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WO1999022889A1 - Elements fertilisants ameliores - Google Patents

Elements fertilisants ameliores Download PDF

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Publication number
WO1999022889A1
WO1999022889A1 PCT/IL1998/000514 IL9800514W WO9922889A1 WO 1999022889 A1 WO1999022889 A1 WO 1999022889A1 IL 9800514 W IL9800514 W IL 9800514W WO 9922889 A1 WO9922889 A1 WO 9922889A1
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WO
WIPO (PCT)
Prior art keywords
potassium
fertilizer
mixture
sulfate
potassium nitrate
Prior art date
Legal status (The legal status is an assumption and is not a legal conclusion. Google has not performed a legal analysis and makes no representation as to the accuracy of the status listed.)
Ceased
Application number
PCT/IL1998/000514
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English (en)
Inventor
Menachem Bareket
Eldad Bareket
Current Assignee (The listed assignees may be inaccurate. Google has not performed a legal analysis and makes no representation or warranty as to the accuracy of the list.)
BAREKET ASAF
BAREKET SHARON
Original Assignee
BAREKET ASAF
BAREKET SHARON
Priority date (The priority date is an assumption and is not a legal conclusion. Google has not performed a legal analysis and makes no representation as to the accuracy of the date listed.)
Filing date
Publication date
Application filed by BAREKET ASAF, BAREKET SHARON filed Critical BAREKET ASAF
Priority to AU96419/98A priority Critical patent/AU9641998A/en
Publication of WO1999022889A1 publication Critical patent/WO1999022889A1/fr
Anticipated expiration legal-status Critical
Ceased legal-status Critical Current

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Classifications

    • C—CHEMISTRY; METALLURGY
    • C05—FERTILISERS; MANUFACTURE THEREOF
    • C05C—NITROGENOUS FERTILISERS
    • C05C5/00—Fertilisers containing other nitrates
    • C05C5/02—Fertilisers containing other nitrates containing sodium or potassium nitrate
    • C—CHEMISTRY; METALLURGY
    • C05—FERTILISERS; MANUFACTURE THEREOF
    • C05G—MIXTURES OF FERTILISERS COVERED INDIVIDUALLY BY DIFFERENT SUBCLASSES OF CLASS C05; MIXTURES OF ONE OR MORE FERTILISERS WITH MATERIALS NOT HAVING A SPECIFIC FERTILISING ACTIVITY, e.g. PESTICIDES, SOIL-CONDITIONERS, WETTING AGENTS; FERTILISERS CHARACTERISED BY THEIR FORM
    • C05G5/00—Fertilisers characterised by their form
    • C05G5/20—Liquid fertilisers
    • C05G5/23—Solutions

