CA1220612A - Process for the preparation of crystalline sheet-type alkali metal silicates - Google Patents
Process for the preparation of crystalline sheet-type alkali metal silicatesInfo
- Publication number
- CA1220612A CA1220612A CA000471395A CA471395A CA1220612A CA 1220612 A CA1220612 A CA 1220612A CA 000471395 A CA000471395 A CA 000471395A CA 471395 A CA471395 A CA 471395A CA 1220612 A CA1220612 A CA 1220612A
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- Prior art keywords
- alkali metal
- sio2
- reaction
- product
- sheet
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- C—CHEMISTRY; METALLURGY
- C01—INORGANIC CHEMISTRY
- C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C
- C01B33/00—Silicon; Compounds thereof
- C01B33/113—Silicon oxides; Hydrates thereof
- C01B33/12—Silica; Hydrates thereof, e.g. lepidoic silicic acid
-
- C—CHEMISTRY; METALLURGY
- C01—INORGANIC CHEMISTRY
- C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C
- C01B33/00—Silicon; Compounds thereof
- C01B33/20—Silicates
- C01B33/36—Silicates having base-exchange properties but not having molecular sieve properties
- C01B33/38—Layered base-exchange silicates, e.g. clays, micas or alkali metal silicates of kenyaite or magadiite type
Abstract
Abstract of the Disclosure:
A process for the preparation of a crystalline sheet-type alkali metal silicate in an aqueous medium is described, in which an acidic compound is added to an amorphous alkali metal silicate, or an alkali metal sili-cate dissolved in water, having a molar ratio M2O/SiO2 (M = alkali metal) of 0.24 to 2.0, in an amount such that a molar ratio M2O (unneutralized)/SiO2 of 0.05 to 0.239 is obtained. If required, the molar ratio SiO2/
H2O is adjusted from 1:5 to 1:100 by dilution, and the reaction mixture is kept at a reaction temperature of 70 to 250°C until the sheet-type alkali metal silicate has crystallized out.
A process for the preparation of a crystalline sheet-type alkali metal silicate in an aqueous medium is described, in which an acidic compound is added to an amorphous alkali metal silicate, or an alkali metal sili-cate dissolved in water, having a molar ratio M2O/SiO2 (M = alkali metal) of 0.24 to 2.0, in an amount such that a molar ratio M2O (unneutralized)/SiO2 of 0.05 to 0.239 is obtained. If required, the molar ratio SiO2/
H2O is adjusted from 1:5 to 1:100 by dilution, and the reaction mixture is kept at a reaction temperature of 70 to 250°C until the sheet-type alkali metal silicate has crystallized out.
Description
2 ~ 2 The invention relates to a process for the prepa-ration of ~rystalline alkali metal silicates, haYing a sheet structure in an aqueous medium.
In ~dd;tion ~o uater-soluble alkali metal sili S cates (hav;ng a Low siO2/a~kali metal oxide ratio) and sparingly soluble 3morphous alkal; metal s;licates, crys-talline alkali metal silicates are also known. Among these~ it is possible to differentiate between silicates having a frame~ork structure (for exampLe zeolites which are free of aluminun or at Least have a lo~ aluminum content) and 5i licates having a sheet structure. The term sheet structure is sometimes called layer structure.
Some crystalline alkali metal silicates having a sheet structure are found to oc~ur naturally, while others have been synthesized. The alkaLi metal silicates having a sheet structure, in particular the sodium salts and the potassium salts, are usually synthesized from a silica gel, silica sol or precipitated silicic acid ~ith the addition of an alkali metal hydroxide, in an a~ueous sys-2n tem~ In sorne cases, an appropriate carbonate solution isalso used instead of an alkali metal hydroxide solution~
The amount of alkali to be added depends on the product desired.
The present invention relates to a process for the preparation of a crystalline sheet-type alkali metal sili-cate in an aqueous medium, ~herein an a~idic compound is added to an alkali metal silicate dissolved ;n ~ater, or an amorphous alkali metal s;licate, having 3 !~olar ratio M2û/SiO2, where M represents an alkali metal~ of D.Z4 to 2~0, in an amount such that a molar ratio M20 (unneu-tralized)lSiO2 of 0.05 to 0.239 is obtained, the molar ratio Si~H~g is, if required9 adjusted to 1-5 to 1:100 by dilution, and the re3ction ~ix~re is kept at a reaction te~perature of 70 to 250c until the sheet-type alkali metal silicate has crystalli~ed out. M preferably represents sodium or potassium. A preferred ratio of Na20 (not neutra1ized)/SiO2 is from 1:5 to 1:7,5.
Soda waterglass having an SiO2 content of about 22 to 37%, an Na20 conten~ of 5 to 1~X and an Al203 content of Less than 0.5% is a preferred, very reactive start;ng compound which, being a large-scale industrial product, is readily available and economical. This is an S alkali metal siLicate dissolved in ~ater~ A soda water-glass containing 22-3Q% by weight of ~iO2 and 5-9X by weight of NazO is particularly preferred. However~ amor-phous alkali metal silicates, in particular solid sodium silica+es and potassium silicates, ~hicll may also be anhy-1û drous but which are soluble in water, at least at the reac~tion temperature, can also be used.
The acidic compound added can be an anhydride or an acidic salt, such as sodium hydrogen sulfate. However, free organic or inorganic acids are preFerably used. In-organ;c acids, such as phosphoric acid or sulFuric acid,are particularly preferred.
The amount of acidic compound to be added depends on the starting silicate and on the end product desired.
~he end product formed v;rtually always has a lower M20/
SiO2 ratio than the reaction mixture from which it is formed. In the end products, the atomic ratio alkali me-tal/silicon is between about 1:4 and 1:11. The pH of the product mixture after the addition of the acidic com-pound is in general higher than 9. Preferably, a pH
of bet~een 10 and 12 is established. The addition of the acidic compound results in buffering of the reaction system.
Using the process according to the invention, it is possible to obtain pure products or mixtures of cystal-line sheet-type alkali metal silicates~ Zeolites, as im-purities, form only when relatively large amounts of alumi-num are present in the react;on mixture. Amorphous silica is found only when the reaction times are very short, while quartz is observed only for very long reaction times.
The sheet-type alkal; metal silicates obtained possess an ion exchange capacity. Their X-ray defraction patterns are similar to those of known sheet-type alkali metal silicates.
In addition to the alkal; metal ions, it is also 6~
-- 4 ~
possible for other metal ions to be present during the synthes;s~ for example german;um, aluminum~ indium, arsenic and antimony, as weLl as the non metals boron and phospho-rus. If the amount of these components is less than 10%, relative to the alkali metal content9 the synthesis is not s;gnif;cantly affected. To prepare a pure sheet-type alkali metal silicate, or ~he free acid~ it is advan-tageous if the addition of foreign metals during the syn-thesis is dispensed ~ith. Pure sheet silicates containing a cation other than an alkali metal can readily be ob-tained in a further step, from the alkali metal salt by ion exchange, or from the corresponding free acid by neutralization.
As mentioned above, relatively large amounts of aluminum in the starting mixture can lead to the formation of zeolite by-products, generally of the ZSM-5 type or of the mordenite type. On the other hand, a low aluminum content, as is present in, for example, technical-grade waterglass, does not present problems.
The process according to the invention can also be carried out in the presence of small amounts of organic compounds; however, the procedure is preferably carried out without any organic compounds, especially without any non-acidic organic compounds. According to German Offenlegungsschrift 3,048,819, the mineral magadiite, Na2Si14029.X H20, is formed in the synthesis of ZSM-5 in the presence of ethylenediamine.
European Patent Application ~2,225 states that, in the preparation of a zeolite of the ZSM-5 type in the presence of alcohols, the product is contaminated by a compound 3û which resembles the mineral kenyaite Na2Si22~4s.X H20.
However~ in this kno~n process, the sheet silicate formed is obtained only in a small amount and as an undesired by-product.
