Barium Chloride Formula: Barium chloride is an inorganic salt formed by barium and chlorine. Since barium \(\left( {{\rm{Ba}}} \right)\) is a metal and chlorine \(\left( {{\rm{Cl}}} \right)\) is a nonmetal, they combine to form an ionic bond. Barium forms as cation \({\rm{B}}{{\rm{a}}^{{\rm{2 + }}}}\) and chlorine forms an anion \({\rm{C}}{{\rm{l}}^ – },\) both combine to form barium chloride having the chemical formula \({\rm{BaC}}{{\rm{l}}_2}.\) It is a white solid also known as Barium Muriate, Muryate of Barytes, or Barium dichloride.

Barium chloride is soluble in water. It is hygroscopic and gives yellow-green colour in the flame test. This helps to detect the presence of \({\rm{B}}{{\rm{a}}^{{\rm{2 + }}}}\) ions in \({\rm{BaC}}{{\rm{l}}_2}.\) This inorganic compound is used for various purposes, such as in the paint industry, paper-making industry, oil refining, chlorine-alkali industry, etc. In this article, we will learn about the chemical formula, properties, and uses of barium chloride in detail.

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Chemical Formula and Structure of Barium Chloride

The chemical formula of Barium chloride is \({\rm{BaC}}{{\rm{l}}_2}.\) As it is an ionic compound, Barium chloride dissociates in water to form \({\rm{B}}{{\rm{a}}^{{\rm{2 + }}}}\) cation and \({\rm{C}}{{\rm{l}}^ – }\) anion. It is a water-soluble compound. As inferred from the chemical formula itself, \({\rm{BaC}}{{\rm{l}}_2}\) is formed from one \({\rm{B}}{{\rm{a}}^{{\rm{2 + }}}}\) cation and two \({\rm{C}}{{\rm{l}}^ – },\) anions. The crystalline structure of barium chloride is either cubic fluorite or orthorhombic. When dissolved in water, it behaves as a simple salt and maintains a neutral \({\rm{pH}}.\)

The chemical formula of Barium chloride is derived by the “Criss-cross method.”

When we investigate the periodic table, we can see that barium is a metal that belongs to Group \(2,\) and chlorine is a nonmetal that belongs to Group \(17.\) Barium readily loses two electrons to form \({\rm{B}}{{\rm{a}}^{2 + }}\) cation and chlorine tends to gain an electron to complete its octet and thus gain \(-1\) charge, forming \({\rm{C}}{{\rm{l}}^ – }\) anion. Both \({\rm{B}}{{\rm{a}}^{2 + }}\) cation and \({\rm{C}}{{\rm{l}}^ – }\) anion will transfer their charge to each other in a criss-cross method, i.e., \(+2\) charge of barium will go to chlorine, and \(-1\) charge of chlorine will go to barium. In this manner, a new compound, barium chloride, with the chemical formula \({\rm{BaC}}{{\rm{l}}_2}\) is formed with a net zero charge. \({\rm{BaC}}{{\rm{l}}_2}\) is an ionic compound.

Physical Properties of Barium Chloride

Chemical Formula	\({\rm{BaC}}{{\rm{l}}_2}\)
Molar mass	\(208.23\,{\rm{gmo}}{{\rm{l}}^{ – 1}}\) (anhydrous) \(244.26\,{\rm{gmo}}{{\rm{l}}^{ – 1}}\) (dihydrate)
Density	\(3.856\,{\rm{gc}}{{\rm{m}}^{ – 3}}\) (anhydrous) \(3.097\,{\rm{gc}}{{\rm{m}}^{ – 3}}\) (dihydrate)
Melting Point	\({962^{\rm{o}}}{\rm{C}}\)
Boiling Point	\({1560^{\rm{o}}}{\rm{C}}\)
Appearance and Texture	White solid powder

Chemical Properties of Barium Chloride

1. Barium chloride shows similar behaviour with water as other binary chlorine salts show. It dissociates in water to produce ions like \({\rm{NaCl}}.\) It does not affect the \({\rm{pH}}\) of the solution as it remains in a neutral state.
\({\rm{BaC}}{{\rm{l}}_2} \to {\rm{B}}{{\rm{a}}^{2 + }} + 2{\rm{C}}{{\rm{l}}^ – }\)
2. Barium chloride gives a double displacement reaction when mixing a solution of barium chloride with sodium sulphate; a white precipitate of barium sulphate is immediately formed at the bottom of the test tube. This is an ionic reaction.
\({\rm{BaC}}{{\rm{l}}_2} + {\rm{N}}{{\rm{a}}_2}{\rm{S}}{{\rm{O}}_4} \to {\rm{BaS}}{{\rm{O}}_4}\left( {{\rm{ppt}}.} \right) + 2{\rm{NaCl}}\)

