Systems and methods for carbon dioxide sequestration and neutralization of water body acidification using alkaline fluids

Abstract

The carbon dioxide sequestration method includes extracting an alkaline fluid from a natural source, such as surface water, shallow subsurface / groundwater, deep subsurface water, hydrothermal brine, oil field brine, subsea brine, and / or evaporite brine. At least one of the alkaline fluid and / or aggregate substrate formed at least in part by the alkaline fluid is transported to a target deployment location in the body of water, such as by transport vessel, flexible barge, well, pipeline, waterway / pipe, natural channel and / or slope, freezing and rafting process, and / or buoy / substrate. The method includes enhancing the alkalinity of at least a portion of the water body based at least in part on the alkaline fluid, thereby facilitating sequestration of atmospheric carbon dioxide in the body of water.

Description

[Technical Field]

[0001] CROSS-REFERENCE TO RELATED APPLICATIONS

[0001] This application claims priority to and the benefit of U.S. Provisional Patent Application No. 63 / 393,381, filed July 29, 2022, entitled "Systems and Method for Sequestering Carbon Dioxide Using Alkaline Fluids," the disclosure of which is incorporated herein by reference in its entirety. [Background technology]

[0002] background FIELD OF THE INVENTION

[0002] Embodiments described herein relate to sequestering atmospheric carbon dioxide and neutralizing the acidification of bodies of water, and more particularly to methods of using and distributing alkaline fluids for carbon dioxide sequestration and / or to enhance carbon dioxide sequestration systems.

[0003]

[0003] Due to human activities, atmospheric carbon dioxide (CO2) has increased by approximately 50% (from about 280 to 420 ppm) over the past 200 to 300 years due to population growth, fossil fuel combustion, land-use change, and other industrial processes. This anthropogenic increase in atmospheric CO2 has led to a variety of environmental and societal problems, including global warming, increased forest fires, increased droughts, increased storm severity and frequency, rising sea levels, melting glaciers, and ocean acidification. One of the major challenges facing humanity in the 21st century is to develop scalable systems and / or methods for removing CO2 from the atmosphere so as to stabilize and reduce atmospheric CO2 and neutralize the acidification of natural water bodies, thereby limiting the environmental and humanitarian damage associated with increased atmospheric CO2. Thus, there is a need for systems, methods, and / or materials for facilitating carbon capture and / or sequestration and neutralizing the acidification of water bodies. Summary of the Invention [Means for solving the problem]

[0004] overview In some implementations, a method for sequestrating carbon dioxide includes extracting an alkaline fluid from a natural source, such as surface water, shallow subsurface / groundwater, deep subsurface water, hydrothermal brine, oil field brine, subsea brine, and / or evaporite brine. At least one of the alkaline fluid and / or aggregate substrates formed at least in part by the alkaline fluid is transported to a target deployment location in the body of water, such as by a transport vessel, flexible barge, well, pipeline, waterway / pipe, natural channel and / or slope, freezing and rafting process, and / or buoy / substrate. The method includes enhancing the alkalinity of at least a portion of the water body based at least in part on the alkaline fluid, thereby facilitating sequestration of atmospheric carbon dioxide and / or neutralization of acidification in the body of water. [Brief explanation of the drawings]

[0005] BRIEF DESCRIPTION OF THE DRAWINGS [Figure 1]

[0005] FIG. 1 is a schematic diagram of a process for using alkaline fluid for CO2 capture and / or sequestration, according to one embodiment. [Figure 2]

[0006] 1 is a flowchart of a method for enhancing alkalinity, according to one embodiment. DETAILED DESCRIPTION OF THE INVENTION

[0006] Detailed Description

[0007] FIELD OF THE INVENTION

[0002] Embodiments described herein relate to the sequestration of atmospheric carbon dioxide, and more particularly to methods of using and distributing alkaline fluids for carbon dioxide sequestration and / or to enhance carbon dioxide sequestration systems. Alkaline fluids suitable for use in CO2 sequestration can be derived from natural or industrial reactions of water with alkaline minerals. For example, alkaline minerals such as metal silicates, carbonates, and / or evaporites are globally abundant—forming approximately 45% of Earth's continental crust (covering approximately 30% of the Earth's surface) and nearly 100% of the subsurface (i.e., below the upper sedimentary layer) oceanic crust (covering approximately 70% of the Earth's surface).

[0007]

[0008] Some examples of idealized metal silicate carbonation reactions that produce alkaline fluids (e.g., water) suitable for CO2 sequestration and / or neutralizing the acidification of water bodies are as follows: Mg2SiO4+2CO2+2H2O→2MgCO3+H4SiO4 (magnesium silicate) CaSiO3 + CO2 + 2H2O → CaCO3 + H4SiO4 (calcium silicate) Fe2SiO4+2CO2+2H2O→2FeCO3+H4SiO4 (iron silicate) Mg3Si2O5(OH)4 + 3CO2 + 2H2O → 3MgCO3 + 2H4SiO4 (hydrated magnesium silicate) Na x (Ca, Mg, Fe) y Si3AlO8+(x+2y+3)H + +(4+y)H2O+yCO2→xNa + +y(Ca,Mg,Fe)CO3+3H4SiO4+2y(H + ) (Plagioclase group silicates)

[0008]

[0009] Some examples of carbonate mineral dissolution reactions that produce alkaline fluids (e.g., water) suitable for CO2 sequestration are as follows: CaCO3 → Ca 2+ +CO3 2- (Limestone) MgCa(CO3)2 → Mg 2++Ca 2+ +2CO3 2- (Dolostone) MgCO3 → Mg 2+ +CO3 2- (magnesite) Na2CO3→Na 2+ +CO3 2- (Soda Ash)

[0009]

[0010] CO3 liberated from these carbonate dissolution reactions 2- The ions form free H via the following reaction: + (proton) is taken up. CO3 2- +H + →HCO3 -

[0010]

[0011] Some examples of metal oxide mineral dissolution reactions that produce alkaline fluids (e.g., water) suitable for CO2 sequestration are as follows: MgO+H2O→Mg 2+ +2OH - (magnesia) CaO+H2O→Ca 2+ +2OH - (Slaked lime)

[0011]

[0012] Some examples of metal hydroxide mineral dissolution reactions that produce alkaline fluids (e.g., water) suitable for CO2 sequestration are as follows: Mg(OH)2 → Mg 2+ +2OH - (Blue Sight) Ca(OH)2 → Ca 2+ +2OH - (Slaked lime)

[0012]

[0013] The OH released from this reaction - The ions form free H via the following reaction: + (protons) can be absorbed. OH - +H + →H2O

[0013]

[0014] Therefore, these dissolution reactions occur in the presence of free H + By decreasing CO₂ and increasing the alkalinity of surface waters (which both increases pH and acts to reverse acidification) (e.g., by ocean alkalinization or alkalinity enhancement), the following carbonate equilibrium shifts to the right, resulting in a net transfer of atmospheric CO₂ to aquatic CO₂ via Henry's law, re-establishing carbonate equilibrium: CO 2(ガス) →H2O+CO 2(aq) →↓H + +HCO3 - →↓2H + +CO3 2-

[0014]

[0015] Underwater HCO3 - and CO3 2- Ions can be stable in natural aqueous systems such as lakes, ponds, rivers, seas, and oceans, and can remain stable for hundreds to thousands of years.

