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WO2002030947A2 - Compositions et procedes pour preparer des chelates et des complexes d'acide amine - Google Patents

Compositions et procedes pour preparer des chelates et des complexes d'acide amine Download PDF

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Publication number
WO2002030947A2
WO2002030947A2 PCT/US2001/031757 US0131757W WO0230947A2 WO 2002030947 A2 WO2002030947 A2 WO 2002030947A2 US 0131757 W US0131757 W US 0131757W WO 0230947 A2 WO0230947 A2 WO 0230947A2
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Prior art keywords
amino acid
metal
sulfate
reaction
ligand
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WO2002030947A3 (fr
Inventor
H. Dewayne Ashmead
Stephen D. Ashmead
David C. Wheelwright
Clayton Ericson
Mark Pedersen
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Albion Laboratories Inc
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Albion International Inc
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Priority claimed from US09/686,413 external-priority patent/US6426424B1/en
Priority claimed from US09/686,047 external-priority patent/US6518240B1/en
Priority claimed from US09/686,683 external-priority patent/US6710079B1/en
Application filed by Albion International Inc filed Critical Albion International Inc
Priority to AU2002213105A priority Critical patent/AU2002213105A1/en
Publication of WO2002030947A2 publication Critical patent/WO2002030947A2/fr
Publication of WO2002030947A3 publication Critical patent/WO2002030947A3/fr
Anticipated expiration legal-status Critical
Ceased legal-status Critical Current

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    • C—CHEMISTRY; METALLURGY
    • C07—ORGANIC CHEMISTRY
    • C07D—HETEROCYCLIC COMPOUNDS
    • C07D233/00—Heterocyclic compounds containing 1,3-diazole or hydrogenated 1,3-diazole rings, not condensed with other rings
    • C07D233/54—Heterocyclic compounds containing 1,3-diazole or hydrogenated 1,3-diazole rings, not condensed with other rings having two double bonds between ring members or between ring members and non-ring members
    • C07D233/64—Heterocyclic compounds containing 1,3-diazole or hydrogenated 1,3-diazole rings, not condensed with other rings having two double bonds between ring members or between ring members and non-ring members with substituted hydrocarbon radicals attached to ring carbon atoms, e.g. histidine
    • C—CHEMISTRY; METALLURGY
    • C07—ORGANIC CHEMISTRY
    • C07C—ACYCLIC OR CARBOCYCLIC COMPOUNDS
    • C07C227/00—Preparation of compounds containing amino and carboxyl groups bound to the same carbon skeleton
    • C07C227/14—Preparation of compounds containing amino and carboxyl groups bound to the same carbon skeleton from compounds containing already amino and carboxyl groups or derivatives thereof
    • C07C227/16—Preparation of compounds containing amino and carboxyl groups bound to the same carbon skeleton from compounds containing already amino and carboxyl groups or derivatives thereof by reactions not involving the amino or carboxyl groups
    • C—CHEMISTRY; METALLURGY
    • C07—ORGANIC CHEMISTRY
    • C07C—ACYCLIC OR CARBOCYCLIC COMPOUNDS
    • C07C319/00—Preparation of thiols, sulfides, hydropolysulfides or polysulfides
    • C07C319/14—Preparation of thiols, sulfides, hydropolysulfides or polysulfides of sulfides
    • C07C319/20—Preparation of thiols, sulfides, hydropolysulfides or polysulfides of sulfides by reactions not involving the formation of sulfide groups

Definitions

  • the present invention is drawn to compositions and methods of preparing --mino acid chelates. More particularly, the present invention is drawn to compositions and methods of preparing arnino acid chelates without the use of added water.
  • a chelate is a definite structure resulting from precise requirements of synthesis. Proper conditions must be present for chelation to take place including proper mole ratios of ligands to metal ions, pH, and solubility of reactants. As such, traditional "wet" methods of preparing chelates have typically been used to prepare chelates. These methods include the step of dissolving raw materials in solution to ionize the solution or create an appropriate electronic configuration in order for bonding to develop. Though wet methods have typically been used to make chelates, chelates and/or complexes have also been made under dry conditions.
  • IR infrared spectrometer analysis
  • metal proteinate The American Association of Feed Control officials (AAFCO) has defined a “metal proteinate” as the product resulting from the chelation of a soluble salt with amino acids and/or partially hydrolyzed proteins. Such products are referred to as the specific metal proteinate, e.g., copper proteinate, zinc proteinate, etc. This definition does not contain any requirements to assure that chelation is actually present. On the basis of the chemical reactant possibilities, there are some real reservations as to the probability of chelation occurring to any great degree.
  • partially hydrolyzed proteins as suitable ligands and the term "and/or" in reference to such ligands implies that products made solely from partially hydrolyzed protein and soluble salts would have the same biochemical and physiological properties as products made from combining amino acids and soluble metal salts. Such an assertion is chemically incorrect.
  • Partially hydrolyzed protein ligands may have molecular weights in the range of thousands of daltons and any bonding between such ligands and a metal ion may be nothing more than a complex or some form of ionic attraction, i.e., the metal drawn in close proximity to carboxyl moiety of such a ligand.
  • the second product when properly formed, is a stable product having one or more five-membered rings formed by reaction between the carboxyl oxygen, and the ⁇ -amino group of an ⁇ -amino acid with the metal ion.
  • a five-membered ring is defined by the metal atom, the carboxyl oxygen, the carbonyl carbon, the ⁇ -carbon and the a--imino nitrogen.
  • the actual structure will depend upon the ligand to metal mole ratio.
  • the ligand to metal mole ratio is at least 1 : 1 and is preferably 2: 1 but, in certain instances, may be 3: 1 or even 4: 1.
