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Process of preparing aluminum chlorhydroxides and aluminum hydroxide

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US3113911A
US3113911A US5414460A US3113911A US 3113911 A US3113911 A US 3113911A US 5414460 A US5414460 A US 5414460A US 3113911 A US3113911 A US 3113911A
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aluminum
compartment
chloride
anode
intermediate
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John L Jones
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Armour Pharmaceutical Co
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    • CCHEMISTRY; METALLURGY
    • C01INORGANIC CHEMISTRY
    • C01FCOMPOUNDS OF THE METALS BERYLLIUM, MAGNESIUM, ALUMINIUM, CALCIUM, STRONTIUM, BARIUM, RADIUM, THORIUM, OR OF THE RARE-EARTH METALS
    • C01F7/00Compounds of aluminium
    • C01F7/48Aluminium halides
    • C01F7/56Chlorides

Description

Dec. 10, 1963 JONES 3 113,911

J. L. PROCESS OF PREPARING ALUMINUM CHLORHYDROXIDES AND ALUMINUM HYDROXIDE Filed Sept. 6, 1960 3,ll3,9ll

Patented Dec. 10, 1963 3,113,911 PROCES F PREPARING ALUMINUM CHM HYDROXEBES AND ALUMINUM HYDRGXIDE John Jones, Berkeley Heights, NJ., assignor, by mesne ass gnments, to Armour Pharmaceutical Company, Chicago, Ill a corporation of Delaware Filed Sept. 6, 1969, Ser. No. 54,144 9 Claims. (61. zet -94) Th s invention relates to a process of preparing aluminum chlorhydroxides, particularly Al (OI-I) Cl, the -76 basic salt, by electrolysis of aluminum chloride, and to an apparatus for carrying out this process.

The electrolysis of aluminum chloride to produce aluminum chlorhydroxide Al (OH) Cl is described in US. Patent No. 2,392,531. An aqueous solution of aluminum chloride is subjected to electrolysis in a diaphragm cell in which catholyte and anolyte are kept in separate compartments. III the course of this process, hydrogen is liberated at the cathode and chlorine at the anode. The reaction is quantitative, so far as the electrolysis of aluminum chloride is concerned. The yield of aluminum chlorhydroxide is not good, however, because of the loss of chlorine at the anode. In order to make the process practical commercially, it is necessary to recover this chlorine, but this is rather difficult to do, and there is also the problem of its contamination with other materials. Consequently, the electrolytic production of aluminum chlorhydroxide has never been fully satisfactory.

In accordance with the instant invention, a process of preparing aluminum chlorhydroxides and aluminum hydroxide by electrolysis of aluminum chloride as the catholyte is provided wherein the loss of chlorine at the anode is prevented by reaction of such chloride ion as migrates from the cathode compartment with aluminum oxide before it reaches the anode compartment, regenerating aluminum chloride, which can be recirculated to the cathode compartment for conversion to aluminum chlorhydroxide. The reactions which take place in this electrolysis can be summarized as follows, using the /6 basic salt as illustrative.

In cathode compartment:

H. 2AlC1 +5 OH- A1 OH C1+5 Cl 40 In compartment adjacent cathode compartment:

III. 2A1 O 6HCl- 2AlCl 3H O In anode compartment: 59

IV. 2H O- O +4H+ It will be apparent that similar reactions occur in the formation of other aluminum chlorhydroxides and aluminum hydroxide. The process can be made to produce any of the compounds, including, for example:

Mixtures of these also can be obtained. The electrolysis proceeds down the series from No. 1 to No. 6, as the ultimate product, and can be followed by observing the pH of the reaction mixture, which ranges from about 1 at the start to about 4.4 at No. 5, the other aluminum chlorhydroxides being intermediate, and the aluminum hydroxide is formed as a precipitate at the end stage of the electrolysis. Hence, any desired aluminum chlorhydroxide can be prepared simply by stopping the electrolysis at the pH value corresponding to the desired chlorhydroxide.

