# Patent

## Title
Use of metal chelates in human or animal feeding

## Abstract

The present invention relates to the use in human and animal nutrition (monogastric and polygastric animals) of known chelates of bivalent metal Mg, Ca, Mn, Co, Cu, Zn and Fe with methionine hydroxy analogue. The present invention further relates to a method for preparing new chelates with methionine hydroxy analogue, both in solid form with iron (II), vanadium (iV) and (V) and molybdenum (V) and (VI), and in liquid form in aqueous solution with iron (II) and (III) and chrome (III). Eventually, the present invention relates to the use of said new chelates, both in solid form with iron (II), vanadium (IV) and (V) and molybdenum (V) and (VI), and in liquid form in aqueous solution with iron (II) and (III) and chrome (III), in human and animal nutrition.

## Background
The present invention relates to the use in human and animal nutrition (monogastric and polygastric animals) of known chelates of bivalent metals Mg, Ca, Mn, Co, Cu, Zn and Fe with methionine hydroxy analogue. The present invention further relates to a method for preparing new chelates with methionine hydroxy analogue, both in solid form with iron (II), vanadium (IV) and (V) and molybdenum (V) and (VI), and in liquid form in aqueous solution with iron (II) and (III) and chrome (III). Eventually, the present invention relates to the use of said new chelates, both in solid form with iron (II), vanadium (IV) and (V) and molybdenum (V) and (VI), and in liquid form in aqueous solution with iron (II) and (III) and chrome (III), in human and animal nutrition.
It is known that a metal chelate is a compound originating from an organic molecule (such as an amino acid or a peptide chain or an alpha-keto acid or an alpha-hydroxy acid) and a metal ion through strong coordination bonds. Some known metal chelates are used in the field of human nutrition. Their use is due to the biological action performed by the metal element involved, as activator in several enzymatic reactions, and as regulator in various metabolic functions in all living organisms. The presence of a chelating molecule promotes the absorption, availability and use of the metal element since the latter is carried by the organic component in all areas of the organism. This results also in a strong reduction of losses of unused metals in dejections, and therefore in a significant economic saving and in an environmental advantage.
The general features that should characterize a highly bioavailable metal chelate are: (a) neutrality of complex (the positive charge of metal is balanced by the negative charge of ligands; (b) absence of negative counter-ions (chlorides, sulfates); (c) low molecular weight of complex (<1,500 Daltons); (d) well defined metal/chelating agent (bidentate) ratio, possibly ≦1:2.
Moreover, metal chelates should be obtained from simple and clean processes with high yields starting from raw materials that can be easily found. These features can be implemented by means of suitable ligands, which should be easy to deproton and have at least two donor atoms in such a position to carry out chelation. Examples of ligands are amino acids and other organic acids suitably functionalized.
As far as iron is concerned, its administration in chelated form is particularly efficient against anemia. Anemia is a pathologic status of blood due to the reduction of the number of red blood cells, to the decrease of the amount of hemoglobin or to both deficiencies. Iron is fundamental for hemoglobin since it is the center in which oxygen is fixed into heme. Classes of people who need a higher amount of iron are menstruated or pregnant women, children under two years of age, vegetarians, people suffering from hemorrhoids, people suffering from ulcers and eventually blood donors. Symptoms felt by an anemic person are weariness, a higher sensibility to cold, irritableness, loss of concentration and heart palpitations.
Furthermore, iron can protect from viral or bacterial infections since it promotes the stimulation of the immune system. In addition, iron promotes the metabolism of vitamins belonging to B group.
It is known that the lack of these vitamins can result in diseases such as dermatitis or even more serious diseases such as pellagra (due to the deficiency of vitamin B3). Iron intervenes in processes of synthesis of adrenaline and noradrenaline. Eventually, the lack of iron leads to a slow cicatrisation of wounds.
A first aim of the present invention is to suggest an integrator for administration in human nutrition. Said integrator is also administered to patients suffering from a deficiency of metal oligoelements such as: Mg, Ca, Mn, Co, Cu, Zn and Fe.
A second aim of the present invention is to suggest an integrator for agro-zootechnical nutrition to be administered to monogastric or polygastric animals. Said integrator is also administered to monogastric or polygastric animals needing an administration of metal oligoelements such as: Mg, Ca, Mn, Co, Cu, Zn and Fe with a higher bioavailability.
A third aim of the present invention is to suggest a method for preparing metal chelates with methionine hydroxy analogue or one of its salts, both in solid form with iron (II), vanadium (IV) and/or vanadium (V) and molybdenum (V) and/or molybdenum (VI), and in liquid form in aqueous solution with iron (II) and (III) and chrome (III), in which said metals are bonded to a bifunctional organic ligand with a strong coordination bond so as to form a stable metal chelate.
A further aim of the present invention is to suggest the use of said new chelates, both in solid form with iron (II), vanadium (IV) and/or vanadium (V) and molybdenum (V) and/or molybdenum (VI), and in liquid form in aqueous solution with iron (II) and (III) and chrome (III), for preparing metal integrators for human and animal nutrition.
In an embodiment of the present invention said first and second aim are achieved by suggesting the use of metal chelates [2:1] having the general formula (I):

