply shops.
However, this material is often contaminated with small amounts of barium sulfide that are left over from the production process.
Therefore, ceramics grade barium carbonate should never be used in mixtures incompatible with sulfides such as chlorate based mixtures.
Barium carbonate is not easily made at home.

White in colour, Barium Carbonate is a solid element that precipitates from a solution of barium hydroxide and Urea.
Barium carbonate has a chemical formula stated as BaCO3.
Barium Carbonate is generally toxic in nature and comes in other forms like a mineral form called witherite and it can also be prepared from barytes with the help of precipitation.
Barium carbonate can also be seen in glazes of turquoise.
Barium carbonate is advisable to take proper protective measures while handling this chemical compound as it’s high toxicity is something that you shouldn’t be messing with.
Barium carbonate should be strictly kept under low quality, preferably below 20%. Barium carbonate is also known as Barium Monocarbonate

Chemical Properties of Barium Carbonate - BaCO3

Calcium salts that are soluble can react with Barium Carbonate to form Barium Sulphate which remains in solution and calcium carbonate.
The related chemical reaction is given below:
BaCO3 + CaSO4 → CaCO3 + BaSO4

Barium Carbonate can react with Hydrochloric Acid to form Barium Chloride, Water, and Carbon Dioxide.

BaCO3 + 2HCl → BaCl2 + H20 + CO2

Various Uses of Barium Carbonate - BaCO3
Being a white insoluble salt that finds its largest usage in the Ceramics Industry, Barium Carbonate is widely used to make ceramic products.

Barium carbonate also finds usage as a raw material for Barium oxide (BaO) and Barium peroxide (BaO2)

Barium Carbonate is widely used as a rodenticide although its whitish flour-like appearance has resulted in many barium poisoning cases.

Some of the major commercial applications of barium carbonate / BaCO3 includes glass, oil-drilling, photographic, ceramic, enamel, barium magnetic materials, paint, brick, and chemical industries.

Barium Carbonate is also used for the manufacturing of electronic ceramics, capacitors, PTC thermistors, and other types of electronic equipment.

Barium carbonate is an important raw material for the production of magnetic components and fibre optical glass.

Production Method of BaCO3
Carbonation Method

The process of production of BaCO3 with the carbonation process involves the following:
First carbon dioxide is passed through a solution of barium sulfide so that it can carbonize,
The barium carbonate slurry obtained from this process is then further subjected to desulphurization wash

Barium carbonate is then passed through vacuum filtration, and then dried at 300℃
The final process involves pulverization before barium carbonate products can be obtained.

The Chemical Reaction
BaS + CO2 + H2O → BaCO3↓+ H2S↑

Metathesis Method
In the Metathesis method, barium sulfide and ammonium carbonate undertake a metathesis reaction resulting in barium carbonate.
The end product is then washed, filtered, and dried in order to obtain bismuth products.

The Chemical Reaction
BaS + (NH4) 2CO3 → BaCO3 ↓ + (NH4) 2S

Poison Nepheline Conversion Method
In this process, soluble barium salt is obtained by reacting witherite with an ammonium salt.
The resultant ammonium carbonate is recycled to be used again.
This ammonium carbonate is then added into the soluble barium slat obtained earlier to precipitate barium carbonate in refined form.
The resultant BaCO3 is then filtered and dried to make barium carbonate based products.

The Chemical Reaction

BaCl2 + NH4HCO3 + NH4OH → BaCO3 ↓ + 2NH4Cl + H2O

Dry Granulation Method

The process goes as follows:

Barium carbonate obtained from heavy precipitation is sieved and placed within the warehouse of raw materials.
Barium carbonate is then stirred well, mixed, and then degassed.
The material is then made to go through the rotary feeder.
The end product is compressed with rollers into tablets in a thickness of 3.7 to 4 mm.
The resultant tablets are then rolled into a sheet in the input granulator and its speed is adjusted accordingly.
This gives semi-finished products of barium.

The semi-finished products are subjected to the knife pulse pneumatic conveying method, which the products input into the vibration feeder to sieve.
The granulator releases barium carbonate in particles larger than 20 mesh.