The anolyte plays no role in these reactions, and preferably is kept isolated therefrom so that chloride ion cannot migrate into it.

It is apparent from the above scheme that one mole of hydrogen chloride is consumed for every mole of Al (OH) Cl produced. Hence, to start the reaction initially it is necessary to have hydrogen chloride present in the aluminum oxide compartment, at least in the proportion of one mole of hydrogen chloride for every mole of aluminum chlorhydroxide Al (OH) C1 produced. If other aluminum chlorhydroxides are desired, such as the /3 basic salt Al (OH) Cl,, or the /3 basic salt Al (OH) Cl the amount of hydrogen chloride will be increased accordingly. The overall effect of the process, therefore, as shown, is to convert water, aluminum oxide and hydrogen chloride into aluminum chlorhydroxide, hydrogen and oxygen.

The process of the invention can be carried out continuously or semicontinuously or batchwise in an electrolytic cell having three compartments, a cathode compartment, an anode compartment, and a third compartment intermediate these two compartments. The type of cell contemplated is shown in cross-section in the FIGURE.

The cathode compartment 1 is equipped with a cathode 2 of material which is not attacked by aqueous aluminum chloride solution, such as carbon. The anode compartment 3 is equipped with an anode 4- of acidresistant material such as platinum. The anode and cathode compartments are separated from the intermediate compartment 5 by diaphragms 6 and 7, which permit the passage of ions required for carrying out the reactions of the invention in their respective compartments, and preferably prevent passage of all others.

In operation, the catholyte, aqueous aluminum chloride solution, is placed in the cathode compartment, and the anolyte, an aqueous acid whose anion is not discharged as a gas at the anode, such as sulfuric acid, is put in the anode compartment. An aqueous slurry of aluminum oxide containing as much hydrogen chloride as is required to start the reaction is put in the intermediate compartment 5. Then the electrolysis is begun.

In the cathode compartment, hydrogen gas: is discharged at the cathode, leaving behind Ol-I ion, and resulting in the formation of 1Xl ((')I-I),,Cl in the catholyte, Where n represents the proportion of OH ion in the product, and can range from 1 to 6. When n is 6, the product is aluminum hydroxide. Chloride ion from the cathode compartment and hydrogen ion from the anode compartment migrate into the intermediate compartment, and there react with aluminum oxide in accordance with reaction HI above to form aluminum chloride. The conditions are so adjusted that a minimum of chloride ion migrates from the intermediate compartment into the anode compartment, inasmuch as chloride ion in the anolyte could be discharged at the anode to form chlorine gas, reducing the yield.

While diaphragms of any of the types commonly employed in diaphragm cells can be used between the various compartments in this cell, it is preferred that the diaphragm between the anode compartment and the intermediate compartment be of cation-permselective material which will not pass chlorine ion. This excludes chlorine ion entirely from the anode compartment. A variety of cation-permselective membrane material useful as diaphragms in electrolytic cells are known to those in the art. Such permselective membranes are in general to those of two types. One type is in the form of sheets, or films formed wholly of the cation-permselective material, such as are described, for example, in US. Patents Nos. 2,636,851 to Juda et al., 2,702,272 to Kasper, 2,730,768, 2,731,408, 2,731,411, 2,756,202 to Clarke, 2,805,196 to Roebersen et al., and 2,858,264 and 2,867,575 to De long. These membranes can be formed directly from monomeric or unpolymerized reactive ingredients, polymerizing them under conditions such that the desired film is formed. The reactive ingredients may include the functional cationexchange groups, or such groups may be incorporated in the film after its formation by appropriate reaction procedures, all of which are well known in the art. Suitable acidic functional groups linked to the matrix include SO3H and CO'OH groups, the former being preferred because of its high dissociation constant. Typical polymeric matrices to which such functional groups are linked include polystyrene, phenol-aldehyde resins, polystyrene-divinyl benzene copolymers, resorcinol-aldehyde polymers, copolymers of divinyl benzene with acrylic acid, copolymers of divinyl benzene with maleic anhydride, copolymers of divinyl benzene with acrylonitrile, copolymers of divinyl benzene and methacrylic acid, cellulose derivatives such as regenerated cellulose, ethyl cellulose and polyvinyl alcohol, and like polymers containing free hydroxyl groups, reactedwith sulfonating agents, and polyethylene reacted with chlorosulfonic acids or other sulfonating agents. Examples of such membranes will be found in the patents referred to.

