Barium acetate

Synthetic Routes and Reaction Conditions: Barium acetate is typically synthesized through the reaction of acetic acid with barium carbonate: [ \text{BaCO}_3 + 2\text{CH}_3\text{COOH} \rightarrow (\text{CH}_3\text{COO})_2\text{Ba} + \text{CO}_2 + \text{H}_2\text{O} ] This reaction is performed in solution, and the this compound crystallizes out at temperatures above 41°C. Between 25°C and 40°C, the monohydrate version crystallizes .

Alternatively, barium sulfide can be used: [ \text{BaS} + 2\text{CH}_3\text{COOH} \rightarrow (\text{CH}_3\text{COO})_2\text{Ba} + \text{H}_2\text{S} ] The solvent is evaporated off, and the this compound crystallizes .

Industrial Production Methods: In industrial settings, this compound is produced by reacting industrial-grade barium carbonate with acetic acid. The process involves acetic acid reflux to decompose barium carbonate, followed by separation, impurity removal, refined filtration, evaporation, crystallization, and drying .

Types of Reactions:

Decomposition: When heated in air, this compound decomposes to form barium carbonate. [ (\text{CH}_3\text{COO})_2\text{Ba} \rightarrow \text{BaCO}_3 + \text{H}_2\text{O} ]

Reaction with Acids: this compound reacts with sulfuric acid, hydrochloric acid, and nitric acid to form barium sulfate, barium chloride, and barium nitrate, respectively. [ (\text{CH}_3\text{COO})_2\text{Ba} + \text{H}_2\text{SO}_4 \rightarrow \text{BaSO}_4 + 2\text{CH}_3\text{COOH} ] [ (\text{CH}_3\text{COO})_2\text{Ba} + 2\text{HCl} \rightarrow \text{BaCl}_2 + 2\text{CH}_3\text{COOH} ] [ (\text{CH}_3\text{COO})_2\text{Ba} + 2\text{HNO}_3 \rightarrow \text{Ba(NO}_3\text{)}_2 + 2\text{CH}_3\text{COOH} ]

Common Reagents and Conditions:

Sulfuric Acid: Used to produce barium sulfate.

Hydrochloric Acid: Used to produce barium chloride.

Nitric Acid: Used to produce barium nitrate.

Major Products:

Barium Carbonate: Formed upon decomposition.

Barium Sulfate, Barium Chloride, Barium Nitrate: Formed upon reaction with respective acids.

Pyrotechnics and Fireworks

Barium acetate is widely used in the pyrotechnics industry. It is a key ingredient that imparts a vibrant green color to flames and fireworks. When combined with other metal salts and oxidizers, it enhances the visual effects of fireworks displays. This application capitalizes on the compound's ability to produce specific colors when combusted, making it invaluable for creating visually stunning pyrotechnic shows .

Analytical Chemistry

In analytical chemistry, this compound serves as a reagent for the gravimetric determination of sulfate ions. By precipitating sulfate ions as insoluble barium sulfate ($\text{BaSO}_4$), it allows for quantitative analysis in various samples. This method is particularly useful in environmental monitoring and quality control processes where sulfate levels need to be accurately measured .

Textile and Leather Industry

This compound functions as a mordant in the dyeing processes of textiles and leather. It helps fix dyes onto fibers, enhancing color fastness and vibrancy. This application is crucial for industries that require durable and vivid colors in their products .

Ceramics and Glass Production

The compound acts as a precursor for synthesizing barium oxide, which is essential in ceramics and glass manufacturing. Barium oxide contributes to improved refractive index and insulation properties in glass products. Additionally, it is used in producing specialty glasses and advanced ceramic materials that require specific optical or thermal properties .

Medical Imaging

This compound is significant in the medical field as a precursor for barium-based contrast agents used in imaging techniques such as X-rays and CT scans. These agents enhance the visibility of internal structures during diagnostic procedures, making them critical for accurate medical assessments .

Functional Materials and Energy Storage

Research has identified this compound as a precursor for various functional materials, including barium titanate ($\text{BaTiO}_3$). Barium titanate is employed in dielectric capacitors, piezoelectric devices, and energy storage systems like batteries and supercapacitors. The exploration of novel synthesis routes aims to enhance the properties of these materials for advanced technological applications .

