Showing papers on "Brine published in 1983"

Measurements of salinity and volume of brine excluded from growing sea ice

Abstract: The volume of brine excluded from growing sea ice and its salinity were measured using a brine sampler. The measurements were made, in both laboratory and field, under various growth conditions of the sea ice. The salinity of the brine becomes higher, and the volume flux decreases as the sea ice growth rate decreases. Consequently, the salt flux of the brine decreases with decreasing growth rate. In the case of sea ice growth at a constant rate, as the sea ice becomes thicker, the salinity of the brine excluded increases while its volume flux decreases. However, the salt flux is nearly independent of the ice thickness increase, at least up to a thickness of 15 cm. For sea ice growth rates between 1.7×10−5 and 1.4×10−4 cm s−1, and for a seawater salinity of 33.0‰, the brine salinity ranged from 42.3‰ to 92.7‰, the volume flux ranged from 6.3×10−6 to 3.4×10−5 cc cm−2 s−1, and the salt flux ranged from 6.4× 0−7 to 1.5×10−6 g cm−2 s−1.

Equilibrium of a microemulsion that coexists with oil or brine

Abstract: When salinity, or an equivalent variable, is increased, microemulsions generally undergo orderly transitions from a lower- to middle- to upper-phase. Even though the significance of such multiphase behavior has been well recognized in the design of surfactant flood processes, their quantitative nature in terms of the molecular structures of the surfactant lipophile, hydrophile, and the oil and brine salinity has not been fully understood. A theory of lower- and upper-phase microemulsions that gives reasonable predictions of their interfacial tensions (IFT's) and phase behavior is presented. In the theory, the surfactant monomers adsorbed at oil/brine interface cause the interface to bend as a result of an imbalance between the hydrophile/brine interaction on the one hand and lipophile/oil interaction on the other. With sufficient imbalance, high local curvature causes small drops of one phase to disperse into the other. In addition, interactions between these drops are taken into account for the microemulsion equilibrium. The theory also offers a possibility of being able to describe the hydrophile/ lipophile-balanced state (optimal salinity state of Healy and Reed/sup 1/) in terms of the tendency of surfactant layer at the oil/brine interface to bend.

Tertiary oil recovery

Abstract: An improved method for the recovery of tertiary oil from oil formations containing connate waters having a high brine concentration. A stable alcohol external microemulsion is formed from specific brine-soluble surfactants and alcohols for employment as a chemical slug. Such a microemulsion may be used to efficiently and effectively recover tertiary oil from formations in high brine concentrations. Specific examples of surfactants which may be employed to form the microemulsions of the present invention include amphoteric surfactants such as bis-2-hydroxyethylcocoamine propane sulfonate and bis-2-hydroxyethyloctadecyl amine propane sulfonate.

Origin of CaCl 2 brines by basalt-seawater interaction: Insights provided by some simple mass balance calculations

Abstract: Modern rift zone hydrothermal brines are typically CaCl2-bearing brines, an unusual chemical signature they share with certain oil field brines, fluid inclusions in ore minerals and a few uncommon saline lakes. Many origins have been suggested for such CaCl2 brines but in the Reykjanes, Iceland, geothermal system a strong empirical case can be made for a basalt-seawater interaction origin. To examine this mechanism of CaCl2 brine evolution some simple mass balance calculations were carried out. Average Reykjanes olivine tholeiite was “reacted” with average North Atlantic seawater to make an albite-chlorite-epidotesphene rock using Al2O3 as the conservative rock component and Cl as the conservative fluid component. The excess components released by the basalt to the fluid were “precipitated” at 275° C as quartz, calcite, anhydrite, magnetite and pyrite to complete the conversion to greenstone. The resulting fluid was a CaCl2 brine of seawater chlorinity with a composition remarkably similar to the actual Reykjanes brine at 1750 m depth. Thus, the calculations strongly support the idea that the Reykjanes CaCl2 brines result from “closed system” oceanic basalt-seawater interaction (albitization — chloritization mechanism) at greenschist facies temperatures. The calculation gives a seawater: basalt mass ratio of 3∶1 to 4∶1 (vol. ratio of 9∶1 to 12∶1), in keeping with experimental results, submarine vent data and with ocean crust cooling calculations. The brine becomes anoxic because there is insufficient dissolved or combined oxygen to balance all the Fe released from the basalt during alteration. Large excesses of Ca are released to the fluid and precipitate out in the form of anhydrite which essentially sweeps the brine free of sulfate leaving an elevated Ca concentration. The calculated rock-water interaction basically involves Na + Mg + SO4 ⇌ Ca + K, simulating chemical differences observed between oceanic basalts and greenstones from many mid-ocean ridges.