For the process according to the invention, the molar rat;o of Hzo/sio2 in the starting products is preferably from 8:1 to 40:1~ For the preparation of sheet silicates having a low alkali metal content (atomic ra~;o of M/Si from 1:7 to 1:11), it is often advantageous if the dilution with water is greater than in the case of the L' ~a ~ 3 preparation of the sheet silicates having a high alkali metal content ~atomic ratio of M/Si about 1:4 to 1:7)~
The reaction temperature is preferably 130-230C, ;n par-ticular 160-Z10C. Relatively long reaction times, high reaction temperatures and low ratios of alkali tunneu-tralized)/SiO2 promote the formation of sheet silicateshaving a low alkali metal content. Short reaction t;mes, low reaction temperatures and high alkali metal/Si ratios promote the formation of sheet silicates having a high alkali metal content.
The reaction time depends to a ~reat extent on the reaction temperature. It can be less than 1 hour, ;t can also be several months. The optimum reaction time for the reaction temperature chosen can be determined by taking samples at various times during the reaction and examining these samples by an X-ray defraction method.
The reaction is preferably carried out in a pres-sure vessel, with thorough stirring. The addition of seed crystals is very advantageous since the purity of the pro-duct is improved and the reaction time shortened. How-ever, the procedure can also be carried out ~ithout seed crystals.
In a batchwise reaction procedure, the amount of seed crystals can be up to 30X by weight, based on the proportion of SiO2 in the added alkali metal silicate, i.e. the amorphous alkali metal silicate, or alkali metal s;licate dissolved in water, which has been added. The addition of less than 0.01X by ~eight of seed crystals has no detectable effect. Instead of adding seed crystals, it may also be sufficient if the small residues from a previous batch remain in the reaction ves-sel. In the continuous reaction procedure~ substantially higher concentrations of crystal nuclei (in steatly-state equilibrium~ have also proven advantageous.
The process according to the invention can be car-ried out batchwise, semi-continuously or continuously in apparatuses having flow-tube, stirred-kettle or cascade characteristics.
Below, the semi~continuous and fully continuous preparation of crystall;ne sheet-type alkali metal 6~
~ ., silicate in a stirred kettle, or in a cascade of s~irred kettles, is to be described in more detail. The continu-ous embodiment of the process according to the invention is generally carried out at temperatures above 100~.
~ecause of the pressure generated above the aqueous reac tion mixture, an autoclave is required in this caseO Fur-ther increasing the pressure by adding an inert gas has no advantages. The temperature of the reaction mixture should be in the range from 70 to 250C, in particular 10from 130 to 230C, even during the addition of the reac-tants. This can be effected particuLarly easily if the substances added have already been heated up. The pres-sure in the reaction vessel should be less than 1~0 bar, in general in the range from 1 to 25 bar.
15If the pressure in the stirred kettle is above 1 bar, a pump is required for metering in the reactants.
A single pump may be sufficient for this purpose; however, ;t is also possible to add the individual components sepa-rately, so that 2 or even 3 pumps are required at various Z0 ~eed points of the autoclave. It is preferable if the ac;d;c compound ~for example sulfuric acid or phosphoric acid) and the basic reactants (water-soluble alkali metal s;licates) are metered in separately, in order to avoid gel formation outside the reaction vessel. If the acidic compound ;s metered in excess, it may also be neces-sary to add an alkali.
~ he starting materials can be added in succession;
however, s;multaneous addition is preferred. If a plu-rality of reaction kettles connected in series are em-ployed, it is advantageous if the time during ~hich eachcomponent is added is 10 to 1~0X, in particular 20 to 80%, of the res;dence time ;n the f;rst stirred kettle.
If product is not removed simultaneously during the addition, the content of the stirred vessel increases.
The addition must then be terminated no later than ~hen the maximum level is reached. When the components are added very rapidly, stirring must be continued in the re-action vessel in order to achieve adequate fornation of the crystalline silicate by subsequent crystallization.
.
The product ;s then removed from the st;ll hot autoclave.
However, it may be advantageous to carry out this subse-quent crystallization in a further vessel, or in further vessels, wh;ch, ;f required, are l;kew;se prov;ded ~ith st;rrers, so that a cascade (of stirred kettles) results.
The durat;on of subsequent crystall;zat;on should be no higher than 99 times, preferably no higher than 2~ times, and in particular (at high temperatures above 200C) only 9 times, preferably less than 4 times, the avera~e resi-dence time in the f;rst stirred kettle. It is poss;bleto carry out the subsequent crystallization at tempera-tures which are substantially lo~er than that in the first stirred kettle.
In th~ continuous reaction procedure, it is advan-tageous if the autoclave is not emptied sompletely but al-ways kept at least partially filled with product m;xture, hhich consists of the crystallized silicate, the mother liquor and unconverted starting materials. Thus, a high proportion of silicate crystals remain in the autoclave and promote the further formation of crystalline silicate.
In the continuous reaction procedure, seed crystals are added only during the start-up period (to establish the equilibrium). During the reaction, the weight ratio of alkali metal silicate crystals to dissolved SiOz in the reaction mixture should be higher than 0.05, prefer-ably higher than 0.1, and in particular higher than û~2.
In the completely cont;nuous reaction procedure, constant values are mainta;ned, these being in general higher than 1~û. In the semi-continuous reaction procedure, the value periodically exceeds and falls below a mean value.
In the completely continuous reaction procedure, and ~ith ideal mixing, it is possible for substantially more crystalline than dissolved silicate to be present in the stirred kettle as well as in the product discharged.
If the product is to be removed from an autoclave which is still under pressure~ this can be ach;eved by means of an appropriate outlet valve ;n the base. If com-plete emptying is not desired, the product is advantageously removed via a siphon tube which dips into the reaction ~2~
m;xture and is closed by means of a valve. The length o~
the siphon tube determines the maximum amount of product which can be removed.
Advantageously, the process according to the in-vent;on ;s carr;ed out completely cont;nuously. In addi-tion to the continuous feed of the starting components, cont;nuous d;scharge of the reaction products is necessary in this procedure. This can be effected~ for example, by means of a siphon tube. In order to monitor ~he reaction vessel, it may be necessary to control the level by means of a level indicator or by determining the weight of the apparatus.
For economic reasons, both in batchwise operation and in the continuous procedure, the reaction time is generally such that at least 10~, in general, however, more than 70X, of ~he alkali metal silicate added is con-verted to the sheet-type alkali metal silicate. At higher reaction temperatures, short reaction times are required.
At temperatures above 180C, times of less than 1 hour are occasionally sufficient~ However, reaction times of several days may also be necessary~ The required reaction t;mes, which depend on the particular reaction conditions, can be determined from X-ray diffraction patterns of indi-vidual samples. Using the process accordin3 to the in-vention, it is possible to prepare silicates ~hich exclu-sively exhibit the X-ray reflections typ;cal of crystalline sheet silicates.
The ratio of crystalline silicate (formed) to dis-solved silicate tadded) is determined mainly by the mean residence time and composition (in particular the molar ratio M20/SiO2). Increasing the mean residence time increases the crystalline fraction but occasionally also promotes the formation of by-products. For economic rea-sons, it may be useful to employ shorter residence times and accept a smaller proportion of crystalline product.
In order to isolate the sheet silicate, the reac-tion mixture is filtered after the reaction~ and the pro-duct ;s washed w;th water or d;lute aLkal; (depending on the alkal; metal s;licate) and, if required, dried.
However, it may also be advantageous for some forms of further processing if the filter-moist product is directly processed further, for example if the alkali metal ions are exchanged for other cations by ~reatment with salt solutions.
The alkali metal silicates prepared by the process according to the invention, and the free sheet silicic acids obtainable from ~hese, can be usecl as adsorbents, analogously to the silicates of German Patent 2~74~,912.
It is surprising that~ in the reaction of alkali metal silicate solutions, in particular waterglass solu-tions, with acidic comp~unds, such as, for example, sul-furic acid, crystalline silicates having a sheet structure can be obtained, instead of amorphous siLica. ComparPd with the known processes for the preparation of sheet-type alkali metal silicates, the process according to the in-vention has the advantage of a comparatively shorter reac-tion time, which is attributable to the high reactivity of the water-soluble or amorphous alkali metal silicates employed.
