What is Barium Chloride BaCl₂?
Barium Chloride (BaCl₂) is an inorganic salt that is composed of Barium cations (Ba⁺) and Chloride anions (Cl⁻). It is also named Barium dichloride or Barium Muriate. It is a white solid chemical compound which is soluble in water, it is hygroscopic, and provides a frail yellow-green colour when put to a flame. BaCl₂ is the chemical formula of Barium Chloride. Barium salts are widely used in the industry. The sulfate is applied in white paints, especially for external use. Barium chloride is toxic in nature.
Structure of Barium Chloride BaCl₂
The chemical formula of Barium Chloride is BaCl₂, and the molar mass of Barium Chloride is 208.23 g mol⁻¹. This salt is formed by one Barium cation (Ba²⁺) and one Chloride anion (Cl⁻). The crystals can be cubic fluorite or orthorhombic. Its chemical structure can be formulated as below, in the common representations applied for organic molecules.
Cl⁻ Cl⁻
Ba²⁺
Preparation of Barium Chloride
Hydrochloric acid (concentrated) 180 ml is diluted with 440 ml of water and emptied in a porcelain evaporating dish. The solid Barium Carbonate in tiny portions is added and mixed after. If Barium Carbonate is added too quickly, the mixture will churn out of the dish. After Barium Carbonate is added, and the solution becomes neutral to litmus, the mixture is ignited to boiling. If Barium Carbonate comprises iron as an impurity, it can be excluded by adding 3g of Barium Peroxide and boiling the solution gently for 5 minutes. The Barium Chloride hot solution is diluted to 600 ml and filtered without suction to a 600 ml beaker, keeping both the beaker and the funnel closed to prevent the solution from crystallizing and cooling untimely. 10 ml of diluted Hydrochloric acid is added to the filtrate, to sustain the acidic medium. After that, the liquid is discharged into the crystallizing dish and left to stand open until a good number of crystals is achieved. The obtained crystals are emptied and cleaned with a small amount of distilled water. Finally, Barium Chloride is entirely wilted in the desiccator at room temperature.
BaCo₃ + 2HCl⟶ BaCl₂ + CO₂ + H₂O
Barium Sulfate at high temperature,
BaSO4 + 4C → BaS + 4CO
Properties of Barium Chloride BaCl₂
Barium Chloride is dispersible in water. It is identified to separate into chloride anions and barium cations when it is dissolved. At a temperature of 20℃, the solubility of Barium Chloride in water is roughly equal to 358 grams per liter. However, the solubility of this mixture in water is temperature-dependent. At 100℃, barium chloride solubility in water is equivalent to 594 grams per liter. This compound is also dissolvable in methanol but not soluble in ethanol. Anhydrous BaCl₂ crystallizes in an orthogonal crystal formation. However, the dihydrate formation of Barium Chloride is identified to have a monoclinic crystal structure.
Uses of Barium Chloride BaCl₂
It is used in wastewater treatment.
It is used in the making of oil lubricants, PVC stabilizers, barium chromate, and barium fluoride.
It is used in the purification of brine (saline) solution in caustic chlorine plants.
It is used as a test for sulfate ion.
It is used in the purification of the manufacture of heat treatment salts.
It is used in the case hardening of steel.
It is used in the production of pigments.
It is used in the manufacture of different barium salts.
It is used used in fireworks to give a bright green colour.
Chemical and Physical Properties
Chemical Properties:
Barium chloride behaves with water like any other binary chlorine salt. It dissociates in water to produce NaCl-like ions. It remains neutral and does not affect the pH of the solution. BaCl2 → Ba2 ++ 2Cl–
When a solution of barium chloride is mixed with sodium sulfate, barium chloride causes a double substitution reaction. At the bottom of the test tube, you will see a white precipitate of barium sulphate is immediately formed. This is an ionic reaction. BaCl2 + Na2SO4 → BaSO4 (ppt.) + 2NaCl.
Physical Properties
Barium chloride is crystalline, orthorhombic in the anhydrous form, and monoclinic in the dehydrated form.
