Barium chloride or BaCl2 is a white crystalline salt commonly used in laboratory experiments to test for sulfate ions. It is also used in the production of pigments, fireworks, and rat poisons.
| IUPAC Name | Barium chloride |
| Molecular Formula | BaCl2 |
| CAS number | 10361-37-2 |
| Synonyms | Barium dichloride, Barium chloride dihydrate, Barium(II) chloride, Barium(2+) chloride |
| InChI | InChI=1S/Ba.2ClH/h;2*1H/q+2;;/p-2 |
Barium chloride formula
The chemical formula for Barium chloride is BaCl2. It represents the number and types of atoms in one molecule of Barium chloride. The formula can be used to calculate the molar mass, as well as the number of moles of Barium chloride in a given mass or volume of the substance. The formula also indicates that one molecule of Barium chloride contains one Barium atom and two Chlorine atoms.
Barium chloride molar mass
Molar mass of BaCl2 is 208.23 g/mol. Molar mass is defined as the mass of one mole of a substance. In the case of Barium chloride, one mole of the substance contains 1 atom of Barium and 2 atoms of Chlorine. Molar mass is an important parameter for calculating the quantities of reactants and products in chemical reactions. It is also used in determining the concentration of solutions in chemistry.
Barium chloride boiling point
The boiling point of Barium chloride is 1560 °C (2836 °F). This temperature is the point at which Barium chloride transitions from a liquid to a gaseous state. The high boiling point of Barium chloride can be attributed to its ionic bond structure. The strong electrostatic attraction between the Barium cation and Chlorine anions requires a large amount of energy to break the bonds and vaporize the compound.
Barium chloride melting point
The melting point of Barium chloride is 963 °C (1765 °F). This temperature is the point at which Barium chloride transitions from a solid to a liquid state. The high melting point of Barium chloride can also be attributed to its ionic bond structure. The strong electrostatic attraction between the Barium cation and Chlorine anions requires a large amount of energy to break the bonds and melt the compound.
Barium chloride density g/ml
The density of Barium chloride is 3.856 g/cm³. Density is defined as the amount of mass per unit volume of a substance. Barium chloride has a relatively high density due to its ionic bond structure. It is denser than water, which has a density of 1 g/cm³.
Barium chloride molecular weight
The molecular weight of Barium chloride is 208.23 g/mol. Molecular weight is the sum of the atomic weights of all atoms in a molecule. In the case of Barium chloride, it is the sum of the atomic weights of one Barium atom and two Chlorine atoms.
Barium chloride Structure
Barium chloride has an ionic crystal lattice structure. It consists of Barium cations (Ba2+) and Chlorine anions (Cl-) arranged in a three-dimensional array. Each Barium cation is surrounded by eight Chlorine anions, and each Chlorine anion is surrounded by eight Barium cations. This structure is responsible for the properties of Barium chloride, such as its high melting and boiling points, and its solubility in water.
| Appearance | White crystalline solid |
| Specific Gravity | 3.856 g/cm³ |
| Color | Colorless |
| Odor | Odorless |
| Molar Mass | 208.23 g/mol |
| Density | 3.856 g/cm³ |
| Melting Point | 963 °C (1765 °F) |
| Boiling Point | 1560 °C (2836 °F) |
| Flash Point | Not applicable |
| Water Solubility | 34.0 g/100 mL (0 °C) 35.7 g/100 mL (20 °C) |
| Solubility | Soluble in water, ethanol, methanol, acetone |
| Vapor Pressure | Negligible at room temperature |
| Vapor Density | Not applicable |
| pKa | Not applicable |
| pH | 5.0 – 9.0 (10 g/L, H₂O, 20 °C) |
Barium chloride Safety and Hazards
Barium chloride can pose safety hazards if not handled and stored properly. It is corrosive and can cause severe eye, skin, and respiratory tract irritation. It can also be harmful if ingested or inhaled, causing nausea, vomiting, and diarrhea. Store Barium chloride tightly sealed and away from oxidizing agents and acids. When handling, wear gloves and goggles for personal protection. Wash skin and eyes immediately if exposed. Seek medical attention promptly if ingested.
| Hazard Symbols | Corrosive |
| Safety Description | Avoid inhalation, ingestion, skin and eye contact. Wear protective clothing and gloves. In case of contact, wash affected area with water. |
| UN IDs | UN1564 |
| HS Code | 28273990 |
| Hazard Class | 6.1 (Poisonous material) |
| Packing Group | II |
| Toxicity | Highly toxic; may be fatal if ingested. |
Barium chloride Synthesis Methods
BaCl2 can be synthesized through various methods.
- One method involves adding barium carbonate to hydrochloric acid, producing BaCl2 and carbon dioxide gas. The mixture is heated and filtered to remove solid impurities. The resulting solution is then evaporated to yield solid BaCl2.
- Another method involves the reaction between barium sulfate and carbon, followed by reaction with hydrochloric acid. This method produces BaCl2 and hydrogen sulfide gas, which is removed. The resulting solution is then evaporated to yield solid BaCl2.
- A third method involves the reaction between barium hydroxide and hydrochloric acid. This method produces BaCl2 and water as the only byproduct.
All synthesis methods require handling of the chemicals safely and with appropriate protective equipment. BaCl2 is highly toxic and corrosive. Appropriate safety measures must be taken to ensure the safety of the chemist and the environment.
Barium chloride Uses
BaCl2 has various uses across different industries.
- BaCl2 is used in the pigments industry to produce brilliant green and pale green pigments, and it imparts a green color to glass and ceramics.
- Laboratories use BaCl2 as a reagent to test for the presence of sulfate ions in a solution and to synthesize other chemicals like Barium hydroxide, Barium carbonate, and Barium nitrate.
- BaCl2 is employed in the purification of brine solutions to eliminate sulfate ions and impurities. This process is standard in chlorine and caustic soda production and salt purification.
- BaCl2 treats wastewater by precipitating impurities and pollutants.
- BaCl2 serves as a component in the production of lubricants, as a flux in the soldering process, and in fireworks, imparting a green color to the finished product.
Overall, BaCl2 has a wide range of applications across different industries, highlighting its versatility and importance in various chemical processes.
Questions:
What is the formula for Barium chloride?
The formula for Barium chloride is BaCl2, which represents one atom of Barium and two atoms of Chlorine. This ionic compound is formed through the transfer of electrons between the Barium and Chlorine atoms, resulting in the formation of positively charged Barium ions and negatively charged Chloride ions.
Is Barium chloride soluble in water?
Yes, Barium chloride is soluble in water. When added to water, it dissociates into its constituent ions, Barium and Chloride ions. The solubility of Barium chloride in water increases with temperature, and at 25°C, the solubility is approximately 360 g/L. The solubility of Barium chloride in water is also affected by the presence of other ions in the solution, such as sulfate ions, which can form insoluble precipitates with Barium ions.