Barium Sulfate

• CAS: 7727-43-7
• Catalog Number: ACM7727437-4
• Category: Main Products

Case Study

StudY on barium sulfate in high-barium formation water

BinMerdhah, Amer Badr, Abu Azam Mohd Yassin, and Mazen Ahmed Muherei. Journal of Petroleum Science and Engineering 70.1-2 (2010): 79-88.

Scaling in surface and underground oil and gas production equipment has been recognized as a major operational problem. The permeability reduction caused by the deposition of barium sulfate in sandstone cores was investigated when injected seawater was mixed with formation water containing high concentrations of barium ions at different temperatures (50-80°C) and pressure differences (100-200°C). The solubility of the formed barium sulfate scale and how changes in salinity and temperature (40-90°C) affect its solubility were also studied. The morphology and particle size of the scale crystals shown by scanning electron microscopy (SEM) are also provided. The results show that the permeability impairment is largely caused by barium sulfate deposited on the rock pore surface. The reduction in rock permeability indicates the effect of barium ion concentration. Scanning electron microscopy (SEM) micrographs show the deposition of BaSO4 scale during the flow of injected water into the porous media.
For each experiment of barium sulfate scaling, 100 ml of each filtered opposite water was poured into a beaker at the same time. The synthetic brine was heated on a hot plate and the solution was stirred by a magnetic stirrer, then filtered through a 0.45 μm filter paper. After filtration, 5 ml of the filtrate was placed in a 50 ml volumetric flask and diluted to 50 ml of solution with distilled water. The instantaneous dilution of the brine containing BaSO4 is to prevent BaSO4 precipitation between filtration and analytical determination of the barium concentration. The determination of barium was calibrated by measuring a BaCl2 standard solution. The barium concentration in the diluted filtrate was determined by atomic absorption spectroscopy. After multiplication by the dilution factor, the exact concentration of barium was calculated.

Morphological and structural studies of barium sulfate

Judat, Bernd, and Matthias Kind. Journal of Colloid and Interface Science 269.2 (2004): 341-353.

Particle formation is the decisive step that controls the crystal morphology. In addition to the classical primary processes, nucleation and molecular growth, the particle size can also be increased by aggregation. The special case of self-assembled aggregation leads to the formation of highly ordered particles, which often have a porous internal structure. In the investigated experiments, the particle formation of barium sulfate was investigated. SEM analysis showed a variety of growth forms, including plate-like, star-shaped and spherical particles, while TEM exposure revealed a porous internal structure at all investigated supersaturation levels. Varying the supersaturation can affect the pore size and volume fraction. By combining a rapid sampling technique with cryo-TEM analysis, it has been shown that particles in the early stages of growth, shortly after the start of nucleation, consist of many small nanocrystallites aggregated in a highly ordered manner. The diffraction pattern shows many small-angle grain boundaries, while the particles at the end of the precipitation process are single crystalline. It is concluded that barium sulfate grows according to a self-assembled aggregation mechanism followed by a rapid recrystallization process.
The experiments were carried out in a precipitation apparatus using two gear pumps (P1A, P1B) to generate the volume flow of the reactant solutions and a Y-type mixer (M) as a mixing device. After mixing, the solution containing barium and sulfate left the nozzle in the form of a free jet. The inlet diameter of the mixer was 1.2 mm and the outlet diameter was 2 mm. The angle between the inlet pipe and the horizontal axis was 15°. At the end of the outlet pipe there was an acceleration section with a diameter of 1.5 mm to suppress turbulence and smooth the free jet. With the help of the mixing chamber, the barium chloride and sodium sulfate solutions were mixed to produce barium sulfate. The measured pressure losses showed that short micromixing times in the range of 10 seconds could be achieved in order to eliminate any influence of mixing on the particle formation process.

The biokinetics of barium sulfate nanoparticles

Konduru, Nagarjun, et al. Particle and fibre toxicology 11 (2014): 1-15.