Example 1 A reaction mixture having the molar composition 0.303 Na20 : 0.0052 Al203 : SiOz : 3a H20 is first prepared by adding 83.5 parts by weight of soda ~aterglass (27X of SiO2, 8.43X of Na20 and 0.24X of Al2U3) to 149 parts of ~ater. Some of a filter-moist crystalline sodium silicate from a previous experiment (71X ~eight loss as a result of heating to 1200C; onLy the amount of water was taken into account ;n calculating the molar composition) is then added. 4.93 parts of 96% strength sulfuric acid are then added slowly~ while stirring. The reaction mixture then has the following molar co~position:
0.174 NazO : 0.0052 Alz03 : SiO2 : 0.129 NazS04 :
30 HzO.
The reaction mixture is heated to 205C in the course of 1.5 hours in a stainless autoclave, kept at this temperature for 2.5 hours and then slowly cooled~ After it has been cooled, the reaction mixture ;s filtered, washed with ~ater and sucked dry in a suction filter~ The filter~moist product has a loss on ignition of 55X. The product is dried in the air for a short time and then examined thermogravimetrically. The weight loss which occurs up to a temperature of about 140C is 43X. Up to about 10û0C9 no further significant decrease in weight is observed. The product dried to constant weight at 120C, Na-SKS-1~ has the following composition, determined by elemental analysis: 3.8% of Na, 0.24% of Alo 41.5% of Si and 0.003X of Fe. This gives a molar SiO2/Na20 ratio of 17.9. The molar SiOz/Al~03 ratio of 332 shows that, in spite of the presence of dissolved Al203 in the reaction m;xture, only very small amounts of AL203 are incorporated in the end product. The X-ray defraction pattern of the sodium silicate dried in the air (Na-SKS-1) is shown in Table 1.
Table 1 d (10 8 cm) _I/Io 20.5 56 10.0 11 207n31 4 4.99 13
In ~dd;tion ~o uater-soluble alkali metal sili S cates (hav;ng a Low siO2/a~kali metal oxide ratio) and sparingly soluble 3morphous alkal; metal s;licates, crys-talline alkali metal silicates are also known. Among these~ it is possible to differentiate between silicates having a frame~ork structure (for exampLe zeolites which are free of aluminun or at Least have a lo~ aluminum content) and 5i licates having a sheet structure. The term sheet structure is sometimes called layer structure.
Some crystalline alkali metal silicates having a sheet structure are found to oc~ur naturally, while others have been synthesized. The alkaLi metal silicates having a sheet structure, in particular the sodium salts and the potassium salts, are usually synthesized from a silica gel, silica sol or precipitated silicic acid ~ith the addition of an alkali metal hydroxide, in an a~ueous sys-2n tem~ In sorne cases, an appropriate carbonate solution isalso used instead of an alkali metal hydroxide solution~
The amount of alkali to be added depends on the product desired.
The present invention relates to a process for the preparation of a crystalline sheet-type alkali metal sili-cate in an aqueous medium, ~herein an a~idic compound is added to an alkali metal silicate dissolved ;n ~ater, or an amorphous alkali metal s;licate, having 3 !~olar ratio M2û/SiO2, where M represents an alkali metal~ of D.Z4 to 2~0, in an amount such that a molar ratio M20 (unneu-tralized)lSiO2 of 0.05 to 0.239 is obtained, the molar ratio Si~H~g is, if required9 adjusted to 1-5 to 1:100 by dilution, and the re3ction ~ix~re is kept at a reaction te~perature of 70 to 250c until the sheet-type alkali metal silicate has crystalli~ed out. M preferably represents sodium or potassium. A preferred ratio of Na20 (not neutra1ized)/SiO2 is from 1:5 to 1:7,5.
Soda waterglass having an SiO2 content of about 22 to 37%, an Na20 conten~ of 5 to 1~X and an Al203 content of Less than 0.5% is a preferred, very reactive start;ng compound which, being a large-scale industrial product, is readily available and economical. This is an S alkali metal siLicate dissolved in ~ater~ A soda water-glass containing 22-3Q% by weight of ~iO2 and 5-9X by weight of NazO is particularly preferred. However~ amor-phous alkali metal silicates, in particular solid sodium silica+es and potassium silicates, ~hicll may also be anhy-1û drous but which are soluble in water, at least at the reac~tion temperature, can also be used.
The acidic compound added can be an anhydride or an acidic salt, such as sodium hydrogen sulfate. However, free organic or inorganic acids are preFerably used. In-organ;c acids, such as phosphoric acid or sulFuric acid,are particularly preferred.
The amount of acidic compound to be added depends on the starting silicate and on the end product desired.
~he end product formed v;rtually always has a lower M20/
SiO2 ratio than the reaction mixture from which it is formed. In the end products, the atomic ratio alkali me-tal/silicon is between about 1:4 and 1:11. The pH of the product mixture after the addition of the acidic com-pound is in general higher than 9. Preferably, a pH
of bet~een 10 and 12 is established. The addition of the acidic compound results in buffering of the reaction system.
Using the process according to the invention, it is possible to obtain pure products or mixtures of cystal-line sheet-type alkali metal silicates~ Zeolites, as im-purities, form only when relatively large amounts of alumi-num are present in the react;on mixture. Amorphous silica is found only when the reaction times are very short, while quartz is observed only for very long reaction times.
The sheet-type alkal; metal silicates obtained possess an ion exchange capacity. Their X-ray defraction patterns are similar to those of known sheet-type alkali metal silicates.
In addition to the alkal; metal ions, it is also 6~
-- 4 ~
possible for other metal ions to be present during the synthes;s~ for example german;um, aluminum~ indium, arsenic and antimony, as weLl as the non metals boron and phospho-rus. If the amount of these components is less than 10%, relative to the alkali metal content9 the synthesis is not s;gnif;cantly affected. To prepare a pure sheet-type alkali metal silicate, or ~he free acid~ it is advan-tageous if the addition of foreign metals during the syn-thesis is dispensed ~ith. Pure sheet silicates containing a cation other than an alkali metal can readily be ob-tained in a further step, from the alkali metal salt by ion exchange, or from the corresponding free acid by neutralization.
As mentioned above, relatively large amounts of aluminum in the starting mixture can lead to the formation of zeolite by-products, generally of the ZSM-5 type or of the mordenite type. On the other hand, a low aluminum content, as is present in, for example, technical-grade waterglass, does not present problems.
The process according to the invention can also be carried out in the presence of small amounts of organic compounds; however, the procedure is preferably carried out without any organic compounds, especially without any non-acidic organic compounds. According to German Offenlegungsschrift 3,048,819, the mineral magadiite, Na2Si14029.X H20, is formed in the synthesis of ZSM-5 in the presence of ethylenediamine.
European Patent Application ~2,225 states that, in the preparation of a zeolite of the ZSM-5 type in the presence of alcohols, the product is contaminated by a compound 3û which resembles the mineral kenyaite Na2Si22~4s.X H20.
However~ in this kno~n process, the sheet silicate formed is obtained only in a small amount and as an undesired by-product.
For the process according to the invention, the molar rat;o of Hzo/sio2 in the starting products is preferably from 8:1 to 40:1~ For the preparation of sheet silicates having a low alkali metal content (atomic ra~;o of M/Si from 1:7 to 1:11), it is often advantageous if the dilution with water is greater than in the case of the L' ~a ~ 3 preparation of the sheet silicates having a high alkali metal content ~atomic ratio of M/Si about 1:4 to 1:7)~
The reaction temperature is preferably 130-230C, ;n par-ticular 160-Z10C. Relatively long reaction times, high reaction temperatures and low ratios of alkali tunneu-tralized)/SiO2 promote the formation of sheet silicateshaving a low alkali metal content. Short reaction t;mes, low reaction temperatures and high alkali metal/Si ratios promote the formation of sheet silicates having a high alkali metal content.
The reaction time depends to a ~reat extent on the reaction temperature. It can be less than 1 hour, ;t can also be several months. The optimum reaction time for the reaction temperature chosen can be determined by taking samples at various times during the reaction and examining these samples by an X-ray defraction method.
The reaction is preferably carried out in a pres-sure vessel, with thorough stirring. The addition of seed crystals is very advantageous since the purity of the pro-duct is improved and the reaction time shortened. How-ever, the procedure can also be carried out ~ithout seed crystals.
