MGRox
- 597
- 143
Did a little looking to see how all these salts for nutes are acquired / manufactured. A few of them were not quite what I expected.
-Ammonia (Anhydrous)
It all starts with Ammonia created by the Haber Process
"The process converts atmospheric nitrogen (N2) to ammonia (NH3) by a reaction with hydrogen (H2) using a metal catalyst under high temperatures and pressures:" "hydrogen gas obtained is from natural gas."....."Over 80% of the total cost of manufacturing NH3 is natural gas."
N2 + 3 H2 → 2 NH3 (ΔH = −92.4 kJ·mol−1)
-Urea
First Anhydrous ammonia is reacted with CO2 to produce Ammonium Carbamate.
"It is prepared by the direct reaction between liquid ammonia and dry ice.
Ammonia and carbon dioxide is excessively fed to a synthesis reactor in this process. Ammonium carbamate is produced as an intermediate in this reactor and can then be dehydrated to urea."
2 NH3(l) + CO2(s) → H2NCOONH4
NH2CO2NH4 → NH2CONH2 + H2O
***NOTE: There is NO Urine in Urea.....but there is Urea in Urine.
-Nitric Acid
"Nitric acid is made by reaction of nitrogen dioxide (NO2) with water."
3 NO2 + H2O → 2 HNO3 + NO
"Nitrogen dioxide typically arises via the oxidation of nitric oxide by oxygen in air"
2 NO + O2 → 2 NO2
"In commercial settings, Nitric Oxide is produced by the oxidation of ammonia (normally at 850 °C) with platinum as catalyst:"
4 NH3 + 5 O2 → 4 NO + 6 H2O
-Ammonium Nitrate"Nitric acid and ammonia are used to make ammonium nitrate. ....The two materials are mixed together in a tank and a neutralization reaction occurs, producing ammonium nitrate."
HNO3 + NH3 → NH4NO3
-Phosphoric Acid
"Phosphoric acid is the starting material for most of the phosphates that are produced industrially. It is obtained from the reaction of the apatite mineral with sulfuric acid."
"Wet process phosphoric acid is prepared by adding sulfuric acid to tricalcium phosphate rock, typically found in nature as apatite."
Ca5(PO4)3X + 5 H2SO4 + 10 H2O → 3 H3PO4 + 5 CaSO4·2 H2O + HX
(where X may include OH, F, Cl, and Br)
-Mono Ammonium Phosphate
"NH4H2PO4, is formed when a solution of phosphoric acid is added to ammonia until the solution is distinctly acidic. It crystallizes in tetragonal prisms."
2NH3 + H3PO4 → (NH4)2HPO4
-Diammonium Phosphate
Similar to mono Diammonium Phosphate is made by a reaction of phosphoric acid and ammonia. Mono Ammonium Phosphate is first made, then it is further reacted to ammonia to produce diammonium.
2NH3 + H3PO4 → (NH4)2HPO4
NH4H2PO4 + NH3 → (NH4)2HPO4
-Calcium Nitrate
"also called Norgessalpeter (Norwegian saltpeter). Nitrocalcite is the name for a mineral which is a hydrated calcium nitrate that forms as an efflorescence where manure contacts concrete or limestone in a dry environment as in stables or caverns."
"It is produced by treating limestone with nitric acid, followed by neutralization with ammonia:"
CaCO3 + 2 HNO3 → Ca(NO3)2 + CO2 + H2O
Ca(NO3)2 + H2O + NH3 → 5Ca(NO3)2.NH4NO3·10H2O
"The fertilizer grade (15.5-0-0 + 19% Ca).....contains ammonium nitrate and water, as the "double salt" This is called calcium ammonium nitrate." "Formulations lacking ammonia are also known: Ca(NO3)2·4H2O (11.9-0-0 + 16.9%Ca)"
-Potassium Nitrate
"On industrial scale it is prepared by the double displacement reaction between sodium nitrate and potassium chloride."
NaNO3 (aq) + KCl (aq) → NaCl (aq) + KNO3 (aq)
-Monopotassium Phosphate
Monopotassium phosphate is produced by the action of phosphoric acid on potassium carbonate.
