Barium chloride dihydrate, a chemical compound frequently utilized in laboratory settings, possesses a specific barium chloride dihydrate molar mass crucial for accurate stoichiometric calculations. Titration experiments, a quantitative analytical technique common in chemistry, rely on precise knowledge of this molar mass to determine concentrations of solutions. Sigma-Aldrich, a prominent supplier of chemical reagents, provides barium chloride dihydrate with rigorously defined specifications, including its molar mass, ensuring reproducibility in research. Understanding this value is also essential for applications in industrial processes, particularly those involving wastewater treatment, where barium chloride dihydrate is sometimes employed to precipitate sulfates.
Unveiling Barium Chloride Dihydrate (BaCl₂·2H₂O): A Foundational Compound
Barium Chloride Dihydrate, chemically denoted as BaCl₂·2H₂O, is an inorganic compound that holds a significant position in both scientific research and industrial processes. Its distinct chemical formula immediately reveals its composition: a barium chloride molecule complexed with two water molecules.
Defining Barium Chloride Dihydrate
At its core, Barium Chloride Dihydrate is a hydrate, meaning it incorporates water molecules within its crystalline structure. This differentiates it from anhydrous barium chloride (BaCl₂), which lacks these water molecules.
The presence of water impacts several of its properties, including its solubility and crystalline appearance. Understanding this fundamental distinction is crucial for predicting its behavior in various chemical reactions and applications.
Significance Across Diverse Fields
The importance of Barium Chloride Dihydrate stems from its versatile applications across a multitude of fields. It serves as a critical laboratory reagent, utilized in qualitative and quantitative analyses.
Its role extends to industrial manufacturing, where it contributes to processes like the production of pigments and the purification of brine solutions. Its ability to react with sulfate ions makes it particularly valuable in certain applications.
Historical Context and Modern Applications
Historically, Barium Chloride Dihydrate has been employed in various processes, ranging from early photographic techniques to the synthesis of other barium compounds.
Today, its applications have evolved. It remains a key component in specialized chemical syntheses, analytical procedures, and select industrial processes.
Its enduring presence underscores its continued relevance in modern science and technology. A thorough understanding of its properties is not only academically valuable but also essential for safe and effective utilization in various practical scenarios.
Deciphering Chemical Properties: Molar Mass, Solubility, and Toxicity
Having established the foundational identity of Barium Chloride Dihydrate, it is imperative to delve into its key chemical properties. These properties dictate its behavior in various applications and, critically, inform the necessary safety precautions for handling this compound. We will explore its molar mass, solubility characteristics, and toxicity profile, each of which plays a vital role in its use and potential hazards.
Molar Mass: A Fundamental Constant
The molar mass of a compound is a fundamental property, representing the mass of one mole of that substance. It is essential for stoichiometric calculations, allowing us to convert between mass and moles, which is crucial in quantitative chemical analysis and synthesis.
Calculating Molar Mass
The molar mass of Barium Chloride Dihydrate (BaCl₂·2H₂O) is calculated by summing the atomic masses of each element in the compound, taking into account the number of atoms of each element. Atomic masses are obtained from the periodic table.
For BaCl₂·2H₂O, the calculation proceeds as follows:
- Barium (Ba): 1 atom × 137.33 g/mol = 137.33 g/mol
- Chlorine (Cl): 2 atoms × 35.45 g/mol = 70.90 g/mol
- Hydrogen (H): 4 atoms × 1.01 g/mol = 4.04 g/mol
- Oxygen (O): 2 atoms × 16.00 g/mol = 32.00 g/mol
Adding these values together, we obtain the molar mass of BaCl₂·2H₂O:
- 33 + 70.90 + 4.04 + 32.00 = 244.27 g/mol.
The unit of measurement is grams per mole (g/mol), reflecting the mass of one mole of the compound.
Solubility: Interaction with Solvents
The solubility of Barium Chloride Dihydrate refers to its ability to dissolve in a solvent, typically water. Solubility is influenced by several factors, most notably temperature and the nature of the solvent.
Factors Affecting Solubility
Temperature plays a significant role in the solubility of most ionic compounds, including Barium Chloride Dihydrate. Generally, solubility increases with increasing temperature, as higher temperatures provide more energy to break the crystal lattice and allow ions to disperse in the solvent.
The solvent also plays a crucial role. While Barium Chloride Dihydrate is readily soluble in water, it is generally insoluble in organic solvents. This is due to the polar nature of water, which effectively solvates the ions, compared to the non-polar nature of many organic solvents.