Wet Granulation Method

This method uses a precipitation system to filter a cake containing barium rich water in the process of manufacturing.
The filter cake should have the capability to control the water content at about 20%.
The material is then passed through the action of rotating blades and the material is rapidly mixed. Barium carbonate is then kneaded and mediated to form semi-dense particles/ wet pellets.
The wet pellets are then put into the rotary kiln’s direct fire and then sintered at 800-1200℃.
Then is it furthered screened, processed through iron removal, weighed, and then packed in particles of barium carbonate.

Interesting Fact:

Barium Carbonate or BaCO3 is also called Whiterite named after William Withering who discovered this white mineral in 1784 from barytes.
Barium carbonate generally occurs in the veins of lead ores and is found naturally in a few places.

Barium carbonate is a common reagent in rodenticides which causes hypokalaemic paralysis and symptoms closely resembling Guillain-Barre syndrome in humans.
Has also been investigated in the laboratory in which it percipitates in alkaline silica-rich environments resulting in crystalline aggregate biomorphs.
New reports have performed biomineralizations of barium carbonate hierarchical structures with self-cleaning ability.

About Barium carbonate
Helpful information
Barium carbonate is registered under the REACH Regulation and is manufactured in and / or imported to the European Economic Area, at ≥ 100 000 to < 1 000 000 tonnes per annum.

Barium carbonate is used by consumers, in articles, by professional workers (widespread uses), in formulation or re-packing, at industrial sites and in manufacturing.

Consumer Uses
Barium carbonate is used in the following products: lubricants and greases. Release to the environment of Barium carbonate can occur from industrial use: formulation of mixtures. Other release to the environment of Barium carbonate is likely to occur from: outdoor use, indoor use (e.g. machine wash liquids/detergents, automotive care products, paints and coating or adhesives, fragrances and air fresheners), indoor use in close systems with minimal release (e.g. cooling liquids in refrigerators, oil-based electric heaters) and outdoor use in close systems with minimal release (e.g. hydraulic liquids in automotive suspension, lubricants in motor oil and break fluids).

Article service life
Other release to the environment of Barium carbonate is likely to occur from: indoor use and outdoor use resulting in inclusion into or onto a materials (e.g. binding agent in paints and coatings or adhesives).
Barium carbonate can be found in products with material based on: metal (e.g. cutlery, pots, toys, jewellery).
Widespread uses by professional workers
Barium carbonate is used in the following products: lubricants and greases, metals, welding & soldering products, metal working fluids and hydraulic fluids.
ECHA has no public registered data on the types of manufacture using Barium carbonate.
Release to the environment of Barium carbonate can occur from industrial use: formulation of mixtures.
Other release to the environment of Barium carbonate is likely to occur from: indoor use (e.g. machine wash liquids/detergents, automotive care products, paints and coating or adhesives, fragrances and air fresheners), outdoor use, indoor use in close systems with minimal release (e.g. cooling liquids in refrigerators, oil-based electric heaters) and outdoor use in close systems with minimal release (e.g. hydraulic liquids in automotive suspension, lubricants in motor oil and break fluids).
Formulation or re-packing
Barium carbonate is used in the following products: welding & soldering products, pH regulators and water treatment products, laboratory chemicals and water treatment chemicals.
Barium carbonate has an industrial use resulting in manufacture of another substance (use of intermediates).
Release to the environment of Barium carbonate can occur from industrial use: formulation of mixtures and formulation in materials.
Uses at industrial sites
Barium carbonate is used in the following products: metal surface treatment products, pH regulators and water treatment products, laboratory chemicals, water treatment chemicals, metals, welding & soldering products and metal working fluids.
Barium carbonate has an industrial use resulting in manufacture of another substance (use of intermediates).
Barium carbonate is used in the following areas: building & construction work, formulation of mixtures and/or re-packaging and health services.
Barium carbonate is used for the manufacture of: chemicals, machinery and vehicles, mineral products (e.g. plasters, cement), electrical, electronic and optical equipment and fabricated metal products.
Release to the environment of Barium carbonate can occur from industrial use: as an intermediate step in further manufacturing of another substance (use of intermediates), as processing aid and in processing aids at industrial sites.
Other release to the environment of Barium carbonate is likely to occur from: indoor use and outdoor use resulting in inclusion into or onto a materials (e.g. binding agent in paints and coatings or adhesives).
Manufacture
Release to the environment of Barium carbonate can occur from industrial use: manufacturing of the substance.