[0015]

[0016] One known method of using alkaline minerals for CO2 sequestration involves mining the minerals from natural deposits and then crushing and pulverizing them to a very small size (e.g., particle size of about 100 microns to 300 microns) to increase their reactive surface area. The crushed / pulverized minerals and alkalinity (e.g., CO3 2- , HCO3-, OH-) and divalent cation concentrations (e.g., Ca 2 +, Mg 2+ , Fe 2+ (e.g., water) to increase its ability to absorb CO2 and mineralize it as solid carbonate minerals (e.g., CaCO3, MgCO3, FeCO3). In this regard, in some cases, crushed and / or finely ground alkaline minerals are added and / or dispensed into natural surface waters, coastlines, and / or rivers, and then react and / or dissolve to increase the alkalinity of these waters. The resulting reaction shifts the carbonate equilibrium of the water in favor of CO2 sequestration from the atmosphere into the alkalized water.

[0016]

[0017] However, this processing of alkaline minerals requires extensive grinding and milling of the minerals to particle sizes of 100 to 300 microns to increase their reactive surface area and increase their CO2 sequestration rate to a level capable of contributing to the stabilization or reduction of atmospheric CO2. Furthermore, the hardness and density of some alkaline minerals (e.g., metal silicates) make them expensive to grind / mill from both an energy standpoint and a CO2 emissions standpoint, which reduces the value of CO2 sequestration on both the top line (i.e., after revenue reduction due to energy costs) and bottom line (after revenue reduction due to CO2 emissions costs), thereby reducing the economic viability of this CO2 sequestration method.

[0017]

[0018] The rate and extent of CO2 sequestration via reaction with alkaline minerals can also be increased by heating the reactants, but this is also expensive from both an energy and CO2 emissions perspective, reducing the economic viability of this CO2 sequestration method. The cost of CO2 sequestration via industrial weathering of crushed, pulverized, and / or heated alkaline minerals can exceed the CO2 credit value generated from the reaction, making this process economically unviable as a method for sequestrating atmospheric CO2. Additionally, quantifying the CO2 sequestered via the release of alkaline minerals into natural water and / or bedrock systems can be difficult due to the open nature and relatively slow reaction times of these systems. Furthermore, the products of the reaction of alkaline minerals with CO2 and water (e.g., clays, solid carbonate minerals, metal silicates, etc.) are chemical by-products / waste products, the disposal of which can incur additional costs (e.g., economic, energy, and / or environmental).

[0018]

[0019] Another conventional method of using alkaline minerals for CO2 sequestration that avoids the high costs of crushing, pulverizing, and / or heating alkaline minerals involves injecting a pure CO2 stream (e.g., from a fossil fuel-burning power plant or other industrial source) into alkaline rock, where the injected CO2 reacts with divalent cations (Ca, Mg, Fe) and alkalinity (CO3) dissolved in groundwater within the rock. 2- , HCO3 - , O.H. - ) and durably sequestered in the form of solid carbonate minerals (e.g., CaCO3, MgCO3, FeCO3). In such applications, the slow reaction kinetics between alkaline fluids and unfinely divided metal silicates are overcome by allowing existing groundwater to react with metal silicate rock over many years to generate the alkalinity and divalent cations needed to sequester the introduced CO2, in some cases at elevated temperatures that accelerate the kinetics of these reactions. Via this route, CO2 is injected (directly or indirectly) into metal silicate rock and associated alkaline and high total dissolved solids (TDS) groundwater and converted to solid carbonate minerals (e.g., CaCO3, MgCO3, FeCO3).

[0019]

[0020] However, in some cases, the conversion of gaseous or liquefied CO2 to solid carbonate minerals after injection into alkaline bedrock can increase the local bedrock volume by up to 30%, causing the bedrock to expand and heave. This can quickly form hills above the injection site, altering the natural landscape and built environment, resulting in increased local earthquake frequency, and potentially contaminating local groundwater, creating environmental, geological, and public health hazards often associated with hydraulic fracturing ("fracking"). Furthermore, CO2 injection sites into alkaline bedrock are limited, and transporting the pure CO2 stream to the injection site can require costly and cumbersome infrastructure and / or delivery methods. The capacity of the injection site to store the pure CO2 stream is also limited. Once the injection site's capacity to store CO2 is exceeded, new injection sites are located and excavated, and infrastructure to deliver the pure CO2 stream is relocated and rebuilt. Typically, there is a lag of 1-10 years between when CO2 is injected into alkaline rock and when the CO2 is stably sequestered as solid carbonate minerals, during which time the injected CO2 can rise back up into the surface layers of the alkaline rock and re-enter the atmosphere. In some cases, alkaline rock can be relatively soluble (e.g., limestone), so a large portion of the rock dissolves in its associated water after CO2 injection, resulting in potential collapse (e.g., sinkholes).

[0020]

[0021] Chemical weathering of alkaline minerals is one of the primary pathways for CO2 sequestration over geological timescales, from Earth's fast carbon cycle in the atmosphere and upper ocean to the slower carbon cycle in the deep ocean, marine sediments, and marine limestones. However, the relatively slow rates of these chemical reactions pose challenges for industrially adapting these reactions so that CO2 can be sequestered by this process at a scale that can stabilize and / or reduce atmospheric CO2 and associated adverse environmental and socioeconomic impacts. The potentially high costs of alkaline fluid and mineral extraction and / or alkaline mineral milling, as well as the potentially high costs of transporting alkaline materials to target locations, typically make conventional CO2 sequestration methods via alkalinity enhancement and / or weathering enhancement economically unfeasible. For at least the reasons set forth above, such known methods of chemical weathering of alkaline minerals to sequester CO2 are not suitable for large-scale, atmospherically significant carbon sequestration.

[0021]

[0022] In contrast, embodiments and / or methods described herein relate to low-energy CO2 sequestration methods, for example, using globally abundant, naturally occurring alkaline fluids. In some implementations, naturally occurring alkaline fluids can be used to capture and / or sequester CO2 from Earth's fast carbon cycle (e.g., the upper ocean and atmosphere) to its slow carbon cycle (deep ocean, marine sediments, rocks, and other upper subsurface reservoirs). Generally, alkaline fluids are naturally high in pH (e.g., alkaline or basic), alkalinity, and divalent cation concentration. This makes alkaline fluids suitable for large-scale CO2 sequestration via alkalinity enhancement (e.g., marine, estuarine, or freshwater) and / or mineralization. In some cases, naturally occurring alkaline fluids can also have high temperatures at the extraction point, which can be advantageous when used, for example, to produce substrates aggregated with cementitious binders and / or polysaccharide hydrogel binders. For example, naturally occurring high temperatures can reduce heat input that could otherwise be used to activate and / or harden such binders. In some cases, high divalent cation concentrations and high alkalinity can also speed up the activation and / or hardening process of cementitious binders and / or hydrogel binders. Such substrates can then be used in CO2 sequestration systems and / or methods, as described in more detail herein.

[0022]

[0023] For example, in some implementations, a method for sequestrating carbon dioxide includes extracting an alkaline fluid from a natural source, such as surface water, shallow subsurface / groundwater, deep subsurface water, hydrothermal brine, oil field brine, subsea brine, and / or evaporite brine. The alkaline fluid is transported to a target deployment location in the body of water by, for example, a transport vessel, a flexible barge, a well, a pipeline, a waterway / pipe, a natural channel and / or slope, a freezing and rafting process, and / or a buoy / substrate. The method includes enhancing the alkalinity of at least a portion of the body of water based at least in part on the alkaline fluid. The method includes enhancing the alkalinity of at least a portion of the body of water based at least in part on the alkaline fluid, thereby facilitating sequestration of atmospheric carbon dioxide in the body of water.