3K2CO3 +2 H3PO4 ------> 3CO2 + 2K3PO4 + 3H2O
-Potassium Carbonate
"Potassium carbonate is prepared by the electrolysis of potassium chloride. The resulting potassium hydroxide is then carbonated using carbon dioxide to form potassium carbonate...."
2KOH + CO2 → K2CO3 + H2O
-Potassium Chloride
"Potash ores are typically rich in potassium chloride (KCl) and sodium chloride (NaCl)...."
"In the evaporation method hot water is injected into the potash which is dissolved and then pumped to the surface where it is concentrated by solar induced evaporation. Amine reagents are then added to either the mined or evaporated solutions. The amine coats the KCl but not NaCl. Air bubbles cling to the amine + KCl and float it to the surface while the NaCl and clay sink to the bottom. The surface is skimmed for the amine + KCl which is then dried and packaged for use as a K rich fertilizer"
-Potash
"Potash refers to potassium compounds and potassium-bearing materials, the most common being potassium chloride (KCl). The term "potash" comes from the Middle Dutch word potaschen ("pot ashes", 16th century). The old method of making potassium carbonate (K2CO3) was by collecting or producing wood ash (an occupation carried out by ash burners), leaching the ashes and then evaporating the resulting solution in large iron pots, leaving a white residue called "pot ash". Approximately 10% by weight of common wood ash can be recovered as pot ash. Later, "potash" became the term widely applied to naturally occurring potassium salts and the commercial product derived from them."
-Potassium Sulfate
"Potassium sulfate is produced according to the following reaction, which is conducted in so-called Mannheim furnaces"
2 KCl + H2SO4 → 2 HCl + K2SO4
-Magnesium Sulfate
"It is often encountered as the heptahydrate sulfate mineral epsomite (MgSO4·7H2O), commonly called Epsom salt..."
"The heptahydrate can be prepared by neutralizing sulfuric acid with magnesium carbonate or oxide, but it is usually obtained directly from natural sources."
-Calcium Sulfate (Gypsum)
"The main sources of calcium sulfate are naturally occurring gypsum and anhydrite which occur at many locations worldwide as evaporites. These may be extracted by open-cast quarrying or by deep mining"
As well from other sources commonly (see phosphoric acid reaction above);
"In the production of phosphoric acid from phosphate rock, calcium phosphate is treated with sulfuric acid and calcium sulfate precipitates"
-Calcium Carbonate
"The vast majority of calcium carbonate used in industry is extracted by mining or quarrying. Pure calcium carbonate (e.g. for food or pharmaceutical use), can be produced from a pure quarried source (usually marble)."
"Alternatively, calcium carbonate is prepared from calcium oxide. Water is added to give calcium hydroxide then carbon dioxide is passed through this solution to precipitate....precipitated calcium carbonate (PCC)"
CaO + H2O → Ca(OH)2
Ca(OH)2 + CO2 → CaCO3 + H2O
-Calcium Chloride
"Calcium chloride can be produced directly from limestone, but large amounts are also produced as a by-product of the Solvay process."
"The Solvay process or ammonia-soda process is the major industrial process for the production of sodium carbonate (soda ash)."....."The Solvay process results in soda ash (predominantly sodium carbonate (Na2CO3)) from brine (as a source of sodium chloride (NaCl)) and from limestone"
2 NaCl + CaCO3 → Na2CO3 + CaCl2
-Sulfur
"Elemental sulfur occurs naturally as the element (native sulfur)..... Being abundant in native form, sulfur was known in ancient times, being mentioned for its uses in ancient India, ancient Greece, China, and Egypt. Sulfur is referred to in the Bible as brimstone."