In a batchwise reaction procedure, the amount of seed crystals can be up to 30X by weight, based on the proportion of SiO2 in the added alkali metal silicate, i.e. the amorphous alkali metal silicate, or alkali metal s;licate dissolved in water, which has been added. The addition of less than 0.01X by ~eight of seed crystals has no detectable effect. Instead of adding seed crystals, it may also be sufficient if the small residues from a previous batch remain in the reaction ves-sel. In the continuous reaction procedure~ substantially higher concentrations of crystal nuclei (in steatly-state equilibrium~ have also proven advantageous.
The process according to the invention can be car-ried out batchwise, semi-continuously or continuously in apparatuses having flow-tube, stirred-kettle or cascade characteristics.
Below, the semi~continuous and fully continuous preparation of crystall;ne sheet-type alkali metal 6~
~ ., silicate in a stirred kettle, or in a cascade of s~irred kettles, is to be described in more detail. The continu-ous embodiment of the process according to the invention is generally carried out at temperatures above 100~.
~ecause of the pressure generated above the aqueous reac tion mixture, an autoclave is required in this caseO Fur-ther increasing the pressure by adding an inert gas has no advantages. The temperature of the reaction mixture should be in the range from 70 to 250C, in particular 10from 130 to 230C, even during the addition of the reac-tants. This can be effected particuLarly easily if the substances added have already been heated up. The pres-sure in the reaction vessel should be less than 1~0 bar, in general in the range from 1 to 25 bar.
15If the pressure in the stirred kettle is above 1 bar, a pump is required for metering in the reactants.
A single pump may be sufficient for this purpose; however, ;t is also possible to add the individual components sepa-rately, so that 2 or even 3 pumps are required at various Z0 ~eed points of the autoclave. It is preferable if the ac;d;c compound ~for example sulfuric acid or phosphoric acid) and the basic reactants (water-soluble alkali metal s;licates) are metered in separately, in order to avoid gel formation outside the reaction vessel. If the acidic compound ;s metered in excess, it may also be neces-sary to add an alkali.
~ he starting materials can be added in succession;
however, s;multaneous addition is preferred. If a plu-rality of reaction kettles connected in series are em-ployed, it is advantageous if the time during ~hich eachcomponent is added is 10 to 1~0X, in particular 20 to 80%, of the res;dence time ;n the f;rst stirred kettle.
If product is not removed simultaneously during the addition, the content of the stirred vessel increases.
The addition must then be terminated no later than ~hen the maximum level is reached. When the components are added very rapidly, stirring must be continued in the re-action vessel in order to achieve adequate fornation of the crystalline silicate by subsequent crystallization.
.
The product ;s then removed from the st;ll hot autoclave.
However, it may be advantageous to carry out this subse-quent crystallization in a further vessel, or in further vessels, wh;ch, ;f required, are l;kew;se prov;ded ~ith st;rrers, so that a cascade (of stirred kettles) results.
The durat;on of subsequent crystall;zat;on should be no higher than 99 times, preferably no higher than 2~ times, and in particular (at high temperatures above 200C) only 9 times, preferably less than 4 times, the avera~e resi-dence time in the f;rst stirred kettle. It is poss;bleto carry out the subsequent crystallization at tempera-tures which are substantially lo~er than that in the first stirred kettle.
In th~ continuous reaction procedure, it is advan-tageous if the autoclave is not emptied sompletely but al-ways kept at least partially filled with product m;xture, hhich consists of the crystallized silicate, the mother liquor and unconverted starting materials. Thus, a high proportion of silicate crystals remain in the autoclave and promote the further formation of crystalline silicate.
In the continuous reaction procedure, seed crystals are added only during the start-up period (to establish the equilibrium). During the reaction, the weight ratio of alkali metal silicate crystals to dissolved SiOz in the reaction mixture should be higher than 0.05, prefer-ably higher than 0.1, and in particular higher than û~2.
In the completely cont;nuous reaction procedure, constant values are mainta;ned, these being in general higher than 1~û. In the semi-continuous reaction procedure, the value periodically exceeds and falls below a mean value.
In the completely continuous reaction procedure, and ~ith ideal mixing, it is possible for substantially more crystalline than dissolved silicate to be present in the stirred kettle as well as in the product discharged.
If the product is to be removed from an autoclave which is still under pressure~ this can be ach;eved by means of an appropriate outlet valve ;n the base. If com-plete emptying is not desired, the product is advantageously removed via a siphon tube which dips into the reaction ~2~
m;xture and is closed by means of a valve. The length o~
the siphon tube determines the maximum amount of product which can be removed.
Advantageously, the process according to the in-vent;on ;s carr;ed out completely cont;nuously. In addi-tion to the continuous feed of the starting components, cont;nuous d;scharge of the reaction products is necessary in this procedure. This can be effected~ for example, by means of a siphon tube. In order to monitor ~he reaction vessel, it may be necessary to control the level by means of a level indicator or by determining the weight of the apparatus.
For economic reasons, both in batchwise operation and in the continuous procedure, the reaction time is generally such that at least 10~, in general, however, more than 70X, of ~he alkali metal silicate added is con-verted to the sheet-type alkali metal silicate. At higher reaction temperatures, short reaction times are required.
At temperatures above 180C, times of less than 1 hour are occasionally sufficient~ However, reaction times of several days may also be necessary~ The required reaction t;mes, which depend on the particular reaction conditions, can be determined from X-ray diffraction patterns of indi-vidual samples. Using the process accordin3 to the in-vention, it is possible to prepare silicates ~hich exclu-sively exhibit the X-ray reflections typ;cal of crystalline sheet silicates.
The ratio of crystalline silicate (formed) to dis-solved silicate tadded) is determined mainly by the mean residence time and composition (in particular the molar ratio M20/SiO2). Increasing the mean residence time increases the crystalline fraction but occasionally also promotes the formation of by-products. For economic rea-sons, it may be useful to employ shorter residence times and accept a smaller proportion of crystalline product.
In order to isolate the sheet silicate, the reac-tion mixture is filtered after the reaction~ and the pro-duct ;s washed w;th water or d;lute aLkal; (depending on the alkal; metal s;licate) and, if required, dried.
However, it may also be advantageous for some forms of further processing if the filter-moist product is directly processed further, for example if the alkali metal ions are exchanged for other cations by ~reatment with salt solutions.
The alkali metal silicates prepared by the process according to the invention, and the free sheet silicic acids obtainable from ~hese, can be usecl as adsorbents, analogously to the silicates of German Patent 2~74~,912.
It is surprising that~ in the reaction of alkali metal silicate solutions, in particular waterglass solu-tions, with acidic comp~unds, such as, for example, sul-furic acid, crystalline silicates having a sheet structure can be obtained, instead of amorphous siLica. ComparPd with the known processes for the preparation of sheet-type alkali metal silicates, the process according to the in-vention has the advantage of a comparatively shorter reac-tion time, which is attributable to the high reactivity of the water-soluble or amorphous alkali metal silicates employed.
Example 1 A reaction mixture having the molar composition 0.303 Na20 : 0.0052 Al203 : SiOz : 3a H20 is first prepared by adding 83.5 parts by weight of soda ~aterglass (27X of SiO2, 8.43X of Na20 and 0.24X of Al2U3) to 149 parts of ~ater. Some of a filter-moist crystalline sodium silicate from a previous experiment (71X ~eight loss as a result of heating to 1200C; onLy the amount of water was taken into account ;n calculating the molar composition) is then added. 4.93 parts of 96% strength sulfuric acid are then added slowly~ while stirring. The reaction mixture then has the following molar co~position:
0.174 NazO : 0.0052 Alz03 : SiO2 : 0.129 NazS04 :
30 HzO.
The reaction mixture is heated to 205C in the course of 1.5 hours in a stainless autoclave, kept at this temperature for 2.5 hours and then slowly cooled~ After it has been cooled, the reaction mixture ;s filtered, washed with ~ater and sucked dry in a suction filter~ The filter~moist product has a loss on ignition of 55X. The product is dried in the air for a short time and then examined thermogravimetrically. The weight loss which occurs up to a temperature of about 140C is 43X. Up to about 10û0C9 no further significant decrease in weight is observed. The product dried to constant weight at 120C, Na-SKS-1~ has the following composition, determined by elemental analysis: 3.8% of Na, 0.24% of Alo 41.5% of Si and 0.003X of Fe. This gives a molar SiO2/Na20 ratio of 17.9. The molar SiOz/Al~03 ratio of 332 shows that, in spite of the presence of dissolved Al203 in the reaction m;xture, only very small amounts of AL203 are incorporated in the end product. The X-ray defraction pattern of the sodium silicate dried in the air (Na-SKS-1) is shown in Table 1.