[0023]

[0024] In some implementations, the alkaline fluid can be used to produce substrates, aggregates, and / or other materials, which in turn are used to capture and / or sequester CO2. For example, in some implementations, a method for sequestrating carbon dioxide includes extracting an alkaline fluid from a natural source and forming an aggregate substrate. At least a portion of the aggregate substrate is activated via the alkaline fluid, the activation resulting in at least one of binding or hardening of at least a portion of the aggregate substrate. The aggregate substrate is deployed at a target deployment location in the body of water. The method includes increasing the alkalinity of at least a portion of the body of water based at least in part on the aggregate substrate deployed therein.

[0024]

[0025] In some embodiments, any suitable system can be used to extract and / or deliver the alkaline fluid in any desired manner. For example, in some embodiments, a system for alkalinity enhancement can include an extractor configured to extract the alkaline fluid from a natural source. The system can further include a conveyor configured to deliver at least one of the alkaline fluid or aggregate substrate at least partially formed by the alkaline fluid to a target deployment location in the body of water, where the at least one of the alkaline fluid or aggregate substrate delivered to the target deployment location is operable to enhance the alkalinity of at least a portion of the body of water.

[0025]

[0026] Any of the embodiments and / or methods described herein may also provide for and / or include determining a target location based on one or more characteristics associated with a portion of a body of water. Additionally, any of the embodiments and / or methods described herein may provide for and / or include estimating the amount of atmospheric CO sequestered via reaction with the dispensed alkaline fluid, which in some cases may be assessed and sold as carbon offset credits.

[0026]

[0027] In some embodiments, the alkaline fluid can be used to neutralize acids or acidic substances released through additional or other processes associated with CO removal, such as the settling of biomass (e.g., macroalgae and / or any other biomass) into a body of water, which in some cases may release small amounts of organic acids into the body of water. In some embodiments, the alkaline fluid can be used to capture and / or durably retain in solution CO released through additional or other processes associated with CO removal, such as the settling of biomass into a body of water, which may release small amounts of CO to the body of water and / or atmosphere, such as through microbial remineralization of particulate organic carbon and / or dissolved organic carbon. Examples of devices, systems, and / or methods for CO removal using water-based (e.g., marine-based) technologies, such as sinking biomass, include, but are not limited to, U.S. Patent No. 11,382, filed June 8, 2021, entitled "Systems and Methods for the Cultivation of Target Product."No. 315 (the "'315 Patent"), U.S. Patent Application Publication No. 2023 / 0106744 (the "'744 Publication"), entitled "Systems and Methods for Quantifying and / or Verifying Ocean-Based Interventions for Sequestering Carbon Dioxide," filed on September 30, 2022, U.S. Patent Application Publication No. 2023 / 0152292 (the "'292 Publication"), entitled "Systems and Methods for Monitoring Ocean-Based Carbon Dioxide Removal Devices and Accumulation of a Target Product," filed on January 19, 2023, International Patent Application No. PCT / US2023 / 064917 (the "'917PCT"), entitled "Floating Substrates for Offshore Cultivation of Target Products and Methods of Making and Using the Same," filed on March 24, 2023, and U.S. Patent Application Publication No. PCT / US2023 / 064917 (the "'917PCT"), entitled "Floating Substrates Including Carbonaceous Coatings for No. PCT / US2023 / 064919 ("'919PCT"), filed March 24, 2023, entitled "Offshore Cultivation of Target Products and Methods of Making and Using the Same," and / or U.S. Provisional Patent Application No. 63 / 401,959 ("'959 Provisional"), filed August 29, 2022, entitled "Ocean-Based Carbon Removal Systems and Methods of Using the Same," the disclosures of each of which are incorporated herein by reference in their entirety.

[0027]

[0028] 1 is a schematic diagram of a process 100 for using alkaline fluid for CO capture and / or sequestration, according to one embodiment. Generally, the process 100 involves extracting alkaline fluid 102 from a natural source 101 and distributing the alkaline fluid 102 into a body of water 104, such as the ocean, where the alkaline fluid can enhance and / or increase the alkalinity of the surrounding water, which in turn can increase its ability to capture and / or sequester CO, as described in detail above.

[0028]

[0029] Naturally occurring alkaline fluid 102 can be found in natural sources 101, such as within alkaline mineral deposits including, for example, metal silicates (e.g., mafic and / or ultramafic igneous rocks), limestone, dolostone, and / or evaporite deposits. More specifically, natural sources 101 can be alkaline mineral deposits that host alkaline groundwater and / or brines, including, for example, metal silicates (e.g., mafic / ultramafic igneous rocks), carbonates (e.g., limestone, dolostone, magnesite), and evaporite deposits (e.g., brucite).

[0029]

[0030] Other natural sources 101 of alkaline fluid 102 may be, for example, surface water, shallow subsurface / groundwater, deep subsurface water, hydrothermal brines, oil field brines, subseafloor brines, and / or evaporitic brines. More specifically, surface waters may include any alkaline water found on the surface of land or ocean, including, for example, alkaline lakes, rivers, cold springs, hot springs, and / or alkaline freshwater lenses that float on the surface of the ocean due to their relative low density; shallow subsurface waters may include, for example, groundwater found in the upper portions of the continental crust; deep subsurface waters may include, for example, basin brines, which are brines trapped in ancient basins (geosynclines) that are now surrounded by land and potentially buried deep beneath sediments and rocks; and hydrothermal brines may be brines formed via the reaction of, for example, water, seawater, or brines with alkaline hot rocks and / or magma. oilfield brines can include, for example, brines coexisting with oil and / or gas deposits, in some cases extracted and isolated via drilling into and / or extracting oil and / or gas from the earth; subsea brines can include, for example, brines derived from reaction with seawater that has infiltrated the oceanic crust and reacted with alkaline basalt in the upper layers of the oceanic crust and / or highly alkaline ultramafic sediments in deeper layers of the oceanic crust; and evaporite brines can include, for example, brines produced from the partial evaporation of meteoric water, seawater, or other natural waters in landlocked or marginal ocean basins and the resulting ionic concentrates. In some implementations, alkaline fluids 102 (e.g., water) can be extracted from these various natural sources 101 via conventional well drilling, recirculation, and / or other surface collection methods.

[0030]

[0031] Although described as occurring naturally and / or extracted from natural sources 101, alkaline fluid 102 can also be produced through industrial reactions (e.g., weathering) of finely divided alkaline minerals with fluids (e.g., water), as described above. However, the mining, transportation, milling, and reaction processes for alkaline minerals are costly in terms of time, money, and CO2 emissions. In contrast, utilizing natural alkaline fluids in CO2 sequestration can be more efficient because the fluid-rock reactions that produce the unique chemistry of alkaline fluids useful for CO2 sequestration have already occurred in natural geological systems for many years, and in some cases at high pressures and temperatures that may be difficult to efficiently replicate in industrial sites. Moreover, extraction and / or transportation of naturally occurring alkaline fluids can be carried out using relatively efficient existing technologies. However, in some cases, industrially produced alkaline fluids and / or alkaline fluids that are waste or by-products of other industrial processes may be used in CO2 sequestration processes, for example, in a manner similar to that described herein for naturally occurring alkaline fluids.