Quantitative Data and Applications
The solubility of Barium Chloride Dihydrate in water is approximately 370 g/L at 20°C. At higher temperatures, such as 100°C, the solubility increases to around 590 g/L. This information is critical in applications such as precipitation reactions, where controlled solubility is essential.
Barium Chloride Dihydrate’s solubility properties are exploited in precipitation reactions. For example, it is commonly used to test for the presence of sulfate ions (SO₄²⁻) in a solution. The addition of Barium Chloride Dihydrate to a solution containing sulfate ions will result in the formation of a white precipitate of Barium Sulfate (BaSO₄), which is practically insoluble in water.
Toxicity: A Critical Safety Consideration
The toxicity of Barium Chloride Dihydrate is a serious concern that necessitates careful handling and adherence to strict safety protocols. Barium compounds are generally toxic, and exposure can lead to adverse health effects.
Acute and Chronic Effects
Acute toxicity refers to the harmful effects that occur shortly after exposure to a substance. In the case of Barium Chloride Dihydrate, acute exposure can cause symptoms such as nausea, vomiting, abdominal pain, muscle weakness, and even cardiac irregularities.
Chronic toxicity refers to the harmful effects that develop over a prolonged period of exposure. Chronic exposure to Barium Chloride Dihydrate can lead to more severe health problems, including kidney damage, hypertension, and paralysis.
Mechanism of Toxicity
The toxicity of Barium Chloride Dihydrate stems from the Barium ion (Ba²⁺), which can interfere with various physiological processes. Barium ions can block potassium channels, disrupting nerve and muscle function. This disruption can lead to the aforementioned symptoms of toxicity.
Importance of Safe Handling
Given the toxicity of Barium Chloride Dihydrate, handling with care and proper safety measures are paramount. This includes wearing appropriate personal protective equipment (PPE), such as gloves, goggles, and lab coats, to prevent skin contact and ingestion. It also involves working in a well-ventilated area to minimize inhalation of dust or vapors. In the event of accidental exposure, immediate medical attention is crucial.
The toxicity of Barium Chloride Dihydrate should never be underestimated. Proper safety practices are not merely recommendations, but essential requirements for anyone working with this compound.
Unlocking the Formula: Chemical Composition and Structure
Having established the foundational identity of Barium Chloride Dihydrate, it is imperative to delve into its key chemical properties. These properties dictate its behavior in various applications and, critically, inform the necessary safety precautions for handling this compound.
This section will dissect the chemical formula, illuminating the roles of each component and providing a comprehensive understanding of its structure.
Decoding BaCl₂·2H₂O: A Molecular Breakdown
The chemical formula BaCl₂·2H₂O represents Barium Chloride Dihydrate. It signifies that each molecule of barium chloride (BaCl₂) is associated with two molecules of water (2H₂O). Understanding the relationship between these components is crucial.
The Interplay of Barium Chloride and Water
Barium chloride (BaCl₂) and water (H₂O) are distinct chemical entities. However, in Barium Chloride Dihydrate, they exist in a defined stoichiometric ratio within the crystal lattice.
The "·2H₂O" part of the formula indicates that two water molecules are incorporated into the crystal structure for every one unit of barium chloride.
Ionic Bonding in Barium Chloride
Barium chloride (BaCl₂) itself is an ionic compound. It is formed through the electrostatic attraction between barium ions (Ba²⁺) and chloride ions (Cl⁻).
Barium, a Group 2 element, readily loses two electrons to form a stable Ba²⁺ ion.
Chlorine, a Group 17 element, readily gains one electron to form a stable Cl⁻ ion. The strong electrostatic forces between these oppositely charged ions result in the formation of the ionic compound barium chloride.
Hydrate Classification: The Role of Water
Barium Chloride Dihydrate is classified as a hydrate. Hydrates are compounds that have water molecules incorporated into their crystal structure.
Water Molecules in Crystal Structure
The water molecules in Barium Chloride Dihydrate are not simply adsorbed onto the surface. They are integrated into the crystal lattice and held in place by electrostatic forces and hydrogen bonds. These water molecules play a crucial role in stabilizing the crystal structure of the hydrate.
The water molecules influence the compound’s properties, such as its melting point and appearance.
Anhydrous Barium Chloride: Stripping Away Water
The anhydrous form of barium chloride, represented as BaCl₂, lacks the water molecules found in the dihydrate.
