A method for quantitatively calculating the transformation process of albite in acidic environment based on the total dissolution model

Abstract

The present invention relates to the field of petroleum exploration technology, and specifically to a method for quantitatively calculating the transformation process of albite in an acidic environment based on a total dissolution model. The method comprises: determining the type of water-rock reaction during the transformation process of albite particles in an acidic fluid environment under the total dissolution-reprecipitation model; calculating the Gibbs energy of water-soluble phase particles formed during the transformation process of albite; calculating the Gibbs energy of pure substances and solvents in the reaction; determining the Gibbs energy change and equilibrium constant of the water-rock reaction; determining the concentration of various types of particles in aqueous solutions under different conditions during the equilibrium period of various types of water-rock reactions; determining the order in which different water-rock reactions reach equilibrium; and calculating the transformation process of albite particles under different temperature, pressure, and pH environments, as well as the conversion amount of various diagenetic products in the process. The method of the present invention has important theoretical significance and practical application value for predicting the type, occurrence, and distribution of secondary pores in deep acidic fluid environments in oil and gas basins.

Description

Technical Field

[0001] The present invention relates to the technical field of petroleum exploration, and in particular to a method for quantitatively calculating a sodium feldspar transformation process in an acidic environment based on a total dissolution model. Background Art

[0002] Feldspar is one of the most important rock-forming minerals in the Earth's crust. The dissolution and transformation of feldspar particles in acidic aqueous solutions is widespread near the surface and deep in sedimentary basins. The dissolution and transformation of feldspar particles near the surface influence processes such as clay formation and groundwater evolution. The dissolution and transformation of feldspar particles during sandstone burial permeate the formation and evolution of clastic reservoirs. Reservoir transformation during CO2 reinjection and oil and gas reservoir development also clearly involves the transformation of feldspar particles in acidic-neutral aqueous environments. Over the past century, numerous researchers have conducted extensive experiments on feldspar particles in static and dynamic laboratory tests under different temperatures, pressures, and pH values. They have also conducted extensive research on the surface characteristics of feldspar particles in soil and the transformation products of feldspar in sandstone reservoirs in sedimentary basins.

[0003] Currently, there are few studies on the quantitative calculation of the transformation process of albite particles. The lack of such research makes it difficult to accurately determine the content and occurrence of secondary pores formed by the transformation of feldspar particles in sandstone reservoirs during burial, which in turn affects the prediction of deep sandstone reservoirs in oil and gas basins.

[0004] There is currently no report on a method for quantitatively calculating the transformation process of albite in acidic environments based on the total dissolution model. Summary of the Invention

[0005] The main purpose of the present invention is to provide a method for quantitatively calculating the transformation process of sodium feldspar in an acidic environment based on a total dissolution model. The method of the present invention is based on the total dissolution-reprecipitation model and uses thermodynamic methods to achieve quantitative calculation of the content of various diagenetic products in the transformation process of sodium feldspar particles under different conditions.

[0006] To achieve the above object, the present invention adopts the following technical solutions:

[0007] The present invention provides a method for quantitatively calculating the transformation process of albite in an acidic environment based on a total dissolution model, which comprises the following steps:

[0008] Determine the water-rock reaction type during the transformation of albite particles in an acidic fluid environment under the complete dissolution-reprecipitation model;

[0009] Calculate the Gibbs energy of water-soluble particles formed during the conversion of albite; calculate the Gibbs energy of pure substances and solvents in the gas, solid, and liquid phases of the reaction;

[0010] Determine the Gibbs energy change and equilibrium constant of water-rock reactions;

[0011] Using equilibrium constants, determine the concentrations of various particles in aqueous solutions at different temperature, pressure, and pH conditions during the equilibrium period of various water-rock reactions.

[0012] According to the conditions of aqueous solution at different water-rock reaction equilibrium periods, the order in which different water-rock reactions reach equilibrium is determined;

[0013] Based on the order in which water-rock reactions reach equilibrium, the transformation process of albite particles and the transformation amounts of various diagenetic products in this process are calculated under different temperature, pressure and pH environments.

