Views: 20 Author: Site Editor Publish Time: 2024-04-10 Origin: Site
Barium carbonate is an inorganic carbonate with the chemical formula BaCO3. It occurs naturally as the mineral witherite and is normally supplied as a white crystalline powder.
Researchers study barium carbonate because it combines several useful characteristics: an ordered orthorhombic crystal structure, very low solubility in neutral water, reactivity toward acids and sulfates, relatively high density, and the ability to act as a barium precursor for advanced ceramic materials.
BaCO3 research currently focuses on five main areas:
Controlled precipitation and crystal growth
Particle-size and morphology engineering
Thermal decomposition and phase transformation
Preparation of barium-containing ceramics
Sulfate immobilization and environmental treatment
Research interest is not limited to chemical composition. Particle size, surface area, morphology, impurity profile and thermal history can all change how a BaCO3 material behaves.
| Property | Typical information |
|---|---|
| Chemical name | Barium carbonate |
| Formula | BaCO3 |
| CAS number | 513-77-9 |
| Molar mass | 197.34 g/mol |
| Natural mineral form | Witherite |
| Appearance | White crystalline powder |
| Crystal system | Orthorhombic |
| Density | Approximately 4.3 g/cm³ |
| Water solubility | Very low |
| Acid behavior | Reacts with acids and may release soluble barium ions |
| Main research roles | Functional particle, sulfate-reactive material and ceramic precursor |
These are general reference properties. Values measured for a specific sample may vary with purity, particle size, porosity, test method and storage history.
At ambient conditions, barium carbonate normally adopts an orthorhombic, aragonite-type crystal structure. It is commonly described using the Pnma space group, although the equivalent Pmcn setting also appears in scientific literature.
The structure contains Ba⊃2;⁺ ions coordinated by oxygen atoms from carbonate groups. Its relatively large barium cation helps distinguish BaCO3 from smaller-cation carbonates such as calcite-type calcium carbonate.
Crystal orientation, defects and exposed surface planes can affect:
Nucleation and growth rates
Agglomeration behavior
Acid reactivity
Thermal decomposition
Interfacial reactions with other ceramic precursors
For this reason, confirming phase identity by X-ray diffraction is more reliable than identifying a sample from color or bulk chemical composition alone.
BaCO3 has very low solubility in neutral water, but “poorly water-soluble” does not mean chemically inert or non-toxic.
In an acidic environment, it can react according to the simplified equation:
BaCO3 + 2H⁺ → Ba⊃2;⁺ + CO2 + H2O
This reaction releases carbon dioxide and can produce bioavailable barium ions. Consequently, water solubility alone must never be used as the basis for a safety assessment.
Barium carbonate can decompose at elevated temperature:
BaCO3 → BaO + CO2
However, it is misleading to describe this transformation using one universal decomposition temperature. The observed behavior depends on:
Carbon dioxide partial pressure
Heating rate
Particle size
Sample thickness
Powder compaction
Crucible geometry
Gas flow and mass transfer
Presence of impurities or reactive phases
Recent kinetic research shows that increasing the surrounding CO2 pressure can move the apparent decomposition onset to higher temperatures. Thin films, loose powders and compacted samples may therefore produce different thermal-analysis curves.
Every publication should report the atmosphere, flow rate, heating program and sample geometry alongside its TGA or DSC results.
A common laboratory route is the precipitation of BaCO3 from a soluble barium source and a carbonate source:
Ba⊃2;⁺ + CO3⊃2;⁻ → BaCO3↓
This route is simple, but the final material is highly sensitive to local supersaturation and mixing conditions.
Important variables include:
Reactant concentration
Addition order and addition rate
Temperature
Solution pH
Agitation and mixing efficiency
Aging time
Ionic strength
Washing and drying conditions
High supersaturation generally promotes rapid nucleation, while lower supersaturation may favor crystal growth. Poor micromixing can create separate nucleation zones and a broader particle-size distribution.
BaCO3 may also be produced by introducing carbon dioxide into a barium-containing alkaline medium.
