BARIUM HYDROXIDE

Barium hydroxide = Baryta

CAS Number: 17194-00-2 
EC Number: 241-234-5
Molecular Weight/ Molar Mass: 171.34 g/mol
Chemical Formula: BaH2O2

Barium hydroxide is a chemical compound with the chemical formula Ba(OH)2(H2O)x. 
The monohydrate (x = 1), known as baryta or baryta-water, is one of the principal compounds of barium. 
This white granular monohydrate , Barium hydroxide , is the usual commercial form.
Barium hydroxide is the chemical compound with the formula Ba(OH)2. 
Also known as baryta, Barium hydroxide is one of the principal compounds of barium. 
The white granular monohydrate is the usual commercial form.

Uses of Barium hydroxide
Industrially, barium hydroxide is used as the precursor to other barium compounds. 
Barium hydroxide is used to dehydrate and remove sulfate from various products.
Barium hydroxide exploits the very low solubility of barium sulfate. 
Barium hydroxide is also applied to laboratory uses.

Laboratory uses of Barium hydroxide
Barium hydroxide is used in analytical chemistry for the titration of weak acids, particularly organic acids. 
Barium hydroxides 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.
Barium hydroxide 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 barium hydroxide such as to hydrolyse one of the two equivalent ester groups in dimethyl hendecanedioate.
Barium hydroxide has also been used, as well, in the decarboxylation of amino acids liberating barium carbonate in the process.
Barium hydroxide is also used in the preparation of cyclopentanone, diacetone alcohol and D-gulonic γ-lactone.

Barium Hydroxide Uses
Barium hydroxide is used for a number of purposes, such as
-In manufacturing alkali
-In constructing glass
-In synthetic rubber vulcanization
-In corrosion inhibitors
-As drilling fluids, pesticides and lubricants
-For boiler scale remedy
-For refining vegetable and animal oils
-For fresco painting
-In softening water
-As an ingredient of homeopathic remedies
-To clean up acidic spills
-Barium hydroxide is also used in the sugar industry for preparing beet sugar.

What is Barium Hydroxide?
Barium hydroxide is also called as baryta with the formula Ba(OH)2. 
Barium hydroxide is a clear white powder with no odour. 
Barium hydroxide is poisonous in nature. 
Barium hydroxide is ionic in nature for example, Ba(OH)2 (barium hydroxide) in aqueous solution can provide two hydroxide ions per molecule. 
Barium hydroxide is the only reagent described for metalizing carboxamidesBarium hydroxide was less degradative as compared to barium oxide.

Uses of Barium hydroxide – Ba(OH)2
Barium hydroxide forms a strong caustic base in aqueous solution. 
Barium hydroxide has many uses, e.g., as a test for sulphides; in pesticides; in the manufacture of alkali and glass.
Use of barium hydroxide lime rather than soda lime, high sevoflurane concentration, high absorbent temperature, and fresh absorbent use.
Barium hydroxide 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. 
Barium Hydroxide reacts with carbon dioxide to form Barium Carbonate, a salt almost insoluble in water, which gives the consolidating effect. 
Besides, Barium hydroxide reacts with Calcium Sulphate (CaSO4), which is present on frescoes as an efflorescence, to form Barium Sulphate (BaSO4), an extremely insoluble salt.

Preparation and structure of Barium hydroxide:
Barium hydroxide can be prepared by dissolving barium oxide (BaO) in water:
BaO + H2O → Ba(OH)2
Barium hydroxide 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 (see picture above). 
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.

Barium Hydroxide is used such as:
-additive in the production of lubricants and grease
-additive in thermoplastic resins, rayon and PVC
-manufacturing of soaps
-chemicals synthesis of other barium salts and organic compounds
-fusing of silicates

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

Definition of Barium hydroxide:
Barium Hydroxide is a white granular compound. 
Barium hydroxide is made up of Barium oxide and water. 
Barium hydroxide is mainly used to produce other Barium products.
Barium hydroxide has the chemical formula Ba(OH)₂ₓ. 
One of the principal compounds of the element barium is Barium hydroxides monohydrate, which is alternatively known as baryta or baryta-water. 
However, in the commercial field, the white granular monohydrate of barium is used for many applications. 