"Today, almost all elemental sulfur is produced as a byproduct of removing sulfur-containing contaminants from natural gas and petroleum. The element's largest commercial use (after mostly being converted to sulfuric acid) is to produce sulfate and phosphate fertilizers"
-Sulfuric Acid
"Sulfuric acid is produced from sulfur, oxygen and water via the conventional contact process (DCDA) or the wet sulfuric acid process (WSA)"
"sulfur is burned to produce sulfur dioxide...then oxidized to sulfur trioxide using oxygen in the presence of a vanadium(V) oxide catalyst...The sulfur trioxide is absorbed into 97–98% H2SO4 to form [URL='https://en.wikipedia.org/wiki/Oleum']oleum (H2S2O7), also known as fuming sulfuric acid."[/URL]
S (s) + O2 (g) → SO2 (g)
2 SO2 (g) + O2 (g)
2 SO3 (g) (in presence of V2O5)
H2SO4 (l) + SO3 (g)→ H2S2O7 (l)
-Ammonia (Anhydrous)
It all starts with Ammonia created by the Haber Process
"The process converts atmospheric nitrogen (N2) to ammonia (NH3) by a reaction with hydrogen (H2) using a metal catalyst under high temperatures and pressures:" "hydrogen gas obtained is from natural gas."....."Over 80% of the total cost of manufacturing NH3 is natural gas."
N2 + 3 H2 → 2 NH3 (ΔH = −92.4 kJ·mol−1)
-Urea
First Anhydrous ammonia is reacted with CO2 to produce Ammonium Carbamate.
"It is prepared by the direct reaction between liquid ammonia and dry ice.
Ammonia and carbon dioxide is excessively fed to a synthesis reactor in this process. Ammonium carbamate is produced as an intermediate in this reactor and can then be dehydrated to urea."
2 NH3(l) + CO2(s) → H2NCOONH4
NH2CO2NH4 → NH2CONH2 + H2O
***NOTE: There is NO Urine in Urea.....but there is Urea in Urine.
-Nitric Acid
"Nitric acid is made by reaction of nitrogen dioxide (NO2) with water."
3 NO2 + H2O → 2 HNO3 + NO
"Nitrogen dioxide typically arises via the oxidation of nitric oxide by oxygen in air"
2 NO + O2 → 2 NO2
"In commercial settings, Nitric Oxide is produced by the oxidation of ammonia (normally at 850 °C) with platinum as catalyst:"
4 NH3 + 5 O2 → 4 NO + 6 H2O
-Ammonium Nitrate"Nitric acid and ammonia are used to make ammonium nitrate. ....The two materials are mixed together in a tank and a neutralization reaction occurs, producing ammonium nitrate."
HNO3 + NH3 → NH4NO3
-Phosphoric Acid
"Phosphoric acid is the starting material for most of the phosphates that are produced industrially. It is obtained from the reaction of the apatite mineral with sulfuric acid."
"Wet process phosphoric acid is prepared by adding sulfuric acid to tricalcium phosphate rock, typically found in nature as apatite."
Ca5(PO4)3X + 5 H2SO4 + 10 H2O → 3 H3PO4 + 5 CaSO4·2 H2O + HX
(where X may include OH, F, Cl, and Br)
-Mono Ammonium Phosphate
"NH4H2PO4, is formed when a solution of phosphoric acid is added to ammonia until the solution is distinctly acidic. It crystallizes in tetragonal prisms."
2NH3 + H3PO4 → (NH4)2HPO4
-Diammonium Phosphate
Similar to mono Diammonium Phosphate is made by a reaction of phosphoric acid and ammonia. Mono Ammonium Phosphate is first made, then it is further reacted to ammonia to produce diammonium.
2NH3 + H3PO4 → (NH4)2HPO4
NH4H2PO4 + NH3 → (NH4)2HPO4
-Calcium Nitrate
"also called Norgessalpeter (Norwegian saltpeter). Nitrocalcite is the name for a mineral which is a hydrated calcium nitrate that forms as an efflorescence where manure contacts concrete or limestone in a dry environment as in stables or caverns."
"It is produced by treating limestone with nitric acid, followed by neutralization with ammonia:"
CaCO3 + 2 HNO3 → Ca(NO3)2 + CO2 + H2O
Ca(NO3)2 + H2O + NH3 → 5Ca(NO3)2.NH4NO3·10H2O
"The fertilizer grade (15.5-0-0 + 19% Ca).....contains ammonium nitrate and water, as the "double salt" This is called calcium ammonium nitrate." "Formulations lacking ammonia are also known: Ca(NO3)2·4H2O (11.9-0-0 + 16.9%Ca)"
-Potassium Nitrate
"On industrial scale it is prepared by the double displacement reaction between sodium nitrate and potassium chloride."