In this method, gas–liquid mass transfer becomes an important experimental variable. Gas flow, bubble size, agitation, temperature and pH influence how quickly carbonate species form and where precipitation occurs.
Carbonation can offer gradual control of carbonate availability, but the result depends strongly on reactor design. Researchers should therefore report more than the total reaction time.
Hydrothermal processing can change nucleation, crystal growth and particle aggregation under elevated temperature and pressure. Surfactants or organic modifiers may adsorb selectively on crystal surfaces and alter relative growth rates.
Reported morphologies include:
Rod-like particles
Needle-like crystals
Spherical aggregates
Flower-like structures
Shuttle-shaped particles
Hierarchical assemblies
The presence of a surfactant does not automatically guarantee nanoscale or monodisperse BaCO3. Its concentration, adsorption behavior and interaction with the precursor solution must be evaluated experimentally.
Polymers, starches, proteins and silica-rich matrices have been investigated as templates or growth modifiers.
These substances may:
Confine nucleation
Stabilize intermediate particles
Change interfacial energy
Direct particle assembly
Delay or accelerate recrystallization
Studies using soluble starch, silk fibroin and silica demonstrate that BaCO3 can form complex hierarchical structures through combinations of nucleation, aggregation, dissolution–recrystallization and Ostwald ripening.
These methods are valuable for studying crystallization mechanisms, although removal of the organic or inorganic template can introduce additional processing steps.
Thin films and supported BaCO3 structures are useful for studying interfaces and decomposition kinetics.
Compared with a powder bed, a thin layer can have shorter CO2 diffusion paths and more clearly defined reaction interfaces. Results obtained from films should therefore not be transferred directly to bulk industrial powders without validation.
| Variable | Possible influence | What should be reported |
| Supersaturation | Changes the balance between nucleation and growth | Initial concentration and mixing method |
| pH | Alters carbonate speciation and surface charge | Initial, final and controlled pH |
| Temperature | Affects reaction, diffusion and recrystallization rates | Actual reaction temperature profile |
| Addition rate | Changes local supersaturation | Flow rate and addition sequence |
| Agitation | Influences mixing and collision frequency | Mixer type and speed |
| Surfactant | May modify surface growth and aggregation | Identity, concentration and purity |
| Aging time | Allows ripening or phase evolution | Time before separation |
| Washing | Removes ions but may promote redispersion or loss | Solvent, cycles and end point |
| Drying | Can increase hard agglomeration | Temperature, pressure and duration |
| Calcination | Changes phase, crystallinity and surface area | Atmosphere and heating program |
A small primary crystallite is not necessarily a freely dispersed nanoparticle. SEM, TEM, laser diffraction and BET measurements may describe different levels of the particle structure and should not be treated as interchangeable.
A reliable BaCO3 study normally combines several complementary methods.
XRD is used to:
Confirm the crystalline BaCO3 phase
Detect secondary crystalline phases
Compare relative crystallinity
Estimate crystallite dimensions when the model is appropriate
Monitor reactions with other ceramic precursors
Crystallite size calculated from peak broadening is not the same as particle size measured by microscopy.
Scanning electron microscopy shows external morphology, agglomeration and approximate particle dimensions. Transmission electron microscopy can provide information about smaller particles, interfaces and local crystal structure.
Representative images should be supported by measurements from a sufficient number of particles rather than a single attractive micrograph.
Vibrational spectroscopy helps identify carbonate groups and can reveal interactions with polymers, surfactants or other phases.
Peak position and band shape may change because of crystallinity, particle size, defects or surface-bound species. Spectra should be interpreted alongside phase and composition data.
Laser diffraction is useful for distributions such as D10, D50 and D90, while dynamic light scattering is more applicable to stable dispersions of sufficiently small particles.
The reported method should include:
Dispersion medium
Dispersant
Sonication conditions
Optical model
Measurement basis
Without this information, particle-size results from different laboratories may not be comparable.
BET analysis can help explain changes in reactivity that are not visible from nominal particle size alone.
Drying, degassing and agglomeration may strongly affect the measured surface area. High surface area can improve reaction kinetics but may also increase moisture adsorption, contamination sensitivity and dust exposure.
