BARYTA

Baryta is a strong inorganic base, typically encountered as a white granular solid, powder, or crystalline hydrate that is highly hygroscopic and moderately soluble in water, producing a strongly alkaline solution with a pH above 12.
Baryta is widely used industrially as a precursor in the manufacture of barium salts, as a reagent in analytical chemistry for titration of weak acids, as a dehydrating agent in organic synthesis, and as an additive in lubricants, plastics stabilizers, glass, and ceramics.
The global market for Baryta is steadily expanding, driven by its diverse applications across chemical, water treatment, lubricant, and electronics industries, with Asia-Pacific leading consumption due to rapid industrialization and large-scale chemical production.

CAS Number: 17194-00-2 
EC Number: 241-234-5
Molecular Formula: (Ba(OH)2)
Molecular Weight: 171.34 g/mol

Synonyms: BARIUM HYDROXIDE, BaH2O2, Barium Hydroxide Anhydrous, Bariumhydroxid, Aetzbaryt, barium(II) hydroxide, barium(2+) hydroxide, barium (II) hydroxide, ACMC-20alr7, CHEBI:32592, DTXSID10892155, AKOS015913958, S289, FT-0622568, D03055, Q407605, 12230-71-6 [RN], 22326-55-2 [RN], Barium hydroxide (Ba(OH)2), monohydrate, Barium hydroxide hydrate (1:2:1) [ACD/IUPAC Name], Barium hydroxide monohydrate, BARIUM HYDROXIDE, OCTAHYDRATE, Bariumhydroxidhydrat (1:2:1) [German] [ACD/IUPAC Name], Hydroxyde de baryum, hydrate (2:1:1) [French] [ACD/IUPAC Name], 40226-30-0 [RN], Barium hydroxide hydrate, barium hydroxide monohydrate, 95%, barium hydroxide, monohydrate, barium(2+) and dihydroxide and hydrate, BARIUM(2+) HYDRATE DIHYDROXIDE, BARIUM(2+) ION HYDRATE DIHYDROXIDE, bariumhydroxidehydrate, bariumhydroxidemonohydrate, MFCD00149151

Baryta is a strong inorganic base, typically encountered as a white granular solid, powder, or colorless crystals that are highly hygroscopic.
Baryta is commercially available in two main forms: Baryta octahydrate (Ba(OH)₂·8H₂O), which is the most common, and the anhydrous form, which is less stable and more reactive.

Baryta is moderately soluble in water, producing a strongly alkaline solution with a pH above 12, and is almost insoluble in alcohol.
As a strong base, Baryta reacts readily with acids to form barium salts, and with carbon dioxide to yield barium carbonate.

Industrially, Baryta is widely used as a precursor in the manufacture of barium salts, as a reagent for analytical chemistry (particularly for titration of weak acids), and as a dehydrating agent in some organic syntheses.
Baryta is also applied in lubricant additives, plastics stabilizers, and glass or ceramics production.

Baryta is a clear white powder with no odour. 
Baryta is poisonous in nature. 
Baryta is ionic in nature for example, Ba(OH)2 (Baryta) in aqueous solution can provide two hydroxide ions per molecule. 

Baryta is primarily used to produce other barium products. 
How these products are used is discussed later on. 

Baryta is also used in laboratories to measure the concentration of weak acids. 
This process is called titration. 

Baryta is also used to make glass, grease or other alkalis. 
Baryta is also used in the treatment of sewage water. 
The Baryta is commonly present in nature, as Baryta is present in so many minerals.

Baryta is the only reagent described for metalizing carboxamidesBaryta was less degradative as compared to barium oxide.
Industrially, Baryta is used as the precursor to other barium compounds. 

Baryta is used to dehydrate and remove sulfate from various products.
Baryta exploits the very low solubility of barium sulfate. 

Baryta is also applied to laboratory uses.
Baryta is a chemical compound with the chemical formula Ba(OH)2(H2O)x. 

Baryta is one of the principal compounds of barium. 
Baryta is the chemical compound with the formula Ba(OH)2. 

