Showing papers on "Brine published in 2003"

Water Soluble Acrylamidomethyl Propane Sulfonate (AMPS) Copolymer as an Enhanced Oil Recovery Chemical

Abstract: A high molecular weight (>106) copolymer of N,N-dimethyl acrylamide with Na-2-acrylamido-2-methylpropanesulfonate (NNDAM-NaAMPS) was prepared and characterized. The efficacy of the copolymer as an enhanced oil recovery (EOR) chemical was studied. Core flood tests using 72−150 mesh size unconsolidated sand having a porosity of 42% were carried out at different brine concentrations and temperatures. Initially, a crude oil fraction (150−300 °C) and, finally, the crude itself were used as the oils to be recovered. The copolymer was brine compatible. After a water flood, about 5.6% original oil in place (OIP) could be recovered by injecting 2000 ppm polymer solution to the sand pack containing oil fraction and 5000 ppm NaCl brine. The polymer solution was found to be thermally stable at 120 °C at least for a period of 1 month. It was further confirmed that the residual oil recovery increased with the increase of temperature. About 11% of OIP could be recovered as additional oil by injecting a 2000 ppm polymer ...

Production of lithium compounds directly from lithium containing brines

Abstract: Methods and apparatus for the production of low sodium lithium carbonate and lithium chloride from a brine concentrated to about 6.0 wt % lithium are disclosed. Methods and apparatus for direct recovery of technical grade lithium chloride from the concentrated brine are also disclosed.

Well treatment fluid and methods with oxidized chitosan-based compound

Abstract: The present invention provides a well treatment fluid that contains water, an oxidized chitosan-based compound, and a water-soluble compound having carbonyl groups, wherein the oxidized chitosan-based compound has the property of being soluble in water up to about 2 wt % while maintaining a viscosity of less than about 1000 cp. The water used for the well treatment fluid is selected from the group consisting of fresh water, seawater, natural brine, formulated brine, 2% KCl solution, and any mixtures in any proportion thereof. The present invention also provides a method of treating a subterranean formation penetrated by a wellbore comprising the steps of: (a) forming the well treatment fluid, and (b) contacting the subterranean formation with the fluid.

Electrically conducting, Ca‐rich brines, rather than water, expected in the Martian subsurface

Abstract: If Mars ever possessed a salty liquid hydrosphere, which later partly evaporated and froze down, then any aqueous fluids left near the surface could have evolved to become dense eutectic brines. Eutectic brines, by definition, are the last to freeze and the first to melt. If CaC12-rich, such brines can remain liquid until temperatures below 220 K, close to the average surface temperature of Mars. In the Martian subsurface, in intimate contact with the Ca-rich basaltic regolith, NaC1-rich early brines should have reacted to become Ca-rich. Fractional crystallization (freezing) and partial melting would also drive brines toward CaC12-rich compositions. In other words, eutectic brine compositions could be present in the shallow subsurface of Mars, for the same reasons that eutectic magma compositions are common on Earth. Don Juan Pond, Antarctica, a CaC12-rich eutectic brine, provides a possible terrestrial analog, particularly because it is fed from a basaltic aquifer. Owing to their relative density and fluid nature, brines in the Martian regolith should eventually become sandwiched between ice above and salts beneath. A thawing brine sandwich provides one explanation (among many) for the young gullies recently attributed to seepage of liquid water on Mars. Whether or not brine seepage explains the gullies phenomenon, dense, CaC12-rich brines are to be expected in the deep subsurface of Mars, although they might be somewhat diluted (temperatures permitting) and of variable salt composition. In any case, they should be good conductors of electricity.

Electrically conducting, Ca-rich brines, rather than water, expected in the Martian subsurface : Geophysical detection of surface water on Mars

Abstract: If Mars ever possessed a salty liquid hydrosphere, which later partly evaporated and froze down, then any aqueous fluids left near the surface could have evolved to become dense eutectic brines. Eutectic brines, by definition, are the last to freeze and the first to melt. If CaCl 2 -rich, such brines can remain liquid until temperatures below 220°K, close to the average surface temperature of Mars. In the Martian subsurface, in intimate contact with the Ca-rich basaltic regolith, NaCI-rich early brines should have reacted to become Ca-rich. Fractional crystallization (freezing) and partial melting would also drive brines toward CaCl 2 -rich compositions. In other words, eutectic brine compositions could be present in the shallow subsurface of Mars, for the same reasons that eutectic magma compositions are common on Earth. Don Juan Pond, Antarctica, a CaCl 2 -rich eutectic brine, provides a possible terrestrial analog, particularly because it is fed from a basaltic aquifer. Owing to their relative density and fluid nature, brines in the Martian regolith should eventually become sandwiched between ice above and salts beneath. A thawing brine sandwich provides one explanation (among many) for the young gullies recently attributed to seepage of liquid water on Mars. Whether or not brine seepage explains the gullies phenomenon, dense, CaCl 2 -rich brines are to be expected in the deep subsurface of Mars, although they might be somewhat diluted (temperatures permitting) and of variable salt composition. In any case, they should be good conductors of electricity.