TGA and DSC can monitor mass loss, thermal stability and reactions with other components. For meaningful comparison, publications should report sample mass, container type, heating rate, atmosphere and gas flow.
ICP-OES, ICP-MS or XRF can measure barium and trace impurities. Depending on the intended research, relevant impurities may include:
Strontium
Calcium
Sodium
Potassium
Iron
Chloride
Sulfate
Sulfide
Acid-insoluble matter
For electronic ceramics, a trace impurity can matter even when the total assay appears acceptable.
Particle engineering affects processing as well as chemical reactivity.
Smaller or more uniform BaCO3 particles can provide:
Shorter diffusion distances
More homogeneous mixing with other precursors
Lower risk of persistent unreacted cores
More predictable slurry behavior
Greater reactive surface area
However, reducing particle size may also increase:
Agglomeration
Dust formation
Surface contamination
Moisture sensitivity
Batch-to-batch variability
Difficulty in filtration and washing
The ideal particle size is therefore application-specific. “Smaller” is not automatically “better.”
Researchers should define the required relationship among particle size, flowability, dispersibility, reactivity and exposure control before selecting a material.
Barium titanate, BaTiO3, is an important electroceramic used in capacitors, thermistors, sensors, actuators and other dielectric components.
A simplified solid-state reaction is:
BaCO3 + TiO2 → BaTiO3 + CO2
In a conventional ceramic route, BaCO3 and TiO2 powders are mixed and heated. Reaction performance depends on:
BaCO3 particle size
TiO2 phase and particle size
Ba-to-Ti stoichiometry
Mixing homogeneity
Milling contamination
Calcination temperature
CO2 removal
Heating and cooling profiles
Fine, well-distributed precursors can reduce diffusion distances and improve the uniformity of BaTiO3 formation.
Nevertheless, BaCO3 is both a useful precursor and a possible residual impurity. Unreacted carbonate in the final powder can interfere with sintering, composition control and electrical performance. Raising the temperature may remove residual carbonate but can also promote grain growth and agglomeration.
Successful processing therefore requires phase analysis after calcination rather than relying only on starting-material ratios.
In ceramic and glass research, barium carbonate is used as a controlled source of barium oxide after heating or reaction.
Barium-containing compositions may be studied for:
Glaze development
Specialty glass
Ceramic flux systems
Dielectric ceramics
Barium ferrites
Pigments and frits
Modification of thermal or optical properties
The final result depends on the entire formulation. BaCO3 should not be described as producing one universal effect in every glass or ceramic body.
Researchers should evaluate:
Reaction with silica and other oxides
Carbon dioxide evolution
Firing shrinkage
Phase formation
Glaze fit
Leaching behavior
Final barium immobilization
A finished ceramic may behave very differently from the unreacted raw powder.
Barium carbonate can react with soluble sulfate species to form highly insoluble barium sulfate. A simplified representation is:
BaCO3 + SO4⊃2;⁻ → BaSO4 + CO3⊃2;⁻
This reaction explains its use in research involving brick scumming, ceramic efflorescence and sulfate-containing water.
Soluble sulfates in clay can migrate during drying and form visible deposits at the surface. If BaCO3 converts these sulfates into less mobile BaSO4 before migration occurs, surface deposits may be reduced.
Performance depends on:
Type and concentration of soluble sulfate
BaCO3 particle size
Mixing uniformity
Moisture movement
Drying rate
Contact time
Clay pH
Firing conditions
Barium carbonate cannot be assumed to remove every form of sulfate. Sulfates produced later during firing or introduced through another process route may respond differently.
BaCO3 has also been investigated for sulfate removal from acid mine drainage and other sulfate-rich waters.
Potential advantages include sulfate immobilization and the formation of a low-solubility BaSO4 phase. Important limitations include reaction-rate control, incomplete conversion, residual dissolved barium and management of the resulting solid waste.
Any environmental process should measure both remaining sulfate and remaining soluble barium. Sulfate removal alone is not sufficient evidence of safe treatment.