Baryta is one of the principal compounds of barium. 
The white granular monohydrate is the usual commercial form.

Baryta is a white granular compound. 
Baryta is made up of Barium oxide and water. 

Baryta is mainly used to produce other Barium products.
Baryta has the chemical formula Ba(OH)2. 

One of the principal compounds of the element barium is Barytas monohydrate.
However, in the commercial field, the white granular monohydrate of barium is used for many applications. 

Baryta is an inorganic compound and one of the principal strong bases among the alkaline earth metal hydroxides.
Baryta is most commonly found as the octahydrate form (Ba(OH)₂·8H₂O), a white crystalline solid that is moderately soluble in water, forming a strongly alkaline solution, while the anhydrous form is less stable, highly hygroscopic, and tends to absorb moisture and carbon dioxide from the air.

When dissolved in water, Baryta dissociates completely, producing hydroxide ions that impart a high pH (typically above 12), making it comparable in basic strength to sodium hydroxide and potassium hydroxide, but with somewhat lower solubility.
This strong alkalinity allows Baryta to neutralize acids efficiently, forming corresponding barium salts, and it reacts with carbon dioxide to yield insoluble barium carbonate, a property exploited in purification and chemical synthesis.

Baryta plays an important role in various industrial processes, including the manufacture of other barium compounds (e.g., barium salts used in ceramics, glassmaking, and pigments), as a precursor in lubricating oil additives, and as a stabilizer in plastics.
In organic chemistry, Baryta is employed as a reagent for saponification, dehydration, and condensation reactions, and in analytical chemistry it is used for titrations of weak acids due to its well-defined alkaline strength.

Baryta is also applied in water softening, removal of sulfate ions through precipitation of barium sulfate, and in refining certain sugars.
Despite these uses, Baryta must be handled with great care: while less caustic to the skin than sodium hydroxide, Baryta is still corrosive and causes irritation or burns upon contact, and the soluble barium ions released are toxic if ingested or inhaled, potentially affecting the cardiovascular and nervous systems.

For this reason, protective equipment such as gloves, goggles, and proper ventilation are essential when handling Baryta.
Storage should be in tightly sealed containers, away from carbon dioxide and moisture, as prolonged exposure can lead to gradual conversion into barium carbonate with loss of reactivity.

Market Overview of Baryta:
The global Baryta market is witnessing steady growth, driven by its wide application in the chemical, glass, ceramics, lubricant, plastic, and water treatment industries.
Valued at around USD 125–140 million in 2022–2024, the market is projected to reach between USD 170 and 240 million by 2031–2033, reflecting a compound annual growth rate (CAGR) of approximately 3.5–6.5% depending on Baryta grade and region.

Demand is fueled by Baryta’s role as a precursor in producing barium salts, its use as an additive in lubricants and polymers, and its ability to remove sulfates in water treatment by precipitating insoluble barium sulfate.
Asia-Pacific, particularly China and India, dominates consumption due to rapid industrialization, large-scale chemical production, and growing infrastructure needs, while North America and Europe maintain steady demand supported by advanced manufacturing and strict environmental regulations.

The high-purity Baryta segment, used in pharmaceuticals, electronics, and specialty applications, is also expanding, with projections reaching nearly USD 800 million by 2034 at a CAGR of around 4%.
Despite positive growth, the industry faces challenges such as raw material price fluctuations, environmental regulations concerning barium compounds, and competition from alternative treatment chemicals.
Nevertheless, ongoing investments in research and development, along with increasing applications in sustainable technologies, are expected to secure a stable upward trajectory for the Baryta market in the coming decade.

Uses of Baryta:
Baryta is a versatile strong base with a wide range of industrial and laboratory uses.
Baryta is extensively employed in the manufacture of other barium compounds, such as barium salts (e.g., barium carbonate, barium sulfate), which are essential in glassmaking, ceramics, pigments, and specialty chemicals.

In the lubricant and polymer industries, Baryta serves as an additive and stabilizer, improving thermal stability and reducing corrosion in greases, oils, and plastics.
Baryta's strong alkalinity makes it valuable in water treatment, where it is used to remove sulfate ions by precipitating insoluble barium sulfate, and to adjust pH levels in industrial effluents.