  • an amino acid chelate may be represented at a ligand to metal ratio of 2: 1 according to Formula 1 as follows:
  • the dashed lines represent coordinate covalent bonds, covalent bonds, or ionic bonds.
  • the solid lines between the ⁇ -amino group and the metal (M) are covalent or coordinate covalent bonds.
  • R is H
  • the amino acid is glycine which is the simplest of the ⁇ -amino acids.
  • R could be representative of any other of the other twenty or so naturally occurring amino acids derived from proteins. These all have the same configuration for the positioning of the carboxyl oxygen and the ⁇ ---mino nitrogen.
  • the chelate ring is defined by the same atoms in each instance.
  • AAFCO American Association of Feed Control Officials
  • one bond is formed from the carboxyl oxygen and the other bond is formed by the ⁇ ---mino nitrogen which contributes both of the electrons used in the bonding. These electrons fill available spaces in the d-orbitals.
  • This type of bond is known as a dative bond or a coordinate covalent bond and is common in chelation.
  • a metal ion with a normal valency of +2 can be bonded by four bonds when fully chelated.
  • the divalent metal ion the chelate is completely satisfied by the bonding electrons and the charge on the metal atom (as well as on the overall molecule) is zero. This neutrality contributes to the bioavailability of metal amino acid chelates.
  • peptide ligands will usually be in the form of dipeptides, tripeptides and sometimes tetrapeptides because larger ligands have molecular weights that are too great for direct assimilation of the chelate formed.
  • peptide ligands will be derived by the hydrolysis of protein.
  • peptides prepared by conventional synthetic techniques or genetic engineering can also be used.
  • a radical of the formula [C(O)CHRNH] e H will replace one of the hydrogens attached to the nitrogen atom in Formula 1.
  • R as defined in Formula 1, can be H, or the residue of any other naturally occurring amino acid and e can be an integer of 1 , 2 or 3.
  • e is 1 the ligand will be a dipeptide, when e is 2 the ligand will be a tripeptide and so forth.
  • amino acid chelates have generally been made by first dissolving a water soluble metal salt in water. An amino acid ligand is then reacted with the metal ion at a ligand to metal molar ratio of about 1 : 1 to 4: 1. Often, the ligand is a hydrolysis product obtained by acid, base, base-acid, base-acid-base, or enzyme hydrolysis. In such cases, the by products from hydrolysis, such as anions including chlorides, sulfates, phosphates and nitrates, and cations, including potassium and sodium remain in the hydrolysate. Reaction products of metal salts with proteins or with acid and/or base hydrolyzed proteins are taught in U.S. Pat. Nos. 2,960,406; 3,396,104; 3,463,858; 3,775,132; 4,020,158; 4,103,003, 4,172,072, the entire teachings of which are incorporated by reference.
  • amino acid chelates may be prepared in a manner that is simple wherein the product produced is stable, granular, dense, dry, and free flowing. Further, the introduction of metal acid salts into solution, such as copper sulfate, resulted in the creation of copper ions which compete with the hydrogen ion for the lone pair of electrons on the NH 2 group.
  • compositions and methods can be prepared using particulate amino acids blended with particulate hydrated metal sulfate salts.
  • the blend can then be placed in an enclosed (preferably substantially sealed) environment and heated under low to moderate temperatures for a time sufficient that the waters of hydration from the hydrated metal sulfate salt are released and provide the moisture necessary to effect a bonding reaction between the electron rich functional groups of the amino acid ligand with the metal ion of the sulfate salt, thereby forming amino acid chelates and complexes.
  • the particulate amino acids and particulate hydrated metal sulfate salts can be blended with certain reaction modifiers (prior to substantially sealing and heating as described previously) in order to form amino acid chelates and complexes with increased granularity, denseness, and free flowing properties than other amino acid chelates prepared under similar reaction conditions without the presence of the reaction modifiers.
  • compositions and methods of preparing -imino acid chelates and complexes essentially free of interfering complex ions can also comprise the steps of a) combining as a particulate blend i) a hydrated metal sulfate salt having one or more waters of hydration, ii) an amino acid ligand, and iii) calcium oxide or hydroxide, at a ratio sufficient to allow substantially all of the particulates to react forming a metal amino acid chelate, calcium sulfate, residual water, and optionally, a hydroxide complex ion, and wherein the metal amino acid chelate has a ligand to metal molar ratio from about 1 : 1 to 3 : 1 ; b) placing the particulate blend in an enclosed environment; and c) applying heat to the particulate blend in the enclosed environment causing the waters of hydration of the hydrated metal sulfate salt to be released into the enclosed environment thereby causing a reaction resulting in the formation of
  • “Hydrated metal sulfate salt,” “metal sulfate hydrate,” or “metal sulfate salt having waters of hydration” include any metal sulfate salt that has one or more waters of hydration capable of being released during the reactions of the present invention.
  • metal and “mineral” may be used interchangeably, and can include any nutritionally relevant metal.
  • metal or “mineral” can include all metals that are generally more soluble as sulfate salts than calcium sulfate.
  • calcium is a metal, for purposes of only those embodiments where amino acid chelates free of interfering ions are formed, calcium is excluded within this definition unless the context clearly dictates otherwise.
  • “Nutritionally relevant metals” include metals that are known to be needed by living organisms, particularly plants and mammals, including humans. Metals such as calcium, copper, zinc, iron, cobalt, magnesium, manganese, chromium, among others are exemplary of nutritionally relevant metals.
  • Hydrophilicity or "n-hydrate” is meant to include any degree of hydration attached to the metal sulfate salts where n is an integer representing the number of waters of hydration, e.g., monohydrate, dihydrate, trihydrate, tetrahydrate, pentahydrate, hexahydrate, septahydrate, octahydrate, nonahydrate, etc.
  • n is an integer of about 1 to 15.
  • amino acid chelates and complexes is meant to include metal ions bonded to amino acid ligands forming one or more heterocyclic ring.