Barium carbonate powder is dense and white and is manufactured either from the mineral barite (BaSO4) or from barium chloride. Subsequently a precipitation process is used to get the carbonate form. There are several crystalline forms of BaCO3, alpha is the most stable.

Barium carbonate is very stable thermally and does not readily disassociate unless at least some CO is available in the kiln atmosphere (i.e. reduction). BaCO3 is reduced to the unstable BaCO2 in the reaction:

BaCO3 + CO -> BaCO2 + CO2

While BaCO2 has a high melting temperature, it will break down more readily in a glaze melt (liberating the BaO for glass building).
Barium carbonate decomposes even more readily during glaze melting in a reduction atmospheres. The dissolution process happen most quickly if BaCO3 is present in small amounts (e.g. 5% or less).
Even if present in larger amounts, the glaze matrix can solidify with both types, one participating in the glass microstructure and the other acting as a refractory filler, opacifier and matting agent (especially in low temperature glazes).
Effects produced when baria is acting as a filler are sometimes mistaken for those of a true baria crystal matte.
Such will likely leach toxic BaO (other oxides will opacify or produce a low fire matte i.e. CaO, MgO, Alumina, Zircon).

Barium carbonate produces gases as it decomposes and these can sometimes cause many pinholes or blisters in glazes.
There are many barium frits available and incorporating one of them to source the BaO instead is a classic application of ceramic chemistry calculations.
The resultant glaze will be more fusible and will have better clarity and fewer defects.

In art ceramics barium carbonate is popular for the production of classic barium crystal mattes, BaO readily forms crystalline phases during cooling.
These are dependent on adequate kiln temperatures, cooling cycle and the chemistry of the host glaze (a slightly reducing atmosphere is also beneficial).
Barium can act to initiate crystal development in other chemistries, for example metallic glazes can benefit by the addition of some barium carbonate.

Barium carbonate is commonly added to clay bodies in small amounts (0.2-0.8%) to halt fired surface scumming or efflorescence.
Barium carbonate is slightly soluble in water and provides Ba++ ions to link with SO4-- ions in the water to form BaSO4 (barium sulfate).
This new sulfate molecular form is much less soluble (2-3 mg/L), so it stays internal (rather than migrating to the surface during drying).
Try to minimize the use of barium because the barium sulphate generates sulphuric acid during firing and it corrodes kiln refractories.
To get the best dissolution it is best to add the barium to the water first and mix as long as possible, then either add the water to the other dry ingredients (for plastic bodies) or add the other ingredients to the water (for slips).

Used to manufacture paper, special glass, ceramics, bricks, enamels, paints, rubber, electrodes, and barium salts.
Used in oil well drilling, especially through gypsum; Used in brines as a precipitant and in baths as a case hardener

Product description : barium carbonate comes as a white powder, with a purity of 99.2% minimum.

Uses : barium carbonate is used in the surface treatment to control chromates and sulfates in chromium baths.
Barium carbonate is also used in ceramics, in the brick, glass, tiling, earthenware, pottery industries and in sugar refineries.

Preparation
Barium carbonate is made commercially from barium sulfide with by treatment with sodium carbonate at 60 to 70 °C (soda ash method) or, more commonly carbon dioxide at 40 to 90 °C:

In the soda ash process, an aqueous solution of barium sulfide is treated with sodium carbonate:
BaS + H2O + CO2 → BaCO3 + H2

Reactions
Barium carbonate reacts with acids such as hydrochloric acid to form soluble barium salts, such as barium chloride:

BaCO3 + 2 HCl → BaCl2 + CO2 + H2O
Pyrolysis of barium carbonate gives barium oxide.