The cation-exchange resins which can be employed in either of these types of films include the sulfonated phenol aldehyde resins described in U.S. Patents Nos. 2,184,943, 2,195,196, 2,204,539, 2,228,159, 2,228,160, 2,230,641, 2,259,455, 2,285,750, 2,319,959 and 2,361,754, the sulfonated cross-linked polymers of styrene described in US. Patent No. 2,366,007, and the carboxylic resins described in Patents Nos. 2,340,110 and 2,340,111.

Porous diaphragms of other materials can be used, such as porous bonded mats or bats of nonwoven chemically resistant fibers, such as glass, asbestos, alundum, nylon and polyacrylonitrile fibers. Perforated plates and microporous corrosion-resistant metal and synthetic resin membranes also can be employed.

The reaction temperatures are not critical. The formation of aluminum chlorhydroxide in the cathode compartment is favored by electrolysis at a temperature above about 70 C. At lower temperatures, there is a tendency to form aluminum hydroxide, which may precipitate out. The upper temperature limit is determined by the boiling point of the catholyte, and is usually approximately The reaction of aluminum oxide with chloride ion or hydrogen chloride to form aluminum chloride in the intermediate compartment proceeds at elevated temperatures, above about 70 C. Thus the reaction proceeds with good efiiciency at the temperatures applied in the cathode com- .paItment.

Chloride ion migration from the intermediate compartment into the anode compartment is less at low temperatures, and it is accordingly preferred that the anode compartment be kept at room temperature or below, or at least as close to room temperature as is convenient. Ionpermselective membranes tend to lose their efiiciency in barring passage of ions as temperature increases, and this is an additional reason for maintaining the anolyte at as low a temperature as possible.

The desired temperature gradient from the cathode compartment to the anode compartment can be achieved by interposing cooling coils in the intermediate compartment adjacent the diaphragm separating the intermediate and anode compartments. The diaphragm would be on the anode side of the cooling coils. Other ways of achieving temperature gradients are known to the art, and are disclosed in the literature on diaphragm type cells, inasmuch as this problem is encountered in other processes.

The concentration of aluminum chloride in the catholyte can be modified as desired, according to the particular aluminum chlorhydroxide that is desired. Solutions of aluminum chloride ranging from about 5 to about 25% AlCl are satisfactory. Usually, the maximum concentration that can be obtained without too high a viscosity is used, because this avoids the necessity of concentrating the anolyte solution, since the aluminum chlorhydroxide is ordinarily sold as a 50% aqueous solu tion.

The concentration of aluminum oxide in the slurry in the intermediate compartment will be determined by the aluminum chloride concentration and the amount of migration of chloride ion from the catholyte into that compartment. More aluminum oxide may be required per mole of aluminum chloride when the /6 basic salt is produced, for example, because more chloride ion is available to migrate into the intermediate compartment. However, it is also possible in a semicontinuous or continuous process to adjust for different concentrations of aluminum chloride and aluminum oxide simply by modifying the rate of removal of the liquor from these compartments to correspond to the amounts of aluminum chlorhydroxide and aluminum chloride, respectively, that are formed therein.

The amount of acid required in the anode compartment is simply enough to permit eflicient electrolysis. An 0.5 to 10% solution of a strong acid, such as sulfuric acid, is quite satisfactory. A somewhat greater concentration of a Weaker acid, such as phosphoric acid, may be necessary because of the lesser ionization of the acid to achieve the same current efliciency as is obtained at these sulfuric acid concentrations.