[0014] Furthermore, under the complete dissolution-reprecipitation model, the types of water-rock reactions during the transformation of albite particles in an acidic fluid environment include:

[0015] Reaction 1: NaAlSi3O8(s)+H + (aq)+7H2O(l)→Na + (aq)+Al(OH)3(aq)+3H4SiO4(aq);

[0016] Reaction 2: Al(OH)3(aq)+H + (aq)→Al(OH)2 + (aq)+H2O(l);

[0017] Reaction 3: Al(OH)3(aq)+2H + (aq)→Al(OH)2 + (aq)+2H2O(l);

[0018] Reaction 4: Al(OH)3(aq)+3H + (aq)→Al 3+ (aq)+3H2O(l);

[0019] Reaction 5: Al(OH)3(aq)+H2O(l)→Al(OH)4 - (aq)+H + (aq);

[0020] Reaction 6: H4SiO4(aq)→H3SiO4 - (aq)+H + (aq);

[0021] Reaction 7: H3SiO4 - (aq)→H2SiO4 2- (aq)+H + (aq);

[0022] Reaction 8: Na +(aq)+H3SiO4 - (aq)→NaH3SiO4(aq);

[0023] Reaction 9: Al(OH)3(aq)→Al(OH)3(s);

[0024] Reaction 10: Al(OH)3(aq)→AlO(OH)(s)+H2O(l);

[0025] Reaction 11: H4SiO4(aq)→SiO2(s)+2H2O(l);

[0026] Reaction 12: 2Al(OH)3(aq)+2H4SiO4(aq)→Al2[Si2O5](OH)4(s)(kaolinite)+5H2O(l)

[0027] Reaction 13: Na + (aq)+3Al(OH)3(aq)+3H4SiO4(aq)→Na[AlSi3O 10 ]Al2(OH)2(s)+H + (aq)+9H2O(l);

[0028] Reaction 14:

[0029] NaAlSi3O8(s)+AlO(OH)(s)+3H2O(l)+H + (aq)→Al2[Si2O5](OH)4(s)+H4SiO4(aq)+Na + (aq);

[0030] Reaction 15:

[0031] NaAlSi3O8(s)+Al(OH)3(s)+H + (aq)+2H2O(l)→Al2[Si2O5](OH)4(s)+H4SiO4(aq)+Na + (aq).

[0032] Furthermore, before new precipitates appear in the aqueous solution, the ratio of the sum of the concentrations of aluminum particles in the water-soluble phase, the sum of the concentrations of sodium particles in the water-soluble phase, and the sum of the concentrations of silicon particles in the water-soluble phase is 1:1:3; the concentration ratios between different particles are calculated based on the reaction equilibrium constant, and the composition and concentration of various particles in the aqueous solution in the early stage of dissolution of albite particles and the stage without precipitate formation are calculated.

[0033] Furthermore, under the total dissolution-reprecipitation model, the order in which different water-rock reactions reach equilibrium includes: the priority of precipitation of boehmite and gibbsite, the priority of precipitation of boehmite or gibbsite and authigenic quartz, and the priority of precipitation of boehmite or gibbsite or euhedral quartz and kaolinite.

[0034] Furthermore, regarding the priority of boehmite and gibbsite precipitation:

[0035] When the temperature is lower than 283.15K, the content of aluminum particles in the aqueous solution is controlled by the solubility of gibbsite, and Al(OH)3(aq) in the aqueous solution precipitates in the form of gibbsite, and no boehmite exists in the precipitate; when the temperature is higher than 283.15K, the content of aluminum particles in the aqueous solution is controlled by the solubility of boehmite, and Al(OH)3(aq) in the aqueous solution precipitates in the form of boehmite, and no gibbsite exists in the precipitate.