  • the bonds may be coordinate covalent, covalent, and/or ionic at the carboxyl oxygen group. However, at the ⁇ -amino group, the bond is typically a covalent or coordinate covalent bond. In some embodiments, other constituents can be bonded to the amino acid chelates and complexes.
  • Electrode neutral refers to amino acid chelates wherein the positively charged metal ion is fully satisfied by a negative charge on the ligand attachment by bond formation, e.g., divalent metals fo ⁇ ning 2: 1 ligand to metal molar ratio amino acid chelates, or trivalent metals foraiing 3: 1 ligand to metal molar ratio amino acid chelates.
  • Complex ion or “interfering complex ion” is meant to include any cation or anion that typically remains in a final composition as a charged group that can interfere with the formation of the chelate and/or remains in the composition to charge balance a charged amino acid chelate. Though hydroxide complex ions are charged, they are not considered to be interfering in the context of certain embodiments of the present invention.
  • Hydroxide complex ion includes hydroxide groups that form in certain embodiments of the present invention, i.e., divalent metal amino acid chelates having a 1: 1 ligand to metal molar ratio, or trivalent metal amino acid chelates having a 2: 1 ligand to metal molar ratio.
  • these arnino acid chelates are sufficiently formed as a result of liberated waters of hydration, the hydroxide complex ions will likely ionically complex with the positively charged amino acid chelates in embodiments where the amino acid chelates formed are not electrically neutral.
  • hydroxide complex ions are not considered to be interfering.
  • Enclosed chamber or “enclosed environment” shall include any system or container that is capable of being substantially sealed or closed such that the waters of hydration released from a hydrate are substantially retained, thereby providing moisture to drive any reaction within the system or container.
  • reaction modifier or “inert reaction modifier” includes any modifier that may be added to the core reactants, i.e., the amino acid ligand and the hydrated sulfate salt, to improve the physical properties of the product.
  • Preferred reaction modifiers include starches, partially hydrolyzed starches, celluloses, partially hydrolyzed celluloses, and combinations thereof. Examples of sources for the reaction modifier include rice flour, corn starch, potato starch, microcrystalline cellulose, powdered cellulose, maltodextrin, and modified food starch.
  • Methods of preparing amino acid chelates and complexes can comprise the steps of blending and heating an amino acid ligand with a hydrated metal sulfate salt in an enclosed environment, resulting in the amino acid chelates and complexes.
  • these compositions can be prepared according to the following steps: (a) combining a hydrated metal sulfate salt and an amino acid ligand to form a particulate blend, wherein the ligand to metal molar ratio is from about 1: 1 to 4: 1; (b) placing the particulate blend in an enclosed environment; and (c) applying heat to the particulate blend in the enclosed environment causing the waters of hydration of the metal sulfate salt to be released into the enclosed environment.
  • This causes a reaction resulting in the formation of an amino acid chelate or complex by effecting the reaction between functional electron rich groups of the amino acid ligand and a metal ion of the metal sulfate salt.
  • the waters of hydration serve to provide the water necessary to enable a bonding reaction to take place between the electron rich functional groups of the amino acid ligand and the metal ion of the hydrated metal sulfate salt.
  • This process results in particulate amino acid chelates and complexes that are stable, granular, dense, dry and/or free flowing, though in some instances, the product must be further ground prior to packaging or using the chelate for its intended purpose.
  • the preferred embodiment of the invention does not include the addition of water, some additional water may be added to effectuate desired results, e.g., copper sulfate monohydrate may not have enough waters of hydration to progress a reaction to substantial completion. Therefore, water may optionally be added in very small amounts to assist specific reactions. If water is added, the water should preferably not be added such that there is a substantial excess after the reaction has progressed to substantial completion. For example, if zinc monohydrate was used as a reactant instead of zinc pentahydrate in a formulation where zinc pentahydrate would likely drive the reaction closer to completion, 4 molar equivalents of water could be added to the blend prior to enclosing the reactants to simulate the effect of adding zinc pentahydrate. In most circumstances and in accordance with this aspect of the present invention, from about 1 to 15 molar equivalents of water can be added.
  • the step of enclosing the particulate blend is important because the waters of hydration must not be allowed to substantially evaporate during the reaction. This is because the waters of hydration are necessary to drive the reaction between the ligand and the metal ion of the hydrated metal sulfate salt. Therefore, a virtually or substantially sealed environment is preferred, though an enclosure that prevents substantial contact between the reaction blend and the atmosphere will also provide desired results.
  • the enclosed chamber may be a device such as a calorimeter, a plastic lined container, a tank, a blender, a kettle, a sealed drum, or a plastic bag capable of being enclosed or even sealed.
  • other enclosed chambers, environments, or systems are within the scope of the invention.
  • time and temperature variables should be considered when dete ⁇ r-ining whether the reaction has been driven to a desired product.
  • a typical temperature range is from about 50°C to 100°C, though temperatures outside of this range may be used.
  • the particulate blend in the enclosed chamber may be heated to from 60°C to 80°C for from 2 to 4 hours. After, heating the particulate blend, the resulting product should be allowed to cool to room temperature. In other embodiments, heating may be for periods of about 15 minutes at temperatures from about 75°C to 85°C.
  • the heating time and temperature as well as the cooling time and temperature will depend largely upon which metal salts, ligands, ratios, batch sizes, and other variables are selected. In other words, the reaction time may be very short or may require multiple days for optimal results, depending on the embodiment.