The following examples in the opinion of the inventor represent the best embodiments of this invention:

Example 1 A diaphragm cell was employed in this run, of the type shown in FIGURE 1. The diaphragms separating the cathode and anode compartments from the intermediate compartment were made of porous alundum sheet. 195 g. (0.3 mole) of a 24 Baum solution of aluminum chloride was placed in the cathode compartment, which was equipped with a carbon cathode. A slurry of 30 g. of aluminum oxide and 5 ml. of hydrogen chloride (2.17 g. chlorine) in 500 ml. of water was put in the intermediate compartment, and ml. of 10% aqueous sulfuric acid solution was put in the anode compartment, which was equipped with a platinum anode. The aluminum oxide slurry was prepared by mixing the water and hydrogen chloride, and bringing the resulting solution to a boil, after which the aluminum oxide was added.

The catholyte was brought to a temperature of 94 to 98 C., and the current then turned on. A current of 2 amperes was applied for 4.5 hours. 8.5 volts was required at first. After one hour, this had dropped to 6 volts. The current was then changed to 1 ampere for 0.5 hour, at the end of which time the pH of the catholyte was 3.25. The current was continued at 1 ampere for three hours, after which the voltage had dropped to 4, and the pH was 4.2.

135.6 g. of catholyte were obtained, having an aluminum content of 2.79%, and a chlorine content of 1.85%. Thus the aluminumzchloride ratio Al/Cl was 1.98. The ratio for A1 (OH) Cl is 2, showing that the product was quite pure.

The liquor in the intermediate compartment showed that 15.2 g. of aluminum oxide was dissolved. The aluminum content was 1.27% and the chlorine content 4.14%. Thus, the Al/Cl ratio was 0.39. This ratio for AlCl is 0.33, showing a very significant conversion of aluminum oxide to aluminum chloride.

The anolyte liquor weighed 131 g., and contained 0.05% aluminum and 0.116% chlorine.

Example 2 The electrolytic cell employed in this run was the same as used in Example 1. 390 g. (0.6 mole) of a 24 Baum solution of aluminum chloride was placed in the cathode compartment. A slurry, prepared as set forth in Example 1, of 40 g. of aluminum oxide and 5 ml. of concentrated hydrochloric acid (2.17 g. chlorine) in 500 ml. of water was placed in the intermediate compartment. 150 m1. of a aqueous sulfuric acid solution was placed in the anode compartment.

The electrolysis was conducted for a total of 22.75 ampere hours at a temperature of 95 to 96 C. in the cathode compartment. The first seven hours were at a current of 3 amperes. At the end of this time, the pH was 3.3, and the voltage 6.2. The current was reduced to 1.5 amperes at 0.75 hour at 6 volts and to 1 ampere for 0.25 hour at 5 volts. The pH then was 3.75. The current was stopped after an additional 0.42 hour at 1 ampere and 6 volts. The pH then was 4.35.

150.5 g. of catholyte were recovered, containing 4% aluminum and 2.62% chlorine. This corresponded to an Al/Cl ratio of 2.005, substantially pure Al (OH) C1.

Analysis of the slurry in the intermediate compartment showed that 21.2 g. of aluminum oxide had reacted. The aluminum content was 2.79%, and the chlorine content 9.34%, giving an Al/Cl ratio of corresponding very closely to the theoretical ratio of AlCl which is 0.33. The SO content was 2.12%.

115.7 g. of anolyte was recovered, containing 0.37% aluminum and 1.14% chlorine.