A 2024 study investigated controlled BaCO3 microcarriers and nanocarriers for experimental SPECT/CT imaging. The reported results show that carefully designed particles may have value as research platforms.
This does not establish BaCO3 as an approved clinical material. Biological behavior depends on:
Particle size and shape
Surface chemistry
Dose
Dissolution rate
Administration route
Coating or functionalization
Biodistribution
Clearance
Formulation-specific toxicity
Biomedical statements must remain limited to the tested formulation and experimental conditions.
Because barium has a relatively high atomic number, barium-containing glasses, polymers and ceramic composites may be studied for radiation attenuation.
The performance of a composite depends on barium loading, dispersion, thickness, energy range and matrix structure. Raw BaCO3 powder should not be marketed as a universal radiation-shielding material without application-specific test data.
BaCO3 can serve as a barium precursor, surface component or intermediate in selected energy-material studies. However, it is not accurate to classify ordinary BaCO3 powder as a general-purpose battery electrolyte or fuel-cell material.
Any energy-related claim should identify the final material, transformation process and measured electrochemical function.
Incorrect. BaCO3 has low water solubility but can release soluble barium in acidic conditions.
Incorrect. Two samples with similar assay values may have different particle sizes, impurity profiles, surface areas and thermal histories.
Incomplete. Smaller particles may improve reaction rates but can also agglomerate, introduce handling risks and complicate reproducibility.
Overstated. Some formulations are under experimental investigation, but research results do not establish general clinical suitability.
Incorrect. Atmosphere, CO2 pressure, particle size, sample geometry and heating conditions affect the observed decomposition behavior.
| Selection factor | Research significance |
| Assay | Indicates overall chemical purity |
| Phase purity | Confirms the required crystalline phase |
| Trace metals | Important for electronic and catalytic studies |
| Chloride and sulfate | May affect reactions and final phases |
| Acid-insoluble matter | Indicates non-reactive contamination |
| Particle-size distribution | Influences dispersion and kinetics |
| Surface area | Influences reactivity and adsorption |
| Morphology | Affects packing, flow and interfacial contact |
| Moisture | Changes weighing accuracy and processing |
| Batch consistency | Required for reproducible experiments |
| Documentation | Supports traceability and risk assessment |
An industrial grade may be suitable for formulation screening or large-scale ceramic trials. High-purity or tightly specified material may be more appropriate for phase-sensitive, analytical or electronic-material research.
The required grade should be selected from the experiment’s failure risks—not simply from the highest available purity claim.
Before purchasing, define the following:
Is BaCO3 the final functional phase or a reactive precursor?
Is chemical purity or particle consistency more important?
Which impurities could interfere with the experiment?
Does the study require a specified D50 or complete D10/D50/D90 distribution?
Is surface area relevant to the reaction?
Will the material be dispersed in water, solvent or a ceramic slurry?
Will it undergo thermal decomposition or solid-state reaction?
Is batch-to-batch comparability required?
Which analytical methods will be used for incoming verification?
What safety and waste procedures apply?
Researchers should request a certificate of analysis, safety data sheet and technical data sheet. For particle-sensitive research, a representative sample should be tested before committing to a larger batch.
A reproducible research report should record:
Supplier and batch number
Nominal purity
Measured impurity data
Crystal phase
Particle-size method
Surface-area method
Pretreatment and drying history
Storage conditions
Reactant concentrations
Addition sequence
Agitation method
Temperature and pH profiles
Washing procedure
Thermal-analysis atmosphere
Heating and cooling rates
Researchers should also retain an archive sample from each important batch. This makes it possible to investigate unexpected differences between experiments conducted at different times.
When scaling a precipitation process, matching reactant ratios is not enough. Mixing time, energy input, gas transfer and heat transfer must also be considered.
Barium carbonate is harmful if swallowed. Its low water solubility should not be interpreted as low biological risk because acidic conditions can release soluble barium ions.