In analytical chemistry, Baryta is used as a standard reagent for titrating weak acids due to its stable alkaline strength and in qualitative testing for sulfates.
In organic synthesis, Baryta functions as a catalyst and dehydrating agent in reactions such as esterification, saponification, and condensation, as well as in refining certain sugars.

High-purity grades find use in electronics, pharmaceuticals, and specialty chemical processes where controlled reactivity and low impurities are essential.
Additionally, Baryta octahydrate is sometimes used as a desiccant for removing water from organic solvents.
Despite Baryta's usefulness, applications are carefully regulated because soluble barium compounds are toxic, requiring strict handling and disposal procedures.

Baryta forms a strong caustic base in aqueous solution. 
Baryta has many uses, e.g., as a test for sulphides; in pesticides; in the manufacture of alkali and glass.

Use of Ba(OH)2 lime rather than soda lime, high sevoflurane concentration, high absorbent temperature, and fresh absorbent use.
Baryta is used in the manufacture of alkalis, glass, oil and grease additives, barium soaps, and other barium compounds.

Barium Hydrate octahydrate is widely used as a consolidant for plasters and wall paintings. 
Baryta reacts with carbon dioxide to form Barium Carbonate, a salt almost insoluble in water, which gives the consolidating effect. 
Besides, Baryta reacts with Calcium Sulphate (CaSO4), which is present on frescoes as an efflorescence, to form Barium Sulphate (BaSO4), an extremely insoluble salt.

Baryta is used in analytical chemistry for the titration of weak acids, particularly organic acids. 
Barytas clear aqueous solution is guaranteed to be free of carbonate, unlike those of sodium hydroxide and potassium hydroxide, as barium carbonate is insoluble in water. 

This allows the use of indicators such as phenolphthalein or thymolphthalein (with alkaline colour changes) without the risk of titration errors due to the presence of weakly basic carbonate ions.
Baryta is used in organic synthesis as a strong base, for example for the hydrolysis of esters and nitriles.

Baryta has been used to hydrolyse one of the two equivalent ester groups in dimethyl hendecanedioate.
Baryta is also used in the preparation of cyclopentanone, diacetone alcohol and D-Gulonic γ-lactone.
Baryta is used in a demonstration of endothermic reactions since, when mixed with an ammonium salt, the reaction becomes cold as heat is absorbed from the surroundings.

Laboratory uses:
Baryta is used in analytical chemistry for the titration of weak acids, particularly organic acids. 
Barytas clear aqueous solution is guaranteed to be free of carbonate, unlike those of sodium hydroxide and potassium hydroxide, as barium carbonate is insoluble in water. 

This allows the use of indicators such as phenolphthalein or thymolphthalein (with alkaline colour changes) without the risk of titration errors due to the presence of carbonate ions, which are much less basic.
Baryta is occasionally used in organic synthesis as a strong base, for example for the hydrolysis of esters and nitriles, and as a base in aldol condensations.

There are several uses for Baryta such as to hydrolyse one of the two equivalent ester groups in dimethyl hendecanedioate.
Baryta has also been used, as well, in the decarboxylation of amino acids liberating barium carbonate in the process.
Baryta is also used in the preparation of cyclopentanone, diacetone alcohol and D-gulonic γ-lactone.

Benefits of Baryta:
Baryta offers several important benefits that make it valuable across multiple industrial sectors.
One of Baryta's primary advantages is its strong alkalinity, which allows it to neutralize acids efficiently, making it highly useful in producing barium salts, in water treatment, and as a reagent in analytical chemistry.

Compared to more common bases like sodium hydroxide or potassium hydroxide, Baryta often provides selectivity and higher efficiency in processes where the precipitation of barium salts (such as barium sulfate) is desired, enabling effective sulfate removal from industrial effluents.
Baryta's moderate solubility in water is also beneficial, as it provides a controlled release of hydroxide ions, reducing excessive causticity and making it easier to handle in some processes than the more aggressive alkali hydroxides.

