Classifications

• • C—CHEMISTRY; METALLURGY
  • C09—DYES; PAINTS; POLISHES; NATURAL RESINS; ADHESIVES; COMPOSITIONS NOT OTHERWISE PROVIDED FOR; APPLICATIONS OF MATERIALS NOT OTHERWISE PROVIDED FOR
  • C09K—MATERIALS FOR MISCELLANEOUS APPLICATIONS, NOT PROVIDED FOR ELSEWHERE
  • C09K15/00—Anti-oxidant compositions; Compositions inhibiting chemical change
  • C09K15/02—Anti-oxidant compositions; Compositions inhibiting chemical change containing inorganic compounds
• • A—HUMAN NECESSITIES
  • A61—MEDICAL OR VETERINARY SCIENCE; HYGIENE
  • A61K—PREPARATIONS FOR MEDICAL, DENTAL OR TOILETRY PURPOSES
  • A61K47/00—Medicinal preparations characterised by the non-active ingredients used, e.g. carriers or inert additives; Targeting or modifying agents chemically bound to the active ingredient
  • A61K47/02—Inorganic compounds

Definitions

• the present invention provides a method of controlling the oxidation of chemicals during storage using a noble gas, a mixture of noble gases or a gaseous mixture containing at least one noble gas. Description of the Background;
• French Patent 1,339,669 discloses that argon may be used to render oxidizable chemicals of biological origin inert to oxidation because it desorbs oxygen.
• this patent specifically states that oxygen must be removed for any inhibitory effect upon oxidation to be observed.
• U.S. 3,143,471 a method is described whereby dry argon is used in the packaging of lyophilized pharmaceuticals, generally, wherein the sole object of the process is the displacement of water and oxygen from the packaging space.
• inert or non-reactive atmospheres which can be either nitrogen or argon are recommended for packaging or storaging chemicals or chemical preparations such as oils (JP 3200568), polyacrylic acids (U.S. 4,622,425), N,N-dialkylaminopropyl compounds (JP 63077848), alpha-cyano-acrylic ester (JP 52097913, 85007609), vinylidene halide compounds (U.S. 3,957,892), sodium products (FR 2,261,518), chemical propellants (DE 3,007,712), medical solutions (U.S. 4,664,256), silicon wafers (U.S.
• HEET CH 589403 AT 7505161, DE 2,437,812, IT 1040412, JP 51035583, JP 83040521
• developer sheets JP 3057689, U.S. 5,064,070
• photosensitive donor media U.S. 4,965,165
• agricultural antiseptic suspensions JP 2104502
• preparation or synthesis of chemicals under generally inert atmospheres in which the use of either nitrogen or argon without distinction is recommended include, as examples, purification and stabilization of catechol-containing proteins (U.S. 4,496,397), preparation of cosmetic dyes (U.S. 4,314,810), synthesis of peptides (FR 1,454,653, AU 6565762), synthesis of antibiotics (JP 58039650, JP 89039416).
• an object of the present invention to provide a method for enhancing the stability of chemicals or chemical preparations during storage thereof.
• a method of controlling the oxidation of chemicals or chemical preparations during at least a portion of storage thereof by contacting the same with a noble gas, a mixture of noble gases or a gaseous mixture containing at least one noble gas.
• Figure 2 illustrates the absorptivity of Quercetin under different atmospheres of oxygen, nitrogen, argon, krypton and xenon at 25°C.
• Figure 3 illustrates the absorptivity of Quercetin under different atmospheres of oxygen, nitrogen, argon, neon and air at 25°C.
• Figure 4 illustrates the absorptivity of morphine sulfate under different atmospheres of oxygen, nitrogen and argon after 31 days of storage at ambient temperature.
• Figure 5 illustrates the absorptivity of apomorphine hydrochloride under different atmospheres of oxygen, nitrogen and argon after 31 days of storage at ambient temperature.
• Figure 6 illustrates the absorptivity of apomorphine hydrochloride under different atmospheres of oxygen, nitrogen and argon after 31 days of storage at ambient temperature.
• Figure 7 illustrates the absorptivity of apomorphine hydrochloride under different atmospheres of nitrogen and argon after 31 days at ambient temperature.
• Figure 8 illustrates the absorptivity of epinephrine hydrochloride under different atmospheres of nitrogen, argon, krypton and xenon after 31 days at ambient temperature.
• Figure 9 illustrates the absorptivity of epinephrine hydrochloride under different atmospheres of nitrogen and xenon for 31 days and three and one-half months, respectively, for each.