Pulmonary exposure to instilled barium sulfate nanoparticles, BaSO4 NPs, resulted in dose-dependent lung injury and inflammation. Inhalation of high concentrations (50 mg/m) of BaSO4 NPs for 4 and 13 weeks induced minimal pulmonary responses and no systemic effects. Instilled and inhaled BaSO4 NPs were rapidly cleared but produced higher tissue retention than when ingested. Particle dissolution is a possible mechanism. Injected BaSO4 NPs localized to the reticuloendothelial organ and redistributed to the bone over time. BaSO4 NPs exhibited lower toxicity and biopersistence in the lungs compared to other poorly soluble nanoparticles.
Tissue distribution was compared 28 days after intratracheal (IT) instillation and 7 days after oral and intravenous (IV) injections of BaSO. Rats were exposed to 50 mg/m BaSO4 aerosol for 4 or 13 weeks (6 h/day for 5 days/week) followed by macroscopic and histopathological, blood, and bronchoalveolar lavage (BAL) fluid analysis. BAL fluid from rat infusions was also analyzed. . At 7 days, only 0.15% of the gavage dose was detected in all organs. Intravenously injected BaSO4 NPs were primarily localized to the liver, spleen, lungs, and bones at 2 h but redistributed from the liver to the bones over time. Fecal excretion was the major elimination route for all three exposure routes.

Interaction studies of EDTA with barium sulfate

Jones, Franca, et al. Journal of colloid and interface science 316.2 (2007): 553-561.

The carboxylic acid molecule EDTA (ethylenediaminetetraacetic acid) is a complexing agent known to interact with many cations. A variety of techniques were employed to elucidate the mechanism of interaction between EDTA and barium sulfate. It was shown that complexation is not sufficient to explain the inhibition of barite crystallization, but that other processes, such as chemisorption, must also occur. Interestingly, EDTA adsorbs in a deprotonated form regardless of solution morphology - indicating that the molecule is able to lose protons at lower pH values upon adsorption. Molecular modeling suggests that the interaction of surface barium ions with carboxylic acid groups is an important factor: this is the underlying reason why these molecules are good at complexing cations. Finally, in situ turbidity measurements were obtained to determine the mechanism of nucleation/growth modification.
The adsorption experiments consisted of equilibrating 30 mL of EDTA solution with 0.10 g of barite solid and adjusting to the desired pH with a small amount of HCl or NaOH. If necessary, the pH was further adjusted after 24 h and re-equilibrated during the final 24 h. The adsorbed organic spectrum was obtained by subtracting the spectrum of barium sulfate in solution at a given pH from the spectrum of organic + barium sulfate in solution at the same pH. However, this does mean that the dissolved organics make some contribution to the spectrum. This contribution is expected to be small given the small penetration depth and large surface area of the barium sulfate used. The differences observed between the solution and adsorbed spectra confirm that the solution species do not significantly affect the IR results.

Custom Q&A

What is the molecular formula of Barium Sulfate?

The molecular formula of Barium Sulfate is BaSO4.

What are the synonyms for Barium Sulfate?

The synonyms for Barium Sulfate are Barite, Barytes, and Barium sulphate.

What is the molecular weight of Barium Sulfate?

The molecular weight of Barium Sulfate is 233.39 g/mol.

Is Barium Sulfate soluble in water?

No, Barium Sulfate is insoluble in water.

What is the density of Barium Sulfate?

The density of Barium Sulfate is 4.25-4.5 g cm-3.

How is Barium Sulfate used in industry?

Barium Sulfate is used as a weighting mud in oil drilling, in paints, paper coatings, linoleum, textiles, and rubber.

How is Barium Sulfate used in medicine?

Barium Sulfate is administered internally as a radio-opaque diagnostic aid, often called a "barium cocktail", and is used as a contrast agent in diagnostic x-ray procedures.

What does the acronym LCSS stand for in relation to Barium Sulfate?

LCSS stands for Laboratory Chemical Safety Summary, which is a datasheet providing information on the chemical safety of Barium Sulfate.

What is the IUPAC name of Barium Sulfate?

The IUPAC name of Barium Sulfate is barium(2+);sulfate.

How is Barium Sulfate ingested for enhanced visualization of the gastrointestinal tract?

Barium Sulfate is ingested by mouth or administered rectally and combined with granules of effervescent bicarbonate to enhance distension of the GI tract.