A study of solubility of strontium sulfate

Abstract: This paper describes the results of a solubility study of strontium sulfate in sodium chloride brine. A predictive equation for the solubility of strontium sulfate is presented, which is useful for calculating solubility in water containing 0 to 200 g/L (0 to 200 g/dm/sup 3/) sodium chloride at temperatures from 100 to 300/sup 0/ F (38 to 149/sup 0/ C), with pressures from 100 to 3,000 psig (689 to 20 684 kPa), and total ionic strengths of 0 to 3.43. This paper also describes the experimental technique employed and the special equipment designed for this study.

Control of metal-containing scale deposition from high temperature brine

Abstract: A method is disclosed for controlling the deposition of metal-containing scales, such as iron silicate scale, from a hot, aqueous, geothermal brine or the like, without substantial corrosion of brine handling equipment The brine is contacted with (1) an amount of an acid sufficient to reduce the pH of the brine between 01 and 05 unit and (2) a greater than stoichiometric amount of a reducing agent for reducing trivalent iron and manganese cations in a high temperature brine solution to divalent ions An overall decrease in scale deposition, especially of iron silicate scale, is achieved while a silver-rich scale can be recovered from silver-containing brines

Solution mining of trona or nahcolite ore with aqueous NaOH and HCl solvents

Abstract: Separate deposits of trona or nahcolite ore are solution mined with two solvents, aqueous sodium hydroxide and aqueous hydrogen chloride. Aqueous sodium carbonate solution is withdrawn from the region of the NaOH-treated ore deposit, for recovery of soda ash. Aqueous sodium chloride brine is withdrawn from the region of the HCl-treated ore deposit and introduced to an electrodialysis cell to regenerate the two solvents and thereby continue the solution mining cycle.

Method of treating well servicing fluids

Abstract: A method for removing heavy metals from brines used as well servicing fluids in which the heavy metal is oxidized to a higher, stable oxidation state of +3 or greater, the oxide or variants thereof of the oxidized metal is formed resulting in a generally water insoluble precipitate which is then removed by filtration leaving the brine free of deleterious amounts of the heavy metal.

Acidifiction of steam condensate for incompatibility control during mixing with geothermal brine

Abstract: A method is provided for combining a high pH steam condensate with a flow of an acidic geothermal brine from which the steam is extracted so as to inhibit the formation of suspended particulate matter by the chemical combining of impurities in the condensate and brine. The method includes acidifying the steam condensate, preferably by hydrochloric acid, to reduce the pH to between about 7 and about 5.5 and then permitting the acidified condensate to outgas such volatiles as hydrogen sulfide and carbon dioxide before combining the condensate with the brine, formation of such insolubles as heavy metal sulfides and calcium carbonate being thereby inhibited. In a silica crystallizer stage in which flashed brine is contacted with a silica seed material to cause silica removal from the brine, the treated condensate is combined with the brine in a low pressure crystallizer upstream of brine clarification and reinjection stages. Part of the treated condensate is flowed to various pumps in the geothermal brine power production system to purge pump seals and prevent pump scaling and excessive wear.

Acrylamide-alkylacrylamide copolymers

Abstract: Water soluble acrylamide/alkylacrylamide copolymers which are efficient viscosifiers of water or brine are described. They are made by processes which finely disperse the water insoluble alkylacrylamide into a water-external microemulsion or a micellar surfactant solution.

