Does ammonium nitrate react with acid?
The industrial production of ammonium nitrate entails the acid-base reaction of ammonia with nitric acid: HNO3 + NH3 → NH4NO. Ammonia is used in its anhydrous form (a gas) and the nitric acid is concentrated. The reaction is violent owing to its highly exothermic nature.
Is ammonium nitrate an acid or base?
Is ammonium nitrate a base or acid? Ammonium nitrate is not acid but a salt but the solution is acidic since it is a salt with a weak base (ammonium hydroxide) and a heavy nitric acid.
What acid base makes ammonium nitrate?
Ammonium nitrate is the ammonium salt of nitric acid. It has a role as a fertilizer, an explosive and an oxidising agent. It is an inorganic molecular entity, an ammonium salt and an inorganic nitrate salt.
What is the chemical reaction when ammonium nitrate explodes?
Once a reaction is sparked, ammonium nitrate explodes violently. The explosive force occurs when solid ammonium nitrate decomposes very rapidly into two gases, nitrous oxide and water vapor.
Will ammonium nitrate explode on its own?
Ammonium nitrate would only explode on its own if its temperature was rapidly raised to 400 degrees Fahrenheit. Compared to most combustible materials, ammonium nitrate itself is not exceptionally explosive. But the compound can contribute to explosions because it belongs to a chemical class known as oxidizers.
What triggers ammonium nitrate to explode?
Over time, the compound absorbs moisture, which can make the beads stick together into a huge rock, says Sella. When such a large quantity of compacted ammonium nitrate is exposed to intense heat — if, say, an accidental fire breaks out — it can trigger an explosion.
What is ammonium nitrate commonly used for?
Ammonium nitrate, (NH4NO3), a salt of ammonia and nitric acid, used widely in fertilizers and explosives. The commercial grade contains about 33.5 percent nitrogen, all of which is in forms utilizable by plants; it is the most common nitrogenous component of artificial fertilizers.
What are the two main uses for ammonium nitrate?
Uses. Ammonium nitrate is used commonly in fertilizers; in pyrotechniques, herbicides, and insecticides; and in the manufacture of nitrous oxide. It is used as an absorbent for nitrogen oxides, an ingredient of freezing mixtures, an oxidizer in rocket propellants, and a nutrient for yeast and antibiotics.
Can ammonium nitrate explode on its own?
Is ammonium nitrate safe to touch?
Under normal handling conditions, ammonium nitrate is not harmful. Ammonium nitrate forms a mild acid when mixed with water. This acid can cause irritation to the eyes, nose, and skin.
What are the hazards of ammonium nitrate?
CAUSES IRRITATION TO SKIN, EYES AND RESPIRATORY TRACT. Inhalation: May cause irritation to the respiratory tract; symptoms may include coughing, sore throat, and shortness of breath. At high temperatures, exposure to toxic nitrogen oxides decomposition products can quickly cause acute respiratory problems.
What is the reaction between ammonium nitrate and pyrite?
Ammonium nitrate and pyrite react to produce nitric oxide and nitrous acid. Thermal decomposition is accelerated by NOx and nitrous acid catalysts. Adsorption of NO x gas slows the decomposition of ammonium nitrate with pyrite. Hydrotalcite adsorbs NOx gases to inhibit the thermal decomposition.
What was the solution of ammonium nitrate with nitric acid called?
The solution of ammonium nitrate with nitric acid, called Cavea-b showed promise for use in spacecraft as a more energetic alternative to the common monopropellant hydrazine.
Which is the conjugate acid of the base ammonia?
The hydroxide ion is the conjugate base of water, which acts as an acid, and the ammonium ion is the conjugate acid of the base, ammonia. Acid-base titration can determine the concentrations of unknown acid or base solutions.
How are the moles of ammonium nitrate produced?
Ammonium nitrate decomposes in an exothermic reaction (ΔH = –36 kJ mol −1) to produce three moles of gaseous products for each mole of solid reactant: (1) NH 4 NO 3 (s) → N 2 O (g) + 2 H 2 O (g)