NaNO3 (aq) + KCl (aq) → NaCl (aq) + KNO3 (aq)
-Monopotassium Phosphate
Monopotassium phosphate is produced by the action of phosphoric acid on potassium carbonate.
3K2CO3 +2 H3PO4 ------> 3CO2 + 2K3PO4 + 3H2O
-Potassium Carbonate
"Potassium carbonate is prepared by the electrolysis of potassium chloride. The resulting potassium hydroxide is then carbonated using carbon dioxide to form potassium carbonate...."
2KOH + CO2 → K2CO3 + H2O
-Potassium Chloride
"Potash ores are typically rich in potassium chloride (KCl) and sodium chloride (NaCl)...."
"In the evaporation method hot water is injected into the potash which is dissolved and then pumped to the surface where it is concentrated by solar induced evaporation. Amine reagents are then added to either the mined or evaporated solutions. The amine coats the KCl but not NaCl. Air bubbles cling to the amine + KCl and float it to the surface while the NaCl and clay sink to the bottom. The surface is skimmed for the amine + KCl which is then dried and packaged for use as a K rich fertilizer"
-Potash
"Potash refers to potassium compounds and potassium-bearing materials, the most common being potassium chloride (KCl). The term "potash" comes from the Middle Dutch word potaschen ("pot ashes", 16th century). The old method of making potassium carbonate (K2CO3) was by collecting or producing wood ash (an occupation carried out by ash burners), leaching the ashes and then evaporating the resulting solution in large iron pots, leaving a white residue called "pot ash". Approximately 10% by weight of common wood ash can be recovered as pot ash. Later, "potash" became the term widely applied to naturally occurring potassium salts and the commercial product derived from them."
-Potassium Sulfate
"Potassium sulfate is produced according to the following reaction, which is conducted in so-called Mannheim furnaces"
2 KCl + H2SO4 → 2 HCl + K2SO4
-Magnesium Sulfate
"It is often encountered as the heptahydrate sulfate mineral epsomite (MgSO4·7H2O), commonly called Epsom salt..."
"The heptahydrate can be prepared by neutralizing sulfuric acid with magnesium carbonate or oxide, but it is usually obtained directly from natural sources."
-Calcium Sulfate (Gypsum)
"The main sources of calcium sulfate are naturally occurring gypsum and anhydrite which occur at many locations worldwide as evaporites. These may be extracted by open-cast quarrying or by deep mining"
As well from other sources commonly (see phosphoric acid reaction above);
"In the production of phosphoric acid from phosphate rock, calcium phosphate is treated with sulfuric acid and calcium sulfate precipitates"
-Calcium Carbonate
"The vast majority of calcium carbonate used in industry is extracted by mining or quarrying. Pure calcium carbonate (e.g. for food or pharmaceutical use), can be produced from a pure quarried source (usually marble)."
"Alternatively, calcium carbonate is prepared from calcium oxide. Water is added to give calcium hydroxide then carbon dioxide is passed through this solution to precipitate....precipitated calcium carbonate (PCC)"
CaO + H2O → Ca(OH)2
Ca(OH)2 + CO2 → CaCO3 + H2O
-Calcium Chloride
"Calcium chloride can be produced directly from limestone, but large amounts are also produced as a by-product of the Solvay process."
"The Solvay process or ammonia-soda process is the major industrial process for the production of sodium carbonate (soda ash)."....."The Solvay process results in soda ash (predominantly sodium carbonate (Na2CO3)) from brine (as a source of sodium chloride (NaCl)) and from limestone"
2 NaCl + CaCO3 → Na2CO3 + CaCl2
-Sulfur
"Elemental sulfur occurs naturally as the element (native sulfur)..... Being abundant in native form, sulfur was known in ancient times, being mentioned for its uses in ancient India, ancient Greece, China, and Egypt. Sulfur is referred to in the Bible as brimstone."