  • the hydrated metal sulfate salt In order for the reaction to be driven forward, the hydrated metal sulfate salt must have at least one water molecule available for release to catalyze the reaction. Thus, anhydrous forms of metal sulfate salts may not be used unless they are used in conjunction with another hydrated metal sulfate salt. However, if for example, a metal sulfate monohydrate is used, the reaction will not advance as far as other, more hydrated, metal salts. Conversely, hydrated metal sulfate salts such as a metal sulfate pentahydrate or heptahydrate (or even higher) are preferred compounds because of the number of water molecules available for liberation during the reaction. For example, ferrous sulfate heptahydrate is one of many ideal salts to utilize as will be exemplified below.
  • the ligands of the present invention are generally -imino acids
  • the naturally occurring -imino acids including alanine, arginine, asparagine, aspartic acid, cysteine, cystine, glutamine, glutamic acid, glycine, histidine, hydroxyproline, isoleucine, leucine, lysine, methionine, ornithine, phenylalanine, proline, serine, threonine, tryptophan, tyrosine, valine, and combinations thereof are preferred.
  • ligands including dipeptides, tripeptides, and tetrapeptides formed by any combination of the aforementioned -imino acids may be used.
  • ligand and/or hydrated metal sulfate salt is in something other than powder form, e.g. larger crystals, etc.
  • an additional step of substantially grinding the raw materials into powder is preferred.
  • large hydrated metal sulfate salts and ligands should be ground in to a maximum particle size of 80 mesh, preferably from 20 to 80 mesh.
  • the product may be ground into an appropriate size.
  • Amino acid chelates and complexes of the present invention have many possible applications. First, they may be used as plant foliars and foods. Either the product could be dissolved for use oh leaves, etc., or used directly as a soil treatment. Second, the product could be dry blended in combination with other metal salts and/or a variety of ligands for more unique applications. These chelates and complexes could also be used in animal feeds by methods currently known in the art. In fact, some processes may create products that could be used in food applications, in pharmaceuticals, and/or nutritional supplements for warmblooded animals, including humans.
  • -imino acid chelates and complexes can be prepared having improved physical properties by adding certain reaction modifiers to the particulate blend prior to the heating step.
  • the addition of reaction modifiers can improve the physical properties of the product.
  • the physical properties that are improved by the present invention include increased particle size, more uniform particle size, increased product density, and/or increased compressibility in the manufacture of solid dosage forms. Additionally, the formation of amorphous masses of product is minimized, thereby drastically reducing or eliminating a grinding step.
  • compositions and methods of preparing amino acid chelates and complexes by blending and heating an amino acid ligand with a hydrated metal sulfate salt in an enclosed environment is disclosed and described.
  • a method of preparing amino acid chelates and complexes comprises the steps of (a) combining a metal sulfate salt having waters of hydration, an amino acid ligand, and a reaction modifier to form a particulate blend, wherein the ligand to metal molar ratio is from about 1 : 1 to 4: 1 ; (b) confining the particulate blend in an enclosed environment; and (c) applying heat to the particulate blend in the enclosed environment causing the waters of hydration of the hydrated metal sulfate salt to be released into the enclosed environment such that the amino acid chelates and complexes formed are granular and have a desirable particle size and density.
  • the waters of hydration serve to provide the water necessary to enable a bonding reaction to take place between the electron rich functional groups of the amino acid ligand and the metal ion of the hydrated metal sulfate salt.
  • the particulate blend should be allowed to react for a sufficient amount of time to drive the waters of hydration from the hydrated sulfate salt into the enclosed environment, thereby causing the formation of an amino acid chelate or complex by effecting the reaction between functional electron rich groups of the ligands and the metal ion of the metal sulfate salt. This process results in particulate -imino acid chelates and complexes that are more stable, granular, dense, dry, and/or free flowing than those described in the prior art.
  • the reaction modifiers that enhance the physical properties of the compositions and methods of the present invention include any combination of starches, partially hydrolyzed starches, particulate cellulose, and/or modified cellulose. These modifiers may be provided from any know source or in any known form, such as from rice flour, corn starch, potato starch, microcrystalline cellulose, powdered cellulose, maltodextrin, modified food starches, and combinations thereof.
  • the amount of any one or combination of the above reaction modifiers required to enhance the physical properties of the product can range from 1-30% of the weight of the product. However, preferred ranges are from about 15-25%.
  • the preferred combination should include a source of starch.
  • the starch acts to gelatinize and absorb any excess water released from the reaction of the hydrated soluble sulfate salt(s) and the amino acid(s).
  • the absorptive qualities of the reaction modifier aids in the granulation effect of the process.
  • the material produced by this process is easier to handle because the product flows from the reaction vessel more continuously rather than forming an amorphous mass that must be mechanically ground (often after drying) to a suitable particle size before packaging.
  • the addition of the reaction modifiers to the process results in a product that has a particle size range of about 16-80 mesh, with only a few oversized particles.
  • the density of the product produced by the present invention increases from about 0.5-0.7 gm/cc (via methods disclosed in T8044 and T8407) to about 0.75-0.95 gm/cc (via methods disclosed in the present invention). Further, in the presence of the reaction modifiers, clumping of the granules is minimized. Further, while cooling, the reaction continues to progress slowly until a dry granule product forms that is stable, dense, and free flowing. The reaction time may be very short or may require multiple days, depending on the embodiment.
  • compositions and methods of preparing amino acid chelates and complexes essentially free of interfering complex ions can comprise the steps of (a) combining as a particulate blend i) a hydrated metal sulfate salt having one or more waters of hydration, ii) an -imino acid ligand, and iii) calcium oxide or hydroxide, at a ratio sufficient to allow substantially all of the particulates to react fo ⁇ r-ing a metal amino acid chelate, calcium sulfate, water, and optionally, a hydroxide complex ion, and wherein the metal amino acid chelate has a ligand to metal molar ratio from about 1: 1 to 3: 1; (b) placing the particulate blend in an enclosed environment; and (c) applying heat to the particulate blend in the enclosed environment causing the waters of hydration of the hydrated metal sulfate salt to be released into the enclosed
  • the particulate blend must be heated for a time and at a temperature sufficient to at least begin to drive the waters of hydration from the hydrated salt into the enclosed environment, though the reaction may continue to occur after the heat has been removed.