Environmental Applications

This compound has been investigated for its potential use in environmental remediation. It can serve as a precursor for barium-based catalysts and adsorbents designed to remove sulfur compounds from fuels or capture CO2 emissions. Such applications are increasingly relevant in efforts to mitigate environmental pollution .

Innovative Synthesis Methods

Researchers are developing environmentally friendly methods for synthesizing high-purity this compound with minimal impurities and waste generation. Techniques such as ion exchange processes and precipitation methods are being explored to improve industrial efficiency while reducing environmental impact .

Case Study 1: this compound in Medical Imaging

A study conducted at a healthcare facility demonstrated the effectiveness of barium-based contrast agents synthesized from this compound during gastrointestinal imaging procedures. The results indicated improved visibility of internal structures compared to traditional methods, leading to more accurate diagnoses.

Case Study 2: Environmental Remediation Using Barium Compounds

Research published on barium-based catalysts showed promising results in removing sulfur compounds from industrial emissions. The study highlighted the potential of using this compound-derived materials for sustainable environmental practices.

Barium acetate exerts its effects primarily through its interaction with various acids to form corresponding barium salts. The molecular targets include the acetate ions, which facilitate the formation of barium salts such as barium sulfate, barium chloride, and barium nitrate. These reactions are crucial in various industrial and chemical processes .

Barium acetate shares functional similarities with other metal acetates, such as calcium acetate , lead acetate , and strontium acetate , but differs in chemical behavior, solubility, and applications. Below is a comparative analysis:

This compound vs. Calcium Acetate (Ca(C₂H₃O₂)₂)

Calcium acetate is less toxic and widely used in food and medicine, whereas this compound’s reactivity makes it suitable for industrial processes.

This compound vs. Lead Acetate (Pb(C₂H₃O₂)₂)

Lead acetate’s neurotoxicity has led to reduced use, while this compound remains relevant in niche chemical reactions.

This compound vs. Strontium Acetate (Sr(C₂H₃O₂)₂)

Strontium acetate’s lower density and distinct flame color make it preferable in pyrotechnics, while this compound’s higher reactivity suits analytical chemistry.

Key Research Findings

• Thermal Decomposition : this compound decomposes at higher temperatures than calcium or strontium acetates, making it a stable intermediate in high-temperature syntheses.
• Toxicity Profile : Studies highlight this compound’s acute toxicity (LD₅₀: 11 mg/kg in rats), necessitating stringent safety protocols compared to calcium acetate .
• Catalytic Efficiency: this compound exhibits superior catalytic activity in esterification reactions compared to lead acetate, which is now avoided due to environmental concerns.

Table 1: Physical Properties Comparison

Barium acetate (Ba(C₂H₃O₂)₂) is a barium salt that has garnered interest due to its various biological activities and applications. This article provides a comprehensive overview of the biological effects, toxicological profiles, and case studies related to this compound, drawing from diverse sources to ensure a thorough understanding.

This compound is a white crystalline compound that is soluble in water. It is primarily used in the chemical industry for synthesizing other barium compounds, particularly barium titanate, which is significant in electronic applications due to its ferroelectric properties. Additionally, it has been explored for its potential use in environmental remediation and as a catalyst in organic transformations .

General Toxicity

Barium compounds, including this compound, are known to be toxic, particularly when ingested or inhaled. The toxicity primarily arises from the barium ion (Ba²⁺), which can interfere with potassium homeostasis in biological systems. Acute exposure can lead to severe hypokalemia (low potassium levels), resulting in muscle weakness, paralysis, and potentially fatal cardiac arrhythmias .

Case Studies

• Acute Barium Poisoning : A notable case involved a 21-year-old male who ingested approximately 100 mL of a concentrated barium chloride solution, which led to acute toxicity symptoms such as abdominal pain and severe hypokalemia. The patient was treated with gastric lavage and potassium supplementation, highlighting the critical need for rapid intervention in cases of barium ingestion .
• Chronic Exposure Studies : Research indicates that chronic oral exposure to this compound in animal models does not significantly alter longevity or reproductive outcomes but can affect calcium and phosphorus metabolism. For instance, studies involving rats showed decreased urinary calcium levels and increased serum phosphorus levels following exposure to barium compounds .