Definitions

  • the present invention relates to an improved fertilizer and, more specifically, to a novel fully water-soluble combination of potassium sulfate and potassium nitrate which is superior to either fertilizer alone.
  • Fertilizers are administered to plants, such as crops in the field or in a greenhouse, in order to improve their growth and to enhance the yield of any desirable portions of the plant, such as the fruits. Fertilizers can also enhance the quality of the soil by increasing the concentration of certain plant nutrients, or even to completely supply these nutrients in situations where they would normally be absent, such as in the hydroponic cultivation of plants.
  • One of the most important groups of commercially available fertilizers is the potassium-containing or potassic fertilizers.
  • the main commercial potassium fertilizers which supply potassium to plants as their main ingredient are potassium chloride, potassium sulfate, and potassium nitrate. Their respective potassium contents, in terms of K 2 0 concentration, are about 60%, 50%, and 46%, depending on the source, producer and purity of the commercial product.
  • each type of potassium fertilizer has both advantages and disadvantages.
  • potassium chloride is relatively inexpensive and easy to produce
  • many crop plants are sensitive to chloride, such as tobacco, citrus, and most of the vegetables and flowers grown intensively, mostly as protected crops.
  • Such crops receive relatively large amounts of fertilizers per unit area, and the residual ions like Cl " (chloride) from fertilizers cause specific, undesirable ion effects or else cause damage through salt accumulation simply by their relatively high concentration.
  • high concentrations of S0 4 ⁇ (sulfate) ions in the environment of protected crops may also cause damage, even though at certain concentrations sulfur is also an important plant nutrient.
  • Potassium nitrate which is currently the major fully water-soluble chloride- free potassic fertilizer, does not share these problems related to ion concentration.
  • potassium nitrate is used as soluble fertilizer applied in solutions mainly for protected crops, where high ion concentrations are particularly problematic, or for "fertigation".
  • fertigation refers to fertilization through irrigation systems, by first dissolving the fertilizer in water tanks and then pumping the solution into the irrigation system, for example.
  • Potassium nitrate thus has many advantages as a chlorine-free, fully water soluble, concentrated potassic and nitrate fertilizer; however, it also has some disadvantages, of which the main ones are listed below:
  • potassium nitrate is relatively quite expensive overall.
  • both the potassium and the nitrate portions are more expensive than, for example, potassium of potassium sulfate or nitrate of ammonium nitrate, a very common nitrogenous fertilizer.
  • the mixture of ammonium and nitrate as sources of nitrogen from ammonium nitrate is more desirable, and of course, less expensive, than nitrate alone from potassium nitrate.
  • potassium nitrate is a very imbalanced plant nutrient source in several respects.
  • the ratio of potassium to nitrogen in terms of %K 2 O:N is about 3.5: 1, which is much higher than most plants require.
  • potassium nitrate does not contain other necessary plant nutrients which could improve its nutritional balance and its performance.
  • Potassium nitrate is also difficult to dissolve in cold water since the dissolution process is endothermic, causing the temperature of the solution to drop considerably during the process of dissolution and further reducing solubility. Such low solubility is particularly inconvenient for fertilizing crops in northern climatic zones in the winter. Under these conditions, the solution requires a longer stirring time, and in many instances, the water and solution must be warmed, causing significant inconvenience to the grower.
  • potassium sulfate An increasing share of "soluble" (fully water-soluble) potassium sulfate is also used in or through solutions, soluble fertilizers, foliar fertilizers, and the like. Since the commercial standard potassium sulfate is usually not clean and not fully water soluble, "soluble" potassium sulfate is a purified crystalline product with smaller particles, usually obtained by re-crystallization of the regular standard fertilizer grade of potassium sulfate. Even so, potassium sulfate is still considerably less expensive than potassium nitrate.
  • potassium sulfate even the "soluble" product, has a number of disadvantages.
  • Potassium sulfate also has low solubility, even lower than that of potassium nitrate at low temperatures of 0°C - 10°C.
  • sulfur is a nutrient element, the ratio of sulfur to potassium is very high, often resulting in an excess of sulfate ions which, as mentioned above, have specific ion and/or "high salt” adverse effects on plants, increase the electrical conductivity of the soil solution and cause stress effects on the environment.