Table 1 d (10 8 cm) _I/Io 20.5 56 10.0 11 207n31 4 4.99 13
3.64 22 3.52 31 3.44 100 253.34 46 3.21 53 2.94 16 Example 2 The crystalline Na silicate from Example 1 is ex-tracted twice with 5X strength hydrochloric acid at 80Cfor 15 m;nutes. The X-ray diffraction pat~ern of the filter-moist product is shown in Table 3. Investigation by dif ferential thermal analysis indicates a pronounced endother-mic transformation at about 120C and a far less pronounced endothermic transformation at about 1180C.
~z~
Table 2 d (10 8 cm~ I/Io 16.1 19 7~89 5 5.21 12 3.85 15 3 n 53 ( S ) 2 7 3 ~39 1 QO
3.22 (S) 17 10S = Shoulder An excess of sodium hydroxide solution is added to the product from Example 2. The X-ray defraction pat-tern of the produ~t dried at 120C ;s shown in Table 4 15Table 3 d (11) 8 cm) I~Io 19.8 62 9 .87 1 3 7~31 5 206.37 3
~z~
Table 2 d (10 8 cm~ I/Io 16.1 19 7~89 5 5.21 12 3.85 15 3 n 53 ( S ) 2 7 3 ~39 1 QO
3.22 (S) 17 10S = Shoulder An excess of sodium hydroxide solution is added to the product from Example 2. The X-ray defraction pat-tern of the produ~t dried at 120C ;s shown in Table 4 15Table 3 d (11) 8 cm) I~Io 19.8 62 9 .87 1 3 7~31 5 206.37 3
4.98 11 4.69 10 4.27 9 3.66 19 253.50 31 3.44 100 3.35 4~
3.33 44 3~21 47 302.94 8 Example 4 10 9 of the product from Example 1, which is dried ;n the a;r for a short t;me beforehand and has a loss on ;gnition of 44.2X, are added to 190 9 of wa~er~ and ti-trated ~ith 0~5 M H2S04. After each addition, suff;cient time is allowed for the pH to become constant to the second decimal place. The duration of the t;tration is consequently several hours. Table 4 sho~s the titration values. In the graph, an equivalence value of 150 mmol .
of Na+/100 9 of ignited product is determined from the point of inflection of the curve at pH 4.5. An ion ex-change capacity of about 95 mmol of Na+/mol of SiO2, corresponding to an SiO2:Na20 ratio, or an SiQ2/2H~
ratio, of 21:1, ;s determined. TabLe 5 shows the X-ray defraction pattern after the titration and dryin~ in the air.
Table 4 ml oF 0O5 M pH mmol of (exchanged~ Na+ ions/
H2so4 100 9 of ignited product 0.0010.22 o.o 1.009.25 17.9 2.008.32 35.8 3.007.52 53.8 4.007.09 71.7
3.33 44 3~21 47 302.94 8 Example 4 10 9 of the product from Example 1, which is dried ;n the a;r for a short t;me beforehand and has a loss on ;gnition of 44.2X, are added to 190 9 of wa~er~ and ti-trated ~ith 0~5 M H2S04. After each addition, suff;cient time is allowed for the pH to become constant to the second decimal place. The duration of the t;tration is consequently several hours. Table 4 sho~s the titration values. In the graph, an equivalence value of 150 mmol .
of Na+/100 9 of ignited product is determined from the point of inflection of the curve at pH 4.5. An ion ex-change capacity of about 95 mmol of Na+/mol of SiO2, corresponding to an SiO2:Na20 ratio, or an SiQ2/2H~
ratio, of 21:1, ;s determined. TabLe 5 shows the X-ray defraction pattern after the titration and dryin~ in the air.
Table 4 ml oF 0O5 M pH mmol of (exchanged~ Na+ ions/
H2so4 100 9 of ignited product 0.0010.22 o.o 1.009.25 17.9 2.008.32 35.8 3.007.52 53.8 4.007.09 71.7
5.006.85 89.6 5.506.73 98.6
6.006.66 107.5 6.506.49 116.5
7.006.36 125.5 7.S06.06 134.4
8.005.44 143.4 8.254.92 147.9 ~.503.58 152.4 8.753.18 156.8
9.002.9Z 161.3 9.252.79 165u8 9O502.65 170.3 9.752~59 174.8
10.002.52 179.2 10.25 2.44 183.7 10~502.39 188.2 10.752.34 192.7 1 1 rOOZ ~30 1 97~Z
11.50 2.22 206.1
12.002.16 215.1 Table 5 X-ray diffraction pattern of H-SKS-1 (Examp le 4)
13 -d (10-8 cm) I/Io 18.0 33 8.93 Q
7.40 7 ~42 7 3.86 15 3.69 20 3.57 25 3.41 100 3.21 20 Example 5 The titration of ExampLe 4 is repeated, except that, instead of the water, 190 9 of 5% strength NaCL
soLution are used. TabLe 6 shows the titration vaLues.
In the graph, an equivaLence value of 145 mmoL/100 9 of ignited product is determined from the point of infLection of the curve at pH 3.75. From this, an ion exchange capa-city of 91 mmoL of Na+/mol of SiO2, corresponding to an SiOz:Na20 ratio, or an SiO2/ZH~ ratio, of 22:1, is determined.
Table 6 ml of 0.5 M pHmmol of (exchanged) Na+ ;ons/
H2S04 100 9 of ignited product 0.00 8.87 0.0 0.5 8.01 8~9 1.0 7.49 17.8 1.5 7.00 26.6 2.0 6.63 35.5 2~5 6.16 44,4 3.0 6.14 53.3 3~5 5.83 62.1 4.0 5.66 71~0 4.5 5.47 7~.~
5.0 5.36 88.8 5.5 5.29 97.7 6.0 5.22106.5 6.5 5.18115.4 7.0 5.08124.3 7.5 4.84133.2
7.40 7 ~42 7 3.86 15 3.69 20 3.57 25 3.41 100 3.21 20 Example 5 The titration of ExampLe 4 is repeated, except that, instead of the water, 190 9 of 5% strength NaCL
soLution are used. TabLe 6 shows the titration vaLues.
In the graph, an equivaLence value of 145 mmoL/100 9 of ignited product is determined from the point of infLection of the curve at pH 3.75. From this, an ion exchange capa-city of 91 mmoL of Na+/mol of SiO2, corresponding to an SiOz:Na20 ratio, or an SiO2/ZH~ ratio, of 22:1, is determined.
Table 6 ml of 0.5 M pHmmol of (exchanged) Na+ ;ons/
H2S04 100 9 of ignited product 0.00 8.87 0.0 0.5 8.01 8~9 1.0 7.49 17.8 1.5 7.00 26.6 2.0 6.63 35.5 2~5 6.16 44,4 3.0 6.14 53.3 3~5 5.83 62.1 4.0 5.66 71~0 4.5 5.47 7~.~
5.0 5.36 88.8 5.5 5.29 97.7 6.0 5.22106.5 6.5 5.18115.4 7.0 5.08124.3 7.5 4.84133.2
- 14 -Table 6 tcont;nued?
ml of 0~5 M pH mmsl of (exchanged) Na+ ions/
H2S04 100 9 of ignited product 8.0 4.20 142.0 8.5 2.96 150.9 9.0 2053 159.8 9.5 2.30 168.7 Example 6 Hydrochloric acid is added gradually to the sodium salt from Example 1 at room temperature in an amount such that a pH of 2.0 is obtained. The reaction mixture is stirred for about 15 minutes and filtered, and dilute hydrochloric acid is once again added to the residue from filtration until the pH reaches 2Ø The crystalline silicic acid formed is filtered off, washed twice with water thoroughly, filtered once again and sucked dry. The loss on ignition of ~he filter-moist product is 34.9X.