Recommended controls include:
Review the current supplier SDS before use
Avoid creating or inhaling dust
Use appropriate gloves and eye protection
Handle powders in a suitable ventilated or enclosed area
Keep the material away from food and drink
Prevent uncontrolled contact with acids
Label experimental dispersions and waste clearly
Do not dispose of barium-containing waste into drains
Heating BaCO3 can release carbon dioxide and may involve very high temperatures. Thermal experiments require equipment appropriate for the selected atmosphere, pressure and temperature range.
Waste containing barium, sulfate, acids or nanoscale particles should be characterized and managed according to applicable local regulations. Precipitation as BaSO4 may reduce solubility, but it does not eliminate the need for proper waste assessment.
Promising research directions include:
Continuous synthesis with real-time particle monitoring
Better control of nucleation and aggregation
Lower-temperature conversion to functional barium oxides
Quantitative links between morphology and reactivity
In-situ study of phase transformation and CO2 release
Safer surface modification of micro- and nanoscale particles
Recovery and reuse of barium from industrial streams
Improved sulfate-treatment processes with residual-barium control
Standardized reporting of particle size and thermal conditions
Life-cycle assessment of barium-containing materials
The most useful future studies will connect synthesis, structure, processing and performance instead of optimizing only one isolated property.
The formula is BaCO3, and its CAS number is 513-77-9.
Natural barium carbonate is known as witherite. At ambient conditions it normally has an orthorhombic, aragonite-type structure.
It has very low solubility in neutral water. It can nevertheless react in acidic media and release soluble barium ions.
It is harmful if swallowed. Appropriate dust control, personal protection, storage and waste procedures are required.
Research routes include controlled precipitation, hydrothermal processing, surfactant-assisted growth and template-assisted crystallization. The term “nanoparticle” should be supported by actual particle measurements.
It supplies barium for reaction with TiO2. Particle size, mixing and calcination conditions affect BaTiO3 formation and the amount of residual carbonate.
There is no single value applicable to every experiment. The observed transition depends on CO2 pressure, heating rate, particle size, sample geometry and atmosphere.
It has been investigated for sulfate removal through formation of poorly soluble BaSO4. The process must also control and measure residual dissolved barium.
Specific engineered particles have been studied experimentally, including as imaging carriers. These results do not establish general medical safety or regulatory approval.
The answer depends on the experiment, but assay, phase purity, trace impurities, particle-size distribution, surface area, moisture and batch consistency are frequently important.
BaCO3 reacts more readily with acids and is used as a reactive barium precursor. BaSO4 is substantially less soluble and is commonly selected where chemical stability and radiopacity are required.
Researchers should request a batch-specific COA, current SDS and technical data sheet. Particle-size or trace-element data may also be needed for sensitive applications.
Ma, M. G. et al. “Hierarchical BaCO3 structures prepared using soluble starch.” CrystEngComm, 2012. DOI: 10.1039/C2CE25832C.
Xu, A. W. and Wu, C. “Bio-inspired crystallization of BaCO3 using silk fibroin and compressed carbon dioxide.” CrystEngComm, 2014. DOI: 10.1039/C3CE41888J.
Karpov, T. E. et al. “Controllable nano- and micro-sized barium carbonate carriers for SPECT/CT imaging.” Journal of Materials Chemistry B, 2024. DOI: 10.1039/D3TB02480F.
Lee, B. W. et al. “Preparation of fine barium titanate powder from coated barium carbonate precursors.” Journal of Asian Ceramic Societies, 2014. DOI: 10.1016/j.jascer.2014.01.007.
Sánchez-Rodríguez, D. et al. “Thermal decomposition kinetics of barium carbonate films and powders.” Journal of Thermal Analysis and Calorimetry, 2024–2025. DOI: 10.1007/s10973-024-13318-x.
Barium carbonate is more than a conventional ceramic raw material. It is a useful model system for studying crystallization, morphology control, solid-state reactions, thermal decomposition and sulfate immobilization.
Reliable research requires attention to phase purity, particle structure, impurities, atmosphere and processing history. It also requires clear separation between established industrial functions and emerging laboratory findings.
AOZUN supplies barium carbonate for industrial processing and research evaluation. Buyers can contact AOZUN to discuss application requirements, available specifications, batch documentation, packaging and sample evaluation before placing a production order.