  • cash or protected crops only limited amounts of potassium sulfate can be administered for optimal yield and quality of the agricultural and horticultural products.
  • a fully water-soluble fertilizer for plants comprising a composition of potassium nitrate and potassium sulfate.
  • the potassium nitrate and the potassium sulfate are present at a ratio in a range of from about 85: 15 to about 50:50 percent weight by weight.
  • the potassium nitrate and the potassium sulfate are independently in a form selected from the group consisting of crystalline, compacted, granulated, prilled and powdered.
  • the composition is a mixture of potassium nitrate and potassium sulfate.
  • the composition is a double salt of potassium nitrate and potassium sulfate.
  • the fertilizer further includes an additional source of nitrogen.
  • the additional source of nitrogen is urea present in a ratio in a range of from about 10% to about 40% weight per weight.
  • the additional source of nitrogen is ammonium nitrate present in a ratio in a range of from about 10% to about 40% weight per weight.
  • a method of administering a fertilizer to a plant in solution comprising the steps of: (a) providing a fertilizer, the fertilizer including a composition of potassium nitrate and potassium sulfate; (b) placing the fertilizer in water to form the solution; and (c) administering the solution to the plant.
  • the potassium nitrate and the potassium sulfate are placed in the water sequentially.
  • the potassium nitrate and the potassium sulfate are placed in the water simultaneously.
  • the composition is a mixture of potassium nitrate and potassium sulfate.
  • the composition is a double salt of potassium nitrate and potassium sulfate.
  • a method of production of a fully water-soluble fertilizer comprising the step of: (a) mixing dry, water-soluble potassium nitrate and dry, water-soluble potassium sulfate to form a dry mixture.
  • the method further includes the step of: (b) grinding the dry mixture to form the fertilizer.
  • a method of production of a fully water-soluble fertilizer comprising the steps of: (a) mixing a brine of potassium nitrate and a brine of potassium sulfate to form a solution; and (b) drying the solution to form a dried composition, the dried composition forming the fertilizer.
  • the method further includes the steps of: (c) grinding the dried composition to form a ground composition; and (d) mixing the ground composition to form the fertilizer.
  • a method of production of a fully water-soluble fertilizer comprising the steps of: (a) mixing nitric acid, sulfuric acid and potassium chloride to form hydrochloric acid, potassium nitrate and potassium sulfate; and (b) removing the hydrochloric acid to form the fertilizer.
  • the hydrochloric acid is removed by a process selected from the group consisting of ion exchange and an extraction process.
  • the nitric acid and the sulfuric acid are mixed first to form a mixture, and the potassium chloride is added to the mixture.
  • step (a) the potassium chloride and the nitric acid are mixed first to form a mixture, and the sulfuric acid is added to the mixture. Also alternatively and preferably, in step (a), the potassium chloride and the sulfuric acid are mixed first to form a mixture, and the nitric acid is added to the mixture.
  • a method of production of a fully water-soluble fertilizer comprising the steps of: (a) mixing potassium chloride, sodium nitrate and sodium sulfate to form potassium nitrate, potassium sulfate and sodium chloride; and (b) removing the sodium chloride by a process of double-decomposition to form the fertilizer.
  • step (a) the potassium chloride and the sodium nitrate are mixed first to form a mixture, and the sodium sulfate is added to the mixture.
  • step (a) the sodium nitrate and the sodium sulfate are mixed first to form a mixture, and the potassium chloride is added to the mixture.
  • step (a) the potassium chloride and the sodium sulfate are mixed first to form a mixture, and the sodium nitrate is added to the mixture.
  • a fully water-soluble fertilizer for plants comprising a composition of potassium nitrate and magnesium sulfate.
  • the potassium nitrate and the magnesium sulfate are present at a ratio in a range of from about 85: 15 to about 50:50 percent weight by weight.
  • the composition is a mixture of the potassium nitrate and the magnesium sulfate.
  • the composition is a double salt of the potassium nitrate and the magnesium sulfate.
  • a method of production of a fully water-soluble fertilizer comprising the step of mixing dried potassium nitrate and dried magnesium sulfate to form the fertilizer.
  • the dried potassium nitrate is formed by drying a solution of potassium nitrate and the dried magnesium sulfate is formed by drying a solution of magnesium sulfate.
  • a method of production of a fully water-soluble fertilizer comprising the steps of: (a) dissolving MgO in a potassium nitrate solution; (b) mixing the solution with H 2 SO 4 to obtain potassium nitrate and magnesium sulfate in a mixed solution; and (c) drying the mixed solution to form the fertilizer.