  • This process results in particulate amino acid chelates and complexes that are stable, granular, dense, dry, and/or free flowing, though in some instances, the product must be further ground prior to packaging or using the chelates for their intended purpose.
  • calcium sulfate, and in some embodiments, hydroxide counter-ions or hydroxide complex ions, and/or water are produced. Many of the same reaction conditions and ingredients can be used with the present embodiment.
  • the same hydrated sulfate salts, reaction conditions, and equipment can be used with the present embodiment, as has been set forth previously.
  • the present embodiment requires the use of a calcium hydroxide or oxide and a hydrated metal sulfate salt such that calcium sulfate precipitates and a metal amino acid is formed.
  • the amino acid chelate produced is not only free of interfering complex ions, but may also be electrically neutral.
  • ferrous iron (Fe 2+ ) is used to prepare amino acid chelates having a ligand to metal molar ratio of about 2: 1, the final product will be free of interfering complex ions and will be electrically neutral.
  • H(AA) is an amino acid selected from the group consisting of naturally occurring amino acids and combinations thereof.
  • H when disassociated from AA, is a hydrogen ion donor from the carboxyl group present on the amino acid.
  • M is a nutritionally relevant metal having a valency of +2 such as Cu, Zn, Fe, Co, Mg, and/or Mn, and n is an integer from about 1 to 15 that is indicative of the waters of hydration of the metal sulfate.
  • Formulas 4a and 4b illustrate the production an electrically neutral composition comprised of calcium sulfate and amino acid chelates having a 3: 1 ligand to metal molar ratio: 3Ca(OH) 2 + 6H(AA) + M' 2 (SO 4 ) 3 «nH 2 O — >
  • H(AA) is an amino acid selected from the group consisting of naturally occurring amino acids and combinations thereof.
  • H when disassociated from AA, is a hydrogen ion donor from the carboxyl group present on the arr-ino acid.
  • M' is a nutritionally relevant metal having a valence of +3 such as Fe(III) and/or Cr, and n is an integer from about 1 to 15.
  • H(AA) is an amino acid selected from the group consisting of naturally occurring amino acids and combinations thereof.
  • H when disassociated from AA, is a hydrogen ion donor from the carboxyl group present on the -imino acid.
  • M is a nutritionally relevant metal having a valency of +2 such as Cu, Zn, Fe, Co, Mg, and/or Mn, and n is an integer from about 1 to 15 that is indicative of the waters of hydration of the metal sulfate.
  • Formulas 6a and 6b illustrate the production non-electrically neutral compositions free of interfering complex ions comprised of calcium sulfate, hydroxide complex ions, and -imino acid chelates having a 2: 1 ligand to metal molar ratio:
  • H(AA) is an amino acid selected from the group consisting of naturally occurring -imino acids and combinations thereof.
  • H when disassociated from AA, is a hydrogen ion donor from the carboxyl group present on the amino acid.
  • M' is a nutritionally relevant metal having a valence of +3 such as Fe(III) and/or Cr, and n is an integer from about 1 to 15 that is indicative of the waters of hydration of the metal sulfate.
  • compositions and methods of the present embodiment always produce amino acid chelates that are free of interfering anions and also produced calcium sulfate which is largely insoluble and essentially inert.
  • the calcium sulfate preferably can remain in the compound as a stabilizer or for other purposes.
  • compositions and methods of preparing the amino acid chelates and complexes of the present invention illustrate compositions and methods of preparing the amino acid chelates and complexes of the present invention.
  • the following examples should not be considered as limitations of the present invention, but should merely teach how to make the best known amino acid chelates and complexes based upon current experimental data.
  • Glycine and ferrous sulfate heptahydrate were screened through an 80 mesh screen and dry blended together for 15 minutes at a ligand to metal molar ratio of about 1: 1.
  • the blend was sealed in a plastic lined barrel and placed in an oven at 70°C for 4 to 12 hours. The barrels were then removed from the oven and allowed to remain at room temperature for 4 to 7 days.
  • the product produced was stable, granular, dense, dry, and free flowing.
  • the resulting ferrous complex product contained about 18% iron and 24% moisture by weight.
  • Glycine and ferrous sulfate heptahydrate were screened to about 80 mesh and dry blended together at a ligand to metal molar ratio of about 2: 1. Once thoroughly admixed, the blend was sealed in a plastic lined barrel and placed in an oven for 4 to 12 hours at 70°C. The barrels were then removed from the oven and allowed to cool to room temperature where they remained for 4 to 7 days.
  • the ferrous chelate product formed contained about 14% iron and 19% moisture by weight.
  • Example 3 Glycine and copper sulfate pentahydrate were screened through an 80 mesh screen and ground together in a dry blend at a ligand to metal molar ratio of about 1: 1.
  • the dry blend was placed in a sealed plastic bag and was oven dried at 70°C for about an hour.
  • the glycine and the copper sulfate pentahydrate began to react.
  • the blend was allowed to cool to room temperature and the sealed plastic bag was allowed to stand for one week.
  • a dry, stable, granular, and free-flowing product ranging from 30 to 60 mesh was formed.
  • the resulting copper complex product contained about 22% copper and 18% moisture by weight.
  • Glycine and manganese sulfate pentahydrate were screened through an 80 mesh screen and dry blended for 15 minutes at a ligand to metal molar ratio of about 1:1.
  • the dry blend was sealed in a plastic bag and oven dried at 70°C for 4 to 12 hours. Once removed from the oven, the blend was allowed to remain in the sealed bag at room temperature for about 7 days.
  • the product formed was granular, crystalline, and stable.