Example 3 The diaphragm cell similar to that described in FIG- URE 1 was employed to prepare an aluminum chlorhydroxide having an Al/Cl ratio of 2.06, essentially pure Al (OH) Cl. The diaphragm separating the cathode and intermediate compartment was made of inch medium porosity alundum sheet. The diaphragm separating the anode and intermediate compartments was a sheet of cation exchange membrane of the sulfonated polystyrene type, comprising particles of sulfonated polystyrene bonded together with an inert resinous binder. The resin is available commercially under the trade name Permutit Q, and the membrane is sold under the trade designation Permutit 3142. In place of this membrane, equally good results are obtained employing the strongly acid sulfonated copolymer of styrene and divinyl benzene prepared in sheet form in accordance with Example 4 of Patent No. 2,636,851.

In the cathode compartment containing a graphite electrode was placed 780 g. (1.20 moles) of 24 Baum aluminum chloride solution. The intermediate compartment was filled with a slurry of 200 g. of hydrated alumina (130 g. A1 0 50 ml. of concentrated hydrochloric acid (21.7 g. chlorine, and about 9 liters of water). Into the anode compartment containing a platinum electrode was placed 9.3 liters of 0.95% sulfuric acid solution. The catholyte was brought to a temperature of 95 C. and the current then turned on. The temperature was maintained at from 95 to 105 C. in the cathode compartment, 79 to 81 C. in the intermediate compartment and 30 to 33 C. in the anode compartment. A current 3 amperes was applied over a period of 31.5 hours, at which point a coating of aluminum oxide was detected on the cathode, and the pH of the catholyte was 4.2.

The catholyte was filtered, and yielded 388 g. of aluminum and 4.20% chlorine, the atomic Al/Cl ratio being 2.06. The intermediate compartment yielded 10,030, g. of liquor, assaying 0.152% aluminum and 1.19% chlorine, showing that 72 g. of aluminum chloride was formed during the reaction.

Example 4 The electrolytic cell in this example shown in FIGURE 1 was employed to prepare an aluminum chlorhydroxide of approximately the composition Al (OH) Cl i.e., a mixture of some Al (OH) Cl with, mostly, Al (OI-I) Cl The cathode compartment contained 780 g. (1.20 moles) of a 24 Baum aluminum chloride solution. The intermediate compartment contained a slurry of 200 g. of hydrated alumina (130 g. A1 0 100 ml. of concentrated hydrochloric acid (43.4 g. of chlorine) and 9 liters of water. The anode compartment contained 9 liters of 0.59% sulfuric acid solution. The catholyte was brought to a temperature of C. and held at 95 to C. for the duration of the run. During this period, the intermediate compartment temperature was held within the range from 82 to 85 C., and the anode compartment at within the range from 33 to 36 C.

A current of 3 amperes was applied as soon as the catholyte had been brought to 95 C., and the current was continued for 19.5 hours, at the end of which time the pH of the catholyte had risen to 3.3. The catholyte was clarified by filtration, and yielded 331 g. of product assaying 7.09% aluminum and 6.42% chlorine, for an atomic Al/Cl ratio of 1.45.

The intermediate compartment yielded 12,000 g. of liquor assaying 0.104% aluminum and 1.01% chlorine, showing that 39.4 g. of aluminum chloride was produced.

Example 5 The electrolytic cell used in Example 1 was employed to prepare an aluminum chlorhydroxide having the approximate composition Al (OH) Cl Into the cathode compartment was placed 780 g. (1.2 mole) of a 24 Baum aluminum chloride solution. The intermediate compartment was filled with a slurry of 200 g. of hydrated alumina g. A1 03), ml. of concentrated hydrochloric acid (65.1 g. of chlorine) and 9 liters of water. The anode compartment contained 9 liters of 0.59% sulfuric acid solution. The catholyte was brought to 95 C. and held at from 95 to 100 C. throughout the electrolysis. The intermediate compartment was held at 83 to 85 C., and the anolyte at 33 to 35 C. during the run.