190 9 of a 5X strength NaCl solution are added to 100 g of the moist silicic acid, and the mixture is then titra-ted ~ith 1 M NaOH. Table 7 shows the titration values~
In the graph, an equivalence value of 155 meq/100 9 of ig-nited product is determined from the point of inflect;on of the curve at pH 9.5. From this, an ion exchange capa=
city of about 94 mmol of H~/mol of SiO2, corresponding to an SiO2:Na20 ratio of 21:1, is determined.
Table 7 ml of 1 M pH mmol of texchanged) protons/
NaOH 100 9 of ignited product 0.00 3.26 0.0 1.00 4.98 15.4 2.00 5.40 30 7 3.00 5~60 46.1 4.00 5.68 61.4 5.00 5.~4 76.
6.00 6.19 92.1 6.50 6.46 99~8 7000 6.76 107.5 7~50 7.08 115.2 8.00 7.37 122.9
ml of 0~5 M pH mmsl of (exchanged) Na+ ions/
H2S04 100 9 of ignited product 8.0 4.20 142.0 8.5 2.96 150.9 9.0 2053 159.8 9.5 2.30 168.7 Example 6 Hydrochloric acid is added gradually to the sodium salt from Example 1 at room temperature in an amount such that a pH of 2.0 is obtained. The reaction mixture is stirred for about 15 minutes and filtered, and dilute hydrochloric acid is once again added to the residue from filtration until the pH reaches 2Ø The crystalline silicic acid formed is filtered off, washed twice with water thoroughly, filtered once again and sucked dry. The loss on ignition of ~he filter-moist product is 34.9X.
190 9 of a 5X strength NaCl solution are added to 100 g of the moist silicic acid, and the mixture is then titra-ted ~ith 1 M NaOH. Table 7 shows the titration values~
In the graph, an equivalence value of 155 meq/100 9 of ig-nited product is determined from the point of inflect;on of the curve at pH 9.5. From this, an ion exchange capa=
city of about 94 mmol of H~/mol of SiO2, corresponding to an SiO2:Na20 ratio of 21:1, is determined.
Table 7 ml of 1 M pH mmol of texchanged) protons/
NaOH 100 9 of ignited product 0.00 3.26 0.0 1.00 4.98 15.4 2.00 5.40 30 7 3.00 5~60 46.1 4.00 5.68 61.4 5.00 5.~4 76.
6.00 6.19 92.1 6.50 6.46 99~8 7000 6.76 107.5 7~50 7.08 115.2 8.00 7.37 122.9
- 15 -Table 7 (continued) ml of 1 MpH mmoL of (exchanged) protons/
NaOH 100 9 of ignited product 8.50 7.76 130.5 9~00 8.25 138.2 9.25 8.55 142.0 9.50 8.77 145.9 9.75 9.10 14g.7 10.10 9.60 155~1 10.25 9.78 157.4 10~50 9.93 1~1.2 10.75 10.30 165.1 11.00 10.58 168.9 11.25 10.75 172.8 11.50 lQ~95 176.6 11.75 11.09 180.4 12.00 11.21 184.3 12.25 11.29 188.1 12.50 11.36 192.0 13.00 11.54 199.6 13.50 11.63 207.3 14.00 11.70 215.0 15.00 11.84 230.3
NaOH 100 9 of ignited product 8.50 7.76 130.5 9~00 8.25 138.2 9.25 8.55 142.0 9.50 8.77 145.9 9.75 9.10 14g.7 10.10 9.60 155~1 10.25 9.78 157.4 10~50 9.93 1~1.2 10.75 10.30 165.1 11.00 10.58 168.9 11.25 10.75 172.8 11.50 lQ~95 176.6 11.75 11.09 180.4 12.00 11.21 184.3 12.25 11.29 188.1 12.50 11.36 192.0 13.00 11.54 199.6 13.50 11.63 207.3 14.00 11.70 215.0 15.00 11.84 230.3
16.00 11.88 245.7 Example 7 A product having the same educt composit;on as that of Example 1 is prepared. Seed crystaLs of a magadi- !
;te-type sil;cate from a previsus experiment are added to the reaction mixture. The reaction mixture is stirred for 19 hours at 165C, cooled and then filtered, and the produrt is washed with water and sucked dry on a suction filter. 10 ~ of the mother liquor from the reaction mix-ture, diluted with 250 ml of water, have a pH of 10.4.
The X-ray diffraction pattern of the product dried for a short time in the air (Na-SKS-2) is shown in Table 8.
The filter-moist product, uhich loses 61.3X of its ~eight ~hen ignited ~> 1000C)9 is titrated with sulfuric acid, analogously to Example 4. TabLe 9 shows the titra~
tion values. In the graph~ an equivalence value of Z15 meq/100 g of ignited product is determined from the point of inflection of the curve at pH 5Ø For a product having the composition Na20~y SiD2, an ion exchainge capa-city of 138 ~mol of Na+/mol of SiO2, correspon~ing to an Sio2:Na2o ratio of 14.5:1~ is determined frorm this.
If the procedure is carried ou~ in the abs~nce of seed crystals, substantially longer reaction times are requ;red.
Table 8 10d (10 8 cm~I/Io 15.5 100 7.76 13 5.15 20 4.69 8 154.44 10 ~.23 7 3.63 18 3.54 24 3.44 79 203.30 49 3.14 65 2.81 11 2.58 8 2.34 6 25Table 9 ml of 0.5 M pH mmol of (exchanged) Na~ ions/
H2S04 100 9 of ignited product 0.00 10.59 OOO
1.00 9.81 25.8 2.00 9.13 51.7 3,00 7.28 77.5 4~45 6.73115.0 5.00 6.61129.2 6.00 6.54155.0 7.00 6.40180.8 8.00 6.01206.7 8.50 3.97219.6 9.00 2.95232.5 ~.25 2.76239.0
;te-type sil;cate from a previsus experiment are added to the reaction mixture. The reaction mixture is stirred for 19 hours at 165C, cooled and then filtered, and the produrt is washed with water and sucked dry on a suction filter. 10 ~ of the mother liquor from the reaction mix-ture, diluted with 250 ml of water, have a pH of 10.4.
The X-ray diffraction pattern of the product dried for a short time in the air (Na-SKS-2) is shown in Table 8.
The filter-moist product, uhich loses 61.3X of its ~eight ~hen ignited ~> 1000C)9 is titrated with sulfuric acid, analogously to Example 4. TabLe 9 shows the titra~
tion values. In the graph~ an equivalence value of Z15 meq/100 g of ignited product is determined from the point of inflection of the curve at pH 5Ø For a product having the composition Na20~y SiD2, an ion exchainge capa-city of 138 ~mol of Na+/mol of SiO2, correspon~ing to an Sio2:Na2o ratio of 14.5:1~ is determined frorm this.
If the procedure is carried ou~ in the abs~nce of seed crystals, substantially longer reaction times are requ;red.
Table 8 10d (10 8 cm~I/Io 15.5 100 7.76 13 5.15 20 4.69 8 154.44 10 ~.23 7 3.63 18 3.54 24 3.44 79 203.30 49 3.14 65 2.81 11 2.58 8 2.34 6 25Table 9 ml of 0.5 M pH mmol of (exchanged) Na~ ions/
H2S04 100 9 of ignited product 0.00 10.59 OOO
1.00 9.81 25.8 2.00 9.13 51.7 3,00 7.28 77.5 4~45 6.73115.0 5.00 6.61129.2 6.00 6.54155.0 7.00 6.40180.8 8.00 6.01206.7 8.50 3.97219.6 9.00 2.95232.5 ~.25 2.76239.0
- 17 ~
Table 9 ~continued) ml of 0.5 M pH mmol of (exchanged~ Na+ ions/
H2S0~ 100 9 of ignited product 9~50 Z~65 245.4 9.75 2.55 251.9 10.00 2.48 258.2 10.50 2.34 271.7 1 1 nOO 2~16 297rl 12.00 2~09 310.0 1 n 12.50 2~03 322u9 13.00 1.98 335.8 Example 8 100 g of moist product from Example 7 are added to 200 ml of 5% strength hydrochlor;c acid, and the mix~ure is stirred for 1~25 hours at room temperature. The pro-duct is f;ltered off and added once again to the same amount of hydrochlor;c ac;d, the m;xture is stirred for 25 hours and f;ltered, and thorough wash;ng w;th water ;s carr;ed out tw;ce, the product be;ng st;rred with wa~er and being ~ashed in the filtration procedure. (The X-ray spectrum of the product dr;ed for a short time in the air ~s sho~n in Table 10). The product is then sucked dry.