Lithium isotope geochemistry and origin of Canadian shield brines.

Abstract: Hypersaline calcium/chloride shield brines are ubiquitous in Canada and areas of northern Europe. The major questions relating to these fluids are the origin of the solutes and the concentration mechanism that led to their extreme salinity. Many chemical and isotopic tracers are used to solve these questions. For example, lithium isotope systematics have been used recently to support a marine origin for the Yellowknife shield brine (Northwest Territories). While having important chemical similarities to the Yellowknife brine, shield brines from the Sudbury/Elliot Lake (Ontario) and Thompson/Snow Lake (Manitoba) regions, which are the focus of this study, exhibit contrasting lithium behavior. Brine from the Sudbury Victor mine has lithium concentrations that closely follow the sea water lithium-bromine concentration trajectory, as well as δ6Li values of approximately—28 %o. This indicates that the lithium in this brine is predominantly marine in origin with a relatively minor component of crustal lithium leached from the host rocks. In contrast, the Thompson/Snow Lake brine has anomalously low lithium concentrations, indicating that it has largely been removed from solution by alteration minerals. Furthermore, brine and nonbrine mine waters at the Thompson mine have large δ6Li variations of ∼30 %o, which primarily reflects mixing between deep brine with δ6Li of—35 ± 2‰ and near surface mine water that has derived higher δ6Li values through interactions with their host rocks. The contrary behavior of lithium in these two brines shows that, in systems where it has behaved conservatively, lithium isotopes can distinguish brines derived from marine sources.

As removal using ion exchange with Spent Brine Recycling

Abstract: A conventional sulfate-selective Type-2 polystyrene strong base anion resin was studied for arsenic (As) removal from Albuquerque, New Mexico, drinking water. Attention was focused on the regeneration aspects of ion exchange and the potential for reusing the spent brine directly without removing As. The major finding was that As-laden spent brine with makeup salt addition to 1 M chloride could be reused up to 20 times with no effect on As leakage and minimal effect on run length. The authors also found that As could be removed from the spent recycle brine using ferric hydroxide coagulation in such a way that the resulting sludge passed the toxicity characteristic leaching procedure test as a nonhazardous waste.

Method for combining heat from solar energy system with heat pump has solar panel output selectively directed to hot water tank or heat pump evaporator

Abstract: The solar panel (5) has a housing (18), glass outer sheet (19) and brine filled absorber (20) whose pumped output is recirculated through the hot water tank (1) heat exchanger (4) or the evaporator (7) of the heat pump (6). Heating (2) and hot water (3) circuits supply the household.

A novel ion exchange process for As removal

Abstract: The major drawback to the use of ion exchange for removal of arsenate [As(V)] from potable water is that other ions, especially sulfate (SO 4 ), compete with the As(V) for exchange sites, leading to early As breakthrough and As chromatographic peaks in the effluent. This article describes a novel approach for operating an ion exchange process in which an As(V)-rich zone is semipermanently retained in the operating columns so that only SO 4 -rich resin is regenerated. When the process was used in this study, essentially all the As(V) fed to the system was retained during treatment of >36,000 bed volumes of influent. This study also investigated the use of calcium or barium chloride salts to precipitate calcium sulfate or barium sulfate from the brine and the subsequent reuse of the brine solution. Overall, results indicate that the combination of modified column operation and brine recovery can dramatically reduce the brine requirement for As treatment by ion exchange.

Compositions for thermal insulation and methods of using the same

Abstract: A thermal insulating packer fluid contains at least one water superabsorbent polymer and optionally water and/or brine, and a viscosifying polymer. The composition is capable of inhibiting unwanted heat loss from production tubing or uncontrolled heat transfer to outer annuli. The viscosity of the composition is sufficient to reduce the convection flow velocity within the annulus.

Washing appliance water softener

Abstract: A water softener particularly for use in a dishwasher. The water softener is located in the dishwasher water supply (238) between the primary supply valve and the wash chamber. The softener includes a resin container (207) with an ion exchange resin (290). Water supplied to the wash chamber optionally passes through the resin container (207). Regenerating brine is developed in a brine container (203). The brine container (203) is supplied manually with solid salt (270) and water diverted into the container from the main supply at an air break (201). In the regenerating cycle brine is delivered from the brine container (203) to the resin container (207) by a pump (206). The duty cycle of the pump (206) determines the degree of regeneration of the resin (290).