The current was turned on as soon as the catholyte had reached 95 C., and was applied over a period of 15.25 hours, at which point the pH of the catholyte had reached 2.7. The catholyte was clarified by filtration, and 438 g. of product recovered, assaying 6.00% aluminum and 10.9% chlorine, indicating an Al/Cl ratio of 0.72. 30.6 g. of aluminum chloride was produced in the intermediate compartment.

I claim:

1. In the process for preparing aluminum chlorhydroxides and aluminum hydroxide from aluminum chloride by electrolyzing an aqueous solution of aluminum chloride as catholyte to liberate hydrogen at the cathode, and form aluminum chlorhydroxides in the catholyte, the improvement which comprises contacting chloride ions migrating towards the anode with aluminum oxide to form aluminum chloride.

2. A process for preparing aluminum chlorhydroxides and aluminum hydroxide from aluminum chloride, which comprises electrolyzing in a compartmented cell an aqueous solution of aluminum chloride as catholyte, thereby liberating hydrogen and forming aluminum chlorhydroxides and aluminum hydroxide in the catholyte, contacting chloride ions migrating towards the anode, with aluminum oxide to form aluminum chloride.

3. A process in accordance with claim 2 in which the proportions of aluminum chloride and the conditions during electrolysis are so adjusted as to produce principally aluminum monochlorhydroxide Al (OH) C1.

4. A process in accordance with claim 2 in which the proportions of aluminum chloride and the conditions during electrolysis are so adjusted as to produce principally aluminum dichlorhydroxide Al (OH) C1 5. A process in accordance with claim 2 in which the proportions of aluminum chloride and the conditions dur- 7 ing electrolysis are so adjusted as to produce principally aluminum tetrachlorhydroxide Al (OH) Cl 6. A process in accordance with claim 2 in which the catholyte is held at a temperature within the range from at least 70 C. up to the boiling point of the catholyte.

7. A process in accordance with claim 2 in which the anolyte is an aqueous solution of an inorganic acid whose anion is not discharged as a gas at the anode.

8. A process in accordance with claim 7 in which the acid is sulfuric acid.

9. A process for continuously producing aluminum chlorhydroxides and aluminum hydroxide from aluminum chloride in a compartmented cell having cathode, anode and intermediate compartments, which comprises electrolyzing an aqeuous solution of aluminum chloride as catholyte, thereby liberating hydrogen and forming aluminum chlorhydroxide and aluminum hydroxide in the catholyte, reacting chloride ion which migrates into an intermediate compartment of the cell with aluminum oxide to form aluminum chloride, continuously withdrawing catholyte and recovering aluminum chlorhydroxides there from, continuously supplying aluminum oxide and hydrogen chloride to the intermediate compartment, and continuously withdrawing aluminum chloride from the intermediate compartment and recirculating this to the cathode compartment.

References Cited in the file of this patent UNITED STATES PATENTS 2,176,343 Howard Oct. 17, 1939 2,392,531 Huehn et a1 Jan. 8, 1946 2,921,005 Bodamer Jan. 12, 1960 2,967,806 Osborne et a1 Jan. 10. 1961 3,017,338 Butler et al Jan. 16, 1962 OTHER REFERENCES Ephraim: Inorganic Chemistry, 5th edition, page 283.

Claims (1)

1. IN THE PROCESS FOR PREPARING ALUMINUM CHLORHYDROXIDES AND ALUMINUM HYDROXIDE FROM ALUMINUM CHLORIDE BY ELECTROLYZING AN AQUEOUS SOLUTION OF ALUMINUM CHLORIDE AS CATHOLYTE TO LIBERATE HYDROGEN AT THE CATHODE, AND FORM ALUMINUM CHLORHYDROXIDES IN THE CATHOLYTE, THE IMPROVEMENT WHICH COMPRISES CONTACTING CHLORIDE IONS MIGRATING TOWARDS THE ANODE WITH ALUMINUM OXIDE TO FORM ALUMINUM CHLORIDE.
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Cited By (16)