Obtaining the Anhydrous Form
The anhydrous form can be obtained by heating Barium Chloride Dihydrate. This process removes the water molecules, leaving behind the anhydrous salt. This process requires careful control of temperature to prevent decomposition of the barium chloride.
Property Differences: Dihydrate vs. Anhydrous
Significant differences exist in the properties of the dihydrate and anhydrous forms. The dihydrate tends to be in crystalline form, whereas the anhydrous form can be hygroscopic (readily absorbs water from the air).
Navigating Chemical Nomenclature: Naming Conventions
The systematic naming of chemical compounds follows the guidelines established by the International Union of Pure and Applied Chemistry (IUPAC). This ensures clarity and consistency in chemical communication.
Deciphering the Name
The name "Barium Chloride Dihydrate" reflects its composition. "Barium Chloride" indicates the presence of Ba²⁺ and Cl⁻ ions. "Dihydrate" specifies that each formula unit is associated with two water molecules.
This naming convention allows chemists worldwide to understand the compound’s structure and composition based on its name.
Chemical Representation: Visualizing the Formula
Visual representation aids understanding of chemical formulas and structures.
From Lewis Structures to Crystal Lattices
Lewis structures, structural formulas, and crystal lattice diagrams can all be used. These help visualize the bonding and arrangement of atoms in Barium Chloride Dihydrate.
The Crystal Structure
The crystal structure of Barium Chloride Dihydrate is complex. It involves the arrangement of Ba²⁺ ions, Cl⁻ ions, and water molecules in a repeating pattern. The water molecules are coordinated to the barium ions, contributing to the stability of the crystal lattice. Understanding the crystal structure is essential for predicting its physical and chemical properties.
Decoding Chemical Identity: CAS Registry Number and PubChem CID
Having established the foundational identity of Barium Chloride Dihydrate, it is imperative to delve into its key chemical properties. These properties dictate its behavior in various applications and, critically, inform the necessary safety precautions for handling this compound.
This section elucidates the vital role of unique identifiers in the vast landscape of chemical databases. We will explore the CAS Registry Number and the PubChem CID, emphasizing their significance in the precise identification and retrieval of information pertaining to Barium Chloride Dihydrate.
The Imperative of Unique Chemical Identifiers
In the realm of chemistry, precision is paramount.
The sheer volume of known chemical substances necessitates a robust system for unambiguous identification. Unique identifiers serve as digital fingerprints, allowing researchers, industries, and regulatory bodies to accurately locate and exchange information about specific compounds. Without such identifiers, confusion and errors could easily arise, leading to potentially hazardous consequences.
CAS Registry Number: A Chemical’s Social Security Number
The CAS Registry Number (CAS RN), assigned by the Chemical Abstracts Service (CAS), is a unique numerical identifier for every chemical substance registered in the CAS registry. Think of it as a chemical’s social security number.
It is a universally recognized identifier that eliminates ambiguity stemming from synonyms, trade names, or varying structural representations.
Understanding the CAS RN Structure
CAS RNs follow a specific format: a series of two or three numbers separated by hyphens. While the specific structure isn’t crucial for the average user, it’s important to know that the number is algorithmically generated and serves as a unique identifier, not a descriptor of chemical properties.
Utilizing the CAS RN for Information Retrieval
The CAS RN is the key to unlocking a wealth of information.
By inputting the CAS RN for Barium Chloride Dihydrate (typically 10233-18-6) into databases like the CAS registry, chemical suppliers’ websites, or scientific literature search engines, users can quickly access critical data, including:
- Chemical and physical properties.
- Safety information (MSDS/SDS).
- Regulatory information.
- Published research articles.
The CAS RN ensures that searches yield the precise information sought, avoiding the pitfalls of relying solely on chemical names.
PubChem CID: Connecting Chemical Data Across Platforms
PubChem, maintained by the National Center for Biotechnology Information (NCBI), is a comprehensive database of chemical molecules and their activities. The PubChem Compound Identifier (CID) is a unique integer assigned to each substance within this database.
PubChem CID’s Role in Data Integration
The PubChem CID acts as a central hub for connecting diverse chemical information. It links data from various sources, including chemical structures, properties, bioactivity data, and related literature.
Leveraging PubChem for Comprehensive Chemical Insights
The PubChem CID for Barium Chloride Dihydrate allows users to access a vast repository of information directly within the PubChem platform.
By searching for the PubChem CID, researchers can explore:
- Chemical structures and properties.
