Sulfamic acid (other names: aminosulfonic acid, amidosulfuric acid, sulfuric acid monoamide) is a substance that is colorless rhombic crystals. The formula for this compound is: NH2SO2OH (or NH2SO3H).
Physical properties of aminosulfonic acid:
1. This substance exists in the form of colorless crystals that are diamond-shaped. Rhombic syngony: b = 0.8025 nm, a = 0.8037 nm, z = 8, c = 0.9237 nm. As a zwitterion, it exists in a crystalline state.
2. Sulfamic acid has the following molecular weight: 97.098 amu The melting point is 205 degrees, the decomposition is 260 degrees Celsius.
3. The solubility in acetone at 25 degrees is 0.04; in water at 20 degrees 17.57, at 40 degrees 22.77 and at 80 degrees - 32.01; in diethyl alcohol at 25 ° C 0.01; in formamide at 25 degrees 0.18; in methanol at 25 degrees 0.4.
4. Has a density of 2.126 grams per centimeter³.
Chemical properties of sulfamic acid:
1. When heated to 260 degrees, it decomposes into SO2 (sulfur oxide ll), SO3 (sulfur oxide lll), N2 (nitrogen) and H2O (water). This is what the reaction looks like:
NH2SO2OH = SO2 (sulfur oxide ll) + SO3 (sulfur oxide lll) + N2 (nitrogen, liberated as gas) + H2O (water).
2. At room temperature, this substance practically does not undergo hydrolysis. But at too high temperatures, it is hydrolyzed to NH4HSO4. Moreover, in an acidic environment, the reaction rate increases significantly.
3. With various metals, their carbonates, hydroxides and oxides, aminosulfonic acid forms salts of NH2SO3M (generic name - sulfamates), with SOCl2 thionyl chloride - NH2SO2Cl sulfamoyl chloride.
4. When interacting with HNO2 (nitrous acid), it undergoes oxidative deamination - NH2SO3H + HNO22 + N2 (nitrogen, liberated in the form of gas) + H2SO4 (sulfuric acid). This reaction is used to determine the amount of sulfuric acid monoamide and to decompose an excess of nitrous acid (HNO2) in the manufacture of azo dyes.
5. Sulfamic acid is oxidized by chlorine (Cl), bromine (Br), potassium permanganate (KMnO4) and chlorates to sulfuric acid (H2SO4) and nitrogen (N2).
6. The reaction of this acid with HClO (hypochlorous acid) or NaClO (sodium hypochlorite) leads to the formation of N, N-dichloro or N-chloro derivatives. Reaction with sodium (Na) in liquid ammonia (NH3) to NaSO3NHNa, with sodium sulfate (Na2SO4) to 6HSO3NH2 · 5Na2SO4 · 15H2O.
7. Sulfur monoamide also reacts with primary alcohols and secondary alcohols with phenols. Tertiary, secondary and primary amines form aminosulfamates with this acid, and carboxylic amides form ammonium N-acyl sulfamates.
8. A reaction with nitrous acid (HNO2) or fusion with benzoin (C14H12O3) is used to identify aminosulfonic acid.
The use of sulfuric acid monoamide
1. Industrial chemistry: for cleaning equipment from beer and milk stone, from various mineral deposits (oxide films, hardness salts, iron compounds). The production of hydrochloric acid in this case becomes disadvantageous, since sulfamic acid is less corrosive.
2. At home and at public catering enterprises: for the processing of kitchen and dining utensils, as part of some detergents.
3. As a raw material for the production of certain chemical compounds, for example, herbicides and fire-resistant materials.
4. In electroplating: for pickling food tin and for creating electrolytes.
5. To remove mucus from pools (their water-cooling systems).
6. When cleaning machines designed to create paper.
7. When processing the zone of oil wells.
How should sulfamic acid be stored properly, and what precautions should be followed when using it?
Sulfur monoamide is a non-combustible substance. According to the degree of impact on a living organism, it belongs to compounds of the third hazard class. Causes severe burns to the skin and mucous membranes.
This acid is stored in double plastic bags (capacity forty kilograms), designed specifically for chemical products. It is worth considering that the product is highly soluble in H2O (water). It is caked during long-term storage.