[0031]

[0032] Any suitable system, device, and / or method for extracting alkaline fluid from any suitable source (e.g., the natural sources described above) can be used in the embodiments described herein. Such systems and / or devices that perform the extraction methods are generally referred to herein as "extractors." For example, a non-exhaustive list of suitable extractors can include, but is not limited to, wells, pumps, pipelines, siphons, hydraulic injection systems, etc.

[0032]

[0033] As described above, the alkaline fluid 102 can be extracted via conventional processes from a natural source 101 (or an industrial source, if industrially produced). Once extracted, it may be desirable to distribute the alkaline fluid 102 throughout an environment where CO2 capture and / or sequestration can be efficiently carried out. For example, as shown in FIG. 1, the alkaline fluid 102 can be distributed to and / or along a target location in a body of water 104, such as an ocean, sea, lake, estuary, river, etc. In some cases, the target location can be determined based at least in part on the efficiency and / or effectiveness of CO2 sequestration (e.g., by the water body 104 or portion thereof having enhanced alkalinity resulting from the presence of the alkaline fluid 102, by the alkaline fluid 102 itself, and / or by any additional / other suitable carbon removal intervention).

[0033]

[0034] In some implementations, the target location may include a location where the water temperature is low enough to inhibit the precipitation of dissolved alkalinity as solid (e.g., mineral) alkalinity. For example, precipitation may release a portion of the CO2 initially removed via the addition of alkaline fluids to a natural water body. Because the solubility of CO2 in seawater increases with decreasing water temperature, delivering cooler water for CO2 removal via alkalinity enhancement may also increase the rate and extent of CO2 removal in response to alkalinity enhancement. In some implementations, the target location may include an upwelling region / zone of a water body (or conversely, avoidance of a downwelling zone), because alkalinity released into an upwelling region / zone can remain in surface waters longer than if released into a non-upwelling or downwelling zone, thereby increasing the amount of time CO2 can enter, be captured, and / or react in the alkalinized surface water and thus increasing the amount of CO2 transferred from the atmosphere to the alkalinity-enhanced water body.

[0034]

[0035] In some implementations, for example, determining the target location can be based on collection and / or historical data associated with the body of water 104, environmental conditions, deployment methods, and / or any other suitable data. In some implementations, determining the target location and / or determining the desired efficiency and / or effectiveness of CO2 sequestration can include using a system and / or method in which one or more machine learning models, etc., are implemented to analyze collected data and / or provide predicted outputs, etc. For example, such a system and / or method can be similar to or substantially identical to any of the systems and / or methods (or portions thereof) described in the '744 Publication previously incorporated by reference.

[0035]

[0036] In some implementations, the amount of CO2 removed via alkalinity enhancement can be quantified and / or verified through measurement and / or prediction of the change in dissolved inorganic carbon (DIC) in the water body before and after alkalinity enhancement and / or by the change in the total alkalinity of the water body before and after deployment. In some implementations, such measurement and / or prediction can include the use of one or more efficiency factors that describe and / or are associated with the increase in dissolved inorganic carbon per unit increase in total alkalinity (e.g., such that the efficiency factor does not exceed 1). If the total volume of the alkalinized portion of the water body is known, the total CO2 removed via alkalinity enhancement can be calculated by multiplying the change in measured DIC concentration (for a given water sample) by the total volume (or predicted, estimated, and / or calculated total volume) of the alkalinized portion of the water body.

[0036]

[0037] If the volume of the alkalinized portion of the water body is unknown (e.g., an open system), but the amount of total alkalinity added to the water body is known, the quantification of CO2 removal and any additional, other, and / or auxiliary processes may be performed using any known elements (e.g., Ca) in (or added to) the alkaline material. 2+ , Mg 2+ , Sr 2+ , Li +, Zn 2+ etc.) and / or the corresponding isotopes (e.g., Ca 45 , Mg 24 , Sr 86 , Li 7 , Zn 67 It is possible to include the use of conservative chemical tracers, including concentrations and / or ratios of any of the elements and / or isotopes (or combinations thereof) that, once dissolved, exhibit a known stoichiometric and / or empirical relationship to alkalinity within the alkaline material and / or to other relevant components of the aqueous carbonate system (e.g., total alkalinity in solution, dissolved inorganic carbon).

[0037]

[0038] In some implementations, such tracer-based approaches for quantifying chemical processes associated with CO removal by alkalinity enhancement of aqueous systems are used. This approach can in turn be used to quantify various parameters of interest, including, but not limited to, the concentration of alkalinity available for CO removal, the concentration of alkalinity consumed by supplemental acids (e.g., organic acids leached from floating biomass used to deliver alkalinity) released via additional and / or other water (e.g., marine) based interventions to remove CO, the concentration of total alkalinity released to the water body (e.g., alkalinity available for CO removal and alkalinity consumed by acids released via supplemental, additional, and / or other water-based interventions), the ratio of alkalinity available for CO removal to acid neutralization compared to total alkalinity released, the CO removal efficiency of the alkaline material, the CO removal rate due to alkalinity enhancement, the total alkalinity released via alkalinity enhancement and / or the change in any suitable parameter (e.g., any of the parameters described above) via normalization to the total water volume affected by the alkalinity enhancement, the dilution factor of the alkalinized water body, and / or the dilution rate of the alkalinized water body, etc. In some implementations, the tracer-based approach described herein may allow for quantification of relevant and / or relevant processes involved in CO removal by alkalinity enhancement, even if, for example, the total volume of water involved in the process is not known (e.g., as long as the total amount of alkaline material deployed is known).

[0038]

[0039] For example, a tracer-based approach, process, and / or method for quantifying a parameter of interest associated with CO removal via alkalinity enhancement may include obtaining samples of alkaline materials and affected water (pre- and post-deployment). The alkaline materials may contain potential tracer ions (e.g., [Ca 2+ ], [Mg 2+ ], [Sr 2+ ], [Li + ], [Zn 2+

[0013] and total alkalinity. In some implementations, one or more tracer ions can be added to the alkaline material. The water sample can then be analyzed for total alkalinity, pH, temperature, conductivity, and / or potential tracer ions, etc. The DIC of the water sample can either be measured directly or calculated from the measured TA, pH, conductivity, and / or temperature, etc. Measurement of alkalinity change in water (e.g., ocean water, seawater, brackish water, etc.) can be performed using, for example, the following: Δ[TA N ]=(TA f -TA i ) (In the formula, TA f is the measured TA after deployment, and TA i is the measured TA before deployment) The cumulative net change in total alkalinity (Δ[TA N ]") or represents the excess alkalinity released per unit of seawater available for CO2 removal after neutralization of organic acids.