Preparation of Barium Chloride

Barium chloride does not exist naturally. It is prepared by conducting a two-step reaction. Firstly, Barium sulphate is heated with carbon at a high temperature to form barium sulphide and carbon monoxide. Secondly, this Barium sulphide reacts with Hydrogen chloride to form Barium chloride.
\({\rm{BaS}}{{\rm{O}}_4} + 4{\rm{C}} \to {\rm{BaS}} + 4{\rm{CO}}\)
\({\rm{BaS}} + 2{\rm{HCl}} \to {\rm{BaC}}{{\rm{l}}_2} + {{\rm{H}}_2}{\rm{S}}\)

Uses of Barium Chloride

1. Barium chloride is used in the firework industry as it produces a green flame on burning.
2. It is used in chlorine-alkali industries to separate sulphate as it precipitates as barium sulphate.
3. Barium chloride is used as a raw material to prepare barium salts.
4. Barium chloride is used in the manufacturing of rubber.
5. It is used in paper industries.
6. Barium chloride is also used in the case of the hardening of steel.
7. We also use it in the thermal treatment of salts.
8. Barium chloride is also used in the petroleum industry, mostly in oil refining.
9. Brine purification is also done by using barium chloride.

Health Hazards of Barium Chloride

Barium chloride has limited use in the laboratory due to its toxicity. It is highly toxic when ingested or inhaled. Barium chloride is toxic and causes irritation in the eyes, skin, and mucous membrane if it comes in contact. It may even be fatal if inhaled, swallowed, or absorbed through the skin. Poisoning caused due to barium chloride may affect the kidneys, cardiovascular system, and central nervous system. It causes serious threats to aquatic life also.

Summary

Barium chloride is an inorganic compound formed by the elements barium and chlorine. As barium \(\left( {{\rm{Ba}}} \right)\) is a metal and chlorine \(\left( {{\rm{Cl}}} \right)\) is a nonmetal, they both combine to form an ionic compound. The chemical formula of barium chloride is \({\rm{BaC}}{{\rm{l}}_2}.\) It is a white solid and is hygroscopic in nature. It gives yellow-green colour in the flame test. Barium chloride has various uses such as in the paint industry, paper-making industry, oil refining, chlorine-alkali industry, etc. This compound is not available in nature; rather, it is prepared mostly by heating barium sulphate with carbon at high temperatures. Though \({\rm{BaC}}{{\rm{l}}_2}\) is useful in some industries, but it is highly toxic to living beings. Due to its toxicity, its use is minimized in some cases where a substitute can work.

FAQs on Barium Chloride Formula

Q.1. What is the name of \({\rm{BaC}}{{\rm{l}}_2}\)?
Ans: The name of \({\rm{BaC}}{{\rm{l}}_2}\) is barium chloride. It is formed by the exchange of charges between \({\rm{B}}{{\rm{a}}^{2 + }}\) cation and \({\rm{C}}{{\rm{l}}^ – }\) anion in a ‘criss-cross method.’

Q.2. What type of chemical bond is present in barium chloride?
Ans: An ionic bond is formed in barium chloride because barium is metal, and chlorine is a nonmetal. When a metal and a nonmetal combine, an ionic bond is formed. Barium forms as cation \({\rm{B}}{{\rm{a}}^{2 + }}\) and chlorine forms an anion \({\rm{C}}{{\rm{l}}^ – },\) both combine to form barium chloride having the chemical formula \({\rm{BaC}}{{\rm{l}}_2}.\)

Q.3. Is Barium and Bromine ionic?
Ans: Both barium and bromine are elements. Barium is a metal of Group \(2\) of Modern Periodic Table, and bromine is a nonmetal of Group \(17\) of Modern Periodic Table. An element has no charge, so they are not ionic. On the other hand, barium cation \(\left( {{\rm{B}}{{\rm{a}}^{2 + }}} \right)\) and Bromide ions \(\left( {{\rm{B}}{{\rm{r}}^ – }} \right)\) are ionic.

Q.4. What happens if you mix barium and chloride ions?
Ans: When barium \(\left( {{\rm{B}}{{\rm{a}}^{2 + }}} \right)\) and chloride \(\left( {{\rm{C}}{{\rm{l}}^ – }} \right)\) ions are mixed they form a white precipitate of barium chloride \(\left( {{\rm{BaC}}{{\rm{l}}_2}} \right).\)

Q.5. Is Barium chloride toxic?
Ans: Barium chloride is highly toxic when ingested or inhaled. It causes irritation in the eyes, skin, and mucous membrane if it comes in contact. It may even be fatal if inhaled, swallowed, or absorbed through the skin. Too much exposure to this chemical compound may affect the kidneys, cardiovascular system, and central nervous system.

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