  • a method of production of a fully water-soluble fertilizer comprising the step of: mixing potassium chloride, magnesium chloride, nitric acid and sulfuric acid to form potassium nitrate and magnesium sulfate.
  • the potassium chloride and magnesium chloride are mixed first to form a mixture, and the nitric acid and the sulfuric acid are added to the mixture.
  • the nitric acid is added to the mixture first.
  • the sulfuric acid is added to the mixture first.
  • tap water refers to water obtained from an ordinary household water supply, without any additional filtration, purification or modification.
  • composition refers to both mixtures and double salts of potassium nitrate and potassium sulfate.
  • the double salts may be either prepared by manufacture as substantially one unit, or by mixture of already manufactured potassium nitrate and potassium sulfate.
  • fully water-soluble is defined according to the usage known in the art of fertigation.
  • the present invention is of a novel fertilizer composition, consisting of a mixture of potassium nitrate and potassium sulfate as fully water soluble compounds in crystalline, granular, compacted or prilled form.
  • the mixture of solid soluble potassium nitrate and potassium sulfate contains these compounds in a ratio of from about 85% potassium nitrate and 15% potassium sulfate to about 50% potassium nitrate and 50% potassium sulfate.
  • a method of using the fertilizer of the present invention to deliver nutrients to plants, in which the fertilizer is dissolved in water and applied to soil or other growth media, and/or directly to plants.
  • potassium nitrate and potassium sulfate could be dissolved simultaneously or sequentially in the same tank of water in order to fertigate or to obtain a solution for plant nutrition.
  • the present invention also encompasses methods for production of the fertilizer of the present invention by dry mixing, by mixing of liquids followed by crystallization and dry mixing, or by simultaneous production of the mixture. Such simultaneous production could be performed according to one of many possible chemical processes.
  • potassium chloride, nitric acid and sulfuric acid could be combined according to the following equation:
  • the present invention has a number of advantages over prior art fertilizers and methods of application and production of these fertilizers.
  • the solubility of the new product at low temperatures is similar or better than that of potassium nitrate alone or potassium sulfate alone, thus enabling better and easier dissolution and application by fertigation, especially in cold climates.
  • the provision of both the sulfate and nitrate ion nutrients provides a more efficient and balanced plant-nutrient source, both in terms of the relative amounts of sulfate and nitrate provided and the ability of sulfate to increase the efficacy of nitrate as a plant nutrient.
  • the present invention provides more efficient and energy-saving methods for production of the fertilizer mixture.
  • the solubility of mixtures of fully water-soluble potassium nitrate and potassium sulfate at various ratios was tested by adding these compounds, alone or in combination, to tap water and measuring both the amount which dissolved and the resultant temperature of the solution. Essentially, at certain ratios of potassium sulfate and potassium nitrate, the solubility of both substances in the mixture is improved as compared to the solubility of either substance alone.
  • the experimental protocol was as follows.
  • the temperature of tap water alone was measured to be 20°C.
  • 30 grams of commercially available fertilizer grade crystalline KN0 3 (potassium nitrate, also designated as "KN" in Table 1 below) of formula 13-0-46 (13% N, 0% P 2 O 5 and 46% K 2 O; product of Haifa Chemicals, Haifa, Israel) were added to 200 cc of tap water and stirred vigorously for 5 minutes to form a solution.
  • the temperature of the resultant solution dropped to 9°C.
  • the amount of potassium nitrate dissolved until saturation measured 28.5 g, or 14.25 g per 100 cc of tap water.
  • the first such mixture to be tested was of potassium nitrate and potassium sulfate in a 1 : 1 ratio.
  • 15 g KN0 3 and 15 g K 2 S0 4 were mixed together in dry form.
  • the mixture was then dissolved in tap water as described previously to form a solution.
  • the temperature of the resultant solution was 13°C.
  • the amount of the dry mixture which dissolved in 200 cc of tap water at saturation was 27 g, or 13.5 g per 100 cc of tap water.
  • the next such mixture to be tested was of potassium nitrate and potassium sulfate in a 2: 1 ratio.