[0039]

[0040] The alkalinity is derived from the dissolution of any known minerals with a fixed stoichiometric and / or empirical molar ratio of alkalinity to any tracer ions (M) (e.g., major, minor, and / or trace elements, e.g., Mg, Sr, Zn, Li, etc. (and / or their isotopes)) in (or added to) alkaline minerals that exist in some fixed stoichiometric and / or empirical relationship to alkalinity, and therefore is known as gross total alkalinity (TA) per unit of seawater. G ) is the cumulative measure of change: Δ[TA G ]=R×([M] f -[M] i ) (In the formula, [M] f is the measured tracer ion [M] after deployment, and [M] iis the measured tracer ion before deployment, and R is the stoichiometric molar ratio of alkalinity / tracer ion in the alkalinity source mineral). The tracer ion molar concentration change can be derived from multiplying the tracer ion molar concentration change by the stoichiometric and / or empirical alkalinity / tracer ion molar ratio (R) in alkaline minerals (e.g., Ca(OH)2 alkalinity sources and Ca(OH)2 alkalinity sources). 2+ Tracer ions include alkalinity (OH - ) / tracer ion (Ca 2+ ) the molar ratio R would be 2 / 1).

[0040]

[0041] As described above, ionic tracers can be, for example, any known element (e.g., Ca) in any concentration or ratio, including any combination of elements and / or isotopes in any concentration and / or ratio. 2+ , Mg 2+ , Sr 2+ , Li + , Zn 2+ etc.) and / or the corresponding isotopes (e.g., Ca 45 , Mg 24 , Sr 86 , Li 7 , Zn 67 The total change in total alkalinity ([ΔTA G ) and the net change in total alkalinity (Δ[TA N The difference between ]) is: Δ[TA A ]=Δ[TA G ]-Δ[TA N ] The cumulative loss of alkalinity per unit of seawater due to the neutralization of organic acids (Δ[TA A ]).

[0041]

[0042] Therefore, the proportion of total alkalinity (total amount) added that can be allocated to acid neutralization (pTA A ) is the following: pTA A =Δ[TA A ] / Δ[TA G ] is.

[0042]

[0043] Similarly, the proportion of total alkalinity (total) addition that can be allocated to alkalinity enhancement (e.g., ocean alkalinity enhancement (OAE)) (pTA N ) is the following: pTA N =Δ[TA N ] / Δ[TA G ] is.

[0043]

[0044] The cumulative measure of change in dissolved inorganic carbon (ΔDIC) per unit of seawater is: Δ[DIC]=DIC f -DIC i (In the formula, DIC f is the measured DIC after deployment, and DIC i is the measured DIC before deployment) It can be derived from the change in the molar concentration of DIC in seawater, as provided in

[0044]

[0045] Therefore, the cumulative measure of carbon dioxide removal (CDR) efficiency by the OAE (CDR e ) is the following: CDR e =Δ[DIC] / Δ[TA N ] It can be calculated from the change in DIC divided by the change in net TA, as provided in

[0045]

[0046] Similarly, the CO2 removal rate per unit change in net alkalinity (CDR r ) is the following: CDR r =Δ[DIC] / Δ[TA N ] / t where t is the amount of time after deployment of the alkaline material that the water sample was taken. It is computable as provided in

[0046]

[0047] Based at least in part on the relationships set forth above, and assuming that the total alkalinity (total) released into the seawater is equivalent to the total moles of alkaline minerals or readily soluble alkalinity in the brine added to the seawater at the time of deployment (ALK), the following absolute values ​​(in moles) are determined to be: Sum of total alkalinity consumed by acid neutralization = AL K ×pTA A =ALK×(Δ[TA A ] / Δ[TA G ]) Sum of total alkalinity available for CO2 removal = ALK × pTA N =ALK×(Δ[TA N ] / Δ[TA G ]) Cumulative CO2 removal by alkalinity enhancement = CDR e ×ALK×pTA N =(Δ[DIC] / Δ[TA N ])×ALK×(Δ[TA N ] / Δ[TA G ]) CO2 removal rate due to alkalinity enhancement = CDR e ×ALK×pTA N / t=(Δ[DIC] / Δ[TA N ])×ALK×((Δ[TA N ] / Δ[TA G ]) / t) As provided herein, the information may be estimated, calculated, and / or predicted.

[0047]

[0048] Assuming that water samples are obtained at approximately the same location within the plume over time, this method also allows for the determination of tracer ions (e.g., Ca(OH)2 for alkalinity) after the maximum tracer [M] has been identified. 2+ The absolute decrease in the measured concentration [M] of ) over time allows for the estimation of the dilution factor ("DF") and dilution rate ("DR"), which can be used, for example, to (at least partially) constrain and / or inform plume dispersion, dilution, and mixing models. For example, the dilution factor can be calculated as follows: DF=Δ[M] max / Δ[M] min -1 (In the formula, Δ[M] max is the maximum difference in measured tracer ion [M] before and after deployment, and Δ[M] min is the minimum difference in measured tracer ion [M] before and after deployment, and DF is Δ [M] max and Δ[M] min is the dilution factor associated with the amount of unreacted seawater mixed into the reaction plume between sampling times) It is computable as provided in

[0048]

[0049] The dilution rate (DR) is as follows: DR=DF / t=(Δ[M] max / Δ[M] min -1) / t (Where t is Δ[M] max and Δ[M] min is the time between samplings, and DR is Δ[M] max is the dilution rate related to the rate of mixing of unreacted seawater into the reacting plume as a percentage of the plume volume at the time of sampling) As provided in Δ[M] max It can be expressed as a percentage of the plume volume at the time of sampling.

[0049]

[0050] The distribution of alkaline fluid 102 into the body of water 104 can be performed via any suitable system, device, method, or combination thereof. As used herein, the terms “distributing” and “conveying” generally refer to one or more processes or methods of storing, transporting, delivering, and / or deploying alkaline fluid 102 into a body of water at a desired target location. Such systems and / or devices that perform the distribution methods are generally referred to herein as “conveyors” and / or “distributors.” For example, a non-exhaustive list of suitable conveyors / distributors can include, but is not limited to, transport vessels, flexible barges, wells, pipelines, waterways / pipes, natural channels and / or slopes, buoys, substrates, and / or systems for performing one or more freezing and / or rafting processes, etc. Provided below is a discussion of non-limiting aspects and / or features of certain distribution methods. While certain aspects and / or features are described, it should be understood that the described concepts and / or distribution methods are provided by way of example only. Other distribution methods and / or combinations thereof are contemplated.

[0050] Alkaline fluid distribution by carrier

[0051] In some implementations, the alkaline fluid 102 can be transported / distributed to a target deployment location / environment in or on a body of water 104 in the hull, holds, and / or storage compartments of a transport vessel, such as those used to transport oil and / or other liquids. The alkaline fluid 102 can also be used as ballast water for ships transporting other goods. In some implementations, the alkaline fluid 102 can be released gradually or all at once to a target surface of the body of water 104 for CO2 sequestration via alkalinity enhancement, for example, when the ballast water is no longer needed.

[0051] Alkaline fluid distribution by flexible barge.

[0052] In some implementations, the alkaline fluid 102 can be transported / dispensed to a target deployment location / environment in or on the body of water 104 on a towable, non-rigid, and / or inflatable barge constructed from fabric, plastic, and / or other flexible, inflatable material, such as a flexible barge used to more efficiently transport oil, chemicals, and potable water to oceans or other bodies of water.

[0052] Alkaline fluid distribution through wells

[0053] In some implementations, the alkaline fluid 102 can be transported / distributed to a target deployment location / environment in or on a body of water 104 (e.g., surface water, etc.) via a well bore, such as that used to extract the alkaline fluid 102 from subsurface deposits. For example, the well bore can be located within ultramafic and / or mafic oceanic crust that contains high fractions of alkalinity-producing minerals, such as olivine. In some implementations, the well bore can extend to a surface platform (similar to an oil well) to efficiently deliver the alkaline fluid 102 to nearby surface waters 104, thereby sequestering CO2 via alkalinization of such surface waters 104.