* Cited by examiner, † Cited by third party
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US3372101A (en) * 1962-10-08 1968-03-05 Kollsman Paul Process of producing highly reactive compounds by metathesis
FR2174118A1 (en) * 1972-03-01 1973-10-12 Snam Progetti
US3767549A (en) * 1970-09-24 1973-10-23 Asahi Chemical Ind Method for producing basic aluminum chloride
US3887692A (en) * 1972-07-10 1975-06-03 Armour Pharma Microspherical basic aluminum halides and method of making same
US3909439A (en) * 1972-03-01 1975-09-30 Snam Progetti Process for the production of aluminum chlorohydroxides
US3925174A (en) * 1973-11-01 1975-12-09 Hooker Chemicals Plastics Corp Electrolytic method for the manufacture of hypochlorites
US3947332A (en) * 1974-06-07 1976-03-30 Gte Sylvania Incorporated Preparation of heteropoly acids of tungsten and molybdenum
US3954577A (en) * 1974-11-27 1976-05-04 Texaco Inc. Electrochemical preparation of aluminum bromide
US4066519A (en) * 1977-03-28 1978-01-03 Olin Corporation Cell and process for electrolyzing aqueous solutions using a porous metal separator
US4203812A (en) * 1977-03-25 1980-05-20 Hoechst Aktiengesellschaft Process for preparing basic aluminum chlorides
US5985234A (en) * 1995-09-18 1999-11-16 Delta Chemical Corporation Polyaluminum chlorides and polyaluminum chlorosulfates methods and compositions
WO2003009811A2 (en) * 2001-07-25 2003-02-06 Haase Richard A Processes and apparatus for the manufacture of polynuclear aluminum compounds and disinfectants, and polynuclear aluminum compounds and disinfectants from such processes and apparatus
WO2007082122A2 (en) * 2006-01-06 2007-07-19 Nextchem, Llc Polyaluminum chloride and aluminum chlorohydrate, processes and compositions: high-basicity and ultra high-basicity products
WO2007082123A2 (en) * 2006-01-06 2007-07-19 Next Chem Polymetal hydroxychloride processes and compositions: enhanced efficacy antiperspirant salt compositions
CN101437753B (en) 2006-01-06 2013-02-06 耐克斯特凯姆股份有限公司 Polyaluminum chloride and aluminum chlorohydrate, processes and compositions: high-basicity and ultra high-basicity products
WO2016179786A1 (en) * 2015-05-11 2016-11-17 毕世飞 Method of preparing ferric salt