(CH3SCH2CH2CH(OH)COO)2M.nH2O  (I)

in which the bifunctional chelating agent is 2-hydroxy-4-methylthiobutanoic acid, an alpha-hydroxy acid, known as “methionine hydroxy analogue” (MHA); M is a bivalent metal cation chosen from the group comprising: Co, Ca, Mg, Zn, Fe, Cu and Mn, and n is the number of water molecules; for preparing metal integrators for treating patients suffering from a deficiency of metal oligoelements or for administration in the agro-zootechnical field to monogastric or polygastric animals. In formula (I) there are zero to twelve water molecules, preferably zero to six. For instance, zero to four. 2-hydroxy-4-methylthiobutanoic acid builds with iron ion a chelate having a well defined stoichiometry, containing two molecules of chelating agent pro iron atom, in the same way as it builds chelates with bivalent metals Mg, Ca, Mn, Co, Cu and Zn.

The method for preparing metal chelates having formula (I) was described in international patent application PCT/IT99/00225, and consists in the direct reaction of MHA with the corresponding carbonates of bivalent metals Mg, Ca, Mn Co, Cu and Zn.
In an embodiment according to the present invention the Applicant has improved a method for preparing metal chelates having formula (I), which envisages the direct reaction of MHA and metals (II) oxides such as: Mg, Ca, Mn, Co, Cu, Zn and Fe.
In this new embodiment oxides of metals (II) are used instead of carbonates as described in application PCT/IT99/00225, and technical and operating conditions are unchanged with respect to those referred to in application PCT/IT99/00225, and therefore said operating conditions are regarded as contained in the present application.
Advantageously, the following are used: magnesium oxide mixed with magnesium carbonate or alternatively completely replacing magnesium carbonate, zinc oxide mixed with zinc carbonate or alternatively completely replacing zinc carbonate, and calcium oxide mixed with calcium carbonate or alternatively completely replacing calcium carbonate.
The Applicant has found it advantageous to use for human nutrition the following metal chelates:

    
    
        (CH3SCH2CH2CH(OH)COO)2Zn.2H2O
    
    


The two water molecules are not bonded to the metal.

    
    
        (CH3SCH2CH2CH(OH)COO)2Cu
    
    


It is an anhydrous complex without water molecules bonded to the metal.

    
    
        (CH3SCH2CH2CH(OH)COO)2Co.2H2O
    
    


The two water molecules are complexed.

    
    
        (CH3SCH2CH2CH(OH)COO)2Mn.2H2O
    
    


The two water molecules are complexed.

    
    
        (CH3SCH2CH2CH(OH)COO)2Ca.2H2O
    
    


The two water molecules are not bonded to the metal.