In the lubricants and polymer industries, Baryta enhances thermal stability, corrosion resistance, and performance of greases and plastics, extending the lifespan of materials exposed to high temperatures or mechanical stress.
In organic synthesis, Baryta serves as both a catalyst and a dehydrating agent, promoting reactions such as esterification, condensation, and saponification with efficiency.

High-purity Baryta is especially beneficial in electronics and pharmaceuticals, where its low impurity profile supports sensitive applications.
Furthermore, Baryta's ability to act as a desiccant and stabilizer adds to its versatility, allowing it to protect systems from moisture and maintain chemical stability.
Collectively, these benefits—strong but controllable alkalinity, selectivity in precipitation, multifunctional reactivity, and performance enhancement—make Baryta a key material in modern chemical manufacturing, environmental management, and advanced technology industries.

Properties of Baryta:

Physical Properties:
Baryta is a white color solid that has no odor. 
Baryta has a density of 3.743 g mL-1(in monohydrate form) and 2.18 g mL-1(in octahydrate form). 

The melting points are 78 ºC (in octahydrate form), 300 ºC (in monohydrate form), and 407 ºC (in, anhydrous form). 
The boiling point is about 780 ºC. 
All the 3 forms are slightly soluble with water at low temperatures but the solubility in water increases with the increase in temperature.

Chemical Properties:
The Baryta produces alkali solutions when we dissolve Baryta in water due to the release of the hydroxyl anions. 
Baryta is useful for making the barium salts because Baryta can react with sulphuric, phosphoric and other acids to produce the respective salts such as barium phosphate, etc.

Preparation and Structure of Baryta:

Baryta can be prepared by dissolving barium oxide (BaO) in water:
BaO + H2O → Ba(OH)2

Baryta crystallises as the octahydrate, which converts to the monohydrate upon heating in air. 
At 100 °C in a vacuum, the monohydrate will yield BaO and water.

The monohydrate adopts a layered structure. 
The Ba2+ centers adopt a square anti-prismatic geometry. 

Each Ba2+ center is bound by two water ligands and six hydroxide ligands, which are respectively doubly and triply bridging to neighboring Ba2+ centre sites.
In the octahydrate, the individual Ba2+ centers are again eight coordinate but do not share ligands.

Reactions of Baryta:
Ba(OH)2 decomposes to barium oxide when heated to 800 °C. 
Baryta reaction with carbon dioxide gives barium carbonate. 

Barytas aqueous solution, being highly alkaline, undergoes neutralization reactions with acids due to it being a strong base. 
Baryta is especially useful on reactions that require the titrations of weak organic acids. 

Thus, Baryta forms barium sulfate and barium phosphate with sulfuric and phosphoric acids, respectively. 
Reaction with hydrogen sulfide produces barium sulfide. 

Precipitation of many insoluble, or less soluble barium salts, may result from double replacement reaction when a Baryta aqueous solution is mixed with many solutions of other metal salts.
Reactions of Baryta with ammonium salts are strongly endothermic. 
The reaction of Baryta octahydrate with ammonium chloride or ammonium thiocyanate is often used as a classroom chemistry demonstration, producing temperatures cold enough to freeze water and enough water to dissolve the resulting mixture.

History of Baryta:
The history of Baryta dates back to the late 18th and early 19th centuries, during the period when alkaline earth metals and their compounds were being systematically studied and identified.
Barium itself was first recognized as a distinct element in 1774 by Carl Wilhelm Scheele and later isolated in pure metallic form by Sir Humphry Davy in 1808 through electrolysis, which laid the foundation for the discovery and preparation of its hydroxide.

Early chemists prepared Baryta by reacting barium oxide (obtained from heating barite, BaSO₄, or witherite, BaCO₃) with water, water—a strongly alkaline solution used historically as a laboratory reagent to test for carbon dioxide, since it precipitates insoluble barium carbonate.
In the 19th century, baryta water was widely employed in qualitative analysis and in the manufacture of barium salts, which were important in glassmaking, ceramics, and pigments.