Chemical Structure of Barium Hydroxide
The chemical formula of Barium Oxide is Ba(OH)₂. 
The chemical formula of Barium Hydroxide is interesting. 
As you can see from the name, Barium Hydroxide is made up of Barium and Hydroxide. 
So, logically speaking, the formula should be Ba(OH). 
Then why do we write Ba(OH)₂ as the formula of Barium Hydroxide? 
This is because Barium has two positive ions while hydroxide has one negative one. 
So in order to show Barium as a neutral compound, we add another hydroxide to Barium Hydroxide and make Barium hydroxide neutral.

Properties of Barium Hydroxide
Molar Mass
In order to find the molar mass of Barium Hydroxide, we need to add the molar masses of the elements that build this compound. 
The molar mass or molecular weight of Barium is 137.33. 
There is only one Barium in the compound. 
The molar mass of hydrogen is 1.008. 
There are two hydrogens in the compound. 
So the total molar mass of the two hydrogens combined is 2.016. 
The molar mass of oxygen is 15.999. 
There are two oxygens and hence the total molar mass of the two oxygens combined is 31.998. 
Now if we add these numbers we get 171.344. 
So the molar mass of Barium Hydroxide is 171.344g/mol.

Barium Oxide: A Strong Base
A base is that chemical species that reacts with water to give out hydroxide ions. 
A strong base is that base that can get completely dissociated in H2O to give out the exact number of anions and cations that the elements in the unbroken base had.

Melting Point
The melting point of Barium Hydroxide differs with the amount of water in Barium hydroxide. 
The octahydrate form of Barium oxide melts at 78-degree celsius. 
The monohydrate form melts at 300-degree Celsius and the anhydrous form melts at 407-degree celsius.

Solubility
Although Barium Hydroxide is soluble in water, Barium hydroxide is only slightly soluble. 
You need a Barium Hydroxide compound with a Molar Concentration of 0.1 M if you want Barium hydroxide to dissolve in water.

Boiling Point
Barium Hydroxide boils at 780-degree celsius. 
If you keep on boiling and the temperature reaches 800-degree celsius, Barium hydroxide will decompose and give out Barium Oxide.
Other Properties of Barium Hydroxide 
Barium hydroxide is white in colour.
Barium hydroxide generally appears as granular solid.
Barium hydroxide is odourless.
The pH of Barium Hydroxide is 11.27
The density of the monohydrate form of Barium Hydroxide is 3.74 g/cubic cm. 
And the density of the octahydrate form is 2.18 g/cubic cm.

Reactions
Barium hydroxide decomposes to barium oxide when heated to 800 °C. 
Barium hydroxide reaction with carbon dioxide gives barium carbonate. 
Barium hydroxides aqueous solution, being highly alkaline, undergoes neutralization reactions with acids due to it being a strong base. 
Barium hydroxide is especially useful on reactions that require the titrations of weak organic acids. 
Thus, Barium hydroxide 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 barium hydroxide aqueous solution is mixed with many solutions of other metal salts.
Reactions of barium hydroxide with ammonium salts are strongly endothermic. 
The reaction of barium hydroxide 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.

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

Barium Hydroxide is a highly water insoluble crystalline Barium source for uses compatible with higher (basic) pH environments. 
Hydroxide, the OH- anion composed of an oxygen atom bonded to a hydrogen atom, is commonly present in nature and is one of the most widely studied molecules in physical chemistry. 
Hydroxide compounds have diverse properties and uses, from base catalysis to detection of carbon dioxide. 
In a watershed 2013 experiment, scientists at JILA (the Joint Institute for Laboratory Astrophysics) achieved evaporative cooling of compounds for the first time using hydroxide molecules, a discovery that may lead to new methods of controlling chemical reactions and could impact a range of disciplines, including atmospheric science and energy production technologies. 
Barium Hydroxide is generally immediately available in most volumes. 
Ultra high purity and high purity compositions improve both optical quality and usefulness as scientific standards. 