The molecular weight of this compound is 208.23 g / mol for anhydrous and 244.26 for dehydrate, density is 3.856 g / ml for anhydrous and 3.098 g / ml for dihydrate, and their melting point and boiling point are 963 ° C and 1560 ° C, respectively.
Barium chloride is very soluble in water and can dissolve 35.8 grams of compound in 100 ml of solvent.
Preparation of Barium Chloride
Barium chloride is not naturally occurring; instead, a 2 step reaction process is performed to obtain them. First, barium sulfate is heated to a high temperature together with carbon to produce barium sulfide and carbon monoxide. Second, this barium sulfide reacts with hydrogen chloride to form barium chloride.
BaSO4 + 4C → BaS + 4CO
BaS + 2HCl → BaCl2 + H2S
Health Hazards Caused due to Barium Chloride
Due to its high toxicity, Barium Chloride has very limited use even in laboratories. Barium chloride is toxic and irritates the eyes, skin, and mucous membranes when in contact. It can even prove to be fatal if inhaled, swallowed, or absorbed through the skin. Barium chloride poisoning can affect the kidneys, cardiovascular system, and central nervous system. It also poses a serious threat to aquatic life.
If it gets in your eyes, make sure you are not wearing contact lenses and in case you are then remove them immediately. Rinse your eyes with cold running water for at least 15 minutes with your eyelids open. If chemicals come into contact with clothing, remove them as soon as possible to protect your hands and body and stand under the cold shower as soon as possible. If inhaled, the victim must stand in a well-ventilated area. In the event of severe inhalation, the victim should evacuate to a safe place as soon as possible.
If swallowed, induce vomiting in the patient as soon as possible only if they are conscious otherwise perform mouth-to-mouth resuscitation.
FAQs on Barium Chloride
1. What are the uses of Barium Chloride?
Barium chloride, though very toxic, is widely used in laboratories and in industries such as paper making, firework industry, oil refining, wastewater treatment, production of rubber, hardening of steel, thermal treatment of salts, etc.
2. What are the health hazards caused by Barium Chloride?
They are very toxic and can be very deadly if they come in contact with the skin, inhaled or ingested. It can cause severe burns, irritation, kidney failure, poison cardiovascular system, and breakdown of the central nervous system.
3. Is Barium chloride ionic bond or a covalent bond?
Barium Chloride forms an ionic bond as both its reactants are ionic in nature. Hence, it is an ionic compound.
4. What happens when Barium Chloride is mixed in water?
Barium chloride is known to dissolve easily in water. It will remain in its neutral state and will not affect the pH of the solution.
5. How is Barium Chloride produced?
Barium chloride is not naturally occurring; instead a 2 step reaction process is performed to obtain them. First, barium sulfate is heated to a high temperature together with the carbon to produce barium sulfide and carbon monoxide. Second, this barium sulfide reacts with hydrogen chloride to form barium chloride.
6. Is Barium Chloride Lethal or Toxic?
Yes, like most Barium salts BaCl₂ is also toxic. The soluble compounds of Barium and Ba+2 ion, mainly nitrate, chloride, hydroxide are lethal to humans. It causes irritation to the eye, skin, and mucous membrane. The inhalation or ingestion of Barium Chloride can also be very deadly. Barium Chloride negatively affects the cardiovascular system, the central nervous system, and the kidneys. It is also toxic to aquatic life. The antidote for poison caused by BaCl₂ is the magnesium or sodium sulfate.
7. What is Barium Chloride Dihydrate?
Barium Chloride Dihydrate is an optimal source of barium for high purity constructions and methods in the optical, electronic, and pharmaceutical industries. Due to its solubility, Barium Chloride Dihydrate is an ideal source of barium, primarily when the pH of the solution is not altered. Barium Chloride Dihydrate is generally used for the production of Barium Titanate by the method of oxalate in rendering special glass and in the manufacture of pharmaceutical intermediates. It is also used in wastewater treatment for the sulfate ion efficient extraction.