[0036] Furthermore, the priority of boehmite or gibbsite versus authigenic quartz precipitation is:

[0037] When the pH of the aqueous solution is 1, and the water temperature is higher than 513.15K, boehmite precipitation precedes euhedral quartz precipitation; when the temperature is lower than 513.15K, quartz crystals precipitate before boehmite or gibbsite;

[0038] When the pH value of the aqueous solution is 2, when the temperature is higher than 413.15K, the euhedral quartz has not yet reached the precipitation concentration when the boehmite reaches the precipitation concentration; when the temperature is lower than 413.15K, the quartz crystals precipitate first;

[0039] When the pH value of the aqueous solution is 3, when the temperature is higher than 353.15K, the euhedral quartz has not yet reached the precipitation concentration when the boehmite reaches the precipitation concentration; when the temperature is lower than 353.15K, the quartz crystals precipitate first;

[0040] When the pH value of the aqueous solution is 4, when the temperature is higher than 303.15K, the euhedral quartz has not reached the precipitation temperature when the boehmite reaches the precipitation concentration; when the temperature is lower than 303.15K, the quartz crystals precipitate first;

[0041] When the pH value of the aqueous solution is 5 or 6, the temperature range of 273.15K-623.15K shows the preferential precipitation of gibbsite or boehmite;

[0042] When the pH value of the aqueous solution is 7 and the temperature is higher than 583.15K, boehmite has not reached the precipitation concentration when crystalline quartz reaches the precipitation concentration; when the temperature is lower than 583.15K, boehmite or gibbsite precipitates first.

[0043] Furthermore, by comparing the concentration product of Al(OH)3(aq)*H4SiO4(aq) in the aqueous solution during the precipitation of boehmite, gibbsite, or quartz, and comparing it with the concentration product of such substances required during the precipitation of kaolinite, the precipitation priority of boehmite, gibbsite, or euhedral quartz over kaolinite can be determined:

[0044] When pH=5 and the temperature is less than 298.15K, kaolinite precipitates first, while in other periods, authigenic quartz, boehmite or gibbsite precipitates first.

[0045] Furthermore, the transformation of albite particles includes the following six modes:

[0046] A: Sodium feldspar dissolution → Sodium feldspar dissolution, quartz precipitation → Sodium feldspar dissolution, quartz precipitation, authigenic kaolinite precipitation → Sodium feldspar dissolution, sodium mica precipitation, quartz precipitation → reaction stops;

[0047] B: Sodium feldspar dissolution → Sodium feldspar dissolution, quartz precipitation → Sodium feldspar dissolution, quartz precipitation, boehmite precipitation, kaolinization of boehmite → Sodium feldspar dissolution, sodium mica precipitation, quartz precipitation → reaction stops;

[0048] C: Sodium feldspar dissolution → Sodium feldspar dissolution, boehmite precipitation, boehmite kaolinization → Feldspar dissolution, quartz precipitation, boehmite precipitation, boehmite kaolinization → Feldspar dissolution, sodium mica precipitation, quartz precipitation → reaction stops;

[0049] D: Feldspar dissolution → Feldspar dissolution, kaolinite precipitation → Feldspar dissolution, kaolinite precipitation, quartz precipitation → Feldspar dissolution, sodium mica, quartz precipitation → reaction stops;

[0050] E: Feldspar dissolution → Feldspar dissolution, boehmite precipitation, kaolinitization of boehmite → Feldspar dissolution, kaolinite precipitation → Feldspar dissolution, kaolinite precipitation, quartz precipitation → Feldspar dissolution, sodium mica precipitation, quartz precipitation → reaction stops;

[0051] F: Feldspar dissolution → Feldspar dissolution, gibbsite precipitation, kaolinitization of gibbsite → Feldspar dissolution, kaolinite precipitation → Feldspar dissolution, kaolinite precipitation, quartz precipitation → Feldspar dissolution, sodium mica precipitation, quartz precipitation → reaction stops.