[0053] Alkaline fluid distribution by pipeline

[0054] In some implementations, the alkaline fluid 102 can be transported / distributed to a target deployment location / environment in or on a body of water 104 (e.g., surface water, etc.) via pipelines located on land and / or under the sea. In such implementations, the pipelines can be used in a manner similar to oil and / or gas pipelines, water distribution systems, and / or sewer systems.

[0054] Distribution of alkaline fluids through waterways / pipes

[0055] In some implementations, the alkaline fluid 102 can be transported / distributed to a target deployment location / environment in or on a body of water 104 (e.g., surface water) via one or more waterways, waterway systems, and / or water pipes. In such implementations, the waterways, waterway systems, and / or water pipes can be used in a manner similar to the distribution of irrigation water and / or drinking water via some known waterways and / or water pipe systems.

[0055] Alkaline fluid distribution by natural channels and / or slopes

[0056] In some implementations, the alkaline fluid 102 can be transported / distributed to a target deployment location / environment in or above a body of water 104 (e.g., surface water, etc.) via naturally occurring flow paths and / or slopes, such as rivers, rivulets, creeks, canyons, arroyos, dry channels, cave systems, hillsides, and / or other sloping topographic systems. In such implementations, the natural flow paths and / or slopes can be used to transport the alkaline fluid 102 to a larger body of water for the purpose of sequestering CO2, for example, in a manner similar to how such natural systems transport meteoric water (e.g., rain, snowmelt, etc.) and discharged groundwater to larger bodies of water.

[0056] Alkaline fluid distribution by freezing and rafting.

[0057] In some implementations, the alkaline fluid 102 can be transported / distributed to a target deployment location / environment in or on a body of water 104 (e.g., surface water) by freezing it and releasing / deploying it in solid form. For example, the frozen alkaline fluid 102 is typically less dense than seawater and therefore floats on the surface water 104, gradually releasing alkalinity into the surface water 104 as the frozen alkaline fluid melts. In some implementations, the alkaline fluid 102 can be frozen in combination with terrestrial biomass to form a "pykrete buoy" or the like configured to gradually release alkalinity and terrestrial biomass as the frozen alkaline fluid melts. Similarly, alkalinity-enhancing minerals, such as fractured limestone, magnesium hydroxide, calcium hydroxide, olivine, and / or other metal silicates, can be frozen along with the alkaline fluid 102, which in some cases can modify the melting rate of the alkaline fluid 102 and deliver additional alkalinity to the surface water 104 through their chemical weathering and / or dissolution.

[0057] Alkaline fluid distribution by buoy / substrate

[0058] In some implementations, the alkaline fluid 102 can be transported / dispensed within and / or via the buoy to a target deployment location / environment in or on a body of water 104 (e.g., surface waters, etc.). For example, such a buoy can be configured to contain, transport, and / or slowly release the alkaline fluid 102. In such implementations, the buoy can be configured to contain sufficient air to maintain positive buoyancy for at least a desired period of time. In some embodiments,

[0058]

[0059] 1 , in some implementations, process 100 can optionally include treating 103 the alkaline fluid in any suitable manner prior to dispensing to the target location. For example, in some implementations, optional treating 103 can include using alkaline fluid 102 during construction of the buoy and / or any other suitable substrate. In such implementations, the buoy / substrate can be configured to gradually deteriorate and / or dissolve in the body of water 104, thereby releasing alkalinity associated with and / or resulting from alkaline fluid 102, even as the fluid precipitates or substantially precipitates as alkaline minerals throughout the process of constructing the buoy / substrate. For example, in some implementations, the buoy can be bound to and / or constructed in part from cementitious materials (e.g., similar to many marine buoys), and alkaline fluid 102 can be used to activate cementitious reactions that bind the buoy together. The alkalinity stored in the cementitious binder will then be released as the buoy dissolves, thereby transporting / distributing the alkalinity from the natural source 101 to the target location / environment in the body of water 104. Non-limiting / non-exhaustive examples of suitable buoys and / or substrates are described, for example, in the '919 PCT previously incorporated by reference.

[0059]

[0060] In other implementations, optional treatment 103 can include the use of alkaline fluid 102 to hydrate polysaccharide binders used in the construction of the buoy / substrate, such as psyllium or rice husk, resulting in a hydrogel and / or a mineralized hydrogel. For example, the formation of a hydrogel can stabilize and / or immobilize the alkaline fluid 102 until the hydrogel binder dissolves or decomposes at the target location, thereby releasing alkalinity into the body of water 104. Non-limiting / non-exhaustive examples of suitable buoys and / or substrates are described, for example, in the '917 PCT application previously incorporated by reference.

[0060]

[0061] In some cases, alkaline fluid 102 may be contained and / or stored in natural source 101 at relatively high temperatures, which may be advantageous when used, for example, in the production of cementitious and / or polysaccharide hydrogel aggregated substrates, by reducing the heat input required for activation and / or hardening of such binders. Also, in some cases, relatively high concentrations of divalent cations and alkalinity may speed up the activation and / or hardening process of cementitious binders and / or hydrogel binders, among other mechanical and / or chemical binders, used in the production of engineered buoys and / or substrates for CO2 sequestration.

[0061]

[0062] In some implementations, the buoy and / or substrate can be configured to provide a structure for cultivating a target product, such as macroalgae. For example, the buoy and / or substrate can be similar to and / or substantially identical to any of the previously incorporated by reference '315 patent, '744 publication, '292 publication, '917 PCT, '919 PCT, and / or '959 provisional. In such implementations, the buoy and / or substrate can be configured to float and / or otherwise provide positive buoyancy for at least a predetermined period of time while the target product grows and accumulates biomass. At the predetermined period (or at one or more discrete times within the predetermined period), the buoy and / or substrate can be configured to at least partially dissolve, degrade, decompose, and / or otherwise become non-buoyant, which in turn can reduce the net buoyancy of the buoy / substrate and target product. In some implementations, after the target product has grown and accumulated a desired amount of biomass, the buoy / substrate and target product are allowed to sink to the bottom of the body of water, so that by accumulating biomass, the target product can capture CO2 through photosynthesis, and by allowing the buoy / substrate and target product to sink, the captured CO2 can be durably sequestered and / or stored.

[0062]

[0063] As described above, the amount of alkaline fluid used to form the buoy / substrate, the alkaline fluid stored and released by the buoy / substrate, and / or the alkaline fluid released or deployed in connection with the deployment of the buoy / substrate can at least partially neutralize acids or acidic materials released through auxiliary processes associated with CO2 capture via, for example, the growth and / or accumulation of target product biomass seeded on, supported by, and / or at least temporarily suspended by the buoy / substrate (e.g., the release of small amounts of organic acids into the water body as the target product grows). In some implementations, the alkaline fluid can be used to capture and / or durably retain in solution CO2 released through auxiliary processes associated with CO2 removal, for example, the settling of biomass into the water body, which may release small amounts of CO2 into the water body and / or atmosphere via, for example, microbial remineralization of particulate organic carbon and / or dissolved organic carbon. In some implementations, the alkaline fluid can replenish and / or supplement the amount of natural alkalinity that may be removed or consumed by the target product as it grows and accumulates biomass.