• Figure 10 illustrates the absorptivity of L-ascorbic acid under different atmospheres of oxygen and nitrogen.
• HEET Figure 11 illustrates the absorptivity of L-ascorbic acid under different atmospheres of nitrogen, argon, krypton, xenon and neon after 30 days at ambient temperature.
• Figure 12 illustrates the absorptivity of retinol under different atmospheres of nitrogen, argon, krypton and xenon after 3 months at ambient temperature in darkness.
• Figure 13 illustrates the absorptivity of tetracycline hydrochloride under different atmospheres of air and nitrogen for 33 days and four months each, respectively.
• Figure 14 illustrates the absorptivity of tetracycline hydrochloride under different atmospheres of air and neon for 33 days and four months each, respectively.
• the present invention it has been surprisingly discovered that it is possible to directly affect the rate of oxidation of chemicals or chemical preparations. That is, in accordance with the present invention it has been discovered that certain gases can directly affect the oxidation rate of chemicals and not merely slow oxidation only as function of physical and inert displacement of oxygen.
• the present invention is effected by contacting the chemicals or chemical preparations during at least a portion of storage thereof to a noble gas, a mixture of noble gases or a gaseous mixture containing at least one noble gas.
• the present invention is predicated upon the discovery that by contacting chemicals or chemical preparations with an atmosphere containing a noble gas, a mixture of noble or a gaseous mixture containing at least one noble gas during at least a portion of storage it is possible to effectively control oxidation reactions which degrade such compounds or preparations.
• noble gases are surprisingly more effective than nitrogen or other inert or non-reactive gases in actually and effectively controlling the oxidation of chemical compounds or chemical preparations.
• the present invention is predicated upon a, heretofore, undiscovered property of noble gases in interfering with oxidation reactions of chemicals and chemical preparations during storage.
• a method is also provided for inhibiting oxidation of chemicals or chemical preparations. Further, the present invention may be advantageously used at any time during storage of chemicals or chemical preparations.
• noble gases possess a surprising ability to control, and specifically inhibit oxidation to a degree quite superior to that exhibited by nitrogen.
• the use of noble gases instead of nitrogen confers additional stability to stored chemical products or chemical preparations.
• the term "noble gas” generally includes argon, xenon, krypton or neon. While other noble gases, such as radon or helium may be used, the use of radon is generally impractical as it is dangerously reactive. While helium confers a positive benefit, and less than the other noble gases, and may be freely admixed with any other noble gas to advantage, its use is limited by its poor solubility in aqueous solutions and its tendency to dissipate by penetrating packaging materials. However, it is reiterated that the present invention is predicated upon the surprising discovery of the ability of all of the noble gases to control the oxidation of chemicals or chemical preparations.
• atmospheres containing noble gases in quantities greater than those normally found in ambient air significantly improve storage characteristics and shelf-life of chemicals or chemical preparations. Further, the effective improvement is of wide practical utility and clear economic benefit.
• any amount of noble gas above that found in normal atmospheric air may be used to advantage in the present invention.
• argon is generally accepted as being present in the atmosphere in the amount of about 0.934% by volume.
• neon, krypton and xenon are normally present in the atmosphere in amounts of 1.82 X 10 ⁇ 3 , 1.14 X 10" 3 and 8.7 X 10 ⁇ 6 , respectively, by % volume.
• Advanced Inorganic Chemistry , Cotton and Wilkinson (Third Edition, Wiley).
• any amount of noble gas may be used which is greater than that found in atmospheric air.
• this amount is preferably at least 1% by volume, and is more preferably in excess of 1% by volume for argon.
• krypton and xenon amounts generally used are at least 0.05% each, by volume. However, it is generally preferred that the amounts of neon, krypton and xenon used be greater than about 0.1% each, by volume.
• any gas, mixtures of gases, liquid or mixtures of liquids may be used in accordance with the present invention as long as they contain an amount of at least one noble gas as described above. Preferably, however, they contain at least the preferred amounts noted above.
• -lo ⁇ in addition to noble gases or noble gas mixtures, any gaseous mixture may be used in accordance with the present invention which contains at least one noble gas.
• unpurified mixtures of gases from air separation plants such as about 90;10 Kr;Xe, and about 1:1 He:Ne, for example.
• atmospheric pressures of from less than one to greater than 1 may be used.
• it has been found acceptable to use quite low pressures such as those near vacuum conditions, such as, for example about 10 ⁇ 9 torr to very high pressures of about 100 atm or greater.
• atmospheres ranging from about 0.5 to 20 atm, preferably about from 1 to 10 atm.