  • potassium nitrate and potassium sulfate were tested in a 1 :2 ratio. 10 g KN0 3 and 20 g K 2 S0 4 were again mixed together in dry form. The mixture was then dissolved in tap water as described previously to form a solution. It should be noted that the temperature of the tap water was 21.5° C, slightly higher than for the previous tests. The temperature of the resultant solution was 15°C. The amount of the dry mixture which dissolved in 200 cc of tap water at saturation was 25.4 g, or 12.7 g per 100 cc of tap water.
  • tap water was heated to 58° C to assess the effect of heating on solubility of the mixture.
  • 60 g of a mixture of potassium nitrate and potassium sulfate in a 1 : 1 ratio was added to 200 cc of tap water at 58° C, and treated as above.
  • the temperature of the resultant solution dropped to 38.5° C and 45.8 g of the mixture was dissolved at saturation, or 22.9 g per 100 cc of tap water.
  • heating the tap water increased the solubility of the mixture.
  • the undissolved residue was not analyzed. However, this residue is known from the literature to be largely composed of K 2 SO 4 .
  • potassium sulfate caused a smaller decrease in the temperature of the tap water, its solubility was lower than that of potassium nitrate.
  • the solubility of the mixture of potassium nitrate and potassium sulfate was even better than that of potassium nitrate alone, even without heating of the tap water, and the drop in temperature of the resultant solution was intermediate.
  • the mixture improves the solubility of potassium nitrate and potassium sulfate at certain ratios and temperatures, while being a better and more complete source of plant nutrients.
  • Example 2 Test of the Mixture as a Fertilizer The most soluble mixture tested in Example 1 , potassium nitrate and potassium sulfate in a 2:1 ratio, was tested as a source of plant nutrients. The plants were cherry tomatoes [Please give me the scientific name], rooted in two types of soil media. For controls, potassium sulfate and potassium nitrate were tested alone, as were mixtures of potassium nitrate or potassium sulfate and magnesium sulfate. Essentially, similar yields were obtained when either the mixture of potassium sulfate and potassium nitrate, or the mixture of potassium nitrate and magnesium sulfate, was added.
  • the experimental method was as follows. First, cherry tomatoes were planted in 2 liter pots, containing one of two types of soil media. The first type of soil media was a sandy soil, obtained from Rehovot, Israel. The second type of soil media was a calcareous silty-clay soil, obtained from Zichron-Jacob, Israel. The pots were placed under a high plastic cover and each pot received 2 g TSP (Triple SuperPhosphate 46%) three times during the growth period, for a total of 6 g of fertilizer. Pots containing sandy soil which did not receive magnesium sulfate as a fertilizer had 10 g of Dolomite added per pot after planting, as this type of soil typically lacks magnesium.
  • the overall concentration of nutrients included 150 ppm nitrogen and 200 ppm potassium. The additional nitrogen was applied as ammonium nitrate.
  • those treatments which included magnesium received magnesium sulfate at a ratio of potassium oxide to magnesium oxide of 4 : 1 , or 60 ppm magnesium oxide per pot, which is about 180 ppm magnesium sulfate with 45 ppm of sulfur.
  • the tomato fruits were picked eight times during the growth period, and were then weighed. The yield results appear in Table 3.
  • potassium nitrate production processes include benefaction of potash ores and mines, treatment with sulfuric acid as employed in the Manheim, Chisso and Climax processes, and treatment of potassium chloride with sulfate salts.
  • soluble potassium sulfate is produced by re-crystallization of the standard, fertilizer grade potassium sulfate.
  • the various mixtures of soluble potassium nitrate and potassium sulfate which are the subject of this invention, can be produced according to several different methods.
  • one method includes thorough mixing of the crystalline or powder potassium nitrate at the desired ratio with the crystalline or powder "soluble" grade potassium sulfate. If necessary and desired, the resultant mixture can be ground and further mixed.
  • the brines of the two compounds can be mixed prior to drying. Also alternatively, the brines can first be dried to form two dried substances, which are then either directly mixed, or else first ground and then mixed.
  • Another possible process is the extraction process of IMI, or Haifa Chemicals, with the necessary modifications.
  • This process could be used to extract a mixture of potassium nitrate and potassium sulfate by treating potassium chloride with the desired ratio of HNO 3 + H 2 S0 4 .
  • One of the advantages here is that the process of formation of potassium nitrate is exothermic while that of the formation of potassium sulfate is endothermic overall, thereby enabling energy to be saved while controlling the temperature of the solutions. Adaptation of the solvents and the usage of catalysts may be required.
  • One advantage of this method is the possibility to directly achieve a fully water-soluble mixture or double salt. The disadvantage is that it will not be practical to produce in this way more than 1 or 2 mixtures with different ratios.