Uses
Barium carbonate is mainly used to remove sulfate impurities from feedstock of the chlor-alkali process.
Otherwise Barium carbonateis a common precursor to barium-containing compounds such as ferrites.[

Other uses
Barium carbonate is widely used in the ceramics industry as an ingredient in glazes.
Barium carbonateacts as a flux, a matting and crystallizing agent and combines with certain colouring oxides to produce unique colours not easily attainable by other means.
Its use is somewhat controversial since some claim that Barium carbonatecan leach from glazes into food and drink.
To provide a safe means of use, BaO is often used in fritted form.

In the brick, tile, earthenware and pottery industries barium carbonate is added to clays to precipitate soluble salts (calcium sulfate and magnesium sulfate) that cause efflorescence.

DESCRIPTION
Barium Carbonate: (BaCO3)
Appearance: White powder

Barium Carbonate BaCO3, is a major raw material in the manufacture of porcelain enamel frits, glazes, ferrite magnets, barium titanate, barium sulfate, miscellaneous barium chemicals and various types of glass including television picture tubes, reflective glass beads and other specialty scientific, optical and art glasses.

Barium carbonate is also used for the precipitation and removal of sulfates in various chemical processes and for the prevention of scum in the manufacture of face brick.

CHEMICAL PROPERTIES

Property Specification Limits
BaCO3 + SrCO3 , % 99 min.
SrCO3H, % 2.5 max.
Iron as Fe, ppm 40 max.
Sulfur as S , % 0.1 max.
Na2CO3,% 0.9 max.
+325 mesh US/TY mesh, % 1.0 max.
Moisture , % 0.25 max.

Used in casting slips (up to 5%)to prevent scumming arising from soluble salts.
A flux in high temperature glazes.
Barium carbonate also produces matt and semi matt surfaces at earthenware temperatures, but an excess will cause a rough, dry glaze surface.

What is Barium Carbonate?
Barium carbonate is a white solid precipitated from a solution of barium hydroxide and urea.
The chemical formula for barium carbonate is BaCO3.
Barium carbonate also occurs in mineral known as witherite and also prepared from barytes through precipitation.
Barium carbonate is toxic in nature.
Barium carbonate is also common in turquoise glazes.
Barium carbonate should be kept under low quality below 20% and protective measure to be taken while handling the chemical compound.

Chemical Properties of Barium Carbonate – BaCO3
Soluble calcium salts reacts with barium carbonate forms barium sulfate which remains in solution and calcium carbonate.
BaCO3 + CaSO4 → CaCO3 + BaSO4

Barium carbonate reacts with hydrochloric acid forming barium chloride and water and carbon dioxide.
BaCO3 + 2HCl → BaCl2 + H2O + CO2

Uses of Barium Carbonate – BaCO3
Barium carbonate has many major commercial applications in the glass, brick, oil-drilling, ceramics, photographic and chemical industries.
Used as a raw material for the manufacture of barium oxide (BaO) and barium peroxide (BaO2).
Used as a rodenticide, its appearance is similar to that of flour which has been responsible for most unintentional barium poisoning.
Barium carbonate is a white insoluble salt which finds its largest use in the ceramics industry in the production of ceramic products.

Barium Carbonate (BaCO3) is a white crystalline inorganic compound.
This is an alkali metal carbonate, which is a white powder-like salt and is poorly soluble in water.
Barium carbonate’s formula is BaCO3 and is also called Barium Monocarbonate.

History
Barium carbonate exists in nature as the mineral witherite.
This mineral was first discovered by William Withering in the year 1784 from barytes.
The mineral witherite was named after William Withering who discovered it.
Withering discovered this chemical from the experiments he conducted on a heavy metal ore found in Cumberland(North west England) called terra ponderosa.
One of the earliest samples of witherite may be in the Matthew Boulton mineral collection of Birmingham Museum and Art Gallery.
The chemical witherite later came to be known as barium carbonate.

Properties of Barium Carbonate
Now, let’s move on to the discussion of properties of this compound which implies physical properties and chemical properties.

