Classifications

• • C—CHEMISTRY; METALLURGY
  • C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
  • C25B—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES FOR THE PRODUCTION OF COMPOUNDS OR NON-METALS; APPARATUS THEREFOR
  • C25B1/00—Electrolytic production of inorganic compounds or non-metals
  • C25B1/01—Products
  • C25B1/34—Simultaneous production of alkali metal hydroxides and chlorine, oxyacids or salts of chlorine, e.g. by chlor-alkali electrolysis
  • C25B1/46—Simultaneous production of alkali metal hydroxides and chlorine, oxyacids or salts of chlorine, e.g. by chlor-alkali electrolysis in diaphragm cells

Definitions

• ABSTRACT 1 alkali cell consisting essentially of a cell enclosure
• anode having an electrically active surface on an electrically conductive substrate metal, and a formaminous metal cathode, the anode and cathode being separated by porous diaphragm containing asbestos wherein the brine solution has been acidified to a pH of less than 2 and continuing the passage of the acidified brine into the cell at least until the hydrogen content of the chlorine produced at the anode is less than 0.5 percent by weight.
• the improved process results not only in purer chlorine product, but also higher current efficiencies and maintainance of the desired head of anolyte liquor of more readily accomplished.
• This invention relates to improvements in the production of alkali metal hydroxide and elemental chlorine in diaphragm type chlor-alkali cells equipped with anodes having an electrically active surface on a electrically conductive substrate metal. It is known that chlorine, and aqueous alkali metal hydroxide, can be produced readily by electrolysis of alkali metal chloride brine in a diaphragm type cell. Such cells consist essentially of a cell enclosure andan anode of a chlorine resistant electro conductive material such as platinum, platinum coated titanium or the like, or graphite and a foraminous cathode usually made of iron within the enclosure.
• the anolyte compartment and the cathode compartment are separated by means of a porous diaphragm usually of asbestos or like material.
• Diaphragm type chlor-alkali cells equipped with graphite anodes do not, in general, exhibit such prob lems of back migration of caustic alkali and hydrogen. Such cells usually operate at an anolyte pH within the pH range of about 3 to about 4. On start-up using a new graphite anode, anolyte pH values of less than 3 have been observed. However, using normal brine feed rates and brine feed having a pH of about 6.5 the anolyte pH quickly increases to within the desired operating range of between about 3 to about 4.
• an improved process for the production of alkali metal hydroxides and elemental chlorine comprises passing a substantially saturated sodium chloride brine solution through a diaphragm type cell consisting essentially of a cell enclosure, an anode having an electrically active surface on an electrically conductive substrate metal, and a cathode of a foraminous metal, the anodeand the cathode being separated by a porous diaphragm containing. asbestos, wherein the brine solution has been acidified to a pH of less than 2 and continuing the passage of the acidified brine. solution into the cell until the hydrogen content of the chlorine produced. at'the anode is less than about 0.5 percent by weight.
• the excess brine solution is withdrawn from the anolyte compartment, the withdrawn solution is replenished with an additional amount of sodium chloride and the pH of the resultant solution is adjusted to within the range of 2 to 4 prior to being recycled back into the cell.
• the diaphragm type chlor-alkali cells useful in the present invention are those equipped with anodes which present an electrically active surface on an electrically conductive substrate material.
• substrate metal it is intended to encompass those metals and metal alloys which become passivated when polarized anodically and remain passive beyond the anodic potential needed to convert a chloride ion to chlorine.
• the phenomenon of passivity in this connection is discussed in an article by Green appearing in the Apr, 1962 issure of Corrosion National Association of Corrosion Engineers, pages l36t to 142! wherein reference may be made to FIG. 1 which describes a typicallyac ⁇ tive-passive transition of a metal toward a corrosive medium.
• the metal substrate employed in the electrodes applicable in this invention will not pass into the transpassive range until a potential is reached which is considerably higher than that needed to produce chlorine from the chloride ion. Hence, the substrate metal remains passive during the operation of the electrolytic cell.
• Illustrative of the substrate metals in a generic sense are the valve metals (with the exclusion of certain metals which obviously are inapplicable such as aluminum, zirconium, and the like). Titanium, tantalum or niobium are acceptable substrate metals.
• the titanium employed is normally of a commercially pure grade of titanium of intermediate strength.
• Alloys of titanium may be employed as long as the alloy meets the criterion of acidity set forth in the above, for example, titanium alloys of aluminum, vanadium, paladium, chromium or tin may be employed in which the latter metals are present as less than about percent of the alloy.
• the surface of the substrate metal is made active by various methods.
• a conductor such as a noble metal (preferably platinum) may be desposited on the surface of the substrate metal by methods known in the art. Mixturesof other noble metals and platinum may be used to activate the surface of the metal substrate.
• the preferred surface metal mixture or alloy is one containing more than about 50 percent platinum.
• noble metal oxides may be used alone or in combination with the noble metals to form the active electrode surface.
• noble metal it is intended to include the platinum and palladium triads of the periodic table with the exclusion of osmium.
• ruthenium, rhodium, palladium, iridium and platinum represent noble metals which are especially applicable in their metallic form, alloys thereof and as oxides.
• the titanium substrate used the commercially pure grade of intermediate strength or a titanium alloy of aluminum, vanadium, palladium, chromium, or tin in which about 90 percent or more of the alloy is titanium.
• the platinumtitanium or noble metal oxide-titanium electrodes are acceptable as well as the platinum or noble metal oxide surfaced titanium or titanium clad copper electrodes wherein the titanium or tantalum is applied to the copper core by mechanical coating or with electrically conductive adhesive materials.
• the anodes may be assembled within the diaphragm type chlor-alkali cell in any manner known to the art.
• the anode current conductor connections may be isolated from the corrosive contents of the electrolytic cell by bituminous materials such as mastic or synthetic resin sealants.
• one typical anode assembly is that disclosed by M. P. Grotheer in U.S. Pat. No. 3,563,878, issued Feb. 16, 1971, wherein an anode assembly is disclosed which is applicable to monopolar and bipolar chlor-alkali cell operation.
• the anode assembly provided therein is a unitary electrode assembly which involves a metallic (preferably steel) base plate or backer plate to which spacer bars of an electrically conductive material such as platinized-titanium, aluminum alloys and preferably copper is attached by welding or tinning to the steel at predetermined intervals based upon the desired pitch of the anodes.
