What is Barium Chloride Definition Formula Reactions and Applications
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 Properties Preparation and Uses
1. What is barium chloride?
Barium chloride is an inorganic ionic compound with the chemical formula BaCl2 composed of barium and chlorine. It consists of Ba2+ and Cl- ions arranged in a crystal lattice. It is typically found as a white crystalline solid and is highly soluble in water. Barium chloride is commonly used in qualitative analysis, laboratory reactions, and industrial processes involving barium salts.
2. What is the formula and molar mass of barium chloride?
The formula of barium chloride is BaCl2 and its molar mass is approximately 208.23 g·mol-1. The molar mass is calculated as follows:
- Barium (Ba) = 137.33 g·mol-1
- Chlorine (Cl) = 35.45 g·mol-1 × 2 = 70.90 g·mol-1
- Total = 137.33 + 70.90 = 208.23 g·mol-1
This value is important for mole calculations and stoichiometry problems involving barium chloride.
3. Is barium chloride soluble in water?
Yes, barium chloride is highly soluble in water and dissociates completely into ions. In aqueous solution, it forms Ba2+(aq) and 2Cl-(aq) as shown:
- BaCl2(s) → Ba2+(aq) + 2Cl-(aq)
Because it is a soluble ionic compound, it is often used in precipitation reactions to test for sulfate ions.
4. What happens when barium chloride reacts with sodium sulfate?
When barium chloride reacts with sodium sulfate, a white precipitate of barium sulfate is formed. The balanced chemical equation is:
- BaCl2(aq) + Na2SO4(aq) → BaSO4(s) + 2NaCl(aq)
This is a double displacement (precipitation) reaction. The formation of insoluble BaSO4 is used as a confirmatory test for sulfate ions (SO42-).
5. Why is barium chloride used to test for sulfate ions?
Barium chloride is used to test for sulfate ions because it forms an insoluble white precipitate of barium sulfate. When BaCl2(aq) is added to a solution containing SO42-, the reaction is:
- Ba2+(aq) + SO42-(aq) → BaSO4(s)
Since BaSO4 is highly insoluble in water, the white precipitate confirms the presence of sulfate ions in qualitative analysis.
6. How is barium chloride prepared?
Barium chloride is commonly prepared by reacting barium carbonate with hydrochloric acid. The balanced equation is:
- BaCO3(s) + 2HCl(aq) → BaCl2(aq) + CO2(g) + H2O(l)
After the reaction, the solution is filtered and evaporated to obtain crystalline BaCl2. This method is widely used in laboratory preparation of barium salts.
7. Is barium chloride toxic?
Yes, barium chloride is toxic because soluble barium ions interfere with muscle and nerve function. The toxicity arises from Ba2+ ions, which can affect potassium ion channels in the body. Symptoms of poisoning may include muscle weakness, irregular heartbeat, and gastrointestinal distress. Therefore, barium chloride must be handled with proper laboratory safety precautions.
8. What type of compound is barium chloride?
Barium chloride is an ionic compound formed between a metal and a non-metal. It contains Ba2+ (a Group 2 alkaline earth metal ion) and Cl- ions held together by strong electrostatic forces. As an ionic salt, it:
- Has a high melting point
- Dissolves in water to form ions
- Conducts electricity in molten or aqueous state
These properties are typical of ionic compounds in inorganic chemistry.
9. What happens when barium chloride reacts with sulfuric acid?
When barium chloride reacts with sulfuric acid, insoluble barium sulfate and hydrochloric acid are formed. The balanced equation is:
- BaCl2(aq) + H2SO4(aq) → BaSO4(s) + 2HCl(aq)
This is a double displacement reaction driven by the formation of solid BaSO4, which precipitates out of solution.
10. What are the common uses of barium chloride?
Barium chloride is commonly used in laboratories, industry, and chemical analysis. Major uses include:
- Testing for sulfate ions in qualitative analysis
- Manufacturing heat-treatment salts
- Producing other barium compounds
- Water purification and pigment production
Its high solubility and ability to form insoluble BaSO4 make it especially important in analytical chemistry.