• the effective stabilization is observed even when the noble gas-containing atmosphere contains other inert gases, such as nitrogen.
• the effect appears to be directly related to the actual quantitative amount of noble gas present and available to the reactive sites on the subject chemical or chemical preparation.
• the effect thereof is observed even when the noble gas- containing atmosphere contains other reactive gases including oxygen, carbon dioxide, water, or nitrous oxide.
• diminution of the antioxidative effect is seen in direct consequence of the inclusion of these oxygen-containing gases, and is a direct, linear function of their concentration.
• the maximum antioxidative effect of argon is seen when argon is present as 100% of the superimposed atmosphere (and effectiveness may be increased by increasing the relative molar concentration of argon by increasing pressure)
• the minimal effect is observed when argon is present in concentrations only slightly greater than its normal concentration in air (0.1% by volume) admixed with any of oxygen, carbon dioxide, water or nitrous oxide.
• the method is most effective when noble gas concentrations in excess of 50% of the atmosphere are used, preferably in excess of 90%, preferably in excess of 95% of the atmosphere.
• the improvement of the present invention is generally noted for noble gas-containing atmospheres which might also contain other gases, except that reactive components of these other gases may promote oxidation and mask the desired effect.
• reactive components of these other gases may promote oxidation and mask the desired effect.
• complex mixtures of gases which include noble gases will promote oxidation less than similar mixtures which do not contain noble gases.
• the antioxidation potential of the noble gases is of the order of:
• the observed effectiveness of the noble gases is partially, but not wholly dependent, upon their relative solubility in the chemicals or chemical preparations treated.
• the observed effectiveness of the noble gases is partially, but not wholly dependent, upon their relative ability to desorb oxygen or water from subject chemical preparations.
• the effects of the noble gases may be either ameliorated or potentiated by the admixture of other gases thereto.
• the observed improvement in accordance with the present invention is notable for noble-containing solutions, either aqueous or non-aqueous, when applied to retard oxidation, in a manner similar to the use of atmospheres.
• the optimal method consists of saturating the solution with the desired gas by sparging or superimposition or by use of pressure or through introduction of cryogenic liquid.
• cryogenic liquid composed of or containing noble gases, such as cryogenic argon
• cryogenic nitrogen inert
• carbon dioxide reactive
• the quantative improvement in sh ⁇ lf-life may be observed is several times that observed with nitrogen, with the improvement being 25 to 100% being obtained with ease.
• the preferred method of use of the present invention is to store the chemicals or chemical preparations under an atmosphere containing a noble gas, mixture of noble gases or gaseous mixture containing at least one noble gas which gases exhibit the best effect, and additionally storing in gas- and moisture-impermeable containers, storing at low temperatures and storing in containers which block incident light or other radiation.
• any chemical or chemical preparation which is susceptible to oxidative degradation may be protected by the present invention.
• such chemicals or preparations may include chemical reagents, deoxygenated solvents, reducing agents and catalysts.
• storage temperatures of from about -20°C to about 60°C, preferably from about -10°C to about 30°C, may be used.
• the progress of the oxidations were monitored either by ultraviolet/visible spectrophoto etry, or by spectrocolorimetry, or by direct visual observation, or by the production of a detectable product (detected chemically, or by gas chromatography/mass spectrometry, or by thin layer chromatography) , or by other standard means, depending upon the nature of the chemical oxidation to be measured.
• the atmospheres tested include argon, xenon, krypton, neon, helium, nitrogen, oxygen, air, carbon dioxide, nitrous oxide, and decile mixtures of each possible pair and triad, and certain representative other combinations. Tests were conducted in the presence or absence of water vapor, light, temperature, and under differing conditions of concentration and pH. In certain cases, atmospheres were changed after a certain time period in order to observe changing effects. For instance, it was observed in every case of noble gas retardation of oxidation that replacing the noble gas-containing atmosphere with air or oxygen immediately produced the maximum degenerative effect, and that replacing the effective noble gas-containing atmosphere with nitrogen immediately ended the observed retardation effect.
• nitrous oxide, carbon dioxide, air and oxygen produced degenerative oxidative effects, nitrogen diminished these effects to the extent that oxygen was excluded from the reaction, and the noble gases diminished the effect further. This further effect was evident even when oxygen was added in amounts greater than could be accounted for by the different desorptive ability of the various noble gases and nitrogen, and in amounts greater than could be accounted for by different solubilities of the gases in solution.
• Vitamin Bl Specific Examples: Example 1: Quercetin
• the 2 vials are stored at room temperature over the week-end (unprotected from light) .