[0052] Compared with the prior art, the present invention has the following advantages:

[0053] Based on a complete dissolution-reprecipitation model and using thermodynamic methods, this study calculates the transformation process of albite particles and the content of various diagenetic products during this process under different temperature, pressure, and pH conditions. This method has important theoretical significance and practical application value for predicting the type, occurrence, and distribution of secondary pores in deep acidic fluid environments in oil and gas basins. BRIEF DESCRIPTION OF THE DRAWINGS

[0054] The accompanying drawings, which constitute a part of the present invention, are used to provide a further understanding of the present invention. The exemplary embodiments of the present invention and their descriptions are used to explain the present invention and do not constitute improper limitations on the present invention.

[0055] Figure 1 is the molar Gibbs energy of formation of the relevant pure substance described in Example 1;

[0056] Figure 2 is the molar Gibbs energy of formation of the relevant water-soluble phase described in Example 1;

[0057] Figure 3 is the equilibrium constant of the relevant water-rock reaction described in Example 1;

[0058] Figure 4 The precipitation priority of boehmite and gibbsite as described in Example 1;

[0059] Figure 5 The priority of boehmite or gibbsite and quartz precipitation described in Example 1;

[0060] Figure 6 The priority of precipitation of boehmite or gibbsite or quartz and authigenic kaolinite as described in Example 1;

[0061] Figure 7 The priority of the authigenic kaolinite precipitation and the sodium mica precipitation described in Example 1;

[0062] Figure 8 This is the transformation path of albite particles under different conditions described in Example 1. DETAILED DESCRIPTION

[0063] It should be noted that the following detailed descriptions are exemplary and intended to provide further explanation of the present invention. Unless otherwise specified, all technical and scientific terms used herein have the same meaning as commonly understood by those skilled in the art to which the present invention belongs.

[0064] It should be noted that the terms used herein are only for describing specific embodiments and are not intended to limit the exemplary embodiments according to the present invention. As used herein, unless the context clearly indicates otherwise, the singular form is intended to include the plural form. In addition, it should be understood that when the terms "comprise" and / or "include" are used in this specification, they indicate the presence of features, steps, operations and / or combinations thereof.

[0065] In order to enable those skilled in the art to more clearly understand the technical solution of the present invention, the technical solution of the present invention will be described in detail below with reference to specific embodiments.

[0066] Example 1

[0067] The method for quantitatively calculating the transformation process of sodium feldspar in an acidic environment based on a total dissolution model comprises the following steps:

[0068] Step 1: Determine all water-rock reaction types during the transformation of albite particles in an acidic fluid environment under the complete dissolution-reprecipitation model, as shown in Table 1.

[0069] Table 1

[0070]

[0071]

[0072] Step 2: Calculate the molar Gibbs energy of formation of the solid substance and the solvent (H2O(l)) using the constant-pressure specific heat model (Formula 1).

[0073]

[0074] Among them: G P,T is the Gibbs energy of molar formation of various substances under the conditions of P (pressure) and T (temperature); H P,T is the molar formation enthalpy of the substance under the conditions of P (pressure) and T (temperature); S P,T is the molar entropy of formation of a substance under the conditions of P (pressure) and T (temperature); r 0.1Mpa; T r is 298.15K; Cp is the constant pressure specific heat capacity of different substances, which can be expressed as Cp = a + b * T + c / T 2 The various parameters of related substances in the calculation process are based on Table 1.

[0075] The molar Gibbs energy of formation of water-soluble phase particles formed during the transformation of albite was calculated using the HKF model (Equation 2).

[0076]

[0077] Where j represents the jth solute component in the aqueous solution. P and T are the pressure (bar) and temperature (K) of interest; Pr and Tr are the reference pressure (1 bar) and reference temperature (298.15K). r =2600(bar);T r = 228 (K). a1-a4, c1-c2 are the fitting parameters of the characteristic ions in the solution. ε is the dielectric constant of pure water. Y is the derivative of the dielectric constant of pure water with respect to temperature (K). is the Born coefficient of particles in aqueous solution, which is itself a function of ionic charge, effective radius, temperature, pressure and the pure water property g.