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US2392531A (en) * 1937-05-15 1946-01-08 Huehn Werner Production of water-soluble basic aluminum compounds
US2921005A (en) * 1952-10-17 1960-01-12 Rohm & Haas Electrolytic conversions with permselective membranes
US2967806A (en) * 1953-04-02 1961-01-10 Hooker Chemical Corp Electrolytic decomposition with permselective diaphragms
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US2176343A (en) * 1937-04-05 1939-10-17 Carnegie Inst Of Technology Process for the separation and purification of organic acids
US2392531A (en) * 1937-05-15 1946-01-08 Huehn Werner Production of water-soluble basic aluminum compounds
US2921005A (en) * 1952-10-17 1960-01-12 Rohm & Haas Electrolytic conversions with permselective membranes
US2967806A (en) * 1953-04-02 1961-01-10 Hooker Chemical Corp Electrolytic decomposition with permselective diaphragms
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Cited By (26)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
US3372101A (en) * 1962-10-08 1968-03-05 Kollsman Paul Process of producing highly reactive compounds by metathesis
US3767549A (en) * 1970-09-24 1973-10-23 Asahi Chemical Ind Method for producing basic aluminum chloride
FR2174118A1 (en) * 1972-03-01 1973-10-12 Snam Progetti
US3909439A (en) * 1972-03-01 1975-09-30 Snam Progetti Process for the production of aluminum chlorohydroxides
US3887692A (en) * 1972-07-10 1975-06-03 Armour Pharma Microspherical basic aluminum halides and method of making same
US3925174A (en) * 1973-11-01 1975-12-09 Hooker Chemicals Plastics Corp Electrolytic method for the manufacture of hypochlorites
US3947332A (en) * 1974-06-07 1976-03-30 Gte Sylvania Incorporated Preparation of heteropoly acids of tungsten and molybdenum
US3954577A (en) * 1974-11-27 1976-05-04 Texaco Inc. Electrochemical preparation of aluminum bromide
US4203812A (en) * 1977-03-25 1980-05-20 Hoechst Aktiengesellschaft Process for preparing basic aluminum chlorides
US4066519A (en) * 1977-03-28 1978-01-03 Olin Corporation Cell and process for electrolyzing aqueous solutions using a porous metal separator
US5985234A (en) * 1995-09-18 1999-11-16 Delta Chemical Corporation Polyaluminum chlorides and polyaluminum chlorosulfates methods and compositions
US5997838A (en) * 1995-09-18 1999-12-07 Delta Chemical Corporation Polyaluminum chlorides and polyaluminum chlorosulfates methods and compositions
US6036935A (en) * 1995-09-18 2000-03-14 Delta Chemical Corporation Polyaluminum chlorides and polyaluminum chlorosulfates methods and compositions
WO2003009811A3 (en) * 2001-07-25 2009-02-26 Richard A Haase Processes and apparatus for the manufacture of polynuclear aluminum compounds and disinfectants, and polynuclear aluminum compounds and disinfectants from such processes and apparatus
WO2003009811A2 (en) * 2001-07-25 2003-02-06 Haase Richard A Processes and apparatus for the manufacture of polynuclear aluminum compounds and disinfectants, and polynuclear aluminum compounds and disinfectants from such processes and apparatus
WO2007082123A2 (en) * 2006-01-06 2007-07-19 Next Chem Polymetal hydroxychloride processes and compositions: enhanced efficacy antiperspirant salt compositions
US20070187256A1 (en) * 2006-01-06 2007-08-16 Pratt Willam E Polyaluminum Chloride and Aluminum Chlorohydrate, Processes and Compositions: High-Basicity and Ultra High-Basicity Products
US20070196302A1 (en) * 2006-01-06 2007-08-23 Pratt William E Polymetal Hydroxychloride Processes and Compositions: Enhanced Efficacy Antiperspirant Salt Compositions
WO2007082123A3 (en) * 2006-01-06 2008-01-03 Next Chem Polymetal hydroxychloride processes and compositions: enhanced efficacy antiperspirant salt compositions
WO2007082122A3 (en) * 2006-01-06 2008-01-03 Nextchem Llc Polyaluminum chloride and aluminum chlorohydrate, processes and compositions: high-basicity and ultra high-basicity products
WO2007082122A2 (en) * 2006-01-06 2007-07-19 Nextchem, Llc Polyaluminum chloride and aluminum chlorohydrate, processes and compositions: high-basicity and ultra high-basicity products
US7846318B2 (en) 2006-01-06 2010-12-07 Nextchem, Llc Polyaluminum chloride and aluminum chlorohydrate, processes and compositions: high-basicity and ultra high-basicity products
EP2418171A1 (en) * 2006-01-06 2012-02-15 Nextchem Method for increasing the hydroxide content of polymetal hydroxychlorides used as antiperspirant salt compositions with enhanced efficacy
CN101437753B (en) 2006-01-06 2013-02-06 耐克斯特凯姆股份有限公司 Polyaluminum chloride and aluminum chlorohydrate, processes and compositions: high-basicity and ultra high-basicity products
US8801909B2 (en) 2006-01-06 2014-08-12 Nextchem, Llc Polymetal hydroxychloride processes and compositions: enhanced efficacy antiperspirant salt compositions
WO2016179786A1 (en) * 2015-05-11 2016-11-17 毕世飞 Method of preparing ferric salt

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