Barium Hydroxide Acid Or Base

Barium Hydroxide Formula: Definition, Molar Mass, IUPAC ID

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Barium Hydroxide Formula: Did you know Baryta or Baryta water is chemically known as Barium hydroxide? It is white and granular and 1 of the principal compounds of Barium. Let's larn everything about the chemical chemical compound barium hydroxide and its chemical formula in particular.

Barium Hydroxide Formula and Structure

The chemical formula of Barium Hydroxide is \({\rm{Ba(OH)}}_2\). It is available in \(3\) forms – Anhydrous, Monohydrate, and Octahydrate. The structure of barium hydroxide consists of \(2\) hydroxyl anions \(({\rm{OH}}^-)\) and one barium cation \(({\rm{Ba}}^{ii+})\).

Preparation of Barium Hydroxide

Barium hydroxide is produced by the reaction of barium oxide\(({\rm{BaO}})\) with the water \(({\rm{H}}_2 {\rm{O}})\).

\({\text{BaO}} + 9{{\text{H}}_2}{\text{O}} \to {\text{Ba}}{\left( {{\text{OH}}} \right)_2} \cdot eight{{\text{H}}_2}{\text{O}}\).

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Physical Properties of Barium Hydroxide

The physical backdrop of barium hydroxide are given below:

Barium hydroxide is an odourless, poisonous, white coloured solid.
The molar mass of Barium Hydroxide is \(171.34\;{\rm{grand/mol}}\).
The melting indicate of Barium Hydroxide varies depending on how much h2o is nowadays. At \(78\) degrees Celsius, the octahydrate phase melts. The monohydrate phase melts at \(300\) degrees Celsius, while the anhydrous form melts at \(407\) degrees Celsius.
All three forms are partially soluble with water at low temperatures. Notwithstanding, the solubility of barium hydroxide in water increases with the increase in temperature.
Barium hydroxide has a density of \(3.743\;{\rm{g/mL}}\) (in monohydrate grade) and \(ii.xviii\;{\rm{g/mL}}\) (in octahydrate form).
Barium Hydroxide boils at \(780\) degrees Celsius and decomposes into Barium oxide at a temperature above \(800\) degrees Celsius.

Chemical Properties of Barium Hydroxide

The chemical properties of barium hydroxide are explained below:

Barium hydroxide is ionic in nature, i.e., in an aqueous solution, it can furnish two hydroxide or hydroxyl ions/molecule.
If it is hydrated, then one or eight h2o molecules will be in the surrounding of the cations and the anions.
Barium hydroxide on dissolution produces brine solutions. This happens due to the release of hydroxyl anions. Hence, it undergoes neutralization reactions with acids.
It undergoes a neutralization reaction with sulphuric and phosphoric acids to form useful barium salts such as barium sulphate and barium phosphate.
When heated above \(800^\circ {\rm{C}}\), Barium hydroxide decomposes into barium oxide.
Barium hydroxide reacts with carbon dioxide to form barium carbonate whereas, hydrogen sulphide information technology forms barium sulphide.
A double replacement reaction forms many insoluble or less soluble barium salts when the barium hydroxide aqueous solution is mixed with other metal salts.
An endothermic reaction takes place when barium hydroxide reacts with ammonium salts.

Uses of Barium Hydroxide

The uses of barium hydroxide are explained beneath:

It is used every bit a source of Barium to produce certain barium salts such every bit barium phosphate, barium sulfide, and barium sulfate.
It is besides used in the analytical standard for the titration of weak acids.
It is used in the manufacture of glass, oil, alkalis and grease additives, barium soaps, and other barium compounds.

Health Risks of Barium Hydroxide

The health risks of barium hydroxide are explained beneath:

Inhalation of barium dust can cause respiratory tract irritation and may produce benign pneumoconiosis known as baritosis.
Barium ions are toxic to muscles and may cause paralysis.
It is an extremely dangerous neurotoxin that has adverse furnishings on the heart and the central nervous system (CNS).

Summary

Barium hydroxide is ane of the chief compounds of Barium. It is a precursor to the synthesis of many barium salts. Its reaction with ammonium chloride is an important endothermic reaction. In this article, nosotros learned the chemical formula, structure, properties, and uses of Barium hydroxide.

FAQs on Barium Hydroxide Formula

Q.ane. What is the formula for barium hydroxide?
Ans: The chemical formula of Barium Hydroxide is \({\rm{Ba(OH)}}_2\). It is available in \(iii\) forms – Anhydrous, Monohydrate, and Octahydrate. The construction of barium hydroxide consists of \(2\) hydroxyl anions \(({\rm{OH}}^-)\) and one barium cation \(({\rm{Ba}}^{2+})\).

Q.2. Why is there a \(ii\) in barium hydroxide formula?
Ans: Barium belongs to the group of alkaline earth metals. These elements tin lose two outermost electrons to attain the noble gas configuration. A charge of \(+2\) is available on these metals. Hydroxide is a negative polyatomic ion with a value of \(one\), and \(-i\) is the charge. They substitution their charges to form an ionic chemical compound \({\rm{Ba(OH)}}_2\).

Q.iii. Is Barium Hydroxide a base or an acid?
Ans: Barium Hydroxide, like \({\rm{NaOH}}\) and \({\rm{KOH}}\), is a stable base. Barium Hydroxide is a metal hydroxide of grouping IIA that dissolves in water to produce hydroxyl ions.

Q.4. What is the charge on \({\rm{Ba(OH)}}_2\)?
Ans: Barium is an atom that belongs to Group \(two\) of the Mod Periodic Table, so it has two valence electrons, and its accuse is \(+two\). Hydroxide is a negative polyatomic ion with a value of \(1\), and \(-ane\) is the charge. They mix to form an ionic compound with no overall charge.

Q.5. What happens when barium hydroxide is heated?
Ans: When heated above \(800^\circ {\rm{C}}\), Barium hydroxide decomposes into barium oxide.

Q.6. What happens when Barium hydroxide is mixed with ammonium chloride?
Ans: When Barium hydroxide is mixed with ammonium chloride, an endothermic reaction takes place. Ammonium Chloride is slightly acidic, whereas Barium Hydroxide is a stiff base of operations. This acrid-base of operations reaction will result in the formation of Barium chloride, ammonia, and h2o.
\({\text{Ba}}{\left( {{\text{OH}}} \right)_2} + two{\text{N}}{{\text{H}}_4}{\text{Cl}} \to {\text{BaC}}{{\text{l}}_2} + 2{\text{Northward}}{{\text{H}}_3} + 2{{\text{H}}_2}{\text{O}}\).

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