    
    
        (CH3SCH2CH2CH(OH)COO)2Mg.2H2O
    
    


The two water molecules are not bonded to the metal.
In another embodiment of the present invention said third aim is achieved by suggesting a method for preparing metal chelates with methionine hydroxy analogue or one of its salts, both in solid form with iron (II), vanadium (IV) and/or vanadium (V) and molybdenum (V) and/or molybdenum (VI), and in liquid form in aqueous solution with iron (II) and (III) and chrome (III).
In the case of vanadium and molybdenum the method for preparing their chelates consists in the reaction of their corresponding oxides with methionine hydroxy analogue.
Alternatively, in the case of vanadium and molybdenum the method for preparing their chelates consists in the reaction of their corresponding metal salts with methionine hydroxy analogue.
For instance, an amount of solid V2O5 or MoO3 is added with a solution of methionine hydroxy analogue at a high temperature and under stirring. A transparent solution and a solid precipitate of a vanadium or molybdenum chelate are obtained from the reaction.
In a preferred embodiment the Applicant has arranged in a receptacle vanadium oxide V2O5 and methionine hydroxy analogue MHA. Vanadium oxide and methionine hydroxy analogue are present in a molar ratio of 1:2 to 1:8, preferably 1:4 to 1:6 (Vanadium/MHA).
The receptacle is equipped with stirring means, heating means and means for reaction reflux. The reaction takes placed under mechanical stirring and under reflux for a time between 20 and 60 minutes, preferably 30 minutes. At the end of the reaction a dark green solution is obtained, from which after cooling a solid green precipitate is obtained. From the chemical and physical analysis of the precipitate the Applicant has found confirmation that it is a vanadium (IV) complex having formula VOL2, where L=deprotoned methionine hydroxy analogue.
During the reaction vanadium (V) oxide reduces to vanadium (IV).
In the case of iron (II) the method of preparation takes place by reaction of sodium salt (or an alkali metal or alkaline-earth metal salt) of MHA with ferrous sulfate (or any other soluble iron (II) salt) in water environment.
The molar ratio MHA/Iron (II) is of 2:1 for completing the reaction. Ferrous chelate precipitates from the reaction environment and is filtered and washed with water so as to eliminate soluble sodium sulfate which builds up.
After filtration and washing the chelated product is then dried so as to reduce the amount of absorbed water. The product is a pale yellow powder, little water soluble, having formula:

(CH3SCH2CH2CH(OH)COO)2Fe.2H2O.

Water molecules are bonded directly to iron (TGA data).
The infrared vibrational spectrum shows the occurred chelation: as a matter of fact, the spectrum has a series of characteristic bands according to the above structure.
In particular, the band due to the asymmetric stretching of carboxylic group can be observed at 1,596 cm−1 significantly moved to low frequencies with respect to free MHA (1,720 cm−1) as expected for deprotonation and coordination. A pure and stable product is thus obtained.
In an embodiment of the present invention stable solutions of iron (II) and chrome (III) chelates with MHA can be obtained by dissolution in water environment of soluble salts of iron or chrome (III) and of MHA in a ration MHA/M(III)≧2, preferably 3, and keeping pH at a suitable value so as to prevent precipitation of the corresponding hydroxides.
In a preferred embodiment the Applicant has improved the preparation of a stable solution of chrome (III) in which a chrome salt, for instance chrome sulfate Cr2(SO4)3 is reacted with methionine hydroxy analogue MHA under stirring, for instance by heating, for a time between 20 and 120 minutes, preferably between 30 and 60 minutes. Chrome salt and methionine hydroxy analogue are present in a molar ration of 1:2 to 1:30, preferably 1:2 to 1:20. At the end of the reaction a solution of chrome(III) complexes with methionine hydroxy analogue is obtained.
In another preferred embodiment of the present invention said fourth aim is achieved by suggesting the use of said new chelates, both in solid form with iron (II), vanadium (IV) and/or vanadium (V) and molybdenum (V) and/or molybdenum (VI), and in liquid form in aqueous solution with iron (II) and (III) and chrome (III), for the preparation of metal integrators for human and animal nutrition.