[0063]

[0064] 2 is a flow chart of an alkalinity enhancement method 200, according to one embodiment. Method 200 can be implemented with and / or using any of the extractors and / or conveyors described herein. Alternatively, method 200 can be implemented with any other system that does not necessarily use a conveyor and / or extractor.

[0064]

[0065] Method 200 includes extracting an alkaline fluid from a natural source at 201. In some cases, the natural source is an alkaline deposit hosting at least one of alkaline groundwater, alkaline brine, carbonate, or evaporite deposit. The extraction can be performed using any suitable method and / or extractor, such as any described herein. For example, the natural source can be alkaline water that can be extracted and / or collected using at least one surface collection method.

[0065]

[0066] In some implementations, the method 200 includes forming an aggregate substrate and activating at least a portion of the aggregate substrate via an alkaline fluid. For example, activating the aggregate substrate can result in at least one of binding or hardening of at least a portion of the aggregate substrate. In some implementations, the aggregate substrate is a buoy including a partially cementitious material. Activating such an aggregate substrate can include binding the partially cementitious material with a binder formed at least in part by the alkaline fluid.

[0066]

[0067] Method 200 includes delivering an alkaline fluid to a target deployment location in a body of water at 202. In some implementations, method 200 optionally includes determining the target deployment location based on at least one of efficiency or effectiveness of CO2 sequestration of at least a portion of the water body in response to alkalinity enhancement. In some implementations, method 200 optionally includes determining the target deployment location based on at least one of the water body, historical data associated with the water body, environmental conditions, or a deployment method.

[0067]

[0068] Conveying can be performed using any suitable method and / or conveyor / distributor, such as any described herein. For example, in some implementations, the alkaline fluid is conveyed in liquid or frozen form. In some implementations, the frozen alkaline fluid delivered to the target deployment location can be allowed to melt within a body of water for a predetermined period of time. In some implementations, the alkaline fluid can be frozen with at least one terrestrial biomass, alkalinity-enhancing minerals, or materials configured to modify the melting rate of the frozen alkaline material.

[0068]

[0069] In some implementations, the alkaline fluid can be transported and / or deployed to a target location via at least one of a transport vessel, a flexible barge, a well, a pipeline, a water pipe, a natural flow path, a buoy, and / or a substrate. In some implementations, the alkaline fluid is used to form, bind, and / or harden an aggregate substrate, which is then transported and / or deployed to a target deployment location in a body of water. After deploying the aggregate substrate, at least a portion of the aggregate substrate can be allowed to dissolve in the body of water for a predetermined period of time.

[0069]

[0070] Method 200 includes, at 203, enhancing the alkalinity of at least a portion of the body of water based at least in part on the alkaline fluid, aggregate substrates formed by the alkaline fluid, and / or (at least in part) the dissolution or degradation of such substrates. In some embodiments, method 200 optionally includes calculating the amount of CO sequestered as a result of the alkalinity enhancement.

[0070]

[0071] Any of the embodiments and / or methods described herein can overcome known challenges and / or high costs (in terms of both energy and emitted CO2) associated with crushing, pulverizing, and / or heating alkaline minerals configured to increase reaction rates for industrially scalable CO2 sequestration (e.g., such processes typically occur naturally over geological timescales in natural subsurface systems at temperatures and / or pressures that support such reactions). Additionally, the embodiments and / or methods described herein can avoid known challenges and / or hazards environmental, geological, and otherwise associated with subsurface injection of CO2 into alkaline rock systems.

[0071]

[0072] In some cases, any of the embodiments and / or methods described herein may use globally ubiquitous and / or abundant natural deposits of alkaline minerals and / or fluids to sequester or otherwise facilitate the sequestration of CO from the fast carbon cycle to the slow carbon cycle at rates and scales capable of substantially offsetting at least a portion of the anthropogenic CO released into the fast carbon cycle via the extraction and combustion of fossil fuels (among other processes).

[0072]

[0073] In some cases, any of the embodiments and / or methods described herein may use natural alkaline fluids that reduce and / or minimize costs (e.g., in terms of money, time, and / or CO2 emissions) associated with large-scale CO2 sequestration, e.g., by utilizing products of reactions that have already taken place over geological timescales in subterranean systems at temperatures and pressures that typically favor the reactions.

[0073]

[0074] In some cases, any of the embodiments and / or methods described herein may utilize naturally occurring alkaline fluids that are naturally high in pH, alkalinity, and divalent cation concentration and are therefore suitable for large-scale CO2 sequestration via alkalinity enhancement and / or mineralization.

[0074]

[0075] In some cases, any of the embodiments and / or methods described herein may use naturally occurring alkaline fluids that may be naturally hot at the extraction point, thereby reducing the heat input that would otherwise be used to activate and cure binders, e.g., cementitious binders and / or polysaccharide hydrogel binders, in aggregate-based materials used in CO2 sequestration.

[0075]

[0076] In some cases, any of the embodiments and / or methods described herein may use naturally occurring alkaline fluids with high concentrations of divalent cations and alkalinity, which in turn may speed up the activation and / or hardening process of cementitious and / or hydrogel binders used to produce aggregate substrates used in CO2 sequestration.

[0076]

[0077] In some cases, any of the embodiments and / or methods described herein may use naturally occurring alkaline fluids that increase and / or enhance alkalinity, thereby increasing the total amount of CO that can be sequestered in and / or by a body of water, thereby shifting the carbonate chemical equilibrium of an aqueous system in favor of transporting CO from the atmosphere to the body of water.

[0077]

[0078] In some cases, any of the embodiments and / or methods described herein may use natural alkaline fluids whose extraction, processing, and / or distribution results in less CO2 being emitted by known processes used and increases the alkaline fluid's ability to sequester atmospheric CO2.

[0078]

[0079] In some cases, any of the embodiments and / or methods described herein may use natural alkaline fluids, which may increase the efficiency of transporting alkalinity to a target site for CO2 sequestration, for example, by maintaining alkalinity in a fluid state, which in some cases may allow for efficient transport / distribution, such as by buoys, transport vessels, flexible barges, wells, pipelines, channels / pipes, and / or natural channels and / or slopes.

[0079]

[0080] In some cases, any of the embodiments and / or methods described herein may use natural alkaline fluids that can reduce and / or substantially minimize potential by-products that would otherwise result from the direct introduction of alkaline minerals into marine and freshwater systems by adding alkalinity to such systems via natural alkaline fluids extracted from alkaline mineral systems that are free of particulate by-products associated with such reactions.

[0080]

[0081] In some cases, any of the embodiments and / or methods described herein may allow for stabilization of the alkaline fluid within a mechanical binder of the floating substrate, for example, within cementitious carbonate minerals and / or polysaccharide hydrogels (e.g., psyllium husk, rice husk), which in some cases may allow for long-term transportation over land or sea, followed by controlled release of alkalinity once at the target location as the binder disaggregates, dissolves, and / or melts.

[0081]

[0082] In some cases, any of the embodiments and / or methods described herein can be configured to provide greater control over the rate, timing, and / or location of alkalinity introduction into a natural system for the purpose of CO2 sequestration, such that alkalinity can be introduced via a fluid that can be systematically and immediately (or substantially immediately) titrated into the system, rather than via solid alkaline minerals that are suspended in and reacted with a natural body of water over a longer time interval to provide a target alkalinity.