Barium's biological effects are primarily mediated through its interaction with cellular ion channels, particularly those regulating potassium. The disruption of potassium homeostasis can lead to various physiological disturbances:

• Neurological Effects : Barium exposure has been linked to neurological impairments due to its ability to block potassium channels, leading to symptoms such as muscle weakness and paralysis .
• Cardiovascular Effects : Hypokalemia induced by barium can result in significant cardiovascular complications, including arrhythmias and elevated blood pressure .

Summary of Research Findings

Basic Research Questions

Q. What is the standard laboratory method for synthesizing barium acetate, and how can researchers optimize reaction conditions?

this compound is typically synthesized via two primary routes:

• Route 1 : Reaction of barium carbonate with acetic acid: $\text{BaCO}_3 + 2\text{CH}_3\text{COOH} \rightarrow \text{Ba(CH}_3\text{COO)}_2 + \text{CO}_2 + \text{H}_2\text{O}$ This method is cost-effective and widely used due to the mild reaction conditions (room temperature, aqueous medium) .
• Route 2 : Reaction of barium sulfide with acetic acid: $\text{BaS} + 2\text{CH}_3\text{COOH} \rightarrow \text{Ba(CH}_3\text{COO)}_2 + \text{H}_2\text{S}$ Researchers must use fume hoods for this route due to toxic H₂S gas emission . Optimization Tips : Monitor pH to ensure complete neutralization, and crystallize the product by slow evaporation for higher purity.

Q. How can the molecular structure and purity of this compound be confirmed experimentally?

• Structural Confirmation : Use X-ray diffraction (XRD) to verify the crystalline structure, complemented by FT-IR spectroscopy to identify acetate anion vibrations (~1560 cm⁻¹ for asymmetric C=O stretching) .
• Purity Analysis : Conduct titration against standardized sulfuric acid to quantify barium content (CNS 1580-1962 standards) . The molar mass (255.42 g/mol) can be verified via mass spectrometry (MS) .

Q. What are the critical solubility and physical properties of this compound relevant to experimental design?

• Solubility : 59 g/100 mL in water at 20°C, decreasing with temperature .
• Density : 2.468 g/cm³ (crystalline form) .
• Thermal Stability : Decomposes to barium carbonate above 200°C . Experimental Note : Pre-saturate solutions to avoid unintended precipitation during reactions.

Advanced Research Questions

Q. How can researchers investigate the thermal decomposition kinetics of this compound?

Use thermogravimetric analysis (TGA) coupled with differential scanning calorimetry (DSC) to study decomposition pathways. Key steps:

• Heat samples at 5–10°C/min under inert (N₂) and oxidative (air) atmospheres.
• Monitor mass loss corresponding to CO₂ release (40–60% weight loss at 200–400°C) .
• Analyze kinetic parameters (activation energy, reaction order) via the Kissinger or Ozawa method.

Q. What advanced analytical techniques are suitable for characterizing this compound in complex matrices (e.g., environmental samples)?

• Extractive Electrospray Ionization Time-of-Flight MS (EESI-TOF-MS) : Enables direct analysis of aerosols or solutions containing this compound with minimal sample preparation (detection limit ~0.1 ppm) .
• Inductively Coupled Plasma Optical Emission Spectroscopy (ICP-OES) : Quantifies trace barium with high sensitivity (detection limit ~0.01 µg/L) .

Q. How should researchers address discrepancies in reported solubility or stability data for this compound?

• Controlled Replication : Repeat experiments under identical conditions (temperature, solvent purity, agitation) to isolate variables.
• Source Verification : Cross-check reagent grades (e.g., ACS vs. technical grade) and hydration states (anhydrous vs. monohydrate, which has a solubility of 72 g/100 mL) .
• Instrument Calibration : Validate spectrophotometric or gravimetric methods against certified standards .

Q. What safety protocols are critical for handling this compound in academic laboratories?

• Exposure Limits : Adhere to occupational exposure limits (0.5 mg/m³ for respirable particles) .
• PPE Requirements : Wear nitrile gloves, lab coats, and safety goggles; use N95 masks during powder handling .
• Emergency Measures : For eye exposure, rinse with water for 15 minutes and seek medical attention .

Q. Key Considerations for Experimental Design

• Purity Standards : Use ACS-grade reagents (≥99% purity) for reproducible results .
• Contradiction Resolution : Document batch-specific variations (e.g., hydration state) when comparing literature data .
• Environmental Impact : Neutralize waste solutions with sodium carbonate to precipitate barium ions before disposal .