It has a loss on ign;tion of 57X. 10 g of the product which has been sucked dry are added to 190 ml of 5X
strength NaCl soLution, and ~he mixture is then titrated w;th 1 M NaOH. Table 11 shows the t;trat;on values.
In the graph, an equivalence value of 235 mmol of H+/100 9 of ign;ted product is determined from the point of in~lec-tion of the curve at pH 8.3. From this, an ion exchange capacity of about 144 meq/moL of SiO2, corresponding to an S;02:Na20 ratio, or an S;02/2~+ rat;o, of 13.9:1, ;s determined.
For a natural as well as synthetic magadiite, the SiO2:Na20 composition determined by eLemental anaLysis is 13.4 to 14.4:1 (Lagaly et al., Am. Mineral.~ 60, 642-649 S1975)). The ratios of 14.5:1 and 13.9:1 determined from the ion exchange capac;t;es of Na-SKS-2 ~Example 7) and H-SKS-2 ~Example 8), respecti~ely, are in good agree-ment with these values.
~2~
Table 9 ~continued) ml of 0.5 M pH mmol of (exchanged~ Na+ ions/
H2S0~ 100 9 of ignited product 9~50 Z~65 245.4 9.75 2.55 251.9 10.00 2.48 258.2 10.50 2.34 271.7 1 1 nOO 2~16 297rl 12.00 2~09 310.0 1 n 12.50 2~03 322u9 13.00 1.98 335.8 Example 8 100 g of moist product from Example 7 are added to 200 ml of 5% strength hydrochlor;c acid, and the mix~ure is stirred for 1~25 hours at room temperature. The pro-duct is f;ltered off and added once again to the same amount of hydrochlor;c ac;d, the m;xture is stirred for 25 hours and f;ltered, and thorough wash;ng w;th water ;s carr;ed out tw;ce, the product be;ng st;rred with wa~er and being ~ashed in the filtration procedure. (The X-ray spectrum of the product dr;ed for a short time in the air ~s sho~n in Table 10). The product is then sucked dry.
It has a loss on ign;tion of 57X. 10 g of the product which has been sucked dry are added to 190 ml of 5X
strength NaCl soLution, and ~he mixture is then titrated w;th 1 M NaOH. Table 11 shows the t;trat;on values.
In the graph, an equivalence value of 235 mmol of H+/100 9 of ign;ted product is determined from the point of in~lec-tion of the curve at pH 8.3. From this, an ion exchange capacity of about 144 meq/moL of SiO2, corresponding to an S;02:Na20 ratio, or an S;02/2~+ rat;o, of 13.9:1, ;s determined.
For a natural as well as synthetic magadiite, the SiO2:Na20 composition determined by eLemental anaLysis is 13.4 to 14.4:1 (Lagaly et al., Am. Mineral.~ 60, 642-649 S1975)). The ratios of 14.5:1 and 13.9:1 determined from the ion exchange capac;t;es of Na-SKS-2 ~Example 7) and H-SKS-2 ~Example 8), respecti~ely, are in good agree-ment with these values.
~2~
- 18 -Table 10 d (10-8 cm) I/Io 12.1 11 7.42 S
5~55 6 4.35 8 3.69 17 3.6Z 18 3.43 100 3.25 16 3.21 16 3.18 15 Table 11 ml of 1 M pHmmol of (exchanged) protons/
15 NaOH 100 9 of ignited product 0.00 2.21 0.0 1.00 4~40 23.3 Z.OO 5.26 ~6.7 3.00 5.44 70.0 204.00 5.55 93-3 5.00 5.62116.6 6.00 5.69140.0 7.00 5.82163.3 7.25 5.89169.1 257.50 5.88174.9 7.75 5.91180.8 8.00 5.99186.6 8.25 6.12192.4 8.50 6~20198.3 308.75 6.44204.1 9.00 6.57210.0 9.25 6.82215.8 9.50 7.17221.6 9.75 7.55227.4 3510.00 8.05233.3 10.25 8O70239.1 10.50 9.15244.9 10.75 9.51250.8 11.00 9.88256.6 , ,
5~55 6 4.35 8 3.69 17 3.6Z 18 3.43 100 3.25 16 3.21 16 3.18 15 Table 11 ml of 1 M pHmmol of (exchanged) protons/
15 NaOH 100 9 of ignited product 0.00 2.21 0.0 1.00 4~40 23.3 Z.OO 5.26 ~6.7 3.00 5.44 70.0 204.00 5.55 93-3 5.00 5.62116.6 6.00 5.69140.0 7.00 5.82163.3 7.25 5.89169.1 257.50 5.88174.9 7.75 5.91180.8 8.00 5.99186.6 8.25 6.12192.4 8.50 6~20198.3 308.75 6.44204.1 9.00 6.57210.0 9.25 6.82215.8 9.50 7.17221.6 9.75 7.55227.4 3510.00 8.05233.3 10.25 8O70239.1 10.50 9.15244.9 10.75 9.51250.8 11.00 9.88256.6 , ,
- 19 -Table 11 (continued) ml of 1 M pH mmol of (exchanged~ protons/
NaOH 100 g of ign;ted product 11.25 10.15 262.
11.50 10.50 268~3
NaOH 100 g of ign;ted product 11.25 10.15 262.
11.50 10.50 268~3
Claims (5)
1. A process for the preparation of a crystalline sheet-type alkali metal silicate in an aqueous medium, wherein an acidic compound is added to an amorphous alkali metal silicate, or an alkali metal silicate dissolved in water, having a molar ratio M2O/SiO2, where M represents an alkali metal, of 0.24 to 2.00 in an amount such that a molar ratio M2O (unneutralized)/SiO2 of 0.05 to 0.239 is obtained, the molar ratio SiO2/H2O is, if required, adjusted to 1:5 to 1:100 by dilution, and the reaction mixture is kept at a reaction temperature of 70 to 250°C until the sheet-type alkali metal silicate has crystallized out.
2. The process as claimed in claim 1, wherein soda waterglass is employed as the alkali metal silicate dis-solved in water.
3. The process as claimed in claim 2, wherein the soda waterglass contains 22 to 30% by weight of SiO2 and 5 to 9% by weight of Na2O.
4. The process as claimed in claim 1, wherein the re-action temperature is 130 to 210°C.
5. The process as claimed in claim 1, wherein seed crystals of the crystalline sheet-type alkali metal sili-cate are added to the reaction mixture, in a weight ratio of 0.01 to 30% (relative to the amount of SiO2 in the amorphous alkali metal silicate, respectively the alkali metal sili-cate dissolved in water).