[0082]

[0083] While various schematic diagrams, embodiments, and / or implementations have been described above, it should be understood that they have been presented by way of example only, and not by way of limitation. Various modifications, changes, and / or variations in form and / or detail may be made without departing from the scope of the present disclosure and / or without altering their function and / or advantages, unless otherwise specified. Similarly, although embodiments and / or features, their elements, configurations, aspects, etc. may be described above in connection with certain implementations, it should be understood that such implementations are presented by way of example only, and not by way of limitation. Any embodiments and / or features, their elements, configurations, aspects, etc., can be used with and / or adapted for use in other implementations, unless otherwise specified. Functionally equivalent embodiments, implementations, and / or methods, in addition to those described herein, will be apparent to those skilled in the art from the foregoing description and are intended to be encompassed within the scope of the present disclosure.

[0083]

[0084] Although the above-described schematics, embodiments, and / or implementations suggest certain elements arranged in certain orientations, configurations, or positions, the arrangement of elements may be modified. Although various embodiments are described as having certain features, configurations, and / or combinations of elements, other embodiments are possible that have any feature, configuration, and / or combination of elements from any of the embodiments described herein, except in mutually exclusive combinations. The embodiments described herein may include various combinations and / or subcombinations of the features, elements, configurations, and / or features of the different embodiments described.

[0084]

[0085] The specific configuration of the various elements can also vary. For example, the size and specific shape of the various elements can differ from the illustrated embodiment while still providing the functionality described herein. More specifically, the size and shape of the various elements can be specifically selected for a desired or intended use. Thus, it should be understood that the size, shape, and / or arrangement of the embodiments and / or their elements can be adapted for a given use unless the context explicitly dictates otherwise.

[0085]

[0086] Although the methods described above suggest certain events occurring in a certain order, the order of certain events may be modified. Additionally, as described above, some of the events may occur in parallel, where possible, as well as sequentially. Although methods are described as having particular steps and / or combinations of steps, other methods having any combination of steps from any of the methods described herein are possible, except in mutually exclusive combinations and / or unless otherwise clearly stated in the context.

Claims

1. Extracting alkaline fluids from natural sources; delivering the alkaline fluid to a target deployment location in a body of water; and enhancing alkalinity of at least a portion of the body of water based at least in part on the alkaline fluid; A method comprising:

2. 10. The method of claim 1, wherein the transporting comprises transporting the alkaline fluid to the target deployment location via at least one of a transport vessel, a flexible barge, a well, a pipeline, a water pipe, a natural flow path, a frozen raft, or a buoy.

3. freezing the alkaline fluid; releasing the frozen alkaline fluid into the body of water at the target deployment location; and allowing said alkaline fluid to melt within said body of water for a predetermined period of time; The method of claim 1 further comprising:

4. 4. The method of claim 3, wherein freezing the alkaline fluid comprises freezing the alkaline fluid with at least one of terrestrial biomass, alkalinity-enhancing minerals, or a material configured to modify a melting rate of the frozen alkaline material.

5. forming an aggregate substrate; activating at least a portion of the aggregate substrate via the alkaline fluid, wherein the activating results in at least one of binding or hardening of at least a portion of the aggregate substrate; The method of claim 1 further comprising:

6. the delivering includes delivering the aggregate substrate to the target deployment location, the method comprising: disposing the aggregate substrate in the body of water; and allowing at least a portion of the aggregate substrate to dissolve in the body of water for a predetermined period of time; The method of claim 5 further comprising:

7. 10. The method of claim 1, wherein the natural source is an alkaline deposit hosting at least one of alkaline groundwater, alkaline brine, carbonate, or evaporite deposit.

8. 10. The method of claim 1, wherein the natural source is alkaline water and extracting the alkaline fluid from the natural source comprises a surface harvesting method.

9. CO of at least a portion of said body of water in response to increasing said alkalinity ２ The method of claim 1 , further comprising determining the target deployment location based on at least one of efficiency or effectiveness of sequestration.

10. The method of claim 1 , further comprising determining the target deployment location based on at least one of collected data associated with at least one of the bodies of water, historical data associated with the bodies of water, environmental conditions, or a deployment method.

11. Extracting alkaline fluids from natural sources; forming an aggregate substrate; activating at least a portion of the aggregate substrate via the alkaline fluid, wherein the activating results in at least one of binding or hardening of at least a portion of the aggregate substrate; deploying the aggregate substrate at a target deployment location in the body of water; and increasing the alkalinity of at least a portion of the body of water based at least in part on the aggregate substrate disposed therein; A method comprising:

12. 12. The method of claim 11 , wherein the aggregate substrate is a buoy comprising a partially cementitious material, and activating at least a portion of the aggregate substrate comprises binding the partially cementitious material with a binder formed at least in part by the alkaline fluid.

13. allowing at least a portion of the aggregate substrate to dissolve in the body of water for a predetermined period of time; enhancing the alkalinity of at least a portion of the body of water based at least in part on the aggregate substrate dissolving over a predetermined period of time; The method of claim 11 further comprising:

14. seeding the aggregate substrate with a target product prior to said deploying, wherein said predetermined time is a predetermined time for said target product to grow and accumulate biomass; 14. The method of claim 13, further comprising:

15. allowing at least a portion of the aggregate substrate and the target product to sink to the bottom of the body of water after the predetermined time; 15. The method of claim 14, further comprising:

16. 15. The method of claim 14, wherein increasing the alkalinity of at least a portion of the body of water neutralizes acidification associated with growth and biomass accumulation of the target product.

17. 1. An alkalinity enhancement system, comprising: an extractor configured to extract the alkaline fluid from the natural source; and a conveyor configured to transport at least one of the alkaline fluid or an aggregate substrate at least partially formed by the alkaline fluid to a target deployment location in a body of water, wherein the at least one of the alkaline fluid or the aggregate substrate transported to the target deployment location is operable to enhance alkalinity of at least a portion of the body of water; Including, the system.

18. The system of claim 17 , wherein the conveyor comprises a buoy.

19. 20. The system of claim 18, wherein the buoy is configured to gradually degrade in the body of water, thereby releasing alkalinity associated with the alkaline fluid.

20. 20. The system of claim 18, wherein the buoy is formed in part from a cementitious material, the binder of the cementitious material being formed at least in part from the alkaline fluid.

21. 20. The system of claim 17, wherein the extractor is configured to extract alkaline fluid via at least one of well drilling, recirculation, or surface extraction.

22. Increasing the alkalinity of at least a portion of the body of water comprises: ２ 20. The system of claim 17, wherein

23. The removed CO ２ 23. The system of claim 22, wherein the amount of is determined based at least in part on measuring the amount of tracer ions.

24. The removed CO ２ is determined without knowing the volume of at least a portion of the body of water having the enhanced alkalinity.

25. 20. The system of claim 17, wherein increasing the alkalinity of at least a portion of the body of water neutralizes acidification of at least a portion of the body of water.

26. 20. The system of claim 17, wherein increasing the alkalinity of at least a portion of the body of water neutralizes acidification of at least a portion of the body of water.

27. Increasing the alkalinity of at least a portion of the body of water comprises: ２ 27. The system of claim 26, wherein the system neutralizes acidification associated with an ancillary process associated with removal.

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