• spacer bar is constructed from platinized titanium, the use of sealants may be dispensed with as protective means against attack by the corrosive materials which contact it.
• the spacer bar is disposed in such a manner that the attached anodes will be aligned with abutting edges vertically situated within the cell unit.
• the spacer bar contains holes through which pass the bolts running parallel to the base plate.
• the holes through the spacer bars are preferably slotted, at an angle downwardly exsure bars depends upon the designed height of the cell.
• anodes are horizontally attached to the spacer bar in a vertically disposed bank of anodes, or the cell width where the anodes are vertically attached to the spacer bar in a bank extending across the cell.
• the pressure bars act, in conjunction with the bolt running through them, the anode and spacer bar, as an electrode clamping device.
• the electrical resistance through the anode-spacer bar contact is a function of the pressure developed at the contacting surfaces.
• the resistance developed through the clamped connection of anode and spacer bar may be controlled by regulating the pressure applied by the clamping bolts. Consideration must also be given to the thermal expansion of the spacer bar during operation of the cell in which temperatures above C., are common.
• the bolts may be of a suitable metal or metal alloy to compensate for the expansion of the spacer bars and pressure bars.
• the pressure bars may be made of any suitable material such as steel.
• any corrosion resistant sealant known to the art may be placed over the connecting members between each electrode.
• natural or synthetic rubbers may be employed by themselves, in combination or in conjunction with other resins.
• Bituminous materials may be employed if desired and the phenolformaldehyde resins and polyester resins are acceptable sealants.
• Especially good sealants may be derived from the reaction of a polyhydric alcohol with a Diels- Alder adduct of hexahalocyclopentadiene and an alpha, beta unsaturated dicarboxylic acid, such as are disclosedin U.S. Pat. No. 3,216,884.
• the sealants employed in this invention may be advantageously highly filled with such materials as sand, Si0, graphite particles, or other inert materials.
• the electrolytic cells contemplated by this invention are those conventionally used in the electrolysis of sodium chloride solutions.
• the electrolytic cell comprises a cell top, a cell bottom, sidewalls, an anode compartment and a cathode compartment separated by a porous diaphragm which may be of deposited asbestos.
• the brine is fed into the anode compartment from which it flows through the diaphragm into the cathode compartment.
• Chlorine and hydrogen are withdrawn from the anode and cathode compartments, respectively.
• the cell liquor containing sodium hydroxide, sodium chloride and other impurities is withdrawn from the cathode compartment.
• a saturated brine containing from about 250 to about 320 grams per liter of sodium chloride is adjusted to a pH below about 2 and preferably below about 1.5 and especially between about 1.2 and about 1.3 is fed to a conventional chlor-alkali cell which consists essentially of a cell enclosure, an anode of a chlorine resistant electro conductive material, and a foraminous cathode having attached thereto a diaphragm of asbestos or like material.
• the pH adjustment of the brine feed is preferably carried out with hydrochloric acid.
• the brine feed is adjusted through the cell under head of about 3 to 30 inches of saturated brine and preferably from about 3 to 18 inches.
• the electrolytic cell may be efficiently operatedwithin the temperature range of about 80 centigrade up to the boiling point of the brine (which depends upon the brine concentration).
• the anode current density of the operating electrolytic cell lyte was decreased to about 2 and maintained for about hours by the addition of aqueous hydrochloric acid.
• the pH increased to about 3.7.
• the anolyte head increased slightly to about 3.2 inches but quickly leveled off to about 3 inches for the balance of the run.
• the hydrogen content of the chlorine was originally 1 .0 percent and after the period of acid addition varied'between about 0.4 and 0.8 percent throughout the dura-' tion of the run.
• an initial head in the anolyte compartment of II- is preferably greater than 0.8 amperes per square inch.
• the electrolysis be operated at least in the initial stages with the highly acidified brine.
• the pH of the brine may be gradually increased during the electrolysis to the normal levels, i.e., pH about 4 either by following the hydrogen content of the chlorine gas produced at the anode orv by monitoring the head of the liquor in the anolyte compartment.
• the pH of the circulating brine may be increased to normal level e.g., about 4.
• EXPERIMENT l A conventional diaphragm type chlor-alkali cell equipped with platinum coated titanium anode, a steel cathode having deposited thereon an asbestos diaphragm was charged with brine containing about 300 grams per liter (gpl) of sodium chloride at about 98 centigrade, to a head of about four inches in the anolyte compartment.
• the current load was maintained at 95 KA and the caustic strength of the catholyte was maintained between 145 and 150 gpl Na0I-I by controlling the brine feed rate to the anolyte compartment.
• the pH of the anolyte liquor during the first three days of operation varied between 3.7 and 4.0 and the head of anolyte liquor varied between about 3.25 and 4.5 inches.
• the pH of the anolyte liquor was reduced to 1.2 by the addition of aqueous hydrochloric acid for about 24 hours.
• the head of anolyte liquor increased within one day to 9 inches and remained constant for the duration of the run at that level.
• the electrolysis was initiated with a current load of 85 KA, which after one day of operation was increased to 90 KA.
• the pH of the anolyte liquor varied between 4.1 and 4.4 during the first 9 days of the run.
• the head of anolyte liquor was initially 3 inches and dropped within 24 hours to about 1 inch.
• the head varied between about I and 3 inches during the first 9 days of cell operation.
• On the ninth day the pH of the anoinches.
• the current load was initially 53 KA and was gradually increasedto 60 KA after 7 days, to KA on the eighth dayand to KA on the ninth day.
• the cell was operated at 80 KA forthe balance of the run'.
• the caustic strength of the catholyte was maintained at -95 gpl Na0H for the firstday and at to l55 gpl:
• N a0H on the second through ninth day then permitted to rise as high as gpl NaOI-I on the final, twelfth day.
• the pH of the anolyte was adjusted to L3 by theaddition of aqueous hydrochloric acid to the brine feedat the start-up of the electrolysis and continued for about 20 hours.
• the pH of the anolyte increased to 4.4 after 24 hours after start-up and varied between 4.3 and"4.”8 thereafter.
• the head of the anolyte liquor increased rapidly to 29 inches after about 20 hours and varied between about 18 and 28 inches throughout the run. After cessation of the acid addition, the head decreased from a maximum of 29 inches (20 hours) to 18 inches (4.5 days) and then increased to 28 inches (8 days), varying thereafter between about 24 and 28 inches.
• the hydro: gen content of the chlorine was about one percent at the beginning of the run but fell to about 0.6 percent" on the first day and from the second 'day to the comple'; tion of the run, varied within the range of 0.1 to 0.4 percent.