[0078] Step 3: Calculate the Gibbs energy change and equilibrium constant of each reaction according to the Gibbs equation ( Figure 2 ,3).

[0079] Step 4: Calculate the concentration and concentration product of various particles in the aqueous solution when different reactions reach equilibrium based on the equilibrium constant of the reaction.

[0080] Step 5: Before new precipitates appear in the aqueous solution, the concentration of aluminum particles in the aqueous phase and (Al 3+ (aq), Al(OH) 2+ (aq), Al(OH)2 + (aq), Al(OH)3(aq), Al(OH)4 - (aq)), the concentration of sodium particles in the aqueous phase and (Na + (aq), NaH3SiO4(aq)), concentration of silicon particles in the water-soluble phase and (NaH3SiO4(aq), H4SiO4(aq), H3SiO4 - (aq), H2SiO4 2- (aq)) ratio is 1; 1:3; at the same time, the concentration ratio between different particles can be calculated based on the reaction equilibrium constant, for example: m(Al(OH)2 + (aq)) / (m(Al(OH)3(aq))*m(H + ))=K2. Among them, m(Al(OH)2 + (aq)) represents Al(OH)2 in aqueous solution + (aq) is the molar concentration of the particle (mol / L); K2 represents the equilibrium constant of reaction 2. Based on this principle, the composition and concentration of various particles in the aqueous solution during the early stage of albite dissolution, when no precipitate is formed, can be calculated.

[0081] Step 6: Based on the concentrations of other particles under these conditions calculated in Step 5, compare the priority of this reaction with other reactions at the time of reaching equilibrium, i.e., the priority of each new mineral precipitation. Compare each reaction one by one to determine the priority of different precipitates.

[0082] The priority of boehmite and gibbsite precipitation: Temperature controls the priority of boehmite and gibbsite precipitation: When the temperature is lower than 283.15K, the content of aluminum particles in the aqueous solution is controlled by the solubility of gibbsite, and Al(OH)3(aq) in the aqueous solution is precipitated in the form of gibbsite, and no boehmite exists in the precipitate; When the temperature is higher than 283.15K, the content of aluminum particles in the aqueous solution is controlled by the solubility of boehmite, and Al(OH)3(aq) in the aqueous solution is precipitated in the form of boehmite, and no gibbsite exists in the precipitate. Figure 4 ).

[0083] The priority of boehmite or gibbsite and authigenic quartz precipitation: when the pH of the aqueous solution is 1 and the water temperature is higher than 513.15K, boehmite precipitation precedes euhedral quartz precipitation; when the temperature is lower than 513.15K, quartz crystals are superior to boehmite or gibbsite precipitation ( Figure 5 -a). When the pH value of the aqueous solution is 2, when the temperature is higher than 413.15K, the euhedral quartz does not reach the precipitation concentration when the boehmite reaches the precipitation concentration; when the temperature is lower than 413.15K, the quartz crystals precipitate first ( Figure 5 -b). When the pH value of the aqueous solution is 3, when the temperature is higher than 353.15K, the euhedral quartz does not reach the precipitation concentration when the boehmite reaches the precipitation concentration; when the temperature is lower than 353.15K, the quartz crystals precipitate first ( Figure 5 -c). When the pH value of the aqueous solution is 4, when the temperature is higher than 303.15K, the euhedral quartz has not reached the precipitation temperature when the boehmite reaches the precipitation concentration; when the temperature is lower than 303.15K, the quartz crystals precipitate first ( Figure 5 -d). When the pH value of the aqueous solution is 5 or 6, the temperature range of 273.15K-623.15K shows the preferential precipitation of gibbsite or boehmite ( Figure 5 -e,f). When the pH value of the aqueous solution is 7, when the temperature is higher than 583.15K, the precipitation concentration of quartz crystals is reached before that of boehmite; when the temperature is lower than 583.15K, boehmite or gibbsite is precipitated first ( Figure 5 -g).