Alteration of clay minerals and zeolites in hydrothermal brines

Abstract: Clay minerals and zeolites, candidate backfill minerals for nuclear waste repositories, were treated with saturated NaC1 brine and Mg-rich (Mg-Ca-Na-K) brine at 200~ and 300~ for 4 weeks under a confining pressure of 30 MPa. The AI concentrations released in NaC1 brine were lower than those in Mg-rich brine at both temperatures indicating that the Mg-rich brine is more acidic than the NaC1 brine under these hydrothermal conditions. The Si concentrations in both brines were low because of the relatively acidic conditions developed during the hydrothermal treatment. As determined by X-ray powder diffraction or by specific Cs and Sr sorption measurements, no alteration could be detected in clay minerals treated with NaCI brine at 200~ Among the zeolites tested, only phillipsite and erionite altered to analcime in NaCI brine at 200~ Zeolites and most of the clay minerals tested did not alter in the Mg-rich brine treated at 200~ Vermiculite altered to randomly interstratified vermiculite/K- vermiculite (mica-like) by selective K uptake from the Mg-rich brine. At 300~ the clay minerals did not greatly alter, whereas the zeolites altered to analcime and/or albite in the presence of the NaC1 brine. In the Mg-rich brine, Al-rich montmorillonite from Wyoming did not alter, whereas Al-poor montmorillonite from Texas altered to randomly interstratified montmorillonite/ illite at 300~ Vermiculite collapsed to form K-vermiculite (~ 10.2 A) by the selective uptake of K from the Mg-rich brine at 300~ Most of the zeoliles altered to smectiles in the Mg-rich brine at 300~ because of the acidic conditions generated by the hydrolysis of Mg. The selective Cs-sorption K~ decreased from 11,700 for untreated phillipsite to 240 and 15 for the hydrothermally produced analcime/albite mixtures from the phillipsite at 200 ~ and 300~ respectively, in NaCI brine. These results suggest that montmo- rillonites and mordenites are relatively more resistant than vermiculite or other zeolites at elevated temperatures and pressures in concentrated hydrothermal brines expected in a salt repository.

Hydrothermal Reaction and Dissolution Studies of CsAISi5Or12 in Water and Brines

Abstract: The alteration of CsAlSi5O12, a possible host for 137Cs in tailored nuclear waste ceramics, was studied under simulated nuclear waste repository conditions of 100°, 200°, and 300°C with a confining pressure of 30 MPa. The cesium radiophase was found to be quite stable in water or 3N CaCl2, or 3N MgCl2 but not in 3N NaCl or 3N KCI or a bittern brine. The acid resistance of CsAlSi5O12 can be deduced from its stability in hydrothermal MgCl2 brine. Possible reaction mechanisms include the formations of pollucite and quartz in deionized water and the formation of Na or K feldspars and quartz in the presence of NaCl or KCl brines, respectively. A comparison of the various cesium aluminosilicates indicates that pollucite (CsAlSi2O6) is the best candidate for cesium-137 immobilization.

Cathode for the electrolytic production of hydrogen, and its use

Abstract: Cathode for the electrolytic production of hydrogen, having an active surface which comprises a nickel substrate and a coating film of dendrites of nickel or cobalt. This cathode can be used in a cell for the electrolysis of sodium chloride brine.

Process for removing aluminum and silica from alkali metal halide brine solutions

Abstract: A process for removing dissolved aluminum and silica contaminants from concentrated alkali metal halide brines used in membrane electrolytic cells is disclosed. The process involves contacting an acidified brine at a pH of between about 2.0 and about 3.0 with a strong macroreticular cationic chelating resin.