  • a manganese complex product containing about 17% manganese and 28% moisture by weight remained.
  • Glycine and manganese sulfate pentahydrate were screened through an 80 mesh screen and ground together for 15 minutes at a ligand to metal molar ratio of about 2: 1.
  • the dry blend was sealed in a plastic bag and oven dried for 4 to 12 hours at 70°C. After oven drying, the blend was allowed to cool to room temperature (while remaining in the sealed bag) where it remained for 7 days.
  • the resulting manganese chelate complex product contained about 13% manganese and 23% moisture by weight.
  • Example 7 Glycine and ferrous sulfate heptahydrate were screened to 80 mesh and dry blended together for 15 minutes at a ligand to metal molar ratio of about 2:1. The dry blend was then added to a sealed bomb calorimeter. The calorimeter was then submersed in a water bath maintained at 70°C. After about 15 minutes, the contents of the calorimeter reached 70°C and began to be exothermic. The 70°C water from the water bath was replaced by cool tap water to maintain the reaction at a temperature range between 75°C to 85°C. When the temperature of the calorimeter dropped below 70°C, the reaction neared completion. The calorimeter containing the reaction blend was then removed from the water and allowed to return to room temperature overnight. The calorimeter was then opened and the contents were allowed to stand overnight. The resulting ferrous chelated complex product contained about 11.5% iron and 4.9% moisture by weight.
  • the reaction was near completion.
  • the calorimeter containing the reacted blend was then removed from the water, allowed to return to room temperature, opened, and allowed to stand overnight.
  • the resulting mixed metal chelate product contained about 10.1% zinc, 8.5% manganese, and 4.8% moisture by weight.
  • One mole of magnesium sulfate nonahydrate powder, one mole of glycine powder, and one mole of L-methionine powder were screened through an 80 mesh screen and ground together for about 15 minutes. This procedure formed a dry blend having a ligand to metal molar ratio of about 2: 1.
  • the blend was then added to a sealed bomb calorimeter and submersed in a water bath maintained at 70°C. After about 15 minutes, the contents of the calorimeter reached 70°C and began to be exothermic. To maintain a temperature range within the calorimeter of between 75°C to 85°C, the 70°C water was replaced by cool tap water. When the temperature of the calorimeter dropped below 70°C, the reaction appeared to be near completion. The calorimeter containing the reaction blend was then removed from the cool tap water and allowed to return to room temperature. After one night at room temperature, the resulting manganese mixed ligand chelate complex product contained about 6.7% magnesium and 5.5% moisture by weight.
  • One mole of zinc sulfate pentahydrate powder, one mole of manganese sulfate pentahydrate powder, one mole of copper sulfate pentahydrate powder, two moles of glycine powder, two moles of L-lysine powder, and two moles of L- histidine powder were screened to 80 mesh dry blended together for 15 minutes.
  • the blend contained a ligand to metal molar ratio of about 2: 1.
  • the blend was then placed in a sealed bomb calorimeter which was submersed in a warm water bath of about 70°C. Once the contents of the calorimeter reached 70°C, the product began to be exothermic.
  • the warm water was replaced by cool water to maintain the reaction at a temperature range of between 75°C to 85°C.
  • the temperature of the calorimeter dropped below 70°C indicating that the reaction was near completion.
  • the calorimeter was then removed from the water and allowed to return to room temperature, opened, and allowed to stand overnight.
  • the resulting mixed metal mixed ligand chelate complex product contained about 4.7% zinc, 3.9% manganese, 4.5% copper, and 5.0%> moisture by weight.
  • Example 12 Glycine and ferric sulfate hydrate were screened through an 80 mesh screen and dry blended together for 15 minutes at a ligand to metal molar ratio of about 3: 1. Next, the blend was sealed in a plastic lined barrel and placed in an oven at 70°C for 4 to 12 hours. The barrels were then removed from the oven and allowed to remain at room temperature for 4 to 7 days. The ferric chelate complex product produced was stable, granular, dense, dry, and free flowing. The resulting product contained about 12% iron and 9% moisture by weight.
  • Glycine and chromium potassium sulfate dodecahydrate were screened through an 80 mesh screen and ground together in a dry blend at a ligand to metal molar ratio of about 3: 1.
  • the dry blend was placed in a sealed plastic bag and was oven dried at 70°C for one hour. As a result, the glycine and the copper sulfate pentahydrate began to react. Once removed from the oven, the blend was allowed to remain at room temperature for one week while remaining sealed in the bag.
  • the resulting chromium chelate complex product contained about 8% chromium, 6% potassium, and 26% moisture by weight.
  • ferrous sulfate heptahydrate powder One mole of ferrous sulfate heptahydrate powder, two moles of glycine powder, and 20%o by weight of rice flour (90%o starch content) were dry blended and placed in a bomb calorimeter. The calorimeter was submersed in a water bath maintained at about 70°C for about 90 minutes. The calorimeter was removed from the water bath and allowed to cool to room temperature. The calorimeter was then opened and the product was allowed to stand overnight. A ferrous glycine chelate complex was formed having ligand to metal molar ratio of about
  • the particle size of the product was then analyzed on a Ro-Tap screen shaker fitted with 16, 20, 40, 60, 80, and 100 mesh screens. About 16%> of the product did not pass through a 20 mesh screen, 49% of the product was between 20-60 mesh, and 35%> of the product passed through a 60 mesh screen. The bulk density of a 20-80 mesh cut of the product measured about 0.95 gm/cc.
  • a manganese glycine chelate complex was also formed having ligand to metal molar ratio of about 2: 1 and a manganese content of about 5.3% by weight.
  • the particle size of the product was then analyzed on a Ro-Tap screen shaker fitted with 16, 20, 40, 60, 80, and 100 mesh screens. About 25%) of the product did not pass through a 20 mesh screen, 56% of the product was between 20-60 mesh, and 19% of the product passed through a 60 mesh screen.