Metal chelates described in the present invention can be used mixed one with the other in various quantitative ratios for preparing metal integrators. Therefore, the integrators suggested both for human and animal nutrition can contain one or more metal chelates according to the present invention.
With reference to the metal chelates described above and according to the present invention the Applicant has made a series of experimental tests.
In Vitro Tests
For in vitro tests cells of human colon adenocarcinoma (CACO-2) have been used, these being the most frequently used in vitro system for studies on intestinal functionality, in particular as far as transepithelial transport is concerned, since said cells (CACO-2) develop ultra-structural, functional and electrical properties that are similar to those of small intestine.
The formation of intercellular links can be monitored through measurements of transepithelial electric resistance (TEER) of the single layer of cells. Since intercellular links limit the (para-cellular) movement of solutes, TEER alterations are commonly used as permeability index of said links.
The equipment used for cell growth and differentiation is shown in FIG. 1.
Said cells, referred to with A in FIG. 1, have been grown and differentiated on a carrier (permeable filter), referred to with B in FIG. 1, until a single layer of differentiated cells joined by functional intercellular links is formed. Said filter B separates the apical environment C, (AP), (simulating intestine lumen) from the basolateral environment D, (BL), placed in the lower chamber, simulating capillary blood flow.
Said cells have been treated for 3 hours with two different concentrations of Fe(III)/MHA (1:3) and Fe(III)/NTA (1:2) (nitriltriacetic acid taken as reference chelate), in a buffer solution at pH 5.5 and 37° C. Said solutions have been placed in the apical compartment C (AP), whereas the basolateral compartment D (BL) contained an iron-free solution of apotransferrin placed in a buffer solution at pH 7.4.
During said experiment, at pre-established time intervals, TEER has been measured in Ω·cm2. FIG. 2 (every 30 minutes over 3 hours) and FIG. 3 after 24 hours.
The results are shown in FIG. 4, indicating the content of intracellular iron after 3 hours of treatment with Fe(III)/MHA and Fe(III)/NTA at different concentrations. Data are expressed in nmoles iron/filter.
As can be inferred from FIG. 4, the passage of iron/MHA chelate from the apical environment, C, to the cell is higher than the one observed in the control.
Moreover, from FIG. 5 (showing iron transport from apical environment C to basolateral environment D after treatment with two different concentrations of Fe(III)/MHA and Fe(III)/NTA) it can be inferred that the concentration of transported iron is comparable. Data are expressed in nmoles iron/filter.
Data shown in FIGS. 4 and 5 confirm that iron chelate is strongly absorbed by cells of intestinal microvilli and moves within blood flow.
From FIG. 2 (showing TEER measurements) it can be inferred that intercellular links are unchanged, thus proving the non-toxicity of iron chelate towards cells, contrarily to what happens in the case of unchelated iron such as ferrous sulfate.
FIG. 3 shows the measurement of TEER 24 hours after the buffer solution at 5.5 containing iron/MHA or iron/NTA has been removed keeping the cells in culture. Said FIG. 3 shows how iron chelate/MHA is stable within cells causing no toxic effect.
Finally, the tests show that MHA/M chelates according to the present invention are efficiently absorbed, stable within intestinal cells and non-toxic.
The results shown above support the use of said new chelates, both in solid form with iron (II), vanadium (IV) and/or vanadium (V) and molybdenum (V) and/or molybdenum (VI), and in liquid form in aqueous solution with iron (II) and (III) and chrome (III), for the preparation of metal integrators for human and animal nutrition.
In Vivo Tests
Said tests have involved both monogastric animals (such as pigs) and polygastric animals (such as calves).
a) Monogastric Animals (Pigs)
Two test groups of pigs (Control and Test) of 35 days of age and weaned at 19 days, were administered a food differing only in the zinc source.
Said food consisted, pro kg of food as such, of 3,500 Kcal ED, 1.15 g of lysine, and a total amount of zinc element of 81 mg (81 ppm), of which 31 mg (31 ppm) were given by raw materials, whereas 50 mg (50 ppm) were respectively in form of zinc sulfate (Control) and zinc chelate with MHA (Test) according to the present invention.