Recovery of silver-containing scales from aqueous media

Abstract: A method is disclosed for controlling the deposition of metal-containing scales, such as iron silicate scale, from a hot, aqueous, geothermal brine or the like, without substantial corrosion of brine handling equipment. The brine is contacted with (1) an amount of an acid sufficient to reduce the pH of the brine between 0.1 and 0.5 unit and (2) a greater than stoichiometric amount of a reducing agent for reducing trivalent iron and manganese cations in a high temperature brine solution to divalent ions. An overall decrease in scale deposition, especially of iron silicate scale, is achieved while a silver-rich scale can be recovered from silver-containing brines.

Improvements in or relating to freezers

Abstract: A freezer, having an outer housing (1) and a door (2), contains a number of shelves (3 to 6) upon which frozen food (7) is stored. Each shelf comprises a casing (8) filled with brine solution (10) having an eutectic temperature a few degrees lower than the desired operating temperature of the freezer. An evaporator coil (9), forming part of a refrigeration system; including a compressor, of the freezer, is immersed in the brine solution (10) in each casing. During the night storage period, the compressor is run on cheap rate electricity and the brine solution (10) gives up heat energy, thereby undergoing a phase change. During the daytime, the compressor is stopped and the brine solution (10) slowly absorbs heat energy from within the freezer, thereby slowly undergoing a reverse phase change and maintaining a substantially constant desired operating temperature of the freezer.

Removal of chlorate from electrolyte cell brine

Abstract: A process for removing chlorate ions from a recirculating anolyte brine as typically used in membrane chlor-alkali cells is disclosed. In this, a portion of the circulating brine after dechlorination and resaturation with additional alkali metal chloride is diverted and treated with a stoichiometric amount of hydrochloric acid to convert substantially all of the chlorate to chlorine gas and chloride ion. When performed in this manner, substantially lower quantities of acid are required as compared to prior art processes and the problems with the generation of ClO 2 are minimized.

Method for utilization of oil field waste brine to develop a salt gradient solar pond

Abstract: A process and method is disclosed for utilizing oil field waste brine to develop and maintain a salt gradient solar pond which in turn provides thermal energy for doing work, including improved separation of oil/brine emulsions into waste brine, crude oil, and natural gas; hot brine from the storage layer of the developed solar pond provides heat to a process heat exchanger which is intended to elevate the temperature of a working fluid such as an emulsion of crude oil and brine coming from producing oil wells prior to a separation process within a conventional heater treater. Less fuel is required to operate the heater treater. Waste brine from the crude oil process is utilized to develop and maintain the solar pond rather than simply being disposed.

Surfactant and alkali metal citrate composition for recharging a water softener

Abstract: Salt composition and method for regenerating spent water softener cation exchange resins, to remove or prevent the accumulation of iron in its various forms, insolubles, and oily deposits. The dry composition comprises from about 10 ppm to about 400 ppm of an alkylated diphenyl oxide disulfonate surfactant, from about 500 ppm to about 8000 ppm of sodium citrate, and as the remainder of the composition sodium chloride. The composition is preferably provided and used in the form of compacted products. The method for regenerating the spent cation exchange resin bed comprises the step of contacting the resin bed with an aqueous brine solution containing from about 25 to about 1200 ppm sodium citrate and from about 0.5 to about 60 ppm of alkylated diphenyl oxide disulfonate surfactant. The method is conveniently practiced by dissolving the composition first set forth above in the water of a conventional brine tank, using known technology.

Removal of Mg++ and Ca++ ions from NaCl brine

Abstract: Alkaline earth metal ions, e.g., Mg++ and/or Ca++, are removed from alkali metal brines, e.g., NaCl, by use of a particulate, macroporous, anion exchange resin containing the in-situ reaction product of polymeric, amorphous, hydrous zirconium oxide and a source of PO4 --- ions, e.g., H3 PO4.