  • the bulk density of a 20-80 mesh cut of the product measured about 0.87 gm/cc.
  • Example 17 One mole of magnesium sulfate nonahydrate powder, one mole of glycine powder, one mole of L-methionine powder, 10%> by weight of potato starch, and 10% powdered cellulose were dry blended and placed in a bomb calorimeter. The calorimeter was submersed in a water bath maintained at about 70°C for about 90 minutes. The calorimeter was removed from the water bath and allowed to cool to room temperature. The calorimeter was then opened and the product was allowed to stand overnight.
  • magnesium amino acid chelate complexes i.e., glycine and methionine ligands
  • glycine and methionine ligands were formed having ligand to metal molar ratio of about 2: 1 and an magnesium content of about 4.5%o by weight.
  • the particle size of the product was then analyzed on a Ro-Tap screen shaker fitted with 16, 20, 40, 60, 80, and 100 mesh screens. About 22% of the product did not pass through a 20 mesh screen, 51% of the product was between 20-60 mesh, and 21% of the product passed through a 60 mesh screen.
  • the bulk density of a 20-80 mesh cut of the product measured about 0.81 gm/cc.
  • Zinc amino acid chelates, manganese amino acid chelates, and copper amino acid chelates having a ligand to metal molar ratio of about 2: 1 were produced having ligand combinations of glycine, lysine, and histidine.
  • the zinc content was about 3.3% by weight
  • the manganese content was about 2.8% by weight
  • the copper content was about 3.2% by weight.
  • the particle size of the product was then analyzed on a Ro-Tap screen shaker fitted with 16, 20, 40, 60, 80, and 100 mesh screens. About 15%> of the product did not pass through a 20 mesh screen, 62% of the product was between 20-60 mesh, and 23% of the product passed through a 60 mesh screen.
  • the bulk density of a 20-80 mesh cut of the product measured about 0.90 gm/cc.
  • One mole of copper sulfate pentahydrate, one mole of glycine, 10%> by weight maltodextrin, 10 % by weight rice flour (90% starch content) were dry blended and placed in a bomb calorimeter.
  • the calorimeter was immersed in a water bath maintained ate about 70°C for about 90 minutes.
  • the calorimeter was removed from the water bath and allowed to cool to room temperature.
  • the calorimeter was then opened and the product was allowed to stand overnight.
  • a granular copper glycine chelate complex was formed having a ligand to metal molar ratio of about 1 : 1 and a copper content of about 16%> by weight.
  • the reaction produced about one mole of a 1 : 1 iron glycine chelate hydroxide ion complex and about one mole of calcium sulfate. By weight, the product contained about 19.9% iron and 5.5%> moisture.
  • the contents of the calorimeter began to be exothermic.
  • the warm water in the bath was replaced by cool tap water.
  • the calorimeter was removed from the cool water bath and allowed to adjust to room temperature. The calorimeter was then opened and the product was allowed to sit overnight.
  • the reaction produced about one mole of a 1: 1 copper L-lysine chelate hydroxide ion complex and about one mole of calcium sulfate.
  • the product produced contained about 17.2% copper and 5.2%> moisture by weight.
  • the calorimeter was opened and the product was allowed to stand overnight.
  • the reaction produced about one half mole of a 1 : 1 magnesium glycine chelate hydroxide ion complex, about one half mole of a 1:1 magnesium L- methionine chelate hydroxide ion complex, and about one mole of calcium sulfate.
  • the product contained about 8.4%> magnesium and 5.5% moisture.
  • Example 25 One mole of zinc sulfate pentahydrate powder, one mole of manganese sulfate pentahydrate powder, one mole of copper sulfate pentahydrate powder, one mole of glycine powder, one mole of L-lysine powder, one mole of L-histidine powder, and three moles of calcium oxide were dry blended and placed in a bomb calorimeter. The calorimeter was heated in a warm water bath which was maintained at about 70°C. After 15 minutes, the contents of the calorimeter began to be exothermic and the warm water in the bath was then replaced by cool tap water so that the contents would remain at from about 75°C to 85°C. Once the reaction mixture dropped below 70°C, the reaction was near completion and the calorimeter was removed from to cool bath. After the contents had cooled to room temperature, the calorimeter was opened the product was allowed to stand overnight.
  • the reaction produced about three moles of -imino acid chelate hydroxide ion complexes having a 1: 1 ligand to metal molar ratio. All combinations were present, i.e., all combinations of zinc, manganese, and copper chelated to glycine, L-lysine, and L-histidine. The reaction also produced about three moles of calcium sulfate. By weight, the product contained about 6.4%) zinc, 5.4%> manganese, 6.2% copper, and 5.1%> moisture.
  • Example 26 One mole of ferrous sulfate heptahydrate powder, one mole of glycine powder, and one mole of calcium hydroxide powder were dry blended and placed in a bomb calorimeter. The calorimeter was then submersed in a warm water bath that was maintained at about 70°C. After a few minutes, the contents of the calorimeter began to be exothermic. The warm water in the bath was then replaced by cool tap water. Though cool water was present in the bath, the temperature of the reactants in the calorimeter remained within a temperature range from about 75°C to 85°C. Once the reaction mixture dropped below 70°C, the reaction neared completion. The contents of the calorimeter were allowed to cool to room temperature.
  • the calorimeter was opened and the product was allowed to stand overnight.
  • the reaction produced about one mole of a 1 : 1 iron glycine chelate hydroxide ion complex and about one mole of calcium sulfate. By weight, the product contained about 18.5% iron and 5.98% moisture.