The two groups of animals were balanced by nest, living weight and sex and were fed for 27 days. Other 4 animals were immediately sacrificed and a sampling was made of them according to the following procedure. The two groups of animals were weighed before starting the test and after 27 days. At the end of the test the pigs were sacrificed and stomach, intestine, left kidney and liver were removed from every pig. Stomach and intestine were emptied and weighed again so as to obtain the net weight of said organs. A sample of kidney, liver and brain was taken and frozen. Stomach, intestine, left kidney and liver were then put together with the remaining carcass and homogenized with a mixer. A sample was then taken from the mass thus obtained and frozen. The samples were then dehydrated with a dehydrating device and underwent chemical analysis.
The level of zinc, copper and iron were determined on the lyophilized samples by atomic absorption spectroscopy. The body levels of zinc were referred to the product.
On the basis of the body's “net” weight (i.e. without the content of the digestive tube) and of its content of zinc at test beginning and end it was possible to determine also daily zinc retention. The results of the chemical analyses carried out on the samples are shown in Table 1. The pigs were sacrificed at an average weight of 16.2 kg. The average daily weight increase was of 324 g.
As can be inferred from the data shown in Table 2 concerning daily zinc retention of the two different sources, the integration of zinc chelate was retained by the organism 26% more (P=0.07) than the integration with zinc sulfate. Table 3 shows the data concerning the effect of the zinc source on the content of zinc, copper and iron in liver, kidney and brain and, therefore, on the interaction with said elements present in the diet under inorganic form. As a matter of fact, it is known about the interaction exerted by said free ions by reducing one the absorption of the other.
The content of said three minerals in liver was not affected by the diet and therefore by the zinc source. Average values were 296 mg/kg for zinc, 63 mg/kg for copper and 220 for iron. Conversely, kidney showed a higher content of zinc (+18%, P=0.07), of iron (+36%, P=0.01) and of copper (+36%, P=0.12), and did not reach only for the latter value the threshold of statistic significance, though it showed a tendency towards an increase in the retention of said metal element.
In brain there was a tendency towards a higher content of zinc (+13%), of copper (+20%), of iron (+25%).
The obtained results point out a higher bioavailability of the metal element in chelated form with respect to inorganic sources such as sulfates, and further a lower interaction with other ions, which results in a higher retention of the latter.
As is known, pigs are one of man-closest animal models and as such they are often used as model for evaluations and studies in the human field.
b) Polygastric Animals (Meat Cattle)
Two groups of female Charolaise calves (30 months old) comprising 6 animals each, with an average starting weight of 567 kg (Control and of 565 kg (Test), were fed for 90 days with the same diet. The only difference was that the Control group was administered zinc carbonate and the Test group zinc chelate according to the present invention. Daily ingestion was of 22 kg/animal and the total daily supply of zinc element was of 700 mg.
Living weight at test beginning and end, dead weight and slaughtering yield were determined for each animal. Data are shown in Table 4.
Animals fed with zinc chelate with respect to those fed with zinc carbonate have a significantly higher final weight (652 kg vs. 642 kg, p<0.05), a significantly higher daily weight increase (1,039 g vs. 934 g, p<0.05), a significantly higher carcass weight (377 kg vs. 366 kg, P<0.01), and a significantly higher yield (57.83% vs. 57.03%, p<0.01). Data are shown in Table 4. The effect due to the presence of zinc chelate in the ratio administered to animals is shown in Table 5.
Said results show an evident improvement of the aforesaid zootechnical performances of zinc chelate with respect to inorganic sources of said element.
Stability constants for the various Fe/MHA complexes have been calculated with potentiometric titrations. The stability of iron (III) complexes is very high and chelated species form also at acid pH. Uncomplexed Fe3+ ions are present only at very low pH values (<2.5), whereas at higher pH values all iron (III) is complexed as chelated species metal/ligand=1:2.