[0084] By comparing the concentration product of Al(OH)3(aq)*H4SiO4(aq) in the aqueous solution during the precipitation period of boehmite, gibbsite or quartz, and comparing it with the concentration product of such substances required during the precipitation period of kaolinite, the precipitation priority of boehmite, gibbsite or euhedral quartz and kaolinite was determined: except when pH = 4, the temperature was between 298.15-318.15K; when pH = 5, the temperature was less than 298.15K, kaolinite was precipitated first, while in other periods, authigenic quartz, boehmite or gibbsite was precipitated first. Figure 6 ).

[0085] At the same time, calculate the Na required in the solution for the simultaneous precipitation of kaolinite and sodium mica + (aq) concentration: As pH and temperature increase, sodium mica preferentially produces the required Na + (aq) concentration decreases, but even so the minimum Na required + The concentration of (aq) also obviously exceeded 1.0*10 7 mol / L. This type of formation fluid environment does not exist in the continental fault basins in eastern China, represented by the Dongying Depression and the Bonan Depression. In other words, the priority of kaolinite precipitation in acidic environments is higher than that of sodium mica ( Figure 7 ).

[0086] Step 7: The sodium feldspar dissolution process includes:

[0087] A: Sodium feldspar dissolution → Sodium feldspar dissolution, quartz precipitation → Sodium feldspar dissolution, quartz precipitation, authigenic kaolinite precipitation → Sodium feldspar dissolution, sodium mica precipitation, quartz precipitation → reaction stops ( Figure 8 -a);

[0088] B: Sodium feldspar dissolution → Sodium feldspar dissolution, quartz precipitation → Sodium feldspar dissolution, quartz precipitation, boehmite precipitation, kaolinization of boehmite → Sodium feldspar dissolution, sodium mica precipitation, quartz precipitation → reaction stops ( Figure 8 -b);

[0089] C: Sodium feldspar dissolution → Sodium feldspar dissolution, boehmite precipitation, boehmite kaolinization → Feldspar dissolution, quartz precipitation, boehmite precipitation, boehmite kaolinization → Feldspar dissolution, sodium mica precipitation, quartz precipitation → reaction stops ( Figure 8 -c);

[0090] D: Feldspar dissolution → Feldspar dissolution, kaolinite precipitation → Feldspar dissolution, kaolinite precipitation, quartz precipitation → Feldspar dissolution, sodium mica, quartz precipitation → reaction stops ( Figure 8 -d);

[0091] E: Feldspar dissolution → Feldspar dissolution, boehmite precipitation, kaolinization of boehmite → Feldspar dissolution, kaolinite precipitation → Feldspar dissolution, kaolinite precipitation, quartz precipitation → Feldspar dissolution, sodium mica precipitation, quartz precipitation → reaction stops ( Figure 8 -e);

[0092] F: Feldspar dissolution → Feldspar dissolution, gibbsite precipitation, kaolinitization of gibbsite → Feldspar dissolution, kaolinite precipitation → Feldspar dissolution, kaolinite precipitation, quartz precipitation → Feldspar dissolution, sodium mica precipitation, quartz precipitation → reaction stops ( Figure 8 -f), a total of six modes.

[0093] The precipitation paths of albite under different temperature, pressure and pH conditions are shown in Table 2.

[0094] Table 2

[0095]

[0096] The above embodiments are preferred implementation modes of the present invention, but the implementation modes of the present invention are not limited to the above embodiments. Any other changes, modifications, substitutions, combinations, and simplifications that do not deviate from the spirit and principles of the present invention should be considered as equivalent replacement methods and are included in the scope of protection of the present invention.