Applications Claiming Priority (2)
| Application Number | Priority Date | Filing Date | Title |
|---|---|---|---|
| DE19843400132 DE3400132A1 (en) | 1984-01-04 | 1984-01-04 | METHOD FOR PRODUCING CRYSTALLINE ALKALINE LAYER SILICATES |
| DEP3400132.8 | 1984-01-04 |
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| CA1220612A true CA1220612A (en) | 1987-04-21 |
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| CA000471395A Expired CA1220612A (en) | 1984-01-04 | 1985-01-03 | Process for the preparation of crystalline sheet-type alkali metal silicates |
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|---|---|
| US (1) | US4578258A (en) |
| EP (1) | EP0151295B1 (en) |
| JP (1) | JPS60161324A (en) |
| AT (1) | ATE38973T1 (en) |
| AU (1) | AU568053B2 (en) |
| BR (1) | BR8500009A (en) |
| CA (1) | CA1220612A (en) |
| DE (2) | DE3400132A1 (en) |
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|---|---|---|---|---|
| DE3416472A1 (en) * | 1984-05-04 | 1985-11-07 | Hoechst Ag, 6230 Frankfurt | DETERGENT CONTAINING SOFTENER |
| DE3416669A1 (en) * | 1984-05-05 | 1985-11-07 | Hoechst Ag, 6230 Frankfurt | SOFTENING DETERGENT |
| DE3426389A1 (en) * | 1984-07-18 | 1986-01-23 | Hoechst Ag, 6230 Frankfurt | SHAPED BODY MADE OF SILICATE MATERIAL, THEIR USE AND METHOD FOR THEIR PRODUCTION |
| DE3434709A1 (en) * | 1984-09-21 | 1986-04-03 | Hoechst Ag, 6230 Frankfurt | ADSORBENTS BASED ON ORGANOPHILIC MODIFIED LAYERED SILICA |
| US4812228A (en) * | 1985-09-10 | 1989-03-14 | Mobil Oil Corporation | Process for hydrotreating residual petroleum oil |
| US4937222A (en) * | 1984-12-28 | 1990-06-26 | Mobil Oil Corporation | Catalyst capable of hydrotreating residual petroleum oil |
| DE3669490D1 (en) * | 1985-06-13 | 1990-04-19 | Hoechst Ag | METHOD FOR PRODUCING CRYSTALLINE ALKALINE LAYER SILICATES. |
| US4626421A (en) * | 1985-06-28 | 1986-12-02 | Chevron Research Company | Preparation of magadiite |
| ZA867945B (en) * | 1985-11-12 | 1988-05-25 | Mobil Oil Corp | Layered silicates |
| AU587075B2 (en) * | 1985-11-12 | 1989-08-03 | Mobil Oil Corporation | Layered silicates |
| CA1272999A (en) * | 1985-11-12 | 1990-08-21 | Guenter H. Kuehl | Crystalline layered and large pore catalytic material |
| DK168988B1 (en) * | 1986-01-24 | 1994-07-25 | Topsoe Haldor As | Crystalline aluminosilicate, process for their preparation and use thereof |
| US5236681A (en) * | 1989-11-30 | 1993-08-17 | Mobil Oil Corp. | Layered silicate |
| US5174888A (en) * | 1990-01-25 | 1992-12-29 | Mobil Oil Corp. | Catalytic conversion |
| US5198203A (en) * | 1990-01-25 | 1993-03-30 | Mobil Oil Corp. | Synthetic mesoporous crystalline material |
| US5102643A (en) * | 1990-01-25 | 1992-04-07 | Mobil Oil Corp. | Composition of synthetic porous crystalline material, its synthesis |
| US5300277A (en) * | 1990-01-25 | 1994-04-05 | Mobil Oil Corporation | Synthesis of mesoporous crystalline material |
| SE468092B (en) * | 1990-11-14 | 1992-11-02 | Eka Nobel Ab | ALKALIMETAL SILICATE IN SOLID FORM CONTAINING SODIUM AND POTASSIUM, PREPARED FOR ITS PREPARATION AND ITS USE IN CLEANING COMPOSITIONS |
| SE468091B (en) * | 1990-11-14 | 1992-11-02 | Eka Nobel Ab | ALKALIMETAL SILICATE IN SOLID FORM CONTAINING SODIUM AND POTENTIAL Potassium, PREPARED FOR ITS PREPARATION AND ITS USE IN CLEANING COMPOSITIONS |
| NZ239112A (en) | 1991-01-29 | 1994-12-22 | Ecolab Inc | Solid alkaline compositions containing the reaction product in water of alkali metal hydroxide and alkali metal silicate; process of manufacture |
| DE4107230C2 (en) * | 1991-03-07 | 1995-04-06 | Hoechst Ag | Process for the production of sodium silicates |
| DE4308062A1 (en) * | 1993-03-13 | 1994-09-15 | Hoechst Ag | Process for the preparation of mixtures of synthetic, crystalline kenyaite and oxygen-releasing salts and their use |
| DE4318242A1 (en) * | 1993-06-02 | 1994-12-08 | Hoechst Ag | Process for the preparation of crystalline sodium layer silicate with kanemite structure |
| ES2150607T3 (en) * | 1995-03-06 | 2000-12-01 | Clariant Gmbh | CRYSTALLINE STRATIFIED SODIUM SILICATE. |
| DE19537957A1 (en) * | 1995-10-12 | 1997-04-17 | Hoechst Ag | Process for the production of highly exchangeable sodium disilicate |
| DE19603838A1 (en) * | 1996-02-05 | 1997-08-07 | Hoechst Ag | Crystalline silicas |
| US7052665B2 (en) * | 2001-11-01 | 2006-05-30 | Silicycle Inc. | Method of preparing highly ordered mesoporous molecular sieves |
| CN102351202B (en) * | 2011-07-06 | 2013-05-01 | 陕西科技大学 | Preparation method of bismuth silicate powder |
Family Cites Families (8)
| Publication number | Priority date | Publication date | Assignee | Title |
|---|---|---|---|---|
| DD63366A (en) * | ||||
| AU497891B2 (en) * | 1974-05-22 | 1979-01-18 | J.M. Huber Corp. | Siliceous pigments & their production |
| DE2742912C3 (en) * | 1977-09-23 | 1980-05-08 | Lagaly, Gerhard, Prof. Dr., 2300 Kiel | Crystalline silica, its potassium salt, process for its preparation and its uses |
| US4285922A (en) * | 1979-09-10 | 1981-08-25 | Mobil Oil Corporation | Method of preparing crystalline zeolite |
| US4430314A (en) * | 1980-06-06 | 1984-02-07 | Mobil Oil Corporation | Method of preparing crystalline zeolite |
| DE3162102D1 (en) * | 1980-06-12 | 1984-03-08 | Ici Plc | Zeolite synthesis |
| DE3211433C2 (en) * | 1982-03-27 | 1984-12-13 | Degussa Ag, 6000 Frankfurt | Crystalline aluminosilicate PZ 1 and process for its production |
| GB2125390B (en) * | 1982-08-16 | 1985-12-24 | Ici Plc | Preparation of zeolites |
-
1984
- 1984-01-04 DE DE19843400132 patent/DE3400132A1/en not_active Withdrawn
- 1984-12-19 DE DE8484115779T patent/DE3475396D1/en not_active Expired
- 1984-12-19 EP EP84115779A patent/EP0151295B1/en not_active Expired
- 1984-12-19 AT AT84115779T patent/ATE38973T1/en active
- 1984-12-28 JP JP59275019A patent/JPS60161324A/en active Granted
-
1985
- 1985-01-02 US US06/688,184 patent/US4578258A/en not_active Expired - Lifetime
- 1985-01-02 ES ES539296A patent/ES8605445A1/en not_active Expired
- 1985-01-03 BR BR8500009A patent/BR8500009A/en not_active IP Right Cessation
- 1985-01-03 PT PT79793A patent/PT79793B/en not_active IP Right Cessation
- 1985-01-03 CA CA000471395A patent/CA1220612A/en not_active Expired
- 1985-01-03 PT PT79788A patent/PT79788A/en unknown
- 1985-01-03 ZA ZA8531A patent/ZA8531B/en unknown
- 1985-01-03 AU AU37348/85A patent/AU568053B2/en not_active Ceased
Also Published As
| Publication number | Publication date |
|---|---|
| ZA8531B (en) | 1985-09-25 |
| DE3475396D1 (en) | 1989-01-05 |
| BR8500009A (en) | 1985-08-13 |
| AU568053B2 (en) | 1987-12-10 |
| PT79793A (en) | 1985-02-01 |
| PT79793B (en) | 1986-11-14 |
| ATE38973T1 (en) | 1988-12-15 |
| EP0151295B1 (en) | 1988-11-30 |
| EP0151295A1 (en) | 1985-08-14 |
| AU3734885A (en) | 1985-07-18 |
| ES8605445A1 (en) | 1986-04-01 |
| DE3400132A1 (en) | 1985-07-11 |
| JPH0553729B2 (en) | 1993-08-10 |
| US4578258A (en) | 1986-03-25 |
| ES539296A0 (en) | 1986-04-01 |
| PT79788A (en) | 1985-02-01 |
| JPS60161324A (en) | 1985-08-23 |
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