  • Example 27 One mole of ferrous sulfate heptahydrate powder, two moles of glycine powder, and one mole of calcium oxide powder were dry blended and placed in a bomb calorimeter. The calorimeter was then submersed in a warm water bath maintained at about 70°C. When the contents of the calorimeter began to be exothermic, the warm water in the bath was then replaced by cool tap water so that the temperature range could be maintained between about 75°C to 85°C. At a point near completion of the reaction, the temperature of the reaction mixture dropped below 70°C and the cool water was removed. The contents of the calorimeter were then allowed to cool to room temperature prior to opening of the calorimeter. The product was allowed to stand overnight. About one mole ferrous bisglycinate and about one mole of calcium sulfate was formed. By weight, the product contained about 15.5% iron and 5.1%> moisture.
  • Example 28 One mole of copper sulfate pentahydrate powder, two moles of L-lysine powder, and one mole of calcium oxide were dry blended and placed in a bomb calorimeter which was subsequently submersed in a 70°C warm water bath. The contents of the calorimeter began to be exothermic after about 15 minutes. The warm water in the bath was then replaced by cool tap water. Though cool water was present in the bath, the temperature of the reactants in the calorimeter remained in the temperature range from about 75°C to 85°C. Once the temperature of the reaction mixture dropped below 70°C, the calorimeter was removed from the cool water where the contents were allowed to cool to room temperature. At this point, the calorimeter was opened and the product was allowed to stand overnight. The reaction produced about one mole of copper bisglycinate and about one mole of calcium sulfate. The product contained about 12.09%> copper and 5.8% moisture by weight.
  • Example 29 One mole of zinc sulfate pentahydrate powder, one mole of manganese sulfate pentahydrate powder, four moles of glycine powder, and two moles of calcium oxide were dry blended and placed in a bomb calorimeter. The calorimeter was then submersed in a warm water bath that was maintained at about 70°C. After 15 minutes, the contents of the calorimeter began to be exothermic. The warm water in the bath was then replaced by cool tap water.
  • the temperature of the reactants in the calorimeter remained in the temperature range from about 75°C to 85°C. Once the temperature of the reaction mixture dropped below 70°C, the reaction neared completion. The contents of the calorimeter were allowed to cool to room temperature. The calorimeter was then opened and the product was allowed to stand overnight.
  • the reaction produced about one mole of zinc bisglycinate, about one mole of manganese bisglycinate, and about two moles of calcium sulfate. By weight, the product contained about 7.9%> zinc, 9.4% manganese, and 4.9% moisture.
  • One mole of magnesium sulfate nonahydrate powder, one mole of glycine powder, one mole of L-methionine powder, and one mole of calcium oxide were dry blended and placed in a bomb calorimeter. The calorimeter was then warmed and maintained at about 70°C in a water bath. Once the reactants became exothermic, the warm water in the bath was then replaced by cool water so that the reactants in the calorimeter remained in the temperature range from about 75°C to 85°C. Once the temperature of the reaction mixture dropped below 70°C, the calorimeter was removed from the water bath, the contents were allowed to cool to room temperature, the calorimeter was opened, and the product was allowed to stand overnight.
  • the reaction produced about one mole magnesium biglycinate, about one mole of magnesium bismethionate, and about one mole of calcium sulfate.
  • the product contained about 6.2%> magnesium and 5.3%> moisture by weight.
  • the reaction produced about one mole ferrous bisglycinate and about one mole of calcium sulfate. By weight, the product contained about 14%> iron and 10%) moisture.
  • the reaction produced about one mole of chromium bisglycinate hydroxide ion complex and about one and one half moles of calcium sulfate.
  • the product contained about 11.0% chromium and about 13% moisture by weight.
  • n-hydrate powder (where n can be a mixture of compounds having from about 1 to 15 waters of hydration)
  • glycine powder two moles of glycine powder
  • calcium hydroxide powder were dry blended and placed in a bomb calorimeter.
  • the calorimeter was then submersed in a warm water bath that was maintained at about 70°C. After a few minutes, the contents of the calorimeter began to be exothermic. The warm water in the bath was then replaced by cool tap water. Though cool water was present in the bath, the temperature of the reactants in the calorimeter remained in the temperature range from about 75°C to 85°C. Once the temperature of the reaction mixture dropped below 70°C, the reaction neared completion. The contents of the calorimeter were allowed to cool to room temperature. The calorimeter was then opened and the product was allowed to stand overnight.
  • the reaction produced about one mole of ferric bisglycinate hydroxide ion complex and one and one half moles of calcium sulfate. By weight, the product contained about 11% iron and 13% moisture.
  • the reaction produced about two moles of chromium trisglycinate and about three moles of calcium sulfate. By weight, the product contained about
  • the reaction produced about two moles of chromium trisglycinate and about three moles of calcium sulfate. By weight, the product contained about 10%) chromium and 9%> moisture.

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  • Organic Chemistry (AREA)
  • Chemical Kinetics & Catalysis (AREA)
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Abstract

L'invention concerne des compositions et des procédés permettant de préparer des chélatés et des complexes d'acide aminé sans addition d'eau. Dans certains modes de réalisation, les compositions préparées sont exemptes d'ions interférants, et sont éventuellement neutres sur le plan électrique. Plus particulièrement, de telles compositions peuvent être obtenues en suivant les étapes suivantes : mélanger un ligand d'acide aminé et un sel de sulfate de métal hydraté (et éventuellement de l'oxyde de calcium, de l'hydroxyde de calcium, et/ou des modificateurs de réaction) ; placer le mélange dans un environnement sensiblement fermé ; chauffer le mélange et faire réagir ledit mélange.
PCT/US2001/031757 2000-10-11 2001-10-10 Compositions et procedes pour preparer des chelates et des complexes d'acide amine Ceased WO2002030947A2 (fr)

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US09/686,047 US6518240B1 (en) 2000-10-11 2000-10-11 Composition and method for preparing amino acid chelates and complexes
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