- Synonyms and related compounds.
- Safety and toxicity data.
- Biological activities and pharmacological information.
- Links to relevant scientific literature.
PubChem’s robust search capabilities and data integration features make it an invaluable resource for anyone working with chemical compounds.
Handling with Care: Safety Protocols for Barium Chloride Dihydrate
Decoding Chemical Identity: CAS Registry Number and PubChem CID
Having established the foundational identity of Barium Chloride Dihydrate, it is imperative to delve into its key chemical properties. These properties dictate its behavior in various applications and, critically, inform the necessary safety precautions for handling this compound.
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The safe handling of Barium Chloride Dihydrate necessitates a rigorous adherence to established safety protocols. Given its inherent toxicity, a comprehensive understanding of potential hazards and the implementation of appropriate protective measures are paramount. This section details the critical aspects of safe handling, focusing on the Material Safety Data Sheet (MSDS/SDS), Personal Protective Equipment (PPE), storage guidelines, and emergency procedures.
The Indispensable MSDS/SDS
The Material Safety Data Sheet (MSDS), now often referred to as the Safety Data Sheet (SDS), is the cornerstone of chemical safety. It is an essential document that provides comprehensive information about the properties of Barium Chloride Dihydrate and its associated hazards.
This includes details on potential health effects, physical and chemical properties, reactivity, and necessary precautions for safe handling and use.
Key Information Within
The SDS contains critical information, including:
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Hazard Identification: This section outlines the specific hazards associated with Barium Chloride Dihydrate, such as acute toxicity (oral, dermal, inhalation), and potential environmental hazards.
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First Aid Measures: Clear instructions are provided for addressing exposure incidents, including inhalation, ingestion, skin contact, and eye contact. Knowing these procedures is crucial for immediate response in case of an accident.
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Handling and Storage: This section details recommended practices for safe handling and storage, including proper ventilation, temperature control, and incompatible materials.
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Exposure Controls/Personal Protection: Information on necessary engineering controls and Personal Protective Equipment (PPE) to minimize exposure is provided.
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Toxicological Information: Comprehensive data on the compound’s toxicity, including acute and chronic effects, is included.
Accessing the SDS
The SDS should be readily accessible to all personnel who handle Barium Chloride Dihydrate. It can typically be obtained from the chemical supplier or manufacturer.
A digital copy is often available on the supplier’s website.
It is imperative to review and understand the SDS before handling the chemical.
Personal Protective Equipment (PPE)
Minimizing exposure to Barium Chloride Dihydrate requires the consistent and correct use of appropriate Personal Protective Equipment (PPE). PPE acts as a barrier between the chemical and the individual, significantly reducing the risk of exposure.
Essential PPE Components
The minimum recommended PPE includes:
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Gloves: Chemical-resistant gloves, such as nitrile or neoprene gloves, are essential to prevent skin contact. The specific type of glove should be selected based on the SDS recommendations. Consider double gloving for extra protection.
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Goggles: Safety goggles that provide splash protection are critical to prevent eye exposure. Regular eyeglasses do not provide adequate protection. In situations where there is a risk of splashing, a face shield should also be worn.
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Lab Coat: A laboratory coat provides a protective barrier for clothing and skin. The lab coat should be made of a chemical-resistant material and should be buttoned up completely during use. It should be promptly removed if contaminated.
Importance of Proper Use
Proper training on the use, maintenance, and disposal of PPE is essential. PPE should be inspected before each use for any signs of damage or degradation. Contaminated PPE should be disposed of properly according to established procedures.
Chemical Storage Guidelines
Proper storage of Barium Chloride Dihydrate is critical to prevent accidents and maintain the integrity of the chemical.
Best Practices
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Segregation: Store Barium Chloride Dihydrate separately from incompatible materials. Consult the SDS for a list of incompatible substances.
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Containers: Use tightly sealed, properly labeled containers made of compatible materials. Avoid storing in metal containers, as corrosion may occur.
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Ventilation: Store in a well-ventilated area to prevent the buildup of dust or vapors.
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Temperature and Humidity: Store in a cool, dry place, away from direct sunlight and sources of heat. Excessive heat and humidity can degrade the compound or increase the risk of accidents.
Incompatible Materials
Barium Chloride Dihydrate is incompatible with strong oxidizing agents, strong acids, and certain metals. Storing it near these substances can lead to hazardous reactions, including the release of toxic gases.