Claims

1. A method for quantitatively calculating the transformation process of sodium feldspar in an acidic environment based on a total dissolution model, characterized in that: The following steps are involved: Determine the water-rock reaction type during the transformation of albite particles in an acidic fluid environment under the complete dissolution-reprecipitation model; Calculate the Gibbs energy of water-soluble particles formed during the conversion of albite; calculate the Gibbs energy of pure substances and solvents in the gas, solid, and liquid phases of the reaction; Determine the Gibbs energy change and equilibrium constant of water-rock reactions; Using equilibrium constants, determine the concentrations of various particles in aqueous solutions at different temperature, pressure, and pH conditions during the equilibrium period of various water-rock reactions. According to the conditions of aqueous solution at different water-rock reaction equilibrium periods, the order in which different water-rock reactions reach equilibrium is determined; Based on the order in which water-rock reactions reach equilibrium, the transformation process of albite particles and the transformation amounts of various diagenetic products in this process are calculated under different temperature, pressure and pH environments.

2. The method according to claim 1, characterized in that Under the complete dissolution-reprecipitation model, the types of water-rock reactions during the transformation of albite particles in an acidic fluid environment include: Reaction 1: NaAlSi3O8(s) + H + (aq) + 7H2O(l) → Na + (aq) + Al(OH)3(aq) + 3H4SiO4(aq); Reaction 2: Al(OH)3(aq) + H + (aq) → Al(OH)2 + (aq) + H2O(l); Reaction 3: Al(OH)3(aq) + 2H + (aq) → Al(OH)2 + (aq) + 2H2O(l); Reaction 4: Al(OH)3(aq)+3H + (aq)→Al 3+ (aq)+3H2O(l); Reaction 5: Al(OH)3(aq) + H2O(l) → Al(OH)4 - (aq) + H + (aq); Reaction 6: H4SiO4(aq)→H3SiO4 - (aq)+H + (aq); Reaction 7: H3SiO4 - (aq) → H2SiO4 2- (aq) + H + (aq); Reaction 8: Na + (aq) + H3SiO4 - (aq) → NaH3SiO4(aq); Reaction 9: Al(OH)3(aq)→Al(OH)3(s); Reaction 10: Al(OH)3(aq)→AlO(OH)(s)+H2O(l); Reaction 11: H4SiO4(aq)→SiO2(s)+2H2O(l); Reaction 12: 2Al(OH)3(aq)+2H4SiO4(aq)→Al2[Si2O5](OH)4(s)(kaolinite)+5H2O(l) Reaction 13: Na + (aq) + 3Al(OH)3(aq) + 3H4SiO4(aq) → Na[AlSi3O 10 Al2(OH)2(s) + H + (aq) + 9H2O(l); Reaction 14: NaAlSi3O8(s)+AlO(OH)(s)+3H2O(l)+H + (aq)→Al2[Si2O5](OH)4(s)+H4SiO4(aq)+Na + (aq) Reaction 15: NaAlSi3O8(s)+Al(OH)3(s)+H + (aq)+2H2O(l)→Al2[Si2O5](OH)4(s)+H4SiO4(aq)+Na + (aq)。 3. The method according to claim 1, characterized in that Before new precipitates appear in the aqueous solution, the ratio of the sum of the concentrations of aluminum particles in the water-soluble phase, the sum of the concentrations of sodium particles in the water-soluble phase, and the sum of the concentrations of silicon particles in the water-soluble phase is 1:1:

3. The concentration ratios between different particles are calculated based on the reaction equilibrium constant, and the composition and concentration of various particles in the aqueous solution in the early stage of albite particle dissolution, when no precipitates are formed, are calculated.

4. The method according to claim 1 or 2, characterized in that Under the total dissolution-reprecipitation model, the order in which different water-rock reactions reach equilibrium includes: the priority of precipitation of boehmite and gibbsite, the priority of precipitation of boehmite or gibbsite and authigenic quartz, and the priority of precipitation of boehmite or gibbsite or euhedral quartz and kaolinite.

5. The method according to claim 4, characterized in that Priority for boehmite and gibbsite precipitation: When the temperature is lower than 283.15K, the content of aluminum particles in the aqueous solution is controlled by the solubility of gibbsite, and Al(OH)3(aq) in the aqueous solution precipitates in the form of gibbsite, and no boehmite exists in the precipitate; when the temperature is higher than 283.15K, the content of aluminum particles in the aqueous solution is controlled by the solubility of boehmite, and Al(OH)3(aq) in the aqueous solution precipitates in the form of boehmite, and no gibbsite exists in the precipitate.