Physical Properties
Appearance: White Powder (Crystalline Solid)
Density: 4.286 g/cm3Melting
Point: 811°C (Polymorphic Transformation)
Boiling Point: 1450°C, Starts decomposing from 1360°C
Solubility: Insoluble in methanol; Partially insoluble in water;Decomposes in acids
Heat Capacity: 85.35 J/mol.K
Odor: Odorless
Refractive Index: 1.676

Chemical Properties
When soluble calcium salts react with BaCO3 they form a barium salt that remains in the solution itself.
An example:
BaCO3 + CaSO4 -> BaSO4 + CaCO3.
Barium carbonate reacts with some acids to form soluble salts.
An example of this is its reaction with hydrochloric acid.
BaCO3 + 2HCl -> BaCl2 + CO2 + H2O.
The pyrolysis of BaCO3 gives barium oxide.
ProductionBaCO3‘s most important chemical form is the mineral witherite which is found naturally, when seen from a commercial point of view, but it is also prepared from barytes.
Witherite is generally found in the veins of lead ores.
From Barium Sulfide Barium carbonate is prepared from barium sulfide for its commercial purposes.
Barium sulfide is treated with sodium carbonate at 60°C to 70°C, this is called the soda ash method.
The more commonly used method is the carbonation method, where barium sulfide is treated with carbon dioxide at 40°C to 90°C instead of sodium carbonate.
BaS + H2O + CO2 -> BaCO3 + H2SBarium carbonate is also prepared from barium sulfide also by a metathesis reaction with ammonium carbonate.
This method is called the metathesis method.
BaS + (NH4)2CO3 -> BaCO3 + (NH4)2S
From the Mineral WitheriteBarium carbonate is also prepared from refining the mineral witherite.
This is done by first reacting witherite with an ammonium salt which produces a soluble barium salt, then again reacting the formed ammonium carbonate with the barium salt to form refined BaCO3.
BaCl2 + NH4HCO3 + NH4OH -> BaCO3 + 2NH4Cl + H2O
Applications of Barium CarbonateUsed to remove the sulfate impurities present in the feedstock of chlor-alkali process.
Barium carbonate is also commonly used in the preparation of barium containing compounds like ferrites.
Used as an ingredient in glazes in the ceramic industry.
Barium carbonate also acts as a flux, and as a matting and crystallizing agent also.
Produces unique colours by combining with some colouring oxides.
Also used to precipitate soluble salts that cause efflorescence in brick, tile, earthenware and pottery industries.
Used as a raw material for the production of barium oxide and peroxide.
Barium carbonate is also used in other industries like photography, oil drilling, barium magnetic materials, paint, chemical industry etc.
Also used in the manufacture of electrical goods like capacitors, PTC thermistors, electronic ceramics and many others.
Barium carbonate is one of the important raw materials for the production of fibre optical glass.

Brief Overview
Barium carbonate or Witherite, has the molecular formula BaCO3.
The mineral Witherite is named after an English chemist, William Withering, who recognized Witherite to be distinctive chemically from barytes in 1784.
Barium carbonate is a white crystalline solid which melts at 1740 ˚C and decomposes at 1300 ˚C.
Barium carbonate could be crystallized in the orthorhombic system.
While it is soluble in acidic solutions, it is insoluble in water and alcohol.

Barium carbonate is normally employed in rat poison, bricks, ceramic glazes and cement.

Manufacturing Process
Barium carbonate is made from barium sulphide or black ash which is dissolved in water.
The clear solution is the raw material in producing barium carbonate.
There are two ways to produce the carbonate anion:
1. Soda ash method: barium sulphide reacts with the solid form or dissolved sodium carbonate to produce barium carbonate and sodium sulphide.
The resulting barium carbonate precipitate is filtered, washed and dried.
2. Straight gassing method: carbon dioxide is passed through barium sulphide to form barium carbonate and hydrogen sulphide gas.
The toxic hydrogen sulphide gas would then be converted to sulphur compounds or the elemental sulphur, while the barium carbonate would undergo precipitation, washing, drying and grinding.

Barium carbonate powder is dense and white and is manufactured either from the mineral barite (BaSO4) or from barium chloride. Subsequently a precipitation process is used to get the carbonate form. There are several crystalline forms of BaCO3, alpha is the most stable.