  • such mixtures could be produced by reacting KC1 + HN0 3 + H 2 SO and removing the hydrochloric acid by physico-chemical methods.
  • the mixtures can be granulated and compacted for easier usage and handling.
  • the mixture of salts of NaNO 3 + Na 2 SO 4 could be reacted with potassium chloride. This step is followed by separation of the sodium chloride, and purification of the resulting mixture of potassium sulfate and potassium nitrate
  • the most preferred ratios for potassium nitrate and potassium sulfate (KNO 3 : K 2 SO 4 ) and the resulting fertilizer formulae are given in Table 4 below.
  • the resulting formulae are given according to the international convention, as the ratio of percent elemental nitrogen, to percent phosphorous as P 2 0 5 , to percent potassium as K 2 O. Since none of the compositions contain P 2 0 5 , the percentage of that substance is zero for all formulae.
  • Example 4 Additional Formulae Additional sources of nitrogen can be added to the mixtures of the present invention in order to adjust the nitrogen content or to produce a more efficient or more complete fertilizer. Although a number of different nitrogen-containing compounds could be added, certain non-limiting illustrative mixtures are described herein, along with methods for their production.
  • ammonium nitrate could be added to a mixture of potassium nitrate and potassium sulfate having a formula of 8-0-49 according to the international convention described above, so that the final ratio of potassium nitrate and potassium sulfate to ammonium nitrate in the mixture is 45.3:54.7.
  • This mixture has a formula of 22-0-22. The mixture must either be done with granulated products, or be granulated by itself.
  • urea in crystalline form was added to the above mixture of potassium nitrate and potassium sulfate.
  • the compounds were then thoroughly mixed together to form a final mixture.
  • the final water-soluble mixture had a ratio of potassium nitrate and potassium sulfate to urea of 47:53, with a formula of 28-0-28 (28% N : 28% K 2 0). The same can be done with the granular forms of these compounds.
  • Example 5 Magnesium Sulfate Mixtures
  • magnesium sulfate can also be used as a source of sulfate.
  • mixtures of potassium nitrate and magnesium sulfate also have improved solubility at lower temperatures when compared to potassium nitrate alone.
  • some of the commercially available potassium nitrate fertilizers have relatively small amounts of soluble magnesium sulfate added to the extent of 2-4% nominal MgO, which is not an effective amount.
  • considerably higher amounts of soluble magnesium sulfate would be added to potassium nitrate to form mixtures according to the present invention.
  • These mixtures would have improved solubility at lower temperatures, as well as sufficient amounts of the important plant nutrients magnesium and sulfur.
  • the most preferred ratios of magnesium sulfate to potassium nitrate would be from about 15% to about 50%.
  • the desired ratio of K 2 O: MgO for tomatoes is about 5:1, meaning about 79% potassium nitrate and about 21% magnesium sulfate in the mixture.
  • Example 2 A similar procedure was followed as for Example 1. 30 g of each mixture I- IV, as well as 30 g of each compound alone, were dissolved in 200 cc of tap water at 28° C and the solubility was determined at saturation. The results are shown in Table 6.
  • magnesium sulfate at any ratio of potassium nitrate to magnesium sulfate enhances the solubility of the mixture beyond that of potassium nitrate alone.
  • certain ratios such as 5: 1 or 3: 1 potassium nitrate to magnesium sulfate, also were more soluble than magnesium sulfate alone.
  • the dissolution of the mixtures was less endothermic and/or more exothermic than the dissolution of potassium nitrate alone.
  • these mixtures display greater solubility than potassium nitrate alone.
  • solubility is even more important at lower temperatures, such as those experienced in more northern climates in the winter season.
  • Mixtures of potassium nitrate and magnesium sulfate can be produced by several methods. For example, fully water soluble crystalline potassium nitrate can be mixed with crystalline soluble magnesium sulfate at the desired ratios, as is currently being done by the relevant producers. Dried material used for the mixtures could also be granulated or compacted. In a second method, powdered MgO could be dissolved in a potassium nitrate solution. The resultant solution would then be mixed with H 2 SO 4 at the desired ratio to obtain potassium nitrate and magnesium sulfate in solution, which could then be crystallized and dried to form the dried fertilizer. Alternatively, solutions of potassium nitrate and magnesium sulfate could be mixed, crystallized and dried. Optionally, potassium nitrate and magnesium sulfate could be produced from potassium chloride, magnesium chloride, HNO 3 and H 2 SO 4 .