6. The method according to claim 4, characterized in that Priority for precipitation of boehmite or gibbsite versus authigenic quartz: When the pH of the aqueous solution is 1, and the water temperature is higher than 513.15K, boehmite precipitation precedes euhedral quartz precipitation; when the temperature is lower than 513.15K, quartz crystals precipitate before boehmite or gibbsite; When the pH value of the aqueous solution is 2, when the temperature is higher than 413.15K, the euhedral quartz has not yet reached the precipitation concentration when the boehmite reaches the precipitation concentration; when the temperature is lower than 413.15K, the quartz crystals precipitate first; When the pH value of the aqueous solution is 3, when the temperature is higher than 353.15K, the euhedral quartz has not yet reached the precipitation concentration when the boehmite reaches the precipitation concentration; when the temperature is lower than 353.15K, the quartz crystals precipitate first; When the pH value of the aqueous solution is 4, when the temperature is higher than 303.15K, the euhedral quartz has not reached the precipitation temperature when the boehmite reaches the precipitation concentration; when the temperature is lower than 303.15K, the quartz crystals precipitate first; When the pH value of the aqueous solution is 5 or 6, the temperature range of 273.15K-623.15K shows the preferential precipitation of gibbsite or boehmite; When the pH value of the aqueous solution is 7 and the temperature is higher than 583.15K, boehmite has not reached the precipitation concentration when crystalline quartz reaches the precipitation concentration; when the temperature is lower than 583.15K, boehmite or gibbsite precipitates first.

7. The method according to claim 4, characterized in that By comparing the concentration product of Al(OH)3(aq)*H4SiO4(aq) in the aqueous solution during the precipitation of boehmite, gibbsite or quartz, and comparing it with the concentration product of such substances required during the precipitation of kaolinite, the precipitation priority of boehmite, gibbsite or euhedral quartz and kaolinite can be determined: When pH=5 and the temperature is less than 298.15K, kaolinite precipitates first, while in other periods, authigenic quartz, boehmite or gibbsite precipitates first.

8. The method according to claim 1, characterized in that The transformation of albite particles includes the following six modes: A: Sodium feldspar dissolution → Sodium feldspar dissolution, quartz precipitation → Sodium feldspar dissolution, quartz precipitation, authigenic kaolinite precipitation → Sodium feldspar dissolution, sodium mica precipitation, quartz precipitation → reaction stops; B: Sodium feldspar dissolution → Sodium feldspar dissolution, quartz precipitation → Sodium feldspar dissolution, quartz precipitation, boehmite precipitation, kaolinization of boehmite → Sodium feldspar dissolution, sodium mica precipitation, quartz precipitation → reaction stops; C: Sodium feldspar dissolution → Sodium feldspar dissolution, boehmite precipitation, boehmite kaolinization → Feldspar dissolution, quartz precipitation, boehmite precipitation, boehmite kaolinization → Feldspar dissolution, sodium mica precipitation, quartz precipitation → reaction stops; D: Feldspar dissolution → Feldspar dissolution, kaolinite precipitation → Feldspar dissolution, kaolinite precipitation, quartz precipitation → Feldspar dissolution, sodium mica, quartz precipitation → reaction stops; E: Feldspar dissolution → Feldspar dissolution, boehmite precipitation, kaolinitization of boehmite → Feldspar dissolution, kaolinite precipitation → Feldspar dissolution, kaolinite precipitation, quartz precipitation → Feldspar dissolution, sodium mica precipitation, quartz precipitation → reaction stops; F: Feldspar dissolution → Feldspar dissolution, gibbsite precipitation, kaolinitization of gibbsite → Feldspar dissolution, kaolinite precipitation → Feldspar dissolution, kaolinite precipitation, quartz precipitation → Feldspar dissolution, sodium mica precipitation, quartz precipitation → reaction stops.

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