System for the purification and reuse of spent brine in a water softener

Abstract: System and method for purifying and recycling spent brine in a water softener are provided. The system may be made up of a cation exchange resin tank fluidly coupled for passing spent brine comprising monovalent and divalent ions. A fluid mixer valve is coupled to the resin tank and to a water tank to dilute the spent brine to a desired concentration of a regenerant salt, e.g., NaCl. An ion-separation device is fluidly coupled to the fluid mixer valve to receive the diluted spent brine and separate the diluted spent brine into first and second streams. The first of the streams comprises monovalent ions and the second of the streams comprises divalent ions.

Water vapor transport in the vicinity of imbibing saline plumes: homogeneous and layered unsaturated porous media

Abstract: [1] Water vapor transport in the vicinity of imbibing saline solutions was investigated in two-dimensional (2-D) chambers using a light transmission technique. Concentrated NaNO3 solutions (brines) were applied as point sources to the surface of homogenous packs of prewetted silica sand for four different sand grades. The same solutions were applied to layered systems, where two horizontal fine layers were embedded within a coarser matrix, mimicking stratified sedimentary deposits. Water vapor transport from the residually saturated sand into the imbibing brine was observed in all sand grades and geometries. Pure water applied to sand prewetted with brine migrated into the surrounding residual brine. Water vapor stripping was found to enhance the lateral transport of brine in layered sand, where capillary barrier effects play a major role. Our observations suggest that osmotic potential and vapor density lowering in saline solutions, often neglected in predictive models, should be taken into account when predicting the transport of brines in the vadose zone.

Capacity investigation of brine-bearing sands for geologic sequestration of CO2

Abstract: Publisher Summary Geologic sequestration of carbon dioxide (CO 2 ) in brine-bearing formations has been proposed as a means of reducing the atmospheric load of greenhouse gases. The capacity of brine-bearing formations to sequester CO 2 is investigated using mathematical modeling of CO 2 injection and storage. CO 2 is injected in a supercritical state that has a much lower density and viscosity than the brine it displaces. In situ , it forms a gas-like phase, and also partially dissolves in the aqueous phase. The capacity factor has been defined as the volume fraction of the subsurface available for CO 2 storage and is conceptualized as a product of four factors that account for (1) two-phase flow and transport processes, (2) formation geometry, (3) formation heterogeneity, and (4) formation porosity. The key properties that impact the capacity factor include permeability anisotropy and relative permeability, brine/CO 2 density and viscosity ratios, brine salinity, the shape of trapping structure, formation porosity, and the presence of low-permeability layering. The space and time domains used to define capacity factor must be chosen carefully to obtain meaningful results. Often, there is no unique choice for the volume on which to base the capacity factor. One possible convention is to define a dynamic capacity factor that makes use of the self-similar nature of the Buckley-Leverett solution for the propagation of the CO 2 front away from the injection well.

Corrosion resistance of cement mortars containing spent catalyst of fluidized bed cracking (FBCC) as an additive

Abstract: The chemical corrosion and the mechanical strength were studied in cement mortars containing an additive of FBCC under conditions of long-term action of sodium sulphate solution or saturated brine. The observations have shown that saturated brine is a more aggressive agent, since it leaches Ca(OH)2 and contributes to the decomposition of the C-S-H phase thus worsening the compressive strength as compared with that of mortars kept in water. The addition of 20% FBCC inhibits the leaching process and counteracts the decrease of compressive strength in mortars kept in brine. On the other hand, sodium sulphate solution changes favourably the mortar microstructure, increases of the content of small pores and improves both the compressive and the flexural strengths, as compared with those of a mortar kept in water.

A reverse osmosis system with a pressure exchanger

Abstract: A pressure exchanger and a method for pressurising a first fluid by the pressure of a second fluid wherein each fluid influences surface areas of a sliding member individually. Due to differences in sizes of the surface areas, the first fluid can be pressurised to a pressure which is different from the pressure of the second fluid. The invention further provides a reverse osmosis desalination system with an RO membrane, an intake leading seawater into the chamber, and an outlet leading brine out of the chamber, wherein the seawater is pressurised by the brine in a pressure exchanger of the above mentioned kind.

Method for synthesizing crystalline magnesium silicates from geothermal brine

Abstract: Crystalline magnesium silicates are synthesized from silica-containing brines, preferably spent geothermal brines, by mixing the brine with a magnesium-containing compound, adjusting the pH of the resultant mixture between 8.0 and 14, and crystallizing the magnesium silicate from the mixture at a temperature between 50° C. and 200° C. Kerolite is preferably synthesized from brine by adjusting the pH in a range between 9.5 and 10.5 and heating the mixture to between 100° C. and 170° C. to precipitate the crystalline kerolite. The brine remaining after the crystallization step is depleted in silica and can be further processed without significant problems caused by silica scaling.