Barium carbonate is very stable thermally and does not readily disassociate unless at least some CO is available in the kiln atmosphere (i.e. reduction). BaCO3 is reduced to the unstable BaCO2 in the reaction:

BaCO3 + CO -> BaCO2 + CO2

Barium carbonate produces gases as it decomposes and these can sometimes cause many pinholes or blisters in glazes.
There are barium frits available (e.g. Fusion F-403 has 35% BaO), incorporating one of them to source it instead is a classic application of glaze chemistry calculations.
The resultant glaze will be more fusible and will have better clarity and fewer defects.

Barium carbonate is commonly added to clay bodies in small amounts (0.2-0.8%) to halt fired surface scumming or efflorescence Barium carbonate is slightly soluble in water and provides Ba++ ions to link with SO4-- ions in the water to form BaSO4 (barium sulfate). This new sulfate molecular form is much less soluble (2-3 mg/L), so it stays internal (rather than migrating to the surface during drying).
However companies try minimize the use of barium (or even high clays with high soluble salts) because the barium sulphate generates sulphuric acid during firing and it corrodes kiln refractories.
To get the best dissolution it is best to add the barium to the water first and mix as long as possible, then either add the water to the other dry ingredients (for plastic bodies) or add the other ingredients to the water (for slips).

Chemical Analysis : Purity as BaCO3 98.00%
Min.Strontium Carbonate (SrCO3) 1.50%
Max Sodium Carbonate (Na2CO3) 0.60%
Max Calcium & Magnesium Carbonate (CaCO3+MgCO3) 0.10%
Max Sulphur as SO4 0.02%
MaxI ron Oxide (Fe2O3) 0.004%
Max Chromium Oxide (Cr2O3) 0.002%
Max Chlorine 0.15% Max Moisture (110A C for 1 hour) 0.20%
Max Packing: 25 / 50 Kg Polythene laminated H.D.P.E. bags
Applications : Used as a laboratory reagent.

Used in making complex super conducting materials.
Used in the manufacture of Ceramic capacitors of various micro and pico farads, those are very important components in electronic industries of defense, entertainment and computers.
Used as a constitute in making Television Picture Tubes and other Cathode Ray Tube shells as Barium Oxide cuts off harmful X-ray emission from these tubes and reduces the hazard to the viewers.

IUPAC NAMES
BaCO3
Bario Carbonato
BARIUM CARBONATE
Barium Carbonate
Barium carbonate
barium carbonate
Barium Carbonate
Barium carbonate
barium carbonate
barium carbonate, natural
barium(+2) cation carbonate
barium(2+) carbonate
barium(2+) ion carbonate
barium(2+);carbonate
Bariumcarbonat

SYNONYMS:
BARIUM CARBONATE
513-77-9
Carbonic acid, barium salt (1:1)
Carbonic acid, barium salt
Barium carbonate (1:1)
UNII-6P669D8HQ8
Barium carbonate (BaCO3)
C.I. Pigment White 10
MFCD00003448
6P669D8HQ8
C.I. 77099
Bariumcarbonate
Barium monocarbonate
Pigment White 10
Caswell No. 069
Witherite
CI Pigment White 10
BW-P
Baryta Carbonica
Barium carbonate, 99+%, ACS reagent
Barium carbonate, 99+%, for analysis
BW-C3; BW-P; Barium carbonate (1:1); Barium carbonate (BaCO3); Barium monocarbonate
BW-C3
HSDB 950
EINECS 208-167-3
Carbonic acid Barium Salt
NSC 83508
EPA Pesticide Chemical Code 007501
CI 77099
Nezudai
EINECS 246-600-8
Barium(II) carbonate
BaCO3
CBaO3
barium(2+);carbonate
ACMC-1AMKV
Carbonic acid,barium salt
Barium Carbonate Nanopowder
EC 208-167-3
SCHEMBL18155
25070-31-9
Barium carbonate, Puratronic?
Barium Carbonate Medicine Powder
DTXSID1029623
s235
AKOS015836318
FT-0622559
FT-0622560
FT-0662478
Barium Carbonate Nanopowder / BaCO3 Nanoparticles
Q409224
Barium Carbonate ACS grade, ~200 mesh, 1 micron