Barium hydroxide,  Ba(OH)2 , is also known as baryta. 
Barium hydroxide can be prepared either by dissolving barium oxide ( BaO ) or barium sulfide ( BaS ) in water:
BaO+H2O→Ba(OH)2+H2O(1)
BaS+H2O→Ba(OH)2+H2S(2)
Barium hydroxide crystallizes as the octahydrate,  Ba(OH)2⋅8H2O , which can be converted to the monohydrate by heating in air. 
The white granular monohydrate is the usual commercially available form. 
Barium hydroxide decomposes to barium oxide when heated to 800°C.
Barium hydroxide forms an alkaline solution in water ("baryta water") which can be used to titrate weak acids, since Barium hydroxides clear aqueous solution is guaranteed to be free of carbonate (barium carbonate is insoluble in water).

Is Barium Hydroxide Soluble In Water?
The solubility of Barium Hydroxide is moderate in water. 
However, this compound is insoluble in acetone. 
At room temperature, Barium hydroxide can produce a solution. 
The Barium Hydroxide solution is found to have an approximate concentration of 0.1 mol dm-3.

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)

Endothermic Reaction
The article on Barium Hydroxide will remain incomplete if we don’t talk about endothermic reaction and the role of Barium Hydroxide in Barium hydroxide. 
Endothermic reaction is any reaction that borrows heat from the surrounding areas. 
The area thus becomes noticeably cool.

You can see this endothermic reaction if you mix Barium hydroxide with ammonium chloride. 
As you mix the two compounds in a beaker the temperature shoots down rather too quickly. 
If you measure the temperature inside the beaker, you will see that Barium hydroxide has gone down below -20 degrees. 
The reaction absorbs the surrounding heat and results in the production of ammonia, barium chloride and water.

Uses of Barium hydroxide:
Barium hydroxide is primarily used to produce other barium products. 
How these products are used is discussed later on. 
Barium hydroxide is also used in laboratories to measure the concentration of weak acids. 
This process is called titration. 
Barium hydroxide is also used to make glass, grease or other alkalis. 
Barium hydroxide is also used in the treatment of sewage water. 
The barium hydroxide is commonly present in nature, as Barium hydroxide is present in so many minerals.
 
Preparation of Barium hydroxide:
We can prepare the barium hydroxide by the process of reacting the barium oxide (BaO) with the water (H2O):
BaO + 9H2O →Ba(OH)2• 8H2O

Physical Properties of Barium hydroxide:
Barium hydroxide is a white color solid that has no odor. 
Barium hydroxide 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 of Barium hydroxide:
The barium hydroxide produces alkali solutions when we dissolve Barium hydroxide in water due to the release of the hydroxyl anions. 
Barium hydroxide is useful for making the barium salts because Barium hydroxide can react with sulphuric, phosphoric and other acids to produce the respective salts such as barium phosphate, etc.

Uses of Barium hydroxide:
The barium hydroxide is capable of using Barium hydroxide as a source of barium to produce other barium salts such as barium phosphate, barium sulfide and barium sulfate that we are using in the chemical industry in various diverse processes. 
Moreover, we can also use the barium hydroxide in an analytical standard for the titration of the weak acids due to Barium hydroxides alkali features.

Laboratory Uses of Barium hydroxide:
Barium hydroxide is used in analytical chemistry, particularly for organic acids. 
However, Barium hydroxides clear aqueous solution is to make sure to be free of carbonate, unlike those of the sodium hydroxide and potassium hydroxide, as barium carbonate is not soluble inside the water.
This permits the use of indicators such as the phenolphthalein or the thymolphthalein (with changes in the alkaline color), without the risk of the titration errors due to the presence of the carbonate ions, that are very less basic.