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  • Chemical & Material Sciences (AREA)
  • Organic Chemistry (AREA)
  • Life Sciences & Earth Sciences (AREA)
  • Pest Control & Pesticides (AREA)
  • Fertilizers (AREA)

Abstract

L'invention concerne un fertilisant pour les plantes, qui renferme une composition de nitrate de potassium et de sulfate de potassium. Le nitrate de potassium et le sulfate de potassium sont présents de préférence dans un rapport allant de 85:15 à environ 50:50 pourcent en poids. Font aussi l'objet de cette invention des procédés de préparation et d'utilisation de fertilisants.
PCT/IL1998/000514 1997-10-31 1998-10-21 Elements fertilisants ameliores Ceased WO1999022889A1 (fr)

Priority Applications (1)

Application Number Priority Date Filing Date Title
AU96419/98A AU9641998A (en) 1997-10-31 1998-10-21 Improved plant nutrients

Applications Claiming Priority (2)

Application Number Priority Date Filing Date Title
IL12208397A IL122083A0 (en) 1997-10-31 1997-10-31 Improved plant nutrients
IL122083 1997-10-31

Publications (1)

Publication Number Publication Date
WO1999022889A1 true WO1999022889A1 (fr) 1999-05-14

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PCT/IL1998/000514 Ceased WO1999022889A1 (fr) 1997-10-31 1998-10-21 Elements fertilisants ameliores

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AU (1) AU9641998A (fr)
IL (1) IL122083A0 (fr)
WO (1) WO1999022889A1 (fr)

Cited By (4)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
CN102276358A (zh) * 2011-07-21 2011-12-14 长子县方兴现代农业有限公司 无土栽培樱桃番茄营养液及制备方法
EP2603476A4 (fr) * 2010-08-11 2017-11-01 AdvanSix Resins & Chemicals LLC Compositions et méthodes pour détecter des utilisations illégales des engrais
US12221400B2 (en) 2017-02-22 2025-02-11 Lucas TYREE Foliar feeding formulation and methods of use
US12221397B2 (en) 2015-08-31 2025-02-11 Lucas Tyree Foliar feeding formulation and methods of use

Citations (3)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
US2050493A (en) * 1933-01-21 1936-08-11 Atmospheric Nitrogen Corp Compositions of matter containing ammonia and potassium nitrate, their preparation and use
US2061534A (en) * 1932-07-20 1936-11-17 Ig Farbenindustrie Ag Fertilizer in granular form
US4175943A (en) * 1973-12-19 1979-11-27 Triomf Fertilizers Water-soluble fertilizers

Patent Citations (3)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
US2061534A (en) * 1932-07-20 1936-11-17 Ig Farbenindustrie Ag Fertilizer in granular form
US2050493A (en) * 1933-01-21 1936-08-11 Atmospheric Nitrogen Corp Compositions of matter containing ammonia and potassium nitrate, their preparation and use
US4175943A (en) * 1973-12-19 1979-11-27 Triomf Fertilizers Water-soluble fertilizers

Cited By (5)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
EP2603476A4 (fr) * 2010-08-11 2017-11-01 AdvanSix Resins & Chemicals LLC Compositions et méthodes pour détecter des utilisations illégales des engrais
CN102276358A (zh) * 2011-07-21 2011-12-14 长子县方兴现代农业有限公司 无土栽培樱桃番茄营养液及制备方法
CN102276358B (zh) * 2011-07-21 2015-10-28 长子县方兴现代农业有限公司 无土栽培樱桃番茄营养液及制备方法
US12221397B2 (en) 2015-08-31 2025-02-11 Lucas Tyree Foliar feeding formulation and methods of use
US12221400B2 (en) 2017-02-22 2025-02-11 Lucas TYREE Foliar feeding formulation and methods of use

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AU9641998A (en) 1999-05-24
IL122083A0 (en) 1998-03-10

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