With the growth of the chemical industry in the late 19th and early 20th centuries, production of Baryta became more controlled and large-scale, particularly in its octahydrate form (Ba(OH)₂·8H₂O), which was easier to handle and store.
By the mid-20th century, Baryta found significant applications as a stabilizer in lubricants and polymers, and as a refining agent in sugar and specialty chemicals.

In more recent decades, the development of high-purity Baryta has expanded its role into electronics, pharmaceuticals, and specialty chemical processes, reflecting the transition from a simple laboratory reagent to a critical industrial base chemical.
Today, while its handling remains strictly regulated due to the toxicity of soluble barium compounds, Baryta continues to occupy an important place in industrial chemistry, environmental applications, and high-technology sectors, building on more than two centuries of scientific and industrial use.

Handling and Storage of Baryta:
Handle Baryta in well-ventilated areas, avoiding dust generation and direct contact with skin, eyes, and clothing.
Do not eat, drink, or smoke while handling the material.

Use corrosion-resistant containers, and keep them tightly sealed when not in use.
Store in a cool, dry, well-ventilated place, away from acids, carbon dioxide, and moisture, since prolonged exposure may lead to conversion into barium carbonate.

Keep away from incompatible materials such as oxidizing agents and ammonium salts.
Clearly label storage areas and restrict access to trained personnel.

Stability and Reactivity of Baryta:
Baryta is stable under recommended storage conditions. 
Baryta is strongly alkaline, hygroscopic, and reacts vigorously with acids to form barium salts.

Baryta also reacts with carbon dioxide in the air, producing insoluble barium carbonate.
At elevated temperatures, decomposition may release toxic fumes including barium oxide.

Incompatible with strong oxidizers, ammonium salts, and carbon dioxide-rich environments.
Hazardous polymerization does not occur.

First Aid Measures of Baryta:

Inhalation:
Remove the affected person to fresh air immediately.
If breathing is difficult, provide oxygen.
Seek medical attention if symptoms persist.

Skin Contact:
Wash affected skin thoroughly with soap and water for at least 15 minutes.
Remove contaminated clothing and wash before reuse.
Seek medical attention if irritation or burns develop.

Eye Contact:
Rinse cautiously with plenty of water for at least 15 minutes, lifting upper and lower eyelids occasionally.
Seek immediate medical attention.

Ingestion:
Rinse mouth with water.
Do not induce vomiting.

Give plenty of water or milk if the person is conscious.
Seek immediate medical help, as soluble barium compounds are toxic.

Firefighting Measures of Baryta:
Baryta is non-combustible, but exposure to heat may cause decomposition and release irritating or toxic fumes (barium oxide, hydroxide dust). 
Use extinguishing media suitable for surrounding fire—water spray, foam, dry chemical, or carbon dioxide.

Firefighters should wear self-contained breathing apparatus (SCBA) and full protective clothing.
Prevent firefighting water from entering drains or natural waterways due to toxicity.

Accidental Release Measures of Baryta:
In case of a spill, evacuate the area and ensure adequate ventilation.
Wear appropriate personal protective equipment (PPE).

For small spills, carefully sweep or vacuum without generating dust and place in a suitable container for disposal.
For large spills, dike the area to prevent spreading, then collect using non-combustible absorbent materials.

Prevent material from entering waterways, sewers, or soil.
Wash spill area thoroughly after cleanup.
Dispose of waste in accordance with local regulations for hazardous materials.

Exposure Controls / Personal Protection of Baryta:

Engineering Controls:
Use in well-ventilated areas, preferably with local exhaust ventilation.
Emergency eyewash and safety shower stations should be available.

Respiratory Protection:
Use a NIOSH-approved respirator if exposure limits are exceeded or dust/aerosols are generated.

Eye Protection:
Safety goggles or face shield to prevent eye exposure.

Skin Protection:
Wear chemical-resistant gloves (e.g., nitrile, neoprene) and protective clothing.

Hygiene Measures:
Wash hands, forearms, and face thoroughly after handling.
Avoid contact with food, beverages, and tobacco during handling.