"Today, almost all elemental sulfur is produced as a byproduct of removing sulfur-containing contaminants from natural gas and petroleum. The element's largest commercial use (after mostly being converted to sulfuric acid) is to produce sulfate and phosphate fertilizers"
-Sulfuric Acid
"Sulfuric acid is produced from sulfur, oxygen and water via the conventional contact process (DCDA) or the wet sulfuric acid process (WSA)"
"sulfur is burned to produce sulfur dioxide...then oxidized to sulfur trioxide using oxygen in the presence of a vanadium(V) oxide catalyst...The sulfur trioxide is absorbed into 97–98% H2SO4 to form [URL='https://en.wikipedia.org/wiki/Oleum']oleum (H2S2O7), also known as fuming sulfuric acid."[/URL]
S (s) + O2 (g) → SO2 (g)
2 SO2 (g) + O2 (g)
H2SO4 (l) + SO3 (g)→ H2S2O7 (l)
https://en.wikipedia.org/wiki/Haber_process
http://www.madehow.com/Volume-3/Fertilizer.html
http://www.chemistryexplained.com/Hy-Kr/Industrial-Chemistry-Inorganic.html
https://en.wikipedia.org/wiki/Nitric_acid
https://en.wikipedia.org/wiki/Nitrogen_dioxide
https://en.wikipedia.org/wiki/Nitric_oxide
https://en.wikipedia.org/wiki/Ammonium_dihydrogen_phosphate
https://en.wikipedia.org/wiki/Calcium_nitrate
https://en.wikipedia.org/wiki/Ammonium_carbamate
https://en.wikipedia.org/wiki/Potassium_nitrate
https://en.wikipedia.org/wiki/Phosphoric_acid
https://en.wikipedia.org/wiki/Potassium_carbonate
https://en.wikipedia.org/wiki/Potash
https://en.wikipedia.org/wiki/Potassium_chloride
https://en.wikipedia.org/wiki/Potassium_sulfate
https://en.wikipedia.org/wiki/Potassium_carbonate
https://en.wikipedia.org/wiki/Magnesium_sulfate
https://en.wikipedia.org/wiki/Calcium_sulfate
https://en.wikipedia.org/wiki/Calcium_carbonate
https://en.wikipedia.org/wiki/Calcium_chloride
https://en.wikipedia.org/wiki/Solvay_process
https://en.wikipedia.org/wiki/Sulfur
https://en.wikipedia.org/wiki/Sulfuric_acid
https://en.wikipedia.org/wiki/Lead_chamber_process
http://www.madehow.com/Volume-3/Fertilizer.html
http://www.chemistryexplained.com/Hy-Kr/Industrial-Chemistry-Inorganic.html
https://en.wikipedia.org/wiki/Nitric_acid
https://en.wikipedia.org/wiki/Nitrogen_dioxide
https://en.wikipedia.org/wiki/Nitric_oxide
https://en.wikipedia.org/wiki/Ammonium_dihydrogen_phosphate
https://en.wikipedia.org/wiki/Calcium_nitrate
https://en.wikipedia.org/wiki/Ammonium_carbamate
https://en.wikipedia.org/wiki/Potassium_nitrate
https://en.wikipedia.org/wiki/Phosphoric_acid
https://en.wikipedia.org/wiki/Potassium_carbonate
https://en.wikipedia.org/wiki/Potash
https://en.wikipedia.org/wiki/Potassium_chloride
https://en.wikipedia.org/wiki/Potassium_sulfate
https://en.wikipedia.org/wiki/Potassium_carbonate
https://en.wikipedia.org/wiki/Magnesium_sulfate
https://en.wikipedia.org/wiki/Calcium_sulfate
https://en.wikipedia.org/wiki/Calcium_carbonate
https://en.wikipedia.org/wiki/Calcium_chloride
https://en.wikipedia.org/wiki/Solvay_process
https://en.wikipedia.org/wiki/Sulfur
https://en.wikipedia.org/wiki/Sulfuric_acid
https://en.wikipedia.org/wiki/Lead_chamber_process