Tenderness and Sodium Content of Pectoralis superficialis from Broilers Chilled in Potassium or Sodium Chloride Ice Slush

Abstract: Cooked light meat (Pectoralis superficialis) from broiler carcasses chilled (4 hr, with agitation) in 5% (w/w) sodium chloride (NaCl), 5% (w/w) potassium chloride (KCl), or ice slush was evaluated for moisture content, tenderness (shear force), chloride ion (Cl) concentration, and sodium ion (Na) concentration. Water uptake of the carcasses during chilling was determined. Chilling in either salt solution increased cooked meat moisture, increased chloride ion concentration, and decreased shear force values. Sodium level and water uptake were increased by NaCl brine ice-slush chilling. Samples chilled in NaCl had higher chloride concentrations and lower shear force than samples chilled in KCl.

Removing contaminates from a well fluid and well system

Abstract: An improved process for removing solid contaminates from a high density, salt-type aqueous drilling/completion packer fluid prior to its introduction into the well bore and for removing contaminates such as drilling mud and fluids from the well system prior to the introduction of brine to maintain the brine in a solids free state. To remove the solid contaminants, small effective amount of an alcohol and a suractant are added to the brine. After the solid contamin­ ates agglomerate, the solids are separated, leaving the brine in a substantially solids-free state. To remove the contaminates from the well system, treated water is prepared with a surfactant and alcohol admixed in clean water. Without interrupting circulation, the treated water displaces the fluids and drilling mud within the well system. Circulation of the treated water continues until substantially all of the contaminates are carried in the circulated treated water. The treated water may be preceded or followed by another fluid which assists in removing the contaminates. The solids-free brine is introduced into the well system to displace the treated water without exposure to the contaminates.

Reduction of available chlorine in alkali brines

Abstract: A process is described for removing available chlorine from a depleted recirculating anolyte brine of a chlor-alkali cell. After the spent brine is removed from the cell, and typically after dechlorination, it is reacted with an amount of an organic hydroxyl moiety-containing compound soluble in said brine for a residence time sufficient to substantially reduce the residual dissolved chlorine and hypohalite ion remaining in said brine prior to resaturation and reuse in said cell. Suitable hydroxyl moiety-containing compounds include alcohols and saccharides.

Treatment of geothermal brine sulfate-rich fluids to facilitate the precipitation of silica

Abstract: A method for the treatment of geothermal brines to control the precipitation of silica is disclosed. A sulfate-rich liquid is introduced into geothermal brine within a production well prior to flashing or is introduced into the residual geothermal brine remaining after the brine has been flashed to produce steam. The sulfate in the liquid reacts with the barium, calcium, and/or lead salts within the brine to produce a colloidal suspension which serves to accelerate precipitation of silica from the brine and to adsorb the precipitated silica particles. The colloidal suspension with its adsorbed silica particles is then removed from the brine by conventional gravimetric or filtration methods. The method of the invention substantially reduces the deposition of silica in wellbores and in energy extraction equipment and facilitates removal of the silica from the brine. The method further reduces the deposition of silica in injection wells wherein the silica cleansed brine is discharged.

Removal and recovery of magnesium, strontium and barium from brines

Abstract: Magnesium is removed from brine by contacting the brine with calcium hydroxide at temperatures above about 80° C but below the boiling point of the brine The contacting results in the formation of magnesium hydroxide precipitate which is substantially insoluble in the mother liquor at those temperatures and strontium hydroxide which is dissolved in the mother liquor When the contacting is carried out at a temperature above about 90° C, magnesium hydroxide precipitate is fast settling and filterable; accordingly, it is removed from the mother liquor by a conventional process, such as filtering The mother liquor is then cooled to cause the precipitation of at least a substantial part of strontium hydroxide present in the mother liquor The precipitate of strontium hydroxide is recovered by a conventional process such as filtering If precipitation upon cooling is insufficient, carbon dioxide gas is introduced into the mother liquor to effect the precipitation of strontium hydroxide Barium can be removed and recovered in the form of barium sulfate by reacting the remaining mother liquor with sodium sulfate In order to produce a faster-settling precipitate of magnesium hydroxide, the brine is contacted with a sufficient amount of a solution or slurry of calcium hydroxide in water to bring the concentration of magnesium in the resulting liquid to the range from about 0023 mols of magnesium per liter to about 004 mols of magnesium per liter