TABLE NO. 1







Chelate
Sulfate
E.M.S.




















Number of days
n
26.3
26.4



Initial living weight
kg
7.54
7.33
0.50


Final living weight
kg
16.14
16.20
0.55


Daily increase
g
327
321
11


Diet
g
544
548
1.9


Conversion index

1.68
1.72
0.054


Initial net living weight
kg
7.31
7.49
0.48


Final net weight
kg
15.57
15.76
0.55


Daily net increase
g
314
313
11




















TABLE NO. 2







Chelate
Sulfate
E.M.S.






















Daily Zn retention
mg
5.40
5.27
0.37






















TABLE NO. 3










Statistic



Chelate
Sulfate
E.M.S.
significance






















Liver







Zinc
292
300
21
P = 0.80



Copper
63.6
62.5
6.3
P = 0.91



Iron
240
199
35
P = 0.44



Kidney



Zinc
97.5
82.3
5.5
P = 0.07



Copper
55.0
40.2
6.4
P = 0.12



Iron
244
179
11.8
P < 0.01



Brain



Zinc
53.9
47.6
3.5
P = 0.23



Copper
28.1
23.3
3.5
P = 0.35



Iron
100.9
80.6
9.9
P = 0.17





















TABLE NO. 4









Diet
Initial weight
E.M.S.







Control
567.700000
31.845747



Zn
565.633333
31.845747








Final weight
E.M.S.







Control
642.
2.694781



Zn
652.
2.691923











Control vs. Zn P < 0.05











Diet
Daily increase
E.M.S.







Co
931.
29.94201



Zn
1,039.
29.91025











Control vs. Zn P < 0.05











Diet
Carcass weight
E.M.S.







Control
366.
1.812368



Zn
377.
1.810445











Control vs. Zn P < 0.01












Slaughtering




Diet
weight
E.M.S.







Control
57.03
0.1132212



Zn
57.85
0.1131011











Control vs. Zn P < 0.01





















TABLE NO. 5








Initial
Final

Total
Dead
Slaughtering



Calf
weight
weight
Daily
increase
weight
weight



number
kg
kg
increase g
kg
kg
kg























CONTROL
1
583.5
670.75
1,050
94.50
383
0.578



2
583.5
670.75
970
87.30
383
0.571



3
599.5
675.96
850
76.50
388
0.574



4
540.9
623.67
920
82.80
353
0.566



5
568.1
649.12
900
81.00
370
0.570



6
532.3
624.13
1,020
91.80
357
0.572


TEST
1
625.6
724.61
1,100
99.0
421
0.581



2
676.8
789.29
1,250
112.5
457
0.579



3
582.7
686.21
1,150
103.5
398
0.580



4
564.0
653.98
1,000
90.00
378
0.578



5
476.5
557.49
900
81.00
320
0.574



6
468.2
548.28
890
80.10
318
0.580

## Claims

1. A method for preparing a metal chelate selected from the metal chelate of general formula (I):


(CH3SCH2CH2CH(OH)COO)2M.nH2O  (I)


wherein:
M is a bivalent metal cation selected from the group consisting of: Mg, Ca, Mn, Co, Cu, Zn and Fe, and n is between 0 and 6,
said method comprising a step in which there is a direct reaction between a metal (II) oxide of M and CH3SCH2CH2CH(OH)COOH and/or salts thereof.

2. The method according to claim 1, wherein the metal chelate is selected from the group consisting of:
(CH3SCH2CH2CH(OH)COO)2Zn.2H2O;
(CH3SCH2CH2CH(OH)COO)2Cu;
(CH3SCH2CH2CH(OH)COO)2Co.2H2O;
(CH3SCH2CH2CH(OH)COO)2Mn.2H2O;
(CH3SCH2CH2CH(OH)COO)2Ca.2H2O;
(CH3SCH2CH2CH(OH)COO)2Mg.2H2O; and
(CH3SCH2CH2CH(OH)COO)2Fe.2H2O.

3. A method for preparing a metal chelate of formula (CH3SCH2CH2CH(OH)COO)2Fe.2H2O comprising a step in which there is a direct reaction between an alkali metal or alkaline-earth metal salt of methionine hydroxy analogue and a soluble iron (II) salt in water.

4. The method according to claim 3, wherein said alkali metal salt is a sodium salt of methionine hydroxy analogue and said soluble iron (II) salt is a ferrous sulfate.

5. The method according to claim 4, wherein said iron (II) chelate obtained from the reaction is filtered and washed with water.