Identifiers of Baryta:
CAS Number:    
17194-00-2 
22326-55-2 (monohydrate) 
12230-71-6 (octahydrate) 
CHEBI:32592  
ChemSpider: 26408 
ECHA InfoCard: 100.037.470  
EC Number: 241-234-5
Gmelin Reference: 846955
PubChem CID: 28387
RTECS number: CQ9200000
UNII: 1OHB71MYBK  
P27GID97XM: (monohydrate)  
L5Q5V03TBN: (octahydrate)  
CompTox Dashboard (EPA): DTXSID10892155

Chemical Name: Baryta
IUPAC Name: Barium dihydroxide

CAS Numbers:
Anhydrous: 17194-00-2
Monohydrate: 22326-55-2
Octahydrate: 12230-71-6

EC Number: 241-234-5 (anhydrous)
Molecular Formula: Ba(OH)₂ · xH₂O (commonly Ba(OH)₂·8H₂O or Ba(OH)₂·H₂O)

Molecular Weight:
Anhydrous: 171.34 g/mol
Monohydrate: 189.36 g/mol
Octahydrate: 315.46 g/mol

Appearance: White/off-white crystalline solid or powder (granules or flakes); octahydrate forms colorless crystals
Odor: Odorless
Solubility: Moderately soluble in water (about 3.9 g/100 mL at 20 °C for octahydrate); insoluble in alcohol
pH (aqueous solution): Strongly alkaline (pH ~12–13 for 0.1 M solution)

Odor: Odorless
pH (0.1 M solution): ~12–13 (strongly alkaline)

Density:
Anhydrous: ~2.18 g/cm³
Octahydrate: ~2.18 g/cm³

Melting Point:
Anhydrous: ~407 °C (decomposes to barium oxide on heating)
Octahydrate: Loses water of crystallization at ~78 °C
Stability: Hygroscopic; reacts with CO₂ to form insoluble barium carbonate

Properties of Baryta:
Compound Formula: BaH2O2
Molecular Weight: 171.36
Appearance: White to off-white powder, crystals or crystalline powder
Melting Point: 78° C (172.4° F)
Boiling Point: 780° C (1,436° F)
Density: 3.74 g/cm3
Monoisotopic Mass: 171.910721

Chemical formula: Ba(OH)2
Molar mass: 
171.34 g/mol (anhydrous)
189.355 g/mol (monohydrate)
315.46 g/mol (octahydrate)
Appearance: white solid
Density: 
3.743 g/cm3 (monohydrate)
2.18 g/cm3 (octahydrate, 16 °C)
Melting point: 
78 °C (172 °F; 351 K) (octahydrate)
300 °C (monohydrate)
407 °C (anhydrous)
Boiling point: 780 °C (1,440 °F; 1,050 K)

Solubility in water, mass of BaO (not Ba(OH)2):
1.67 g/100 mL (0 °C)
3.89 g/100 mL (20 °C)
4.68 g/100 mL (25 °C)
5.59 g/100 mL (30 °C)
8.22 g/100 mL (40 °C)
11.7 g/100 mL (50 °C)
20.94 g/100 mL (60 °C)
101.4 g/100 mL (100 °C) 
Solubility in other solvents: low
Basicity (pKb): 0.15 (first OH–), 0.64 (second OH–) 
Magnetic susceptibility (χ): −53.2·10−6 cm3/mol
Refractive index (nD): 1.50 (octahydrate)

Ba(OH)2: Baryta
Density: 3.74 g/cm³
Molecular Weight/ Molar Mass: 171.34 g/mol
Boiling Point: 780 °C
Melting Point: 78 °C
Chemical Formula: BaH2O2

grade: technical grade
Quality Level: 100
assay: ~95%
form: powder
mp: >300 °C (lit.)
density: 2.2 g/mL at 25 °C (lit.)
SMILES string: O[Ba]O
InChI: 1S/Ba.2H2O/h;2*1H2/q+2;;/p-2
InChI key: RQPZNWPYLFFXCP-UHFFFAOYSA-L