Ammonium
nitrateAmmonium Nitrate How they are manufactured?
Ammonium nitrate is made commercially by passing ammonia gas (NH3) and a water solution of nitric acid (HNO3) through a pipe. The ammonia combines with the nitric acid to form ammonium nitrate. The formula for this reaction can be written as NH3 + HNO3 → NH4NO3.
Large amounts of heat are released during the reaction, so the pipe and supporting equipment must be very strong. The solution of ammonium nitrate in water is allowed to evaporate, leaving behind pure white crystals of the compound. Key information
Other names: German saltpeter; Norway saltpeter; nitric acid, ammonium salt
Formula:
NH4NO3
Elements:
Nitrogen, hydrogen, oxygen
Compound Type:
Inorganic salt
State: solid
Some other uses of ammonium nitrate include the following: * In fireworks, where it provides the oxygen needed to ignite other chemicals; * In the manufacture of nitrous oxide (N2O), commonly known as laughing gas; * In rocket engines, where it provides oxygen needed to burn the rocket fuel; * In the manufacture of safety matches, where the compound supplies oxygen to substances that catch fire when the match is struck; and * As a nutrient in commercial processing for growing yeasts and antibiotics. (Reference 1) Advantages * Good for fertigation * high solubility * low volatility * High N (35%) * Low volatility losses * Immediately available to plant * Doesn’t react with lime * Doesn’t raise pH * High potential acidity * Remains available longer * Can be left on surface Disadvantages * Excessively leached on sandy soil * Relatively expensive * High salt index (49). Burns seedlings * Leaches immediately if over irrigated * Contains no P * Storage problems (Reference 2) Ammonium sulphate
Ammonium Sulphate
Overview
Ammonium sulphate (uh-MOH-ni-um SUL-fate) is an odourless, colourless to white crystalline solid
Ammonium nitrate is made commercially by passing ammonia gas (NH3) and a water solution of nitric acid (HNO3) through a pipe. The ammonia combines with the nitric acid to form ammonium nitrate. The formula for this reaction can be written as NH3 + HNO3 → NH4NO3.
Large amounts of heat are released during the reaction, so the pipe and supporting equipment must be very strong. The solution of ammonium nitrate in water is allowed to evaporate, leaving behind pure white crystals of the compound. Key information
Other names: German saltpeter; Norway saltpeter; nitric acid, ammonium salt
Formula:
NH4NO3
Elements:
Nitrogen, hydrogen, oxygen
Compound Type:
Inorganic salt
State: solid
Some other uses of ammonium nitrate include the following: * In fireworks, where it provides the oxygen needed to ignite other chemicals; * In the manufacture of nitrous oxide (N2O), commonly known as laughing gas; * In rocket engines, where it provides oxygen needed to burn the rocket fuel; * In the manufacture of safety matches, where the compound supplies oxygen to substances that catch fire when the match is struck; and * As a nutrient in commercial processing for growing yeasts and antibiotics. (Reference 1) Advantages * Good for fertigation * high solubility * low volatility * High N (35%) * Low volatility losses * Immediately available to plant * Doesn’t react with lime * Doesn’t raise pH * High potential acidity * Remains available longer * Can be left on surface Disadvantages * Excessively leached on sandy soil * Relatively expensive * High salt index (49). Burns seedlings * Leaches immediately if over irrigated * Contains no P * Storage problems (Reference 2) Ammonium sulphate
Ammonium Sulphate
Overview
Ammonium sulphate (uh-MOH-ni-um SUL-fate) is an odourless, colourless to white crystalline solid