• Vial C/0 2 (see 09/13/91 QUERC01.WP) has turned orange, while vial C/N 2 is still yellow. No further color changes are observed on the following days. 2. Full Range Scans (900-190 nm) : 09/16/91
• Purge cuvet 1 with 0 2 on-line for 30 s.
• Purge cuvet 2 with N 2 on-line for 30 s.
• Blank cuvet acrylic cuvet filled with 3 ml D.I. H 2 0. Using a 3cc syringe previously purged with 0 , transfer 3 ml from vial C/0 2 into cuvet 1.
• Blank cuvet acrylic cuvet filled with 2.5 ml of TRIS buffer pH 9.0.
• Label and stopper 5 acrylic cuvets with blue silicone (gas-tight) .
• Label QT4Gn, where:
• the gassing order is still: N 2 , Ar, Kr, Xe and finally 0 2 .
• Blank cuvet acrylic cuvet filled with 2.5 ml of TRIS buffer pH 9.0.
• the 100 ⁇ g/ml quercetin solution is stored in refrigerator (serum vial being wrapped in aluminum foil to prevent light degradation) .
• Blank cuvet acrylic cuvet filled with 2.5 ml of TRIS buffer pH 9.0.
• Stopper 1 acrylic cuvet with blue silicone (gas- tight) . Flush cuvet with on-line nitrogen for 1 min. Using a 3cc B-D syringe (purged with N 2 ) , transfer 2.5 ml of solution C into the cuvet. Run a full range scan (900-190 nm) of sample cuvet vs blank.
• Bubble 3x3Occ of the appropriate gas through each vial Inject an additional lOcc of the appropriate gas to leave vial under positive pressure.
• Gassing is done in the following order: N , Ne, Ar, Kr, Xe, Air, and finally 0 2 .
• the lOcc vials are left on the lab bench at room temperature.
• the vials are regularly observed visually for color changes.
• Blank cuvet acrylic cuvet filled with 2.5 ml of TRIS buffer pH 9.0.
• Figure 1 shows that following ABS at 400 nm will reveal the progressive oxidation of the molecule.
• Figure 2 shows that nitrogen retards oxidation poorly compared to argon, and krypton and xenon inhibit oxidation much better than argon.
• Figure 3 shows a replicate (differences between Figs. 2 and 3 are due to different start times) which shows additionally that neon inhibits about as well as argon. Since the solubilities of argon and neon are very different yet that of neon and nitrogen very similar, the activity is clearly at least partly independent of solubility.
• Figure 9 demonstrates the same for nitrogen and xenon in comparing degree of oxidation after 1 month versus 3 1/2 months of storage.
• Example 5 L-Ascorbic acid
• Figure 10 shows the oxidative abscissal absorbance shift.
• Figure 11 shows that preservation is in the order Kr>Ar>Ne>N 2 >Xe after 30 days.
• Figure 12 shows the very great improvement obtained in storing retinol under noble gases compared with nitrogen.
• diminution of absorbance in the 320-324 nm range is indicative of oxidation.
• Figure 13 compares oxidation over this time period in an oxygen atmosphere versus a nitrogen atmosphere. Comparing Figure 13 with Figure 14 demonstrates clearly that a neon atmosphere provides greater protection.
• the present invention is surprisingly effective in controlling oxidation of chemicals or chemical preparations or both in storage.
• binary mixtures such as argon-krypton, krypton-neon, xenon-krypton or argon-neon, for example, ternary mixtures or even quaternary mixtures of noble gases may be used.
• deoxygenated air generally means an oxygen content of less than about 15%, better yet less than about 10%, and more preferably less than about 5% by volume.
• the gases or gas mixture may be introduced either in gaseous or liquid form. If liquid form, the noble gases may be used neat or dissolved in a suitable liquid gas such as liquid nitrogen.
• the advantage of the present invention may be obtained even if the chemicals or chemical preparations are contacted with the gases of the present invention for only a portion of the storage period. However, it is generally preferably to effect such contact throughout the entire storage period.

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• 1993
  • 1993-03-31 CA CA002102779A patent/CA2102779A1/en not_active Abandoned
  • 1993-03-31 WO PCT/EP1993/000802 patent/WO1993020168A1/en not_active Application Discontinuation
  • 1993-03-31 JP JP5517101A patent/JPH06507940A/ja active Pending
  • 1993-03-31 EP EP93908878A patent/EP0596059A1/de not_active Withdrawn
  • 1993-03-31 AU AU39504/93A patent/AU3950493A/en not_active Abandoned
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