Here’s a Recap
Barium hydroxide is a white, granular compound.
Barium hydroxide is made of Barium and Hydroxide ions.
In Barium hydroxides original form, Barium hydroxide is ionic in nature.
Barium hydroxide has a molecular weight of 171.344 g/mol.
Barium hydroxide is a strong base as Barium hydroxide dissociates itself completely in water and gives out BaO cation and Hydroxide cation.
Barium hydroxide takes 78-degree Celsius for the octahydrate form of barium hydroxide to melt. 
Barium hydroxide takes 300 degrees and 407-degree Celsius for the monohydrate and the anhydrous forms to melt.
The boiling point of Barium hydroxide is 780-degree Celsius. 
If you heat the compound further, Barium hydroxide will result in thermal decomposition and you will get Barium Oxide.
Barium Hydroxide can get dissolved in water, Barium hydroxide is only slightly soluble. 
Barium Hydroxide compound with a Molar Concentration of 0.1 M will dissolve in water. 
The compound with higher molar concentration cannot dissolve in water.

Barium Hydroxide offered by us is used chemical industry, machinery manufacturing, and metal processing. 
In Chemical industry Barium hydroxide is used for the manufacture of barium salt. 
Barium hydroxide is used for the manufacture of heat treatment salts; Barium hydroxide is also used for boiler water treatment and Sulfate salt electrolysis. 
Barium hydroxide is used to make pigments, ceramic products to prevent fading. 
Barium hydroxide is also used in textile industry and leather industry as mordant and artificial matting agents and in electronic industry. 
Barium hydroxide is the chemical compound with the formula Ba(OH)2. 
Also known as baryta, or baryta-water, Barium hydroxide is one of the principal compounds of barium.

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)

Barium hydroxide has the molecular formula of Ba(OH)2 and the molecular weight of 121.6324 g/mol. 
Barium hydroxide occurs as an anhydrate whose prismatic, colorless crystals are very deliquescent. 
Barium hydroxide can be prepared by dissolving barium oxide (BaO) in water:

BaO + 9H2O ⇒ Ba(OH)2·8H2O
Barium hydroxide crystallizes as the octahydrate, which converts to the monohydrate upon heating in air. 
Barium oxide has been found to react with water vapor at temperatures from 1443 to 1593 K to form gaseous Ba(OH)2 according to the reaction:

BaO(solid) + H2O(gas) ⇒ Ba(OH)2(gas)
The standard free energy of formation is given by the equation, ΔGr° = 49,400 – 16.6 T (cal/mol) in the present temperature range. 
From the thermodynamic cycle, the bond energy between barium and two hydroxyl groups has been found to be 196.8 kcal/mol.

A better method of preparation involves addition of NaOH to the nitrate. 
Since barium hydroxide is fairly soluble, Barium hydroxide is necessary to evaporate the solution to crystallize Ba(OH)2·8H2O. 
Ethanol is added to aid in this crystallization. 
The crystals are washed in cold ethanol to remove sodium ions and then dried. 
Barium hydroxide octahydrate forms crystalline precipitates which do not show changes in solubility on aging and whose solubility in water increases with increasing temperature.

When heated, the octahydrate decomposes to the monohydrate at about 78 °C and to the anhydrate at about 375 °C. 
The thermal dehydration of crystalline barium hydroxide octahydrate has been studied. 
The octahydrate first dissolves in Barium hydroxides own waters of hydration (78 °C) and then loses four waters to form the trihydrate at about 125 °C. 
The trihydrate is not stable and it is the monohydrate which is obtained at 180 °C. 
Gradual thermal treatment in air leads to the formation of anhydrous barium hydroxide at 375 °C. 
Barium oxide is formed at about 410 °C in an inert atmosphere. 
The hydroxide is converted directly to the peroxide in the temperature range 400–600 °C.

Application of Barium hydroxide:
Reagent used in wet chemical gel-to-crystallite conversion to form BaTiO3 at low temperatures.

Preparation of Barium hydroxide:
Barium hydroxide can be prepared by dissolving barium oxide (BaO) in water.
BaO + 9H2O → Ba(OH)2·8H2O
Barium hydroxide crystallises as the octahydrate, which converts to the monohydrate upon heating in air. 
At 100 °C in a vacuum, the monohydrate gives BaO.

Uses of Barium hydroxide:
Barium hydroxide is used in analytical chemistry for the titration of weak acids, particularly organic acids. 
Barium hydroxides 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.
Barium hydroxide is used in organic synthesis as a strong base, for example for the hydrolysis of esters and nitriles.
Barium hydroxide has been used to hydrolyse one of the two equivalent ester groups in dimethyl hendecanedioate.
Barium hydroxide is also used in the preparation of cyclopentanone, diacetone alcohol and D-Gulonic γ-lactone.
Barium hydroxide 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.