Emergency Procedures: Poison Control Centers
In the event of accidental exposure to Barium Chloride Dihydrate, immediate action is crucial. Contacting a Poison Control Center is a critical step in obtaining expert advice and guidance.
Contact Information and Actions
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Poison Control Center Number: The national Poison Control Center hotline number in the United States is 1-800-222-1222. This number should be readily available in all areas where Barium Chloride Dihydrate is used or stored.
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Accidental Ingestion: If Barium Chloride Dihydrate is ingested, immediately call Poison Control. Do not induce vomiting unless directed to do so by a medical professional.
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Skin or Eye Contact: In case of skin or eye contact, immediately flush the affected area with copious amounts of water for at least 15 minutes. Seek medical attention.
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Inhalation: If Barium Chloride Dihydrate is inhaled, move the affected person to fresh air. Seek medical attention.
It is vital to provide the Poison Control Center with as much information as possible, including the amount of chemical involved, the route of exposure, and the victim’s age and weight. Following their instructions carefully can significantly improve the outcome of an exposure incident.
Real-World Applications: Uses of Barium Chloride Dihydrate
Having established the foundational safety parameters for handling Barium Chloride Dihydrate, it is critical to examine its diverse range of practical applications. These applications underscore its significance across various scientific and industrial domains, highlighting the pivotal role it plays in numerous processes.
Pigment Manufacturing
Barium Chloride Dihydrate serves as a crucial precursor in the synthesis of various pigments, particularly those prized for their brilliance and stability.
Its primary function lies in facilitating the precipitation of sulfate-based pigments. This results in materials that exhibit exceptional resistance to fading and degradation, making them highly valued in artistic and industrial applications.
Lithopone Production
A prime example is its use in the production of lithopone, a white pigment comprised of barium sulfate (BaSO₄) and zinc sulfide (ZnS). Barium Chloride Dihydrate reacts with zinc sulfate to precipitate barium sulfate, which then combines with zinc sulfide to form the final lithopone pigment.
This pigment is widely utilized in paints, coatings, and plastics, offering a cost-effective alternative to titanium dioxide in certain applications.
The controlled precipitation facilitated by Barium Chloride Dihydrate ensures the desired particle size and uniformity, contributing to the pigment’s overall quality and performance.
Laboratory Reagent
In the realm of chemical analysis and research, Barium Chloride Dihydrate functions as a versatile laboratory reagent, enabling precise detection and quantification of specific ions.
Its most notable application lies in the qualitative and quantitative determination of sulfate ions (SO₄²⁻) in solution.
Sulfate Detection and Precipitation
When Barium Chloride Dihydrate is introduced to a solution containing sulfate ions, a characteristic white precipitate of barium sulfate (BaSO₄) forms.
The formation of this precipitate serves as a definitive indicator of the presence of sulfate ions.
The reaction proceeds according to the following net ionic equation:
Ba²⁺(aq) + SO₄²⁻(aq) → BaSO₄(s)
By carefully controlling the reaction conditions and measuring the mass of the precipitated barium sulfate, the concentration of sulfate ions in the original solution can be accurately determined.
This method is extensively employed in environmental monitoring, industrial process control, and various research applications requiring precise sulfate quantification.
Other Industrial Applications
Beyond pigment production and laboratory analysis, Barium Chloride Dihydrate finds application in several other industrial processes. These applications leverage its unique chemical properties to achieve specific outcomes.
Heat Treatment of Steel
Barium Chloride Dihydrate is utilized in heat treatment processes for steel. When molten, it forms a salt bath that provides a uniform and controlled heating environment.
This allows for precise tempering and hardening of steel components, enhancing their mechanical properties and extending their service life.
The salt bath method offers advantages such as reduced oxidation and decarburization of the steel surface, resulting in improved product quality.
Water Treatment
In specific water treatment applications, Barium Chloride Dihydrate can be employed to remove dissolved sulfate ions.
Excessive sulfate concentrations in water can contribute to corrosion problems in pipelines and infrastructure, as well as undesirable taste and odor.
By precipitating sulfate ions as barium sulfate, Barium Chloride Dihydrate helps mitigate these issues and improve water quality.
However, due to the toxicity of barium compounds, this application is carefully controlled and typically limited to specialized industrial settings where the removal of barium ions from the treated water can be ensured.
So, there you have it! Hopefully, this guide cleared up any confusion you had about barium chloride dihydrate molar mass and its various applications. It might sound like complex chemistry, but breaking it down reveals some pretty fascinating uses for this compound.