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• Chemical & Material Sciences (AREA)
• Inorganic Chemistry (AREA)
• Engineering & Computer Science (AREA)
• Chemical Kinetics & Catalysis (AREA)
• Electrochemistry (AREA)
• Materials Engineering (AREA)
• Metallurgy (AREA)
• Organic Chemistry (AREA)
• Electrolytic Production Of Non-Metals, Compounds, Apparatuses Therefor (AREA)
• Electrodes For Compound Or Non-Metal Manufacture (AREA)

Applications Claiming Priority (1)

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Cited By (3)

Citations (6)

• 0
  • BE BE786660D patent/BE786660A/xx unknown
• 1971
  • 1971-07-30 US US00167804A patent/US3755103A/en not_active Expired - Lifetime
• 1972
  • 1972-06-20 CA CA145,261A patent/CA1007194A/en not_active Expired
  • 1972-07-03 AU AU44148/72A patent/AU469834B2/en not_active Expired
  • 1972-07-12 GB GB3258172A patent/GB1351431A/en not_active Expired
  • 1972-07-17 DE DE2235027A patent/DE2235027A1/de active Pending
  • 1972-07-25 FR FR7226718A patent/FR2148024B1/fr not_active Expired
  • 1972-07-25 NL NL7210211A patent/NL7210211A/xx unknown
  • 1972-07-26 IT IT27439/72A patent/IT963381B/it active
  • 1972-07-31 BR BR5126/72A patent/BR7205126D0/pt unknown

Patent Citations (6)

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