Miscellaneous applications of Barium hydroxide:
Under the name baryta Barium hydroxide is used in homeopathic remedies.
Barium hydroxide is also used to clean up acid spills.
Also under the name of baryta Barium hydroxide is used in the production of photographic paper for printing.

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

We also know the barium hydroxide as ‘baryta’ with the formula i.e. Ba(OH)2. 
Barium hydroxide is a powder that is crystal white in color and has no odor. 
Moreover, Barium hydroxide is very poisonous in nature due to some of its dangerous characteristics. 
Barium hydroxide is ionic in nature for example, Ba(OH)2(barium hydroxide) in aqueous solution can give 2 hydroxide ions/molecule. 
However, the barium hydroxide is the only reagent we describe for metalizing carboxamides. 
In addition, the barium hydroxide was less degradative than the barium oxide. 
Let’s take a look at Barium Hydroxide Formula below.

What is Barium Hydroxide?
Barium Hydroxide is the chemical compound with the formula Ba(OH)2. 
Barium Hydroxide can be prepared by dissolving Barium Oxide (BaO) in water:
BaO + 9 H2O → Ba(OH)2·8H2O
Barium hydroxide crystallizes as the Octahydrate, which converts to the Monohydrate upon heating in air. 
Both grades are used frequently in PVC Stabilizers / Lubricants as well as an excellent heat stabilizer. 

Formula and Structure of Barium hydroxide:
The barium hydroxide has a chemical formula i.e. Ba(OH)2. 
Barium hydroxide can be available in 3 types that are anhydrous, monohydrate and octal hydrate with the molar mass of 171.34 g mol-1, 189.955 and 315.46 g mol-1respectively. 
The structure of the compound is formed with 2 hydroxyl anions, (OH–) and 1 barium cation (Ba2+).

If Barium hydroxide is hydrated then one or eight water molecules will be in the surrounding of the cations and the anions. 
In addition, Barium hydroxides chemical structure is present below in the form of an image, in the common representations that we basically use for the organic molecules.

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

What are the uses of barium hydroxide?
Industrially, barium hydroxide is used as a precursor to several other barium compounds. 
The monohydrate of this compound is widely used to dehydrate and extract sulfate from different products. 
The very low solubility of barium sulfate is utilized in this application.

How is barium hydroxide prepared?
Barium hydroxide is usually prepared by dissolving barium oxide (chemical formula: BaO) in water. 
The chemical equation for this reaction is provided below.
BaO + 9 H2O → Ba(OH)2·8H2O
Barium hydroxide can be noted that this compound crystallizes into the octahydrate form, which is then converted into a monohydrate by heating it in air.

What happens when barium hydroxide is heated?
When heated to 800° C, barium hydroxide decomposes to yield barium oxide. 
Barium carbonate is provided by reaction with carbon dioxide. 
The strongly alkaline, aqueous solution undergoes neutralization reactions with acids.

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]

Stability of Barium hydroxide:
Barium hydroxide is a stable compound. 
Barium hydroxide is incompatible with carbon dioxide, acids, and moisture. 
Barium hydroxide is necessary to avoid making contact with this substance with incompatible materials.

Appearance of Barium hydroxide: Barium hydroxide is a crystalline substance that can range from white to transparent in appearance.
Specific Gravity: The specific gravity of Barium hydroxide is 2.18.
Melting Point: Barium hydroxide melts at a temperature of 408 °C.
Boiling Point: Barium hydroxide boils at a temperature of 780 °C.

pH Value of Barium hydroxide:
The ph value of barium hydroxide actually depends on Barium hydroxides concentration. 
That said, the pH of Barium hydroxide is around -2. 
This indicates that Barium hydroxide is highly basic in nature.

Density: Barium hydroxide has a density of 2.18 per g cm-3
Molecular Formula: The molecular formula of Barium Hydroxide Octahydrate is BaH18O10.

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

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